**Determining \( E^\circ \), \( \Delta G^\circ \), and \( K \) for the Overall Reaction**To find the standard cell potential (\( E^\circ \)), Gibbs free energy change (\( \Delta G^\circ \)), and equilibrium constant (\( K \)) for the overall reaction, we begin with the given balanced half-reactions and their standard reduction potentials.The overall reaction is:\[ 4 \text{Fe}^{3+} + 2 \text{H}_2\text{O} \rightleftharpoons 4 \text{Fe}^{2+} + \text{O}_2 + 4 \text{H}^+ \]**Half-Reactions and Standard Reduction Potentials:**1. **Reduction of Iron:** \[ \text{Fe}^{3+} + e^- \rightleftharpoons \text{Fe}^{2+} \] \[ E^\circ = 0.771 \, \text{V} \]2. **Reduction of Oxygen:** \[ \frac{1}{2} \text{O}_2 + 2 \text{H}^+ + 2 e^- \rightleftharpoons \text{H}_2\text{O} \] \[ E^\circ = 1.229 \, \text{V} \]These half-reactions represent the basic redox processes taking place in the overall reaction. The standard reduction potentials \( E^\circ \) are crucial for calculating the standard cell potential of the full reaction.**Calculation Overview:**- By using these half-reactions and their potentials, one can calculate the overall standard cell potential (\( E^\circ \)).- Using \( E^\circ \), the Gibbs free energy change (\( \Delta G^\circ \)) can be found with the relation: \[ \Delta G^\circ = -nFE^\circ \] where \( n \) is the number of moles of electrons transferred and \( F \) is Faraday's constant.- The equilibrium constant (\( K \)) can be determined from \( \Delta G^\circ \) using: \[ \Delta G^\circ = -RT \ln K \]These calculations allow us to understand the energetic and equilibrium characteristics of the redox reaction.

We have to find ∆G, ∆E and K for given reaction And using given reduction potential of half cell

termine E°, AG" , and K for the overall reaction from the balanced half-reactions and their standard reduction potentials. 4 Fe3+ + 2H,0 2 4 Fe²+ + O, + 4 H+ Fe3+ + e-= Fe2+ 0, + 2 H* + 2 e¯ H,0 E° = 0.771 V E' = 1.229 V

termine E°, AG" , and K for the overall reaction from the balanced half-reactions and their standard reduction potentials. 4 Fe3+ + 2H,0 2 4 Fe²+ + O, + 4 H+ Fe3+ + e-= Fe2+ 0, + 2 H* + 2 e¯ H,0 E° = 0.771 V E' = 1.229 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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