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Q. 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?

NTA AbhyasNTA Abhyas 2022

Solution:

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.