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When considering the effect of changing the concentration of products on the equilibrium of a chemical reaction, it is important to refer to Le Chatelier's principle. This principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium will shift to counteract that change.
If the concentration of products in a reaction is increased, the system will respond by shifting the equilibrium to the left, toward the reactants. This occurs in order to reduce the concentration of the products, which helps restore the balance of the reaction. Essentially, the system tries to decrease the effect of the added products by favoring the formation of reactants.
Therefore, increasing the concentration of products causes the equilibrium to shift toward the reactants, which aligns with the behavior predicted by Le Chatelier's principle.