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H 2 S 2 O 5 +5 (of the sulfur atom bonded to 3 oxygen atoms), +3 (of other sulfur atom) Disulfite commonly known as metabisulfite, S 2 O 2− 5: Not known. Sulfurous acid: H 2 SO 3 +4 Bisulfite, HSO − 3 and sulfite, SO 2− 3: Not known. Dithionous acid: H 2 S 2 O 4 +3 Dithionite, O 2 SSO 2− 2: Not known. Sulfoxylic acid: H 2 SO 2 +2 ...
The compound is prepared by treating V 2 O 5 in sulfuric acid with elemental sulfur: [2] V 2 O 5 + S + 3 H 2 SO 4 → V 2 (SO 4) 3 + SO 2 + 3 H 2 O. This transformation is a rare example of a reduction by elemental sulfur. When heated in vacuum at or slightly below 410 °C, it decomposes into vanadyl sulfate (VOSO 4) and SO 2. Vanadium(III ...
Lithium oxide forms along with small amounts of lithium peroxide when lithium metal is burned in the air and combines with oxygen at temperatures above 100 °C: [3] 4Li + O 2 → 2 Li 2 O. Pure Li 2 O can be produced by the thermal decomposition of lithium peroxide, Li 2 O 2, at 450 °C [3] [2] 2 Li 2 O 2 → 2 Li 2 O + O 2
The group SO(3) can therefore be identified with the group of these matrices under matrix multiplication. These matrices are known as "special orthogonal matrices", explaining the notation SO(3). The group SO(3) is used to describe the possible rotational symmetries of an object, as well as the possible orientations of an object in space.
Basic gallium sulfate is known with the formula (H 3 O)Ga 3 (SO 4) 2 (OH) 6. [6] Double gallium sulfates are known with composition NaGa 3 (SO 4) 2 (OH) 6, KGa 3 (SO 4) 2 (OH) 6, RbGa 3 (SO 4) 2 (OH) 6, NH 4 Ga 3 (SO 4) 2 (OH) 6. These compounds are isostructural with jarosite and alunite. Jarosite and alunite can contain a small amount of ...
There are several general reasons for this: (1) they may condense to form oligomers (e.g., H 2 CrO 4 to H 2 Cr 2 O 7), or dehydrate all the way to form the anhydride (e.g., H 2 CO 3 to CO 2), (2) they may disproportionate to one compound of higher and another of lower oxidation state (e.g., HClO 2 to HClO and HClO 3), or (3) they might exist ...
Lithium sulfite, or lithium sulphite, is an ionic compound with the formula Li 2 SO 3. [1] References
Sodium oxalate starts to decompose above 290 °C into sodium carbonate and carbon monoxide: [2]. Na 2 C 2 O 4 → Na 2 CO 3 + CO. When heated at between 200 and 525°C with vanadium pentoxide in a 1:2 molar ratio, the above reaction is suppressed, yielding instead a sodium vanadium oxibronze with release of carbon dioxide [6]