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2 Given the followin give the cell reacti balanced equation and AG°.

2 Given the followin give the cell reacti balanced equation and AG°.

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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Can you please answer 17.62 and show all of the steps to the solution 

**Transcription of Text for Educational Use** --- **17.62** Given the following half-reactions, combine the two that give the cell reaction with the most positive E°. Write a balanced equation for the cell reaction and calculate E° and ΔG°. **17.63** Combine the two half-reactions in Problem 17.62 that give the cell reaction with the smallest E°. Write a balanced equation for the cell reaction and calculate E° and ΔG°. - \( \text{Co}^{2+}(aq) + 2e^- \rightarrow \text{Co}(s) \) \( E° = -0.28 \, \text{V} \) - \( \text{I}_2(s) + 2e^- \rightarrow 2\text{I}^-(aq) \) \( E° = 0.54 \, \text{V} \) - \( \text{Cu}^{2+}(aq) + 2e^- \rightarrow \text{Cu}(s) \) \( E° = 0.34 \, \text{V} \) **17.64** Calculate the standard cell potential and the standard free-energy change (in kilojoules) for each reaction in Problem 17.63. (See Appendix D for standard reduction potentials.) **17.65** Calculate E° and ΔG° for the cell reactions in Problem 17.62. (See Appendix D for standard reduction potentials.) **17.66** Predict the products of the following reactions, and tell which are spontaneous under standard-state conditions: (a) \( 2\text{Fe}^{3+}(aq) + 2\text{I}^-(aq) \rightarrow \) (b) \( \text{Pb}^{2+}(aq) + \text{Pb}(s) \rightarrow \) --- The problems reference standard electrochemical reactions and calculations involving standard cell potentials (E°) and free energy changes (ΔG°). Students are tasked with selecting combinations of half-reactions, calculating associated electrochemical parameters, and predicting reaction spontaneity. No graphs or additional diagrams are present in the text.
Transcribed Image Text:**Transcription of Text for Educational Use** --- **17.62** Given the following half-reactions, combine the two that give the cell reaction with the most positive E°. Write a balanced equation for the cell reaction and calculate E° and ΔG°. **17.63** Combine the two half-reactions in Problem 17.62 that give the cell reaction with the smallest E°. Write a balanced equation for the cell reaction and calculate E° and ΔG°. - \( \text{Co}^{2+}(aq) + 2e^- \rightarrow \text{Co}(s) \) \( E° = -0.28 \, \text{V} \) - \( \text{I}_2(s) + 2e^- \rightarrow 2\text{I}^-(aq) \) \( E° = 0.54 \, \text{V} \) - \( \text{Cu}^{2+}(aq) + 2e^- \rightarrow \text{Cu}(s) \) \( E° = 0.34 \, \text{V} \) **17.64** Calculate the standard cell potential and the standard free-energy change (in kilojoules) for each reaction in Problem 17.63. (See Appendix D for standard reduction potentials.) **17.65** Calculate E° and ΔG° for the cell reactions in Problem 17.62. (See Appendix D for standard reduction potentials.) **17.66** Predict the products of the following reactions, and tell which are spontaneous under standard-state conditions: (a) \( 2\text{Fe}^{3+}(aq) + 2\text{I}^-(aq) \rightarrow \) (b) \( \text{Pb}^{2+}(aq) + \text{Pb}(s) \rightarrow \) --- The problems reference standard electrochemical reactions and calculations involving standard cell potentials (E°) and free energy changes (ΔG°). Students are tasked with selecting combinations of half-reactions, calculating associated electrochemical parameters, and predicting reaction spontaneity. No graphs or additional diagrams are present in the text.
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