Podcast
Questions and Answers
In the reaction $2H_2S + 3O_2 \rightarrow 2H_2O + 2SO_2$, which element undergoes oxidation?
In the reaction $2H_2S + 3O_2 \rightarrow 2H_2O + 2SO_2$, which element undergoes oxidation?
- None of the elements are oxidized
- Oxygen
- Hydrogen
- Sulfur (correct)
Which of the following statements accurately describes the relationship between oxidation number and reduction?
Which of the following statements accurately describes the relationship between oxidation number and reduction?
- Oxidation number remains constant during reduction.
- Oxidation and reduction both result in an increase in oxidation number.
- Reduction is indicated by an increase in oxidation number.
- Reduction is indicated by a decrease in oxidation number. (correct)
In an electrochemical cell, what process occurs at the anode?
In an electrochemical cell, what process occurs at the anode?
- Reduction
- No reaction
- Electron transfer only
- Oxidation (correct)
Consider the reaction $Fe + CuSO_4 \rightarrow FeSO_4 + Cu$. Which species is the oxidizing agent?
Consider the reaction $Fe + CuSO_4 \rightarrow FeSO_4 + Cu$. Which species is the oxidizing agent?
What condition defines standard cell potential ($E^\circ$) measurement?
What condition defines standard cell potential ($E^\circ$) measurement?
A substance has a very high positive reduction potential. What does this indicate about its properties?
A substance has a very high positive reduction potential. What does this indicate about its properties?
In an electrolytic cell, which of the following statements is true regarding the electrodes?
In an electrolytic cell, which of the following statements is true regarding the electrodes?
What is the role of the electrolyte in an electrochemical cell?
What is the role of the electrolyte in an electrochemical cell?
Which of the following correctly describes the flow of electrons in a voltaic cell?
Which of the following correctly describes the flow of electrons in a voltaic cell?
Which of the following best describes electrochemistry?
Which of the following best describes electrochemistry?
In a redox reaction, which statement accurately describes the relationship between oxidation and reduction?
In a redox reaction, which statement accurately describes the relationship between oxidation and reduction?
Which of the following options correctly defines an oxidizing agent in a redox reaction?
Which of the following options correctly defines an oxidizing agent in a redox reaction?
What is the oxidation number of an element in its elemental form?
What is the oxidation number of an element in its elemental form?
In which of the following compounds does hydrogen have an oxidation number of -1?
In which of the following compounds does hydrogen have an oxidation number of -1?
What is the oxidation number of oxygen in hydrogen peroxide ($H_2O_2$)?
What is the oxidation number of oxygen in hydrogen peroxide ($H_2O_2$)?
Determine the oxidation number of sulfur (S) in the sulfate ion ($SO_4^{2-}$).
Determine the oxidation number of sulfur (S) in the sulfate ion ($SO_4^{2-}$).
In the following reaction, which species is being oxidized? $Zn(s) + Cu^{2+}(aq) \rightarrow Zn^{2+}(aq) + Cu(s)$
In the following reaction, which species is being oxidized? $Zn(s) + Cu^{2+}(aq) \rightarrow Zn^{2+}(aq) + Cu(s)$
Consider the reaction: $2Fe^{3+}(aq) + 2I^-(aq) \rightarrow 2Fe^{2+}(aq) + I_2(s)$. Which species acts as the reducing agent?
Consider the reaction: $2Fe^{3+}(aq) + 2I^-(aq) \rightarrow 2Fe^{2+}(aq) + I_2(s)$. Which species acts as the reducing agent?
Which of the following statements accurately describes how to identify oxidation in terms of oxidation number change?
Which of the following statements accurately describes how to identify oxidation in terms of oxidation number change?
What is the oxidation number of carbon in $CO_3^{2-}$?
What is the oxidation number of carbon in $CO_3^{2-}$?
For a given electrochemical reaction, what indicates that the reaction will proceed spontaneously?
For a given electrochemical reaction, what indicates that the reaction will proceed spontaneously?
In an electrochemical cell, if a more reactive metal is placed at the cathode and a less reactive metal at the anode, what can be predicted about the cell potential (E) and the reaction's spontaneity?
In an electrochemical cell, if a more reactive metal is placed at the cathode and a less reactive metal at the anode, what can be predicted about the cell potential (E) and the reaction's spontaneity?
Which of the following correctly represents the oxidation half-reaction for the given overall reaction: $2Al + 3Mg^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Mg$?
Which of the following correctly represents the oxidation half-reaction for the given overall reaction: $2Al + 3Mg^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Mg$?
Given the half-cell reactions: $Zn \rightarrow Zn^{2+}(aq) + 2e^-$ $E° = +0.76V$ and $Cu^{2+}(aq) + 2e^- \rightarrow Cu$ $E° = +0.34V$, what is the standard cell potential ($E°_{cell}$) for the reaction $Zn + Cu^{2+}(aq) \rightarrow Zn^{2+}(aq) + Cu$?
Given the half-cell reactions: $Zn \rightarrow Zn^{2+}(aq) + 2e^-$ $E° = +0.76V$ and $Cu^{2+}(aq) + 2e^- \rightarrow Cu$ $E° = +0.34V$, what is the standard cell potential ($E°_{cell}$) for the reaction $Zn + Cu^{2+}(aq) \rightarrow Zn^{2+}(aq) + Cu$?
In the reaction $2Al + 3Mg^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Mg$, knowing that $E°{Al} = +1.66V$ and $E°{Mg} = -2.36V$, and that Magnesium is more reactive than Aluminum, what is the $E°_{cell}$ and is the reaction spontaneous?
In the reaction $2Al + 3Mg^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Mg$, knowing that $E°{Al} = +1.66V$ and $E°{Mg} = -2.36V$, and that Magnesium is more reactive than Aluminum, what is the $E°_{cell}$ and is the reaction spontaneous?
Which of the following statements correctly describes how to determine cell spontaneity based on the relative reactivity of metals in an electrochemical cell?
Which of the following statements correctly describes how to determine cell spontaneity based on the relative reactivity of metals in an electrochemical cell?
Given the overall cell reaction: $Zn + Cu^{2+}(aq) \rightarrow Zn^{2+}(aq) + Cu$, which of the following cell representations is correct?
Given the overall cell reaction: $Zn + Cu^{2+}(aq) \rightarrow Zn^{2+}(aq) + Cu$, which of the following cell representations is correct?
For the reaction: $Zn + Cu^{2+}(aq) \rightarrow Zn^{2+}(aq) + Cu$, what are the oxidation states of Zinc ($Zn$) and Copper ($Cu$) on the reactant and product sides respectively?
For the reaction: $Zn + Cu^{2+}(aq) \rightarrow Zn^{2+}(aq) + Cu$, what are the oxidation states of Zinc ($Zn$) and Copper ($Cu$) on the reactant and product sides respectively?
Which of the following is the correct application of a redox reaction?
Which of the following is the correct application of a redox reaction?
Which of the following statements accurately describes the role of a reducing agent in a redox reaction?
Which of the following statements accurately describes the role of a reducing agent in a redox reaction?
In the reaction $2Na + Cl_2 \rightarrow 2NaCl$, which element is being reduced?
In the reaction $2Na + Cl_2 \rightarrow 2NaCl$, which element is being reduced?
Which of the following statements accurately describes oxidation in redox reactions?
Which of the following statements accurately describes oxidation in redox reactions?
In the electrochemical cell, which process occurs at the anode?
In the electrochemical cell, which process occurs at the anode?
Which of the following is true for voltaic cells?
Which of the following is true for voltaic cells?
In the reaction $Fe + CuSO_4 \rightarrow FeSO_4 + Cu$, which species is the reducing agent?
In the reaction $Fe + CuSO_4 \rightarrow FeSO_4 + Cu$, which species is the reducing agent?
Which of the following best describes a strong oxidizing agent?
Which of the following best describes a strong oxidizing agent?
Which of the following conditions are standard conditions for measuring standard cell potential?
Which of the following conditions are standard conditions for measuring standard cell potential?
In an electrolytic cell, what is the charge of the electrode where reduction occurs, and what is this electrode called?
In an electrolytic cell, what is the charge of the electrode where reduction occurs, and what is this electrode called?
What is the purpose of the cell potential ($E_{cell}$) value?
What is the purpose of the cell potential ($E_{cell}$) value?
In the reaction $Cl_2 + 2NaBr \rightarrow 2NaCl + Br_2$, identify the oxidizing agent.
In the reaction $Cl_2 + 2NaBr \rightarrow 2NaCl + Br_2$, identify the oxidizing agent.
In a redox reaction, if a species loses electrons, which of the following processes correctly describes this change?
In a redox reaction, if a species loses electrons, which of the following processes correctly describes this change?
Which of the following statements accurately describes the roles of oxidizing and reducing agents in a redox reaction?
Which of the following statements accurately describes the roles of oxidizing and reducing agents in a redox reaction?
What is the oxidation number of oxygen in peroxides such as $H_2O_2$?
What is the oxidation number of oxygen in peroxides such as $H_2O_2$?
Determine the oxidation number of sulfur in the $H_2SO_4$ molecule.
Determine the oxidation number of sulfur in the $H_2SO_4$ molecule.
What is the oxidation number of carbon in the carbonate ion, $CO_3^{2-}$?
What is the oxidation number of carbon in the carbonate ion, $CO_3^{2-}$?
Consider the reaction: $2Mg(s) + O_2(g) \rightarrow 2MgO(s)$. Which species is the reducing agent?
Consider the reaction: $2Mg(s) + O_2(g) \rightarrow 2MgO(s)$. Which species is the reducing agent?
In the following reaction, identify which species is oxidized: $Zn(s) + Cu^{2+}(aq) \rightarrow Zn^{2+}(aq) + Cu(s)$
In the following reaction, identify which species is oxidized: $Zn(s) + Cu^{2+}(aq) \rightarrow Zn^{2+}(aq) + Cu(s)$
Which of the following is NOT a typical application of redox reactions?
Which of the following is NOT a typical application of redox reactions?
What is the oxidation number of chlorine in perchlorate ($ClO_4^−$) anion?
What is the oxidation number of chlorine in perchlorate ($ClO_4^−$) anion?
Which of the conditions below will result in a spontaneous electrochemical reaction?
Which of the conditions below will result in a spontaneous electrochemical reaction?
Consider the reaction: $Ni^{2+}(aq) + Zn(s) \rightarrow Ni(s) + Zn^{2+}(aq)$. Given that nickel is less reactive than zinc, what can be predicted about the spontaneity of the reaction and the standard cell potential?
Consider the reaction: $Ni^{2+}(aq) + Zn(s) \rightarrow Ni(s) + Zn^{2+}(aq)$. Given that nickel is less reactive than zinc, what can be predicted about the spontaneity of the reaction and the standard cell potential?
Which of the following statements is correct regarding the relationship between the standard cell potential (E°) and the spontaneity of an electrochemical reaction?
Which of the following statements is correct regarding the relationship between the standard cell potential (E°) and the spontaneity of an electrochemical reaction?
In an electrochemical cell, if a more reactive metal is acting as the cathode, what does this indicate about the standard cell potential and the spontaneity of the reaction?
In an electrochemical cell, if a more reactive metal is acting as the cathode, what does this indicate about the standard cell potential and the spontaneity of the reaction?
Given the cell representation: $Ag/Ag^+ // Fe^{2+}/Fe$, and knowing that silver is less reactive than iron, what can be inferred about the cell's standard potential (E°) and spontaneity?
Given the cell representation: $Ag/Ag^+ // Fe^{2+}/Fe$, and knowing that silver is less reactive than iron, what can be inferred about the cell's standard potential (E°) and spontaneity?
For the reaction $2Al(s) + 3Cu^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Cu(s)$, if the standard reduction potential of $Al^{3+}$ to $Al$ is -1.66 V and $Cu^{2+}$ to $Cu$ is +0.34 V, calculate the standard cell potential (E°cell) and determine the spontaneity.
For the reaction $2Al(s) + 3Cu^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Cu(s)$, if the standard reduction potential of $Al^{3+}$ to $Al$ is -1.66 V and $Cu^{2+}$ to $Cu$ is +0.34 V, calculate the standard cell potential (E°cell) and determine the spontaneity.
Given the following half-reactions and their standard reduction potentials:
$Zn^{2+}(aq) + 2e^- \rightarrow Zn(s)$ E° = -0.76 V
$Fe^{2+}(aq) + 2e^- \rightarrow Fe(s)$ E° = -0.44 V
You construct a galvanic cell using these half-reactions. What is the standard cell potential (E°cell)?
Given the following half-reactions and their standard reduction potentials: $Zn^{2+}(aq) + 2e^- \rightarrow Zn(s)$ E° = -0.76 V $Fe^{2+}(aq) + 2e^- \rightarrow Fe(s)$ E° = -0.44 V You construct a galvanic cell using these half-reactions. What is the standard cell potential (E°cell)?
Consider the electrochemical reaction: $2Ag^+ (aq) + Cu(s) \rightarrow 2Ag(s) + Cu^{2+}(aq)$. Which of the following cell representations accurately depicts this reaction?
Consider the electrochemical reaction: $2Ag^+ (aq) + Cu(s) \rightarrow 2Ag(s) + Cu^{2+}(aq)$. Which of the following cell representations accurately depicts this reaction?
Which of the following is NOT a typical component covered in the topic of electrochemistry, based on the content provided?
Which of the following is NOT a typical component covered in the topic of electrochemistry, based on the content provided?
Given the overall cell reaction: $Zn(s) + 2H^+(aq) \rightarrow Zn^{2+}(aq) + H_2(g)$, determine the half-cell reactions occurring at the anode and cathode, respectively.
Given the overall cell reaction: $Zn(s) + 2H^+(aq) \rightarrow Zn^{2+}(aq) + H_2(g)$, determine the half-cell reactions occurring at the anode and cathode, respectively.
In a redox reaction, if an atom's oxidation number increases after the reaction, which of the following processes has occurred?
In a redox reaction, if an atom's oxidation number increases after the reaction, which of the following processes has occurred?
Which statement accurately describes the relationship between an oxidizing agent and a reducing agent in a redox reaction?
Which statement accurately describes the relationship between an oxidizing agent and a reducing agent in a redox reaction?
What is the oxidation number of an element in its elemental form, such as $O_2$ or $Cu(s)$?
What is the oxidation number of an element in its elemental form, such as $O_2$ or $Cu(s)$?
Considering the rules for assigning oxidation numbers, what is the oxidation number of hydrogen when combined with a metal such as sodium (Na) in $NaH$?
Considering the rules for assigning oxidation numbers, what is the oxidation number of hydrogen when combined with a metal such as sodium (Na) in $NaH$?
What is the oxidation number of fluorine in any compound it forms?
What is the oxidation number of fluorine in any compound it forms?
What is the oxidation number of oxygen in $OF_2$?
What is the oxidation number of oxygen in $OF_2$?
Determine the oxidation number of chromium (Cr) in the dichromate ion, $Cr_2O_7^{2-}$
Determine the oxidation number of chromium (Cr) in the dichromate ion, $Cr_2O_7^{2-}$
In the reaction $2K(s) + Cl_2(g)
ightarrow 2KCl(s)$, which species is the reducing agent?
In the reaction $2K(s) + Cl_2(g) ightarrow 2KCl(s)$, which species is the reducing agent?
Given the unbalanced equation: $MnO_4^-(aq) + Fe^{2+}(aq)
ightarrow Mn^{2+}(aq) + Fe^{3+}(aq)$, which species undergoes oxidation?
Given the unbalanced equation: $MnO_4^-(aq) + Fe^{2+}(aq) ightarrow Mn^{2+}(aq) + Fe^{3+}(aq)$, which species undergoes oxidation?
Which of the following is the correct half-reaction for the oxidation of $Al$ to $Al^{3+}$?
Which of the following is the correct half-reaction for the oxidation of $Al$ to $Al^{3+}$?
In the balanced redox reaction $2H_2S + 3O_2
ightarrow 2H_2O + 2SO_2$, what is the change in oxidation number for sulfur?
In the balanced redox reaction $2H_2S + 3O_2 ightarrow 2H_2O + 2SO_2$, what is the change in oxidation number for sulfur?
Which of the following correctly describes what happens at the cathode in an electrolytic cell?
Which of the following correctly describes what happens at the cathode in an electrolytic cell?
Given the reaction: $Fe + CuSO_4
ightarrow FeSO_4 + Cu$, what is being reduced and what is the oxidizing agent?
Given the reaction: $Fe + CuSO_4 ightarrow FeSO_4 + Cu$, what is being reduced and what is the oxidizing agent?
A substance has a high positive oxidation potential. What does this suggest about its tendency in redox reactions?
A substance has a high positive oxidation potential. What does this suggest about its tendency in redox reactions?
What is the primary difference between a voltaic cell and an electrolytic cell regarding spontaneity?
What is the primary difference between a voltaic cell and an electrolytic cell regarding spontaneity?
In the reaction $Cl_2 + 2NaBr
ightarrow 2NaCl + Br_2$, which species is being oxidized?
In the reaction $Cl_2 + 2NaBr ightarrow 2NaCl + Br_2$, which species is being oxidized?
If a cell has a negative standard cell potential ($E_{cell}$), what does this indicate about the spontaneity of the reaction under standard conditions?
If a cell has a negative standard cell potential ($E_{cell}$), what does this indicate about the spontaneity of the reaction under standard conditions?
For the half-reaction $Zn^{2+}(aq) + 2e^-
ightarrow Zn(s)$, $E = -0.76V$. What does the negative sign indicate?
For the half-reaction $Zn^{2+}(aq) + 2e^- ightarrow Zn(s)$, $E = -0.76V$. What does the negative sign indicate?
Which statement accurately describes the relationship between electrode potential and the strength of an oxidizing agent?
Which statement accurately describes the relationship between electrode potential and the strength of an oxidizing agent?
In an electrochemical cell, if you reverse the direction of the reaction, how does this affect the sign of the cell potential ($E_{cell}$)?
In an electrochemical cell, if you reverse the direction of the reaction, how does this affect the sign of the cell potential ($E_{cell}$)?
For an electrochemical cell, what indicates that the reaction will proceed spontaneously?
For an electrochemical cell, what indicates that the reaction will proceed spontaneously?
In an electrochemical cell, if the less reactive metal is placed at the anode, what can be predicted about the cell potential ($E$) and the reaction's spontaneity?
In an electrochemical cell, if the less reactive metal is placed at the anode, what can be predicted about the cell potential ($E$) and the reaction's spontaneity?
Given the half-cell reactions: $Al
ightarrow Al^{3+}(aq) + 3e^-$ $E = +1.66V$ and $Mg^{2+}(aq) + 2e^-
ightarrow Mg$ $E = -2.36V$, and the overall reaction: $2Al + 3Mg^{2+}(aq)
ightarrow 2Al^{3+}(aq) + 3Mg$. What is the standard cell potential ($E_{cell}$)?
Given the half-cell reactions: $Al ightarrow Al^{3+}(aq) + 3e^-$ $E = +1.66V$ and $Mg^{2+}(aq) + 2e^- ightarrow Mg$ $E = -2.36V$, and the overall reaction: $2Al + 3Mg^{2+}(aq) ightarrow 2Al^{3+}(aq) + 3Mg$. What is the standard cell potential ($E_{cell}$)?
Given the reaction $2Al + 3Mg^{2+}(aq)
ightarrow 2Al^{3+}(aq) + 3Mg$, knowing that $E_{Al} = +1.66V$ and $E_{Mg} = -2.36V$, and that Magnesium is more reactive than Aluminum, what is the $E_{cell}$ and is the reaction spontaneous?
Given the reaction $2Al + 3Mg^{2+}(aq) ightarrow 2Al^{3+}(aq) + 3Mg$, knowing that $E_{Al} = +1.66V$ and $E_{Mg} = -2.36V$, and that Magnesium is more reactive than Aluminum, what is the $E_{cell}$ and is the reaction spontaneous?
What is the standard cell potential ($E_{cell}$) for the reaction $Zn + Cu^{2+}(aq)
ightarrow Zn^{2+}(aq) + Cu$, given the half-cell reactions: $Zn
ightarrow Zn^{2+}(aq) + 2e^-$ $E = +0.76V$ and $Cu^{2+}(aq) + 2e^-
ightarrow Cu$ $E = +0.34V$?
What is the standard cell potential ($E_{cell}$) for the reaction $Zn + Cu^{2+}(aq) ightarrow Zn^{2+}(aq) + Cu$, given the half-cell reactions: $Zn ightarrow Zn^{2+}(aq) + 2e^-$ $E = +0.76V$ and $Cu^{2+}(aq) + 2e^- ightarrow Cu$ $E = +0.34V$?
In a redox reaction, if one species is oxidized, what must also occur?
In a redox reaction, if one species is oxidized, what must also occur?
Which statement accurately describes the role of an oxidizing agent in a redox reaction?
Which statement accurately describes the role of an oxidizing agent in a redox reaction?
When assigning oxidation numbers, what is the oxidation number of an element in its standard, elemental state?
When assigning oxidation numbers, what is the oxidation number of an element in its standard, elemental state?
According to the rules for assigning oxidation numbers, what is the oxidation number of fluorine in chemical compounds?
According to the rules for assigning oxidation numbers, what is the oxidation number of fluorine in chemical compounds?
Determine the oxidation number of sulfur in the bisulfate ion, $HSO_4^-$.
Determine the oxidation number of sulfur in the bisulfate ion, $HSO_4^-$.
Identify the species that is oxidized in the following reaction: $Zn(s) + 2H^+(aq)
ightarrow Zn^{2+}(aq) + H_2(g)$.
Identify the species that is oxidized in the following reaction: $Zn(s) + 2H^+(aq) ightarrow Zn^{2+}(aq) + H_2(g)$.
Consider the incomplete redox reaction: $MnO_4^- (aq) + e^-
ightarrow Mn^{2+}(aq)$. What is the oxidation number change for manganese (Mn)?
Consider the incomplete redox reaction: $MnO_4^- (aq) + e^- ightarrow Mn^{2+}(aq)$. What is the oxidation number change for manganese (Mn)?
Which process characterizes reduction in terms of oxidation number?
Which process characterizes reduction in terms of oxidation number?
In the reaction $2Na(s) + Cl_2(g)
ightarrow 2NaCl(s)$, which element undergoes reduction?
In the reaction $2Na(s) + Cl_2(g) ightarrow 2NaCl(s)$, which element undergoes reduction?
In the reaction $Pb(NO_3)_2 + 2KI \rightarrow PbI_2 + 2KNO_3$, which species undergoes neither oxidation nor reduction?
In the reaction $Pb(NO_3)_2 + 2KI \rightarrow PbI_2 + 2KNO_3$, which species undergoes neither oxidation nor reduction?
Which of the following statements accurately describes the relationship between the electrode potential and the strength of a reducing agent?
Which of the following statements accurately describes the relationship between the electrode potential and the strength of a reducing agent?
What conditions are defined for measuring standard electrode potentials?
What conditions are defined for measuring standard electrode potentials?
Which of the following describes what occurs at the anode in both voltaic and electrolytic cells?
Which of the following describes what occurs at the anode in both voltaic and electrolytic cells?
In an electrochemical cell, if you increase the concentration of the reactants, how does this affect the cell potential ($E_{cell}$)?
In an electrochemical cell, if you increase the concentration of the reactants, how does this affect the cell potential ($E_{cell}$)?
