Difference between revisions of "Barium peroxide"

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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 + O<sub>2</sub> ⇌ 2 BaO<sub>2</sub>
+
: 2 BaO + O<sub>2</sub> ⇌ 2 BaO<sub>2</sub>
  
 
==Projects==
 
==Projects==

Latest revision as of 21:15, 8 June 2020

Barium peroxide
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.

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

Projects

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.

References

Relevant Sciencemadness threads