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?

The reaction A + B hArr C + D is studied in a one litre vessel at 250^(@)C . The initial concentration of A was 3n and that of B was n. When equilibrium was attained, equilibrium concentration of C was found to the equal to the equilibrium concentration of B. What is the concentration of D at equilibrium ?

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 :

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 ………..

In a gaseous reaction A+2B iff 2C+D the initial concentration of B was 1.5 times that of A. At equilibrium the concentration of A and D were equal. Calculate the equilibrium constant K_(C) .

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

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

A reaction, A(g)+2B(g)hArr 2C(g)+D(g) was studied using an initial concentraction of B which was 1.5 times that of A. But the equilibrium concentrations of A and B were found to be equal. The vlue of K_(p) for the equilibrium is