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3 Co(s) + 2 NO 3- (aq) + 8 H+ (aq) = 3 Co 2+ (aq) + 2 NO (g) + 4 H2O (l) What would be the pH of the solution at standard conditions? Determine the cell potential for the reaction at a ph of 4.0 Is the reaction more favorable at a higher pH or a lower pH?

3 Co(s) + 2 NO 3- (aq) + 8 H+ (aq) = 3 Co 2+ (aq) + 2 NO (g) + 4 H2O (l) What would be the pH of the solution at standard conditions? Determine the cell potential for the reaction at a ph of 4.0 Is the reaction more favorable at a higher pH or a lower pH?

Chemistry
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
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3 Co(s) + 2 NO 3- (aq) + 8 H+ (aq) = 3 Co 2+ (aq) + 2 NO (g) + 4 H2O (l)

What would be the pH of the solution at standard conditions?

Determine the cell potential for the reaction at a ph of 4.0

Is the reaction more favorable at a higher pH or a lower pH?

4. The cell potentials of many oxidation-reduction reactions are highly dependent on pH. Consider the following equation: 3 Co(s) + 2 NO3"(aq) + 8 H*(aq) -----> 3 Co2+(aq) + 2 NOg) + 4 H2O) a) Determine the standard cell potential for the reaction. Cas> Coa 11 28V 2 NO3+ 184t. +be >aNOcg) +4 Hao =1.92v b) What would be the pH of the solution at standard conditions? (HINT: What are the concentrations of all aqueous species at standard conditions?) c) Determine the cell potential for the reaction at a pH of4.0. (Hint: You will need to use the Nernst equation.) ASsume that all concentrations, other than that of H*, are standard. d) Based on your answers above, would you say that the reaction is more favorable (i.e.., more spontaneous) at higher pH or lower pH? Explain.
Transcribed Image Text:4. The cell potentials of many oxidation-reduction reactions are highly dependent on pH. Consider the following equation: 3 Co(s) + 2 NO3"(aq) + 8 H*(aq) -----> 3 Co2+(aq) + 2 NOg) + 4 H2O) a) Determine the standard cell potential for the reaction. Cas> Coa 11 28V 2 NO3+ 184t. +be >aNOcg) +4 Hao =1.92v b) What would be the pH of the solution at standard conditions? (HINT: What are the concentrations of all aqueous species at standard conditions?) c) Determine the cell potential for the reaction at a pH of4.0. (Hint: You will need to use the Nernst equation.) ASsume that all concentrations, other than that of H*, are standard. d) Based on your answers above, would you say that the reaction is more favorable (i.e.., more spontaneous) at higher pH or lower pH? Explain.
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