`A_2(g)+B_2(g)

Given, the reaction between two gases represented by A_2 and B_2 to give the compound AB(g). A_2(g) + B_2(g) iff 2AB(g) At equilibrium, the concentration of A_2 = 3.0xx10^-3M of B_2 = 4.2 xx 10^-3M of AB = 2.8 xx 10^-3M If the reaction takes place in a sealed vessel at 527^@C , then the value of K_c will be

Given the reaction between 2 gases represented by A_2 and B_2 to give the compound AB(g) is A_2(g)+B_2(g) hArr 2AB(g) . At equilibrium, concentration of A_2=3.0xx10^(-3)(M) . If the reaction takes place in a sealed vessel at 527^(@)C , then value of K_c will be-

At given temperature the reaction A_2(g)+B_2(g)hArr2AB(g) was started with 0.4 mol of A_2(g) and 0.6 mol of B_2(g) in a flask of volume 2 L. When the reaction achieved equilibrium, it was found that the reaction mixture contained 0.5 mol of AB. The equilibrium constant (K_c) for the reaction is-

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.

The dissociation equilibrium of AB_2 gas is : 2AB_2(g) overset (rarr)(larr) 2AB(g)+ B_2(g) .the degree of dissociation of AB_2 (g) is x and x << 1. Establish the relation among the degree of dissociation (x), equilibrium constant (K_p) and'total pressure (P).

If the equilibrium constant for N_2(g) + O_2(g) iff 2NO(g) is K, the equilibrium constant for 1/2N_2(g) +1/2 O_2(g) iff NO(g) will be:

A_2(g)rarr B(g)+1/2 C(g) , the increases in pressure from 100mm to 120 mm is 5 min. The rate of disappearance of A_2 in mm/min is

Given : N_2(g) + 3H_2(g) iff 2NH_3(g), K_1 N_2(g) + O_2(g) iff 2NO(g), K_2 H_2(g) + 1/2 O_2(g) iff H_2O(g), K_3 The equilibrium constant for, 2NH_3(g) + 5/2 O_2(g) iff 2NO(g) + 3H_2O(g) will be :

For the equilibrium N_2 (g) + O_2(g) = 2 NO (g)

If equilibrium constant for N_2(g)+O_2(g)