Le-Chatelier's Principle: Adding a catalyst | Equilibrium | Chemistry | Khan Academy

⁣Le Chatelier's Principle is a fundamental concept in chemistry that explains how systems at equilibrium respond to changes in conditions. According to this principle, when a system at equilibrium is subjected to an external influence, it will adjust in such a way as to counteract the change and reestablish equilibrium.

Adding a catalyst to a reaction is one such external influence. However, unlike changes in temperature, pressure, or concentrations, adding a catalyst does not directly affect the position of the equilibrium or alter the concentrations of reactants or products. Instead, a catalyst provides an alternative pathway for the reaction to occur, lowering the activation energy barrier. This allows the reaction to proceed at a faster rate without being consumed itself.

In the context of Le Chatelier's Principle, adding a catalyst to a reaction at equilibrium does not cause any immediate response. The equilibrium composition and concentrations of reactants and products remain unaffected. However, the presence of a catalyst can increase the rate at which the reaction reaches equilibrium.

It's important to note that catalysts do not shift the equilibrium position or favor the formation of products or reactants. They only enhance the rate at which the equilibrium is reached by providing an alternative reaction pathway with lower activation energy. Once equilibrium is attained, the catalyst does not affect the equilibrium concentrations.

On Khan Academy, you can find more detailed explanations and examples of Le Chatelier's Principle, as well as related topics in equilibrium chemistry. Their resources, including videos, articles, and practice exercises, can help you fully understand the principles and applications of equilibrium reactions in chemistry.

Enjoy your learning and exploration of this fascinating field!