question_answer

The exothermic formation of \[Cl{{F}_{3}}\] is represented by the equation: \[C{{l}_{2(g)}}+3{{F}_{2(g)}}\rightleftharpoons 2Cl{{F}_{3(g)}}\];  \[\Delta H=-329\,KJ\] Which of the following will increase the quantity to \[Cl{{F}_{3}}\] 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 container

D) Adding \[{{F}_{2}}\]