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UF 6 reacts with water, releasing hydrofluoric acid. The compound reacts with aluminium, forming a surface layer of AlF 3 that resists any further reaction from the compound. Uranium hexafluoride is a mild oxidant. [10] It is a Lewis acid as evidenced by its binding to form heptafluorouranate(VI), [UF 7] −. [11]
UF 4 is formed by the reaction of UF 6 with hydrogen gas in a vertical tube-type reactor. The bulk density of UF 4 varies from about 2.0 g/cm 3 to about 4.5 g/cm 3 depending on the production process and the properties of the starting uranium compounds.
It is an oxidant [10] and a Lewis acid which is able to bind to fluoride, for instance the reaction of copper(II) fluoride with uranium hexafluoride in acetonitrile is reported to form copper(II) heptafluorouranate(VI), Cu(UF 7) 2. [11] It reacts with water to form a solid compound, and is very difficult to handle on an industrial scale. [6]
Tungsten(VI) fluoride, also known as tungsten hexafluoride, is an inorganic compound with the formula W F 6.It is a toxic, corrosive, colorless gas, with a density of about 13 kg/m 3 (22 lb/cu yd) (roughly 11 times heavier than air).
The following chart shows the solubility of various ionic compounds in water at 1 atm pressure and room temperature (approx. 25 °C, 298.15 K). "Soluble" means the ionic compound doesn't precipitate, while "slightly soluble" and "insoluble" mean that a solid will precipitate; "slightly soluble" compounds like calcium sulfate may require heat to precipitate.
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This salt is very soluble in water as well as hygroscopic. It is formed in the hydrolysis of uranium hexafluoride (UF 6): UF 6 + 2 H 2 O → UO 2 F 2 + 4 HF. It can also be formed in the hydrofluorination of uranium trioxide (UO 3): UO 3 + 2 HF → UO 2 F 2 + H 2 O [3]
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