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?1s?1 at 737 ?C and 0.0815 M?1s?1 at 947 ?C.

Calculate the activation energy for the reaction.

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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 737oC and 0.0815 M-1 s-1 at 947oC. Calculate the activation energy for the reaction (in kJ/mol). Give your answer using 3 significant figures.

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 Mâ1â sâ1 at 737âC and 0.0815 Mâ1â sâ1 at 947âC.

Part A

Calculate the activation energy for the reaction.

Express the activation energy in kilojoules per mole to three significant digits.

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