Topic overview

Start with the big picture

The Arrhenius equation, k = A exp(−Ea/RT), relates a reaction’s rate constant to absolute temperature, the pre-exponential factor, and activation energy. In its linearized form, a plot of ln k against 1/T has slope −Ea/R and intercept ln A, providing a route to estimate these parameters from experimental data. The lesson also introduces the empirical Q₁₀ measure of temperature sensitivity and uses collision theory to explain why warming can increase reaction rates. It places Arrhenius behavior alongside transition-state theory, catalysis, and the isokinetic relationship, while noting practical limits such as temperature-dependent parameters and solution effects. Finally, it distinguishes kinetic temperature sensitivity from the effect of reaction enthalpy on equilibrium.