In which direction does the equilibrium shift if there is a decrease in the concentration of products?

When there is a decrease in the concentration of products in a chemical reaction at equilibrium, the system responds by attempting to restore balance. This phenomenon is governed by Le Chatelier's Principle, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract that change.

In this case, a decrease in the concentration of products means that the system will shift in the direction that produces more products. Thus, the equilibrium shifts to the right, favoring the formation of more products to compensate for the reduction of their concentration. As a result, the concentration of reactants will increase as they are converted into products.

The correct understanding of Le Chatelier's Principle here illustrates why the equilibrium shifts to the right, increasing the concentration of products to restore equilibrium.