Question

Formation of $CIF_{3}$ from $Cl_{2}$ and $F_{2}$ is an exothermic process. The equilibrium system can be represented as

$Cl_{2}\left(\right.g\left.\right)+3F_{2}\left(\right.g\left.\right)\rightleftharpoons2CIF_{3};\Delta H=-329$ $kJ$

Which of the following will increase quantity of $CIF_{3}$ in the equilibrium mixture?

• A. Increase in temperature, decrease in pressure, addition of $Cl_{2}$
• B. Decrease in temperature and pressure, addition of $CIF_{3}$
• C. Increase in temperature and pressure, removal of $Cl_{2}$
• D. Decrease in temperature, increase in pressure, addition of $F_{2}$

Answer 1

Answer: (D)

Using Le-chetelier principle the formation of $ClF_{3}$ is favoured by

(i) Decrease in temperature as it is an exothermic reaction.

(ii) Increase in pressure as volume is decreasing here.

(iii) Increasing concentration of chlorine and fluorine.