5. Calculate the cell potential (in volts) at 298.15 K of the following electrochemical cell below if themolal concentration of ZnCl2 is 0.03 mol/kg. Assume a non-ideal solution on the formation of ZnCl2. Usethe Davies equation to estimate the activity coefficient. In your solution, indicate the value of theactivity coefficient.Zns)Zn2+ + 2e-AgCls) + e-Ags) + Cl-Cell potentials:Zn(s)Zn2+ + 2e- (-0.762 V)AgCls) + e- →Ag(s) + Cl- (0.2222 V)A. 0.984 VB. 1.02 VС. 1.12 VD. 0.946 VЕ. 1.21 V

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Answered: 5. Calculate the cell potential (in…

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5. Calculate the cell potential (in volts) at 298.15 K of the following electrochemical cell below if th

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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5. Calculate the cell potential (in volts) at 298.15 K of the following electrochemical cell below if the
molal concentration of ZnCl2 is 0.03 mol/kg. Assume a non-ideal solution on the formation of ZnCl2. Use
the Davies equation to estimate the activity coefficient. In your solution, indicate the value of the
activity coefficient.
Zns)
Zn2+ + 2e-
AgCls) + e-
Ags) + Cl-
Cell potentials:
Zn(s)
Zn2+ + 2e- (-0.762 V)
AgCls) + e- →
Ag(s) + Cl- (0.2222 V)
A. 0.984 V
B. 1.02 V
С. 1.12 V
D. 0.946 V
Е. 1.21 V

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