Consider a galvanic cell for which the anode reaction is Pb(s) → Pb+2 (0.010 M) + 2e- , E= -0.1263 V And the cathode reaction is VO2+ (0.10 M) + 2H+ (0.10 M) + e- → V3+ (1.0×10-5 M) + H2O (l) , E =? The measured cell potential is 0.640 V. a) Calculate the E cell for the cathode. b) Calculate the equilibrium constant for the overall reaction. c)Calculate ΔG for this reaction in kJ
Consider a galvanic cell for which the anode reaction is Pb(s) → Pb+2 (0.010 M) + 2e- , E= -0.1263 V And the cathode reaction is VO2+ (0.10 M) + 2H+ (0.10 M) + e- → V3+ (1.0×10-5 M) + H2O (l) , E =? The measured cell potential is 0.640 V. a) Calculate the E cell for the cathode. b) Calculate the equilibrium constant for the overall reaction. c)Calculate ΔG for this reaction in kJ
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 137CWP: Consider a galvanic cell based on the following half-reactions: a. What is the standard potential...
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Consider a galvanic cell for which the anode reaction is
Pb(s) → Pb+2 (0.010 M) + 2e- , E= -0.1263 V
And the cathode reaction is
VO2+ (0.10 M) + 2H+ (0.10 M) + e- → V3+ (1.0×10-5 M) + H2O (l) , E =?
The measured cell potential is 0.640 V.
a) Calculate the E cell for the cathode.
b) Calculate the equilibrium constant for the overall reaction.
Pb(s) → Pb+2 (0.010 M) + 2e- , E= -0.1263 V
And the cathode reaction is
VO2+ (0.10 M) + 2H+ (0.10 M) + e- → V3+ (1.0×10-5 M) + H2O (l) , E =?
The measured cell potential is 0.640 V.
a) Calculate the E cell for the cathode.
b) Calculate the equilibrium constant for the overall reaction.
c)Calculate ΔG for this reaction in kJ
d) Determine the pH of this cell
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