What does Le Chatelier's Principle indicate about equilibrium systems?

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will respond by shifting in a direction that counteracts the disturbance and helps restore equilibrium. This means that if a concentration of reactants or products is changed, the temperature is altered, or the pressure is modified in a gaseous system, the equilibrium will shift to either favor the formation of more products or more reactants to re-establish a new equilibrium state.

For instance, if the concentration of reactants is increased, the system will shift towards the products to consume some of the added reactants. Similarly, if the temperature of an exothermic reaction is increased, the equilibrium will shift to favor the endothermic direction, which absorbs heat. This principle is essential in predicting how changes in conditions affect the position of equilibrium in chemical reactions.

The other options do not accurately reflect the principle. The reaction does not cease; instead, it continues to occur at a new equilibrium point after a disturbance. The system does not always favor the forward reaction, as it can equally favor the reverse reaction depending on the specific changes made. Lastly, reactions are indeed ongoing at equilibrium, and the term "halted" is an inaccurate portrayal of the dynamic