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Liquid helium

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Liquid helium is a physical state of helium at very low temperatures at standard atmospheric pressures. Liquid helium may show superfluidity.

Liquid helium

Liquid helium in a transparent bowl, cooled below the Lambda point, where it exhibits properties of superfluidity
Properties
He
Molar mass 4.002602 g·mol−1
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

At standard pressure, the chemical element helium exists in a liquid form only at the extremely low temperature of −269 °C (−452.20 °F; 4.15 K). Its boiling point and critical point depend on which isotope of helium is present: the common isotope helium-4 or the rare isotope helium-3. These are the only two stable isotopes of helium. See the table below for the values of these physical quantities. The density of liquid helium-4 at its boiling point and a pressure of one atmosphere (101.3 kilopascals) is about 125 g/L (0.125 g/ml), or about one-eighth the density of liquid water.[1]

Liquefaction

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Helium was first liquefied on July 10, 1908, by the Dutch physicist Heike Kamerlingh Onnes at the University of Leiden in the Netherlands.[2] At that time, helium-3 was unknown because the mass spectrometer had not yet been invented. In more recent decades, liquid helium has been used as a cryogenic refrigerant (which is used in cryocoolers), and liquid helium is produced commercially for use in superconducting magnets such as those used in magnetic resonance imaging (MRI), nuclear magnetic resonance (NMR), magnetoencephalography (MEG), and experiments in physics, such as low temperature Mössbauer spectroscopy. The Large Hadron Collider contains superconducting magnets that are cooled with 120 tonnes of liquid helium.[3]

Liquified helium-3

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See also: Fermionic condensate § Helium-3 superfluid

A helium-3 atom is a fermion and at very low temperatures, they form two-atom Cooper pairs which are bosonic and condense into a superfluid. These Cooper pairs are substantially larger than the interatomic separation.

Characteristics

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Phase diagram of helium-4
 
Liquid helium 3 and 4 isotopes in phase diagram, showing the demixing zone.

The temperature required to produce liquid helium is low because of the weakness of the attractions between the helium atoms. These interatomic forces in helium are weak to begin with because helium is a noble gas, but the interatomic attractions are reduced even more by the effects of quantum mechanics. These are significant in helium because of its low atomic mass of about four atomic mass units. The zero point energy of liquid helium is less if its atoms are less confined by their neighbors. Hence in liquid helium, its ground state energy can decrease by a naturally occurring increase in its average interatomic distance. However at greater distances, the effects of the interatomic forces in helium are even weaker.[4]

Because of the very weak interatomic forces in helium, the element remains a liquid at atmospheric pressure all the way from its liquefaction point down to absolute zero. At temperatures below their liquefaction points, both helium-4 and helium-3 undergo transitions to superfluids. (See the table below.)[4] Liquid helium can be solidified only under very low temperatures and high pressures.[5]

Liquid helium-4 and the rare helium-3 are not completely miscible.[6] Below 0.9 kelvin at their saturated vapor pressure, a mixture of the two isotopes undergoes a phase separation into a normal fluid (mostly helium-3) that floats on a denser superfluid consisting mostly of helium-4.[7] This phase separation happens because the overall mass of liquid helium can reduce its thermodynamic enthalpy by separating.

At extremely low temperatures, the superfluid phase, rich in helium-4, can contain up to 6% helium-3 in solution. This makes the small-scale use of the dilution refrigerator possible, which is capable of reaching temperatures of a few millikelvins.[6][8]

Superfluid helium-4 has substantially different properties from ordinary liquid helium.

History

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In 1908, Kamerlingh-Onnes succeeded in liquifying a small quantity of helium. In 1923, he provided advice to the Canadian physicist John Cunningham McLennan, who was the first to produce quantities of liquid helium almost on demand.[9]

In 1932 Einstein reported that the liquid helium could help in creating an atomic bomb.

Important early work on the characteristics of liquid helium was done by the Soviet physicist Lev Landau, later extended by the American physicist Richard Feynman.

In 1961, Vignos and Fairbank reported the existence of a different phase of solid helium-4, designated the gamma-phase. It exists for a narrow range of pressure between 1.45 and 1.78 K.[10]

Data

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Properties of liquid helium Helium-4 Helium-3
Critical temperature[4] 5.2 K (−267.95 °C) 3.3 K (−269.85 °C)
Boiling point at one atmosphere[4] 4.2 K (−268.95 °C) 3.2 K (−269.95 °C)
Minimum melting pressure[11] 25 bar (360 psi) 29 bar (420 psi) at 0.3 K (−272.850 °C)
Superfluid transition temperature at saturated vapor pressure 2.17 K (−270.98 °C)[12] 1 mK in the absence of a magnetic field[13]
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  •  
    Liquid helium (in a vacuum bottle) at 4.2 K (−268.95 °C) and 1 bar (15 psi) boiling slowly.
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    Lambda point transition: as the liquid is cooled down through 2.17 K (−270.98 °C), the boiling suddenly becomes violent for a moment.
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    Superfluid phase at temperature below 2.17 K (−270.98 °C). In this state, the thermal conductivity is extremely high. This causes heat in the body of the liquid to be transferred to its surface so quickly that vaporization takes place only at the free surface of the liquid. Thus, there are no gas bubbles in the body of the liquid.
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    The liquid helium is in the superfluid phase. A thin invisible film creeps up the inside wall of the bowl and down on the outside. A drop forms. It will fall off into the liquid helium below. This will repeat until the cup is empty—provided the liquid remains superfluid.

See also

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References

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  1. ^ "The Observed Properties of Liquid Helium at the Saturated Vapor Pressure". University of Oregon. 2004.
  2. ^ Wilks (1967), p. 7.
  3. ^ "Cryogenics: Low temperatures, high performance". CERN. 28 June 2023.
  4. ^ a b c d Wilks (1967), p. 1.
  5. ^ Horbaniuc, Bogdan D. (2004). "Refrigeration and Air-Conditioning". Encyclopedia of Energy: 261–289. doi:10.1016/B0-12-176480-X/00085-1. ISBN 9780121764807.
  6. ^ a b D. O. Edwards; D. F. Brewer; P. Seligman; M. Skertic & M. Yaqub (1965). "Solubility of He3 in Liquid He4 at 0K". Phys. Rev. Lett. 15 (20): 773. Bibcode:1965PhRvL..15..773E. doi:10.1103/PhysRevLett.15.773.
  7. ^ Pricaupenko, L; Triener, J. (16 January 1995). "Phase Separation of Liquid 3He–4He Mixtures: Effect of Confinement". Physical Review Letters. 74 (3): 430–433. Bibcode:1995PhRvL..74..430P. doi:10.1103/PhysRevLett.74.430. PMID 10058756.
  8. ^ Wilks (1967), p. 244.
  9. ^ "THE LIFE OF SIR JOHN CUNNINGHAM McLENNAN Ph.D, F.R.S.C, F.R.S., O.B.E., K.B.E. (1867 - 1935)". University of Toronto Physics. Archived from the original on 2006-05-05.
  10. ^ Vignos, James H.; Fairbank, Henry A. (1961-03-15). "New Solid Phase in H4". Physical Review Letters. 6 (6): 265–267. Bibcode:1961PhRvL...6..265V. doi:10.1103/PhysRevLett.6.265.
  11. ^ Wilks (1967), pp. 474–478.
  12. ^ Wilks (1967), p. 289.
  13. ^ Dieter Vollhart & Peter Wölfle (1990). The Superfluid Phases of Helium 3. Taylor and Francis. p. 3.
General
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