In the reaction
`2FeCl_(3)+H_(2)Srarr2FeCl_(2)+2HCl+S`

Options

A. `FeCl_(3)` acts as an oxidising agent
B. Both `H_(2)S` and `FeCl_(3)` are oxidised
C. `FeCl_(3)` is oxidised while `H_(2)S` is reduced
D. `H_(2)S` acts as an oxidising agent

Explanation

To analyze the given reaction and identify the oxidizing and reducing agents, we can follow these steps:

### Step-by-Step Solution:

1. **Write the Reaction**:
The reaction provided is:
\[ 2 \text{FeCl}_3 + \text{H}_2\text{S} \rightarrow 2 \text{FeCl}_2 + 2 \text{HCl} + \text{S} \]

2. **Determine Oxidation States**:
- For **Iron (Fe)** in FeCl₃:
The oxidation state is +3.
- For **Iron (Fe)** in FeCl₂:
The oxidation state is +2.
- For **Sulfur (S)** in H₂S:
The oxidation state is -2.
- For **Sulfur (S)** in elemental form (S):
The oxidation state is 0.

3. **Identify Changes in Oxidation States**:
- Iron (Fe) changes from +3 in FeCl₃ to +2 in FeCl₂. This indicates a **reduction** (gain of electrons).
- Sulfur (S) changes from -2 in H₂S to 0 in elemental sulfur (S). This indicates an **oxidation** (loss of electrons).

4. **Determine the Agents**:
- Since FeCl₃ is reduced (its oxidation state decreases), it acts as an **oxidizing agent**.
- Since H₂S is oxidized (its oxidation state increases), it acts as a **reducing agent**.

5. **Conclusion**:
- The correct identification is:
- FeCl₃ is the oxidizing agent.
- H₂S is the reducing agent.

### Final Answer:
- The correct option is that **FeCl₃ acts as an oxidizing agent**.