Le Chatelier's Principle Le Chatelier's principle states that when the concentration of a reactant or product in a chemical equilibrium reaction is changed,...
Le Chatelier's Principle
Le Chatelier's principle states that when the concentration of a reactant or product in a chemical equilibrium reaction is changed, the position of equilibrium will shift in the direction that results in the largest number of moles of that species being present. This principle helps chemists predict the direction in which a reaction will proceed under different conditions.
Effect of Concentration:
Increasing the concentration of a reactant shifts the equilibrium reaction towards the products.
Increasing the concentration of a product shifts the equilibrium reaction towards the reactants.
Effect of Pressure:
Increasing the pressure of a gas affects the equilibrium position.
Increasing the pressure of a gas shifts the equilibrium reaction towards the side with fewer moles of gas.
Decreasing the pressure of a gas shifts the equilibrium reaction towards the side with more moles of gas.
Effect of Temperature:
Increasing the temperature of a reaction shifts the equilibrium reaction towards the endothermic direction (reaction proceeds with the release of heat).
Decreasing the temperature of a reaction shifts the equilibrium reaction towards the exothermic direction (reaction proceeds with the absorption of heat).
Examples:
For the reaction A + B ⇌ C, increasing the concentration of A or B will shift the equilibrium reaction towards the products.
For the reaction A + B ⇌ C, increasing the temperature will shift the equilibrium reaction towards the endothermic direction.
For the reaction A + B ⇌ C, increasing the pressure will shift the equilibrium reaction towards the side with fewer moles of gas