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Q.

Exothermic formation represented by equation $\large C{l_{2(g)}}\, + \,3{F_{2(g)}}\, \rightleftharpoons \,2Cl{F_{3(g)}},$ $\large \Delta H\, = \, - 339$ kJ. Which of the following will increase the quantity of ClF₃ in equilibrium mixture ?

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a

Increasing temperature

b

Increasing volume of vessel

c

Removing Cl₂

d

Adding F₂

answer is D.

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Detailed Solution

$\large C{l_2}\left( g \right) + 3{F_2}\left( g \right) \rightleftharpoons 2Cl{F_3}\left( g \right);\Delta H = - 339kJ$

Formation of ClF₃(g) is exothermic $\large \therefore$ favoured at low T

Formation of ClF₃(g) involves decrease in volume $\large \therefore$ favoured at high P

Addition Cl₂ (or) F₂ and removal of ClF₃

Favour the formation of ClF₃

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