We’re being asked to determine the activation energy (Ea) when nitrogen tetraoxide, N2O4, decomposes to nitrogen dioxide, NO2.
We’re given the rates 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)
Dinitrogen tetraoxide, N2O4, decomposes to nitrogen dioxide, NO2, in a first-order process. If k = 1.5 x 103 s-1 at 10 °C and k = 4.0 x 103 s-1 at 30 °C, what is the activation energy for the decomposition?
a. 34998 kJ/mol
b. -35.0 kJ/mol
c. 34998 kJ/mol
d. 35.0 kJ/mol
e. 14.7 kJ/mol
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