In the reaction `H_(2)S + C1_(2) to 2HC1 + S`, the oxidizing agent is

Options

A. `H_(2)S`
B. `C1_(2)`
C. HC1
D. S

Answer

To determine the oxidizing agent in the reaction \( H_2S + Cl_2 \rightarrow 2HCl + S \), we need to analyze the changes in oxidation states of the elements involved in the reaction.

### Step-by-Step Solution:

1. **Identify the Reactants and Products**:
The reactants are hydrogen sulfide (\( H_2S \)) and chlorine gas (\( Cl_2 \)). The products are hydrochloric acid (\( HCl \)) and sulfur (\( S \)).

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

3. **Analyze the Changes in Oxidation States**:
- For sulfur in \( H_2S \):
- Changes from -2 (in \( H_2S \)) to 0 (in \( S \)). This is an increase in oxidation state, indicating that sulfur is oxidized.
- For chlorine in \( Cl_2 \):
- Changes from 0 (in \( Cl_2 \)) to -1 (in \( HCl \)). This is a decrease in oxidation state, indicating that chlorine is reduced.

4. **Identify the Oxidizing Agent**:
- An oxidizing agent is a substance that causes oxidation in another substance while being reduced itself.
- In this reaction, chlorine (\( Cl_2 \)) is reduced (its oxidation state decreases from 0 to -1), and it causes the oxidation of sulfur in \( H_2S \) (oxidation state increases from -2 to 0).
- Therefore, the oxidizing agent in this reaction is \( Cl_2 \).

### Final Answer:
The oxidizing agent in the reaction \( H_2S + Cl_2 \rightarrow 2HCl + S \) is \( Cl_2 \).

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