Explain chatelier's principle
https://www.khanacademy.org/science/chemistry/chemical-equilibrium/factors-that-affect-chemical-equilibrium/v/le-chatelier-s-principle
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Chatelier's Principle, also known as the Le Chatelier's Principle, helps in predicting the effects of changes in conditions on a chemical equilibrium. It states that if a system at equilibrium is subjected to a change in temperature, pressure, concentration, or volume, the equilibrium will shift in a way that tends to counteract the change and restore equilibrium.
To understand Chatelier's Principle, let's consider a chemical equilibrium involving reactants and products. Reactants are the substances that react together to form products, while products are the substances formed as a result of the reaction.
When the conditions of the system are altered, the equilibrium will respond to minimize the effect of the change. Here are some examples that illustrate how Chatelier's Principle works for different types of changes:
1. Changes in concentration: If the concentration of a reactant or product is increased, the equilibrium will shift in the direction that reduces the concentration of that species. Conversely, if the concentration is decreased, the equilibrium will shift to increase the concentration of that species. This principle is based on the fact that increasing the concentration of a reactant or product favors the reaction that consumes it to restore equilibrium.
2. Changes in pressure: When the pressure is increased, Chatelier's Principle predicts that the equilibrium will shift in the direction that reduces the total number of moles of gas. Conversely, if the pressure is decreased, the equilibrium will shift to increase the total number of moles of gas. This principle applies to reactions involving gases since increasing pressure compresses the gases, and the system responds by favoring the reaction that occupies less volume.
3. Changes in temperature: Altering the temperature affects the equilibrium depending on whether the reaction is exothermic or endothermic. An exothermic reaction releases heat, while an endothermic reaction absorbs heat. According to Chatelier's Principle, increasing the temperature of an exothermic reaction will shift the equilibrium towards the reactants, which is the direction that absorbs heat and cools down the system. Conversely, increasing the temperature of an endothermic reaction will shift the equilibrium towards the products, which is the direction that releases heat and warms up the system.
In summary, Chatelier's Principle helps us understand how a system at equilibrium responds to changes in temperature, pressure, concentration, and volume. By predicting the direction of the equilibrium shift, it allows us to understand and control chemical reactions and their conditions.