**Standard State Electrochemical Cells**1. In each of the following systems, two half-reactions are provided. For each system: a) Write the balanced reaction occurring for a spontaneous system. b) Calculate the overall standard cell potential. a. | **Half Reaction** | \( E^\circ_{\text{red}} \) (V) | |------------------------------------|--------------------------------| | \( \text{I}_2(s) + 2e^- \rightarrow 2 \text{I}^-(aq) \) | +0.53 | | \( \text{Co}^{3+}(aq) + e^- \rightarrow \text{Co}^{2+}(aq) \) | +1.82 |

Overall standard cell potential is calculated using this formula,E°cell=Ecathode-Eanode Balanced…

Standard State Electrochemical Cells 1. In each of the following systems two half-reactions are provided. For each system, a) write the balanced reaction occurring for a spontaneous system, and b) calculate the overall standard cell potential. a. E°red (V) Half Reaction +0.53 I2(s) + 2e = 2 I"(aq) +1.82 Co3+ (aq) + e = Co2*(aq)

Standard State Electrochemical Cells 1. In each of the following systems two half-reactions are provided. For each system, a) write the balanced reaction occurring for a spontaneous system, and b) calculate the overall standard cell potential. a. E°red (V) Half Reaction +0.53 I2(s) + 2e = 2 I"(aq) +1.82 Co3+ (aq) + e = Co2*(aq)

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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