An increase in the concentration of a product will cause the equilibrium to shift in the reverse direction, meaning it will shift towards the reactants. This shift occurs as the system tries to counteract the added product by consuming it and forming more reactants, thereby reducing the concentration of the added product.
This video explains Le Chatelier's Principle, which states that if a system at equilibrium is subjected to a change, the system will shift in a direction that counteracts that change. The video uses chemical reaction examples to illustrate how changes in concentration, pressure, and volume affect the equilibrium position.