Complete and balance the following half-reaction in basic solution. Be sure to include the proper phases for all species within the reaction. Cr₂O72- (aq) → Cr³+ (aq)
Complete and balance the following half-reaction in basic solution. Be sure to include the proper phases for all species within the reaction. Cr₂O72- (aq) → Cr³+ (aq)
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 Redox Reactions in Basic Solution
**Objective:** Complete and balance the following half-reaction in basic solution. Be sure to include the proper phases for all species within the reaction.
**Given Reaction:**
\[ \text{Cr}_2\text{O}_7^{2-} \,(\text{aq}) \rightarrow \text{Cr}^{3+} \,(\text{aq}) \]
When balancing redox reactions in basic solution:
1. **Identify the reaction as a redox process**, which involves a change in the oxidation state of the elements.
2. **Split the equation into two half-reactions**: oxidation and reduction.
3. **Balance each half-reaction** for mass and charge:
- Balance all elements except for hydrogen and oxygen.
- Balance oxygen atoms by adding \(\text{H}_2\text{O}\).
- Balance hydrogen atoms by adding \(\text{OH}^-\) (since the solution is basic).
- Balance the charges by adding electrons (\(e^-\)).
4. **Combine the half-reactions**, ensuring that electrons are canceled out.
5. **Verify** that the elements and charges are balanced in the final equation.
**Example Process:**
For the given \(\text{Cr}_2\text{O}_7^{2-} \rightarrow \text{Cr}^{3+}\), there will be steps such as balancing chromium and oxygen, adding water molecules, balancing with hydroxide ions, and adding electrons appropriately.
This approach ensures a thorough understanding of how redox reactions are balanced in a basic solution, which is crucial for chemistry students.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fed07e6d7-5565-4362-9c55-0d05e0f82a2a%2F5b372167-7a7a-4b21-ab25-a48714bd777e%2Fqiw2jid_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Balancing Redox Reactions in Basic Solution
**Objective:** Complete and balance the following half-reaction in basic solution. Be sure to include the proper phases for all species within the reaction.
**Given Reaction:**
\[ \text{Cr}_2\text{O}_7^{2-} \,(\text{aq}) \rightarrow \text{Cr}^{3+} \,(\text{aq}) \]
When balancing redox reactions in basic solution:
1. **Identify the reaction as a redox process**, which involves a change in the oxidation state of the elements.
2. **Split the equation into two half-reactions**: oxidation and reduction.
3. **Balance each half-reaction** for mass and charge:
- Balance all elements except for hydrogen and oxygen.
- Balance oxygen atoms by adding \(\text{H}_2\text{O}\).
- Balance hydrogen atoms by adding \(\text{OH}^-\) (since the solution is basic).
- Balance the charges by adding electrons (\(e^-\)).
4. **Combine the half-reactions**, ensuring that electrons are canceled out.
5. **Verify** that the elements and charges are balanced in the final equation.
**Example Process:**
For the given \(\text{Cr}_2\text{O}_7^{2-} \rightarrow \text{Cr}^{3+}\), there will be steps such as balancing chromium and oxygen, adding water molecules, balancing with hydroxide ions, and adding electrons appropriately.
This approach ensures a thorough understanding of how redox reactions are balanced in a basic solution, which is crucial for chemistry students.
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