The free energy change for the following reaction at 25 °C, when [Cr**]= 2.80×10-3 M and [H*]= 1.11 M, is 94.0 kJ: 2Cr**(2.80x10 M) + H,(g)2Cr*+*(aq) + 2.00H*(1.11 M) AG=94.0 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?
The free energy change for the following reaction at 25 °C, when [Cr**]= 2.80×10-3 M and [H*]= 1.11 M, is 94.0 kJ: 2Cr**(2.80x10 M) + H,(g)2Cr*+*(aq) + 2.00H*(1.11 M) AG=94.0 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?
Chemistry by OpenStax (2015-05-04)
1st Edition
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 [Cr**]= 2.80×103
M and [H= 1.11 M, is 94.0 kJ:
2Cr*(2.80×10³ M) + H,(g)2Cr*(aq) + 2.00H*(1.11 M)
AG = 94.0 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%2F49010e4c-a840-42bd-99dd-c27d32350ecc%2Ff747b054-a050-42bc-83a4-d29a39afc4b5%2Fefqn7u7_processed.png&w=3840&q=75)
Transcribed Image Text:The free energy change for the following reaction at 25 °C, when [Cr**]= 2.80×103
M and [H= 1.11 M, is 94.0 kJ:
2Cr*(2.80×10³ M) + H,(g)2Cr*(aq) + 2.00H*(1.11 M)
AG = 94.0 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?
![The free energy change for the following reaction at 25 °C, when [Pb4*1=1.15 M and
[Fe?+] = 5.40x10-3 M, is -73.9 kJ:
Pb2
(1.15 M) + Fe(s)– Pb(s) + Fe²*(5.40×10 M) AG = -73.9 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%2F49010e4c-a840-42bd-99dd-c27d32350ecc%2Ff747b054-a050-42bc-83a4-d29a39afc4b5%2Fmtvpcml_processed.png&w=3840&q=75)
Transcribed Image Text:The free energy change for the following reaction at 25 °C, when [Pb4*1=1.15 M and
[Fe?+] = 5.40x10-3 M, is -73.9 kJ:
Pb2
(1.15 M) + Fe(s)– Pb(s) + Fe²*(5.40×10 M) AG = -73.9 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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