Question:
The reaction, \( \text{SO}_2 + \text{Cl}_2 \to \text{SO}_2 \text{Cl}_2 \), is exothermic and reversible. A mixture of \( \text{SO}_2 \), \( \text{Cl}_2 \), and \( \text{SO}_2 \text{Cl}_2 \) is at equilibrium in a closed container. Now a certain quantity of extra \( \text{SO}_2 \) is introduced into the container, the volume remaining the same. Which of the following is/are true?
The reaction, \( \text{SO}_2 + \text{Cl}_2 \to \text{SO}_2 \text{Cl}_2 \), is exothermic and reversible. A mixture of \( \text{SO}_2 \), \( \text{Cl}_2 \), and \( \text{SO}_2 \text{Cl}_2 \) is at equilibrium in a closed container. Now a certain quantity of extra \( \text{SO}_2 \) is introduced into the container, the volume remaining the same. Which of the following is/are true?
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For exothermic reactions, increasing the concentration of reactants shifts the equilibrium towards the products, and heat is released.
Updated On: Mar 25, 2026
- The pressure inside the container will not change.
- The temperature will not change.
- The temperature will increase.
- The temperature will decrease.
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The Correct Option is C
Solution and Explanation
Step 1: Le Chatelier's Principle.
According to Le Chatelier's principle, if the concentration of \( \text{SO}_2 \) is increased, the equilibrium will shift to the right to produce more \( \text{SO}_2 \text{Cl}_2 \), releasing heat since the reaction is exothermic.
Thus, the correct answer is (3).
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