Multiple Choice
Which of the following methods is most appropriate for determining the activation energy of the redox reaction q^{2+} + 2 r^{+} ightarrow q^{0} + 2 r^{2+}?
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6. Chemical Quantities & Aqueous Reactions
Redox Reactions
Multiple Choice
Given the redox reaction: Zn + Cu^{2+} → Zn^{2+} + Cu, which of the following correctly separates the reaction into its oxidation and reduction half-reactions?
A
Oxidation: Zn → Zn^{2+} + 2e^{-}; Reduction: Cu^{2+} + 2e^{-} → Cu
B
Oxidation: Cu^{2+} + 2e^{-} → Cu; Reduction: Zn → Zn^{2+} + 2e^{-}
C
Oxidation: Cu → Cu^{2+} + 2e^{-}; Reduction: Zn^{2+} + 2e^{-} → Zn
D
Oxidation: Zn^{2+} + 2e^{-} → Zn; Reduction: Cu → Cu^{2+} + 2e^{-}
Verified step by step guidance1
Identify the species that undergo oxidation and reduction by examining the changes in oxidation states in the reaction: \(\mathrm{Zn} + \mathrm{Cu}^{2+} \rightarrow \mathrm{Zn}^{2+} + \mathrm{Cu}\).
Determine the oxidation half-reaction by finding the species that loses electrons. Here, zinc (Zn) goes from an oxidation state of 0 to +2, indicating it loses 2 electrons. Write this as: \(\mathrm{Zn} \rightarrow \mathrm{Zn}^{2+} + 2e^{-}\).
Determine the reduction half-reaction by finding the species that gains electrons. Copper ion (\(\mathrm{Cu}^{2+}\)) goes from +2 to 0, indicating it gains 2 electrons. Write this as: \(\mathrm{Cu}^{2+} + 2e^{-} \rightarrow \mathrm{Cu}\).
Verify that the number of electrons lost in the oxidation half-reaction equals the number of electrons gained in the reduction half-reaction to ensure electron balance.
Combine the two half-reactions to confirm they sum to the original overall reaction, ensuring the half-reactions are correctly separated.
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