At combustion temperatures, the equilibrium constant for thereaction of N2 with O2 is about 10^-14. Calculate theconcentration of NO that is in equilibrium with atmospheric levelsof nitrogen and oxygen. Repeat the calculation for normalatmospheric temperatures, at which the equilibrium constant isabout 10^-30. Given that the concentration of NO that exitsfrom the combustion zone in a vehicle is much higher than thisatter equilibrium value, what does that imply about equilibrium inthe reaction mixture?