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Fe + 2 HClO 4 + 6 H 2 O → Fe(ClO 4) 2 ·6H 2 O + H 2. Although the ferrous cation is a reductant and the perchlorate anion is a strong oxidant, in the absence of atmospheric oxygen, dissolved ferrous perchlorate is stable in aqueous solution because the electron transfer between both species Fe 2+ and ClO − 4 is hindered by severe kinetic ...
Cu(ClO 4) 2 + 6 H 2 O → [Cu(H 2 O) 6](ClO 4) 2. Upon heating, perchlorate complexes yield oxides, evolving chlorine oxides in the process. For example, thermolysis of titanium perchlorate gives TiO 2, ClO 2, and O 2 The titanyl species TiO(ClO 4) 2 is an intermediate in this decomposition. [7] Ti(ClO 4) 4 → TiO 2 + 4ClO 2 + 3O 2 ΔH = +6 ...
4 clo − 2 + 2 h 2 so 4 → 2 clo 2 + hclo 3 + 2 so 2− 4 + h 2 o + hcl All three methods can produce chlorine dioxide with high chlorite conversion yield. Unlike the other processes, the chlorite–sulfuric acid method is completely chlorine-free, although it suffers from the requirement of 25% more chlorite to produce an equivalent amount ...
Chlorine perchlorate is a chemical compound with the formula Cl 2 O 4. This chlorine oxide is an asymmetric oxide, with one chlorine atom in +1 oxidation state and the other +7, with proper formula ClOClO 3. It is produced by the photodimerization of chlorine dioxide (ClO 2) at room temperature by 436 nm ultraviolet light: [2] [3] [4] 2ClO 2 ...
This reaction gives the methanol solvate of the dichloride, which upon heating in a vacuum at about 160 °C converts to anhydrous FeCl 2. [4] The net reaction is shown: Fe + 2 HCl → FeCl 2 + H 2. FeBr 2 and FeI 2 can be prepared analogously. An alternative synthesis of anhydrous ferrous chloride is the reduction of FeCl 3 with chlorobenzene: [5]
dichlorine pentoxide, Cl 2 O 5 or ClOOClO 3, is hypothetical; dichlorine hexoxide or chloryl perchlorate, Cl 2 O 6 or [ClO 2] + [ClO 4] −, chlorine (V,VII) oxide; dichlorine heptoxide, Cl 2 O 7, chlorine (VII) oxide; dichlorine octoxide, chlorine (VII) oxide peroxide or dimer of chlorine tetroxide radical, Cl 2 O 8 or (OClO 3) 2; Several ions ...
Fe 0 + 2 H + → Fe 2+ + H 2. Iron(II) is oxidized by hydrogen peroxide to iron(III), forming a hydroxyl radical and a hydroxide ion in the process. This is the Fenton reaction. Iron(III) is then reduced back to iron(II) by another molecule of hydrogen peroxide, forming a hydroperoxyl radical and a proton.
2 instead of Fe (ClO 4) 2) at 0.2 M to prepare amorphous FeCO 3. [8] Care must be taken to exclude oxygen O 2 from the solutions, because the Fe 2+ ion is easily oxidized to Fe 3+, especially at pH above 6.0. [7] Ferrous carbonate also forms directly on steel or iron surfaces exposed to solutions of carbon dioxide, forming an "iron carbonate ...