How can you predict the following stages of a reaction by comparing the value of Kc and Qc ?
(i) Net reaction proceeds in the forward direction.
(ii) Net reaction proceeds in the backward direction.
(iii) No net reaction occurs.
Kc (Equilibrium constant) is the ratio of concentration of products to that of reactants each raise to their stoichiometric coefficients at Equilibrium.
Whereas, Qc (reaction quotient) is the ratio of concentration of products to that of reactants each raise to their stoichiometric coefficients at any time during the reaction.
By comparing of values of K and Q we can know that in which direction the reaction will proceed.
(i) If Q < K, it means concentration of products is to be increased so as to reach Equilibrium concentration thus the net reaction proceeds in the forward direction.
(ii) If Q > K, it means reaction concentration of products is to be decreased so as to reach Equilibrium concentration thus the net reaction proceeds backward direction.
(iii) If Q = K, that means Equilibrium is achieved and thus no net reaction occurs.