How the Arrhenius Equation Explains Why Temperature Doubles Reaction Rates

The Arrhenius equation, proposed by Swedish chemist Svante Arrhenius in 1889, mathematically describes how reaction rates change exponentially with temperature rather than linearly. The equation, k = A × exp(-Ea/RT), links a reaction's rate constant to its activation energy, temperature in kelvin, and the universal gas constant. A practical example shows that for a reaction with a typical activation energy of 50,000 J/mol, a mere 10-degree kelvin rise — say from 300 K to 310 K — nearly doubles the reaction rate, with a calculated ratio of approximately 1.91. This principle underpins real-world processes including food spoilage, drug degradation, battery aging, and industrial refinery reactions, all of which accelerate exponentially with heat. Engineers use the equation in accelerated life testing, running products at elevated temperatures for short periods to reliably predict long-term performance under normal conditions.