Lithium peroxide
From Wikipedia, the free encyclopedia
| Lithium peroxide | |
|---|---|
| Image:Lithium peroxide.jpg | |
| Other names | Dilithium peroxide, Lithium (I) peroxide |
| Identifiers | |
| CAS number | [12031-80-0] |
| Properties | |
| Molecular formula | Li2O2 |
| Molar mass | 45.881 g/mol |
| Appearance | fine odorless, white powder |
| Density | 2.14 g/cm3, solid (25°C) |
| Melting point |
195°C |
| Boiling point |
Decomposes to Li2O |
| Solubility in water | soluble |
| Hazards | |
| EU classification | not listed |
| NFPA 704 |
 0
3
2
|
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references |
|
Lithium peroxide (Li2O2) is a chemical compound. It decomposes above 195°C to give lithium oxide, Li2O:
- 2Li2O2 → Li2O + O2
Contents |
[edit] Preparation
It is prepared industrially by the reaction of hydrogen peroxide and lithium hydroxide to produce the hydroperoxide which is then dehydrated[1]:
- LiOH.H2O + H2O2 → LiOOH.H2O + H2O
- 2LiOOH.H2O → Li2O2 + H2O2 + 2H2O
[edit] Uses
It is used in air purifiers where weight is important e.g. spacecraft to absorb carbon dioxide and release oxygen in the reaction[1]:
- 2Li2O2 + 2CO2 → 2Li2CO3 + O2
[edit] Precautions
Lithium peroxide reacts with and should be isolated from water, steam, reducing agents, organic material, metallic oxides and salts.
[edit] See also
[edit] References
 |
This article needs additional citations for verification. Please help improve this article by adding reliable references. Unsourced material may be challenged and removed. (May 2008) |
- ^ a b Greenwood, N. N.; Earnshaw, A. (1997). Chemistry of the Elements, 2nd Edition, Oxford:Butterworth-Heinemann. ISBN 0-7506-3365-4.
[edit] External links
 |
This inorganic compound-related article is a stub. You can help Wikipedia by expanding it. |
