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 a reaction A + B hArrC + D , the concentration of A, B, C and D (in moles/litre) are 0.5, 0.8, 0.4 and 1.0 respectively. The equilibrium constant is

In a reaction A+Bharr C+D the concentrations of A,B,C and D in (moles/litre) are 0.5, 0.8, 0.4 and 1.0 respectively. The equillibrium constant 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

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 ………..

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) .