According to the Arrhenius equation (k = Ae^(-Ea/RT)), the rate constant is temperature dependent. As temperature increases, the exponential factor e^(-Ea/RT) increases, leading to an increase in the rate constant. The textbook specifically states that for a rise in temperature by 10°, the rate constant is nearly doubled. This is because increasing temperature increases the fraction of molecules that collide with energies greater than the activation energy (Ea).