Pt | H₂ (0.50 atm) | H+ (0.10 M) || MnO4- (0.10 M), Mn²+ (1.0 M), H* (0.10 M) | Pt 2H+ + 2e →→ H₂ Eº = 0.00 V Eº = -0.80 V MnO4 + 8H+ + 5e-→Mn²+ + 4H₂O a. Write the balanced chemical equation for the above redox reaction. Calculate the cell potential of the cell. b. C. Determine the free energy change for the overall redox reaction in the cell.
Pt | H₂ (0.50 atm) | H+ (0.10 M) || MnO4- (0.10 M), Mn²+ (1.0 M), H* (0.10 M) | Pt 2H+ + 2e →→ H₂ Eº = 0.00 V Eº = -0.80 V MnO4 + 8H+ + 5e-→Mn²+ + 4H₂O a. Write the balanced chemical equation for the above redox reaction. Calculate the cell potential of the cell. b. C. Determine the free energy change for the overall redox reaction in the cell.
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
Chapter18: Principles Of Chemical Reactivity: Entropy And Free Energy
Section: Chapter Questions
Problem 44PS
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Question
Consider the following.
![Pt | H₂ (0.50 atm) | H* (0.10 M) || MnO4- (0.10 M), Mn²+ (1.0 M), H* (0.10 M) | Pt
2H+ + 2e →→ H₂
Eº = 0.00 V
Eº = -0.80 V
MnO4 + 8H+ + 5e-→Mn²+ + 4H₂O
a. Write the balanced chemical equation for the above redox reaction.
b. Calculate the cell potential of the cell.
C.
Determine the free energy change for the overall redox reaction in the cell.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc28e2967-0741-42bb-bc83-5ec959491e36%2F7cb176ac-ed10-48bb-89be-8507becf15c0%2F5pinyy3_processed.png&w=3840&q=75)
Transcribed Image Text:Pt | H₂ (0.50 atm) | H* (0.10 M) || MnO4- (0.10 M), Mn²+ (1.0 M), H* (0.10 M) | Pt
2H+ + 2e →→ H₂
Eº = 0.00 V
Eº = -0.80 V
MnO4 + 8H+ + 5e-→Mn²+ + 4H₂O
a. Write the balanced chemical equation for the above redox reaction.
b. Calculate the cell potential of the cell.
C.
Determine the free energy change for the overall redox reaction in the cell.
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