`3 g` mol of phosphorus is heated in a flask of `4 L` volume. At equilibrium, it dissociates to give `40%` of phosphorus trichloride and chlorine. Calculate the equilibrium constant.

2.2 moles of phosphorus penta chloride were taken in a closed vessel and dissociated into phosphorus trichloride and chlorine . At equilibrium , the total number of moles of the reactants and the products was 2.53 . The degree of dissociation is ,

Phosphorus pentachloride decomposes according to the reaction : PCl_5(g) hArr PCl_3(g) + Cl_2(g) 1.50 mol of PCl_5 is placed in a 500 mL of closed reaction vessel and allowed to reach equilibrium with its decomposition products, phosphorus trichloride and chlorine at 523 K. Equilibrium constant K_c is 1.80. What is the composition of mixture of equilibrium ?

Mole of PCl_(5) is heated in a closed vessel of 1 litre capacity. At equilibrium 0.4 moles of chlorine is found. 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.

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 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.

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.