Mole of `PCl_(5)` is heated in a closed vessel of 1 litre capacity. At equilibrium 0.4 moles of chlorine is found. Calculate the equilibrium constant.

Explanation

`PCl_(s_((g))) hArr PCl_(3_((g)))+Cl_(2_(g))`
Initial `[PCl_(5)]=1` moles/lit
At eqilibrium `[Cl_(2)]=0.4` moles/lit
`[PCl_(3)]` at equilibrium `0.4` moles/lit
`[PCl_(5)]` at equilibrium `0.6` moles/lit
`K_(C)=([PCl_(3)][Cl_(2)])/([PCl_(5)])`
`=(0.4xx0.4)/(0.6)=(0.16)/(0.6)`
`=0.2606`