What is an example of a factor that can shift equilibrium according to Le Chatelier's principle?

Changing the temperature of the system is indeed a factor that can shift the equilibrium of a reaction, as described by Le Chatelier's principle. This principle states that if a system at equilibrium experiences a change in concentration, temperature, or pressure, the equilibrium will shift in a direction that counteracts that change.

When the temperature of a system is altered, the equilibrium can shift toward either the products or the reactants depending on whether the reaction is exothermic or endothermic. For example, if heat is added to an exothermic reaction, the system will shift toward the reactants to absorb that excess heat, whereas for an endothermic reaction, adding heat will shift the equilibrium toward the products.

In contrast, altering the activation energy (which is related to the speed of the reaction and not the equilibrium state) and adding a catalyst (which speeds up both the forward and reverse reactions equally without changing the equilibrium position) do not shift the equilibrium position. Removing a product from a reaction could shift the equilibrium toward the side of the products, but it is specifically a change in concentration, rather than a temperature change.