Which of the following factors does not affect K?

The equilibrium constant, represented as K, is a measure of the ratio of the concentrations of products to reactants at equilibrium for a reversible chemical reaction. It is essential to understand how various factors influence K to grasp the concept of chemical equilibrium effectively.

Temperature is a fundamental factor that affects K because the equilibrium constant is derived from the Gibbs free energy of a reaction, which varies with temperature. As temperature changes, the position of equilibrium shifts, leading to a change in K.

The concentration of reactants and products does not affect the value of the equilibrium constant K. Instead, changes in concentration will shift the position of equilibrium according to Le Châtelier’s principle but will not alter the value of K itself. This is a crucial distinction in understanding equilibrium: while the concentrations of the reactants and products dictate the state of equilibrium, they do not change the constant that describes it.

Pressure is particularly relevant for gaseous reactions, where changes in pressure can shift the position of equilibrium to favor either the reactants or products. However, similar to concentration changes, pressure does not alter the value of K for a reaction at a constant temperature.

Lastly, the nature of the reactants and products, such as the identity and phase of substances involved, certainly impacts K