The first-order isomerization reaction: cyclopropane → propene, has a rate constant of 1.10 × 10-4 s-1 at 470°C and 5.70 × 10-4 s-1 at 500°C. What is the activation energy, Ea, for the reaction?

Answer 1

Rearrange the two point Arrhenius equation to solve for activation energy (Ea)

ln (k₂/k₁) = (-E_a/R) (1/T₂ - 1/T₁)

Rearranged:

E_a = (R T₁ T₂) / (T₁ - T₂) x ln k₁/k₂

Temps must be in Kelvin, and R is the constant 8.314 J/ mol-K