For the reaction `A+B hArr C+D`, the initial concentrations of A and B are equal. The equilibrium concentration of C is two times the equilibrium concentration of A. The value of equilibrium constant is ………..

For the reaction A + B hArr C + D , the concentrations of A and B are equal . The equilibrium concentration of C is twice that of A . K_(C) of the reaction is

For a reaction A_((g)) + B_((g))hArrC_((g)) + D_((g)) the intial concentration of A and B are equals but the equilibrium constant of C is twice that of equilibrium concentration of A. Then K is

At equilibrium concentration quotient is equal to the equilibrium constant.

A+3B iff 4C . The initial concentration of A and B were equal. The equilibrium concentration of A and C also are equal. Hence the K_(c) of the reaction is

In a reaction : A+B hArr C+D , the initial concentrations of A and B were 0.9 mol dm^(-3) each. At equilibrium, the concentration of D was found to be 0.6 mol dm^(-3) . What is the value of equilibrium constant for the reaction ?