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Questions and Answers
What is the electrical work done in a Galvanic cell equivalent to?
What is the electrical work done in a Galvanic cell equivalent to?
When a lead storage battery is charged, what type of cell does it function as?
When a lead storage battery is charged, what type of cell does it function as?
In a Galvanic cell, the direction of current flows from which electrode to which electrode?
In a Galvanic cell, the direction of current flows from which electrode to which electrode?
Which metal does not react with water to produce an oxide or hydroxide and hydrogen?
Which metal does not react with water to produce an oxide or hydroxide and hydrogen?
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What is the result of the electrolysis of aqueous CuSO4?
What is the result of the electrolysis of aqueous CuSO4?
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Which ion cannot be displaced by Zn from its aqueous solution?
Which ion cannot be displaced by Zn from its aqueous solution?
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Which one of the following is not categorized as a secondary battery?
Which one of the following is not categorized as a secondary battery?
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What happens to molar conductance with an increase in concentration?
What happens to molar conductance with an increase in concentration?
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What is the mass of zinc deposited when 1295.6 C of electricity is passed through a solution containing Zn2+ ions?
What is the mass of zinc deposited when 1295.6 C of electricity is passed through a solution containing Zn2+ ions?
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What is the formula used to calculate the time when the charge and current are given?
What is the formula used to calculate the time when the charge and current are given?
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What is the molar conductivity at infinite dilution for CH3COOH based on the relation provided?
What is the molar conductivity at infinite dilution for CH3COOH based on the relation provided?
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How much charge is required to deposit 108 g of silver?
How much charge is required to deposit 108 g of silver?
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What is the mass of copper deposited with 1295.6 C of electricity?
What is the mass of copper deposited with 1295.6 C of electricity?
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According to Kohlraush's law, what can molar conductivity be expressed as?
According to Kohlraush's law, what can molar conductivity be expressed as?
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What is the definition of a strong electrolyte?
What is the definition of a strong electrolyte?
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Which of the following ions contributes to the molar conductivity calculation for CH3COOH?
Which of the following ions contributes to the molar conductivity calculation for CH3COOH?
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Which oxidizing agent is the weakest among the following options?
Which oxidizing agent is the weakest among the following options?
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What is the molar conductivity of a 0.02M NaCl solution if its conductivity is $2.6 \times 10^{-2}$ S cm$^{-1}$?
What is the molar conductivity of a 0.02M NaCl solution if its conductivity is $2.6 \times 10^{-2}$ S cm$^{-1}$?
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What is electrochemistry primarily concerned with?
What is electrochemistry primarily concerned with?
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During the electrolysis of an aqueous solution of AgNO3, what are the products formed at the anode?
During the electrolysis of an aqueous solution of AgNO3, what are the products formed at the anode?
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Which type of cell converts spontaneous redox reaction into electrical work?
Which type of cell converts spontaneous redox reaction into electrical work?
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What does the conductivity equation $k = \frac{1}{R} \cdot \frac{l}{A}$ represent?
What does the conductivity equation $k = \frac{1}{R} \cdot \frac{l}{A}$ represent?
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In an electrolytic cell, how is the amount of copper deposited at the cathode related to the charge passed?
In an electrolytic cell, how is the amount of copper deposited at the cathode related to the charge passed?
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For the galvanic cell described by the reaction $Zn (s) + 2Ag^+ \to Zn^{2+} + 2Ag (s)$, which electrode serves as the anode?
For the galvanic cell described by the reaction $Zn (s) + 2Ag^+ \to Zn^{2+} + 2Ag (s)$, which electrode serves as the anode?
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According to Kohlrausch's law, limiting molar conductivity is expressed as $\Lambda \degree m = v+ \lambda \degree + + v− \lambda \degree -$. What does $v+$ represent?
According to Kohlrausch's law, limiting molar conductivity is expressed as $\Lambda \degree m = v+ \lambda \degree + + v− \lambda \degree -$. What does $v+$ represent?
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Which component acts as the carrier of current within the galvanic cell?
Which component acts as the carrier of current within the galvanic cell?
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How is the degree of dissociation ($\alpha$) calculated?
How is the degree of dissociation ($\alpha$) calculated?
