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  Le Chateliers Principle

Le Chatelier’s Principle:

There are three main factors which modify the state of equilibrium. They are temperature, concentration, and pressure. The adding up of a catalyst has no effect on the state of equilibrium. Its existence merely hastens the approach of the equilibrium.

Le Chatelier’s Principle:

According to this theory when a system at equilibrium is subjected to a stress or disturbance, then the equilibrium shifts in the direction which tends to nullify the effect of the disturbance or stress. Let us assume the effects of changes in temperature, concentration &pressure, on equilibrium reactions, and the predictions of Le Chatelier’s principle.

Effect of change of concentration:

Consider the equilibrium reaction shown below:

N2(g) + O2(g) ↔ 2NO(g)

At equilibrium conditions the reaction mixture has both the reactant and product molecules, that is, N2, O2 and NO molecules. The concentrations of reactant and product molecules are constant and stay similar as long as the equilibrium conditions are sustained similar. When a change is imposed on the system by intentionally adding NO into the reaction mixture then the product concentration is increased. As the system possesses equilibrium concentrations of reactants and products, the excess quantity of NO react in the reverse direction to generate back the reactants and this outcomes in the raise in concentrations of N2 and O2. Likewise if the concentration of reactants like N2 and O2 are intentionally raised whenever the system is already in the state of equilibrium, the surplus concentrations of N2 and O2 favor forward reaction. The concentration of NO is increased in the reaction mixture.

In common, a chemical equilibrium raising the concentrations of the reactants outcomes in shifting the equilibrium in favor of the products while rising the concentrations of the products outcomes in shifting the equilibrium in favor of reactants.

 

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