Which of the following equations depicts the oxidizing nature of `H_2O_2`

Options

A. `KIO_4+H_2O_2rarrKIO_3+H_2O+O_2`
B. `2I^(-)+H_2O_2+2H^+rarrI_2+H_2O`
C. `I_2+H_2O_2+2OH^(-)rarr2I^(-)+2H_2O+O_2`
D. `Cl_2+H_2O_2rarr2HCL+O_2`

Answer

To determine which equation depicts the oxidizing nature of \( H_2O_2 \) (hydrogen peroxide), we need to analyze the given reactions and identify where \( H_2O_2 \) is acting as an oxidizing agent. An oxidizing agent is a substance that oxidizes another substance while itself being reduced.

### Step-by-Step Solution:

1. **Understanding Oxidizing Agents**:
- An oxidizing agent is a substance that causes another substance to lose electrons (be oxidized) while itself gains electrons (is reduced).

2. **Analyzing Each Reaction**:
- We are provided with four reactions involving \( H_2O_2 \). We need to check each reaction to see if \( H_2O_2 \) is oxidizing another substance.

3. **Reaction 1**:
- Involves \( KI \) and \( H_2O_2 \).
- Here, \( I \) is in the +7 oxidation state in \( KIO_4 \) and is reduced to \( KIO_3 \). Since iodine is already in its highest oxidation state, \( H_2O_2 \) cannot oxidize it further. Therefore, it acts as a reducing agent here.

4. **Reaction 2**:
- Involves iodine in the 0 oxidation state converting to iodide (-1).
- In this case, iodine is being reduced, indicating that \( H_2O_2 \) is not acting as an oxidizing agent but rather as a reducing agent.

5. **Reaction 3**:
- Involves \( H_2O_2 \) converting to iodine.
- Here, \( H_2O_2 \) is in the -1 oxidation state and is oxidizing to iodine (0 oxidation state). This indicates that \( H_2O_2 \) is indeed acting as an oxidizing agent because it is oxidizing another species while itself being reduced.

6. **Reaction 4**:
- Involves chlorine (0) converting to chloride (-1).
- Similar to the previous reactions, chlorine is being reduced, indicating that \( H_2O_2 \) is not acting as an oxidizing agent here.

7. **Conclusion**:
- The only reaction where \( H_2O_2 \) acts as an oxidizing agent is in Reaction 3, where it oxidizes another substance while being reduced itself.

### Final Answer:
The equation that depicts the oxidizing nature of \( H_2O_2 \) is **Reaction 3**.