Pure `PCl_(5)(g)` was introduced into an evacuated vessel and comes to equilibrium at `24^(@)C` and 2 atm pressure. At equilibrium mixture contains `40%` by volume of `Cl_(2)(g)`
`PCl_(5)(g)hArr(PCl_(3)(g)+Cl_(2)(g)`
Which of the following statement(s) regarding the above equilibrium is/are correct?

Options

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)`.

Answer

A, C

Explanation

`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)`.