Balance the following equations
`(a ) MnO_(4)^(-) + Fe^(2+) + H^(+) to`

Explanation

To balance the redox reaction \( \text{MnO}_4^{-} + \text{Fe}^{2+} + \text{H}^{+} \rightarrow \) products, we will follow a systematic approach.

### Step-by-Step Solution:

1. **Identify the Oxidation and Reduction Half-Reactions**:
- **Oxidation**: Iron (\( \text{Fe}^{2+} \)) is oxidized to \( \text{Fe}^{3+} \).
- **Reduction**: Manganese (\( \text{MnO}_4^{-} \)) is reduced from \( +7 \) in \( \text{MnO}_4^{-} \) to \( +2 \) in \( \text{Mn}^{2+} \).

...