Complete and balance the following redox reaction in acidic solution 2+ MnO4 (aq) + S₂O3(aq) → S4062- (aq) + Mn²+ (aq) 3C22 1 + (s) O 2 3 4 D₁ H Reset e (1) LO 5 H₂O OH 6 (g) Mn S 7 8 H₂O+ 9 (aq) xH₂O H* X 0
Complete and balance the following redox reaction in acidic solution 2+ MnO4 (aq) + S₂O3(aq) → S4062- (aq) + Mn²+ (aq) 3C22 1 + (s) O 2 3 4 D₁ H Reset e (1) LO 5 H₂O OH 6 (g) Mn S 7 8 H₂O+ 9 (aq) xH₂O H* X 0
Chemistry
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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 Acidic Solutions
**Objective:**
Complete and balance the following redox reaction in acidic solution:
\[ \text{MnO}_4^- \, (\text{aq}) + \text{S}_2\text{O}_3^{2-} \, (\text{aq}) \rightarrow \text{S}_4\text{O}_6^{2-} \, (\text{aq}) + \text{Mn}^{2+} \, (\text{aq}) \]
**Steps to Balance the Reaction:**
#### Step 1: Write the Unbalanced Reaction
\[ \text{MnO}_4^- + \text{S}_2\text{O}_3^{2-} \rightarrow \text{S}_4\text{O}_6^{2-} + \text{Mn}^{2+} \]
#### Step 2: Split into Half-Reactions
Identify the oxidation and reduction half-reactions.
Oxidation half-reaction:
\[ \text{S}_2\text{O}_3^{2-} \rightarrow \text{S}_4\text{O}_6^{2-} \]
Reduction half-reaction:
\[ \text{MnO}_4^- \rightarrow \text{Mn}^{2+} \]
#### Step 3: Balance Elements in Each Half-Reaction
For the reduction half-reaction:
\[ \text{MnO}_4^- \rightarrow \text{Mn}^{2+} \]
1. Balance the manganese (Mn) atoms.
\[ \text{MnO}_4^- \rightarrow \text{Mn}^{2+} \]
2. Balance oxygen atoms by adding H₂O.
\[ \text{MnO}_4^- \rightarrow \text{Mn}^{2+} + 4 \text{H}_2\text{O} \]
3. Balance hydrogen atoms by adding H⁺.
\[ \text{MnO}_4^- + 8 \text{H}^+ \rightarrow \text{Mn}^{2+} + 4 \text{H}_2\text{O} \]
4. Balance the charges by adding electrons.
\[ \text{MnO}_4^- + 8 \text{H}^+ + 5 \text{e}^- \rightarrow \text{Mn](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F18d0a7dc-afe1-42e7-9349-84d2cfc69c53%2F9174a243-e205-4ee4-b654-c14f025c1670%2Ftktm2v_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Balancing Redox Reactions in Acidic Solutions
**Objective:**
Complete and balance the following redox reaction in acidic solution:
\[ \text{MnO}_4^- \, (\text{aq}) + \text{S}_2\text{O}_3^{2-} \, (\text{aq}) \rightarrow \text{S}_4\text{O}_6^{2-} \, (\text{aq}) + \text{Mn}^{2+} \, (\text{aq}) \]
**Steps to Balance the Reaction:**
#### Step 1: Write the Unbalanced Reaction
\[ \text{MnO}_4^- + \text{S}_2\text{O}_3^{2-} \rightarrow \text{S}_4\text{O}_6^{2-} + \text{Mn}^{2+} \]
#### Step 2: Split into Half-Reactions
Identify the oxidation and reduction half-reactions.
Oxidation half-reaction:
\[ \text{S}_2\text{O}_3^{2-} \rightarrow \text{S}_4\text{O}_6^{2-} \]
Reduction half-reaction:
\[ \text{MnO}_4^- \rightarrow \text{Mn}^{2+} \]
#### Step 3: Balance Elements in Each Half-Reaction
For the reduction half-reaction:
\[ \text{MnO}_4^- \rightarrow \text{Mn}^{2+} \]
1. Balance the manganese (Mn) atoms.
\[ \text{MnO}_4^- \rightarrow \text{Mn}^{2+} \]
2. Balance oxygen atoms by adding H₂O.
\[ \text{MnO}_4^- \rightarrow \text{Mn}^{2+} + 4 \text{H}_2\text{O} \]
3. Balance hydrogen atoms by adding H⁺.
\[ \text{MnO}_4^- + 8 \text{H}^+ \rightarrow \text{Mn}^{2+} + 4 \text{H}_2\text{O} \]
4. Balance the charges by adding electrons.
\[ \text{MnO}_4^- + 8 \text{H}^+ + 5 \text{e}^- \rightarrow \text{Mn
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