Question

The exothermic equilibrium represented be expression $C{l}_2\left(g\right)+3F_2\left(g\right)\rightleftharpoons 2Cl{F}_3\left(g\right)$. Which of the following will increase the quantity of $Cl{F}_3$ in an equilibrium mixture of $C{l}_2$, $F_2$ and $Cl{F}_3$ ?

• A. Increasing the temperature
• B. Removing $C{l}_2$
• C. Increasing the volume of the container
• D. Adding $F_2$

Answer 1

The correct option is D Adding $F_2$

Solution:- (D) Adding $F_2$

${{Cl}_2}_{\left(g\right)}+3{F_2}_{\left(g\right)}\rightleftharpoons 2{Cl{F}_3}_{\left(g\right)}\Delta H=-329kJ$

Favourable conditions-

(i) As the reaction is exothermic, hence decrease in temperature will favour the forward reaction.

(ii) Addition of reactants or removal of product will favour the forward reaction.

(iii) Here $\Delta n_g=-2$, i.e., negative, hence decrease in volume or increase in pressure will favour the forward reaction.

Hence among all the given option, adding $F_2$ will increase the quantity of $Cl{F}_3$.