We are currently studying reactions in terms of kinetic energy, reaction rates, collision theory, and so on. There is a question on my assignment that is kind of boggling me right now: An increase in temperature of 10 C rarely doubles the kinetic energy of particles, and hence the number of collisions is not doubled. Yet, this temperature increase may be enough to double the rate of a slow reaction. How can this be explained? I'm not sure if it has to do with the wording of the question, but I'm really not getting this question.