Which of these factors can change the position of equilibrium in a chemical reaction?

In a chemical reaction at equilibrium, Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.

A change in pressure can affect the equilibrium position, particularly in reactions involving gases. When the pressure is increased, the equilibrium shifts toward the side with fewer moles of gas, while a decrease in pressure favors the side with more moles of gas.

Changing the volume of a gaseous reaction system directly impacts the pressure. Decreasing the volume increases pressure, which can similarly shift the equilibrium in favor of the side with fewer gas molecules, while increasing the volume decreases pressure and shifts the equilibrium towards the side with more gas molecules.

A change in concentration of either the reactants or products will also affect the equilibrium position. Adding more reactants will shift the equilibrium to the right, producing more products, while removing reactants or adding more products will shift it to the left, favoring the formation of the reactants.

Given that all these factors can cause shifts in the equilibrium position, it is correct to conclude that changes in pressure, volume, and concentration can all lead to alterations in the established equilibrium of a chemical reaction.