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A galvanic cell is powered by the following redox reaction: 2CrO2−4(aq) + 8H2O(l) + 3Zn(s)→  2CrOH3(s) + 10OH−(aq) + 3Zn2+(aq) 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.

A galvanic cell is powered by the following redox reaction: 2CrO2−4(aq) + 8H2O(l) + 3Zn(s)→  2CrOH3(s) + 10OH−(aq) + 3Zn2+(aq) 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.

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
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A galvanic cell is powered by the following redox reaction:

2CrO2−4(aq) + 8H2O(l) + 3Zn(s)→  2CrOH3(s) + 10OH−(aq) + 3Zn2+(aq)

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.

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