What typically happens to the reaction rate when temperature increases?

When the temperature of a reaction is increased, the reaction rate generally increases. This is due to the fact that an increase in temperature raises the kinetic energy of the molecules involved in the reaction. As the molecules move faster, they collide more frequently and with more energy. This greater frequency and energy of collisions result in a higher probability that the reactants will overcome the activation energy barrier necessary for the reaction to occur, thus leading to an increased reaction rate.

Additionally, many reactions are characterized by an Arrhenius equation, which shows that the rate constant increases exponentially with temperature. Therefore, at higher temperatures, not only are collisions more frequent, but they are also more likely to result in successful reactions as molecules have sufficient energy to surpass the activation energy threshold. This principle is widely observed in chemical kinetics and helps to explain why many reactions proceed faster when heated.