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Complete and balance the following half-reaction in basic solution. Be sure to include the proper phases for all species within the reaction. 2+ Mn²+ (aq) → Mn O₂ (s)

Complete and balance the following half-reaction in basic solution. Be sure to include the proper phases for all species within the reaction. 2+ Mn²+ (aq) → Mn O₂ (s)

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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**Title: Balancing Half-Reactions in Basic Solutions** **Instruction:** Complete and balance the following half-reaction in a basic solution. Ensure that you include the correct phases for all species within the reaction. **Half-Reaction:** \[ \text{Mn}^{2+}(\text{aq}) \rightarrow \text{MnO}_2(\text{s}) \] **Explanation:** When balancing half-reactions, especially in basic solutions, it is crucial to ensure that both mass and charge are balanced. The reaction involves the oxidation of manganese ions in aqueous form (\[\text{Mn}^{2+}(\text{aq})\]) to manganese dioxide as a solid (\[\text{MnO}_2(\text{s})\]). **Steps to Balance:** 1. **Balance the Atoms:** - Ensure that the number of manganese atoms is the same on both sides. 2. **Balance the Oxygen Atoms:** - Add water molecules (\[\text{H}_2\text{O}\]) to the side lacking oxygen. 3. **Balance the Hydrogen Atoms:** - Add hydroxide ions (\[\text{OH}^-\]) to balance hydrogen atoms introduced by water. 4. **Balance the Charge:** - Add electrons (\[\text{e}^-\]) to make the charges equal on both sides. In this scenario, the oxygen balance and addition of \[\text{OH}^-\] and electrons are critical steps in obtaining the correctly balanced reaction in a basic medium.
Transcribed Image Text:**Title: Balancing Half-Reactions in Basic Solutions** **Instruction:** Complete and balance the following half-reaction in a basic solution. Ensure that you include the correct phases for all species within the reaction. **Half-Reaction:** \[ \text{Mn}^{2+}(\text{aq}) \rightarrow \text{MnO}_2(\text{s}) \] **Explanation:** When balancing half-reactions, especially in basic solutions, it is crucial to ensure that both mass and charge are balanced. The reaction involves the oxidation of manganese ions in aqueous form (\[\text{Mn}^{2+}(\text{aq})\]) to manganese dioxide as a solid (\[\text{MnO}_2(\text{s})\]). **Steps to Balance:** 1. **Balance the Atoms:** - Ensure that the number of manganese atoms is the same on both sides. 2. **Balance the Oxygen Atoms:** - Add water molecules (\[\text{H}_2\text{O}\]) to the side lacking oxygen. 3. **Balance the Hydrogen Atoms:** - Add hydroxide ions (\[\text{OH}^-\]) to balance hydrogen atoms introduced by water. 4. **Balance the Charge:** - Add electrons (\[\text{e}^-\]) to make the charges equal on both sides. In this scenario, the oxygen balance and addition of \[\text{OH}^-\] and electrons are critical steps in obtaining the correctly balanced reaction in a basic medium.
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