We’re being asked to determine the activation energy of the reaction when the rate increases from 0.27 min-1 to 0.90 min-1 at 45 to 55°C
This means we need to use the two-point form of the Arrhenius Equation:
k1 = rate constant at T1
k2 = rate constant at T2
Ea = activation energy (in J/mol)
R = gas constant (8.314 J/mol•K)
T1 and T2 = temperature (in K).
A reaction has rate constant of 0.27 min-1 at 45 C and 0.90 min-1 at 55 C. What is the activation energy for the reaction (in kJ/mol)?
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