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| Barium peroxide | |
|---|---|
| IUPAC name | barium peroxide |
| Other names | Barium binoxide, Barium dioxide, Barium superoxide, UN 1449 |
| Identifiers | |
| CAS number | [1304-29-6] |
| PubChem | |
| EINECS number | |
| RTECS number | CR0175000 |
| Properties | |
| Molecular formula | BaO2 |
| Molar mass | 169.33 g/mol |
| Appearance | Grey-white crystalline solid |
| Density | 4.95 g/cm³, solid |
| Melting point |
450 °C (723 K) |
| Boiling point |
800 °C (1073 K) (decomp. to BaO + O2) |
| Solubility in water | Slightly soluble |
| Hazards | |
| Main hazards | Harmful (Xn) |
| NFPA 704 |
 0
1
0
OX
|
| R-phrases | R8 R20/22 |
| S-phrases | (S2) S13 S27 |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox references |
|
Barium peroxide is the chemical compound with the formula BaO2. This grey-white solid is one of the most common inorganic peroxides. Barium peroxide is an oxidizing agent, which is used for bleaching. It is used in fireworks as an oxidizer,[1] which also gives a vivid green colour, as do all barium compounds.
Barium peroxide is a peroxide, containing O22− subunits wherein the oxygen atoms bond to each other as well as to the barium. The solid adopts the same structure as calcium carbide, CaC2.
Barium peroxide arises by the reversible absorption of O2 by barium oxide. The oxygen is released above 700°C.
- BaO + 1/2 O2 ⇌ BaO2
This reaction is the basis for the now-obsolete Brin Process for separating oxygen from the atmosphere. Other oxides, e.g. Na2O, behave similarly.[2]
Hydrogen peroxide can also be prepared via the related reaction:
- BaO2 + H2SO4 → H2O2 + BaSO4
Footnotes
- ^ "Data Sheet". Data Sheet. Hummel Croton Inc. Retrieved on 2007-02-01.
- ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
See also
External links
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Wikipedia content modification information:
- This page was last modified on 13 August 2008, at 18:45.
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