If a voltaic cell is constructed with a zinc electrode in $Zn^{2+}$ solution and a copper electrode in $Cu^{2+}$ solution, and the solutions are connected by a salt bridge, what is the purpose of the salt bridge?
If a voltaic cell is constructed with a zinc electrode in $Zn^{2+}$ solution and a copper electrode in $Cu^{2+}$ solution, and the solutions are connected by a salt bridge, what is the purpose of the salt bridge?
In the overall redox reaction: $2Al(s) + 3Cu^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Cu(s)$, which species is the oxidizing agent?
In the overall redox reaction: $2Al(s) + 3Cu^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Cu(s)$, which species is the oxidizing agent?
What is the role of a strong oxidizing agent in an electrochemical reaction?
What is the role of a strong oxidizing agent in an electrochemical reaction?
Consider the reaction: $2H_2S(g) + 3O_2(g) \rightarrow 2H_2O(l) + 2SO_2(g)$. What is the change in the oxidation state of sulfur?
Consider the reaction: $2H_2S(g) + 3O_2(g) \rightarrow 2H_2O(l) + 2SO_2(g)$. What is the change in the oxidation state of sulfur?
What is the difference between electrolytic and voltaic cells?
What is the difference between electrolytic and voltaic cells?
For the reaction $Ni^{2+}(aq) + 2e^-
ightarrow Ni(s)$, the standard reduction potential ($E^\circ$) is -0.25 V. If this half-cell is connected to a standard hydrogen electrode (SHE) to form a voltaic cell, what is the standard cell potential ($E^\circ_{cell}$)?
For the reaction $Ni^{2+}(aq) + 2e^- ightarrow Ni(s)$, the standard reduction potential ($E^\circ$) is -0.25 V. If this half-cell is connected to a standard hydrogen electrode (SHE) to form a voltaic cell, what is the standard cell potential ($E^\circ_{cell}$)?
Consider an electrochemical cell constructed with a Zinc electrode in a $Zn^{2+}$ solution and a Copper electrode in a $Cu^{2+}$ solution. Given that Zinc is more reactive than Copper, what can be predicted about the spontaneity of the reaction and the cell voltage under standard conditions?
Consider an electrochemical cell constructed with a Zinc electrode in a $Zn^{2+}$ solution and a Copper electrode in a $Cu^{2+}$ solution. Given that Zinc is more reactive than Copper, what can be predicted about the spontaneity of the reaction and the cell voltage under standard conditions?
In an electrochemical cell, the standard reduction potential for $Ag^+ + e^-
ightarrow Ag$ is +0.80 V, and for $Zn^{2+} + 2e^-
ightarrow Zn$ is -0.76 V. If a cell is constructed using these two half-cells, what is the standard cell potential?
In an electrochemical cell, the standard reduction potential for $Ag^+ + e^- ightarrow Ag$ is +0.80 V, and for $Zn^{2+} + 2e^- ightarrow Zn$ is -0.76 V. If a cell is constructed using these two half-cells, what is the standard cell potential?
Given the cell notation: $Mg(s) | Mg^{2+}(aq) || Al^{3+}(aq) | Al(s)$. If the standard reduction potential of $Mg^{2+}$ to $Mg$ is -2.37 V, and that of $Al^{3+}$ to $Al$ is -1.66 V, what is the standard cell potential ($E^\circ_{cell}$) for this electrochemical cell?
Given the cell notation: $Mg(s) | Mg^{2+}(aq) || Al^{3+}(aq) | Al(s)$. If the standard reduction potential of $Mg^{2+}$ to $Mg$ is -2.37 V, and that of $Al^{3+}$ to $Al$ is -1.66 V, what is the standard cell potential ($E^\circ_{cell}$) for this electrochemical cell?
For the electrochemical cell represented by $Zn | Zn^{2+} || Cu^{2+} | Cu$, which of the following statements is correct regarding the flow of electrons and ion movement?
For the electrochemical cell represented by $Zn | Zn^{2+} || Cu^{2+} | Cu$, which of the following statements is correct regarding the flow of electrons and ion movement?
Consider a voltaic cell with the following half-reactions:
$Fe^{2+}(aq) + 2e^-
ightarrow Fe(s)$ $E^\circ = -0.44V$
$Sn^{2+}(aq) + 2e^-
ightarrow Sn(s)$ $E^\circ = -0.14V$
Which reaction occurs at the anode under standard conditions?
Consider a voltaic cell with the following half-reactions: $Fe^{2+}(aq) + 2e^- ightarrow Fe(s)$ $E^\circ = -0.44V$ $Sn^{2+}(aq) + 2e^- ightarrow Sn(s)$ $E^\circ = -0.14V$ Which reaction occurs at the anode under standard conditions?
Given the overall reaction: $2Ag^+ (aq) + Ni(s)
ightarrow 2Ag(s) + Ni^{2+}(aq)$. If the standard reduction potential for $Ag^+/Ag$ is +0.80 V and for $Ni^{2+}/Ni$ is -0.25 V, calculate the standard cell potential ($E^\circ_{cell}$) for this reaction.
Given the overall reaction: $2Ag^+ (aq) + Ni(s) ightarrow 2Ag(s) + Ni^{2+}(aq)$. If the standard reduction potential for $Ag^+/Ag$ is +0.80 V and for $Ni^{2+}/Ni$ is -0.25 V, calculate the standard cell potential ($E^\circ_{cell}$) for this reaction.
Consider the following half-reactions and their standard reduction potentials:
$Cu^{2+}(aq) + 2e^-
ightarrow Cu(s)$ $E^\circ = +0.34 V$
$Cr^{3+}(aq) + 3e^-
ightarrow Cr(s)$ $E^\circ = -0.74 V$
A voltaic cell is constructed using these half-reactions. What is the standard cell potential ($E^\circ_{cell}$)?
Consider the following half-reactions and their standard reduction potentials: $Cu^{2+}(aq) + 2e^- ightarrow Cu(s)$ $E^\circ = +0.34 V$ $Cr^{3+}(aq) + 3e^- ightarrow Cr(s)$ $E^\circ = -0.74 V$ A voltaic cell is constructed using these half-reactions. What is the standard cell potential ($E^\circ_{cell}$)?
Given the electrochemical reaction: $3Cu^{2+}(aq) + 2Al(s)
ightarrow 3Cu(s) + 2Al^{3+}(aq)$. Which of the following cell notations correctly represents this reaction?
Given the electrochemical reaction: $3Cu^{2+}(aq) + 2Al(s) ightarrow 3Cu(s) + 2Al^{3+}(aq)$. Which of the following cell notations correctly represents this reaction?
An electrochemical cell is set up such that the half-reaction at the anode is $Zn(s)
ightarrow Zn^{2+}(aq) + 2e^-$ and the half-reaction at the cathode is $Cu^{2+}(aq) + 2e^-
ightarrow Cu(s)$. What will happen to the voltage of the cell if the concentration of $Cu^{2+}$ is decreased?
An electrochemical cell is set up such that the half-reaction at the anode is $Zn(s) ightarrow Zn^{2+}(aq) + 2e^-$ and the half-reaction at the cathode is $Cu^{2+}(aq) + 2e^- ightarrow Cu(s)$. What will happen to the voltage of the cell if the concentration of $Cu^{2+}$ is decreased?
In a redox reaction, if species A is the oxidizing agent, what effect does it have on species B?
In a redox reaction, if species A is the oxidizing agent, what effect does it have on species B?
When assigning oxidation numbers, which of the following statements is generally true for oxygen?
When assigning oxidation numbers, which of the following statements is generally true for oxygen?
What is the oxidation number of hydrogen (H) in sodium hydride ($NaH$)?
What is the oxidation number of hydrogen (H) in sodium hydride ($NaH$)?
In potassium perchlorate ($KClO_4$), what is the oxidation number of chlorine (Cl)?
In potassium perchlorate ($KClO_4$), what is the oxidation number of chlorine (Cl)?
In the following reaction, $2Al(s) + 3Cu^{2+}(aq)
ightarrow 2Al^{3+}(aq) + 3Cu(s)$, which species is the reducing agent?
In the following reaction, $2Al(s) + 3Cu^{2+}(aq) ightarrow 2Al^{3+}(aq) + 3Cu(s)$, which species is the reducing agent?
Consider the reaction: $MnO_2(s) + 4H^+(aq) + 2e^-
ightarrow Mn^{2+}(aq) + 2H_2O(l)$. What is being reduced in this reaction?
Consider the reaction: $MnO_2(s) + 4H^+(aq) + 2e^- ightarrow Mn^{2+}(aq) + 2H_2O(l)$. What is being reduced in this reaction?
In the compound $OF_2$, what is the oxidation number of oxygen?
In the compound $OF_2$, what is the oxidation number of oxygen?
What is the oxidation number of carbon in the oxalate ion, $C_2O_4^{2-}$?
What is the oxidation number of carbon in the oxalate ion, $C_2O_4^{2-}$?
A chemist is analyzing a new compound and finds that an element within it has an unusually high positive oxidation number. What might this indicate about the compound?
A chemist is analyzing a new compound and finds that an element within it has an unusually high positive oxidation number. What might this indicate about the compound?
During a redox reaction, it is observed that the oxidation number of an element changes from +2 to +5. Which of the following processes has occurred?
During a redox reaction, it is observed that the oxidation number of an element changes from +2 to +5. Which of the following processes has occurred?
In the balanced redox reaction $2Na + Cl_2 \rightarrow 2NaCl$, what happens to the oxidation number of chlorine?
In the balanced redox reaction $2Na + Cl_2 \rightarrow 2NaCl$, what happens to the oxidation number of chlorine?
In an electrochemical cell, if a metal with a high positive reduction potential is used, what is likely to occur?
In an electrochemical cell, if a metal with a high positive reduction potential is used, what is likely to occur?
Which of the following characteristics best describes a voltaic cell?
Which of the following characteristics best describes a voltaic cell?
Consider the following unbalanced reaction: $MnO_4^-(aq) + I^-(aq) \rightarrow Mn^{2+}(aq) + I_2(s)$. Which species is oxidized in this reaction?
Consider the following unbalanced reaction: $MnO_4^-(aq) + I^-(aq) \rightarrow Mn^{2+}(aq) + I_2(s)$. Which species is oxidized in this reaction?
How does an increase in temperature typically affect the standard cell potential ($E°$) of an electrochemical cell, and what adjustments are made to account for this?
How does an increase in temperature typically affect the standard cell potential ($E°$) of an electrochemical cell, and what adjustments are made to account for this?
You have a voltaic cell with a zinc anode and a copper cathode. What happens to the mass of each electrode as the cell discharges?
You have a voltaic cell with a zinc anode and a copper cathode. What happens to the mass of each electrode as the cell discharges?
In an electrolytic cell used for electroplating, what is the correct setup for plating silver ($Ag$) onto a metal spoon?
In an electrolytic cell used for electroplating, what is the correct setup for plating silver ($Ag$) onto a metal spoon?
Consider a redox reaction: $A + B^+ \rightarrow A^+ + B$. If substance A has a significantly higher oxidation potential than substance B, what can be predicted about the reaction?
Consider a redox reaction: $A + B^+ \rightarrow A^+ + B$. If substance A has a significantly higher oxidation potential than substance B, what can be predicted about the reaction?
What conditions define the standard cell potential ($E°$) measurement?
What conditions define the standard cell potential ($E°$) measurement?
Which of the following statements accurately describes the relationship between the half-cell potentials and the overall cell potential in an electrochemical cell?
Which of the following statements accurately describes the relationship between the half-cell potentials and the overall cell potential in an electrochemical cell?
For the reaction $2Al + 3Mg^{2+}(aq)
ightarrow 2Al^{3+}(aq) + 3Mg$, given that $E°{Al} = +1.66V$ and $E°{Mg} = -2.36V$, and that Magnesium is more reactive than Aluminum, what is the $E°_{cell}$?
For the reaction $2Al + 3Mg^{2+}(aq) ightarrow 2Al^{3+}(aq) + 3Mg$, given that $E°{Al} = +1.66V$ and $E°{Mg} = -2.36V$, and that Magnesium is more reactive than Aluminum, what is the $E°_{cell}$?
Consider the reaction: $Zn + Cu^{2+}(aq)
ightarrow Zn^{2+}(aq) + Cu$. If the standard reduction potentials are $E°{Zn} = -0.76V$ and $E°{Cu} = +0.34V$, what is the standard cell potential ($E°_{cell}$)?
Consider the reaction: $Zn + Cu^{2+}(aq) ightarrow Zn^{2+}(aq) + Cu$. If the standard reduction potentials are $E°{Zn} = -0.76V$ and $E°{Cu} = +0.34V$, what is the standard cell potential ($E°_{cell}$)?
Given the overall cell reaction: $Zn + Cu^{2+}(aq)
ightarrow Zn^{2+}(aq) + Cu$, which of the following correctly represents the half-cell reactions?
Given the overall cell reaction: $Zn + Cu^{2+}(aq) ightarrow Zn^{2+}(aq) + Cu$, which of the following correctly represents the half-cell reactions?
If a voltaic cell is set up with Zinc and Copper, and it is observed that the reaction is spontaneous, which metal should be placed at the anode and which at the cathode?
If a voltaic cell is set up with Zinc and Copper, and it is observed that the reaction is spontaneous, which metal should be placed at the anode and which at the cathode?
An electrochemical cell is constructed such that a more reactive metal is at the cathode, causing the cell potential to have a negative value. What does this indicate about the reaction?
An electrochemical cell is constructed such that a more reactive metal is at the cathode, causing the cell potential to have a negative value. What does this indicate about the reaction?
What is the standard cell potential ($E°_{cell}$) for the reaction $2Al(s) + 3Cu^{2+}(aq)
ightarrow 2Al^{3+}(aq) + 3Cu(s)$, given the half-cell reactions: $Al
ightarrow Al^{3+}(aq) + 3e^-$ $E° = +1.66V$ and $Cu^{2+}(aq) + 2e^-
ightarrow Cu$ $E° = +0.34V$?
What is the standard cell potential ($E°_{cell}$) for the reaction $2Al(s) + 3Cu^{2+}(aq) ightarrow 2Al^{3+}(aq) + 3Cu(s)$, given the half-cell reactions: $Al ightarrow Al^{3+}(aq) + 3e^-$ $E° = +1.66V$ and $Cu^{2+}(aq) + 2e^- ightarrow Cu$ $E° = +0.34V$?
Given the reaction: $2Al + 3Mg^{2+}(aq)
ightarrow 2Al^{3+}(aq) + 3Mg$. Aluminum ($Al$) has $E° = +1.66V$ and Magnesium ($Mg$) $E° = -2.36V$. Since Magnesium is more reactive than Aluminum, is the reaction spontaneous?
Given the reaction: $2Al + 3Mg^{2+}(aq) ightarrow 2Al^{3+}(aq) + 3Mg$. Aluminum ($Al$) has $E° = +1.66V$ and Magnesium ($Mg$) $E° = -2.36V$. Since Magnesium is more reactive than Aluminum, is the reaction spontaneous?
Which of the following scenarios would result in a spontaneous electrochemical reaction?
Which of the following scenarios would result in a spontaneous electrochemical reaction?
For the given cell reaction: $2Al(s) + 3Mg^{2+}(aq)
ightarrow 2Al^{3+}(aq) + 3Mg(s)$, what are the respective oxidation states of $Al$ and $Mg$ on the reactant side, and how do they change on the product side?
For the given cell reaction: $2Al(s) + 3Mg^{2+}(aq) ightarrow 2Al^{3+}(aq) + 3Mg(s)$, what are the respective oxidation states of $Al$ and $Mg$ on the reactant side, and how do they change on the product side?
Given the half-cell reactions: $Zn
ightarrow Zn^{2+}(aq) + 2e^-$ with $E° = +0.76V$ and $Cu^{2+}(aq) + 2e^-
ightarrow Cu$ with $E° = +0.34V$, which of the following statements correctly describes the spontaneity of the reaction $Zn + Cu^{2+}(aq)
ightarrow Zn^{2+}(aq) + Cu$?
Given the half-cell reactions: $Zn ightarrow Zn^{2+}(aq) + 2e^-$ with $E° = +0.76V$ and $Cu^{2+}(aq) + 2e^- ightarrow Cu$ with $E° = +0.34V$, which of the following statements correctly describes the spontaneity of the reaction $Zn + Cu^{2+}(aq) ightarrow Zn^{2+}(aq) + Cu$?
In a redox reaction, if a species is reduced, which of the following must also occur?
In a redox reaction, if a species is reduced, which of the following must also occur?
Which of the following options correctly describes the role of an oxidizing agent in a chemical reaction?
Which of the following options correctly describes the role of an oxidizing agent in a chemical reaction?
What is the oxidation number of an element in its elemental or standard state, such as $N_2(g)$ or $Au(s)$?
What is the oxidation number of an element in its elemental or standard state, such as $N_2(g)$ or $Au(s)$?
In the reaction $Zn(s) + 2H^+(aq)
ightarrow Zn^{2+}(aq) + H_2(g)$, which species is oxidized?
In the reaction $Zn(s) + 2H^+(aq) ightarrow Zn^{2+}(aq) + H_2(g)$, which species is oxidized?
For the incomplete redox reaction: $MnO_4^- (aq) + 8H^+ + 5e^-
ightarrow Mn^{2+}(aq) + 4H_2O(l)$, what is the oxidation number change for manganese (Mn)?
For the incomplete redox reaction: $MnO_4^- (aq) + 8H^+ + 5e^- ightarrow Mn^{2+}(aq) + 4H_2O(l)$, what is the oxidation number change for manganese (Mn)?
Which process accurately defines reduction in terms of oxidation number?
Which process accurately defines reduction in terms of oxidation number?
In the reaction $2Na(s) + Cl_2(g)
ightarrow 2NaCl(s)$, which element is being reduced?
In the reaction $2Na(s) + Cl_2(g) ightarrow 2NaCl(s)$, which element is being reduced?
In the reaction $4Fe + 3O_2 \rightarrow 2Fe_2O_3$, what are the changes in oxidation numbers for iron (Fe) and oxygen (O) respectively?
In the reaction $4Fe + 3O_2 \rightarrow 2Fe_2O_3$, what are the changes in oxidation numbers for iron (Fe) and oxygen (O) respectively?
Which of the following statements regarding electrodes in electrochemical cells is correct?
Which of the following statements regarding electrodes in electrochemical cells is correct?
A metal X has a high positive oxidation potential. How will this metal likely behave in a redox reaction?
A metal X has a high positive oxidation potential. How will this metal likely behave in a redox reaction?
What conditions are typically defined for measuring standard cell potential ($E^\circ$)?
What conditions are typically defined for measuring standard cell potential ($E^\circ$)?
Which of the following is a correct representation of an electrochemical cell?
Which of the following is a correct representation of an electrochemical cell?
If a cell reaction has a positive $E_{cell}$, what does this indicate about the reaction's spontaneity?
If a cell reaction has a positive $E_{cell}$, what does this indicate about the reaction's spontaneity?
Consider two half-cells: $A^{2+}(aq) + 2e^- \rightarrow A(s)$ with $E^\circ = +0.80V$ and $B^{2+}(aq) + 2e^- \rightarrow B(s)$ with $E^\circ = -0.34V$. In a voltaic cell using these half-cells, which metal will act as the anode?
Consider two half-cells: $A^{2+}(aq) + 2e^- \rightarrow A(s)$ with $E^\circ = +0.80V$ and $B^{2+}(aq) + 2e^- \rightarrow B(s)$ with $E^\circ = -0.34V$. In a voltaic cell using these half-cells, which metal will act as the anode?
In the reaction: $Cl_2 + 2NaBr \rightarrow 2NaCl + Br_2$, which species is getting oxidized based on the oxidation number change?
In the reaction: $Cl_2 + 2NaBr \rightarrow 2NaCl + Br_2$, which species is getting oxidized based on the oxidation number change?
What is the function of an electrolyte in an electrochemical cell?
What is the function of an electrolyte in an electrochemical cell?
Consider an electrochemical cell where a more reactive metal is at the cathode and a less reactive metal is at the anode. How will this setup primarily affect the cell's spontaneity and standard cell potential?
Consider an electrochemical cell where a more reactive metal is at the cathode and a less reactive metal is at the anode. How will this setup primarily affect the cell's spontaneity and standard cell potential?
In an electrochemical cell, which of the following conditions will result in a spontaneous reaction?
In an electrochemical cell, which of the following conditions will result in a spontaneous reaction?
For the cell reaction $Zn + Cu^{2+}(aq)
ightarrow Zn^{2+}(aq) + Cu$, given that zinc is more reactive than copper, what can be inferred about the standard cell potential and the reaction's spontaneity?
For the cell reaction $Zn + Cu^{2+}(aq) ightarrow Zn^{2+}(aq) + Cu$, given that zinc is more reactive than copper, what can be inferred about the standard cell potential and the reaction's spontaneity?
Which of the following cell representations accurately describes a voltaic cell with a spontaneous reaction, where $Zn$ is oxidized and $Ag^+$ is reduced?
Which of the following cell representations accurately describes a voltaic cell with a spontaneous reaction, where $Zn$ is oxidized and $Ag^+$ is reduced?
What does a negative value for the standard cell potential ($E°_{cell}$) indicate about a redox reaction under standard conditions?
What does a negative value for the standard cell potential ($E°_{cell}$) indicate about a redox reaction under standard conditions?
For the reaction $2Al(s) + 3Mg^{2+}(aq)
ightarrow 2Al^{3+}(aq) + 3Mg(s)$, given $E°{Al} = +1.66V$ and $E°{Mg} = -2.36V$, how would you determine the $E°_{cell}$ and the spontaneity of the reaction?
For the reaction $2Al(s) + 3Mg^{2+}(aq) ightarrow 2Al^{3+}(aq) + 3Mg(s)$, given $E°{Al} = +1.66V$ and $E°{Mg} = -2.36V$, how would you determine the $E°_{cell}$ and the spontaneity of the reaction?
In the reaction: $Zn(s) + Cu^{2+}(aq)
ightarrow Zn^{2+}(aq) + Cu(s)$, how does calculating the standard cell potential ($E°_{cell}$) allow us to predict the spontaneity of the reaction?
In the reaction: $Zn(s) + Cu^{2+}(aq) ightarrow Zn^{2+}(aq) + Cu(s)$, how does calculating the standard cell potential ($E°_{cell}$) allow us to predict the spontaneity of the reaction?
The standard reduction potentials for two half-cells are: $Zn^{2+}(aq) + 2e^-
ightarrow Zn(s)$, $E° = -0.76V$ and $Cu^{2+}(aq) + 2e^-
ightarrow Cu(s)$, $E° = +0.34V$. If a voltaic cell is constructed using these half-cells, what will be the standard cell potential ($E°_{cell}$)?
The standard reduction potentials for two half-cells are: $Zn^{2+}(aq) + 2e^- ightarrow Zn(s)$, $E° = -0.76V$ and $Cu^{2+}(aq) + 2e^- ightarrow Cu(s)$, $E° = +0.34V$. If a voltaic cell is constructed using these half-cells, what will be the standard cell potential ($E°_{cell}$)?
For the reaction $2Ag^+ (aq) + Cu(s)
ightarrow 2Ag(s) + Cu^{2+}(aq)$, knowing that silver is less reactive than copper, how does this affect the cell's spontaneity and what can be inferred about the cell's standard potential ($E°$)?
