According to Le Chatelier's principle, what happens when the concentration of reactants is increased?

When the concentration of reactants is increased, the system will respond by shifting the equilibrium position to favor the forward reaction, producing more products. This response aligns with Le Chatelier's principle, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract that change.

In this case, increasing the concentration of the reactants provides more of the starting materials necessary for the reaction to proceed. Consequently, the reaction will favor the formation of products to reduce the higher concentration of reactants, thus restoring a new equilibrium.

This principle can be illustrated with a simple chemical reaction: if you have a reaction where certain reactants combine to form products, increasing the amount of reactants will induce the system to produce more products until a new equilibrium is established.