**Galvanic Cell Powered by a Redox Reaction**A galvanic cell is powered by the following redox reaction:\[ 2 \text{Zn}^{2+} (aq) + \text{N}_2\text{H}_4(aq) + 4 \text{OH}^- (aq) \rightarrow 2 \text{Zn} (s) + \text{N}_2 (g) + 4 \text{H}_2\text{O} (l) \]Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS *Data* tab.---1. **Write a balanced equation for the half-reaction that takes place at the cathode.** \[ \square \]2. **Write a balanced equation for the half-reaction that takes place at the anode.** \[ \square \]3. **Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places.** \[ E^0 = \square \text{ V} \]---**Diagram Explanation:**- The diagram on the right displays small icons representing reactions and processes related to electrons (e.g., electron transfer). The first icon shows a small arrow pointing to the right, next to boxes representing substances involved in the cell. Below, an electron symbol (\(e^-\)) is used to denote electron flow. There are also symbols for resetting or canceling input actions.

In Galvanic cell, Oxidation takes place at anode and reduction takes place at cathode. E°cell =…

A galvanic cell is powered by the following redox reaction: 2+ 2 Zn (aq) + N₂H4(aq) + 4OH (aq) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places. 0 E = v - 2 Zn(s) + N₂(g) + 4H₂O(1) ローロ X

A galvanic cell is powered by the following redox reaction: 2+ 2 Zn (aq) + N₂H4(aq) + 4OH (aq) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places. 0 E = v - 2 Zn(s) + N₂(g) + 4H₂O(1) ローロ X

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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