What effect does a 10-degree Kelvin increase in temperature have on reaction rates?

A 10-degree Kelvin increase in temperature generally leads to a significant increase in the rate of chemical reactions, often approximated to roughly double the reaction rate. This relationship is rooted in the principles of kinetic molecular theory and the Arrhenius equation, which indicates that as temperature rises, the kinetic energy of the molecules also increases.

Higher kinetic energy results in more frequent collisions between reactant molecules and these collisions are more likely to have enough energy to overcome the activation energy barrier necessary for the reaction to occur. This increased frequency and energy of collisions is why the reaction rate can double with a relatively small temperature increase, making the more common rule of thumb that for many reactions, a 10-degree Celsius (or Kelvin) temp increase can double the reaction rate applicable in numerous cases, particularly in organic and aqueous reactions.

This significant effect emphasizes the sensitivity of reaction rates to temperature changes, showcasing the importance of temperature control in chemical processes.