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A concentration of cell based on the following half reaction at 288K Cu²+ + 2e → Cu; Eº = 0.34V Is made from two 1.00L solution of Cu²+, 1.23M and 0.25M; two 100.0g pieces of Cu metal, a wire, and a salt bridge. Under these conditions the potential of the cell is 0.01977 V. How much Cu metal will need to be oxidized for the potential of the cell to decrease by 0.0092966V?

A concentration of cell based on the following half reaction at 288K Cu²+ + 2e → Cu; Eº = 0.34V Is made from two 1.00L solution of Cu²+, 1.23M and 0.25M; two 100.0g pieces of Cu metal, a wire, and a salt bridge. Under these conditions the potential of the cell is 0.01977 V. How much Cu metal will need to be oxidized for the potential of the cell to decrease by 0.0092966V?

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
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9. A concentration of cell based on the following half reaction at 288K Cu²+ + 2e → Cu; E° = 0.34V Is made from two 1.00L solution of Cu²+, 1.23M and 0.25M; two 100.0g pieces of Cu metal, a wire, and a salt bridge. Under these conditions the potential of the cell is 0.01977 V. How much Cu metal will need to be oxidized for the potential of the cell to decrease by 0.0092966V?
Transcribed Image Text:9. A concentration of cell based on the following half reaction at 288K Cu²+ + 2e → Cu; E° = 0.34V Is made from two 1.00L solution of Cu²+, 1.23M and 0.25M; two 100.0g pieces of Cu metal, a wire, and a salt bridge. Under these conditions the potential of the cell is 0.01977 V. How much Cu metal will need to be oxidized for the potential of the cell to decrease by 0.0092966V?
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