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

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

This principle is important in understanding how changes in temperature, pressure, and concentration affect the position of equilibrium. For example, if the concentration of a reactant is increased, the equilibrium will shift to the right to produce more products and restore equilibrium. Similarly, if the temperature is increased, the equilibrium will shift in the endothermic direction to absorb the excess heat.

Le Chatelier's principle also relates to the equilibrium constant, which is a measure of the extent to which a reaction proceeds to form products. The equilibrium constant is calculated by dividing the concentration of products by the concentration of reactants, each raised to their stoichiometric coefficients. If the equilibrium constant is large, it means that the reaction proceeds almost completely to form products. Conversely, if the equilibrium constant is small, it means that the reaction hardly proceeds to form products.

Changes in temperature, pressure, and concentration can affect the equilibrium constant by shifting the position of equilibrium. However, the equilibrium constant itself does not change with changes in these factors. Therefore, Le Chatelier's principle can be used to predict the effect of changes in these factors on the position of equilibrium and the equilibrium constant.