Chemistry - Chemical Equilibrium Question with Solution | TestHub

The reaction is ${\mathrm{Cl}}_{2(g)}+3{\mathrm{F}}_{2(g)}\rightleftharpoons 2{\mathrm{ClF}}_{3(g)}$ with $\Delta \mathrm{rH}=-329\mathrm{kJ}$ (exothermic).

According to Le Chatelier's principle:

A. Increasing temperature shifts equilibrium left (endothermic direction), decreasing ${\mathrm{ClF}}_3$.

B. Removing ${\mathrm{Cl}}_2$ shifts equilibrium left, decreasing ${\mathrm{ClF}}_3$.

C. Increasing volume (decreasing pressure) shifts equilibrium to the side with more moles of gas. There are 4 moles on the left and 2 moles on the right, so it shifts left, decreasing ${\mathrm{ClF}}_3$.

D. Adding ${\mathrm{F}}_2$ (a reactant) shifts equilibrium right, increasing ${\mathrm{ClF}}_3$.