What is Le Chatelier's principle and how does it relate to chemical equilibrium?

Le Chatelier's principle states that a system at equilibrium will respond to any stress by shifting the equilibrium position.

Chemical equilibrium is a state where the rate of the forward reaction is equal to the rate of the reverse reaction, resulting in no net change in the concentrations of reactants and products. Le Chatelier's principle helps us understand how changes in conditions such as temperature, pressure, and concentration affect the equilibrium position of a reaction.

For example, if the concentration of one of the reactants is increased, the equilibrium will shift towards the side with fewer moles of gas to reduce the stress. Similarly, if the pressure is increased, the equilibrium will shift towards the side with fewer moles of gas to reduce the pressure. If the temperature is increased, the equilibrium will shift in the endothermic direction to absorb the excess heat.

Le Chatelier's principle is useful in predicting the effect of changes in conditions on the equilibrium position of a reaction. It allows us to manipulate the conditions to favour the formation of a desired product or to increase the yield of a reaction. However, it is important to note that Le Chatelier's principle only applies to reversible reactions and does not predict the rate of the reaction.