How does temperature affect endothermic and exothermic reactions?

Temperature has a significant role in influencing both endothermic and exothermic reactions due to the nature of energy exchange during these processes. In an endothermic reaction, which absorbs heat from its surroundings, increasing the temperature provides additional energy that can be utilized for the reaction to proceed. Essentially, this elevated energy state allows for the reactants to overcome activation energy barriers more easily, thus favoring the formation of products.

In contrast, exothermic reactions release energy, often in the form of heat, to the surroundings. As temperature increases, the equilibrium for an exothermic reaction can shift, often leading to a decreased extent of the reaction. According to Le Chatelier's principle, if a system at equilibrium is subjected to a change in temperature, the system will adjust to counteract that change. Therefore, increasing the temperature would typically favor the reactants in an exothermic context, as the system will attempt to absorb the excess heat.

This combination of principles illustrates why higher temperatures particularly favor endothermic reactions. As they require heat to proceed, supplying additional heat increases the likelihood of the reaction by providing the necessary energy for the transformation of reactants to products.