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The equilibrium constant for the equilib...

The equilibrium constant for the equilibirm `PCl_(5)(g)hArrPCl_(3)(g)+Cl_(2)(g)` at a particular temperature is `2xx10^(-2)" mol"L^(-1)`. The number of moles of `PCl_(5)` that must be taken in a one litre flask at the same temperature to obtain a concentration of 0.20 mole of chlorine at equilibrium is

A

`2.2`

B

`2.0`

C

`1.8`

D

`0.2`

Text Solution

Verified by Experts

The correct Answer is:
B
`PCl_(5)(g)hArrPCl_(3)(g)+Cl_(2)(g)`
`{:("Moles at initial",x,0,0),("Moles at",x-0.2,0.2,0.2),("equilibrium",,,):}`
so, equilibrium constant, `K=(|PCl_(3)||Cl_(2)|)/([PCl_(5)])`
[given, `K=2xx10^(-2)"mol/L"`]
`therefore2xx10^(-2)=(0.2xx0.2)/(x-0.2)`
`rArrx=2.2"moles"`
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