Liquid nitrogen

From Infogalactic: the planetary knowledge core
Jump to: navigation, search
"LN2" redirects here. For the high-speed railway line in France, see LGV Atlantique.
Liquid nitrogen
A demonstration of liquid nitrogen at the Freeside maker space in Atlanta, Georgia during the Online News Association conference in 2013
Students preparing homemade ice cream with liquid nitrogen.

Liquid nitrogen is nitrogen in a liquid state at an extremely low temperature. It is produced industrially by fractional distillation of liquid air. Liquid nitrogen is a colorless clear liquid with density of 0.807 g/ml at its boiling point and a dielectric constant of 1.43.[1] Liquid nitrogen is often referred to by the abbreviation, LN2 or "LIN" or "LN" and has the UN number 1977. Liquid nitrogen is a diatomic liquid, which means that the diatomic character of the covalent N bonding in N2 gas is retained after liquefaction.[2]

At atmospheric pressure, liquid nitrogen boils at −195.79 °C (77 K; −320 °F) and is a cryogenic fluid that can cause rapid freezing on contact with living tissue. When appropriately insulated from ambient heat, liquid nitrogen can be stored and transported, for example in vacuum flasks. Here, the very low temperature is held constant at 77 K by slow boiling of the liquid, resulting in the evolution of nitrogen gas. Depending on the size and design, the holding time of vacuum flasks (Dewars) ranges from a few hours to a few weeks. The development of pressurised super-insulated vacuum vessels has enabled liquefied nitrogen to be stored and transported over longer time periods with losses reduced to 2% per day or less.[3]

Liquid nitrogen can easily be converted to a solid by placing it in a vacuum chamber pumped by a rotary vacuum pump.[4] Liquid nitrogen freezes at 63 K (−210 °C; −346 °F). Despite its reputation, liquid nitrogen's efficiency as a coolant is limited by the fact that it boils immediately on contact with a warmer object, enveloping the object in insulating nitrogen gas. This effect, known as the Leidenfrost effect, applies to any liquid in contact with an object significantly hotter than its boiling point. More-rapid cooling may be obtained by plunging an object into a slush of liquid and solid nitrogen rather than liquid nitrogen alone.

Nitrogen was first liquefied at the Jagiellonian University on 15 April 1883 by Polish physicists, Zygmunt Wróblewski and Karol Olszewski.[5]


Liquid nitrogen is a compact and readily transported source of nitrogen gas, as it does not require pressurization. Further, its ability to maintain temperatures far below the freezing point of water makes it extremely useful in a wide range of applications, primarily as an open-cycle refrigerant, including:

Culinary use of liquid nitrogen

The culinary use of liquid nitrogen is mentioned in an 1890 recipe book titled Fancy Ices authored by Mrs. Agnes Marshall,[14] but has been employed in more recent times by restaurants in the preparation of frozen desserts, such as ice cream, which can be created within moments at the table because of the speed at which it cools food.[14] The rapidity of chilling also leads to the formation of smaller ice crystals, which provides the dessert with a smoother texture.[14] The technique is employed by chef Heston Blumenthal who has used it at his restaurant, The Fat Duck to create frozen dishes such as egg and bacon ice cream.[14][15] Liquid nitrogen has also become popular in the preparation of cocktails because it can be used to quickly chill glasses or freeze ingredients.[16] It is also added to drinks to create a smoky effect, which occurs as tiny droplets of the liquid nitrogen come into contact with the surrounding air, condensing the vapour that is naturally present.[16]


Filling a liquid nitrogen Dewar from a storage tank

Because the liquid-to-gas expansion ratio of nitrogen is 1:694 at 20 °C (68 °F), a tremendous amount of force can be generated if liquid nitrogen is rapidly vaporized. In an incident on January 12, 2006 at Texas A&M University, the pressure-relief devices of a tank of liquid nitrogen were malfunctioning and later sealed. As a result of the subsequent pressure buildup, the tank failed catastrophically. The force of the explosion was sufficient to propel the tank through the ceiling immediately above it, shatter a reinforced concrete beam immediately below it, and blow the walls of the laboratory 0.1–0.2 m off their foundations.[17]

Because of its extremely low temperature, careless handling of liquid nitrogen may result in cold burns. In that case, use special gloves while handling.

