Problem: 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/molb. -35.0 kJ/molc. 34998 kJ/mold. 35.0 kJ/mole. 14.7 kJ/mol

FREE Expert Solution

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:


ln k2k1=-EaR[1T2-1T1]


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)


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Problem Details

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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