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)

The equilibrium constant (K) for the reaction. A+2BhArr2C+D is:

The equilibrium constant at 298K for a reaction, A+BhArrC+D is 100. If the initial concentrations of all the four species were 1M each, then equilibirum concentration of D (in mol L^(-1) ) will be

In the reaction A+B hArr C+D , What will happen to the equilibrium if concentration of A is increased ?

For the reaction A + B hArr 2C the value of equilibrium constant is 100 at 298 K. If the initial concentration of all the three species is 1 M each, then the equilibrium concentration of C is x xx 10^(-1) M . The value of x is _______ (Nearest integer)