The free energy change for the following reaction at 25 °C, when [H]= 3.34×103 M and [Hg**]= 1.15 M, is 180. kJ: 2H*(3.34×103 M) – Hg() H2(g) - Hg*1.15 M) AG = 180. kJ What is the cell potential for the reaction as written under these conditions? Answer: -0.932 |v Would this reaction be spontaneous in the forward or the reverse direction? forward v
The free energy change for the following reaction at 25 °C, when [H]= 3.34×103 M and [Hg**]= 1.15 M, is 180. kJ: 2H*(3.34×103 M) – Hg() H2(g) - Hg*1.15 M) AG = 180. kJ What is the cell potential for the reaction as written under these conditions? Answer: -0.932 |v Would this reaction be spontaneous in the forward or the reverse direction? forward v
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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![The free energy change for the following reaction at 25 °C, when [H*] = 3.34x103 M and [Hg*] = 1.15 M, is 180. kJ:
2H*(3.34x10-3 M) + Hg() H2(g) + Hg²*(1.15 M) AG = 180. kJ
What is the cell potential for the reaction as written under these conditions?
Answer: -0.932
Would this reaction be spontaneous in the forward or the reverse direction? forward v](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd5ecb641-0fa2-4271-99ab-dc511ca048ad%2Fc258fea3-6caf-4068-afc1-26d26dd501f5%2F6jwlyka_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The free energy change for the following reaction at 25 °C, when [H*] = 3.34x103 M and [Hg*] = 1.15 M, is 180. kJ:
2H*(3.34x10-3 M) + Hg() H2(g) + Hg²*(1.15 M) AG = 180. kJ
What is the cell potential for the reaction as written under these conditions?
Answer: -0.932
Would this reaction be spontaneous in the forward or the reverse direction? forward v
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