What direction does a reaction proceed if ln Q/K is negative?

When considering the relationship between the reaction quotient (Q) and the equilibrium constant (K), the term ln(Q/K) is pivotal in determining the direction in which a reaction will proceed.

If ln(Q/K) is negative, it implies that Q < K. This situation indicates that the current concentrations of the reactants and products are such that there are more reactants relative to the products than is present at equilibrium. As a result, the reaction will shift to the right, meaning it will favor the formation of products in order to reach equilibrium.

In this scenario, the shift to the right increases the concentration of products, thus helping the system attain a state where Q becomes equal to K. Understanding this concept is fundamental in applying Le Chatelier’s principle for predicting how a system at equilibrium responds to changes in concentration, temperature, or pressure.