Podcast
Questions and Answers
In the reaction $Fe^{3+}(aq) + SO_2(g) \rightarrow Fe^{2+}(aq) + SO_4^{2-}(aq)$, which of the following correctly identifies the oxidation and reduction half-reactions?
In the reaction $Fe^{3+}(aq) + SO_2(g) \rightarrow Fe^{2+}(aq) + SO_4^{2-}(aq)$, which of the following correctly identifies the oxidation and reduction half-reactions?
- Oxidation: $SO_2(g) + 2H_2O(l) \rightarrow SO_4^{2-}(aq) + 4H^+(aq) + 2e^-$, Reduction: $Fe^{3+}(aq) + e^- \rightarrow Fe^{2+}(aq)$ (correct)
- Oxidation: $Fe^{2+}(aq) \rightarrow Fe^{3+}(aq) + e^-$, Reduction: $SO_4^{2-}(aq) + 4H^+(aq) + 2e^- \rightarrow SO_2(g) + 2H_2O(l)$
- Oxidation: $SO_4^{2-}(aq) + 4H^+(aq) + 2e^- \rightarrow SO_2(g) + 2H_2O(l)$, Reduction: $Fe^{2+}(aq) \rightarrow Fe^{3+}(aq) + e^-$
- Oxidation: $Fe^{3+}(aq) + e^- \rightarrow Fe^{2+}(aq)$, Reduction: $SO_2(g) + 2H_2O(l) \rightarrow SO_4^{2-}(aq) + 4H^+(aq) + 2e^-$
Consider the reaction: $H_2O_2(aq) + I^-(aq) \rightarrow H_2O(l) + I_2(s)$. Which statement accurately describes the role of each reactant?
Consider the reaction: $H_2O_2(aq) + I^-(aq) \rightarrow H_2O(l) + I_2(s)$. Which statement accurately describes the role of each reactant?
- $H_2O_2$ is the oxidizing agent, accepting electrons, and $I^-$ is the reducing agent, donating electrons. (correct)
- $H_2O_2$ and $I^-$ are both reducing agents, donating electrons.
- $H_2O_2$ is the reducing agent, donating electrons, and $I^-$ is the oxidizing agent, accepting electrons.
- $H_2O_2$ and $I^-$ are both oxidizing agents, accepting electrons.
For the reaction: $MnO_4^-(aq) + Br^-(aq) \rightarrow Mn^{2+}(aq) + Br_2(aq)$, what is the coefficient of $Br^-(aq)$ when the equation is balanced using the smallest whole-number coefficients?
For the reaction: $MnO_4^-(aq) + Br^-(aq) \rightarrow Mn^{2+}(aq) + Br_2(aq)$, what is the coefficient of $Br^-(aq)$ when the equation is balanced using the smallest whole-number coefficients?
- 5
- 10 (correct)
- 16
- 2
In the reaction between dichromate ions and bisulfite ions: $Cr_2O_7^{2-}(aq) + HSO_3^-(aq) \rightarrow Cr^{3+}(aq) + SO_4^{2-}(aq)$, what color change would you expect to observe as the reaction proceeds?
In the reaction between dichromate ions and bisulfite ions: $Cr_2O_7^{2-}(aq) + HSO_3^-(aq) \rightarrow Cr^{3+}(aq) + SO_4^{2-}(aq)$, what color change would you expect to observe as the reaction proceeds?
When chlorine gas is bubbled into a solution of potassium bromide, a color change is observed. What is the correct explanation for why this color change occurs?
When chlorine gas is bubbled into a solution of potassium bromide, a color change is observed. What is the correct explanation for why this color change occurs?
Which of the following correctly ranks the halogens chlorine ($Cl_2$), bromine ($Br_2$), and iodine ($I_2$) in order of decreasing oxidizing strength?
Which of the following correctly ranks the halogens chlorine ($Cl_2$), bromine ($Br_2$), and iodine ($I_2$) in order of decreasing oxidizing strength?
What are the products formed when chlorine gas reacts with water, and what is the common name for the resulting solution?
What are the products formed when chlorine gas reacts with water, and what is the common name for the resulting solution?
When iron metal (steel wool) reacts with chlorine gas, what is the formula of the major iron-containing product formed?
When iron metal (steel wool) reacts with chlorine gas, what is the formula of the major iron-containing product formed?
Flashcards
What is oxidation?
What is oxidation?
Loss of electrons, increase in oxidation number.
What is reduction?
What is reduction?
Gain of electrons, decrease in oxidation number.
What is a redox reaction?
What is a redox reaction?
A reaction involving both oxidation and reduction processes.
What is an oxidant (oxidizing agent)?
What is an oxidant (oxidizing agent)?
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What is a reductant (reducing agent)?
What is a reductant (reducing agent)?
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What color change occurs when chlorine gas is bubbled into potassium bromide solution?
What color change occurs when chlorine gas is bubbled into potassium bromide solution?
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Which halide is the strongest oxidant?
Which halide is the strongest oxidant?
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What is the name of the ion OCl-?
What is the name of the ion OCl-?
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Study Notes
- Redox reactions involve oxidation and reduction processes.
- Ion-electron half equations are used to represent oxidation and reduction separately.
- Balancing redox equations involves balancing both mass and charge.
- Colour changes can indicate the progress of a redox reaction.
Balancing Redox Reaction (a)
- Reactants: Fe3+(aq) and SO2(g).
- Products: Fe2+(aq) and SO42-(aq).
Balancing Redox Reaction (b)
- Reactants: Fe2+(aq) and Cl2(g).
- Products: Fe3+(aq) and Cl-(aq).
Balancing Redox Reaction (c)
- Reactants: H2O2(aq) and I-(aq).
- Products: H2O(l) and I2(s).
Balancing Redox Reaction (d)
- Reactants: MnO4-(aq) and Br-(aq).
- Products: Mn2+(aq) and Br2(aq).
Balancing Redox Reaction (e)
- Reactants: Cr2O72-(aq) and HSO3-(aq).
- Products: Cr3+(aq) and SO42-(aq).
Chlorine Gas and Potassium Bromide
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When chlorine gas is bubbled into potassium bromide solution, a colour change is observed.
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The colour change in the solution needs to be described.
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The oxidant and reductant in this reaction must be named.
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For oxidation and reduction reactions, balanced half-equations need to be formulated.
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The balanced equation for the oxidation-reduction reaction can be derived by combining the half-equations.
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Observations can be explained by referring to species in the balanced equation.
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The strongest oxidant among chlorine, bromine, and iodine needs to be identified.
Reactions Involving Halogens
- Balanced equations are required for reactions involving halogens:
- Magnesium metal and chlorine gas.
- Hydrogen gas and chlorine gas.
- Aluminium metal powder and iodine powder.
- Iron metal (steel wool) and chlorine gas.
- Chlorine gas and water, naming the two acids that are produced.
Hypochlorite Ion
- The formula for the hypochlorite ion must be stated
- The common name of a solution containing this ion must be noted.
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