How does increasing the temperature affect reaction rates?

Increasing the temperature typically leads to an increase in reaction rates due to several key factors grounded in the principles of kinetic molecular theory. As temperature rises, the kinetic energy of the reacting molecules increases. This means that the molecules move more rapidly, leading to more frequent collisions among them.

Furthermore, not only do the collisions become more frequent, but the increased kinetic energy also allows molecules to collide with greater force. This elevated energy can help overcome the activation energy barrier required for a reaction to occur, enhancing the likelihood of overcoming this threshold during molecular interactions.

Ultimately, these factors contribute to a faster reaction rate as the molecules are both colliding more often and colliding with the necessary energy to facilitate a reaction. This is why increasing temperature generally correlates with increased reaction rates, making it the correct choice in this scenario.