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`.

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.

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) .

1 mole N_2 and 3 moles of H_2 are taken in a 4 litre flask. If 0.25% of N_2 is converted to NH_3 at equilibrium and the reaction is N_2(g)+3H_2(g)iff2NH_3(g) . Then calculate the value of K_c under that condition. Prove that for the reaction aA_2(g)+bB_2(g)iffcAB(g) the value of the ratio K_p/K_c is 1 when a+b=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) .

A sample of pure PC l_(5) was introduced into an evacuated vessel at 473 K. after equilibrium was attained, concentration of PCl_(5) was found to be 0.5xx10^(-1)mol*L^(-1) , if value of K_(c) is 8.3xx10^(-3) , what are the concentration of PCl_(3) and Cl_(2) at equilibrium?

H_2(g)+l_2(g)iff2Hl(g) , This reaction is carried in a 2 litre flask taking 0.4 mol H_2 and 0.4 mol l_2 . At equilibrium if 0.5 mol Hl is produced then calculate the value of equilibrium constant K_c .

One mole of H_(2)O and one mole of CO are taken in 10 L vessel and heated to 725 K. at equilibrium 40% of water (by mass) reacts with CO according to the equation H_(2)O(g)+CO(g)hArr H_(2)(g)+CO_(2)(g) . Calculate the equilibrium constant for the reaction.