### Electrochemical Cell Potential Calculation**Problem Statement:**Enter your answer in the provided box.What is the potential of a cell made up of Zn / Zn²⁺ and Cu / Cu²⁺ half-cells at 25°C if \[ \left[ \text{Zn}^{2+} \right] = 0.11 \, \text{M} \]and \[ \left[ \text{Cu}^{2+} \right] = 0.81 \, \text{M} ? \]**Answer Box:**\[ \boxed{} \text{ V} \]**Explanation:**To find the potential of the electrochemical cell, use the Nernst Equation:\[ E_{\text{cell}} = E^\circ_{\text{cell}} - \frac{0.0592}{n} \log Q \]Where:- \( E^\circ_{\text{cell}} \) is the standard cell potential- \( n \) is the number of moles of electrons transferred- \( Q \) is the reaction quotient For the Zn/Cu cell, the redox reactions and their standard potentials (at 25°C) are:\[ \text{Zn} \rightarrow \text{Zn}^{2+} + 2e^- \quad (E^\circ_{\text{Zn/Zn}^{2+}} = -0.76\, \text{V}) \]\[ \text{Cu}^{2+} + 2e^- \rightarrow \text{Cu} \quad (E^\circ_{\text{Cu}^{2+}/\text{Cu}} = +0.34 \, \text{V}) \]So, the overall standard cell potential is:\[ E^\circ_{\text{cell}} = E^\circ_{\text{Cu}^{2+}/\text{Cu}} - E^\circ_{\text{Zn}/\text{Zn}^{2+}} \]\[ E^\circ_{\text{cell}} = 0.34\, \text{V} - (-0.76\, \text{V}) \]\[ E^\circ_{\text{cell}} = 1.10\, \text{V} \]Next, calculate the reaction quotient \( Q \):\[ Q = \frac{ \left[ \text{Zn}^{2+} \right] }{ \left[ \text

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What is the potential of a cell made up of Zn/ Zn2+ and Cu/ Cu+ half-cells at 25°C if [Zn2*1 = 0.11 M and [Cu2] = 0.81 M ? 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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