In the reaction `2Ag+H_2SO_4 to Ag_2SO_4+2H_2O+SO_2+H_2SO_4` acts as :

Options

A. Reducing agent as well as acid
B. Oxidising agent as well as acid
C. Catalytic agent
D. Dehydrating agent as well as acid

Explanation

To determine the role of sulfuric acid (H₂SO₄) in the reaction \(2Ag + H_2SO_4 \rightarrow Ag_2SO_4 + 2H_2O + SO_2\), we need to analyze the components and their functions in the reaction.

### Step-by-Step Solution:

1. **Identify the Reactants and Products**:
- The reactants are silver (Ag) and sulfuric acid (H₂SO₄).
- The products are silver sulfate (Ag₂SO₄), water (H₂O), and sulfur dioxide (SO₂).

2. **Determine the Oxidation States**:
- In elemental silver (Ag), the oxidation state is 0.
- In silver sulfate (Ag₂SO₄), silver has an oxidation state of +1.
- In sulfuric acid (H₂SO₄), sulfur has an oxidation state of +6, and in sulfur dioxide (SO₂), sulfur has an oxidation state of +4.

3. **Analyze the Changes in Oxidation States**:
- Silver (Ag) is oxidized from 0 to +1.
- Sulfur in H₂SO₄ is reduced from +6 to +4 (in SO₂).
- This indicates that sulfuric acid is facilitating the oxidation of silver while itself being reduced.

4. **Identify the Role of Sulfuric Acid**:
- Since sulfuric acid is causing the oxidation of silver (by accepting electrons), it acts as an oxidizing agent.
- Additionally, sulfuric acid is an acid by nature, as it donates protons (H⁺ ions) in the reaction.

5. **Conclusion**:
- Therefore, in this reaction, sulfuric acid (H₂SO₄) acts as both an oxidizing agent and an acid.

### Final Answer:
Sulfuric acid (H₂SO₄) acts as an oxidizing agent as well as an acid in the reaction.

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