A chemist designs a galvanic cell that uses these two half-reactions: MnO₂(aq) +8 H (aq)+5e¯ →Mn(aq) + 4H₂O(1) Fe³+ (aq) +e → Fe²+ (aq) Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do you have enough information to calculate the cell voltage under standard conditions? If you said it was possible to calculate the cell voltage, do so and half-reaction enter your answer here. Be sure your answer has the correct number of significant digits. 0 Yes No standard reduction potential = +1.51 V E Ered = +0.771 V 0-0 00 la X 20 3
A chemist designs a galvanic cell that uses these two half-reactions: MnO₂(aq) +8 H (aq)+5e¯ →Mn(aq) + 4H₂O(1) Fe³+ (aq) +e → Fe²+ (aq) Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do you have enough information to calculate the cell voltage under standard conditions? If you said it was possible to calculate the cell voltage, do so and half-reaction enter your answer here. Be sure your answer has the correct number of significant digits. 0 Yes No standard reduction potential = +1.51 V E Ered = +0.771 V 0-0 00 la X 20 3
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![### Galvanic Cell Design and Analysis
A chemist designs a galvanic cell that uses these two half-reactions:
| half-reaction | standard reduction potential |
|--------------------------------------------------|-----------------------------------------------|
| \( \text{MnO}_4^- (aq) + 8 \text{H}^+ (aq) + 5e^- \rightarrow \text{Mn}^{2+} (aq) + 4 \text{H}_2\text{O} (l) \) | \( E_{\text{red}}^0 = +1.51 \, \text{V} \) |
| \( \text{Fe}^{3+} (aq) + e^- \rightarrow \text{Fe}^{2+} (aq) \) | \( E_{\text{red}}^0 = +0.771 \, \text{V} \) |
Answer the following questions about this cell:
1. **Write a balanced equation for the half-reaction that happens at the cathode.**
\[ \boxed{} \]
2. **Write a balanced equation for the half-reaction that happens at the anode.**
\[ \boxed{} \]
3. **Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.**
\[ \boxed{} \]
4. **Do you have enough information to calculate the cell voltage under standard conditions?**
- [ ] Yes
- [ ] No
5. **If you said it was possible to calculate the cell voltage, do so and enter your answer here. Be sure your answer has the correct number of significant digits.**
\[ \boxed{} \, \text{V} \]
#### Explanation of Tables and Diagrams:
- The table lists two half-reactions involved in the galvanic cell and their associated standard reduction potentials. The standard reduction potential indicates the tendency of a species to gain electrons and be reduced.
- Each half-reaction is described with species involved and the number of electrons transferred.
This exercise is designed to test your understanding of galvanic cells, including writing balanced half-reactions, determining the overall cell reaction, and calculating the cell voltage under standard conditions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F12c0a0e9-4d98-45bb-8c42-bb6fd08d9097%2Ff5789e80-13f8-45d9-86ca-f2655b3134b0%2F7o29rvf_processed.png&w=3840&q=75)
Transcribed Image Text:### Galvanic Cell Design and Analysis
A chemist designs a galvanic cell that uses these two half-reactions:
| half-reaction | standard reduction potential |
|--------------------------------------------------|-----------------------------------------------|
| \( \text{MnO}_4^- (aq) + 8 \text{H}^+ (aq) + 5e^- \rightarrow \text{Mn}^{2+} (aq) + 4 \text{H}_2\text{O} (l) \) | \( E_{\text{red}}^0 = +1.51 \, \text{V} \) |
| \( \text{Fe}^{3+} (aq) + e^- \rightarrow \text{Fe}^{2+} (aq) \) | \( E_{\text{red}}^0 = +0.771 \, \text{V} \) |
Answer the following questions about this cell:
1. **Write a balanced equation for the half-reaction that happens at the cathode.**
\[ \boxed{} \]
2. **Write a balanced equation for the half-reaction that happens at the anode.**
\[ \boxed{} \]
3. **Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.**
\[ \boxed{} \]
4. **Do you have enough information to calculate the cell voltage under standard conditions?**
- [ ] Yes
- [ ] No
5. **If you said it was possible to calculate the cell voltage, do so and enter your answer here. Be sure your answer has the correct number of significant digits.**
\[ \boxed{} \, \text{V} \]
#### Explanation of Tables and Diagrams:
- The table lists two half-reactions involved in the galvanic cell and their associated standard reduction potentials. The standard reduction potential indicates the tendency of a species to gain electrons and be reduced.
- Each half-reaction is described with species involved and the number of electrons transferred.
This exercise is designed to test your understanding of galvanic cells, including writing balanced half-reactions, determining the overall cell reaction, and calculating the cell voltage under standard conditions.
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