Which of the following equations depict theoxidising nature of `H_(2)O_(2)` ?

Options

A. `2MnO_(4)^(-) + 6H^(+)+5H_(2)O_(2) to 2Mn^(2+) + 8H_(2)O+ 5O_(2)`
B. `2Fe^(3+) + 2H^(+) +H_(2) O_(2) to 2F^(2+) + 2H_(2)O+O_(2)`
C. `2I^(-) + 2H^(+) + H_(2)O_(2) to I_(2) + 2H_(2)O `
D. `KIO_(4) + H_(2)O_(2) to KIO_(3) + H_(3)O + O_(2)`

Explanation

To determine which of the given equations depict the oxidizing nature of hydrogen peroxide (H₂O₂), we need to analyze the oxidation states of the elements involved in each reaction. An oxidizing agent is a substance that gains electrons (is reduced) while causing another substance to lose electrons (is oxidized).

### Step-by-Step Solution:

1. **Understanding Oxidation and Reduction**:
- Oxidation is the loss of electrons or an increase in oxidation state.
- Reduction is the gain of electrons or a decrease in oxidation state.
- An oxidizing agent is reduced while it oxidizes another species.

2. **Analyzing Each Option**:
- **Option 1**: MnO₄⁻ + H₂O₂ →
- Manganese in MnO₄⁻ has an oxidation state of +7, and in the product, it has an oxidation state of +2. This means Mn is being reduced (gaining electrons).
- H₂O₂ has oxygen in the -1 state and is converted to 0, indicating that H₂O₂ is being oxidized (losing electrons).
- Since H₂O₂ is not oxidizing another species but reducing Mn, this option does not depict the oxidizing nature of H₂O₂.

- **Option 2**: Fe³⁺ + H₂O₂ →
- Iron (Fe) in the +3 state is reduced to +2, indicating that Fe is being reduced.
- H₂O₂ does not show any change in oxidation state that indicates it is oxidizing another species.
- Therefore, this option also does not depict the oxidizing nature of H₂O₂.

- **Option 3**: I⁻ + H₂O₂ →
- Iodine (I) in the -1 state is oxidized to 0, indicating that it is losing electrons.
- H₂O₂ is reduced from -1 to -2, indicating that it is gaining electrons.
- Here, H₂O₂ is oxidizing iodine, which shows its oxidizing nature.

- **Option 4**: IO₄⁻ + H₂O₂ →
- Iodine in IO₄⁻ has an oxidation state of +7 and is reduced to +5, indicating that it is being reduced.
- H₂O₂ does not oxidize another species in this reaction, so this option does not depict the oxidizing nature of H₂O₂.

3. **Conclusion**:
- The only equation that depicts the oxidizing nature of H₂O₂ is **Option 3**, where H₂O₂ oxidizes iodine (I⁻) while itself is reduced.

### Final Answer:
The correct option that depicts the oxidizing nature of H₂O₂ is **Option 3**.