We’re being asked to determine the activation energy of the reaction when k = 2.5 x 10 3 s -1 at 5°C and k = 7.0 x 10 4 s -1 at 25°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).
Dinitrogen tetraoxide, N 2O 4, decomposes to nitrogen dioxide, NO 2, in a first-order process. If k = 2.5 x 10 3 s -1 at 5 oC and k = 7.0 x 10 4 s -1 at 25°C, what is the activation energy for the decomposition?
a. 214 kJ/mol
b. 361 kJ/mol
c. 323 kJ/mol
d. 115 kJ/mol
e. 151 kJ/mol
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