The free energy change for the following reaction at 25 °C, when [H+] = 1.15 M and [Co²+] = 0.00897 M, is -66.1 kJ: 2H+ (1.15 M) + Co(s) → H₂(g) + Co²+ (0.00897 M) What is the cell potential for the reaction as written under these conditions? Ecell AG=-66.1 kJ 1 V Would this reaction be spontaneous in the forward or the reverse direction? O forward direction O reverse direction
The free energy change for the following reaction at 25 °C, when [H+] = 1.15 M and [Co²+] = 0.00897 M, is -66.1 kJ: 2H+ (1.15 M) + Co(s) → H₂(g) + Co²+ (0.00897 M) What is the cell potential for the reaction as written under these conditions? Ecell AG=-66.1 kJ 1 V Would this reaction be spontaneous in the forward or the reverse direction? O forward direction O reverse direction
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 18.44QE: For each of the reactions, calculate E from the table of standard potentials, and state whether the...
Related questions
Question
100%
![The free energy change for the following reaction at 25 °C, when [H+] = 1.15 M and
[Co²+] = = 0.00897 M, is -66.1 kJ:
2H+ (1.15 M) + Co(s) → H₂(g) + Co²+ (0.00897 M)
What is the cell potential for the reaction as written under these conditions?
Ecell
AG=-66.1 kJ
=
V
Would this reaction be spontaneous in the forward or the reverse direction?
O forward direction
O reverse direction](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F44bcc854-a672-4b6c-b0fb-367be49d6297%2F280245e4-be3c-4732-99f1-c21fd0b373c8%2Fqh5z7nm_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The free energy change for the following reaction at 25 °C, when [H+] = 1.15 M and
[Co²+] = = 0.00897 M, is -66.1 kJ:
2H+ (1.15 M) + Co(s) → H₂(g) + Co²+ (0.00897 M)
What is the cell potential for the reaction as written under these conditions?
Ecell
AG=-66.1 kJ
=
V
Would this reaction be spontaneous in the forward or the reverse direction?
O forward direction
O reverse direction
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 4 steps with 4 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:
9781938168390
Author:
Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:
OpenStax
Physical Chemistry
Chemistry
ISBN:
9781133958437
Author:
Ball, David W. (david Warren), BAER, Tomas
Publisher:
Wadsworth Cengage Learning,
Chemistry: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:
9781938168390
Author:
Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:
OpenStax
Physical Chemistry
Chemistry
ISBN:
9781133958437
Author:
Ball, David W. (david Warren), BAER, Tomas
Publisher:
Wadsworth Cengage Learning,
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
General Chemistry - Standalone book (MindTap Cour…
Chemistry
ISBN:
9781305580343
Author:
Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:
Cengage Learning