For the reaction $2Ag^+ (aq) + Cu(s) ightarrow 2Ag(s) + Cu^{2+}(aq)$, knowing that silver is less reactive than copper, how does this affect the cell's spontaneity and what can be inferred about the cell's standard potential ($E°$)?
Given the half-reactions: $Al(s)
ightarrow Al^{3+}(aq) + 3e^-$ , $E° = +1.66V$ and $Mg^{2+}(aq) + 2e^-
ightarrow Mg(s)$, $E° = -2.36V$. In the overall reaction: $2Al(s) + 3Mg^{2+}(aq)
ightarrow 2Al^{3+}(aq) + 3Mg(s)$, what is the standard cell potential ($E_{cell}$)?
Given the half-reactions: $Al(s) ightarrow Al^{3+}(aq) + 3e^-$ , $E° = +1.66V$ and $Mg^{2+}(aq) + 2e^- ightarrow Mg(s)$, $E° = -2.36V$. In the overall reaction: $2Al(s) + 3Mg^{2+}(aq) ightarrow 2Al^{3+}(aq) + 3Mg(s)$, what is the standard cell potential ($E_{cell}$)?
In a redox reaction, if a species is described as the reducing agent, which of the following occurs?
In a redox reaction, if a species is described as the reducing agent, which of the following occurs?
Which of the following statements correctly describes the behavior of oxidation numbers in a redox reaction?
Which of the following statements correctly describes the behavior of oxidation numbers in a redox reaction?
In the reaction $4Fe + 3O_2 \rightarrow 2Fe_2O_3$, what happens to the oxidation number of iron (Fe) and oxygen ($O_2$) respectively?
In the reaction $4Fe + 3O_2 \rightarrow 2Fe_2O_3$, what happens to the oxidation number of iron (Fe) and oxygen ($O_2$) respectively?
What must occur for a chemical reaction to be classified as a redox reaction?
What must occur for a chemical reaction to be classified as a redox reaction?
In the compound $KNO_3$, what is the oxidation number of nitrogen (N)?
In the compound $KNO_3$, what is the oxidation number of nitrogen (N)?
Which of the following statements is correct regarding the relationship between oxidation number and the process occurring in a redox reaction?
Which of the following statements is correct regarding the relationship between oxidation number and the process occurring in a redox reaction?
According to the rules for assigning oxidation numbers, what is the oxidation number of oxygen in most compounds, and what is the exception?
According to the rules for assigning oxidation numbers, what is the oxidation number of oxygen in most compounds, and what is the exception?
In an electrochemical cell, what is the relationship between the anode and oxidation?
In an electrochemical cell, what is the relationship between the anode and oxidation?
In $NaHSO_4$, which element has an oxidation number of +6?
In $NaHSO_4$, which element has an oxidation number of +6?
Given the electrochemical cell notation: $Zn(s) | Zn^{2+}(aq) || Cu^{2+}(aq) | Cu(s)$, which of the following statements is correct about the reactions at each electrode?
Given the electrochemical cell notation: $Zn(s) | Zn^{2+}(aq) || Cu^{2+}(aq) | Cu(s)$, which of the following statements is correct about the reactions at each electrode?
What distinguishes a voltaic cell from an electrolytic cell in terms of spontaneity and energy conversion?
What distinguishes a voltaic cell from an electrolytic cell in terms of spontaneity and energy conversion?
A metal 'X' has a high positive reduction potential. What does this indicate about its properties as a reducing or oxidizing agent?
A metal 'X' has a high positive reduction potential. What does this indicate about its properties as a reducing or oxidizing agent?
When hydrogen combines with metals, what is its oxidation number?
When hydrogen combines with metals, what is its oxidation number?
In the reaction $2Na + Cl_2 \rightarrow 2NaCl$, which species is the oxidizing agent and what happens to its oxidation number?
In the reaction $2Na + Cl_2 \rightarrow 2NaCl$, which species is the oxidizing agent and what happens to its oxidation number?
Which conditions define the standard cell potential ($E^\circ$) of an electrochemical cell?
Which conditions define the standard cell potential ($E^\circ$) of an electrochemical cell?
In an electrolytic cell, which of the following statements accurately describes the charge and process at the cathode?
In an electrolytic cell, which of the following statements accurately describes the charge and process at the cathode?
What role does fluorine play in chemical compounds regarding oxidation numbers, and why?
What role does fluorine play in chemical compounds regarding oxidation numbers, and why?
How does the cell potential ($E_{cell}$) relate to the spontaneity of a redox reaction in an electrochemical cell?
How does the cell potential ($E_{cell}$) relate to the spontaneity of a redox reaction in an electrochemical cell?
Which statement is true regarding the strength of oxidizing and reducing agents based on their respective potentials?
Which statement is true regarding the strength of oxidizing and reducing agents based on their respective potentials?
For a voltaic cell based on the reaction $Sn^{2+}(aq) + Fe(s)
ightarrow Sn(s) + Fe^{2+}(aq)$, which species is at the anode and what is the sign of its electrode?
For a voltaic cell based on the reaction $Sn^{2+}(aq) + Fe(s) ightarrow Sn(s) + Fe^{2+}(aq)$, which species is at the anode and what is the sign of its electrode?
Given the reaction $Zn + 2Ag^+(aq)
ightarrow Zn^{2+}(aq) + 2Ag$, which of the following cell representations is correct?
Given the reaction $Zn + 2Ag^+(aq) ightarrow Zn^{2+}(aq) + 2Ag$, which of the following cell representations is correct?
If a more reactive metal is acting as the cathode in an electrochemical cell, what does this indicate about the cell's standard potential (E°) and the reaction's spontaneity?
If a more reactive metal is acting as the cathode in an electrochemical cell, what does this indicate about the cell's standard potential (E°) and the reaction's spontaneity?
For the cell representation $Al/Al^{3+} // Cu^{2+}/Cu$, what are the half-reactions occurring at the anode and cathode, respectively?
For the cell representation $Al/Al^{3+} // Cu^{2+}/Cu$, what are the half-reactions occurring at the anode and cathode, respectively?
Given a redox reaction with a negative standard cell potential ($E°_{cell}$), what does this indicate about the spontaneity of the reaction under standard conditions?
Given a redox reaction with a negative standard cell potential ($E°_{cell}$), what does this indicate about the spontaneity of the reaction under standard conditions?
Consider the reaction: $2Ag^+(aq) + Cu(s)
ightarrow 2Ag(s) + Cu^{2+}(aq)$. If the standard reduction potential for $Ag^+/Ag$ is +0.80 V and for $Cu^{2+}/Cu$ is +0.34 V, what is the standard cell potential ($E°$) for this reaction?
Consider the reaction: $2Ag^+(aq) + Cu(s) ightarrow 2Ag(s) + Cu^{2+}(aq)$. If the standard reduction potential for $Ag^+/Ag$ is +0.80 V and for $Cu^{2+}/Cu$ is +0.34 V, what is the standard cell potential ($E°$) for this reaction?
If a more reactive metal is placed at the cathode in an electrolytic cell, what effect does this have on the cell potential and the spontaneity of the reaction?
If a more reactive metal is placed at the cathode in an electrolytic cell, what effect does this have on the cell potential and the spontaneity of the reaction?
For the reaction $2Al(s) + 3Mg^{2+}(aq)
ightarrow 2Al^{3+}(aq) + 3Mg(s)$, given $E°{Al^{3+}/Al} = -1.66V$ and $E°{Mg^{2+}/Mg} = -2.36V$. Calculate the $E°cell$ and determine if the reaction is spontaneous as written.
For the reaction $2Al(s) + 3Mg^{2+}(aq) ightarrow 2Al^{3+}(aq) + 3Mg(s)$, given $E°{Al^{3+}/Al} = -1.66V$ and $E°{Mg^{2+}/Mg} = -2.36V$. Calculate the $E°cell$ and determine if the reaction is spontaneous as written.
Given the following cell representation: $Pt(s) | Fe^{2+}(aq), Fe^{3+}(aq) || MnO_4^-(aq), H^+(aq) | Mn^{2+}(aq) | Pt(s)$. Which half-reaction occurs at the anode?
Given the following cell representation: $Pt(s) | Fe^{2+}(aq), Fe^{3+}(aq) || MnO_4^-(aq), H^+(aq) | Mn^{2+}(aq) | Pt(s)$. Which half-reaction occurs at the anode?
Which of the following statements accurately describes the relationship between the cell potential ($E_{cell}$) and the concentrations of reactants and products in an electrochemical cell?
Which of the following statements accurately describes the relationship between the cell potential ($E_{cell}$) and the concentrations of reactants and products in an electrochemical cell?
In a redox reaction, if a species is described as the 'reducing agent', what is it directly responsible for?
In a redox reaction, if a species is described as the 'reducing agent', what is it directly responsible for?
Which statement accurately describes the fundamental relationship between oxidation and reduction processes in a redox reaction?
Which statement accurately describes the fundamental relationship between oxidation and reduction processes in a redox reaction?
In the compound $KMnO_4$, what is the oxidation number of manganese (Mn)?
In the compound $KMnO_4$, what is the oxidation number of manganese (Mn)?
Given the compound $Na_2S_2O_3$, what is the oxidation number of sulfur (S)?
Given the compound $Na_2S_2O_3$, what is the oxidation number of sulfur (S)?
If an element is in its elemental form (e.g., $N_2$, $Fe(s)$), what is its oxidation number?
If an element is in its elemental form (e.g., $N_2$, $Fe(s)$), what is its oxidation number?
In which of the following compounds does oxygen NOT have an oxidation number of -2?
In which of the following compounds does oxygen NOT have an oxidation number of -2?
Which process defines reduction in terms of oxidation number change?
Which process defines reduction in terms of oxidation number change?
In the reaction $2Al(s) + 3Cu^{2+}(aq)
ightarrow 2Al^{3+}(aq) + 3Cu(s)$, which species is the oxidizing agent?
In the reaction $2Al(s) + 3Cu^{2+}(aq) ightarrow 2Al^{3+}(aq) + 3Cu(s)$, which species is the oxidizing agent?
During a redox reaction, if a substance $X$ increases in oxidation number from +2 to +5, what has occurred?
During a redox reaction, if a substance $X$ increases in oxidation number from +2 to +5, what has occurred?
Consider the unbalanced reaction: $MnO_4^-(aq) + I^-(aq)
ightarrow MnO_2(s) + I_2(s)$. Which species undergoes reduction?
Consider the unbalanced reaction: $MnO_4^-(aq) + I^-(aq) ightarrow MnO_2(s) + I_2(s)$. Which species undergoes reduction?
In the reaction $4Fe + 3O_2 \rightarrow 2Fe_2O_3$, which element undergoes an increase in oxidation number?
In the reaction $4Fe + 3O_2 \rightarrow 2Fe_2O_3$, which element undergoes an increase in oxidation number?
In an electrochemical cell, which of the following is true regarding the anode?
In an electrochemical cell, which of the following is true regarding the anode?
Which of the following statements correctly compares voltaic and electrolytic cells?
Which of the following statements correctly compares voltaic and electrolytic cells?
Consider a half-cell with a very high positive reduction potential. What does this suggest about the substance in that half-cell?
Consider a half-cell with a very high positive reduction potential. What does this suggest about the substance in that half-cell?
In an electrolytic cell, what is the charge of the cathode and what process occurs there?
In an electrolytic cell, what is the charge of the cathode and what process occurs there?
If a proposed half-cell reaction has a negative $E_{cell}$ value, what does this indicate about the spontaneity of the reaction?
If a proposed half-cell reaction has a negative $E_{cell}$ value, what does this indicate about the spontaneity of the reaction?
How does increasing the concentration of reactants generally affect the cell potential ($E_{cell}$) of an electrochemical cell, and what principle explains this?
How does increasing the concentration of reactants generally affect the cell potential ($E_{cell}$) of an electrochemical cell, and what principle explains this?
Given the standard cell potential ($E°$) for a reaction, how can you determine if the reaction will proceed spontaneously under standard conditions?
Given the standard cell potential ($E°$) for a reaction, how can you determine if the reaction will proceed spontaneously under standard conditions?
In a voltaic cell, what is the role of the salt bridge?
In a voltaic cell, what is the role of the salt bridge?
Consider the reaction: $Pb(NO_3)_2 + 2KI \rightarrow PbI_2 + 2KNO_3$. Which species undergoes neither oxidation nor reduction?
Consider the reaction: $Pb(NO_3)_2 + 2KI \rightarrow PbI_2 + 2KNO_3$. Which species undergoes neither oxidation nor reduction?
For a cell reaction to be spontaneous, which of the following conditions must be met regarding the standard cell potential (E°) and the placement of metals based on their reactivity?
For a cell reaction to be spontaneous, which of the following conditions must be met regarding the standard cell potential (E°) and the placement of metals based on their reactivity?
In an electrochemical cell, if a less reactive metal is placed at the anode, what does this indicate about the standard cell potential (E°) and the spontaneity of the reaction?
In an electrochemical cell, if a less reactive metal is placed at the anode, what does this indicate about the standard cell potential (E°) and the spontaneity of the reaction?
Consider a voltaic cell constructed with aluminum and magnesium electrodes. Given that magnesium is more reactive than aluminum, and the reaction is: $2Al + 3Mg^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Mg$, what can be predicted about the cell's standard potential (E°) and spontaneity?
Consider a voltaic cell constructed with aluminum and magnesium electrodes. Given that magnesium is more reactive than aluminum, and the reaction is: $2Al + 3Mg^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Mg$, what can be predicted about the cell's standard potential (E°) and spontaneity?
Given the half-reactions: $Zn \rightarrow Zn^{2+}(aq) + 2e^-$ $E° = +0.76V$ and $Cu^{2+}(aq) + 2e^- \rightarrow Cu$ $E° = +0.34V$, and the overall reaction: $Zn + Cu^{2+}(aq) \rightarrow Zn^{2+}(aq) + Cu$, is the reaction spontaneous, and why?
Given the half-reactions: $Zn \rightarrow Zn^{2+}(aq) + 2e^-$ $E° = +0.76V$ and $Cu^{2+}(aq) + 2e^- \rightarrow Cu$ $E° = +0.34V$, and the overall reaction: $Zn + Cu^{2+}(aq) \rightarrow Zn^{2+}(aq) + Cu$, is the reaction spontaneous, and why?
Which of the following statements is NOT correct regarding the calculation and interpretation of standard cell potential (E°) in electrochemical cells?
Which of the following statements is NOT correct regarding the calculation and interpretation of standard cell potential (E°) in electrochemical cells?
A cell is represented as $M / M^{2+} // N^{2+} / N$, where M is more reactive than N. Which of the following statements accurately describes the spontaneity of the cell reaction?
A cell is represented as $M / M^{2+} // N^{2+} / N$, where M is more reactive than N. Which of the following statements accurately describes the spontaneity of the cell reaction?
Given the reaction: $Zn + Cu^{2+}(aq) \rightarrow Zn^{2+}(aq) + Cu$, which of the following cell representations accurately describes this reaction in an electrochemical cell?
Given the reaction: $Zn + Cu^{2+}(aq) \rightarrow Zn^{2+}(aq) + Cu$, which of the following cell representations accurately describes this reaction in an electrochemical cell?
Determine the E°cell for the following reaction and half-cells, and determine if the reaction is spontaneous. $2Al(s) + 3Mg^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Mg(s)$. $E_{Al} = +1.66V$ and $E_{Mg} = -2.36V$.
Determine the E°cell for the following reaction and half-cells, and determine if the reaction is spontaneous. $2Al(s) + 3Mg^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Mg(s)$. $E_{Al} = +1.66V$ and $E_{Mg} = -2.36V$.
For the voltaic cell $Ag/Ag^+ // Fe^{2+}/Fe$, and knowing that silver is less reactive than iron, what can be inferred about the cell's standard potential (E°) and spontaneity?
For the voltaic cell $Ag/Ag^+ // Fe^{2+}/Fe$, and knowing that silver is less reactive than iron, what can be inferred about the cell's standard potential (E°) and spontaneity?
Which of the following correctly identifies the anode and cathode reactions for the overall cell reaction: $Zn(s) + Cu^{2+}(aq) \rightarrow Zn^{2+}(aq) + Cu(s)$?
Which of the following correctly identifies the anode and cathode reactions for the overall cell reaction: $Zn(s) + Cu^{2+}(aq) \rightarrow Zn^{2+}(aq) + Cu(s)$?
In a redox reaction, if a species is described as the 'reducing agent', what happens to its oxidation number?
In a redox reaction, if a species is described as the 'reducing agent', what happens to its oxidation number?
Which of the following statements accurately describes the relationship between oxidation and reduction in a redox reaction?
Which of the following statements accurately describes the relationship between oxidation and reduction in a redox reaction?
Applying the rules for assigning oxidation numbers, what is the oxidation number of an element in its elemental or diatomic form?
Applying the rules for assigning oxidation numbers, what is the oxidation number of an element in its elemental or diatomic form?
Given the compound $NaH$, what is the oxidation number of hydrogen?
Given the compound $NaH$, what is the oxidation number of hydrogen?
What is the oxidation number of fluorine in $OF_2$?
What is the oxidation number of fluorine in $OF_2$?
Determine the oxidation number of sulfur in the sulfuric acid molecule, $H_2SO_4$.
Determine the oxidation number of sulfur in the sulfuric acid molecule, $H_2SO_4$.
Consider the reaction: $2K(s) + Cl_2(g)
ightarrow 2KCl(s)$. Which species undergoes reduction?
Consider the reaction: $2K(s) + Cl_2(g) ightarrow 2KCl(s)$. Which species undergoes reduction?
What is the oxidation number of chromium (Cr) in the dichromate ion, $Cr_2O_7^{2-}$?
What is the oxidation number of chromium (Cr) in the dichromate ion, $Cr_2O_7^{2-}$?
In the unbalanced redox reaction: $MnO_4^-(aq) + Fe^{2+}(aq)
ightarrow Mn^{2+}(aq) + Fe^{3+}(aq)$, which species is oxidized?
In the unbalanced redox reaction: $MnO_4^-(aq) + Fe^{2+}(aq) ightarrow Mn^{2+}(aq) + Fe^{3+}(aq)$, which species is oxidized?
What change in oxidation number signifies reduction?
What change in oxidation number signifies reduction?
In the reaction $4Fe + 3O_2 \rightarrow 2Fe_2O_3$, what are the oxidation number changes for iron (Fe) and oxygen ($O$) respectively?
In the reaction $4Fe + 3O_2 \rightarrow 2Fe_2O_3$, what are the oxidation number changes for iron (Fe) and oxygen ($O$) respectively?
In the reaction $Pb(NO_3)_2 + 2KI \rightarrow PbI_2 + 2KNO_3$, which species is the oxidizing agent?
In the reaction $Pb(NO_3)_2 + 2KI \rightarrow PbI_2 + 2KNO_3$, which species is the oxidizing agent?
A voltaic cell is set up with a zinc electrode and a copper electrode. Given that zinc has a greater tendency to be oxidized than copper, which electrode will be the anode, and what will be its charge?
A voltaic cell is set up with a zinc electrode and a copper electrode. Given that zinc has a greater tendency to be oxidized than copper, which electrode will be the anode, and what will be its charge?
Which of the following conditions would lead to a decrease in the cell potential ($E_{cell}$) of an electrochemical cell?
Which of the following conditions would lead to a decrease in the cell potential ($E_{cell}$) of an electrochemical cell?
In an electrolytic cell, what is the role of an external power source?
In an electrolytic cell, what is the role of an external power source?
If a substance has a high positive oxidation potential, what does this indicate about its properties?
If a substance has a high positive oxidation potential, what does this indicate about its properties?
Which of the following factors affects the voltage, electromotive force or emf, of an electrochemical cell under non-standard conditions?
Which of the following factors affects the voltage, electromotive force or emf, of an electrochemical cell under non-standard conditions?
For the voltaic cell $Zn(s) | Zn^{2+}(1 M) || Cu^{2+}(1 M) | Cu(s)$, the standard cell potential ($E_{cell}^{\circ}$) is +1.10 V. What happens to $E_{cell}$ if the concentration of $Cu^{2+}$ is increased?
For the voltaic cell $Zn(s) | Zn^{2+}(1 M) || Cu^{2+}(1 M) | Cu(s)$, the standard cell potential ($E_{cell}^{\circ}$) is +1.10 V. What happens to $E_{cell}$ if the concentration of $Cu^{2+}$ is increased?
In a redox reaction, if the standard reduction potential of a metal A is more positive than that of metal B, what can be inferred about their reactivity and spontaneity?
In a redox reaction, if the standard reduction potential of a metal A is more positive than that of metal B, what can be inferred about their reactivity and spontaneity?
If a voltaic cell is constructed with a zinc electrode in $Zn^{2+}$ solution and a silver electrode in $Ag^+$ solution, connected by a salt bridge, what is the primary function of the salt bridge?
If a voltaic cell is constructed with a zinc electrode in $Zn^{2+}$ solution and a silver electrode in $Ag^+$ solution, connected by a salt bridge, what is the primary function of the salt bridge?
In an electrochemical cell, if the standard cell potential ($E_{cell}$) is positive, what does this indicate about the spontaneity of the reaction?
In an electrochemical cell, if the standard cell potential ($E_{cell}$) is positive, what does this indicate about the spontaneity of the reaction?
Consider an electrochemical cell with zinc ($Zn$) as the anode and copper ($Cu$) as the cathode. Given that zinc is more reactive than copper, what is the expected sign of the standard cell potential ($E_{cell}$), and will the reaction be spontaneous?
Consider an electrochemical cell with zinc ($Zn$) as the anode and copper ($Cu$) as the cathode. Given that zinc is more reactive than copper, what is the expected sign of the standard cell potential ($E_{cell}$), and will the reaction be spontaneous?
Given the cell representation $Mg / Mg^{2+} // Ag^+ / Ag$, and knowing that magnesium is more reactive than silver, what can be inferred about the spontaneity of the cell reaction and the sign of $E_{cell}$?
Given the cell representation $Mg / Mg^{2+} // Ag^+ / Ag$, and knowing that magnesium is more reactive than silver, what can be inferred about the spontaneity of the cell reaction and the sign of $E_{cell}$?
For the reaction $3Mg^{2+}(aq) + 2Al(s)
ightarrow 3Mg(s) + 2Al^{3+}(aq)$, the standard reduction potentials are $E°(Mg^{2+}/Mg) = -2.36V$ and $E°(Al^{3+}/Al) = -1.66V$. Calculate the standard cell potential, $E°_{cell}$.
For the reaction $3Mg^{2+}(aq) + 2Al(s) ightarrow 3Mg(s) + 2Al^{3+}(aq)$, the standard reduction potentials are $E°(Mg^{2+}/Mg) = -2.36V$ and $E°(Al^{3+}/Al) = -1.66V$. Calculate the standard cell potential, $E°_{cell}$.
Consider an electrochemical cell in which the following reaction occurs: $Zn(s) + Cu^{2+}(aq)
ightarrow Zn^{2+}(aq) + Cu(s)$. Which of the following cell representations correctly describes this cell?
Consider an electrochemical cell in which the following reaction occurs: $Zn(s) + Cu^{2+}(aq) ightarrow Zn^{2+}(aq) + Cu(s)$. Which of the following cell representations correctly describes this cell?
