Liquid nitrogen explained

Liquid nitrogen is a liquefied atmospheric gas produced industrially in large quantities by fractional distillation of liquid air. It is pure nitrogen in a liquid state at very low temperature. Liquid nitrogen is a colourless clear liquid with density at its boiling point of 0.807 g/mL and a dielectric constant of 1.4.[1] Liquid nitrogen is often referred to by the abbreviation, LN2 and has the UN number 1977.

At atmospheric pressure, liquid nitrogen boils at 77K and is a cryogenic fluid which can cause rapid freezing on contact with living tissue, which may lead to frostbite. 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 ranges from a few hours to a few weeks.

Liquid nitrogen can easily be converted to the solid by placing it in a vacuum chamber pumped by a rotary vacuum pump.[2] Liquid nitrogen freezes at 63K. 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 than into liquid nitrogen alone.


Liquid nitrogen is a compact and readily transported source of nitrogen gas without 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:


Since the liquid to gas expansion ratio of this substance is 1:694,[4] a tremendous amount of force can be generated when liquid nitrogen boils off for whatever reason. In an incident in 2006 at Texas A&M University, the pressure-relief devices of a tank of liquid nitrogen were sealed with brass plugs. As a result, the tank failed catastrophically, and exploded. The force of the explosion was sufficient to propel the tank through the ceiling immediately above it.[5]

Due to its extremely low temperature, careless handling of liquid nitrogen may result in cold burns. As liquid nitrogen evaporates it will reduce the oxygen concentration in the air and might act as an asphyxiant, especially in confined spaces. Nitrogen is odourless, colourless and tasteless, and may produce asphyxia without any sensation or prior warning.[6]

Vessels containing liquid nitrogen can condense oxygen from air. The liquid in such a vessel becomes increasingly enriched in oxygen (boiling point = 90 K) as the nitrogen evaporates, and can cause violent oxidation of organic material.


The cost of liquid nitrogen depends on the distance from related facilities and the price of energy; the actual cost tends to range between US$0.10 and US$0.50 per liter. [7]

See also


  1. Web site: Dielectric Constants.
  2. Umrath, W. (1974) Cooling bath for rapid freezing in electron microscopy. Journal of Microscopy 101, 103–105.
  3. Book: Wainner, Scott. The Book of Overclocking: Tweak Your PC to Unleash Its Power. Robert Richmond. 44. 188641176X. No Starch Press. 2003.
  4. Web site: Information Specific to Liquid Nitrogen. 30 July 2003. Harvard University.
  5. Web site: Investigative Report on Chemistry 301A Cylinder Explosion. Brent S. Mattox. Texas A&M University. reprint.
  6. British Compressed Gases Association (2000) BCGA Code of Practice CP30. The Safe Use of Liquid nitrogen dewars up to 50 litres. ISSN 0260-4809.
  7. Web site: Price of Liquid Nitrogen. 2008-08-29. The Physics Factbook. 2007.

External links