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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![**Balancing a Redox Reaction in Acidic Solution**
The task is to balance the following redox reaction in an acidic solution:
\[ \text{Cl}^- (aq) + \text{MnO}_4^- (aq) \rightarrow \text{Cl}_2 (g) + \text{Mn}^{2+} (aq) \]
**Current Equation:**
\[ \text{Cl}^- (aq) + \text{MnO}_4^- (aq) \rightarrow \text{Cl}_2 (g) + \text{Mn}^{2+} (aq) \]
**Explanation of Diagram:**
The diagram contains a tool that appears to assist in balancing the equation, specifically for the electrons in the half-reactions. This tool includes symbols for square boxes and an electron symbol (\(e^-\)). It is likely used to track and balance electrons between the oxidation and reduction processes.
- Arrows between boxes suggest indicating electron transfer.
- It aids in ensuring that both mass and charge are balanced, a crucial step for redox reactions.
To fully balance the redox equation, follow these general steps:
1. Separate the reactions into oxidation and reduction half-reactions.
2. Balance each half-reaction for atoms and charge, adding \(H_2O\), \(H^+\), and electrons (\(e^-\)) as needed.
3. Combine the half-reactions, ensuring electrons are balanced and simplify the equation.
This approach ensures completeness and accuracy, following the redox balancing rules in acidic conditions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2e8de085-3521-4e76-9213-315082e7bc47%2Fe144309b-89e1-4f65-8a29-7bfcc419ed07%2F82xh5q_processed.png&w=3840&q=75)
Transcribed Image Text:**Balancing a Redox Reaction in Acidic Solution**
The task is to balance the following redox reaction in an acidic solution:
\[ \text{Cl}^- (aq) + \text{MnO}_4^- (aq) \rightarrow \text{Cl}_2 (g) + \text{Mn}^{2+} (aq) \]
**Current Equation:**
\[ \text{Cl}^- (aq) + \text{MnO}_4^- (aq) \rightarrow \text{Cl}_2 (g) + \text{Mn}^{2+} (aq) \]
**Explanation of Diagram:**
The diagram contains a tool that appears to assist in balancing the equation, specifically for the electrons in the half-reactions. This tool includes symbols for square boxes and an electron symbol (\(e^-\)). It is likely used to track and balance electrons between the oxidation and reduction processes.
- Arrows between boxes suggest indicating electron transfer.
- It aids in ensuring that both mass and charge are balanced, a crucial step for redox reactions.
To fully balance the redox equation, follow these general steps:
1. Separate the reactions into oxidation and reduction half-reactions.
2. Balance each half-reaction for atoms and charge, adding \(H_2O\), \(H^+\), and electrons (\(e^-\)) as needed.
3. Combine the half-reactions, ensuring electrons are balanced and simplify the equation.
This approach ensures completeness and accuracy, following the redox balancing rules in acidic conditions.
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