If a reaction is initiated with a higher concentration of products, what is the expected shift in equilibrium?

In a chemical equilibrium, the position of the equilibrium can be influenced by changes in concentration of reactants or products. According to Le Chatelier's principle, if a system at equilibrium experiences a change (in this case, an increase in the concentration of products), the equilibrium will shift in a direction that counteracts that change.

In this scenario, starting with a higher concentration of products means that the system is already influenced to have a greater amount of products compared to reactants. To counterbalance this increase and restore equilibrium, the reaction will shift to the left, favoring the formation of reactants. This shift helps to decrease the concentration of products and brings the system back toward a state of equilibrium.

Therefore, the correct answer reflects how the increase in product concentration affects the equilibrium by shifting it towards the reactants to maintain balance.