One mole of a compound AB reacts with 1 mole of a compound CD according to the equation `AB + CD hArr AD + CB`.
When equilibrium had been established it was found that `(3)/(4)` mole each of reactant AB and CD has been converted to AD and CB. There is no change in volume. The equilibrium constant for the reaction is

One mole of compound AB reacts with one mole of a compound CD according to the equation AB_((g)) + CD_((g)) hArr AD_((g)) + CB_((g)) . When equilibrium had been established it was found that 3/4 mole of reactants AB and CD had been converted to AD and CB . There is no change in volume . The equilibrium constant for the reaction is

4 moles of A are mixed with 4 moles of B, when 2 moles of C are formed at equilibrium according to the reaction A+B hArr C+D . The value of equilibrium constant is

4 moles of A are mixed with 4 moles of B, when 2 moles of C are formed at equilibrium according to the reaction A+B hArr C+D . The value of equilibrium constant is

The equilibrium constant for the reaction w+x hArr y+z is 9 . If one mole of each of w and x are mixed and there is no change in volume, the number of moles of y for formed is

The equilibrium constant for the reaction w+x hArr y+z is 9 . If one mole of each of w and x are mixed and there is no change in volume, the number of moles of y for formed is

In a gaseous reaction at equilibrium , 'n' mole of reactant 'A' decompose to give 1 mole each of C and D.It has been found that degree of dissociation of A at equilibrium is independent of total pressure.Value of 'n' is :

In a gaseous reaction at equilibrium , 'n' mole of reactant 'A' decompose to give 1 mole each of C and D.It has been found that degree of dissociation of A at equilibrium is independent of total pressure.Value of 'n' is :