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Pure PCl(5) is introduced into an evacu...

Pure `PCl_(5) ` is introduced into an evacuated chamber and to equilibrium at `247^(@)C` and 2.0 atm .The equilibrium gases mixture contains 40% chlorine by volume .
Calculate `K_(p)` at `247^(@)C` for the reaction
`PCl_(5)(g)hArrPCl_(3)(g)+Cl_(2)(g)`

A

`K_(P)` for the equilibrium is `1.6` atm

B

`K_(c)` for the equilibrium is `0.071`

C

Addition of inert gas to the equilibrium mixture at constant pressure increase the number of moles of `PCl_(3)`

D

Increase in pressure increases the number of moles of `Cl_(2)`.

Text Solution

Verified by Experts

The correct Answer is:
A, C
`Vpropn`
`P_(PCl_(3))=P_(Cl_(2))=2xx40/100=0.8atm`
`K_(P)=(0.8xx0.8)/0.40=1.6atm`
`K_(C)=(K_(P))/((RT)^(Deltan))=1.6/(0.0821xx520)=0.037`
Increase in pressure increases the number of mols `PCl_(5)(g)`.
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