For a system of gases A, B, C, and D at equilibrium `A+2B hArr C+3D`, the partial pressures are found to be `A=2.0, B=2.0, C=3.0,` and `D=5.0` atm. The value of equilibrium constant is ………….

For a gaseous equilibrium, A +2B hArr C + 3D the partial pressures of A, B, C and D are found to be 0.20, 0.10, 0.30 and 0.50 atm respectively. Predict the value of equilibrium constant.

Partial pressure of A, B, C, and D on the basis of gaseous system A + 2B hArr C + 3D are A = 0.02, B = 0.10, C = 0.30 and D = 0.05 atm. The numerical value of equilibrium constant is

Partial pressure of A, B, C, and D on the basis of gaseous system A + 2B hArr C + 3D are A = 0.02, B = 0.10, C = 0.30 and D = 0.05 atm. The numerical value of equilibrium constant is

Concentration of reaction and products at equilibrium for A + 2B hArr C + D are, [A] = 0.20, [B] =0.10, [C] = 0.30, [D] = 0.50 . The value of equilibrium constant is:

The reaction, 2A(g) + B(g)hArr3C(g) + D(g) is begun with the concentration of A and B both at an intial value of 1.00 M. When equilibrium is reached, the concentration of D is measured and found to be 0.25 M. The value for the equilibrium constant for this reaction is given by the expression:

The reaction, 2A(g) + B(g)hArr3C(g) + D(g) is begun with the concentration of A and B both at an intial value of 1.00 M. When equilibrium is reached, the concentration of D is measured and found to be 0.25 M. The value for the equilibrium constant for this reaction is given by the expression:

For a reaction 2A+B hArr C+D , the partial pressures of A, B , C and D at equilibrium are 0.5, 0.8, 0.7 and 1.2 atmospheres respectively. The value of K_(p) for this reaction is

In the reversible gaseous reaction , A + 2B hArr C+3D The partial pressure of A B C and D are 0.20 , 0.10 , 0.30 ,0.50 atm respectively at equilibrium. The numerical value of K_p is :