4) The Zn/Cu battery operates using the following redox reactions:Cu + 2e- → Cu(0) E° = 0.34VZn + 2e- → Zn E° = -0.76Va) What is the cell potential E for ion concentrations [Cu?+]=0.02M and [Zn²+]=0.05M?(assume all activity coefficients y = 1)b) If an external voltage of Et = -1.0 V, is applied to the cell, what is the equilibriumconcentration of Zn²+ ions if [Cu²*]«q=0.001M? (assume all activity coefficients y = 1)c) An alkaline battery utilizes the following overall reactionZn(s) + 2MnO2(s) → Zn0(s) + Mn2Os(s)unlike the Zn/Cu battery, the cell potential of the alkaline battery does not change as thebattery discharges. Explain why this is based on the Nernst equation.

Zn2+(aq) + 2e- -> Zn(s) Eo = -0.76 Cu2+(aq) + 2e- -> Cu(s) Eo = 0.34…

4) The Zn/Cu battery operates using the following redox reactions: + 2e → Cu) E° = 0.34V Cua Zn + 2e → Zn E° = -0.76V a) What is the cell potential E for ion concentrations [Cu²+]=0.02M and [Zn²+]=0.05M? (assume all activity coefficients y = 1)

4) The Zn/Cu battery operates using the following redox reactions: + 2e → Cu) E° = 0.34V Cua Zn + 2e → Zn E° = -0.76V a) What is the cell potential E for ion concentrations [Cu²+]=0.02M and [Zn²+]=0.05M? (assume all activity coefficients y = 1)

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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