In the reaction given below sulphuric acid acts as a /an:
S + 2H2SO4 → 3SO2 + 2H2O
(a) Non-volatile acid
(b) Dibasic acid
(c) Oxidising agent
(d) Reducing agent
Ans: (c) Oxidising Agent
Here’s how to determine the role of sulfuric acid in the given reaction:
1. Analyze the Reaction:
- S + 2H₂SO₄ → 3SO₂ + 2H₂O
- Sulfur (S) is being oxidized to sulfur dioxide (SO₂).
- Sulfuric acid (H₂SO₄) is being reduced to sulfur dioxide (SO₂).
2. Oxidation States:
- In H₂SO₄, sulfur has an oxidation state of +6.
- In SO₂, sulfur has an oxidation state of +4.
- Sulfur (S) elemental form has an oxidation state of 0.
3. Determine the Role:
- Since the oxidation state of sulfur in H₂SO₄ decreases from +6 to +4, it is being reduced.
- A substance that is reduced acts as an oxidizing agent.
4. Conclusion:
- Therefore, sulfuric acid (H₂SO₄) acts as an oxidizing agent in this reaction.
The correct answer is (c) Oxidising agent.
