You can say that the rate of the reaction approximately doubles for each 10 °C rise in the temperature.
This rule of thumb comes from the Arrhenius equation:
#color(blue)(|bar(ul(color(white)(a/a) ln(k_2/k_1) = E_a/R(1/T_1 -1/T_2)color(white)(a/a)|)))" "#
For example, if
That is, an increase of 10 °C in temperature doubles the rate.
The rule holds approximately at ambient temperatures for activation energies between 35 kJ/mol and 65 kJ/mol.