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Balancing Oxidatic 29. Balance the fol cur in acidic so

Balancing Oxidatic 29. Balance the fol cur in acidic so

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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**Exercises: Balancing Oxidation-Reduction Equations** In this section, similar exercises are paired. **29.** Balance the following oxidation-reduction reactions that occur in acidic solutions using the half-reaction method. a. \( \text{I}^- (aq) + \text{ClO}^- (aq) \rightarrow \text{I}_2 (aq) + \text{Cl}^- (aq) \) b. \( \text{AsO}_3^{3-} (s) + \text{NO}_3^- (aq) \rightarrow \text{H}_3\text{AsO}_4 (aq) + \text{NO} (g) \) c. \( \text{Br}^- (aq) + \text{MnO}_4^- (aq) \rightarrow \text{Br}_2 (l) + \text{Mn}^{2+} (aq) \) d. \( \text{CH}_3\text{OH} (aq) + \text{Cr}_2\text{O}_7^{2-} (aq) \rightarrow \text{CH}_2\text{O} (aq) + \text{Cr}^{3+} (aq) \) **Instructions for Balancing:** 1. Identify the oxidation and reduction half-reactions. 2. Balance all elements except hydrogen and oxygen. 3. Balance oxygen using \( \text{H}_2\text{O} \). 4. Balance hydrogen using \( \text{H}^+ \). 5. Balance charges using electrons. 6. Multiply half-reactions to equalize electron transfer. 7. Add the half-reactions to give the balanced redox equation. 8. Verify that mass and charge are balanced.
Transcribed Image Text:**Exercises: Balancing Oxidation-Reduction Equations** In this section, similar exercises are paired. **29.** Balance the following oxidation-reduction reactions that occur in acidic solutions using the half-reaction method. a. \( \text{I}^- (aq) + \text{ClO}^- (aq) \rightarrow \text{I}_2 (aq) + \text{Cl}^- (aq) \) b. \( \text{AsO}_3^{3-} (s) + \text{NO}_3^- (aq) \rightarrow \text{H}_3\text{AsO}_4 (aq) + \text{NO} (g) \) c. \( \text{Br}^- (aq) + \text{MnO}_4^- (aq) \rightarrow \text{Br}_2 (l) + \text{Mn}^{2+} (aq) \) d. \( \text{CH}_3\text{OH} (aq) + \text{Cr}_2\text{O}_7^{2-} (aq) \rightarrow \text{CH}_2\text{O} (aq) + \text{Cr}^{3+} (aq) \) **Instructions for Balancing:** 1. Identify the oxidation and reduction half-reactions. 2. Balance all elements except hydrogen and oxygen. 3. Balance oxygen using \( \text{H}_2\text{O} \). 4. Balance hydrogen using \( \text{H}^+ \). 5. Balance charges using electrons. 6. Multiply half-reactions to equalize electron transfer. 7. Add the half-reactions to give the balanced redox equation. 8. Verify that mass and charge are balanced.
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