If a more reactive metal is placed at the cathode in an electrochemical cell, what can you generally predict about the standard cell potential ($E°$) and the spontaneity of the reaction?
If a more reactive metal is placed at the cathode in an electrochemical cell, what can you generally predict about the standard cell potential ($E°$) and the spontaneity of the reaction?
For the half-reactions, $Zn(s)
ightarrow Zn^{2+}(aq) + 2e^−$ with $E° = +0.76 V$ and $Cu^{2+}(aq) + 2e^−
ightarrow Cu(s)$ with $E° = +0.34 V$, what is the standard cell potential ($E°_{cell}$) for the reaction $Zn(s) + Cu^{2+}(aq)
ightarrow Zn^{2+}(aq) + Cu(s)$?
For the half-reactions, $Zn(s) ightarrow Zn^{2+}(aq) + 2e^−$ with $E° = +0.76 V$ and $Cu^{2+}(aq) + 2e^− ightarrow Cu(s)$ with $E° = +0.34 V$, what is the standard cell potential ($E°_{cell}$) for the reaction $Zn(s) + Cu^{2+}(aq) ightarrow Zn^{2+}(aq) + Cu(s)$?
What is the purpose of using cell representations (e.g., $Zn / Zn^{2+} // Cu^{2+} / Cu$) in electrochemistry?
What is the purpose of using cell representations (e.g., $Zn / Zn^{2+} // Cu^{2+} / Cu$) in electrochemistry?
In the reaction $2Al(s) + 3Mg^{2+}(aq)
ightarrow 2Al^{3+}(aq) + 3Mg(s)$, given $E°{Al} = -1.66V$ and $E°{Mg} = -2.36V$, and knowing that Magnesium is more reactive than Aluminum, is the reaction spontaneous and what is the $E°_{cell}$?
In the reaction $2Al(s) + 3Mg^{2+}(aq) ightarrow 2Al^{3+}(aq) + 3Mg(s)$, given $E°{Al} = -1.66V$ and $E°{Mg} = -2.36V$, and knowing that Magnesium is more reactive than Aluminum, is the reaction spontaneous and what is the $E°_{cell}$?
For an electrochemical reaction to be spontaneous, which of the following must be true regarding the standard cell potential ($E°_{cell}$)?
For an electrochemical reaction to be spontaneous, which of the following must be true regarding the standard cell potential ($E°_{cell}$)?
In a redox reaction, if a species is described as the 'reducing agent', what is it actually doing?
In a redox reaction, if a species is described as the 'reducing agent', what is it actually doing?
When assigning oxidation numbers, which of the following elements is almost always assigned an oxidation number of -1 in its compounds?
When assigning oxidation numbers, which of the following elements is almost always assigned an oxidation number of -1 in its compounds?
What is the oxidation number of sulfur (S) in the sulfite ion, $SO_3^{2-}$?
What is the oxidation number of sulfur (S) in the sulfite ion, $SO_3^{2-}$?
Consider the unbalanced reaction: $MnO_4^−(aq) + I^−(aq)
ightarrow MnO_2(s) + I_2(s)$. Which species is the oxidizing agent?
Consider the unbalanced reaction: $MnO_4^−(aq) + I^−(aq) ightarrow MnO_2(s) + I_2(s)$. Which species is the oxidizing agent?
In the balanced redox reaction: $5Fe^{2+}(aq) + MnO_4^−(aq) + 8H^+(aq)
ightarrow 5Fe^{3+}(aq) + Mn^{2+}(aq) + 4H_2O(l)$, which species is oxidized?
In the balanced redox reaction: $5Fe^{2+}(aq) + MnO_4^−(aq) + 8H^+(aq) ightarrow 5Fe^{3+}(aq) + Mn^{2+}(aq) + 4H_2O(l)$, which species is oxidized?
During the reaction $Zn(s) + Cu^{2+}(aq)
ightarrow Zn^{2+}(aq) + Cu(s)$, what happens to the oxidation number of copper?
During the reaction $Zn(s) + Cu^{2+}(aq) ightarrow Zn^{2+}(aq) + Cu(s)$, what happens to the oxidation number of copper?
Which of the following is a characteristic of a substance that is likely to act as a strong oxidizing agent?
Which of the following is a characteristic of a substance that is likely to act as a strong oxidizing agent?
Given the unbalanced equation: $Cr_2O_7^{2-}(aq) + Fe^{2+}(aq)
ightarrow Cr^{3+}(aq) + Fe^{3+}(aq)$, what is the change in the oxidation number of chromium (Cr)?
Given the unbalanced equation: $Cr_2O_7^{2-}(aq) + Fe^{2+}(aq) ightarrow Cr^{3+}(aq) + Fe^{3+}(aq)$, what is the change in the oxidation number of chromium (Cr)?
Which type of electrochemical cell uses electrical energy to drive non-spontaneous chemical reactions?
Which type of electrochemical cell uses electrical energy to drive non-spontaneous chemical reactions?
In an electrochemical cell under standard conditions, what concentrations are all ion solutions set to for measuring standard cell potential?
In an electrochemical cell under standard conditions, what concentrations are all ion solutions set to for measuring standard cell potential?
A substance has a high positive oxidation potential. What does this suggest about its properties in redox reactions?
A substance has a high positive oxidation potential. What does this suggest about its properties in redox reactions?
In an electrolytic cell, which of the following statements regarding the anode is correct?
In an electrolytic cell, which of the following statements regarding the anode is correct?
In the reaction $Cl_2 + 2NaBr \rightarrow 2NaCl + Br_2$, which element undergoes reduction?
In the reaction $Cl_2 + 2NaBr \rightarrow 2NaCl + Br_2$, which element undergoes reduction?
How can the cell potential ($E_{cell}$) be used to predict the spontaneity of a redox reaction?
How can the cell potential ($E_{cell}$) be used to predict the spontaneity of a redox reaction?
In the reaction $Pb(NO_3)_2 + 2KI \rightarrow PbI_2 + 2KNO_3$, which species is neither oxidized nor reduced?
In the reaction $Pb(NO_3)_2 + 2KI \rightarrow PbI_2 + 2KNO_3$, which species is neither oxidized nor reduced?
In electrochemistry, what distinguishes a voltaic cell from an electrolytic cell?
In electrochemistry, what distinguishes a voltaic cell from an electrolytic cell?
What is the relationship between electrode potential and the strength of an oxidizing agent?
What is the relationship between electrode potential and the strength of an oxidizing agent?
Which of the following conditions will result in a spontaneous electrochemical reaction?
Which of the following conditions will result in a spontaneous electrochemical reaction?
Consider an electrochemical cell where a less reactive metal is placed at the anode. What can be predicted about the cell potential (E) and the reaction's spontaneity?
Consider an electrochemical cell where a less reactive metal is placed at the anode. What can be predicted about the cell potential (E) and the reaction's spontaneity?
An electrochemical cell is constructed with aluminum and magnesium electrodes. Given $E^\circ_{Al} = +1.66V$ and $E^\circ_{Mg} = -2.36V$, if magnesium is placed at the anode, what is the $E^\circ_{cell}$ and is the reaction spontaneous?
An electrochemical cell is constructed with aluminum and magnesium electrodes. Given $E^\circ_{Al} = +1.66V$ and $E^\circ_{Mg} = -2.36V$, if magnesium is placed at the anode, what is the $E^\circ_{cell}$ and is the reaction spontaneous?
Given the half-cell reactions: $Zn ightarrow Zn^{2+}(aq) + 2e^-$ $E = +0.76V$ and $Cu^{2+}(aq) + 2e^- ightarrow Cu$ $E = +0.34V$, and the overall reaction $Zn + Cu^{2+}(aq) ightarrow Zn^{2+}(aq) + Cu$, what is the correct cell representation?
Given the half-cell reactions: $Zn ightarrow Zn^{2+}(aq) + 2e^-$ $E = +0.76V$ and $Cu^{2+}(aq) + 2e^- ightarrow Cu$ $E = +0.34V$, and the overall reaction $Zn + Cu^{2+}(aq) ightarrow Zn^{2+}(aq) + Cu$, what is the correct cell representation?
In the reaction $2Al + 3Mg^{2+}(aq) ightarrow 2Al^{3+}(aq) + 3Mg$, given that aluminum has a standard oxidation potential of +1.66V and magnesium has a standard oxidation potential of -2.36V, which setup will result in a spontaneous reaction?
In the reaction $2Al + 3Mg^{2+}(aq) ightarrow 2Al^{3+}(aq) + 3Mg$, given that aluminum has a standard oxidation potential of +1.66V and magnesium has a standard oxidation potential of -2.36V, which setup will result in a spontaneous reaction?
For the reaction $Zn + Cu^{2+}(aq) ightarrow Zn^{2+}(aq) + Cu$, which option correctly identifies the half-reactions and their locations in an electrochemical cell?
For the reaction $Zn + Cu^{2+}(aq) ightarrow Zn^{2+}(aq) + Cu$, which option correctly identifies the half-reactions and their locations in an electrochemical cell?
Which set of conditions will result in an electrochemical cell with a positive standard cell potential ($E^\circ_{cell}$), indicating a spontaneous reaction?
Which set of conditions will result in an electrochemical cell with a positive standard cell potential ($E^\circ_{cell}$), indicating a spontaneous reaction?
Given the half-reactions: $Al ightarrow Al^{3+}(aq) + 3e^-$ $E = +1.66Vand$Mg^{2+}(aq) + 2e^-
ightarrow Mg$ $E = -2.36V, what is the standard cell potential ($E_{cell}$) for the reaction when they are combined in a voltaic cell?
Given the half-reactions: $Al ightarrow Al^{3+}(aq) + 3e^-$ $E = +1.66Vand$Mg^{2+}(aq) + 2e^-
ightarrow Mg$ $E = -2.36V, what is the standard cell potential ($E_{cell}$) for the reaction when they are combined in a voltaic cell?
For the overall reaction $2Al(s) + 3Cu^{2+}(aq) ightarrow 2Al^{3+}(aq) + 3Cu(s)$, if the $E$ for $Al^{3+}/Al$ is -1.66 V and the $E$ for $Cu^{2+}/Cu$ is +0.34 V, what is the standard cell potential ($E_{cell}$)?
For the overall reaction $2Al(s) + 3Cu^{2+}(aq) ightarrow 2Al^{3+}(aq) + 3Cu(s)$, if the $E$ for $Al^{3+}/Al$ is -1.66 V and the $E$ for $Cu^{2+}/Cu$ is +0.34 V, what is the standard cell potential ($E_{cell}$)?
Consider a voltaic cell using zinc and copper half-cells. If the zinc electrode is the anode, what processes occur at each electrode, and how does this affect cell potential?
Consider a voltaic cell using zinc and copper half-cells. If the zinc electrode is the anode, what processes occur at each electrode, and how does this affect cell potential?
In a redox reaction, if a species gains electrons, which of the following terms describes this process?
In a redox reaction, if a species gains electrons, which of the following terms describes this process?
Which statement accurately describes the relationship between an oxidizing agent and the species it interacts with in a redox reaction?
Which statement accurately describes the relationship between an oxidizing agent and the species it interacts with in a redox reaction?
In a chemical compound, if oxygen is not bonded to fluorine and it is not a peroxide, what is its oxidation number?
In a chemical compound, if oxygen is not bonded to fluorine and it is not a peroxide, what is its oxidation number?
Determine the oxidation number of manganese (Mn) in the permanganate ion, $MnO_4^-$.
Determine the oxidation number of manganese (Mn) in the permanganate ion, $MnO_4^-$.
In the reaction $Zn(s) + Cu^{2+}(aq)
ightarrow Zn^{2+}(aq) + Cu(s)$, which species is the reducing agent?
In the reaction $Zn(s) + Cu^{2+}(aq) ightarrow Zn^{2+}(aq) + Cu(s)$, which species is the reducing agent?
Consider the incomplete redox reaction: $Cr_2O_7^{2-}(aq)
ightarrow Cr^{3+}(aq)$. What is the oxidation number change for chromium (Cr)?
Consider the incomplete redox reaction: $Cr_2O_7^{2-}(aq) ightarrow Cr^{3+}(aq)$. What is the oxidation number change for chromium (Cr)?
In the reaction $2H_2(g) + O_2(g)
ightarrow 2H_2O(g)$, which species is the oxidizing agent?
In the reaction $2H_2(g) + O_2(g) ightarrow 2H_2O(g)$, which species is the oxidizing agent?
Which of the following describes what happens at the cathode in an electrolytic cell?
Which of the following describes what happens at the cathode in an electrolytic cell?
For the reaction $Ni^{2+}(aq) + 2Ag(s) \rightarrow Ni(s) + 2Ag^+(aq)$, the standard cell potential ($E°_{cell}$) is -1.05 V. What does this indicate about the reaction?
For the reaction $Ni^{2+}(aq) + 2Ag(s) \rightarrow Ni(s) + 2Ag^+(aq)$, the standard cell potential ($E°_{cell}$) is -1.05 V. What does this indicate about the reaction?
Consider an electrochemical cell made of a Zinc electrode in $Zn^{2+}$ solution and a Silver electrode in $Ag^+$ solution. Given that Zinc is more reactive than Silver, which of the following statements is true if the reaction is spontaneous?
Consider an electrochemical cell made of a Zinc electrode in $Zn^{2+}$ solution and a Silver electrode in $Ag^+$ solution. Given that Zinc is more reactive than Silver, which of the following statements is true if the reaction is spontaneous?
What is the correct cell representation for the reaction $Mg(s) + Fe^{2+}(aq) \rightarrow Mg^{2+}(aq) + Fe(s)$?
What is the correct cell representation for the reaction $Mg(s) + Fe^{2+}(aq) \rightarrow Mg^{2+}(aq) + Fe(s)$?
Given the half-reactions: $Cu^{2+}(aq) + 2e^- \rightarrow Cu(s)$ $E° = +0.34V$ and $Sn^{2+}(aq) + 2e^- \rightarrow Sn(s)$ $E° = -0.14V$, calculate the standard cell potential ($E°_{cell}$) for the spontaneous reaction.
Given the half-reactions: $Cu^{2+}(aq) + 2e^- \rightarrow Cu(s)$ $E° = +0.34V$ and $Sn^{2+}(aq) + 2e^- \rightarrow Sn(s)$ $E° = -0.14V$, calculate the standard cell potential ($E°_{cell}$) for the spontaneous reaction.
In the electrolytic process of water ($H_2O$) into hydrogen ($H_2$) and oxygen ($O_2$), what occurs at the cathode?
In the electrolytic process of water ($H_2O$) into hydrogen ($H_2$) and oxygen ($O_2$), what occurs at the cathode?
Consider the half-reactions:
$Ag^+(aq) + e^- \rightarrow Ag(s)$ $E° = +0.80V$
$Ni^{2+}(aq) + 2e^- \rightarrow Ni(s)$ $E° = -0.25V$
If a voltaic cell is constructed using these half-reactions, what is the standard cell potential if Nickel is at the anode?
Consider the half-reactions: $Ag^+(aq) + e^- \rightarrow Ag(s)$ $E° = +0.80V$ $Ni^{2+}(aq) + 2e^- \rightarrow Ni(s)$ $E° = -0.25V$ If a voltaic cell is constructed using these half-reactions, what is the standard cell potential if Nickel is at the anode?
For the voltaic cell $Zn(s) | Zn^{2+}(aq) || Cu^{2+}(aq) | Cu(s)$, how does the concentration of $Zn^{2+}$ ions in the anode compartment change as the cell operates?
For the voltaic cell $Zn(s) | Zn^{2+}(aq) || Cu^{2+}(aq) | Cu(s)$, how does the concentration of $Zn^{2+}$ ions in the anode compartment change as the cell operates?
In a redox reaction, $MnO_4^−(aq)$ is converted to $Mn^{2+}(aq)$ in an acidic solution. Which of the following is true about the role of $MnO_4^−(aq)$?
In a redox reaction, $MnO_4^−(aq)$ is converted to $Mn^{2+}(aq)$ in an acidic solution. Which of the following is true about the role of $MnO_4^−(aq)$?
Which of the following describes the change in oxidation number for a substance that is acting as a reducing agent?
Which of the following describes the change in oxidation number for a substance that is acting as a reducing agent?
Consider the reaction: $2Al(s) + 3Cu^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Cu(s)$.
Given the following standard reduction potentials:
$Al^{3+}(aq) + 3e^- \rightarrow Al(s)$ $E° = -1.66 V$
$Cu^{2+}(aq) + 2e^- \rightarrow Cu(s)$ $E° = +0.34 V$
Calculate the standard cell potential.
Consider the reaction: $2Al(s) + 3Cu^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Cu(s)$. Given the following standard reduction potentials: $Al^{3+}(aq) + 3e^- \rightarrow Al(s)$ $E° = -1.66 V$ $Cu^{2+}(aq) + 2e^- \rightarrow Cu(s)$ $E° = +0.34 V$ Calculate the standard cell potential.
Which of the following best describes what happens to a strong reducing agent during a chemical reaction?
Which of the following best describes what happens to a strong reducing agent during a chemical reaction?
In an electrochemical cell, if a metal with a high positive oxidation potential is used as an electrode, what does this indicate about its role?
In an electrochemical cell, if a metal with a high positive oxidation potential is used as an electrode, what does this indicate about its role?
Consider the reaction: $Pb(NO_3)_2 + 2KI \rightarrow PbI_2 + 2KNO_3$. Which species remains unchanged in terms of oxidation number?
Consider the reaction: $Pb(NO_3)_2 + 2KI \rightarrow PbI_2 + 2KNO_3$. Which species remains unchanged in terms of oxidation number?
If the standard reduction potential ($E°$) for $Zn^{2+} + 2e^- \rightarrow Zn$ is -0.76 V, what does this indicate about the reaction under standard conditions?
If the standard reduction potential ($E°$) for $Zn^{2+} + 2e^- \rightarrow Zn$ is -0.76 V, what does this indicate about the reaction under standard conditions?
In the reaction $2Na + Cl_2 \rightarrow 2NaCl$, which species is the oxidizing agent?
In the reaction $2Na + Cl_2 \rightarrow 2NaCl$, which species is the oxidizing agent?
For an electrochemical cell, what conditions define the standard cell potential ($E°$)?
For an electrochemical cell, what conditions define the standard cell potential ($E°$)?
In an electrolytic cell, what is the role of an external source of electricity?
In an electrolytic cell, what is the role of an external source of electricity?
If a voltaic cell is set up under non-standard conditions, how would increasing the concentration of the reactants generally affect the cell potential?
If a voltaic cell is set up under non-standard conditions, how would increasing the concentration of the reactants generally affect the cell potential?
In a redox reaction, if a substance gains electrons, what happens to its oxidation number and what is this process called?
In a redox reaction, if a substance gains electrons, what happens to its oxidation number and what is this process called?
In a redox reaction, if a substance is reduced, what happens to its oxidation number and what role does it play?
In a redox reaction, if a substance is reduced, what happens to its oxidation number and what role does it play?
Consider the compound $Na_2S_2O_3$. What is the oxidation number of sulfur (S) in this compound, given that sodium (Na) has an oxidation number of +1 and oxygen (O) has an oxidation number of -2?
Consider the compound $Na_2S_2O_3$. What is the oxidation number of sulfur (S) in this compound, given that sodium (Na) has an oxidation number of +1 and oxygen (O) has an oxidation number of -2?
In the reaction $MnO_4^- + 5Fe^{2+} + 8H^+ \longrightarrow Mn^{2+} + 5Fe^{3+} + 4H_2O$, which species is the oxidizing agent?
In the reaction $MnO_4^- + 5Fe^{2+} + 8H^+ \longrightarrow Mn^{2+} + 5Fe^{3+} + 4H_2O$, which species is the oxidizing agent?
When balancing redox reactions using the half-reaction method, what is the first step after separating the unbalanced reaction into two half-reactions?
When balancing redox reactions using the half-reaction method, what is the first step after separating the unbalanced reaction into two half-reactions?
Which set of oxidation numbers is correctly assigned to all elements in $Ca(ClO_3)_2$?
Which set of oxidation numbers is correctly assigned to all elements in $Ca(ClO_3)_2$?
In a redox reaction, the reducing agent:
In a redox reaction, the reducing agent:
In the following unbalanced reaction, $Cr_2O_7^{2-} + I^- \longrightarrow Cr^{3+} + I_2$, which species is oxidized?
In the following unbalanced reaction, $Cr_2O_7^{2-} + I^- \longrightarrow Cr^{3+} + I_2$, which species is oxidized?
For the reaction: $Zn(s) + 2H^+(aq)
ightarrow Zn^{2+}(aq) + H_2(g)$, which species acts as the reducing agent?
For the reaction: $Zn(s) + 2H^+(aq) ightarrow Zn^{2+}(aq) + H_2(g)$, which species acts as the reducing agent?
Balance the following equation: $MnO_4^- + Fe^{2+} \longrightarrow Mn^{2+} + Fe^{3+}$ (acidic conditions). What is the coefficient for $Fe^{2+}$ in the balanced equation?
Balance the following equation: $MnO_4^- + Fe^{2+} \longrightarrow Mn^{2+} + Fe^{3+}$ (acidic conditions). What is the coefficient for $Fe^{2+}$ in the balanced equation?
For the reaction $Ni^{2+}(aq) + 2Ag(s) \rightarrow Ni(s) + 2Ag^+(aq)$, given that the standard cell potential ($E_{cell}^\circ$) is -1.05 V, what can be concluded about the reaction at standard conditions?
For the reaction $Ni^{2+}(aq) + 2Ag(s) \rightarrow Ni(s) + 2Ag^+(aq)$, given that the standard cell potential ($E_{cell}^\circ$) is -1.05 V, what can be concluded about the reaction at standard conditions?
Consider a voltaic cell constructed with a zinc electrode in a $Zn^{2+}$ solution and a copper electrode in a $Cu^{2+}$ solution. Given that zinc is more reactive than copper, which of the following statements is true regarding the spontaneity of the reaction and the cell potential?
Consider a voltaic cell constructed with a zinc electrode in a $Zn^{2+}$ solution and a copper electrode in a $Cu^{2+}$ solution. Given that zinc is more reactive than copper, which of the following statements is true regarding the spontaneity of the reaction and the cell potential?
Given the reaction: $3Mg^{2+}(aq) + 2Al(s) \rightarrow 3Mg(s) + 2Al^{3+}(aq)$, and knowing that magnesium is more reactive than aluminum, what would you expect the sign of $E_{cell}$ to be for this reaction as written, and what does this indicate about its spontaneity?
Given the reaction: $3Mg^{2+}(aq) + 2Al(s) \rightarrow 3Mg(s) + 2Al^{3+}(aq)$, and knowing that magnesium is more reactive than aluminum, what would you expect the sign of $E_{cell}$ to be for this reaction as written, and what does this indicate about its spontaneity?
Consider the following cell representation: $Fe(s) | Fe^{2+}(aq) || Ag^+(aq) | Ag(s)$. If the standard reduction potential of $Ag^+/Ag$ is +0.80 V and $Fe^{2+}/Fe$ is -0.44 V, what is the standard cell potential ($E_{cell}^\circ$) for this voltaic cell?
