Science & Technology

ChemHistory: Ammonia and The Haber-Bosch Process

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It’s a well-known fact that we, as heterotrophic organisms, require food sources in order to survive. It also should be rather obvious that the current population of humans is well over 7 billion— a surmountable number of mouths to feed, even if some are more well-fed than others. The incredible scientific breakthrough that made such a large population even remotely feasible to sustain is credited to Fritz Haber and Carl Bosch, in a process that industrialized that which nature could not produce at the level we required: the production of reactive ammonia-based compounds.

The process of nitrogen fixation is one of the most fundamental processes that allows for life as we know it to exist. It converts (or ‘fixes’) the incredibly inert gaseous nitrogen that comprises over 70% of our atmosphere into the more reactive ammonia-group of molecules, which plants can use to biosynthesize the most fundamental molecules in life, such as nucleic acids and nucleotides. In nature, the majority of nitrogen fixation is conducted by various forms of bacteria, fungi, and legumes, with the help of an aptly named enzyme: nitrogenase. There are many biochemical quirks to this enzyme— for example, it is heavily prone to oxidative damage, and as a result nitrogen fixation is all but halted when the organism is subjected to significant oxygen levels.

In the early twentieth century, there were incredible concerns that the rapidly increasing human population could not be sustained with the plateauing agricultural growth. But this was not the only concern on people’s mind, as World War I was also a large influence on worldwide affair—and is partially the reason why the Haber-Bosch Process came to fruition. Germany, the home country of both Haber and Bosch, had munitions supplies crippled when Allied forced blockaded trade routes from South America, preventing shipments of guano and saltpeter, which was the country’s primary source for fixed nitrogen. Loss of access to these prevented Germany from producing any nitric acid— a primary chemical for the manufacturing of explosives. Haber and Bosch’s research into industrial-level nitrogen production is suspected to be primarily motivated by this deficit of nitric acid during the war, and not the impending threat of worldwide famine.

The reaction is about as simple as they come: nitrogen and hydrogen gases are combined in a 1:3 ratio, producing two equivalents of ammonia. From a thermodynamic perspective, the process is relatively straightforward to explain through a simple analysis of the reaction’s equilibria. Although the reaction does favour the ammonia products at room temperature, it has an incredibly slow rate of reaction. As a result, increasing the temperature of the reaction is required in order to have sufficient molecular collisions, but these temperatures do not favour the exothermic reaction. The final factor that allows the reaction to proceed forward, but at a sufficiently fast rate, is to increase the pressure of the reaction. As there are twice as many moles of reactants per mole of product, Le Châtelier’s principle suggests that conducting the reaction under sufficiently high pressure conditions will favour products, regardless of the temperature of the reaction. These high temperature and pressures typically correspond to 500˚C and 25 MPa in industrial settings.
Thermodynamics aside, the process also requires a catalyst in order to facilitate the breaking of the incredibly stable nitrogen-nitrogen double bonds. Today, it is a cornerstone process in the world’s resource consumption as a whole— it is suggested that 3-5% of natural gas produced in the world is consumed during the Haber-Bosch’s steam reformation to attain the hydrogen gas needed. Were it not for this revolutionary technology, the exponential increase of human population observed in the last century would not be possible, although the long term environmental impacts of this growth are not likely to be as beneficial.

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