When `H_2S` reacts with halogens, halogens are

Options

A. Form sulphur halides
B. Are oxidised
C. Are reduced
D. None of these

Explanation

To solve the question of what happens to halogens when hydrogen sulfide (H₂S) reacts with them, we need to analyze the reaction and the changes in oxidation states of the elements involved.

### Step-by-Step Solution:

1. **Identify the Reaction**:
The general reaction of hydrogen sulfide with halogens can be represented as:
\[ H_2S + X_2 \rightarrow 2HX + S \]
where \(X_2\) represents a diatomic halogen (like Cl₂, Br₂, or I₂).

2. **Example Reaction**:
Let's consider the reaction of hydrogen sulfide with chlorine:
\[ H_2S + Cl_2 \rightarrow 2HCl + S \]

3. **Determine Oxidation States**:
- In \(H_2S\):
- Hydrogen (H) has an oxidation state of +1.
- Sulfur (S) has an oxidation state of -2.
- In \(Cl_2\):
- Chlorine (Cl) in its elemental form has an oxidation state of 0.
- In the products \(2HCl\) and \(S\):
- In \(HCl\), hydrogen is +1 and chlorine is -1.
- Sulfur (S) in its elemental form has an oxidation state of 0.

4. **Analyze Changes in Oxidation States**:
- For chlorine:
- Oxidation state changes from 0 (in Cl₂) to -1 (in HCl).
- This is a decrease in oxidation state, indicating that chlorine is reduced.
- For sulfur:
- Oxidation state changes from -2 (in H₂S) to 0 (in elemental S).
- This is an increase in oxidation state, indicating that sulfur is oxidized.

5. **Conclusion**:
Since the halogens (like chlorine in this case) undergo a decrease in their oxidation state, we conclude that halogens are **reduced** when they react with hydrogen sulfide.

### Final Answer:
When \(H_2S\) reacts with halogens, the halogens are **reduced**.

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