Consider the following cell representation: $Fe(s) | Fe^{2+}(aq) || Ag^+(aq) | Ag(s)$. If the standard reduction potential of $Ag^+/Ag$ is +0.80 V and $Fe^{2+}/Fe$ is -0.44 V, what is the standard cell potential ($E_{cell}^\circ$) for this voltaic cell?
If a more reactive metal, M, is used as the anode in a voltaic cell and a less reactive metal, L, is used as the cathode, which of the following statements is most accurate?
If a more reactive metal, M, is used as the anode in a voltaic cell and a less reactive metal, L, is used as the cathode, which of the following statements is most accurate?
Given the half-reactions: $Zn(s) \rightarrow Zn^{2+}(aq) + 2e^-$ $E^\circ = +0.76V$ and $Cu^{2+}(aq) + 2e^- \rightarrow Cu(s)$ $E^\circ = +0.34V$, which of the following correctly represents the overall spontaneous cell reaction and its standard cell potential?
Given the half-reactions: $Zn(s) \rightarrow Zn^{2+}(aq) + 2e^-$ $E^\circ = +0.76V$ and $Cu^{2+}(aq) + 2e^- \rightarrow Cu(s)$ $E^\circ = +0.34V$, which of the following correctly represents the overall spontaneous cell reaction and its standard cell potential?
For the cell representation $Mg(s) | Mg^{2+}(aq) || Ag^+(aq) | Ag(s)$, what is the overall balanced cell reaction?
For the cell representation $Mg(s) | Mg^{2+}(aq) || Ag^+(aq) | Ag(s)$, what is the overall balanced cell reaction?
Which of the following is an application of redox reactions?
Which of the following is an application of redox reactions?
In a redox reaction, the reducing agent ________.
In a redox reaction, the reducing agent ________.
When assigning oxidation numbers, which of the following rules always takes precedence?
When assigning oxidation numbers, which of the following rules always takes precedence?
In a redox reaction, if a substance is reduced, which of the following must also be true?
In a redox reaction, if a substance is reduced, which of the following must also be true?
In the reaction $4Fe + 3O_2 \rightarrow 2Fe_2O_3$, what is the change in oxidation number for iron (Fe)?
In the reaction $4Fe + 3O_2 \rightarrow 2Fe_2O_3$, what is the change in oxidation number for iron (Fe)?
Which of the following statements correctly describes the roles of the oxidizing and reducing agents in a redox reaction?
Which of the following statements correctly describes the roles of the oxidizing and reducing agents in a redox reaction?
Which of the following describes what happens at the anode in voltaic and electrolytic cells?
Which of the following describes what happens at the anode in voltaic and electrolytic cells?
According to the rules for assigning oxidation numbers, what is the oxidation number of alkali metals (Group 1A) in compounds?
According to the rules for assigning oxidation numbers, what is the oxidation number of alkali metals (Group 1A) in compounds?
For a voltaic cell constructed with a zinc electrode in $Zn^{2+}$ solution and a copper electrode in $Cu^{2+}$ solution, and the solutions are connected by a salt bridge, what is the role of the copper electrode?
For a voltaic cell constructed with a zinc electrode in $Zn^{2+}$ solution and a copper electrode in $Cu^{2+}$ solution, and the solutions are connected by a salt bridge, what is the role of the copper electrode?
Which of the following statements correctly describes the purpose of the cell potential ($E_{cell}$) value?
Which of the following statements correctly describes the purpose of the cell potential ($E_{cell}$) value?
What is the oxidation number of oxygen in most compounds, excluding when it is bonded to fluorine or in peroxides?
What is the oxidation number of oxygen in most compounds, excluding when it is bonded to fluorine or in peroxides?
Determine the oxidation number of sulfur in the sulfite ion, $SO_3^{2-}$.
Determine the oxidation number of sulfur in the sulfite ion, $SO_3^{2-}$.
In the reaction $Cl_2 + 2NaBr \rightarrow 2NaCl + Br_2$, which element is being oxidized?
In the reaction $Cl_2 + 2NaBr \rightarrow 2NaCl + Br_2$, which element is being oxidized?
Which of the following is true of electrolytic cells?
Which of the following is true of electrolytic cells?
Which of the following conditions are standard conditions for measuring standard cell potential ($E^\circ$)?
Which of the following conditions are standard conditions for measuring standard cell potential ($E^\circ$)?
In the reaction $2KBr(aq) + Cl_2(g)
ightarrow 2KCl(aq) + Br_2(l)$, which element is being oxidized?
In the reaction $2KBr(aq) + Cl_2(g) ightarrow 2KCl(aq) + Br_2(l)$, which element is being oxidized?
Which statement correctly describes the relationship between electrode potential and the strength of a reducing agent?
Which statement correctly describes the relationship between electrode potential and the strength of a reducing agent?
For the reaction $Ni^{2+}(aq) + Fe(s)
ightarrow Ni(s) + Fe^{2+}(aq)$, if the standard cell potential ($E_{cell}^\circ$) is positive, and iron is known to be more reactive than nickel, placing iron at the anode would cause the reaction to be what?
For the reaction $Ni^{2+}(aq) + Fe(s) ightarrow Ni(s) + Fe^{2+}(aq)$, if the standard cell potential ($E_{cell}^\circ$) is positive, and iron is known to be more reactive than nickel, placing iron at the anode would cause the reaction to be what?
Which of the following conditions would result in a non-spontaneous electrochemical reaction?
Which of the following conditions would result in a non-spontaneous electrochemical reaction?
Given the half-reactions: $Zn(s)
ightarrow Zn^{2+}(aq) + 2e^-$ $E^\circ = +0.76V$ and $Ag^+(aq) + e^-
ightarrow Ag(s)$ $E^\circ = +0.80V$. What is the standard cell potential ($E^\circ_{cell}$) for the reaction $Zn(s) + 2Ag^+(aq)
ightarrow Zn^{2+}(aq) + 2Ag(s)$?
Given the half-reactions: $Zn(s) ightarrow Zn^{2+}(aq) + 2e^-$ $E^\circ = +0.76V$ and $Ag^+(aq) + e^- ightarrow Ag(s)$ $E^\circ = +0.80V$. What is the standard cell potential ($E^\circ_{cell}$) for the reaction $Zn(s) + 2Ag^+(aq) ightarrow Zn^{2+}(aq) + 2Ag(s)$?
Consider a voltaic cell with the following half-reactions: $Cu^{2+}(aq) + 2e^-
ightarrow Cu(s)$ $E^\circ = +0.34V$ and $Zn^{2+}(aq) + 2e^-
ightarrow Zn(s)$ $E^\circ = -0.76V$. If the zinc electrode is the anode, what is the $E^\circ_{cell}$?
Consider a voltaic cell with the following half-reactions: $Cu^{2+}(aq) + 2e^- ightarrow Cu(s)$ $E^\circ = +0.34V$ and $Zn^{2+}(aq) + 2e^- ightarrow Zn(s)$ $E^\circ = -0.76V$. If the zinc electrode is the anode, what is the $E^\circ_{cell}$?
If a voltaic cell is set up such that the standard cell potential ($E^\circ_{cell}$) is negative, what does this indicate about the reaction under standard conditions?
If a voltaic cell is set up such that the standard cell potential ($E^\circ_{cell}$) is negative, what does this indicate about the reaction under standard conditions?
Given the reaction: $2Ag^+(aq) + Cu(s)
ightarrow 2Ag(s) + Cu^{2+}(aq)$, which of the following cell representations accurately describes this electrochemical cell?
Given the reaction: $2Ag^+(aq) + Cu(s) ightarrow 2Ag(s) + Cu^{2+}(aq)$, which of the following cell representations accurately describes this electrochemical cell?
For an electrochemical cell, the standard reduction potential ($E^\circ$) of $Cu^{2+}(aq) + 2e^-
ightarrow Cu(s)$ is +0.34 V, and $Zn^{2+}(aq) + 2e^-
ightarrow Zn(s)$ is -0.76 V. If the cell reaction is $Zn(s) + Cu^{2+}(aq)
ightarrow Zn^{2+}(aq) + Cu(s)$, what is the standard cell potential ($E^\circ_{cell}$)?
For an electrochemical cell, the standard reduction potential ($E^\circ$) of $Cu^{2+}(aq) + 2e^- ightarrow Cu(s)$ is +0.34 V, and $Zn^{2+}(aq) + 2e^- ightarrow Zn(s)$ is -0.76 V. If the cell reaction is $Zn(s) + Cu^{2+}(aq) ightarrow Zn^{2+}(aq) + Cu(s)$, what is the standard cell potential ($E^\circ_{cell}$)?
How does the placement of a more reactive metal at the cathode affect the spontaneity of an electrochemical cell?
How does the placement of a more reactive metal at the cathode affect the spontaneity of an electrochemical cell?
In the redox reaction $2Al(s) + 3Mg^{2+}(aq)
ightarrow 2Al^{3+}(aq) + 3Mg(s)$, if the standard reduction potential for $Al^{3+}$ is -1.66V and for $Mg^{2+}$ is -2.36V, what is the standard cell potential ($E^\circ_{cell}$)?
In the redox reaction $2Al(s) + 3Mg^{2+}(aq) ightarrow 2Al^{3+}(aq) + 3Mg(s)$, if the standard reduction potential for $Al^{3+}$ is -1.66V and for $Mg^{2+}$ is -2.36V, what is the standard cell potential ($E^\circ_{cell}$)?
Which of the following factors primarily determines the spontaneity of a redox reaction in an electrochemical cell?
Which of the following factors primarily determines the spontaneity of a redox reaction in an electrochemical cell?
In a redox reaction, if a species is identified as the reducing agent, what specifically is it doing?
In a redox reaction, if a species is identified as the reducing agent, what specifically is it doing?
Which statement correctly describes the relationship between oxidation numbers and the processes of oxidation and reduction in a redox reaction?
Which statement correctly describes the relationship between oxidation numbers and the processes of oxidation and reduction in a redox reaction?
In a chemical reaction, if an atom's oxidation number increases, which of the following processes has occurred?
In a chemical reaction, if an atom's oxidation number increases, which of the following processes has occurred?
What is the oxidation number of hydrogen in $NaH$?
What is the oxidation number of hydrogen in $NaH$?
What is the correct half-reaction for the oxidation of $Al$ to $Al^{3+}$?
What is the correct half-reaction for the oxidation of $Al$ to $Al^{3+}$?
In the reaction $4Fe + 3O_2 \rightarrow 2Fe_2O_3$, which species is being oxidized, and what is the change in its oxidation number?
In the reaction $4Fe + 3O_2 \rightarrow 2Fe_2O_3$, which species is being oxidized, and what is the change in its oxidation number?
Consider the reaction $Pb(NO_3)_2 + 2KI \rightarrow PbI_2 + 2KNO_3$. Which species undergoes double displacement but no change in oxidation number?
Consider the reaction $Pb(NO_3)_2 + 2KI \rightarrow PbI_2 + 2KNO_3$. Which species undergoes double displacement but no change in oxidation number?
In an electrochemical cell, the anode is defined as the electrode where what occurs, and what is its charge in an electrolytic cell?
In an electrochemical cell, the anode is defined as the electrode where what occurs, and what is its charge in an electrolytic cell?
How does a high positive reduction potential relate to a substance's ability to act as an oxidizing agent?
How does a high positive reduction potential relate to a substance's ability to act as an oxidizing agent?
What is the role of electrical energy in voltaic and electrolytic cells?
What is the role of electrical energy in voltaic and electrolytic cells?
If a metal strip is immersed in a solution containing its ions, what determines the electrode potential?
If a metal strip is immersed in a solution containing its ions, what determines the electrode potential?
In the reaction $Cl_2 + 2NaBr \rightarrow 2NaCl + Br_2$, identify which species is reduced and what is the change in its oxidation number.
In the reaction $Cl_2 + 2NaBr \rightarrow 2NaCl + Br_2$, identify which species is reduced and what is the change in its oxidation number.
What is the relationship between a substance's oxidation potential and its effectiveness as a reducing agent?
What is the relationship between a substance's oxidation potential and its effectiveness as a reducing agent?
If the voltage of an electrochemical cell is measured to be zero, what does this indicate about the reaction at standard conditions?
If the voltage of an electrochemical cell is measured to be zero, what does this indicate about the reaction at standard conditions?
For a voltaic cell with a positive standard cell potential ($E^\circ_{cell}$), which statement is correct regarding the spontaneity of the reaction?
For a voltaic cell with a positive standard cell potential ($E^\circ_{cell}$), which statement is correct regarding the spontaneity of the reaction?
In an electrochemical cell, if a less reactive metal is used as the anode, what can be inferred about the spontaneity of the reaction?
In an electrochemical cell, if a less reactive metal is used as the anode, what can be inferred about the spontaneity of the reaction?
Consider the reaction: $Ni^{2+}(aq) + Zn(s) \rightarrow Ni(s) + Zn^{2+}(aq)$. Given that zinc is more reactive than nickel, which of the following statements is true?
Consider the reaction: $Ni^{2+}(aq) + Zn(s) \rightarrow Ni(s) + Zn^{2+}(aq)$. Given that zinc is more reactive than nickel, which of the following statements is true?
Given the cell representation: $Ag(s)|Ag^+(aq)||Cu^{2+}(aq)|Cu(s)$, and knowing that copper is more reactive than silver, what can be inferred?
Given the cell representation: $Ag(s)|Ag^+(aq)||Cu^{2+}(aq)|Cu(s)$, and knowing that copper is more reactive than silver, what can be inferred?
Given the half-reactions: $\begin{aligned}Zn(s) &\rightarrow Zn^{2+}(aq) + 2e^- & E^\circ &= +0.76 \text{ V} \ Cu^{2+}(aq) + 2e^- &\rightarrow Cu(s) & E^\circ &= +0.34 \text{ V}\end{aligned}$ What is the standard cell potential ($E^\circ_{cell}$) for a cell using these half-reactions?
Given the half-reactions: $\begin{aligned}Zn(s) &\rightarrow Zn^{2+}(aq) + 2e^- & E^\circ &= +0.76 \text{ V} \ Cu^{2+}(aq) + 2e^- &\rightarrow Cu(s) & E^\circ &= +0.34 \text{ V}\end{aligned}$ What is the standard cell potential ($E^\circ_{cell}$) for a cell using these half-reactions?
Consider the reaction: $2Al(s) + 3Mg^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Mg(s)$. Given that $E^\circ_{Al^{3+}/Al} = -1.66 \text{ V}$ and $E^\circ_{Mg^{2+}/Mg} = -2.36 \text{ V}$, calculate the standard cell potential ($E^\circ_{cell}$).
Consider the reaction: $2Al(s) + 3Mg^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Mg(s)$. Given that $E^\circ_{Al^{3+}/Al} = -1.66 \text{ V}$ and $E^\circ_{Mg^{2+}/Mg} = -2.36 \text{ V}$, calculate the standard cell potential ($E^\circ_{cell}$).
Which of the following is a correct cell representation for the reaction: $Zn(s) + 2Ag^+(aq) \rightarrow Zn^{2+}(aq) + 2Ag(s)$?
Which of the following is a correct cell representation for the reaction: $Zn(s) + 2Ag^+(aq) \rightarrow Zn^{2+}(aq) + 2Ag(s)$?
In the reaction $MnO_4^-(aq) + 5Fe^{2+}(aq) + 8H^+(aq) \rightarrow Mn^{2+}(aq) + 5Fe^{3+}(aq) + 4H_2O(l)$, which species is the oxidizing agent?
In the reaction $MnO_4^-(aq) + 5Fe^{2+}(aq) + 8H^+(aq) \rightarrow Mn^{2+}(aq) + 5Fe^{3+}(aq) + 4H_2O(l)$, which species is the oxidizing agent?
Which of the following statements correctly describes the application of redox reactions?
Which of the following statements correctly describes the application of redox reactions?
Which of the following statements correctly describes the role of a reducing agent in a redox reaction?
Which of the following statements correctly describes the role of a reducing agent in a redox reaction?
What is the oxidation number of an element in its standard, elemental state?
What is the oxidation number of an element in its standard, elemental state?
In the reaction $4Fe + 3O_2 \rightarrow 2Fe_2O_3$, which element undergoes oxidation, and what is the change in its oxidation number?
In the reaction $4Fe + 3O_2 \rightarrow 2Fe_2O_3$, which element undergoes oxidation, and what is the change in its oxidation number?
What is the primary distinction between voltaic cells and electrolytic cells?
What is the primary distinction between voltaic cells and electrolytic cells?
In an electrochemical cell, what does a high positive reduction potential of a substance indicate?
In an electrochemical cell, what does a high positive reduction potential of a substance indicate?
What is the role of the anode in both voltaic and electrolytic cells?
What is the role of the anode in both voltaic and electrolytic cells?
Consider an electrochemical cell where the concentration of reactants is increased. What effect does this have on the cell potential ($E_{cell}$)?
Consider an electrochemical cell where the concentration of reactants is increased. What effect does this have on the cell potential ($E_{cell}$)?
In an electrochemical cell consisting of a zinc electrode in $Zn^{2+}$ solution and a silver electrode in $Ag^{+}$ solution, which is the anode and which reaction occurs there?
In an electrochemical cell consisting of a zinc electrode in $Zn^{2+}$ solution and a silver electrode in $Ag^{+}$ solution, which is the anode and which reaction occurs there?
What conditions are specified when measuring standard electrode potentials?
What conditions are specified when measuring standard electrode potentials?
Given the reaction: $Pb(NO_3)_2 + 2KI \rightarrow PbI_2 + 2KNO_3$, identify which species undergoes neither oxidation nor reduction.
Given the reaction: $Pb(NO_3)_2 + 2KI \rightarrow PbI_2 + 2KNO_3$, identify which species undergoes neither oxidation nor reduction.
If a voltaic cell is constructed with a zinc electrode in $Zn^{2+}$ solution and a copper electrode in $Cu^{2+}$ solution, and the solutions are connected by a salt bridge, what is the salt bridge's primary function?
If a voltaic cell is constructed with a zinc electrode in $Zn^{2+}$ solution and a copper electrode in $Cu^{2+}$ solution, and the solutions are connected by a salt bridge, what is the salt bridge's primary function?
For an electrochemical reaction to be spontaneous, which of the following conditions must be met regarding the placement of metals and the cell potential?
For an electrochemical reaction to be spontaneous, which of the following conditions must be met regarding the placement of metals and the cell potential?
In an electrochemical cell, if the standard cell potential ($E°_{cell}$) is negative, what does this indicate about the spontaneity of the reaction under standard conditions?
In an electrochemical cell, if the standard cell potential ($E°_{cell}$) is negative, what does this indicate about the spontaneity of the reaction under standard conditions?
Given the reaction: $Zn + Cu^{2+}(aq)
ightarrow Zn^{2+}(aq) + Cu$, with $E°{Zn} = +0.76V$ and $E°{Cu} = +0.34V$, what is the cell representation for this reaction?
Given the reaction: $Zn + Cu^{2+}(aq) ightarrow Zn^{2+}(aq) + Cu$, with $E°{Zn} = +0.76V$ and $E°{Cu} = +0.34V$, what is the cell representation for this reaction?
For the reaction $2Al + 3Mg^{2+}(aq)
ightarrow 2Al^{3+}(aq) + 3Mg$, given $E°{Al} = +1.66V$ and $E°{Mg} = -2.36V$, and knowing that Magnesium is more reactive than Aluminum, what is the $E°_{cell}$ and is the reaction spontaneous?
For the reaction $2Al + 3Mg^{2+}(aq) ightarrow 2Al^{3+}(aq) + 3Mg$, given $E°{Al} = +1.66V$ and $E°{Mg} = -2.36V$, and knowing that Magnesium is more reactive than Aluminum, what is the $E°_{cell}$ and is the reaction spontaneous?
Given the half-cell reactions: $Zn
ightarrow Zn^{2+}(aq) + 2e^-$ $E° = +0.76V$ and $Cu^{2+}(aq) + 2e^-
ightarrow Cu$ $E° = +0.34V$, what is the standard cell potential ($E°_{cell}$) for the reaction $Zn + Cu^{2+}(aq)
ightarrow Zn^{2+}(aq) + Cu$?
Given the half-cell reactions: $Zn ightarrow Zn^{2+}(aq) + 2e^-$ $E° = +0.76V$ and $Cu^{2+}(aq) + 2e^- ightarrow Cu$ $E° = +0.34V$, what is the standard cell potential ($E°_{cell}$) for the reaction $Zn + Cu^{2+}(aq) ightarrow Zn^{2+}(aq) + Cu$?
What is the standard cell potential ($E^\circ$) for a reaction where $Al$ is oxidized to $Al^{3+}$ and $Mg^{2+}$ is reduced to $Mg$, given $E^\circ_{Al} = +1.66V$ and $E^\circ_{Mg} = -2.36V$?
What is the standard cell potential ($E^\circ$) for a reaction where $Al$ is oxidized to $Al^{3+}$ and $Mg^{2+}$ is reduced to $Mg$, given $E^\circ_{Al} = +1.66V$ and $E^\circ_{Mg} = -2.36V$?
Which of the following correctly describes the relationship between the reactivity of metals, their placement in an electrochemical cell, and the resulting cell's spontaneity?
Which of the following correctly describes the relationship between the reactivity of metals, their placement in an electrochemical cell, and the resulting cell's spontaneity?
Consider the overall reaction: $Zn(s) + Cu^{2+}(aq)
ightarrow Zn^{2+}(aq) + Cu(s)$. If the standard reduction potential for $Cu^{2+}$ to $Cu$ is $+0.34V$ and for $Zn^{2+}$ to $Zn$ is $-0.76V$, what is the standard cell potential ($E°_{cell}$), and is the reaction spontaneous under standard conditions?
Consider the overall reaction: $Zn(s) + Cu^{2+}(aq) ightarrow Zn^{2+}(aq) + Cu(s)$. If the standard reduction potential for $Cu^{2+}$ to $Cu$ is $+0.34V$ and for $Zn^{2+}$ to $Zn$ is $-0.76V$, what is the standard cell potential ($E°_{cell}$), and is the reaction spontaneous under standard conditions?
Given the standard reduction potentials, which of the following pairs of half-cells would produce a spontaneous reaction under standard conditions when combined in an electrochemical cell?
Given the standard reduction potentials, which of the following pairs of half-cells would produce a spontaneous reaction under standard conditions when combined in an electrochemical cell?
Which of the following descriptions accurately relates a cell's spontaneity to the relative activity of the metals used as electrodes in an electrochemical cell?
Which of the following descriptions accurately relates a cell's spontaneity to the relative activity of the metals used as electrodes in an electrochemical cell?
In a redox reaction, if a species is considered the oxidizing agent, what is its primary role?
In a redox reaction, if a species is considered the oxidizing agent, what is its primary role?
Which of the following statements accurately describes what occurs during reduction in a redox reaction?
Which of the following statements accurately describes what occurs during reduction in a redox reaction?
In $H_2SO_4$, what is the oxidation number of sulfur?
In $H_2SO_4$, what is the oxidation number of sulfur?
In the perchlorate ion ($ClO_4^−$), what is the oxidation number of chlorine (Cl)?
In the perchlorate ion ($ClO_4^−$), what is the oxidation number of chlorine (Cl)?
In the compound $NaHSO_4$, what is the oxidation number of sulfur?
In the compound $NaHSO_4$, what is the oxidation number of sulfur?
