`H_(2)O_(2)rarr 2H^(+)+O_(2)+2e^(-),E^(@)=-0.68V`.
This equation represents which of the following behaviour of `H_(2)O_(2)`

Options

A. reducing
B. oxidising
C. basic
D. catalytic

Answer

To determine the behavior of hydrogen peroxide (H₂O₂) as represented by the given reaction, we can analyze the reaction step by step.

### Step-by-Step Solution:

1. **Identify the Reaction**: The reaction given is:
\[ \text{H}_2\text{O}_2 \rightarrow 2\text{H}^+ + \text{O}_2 + 2e^- \]

2. **Analyze the Reaction**: In this reaction, hydrogen peroxide (H₂O₂) is decomposing into protons (H⁺), oxygen gas (O₂), and electrons (e⁻).

3. **Determine Electron Transfer**: The production of electrons indicates that H₂O₂ is losing electrons. This process is known as oxidation.

4. **Define Oxidation**: Oxidation is defined as the loss of electrons. Since H₂O₂ is losing electrons, it is undergoing oxidation.

5. **Identify the Role of H₂O₂**: Since H₂O₂ is being oxidized, it means that it is acting as a reducing agent. A reducing agent is a substance that donates electrons to another substance and is itself oxidized in the process.

6. **Conclusion**: Therefore, based on the reaction and the analysis, we conclude that H₂O₂ behaves as a reducing agent in this context.

### Final Answer:
The behavior of H₂O₂ as depicted in the reaction is that it acts as a **reducing agent**.

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