Jump to content

Liquid nitrogen

From Wikipedia, the free encyclopedia

This is an old revision of this page, as edited by Knotsofunny (talk | contribs) at 00:03, 3 October 2024 (→Uses: typo). The present address (URL) is a permanent link to this revision, which may differ significantly from the current revision.

"LN2" redirects here. For the high-speed railway line in France, see LGV Atlantique. For the number expressed by ln 2, see Natural logarithm of 2.
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 a dewar of liquid nitrogen

Liquid nitrogen (LN2) is nitrogen in a liquid state at low temperature. Liquid nitrogen has a boiling point of about −196 °C (−321 °F; 77 K). It is produced industrially by fractional distillation of liquid air. It is a colorless, mobile liquid whose viscosity is about one-tenth that of acetone (i.e. roughly one-thirtieth that of water at room temperature). Liquid nitrogen is widely used as a coolant.

Physical properties

The diatomic character of the N2 molecule is retained after liquefaction. The weak van der Waals interaction between the N2 molecules results in little interatomic attraction. This is the cause of nitrogen's unusually low boiling point.[1]

The temperature of liquid nitrogen can readily be reduced to its freezing point −210 °C (−346 °F; 63 K) by placing it in a vacuum chamber pumped by a vacuum pump.[2] 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 an insulating layer of nitrogen gas bubbles. This effect, known as the Leidenfrost effect, occurs when any liquid comes in contact with a surface which is significantly hotter than its boiling point. Faster cooling may be obtained by plunging an object into a slush of liquid and solid nitrogen rather than liquid nitrogen alone.[2]

Handling

As a cryogenic fluid that rapidly freezes living tissue, its handling and storage require thermal insulation. It can be stored and transported in vacuum flasks, the temperature being held constant at 77 K by slow boiling of the liquid. Depending on the size and design, the holding time of vacuum flasks ranges from a few hours to a few weeks. The development of pressurised super-insulated vacuum vessels has enabled liquid nitrogen to be stored and transported over longer time periods with losses reduced to 2 percent per day or less.[3]

Uses

Liquid nitrogen may be used for cooling an overclocked computer, when an extreme measure of cooling is needed.

Liquid nitrogen is a compact and readily transported source of dry nitrogen gas, as it does not require pressurization. Further, its ability to maintain temperatures far below the freezing point of water, specific heat of 1040 J⋅kg-1⋅K-1 and heat of vaporization of 200 kJ⋅kg-1 makes it extremely useful in a wide range of applications, primarily as an open-cycle refrigerant, including:

Culinary

See also: Ice cream § Cryogenics

The culinary use of liquid nitrogen is mentioned in an 1890 recipe book titled Fancy Ices authored by 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]

History

Nitrogen was first liquefied at the Jagiellonian University on 15 April 1883 by Polish physicists Zygmunt Wróblewski and Karol Olszewski.[17]

Safety

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 vaporized in an enclosed space. 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.[18] In January 2021, a line carrying liquid nitrogen ruptured at a poultry processing plant in the U.S. state of Georgia, killing six people and injuring 11 others.[19]

Because of its extremely low temperature, careless handling of liquid nitrogen and any objects cooled by it may result in cold burns. In that case, special gloves should be used while handling. However, a small splash or even pouring down skin will not burn immediately because of the Leidenfrost effect, the evaporating gas thermally insulates to some extent, like touching a hot element very briefly with a wet finger. If the liquid nitrogen manages to pool anywhere, it will burn severely.

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.[20][21][22]

Oxygen sensors are sometimes used as a safety precaution when working with liquid nitrogen to alert workers of gas spills into a confined space.[23]

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.[24]

Ingestion of liquid nitrogen can cause severe internal damage, due to freezing of the tissues which come in contact with it and to the volume of gaseous nitrogen evolved as the liquid is warmed by body heat. In 1997, a physics student demonstrating the Leidenfrost effect by holding liquid nitrogen in his mouth accidentally swallowed the substance, resulting in near-fatal injuries. This was apparently the first case in medical literature of liquid nitrogen ingestion.[25] In 2012, a young woman in England had her stomach removed after ingesting a cocktail made with liquid nitrogen.[26]

Production

Main article: Air separation

Liquid nitrogen is produced commercially from the cryogenic distillation of liquified air or from the liquefaction 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.[citation needed] 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.[27]

