The Haber Process A Commercial Application of Equilibrium

Nitrogen, N2, is very unreactive. The Haber process is the economically important industrial process by which atmospheric N2 is converted to ammonia, NH3, a soluble, reactive compound. Innumerable dyes, plastics, explosives, fertilizers, and s)mthetic fibers are made from ammonia. The Haber process is an excellent practical apphcation of LeChateher Principle. It provides insight into kinetic and thermodynamic factors that influence reaction rates and the positions of equilibria. In this process the reaction between N2 and H2 to produce NH3 is never allowed to reach equilibrium, but moves toward it. 

The value of /Ilc is 3.6 X 10 at 25°C.This very large value of IQ indicates that if equilibrium were reached at 25°C, virtually all of the N2 and H2 (mixed in a 1 3 mole ratio) would be converted into NH3. At 25°C, the reaction occurs so slowly, however, that no measurable amount of NH3 is produced within a reasonable time. Thus, the large equihbrium constant (a thermod)mamic factor) indicates that the reaction proceeds toward the right almost completely. It tells us nothing, however, about how fast the reaction occurs (a kinetic factor). 

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