What is the calculated value of the cell potential 298 K for an electrochemical cell with the following reaction, when the Ag concentration is 5.86 x 10-4 M and the Zn²+ concentration is 1.34 M? 2Ag (aq) + Zn(s)→ 2Ag(s) + Zn²+ (aq) Ag+ (aq) + e → Ag(s) E = 0.799 V =-0.763 V red Zn²+ (aq) + 2e → Zn(s) Ee red Ecell = The cell reaction as written above is spontaneous for the concentrations given: Otrue Ofalse V

What is the calculated value of the cell potential 298 K for an electrochemical cell with the following reaction, when the Ag concentration is 5.86 x 10-4 M and the Zn²+ concentration is 1.34 M? 2Ag (aq) + Zn(s)→ 2Ag(s) + Zn²+ (aq) Ag+ (aq) + e → Ag(s) E = 0.799 V =-0.763 V red Zn²+ (aq) + 2e → Zn(s) Ee red Ecell = The cell reaction as written above is spontaneous for the concentrations given: Otrue Ofalse V

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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