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.

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Casey DurganLv2

13 Feb 2019

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

Calculate the activation energy for the reaction.

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.