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(typed answer please) At combustion temperatures, the equilibrium constant for the reaction of N2 with O2...

(typed answer please)

At combustion temperatures, the equilibrium constant for the reaction of N2 with O2 is about
10-14. Calculate the concentration of nitric oxide that is in equilibrium with atmospheric levels of nitrogen and oxygen. Repeat the calculation for normal atmospheric temperatures, at which the equilibrium constant is about 10-30. Given that the concentration of NO that exits from the combustion zone in a vehicle is much higher than this latter equilibrium value, what does that imply about equilibrium in the reaction mixture? [Hint: Use the stoichiometry of the reaction to reduce the number of unknowns in the expression for K.]

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