For a reaction $\mathrm{A}⟶\mathrm{B}$ with activation energy ${\mathrm{E}}_a$ and rate constant $\mathrm{k}={\mathrm{Ae}}^{-\mathrm{E}a/\mathrm{RT}}$. The rate of the reaction (Rate =k[A] ) increases by increasing the temperature because

Boltzmann factor $\left(\frac{\mathrm{n}}{\mathrm{N}}\right)$=$\frac{\mathrm{k}}{\mathrm{A}}={\mathrm{e}}^{-\frac{{\mathrm{E}}_{\mathrm{a}}}{\mathrm{RT}}}$

With increase in temperature ${\mathrm{e}}^{-\frac{{\mathrm{E}}_{\mathrm{a}}}{\mathrm{RT}}}$ increases ,fraction of total reacting species having energy equal or greater than threshold energy increases ,effective collisions increases and rate of reaction increases