Le Chatelier’s principle is a fundamental principle of chemistry that states that when a system at equilibrium is subjected to a stress, the equilibrium shifts in the direction that tends to counteract the stress. In simpler terms, when a system at equilibrium is disturbed, it will respond in a way that minimizes that disturbance.
There are three types of stresses that may be applied to an equilibrium system that Le Chatelier’s principle is concerned with: changes in concentration, pressure, and temperature.
1. Concentration Changes: If the concentration of reactants or products is changed, the equilibrium will shift in the direction that counteracts the change in concentration. For example, if more reactants are added to a system, the equilibrium will shift to favor the formation of products to decrease the concentration of the reactants.
2. Pressure Changes: If the pressure of a system is changed, the equilibrium will shift in the direction that counteracts the change in pressure. For example, increasing the pressure of a system with fewer gaseous molecules will cause the equilibrium to shift in the direction that reduces the number of gas molecules to decrease the pressure.
3. Temperature Changes: If the temperature of a system is changed, the equilibrium will shift in the direction that counteracts the change in temperature. For example, if a reaction is exothermic, an increase in temperature will cause the equilibrium to shift in the direction that reduces the temperature by favoring the reaction that releases heat.
Le Chatelier’s principle is a powerful tool used in predicting and understanding how an equilibrium system will respond to changes. It is used in a wide range of fields, including chemical engineering, environmental science, and industrial chemistry.
Explain Le Chatelier’s principle
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