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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.
In organic chemistry, ethoxylation is a chemical reaction in which ethylene oxide (C 2 H 4 O) adds to a substrate. It is the most widely practiced alkoxylation, which involves the addition of epoxides to substrates. In the usual application, alcohols and phenols are converted into R(OC 2 H 4) n OH, where n ranges from 1 to 10. Such compounds ...
BaAl 4 is an intermediate reacted with barium oxide to produce the metal. Note that not all barium is reduced. [9]: 3 8 BaO + BaAl 4 → Ba↓ + 7 BaAl 2 O 4. The remaining barium oxide reacts with the formed aluminium oxide: [9]: 3 BaO + Al 2 O 3 → BaAl 2 O 4. and the overall reaction is [9]: 3 4 BaO + 2 Al → 3 Ba↓ + BaAl 2 O 4
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 ]
Barium and calcium salts of nonylphenol are also used as heat stabilizers for polyvinyl chloride (PVC). [18] Nonylphenol is also often used an intermediate in the manufacture of the non-ionic surfactants nonylphenol ethoxylates, which are used in detergents , paints, pesticides , personal care products, and plastics.
Narrow-range ethoxylates (NREs) in chemistry are fatty alcohol polyglycol ethers with a narrow homolog distribution and are known nonionic surfactants.They can be produced industrially, for example, by the addition of ethylene oxide onto fatty alcohols in the presence of suitable catalysts (layer compounds which have been calcined or hydrophobized with fatty acids).
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]
Barium oxide – BaO [100] Barium permanganate – Ba(MnO 4) 2 [101] Barium peroxide – BaO 2 [102] Barium sulfate – BaSO 4 [103] Barium sulfide – BaS [104]