Answer:
a. adjust to re-reach equilibrium
Step-by-step explanation:
Le Chatelier's Principle can be logically understood based on the concept of equilibrium in chemical reactions. When a chemical reaction is in equilibrium, it means that the rate of the forward reaction (from reactants to products) is equal to the rate of the reverse reaction (from products to reactants), and the concentrations of reactants and products remain constant over time.
When an equilibrium reaction is subjected to a stress, such as a change in concentration, temperature, or pressure, it disrupts the original balance between reactants and products. In response to this stress, Le Chatelier's Principle predicts that the system will adjust its position of equilibrium to counteract the change and restore balance.
For example, if the concentration of one of the reactants is increased, the system will shift the equilibrium position to the side that consumes that reactant in order to reduce its concentration and restore the original balance. Similarly, if the temperature of the system is increased, the system will shift the equilibrium position in the endothermic or exothermic direction to counteract the change in temperature. If the pressure of the system is increased, the system will shift the equilibrium position to the side with fewer moles of gas in order to reduce the pressure.
In other words, Le Chatelier's Principle states that a system at equilibrium will adjust its position of equilibrium in response to external stresses in order to re-establish a new equilibrium and restore balance between reactants and products. This logical understanding helps to explain why option a, "adjust to re-reach equilibrium," is the correct answer.