Maxwell Boltzmann energy distribution?

Question

The temp of a gas is now 400 K, raised from 300K. We have a Maxwell Boltzmann energy distribution function which is asymetric

Why would a chemical reaction proceed faster at a higher temperature? ( you may assume that the activation energy does not change significantly with temperature)

Answer 1

Chemical reactions would proceed faster at higher temperatures because temperature is a measure of how fast particles are moving so if there are faster moving particles then they are move likely to collide and react. The higher temperature works as a catalyst.

Answer 2

In any gas, different molecules have different amounts of kinetic energy. The Maxwell Boltzmann distribution describes quantitatively the distribution of kinetic energies of molecules at different temperatures. At a higher temperature, a larger fraction of molecules in the sample will have an energy greater than the activation energy, and so the reaction will proceed more rapidly.