The free energy change for the following reaction at 25 °C, when [Zn“]= 6.68×10³ M and [H"]= 1.17 M, is 160. kJ: Zn2*(6.68x103 M) + H,(g) Zn(s) + 2H*(1.17 M) AG = 160. kJ What is the cell potential for the reaction as written under these conditions? Answer: Would this reaction be spontaneous in the forward or the reverse direction?

The free energy change for the following reaction at 25 °C, when [Zn“]= 6.68×10³ M and [H"]= 1.17 M, is 160. kJ: Zn2(6.68x103 M) + H,(g) Zn(s) + 2H(1.17 M) AG = 160. kJ What is the cell potential for the reaction as written under these conditions? Answer: Would this reaction be spontaneous in the forward or the reverse direction?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 73QAP: Consider the reaction below at 25°C: 2MnO4(aq)+16H+(aq)+10Br(aq)2Mn2+(aq)+5Br2(l)+8H2O Use Table...

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