2 moles of `PCl_5` were heated at `327^@C` in a 2 litre flask. It was found that `40%` of PCl_5` dissociates to give `PCl_3` and `Cl_2` at equilibrium. Calculate the equilibrium constant for the dissociation of `PCl_5` at equilibrium.

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 introduced in a 2 litre flask and heated at 600K to attain equilibrium. PCl_5 was found to be 40% dissociate into PCl_3 and Cl_2 . Calculate the value of K_c .

2 mol of HI were heated in a sealed tube at 440^(@)C until the equilibrium was reched. HI was found to be 22% dissociated. Calculate the equilibrium constant for the reaction 2HI(g)hArr H_(2)(g)+I_(2)(g) .

For the reaction A+BhArr3C at 25^(@)C , a 3 litre volume reaction vessel contains 1,2 and 4 moles of A,B and C respectively at equilibrium, calculate the equilibrium constant K_(c) of the reaction at 25^(@)C .

Two moles of HI were heated in a scaled tube at 440^@C until the equilibrium was reached. HI was found to be 22% dissociated. Calculate equilibrium constant for the reaction 2HI(g) rarr H_2(g) + I_2(g) .

A quantity of PCl_5 was heated in a 10 dm^3 vessel at 250^@C . PCl_5(g) iff PCl_3(g) + Cl_2(g) At equilibrium the vessel contains 0.1 mole of PCl_5 and 0.2 mole of Cl_2 The equilibrium constant of the reaction is

2 mol of PCl_5(g) is heated at a given temperature in a closed vessel of volume 2L. As a result, PCl_5(g) dissociates and forms PCl_3(g) and Cl_2(g) . When the dissociation reaction reaches equilibrium, it is found that 50% of PCl_5(g) has dissociated. K_c for the reaction is

At 540, the equilibrium constant K_(p) for PCl_(5) dissociation equilibrium at 1.0 atm 1.77 atm. Calculate equilibrium constant in molar concentration (K_(c)) at same temperature and pressure.

8 moles ofa gas AB_3 are introduced into 1.0 dm^3 vessel. it dissociates as 2AB_3(g) iff A_2(g) + 3B_2(g) . At equilibrium 2 mol of A_2 are found to be present. The equilibrium constant of the reaction is.

1 mol PCl_(2)(g) is heated in a closed container of 2 litre capacity. If at equilibrium, the quantity of PCl_(5)(g) be 0.2 mol then calculate the value of equilibrium constant for the given reaction, PCl_(5)(g)hArr PCl_(3)(g)+Cl_(2)(g) .