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 for the reaction in kj/mol

Answer : The activation energy for the reaction is, 1.151 KJ

Explanation :

According to the Arrhenius equation,

or,

where,

= rate constant at =

= rate constant at =

= activation energy for the reaction = ?

R = gas constant = 8.314 J/mole.K

= initial temperature =

= final temperature =

Now put all the given values in this formula, we get:

Therefore, the activation energy for the reaction is, 1.151 KJ