A concentration cell based on the following half reaction at 313 K Ag* + e¯ → Ag; SRP=0.80V is made from two 1.00 L solutions of Ag*, 1.32 M and 0.269 M; two 100.0 g pieces of Ag metal, a wire, and a salt bridge. Under these conditions the potential of the cell is 0.042902 V. How much Ag metal will need to be oxidized for the potential of the cell to decrease by 0.026938 V? Give your answer to 3 decimal places. 0.1 e x0% (6)

A concentration cell based on the following half reaction at 313 K Ag* + e¯ → Ag; SRP=0.80V is made from two 1.00 L solutions of Ag*, 1.32 M and 0.269 M; two 100.0 g pieces of Ag metal, a wire, and a salt bridge. Under these conditions the potential of the cell is 0.042902 V. How much Ag metal will need to be oxidized for the potential of the cell to decrease by 0.026938 V? Give your answer to 3 decimal places. 0.1 e x0% (6)

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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