Nitrogen monoxide is a pollutant in the lower atmosphere that irriates the eyes and lungs and leads to the formation of acid rain. Nitrogen monoxide forms naturally in atmosphere according to the endothermic 2. reaction: N2(g) + 02 (g) → 2 NO (g) K. = 4.1 * 10-31 Assume that nitrogen composes 78% of air by volume and that oxygen composes 21% of air by volume. Given 1.0 atmospheric pressure, find the "natural" equilibrium concentration of NO in air in units of molecules/cm3. How would you expect this concentration to change in an automobile engine in which combustion is occuring? at 298 K

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Hazard Analysis and Design in Chemical Engineering

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