The free energy change for the following reaction at 25 °C, when [Ag*]= 1.16 M and [Cd²+]= 3.49×10-3 M, is -246 kJ:2Ag*(1.16 M) + Cd(s)→2Ag(s) + Cd²+(3.49×10-3 M)AG = -246 kJWhat is the cell potential for the reaction as written under these conditions?Answer:VWould this reaction be spontaneous in the forward or the reverse direction?

Answered: Image /qna-images/answer/4bd0f36a-a914-4356-a628-27058b5b55f9.jpg

The free energy change for the following reaction at 25 °C, when [Ag*]= 1.16 M and [Cd²+]= 3.49×10-3 M, is -246 kJ: 2Ag*(1.16 M) + Cd(s)→2Ag(s) + Cd²+(3.49×10-3 M) AG = -246 kJ

The free energy change for the following reaction at 25 °C, when [Ag]= 1.16 M and [Cd²+]= 3.49×10-3 M, is -246 kJ: 2Ag(1.16 M) + Cd(s)→2Ag(s) + Cd²+(3.49×10-3 M) AG = -246 kJ

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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The free energy change for the following reaction at 25 °C, when [Ag*]= 1.16 M and [Cd²+]= 3.49×10-3 M, is -246 kJ:
2Ag*(1.16 M) + Cd(s)→2Ag(s) + Cd²+(3.49×10-3 M)
AG = -246 kJ
What is the cell potential for the reaction as written under these conditions?
Answer:
V
Would this reaction be spontaneous in the forward or the reverse direction?

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