### Redox Reaction Exercise**Main Reaction:**\[ \text{PbSO}_4(s) + \text{H}^+(aq) + 2\text{Br}^-(aq) \rightarrow \text{Pb}(s) + \text{HSO}_4^-(aq) + \text{Br}_2(l) \]**Half-Reactions:**1. \(\text{PbSO}_4(s) + \text{H}^+(aq) + 2e^- \rightarrow \text{Pb}(s) + \text{HSO}_4^-(aq)\) - \(E^\circ = -0.31 \, \text{V}\)2. \(\text{Br}_2(l) + 2e^- \rightarrow 2\text{Br}^-(aq)\) - \(E^\circ = +1.07 \, \text{V}\)### Fill in the Blanks- **__________ is being oxidized.**- **__________ is being reduced.**- **__________ is acting as a reducing agent.**- **__________ is acting as an oxidizing agent.**- **__________ moles of electrons are transferred.**- **The reaction is a(n) __________ cell.**### Options:- \(\text{Br}_2(l)\)- \(\text{Pb}(s)\)- 6- \(\text{HSO}_4^-(aq)\)- electrolytic- \(\text{H}^+(aq)\)- 2- 3- 4- \(\text{PbSO}_4(s)\)- voltaic- 1- \(\text{Br}^-(aq)\)- 5This exercise involves understanding the components of a redox reaction, identifying oxidation and reduction processes, and determining the type of electrochemical cell involved. The options provided are used to complete the statements regarding the redox reaction.

Complete the statements about the redox reaction below. PbSO,(s) + H*(aq) + 2Br (aq) - Pb(s) + HSO, (aq) + Br2(1) Half-reactions: Pb(s) + HSO4"(aq) → 2Br(aq) PBSO4(s) + H*(aq) + 2e- E° = -0.31 V Br2(1) + 2e- → E° = +1.07 V Br2(1) Pb(s) is being oxidized. 6 HSO,"(aq) is being reduced. electrolytic H*(aq) is acting as an reducing agent. 3 is acting as an oxidizing agent. 4 PBSO4(s) voltaic moles of electrons are transferred. Br (aq) The reaction is a(n) cell.

Complete the statements about the redox reaction below. PbSO,(s) + H(aq) + 2Br (aq) - Pb(s) + HSO, (aq) + Br2(1) Half-reactions: Pb(s) + HSO4"(aq) → 2Br(aq) PBSO4(s) + H(aq) + 2e- E° = -0.31 V Br2(1) + 2e- → E° = +1.07 V Br2(1) Pb(s) is being oxidized. 6 HSO,"(aq) is being reduced. electrolytic H*(aq) is acting as an reducing agent. 3 is acting as an oxidizing agent. 4 PBSO4(s) voltaic moles of electrons are transferred. Br (aq) The reaction is a(n) cell.

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

### Redox Reaction Exercise

**Main Reaction:**
\[ \text{PbSO}_4(s) + \text{H}^+(aq) + 2\text{Br}^-(aq) \rightarrow \text{Pb}(s) + \text{HSO}_4^-(aq) + \text{Br}_2(l) \]

**Half-Reactions:**

1. \(\text{PbSO}_4(s) + \text{H}^+(aq) + 2e^- \rightarrow \text{Pb}(s) + \text{HSO}_4^-(aq)\)
- \(E^\circ = -0.31 \, \text{V}\)

2. \(\text{Br}_2(l) + 2e^- \rightarrow 2\text{Br}^-(aq)\)
- \(E^\circ = +1.07 \, \text{V}\)

### Fill in the Blanks

- **__________ is being oxidized.**
- **__________ is being reduced.**
- **__________ is acting as a reducing agent.**
- **__________ is acting as an oxidizing agent.**
- **__________ moles of electrons are transferred.**
- **The reaction is a(n) __________ cell.**

### Options:

- \(\text{Br}_2(l)\)
- \(\text{Pb}(s)\)
- 6
- \(\text{HSO}_4^-(aq)\)
- electrolytic
- \(\text{H}^+(aq)\)
- 2
- 3
- 4
- \(\text{PbSO}_4(s)\)
- voltaic
- 1
- \(\text{Br}^-(aq)\)
- 5

This exercise involves understanding the components of a redox reaction, identifying oxidation and reduction processes, and determining the type of electrochemical cell involved. The options provided are used to complete the statements regarding the redox reaction.

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