**Electrochemical Cell and Cathode Half-Reaction**In the electrochemical cell using the redox reaction below, the cathode half-reaction is ______.\(2H^+ (aq) + Sn (s) \rightarrow Sn^{2+} (aq) + H_2 (g)\)Select one:A. Sn + 2e⁻ → Sn²⁺B. Sn → Sn²⁺ + 2e⁻C. 2H⁺ + 2e⁻ → H₂D. 2H⁺ → H₂ + 2e⁻E. Sn + 2e⁻ → H₂Explanation:- The provided reaction shows an overall redox process involving the reduction of \(2H^+\) ions and the oxidation of Sn.- To identify the cathode half-reaction, note that reduction occurs at the cathode.Choices Analysis:- Option A: Sn + 2e⁻ → Sn²⁺ (represents oxidation, incorrect for the cathode reaction)- Option B: Sn → Sn²⁺ + 2e⁻ (represents oxidation, incorrect for the cathode reaction)- Option C: 2H⁺ + 2e⁻ → H₂ (represents reduction, correct for the cathode reaction)- Option D: 2H⁺ → H₂ + 2e⁻ (incorrect stoichiometry)- Option E: Sn + 2e⁻ → H₂ (incorrect species involved)Answer: C. 2H⁺ + 2e⁻ → H₂

Given Reaction 2H+(s) + Sn(s) -----> Sn2+( aq ) + H2(g) Cathode Half reaction = ?

In the electrochemical cell using the redox reaction below, the cathode half-reaction is 2H (s) + Sn (s) Sn2+ (aq) + H2 (g) Select one: O A. Sn + 2e→ Sn2+ O B. Sn → Sn2+ + 2e O C. 2H+ + 2e H2 O D. 2H+ → H2 + 2e O E. Sn + 2e H2

In the electrochemical cell using the redox reaction below, the cathode half-reaction is 2H (s) + Sn (s) Sn2+ (aq) + H2 (g) Select one: O A. Sn + 2e→ Sn2+ O B. Sn → Sn2+ + 2e O C. 2H+ + 2e H2 O D. 2H+ → H2 + 2e O E. Sn + 2e H2

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

**Electrochemical Cell and Cathode Half-Reaction**

In the electrochemical cell using the redox reaction below, the cathode half-reaction is ______.

\(2H^+ (aq) + Sn (s) \rightarrow Sn^{2+} (aq) + H_2 (g)\)

Select one:

A. Sn + 2e⁻ → Sn²⁺

B. Sn → Sn²⁺ + 2e⁻

C. 2H⁺ + 2e⁻ → H₂

D. 2H⁺ → H₂ + 2e⁻

E. Sn + 2e⁻ → H₂

Explanation:
- The provided reaction shows an overall redox process involving the reduction of \(2H^+\) ions and the oxidation of Sn.
- To identify the cathode half-reaction, note that reduction occurs at the cathode.

Choices Analysis:
- Option A: Sn + 2e⁻ → Sn²⁺ (represents oxidation, incorrect for the cathode reaction)
- Option B: Sn → Sn²⁺ + 2e⁻ (represents oxidation, incorrect for the cathode reaction)
- Option C: 2H⁺ + 2e⁻ → H₂ (represents reduction, correct for the cathode reaction)
- Option D: 2H⁺ → H₂ + 2e⁻ (incorrect stoichiometry)
- Option E: Sn + 2e⁻ → H₂ (incorrect species involved)

Answer: C. 2H⁺ + 2e⁻ → H₂

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