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Calculate E, E, and AG for the following cell reaction: Mg(s) + Sn²+ (aq) = Mg²+ (aq) + Sn (s) where [Mg²+] = 0.040 M and [Sn²+] = 0.030 M. Round each of your answers to 4 significant digits. Note: Reference the Standard reduction potentials at 25 °C table for additional information. Note: The Faraday constant is 9.649 × 104 Part 1 of 3 E = 2.235 V V mol

Calculate E, E, and AG for the following cell reaction: Mg(s) + Sn²+ (aq) = Mg²+ (aq) + Sn (s) where [Mg²+] = 0.040 M and [Sn²+] = 0.030 M. Round each of your answers to 4 significant digits. Note: Reference the Standard reduction potentials at 25 °C table for additional information. Note: The Faraday constant is 9.649 × 104 Part 1 of 3 E = 2.235 V V mol

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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Find E=....V  and Delta G=......kJ/mol

**Calculate \( E^0 \), \( E \), and \( \Delta G \) for the following cell reaction:** \[ \text{Mg}(s) + \text{Sn}^{2+}(aq) \rightleftharpoons \text{Mg}^{2+}(aq) + \text{Sn}(s) \] where \([ \text{Mg}^{2+} ] = 0.040 \, \text{M}\) and \([ \text{Sn}^{2+} ] = 0.030 \, \text{M}\). Round each of your answers to 4 significant digits. *Note: Reference the **Standard reduction potentials at 25 °C** table for additional information.* *Note: The Faraday constant is \( 9.649 \times 10^4 \, \frac{J}{V \cdot \text{mol}} \).* **Part 1 of 3** \[ E^0 = \boxed{2.235} \, \text{V} \] **Explanation:** In this exercise, you are asked to calculate the standard cell potential (\( E^0 \)), the cell potential (\( E \)), and the Gibbs free energy change (\( \Delta G \)) for a given electrochemical cell reaction between magnesium metal and tin ions. 1. **Chemical Equation:** - Magnesium solid (\(\text{Mg}(s)\)) reacts with aqueous tin ions (\(\text{Sn}^{2+}(aq)\)) to form aqueous magnesium ions (\(\text{Mg}^{2+}(aq)\)) and solid tin (\(\text{Sn}(s)\)). 2. **Concentrations:** - The concentration of magnesium ions is 0.040 M. - The concentration of tin ions is 0.030 M. 3. **Standard Reduction Potentials:** - These must be referenced from a standard table at 25 °C to calculate the \( E^0 \). 4. **Calculation:** - This part provides \( E^0 = 2.235 \, \text{V} \), indicating the standard potential for the reaction under standard conditions. 5. **The Faraday Constant:** - Given as \( 9.649 \times 10^4 \, \frac{J}{V \cdot \text{mol}} \), this is used for
Transcribed Image Text:**Calculate \( E^0 \), \( E \), and \( \Delta G \) for the following cell reaction:** \[ \text{Mg}(s) + \text{Sn}^{2+}(aq) \rightleftharpoons \text{Mg}^{2+}(aq) + \text{Sn}(s) \] where \([ \text{Mg}^{2+} ] = 0.040 \, \text{M}\) and \([ \text{Sn}^{2+} ] = 0.030 \, \text{M}\). Round each of your answers to 4 significant digits. *Note: Reference the **Standard reduction potentials at 25 °C** table for additional information.* *Note: The Faraday constant is \( 9.649 \times 10^4 \, \frac{J}{V \cdot \text{mol}} \).* **Part 1 of 3** \[ E^0 = \boxed{2.235} \, \text{V} \] **Explanation:** In this exercise, you are asked to calculate the standard cell potential (\( E^0 \)), the cell potential (\( E \)), and the Gibbs free energy change (\( \Delta G \)) for a given electrochemical cell reaction between magnesium metal and tin ions. 1. **Chemical Equation:** - Magnesium solid (\(\text{Mg}(s)\)) reacts with aqueous tin ions (\(\text{Sn}^{2+}(aq)\)) to form aqueous magnesium ions (\(\text{Mg}^{2+}(aq)\)) and solid tin (\(\text{Sn}(s)\)). 2. **Concentrations:** - The concentration of magnesium ions is 0.040 M. - The concentration of tin ions is 0.030 M. 3. **Standard Reduction Potentials:** - These must be referenced from a standard table at 25 °C to calculate the \( E^0 \). 4. **Calculation:** - This part provides \( E^0 = 2.235 \, \text{V} \), indicating the standard potential for the reaction under standard conditions. 5. **The Faraday Constant:** - Given as \( 9.649 \times 10^4 \, \frac{J}{V \cdot \text{mol}} \), this is used for
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