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4. The cell potentials of many oxidation-reduction reactions are highly dependent on pH. Consider the following equation: 3 Co(s) + 2NO3(aq) + 8 H+ (aq) -----> 3 Co2+ (aq) + 2NO(g) + 4H₂O(1) a) Determine the standard cell potential for the reaction. 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 of_2.0. (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.

4. The cell potentials of many oxidation-reduction reactions are highly dependent on pH. Consider the following equation: 3 Co(s) + 2NO3(aq) + 8 H+ (aq) -----> 3 Co2+ (aq) + 2NO(g) + 4H₂O(1) a) Determine the standard cell potential for the reaction. 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 of_2.0. (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.

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 18.101QE: At 298 K, the solubility product constant for PbC2O4 is 8.5 1010, and the standard reduction...
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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) + +(aq) + 2 NO(g) + 4H₂O) a) Determine the standard cell potential for the reaction. 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 of_2.0. (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) + +(aq) + 2 NO(g) + 4H₂O) a) Determine the standard cell potential for the reaction. 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 of_2.0. (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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For part, b would the calculations be the same for NO3^- (aq) and CO^2+ (aq), meaning those species PH would also equal 0?

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Why is the reaction more favorable at lower pH?

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