With a clear explanation, find the standard cell potential, the standard change in free energy, and the equilibrium constant for the forward reaction described by the balanced chemical equation below. 3 Fe2-(aq) + Cr3+(ag) = Cr(s) + 3 Fe3-(aq)
With a clear explanation, find the standard cell potential, the standard change in free energy, and the equilibrium constant for the forward reaction described by the balanced chemical equation below. 3 Fe2-(aq) + Cr3+(ag) = Cr(s) + 3 Fe3-(aq)
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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please explain. thank you
Transcribed Image Text:With a clear explanation, find the standard cell potential, the standard change in free
energy, and the equilibrium constant for the forward reaction described by the balanced
chemical equation below.
3 Fe2+(aq) + Cr3+(aq) = Cr(s) + 3 Fe3-(aq)
Expert Solution
Step 1
The balanced reaction taking place is is,
=> 3 Fe2+ (aq) + Cr3+ (aq) -------> Cr (s) + 3 Fe3+ (aq)
Step 2
In the above reaction, the oxidation of Fe2+ to Fe3+ is taking place and reduction of Cr3+ to Cr.
Hence the standard cell potential of the reaction is given by,
=> Eocell = Eored Cr3+/Cr - Eored Fe3+/Fe2+
where Eored Cr3+/Cr = standard reduction potential of Cr3+ to Cr = -0.74 V (using appendix)
And Eored Fe3+/Fe2+ = standard reduction potential of Fe2+ to Fe3+ = -0.77 V
Hence substituting the values e get,
=> Eocell = -0.74 - (-0.77) = 0.03 V
Hence the standard cell potential is 0.03 V.
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