For the reaction , `A+BhArr 3C`, if 'a' mol/litre of each 'A' and 'B' are taken initially then at equilibrium the incorrect relation is :

For the reaction : A(g)+B(g)hArr C(g)+D(g) , two moles of each A and B were taken into a flask which of following relation between the concentration terms is true when the system attains equilibrium

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 reaction A+2BhArr2C , 2.0 mole of 'A' , 3.0 mole of 'B' and 1 mole of 'C' are placed in a 2.0 L flask and the equilibrium concentration of 'C' is 1.0 mole/L.The equilibrium constant (K) for the reaction is :

In a reaction : A+B hArr C+D , the initial concentrations of A and B were 0.9 mol dm^(-3) each. At equilibrium, the concentration of D was found to be 0.6 mol dm^(-3) . What is the value of equilibrium constant for the reaction ?

For the reaction, A+B hArr 2C, 2 mol of A and 3 mol of B are allowed to react. If the equilibrium constant is 4 at 400^(@)C , what will be the moles of C at equilibrium?