temperature T1 = 63 oC = 336 K
T2 = 73 oC = 346 K
rate doubles . so k2 = 2 k1
ln (k2 / k1) = Ea / R [1 / T1 - 1 / T2]
ln (2 k1 / k1) = Ea / 8.314 x 10^-3 [1/336 - 1/346]
ln 2 = Ea / 8.314 x 10^-3 [1/336 - 1/346]
Ea = 67.0 kJ/mol
activation energy = 67 kJ/mol
Chemists commonly use a rule of thumb that an increase of 10 K in temperature doubles...
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