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Determine E° for the half-reaction Fe³⁺(aq) + e⁻ → Fe²⁺(aq).

Determine E° for the half-reaction Fe³⁺(aq) + e⁻ → Fe²⁺(aq).

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
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Determine E° for the half-reaction Fe³⁺(aq) + e⁻ → Fe²⁺(aq).
 
### Redox Reaction and Standard Electrode Potential **Chemical Reaction:** \[ \text{Fe}^{3+}(\text{aq}) + \text{H}_2(\text{g}) \rightarrow 2\text{H}^+(\text{aq}) + \text{Fe}^{2+}(\text{aq}) \] **Description:** This is a redox reaction involving the reduction of iron(III) ions (\(\text{Fe}^{3+}\)) and the oxidation of hydrogen (\(\text{H}_2\)) gas. The products formed are hydrogen ions (\(\text{H}^+\)) in aqueous solution and iron(II) ions (\(\text{Fe}^{2+}\)). **Standard Electrode Potential:** \[ E^\circ = +0.77 \, \text{V} \] **Explanation:** The standard electrode potential (\(E^\circ\)) of +0.77 V indicates the voltage or potential difference under standard conditions (1 M concentration for each aqueous species, 1 atm pressure for gases, and 25°C temperature) for this redox reaction. A positive \(E^\circ\) value suggests that the reaction is spontaneous under standard conditions.
Transcribed Image Text:### Redox Reaction and Standard Electrode Potential **Chemical Reaction:** \[ \text{Fe}^{3+}(\text{aq}) + \text{H}_2(\text{g}) \rightarrow 2\text{H}^+(\text{aq}) + \text{Fe}^{2+}(\text{aq}) \] **Description:** This is a redox reaction involving the reduction of iron(III) ions (\(\text{Fe}^{3+}\)) and the oxidation of hydrogen (\(\text{H}_2\)) gas. The products formed are hydrogen ions (\(\text{H}^+\)) in aqueous solution and iron(II) ions (\(\text{Fe}^{2+}\)). **Standard Electrode Potential:** \[ E^\circ = +0.77 \, \text{V} \] **Explanation:** The standard electrode potential (\(E^\circ\)) of +0.77 V indicates the voltage or potential difference under standard conditions (1 M concentration for each aqueous species, 1 atm pressure for gases, and 25°C temperature) for this redox reaction. A positive \(E^\circ\) value suggests that the reaction is spontaneous under standard conditions.
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