Lithium peroxide

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Lithium peroxide
Other names

Dilithium peroxide, Lithium (I) peroxide

Identifiers
CAS number 12031-80-0 YesY
PubChem 25489
ChemSpider 23787 YesY
Jmol-3D images {{#if:[Li+].[Li+].[O-][O-]|Image 1
Properties
Molecular formula Li2O2
Molar mass 45.881 g/mol
Appearance fine, white powder
Odor odorless
Density 2.31 g/cm3[1][2]
Melting point 195 °C
Boiling point Decomposes to Li2O
Solubility in water soluble
Solubility insoluble in alcohol
Structure
Crystal structure hexagonal
Thermochemistry
Std enthalpy of
formation ΔfHo298		 -13.82 kJ/g
Hazards
EU classification not listed
NFPA 704
0
3
2
OX
 YesY (verify) (what is: YesY/N?)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
Infobox references

Lithium peroxide is the inorganic compound with the formula Li2O2. It is a white, nonhygroscopic solid. Because of its low density, solid has been used to remove CO2 from the atmosphere in spacecraft.[3]

Preparation

It is prepared by the reaction of hydrogen peroxide and lithium hydroxide. This reaction initially produces lithium hydroperoxide:[3]

LiOH.H2O + H2O2 → LiOOH·H2O + H2O

This lithium hydroperoxide has also been described as lithium peroxide monoperoxohydrate trihydrate (Li2O2·H2O2·3H2O). Dehydration of this material gives the anhydrous peroxide salt:

2 LiOOH·H2O → Li2O2 + H2O2 + 2 H2O

Li2O2 decomposes at about 450 °C to give lithium oxide:

2 Li2O2 → 2 Li2O + O2

The structure of solid Li2O2 has been determined by X-ray crystallography and density funcitonal theory. The solid features an eclipsed "ethane-like" Li6O2 subunits with an O-O distance of around 1.5 Å.[4]

Uses

It is used in air purifiers where weight is important, e.g., spacecraft to absorb carbon dioxide and release oxygen in the reaction:[3]

2 Li2O2 + 2 CO2 → 2 Li2CO3 + O2

It absorbs more CO2 than does the same weight of lithium hydroxide and offers the bonus of releasing oxygen.[5] Furthermore, unlike most other alkali metal peroxides, it is not hygroscopic.

The reversible lithium peroxide reaction is the basis for prototye Lithium–air battery. Using oxygen from the atmosphere allows the battery to eliminate storage of oxygen for its reaction, saving battery weight and size.[6]

See also

References

  1. ↑ "Physical Constants of Inorganic Compounds," in CRC Handbook of Chemistry and Physics, 91st Edition (Internet Version 2011), W. M. Haynes, ed., CRC Press/Taylor and Francis, Boca Raton, FL. (pp: 4-72).
  2. ↑ Speight, James G. (2005). Lange's Handbook of Chemistry (16th Edition). (pp: 1.40). McGraw-Hill. Online version available at: http://www.knovel.com/web/portal/browse/display?_EXT_KNOVEL_DISPLAY_bookid=1347&VerticalID=0
  3. ↑ 3.0 3.1 3.2 Greenwood, Norman N.; Earnshaw, Alan (1984). Chemistry of the Elements. Oxford: Pergamon Press. p. 98. ISBN 0-08-022057-6. 
  4. ↑ L. G. Cota and P. de la Mora "On the structure of lithium peroxide, Li2O2" Acta Cryst. 2005, vol. B61, pages 133-136. doi:10.1107/S0108768105003629
  5. ↑ Günter Petzow, Fritz Aldinger, Sigurd Jönsson, Peter Welge, Vera van Kampen, Thomas Mensing, Thomas Brüning"Beryllium and Beryllium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry 2005, Wiley-VCH, Weinheim. doi:10.1002/14356007.a04_011.pub2
  6. ↑ Girishkumar, G.; B. McCloskey, AC Luntz, S. Swanson, W. Wilcke (July 2, 2010). "Lithium- air battery: Promise and challenges". The Journal of Physical Chemistry Letters: 2193–2203. doi:10.1021/jz1005384. Retrieved 12 May 2013. 

External links

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