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A chemist designs a galvanic cell that uses these two half-reactions: 2+ Zn (aq) +2e MnO4(aq) + 2 H₂O(1)+3e Write a balanced equation for the half-reaction that happens at the cathode. half-reaction Write a balanced equation for the half-reaction that happens at the anode. Answer the following questions about this cell. 0 Zn(s) MnO₂(s)+4OH (aq) standard reduction potential E-0.763 V red Ed=+0.59 V 'red

A chemist designs a galvanic cell that uses these two half-reactions: 2+ Zn (aq) +2e MnO4(aq) + 2 H₂O(1)+3e Write a balanced equation for the half-reaction that happens at the cathode. half-reaction Write a balanced equation for the half-reaction that happens at the anode. Answer the following questions about this cell. 0 Zn(s) MnO₂(s)+4OH (aq) standard reduction potential E-0.763 V red Ed=+0.59 V 'red

Chemistry
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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A chemist designs a galvanic cell that uses these two half-reactions: | half-reaction | standard reduction potential | |-------------------------------------------------|-------------------------------------| | \( \text{Zn}^{2+}(aq) + 2e^- \rightarrow \text{Zn}(s) \) | \( E^\circ_{\text{red}} = -0.763 \, \text{V} \) | | \( \text{MnO}_4^-(aq) + 2 \text{H}_2\text{O}(l) + 3e^- \rightarrow \text{MnO}_2(s) + 4 \text{OH}^-(aq) \) | \( E^\circ_{\text{red}} = +0.59 \, \text{V} \) | Answer the following questions about this cell. 1. Write a balanced equation for the half-reaction that happens at the cathode. [Cathode space for answer] 2. Write a balanced equation for the half-reaction that happens at the anode. [Anode space for answer]
Transcribed Image Text:A chemist designs a galvanic cell that uses these two half-reactions: | half-reaction | standard reduction potential | |-------------------------------------------------|-------------------------------------| | \( \text{Zn}^{2+}(aq) + 2e^- \rightarrow \text{Zn}(s) \) | \( E^\circ_{\text{red}} = -0.763 \, \text{V} \) | | \( \text{MnO}_4^-(aq) + 2 \text{H}_2\text{O}(l) + 3e^- \rightarrow \text{MnO}_2(s) + 4 \text{OH}^-(aq) \) | \( E^\circ_{\text{red}} = +0.59 \, \text{V} \) | Answer the following questions about this cell. 1. Write a balanced equation for the half-reaction that happens at the cathode. [Cathode space for answer] 2. Write a balanced equation for the half-reaction that happens at the anode. [Anode space for answer]
### Electrochemical Cell Analysis **Task 1: Write a balanced equation for the overall reaction that powers the cell.** - Ensure the reaction is spontaneous as written. - **Input box provided for the equation.** **Task 2: Determine if you have enough information to calculate the cell voltage under standard conditions.** - Options: - ○ Yes - ○ No **Task 3: If it is possible to calculate the cell voltage, perform the calculation.** - Enter your answer in the provided space. - Ensure the answer is rounded to 3 significant digits. - **Input box provided for the voltage calculation (V).**
Transcribed Image Text:### Electrochemical Cell Analysis **Task 1: Write a balanced equation for the overall reaction that powers the cell.** - Ensure the reaction is spontaneous as written. - **Input box provided for the equation.** **Task 2: Determine if you have enough information to calculate the cell voltage under standard conditions.** - Options: - ○ Yes - ○ No **Task 3: If it is possible to calculate the cell voltage, perform the calculation.** - Enter your answer in the provided space. - Ensure the answer is rounded to 3 significant digits. - **Input box provided for the voltage calculation (V).**
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