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The standard reduction potentials for two pairs of redox species are shown below. These two reactions are used to design a spontaneous, galvanic cell to light a light bulb. Which half-cell reaction happens at the cathode?   Cd2+ (aq) + 2e- → Cd(s)                                               E° = -0.40 V NO3- (aq) + 4H+ (aq) + 3e- → NO (g) + 2H2O (l)       E° = +0.96 V     Cd(s) → Cd2+ (aq) + 2e-     NO (g) + 2H2O (l) → NO3- (aq) + 4H+ (aq) + 3e-     Cd2+ (aq) + 2e- → Cd(s)     NO3- (aq) + 4H+ (aq) + 3e- → NO (g) + 2H2O (l)

The standard reduction potentials for two pairs of redox species are shown below. These two reactions are used to design a spontaneous, galvanic cell to light a light bulb. Which half-cell reaction happens at the cathode?   Cd2+ (aq) + 2e- → Cd(s)                                               E° = -0.40 V NO3- (aq) + 4H+ (aq) + 3e- → NO (g) + 2H2O (l)       E° = +0.96 V     Cd(s) → Cd2+ (aq) + 2e-     NO (g) + 2H2O (l) → NO3- (aq) + 4H+ (aq) + 3e-     Cd2+ (aq) + 2e- → Cd(s)     NO3- (aq) + 4H+ (aq) + 3e- → NO (g) + 2H2O (l)

Chemistry: An Atoms First Approach
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 118AE
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The standard reduction potentials for two pairs of redox species are shown below. These two reactions are used to design a spontaneous, galvanic cell to light a light bulb. Which half-cell reaction happens at the cathode?

 

Cd2+ (aq) + 2e- → Cd(s)                                               E° = -0.40 V

NO3- (aq) + 4H+ (aq) + 3e- → NO (g) + 2H2O (l)       E° = +0.96 V

   

Cd(s) → Cd2+ (aq) + 2e-
   

NO (g) + 2H2O (l) → NO3- (aq) + 4H+ (aq) + 3e-
   

Cd2+ (aq) + 2e- → Cd(s)
   

NO3- (aq) + 4H+ (aq) + 3e- → NO (g) + 2H2O (l)
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