Which statement best describes the relationship between Qp and Kp at equilibrium?

At equilibrium, the reaction quotient Qp, which reflects the ratio of the concentrations of the products to the reactants at any point in time, is equal to the equilibrium constant Kp, which specifically denotes this ratio at equilibrium. This equality signifies that the forward and reverse reactions occur at the same rate, and there is no net change in the concentrations of the reactants and products.

Kp is derived from the ideal gas law and is temperature-dependent, reflecting the state of the system when it has reached equilibrium. When the system reaches this state, the values of Qp and Kp converge, indicating a balance has been achieved in the chemical reaction. Therefore, at equilibrium, the relationship between Qp and Kp is one of equality, which represents a fundamental concept in chemical thermodynamics related to the behavior of reactions in equilibrium.