Homework Help is Here – Start Your Trial Now!
Science
Chemistry
We can use the Nernst equation to find E from Q and vice versa. Therefore, if you know the Ksp of a salt, you can use it to find the cell potential. Imagine a concentration cell in which one half-cell has a silver electrode in a saturated solution of Ag2SO4 and the other half-cell is a silver electrode in a 0.5 M solution of AGNO3. Use 310 K as the temperature, F = 96485 C/mol, R = 8.314 J/ mol K 1. Given that Ksp of silver sulphate is 1.2 x 10-5, what is the concentration of Ag+ in the saturated solution? 2. The cell notation can be written as: Ag(S) || Ag+(aq) (saturated conc.) || Ag+ (aq) (0.5M) || Ag(s) Use the Nernst equation to solve for Ecell under these conditions. 3. Write the chemical equation for the precipitation of A92SO4, and use Ksp to solve for Delta G°

We can use the Nernst equation to find E from Q and vice versa. Therefore, if you know the Ksp of a salt, you can use it to find the cell potential. Imagine a concentration cell in which one half-cell has a silver electrode in a saturated solution of Ag2SO4 and the other half-cell is a silver electrode in a 0.5 M solution of AGNO3. Use 310 K as the temperature, F = 96485 C/mol, R = 8.314 J/ mol K 1. Given that Ksp of silver sulphate is 1.2 x 10-5, what is the concentration of Ag+ in the saturated solution? 2. The cell notation can be written as: Ag(S) || Ag+(aq) (saturated conc.) || Ag+ (aq) (0.5M) || Ag(s) Use the Nernst equation to solve for Ecell under these conditions. 3. Write the chemical equation for the precipitation of A92SO4, and use Ksp to solve for Delta G°

Chemistry
Chemistry
9th Edition
ISBN:9781133611097
Author:Steven S. Zumdahl
Publisher:Steven S. Zumdahl
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 83E: Consider a concentration cell that has both electrodes made of some metal M. Solution A in one...
See similar textbooks
icon
Related questions
Question
Chemistry -Please answer all 5 questions: We can use the Nernst equation to find E from Q and vice versa. Therefore, if you know the Ksp of a salt, you can use it to find the cell potential. Imagine a concentration cell in which one half-cell has a silver electrode in a saturated solution of Ag2SO4 and the other half-cel is a silver electrode in a 0.5 M solution of AGNO3. Use 310 K as the temperature, F = 96485 C/mol, R = 8.314 J/ mol K 1. Given that Ksp of silver sulphate is 1.2 x 10-5, what is the concentration of Ag+ in the saturated solution? 2. The cell notation can be written as: Ag(S) || Ag+(aq) (saturated conc.) || Ag+ (aq) (0.5M) || Ag(s) Use the Nernst equation to solve for Ecell under these conditions. 3. Write the chemical equation for the precipitation of A92SO4, and use Ksp to solve for Delta G° 4. Using the thermodynamic values given, calculate Delta H° and Delta S° for the precipitation reaction at 310 K. Delta H° kJ/mol. Delta S° J/mol-K Ag+ (ag). 105. 78 S042- (aa). -909. 25.1 AgaS04 (s). -716. 203 5. At what temperature does the spontaneity reverse? If there isn't a temperature at which this occurs, explain why not.
Transcribed Image Text:Chemistry -Please answer all 5 questions: We can use the Nernst equation to find E from Q and vice versa. Therefore, if you know the Ksp of a salt, you can use it to find the cell potential. Imagine a concentration cell in which one half-cell has a silver electrode in a saturated solution of Ag2SO4 and the other half-cel is a silver electrode in a 0.5 M solution of AGNO3. Use 310 K as the temperature, F = 96485 C/mol, R = 8.314 J/ mol K 1. Given that Ksp of silver sulphate is 1.2 x 10-5, what is the concentration of Ag+ in the saturated solution? 2. The cell notation can be written as: Ag(S) || Ag+(aq) (saturated conc.) || Ag+ (aq) (0.5M) || Ag(s) Use the Nernst equation to solve for Ecell under these conditions. 3. Write the chemical equation for the precipitation of A92SO4, and use Ksp to solve for Delta G° 4. Using the thermodynamic values given, calculate Delta H° and Delta S° for the precipitation reaction at 310 K. Delta H° kJ/mol. Delta S° J/mol-K Ag+ (ag). 105. 78 S042- (aa). -909. 25.1 AgaS04 (s). -716. 203 5. At what temperature does the spontaneity reverse? If there isn't a temperature at which this occurs, explain why not.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 4 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Electrochemical Cells
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.
Similar questions
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781133611097
Author:
Steven S. Zumdahl
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Principles of Modern Chemistry
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
General Chemistry - Standalone book (MindTap Cour…
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
SEE MORE TEXTBOOKS