**Title:** Constructing a Voltaic Cell with a Specific Standard Cell Potential**Objective:** Use the following half-reactions to create a voltaic cell with the given standard cell potential of 1.69 V.**Half-Reactions and Standard Reduction Potentials:**1. \( \text{Ce}^{4+} (\text{aq}) + e^- \rightarrow \text{Ce}^{3+} (\text{aq}) \) \( \text{E}^\circ = +1.61 \, \text{V} \)2. \( \text{Fe}^{3+} (\text{aq}) + e^- \rightarrow \text{Fe}^{2+} (\text{aq}) \) \( \text{E}^\circ = +0.77 \, \text{V} \)3. \( 2\text{H}^+ (\text{aq}) + 2e^- \rightarrow \text{H}_2(\text{g}) \) \( \text{E}^\circ = +0.00 \, \text{V} \)4. \( \text{Cu}^{2+} (\text{aq}) + e^- \rightarrow \text{Cu}^+ (\text{aq}) \) \( \text{E}^\circ = +0.15 \, \text{V} \)5. \( \text{Cl}_2(\text{g}) + 2e^- \rightarrow 2\text{Cl}^- (\text{aq}) \) \( \text{E}^\circ = +1.36 \, \text{V} \)6. \( \text{Sn}^{4+} (\text{aq}) + 2e^- \rightarrow \text{Sn}^{2+} (\text{aq}) \) \( \text{E}^\circ = +0.13 \, \text{V} \)7. \( \text{Pb}^{2+} (\text{aq}) + 2e^- \rightarrow \text{Pb} (\text{s}) \) \( \text{E}^\circ = -0.13 \, \text{V} \)8. \( \text{Co}^{3+} (\text{aq}) + e^- \rightarrow \text{

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Use the half-reactions below to produce a voltaic cell with the given standard cell potential. Standard Cell Potential Ce4+ (aq) + e¯ → Ce³+ (aq) E° = +1.61 V 1.69 V Fe3+ (aq) + e → Fe2+ (aq) E° = +0.77 V 2H*(aq) + 2e¯ → H2(g) E° = +0.00 V Cu2+ (aq) + e¯ → E° = +0.15 V Cu*(aq) Cl2(g) + 2e¯ → 2C1¯(aq) E° = +1.36 V Sn4+ (aq) + 2e → Sn2+ (aq) E° = +0.13 V Pb2+ (ag) + 2e¯ → Pb(s) E° = -0.13 V Co3+ (aq) + e¯ → Co2+ (aq) E° = +1.82 V Sn2+ (aq) + 2e¯ → Sn(s) E° = -0.14 V Anode Compartment Cathode Compartment Ag+(aq) + e¯ → Ag(s) E° = +0.80 V

Use the half-reactions below to produce a voltaic cell with the given standard cell potential. Standard Cell Potential Ce4+ (aq) + e¯ → Ce³+ (aq) E° = +1.61 V 1.69 V Fe3+ (aq) + e → Fe2+ (aq) E° = +0.77 V 2H(aq) + 2e¯ → H2(g) E° = +0.00 V Cu2+ (aq) + e¯ → E° = +0.15 V Cu(aq) Cl2(g) + 2e¯ → 2C1¯(aq) E° = +1.36 V Sn4+ (aq) + 2e → Sn2+ (aq) E° = +0.13 V Pb2+ (ag) + 2e¯ → Pb(s) E° = -0.13 V Co3+ (aq) + e¯ → Co2+ (aq) E° = +1.82 V Sn2+ (aq) + 2e¯ → Sn(s) E° = -0.14 V Anode Compartment Cathode Compartment Ag+(aq) + e¯ → Ag(s) E° = +0.80 V

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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