The value of the equilibrium constant K depends on: I. the initial concentrations of the reactants. II. the initial concentrations of the products. III. the final concentrations of the reactants. IV. the final concentrations of the products.

None of these

Explanation:

For a reaction;

aA + bB >cC + dD

The equilibrium constant K is given as;

K = [C]^c [D]^d/[A]^a [B]^b

The equilibrium constant neither depends on the concentrations of the reactants nor on that of the products.

Let us recall that at equilibrium, the concentrations of reactants and products remain largely constant. This implies that, concentration of species do not appreciably change at equilibrium because the rates of forward and reverse reactions are equal.

Hence, the equilibrium constant neither depends on the initial/final concentrations of the reactants nor on the initial/final concentrations of the products.

23.5

23.5

47.0