Which statement is true regarding the relationship between temperature and the equilibrium of exothermic reactions?

In an exothermic reaction, heat is released as a product of the reaction process. According to Le Chatelier's principle, if you change the conditions of a system at equilibrium, the system will adjust itself to counteract that change.

When the temperature is decreased in an exothermic reaction, it is akin to removing heat from the system. To counteract this change, the equilibrium will shift in the direction that produces more heat, which is the forward reaction that produces products. As a result, this shift will increase the concentration of the products.

On the contrary, increasing the temperature of an exothermic reaction adds heat to the system. In response, the equilibrium will shift to the left, favoring the reactants in order to absorb the excess heat, thus decreasing product concentration.

The other options suggest that temperature either increases product concentration or has no effect at all, both of which contradict the established principles of chemical equilibrium in exothermic systems. Pressure changes can influence gaseous equilibria, but they do not directly affect the temperature-dependent behavior of the reaction in question.