Nitric acid manufacture Haber Process

The modem process for manufacturing nitric acid depends on the catalytic oxidation of NH3 over heated Pt to give NO in preference to other thermodynamically more favour products (p. 423). The reaction was first systematically studied in 1901 by W. Ostwald (Nobel Prize 1909) and by 1908 a commercial plant near Bochum. Germany, was producing 3 tonnes/day. However, significant expansion in production depended on the economical availability of synthetic ammonia by the Haber-Bosch process (p. 421). The reactions occurring, and the enthalpy changes per mole of N atoms at 25 C are ... 

NH3. Ammonia is a colorless gas. It is a strong base, forms hydrogen bonds, is soluble in water, and is a fairly reactive molecule. Each year 12.4 million metric tons are manufactured by the Haber process (N2 + 3H2 2NH3 at 400°C and 250 atm), principally for nitric acid production, which is then used to make fertilizers and explosives. As a fertilizer, ammonia can be utilized in three ways first by direct injection... 

Ammonia, another well known cleaner, is also used to manufacture fertilizers, nitric acid, sodium carbonate (washing soda), explosives, nylon, and baking soda. Ammonia is produced by combining nitrogen gas (obtained from the air) and hydrogen gas (obtained from natural gas) in a process called the Haber-Bosch process ... 

Bosch also helped develop Haber s process into an industrial process. In 1913, Haber and Bosch opened an ammonia manufacturing plant in Germany. A year later, World War I started. Saltpeter had another use besides making fertilizer. It was also necessary to make nitric acid that was used to make explosives. When the war started, the British Navy quickly cut off Germany s supply of Chilean saltpeter. If not for the Haber process, some historians estimate that Germany would have run out of nitrates to make explosives by 1916. The war lasted another two years, however, because Germany did not need to rely on outside sources of nitrates for fertilizers or explosives. 

N2 + 3 H2 > 2 NH3 Fe, K20, and A1203 Haber process for synthesis of ammonia NH3 Manufacture of fertilizers, nitric acid... 

Nitrogen In the production of ammonia by the Haber process (see p. 176) the ammonia is then used to make nitric acid, which is used in the manufacture of dyes, explosives and fertilisers In liquid form, as a refrigerant As an inert atmosphere for some processes and chemical reactions, because of its unreactive nature for example, empty oil tankers are filled with nitrogen to prevent fires In food packaging to keep the food fresh, for example in crisp packets where it also prevents the crisps being crushed (Figure 11.10)... 

The demand for nitrogen in a chemically fixed form (as opposed to elemental nitrogen gas) drives a huge international industry that encompasses the production of seven key chemical nitrogen products ammonia, urea, nitric acid, ammonium nitrate, nitrogen solutions, ammonium sulfate and ammonium phosphates. Such nitrogen products had a total worldwide annual commercial value of about US 50 billion in 1996. The cornerstone of this industry is ammonia. Virtually all ammonia is produced in anhydrous form via the Haber process (as described in Chapter 2). Anhydrous ammonia is the basic raw material in a host of applications and in the manufacture of fertilizers, livestock feeds, commercial and military explosives, polymer intermediates, and miscellaneous chemicals35. 

Ammonia is an important base, used to make fertilizers, nylon, and nitric acid. The manufacture of ammonia depends on a process discovered by Fritz Haber (1868-1934). After gathering information from print or electronic resources, write an obituary for Haber. Describe his accomplishments and the effect on society of plentiful supplies of ammonia. 

Much of the ammonia made by the Haber Process is used directly in the manufacture of fertilisers, but large quantities are also converted to nitric acid which is used in the ... 

Nitric acid is an important industrial chemical and is manufactured on a large scale in the Haber-Bosch process closely tied to NH3 production the first step is the oxidation of NH3 to NO (equation 14.21). After cooling, NO is mixed with air and absorbed in a countercurrent of water. The reactions involved are summarized in scheme 14.109 this produces HNO3 in a concentration of a 60% by weight and it can be concentrated to 68 %> by distillation. 

Haber process /hay-ber/ An important industrial process for the manufacture of ammonia, which is used for fertilizers and for making nitric acid. The reaction is the equilibrium ... 

Nitric acid is an important industrial chemical (see Box 15.8) and is manufactured on a large scale in the Ostwald process, which is closely tied to NH3 production in the Haber-Bosch... 

Pritz Haber s successful synthesis of ammonia a few years before the First World War had a profound impact on world history. Nitric acid and nitrates are essential in the manufacture of fertilizers and explosives. Haber s synthesis of ammonia without impurities made it possible to manufacture nitric acid by the Ostwald process. Unfortunately the first major application of ammonia production was manufacture of explosives which prolonged the war. 

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