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Question

The reactions PCl5(g)PCl3(g)+Cl2(g) and COCl2(g)CO(g)+Cl2(g) are simultaneously in equilibrium at constant volume. A few moles of CO(g) are introduced into the vessel. After some time, the new equilibrium concentration of

A
PCl5 will remain unchanged
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B
Cl2 will be greater
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C
PCl5 will become less
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D
PCl5 will become greater
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Solution

The correct option is C PCl5 will become less
When CO is added to the above system, the second reaction will go backwards in accordance with Le Chatelier's principle and hence, the concentration of the common molecule, i.e. Cl2 will also reduce.
So, to counter the decreased concentration of chlorine, first equilibrium will go forward and hence, the concentration of PCl5 will decreased.

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