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.

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.

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)

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