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Barium peroxide arises by the reversible reaction of O 2 with barium oxide. The peroxide forms around 500 °C and oxygen is released above 820 °C. [1] 2 BaO + O 2 ⇌ 2 BaO 2. This reaction is the basis for the now-obsolete Brin process for separating oxygen from the atmosphere. Other oxides, e.g. Na 2 O and SrO, behave similarly. [4]
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Barium peroxide was once used to produce pure oxygen from air. This process relies on the temperature-dependent chemical equilibrium between barium oxide and peroxide: the reaction of barium oxide with air at 500 °C results in barium peroxide, which upon heating to above 700 °C decomposes back to barium oxide with release pure oxygen. [3]
In this process barium oxide reacts at 500–600 °C (932–1,112 °F) with air to form barium peroxide, which decomposes above 700 °C (1,292 °F) by releasing oxygen: [21] [22] 2 BaO + O 2 ⇌ 2 BaO 2. Barium sulfate was first applied as a radiocontrast agent in X-ray imaging of the digestive system in 1908. [23]
The peroxide group is marked in blue. R, R 1 and R 2 mark hydrocarbon moieties. The most common peroxide is hydrogen peroxide (H 2 O 2), colloquially known simply as "peroxide". It is marketed as solutions in water at various concentrations. Many organic peroxides are known as well. In addition to hydrogen peroxide, some other major classes of ...
Chemical formula Synonyms CAS number Ac 2 O 3: actinium(III) oxide: 12002-61-8 AgBF 4: Silver tetrafluoroborate: 14104-20-2 AgBr: silver bromide: 7785-23-1 AgBrO: silver hypobromite
Chemical formula. RaO Molar mass: 242 g/mol Appearance solid ... This reaction also produces radium nitride and possibly radium peroxide: 3Ra + N 2 → Ra 3 N 2
Barium oxide, also known as baria, is a white hygroscopic non-flammable compound with the formula BaO. It has a cubic structure and is used in cathode-ray tubes , crown glass, and catalysts. It is harmful to human skin and if swallowed in large quantity causes irritation.