In the equilibrium constant for `AhArr B+C` is `K_(eq)^((1))` and that of `B+C=P` is `K_(eq)^((2))`, the equilibrium constant for `AhArr P` is :

For reaction 2A+B hArr 2C, K=x Equilibrium constant for C hArr A+1//2 B will be

For reaction 2A+B hArr 2C, K=x Equilibrium constant for C hArr A+1//2 B will be

The unit of equilibrium constant (K_(c)) in general is

For A+BhArrC+D , the equilibrium constant is K_(1) and for C+DhArA+B , the equilibrium constant is K_(2) . The correct relation between K_(1) and K_(2) is

For A+BhArrC+D , the equilibrium constant is K_(1) and for C+DhArrA+B , the equilibrium constant is K_(2) . The correct relation between K_(1) and K_(2) is

Given i) A harr B+C K_(eq)(1) ii) B+C harr P K_(eq)(2) then K_(eq) for reaction Aharrp is

Given i) A harr B+C K_(eq)(1) ii) B+C harr P K_(eq)(2) then K_(eq) for reaction Aharrp is

1 mol of A in 1 litre vessel maintained at constant T shows the equilibrium A(g) hArr B(g) +2C(g) " " K_(C_(1)) C(g) hArr 2D(g)+3B(g) " " K_(C_(2)) If the equilibrium pressure is 13/6 times of initial pressure and [C]_(eq)=4/9[A]_(eq) , Calculate K_(C_(1)) and K_(C_(2)) .

1 mol of A in 1 litre vessel maintained at constant T shows the equilibrium A(g) hArr B(g) +2C(g) " " K_(C_(1)) C(g) hArr 2D(g)+3B(g) " " K_(C_(2)) If the equilibrium pressure is 13/6 times of initial pressure and [C]_(eq)=4/9[A]_(eq) , Calculate K_(C_(1)) and K_(C_(2)) .