Applications of equilibrium constant

         (1) Judging the extent of reaction

(i) If K_c > 10³, products predominate over reactants. If K_c is very large, the reaction proceeds almost all the way to completion.

(ii) If K_c < 10^-3, reactants predominate over products. If K_c is extremely small, the reaction progress hardly at all.

(iii) If K_c is in the range 10^-3 to 10³, appreaciable concentration of both reactants and products are present.

(2) The prediction of direction of the reaction: The concentration ratio, that is ratio of the product of concentrations of products to that of reactants is also known as concentration quotient and is denoted by Q.

Concentration quotient, 

It may be noted that Q becomes equal to equilibrium constant (K) when the reaction is at the equilibrium state. At equilibrium, Q = K =K_c = K_p. Thus,

(i) If Q > K, the reaction will progress in the direction of reactants (reverse reaction).

(ii) If Q < K, reaction will progress in the direction of the products (forward reaction).

        (iii) If Q = K, then the reaction mixture is already at equilibrium.

Therefore, a reaction has the tendency to form products if Q < K and to form reactants if Q > K.

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