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What is the total charge (in coulombs) passed if a current of 1.5 Amperes is maintained for 10 minutes?
What is the total charge (in coulombs) passed if a current of 1.5 Amperes is maintained for 10 minutes?
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In an electrolytic cell, what is the primary purpose of electrical energy?
In an electrolytic cell, what is the primary purpose of electrical energy?
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Which of the following correctly depicts the half-reaction at the cathode in the electrolysis of AgNO3?
Which of the following correctly depicts the half-reaction at the cathode in the electrolysis of AgNO3?
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What is molar conductivity ($\Lambda_m$) defined as?
What is molar conductivity ($\Lambda_m$) defined as?
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What do the symbols $\lambda \degree +$ and $\lambda \degree -$ represent in Kohlrausch's law?
What do the symbols $\lambda \degree +$ and $\lambda \degree -$ represent in Kohlrausch's law?
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How much electricity in Coulombs is required for the oxidation of 1 mole of FeO to Fe2O3?
How much electricity in Coulombs is required for the oxidation of 1 mole of FeO to Fe2O3?
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What is the molar conductivity of a 0.20M KCl solution at 298K?
What is the molar conductivity of a 0.20M KCl solution at 298K?
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Which of the following correctly defines electrical conductivity?
Which of the following correctly defines electrical conductivity?
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What reaction occurs at the cathode in a fuel cell?
What reaction occurs at the cathode in a fuel cell?
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What is the cell constant if the resistance of a 0.001M KCl solution is 1500Ω and its conductivity is 0.146 × 10⁻³ S cm⁻¹?
What is the cell constant if the resistance of a 0.001M KCl solution is 1500Ω and its conductivity is 0.146 × 10⁻³ S cm⁻¹?
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According to Kohlrausch’s law of independent migration of ions, at infinite dilution, what does molar conductivity equal?
According to Kohlrausch’s law of independent migration of ions, at infinite dilution, what does molar conductivity equal?
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What is the standard reduction potential for the Zn2+/Zn half-cell?
What is the standard reduction potential for the Zn2+/Zn half-cell?
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Which equation represents the overall reaction in a fuel cell?
Which equation represents the overall reaction in a fuel cell?
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What is the cell constant for a conductivity cell containing a 0.001M KCl solution if its resistance is 1500 Ω and the conductivity is $0.146 \times 10^{-3}$ S cm$^{-1}$?
What is the cell constant for a conductivity cell containing a 0.001M KCl solution if its resistance is 1500 Ω and the conductivity is $0.146 \times 10^{-3}$ S cm$^{-1}$?
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In the electrolysis of an aqueous solution of AgNO3 with platinum electrodes, what is produced at the anode?
In the electrolysis of an aqueous solution of AgNO3 with platinum electrodes, what is produced at the anode?
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During the reduction at the cathode of an electrolysis process in CuCl2 solution, which species is reduced?
During the reduction at the cathode of an electrolysis process in CuCl2 solution, which species is reduced?
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What is the value of Gibbs free energy change (∆Gθ) for the reaction $\text{Ni (s)} + 2\text{Ag}^+ (aq) \rightarrow \text{Ni}^{2+} (aq) + 2\text{Ag (s)}$ if $E^\theta_{cell}$ is 1.05 V?
What is the value of Gibbs free energy change (∆Gθ) for the reaction $\text{Ni (s)} + 2\text{Ag}^+ (aq) \rightarrow \text{Ni}^{2+} (aq) + 2\text{Ag (s)}$ if $E^\theta_{cell}$ is 1.05 V?
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What conclusion can be drawn about the products of electrolysis in aqueous CuCl2 solution?
What conclusion can be drawn about the products of electrolysis in aqueous CuCl2 solution?
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What is the equilibrium constant (Kc) for the reaction $\text{Ni (s)} + 2\text{Ag}^+ (aq) \rightarrow \text{Ni}^{2+} (aq) + 2\text{Ag (s)}$?
What is the equilibrium constant (Kc) for the reaction $\text{Ni (s)} + 2\text{Ag}^+ (aq) \rightarrow \text{Ni}^{2+} (aq) + 2\text{Ag (s)}$?