See also

References

  1. ^ Henshaw, D. G.; Hurst, D. G.; Pope, N. K. (1953). "Structure of Liquid Nitrogen, Oxygen, and Argon by Neutron Diffraction". Physical Review. 92 (5): 1229–1234. Bibcode:1953PhRv...92.1229H. doi:10.1103/PhysRev.92.1229.
  2. ^ a b 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. S2CID 96286845.
  3. ^ DATA BOOK for Cryogenic Gases and Equipment Archived 2014-05-17 at the Wayback Machine. aspenycap.org
  4. ^ Wainner, Scott; Richmond, Robert (2003). The Book of Overclocking: Tweak Your PC to Unleash Its Power. No Starch Press. pp. 44. ISBN 1-886411-76-X.
  5. ^ Karam, Robert D. (1998). Satellite Thermal Control for System Engineers. AIAA. p. 89. ISBN 1-56347-276-7.
  6. ^ ACI Committee 207 – Report on Cooling and Insulating Systems for Mass Concrete
  7. ^ Liquid Nitrogen Ice Cream Recipe Archived 2009-12-20 at the Wayback Machine, March 7, 2006
  8. ^ Liquid nitrogen – how to dose effectively Archived 2013-06-16 at the Wayback Machine, June 19, 2012
  9. ^ Chart Dosers Dosing Products Archived 2013-03-04 at the Wayback Machine, June 19, 2012
  10. ^ Harrabin, Roger (2 October 2012). "Liquid air 'offers energy storage hope'". BBC. Archived from the original on 16 February 2019. Retrieved 22 June 2018.
  11. ^ Markham, Derek (October 3, 2012). "Frozen Air Batteries Could Store Wind Energy for Peak Demand". Treehugger. Discovery Communications. Archived from the original on November 5, 2012. Retrieved October 22, 2012.
  12. ^ Dyer, Ted G. (February 2010). "Freeze-branding cattle" (PDF).[dead link]
  13. ^ "Soil Freezing".
  14. ^ a b c d "Who What Why: How dangerous is liquid nitrogen?". BBC News. 9 October 2012. Archived from the original on 9 October 2012. Retrieved 9 October 2012.
  15. ^ Wallop, Harry (9 October 2012). "The dark side of liquid nitrogen cocktails". The Daily Telegraph. Archived from the original on 10 October 2012. Retrieved 12 October 2012.
  16. ^ a b Gladwell, Amy (9 October 2012). "Teenager's stomach removed after drinking cocktail". Newsbeat. BBC. Archived from the original on 9 October 2012. Retrieved 9 October 2012.
  17. ^ Tilden, William Augustus (2009). A Short History of the Progress of Scientific Chemistry in Our Own Times. BiblioBazaar, LLC. p. 249. ISBN 978-1-103-35842-7. Archived from the original on 2013-12-31. Retrieved 2016-02-28.
  18. ^ Mattox, Brent S. "Investigative Report on Chemistry 301A Cylinder Explosion" (PDF). Texas A&M University. Archived from the original (reprint) on 2008-10-31.
  19. ^ Fausset, William; Levenson, Michael (January 28, 2021). "6 Die After Liquid Nitrogen Leak at Georgia Poultry Plant". The New York Times. Archived from the original on January 29, 2021.
  20. ^ British Compressed Gases Association (2000) BCGA Code of Practice CP30. The Safe Use of Liquid nitrogen Dewars up to 50 litres. Archived 2007-07-18 at the Wayback Machine ISSN 0260-4809.
  21. ^ Confined Space Entry - Worker and Would-be Rescuer Asphyxiated Archived 2017-08-29 at the Wayback Machine, Valero Refinery Asphyxiation Incident Case Study.
  22. ^ Inquiry after man dies in chemical leak Archived 2017-01-07 at the Wayback Machine, BBC News, October 25, 1999.
  23. ^ Liquid Nitrogen – Code of practice for handling. United Kingdom: Birkbeck, University of London. 2007. Archived from the original on 2018-06-12. Retrieved 2012-02-08.
  24. ^ Levey, Christopher G. "Liquid Nitrogen Safety". Thayer School of Engineering at Dartmouth. Archived from the original on 2016-03-05. Retrieved 2012-06-23.
  25. ^ "Student Gulps Into Medical Literature". Worcester Polytechnic Institute. 20 January 1999. Archived from the original on 22 February 2014. Retrieved 11 October 2014.
  26. ^ Liquid nitrogen cocktail leaves teen in hospital Archived 2017-04-12 at the Wayback Machine, BBC News, October 8, 2012.
  27. ^ Almqvist, Ebbe (2003) History of Industrial Gases, Springer, ISBN 0306472775 p. 163
Retrieved from "https://en.wikipedia.org/w/index.php?title=Liquid_nitrogen&oldid=1249067823"