`A+B harr C+D`
Initially all are 1M, `K_c`= 100. Final concentration of D will be

For the reaction 3AhArr C+2D , initially A was taken. At equilibrium the concentration of D is twice that of A. The value of K_(c) 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)

The reaction A(aq)+ 2B(aq) harr 2C(aq) + D studied in a one litre vessel at 250^(@)C , K_(C) = 0.5 .The initial concentration of A is '3n',equilibrium concentration of "C" is found to the equal to the equilibrium concentration of "B" .What is the concentration of "D" at equilibrium?

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

The reaction A + 2B rarr 2C + D was studied using an initial concentration of B which was 1.5 times that of A. But the equilibrium concentrations of A and C were found to be equal. Then the K_(c) for the equilibrium is :