Difference between revisions of "Barium oxide"
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==Properties== | ==Properties== | ||
===Chemical=== | ===Chemical=== | ||
| − | Barium oxide reacts with water to give [[barium hydroxide]]. | + | Barium oxide reacts exothermically with water to give [[barium hydroxide]]. |
| + | |||
| + | : BaO + H<sub>2</sub>O → Ba(OH)<sub>2</sub> | ||
Reaction with acids yields barium salts. | Reaction with acids yields barium salts. | ||
| + | |||
| + | : BaO + 2 HX → BaX<sub>2</sub> + H<sub>2</sub>O | ||
| + | |||
| + | Barium oxide reacts with oxygen to form [[barium peroxide]], above 500 °C, but breaks down to barium oxide and oxygen above 820 °C. | ||
| + | |||
| + | : 2 BaO + O<sub>2</sub> ⇌ 2 BaO<sub>2</sub> | ||
===Physical=== | ===Physical=== | ||
| Line 125: | Line 133: | ||
Barium oxide can be prepared by burning [[barium]] metal in an [[oxygen]] atmosphere. | Barium oxide can be prepared by burning [[barium]] metal in an [[oxygen]] atmosphere. | ||
| − | Reducing [[barium carbonate]] with carbon will also give barium oxide. | + | : 2 Ba + O<sub>2</sub> → 2 BaO |
| + | |||
| + | Thermal decomposition of barium carbonate will yield barium oxide. | ||
| + | |||
| + | : BaCO<sub>3</sub> → BaO + CO<sub>2</sub> | ||
| + | |||
| + | Reducing [[barium carbonate]] with [[carbon]] will also give barium oxide. | ||
| + | |||
| + | : BaCO<sub>3</sub> + C → BaO + 2 CO | ||
==Projects== | ==Projects== | ||
Latest revision as of 20:32, 13 March 2024
| Names | |
|---|---|
| IUPAC name
Barium oxide
| |
| Other names
Baria
Barium protoxide Barium monoxide Calcined baryta | |
| Properties | |
| BaO | |
| Molar mass | 153.326 g/mol |
| Appearance | White solid |
| Odor | Odorless |
| Density | 5.72 g/cm3 |
| Melting point | 1,923 °C (3,493 °F; 2,196 K) |
| Boiling point | 2,000 °C (3,630 °F; 2,270 K) |
| Reacts | |
| Solubility | Reacts with alcohols, acids, bromine, phenol Insoluble in liq. ammonia, organic solvents |
| Vapor pressure | ~0 mmHg |
| Thermochemistry | |
| Std molar
entropy (S |
70 J·mol−1·K−1 |
| Std enthalpy of
formation (ΔfH |
−582 kJ/mol |
| Hazards | |
| Safety data sheet | Sigma-Aldrich |
| Flash point | Non-flammable |
| Lethal dose or concentration (LD, LC): | |
| LD50 (Median dose)
|
146 mg/kg (rat, oral) |
| Related compounds | |
| Related compounds
|
Strontium oxide Calcium oxide Magnesium oxide |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Barium oxide is a white hygroscopic compound with the chemical formula BaO.
Contents
Properties
Chemical
Barium oxide reacts exothermically with water to give barium hydroxide.
- BaO + H2O → Ba(OH)2
Reaction with acids yields barium salts.
- BaO + 2 HX → BaX2 + H2O
Barium oxide reacts with oxygen to form barium peroxide, above 500 °C, but breaks down to barium oxide and oxygen above 820 °C.
- 2 BaO + O2 ⇌ 2 BaO2
Physical
Barium oxide is a white solid, insoluble in solvents.
Availability
Barium oxide is sold by chemical suppliers. Can also be bought online.
Preparation
Barium oxide can be prepared by burning barium metal in an oxygen atmosphere.
- 2 Ba + O2 → 2 BaO
Thermal decomposition of barium carbonate will yield barium oxide.
- BaCO3 → BaO + CO2
Reducing barium carbonate with carbon will also give barium oxide.
- BaCO3 + C → BaO + 2 CO
Projects
- Make barium salts
- Make barium peroxide
- Ethoxylation catalyst
- Make crown glass
Handling
Safety
Barium oxide is caustic and very toxic.
Storage
In closed plastic bottles, away from moisture and acids.
Disposal
Should be converted to barium sulfate, which can be dumped in trash.
References
Relevant Sciencemadness threads
