A system in equilibrium is described by the gaseous phase equation.
Heat`+SO_(2)Cl_(2)hArrSO_(2)+Cl_(2)`
Which of the following statement is true

Options

A. Addition of `Cl_(2)` will shift the euilibrium towards right and
temperature is raised.
B. Addition of `Cl_(2)` will shift the equilibrium towards left and
temperature is raised.
C. Withdrawal of `Cl_(2)` and `SO_(2)` will shift the equilibrium towards left
and temperature is raised
D. Withdrawal of `Cl_(2)` and `SO_(2)` will shift the equilibrium towards left
and temperature is lowered

Explanation

To solve the problem, we need to analyze the given equilibrium reaction and apply Le Chatelier's principle to determine which statement is true.

### Step-by-Step Solution:

1. **Identify the Reaction**: The reaction given is:
\[ \text{Heat} + \text{SO}_2\text{Cl}_2 \rightleftharpoons \text{SO}_2 + \text{Cl}_2 \]
This indicates that sulfur dichloride (SO₂Cl₂) decomposes into sulfur dioxide (SO₂) and chlorine gas (Cl₂) while absorbing heat.

2. **Determine the Nature of the Reaction**: Since heat is a reactant, this reaction is endothermic. In endothermic reactions, heat is absorbed, and increasing temperature favors the forward reaction.

3. **Apply Le Chatelier's Principle**: Le Chatelier's principle states that if a system at equilibrium is subjected to a change in concentration, pressure, or temperature, the equilibrium will shift in a direction that counteracts the change.

4. **Analyze the Effects of Changes**:
- **Addition of Cl₂**: If Cl₂ (a product) is added, the equilibrium will shift to the left (towards the reactants) to reduce the concentration of Cl₂.
- **Withdrawal of Cl₂**: If Cl₂ is removed, the equilibrium will shift to the right (towards the products) to replace the removed Cl₂.
- **Change in Temperature**: Since the reaction is endothermic, increasing the temperature will shift the equilibrium to the right (towards the products), while decreasing the temperature will shift it to the left (towards the reactants).

5. **Evaluate the Statements**: Based on the analysis:
- If Cl₂ is added, the equilibrium shifts to the left.
- If Cl₂ is withdrawn, the equilibrium shifts to the right.
- Increasing temperature favors the formation of products.

6. **Conclusion**: The correct statement regarding the equilibrium is that the addition of Cl₂ will shift the equilibrium towards the left.

### Final Answer:
The true statement is that the addition of Cl₂ will shift the equilibrium towards the left.