When 3 moles of A and 1 mole of B are mixed in 1 litre vessel, the following reaction takes place `A_((g)) + B_((g))hArr2C_((g)). 1.5` moles of C are formed. The equilibrium constant for the reaction is

When 3.00 mole of A and 1.00 mole of B are mixed in a 1,00 litre vessel , the following reaction takes place A(g) +B(g) hArr 2C(g) the equilibrium mixture contains 0.5 mole of C. What is the value of equilibrium constant for the reaction ?

When 3.00 mole of A and 1.00 mole of B are mixed in a 1,00 litre vessel , the following reaction takes place A(g) +B(g) hArr 2C(g) the equilibrium mixture contains 0.5 mole of C. What is the value of equilibrium constant for the reaction ?

3 mols of A and 1 mol of B are mixed in a 1L container. The reaction taking place is A(g)+B(g) iff 2C(g) . If 1.5 mol of C is formed at equilibrium, the K_(c) of the reaction is

3 mole of reactant A and one mole of reactant B are mixed in a vessel of volume 1 litre . The reaction taking place is A + B hArr 2 C . If 1.5 mol of C is formed at equilibrium , the value of K_(c) is

1.1 mole of A are mixed with 2.2 mole of B and the mixture is then kept in a 1 L vessel till the equilibrium : A+2B hArr 2C+D is reached. At equilibrium 0.2 moles of C are formed. The equilibrium constant for the reaction is :

One mole of A_((g)) is heated to 300^(@) C in a closed one litre vessel till the following equilibrium is reached. A_((g)) hArr B_((g) . The equilibrium constant of the reaction at 300^(@) C is 4. What is the conc. of B ("in. mole. lit"^(-1)) at equilibrium ?