Two moles of `NH_3` are introduced into one litre flask in which it dissociates at high temperature as `2NH_3(g) hArr N_2(g) + 3H_2(g)` Find the value of `K_C`.

8 mole of a gas AB_3 are introduced into a 1.0 dm^3 vessel. It dissociates as, 2AB_3 (g) ⇌ A_2 (g) + 3B_2 (g) At equilibrium, 2 mole of A_2 are found ot be present. What is the equilibrium constant of rection ?

If one third HI decomposes at a particular temperature: K_c for 2HI hArr H_2+ I_2 is :

If 1 mole of I_2 is introduced into 1.o litre flask at 1000 K, at equilibrium (K_c = 10^-6) which one is correct ?

Name the process employed for manufacture of NH_3 from N_2 and H_2 .

If one mole of water and one mole of CO are taken in a 10 litre vessel and heated to 986^@C , 40% of water reacts with CO as in H_2 O (l) + CO(g) harr H_2(g) + CO_2(g) . Calculate the equilibrium constant for the reaction at the temperature mentioned.

The value of K_p for the reaction N_2(g) + 3H_2(g) hArr 2NH_3 (g) is ____ than K_c .

What is the relation between K_p and K_c for the following reaction ? NH_4 Cl (s) harr NH_3 (g) + HCl(g)