Barium oxide
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Other names
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Identifiers | |
3D model (
JSmol ) |
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ChemSpider | |
ECHA InfoCard
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100.013.753 |
EC Number |
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PubChem CID
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RTECS number
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UNII | |
UN number | 1884 |
CompTox Dashboard (EPA)
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Properties | |
BaO | |
Molar mass | 153.326 g/mol |
Appearance | white solid |
Density | 5.72 g/cm3, solid |
Melting point | 1,923 °C (3,493 °F; 2,196 K) |
Boiling point | ~ 2,000 °C (3,630 °F; 2,270 K) |
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Solubility | soluble in ethanol, dilute mineral acids and alkalies; insoluble in acetone and liquid ammonia |
-29.1·10−6 cm3/mol | |
Structure | |
cubic, cF8 | |
Fm3m, No. 225 | |
Octahedral | |
Thermochemistry | |
Heat capacity (C)
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47.7 J/K mol |
Std molar
entropy (S⦵298) |
70 J·mol−1·K−1[1] |
Std enthalpy of (ΔfH⦵298)formation |
−582 kJ·mol−1[1] |
Hazards | |
GHS labelling: | |
Danger | |
H301, H302, H314, H315, H332, H412 | |
P210, P220, P221, P260, P261, P264, P270, P271, P273, P280, P283, P301+P310, P301+P312, P301+P330+P331, P302+P352, P303+P361+P353, P304+P312, P304+P340, P305+P351+P338, P306+P360, P310, P312, P321, P330, P332+P313, P362, P363, P370+P378, P371+P380+P375, P405, P501 | |
NFPA 704 (fire diamond) | |
Flash point | Non-flammable |
Related compounds | |
Other anions
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Other cations
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Supplementary data page | |
Barium oxide (data page) | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Barium oxide, also known as baria, is a white
It is prepared by heating barium carbonate with coke, carbon black or tar or by thermal decomposition of barium nitrate.[citation needed]
Uses
Barium oxide is used as a coating for
It is also a source of pure oxygen through heat fluctuation. It readily oxidises to BaO2 by formation of a peroxide ion. The complete peroxidation of BaO to BaO2 occurs at moderate temperatures but the increased entropy of the O2 molecule at high temperatures means that BaO2 decomposes to O2 and BaO at 1175K.[4] The reaction was used as a large scale method to produce oxygen before air separation became the dominant method in the beginning of the 20th century. The method was named the Brin process, after its inventors.[5]
Preparation
Barium oxide is made by heating
- 2 Ba + O2 → 2 BaO
- BaCO3 → BaO + CO2
Safety issues
Barium oxide is an irritant. If it contacts the skin or the eyes or is inhaled it causes pain and redness. However, it is more dangerous when ingested. It can cause nausea and diarrhea, muscle paralysis, cardiac arrhythmia, and can cause death. If ingested, medical attention should be sought immediately.
Barium oxide should not be released environmentally; it is harmful to aquatic organisms.[8]
See also
- Barium – chemical element with symbol Ba and atomic number 56
References
- ^ ISBN 978-0-618-94690-7.
- ^ "Barium Oxide (chemical compound)". Encyclopædia Britannica. Encyclopædia Britannica. 2007. Retrieved 2007-02-19.
- ^ Nield, Gerald; Washecheck, Paul; Yang, Kang (1980-07-01). "United States Patent 4210764". Retrieved 2007-02-20.
- ^ S.C. Middleburgh; K.P.D. Lagerlof; R.W. Grimes (2012-09-29). "Accommodation of Excess Oxygen in Group II Oxides". Journal of the American Ceramic Society. Retrieved 2022-03-27.
- .
- ISBN 0-07-049439-8
- ^ "Compounds of barium: barium (II) oxide". Web Elements. The University of Sheffield. 2007-01-26. Retrieved 2007-02-22.
- ^ "Barium Oxide (ICSC)". IPCS. October 1999. Archived from the original on 26 February 2007. Retrieved 2007-02-19.