As liquid nitrogen evaporates it reduces the oxygen concentration in the air and can act as an asphyxiant, especially in confined spaces. Nitrogen is odorless, colorless, and tasteless and may produce asphyxia without any sensation or prior warning.[18] A laboratory assistant died in Scotland in 1999, apparently from asphyxiation caused by liquid nitrogen spilled in a basement storage room.[19] In 2012, a young woman in England had her stomach removed after ingesting a cocktail made with liquid nitrogen.[20]

Oxygen sensors are sometimes used as a safety precaution when working with liquid nitrogen to alert workers of gas spills into a confined space.[21]

Vessels containing liquid nitrogen can condense oxygen from air. The liquid in such a vessel becomes increasingly enriched in oxygen (boiling point 90 K; −183 °C; −298 °F) as the nitrogen evaporates, and can cause violent oxidation of organic material.[22]


Main article: Air separation

Liquid nitrogen is produced commercially from the cryogenic distillation of liquified air or from the liquefication of pure nitrogen derived from air using pressure swing adsorption. An air compressor is used to compress filtered air to high pressure; the high-pressure gas is cooled back to ambient temperature, and allowed to expand to a low pressure. The expanding air cools greatly (the Joule–Thomson effect), and oxygen, nitrogen, and argon are separated by further stages of expansion and distillation. Small-scale production of liquid nitrogen is easily achieved using this principle. Liquid nitrogen may be produced for direct sale, or as a byproduct of manufacture of liquid oxygen used for industrial processes such as steelmaking. Liquid-air plants producing on the order of tons per day of product started to be built in the 1930s but became very common after the Second World War; a large modern plant may produce 3000 tons/day of liquid air products.[23]

See also


  1. Murphy, E. J.; Morgan, S. O. "The Dielectric Properties of Insulating Materials" (PDF). Retrieved October 2, 2012. 
  2. Henshaw, D. G.; Hurst, D. G.; Pope, N. K. (1953). "Structure of Liquid Nitrogen, Oxygen, and Argon by Neutron Diffraction". Physical Review. 92: 1229. doi:10.1103/PhysRev.92.1229. 
  3. DATA BOOK for Cryogenic Gases and Equipment.
  4. Umrath, W. (1974). "Cooling bath for rapid freezing in electron microscopy". Journal of Microscopy. 101: 103–105. doi:10.1111/j.1365-2818.1974.tb03871.x. 
  5. Tilden, William Augustus (2009). A Short History of the Progress of Scientific Chemistry in Our Own Times. BiblioBazaar, LLC. p. 249. ISBN 1-103-35842-1. 
  6. Wainner, Scott; Richmond, Robert (2003). The Book of Overclocking: Tweak Your PC to Unleash Its Power. No Starch Press. p. 44. ISBN 1-886411-76-X. 
  7. Karam, Robert D. (1998). Satellite Thermal Control for System Engineers. AIAA. p. 89. ISBN 1-56347-276-7. 
  8. Liquid Nitrogen Ice Cream Recipe, March 7, 2006
  9. Liquid nitrogen – how to dose effectively, June 19, 2012
  10. Chart Dosers Dosing Products, June 19, 2012
  11. Harrabin, Roger (2 October 2012). "Liquid air 'offers energy storage hope'". BBC. 
  12. Markham, Derek (October 3, 2012). "Frozen Air Batteries Could Store Wind Energy for Peak Demand". Treehugger. Discovery Communications. 
  13. Dyer, Ted G. (February 2010). "Freeze-branding cattle" (PDF). 
  14. 14.0 14.1 14.2 14.3 "Who What Why: How dangerous is liquid nitrogen?". BBC News. BBC. 9 October 2012. Retrieved 9 October 2012. 
  15. Wallop, Harry (9 October 2012). "The dark side of liquid nitrogen cocktails". The Daily Telegraph. Telegraph Media Group. Retrieved 12 October 2012. 
  16. 16.0 16.1 Gladwell, Amy (9 October 2012). "Teenager's stomach removed after drinking cocktail". Newsbeat. BBC. Retrieved 9 October 2012. 
  17. Mattox, Brent S. "Investigative Report on Chemistry 301A Cylinder Explosion" (reprint). Texas A&M University. 
  18. British Compressed Gases Association (2000) BCGA Code of Practice CP30. The Safe Use of Liquid nitrogen Dewars up to 50 litres. ISSN 0260-4809.
  19. Inquiry after man dies in chemical leak, BBC News, October 25, 1999.
  20. Liquid nitrogen cocktail leaves teen in hospital, BBC News, October 8, 2012.
  21. Liquid Nitrogen – Code of practice for handling. United Kingdom: Birkbeck, University of London. 2007. Retrieved 2012-02-08. 
  22. Levey, Christopher G. "Liquid Nitrogen Safety". Thayer School of Engineering at Dartmouth. 
  23. Almqvist, Ebbe (2003) History of Industrial Gases, Springer, ISBN 0306472775 p. 163