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For a particular redox reaction, Cr is oxidized to CrO2- and Fe³+ is reduced to Fe²+. Complete and balance the equation for this reaction in basic solution. The phases are optional.

For a particular redox reaction, Cr is oxidized to CrO2- and Fe³+ is reduced to Fe²+. Complete and balance the equation for this reaction in basic solution. The phases are optional.

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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### Redox Reaction Balancing in Basic Solution **Problem Statement:** For a particular redox reaction, chromium (Cr) is oxidized to chromate ion \(\text{CrO}_4^{2-}\) and iron (Fe\(^3+\)) is reduced to iron(II) ion (Fe\(^2+\)). Complete and balance the equation for this reaction in a basic solution. The phases are optional. **Equation to Balance:** \[ \text{Cr} + 6\text{Fe}^{3+} + 8\text{OH}^- \longrightarrow \text{CrO}_4^{2-} + 6\text{Fe}^{2+} + 4\text{H}_2\text{O} \] **Solution:** The provided equation is not correctly balanced for the redox reaction in a basic solution as indicated by the "Incorrect" label. Ensure the final balanced equation satisfies the following: 1. **Mass Balance**: The same number of each type of atom on both sides of the equation. 2. **Charge Balance**: The total charge should be the same on both sides of the equation. **Detailed Steps for Balancing:** 1. **Identify Oxidation and Reduction Half-Reactions:** - **Oxidation**: Cr is being oxidized to CrO₄²⁻. - **Reduction**: Fe³⁺ is being reduced to Fe²⁺. 2. **Balance Each Half-Reaction Separately:** - **Oxidation Half-Reaction:** \[ \text{Cr} \rightarrow \text{CrO}_4^{2-} \] To balance oxygen, add H₂O to the right side: \[ \text{Cr} \rightarrow \text{CrO}_4^{2-} + 4\text{H}_2\text{O} \] To balance hydrogen, add OH⁻ to both sides: \[ \text{Cr} + 8\text{OH}^- \rightarrow \text{CrO}_4^{2-} + 4\text{H}_2\text{O} \] Balance the charges by adding electrons to the left side: \[ \text{Cr} + 8\text{OH}^- \rightarrow \text{CrO}_4^{
Transcribed Image Text:### Redox Reaction Balancing in Basic Solution **Problem Statement:** For a particular redox reaction, chromium (Cr) is oxidized to chromate ion \(\text{CrO}_4^{2-}\) and iron (Fe\(^3+\)) is reduced to iron(II) ion (Fe\(^2+\)). Complete and balance the equation for this reaction in a basic solution. The phases are optional. **Equation to Balance:** \[ \text{Cr} + 6\text{Fe}^{3+} + 8\text{OH}^- \longrightarrow \text{CrO}_4^{2-} + 6\text{Fe}^{2+} + 4\text{H}_2\text{O} \] **Solution:** The provided equation is not correctly balanced for the redox reaction in a basic solution as indicated by the "Incorrect" label. Ensure the final balanced equation satisfies the following: 1. **Mass Balance**: The same number of each type of atom on both sides of the equation. 2. **Charge Balance**: The total charge should be the same on both sides of the equation. **Detailed Steps for Balancing:** 1. **Identify Oxidation and Reduction Half-Reactions:** - **Oxidation**: Cr is being oxidized to CrO₄²⁻. - **Reduction**: Fe³⁺ is being reduced to Fe²⁺. 2. **Balance Each Half-Reaction Separately:** - **Oxidation Half-Reaction:** \[ \text{Cr} \rightarrow \text{CrO}_4^{2-} \] To balance oxygen, add H₂O to the right side: \[ \text{Cr} \rightarrow \text{CrO}_4^{2-} + 4\text{H}_2\text{O} \] To balance hydrogen, add OH⁻ to both sides: \[ \text{Cr} + 8\text{OH}^- \rightarrow \text{CrO}_4^{2-} + 4\text{H}_2\text{O} \] Balance the charges by adding electrons to the left side: \[ \text{Cr} + 8\text{OH}^- \rightarrow \text{CrO}_4^{
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