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Two systems, ...

Question

Two systems, $P C l_{5 (g)} ⇌ P C l_{3 (g)} + C l_{2 (g)}$ and $C O C l_{2 (g)} ⇌ C O_{(g)} + C l_{2 (g)}$ are simultaneously in equilibrium in a vessel at constant volume. If some $C O$ is introduced into the vessel then at the new equilibrium, the concentration of :

A

P C l_{5}

is increased

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B

P C l_{3}

remains unchanged

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C

P C l_{5}

is decreased

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D

C l_{2}

is increased

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Solution

The correct option is C $P C l_{5}$ is decreased
When $C O$ 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., $C l_{2}$ will also reduce.
So, to counteract the decreased concentration of chlorine, first equilibrium will go forward and hence, the concentration of $P C l_{5}$ will decreased.

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Similar questions

Q. The reactions,

P C l_{5} (g) ⇌ P C l_{3} (g) + C l_{2} (g)

C O C l_{2} (g) ⇌ C O (g) + C l_{2} (g)

are simultaneously in equilibrium in a vessel at a constant volume. If some

C O

is introduced into the vessel then at the new equilibrium, the concentration of:

Q. Two systems,

P {C l}_{5} (g) ⇌ P {C l}_{3} (g) + {C l}_{2} (g)

C O {C l}_{2} (g) ⇌ C O (g) + {C l}_{2} (g)

are simultaneously in equilibrium in a vessel at constant volume. If some

C O (g)

is introduced in the vessel at constant volume, then at new equilibrium, the concentration of:

Q. The reactions

P C l_{5} (g) ⇌ P C l_{3} (g) + C l_{2} (g)

C O C l_{2} (g) ⇌ C O (g) + C l_{2} (g)

are simultaneously in equilibrium at constant volume. A few moles of

C O (g)

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P C l_{5} ⇌ P C l_{3} (g) + C l_{2} (g)

C O C l_{2} (g) ⇌ C O (g) + C l_{2} (g)

are simultaneously in equilibrium at constat volume. A few moles of CO(g) are introduced into the vessel. After some time, the new equlibrium concentration of:

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P C l_{5} (g) ⇌ P C l_{3} (g) + {C l}_{2} (g) a n d C O C l_{2} (g) ⇌ C O (g) + {C l}_{2} (g)

are simultaneously in equilibrium at constant volume. A few moles of

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