Given the unbalanced reaction: $Zn(s) + HNO_3(aq)
ightarrow Zn(NO_3)_2(aq) + N_2O(g) + H_2O(l)$, which element is reduced?
Given the unbalanced reaction: $Zn(s) + HNO_3(aq) ightarrow Zn(NO_3)_2(aq) + N_2O(g) + H_2O(l)$, which element is reduced?
Consider the unbalanced redox reaction: $MnO_4^−(aq) + I^−(aq)
ightarrow MnO_2(s) + I_2(s)$. Which species acts as the reducing agent?
Consider the unbalanced redox reaction: $MnO_4^−(aq) + I^−(aq) ightarrow MnO_2(s) + I_2(s)$. Which species acts as the reducing agent?
Which of the following statements is true regarding the change in oxidation number for a species that is oxidized in a redox reaction?
Which of the following statements is true regarding the change in oxidation number for a species that is oxidized in a redox reaction?
In the reaction $2Na(s) + H_2(g)
ightarrow 2NaH(s)$, what is the oxidation number of hydrogen in the product $NaH$?
In the reaction $2Na(s) + H_2(g) ightarrow 2NaH(s)$, what is the oxidation number of hydrogen in the product $NaH$?
In the reaction $4Fe + 3O_2 \rightarrow 2Fe_2O_3$, which species is the oxidizing agent, and what is being oxidized?
In the reaction $4Fe + 3O_2 \rightarrow 2Fe_2O_3$, which species is the oxidizing agent, and what is being oxidized?
Which of the following statements correctly describes the relationship between the electrode potential and the tendency of a substance to be reduced?
Which of the following statements correctly describes the relationship between the electrode potential and the tendency of a substance to be reduced?
In an electrochemical cell, what is the significance of a positive $E_{cell}$ value?
In an electrochemical cell, what is the significance of a positive $E_{cell}$ value?
What is the standard temperature and ion concentration to measure standard cell potential?
What is the standard temperature and ion concentration to measure standard cell potential?
In the reaction $Cl_2 + 2NaBr \rightarrow 2NaCl + Br_2$, identify which species is the reducing agent.
In the reaction $Cl_2 + 2NaBr \rightarrow 2NaCl + Br_2$, identify which species is the reducing agent.
Which of the following is a key difference between voltaic and electrolytic cells?
Which of the following is a key difference between voltaic and electrolytic cells?
In the electrochemical cell, what distinguishes the anode from the cathode?
In the electrochemical cell, what distinguishes the anode from the cathode?
In the general redox reaction $Fe + CuSO_4 \rightarrow FeSO_4 + Cu$, what changes do you observe in the oxidation numbers of iron (Fe) and copper (Cu), respectively?
In the general redox reaction $Fe + CuSO_4 \rightarrow FeSO_4 + Cu$, what changes do you observe in the oxidation numbers of iron (Fe) and copper (Cu), respectively?
Based on standard reduction potentials, which of the following metals would be the strongest reducing agent?
Based on standard reduction potentials, which of the following metals would be the strongest reducing agent?
In the reaction $2Na + Cl_2 \rightarrow 2NaCl$, identify which element is undergoing reduction by observing changes in oxidation numbers.
In the reaction $2Na + Cl_2 \rightarrow 2NaCl$, identify which element is undergoing reduction by observing changes in oxidation numbers.
For an electrochemical cell, which of the following scenarios will result in a spontaneous reaction?
For an electrochemical cell, which of the following scenarios will result in a spontaneous reaction?
Consider a voltaic cell with a standard cell potential (E°cell) of -0.50 V. Which statement is correct regarding the spontaneity of the reaction and the placement of metals?
Consider a voltaic cell with a standard cell potential (E°cell) of -0.50 V. Which statement is correct regarding the spontaneity of the reaction and the placement of metals?
Given the cell representation: $X/X^{2+} // Y^{2+}/Y$, and knowing that metal X is more reactive than metal Y, what can be inferred about the cell's spontaneity and standard potential?
Given the cell representation: $X/X^{2+} // Y^{2+}/Y$, and knowing that metal X is more reactive than metal Y, what can be inferred about the cell's spontaneity and standard potential?
Consider the reaction: $Mg(s) + 2Ag^+(aq) \rightarrow Mg^{2+}(aq) + 2Ag(s)$. The half-cell potentials are $E°{Mg^{2+}/Mg} = -2.37 V$ and $E°{Ag^+/Ag} = +0.80 V$. Calculate the standard cell potential (E°cell) for the reaction.
Consider the reaction: $Mg(s) + 2Ag^+(aq) \rightarrow Mg^{2+}(aq) + 2Ag(s)$. The half-cell potentials are $E°{Mg^{2+}/Mg} = -2.37 V$ and $E°{Ag^+/Ag} = +0.80 V$. Calculate the standard cell potential (E°cell) for the reaction.
You have a voltaic cell with the following half-reactions: $Zn(s) \rightarrow Zn^{2+}(aq) + 2e^-$ $E° = +0.76 V$ and $Fe^{2+}(aq) + 2e^- \rightarrow Fe(s)$ $E° = -0.44 V$. What is the standard cell potential ($E°_{cell}$) for this reaction?
You have a voltaic cell with the following half-reactions: $Zn(s) \rightarrow Zn^{2+}(aq) + 2e^-$ $E° = +0.76 V$ and $Fe^{2+}(aq) + 2e^- \rightarrow Fe(s)$ $E° = -0.44 V$. What is the standard cell potential ($E°_{cell}$) for this reaction?
Given the standard reduction potentials:
$Cu^{2+}(aq) + 2e^- \rightarrow Cu(s)$ $E° = +0.34 V$
$Ag^{+}(aq) + e^- \rightarrow Ag(s)$ $E° = +0.80 V$
If a galvanic cell is constructed using copper and silver, what is the standard cell potential?
Given the standard reduction potentials: $Cu^{2+}(aq) + 2e^- \rightarrow Cu(s)$ $E° = +0.34 V$ $Ag^{+}(aq) + e^- \rightarrow Ag(s)$ $E° = +0.80 V$ If a galvanic cell is constructed using copper and silver, what is the standard cell potential?
For the overall reaction: $2Ag^+ (aq) + Ni(s) \rightarrow 2Ag(s) + Ni^{2+}(aq)$, which of the following cell representations is correct?
For the overall reaction: $2Ag^+ (aq) + Ni(s) \rightarrow 2Ag(s) + Ni^{2+}(aq)$, which of the following cell representations is correct?
Consider the reaction: $3Mg(s) + 2Al^{3+}(aq) \rightarrow 3Mg^{2+}(aq) + 2Al(s)$. Given the half-reactions: $Mg \rightarrow Mg^{2+} + 2e^-$, $E° = 2.37 V$ and $Al \rightarrow Al^{3+} + 3e^-$, $E° = 1.66 V$. Calculate the standard cell potential and determine if the reaction is spontaneous.
Consider the reaction: $3Mg(s) + 2Al^{3+}(aq) \rightarrow 3Mg^{2+}(aq) + 2Al(s)$. Given the half-reactions: $Mg \rightarrow Mg^{2+} + 2e^-$, $E° = 2.37 V$ and $Al \rightarrow Al^{3+} + 3e^-$, $E° = 1.66 V$. Calculate the standard cell potential and determine if the reaction is spontaneous.
If a more reactive metal is placed at the cathode in an electrochemical cell, how does this affect the spontaneity of the cell reaction?
If a more reactive metal is placed at the cathode in an electrochemical cell, how does this affect the spontaneity of the cell reaction?
Which of the following is a correct representation of a redox reaction in an electrochemical cell, showing the oxidation half-cell on the left and the reduction half-cell on the right?
Which of the following is a correct representation of a redox reaction in an electrochemical cell, showing the oxidation half-cell on the left and the reduction half-cell on the right?
In a redox reaction, if a species is identified as the reducing agent, what is its primary role?
In a redox reaction, if a species is identified as the reducing agent, what is its primary role?
Which of the following statements accurately describes the fundamental relationship between oxidation and reduction in a redox reaction?
Which of the following statements accurately describes the fundamental relationship between oxidation and reduction in a redox reaction?
When determining the oxidation number of elements in a compound, which rule takes precedence if multiple rules appear to conflict?
When determining the oxidation number of elements in a compound, which rule takes precedence if multiple rules appear to conflict?
What is the oxidation number of an individual atom in a substance consisting of only one element?
What is the oxidation number of an individual atom in a substance consisting of only one element?
In $KH$, what is the oxidation number of hydrogen?
In $KH$, what is the oxidation number of hydrogen?
Consider the unbalanced reaction: $Zn(s) + HNO_3(aq)
ightarrow Zn(NO_3)_2(aq) + N_2O(g) + H_2O(l)$. Which species is the oxidizing agent?
Consider the unbalanced reaction: $Zn(s) + HNO_3(aq) ightarrow Zn(NO_3)_2(aq) + N_2O(g) + H_2O(l)$. Which species is the oxidizing agent?
In the reaction $2H_2S(g) + 3O_2(g)
ightarrow 2SO_2(g) + 2H_2O(g)$, which substance is oxidized?
In the reaction $2H_2S(g) + 3O_2(g) ightarrow 2SO_2(g) + 2H_2O(g)$, which substance is oxidized?
What must occur for a chemical species to be identified as undergoing reduction in a redox reaction?
What must occur for a chemical species to be identified as undergoing reduction in a redox reaction?
Given the incomplete redox reaction: $MnO_4^−(aq)
ightarrow Mn^{2+}(aq)$. What is the change in oxidation number of manganese?
Given the incomplete redox reaction: $MnO_4^−(aq) ightarrow Mn^{2+}(aq)$. What is the change in oxidation number of manganese?
In the reaction $4Fe + 3O_2 \rightarrow 2Fe_2O_3$, what is the change in the oxidation number of iron (Fe)?
In the reaction $4Fe + 3O_2 \rightarrow 2Fe_2O_3$, what is the change in the oxidation number of iron (Fe)?
In an electrochemical cell, which of the following is true regarding the electrode where oxidation occurs?
In an electrochemical cell, which of the following is true regarding the electrode where oxidation occurs?
How does a substance with a high positive reduction potential behave in a redox reaction?
How does a substance with a high positive reduction potential behave in a redox reaction?
Which of the following correctly relates the standard cell potential ($E^\circ$) to the spontaneity of a redox reaction at standard conditions?
Which of the following correctly relates the standard cell potential ($E^\circ$) to the spontaneity of a redox reaction at standard conditions?
What is the role of a metal or semiconductor electrode in an electrochemical reaction?
What is the role of a metal or semiconductor electrode in an electrochemical reaction?
Consider the reaction: $Cl_2 + 2NaBr \rightarrow 2NaCl + Br_2$. Which species is the oxidizing agent?
Consider the reaction: $Cl_2 + 2NaBr \rightarrow 2NaCl + Br_2$. Which species is the oxidizing agent?
How would increasing the temperature affect the cell potential in an electrochemical reaction? Assume nonstandard conditions are present.
How would increasing the temperature affect the cell potential in an electrochemical reaction? Assume nonstandard conditions are present.
In the reaction: $Pb(NO_3)_2 + 2KI \rightarrow PbI_2 + 2KNO_3$, which element undergoes neither oxidation nor reduction?
In the reaction: $Pb(NO_3)_2 + 2KI \rightarrow PbI_2 + 2KNO_3$, which element undergoes neither oxidation nor reduction?
Which of the following defines electrochemistry most accurately?
Which of the following defines electrochemistry most accurately?
What is the purpose of using a reference cell in electrochemistry?
What is the purpose of using a reference cell in electrochemistry?
Which of the following conditions will result in a spontaneous electrochemical reaction in a voltaic cell?
Which of the following conditions will result in a spontaneous electrochemical reaction in a voltaic cell?
Consider the reaction: $Ni^{2+}(aq) + Zn(s) \rightarrow Ni(s) + Zn^{2+}(aq)$. Given that zinc is more reactive than nickel, what can be predicted about the spontaneity of the reaction and the standard cell potential?
Consider the reaction: $Ni^{2+}(aq) + Zn(s) \rightarrow Ni(s) + Zn^{2+}(aq)$. Given that zinc is more reactive than nickel, what can be predicted about the spontaneity of the reaction and the standard cell potential?
Which of the following statements is correct regarding the relationship between the standard cell potential ($E^\circ$) and the spontaneity of an electrochemical reaction?
Which of the following statements is correct regarding the relationship between the standard cell potential ($E^\circ$) and the spontaneity of an electrochemical reaction?
Given the cell representation: $Ag/Ag^+ // Fe^{2+}/Fe$, and knowing that silver is less reactive than iron, what can be inferred about the cell's standard potential ($E^\circ$) and spontaneity?
Given the cell representation: $Ag/Ag^+ // Fe^{2+}/Fe$, and knowing that silver is less reactive than iron, what can be inferred about the cell's standard potential ($E^\circ$) and spontaneity?
For the reaction $2Al(s) + 3Cu^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Cu(s)$, if the standard reduction potential of $Al^{3+}$ to $Al$ is -1.66 V and $Cu^{2+}$ to $Cu$ is +0.34 V, calculate the standard cell potential ($E^\circ_{cell}$) and determine the spontaneity.
For the reaction $2Al(s) + 3Cu^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Cu(s)$, if the standard reduction potential of $Al^{3+}$ to $Al$ is -1.66 V and $Cu^{2+}$ to $Cu$ is +0.34 V, calculate the standard cell potential ($E^\circ_{cell}$) and determine the spontaneity.
Given the following half-reactions and their standard reduction potentials:
$Zn^{2+}(aq) + 2e^- \rightarrow Zn(s)$ $E^\circ$ = -0.76 V
$Fe^{2+}(aq) + 2e^- \rightarrow Fe(s)$ $E^\circ$ = -0.44 V
You construct a galvanic cell using these half-reactions. Assuming that Zinc is oxidized, what is the standard cell potential ($E^\circ_{cell}$)?
Given the following half-reactions and their standard reduction potentials: $Zn^{2+}(aq) + 2e^- \rightarrow Zn(s)$ $E^\circ$ = -0.76 V $Fe^{2+}(aq) + 2e^- \rightarrow Fe(s)$ $E^\circ$ = -0.44 V You construct a galvanic cell using these half-reactions. Assuming that Zinc is oxidized, what is the standard cell potential ($E^\circ_{cell}$)?
Consider the reaction: $2Al(s) + 3Mg^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Mg(s)$. Knowing that $E^\circ_{Al} = -1.66V$ and $E^\circ_{Mg} = -2.36V$, what is the $E^\circ_{cell}$?
Consider the reaction: $2Al(s) + 3Mg^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Mg(s)$. Knowing that $E^\circ_{Al} = -1.66V$ and $E^\circ_{Mg} = -2.36V$, what is the $E^\circ_{cell}$?
Which of the following species would be considered the reducing agent in the reaction: $2Na(s) + Cl_2(g) \rightarrow 2NaCl(s)$?
Which of the following species would be considered the reducing agent in the reaction: $2Na(s) + Cl_2(g) \rightarrow 2NaCl(s)$?
Using the rules for assigning oxidation numbers, what is the oxidation number of potassium (K) in $K_2O$?
Using the rules for assigning oxidation numbers, what is the oxidation number of potassium (K) in $K_2O$?
In the following unbalanced redox reaction: $MnO_4^-(aq) + I^-(aq)
ightarrow MnO_2(s) + I_2(s)$, which species is the oxidizing agent?
In the following unbalanced redox reaction: $MnO_4^-(aq) + I^-(aq) ightarrow MnO_2(s) + I_2(s)$, which species is the oxidizing agent?
Consider the reaction: $Zn(s) + 2Ag^+(aq)
ightarrow Zn^{2+}(aq) + 2Ag(s)$. Which species undergoes reduction?
Consider the reaction: $Zn(s) + 2Ag^+(aq) ightarrow Zn^{2+}(aq) + 2Ag(s)$. Which species undergoes reduction?
Which of the following represents a balanced half-reaction for the oxidation of $Fe^{2+}$ to $Fe^{3+}$?
Which of the following represents a balanced half-reaction for the oxidation of $Fe^{2+}$ to $Fe^{3+}$?
During a redox reaction, the species that causes another species to be oxidized while being reduced itself is referred to as what?
During a redox reaction, the species that causes another species to be oxidized while being reduced itself is referred to as what?
What changes in oxidation number signifies that a species has been oxidized?
What changes in oxidation number signifies that a species has been oxidized?
In an electrolytic cell, which of the following statements accurately describes the processes occurring at each electrode?
In an electrolytic cell, which of the following statements accurately describes the processes occurring at each electrode?
In the reaction $CuO(s) + H_2(g)
ightarrow Cu(s) + H_2O(l)$, which species is acting as the oxidizing agent.
In the reaction $CuO(s) + H_2(g) ightarrow Cu(s) + H_2O(l)$, which species is acting as the oxidizing agent.
Based on standard reduction potentials ($E°$), how can one effectively determine the strength of an oxidizing agent?
Based on standard reduction potentials ($E°$), how can one effectively determine the strength of an oxidizing agent?
Consider the standard cell potential ($E°$) values. Which statement accurately describes their utility in evaluating redox reactions?
Consider the standard cell potential ($E°$) values. Which statement accurately describes their utility in evaluating redox reactions?
Which of the following conditions is essential for measuring the standard electrode potential of a half-cell?
Which of the following conditions is essential for measuring the standard electrode potential of a half-cell?
In the balanced redox reaction $2Na + Cl_2 \rightarrow 2NaCl$, what changes occur to the oxidation numbers of sodium (Na) and chlorine ($Cl_2$) as they react?
In the balanced redox reaction $2Na + Cl_2 \rightarrow 2NaCl$, what changes occur to the oxidation numbers of sodium (Na) and chlorine ($Cl_2$) as they react?
What is the primary distinction between voltaic and electrolytic cells?
What is the primary distinction between voltaic and electrolytic cells?
Considering the electrochemical series, which of the following statements accurately predicts reactivity and spontaneity in electrochemical cells?
Considering the electrochemical series, which of the following statements accurately predicts reactivity and spontaneity in electrochemical cells?
In the reaction $Fe + CuSO_4 \rightarrow FeSO_4 + Cu$, how can we correctly describe the role of iron (Fe)?
In the reaction $Fe + CuSO_4 \rightarrow FeSO_4 + Cu$, how can we correctly describe the role of iron (Fe)?
If a substance is described as a strong reducing agent, which of the following properties would it likely possess?
If a substance is described as a strong reducing agent, which of the following properties would it likely possess?
Which of the following correctly describes the relationship between a metal's reactivity, its placement in an electrochemical cell, and the cell's spontaneity?
Which of the following correctly describes the relationship between a metal's reactivity, its placement in an electrochemical cell, and the cell's spontaneity?
Consider an electrochemical cell where zinc (Zn) is the anode and copper (Cu) is the cathode. Given that zinc is more reactive than copper, what can be predicted about the cell potential ($E_{cell}$) and the reaction's spontaneity?
Consider an electrochemical cell where zinc (Zn) is the anode and copper (Cu) is the cathode. Given that zinc is more reactive than copper, what can be predicted about the cell potential ($E_{cell}$) and the reaction's spontaneity?
In an electrochemical cell with the overall reaction $2Al + 3Mg^{2+}(aq)
ightarrow 2Al^{3+}(aq) + 3Mg$, it is found that the cell potential is negative. Based on this information, what can be concluded?
In an electrochemical cell with the overall reaction $2Al + 3Mg^{2+}(aq) ightarrow 2Al^{3+}(aq) + 3Mg$, it is found that the cell potential is negative. Based on this information, what can be concluded?
Which of the following cell representations accurately describes an electrochemical cell with the overall reaction $Zn + Cu^{2+}(aq)
ightarrow Zn^{2+}(aq) + Cu$?
Which of the following cell representations accurately describes an electrochemical cell with the overall reaction $Zn + Cu^{2+}(aq) ightarrow Zn^{2+}(aq) + Cu$?
Given the half-reactions: $Zn
ightarrow Zn^{2+}(aq) + 2e^-$ $E° = +0.76V$ and $Cu^{2+}(aq) + 2e^-
ightarrow Cu$ $E° = +0.34V$, what is the standard cell potential ($E°_{cell}$) for the reaction $Zn + Cu^{2+}(aq)
ightarrow Zn^{2+}(aq) + Cu$?
Given the half-reactions: $Zn ightarrow Zn^{2+}(aq) + 2e^-$ $E° = +0.76V$ and $Cu^{2+}(aq) + 2e^- ightarrow Cu$ $E° = +0.34V$, what is the standard cell potential ($E°_{cell}$) for the reaction $Zn + Cu^{2+}(aq) ightarrow Zn^{2+}(aq) + Cu$?
Consider an electrochemical cell with the following standard reduction potentials: $Ag^+ + e^-
ightarrow Ag$ $E° = +0.80V$ and $Fe^{2+} + 2e^-
ightarrow Fe$ $E° = -0.44V$. What is the standard cell potential if iron is oxidized to $Fe^{2+}$ and silver ions are reduced to silver metal?
Consider an electrochemical cell with the following standard reduction potentials: $Ag^+ + e^- ightarrow Ag$ $E° = +0.80V$ and $Fe^{2+} + 2e^- ightarrow Fe$ $E° = -0.44V$. What is the standard cell potential if iron is oxidized to $Fe^{2+}$ and silver ions are reduced to silver metal?
In the reaction $2Al(s) + 3Mg^{2+}(aq)
ightarrow 2Al^{3+}(aq) + 3Mg(s)$, given that $E°{Al} = +1.66V$ and $E°{Mg} = -2.36V$, what is the $E°_{cell}$ and is the reaction spontaneous?
In the reaction $2Al(s) + 3Mg^{2+}(aq) ightarrow 2Al^{3+}(aq) + 3Mg(s)$, given that $E°{Al} = +1.66V$ and $E°{Mg} = -2.36V$, what is the $E°_{cell}$ and is the reaction spontaneous?
In a redox reaction, if a species is described as the 'reducing agent', what role is it fulfilling?
In a redox reaction, if a species is described as the 'reducing agent', what role is it fulfilling?
Which of the following statements correctly describes the oxidation number of an element in a compound?
Which of the following statements correctly describes the oxidation number of an element in a compound?
In the compound $H_2PO_4^-$, what is the oxidation number of phosphorus (P)?
In the compound $H_2PO_4^-$, what is the oxidation number of phosphorus (P)?
In which of the following scenarios would hydrogen be assigned an oxidation number of -1?
In which of the following scenarios would hydrogen be assigned an oxidation number of -1?
Consider the unbalanced reaction: $MnO_4^−(aq) + I^−(aq)
ightarrow Mn^{2+}(aq) + I_2(s)$. Which species is oxidized in this reaction?
Consider the unbalanced reaction: $MnO_4^−(aq) + I^−(aq) ightarrow Mn^{2+}(aq) + I_2(s)$. Which species is oxidized in this reaction?
In the reaction: $2H_2S(g) + SO_2(g)
ightarrow 3S(s) + 2H_2O(l)$, which species functions as the oxidizing agent?
In the reaction: $2H_2S(g) + SO_2(g) ightarrow 3S(s) + 2H_2O(l)$, which species functions as the oxidizing agent?
Which of the following statements is correct regarding oxidation numbers in the compound $H_2SO_4$?
Which of the following statements is correct regarding oxidation numbers in the compound $H_2SO_4$?
