What is an equilibrium constant (K)?

The equilibrium constant (K) is defined as the ratio of the concentrations of products to the concentrations of reactants at equilibrium for a reversible chemical reaction, with each concentration raised to the power of its respective coefficient in the balanced equation. This ratio reflects the extent to which a reaction proceeds towards the formation of products versus the remaining reactants when the system has reached a state of balance.

This ratio is essential in understanding the dynamics of chemical reactions, as it provides insight into how favorably a reaction proceeds in the forward direction compared to the reverse direction at equilibrium. A larger value of K indicates that the products are favored at equilibrium, while a smaller value suggests that the reactants are favored.

It's important to note that the equilibrium constant is specific to a particular reaction at a given temperature, and while K remains constant for that reaction at that temperature, it will change if the temperature changes. This understanding of K is crucial for predicting the concentrations of reactants and products at equilibrium, which is a fundamental aspect of chemical equilibrium concepts in the study of chemistry.