The rate of a chemical reaction increases with the increase of temperature. This is described by the Arrhenius eqaution.

$$k = \mathrm{A} e^{-\mathrm{E_a/R}T}$$

In the above equation, $\mathrm{A}$ is the Arrhenius factor or the frequency factor or the pre-exponential factor. It is specific to a given reation. $\mathrm{R}$ is the gas constant and $\mathrm{E_a}$ is the activation energy measured in joules/mol. The fraction $\mathrm{E_a/R}T$ denotes the fraction of molecules which have the energy greater than the activation energy, the energy required to make a activated complex.