Complete and balance the following redox reaction in basic solution Cr,0,2-(aq) + Hg(1) → Hg²*(aq) + Cr3*(aq) 04- 03- D²- O- D2+ 03+ O4+ 1 4 7 8 9. 3 14 17 (s) (1) (g) |(aq) e- H,0 Hg OH- H;O* H* Cr 1L
Complete and balance the following redox reaction in basic solution Cr,0,2-(aq) + Hg(1) → Hg²*(aq) + Cr3*(aq) 04- 03- D²- O- D2+ 03+ O4+ 1 4 7 8 9. 3 14 17 (s) (1) (g) |(aq) e- H,0 Hg OH- H;O* H* Cr 1L
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 redox reaction:
\[ \text{Cr}_2\text{O}_7^{2-}(aq) + \text{Hg}(l) \rightarrow \text{Hg}^{2+}(aq) + \text{Cr}^{3+}(aq) \]
**Instructions:**
1. **Identify Oxidation and Reduction:**
- Chromium undergoes reduction: \( \text{Cr}_2\text{O}_7^{2-} \rightarrow \text{Cr}^{3+} \)
- Mercury undergoes oxidation: \( \text{Hg} \rightarrow \text{Hg}^{2+} \)
2. **Use the Ion-Electron Method:**
- Balance atoms except for O and H in each half-reaction.
- Balance O atoms by adding \( \text{H}_2\text{O} \).
- Balance H atoms by adding \( \text{OH}^- \) (since the solution is basic).
3. **Balance Charge with Electrons:**
- Add electrons to balance the charge on each side.
- Equalize the number of electrons in the two half-reactions by multiplying them by appropriate coefficients.
4. **Combine and Simplify:**
- Add the balanced half-reactions together.
- Cancel out identical species on both sides.
**Interactive Elements:**
The interface provides options to input ions, molecules, and charges. You can enter coefficients and elements to balance the equation interactively. This includes:
- Charges: \(4^-, 3^-, 2^-, 1^+, 2^+, 3^+, 4^+\)
- Numbers: \(1\) through \(9\)
- Other components: \(e^-\), \(\text{H}_2\text{O}\), \(\text{OH}^-\), \(\text{H}_3\text{O}^+\), and elements like \(\text{Cr}\) and \(\text{Hg}\).
**Outcome:**
Once completed, ensure that the equation is balanced in terms of mass and charge across all components.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F66f02499-6a2e-4c33-a9a6-3b6555c8b394%2F8dd9fc54-b742-4943-849c-20e225530950%2Fjaipm6i_processed.png&w=3840&q=75)
Transcribed Image Text:**Balancing Redox Reactions in Basic Solution**
**Objective:**
Complete and balance the following redox reaction:
\[ \text{Cr}_2\text{O}_7^{2-}(aq) + \text{Hg}(l) \rightarrow \text{Hg}^{2+}(aq) + \text{Cr}^{3+}(aq) \]
**Instructions:**
1. **Identify Oxidation and Reduction:**
- Chromium undergoes reduction: \( \text{Cr}_2\text{O}_7^{2-} \rightarrow \text{Cr}^{3+} \)
- Mercury undergoes oxidation: \( \text{Hg} \rightarrow \text{Hg}^{2+} \)
2. **Use the Ion-Electron Method:**
- Balance atoms except for O and H in each half-reaction.
- Balance O atoms by adding \( \text{H}_2\text{O} \).
- Balance H atoms by adding \( \text{OH}^- \) (since the solution is basic).
3. **Balance Charge with Electrons:**
- Add electrons to balance the charge on each side.
- Equalize the number of electrons in the two half-reactions by multiplying them by appropriate coefficients.
4. **Combine and Simplify:**
- Add the balanced half-reactions together.
- Cancel out identical species on both sides.
**Interactive Elements:**
The interface provides options to input ions, molecules, and charges. You can enter coefficients and elements to balance the equation interactively. This includes:
- Charges: \(4^-, 3^-, 2^-, 1^+, 2^+, 3^+, 4^+\)
- Numbers: \(1\) through \(9\)
- Other components: \(e^-\), \(\text{H}_2\text{O}\), \(\text{OH}^-\), \(\text{H}_3\text{O}^+\), and elements like \(\text{Cr}\) and \(\text{Hg}\).
**Outcome:**
Once completed, ensure that the equation is balanced in terms of mass and charge across all components.
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