Understanding the high-temperature formation and breakdown of the nitrogen oxides is essential for controlling the pollutants generated by car engines. the second-order reaction for the breakdown of nitric oxide to its elements has rate constants of 0.0796 l/mol-s at 737°c and 0.0815 l/mol-s at 947°c. what is the activation energy of this reaction? give your answer in scientific notation.

Explanation:

Using the Arrhenius equation for the give problem:

Taking the natural log (ln) of both sides, we have:

In the given problem, we have two rate constants at two different temperatures. Thus:

           (1)

         (2)

Subtracting equation (1) from equation (2), we have:

     (3)

;  

;  

Therefore, equation (3) becomes:

-2.507 - (2.531) = Ea*[0.00012 - 0.000099]

Ea = 0.024/0.000021 = 1142.86 J/mol

The activation energy of the reaction in scientific notation is

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