The exothermic formation of $ClF_{3}$ is represented by the equation $Cl_{2}(g) + 3F_{2}(g) \rightleftharpoons 2ClF_{3}(g);\ \ \ \ \$ $\mathrm{\Delta}H = - 329\ kJ$ Which of the following will increase the quantity of $ClF_{3}$ in an equilibrium mixture of $Cl_{2},\ F_{2}\ and\ ClF_{3}$?

Question

Dr. Abubacker · Accepted Answer

(a)
Reaction is exothermic. By Le-Chatelier’s principle, a reaction is spontaneous in forward side (in the direction of formation of more $ClF_{3})\ if\ F_{2}$ is added, temperature is lowered and $ClF_{3}$ is removed.

Q. The exothermic formation of $ClF_{3}$ is represented by the equation $Cl_{2}(g) + 3F_{2}(g) \rightleftharpoons 2ClF_{3}(g);\ \ \ \ \$ $\mathrm{\Delta}H = - 329\ kJ$ Which of the following will increase the quantity of $ClF_{3}$ in an equilibrium mixture of $Cl_{2},\ F_{2}\ and\ ClF_{3}$?

Explanation

Reviewed by Dr. Abubacker

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