i. When the oxidation half reaction is balanced (for the reaction given below which occurs in acid) using the smallest integer coefficients possible, what is the coefficient of H2O in the balanced half reaction? MnO4 + HSO3→ MnO42- + SO2- a 2 1 d. 4 e

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### Oxidation Half Reaction Balancing in Acidic Solution

**Question:**
When the oxidation half reaction is balanced (for the reaction given below which occurs in acid) using the smallest integer coefficients possible, what is the coefficient of H₂O in the balanced half reaction?

\[ \text{MnO}_4^- + \text{HSO}_3^- \rightarrow \text{MnO}_4^{2-} + \text{SO}_4^{2-} \]

**Options:**
- a. 2
- b. 0
- c. 1
- d. 4
- e. 3

### Explanation:
To answer this question, we need to balance the oxidation half-reaction for the given chemical equation in an acidic solution step-by-step.

1. **Write the unbalanced oxidation half-reaction:**
   \[ \text{MnO}_4^- + \text{HSO}_3^- \rightarrow \text{MnO}_4^{2-} + \text{SO}_4^{2-} \]

2. **Separate the reaction into two half-reactions (oxidation and reduction):**
   - _Oxidation half-reaction:_
     \[ \text{HSO}_3^- \rightarrow \text{SO}_4^{2-} \]
   
   - _Reduction half-reaction:_
     \[ \text{MnO}_4^- \rightarrow \text{MnO}_4^{2-} \]

3. **Balance each half-reaction separately:**
   - _Balance atoms other than O and H._
   - _Balance oxygen atoms by adding H₂O._
   - _Balance hydrogen atoms by adding H⁺._
   - _Balance the charges by adding electrons (e⁻)._

4. **Combine the half-reactions and ensure electron balancing.**

**Through these steps, you will find the correct coefficient for H₂O.**

### Answer:
After going through the balancing and combination process, the coefficient of H₂O in the balanced half reaction is determined to be **3**.

Therefore, the correct answer is:
- e. 3
Transcribed Image Text:### Oxidation Half Reaction Balancing in Acidic Solution **Question:** When the oxidation half reaction is balanced (for the reaction given below which occurs in acid) using the smallest integer coefficients possible, what is the coefficient of H₂O in the balanced half reaction? \[ \text{MnO}_4^- + \text{HSO}_3^- \rightarrow \text{MnO}_4^{2-} + \text{SO}_4^{2-} \] **Options:** - a. 2 - b. 0 - c. 1 - d. 4 - e. 3 ### Explanation: To answer this question, we need to balance the oxidation half-reaction for the given chemical equation in an acidic solution step-by-step. 1. **Write the unbalanced oxidation half-reaction:** \[ \text{MnO}_4^- + \text{HSO}_3^- \rightarrow \text{MnO}_4^{2-} + \text{SO}_4^{2-} \] 2. **Separate the reaction into two half-reactions (oxidation and reduction):** - _Oxidation half-reaction:_ \[ \text{HSO}_3^- \rightarrow \text{SO}_4^{2-} \] - _Reduction half-reaction:_ \[ \text{MnO}_4^- \rightarrow \text{MnO}_4^{2-} \] 3. **Balance each half-reaction separately:** - _Balance atoms other than O and H._ - _Balance oxygen atoms by adding H₂O._ - _Balance hydrogen atoms by adding H⁺._ - _Balance the charges by adding electrons (e⁻)._ 4. **Combine the half-reactions and ensure electron balancing.** **Through these steps, you will find the correct coefficient for H₂O.** ### Answer: After going through the balancing and combination process, the coefficient of H₂O in the balanced half reaction is determined to be **3**. Therefore, the correct answer is: - e. 3
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