According to general principles, how does temperature affect chemical reaction rates?

The correct choice reflects a fundamental principle in chemistry: as the temperature increases, the rate of chemical reactions typically increases. This relationship is primarily due to the fact that higher temperatures provide reactant molecules with greater kinetic energy. As a result, molecules move faster and collide more frequently with sufficient energy to overcome the activation energy barrier for the reaction to occur.

Additionally, the increased movement means that the orientation of incoming reactants during collisions is more likely to be favorable for productive interactions, further enhancing the reaction rate. This principle is well-supported by both experimental data and the Arrhenius equation, which quantitatively describes how reaction rates increase exponentially with temperature.

In summary, higher temperatures lead to increased molecular motion, more frequent collisions, and a greater likelihood of overcoming activation energy, which collectively explain why reaction rates typically increase with temperature.