The “Haber Process”, concerning the manufacture of ammonia (NH3) with the utilization of its components Nitrogen (N2) and Hydrogen (H2), is largely recognized as an excellent example of a chemical equilibrium. Initially, this process was not too successful, since the reaction between Nitrogen and Hydrogen to produce ammonia was too time-consuming and was formed in small amounts. However, eventually Mr. Haber established the solution in order for the process to perform more profitably. He realised that the catalysts necessary were high pressure and medium temperature (500oC), whereas the most effective catalyst turned out to be oxides (compounds of oxygen and one other element) of porous iron, and slight extractions of other elements ().
The form of Ammonia materialising into gas also occurred by Fritz Haber during World War I. When the allies had blocked trades with Germany, they blocked off imports of Potassium Nitrate and Sodium Nitrate along with it. This triggered a problem for Germany as trades were their only sources of Nitrogen. After meticulous study, it was discovered by the Germans that their nitrogen source was ‘right under their noses’… literally. Their supply of Nitrogen was in the air, which consisted of about 80% of the element. With this information, Haber invented the process of extracting nitrogen from the air and using it to from Ammonia gas by coalescing it with hydrogen. (). This brings the equilibrium reaction of the “Haber Process” to be:
The breakthrough of the “Haber Process” has not only stopped at the procedure of ammonia with the two elements. Through this discovery followed the manufacture of nitric acid, which can be reacted with ammonia to form ammonium nitrate. This is used to make the highest prevalent fertilizer at present. There are three raw materials used in the procedure to manufacture ammonia. These are: Air (to produce nitrogen), and methane and water (to produce hydrogen). When methane and steam is reacted, carbon dioxide and hydrogen are created. The hydrogen that is used in the “Haber Process” is extracted from the ‘CO2–H2’ compound by *fractional distillation. There are specific conditions in order to produce ammonia. The higher the temperature, the faster the reaction ().
It is definite that the short-term impact of the “Haber Process” on societies was quite lucrative. However the discovery still has a massive impact on us today. The process encouraged people to invent more advanced, improved ways of manufacturing weaponry, and encouraged the use and creation of fertilizers. The more significant one in the urban civilization is the issue of artillery. It is believed that the “Haber Process” inspired more chemical warfare as well as the idea of armaments and war on a larger perspective. This sort of thinking could have somewhat been responsible for the commencing of World War II. In rural areas, the ‘fertilizer’ issue is more important. The reason for this is that survival is extremely crucial in the bucolic parts of the world, and the most important way of doing this is to obtain nutrition and market goods. The most common means of achieving this is to grow crops and to eat or sell them. The discovery of the “Haber Process” increased agricultural growth greatly and makes life much easier for the people of the rural areas. Another way in which Fritz Haber has ‘left his mark’ is mining. Mining includes explosives, of which plays into the “Haber Process”. Although explosives today are made much more safer and effective, they still involve some of the chemicals involved in the “Haber Process”.
There are both affirmative and pessimistic outcomes of the “Haber Process” on the environment. The fertilizers created from ammonium nitrate proved to be a great plus. It improved the health and increased the growth of crops. This causes the rate of selling to be cheaper and of good value. A major advantage is that hunger problems are solved rather easily. However, it isn’t that simple, since there are a few disadvantages as well. The application of fertilizer to the earth is sometimes overdone. This causes a harmful influence on the eco-system and the food chain as well. The fertilizer chemicals are usually washed into the river by rain, they cause plants such as algae to grow, which disrupts a lengthy cycle and eventually reaches to a point where it harms underwater life. A fertilizer negative also extends to a situation where it puts human beings in danger. This is because the nitrates from the fertilizer are flowed into the river, which is drunk by locals, and initiates them to severe illness ().
Moral and ethical considerations are always around, whether people like it or not. The main two issues surrounding this opening statement that relate to the “Haber Process” are (as usual) Fertilizers and Explosives. If used as an explosive, the “Haber Process” can have a big effect on the earth, damaging its environment. Where war is concerned, millions could be obliterated. The possible damage that could be done makes us wonder whether the use of the Process is worth the destruction. In the aspect of agriculture, the “Haber Process” is more successful. To summarize, Fertilizers help crops to sustain best possible growth. This increases the land-value, raises market sale, and feeds hungry individuals. On the down side, too much fertilizer can harm the environment. Of both these “Haber Process” issues, which do you think may be worse? The controversy of this issue is still at large, and both arguments have valid points.
Above all the debate and dispute going on over this issue, Fritz Haber still stands at the very top. His simple Nitrogen and Hydrogen combination to produce ammonia caused such commotion and questions till today, over 50 years after. It all began in Germany, and it is now spread around the world like wildfire. Life would not be as it is today without the ‘Father of Chemical Warfare’.
*Fractional Distillation: When the liquid or mixture is boiled to vaporize (liquid => gas), then is cooled by cold water to condense (gas => liquid) it back to a liquid which is collected.
BIBLIOGRAPHY
McCoy, Sara and Philips, Judy. Fritz Haber: Chemist and Patriot. [Online] Available , 1991.
-
Clark, Jim. Haber Process. [Online] Available , 2002.
-
Saunders, Nigel. Making Ammonia- the Haber Process. [Online] Available , 2000.
Aus-e-Tute. Uses and Production of Ammonia (Haber Process) [Online] Available , 2001.
-
Zmaczynski, Raymond. The Effect of the Haber process on fertilizers. [Online] Available , 1999.
