What is the term used to denote the equilibrium constant in chemical reactions?

The term used to denote the equilibrium constant in chemical reactions is represented as Kc. This constant expresses the relationship between the concentrations of the reactants and products at equilibrium for a reversible chemical reaction. Specifically, Kc is calculated using the molarity of the products raised to the power of their coefficients in the balanced chemical equation, divided by the molarity of the reactants raised to the power of their coefficients.

In the context of chemical reactions, Kc provides crucial information about the position of the equilibrium: a larger Kc value indicates that at equilibrium, the concentration of products is significantly higher than that of the reactants, suggesting the reaction favors the formation of products. Conversely, a smaller Kc value implies that reactants are favored at equilibrium.

Other terms listed, such as Ka and Kd, have specific meanings in chemistry, with Ka relating to the acid dissociation constant and Kd to the dissociation constant, each relevant to particular types of reactions or processes. However, Kc is specifically designated for equilibrium constants in general chemical reactions, making it the appropriate choice for this question.