Given the two half reactions below and the Table of Standard Reduction Potentials, answer the following questions: Al3+ + 3 e → Al Zn2+ + 2 e → Zn a) How many electrons are transferred in the balanced redox reaction? [ Select ] b) What is the standard cell potential (E°cell)? [ Select ]
Given the two half reactions below and the Table of Standard Reduction Potentials, answer the following questions: Al3+ + 3 e → Al Zn2+ + 2 e → Zn a) How many electrons are transferred in the balanced redox reaction? [ Select ] b) What is the standard cell potential (E°cell)? [ Select ]
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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Boxes 1-2.
box 1 answer choices: 6, 3, 5, 4, 1, or 2.
box 2 answer choices: -0.90 V, +0.90 V, +2.42 V, +1.04 V, -2.42 V, or -1.04 V.
![### Redox Reaction Analysis
**Given the two half reactions below and the Table of Standard Reduction Potentials, answer the following questions:**
**Half Reactions:**
- \( \text{Al}^{3+} + 3 \text{e}^- \rightarrow \text{Al} \)
- \( \text{Zn}^{2+} + 2 \text{e}^- \rightarrow \text{Zn} \)
---
**Questions:**
a) **How many electrons are transferred in the balanced redox reaction?**
- [Select from dropdown]
b) **What is the standard cell potential (\(E^\circ_{\text{cell}}\))?**
- [Select from dropdown]
### Discussion:
To solve these questions, refer to the Table of Standard Reduction Potentials to find \(E^\circ\) values for each half-reaction.
1. **Balancing Electrons:**
- The first step is to balance the number of electrons lost in the oxidation process with those gained in the reduction process.
2. **Calculating \(E^\circ_{\text{cell}}\):**
- Use the formula \(E^\circ_{\text{cell}} = E^\circ_{\text{cathode}} - E^\circ_{\text{anode}}\).
**Note:** The specific values are needed for calculations, which should be obtained from the standard reduction potential table.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F587f9f8f-b9b6-467a-a476-89151f1449a5%2F1173c7ad-47d6-4584-b78a-53a37686f098%2Fsdel32_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Redox Reaction Analysis
**Given the two half reactions below and the Table of Standard Reduction Potentials, answer the following questions:**
**Half Reactions:**
- \( \text{Al}^{3+} + 3 \text{e}^- \rightarrow \text{Al} \)
- \( \text{Zn}^{2+} + 2 \text{e}^- \rightarrow \text{Zn} \)
---
**Questions:**
a) **How many electrons are transferred in the balanced redox reaction?**
- [Select from dropdown]
b) **What is the standard cell potential (\(E^\circ_{\text{cell}}\))?**
- [Select from dropdown]
### Discussion:
To solve these questions, refer to the Table of Standard Reduction Potentials to find \(E^\circ\) values for each half-reaction.
1. **Balancing Electrons:**
- The first step is to balance the number of electrons lost in the oxidation process with those gained in the reduction process.
2. **Calculating \(E^\circ_{\text{cell}}\):**
- Use the formula \(E^\circ_{\text{cell}} = E^\circ_{\text{cathode}} - E^\circ_{\text{anode}}\).
**Note:** The specific values are needed for calculations, which should be obtained from the standard reduction potential table.
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