`Cl_(2)` reacts with `CS_(2)` in presence of AlCl3 to form:

Options

A. `CHCl_(3)`
B. `"CCl"_(4)`
C. `C_(3)HCl_(3)`
D. `C_(2)H_(6)`

Answer

To solve the question, we need to analyze the reaction between chlorine gas (Cl₂) and carbon disulfide (CS₂) in the presence of aluminum chloride (AlCl₃).

### Step-by-Step Solution:

1. **Identify the Reactants**:
The reactants in this reaction are chlorine gas (Cl₂) and carbon disulfide (CS₂). Additionally, aluminum chloride (AlCl₃) acts as a catalyst.

2. **Role of Aluminum Chloride (AlCl₃)**:
AlCl₃ is a Lewis acid, meaning it can accept electron pairs. In this reaction, it helps generate a more reactive electrophile from Cl₂.

3. **Formation of Electrophile**:
When Cl₂ interacts with AlCl₃, it forms a complex where one chlorine atom is abstracted, leading to the formation of Cl⁺ (a positively charged chlorine ion) and AlCl₄⁻ (a negatively charged complex). The Cl⁺ ion acts as an electrophile.

4. **Nucleophilic Attack**:
The electrophile (Cl⁺) attacks the carbon atom in CS₂. The carbon in CS₂ has a partial positive charge due to the electronegativity of sulfur, which makes it susceptible to nucleophilic attack.

5. **Formation of Products**:
The reaction results in the substitution of chlorine for sulfur in CS₂. The products formed are carbon tetrachloride (CCl₄) and disulfur dichloride (S₂Cl₂).

The overall reaction can be summarized as:
\[ CS₂ + 3Cl₂ \xrightarrow{AlCl₃} CCl₄ + S₂Cl₂ \]

### Final Answer:
The reaction of Cl₂ with CS₂ in the presence of AlCl₃ produces carbon tetrachloride (CCl₄) and disulfur dichloride (S₂Cl₂).

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