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Question

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

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

The correct option is D Adding F2
The formation of ClF3 is represented by the equation Cl2(g)+3F2(g)2ClF3(g); Δ H=329 kJ.
According to the Le-chatelier`s principle if any changes happen in any component then equilibirium will move that direction where the effect of that change neutralize.

(a)As this reaction is exothermic so on increasing the tempreture the reaction will go in backward direction hence this is not suitable for ClF3 to increase.

(b)On removing Cl2 reaction will go in backward direction hence this is not suitable for ClF3 to increase.

(c)On increasing the volume the reaction would go towards more no. of moles which means reaction will go in backward direction hence this is not suitable for ClF3 to increase.

(d)On adding F2 reaction will go in forward direction hence this is suitable for ClF3 to increase.




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