Consider the following pairs of reactions: Fe2+ (aq) + 2 e- → Fe (s) E° = – 0.44 V Au3+ (aq) + 3 e-→Au (s) E° = +1.50 V Write a balanced spontaneous reaction. Calculate the standard cell potential (E°) of the cell. Calculate the cell potential (E) when [Au3+] = 0.250 M and [Fe2+] = 0.180 M. Assume standard conditions.
Consider the following pairs of reactions: Fe2+ (aq) + 2 e- → Fe (s) E° = – 0.44 V Au3+ (aq) + 3 e-→Au (s) E° = +1.50 V Write a balanced spontaneous reaction. Calculate the standard cell potential (E°) of the cell. Calculate the cell potential (E) when [Au3+] = 0.250 M and [Fe2+] = 0.180 M. Assume standard conditions.
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter19: Principles Of Chemical Reactivity: Electron Transfer Reactions
Section: Chapter Questions
Problem 94GQ: A voltaic cell is constructed in which one half-cell consists of a silver wire in an aqueous...
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Question
Consider the following pairs of reactions:
Fe2+ (aq) + 2 e- → Fe (s) E° = – 0.44 V
Au3+ (aq) + 3 e-→Au (s) E° = +1.50 V
-
Write a balanced spontaneous reaction.
-
Calculate the standard cell potential (E°) of the cell.
-
Calculate the cell potential (E) when [Au3+] = 0.250 M and [Fe2+] = 0.180 M. Assume standard conditions.
-
What is the value of ΔG° (in kJ/mol) for the reaction?
-
Write the shorthand notation for the cell.
-
Identify the:
Oxidizing agent: _______
Reducing agent: _______
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