One of the principal goals of chemical synthesis is to maximize the conversion of the reactants to products while minimizing the expenditure of energy.
This implies maximum yield of products at mild temperature and pressure conditions.
If it does not happen, then the experimental conditions need to be adjusted. For example, in the Haber process for the synthesis of ammonia from N2 and H2, the choice of experimental conditions is of real economic importance.
Annual world production of ammonia is about hundred million tones, primarily for use as fertilizers.
Equilibrium constant, Kc is independent of initial concentrations. But if a system at equilibrium is subjected to a change in the concentration of one or more of the reacting substances, then the system is no longer at equilibrium; and net reaction takes place in some direction until the system returns to equilibrium once again.
Similarly, a change in temperature or pressure of the system may also alter the equilibrium. In order to decide what course the reaction adopts and make a qualitative prediction about the effect of a change in conditions on equilibrium we use Le Chatelier’s principle.
It states that a change in any of the factors that determine the equilibrium conditions of a system will cause the system to change in such a manner to reduce or to counteract the effect of the change. This is applicable to all physical and chemical equilibria.
We shall now be discussing factors which can influence the equilibrium.