According to the concept of concentration shifts, what happens when additional product is added to a system at equilibrium?

When additional product is added to a system at equilibrium, the principle of Le Chatelier's principle applies. This principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change and restore equilibrium.

In this case, when more product is introduced into the system, it increases the concentration of the products. To restore equilibrium, the system will shift towards the left, which is the direction of the reactants. This shift helps to consume the excess product and mitigate the disturbance caused by its addition, hence restoring a new equilibrium state.

This understanding is fundamental in predicting how changes in concentration impact equilibrium systems and is critical in various chemical applications, including reaction optimization in industrial processes.