We’re being asked to determine the activation energy (Ea) of a reaction. We’re given the rate constants at two different temperatures.
This means we need to use the two-point form of the Arrhenius Equation:
where 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 first-order reaction proceeds with a rate constant of 1.5x10 -5 s-1 at 25°C and 2.7x10-3 s-1 at 75°C. According to the Arrhenius equation, what is the activation energy of this reaction in kJ/mol?
A. 89.5 kJ/mol
B. 1.30 kJ/mol
C. 16.2 kJ/mol
D. 95.8 kJ/mol
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