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.

For the reaction : 2NO(g) + Cl_(2) (g) hArr 2NOCl (g), NO and Cl_(2) are initially taken in mole ratio 2 : 1 . The total pressure at equilibrium is found to be 1 atm . If mole of NOCl are one fourth of that of Cl_(2) at equilibrium, K_(p) for the reaction is:

For the reaction : 2NO(g) + Cl_(2) (g) hArr 2NOCl (g), NO and Cl_(2) are initially taken in mole ratio 2 : 1 . The total pressure at equilibrium is found to be 1 atm . If mole of NOCl are one fourth of that of Cl_(2) at equilibrium, K_(p) for the reaction is:

Two moles of PCl_(5) were heated to 327^(@)C in a closed two-litre vessel, and when equilibrium was achieved, PCl_(5) was found to be 40% dissociated into PCl_(3) and Cl_(2) . Calculate the equilibrium constant K_(p) and K_(c) for this reaction.

Two moles of PCl_(5) were heated to 327^(@)C in a closed two-litre vessel, and when equilibrium was achieved, PCl_(5) was found to be 40% dissociated into PCl_(3) and Cl_(2) . Calculate the equilibrium constant K_(p) and K_(c) for this reaction.

Two moles of PCl_(5) were heated to 327^(@)C in a closed two-litre vessel, and when equilibrium was achieved, PCl_(5) was found to be 40% dissociated into PCl_(3) and Cl_(2) . Calculate the equilibrium constant K_(p) and K_(c) for this reaction.

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 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.

1.5 mol of PCl_(5) are heated at constant temperature in a closed vessel of 4 L capacity. At the equilibrium point, PCl_(5) is 35% dissociated into PCl_(3) and Cl_(2) . Calculate the equilibrium constant.