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?

When A_2 and B_2 are allowed to react, the equilibrium constant of the reaction at 27^@C is K_C = 4 What will be the equilibrium concentration of AB?

For the reaction, A(g)+2B(g)hArr2C(g) one mole of A and 1.5 mol of B are taken in a 2.0 L vessel. At equilibrium, the concentration of C was found to be 0.35 M. The equilibrium constant (K_(c)) of the reaction would be

For the reaction, A(g)+2B(g)hArr2C(g) one mole of A and 1.5 mol of B are taken in a 2.0 L vessel. At equilibrium, the concentration of C was found to be 0.35 M. The equilibrium constant (K_(c)) of the reaction would be

In a reaction A+2B hArr 2C, 2.0 moles of 'A' 3 moles of 'B' and 2.0 moles of 'C' are placed in a 2.0 L flask and the equilibrium concentration of 'C' is 0.5 mol // L . The equilibrium constant (K) for the reaction is

In a reaction A+2B hArr 2C, 2.0 moles of 'A' 3 moles of 'B' and 2.0 moles of 'C' are placed in a 2.0 L flask and the equilibrium concentration of 'C' is 0.5 mol // L . The equilibrium constant (K) for the reaction is

For the reaction A hArr B, DeltaE for the reaction is –33.0 kJ mol^(–1) . Calculate equilibrium constant K_C for the reaction at 300 K

For the reaction A+3B hArr 2C+D initial mole of A is twice that of B . If at equilibrium moles of B and C are equal , then percent of B reacted is