Question

Understanding the high-temperature behavior of nitrogen oxides is essential for controlling pollution generated in automobile engines. The decomposition of nitric oxide (NO) to N2 and O2 is second order with a rate constant of 0.0796 M−1*s−1 at 737∘C and 0.0815 M−1*s−1 at 947∘C. Calculate the activation energy in kJ/mol.

I'm not exactly sure which equation to use out of the almost 50 equations I have...

Answer 1

Use the following equation:

Ln(k2/k1)=Ea/R[(1/T1)-(1/T2)]

Where

k1=0.0796 M−1*s−1
k2=0.0815 M−1*s−1
R=8.314 J/mol K.
T1=273+737=1010K
T2=273+947=1220K
and
Ea=????


Solve for Ea:


Ea={R*[Ln(k1/k2)]}/[(1/T1)-(1/T2)]

Answer 2

-1150.75