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 PCI_5 were heated to 327^@C in a closed two litre vessel and when equilibrium was achieved, PCI_5 was found to be 40% dissociated into PCI_3 and CI_2 calculate the equilibrium constant (K_c) for the reaction.

Two moles of PCl_(5) were heated at 327^(@)C in a closed two litre vessel and when equilibrium was reached, PCl_(5) was found to be 40% dissociated into PCl_(3) and Cl_(2) The equilibrium constant K_(rho) for the above reaction is (approx)

Two moles of PCl_(5) were heated at 327^(@)C in a closed two litre vessel and when equilibrium was reached, PCl_(5) was found to be 40% dissociated into PCl_(3) and Cl_(2) The equilibrium constant K_(C ) for this reaction (approx) PCl_(5)(g)iffPCl_(3)(g)+Cl_(2)(g) for this reaction (approx)

Two moles of PCl_5 are heated at 327^(@) C in a closed vessel of volume 21. When equilibrium is established, it is found that 40% of PCl_5 has dissociated into PCl_3 and Cl_2 . Calculate the equilibrium constant 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.

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.

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 :

2 g molecule of PCl_5 are heated in a closed vessel of two litre capacity. When the equilibrium is attained , PCl_5 is 40% dissociated into PCl_3 and Cl_2 . The equilibrium constant is