Question

The exothermic formation of ClF₃ is represented by the equation: Cl_2(g) + 3F_2(g) ⇋ 2ClF_3(g); ΔH = –329kJ Which of the following will increase the quantity of ClF₃ in an equilibrium mixture of Cl₂ , F₂ and ClF₃ ?
(a) Increasing the temperature
(b) Removing Cl₂
(c) Increasing the volume of the container
(d) Adding F₂

Answer 1

(d) : Cl_2(g) + 3F_2(g) ⇋ 2ClF_3(g) ; ΔH = –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 farour the forward reaction.
(iii) Here Δn = 2 – 4 = –2 (i.e., –ve) hence decrease in volume or increase in pressure will favour the forward reaction.