Question 3According to the following equations.2Ag* + Zn(s) = Zn2 + 2Ag(s) where,Ag* +e = Ag(s), E° = 0.800 VZn2* + 2 e = Zn(s), E° = -0.763 VA) The E°cell =B) The standard free energy change AG° =.V.KJ/ mol.C) If the concentration of Zn²* increased, what effect does this have on cell potential? Would Ecell increase or decrease?

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Question 3 According to the following equations. 2Ag* + Zn(s) = Zn2* + 2Ag(s) where, Ag* +e = Ag(s), ° = 0.800 V Zn2* + 2 e = Zn(s) , E° = -0.763 V A) The E°cell %3D .V. B) The standard free energy change AG° = .KJ/ mol. C) If the concentration of Zn2* increased, what effect does this have on cell potential? Would Ecell increase or decrease?

Question 3 According to the following equations. 2Ag* + Zn(s) = Zn2* + 2Ag(s) where, Ag* +e = Ag(s), ° = 0.800 V Zn2* + 2 e = Zn(s) , E° = -0.763 V A) The E°cell %3D .V. B) The standard free energy change AG° = .KJ/ mol. C) If the concentration of Zn2* increased, what effect does this have on cell potential? Would Ecell increase or decrease?

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

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 122AE: The overall reaction and equilibrium constant value for a hydrogen-oxygen fuel cell at 298 K is...

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