In the reaction $Pb(NO_3)_2 + 2KI
ightarrow PbI_2 + 2KNO_3$, which species neither oxidizes nor reduces?
In the reaction $Pb(NO_3)_2 + 2KI ightarrow PbI_2 + 2KNO_3$, which species neither oxidizes nor reduces?
What is the standard condition for measuring the electromotive force (emf) of a cell?
What is the standard condition for measuring the electromotive force (emf) of a cell?
If a substance has a high positive oxidation potential, what does this suggest about its properties?
If a substance has a high positive oxidation potential, what does this suggest about its properties?
Which of the following statements accurately describes the relationship between the cell potential ($E_{cell}$) and the spontaneity of a redox reaction?
Which of the following statements accurately describes the relationship between the cell potential ($E_{cell}$) and the spontaneity of a redox reaction?
In an electrochemical cell, what is the role of the anode and the cathode?
In an electrochemical cell, what is the role of the anode and the cathode?
If a voltaic cell is set up with a zinc electrode in a $Zn^{2+}$ solution and a copper electrode in a $Cu^{2+}$ solution, which metal will act as the anode, given that zinc is more reactive than copper?
If a voltaic cell is set up with a zinc electrode in a $Zn^{2+}$ solution and a copper electrode in a $Cu^{2+}$ solution, which metal will act as the anode, given that zinc is more reactive than copper?
In the redox reaction $Cl_2 + 2NaBr
ightarrow 2NaCl + Br_2$, which species is the oxidizing agent?
In the redox reaction $Cl_2 + 2NaBr ightarrow 2NaCl + Br_2$, which species is the oxidizing agent?
During a redox reaction, if a substance's oxidation number increases, which process has occurred?
During a redox reaction, if a substance's oxidation number increases, which process has occurred?
How could you use the provided information to evaluate redox reactions?
How could you use the provided information to evaluate redox reactions?
In an electrochemical cell, what condition typically results in a spontaneous reaction?
In an electrochemical cell, what condition typically results in a spontaneous reaction?
Which of the following statements accurately describes how the relative reactivity of metals influences the spontaneity of a reaction in an electrochemical cell?
Which of the following statements accurately describes how the relative reactivity of metals influences the spontaneity of a reaction in an electrochemical cell?
Consider the reaction $Ni^{2+}(aq) + Zn(s)
ightarrow Ni(s) + Zn^{2+}(aq)$. Given that zinc is more reactive than nickel, what can be predicted about the spontaneity of this reaction and the sign of $E°_{cell}$?
Consider the reaction $Ni^{2+}(aq) + Zn(s) ightarrow Ni(s) + Zn^{2+}(aq)$. Given that zinc is more reactive than nickel, what can be predicted about the spontaneity of this reaction and the sign of $E°_{cell}$?
Given the half-reactions: $A^+ + e^-
ightarrow A$ $E° = +0.80V$ and $B^{2+} + 2e^-
ightarrow B$ $E° = -0.40V$. If these half-cells are combined to form a voltaic cell, which metal will act as the anode, and what is the $E°_{cell}$?
Given the half-reactions: $A^+ + e^- ightarrow A$ $E° = +0.80V$ and $B^{2+} + 2e^- ightarrow B$ $E° = -0.40V$. If these half-cells are combined to form a voltaic cell, which metal will act as the anode, and what is the $E°_{cell}$?
For the cell representation $M | M^{2+} || N^{2+} | N$, and given that metal M is more reactive than metal N, what are the expected signs of $\Delta G$ and $E°_{cell}$ for this electrochemical cell?
For the cell representation $M | M^{2+} || N^{2+} | N$, and given that metal M is more reactive than metal N, what are the expected signs of $\Delta G$ and $E°_{cell}$ for this electrochemical cell?
In the reaction $2Al(s) + 3Cu^{2+}(aq)
ightarrow 2Al^{3+}(aq) + 3Cu(s)$, where $E°{Al^{3+}/Al} = -1.66 V$ and $E°{Cu^{2+}/Cu} = +0.34 V$, calculate the standard cell potential ($E°_{cell}$) and determine whether the reaction is spontaneous.
In the reaction $2Al(s) + 3Cu^{2+}(aq) ightarrow 2Al^{3+}(aq) + 3Cu(s)$, where $E°{Al^{3+}/Al} = -1.66 V$ and $E°{Cu^{2+}/Cu} = +0.34 V$, calculate the standard cell potential ($E°_{cell}$) and determine whether the reaction is spontaneous.
Using the standard reduction potentials, determine which of the following reactions is spontaneous under standard conditions:
I. $Cu^{2+}(aq) + 2Ag(s)
ightarrow Cu(s) + 2Ag^+(aq)$.
II. $2Ag^+(aq) + Cu(s)
ightarrow 2Ag(s) + Cu^{2+}(aq)$.
(Given: $E°{Cu^{2+}/Cu} = +0.34 V$, $E°{Ag^{+}/Ag} = +0.80 V$)
Using the standard reduction potentials, determine which of the following reactions is spontaneous under standard conditions:
I. $Cu^{2+}(aq) + 2Ag(s) ightarrow Cu(s) + 2Ag^+(aq)$. II. $2Ag^+(aq) + Cu(s) ightarrow 2Ag(s) + Cu^{2+}(aq)$.
(Given: $E°{Cu^{2+}/Cu} = +0.34 V$, $E°{Ag^{+}/Ag} = +0.80 V$)
What is the overall cell reaction for the cell representation $Zn | Zn^{2+} || Ag^+ | Ag$?
What is the overall cell reaction for the cell representation $Zn | Zn^{2+} || Ag^+ | Ag$?
Given the half-reactions: $Fe^{2+}(aq) + 2e^-
ightarrow Fe(s)$ $E° = -0.44V$ and $Cd^{2+}(aq) + 2e^-
ightarrow Cd(s)$ $E° = -0.40V$. If a voltaic cell is constructed using these half-cells, which metal will be the cathode, and what will the $E°_{cell}$ be?
Given the half-reactions: $Fe^{2+}(aq) + 2e^- ightarrow Fe(s)$ $E° = -0.44V$ and $Cd^{2+}(aq) + 2e^- ightarrow Cd(s)$ $E° = -0.40V$. If a voltaic cell is constructed using these half-cells, which metal will be the cathode, and what will the $E°_{cell}$ be?
If a more reactive metal is used as the cathode in an electrochemical cell, what does this indicate about the cell potential (E) and the spontaneity of the reaction?
If a more reactive metal is used as the cathode in an electrochemical cell, what does this indicate about the cell potential (E) and the spontaneity of the reaction?
In a redox reaction, if a substance is oxidized, what happens to its oxidation number and what role does it play in the reaction?
In a redox reaction, if a substance is oxidized, what happens to its oxidation number and what role does it play in the reaction?
Which of the following statements correctly describes the behaviour of oxidizing and reducing agents in a redox reaction?
Which of the following statements correctly describes the behaviour of oxidizing and reducing agents in a redox reaction?
What is the oxidation number of an element when it is in its elemental or diatomic form?
What is the oxidation number of an element when it is in its elemental or diatomic form?
Determine the oxidation number of sulfur (S) in sulfuric acid ($H_2SO_4$).
Determine the oxidation number of sulfur (S) in sulfuric acid ($H_2SO_4$).
In the unbalanced equation: $MnO_4^-(aq) + I^-(aq) \rightarrow Mn^{2+}(aq) + I_2(s)$, which species undergoes oxidation?
In the unbalanced equation: $MnO_4^-(aq) + I^-(aq) \rightarrow Mn^{2+}(aq) + I_2(s)$, which species undergoes oxidation?
Given the following incomplete half-reaction: $Cr_2O_7^{2-}(aq) \rightarrow 2Cr^{3+}(aq)$. What is the oxidation number change for chromium (Cr)?
Given the following incomplete half-reaction: $Cr_2O_7^{2-}(aq) \rightarrow 2Cr^{3+}(aq)$. What is the oxidation number change for chromium (Cr)?
Considering the standard conditions for measuring electrode potentials $(25^\circ C, 1 , atm, 1 , M)$, what is the significance of these standardized conditions?
Considering the standard conditions for measuring electrode potentials $(25^\circ C, 1 , atm, 1 , M)$, what is the significance of these standardized conditions?
In an electrolytic cell, why is an external power source required?
In an electrolytic cell, why is an external power source required?
How does the magnitude of the cell potential ($E_{cell}$) relate to the amount of work that can be done by an electrochemical cell?
How does the magnitude of the cell potential ($E_{cell}$) relate to the amount of work that can be done by an electrochemical cell?
For a voltaic cell based on the reaction $Sn^{2+}(aq) + Fe(s) \rightarrow Sn(s) + Fe^{2+}(aq)$, what conditions would indicate a spontaneous reaction based on the relative reactivity of the metals?
For a voltaic cell based on the reaction $Sn^{2+}(aq) + Fe(s) \rightarrow Sn(s) + Fe^{2+}(aq)$, what conditions would indicate a spontaneous reaction based on the relative reactivity of the metals?
Consider an electrochemical cell with the overall reaction: $2Ag^+(aq) + Zn(s) \rightarrow 2Ag(s) + Zn^{2+}(aq)$. If silver is known to be less reactive than zinc, what can be predicted about the spontaneity of the reaction as written and the sign of $E_{cell}$?
Consider an electrochemical cell with the overall reaction: $2Ag^+(aq) + Zn(s) \rightarrow 2Ag(s) + Zn^{2+}(aq)$. If silver is known to be less reactive than zinc, what can be predicted about the spontaneity of the reaction as written and the sign of $E_{cell}$?
Given the half-reactions: $Cu^{2+}(aq) + 2e^- \rightarrow Cu(s)$ $E^\circ = +0.34V$ and $Zn^{2+}(aq) + 2e^- \rightarrow Zn(s)$ $E^\circ = -0.76V$. If a voltaic cell is constructed using these half-reactions, what is the standard cell potential ($E^\circ_{cell}$) for the spontaneous reaction?
Given the half-reactions: $Cu^{2+}(aq) + 2e^- \rightarrow Cu(s)$ $E^\circ = +0.34V$ and $Zn^{2+}(aq) + 2e^- \rightarrow Zn(s)$ $E^\circ = -0.76V$. If a voltaic cell is constructed using these half-reactions, what is the standard cell potential ($E^\circ_{cell}$) for the spontaneous reaction?
Consider the reaction: $Ni(s) + 2Ag^+(aq) \rightarrow Ni^{2+}(aq) + 2Ag(s)$. Given that the standard reduction potential for $Ag^+/Ag$ is +0.80V and for $Ni^{2+}/Ni$ is -0.25V, calculate $E^\circ_{cell}$ and determine whether the reaction is spontaneous under standard conditions.
Consider the reaction: $Ni(s) + 2Ag^+(aq) \rightarrow Ni^{2+}(aq) + 2Ag(s)$. Given that the standard reduction potential for $Ag^+/Ag$ is +0.80V and for $Ni^{2+}/Ni$ is -0.25V, calculate $E^\circ_{cell}$ and determine whether the reaction is spontaneous under standard conditions.
Which of the following cell representations correctly describes the redox reaction: $Cd(s) + 2H^+(aq) \rightarrow Cd^{2+}(aq) + H_2(g)$?
Which of the following cell representations correctly describes the redox reaction: $Cd(s) + 2H^+(aq) \rightarrow Cd^{2+}(aq) + H_2(g)$?
Consider a voltaic cell using the half-reactions:
$Zn(s) \rightarrow Zn^{2+}(aq) + 2e^-$ and $Ag^+(aq) + e^- \rightarrow Ag(s)$. What adjustments must be made when calculating the overall $E^\circ_{cell}$?
Consider a voltaic cell using the half-reactions: $Zn(s) \rightarrow Zn^{2+}(aq) + 2e^-$ and $Ag^+(aq) + e^- \rightarrow Ag(s)$. What adjustments must be made when calculating the overall $E^\circ_{cell}$?
For the reaction $2Al(s) + 3Cu^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Cu(s)$, the half-reactions are $Al \rightarrow Al^{3+} + 3e^-$ and $Cu^{2+} + 2e^- \rightarrow Cu$. Which of the following statements correctly describes the electron transfer process?
For the reaction $2Al(s) + 3Cu^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Cu(s)$, the half-reactions are $Al \rightarrow Al^{3+} + 3e^-$ and $Cu^{2+} + 2e^- \rightarrow Cu$. Which of the following statements correctly describes the electron transfer process?
Given the following solutions: one containing $Zn^{2+}$ ions and another containing $Ag^+$ ions, and knowing that zinc is more reactive than silver, how can a spontaneous redox reaction be created using these materials?
Given the following solutions: one containing $Zn^{2+}$ ions and another containing $Ag^+$ ions, and knowing that zinc is more reactive than silver, how can a spontaneous redox reaction be created using these materials?
Two half-cells, one with $Fe^{2+}/Fe$ ($E^\circ = -0.44$ V) and another with $Cu^{2+}/Cu$ ($E^\circ = +0.34$ V), are used to construct a voltaic cell under standard conditions. Which metal will act as the anode, and what will be the cell potential?
Two half-cells, one with $Fe^{2+}/Fe$ ($E^\circ = -0.44$ V) and another with $Cu^{2+}/Cu$ ($E^\circ = +0.34$ V), are used to construct a voltaic cell under standard conditions. Which metal will act as the anode, and what will be the cell potential?
What is the purpose of using Pt as an electrode in a half-cell such as $Pt(s) | H_2(g) | H^+(aq)$?
What is the purpose of using Pt as an electrode in a half-cell such as $Pt(s) | H_2(g) | H^+(aq)$?
In a redox reaction, if a species is described as the 'reducing agent', what role does it play?
In a redox reaction, if a species is described as the 'reducing agent', what role does it play?
If an atom's oxidation number increases during a chemical reaction, which of the following processes has occurred?
If an atom's oxidation number increases during a chemical reaction, which of the following processes has occurred?
Considering the rules for assigning oxidation numbers, what is the oxidation number of potassium (K) in potassium oxide ($K_2O$)?
Considering the rules for assigning oxidation numbers, what is the oxidation number of potassium (K) in potassium oxide ($K_2O$)?
What is the oxidation number of hydrogen when it is combined with metals?
What is the oxidation number of hydrogen when it is combined with metals?
In an electrochemical cell, if a less reactive metal is spontaneously oxidizing, where is it likely located?
In an electrochemical cell, if a less reactive metal is spontaneously oxidizing, where is it likely located?
For the cell reaction $Zn + Cu^{2+}(aq)
ightarrow Zn^{2+}(aq) + Cu$, what changes would likely cause the reaction to become non-spontaneous?
For the cell reaction $Zn + Cu^{2+}(aq) ightarrow Zn^{2+}(aq) + Cu$, what changes would likely cause the reaction to become non-spontaneous?
Given the half-reactions and their standard potentials, $Ag^+ + e^-
ightarrow Ag$ ($E = +0.80V$) and $Fe^{2+} + 2e^-
ightarrow Fe$ ($E = -0.44V$), which overall reaction is spontaneous under standard conditions?
Given the half-reactions and their standard potentials, $Ag^+ + e^- ightarrow Ag$ ($E = +0.80V$) and $Fe^{2+} + 2e^- ightarrow Fe$ ($E = -0.44V$), which overall reaction is spontaneous under standard conditions?
In the electrolytic process of water ($H_2O$) splitting into hydrogen ($H_2$) and oxygen ($O_2$), what minimum voltage is required, given the half-reactions $2H^+ + 2e^-
ightarrow H_2$ ($E = 0.00V$) and $O_2 + 4H^+ + 4e^-
ightarrow 2H_2O$ ($E = +1.23V$)?
In the electrolytic process of water ($H_2O$) splitting into hydrogen ($H_2$) and oxygen ($O_2$), what minimum voltage is required, given the half-reactions $2H^+ + 2e^- ightarrow H_2$ ($E = 0.00V$) and $O_2 + 4H^+ + 4e^- ightarrow 2H_2O$ ($E = +1.23V$)?
For the cell representation $Al / Al^{3+} // Ag^+ / Ag$, what is the overall balanced reaction, and which electrode is negative when the cell operates spontaneously?
For the cell representation $Al / Al^{3+} // Ag^+ / Ag$, what is the overall balanced reaction, and which electrode is negative when the cell operates spontaneously?
Consider the reaction: $Pb(NO_3)_2 + 2KI
ightarrow PbI_2 + 2KNO_3$. Which species undergoes a change in oxidation number?
Consider the reaction: $Pb(NO_3)_2 + 2KI ightarrow PbI_2 + 2KNO_3$. Which species undergoes a change in oxidation number?
Which of the following statements is true regarding the anode in both voltaic and electrolytic cells?
Which of the following statements is true regarding the anode in both voltaic and electrolytic cells?
What is the purpose of using a platinum electrode ($Pt$) in certain electrochemical cells?
What is the purpose of using a platinum electrode ($Pt$) in certain electrochemical cells?
Under what circumstances would a voltaic cell have a cell potential of zero?
Under what circumstances would a voltaic cell have a cell potential of zero?
In an electrochemical cell, what happens to the cell potential ($E_{cell}$) if the temperature is significantly increased above standard conditions (25°C)?
In an electrochemical cell, what happens to the cell potential ($E_{cell}$) if the temperature is significantly increased above standard conditions (25°C)?
Which of the following best describes the role of a substance with a high positive oxidation potential?
Which of the following best describes the role of a substance with a high positive oxidation potential?
In the context of electrochemistry, what is the relationship between the Gibbs free energy change ($\Delta G$) and the cell potential ($E_{cell}$)?
In the context of electrochemistry, what is the relationship between the Gibbs free energy change ($\Delta G$) and the cell potential ($E_{cell}$)?
If the standard reduction potential for $Zn^{2+}(aq) + 2e^-
ightarrow Zn(s)$ is -0.76 V, and for $Cu^{2+}(aq) + 2e^-
ightarrow Cu(s)$ is +0.34 V, what conditions would be required to make the reduction of $Zn^{2+}$ spontaneous when coupled with the oxidation of $Cu(s)$?
If the standard reduction potential for $Zn^{2+}(aq) + 2e^- ightarrow Zn(s)$ is -0.76 V, and for $Cu^{2+}(aq) + 2e^- ightarrow Cu(s)$ is +0.34 V, what conditions would be required to make the reduction of $Zn^{2+}$ spontaneous when coupled with the oxidation of $Cu(s)$?
For a voltaic cell based on the reaction: $Zn(s) + Cu^{2+}(aq)
ightarrow Zn^{2+}(aq) + Cu(s)$, how is electrical energy produced?
For a voltaic cell based on the reaction: $Zn(s) + Cu^{2+}(aq) ightarrow Zn^{2+}(aq) + Cu(s)$, how is electrical energy produced?
Which of the following factors would likely increase the voltage (electromotive force) of a voltaic cell?
Which of the following factors would likely increase the voltage (electromotive force) of a voltaic cell?
For the reaction $2Al(s) + 3Cu^{2+}(aq)
ightarrow 2Al^{3+}(aq) + 3Cu(s)$, how does an increase in the concentration of $Al^{3+}(aq)$ affect the cell potential, and what law governs this relationship?
For the reaction $2Al(s) + 3Cu^{2+}(aq) ightarrow 2Al^{3+}(aq) + 3Cu(s)$, how does an increase in the concentration of $Al^{3+}(aq)$ affect the cell potential, and what law governs this relationship?
In the electrochemical reaction $Cl_2 + 2NaBr
ightarrow 2NaCl + Br_2$, which species is the oxidizing agent, and what happens to its oxidation number?
In the electrochemical reaction $Cl_2 + 2NaBr ightarrow 2NaCl + Br_2$, which species is the oxidizing agent, and what happens to its oxidation number?
Given the standard reduction potentials: $Ag^+(aq) + e^-
ightarrow Ag(s)$ $E° = +0.80V$ and $Zn^{2+}(aq) + 2e^-
ightarrow Zn(s)$ $E° = -0.76V$. Which metal, silver or zinc, will act as the anode in a voltaic cell, and what is the overall standard cell potential?
Given the standard reduction potentials: $Ag^+(aq) + e^- ightarrow Ag(s)$ $E° = +0.80V$ and $Zn^{2+}(aq) + 2e^- ightarrow Zn(s)$ $E° = -0.76V$. Which metal, silver or zinc, will act as the anode in a voltaic cell, and what is the overall standard cell potential?
Consider a scenario where a non-spontaneous redox reaction is forced to occur by applying an external electric current. Which type of electrochemical cell is being utilized, and at which electrode does reduction take place?
Consider a scenario where a non-spontaneous redox reaction is forced to occur by applying an external electric current. Which type of electrochemical cell is being utilized, and at which electrode does reduction take place?
Which of the following options correctly describes the change in oxidation number for a species that is undergoing reduction?
Which of the following options correctly describes the change in oxidation number for a species that is undergoing reduction?
In $NaHSO_4$, what is the oxidation number of sulfur (S)?
In $NaHSO_4$, what is the oxidation number of sulfur (S)?
Which of the following compounds contains oxygen with an oxidation number that is NOT -2?
Which of the following compounds contains oxygen with an oxidation number that is NOT -2?
In the compound $CaO$, what are the oxidation numbers of calcium (Ca) and oxygen (O), respectively?
In the compound $CaO$, what are the oxidation numbers of calcium (Ca) and oxygen (O), respectively?
For the following unbalanced reaction: $MnO_4^-(aq) + Fe^{2+}(aq)
ightarrow Mn^{2+}(aq) + Fe^{3+}(aq)$, which species gets oxidized?
For the following unbalanced reaction: $MnO_4^-(aq) + Fe^{2+}(aq) ightarrow Mn^{2+}(aq) + Fe^{3+}(aq)$, which species gets oxidized?
What is always true regarding oxidation and reduction processes in a redox reaction?
What is always true regarding oxidation and reduction processes in a redox reaction?
Which of the following best describes the role of the anode in both voltaic and electrolytic cells?
Which of the following best describes the role of the anode in both voltaic and electrolytic cells?
For the reaction: $Pb(NO_3)_2 + 2KI \rightarrow PbI_2 + 2KNO_3$, which species remains unchanged in terms of oxidation number and does not participate in the redox process?
For the reaction: $Pb(NO_3)_2 + 2KI \rightarrow PbI_2 + 2KNO_3$, which species remains unchanged in terms of oxidation number and does not participate in the redox process?
What is the significance of a substance having a high positive oxidation potential?
What is the significance of a substance having a high positive oxidation potential?
In an electrochemical cell, which conditions must be met to measure the standard cell potential ($E^\circ$)?
In an electrochemical cell, which conditions must be met to measure the standard cell potential ($E^\circ$)?
What is the role of electrical energy in an electrolytic cell?
What is the role of electrical energy in an electrolytic cell?
How can the cell potential ($E_{cell}$) values be used to predict the spontaneity of a redox reaction under standard conditions?
How can the cell potential ($E_{cell}$) values be used to predict the spontaneity of a redox reaction under standard conditions?
Consider a voltaic cell constructed with two half-cells. One contains a metal A in a solution of $A^{2+}$ ions, and the other contains metal B in a solution of $B^{2+}$ ions. If metal A is a stronger reducing agent than metal B, what does this imply about the standard cell potential ($E^\circ_{cell}$)?
