15.3 from Jack Winnick, Chemical Engineering Thermodynamics, John Wiley and Sons

Question

15.3 from Jack Winnick, Chemical Engineering Thermodynamics, John Wiley and Sons, 1997.

Nitric oxide is formed in combustion processes using atmospheric air via the reaction:

N2 + O2 =2NO

The reaction is slow to proceed at low temperatures, where the equilibrium favor NO; but at typical combustion-chamber temperatures the reactions attains equilibrium rapidly. Taking a gas containing 8 mol% oxygen and 60mol% nitrogen, what would be the equilibrium NO concentration at 1000K, 1 bar? Assume no other reactions are occuring.

Explanation / Answer

Given,

oxygen = 8mole%

nitrogen= 60mol%

So, NO will be 32mol%

So, K = [NO]2/[N2][O2] = 322/60x 8 = 2.133

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