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Question

The exothermic formation of ClF3 is represented by the equation -Cl2(g)+3F2(g)2 ClF3(g);ΔrH=329 kJ
Which of the following will increase the quantity of ClF3 in an equilibrium mixture of Cl2,F2 and CIF3 ?

A
Removing Cl2
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B
Increasing the temperature
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C
Adding F2
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D
Increasing the volume of the container
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Solution

The correct option is C Adding F2
According to the Le Chatlier's principle, A system in chemical equilibrium changes towards a new equilibrium when subjected to a change in pressure, temperature, volume, or concentration. The equilibrium shift partly counteracts the change that was applied to the system initially.

Here, as the concentration of F2 is increased, the equilibrium shifts towards the opposite side resulting in the formation of ClF3

Also, as temperature is increased and the reaction is exothermic, the equilibrium constant value decreases.

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