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 by OpenStax (2015-05-04)
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ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 24E: For each reaction listed, determine its standard cell potential at 25 C and whether the reaction is...
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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?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb2c2bfdd-c795-4c13-bc09-4b743040f0d9%2F4bd0f36a-a914-4356-a628-27058b5b55f9%2F8ngx3y_processed.png&w=3840&q=75)
Transcribed Image Text: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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