Arrhenius equation and activation energy
Chemical Kinetics · Chemistry
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A reaction's k doubles from 300 K to 310 K. Estimate E_a. Step 1: log(k₂/k₁) = log 2 = 0.301. Step 2: 0.301 = (E_a/2.303×8.314) × (1/300 − 1/310). Step 3: (1/300 − 1/310) = 1.075×10⁻⁴ K⁻¹. Step 4: E_a = 0.301 × 2.303 × 8.314/1.075×10⁻⁴ ≈ 53.6 kJ/mol. The 'doubles per 10 K' rule implies E_a ≈ 50–55 kJ/mol.