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For the Ag+/Ag electrode in a KCl solution, given that $E^\theta_{Ag/Ag^+} = 0.80$ V, what is the nature of the electrode potential?
For the Ag+/Ag electrode in a KCl solution, given that $E^\theta_{Ag/Ag^+} = 0.80$ V, what is the nature of the electrode potential?
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What are the oxidation products at the anode during the electrolysis of AgNO3 with platinum electrodes?
What are the oxidation products at the anode during the electrolysis of AgNO3 with platinum electrodes?
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Study Notes
Electrochemistry Concepts
- Electrochemistry is the branch of chemistry studying the interrelationship between chemical and electrical energy, including their conversion.
- Cells can be categorized into two types:
- Galvanic cells convert spontaneous redox reactions into electrical energy.
- Electrolytic cells use electrical energy to drive non-spontaneous redox reactions.
- Conductivity (k) is a measure of a material's ability to conduct electricity.
- k = 1/ρ * (l/A), where ρ is resistivity, l is the length of the material, and A is the cross-sectional area.
- Molar conductivity (Λm) is a measure of the conductivity of a solution per mole of solute.
- Λm = k/C, where k is conductivity and C is the molar concentration of the solute.
- Kohlrausch's law states that the limiting molar conductivity of an electrolyte is the sum of the limiting molar conductivities of its ions.
- Λ° = v₁λ°⁺ + v₂λ°⁻ where v₁ and v₂ are the number of cations and anions, respectively, and λ°⁺ and λ°⁻ are the limiting molar conductivities of the cation and anion.
- The degree of dissociation (α) can also be calculated by its formula which is α = Λm/Λ°m where Λm is the molar conductivity at some concentration and Λ°m is the limiting molar conductivity of the electrolyte
Dry Cell
- At the anode (oxidation): Zn → Zn2+ + 2e-
- At the cathode (reduction): 2NH₄⁺ + 2MnO₂ + 2e⁻ → 2MnO(OH) + 2NH₃
- Overall reaction: Zn + 2NH₄⁺ + 2MnO₂ → Zn²⁺ + 2MnO(OH) + 2NH₃
Mercury Cell
- At the anode (oxidation): Zn(Hg) + 2OH⁻ → ZnO (s) + H₂O + 2e⁻
- At the cathode (reduction): HgO (s) + H₂O + 2e⁻ → Hg (l) + 2OH⁻
- Overall reaction: Zn(Hg) + HgO (s) → ZnO(s) + Hg(l)
Lead Storage Cell
- At the anode (oxidation): Pb (s) → Pb²⁺ + 2e⁻ , Pb²⁺ + SO₄²⁻ → PbSO₄
- At the cathode (reduction): PbO₂ + 4H⁺ + 2e⁻ → Pb²⁺ + 2H₂O, Pb²⁺ + SO₄²⁻ → PbSO₄
- Overall reaction: Pb (s) + PbO₂ (s) + 2H₂SO₄ (aq) → 2PbSO₄ (s) + 2H₂O (l)
Nernst Equation
- E = E° - (RT/nF)lnQ (where E is the cell potential, E° is the standard cell potential, R is the ideal gas constant, T is absolute temperature, n is the number of moles of electrons transferred, F is Faraday's constant, and Q is the reaction quotient.)
Corrosion
- Corrosion is the electrochemical process where a metal reacts with substances in its environment to form compounds.
- Metals are oxidized by losing electrons to form oxides or other compounds.
- Example: 2Fe(s) + O2(g) + 4H+(aq) → 2Fe²⁺(aq) + 2H₂O(l)
Multiple Choice Questions (Examples are included based on the provided text)
- KCl is used in a salt bridge because it is a strong electrolyte and its ions migrate equally.
- The nature of the curve of E°cell against log K is a straight line.
- A spontaneous reaction has a negative ∆G, an equilibrium constant (K) > 1, and a negative E°cell value, but this is not always true in all cases.
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Description
Test your knowledge on the principles of electrochemistry, including the differences between galvanic and electrolytic cells. Explore key concepts such as conductivity and Kohlrausch's law, which are fundamental to understanding electricity in chemical reactions. This quiz is designed for students studying electrochemistry.
