What is the expected shift in equilibrium when products are added?

When products are added to a system at equilibrium, Le Chatelier's principle states that the system will respond by trying to counteract the change that's been imposed on it. In this case, the addition of products increases their concentration. To restore equilibrium, the reaction will shift in the direction that reduces the concentration of the products, thus favoring the reverse reaction.

This means that the equilibrium will shift to the left, favoring the reactants. The system seeks to balance out the concentrations by consuming some of the added products, leading to the formation of more reactants. This principle can be applied universally to any reversible reaction, illustrating how changes in concentration, pressure, or temperature can affect the position of equilibrium.

Therefore, as products are added, the expected shift in equilibrium is towards the left.