What happens when the concentration of a product is decreased in a reversible reaction?

In a reversible reaction, when the concentration of a product is decreased, the system responds by shifting the equilibrium position to restore balance. According to Le Chatelier's principle, a system at equilibrium will adjust to counteract any changes made to it; in this case, reducing the concentration of the product disturbs the equilibrium.

As a result, more reactants will convert into products in an effort to increase the concentration of the product back to its original equilibrium state. This means that the reaction will proceed in the forward direction until a new equilibrium is established, where the concentrations of reactants and products are balanced again. Therefore, increasing the formation of products from reactants is the correct outcome of the decreased product concentration.