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For a reaction, the rate constant increases by a factor of 4 when…
Question
For a reaction, the rate constant increases by a factor of 4 when temperature rises from 300 K to 320 K. Using the Arrhenius equation with R = 8.314 J/mol/K, determine the activation energy in kJ/mol, rounded to 3 decimal places.
✓ Verified answer: 55.323checked by our engine — not a guess
Step-by-step solution
ln(k2/k1) = (Ea/R)(1/T1 - 1/T2). ln4 = (Ea/8.314)(1/300 - 1/320). (1/300 - 1/320) = 0.00033333 - 0.0003125 = 2.08333e-5. Ea = 8.314 * 1.38629 / 2.08333e-5 = 553234 J/mol = 55.323 kJ/mol. Final answer: 55.323
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