What effect does an increase in products have on the reaction rate of a mixture at equilibrium?

In a chemical reaction at equilibrium, the forward and reverse reactions occur at the same rate, resulting in a dynamic balance between reactants and products.

Le Chatelier's Principle helps explain how changes in conditions can affect the position of an equilibrium.

If you increase the concentration of products in a reaction mixture at equilibrium, Le Chatelier's Principle predicts that the system will shift to counteract that change. In other words:

If the concentration of products increases,

Then the equilibrium position will shift to the left (toward the reactants),

Because the system attempts to reduce the excess of products by favoring the reverse reaction.

This shift helps to alleviate the stress imposed by the increase in product concentration, restoring a new equilibrium state where the rates of the forward and reverse reactions are once again equal.

It's important to note that this explanation assumes other factors, such as temperature and pressure, remain constant. Changes in these factors can influence the direction of the shift differently.