Which of the following equation depicts reducing nature of `H_(2)O_(2)`?

Options

A. `2[Fe(CN)_(6)]^(4-)+2H^(+)+H_(2)O_(2)rarr2[Fe(CN)_(6)]^(3-)+2H_(2)O`
B. `I_(2)+H_(2)O_(2)+2OH^(-)rarr 2I^(-)+2H_(2)O+O_(2)`
C. `Mn^(2+)+H_(2)O_(2)rarr Mn^(4+)+2OH^(-)`
D. `PbS+4H_(2)O_(2)rarr PbSO_(4)+4H_(2)O`

Explanation

To determine which equation depicts the reducing nature of hydrogen peroxide (H₂O₂), we need to analyze the reactions provided and identify where H₂O₂ acts as a reducing agent. A reducing agent is a substance that donates electrons to another species, causing that species to be reduced.

### Step-by-Step Solution:

1. **Understanding Reducing Agents**: A reducing agent is a substance that loses electrons and causes another substance to gain electrons. In a chemical reaction, the species that is reduced will have a decrease in oxidation state.

2. **Analyzing the Reactions**:
- **Reaction 1**: Fe²⁺ → Fe³⁺
- In this reaction, Fe²⁺ is oxidized to Fe³⁺, meaning it loses an electron. Therefore, H₂O₂ is not acting as a reducing agent here.

- **Reaction 2**: I₂ → 2I⁻
- In this reaction, I₂ is reduced to I⁻, meaning it gains electrons. Here, H₂O₂ is acting as a reducing agent because it donates electrons to I₂, allowing it to be reduced.

- **Reaction 3**: Mn²⁺ → Mn⁴⁺
- In this reaction, Mn²⁺ is oxidized to Mn⁴⁺, meaning it loses electrons. Therefore, H₂O₂ is not acting as a reducing agent here.

- **Reaction 4**: S²⁻ → S⁶⁺
- In this reaction, the sulfur anion (S²⁻) is oxidized to S⁶⁺, meaning it loses electrons. Thus, H₂O₂ is not acting as a reducing agent here.

3. **Conclusion**: The only reaction where H₂O₂ acts as a reducing agent is in Reaction 2, where I₂ is reduced to I⁻. Therefore, the correct answer is **Reaction 2**.

### Final Answer:
The equation that depicts the reducing nature of H₂O₂ is the one where I₂ is reduced to I⁻ (Reaction 2).

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