`K_(c) = 9` for the reaction, `A + B hArrC + D`. If A and B are taken in equal amounts, then amount of C in equilibrium 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

The equilibrium constant K_c at 298 K for the reaction A + B = C + D is 100. Starting with an equimolar solution with concentrations of A, B, C and D all equal to 1 M, the equilibrium concentration of D is xx 10^(-2) M. (Nearest integer)

In the reversible reaction A + B hArr C + D, the concentration of each C and D at equilobrium was 0.8 mole/litre, then the equilibrium constant K_(c) will be

In the reversible reaction A + B hArr C + D, the concentration of each C and D at equilobrium was 0.8 mole/litre, then the equilibrium constant K_(c) will be

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

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 ………..