At `540 K, 0.10 mol` of `PCl_(5)` is heated in a `8L` flask. The pressure of equilibrium mixture is found to be `1.0 atm`. Calculate `K_(p)` and `K_(c )` for the reaction.

At 87^(@)C , the following equilibrium is established H_(2) (g)+S(s)hArrH_(2)S(s)(g), K_(p)=7xx10^(-2) If 0.50 mole of hydrogen and 1.0 mole of sulphuur are heated to 87^(@)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)

When PCl_(5) is heated in a closed vessel at 575 K, the total pressure at equilibrium is found to be 1 atm and partial pressure of Cl_(2) is found to the 0.324 atm . Calculate the equilibrium constant (K_(p)) for the decomposition reaction.

Two moles of PCl_(5) were introduced in a 2L, flask and heated at 600 K to attain the equilibrium, PCl_(5) was found to be 40% dissociated into PCl_(3) and Cl_(2).K_(c ) for the reaction is :