Ostwald process
The Ostwald process is a chemical process for making nitric acid (HNO3). Wilhelm Ostwald developed the process, and he patented it in 1902.[1][2] The Ostwald process is a mainstay of the modern chemical industry, and it provides the main raw material for the most common type of fertilizer production. Historically and practically, the Ostwald process is closely associated with the Haber process, which provides the requisite raw material, ammonia (NH3).
Description
Ammonia is converted to nitric acid in 2 stages. It is oxidized by heating with oxygen in the presence of a catalyst such as platinum with 10% rhodium, to form nitric oxide /nitrogen(ii)oxide and water/steam. This reaction is strongly exothermic, making it a useful heat source once initiated:[3]
- 4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O (g) (ΔH = −905.2 kJ/mol)
Stage two encompasses two reactions and is carried out in an absorption apparatus containing water. Initially nitric oxide is oxidized again to yield nitrogen dioxide/nitrogen(iv)oxide.[3] This gas is then readily absorbed by the water, yielding the desired product (nitric acid, albeit in a dilute form), while reducing a portion of it back to nitric oxide:[3]
- 2 NO (g) + O2 (g) → 2 NO2 (g) (ΔH = −114 kJ/mol)
- 3 NO2 (g) + H2O (l) → 2 HNO3 (aq) + NO (g) (ΔH = −117 kJ/mol)
The NO is recycled, and the acid is concentrated to the required strength by distillation.
Alternatively, if the last step is carried out in air:
- 4 NO2 (g) + O2 (g) + 2 H2O (l) → 4 HNO3 (aq)
Typical conditions for the first stage, which contribute to an overall yield of about 98%, are:
- pressure is between 4–10 standard atmospheres (410–1,000 kPa; 59–150 psi) and
- temperature is about 870–1,073 K (600–800 °C; 1,100–1,500 °F).
A complication that needs to be taken into consideration involves a side-reaction in the first step that reverts the nitric oxide back to N
2:
- 4 NH
3 + 6 NO → 5 N
2 + 6 H
2O
This is a secondary reaction that is minimised by reducing the time the gas mixtures are in contact with the catalyst.[4]
References
- ^ Improvements in the Manufacture of Nitric Acid and Nitrogen Oxides, January 9, 1902
{{citation}}: Cite has empty unknown parameter:|description=(help); Unknown parameter|country-code=ignored (help); Unknown parameter|inventor-first=ignored (help); Unknown parameter|inventor-last=ignored (help); Unknown parameter|inventorlink=ignored (help); Unknown parameter|issue-date=ignored (help); Unknown parameter|patent-number=ignored (help) - ^ Improvements in and relating to the Manufacture of Nitric Acid and Oxides of Nitrogen, December 18, 1902
{{citation}}: Cite has empty unknown parameter:|description=(help); Unknown parameter|country-code=ignored (help); Unknown parameter|inventor-first=ignored (help); Unknown parameter|inventor-last=ignored (help); Unknown parameter|inventorlink=ignored (help); Unknown parameter|issue-date=ignored (help); Unknown parameter|patent-number=ignored (help) - ^ a b c Alan V. Jones; M. Clemmet; A. Higton; E. Golding (1999). Alan V. Jones (ed.). Access to chemistry. Royal Society of Chemistry. p. 250. ISBN 0-85404-564-3.
- ^ Harry Boyer Weiser (2007). Inorganic Colloid Chemistry -: The Colloidal Elements. Read Books. p. 254. ISBN 1-4067-1303-1.
External links
- Nitrogen & Phosphorus (General Chemistry course), Purdue University
- Drake, G; "Processes for the Manufacture of Nitric Acid" (1963), International Fertiliser Society (paysite/password)
- Manufacturing Nitrates: the Ostwald process Carlton Comprehensive High School; Prince Albert; Saskatchewan, Canada.