Balance the following redox reactions by ion-electron method.
`MnO_(4)^(-)(aq)+SO_(2)(g)toMn^(2+)(aq)+HSO_(4)^(-)(aq)` (in acidic solution)

Explanation

To balance the redox reaction `MnO4^(-)(aq) + SO2(g) → Mn^(2+)(aq) + HSO4^(-)(aq)` in acidic solution using the ion-electron method, we will follow these steps:

### Step 1: Identify the oxidation and reduction half-reactions
- **Oxidation Half-Reaction**: Sulfur in SO2 is oxidized to HSO4^(-). The oxidation state of sulfur changes from +4 in SO2 to +6 in HSO4^(-).
- **Reduction Half-Reaction**: Manganese in MnO4^(-) is reduced to Mn^(2+). The oxidation state of manganese changes from +7 in MnO4^(-) to +2 in Mn^(2+).

### Step 2: Write the half-reactions
1. **Oxidation Half-Reaction**:
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