Chemistry Regents Practice Test 2026 – Complete Prep Resource

Le Chatelier's principle states that when a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust itself to partially counteract that change and establish a new equilibrium. This means that if a reactant or product is added to the system, the system will shift in a direction that consumes some of the added substance. Similarly, if the temperature of an exothermic reaction is increased, the system will shift to favor the reactants, reducing the effect of the temperature increase.

Understanding this principle is crucial for predicting how changes in conditions can influence the position of an equilibrium, enabling chemists to design processes and reactions more effectively. It is especially relevant in fields such as industrial chemistry, where maximizing yield or controlling reaction rates is necessary.

Other options do not accurately describe Le Chatelier's principle. The first option relates to solubility, which is not directly connected to the equilibrium shifts described by Le Chatelier. The second option misleadingly suggests that reactions remain unchanged at equilibrium, overlooking the dynamic nature of equilibrium where reactants and products are continuously interconverting. Lastly, the fourth option pertains to electron arrangements, which fall under atomic structure and chemical bonding rather than equilibrium dynamics.