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. You may want to reference (page) section 14.5 while completing this problem. Part a calculate the activation energy for the reaction. Express the activation energy in kilojoules per mole to three significant digits.

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

Activation energy

Generally the equation for the Activation energy is mathematically given as

[tex]10(\frac{kr}{ki})=\frac{Ea}{2.303R}(\frac{1}{t_1}-\frac{1}{t_2}})\\\\Therefore\\\\10(\frac{0.0815}{0.0796})=\frac{Ea}{2.303*8.314}(\frac{1}{1010}-\frac{1}{1220}})\\\\Ea=\frac{0.01024}{8.9*10^{-6}}/mol\\\\[/tex]

Ea=1.150KJ/mol

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