Difference between revisions of "Barium peroxide"
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| − | '''Barium peroxide''' is the inorganic compound with the formula '''BaO<sub>2</sub>'''. | + | '''Barium peroxide''' is the inorganic compound with the formula '''BaO<sub>2</sub>'''. It is the barium salt of [[hydrogen peroxide]]. |
==Properties== | ==Properties== | ||
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Barium peroxide can be used to produce highly concentrated [[hydrogen peroxide]] via its reaction with conc. [[sulfuric acid]]. | Barium peroxide can be used to produce highly concentrated [[hydrogen peroxide]] via its reaction with conc. [[sulfuric acid]]. | ||
| − | :BaO<sub>2</sub> + H<sub>2</sub>SO<sub>4</sub> → H<sub>2</sub>O<sub>2</sub> + BaSO<sub>4</sub> | + | : BaO<sub>2</sub> + H<sub>2</sub>SO<sub>4</sub> → H<sub>2</sub>O<sub>2</sub> + BaSO<sub>4</sub> |
The insoluble [[barium sulfate]] is filtered from the mixture. | The insoluble [[barium sulfate]] is filtered from the mixture. | ||
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Barium peroxide can be made by the reversible reaction of O<sub>2</sub> with [[barium oxide]]. The peroxide forms around 500 °C and oxygen is released above 820 °C. | Barium peroxide can be made by the reversible reaction of O<sub>2</sub> with [[barium oxide]]. The peroxide forms around 500 °C and oxygen is released above 820 °C. | ||
| − | : 2 BaO | + | : 2 BaO + O<sub>2</sub> ⇌ 2 BaO<sub>2</sub> |
| + | |||
| + | A different, aqueous preparation is performed through a metathesis reaction with barium nitrate and hydrogen peroxide: | ||
| + | |||
| + | : Ba(NO<sub>3</sub>)<sub>2</sub> + H<sub>2</sub>O<sub>2</sub> ⇌ BaO<sub>2</sub> + 2HNO<sub>3</sub> | ||
| + | |||
| + | Cool the mixed solution to near freezing, and the crystallohydrate BaO<sub>2</sub>*8H<sub>2</sub>O will precipitate. Calcine the crystallohydrate carefully at the temperature of 100-120 degrees Celsius to convert it to the anhydrous salt. | ||
==Projects== | ==Projects== | ||
Latest revision as of 17:04, 13 February 2022
| Names | |
|---|---|
| IUPAC name
Barium peroxide
| |
| Other names
Barium binoxide
Barium dioxide | |
| Properties | |
| BaO2 | |
| Molar mass | 169.33 g/mol (anhydrous) 313.45 (octahydrate) |
| Appearance | Grey-white crystalline (anhydrous) Colorless solid (octahydrate) |
| Odor | Odorless |
| Density | 5.68 g/cm3 (anhydrous) 2.292 g/cm3 (octahydrate) |
| Melting point | 450 °C (842 °F; 723 K) |
| Boiling point | 800 °C (1,470 °F; 1,070 K) (decomposes) |
| anhydrous 0.091 g/100 ml (20 °C) octahydrate 0.168 g/100 ml | |
| Solubility | Reacts with acids Insoluble in hydrocarbons |
| Vapor pressure | ~0 mmHg |
| Hazards | |
| Safety data sheet | Sigma-Aldrich |
| Flash point | Non-flammable |
| Related compounds | |
| Related compounds
|
Barium oxide |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Barium peroxide is the inorganic compound with the formula BaO2. It is the barium salt of hydrogen peroxide.
Contents
Properties
Chemical
Barium peroxide can be used to produce highly concentrated hydrogen peroxide via its reaction with conc. sulfuric acid.
- BaO2 + H2SO4 → H2O2 + BaSO4
The insoluble barium sulfate is filtered from the mixture.
Physical
Barium peroxide is a white solid, insoluble in water.
Availability
Barium peroxide is sold by lab suppliers. So far there aren't any sellers on eBay and Amazon.
Preparation
Barium peroxide can be made by the reversible reaction of O2 with barium oxide. The peroxide forms around 500 °C and oxygen is released above 820 °C.
- 2 BaO + O2 ⇌ 2 BaO2
A different, aqueous preparation is performed through a metathesis reaction with barium nitrate and hydrogen peroxide:
- Ba(NO3)2 + H2O2 ⇌ BaO2 + 2HNO3
Cool the mixed solution to near freezing, and the crystallohydrate BaO2*8H2O will precipitate. Calcine the crystallohydrate carefully at the temperature of 100-120 degrees Celsius to convert it to the anhydrous salt.
Projects
- Flash powders and fireworks
- Make concentrated hydrogen peroxide
Handling
Safety
Barium peroxide is corrosive and an oxidizer. Proper protection must be worn when handling this compound.
Storage
Barium peroxide should be kept in closed plastic or glass bottles.
Disposal
Can be neutralized by adding diluted sulfuric acid then iron oxide, to decompose the hydrogen peroxide.
