Question

The exothermic formation of \( \text{ClF}_3 \) is represented by the equation: \[ \text{Cl}_2(g) + 3\text{F}_2(g) \rightarrow 2\text{ClF}_3(g); \Delta H = -329 \, \text{kJ} \] Which of the following will increase the quantity of \( \text{ClF}_3 \) in an equilibrium mixture of \( \text{Cl}_2 \), \( \text{F}_2 \), and \( \text{ClF}_3 \)?

• A. Adding \( \text{F}_2 \)
• B. Increasing the volume of the container
• C. Removing \( \text{Cl}_2 \)
• D. Increasing the temperature

Hint:

According to Le Chatelier's principle, adding more reactant will shift the equilibrium towards the products in an exothermic reaction.

Answer 1

The Correct Option is A

Step 1: Apply Le Chatelier's principle.
To increase the quantity of \( \text{ClF}_3 \), we can shift the equilibrium towards the product side. Adding more \( \text{F}_2 \) will push the reaction towards the formation of \( \text{ClF}_3 \).
Step 2: Conclusion.
Thus, adding more \( \text{F}_2 \) will increase the quantity of \( \text{ClF}_3 \).
Final Answer: \[ \boxed{\text{Adding F}_2} \]