The equilibrium constant, K, for a redox reaction is related to the standard potential, E, by the equation In K = nFE RT where n is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96,500 C/(mol e), R (the gas constant) is equal to 8.314 J/(mol K), and T is the Kelvin temperature. Standard reduction potentials ▶ Part A Part B Calculate the standard cell potential (E°) for the reaction Eo == Submit D μA Reduction half-reaction Ag+ (aq) + e→Ag(s) Cu²+ (aq) + 2e →Cu(s) Sn+ (aq) + 4e →Sn(s) -0.125 Previous Answers 2H+ (aq) + 2e →H₂(g) Ni2+ (aq) + 2e →Ni(s) Fe2+ (aq) + 2e →Fe(s) Zn²+ (aq) + 2e →Zn(s) Al³+ (aq) + 3e →Al(s) -1.66 Mg2+ (aq) + 2e →Mg(s) -2.37 V E° (V) 0.80 if K = 2.80x10-4. Express your answer to three significant figures and include the appropriate units. ► View Available Hint(s) 0.34 ? 0.15 X Incorrect; Try Again; 4 attempts remaining 0 -0.26 -0.45 -0.76 X(s) +Y+ (aq) →X+ (aq) + Y(s) Review | Constants I Periodic Table
The equilibrium constant, K, for a redox reaction is related to the standard potential, E, by the equation In K = nFE RT where n is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96,500 C/(mol e), R (the gas constant) is equal to 8.314 J/(mol K), and T is the Kelvin temperature. Standard reduction potentials ▶ Part A Part B Calculate the standard cell potential (E°) for the reaction Eo == Submit D μA Reduction half-reaction Ag+ (aq) + e→Ag(s) Cu²+ (aq) + 2e →Cu(s) Sn+ (aq) + 4e →Sn(s) -0.125 Previous Answers 2H+ (aq) + 2e →H₂(g) Ni2+ (aq) + 2e →Ni(s) Fe2+ (aq) + 2e →Fe(s) Zn²+ (aq) + 2e →Zn(s) Al³+ (aq) + 3e →Al(s) -1.66 Mg2+ (aq) + 2e →Mg(s) -2.37 V E° (V) 0.80 if K = 2.80x10-4. Express your answer to three significant figures and include the appropriate units. ► View Available Hint(s) 0.34 ? 0.15 X Incorrect; Try Again; 4 attempts remaining 0 -0.26 -0.45 -0.76 X(s) +Y+ (aq) →X+ (aq) + Y(s) Review | Constants I Periodic Table
General Chemistry - Standalone book (MindTap Course List)
11th Edition
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:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter19: Electrochemistry
Section: Chapter Questions
Problem 19.144QP
Related questions
Question
100%
29b
![The equilibrium constant, K, for a redox reaction is
related to the standard potential, E, by the
equation
In K =
nFE
where n is the number of moles of electrons
transferred, F (the Faraday constant) is equal to
96,500 C/(mol e), R (the gas constant) is
equal to 8.314 J/(mol K), and T is the Kelvin
temperature.
Standard reduction potentials
▶
Part A
Part B
Calculate the standard cell potential (E°) for the reaction
Eo ==
Submit
D
μA
Reduction half-reaction
Ag+ (aq) + e→Ag(s)
Cu²+ (aq) + 2e →Cu(s)
Sn+ (aq) + 4e¯→Sn(s)
2H+ (aq) + 2e →H₂(g)
Ni2+ (aq) + 2e →Ni(s)
Fe2+ (aq) + 2e →Fe(s)
0.125
Previous Answers
V
E° (V)
0.80
if K = 2.80x10-4.
Express your answer to three significant figures and include the appropriate units.
► View Available Hint(s)
0.34
?
0.15
Zn²+ (aq) +2e →Zn(s)
-0.76
Al³+ (aq) + 3e →Al(s) -1.66
Mg2+ (aq) + 2e →Mg(s) -2.37
X Incorrect; Try Again; 4 attempts remaining
0
-0.26
-0.45
X(s) + Y+ (aq) →X+ (aq) + Y(s)
Review | Constants I Periodic Table](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb0be78df-234d-4653-8235-8227b9098990%2Fe4dd22b4-01de-4214-afee-86fddd6f192f%2Fc8lloxn_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The equilibrium constant, K, for a redox reaction is
related to the standard potential, E, by the
equation
In K =
nFE
where n is the number of moles of electrons
transferred, F (the Faraday constant) is equal to
96,500 C/(mol e), R (the gas constant) is
equal to 8.314 J/(mol K), and T is the Kelvin
temperature.
Standard reduction potentials
▶
Part A
Part B
Calculate the standard cell potential (E°) for the reaction
Eo ==
Submit
D
μA
Reduction half-reaction
Ag+ (aq) + e→Ag(s)
Cu²+ (aq) + 2e →Cu(s)
Sn+ (aq) + 4e¯→Sn(s)
2H+ (aq) + 2e →H₂(g)
Ni2+ (aq) + 2e →Ni(s)
Fe2+ (aq) + 2e →Fe(s)
0.125
Previous Answers
V
E° (V)
0.80
if K = 2.80x10-4.
Express your answer to three significant figures and include the appropriate units.
► View Available Hint(s)
0.34
?
0.15
Zn²+ (aq) +2e →Zn(s)
-0.76
Al³+ (aq) + 3e →Al(s) -1.66
Mg2+ (aq) + 2e →Mg(s) -2.37
X Incorrect; Try Again; 4 attempts remaining
0
-0.26
-0.45
X(s) + Y+ (aq) →X+ (aq) + Y(s)
Review | Constants I Periodic Table
Expert Solution
![](/static/compass_v2/shared-icons/check-mark.png)
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 3 steps with 1 images
![Blurred answer](/static/compass_v2/solution-images/blurred-answer.jpg)
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
![General Chemistry - Standalone book (MindTap Cour…](https://www.bartleby.com/isbn_cover_images/9781305580343/9781305580343_smallCoverImage.gif)
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
![Chemistry: Principles and Practice](https://www.bartleby.com/isbn_cover_images/9780534420123/9780534420123_smallCoverImage.gif)
Chemistry: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning
![Chemistry: The Molecular Science](https://www.bartleby.com/isbn_cover_images/9781285199047/9781285199047_smallCoverImage.gif)
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
![General Chemistry - Standalone book (MindTap Cour…](https://www.bartleby.com/isbn_cover_images/9781305580343/9781305580343_smallCoverImage.gif)
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
![Chemistry: Principles and Practice](https://www.bartleby.com/isbn_cover_images/9780534420123/9780534420123_smallCoverImage.gif)
Chemistry: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning
![Chemistry: The Molecular Science](https://www.bartleby.com/isbn_cover_images/9781285199047/9781285199047_smallCoverImage.gif)
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
![Principles of Modern Chemistry](https://www.bartleby.com/isbn_cover_images/9781305079113/9781305079113_smallCoverImage.gif)
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
![Chemistry by OpenStax (2015-05-04)](https://www.bartleby.com/isbn_cover_images/9781938168390/9781938168390_smallCoverImage.gif)
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:
9781938168390
Author:
Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:
OpenStax
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning