In a reversible reaction `Aunderset(K_2)overset(K_1)hArrB` the initial concentration of A and B are a and b in moles per litre and the equilibrium concentrations are (a-x) and (b+x) respectively, Express x in terms of `K_1, K_2, a and b`.

The initial concentrations of A and B are same for A +2B harr 3C and when equilibrium concentrations of B and C are same then K_(c) is

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 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

A+3B iff 4C . The initial concentration of A and B were equal. The equilibrium concentration of A and C also are equal. Hence the K_(c) of the reaction is

In a chemical reaction , A+2Boverset(K)hArr2c+D, the initial concentration of B was 1.5 times of the concentrations of A , but the equilibrium concentrations of A and B were found to be equal . The equilibrium constant (K) for the aforesaid chemical reaction is :

In a chemical reaction , A+2Boverset(K)hArr2c+D, the initial concentration of B was 1.5 times of the concentrations of A , but the equilibrium concentrations of A and B were found to be equal . The equilibrium constant (K) for the aforesaid chemical reaction is :