3. Calculate the concentration of the chromic ion in the cell which has an electrode potential of 0.688 at 298.15 K for the given reaction: Cr20, 2- (aq) + 14 H* (aq) + 61-1 (aq) → 2 Cr ³"(aq) + 31z{s) +7 H2OM When [Cr20, 2-] = 2.25 M; [H*] = 1.0 M ; [1-1] = 1.0 M ; [H2O] = 1.0 x 10 -5 M %3D Calculate the Gibbs free-energy and the standard Gibbs Free-Energy occur in the system
3. Calculate the concentration of the chromic ion in the cell which has an electrode potential of 0.688 at 298.15 K for the given reaction: Cr20, 2- (aq) + 14 H* (aq) + 61-1 (aq) → 2 Cr ³"(aq) + 31z{s) +7 H2OM When [Cr20, 2-] = 2.25 M; [H*] = 1.0 M ; [1-1] = 1.0 M ; [H2O] = 1.0 x 10 -5 M %3D Calculate the Gibbs free-energy and the standard Gibbs Free-Energy occur in the system
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter17: Electrochemistry And Its Applications
Section: Chapter Questions
Problem 50QRT
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![3. Calculate the concentration of the chromic ion in the cell which has an electrode potential of
0.688 at 298.15 K for the given reaction:
Cr20, 2- (ag) + 14 H* (aq) + 61-1 (aq) → 2 Cr 3* aq) + 312(s) + 7 H2O)
When
[Cr20, 2-] = 2.25 M; [H*] = 1.0 M ; [I-1] = 1.0 M ; [H2O] = 1.0 x 10 -5 M
%3D
Calculate the Gibbs free-energy and the standard Gibbs Free-Energy occur in the system](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3e44f20a-1df4-4428-81f4-a006a57bd27c%2F5f92e9cc-d10e-4ba8-bf08-d7993a8c943a%2F2a3b41q_processed.png&w=3840&q=75)
Transcribed Image Text:3. Calculate the concentration of the chromic ion in the cell which has an electrode potential of
0.688 at 298.15 K for the given reaction:
Cr20, 2- (ag) + 14 H* (aq) + 61-1 (aq) → 2 Cr 3* aq) + 312(s) + 7 H2O)
When
[Cr20, 2-] = 2.25 M; [H*] = 1.0 M ; [I-1] = 1.0 M ; [H2O] = 1.0 x 10 -5 M
%3D
Calculate the Gibbs free-energy and the standard Gibbs Free-Energy occur in the system
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