Which of the following reactions depicts the oxidising property of `SO_(2)` ?

Options

A. `SO_(2)+H_(2)O to H_(2)SO_(4)`
B. `2H_(2)S+SO_(2) to 3S+2H_(2)O`
C. `Cl_(2)+SO_(2) to SO_(2)Cl_(2)`
D. `2MnO_(4)^(-)+5SO_(2)+2H_(2)O to 5SO_(4)^(2-)+2Mn^(2+)+4H^(+)`

Explanation

To determine which reaction depicts the oxidizing property of \( SO_2 \), we need to identify a reaction where \( SO_2 \) acts as an oxidizing agent. An oxidizing agent is a substance that causes another substance to be oxidized while itself being reduced.

### Step-by-Step Solution:

1. **Understanding Oxidizing Agent**:
- An oxidizing agent gains electrons and is reduced in the process. Therefore, we need to look for a reaction where \( SO_2 \) is reduced (its oxidation state decreases) while another species is oxidized (its oxidation state increases).

2. **Analyzing the Reactions**:
- Let's consider the reactions provided:
1. \( SO_2 + H_2O \rightarrow H_2SO_4 \)
2. \( H_2S + SO_2 \rightarrow 3S + H_2O \)
3. \( SO_2 + Cl_2 \rightarrow SO_2Cl_2 \)
4. \( MnO_4^- + SO_2 \rightarrow Mn^{2+} + H_2SO_4 \)

3. **Evaluating Each Reaction**:
- **Reaction 1**: \( SO_2 + H_2O \rightarrow H_2SO_4 \)
- In this reaction, sulfur in \( SO_2 \) is in the +4 oxidation state and in \( H_2SO_4 \) it is +6. This indicates that \( SO_2 \) is being oxidized, not reduced. **Not an oxidizing reaction**.

- **Reaction 2**: \( H_2S + SO_2 \rightarrow 3S + H_2O \)
- Here, sulfur in \( H_2S \) is in the -2 oxidation state and in elemental sulfur (S), it is 0. \( SO_2 \) is in +4 oxidation state. The sulfur in \( SO_2 \) is reduced to 0, while \( H_2S \) is oxidized from -2 to 0. This indicates that \( SO_2 \) is acting as an oxidizing agent. **This is a valid oxidizing reaction**.

- **Reaction 3**: \( SO_2 + Cl_2 \rightarrow SO_2Cl_2 \)
- In this reaction, chlorine is reduced from 0 to -1, while sulfur remains at +4. Thus, \( SO_2 \) is not acting as an oxidizing agent here. **Not an oxidizing reaction**.

- **Reaction 4**: \( MnO_4^- + SO_2 \rightarrow Mn^{2+} + H_2SO_4 \)
- Manganese is reduced from +7 to +2, while sulfur in \( SO_2 \) remains at +4 and is oxidized to +6 in \( H_2SO_4 \). Here, \( SO_2 \) is acting as a reducing agent. **Not an oxidizing reaction**.

4. **Conclusion**:
- The only reaction where \( SO_2 \) acts as an oxidizing agent is **Reaction 2**: \( H_2S + SO_2 \rightarrow 3S + H_2O \).

### Final Answer:
The reaction that depicts the oxidizing property of \( SO_2 \) is:
**\( H_2S + SO_2 \rightarrow 3S + H_2O \)**.