Consider a voltaic cell constructed with two half-cells. One contains a metal A in a solution of $A^{2+}$ ions, and the other contains metal B in a solution of $B^{2+}$ ions. If metal A is a stronger reducing agent than metal B, what does this imply about the standard cell potential ($E^\circ_{cell}$)?
Why is it essential to balance redox equations when analyzing electrochemical processes?
Why is it essential to balance redox equations when analyzing electrochemical processes?
In the reaction $2Na + Cl_2 \rightarrow 2NaCl$, how does the oxidation number of chlorine change, and what process does this indicate?
In the reaction $2Na + Cl_2 \rightarrow 2NaCl$, how does the oxidation number of chlorine change, and what process does this indicate?
In an electrochemical cell, a reaction is deemed spontaneous under which of the following conditions?
In an electrochemical cell, a reaction is deemed spontaneous under which of the following conditions?
Given the reaction: $Zn + Cu^{2+}(aq) \rightarrow Zn^{2+}(aq) + Cu$, and knowing that Zinc is more reactive than Copper, what can be definitively stated about the cell's spontaneity?
Given the reaction: $Zn + Cu^{2+}(aq) \rightarrow Zn^{2+}(aq) + Cu$, and knowing that Zinc is more reactive than Copper, what can be definitively stated about the cell's spontaneity?
Which of the following cell representations accurately describes a setup where Aluminum (Al) is oxidized to $Al^{3+}$ and Magnesium ($Mg^{2+}$) is reduced to Mg?
Which of the following cell representations accurately describes a setup where Aluminum (Al) is oxidized to $Al^{3+}$ and Magnesium ($Mg^{2+}$) is reduced to Mg?
For the reaction $2Al + 3Mg^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Mg$, the standard reduction potentials are $E°{Al} = +1.66V$ and $E°{Mg} = -2.36V$. What is the standard cell potential ($E°_{cell}$)?
For the reaction $2Al + 3Mg^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Mg$, the standard reduction potentials are $E°{Al} = +1.66V$ and $E°{Mg} = -2.36V$. What is the standard cell potential ($E°_{cell}$)?
Given the reaction $2Al + 3Mg^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Mg$ with $E°{Al} = +1.66V$ and $E°{Mg} = -2.36V$, and knowing Magnesium is more reactive than Aluminum, predict the $E°_{cell}$ and spontaneity.
Given the reaction $2Al + 3Mg^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Mg$ with $E°{Al} = +1.66V$ and $E°{Mg} = -2.36V$, and knowing Magnesium is more reactive than Aluminum, predict the $E°_{cell}$ and spontaneity.
What is the role of a reducing agent in a redox reaction, and how does this affect its own oxidation number?
What is the role of a reducing agent in a redox reaction, and how does this affect its own oxidation number?
According to the standard rules for assigning oxidation numbers, what is the oxidation number of an individual atom in a polyatomic ion?
According to the standard rules for assigning oxidation numbers, what is the oxidation number of an individual atom in a polyatomic ion?
In the balanced redox reaction: $2Al(s) + 3Cu^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Cu(s)$, which species undergoes reduction?
In the balanced redox reaction: $2Al(s) + 3Cu^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Cu(s)$, which species undergoes reduction?
Given the half-reactions: $Zn(s) \rightarrow Zn^{2+}(aq) + 2e^-$ with $E° = +0.76V$ and $Cu^{2+}(aq) + 2e^- \rightarrow Cu(s)$ with $E° = +0.34V$, what is the standard cell potential ($E°_{cell}$) for the reaction $Zn + Cu^{2+}(aq) \rightarrow Zn^{2+}(aq) + Cu$?
Given the half-reactions: $Zn(s) \rightarrow Zn^{2+}(aq) + 2e^-$ with $E° = +0.76V$ and $Cu^{2+}(aq) + 2e^- \rightarrow Cu(s)$ with $E° = +0.34V$, what is the standard cell potential ($E°_{cell}$) for the reaction $Zn + Cu^{2+}(aq) \rightarrow Zn^{2+}(aq) + Cu$?
In a voltaic cell, if the standard reduction potential of the cathode is significantly lower than that of the anode, what does this imply about the cell's overall potential and spontaneity?
In a voltaic cell, if the standard reduction potential of the cathode is significantly lower than that of the anode, what does this imply about the cell's overall potential and spontaneity?
What must occur for a redox reaction to take place?
What must occur for a redox reaction to take place?
Which statement correctly describes the change in oxidation number for a substance that has been oxidized?
Which statement correctly describes the change in oxidation number for a substance that has been oxidized?
Which of the following is the correct half-reaction for the reduction of $Cl_2$ to $Cl^−$?
Which of the following is the correct half-reaction for the reduction of $Cl_2$ to $Cl^−$?
In the reaction $2Na + Cl_2 → 2NaCl$, which compound is the oxidizing agent?
In the reaction $2Na + Cl_2 → 2NaCl$, which compound is the oxidizing agent?
When balancing redox equations using the oxidation number method, what is the significance of determining the change in oxidation number for each element?
When balancing redox equations using the oxidation number method, what is the significance of determining the change in oxidation number for each element?
In an electrochemical cell, if a less reactive metal is at the anode and the calculated cell potential (E) is negative, what does this indicate about the spontaneity of the reaction?
In an electrochemical cell, if a less reactive metal is at the anode and the calculated cell potential (E) is negative, what does this indicate about the spontaneity of the reaction?
How does a high positive oxidation potential relate to the strength of a reducing agent?
How does a high positive oxidation potential relate to the strength of a reducing agent?
In electrochemistry, what is the crucial distinction between voltaic and electrolytic cells regarding spontaneity and energy input?
In electrochemistry, what is the crucial distinction between voltaic and electrolytic cells regarding spontaneity and energy input?
Given the half-reactions $Zn \rightarrow Zn^{2+}(aq) + 2e^-$ and $Cu^{2+}(aq) + 2e^- \rightarrow Cu$, where zinc is more reactive than copper, what conditions would result in a non-spontaneous reaction?
Given the half-reactions $Zn \rightarrow Zn^{2+}(aq) + 2e^-$ and $Cu^{2+}(aq) + 2e^- \rightarrow Cu$, where zinc is more reactive than copper, what conditions would result in a non-spontaneous reaction?
If substance 'X' has a substantially higher positive reduction potential than substance 'Y', what can be inferred about their behavior in a redox reaction?
If substance 'X' has a substantially higher positive reduction potential than substance 'Y', what can be inferred about their behavior in a redox reaction?
Consider a voltaic cell constructed with aluminum and magnesium electrodes. Given that magnesium is more reactive than aluminum, which of the following setups would result in a spontaneous reaction?
Consider a voltaic cell constructed with aluminum and magnesium electrodes. Given that magnesium is more reactive than aluminum, which of the following setups would result in a spontaneous reaction?
For the overall reaction $Zn + Cu^{2+}(aq) \rightarrow Zn^{2+}(aq) + Cu$, what does the cell representation $Zn | Zn^{2+} || Cu^{2+} | Cu$ signify?
For the overall reaction $Zn + Cu^{2+}(aq) \rightarrow Zn^{2+}(aq) + Cu$, what does the cell representation $Zn | Zn^{2+} || Cu^{2+} | Cu$ signify?
When measuring the voltage (electromotive force) of an electrochemical cell, what conditions define the 'standard cell potential' ($E^\circ$)?
When measuring the voltage (electromotive force) of an electrochemical cell, what conditions define the 'standard cell potential' ($E^\circ$)?
Given the reaction: $2Al(s) + 3Mg^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Mg(s)$ with $E°{Al} = +1.66V$ and $E°{Mg} = -2.36V$, what is the calculated standard cell potential ($E°_{cell}$), and is the reaction spontaneous as written?
Given the reaction: $2Al(s) + 3Mg^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Mg(s)$ with $E°{Al} = +1.66V$ and $E°{Mg} = -2.36V$, what is the calculated standard cell potential ($E°_{cell}$), and is the reaction spontaneous as written?
Consider an electrochemical cell where a metal 'A' is more reactive than metal 'B'. If metal 'A' is used as the anode and metal 'B' as the cathode, what can be concluded about the cell potential ($E_{cell}$) and the spontaneity of the reaction?
Consider an electrochemical cell where a metal 'A' is more reactive than metal 'B'. If metal 'A' is used as the anode and metal 'B' as the cathode, what can be concluded about the cell potential ($E_{cell}$) and the spontaneity of the reaction?
How does the electrode potential relate to the designation of anode and cathode in an electrochemical cell?
How does the electrode potential relate to the designation of anode and cathode in an electrochemical cell?
For the cell representation $Ag | Ag^+ || Fe^{2+} | Fe$, knowing that silver is less reactive than iron, what can be inferred about the spontaneity of the cell reaction as written?
For the cell representation $Ag | Ag^+ || Fe^{2+} | Fe$, knowing that silver is less reactive than iron, what can be inferred about the spontaneity of the cell reaction as written?
In the reaction $Pb(NO_3)_2 + 2KI \rightarrow PbI_2 + 2KNO_3$, which species does NOT undergo a change in oxidation number?
In the reaction $Pb(NO_3)_2 + 2KI \rightarrow PbI_2 + 2KNO_3$, which species does NOT undergo a change in oxidation number?
When an electrochemical cell reaches equilibrium, what is the value of the cell potential ($E_{cell}$)?
When an electrochemical cell reaches equilibrium, what is the value of the cell potential ($E_{cell}$)?
Given the half-reactions $Zn \rightarrow Zn^{2+}(aq) + 2e^-$ $E° = +0.76V$ and $Cu^{2+}(aq) + 2e^- \rightarrow Cu$ $E° = +0.34V$, what would happen if the positions of Zinc and Copper were switched such that Copper was undergoing oxidation while Zinc was undergoing reduction?
Given the half-reactions $Zn \rightarrow Zn^{2+}(aq) + 2e^-$ $E° = +0.76V$ and $Cu^{2+}(aq) + 2e^- \rightarrow Cu$ $E° = +0.34V$, what would happen if the positions of Zinc and Copper were switched such that Copper was undergoing oxidation while Zinc was undergoing reduction?
Why is it important to consider the relative reactivity series of metals when predicting the spontaneity of a redox reaction in an electrochemical cell?
Why is it important to consider the relative reactivity series of metals when predicting the spontaneity of a redox reaction in an electrochemical cell?
How does a negative standard cell potential ($E°_{cell}$) correlate with the Gibbs free energy change ($\Delta G$) for an electrochemical reaction?
How does a negative standard cell potential ($E°_{cell}$) correlate with the Gibbs free energy change ($\Delta G$) for an electrochemical reaction?
Flashcards
Redox Reaction
Redox Reaction
Reactions involving the oxidation and reduction of chemical species.
OIL
OIL
Oxidation Is Loss of electrons.
RIG
RIG
Reduction Is Gaining of electrons.
Oxidizing Agent
Oxidizing Agent
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Reducing Agent
Reducing Agent
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Oxidation Number
Oxidation Number
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Group 1A Oxidation Number
Group 1A Oxidation Number
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Group 2A Oxidation Number
Group 2A Oxidation Number
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Hydrogen Oxidation Number
Hydrogen Oxidation Number
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Identifying Oxidation
Identifying Oxidation
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Oxidation
Oxidation
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Reduction
Reduction
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Electrochemistry
Electrochemistry
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Electrodes
Electrodes
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Anode
Anode
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Cathode
Cathode
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Voltaic cell
Voltaic cell
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Electrolytic cell
Electrolytic cell
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Electrode Potential
Electrode Potential
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Standard Cell Potential
Standard Cell Potential
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Spontaneous Reaction
Spontaneous Reaction
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Nonspontaneous Reaction
Nonspontaneous Reaction
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Cell Representation
Cell Representation
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Standard Cell Potential (E°cell)
Standard Cell Potential (E°cell)
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What are Redox Reactions?
What are Redox Reactions?
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What is an Oxidizing Agent?
What is an Oxidizing Agent?
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What is a Reducing Agent?
What is a Reducing Agent?
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What is Oxidation Number?
What is Oxidation Number?
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Group 1A Oxidation Number Rule
Group 1A Oxidation Number Rule
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Group 2A Oxidation Number Rule
Group 2A Oxidation Number Rule
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Fluorine's Oxidation Number
Fluorine's Oxidation Number
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Identifying Reduction
Identifying Reduction
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Standard Cell Potential (E°)
Standard Cell Potential (E°)
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Positive E°cell
Positive E°cell
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Negative E°cell
Negative E°cell
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Overall Cell Reaction
Overall Cell Reaction
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Electrode Reactions
Electrode Reactions
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Anode Location
Anode Location
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Cathode Location
Cathode Location
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Reactive Metal at Anode
Reactive Metal at Anode
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Calculating E°cell
Calculating E°cell
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Oxidation Number (O.N.)
Oxidation Number (O.N.)
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Group 1A O.N.
Group 1A O.N.
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Group 2A O.N.
Group 2A O.N.
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Hydrogen O.N.
Hydrogen O.N.
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Fluorine's O.N.
Fluorine's O.N.
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Spontaneous Reaction (E°cell)
Spontaneous Reaction (E°cell)
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Nonspontaneous Reaction (E°cell)
Nonspontaneous Reaction (E°cell)
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More Reactive Metal at Anode
More Reactive Metal at Anode
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E° for Oxidation
E° for Oxidation
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E° for Reduction
E° for Reduction
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Zn + Cu2+ Reaction
Zn + Cu2+ Reaction
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Al + Mg2+ Reaction
Al + Mg2+ Reaction
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Hydrogen: O.N. with metals/Boron
Hydrogen: O.N. with metals/Boron
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Hydrogen: O.N. with Nonmetals
Hydrogen: O.N. with Nonmetals
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Oxygen's Oxidation Number
Oxygen's Oxidation Number
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Group 1A Rule
Group 1A Rule
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Group 2A Rule
Group 2A Rule
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What is Oxidizing Agent?
What is Oxidizing Agent?
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Electrochemistry Definition
Electrochemistry Definition
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What are Electrodes?
What are Electrodes?
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Standard Electrode Potential
Standard Electrode Potential
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Strong Oxidizing Agent
Strong Oxidizing Agent
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Strong Reducing Agent
Strong Reducing Agent
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Ecell Significance
Ecell Significance
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Voltaic Cell Electrode Sign
Voltaic Cell Electrode Sign
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Overall Cell Reaction Representation
Overall Cell Reaction Representation
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Electrode Reactions Representation
Electrode Reactions Representation
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Spontaneous Reaction Condition
Spontaneous Reaction Condition
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Non-spontaneous Reaction Condition
Non-spontaneous Reaction Condition
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Zn/Cu Cell Potential
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Al/Mg Cell Potential
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Defining Oxidation
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Defining Reduction
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What is the Anode?
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Voltaic Cell Poles
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What is a Redox Reaction?
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Spontaneous Reaction (E°cell > 0)
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Nonspontaneous Reaction (E°cell < 0)
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Anode in Cell Representation
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Cathode in Cell Representation
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Spontaneous Condition
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Zn-Cu Cell
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Reaction for Aluminum-Magnesium ions
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Reduction Potential
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Oxidation Potential
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Ion Concentration
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Standard Temperature
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Electrolytic cell: Cathode
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Electrolytic cell: Anode
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Oxygen O.N.
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Group 7A (Halogens) O.N.
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What indicates Oxidation?
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What indicates Reduction?
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What are Oxidizing Agents
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What are Reducing Agents
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What is Fluorine oxidation number?
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Oxidation Number Increase
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OIL meaning
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Reaction is non-spontaneous
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Voltaic Cell Reactions
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Electrolytic Cell Reactions
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Products Oxidation Numbers
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Products Reduction Numbers
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Reducing Agent Ability
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Oxidizing Agent Ability
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Standard Ion Concentration
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Spontaneous Reaction (E>0)
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Non-Spontaneous Reaction (E<0)
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Anode (Oxidation)
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Cathode (Reduction)
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E° Cathode
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E° Anode
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Positive E°cell (Spontaneous)
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O.N. of Group 1A Elements
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O.N. of Group 2A Elements
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O.N. of Hydrogen (H)
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O.N. of Fluorine (F)
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O.N. of Oxygen (O)
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Oxidation at the Anode
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Reduction at the Cathode
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High Reduction Potential
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Application of redox reaction
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Coverage for the exam for this topic:
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Group 1A elements
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Group 2A Elements
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Electrode-Electrolyte Interface
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Electrode Potential Definition
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E° Values Use
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E°cell > 0
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E°cell < 0
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Electrochemical Cell Representation
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Anode Reaction
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Cathode Reaction
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Overall Cell Reaction description
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Electrode Reactions description
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Spontaneous Reaction Setup
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Cell Reaction
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Nonspontaneous Reaction reaction
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Hydrogen's Oxidation Number?
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What charge does the Anode have?
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What charge does the Cathode have?
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What is standard temperature?
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Ecell (cell potential)
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Zinc reacting with Copper
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Aluminum reacting with Magnesium
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Cell Potential (Ecell)
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Voltaic cell electrodes
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Positive E°cell Implications
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Negative E°cell Implications
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Half-Cell Potential
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Oxidation Number Definition
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Oxidation Sign
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Reduction Sign
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Anode Definition
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Cathode Definition
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Voltaic cell: Cathode +
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Voltaic cell: Anode -
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Cell Notation
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Positive Oxidation Potential
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Assigning Oxidation Number
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Reaction Representation, Overall cell
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Reaction Representation, Electrode
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Zn+ Cu2+ (aq) → Zn2+(aq) + Cu
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Al+ Mg2+(aq) → Al+3(aq) +Mg
Al+ Mg2+(aq) → Al+3(aq) +Mg
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Anode Location in Cell Notation
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Cathode Location in Cell Notation
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Oxygen's Most Common O.N.
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What is Voltaic Cell?
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What is Electrolytic Cell?
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Voltaic cell electrode polarity
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Electrolytic cell electrode polarity
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Electrochemical Cell Notation
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Anode in Cell Notation
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Cathode in Cell Notation
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Zn/Cu Reaction
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Al/Mg Reaction
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Electrochemical Reactions
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Group 1A O.N. Rule
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Group 2A O.N. Rule
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Electrochemical Spontaneity (E°)
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Electrochemical Non-spontaneity (E°)
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Cell Reaction Representation
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E°cell and Spontaneity
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Cell Representation Components
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Cell Potential
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Standard Cell Conditions
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Spontaneous Reaction (E° > 0)
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Nonspontaneous Reaction (E° < 0)
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Overall Electrochemical Reaction
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Electrode Half Reactions
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Zn more reactive than Cu at the anode
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What is Oxidation Number (O.N.)?
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Ecell values
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Anode Half-Cell Notation
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Cathode Half-Cell Notation
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Group 1A elements O.N.
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Group 2A elements O.N.
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How to Identify Oxidation
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How to Identify Reduction
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What does Oxidizing agent do?
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What does Reducing agent do?
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What's Group 1A oxidation #?
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What's Group 2A oxidation #?
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What is an Electrolytic Cell?
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What is Electrode Potential?
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What is Standard Cell Potential?
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What is a Strong Oxidizing Agent?
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What is a Strong Reducing Agent?
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What is Ecell Significance?
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Representing Cell Reaction
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Electrode Reactions Notation
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Spontaneous Electrochemical Reaction
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Non-Spontaneous Electrochemical Reaction
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Zinc and Copper Cell
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Reaction of Aluminum with Magnesium ions
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Electrolytic Cathode
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Electrolytic Anode
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Voltaic Cell Cathode
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Voltaic Cell Anode
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Reaction at Anode
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Reaction at Cathode
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Calculate Standard Cell Potential
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Positive Cell Potential
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Redox Co-occurrence
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Oxidizing Agent's Fate
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Reducing Agent's Fate
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Hydrogen: O.N. with Metals
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Anode of Voltaic Cell
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Anode of Electrolytic Cell
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Representing Overall Cell Reaction
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Representing Electrode Reactions
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Example of Spontaneous Reaction
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Example of Non-Spontaneous Reaction
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Calculating Standard Cell Potential (E°cell)
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Determining Cell Spontaneity
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Standard Conditions: Concentration
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Standard Conditions: Temperature
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Standard Conditions: Pressure
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Study Notes
Redox Reactions
- Redox reactions involve oxidation and reduction processes
- Oxidation is the loss of electrons
- Reduction is the gaining of electrons
- Oxidation and reduction always occur together
Oxidizing and Reducing Agents
- The oxidizing agent are species that performs oxidizing
- The reducing agent are species that performs reducing
Oxidation Number
- The oxidation number is how much charge an atom would have if electrons were completely transferred rather than shared
Rules for Oxidation Numbers
- Group 1A(1) elements have an ON of +1 in compounds.
- Group 2A(2) elements have an ON of +2 in all compounds.
- Hydrogen has an ON of +1 when combined with nonmetals
- Hydrogen has an ON of -1 metals and boron.
- Fluorine always has an ON of -1.
- Oxygen has an ON of -1 in peroxides
- Oxygen has an ON of -2 in other compounds except with fluorine
- Group 7A(17) elements have an ON of -1 when combined with metals and nonmetals (except O), and other halogens lower in the group
Identifying Oxidation and Reduction
- Oxidation numbers must be assigned and compared
- Oxidation is represented by an increase in oxidation number
- Reduction is represented by a decrease in oxidation number
Balancing Redox Equations
- Assign oxidation numbers to all elements.
- Identify oxidized and reduced species.
- Compute the number of electrons lost and gained.
- Multiply by factors to equalize electron loss and gain, using the factors as coefficients.
- Complete the balancing by inspection
Application of Redox Reactions
- When an apple is cut, the polyphenol oxidase (PPO) reacts with oxygen, causing oxidation and producing melanin (browning)
- Hair perming or straightening involves breaking disulfide bonds by adding hydrogen atoms
- This is called reduction
- Broken bones are then oxidized to remove the hydrogen atoms and reform the disulfide bonds, retaining the new hair shape
Electrochemistry
- Electrochemistry studies chemical reactions at the interface of an electrode and an electrolyte
- It also deals with interactions between electrical energy and chemical change
Definition of Terms
- Electrodes are metal strips/wires connected by an electrically conducting wire
- The anode is the electrode where oxidation takes place
- The cathode is the electrode where reduction takes place
Electrochemical reactions
- Voltaic cells produce electricity from chemical reactions
- Electrolytic cells use electricity to cause the reactions to occur
- Both voltaic and electrolytic cells are electrochemical cells
Electrode potential
- The voltage (electromotive force or emf) of a cell is measured in volts
- It is the sum of two half-cell potentials using the standard cell potential values
- Electromotive force is measured under standard conditions
- All ion concentrations at 1M, temperature at 25°C, pressure is one of the cell with a reference cells
- Substances with high positive reduction potential are strong oxidizing agents,
- Substances with high positive oxidation potential are strong Reducing agents
Cell potential values
- These determine if half-cell reactions will occur
- Reactions are spontaneous when cell potential is positive
- Reactions are nonspontaneous potentials are negative
- Spontaneous reaction when more reactive metal is placed in the anode and less reactive metal is placed in the cathode
Cell representation
- Electrochemical cells can be represented using overall cell reactions
- Electrochemical cells can be represented using the electrode reactions
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Description
Test your knowledge of electrochemistry principles. Questions cover oxidation, reduction, electrochemical cells, and standard cell potential. Review the key concepts and definitions in electrochemistry.
