In the reaction
`Ag_(2)O+H_(2)O_(2) rarr 2Ag+H_(2)O+O_(2)`
`H_(2)O_(2)` acts as

Options

A. reducing agent
B. oxidising agent
C. bleaching agent
D. none of these

Explanation

To determine the role of \( H_2O_2 \) in the reaction \( Ag_2O + H_2O_2 \rightarrow 2Ag + H_2O + O_2 \), we need to analyze the changes in oxidation states of the elements involved.

### Step-by-Step Solution:

1. **Identify the Reactants and Products**:
The reactants are silver(I) oxide (\( Ag_2O \)) and hydrogen peroxide (\( H_2O_2 \)). The products are silver (\( Ag \)), water (\( H_2O \)), and oxygen (\( O_2 \)).

2. **Assign Oxidation States**:
- In \( Ag_2O \), the oxidation state of silver (Ag) is +1 (since \( O \) is -2).
- In \( H_2O_2 \), the oxidation state of oxygen is -1.
- In the products:
- The oxidation state of silver (Ag) is 0 (elemental form).
- In water (\( H_2O \)), the oxidation state of oxygen is -2.
- In molecular oxygen (\( O_2 \)), the oxidation state of oxygen is 0.

3. **Determine Changes in Oxidation States**:
- For silver: The oxidation state changes from +1 in \( Ag_2O \) to 0 in \( Ag \). This is a reduction (gain of electrons).
- For oxygen in \( H_2O_2 \): The oxidation state changes from -1 in \( H_2O_2 \) to 0 in \( O_2 \). This is an oxidation (loss of electrons).

4. **Identify the Role of \( H_2O_2 \)**:
Since \( H_2O_2 \) causes the oxidation of oxygen (from -1 to 0), it is acting as a reducing agent. A reducing agent is a substance that donates electrons, causing another substance to be reduced.

5. **Conclusion**:
Based on the changes in oxidation states, \( H_2O_2 \) acts as a reducing agent in this reaction.

### Final Answer:
\( H_2O_2 \) acts as a **reducing agent**.