The equilibrium constant, Kc, is independent of initial concentrations.

Changes in concentration of reacting substances alter equilibrium.

Temperature or pressure changes can also alter equilibrium.

Le Chatelier's principle is used to predict the reaction course and effect of changes in conditions.Le Chatelier’s principle 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 so as to reduce or to counteract the effect of the change.

When the concentration of any of the reactants or products in a reaction at equilibrium is changed, the composition of the equilibrium mixture changes so as to minimize the effect of concentration changes.

Removing a product enhances the forward reaction and increases product concentration, with commercial applications in gas or volatile substance manufacturing.

In a gaseous reaction, pressure changes can affect product yield if the total number of moles of reactants and products differs.

In a heterogeneous equilibrium, the effect of pressure changes on solids and liquids can be ignored. In a reaction like CO(g) + 3H2(g) ⇌ CH4(g) + H2O(g), the equilibrium mixture is compressed to half its original volume, doubling total pressure.This changes the partial pressure and concentration of reactants and products, and the mixture is no longer at equilibrium.

To predict the direction of the reaction to re-establish equilibrium, apply Le Chatelier's principle, which states that the equilibrium shifts in the forward direction, decreasing the number of moles of gas or pressure.

The equilibrium remains undisturbed when an inert gas like argon is added to a reaction, Addition of inert gas as it doesn't alter the partial pressures or molar concentrations of the substance involved.

When an equilibrium is disturbed by changes in concentration, pressure, or volume, the equilibrium mixture's composition changes.

Temperature changes affect the equilibrium constant's value.

The temperature dependence of the equilibrium constant depends on the sign of ∆H for the reaction. Exothermic reactions have a negative equilibrium constant, while endothermic reactions have a positive one. Temperature changes affect the equilibrium constant and reaction rates.

The production of ammonia is an exothermic process, with low temperatures promoting high yield but slowing down the reaction and requiring a catalyst.Temperature changes impact equilibrium constant and reaction rates.

In an exothermic process, the production of ammonia involves N2(g) + 3H2(g) 2NH3(g), where raising temperature shifts equilibrium to the left and decreases ammonia concentration.Low temperatures yield high ammonia yield, but very low temperatures slow down the reaction.

A catalyst is a device that increases the rate of a chemical reaction by providing a low energy pathway for the conversion of reactants to products. It lowers the activation energy for forward and reverse reactions by the same amount and does not affect the equilibrium composition of a reaction mixture.

In the case of the formation of NH3 from dinitrogen and dihydrogen, the equilibrium constant decreases with temperature, and high temperatures yield satisfactory rates but poor yields.The optimal conditions for NH3 synthesis using a catalyst are around 500°C and 200 atm.

German chemist Fritz Haber discovered that a catalyst made of iron can improve the yield of NH3 by increasing the pressure.

In the manufacture of Sulphuric acid by contact process, platinum or vanadium penta-oxide (V2O5) is used to increase the reaction rate.