(I) `H_(2)O_(2)+O_(3) to H_(2)O+2O_(2)`
(II) `H_(2)O_(2)+Ag_(2)O to 2Ag+H_(2)O+O_(2)`
Role of hydrogen peroxide in the above reactions is respectively

Options

A. oxidising in (I) and reducing in (II)
B. reducing in (I) and oxidising in (II)
C. Reducing in (I) and (II)
D. oxidisng in (I) and (II)

Answer

To determine the role of hydrogen peroxide (H₂O₂) in the given reactions, we need to analyze each reaction step by step, focusing on the changes in oxidation states of the elements involved.

### Step-by-Step Solution:

**Reaction (I):**
\[ \text{H}_2\text{O}_2 + \text{O}_3 \rightarrow \text{H}_2\text{O} + 2\text{O}_2 \]

1. **Identify Oxidation States:**
- In H₂O₂, the oxidation state of oxygen is -1.
- In O₃ (ozone), the oxidation state of oxygen is 0.
- In H₂O, the oxidation state of oxygen is -2.
- In O₂, the oxidation state of oxygen is 0.

2. **Determine Changes:**
- Ozone (O₃) is reduced to H₂O, where the oxidation state of oxygen decreases from 0 to -2.
- H₂O₂ is oxidized to O₂, where the oxidation state of oxygen increases from -1 to 0.

3. **Conclusion:**
- Since H₂O₂ helps O₃ to undergo reduction (by providing electrons), it acts as a reducing agent in this reaction.

**Reaction (II):**
\[ \text{H}_2\text{O}_2 + \text{Ag}_2\text{O} \rightarrow 2\text{Ag} + \text{H}_2\text{O} + \text{O}_2 \]

1. **Identify Oxidation States:**
- In H₂O₂, the oxidation state of oxygen is -1.
- In Ag₂O, silver (Ag) has an oxidation state of +1 and oxygen is -2.
- In elemental silver (Ag), the oxidation state is 0.
- In H₂O, the oxidation state of oxygen is -2.
- In O₂, the oxidation state of oxygen is 0.

2. **Determine Changes:**
- Silver (Ag) in Ag₂O is reduced from +1 to 0 (reduction).
- H₂O₂ is oxidized to O₂, where the oxidation state of oxygen increases from -1 to 0.

3. **Conclusion:**
- H₂O₂ facilitates the reduction of Ag₂O to Ag, thus acting as a reducing agent in this reaction as well.

### Final Answer:
In both reactions, hydrogen peroxide (H₂O₂) acts as a **reducing agent**.