Nitrogen monoxide is a pollutant in the lower atmosphere that irritates the eyes and lungs and leads to the formation of acid rain. Nitrogen monoxide forms naturally in atmosphere according to the endothermic reaction:

Use the ideal gas law to calculate the concentrations of nitrogen and oxygen present in air at a pressure of 1.0 atm and a temperature of 298 K. Assume that nitrogen composes 78% of air by volume and that oxygen composes 21% of air. 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 occurring?

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N₂(g) + O₂(g) 2 NO(g) Kp = 4.1 x 10-31 at 298 K