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Hydrogen chloride is produced by combining chlorine and hydrogen: Cl 2 + H 2 → 2 HCl. As the reaction is exothermic, the installation is called an HCl oven or HCl burner. The resulting hydrogen chloride gas is absorbed in deionized water, resulting in chemically pure hydrochloric acid. This reaction can give a very pure product, e.g. for use ...
This list is sorted by boiling point of gases in ascending order, ... Hydrogen chloride: HCl −85 −114.17 36.5 ... Chlorine trifluoride dioxide: ClO 2 F 3: −21.6 ...
17 Cl chlorine (Cl 2) use: 239.11 K: ... Boiling points of the elements (data page) ... Melting points of the elements (data page)
17 Cl chlorine (Cl 2) use: 171.6 K: ... melting point 302.9146 K ... Boiling points of the elements (data page) List of chemical elements
Chlorine dioxide is also superior to chlorine when operating above pH 7, [17]: 4–33 in the presence of ammonia and amines, [28] and for the control of biofilms in water distribution systems. [25] Chlorine dioxide is used in many industrial water treatment applications as a biocide, including cooling towers, process water, and food processing ...
The large-scale production of hydrochloric acid is almost always integrated with the industrial scale production of other chemicals, such as in the chloralkali process which produces hydroxide, hydrogen, and chlorine, the latter of which can be combined to produce HCl. [31] [32] Hydrogen chloride is produced by combining chlorine and hydrogen ...
The hydrogen halides are colourless gases at standard conditions for temperature and pressure (STP) except for hydrogen fluoride, which boils at 19 °C. Alone of the hydrogen halides, hydrogen fluoride exhibits hydrogen bonding between molecules, and therefore has the highest melting and boiling points of the HX series. From HCl to HI the ...
Unlike hydrogen fluoride, anhydrous liquid hydrogen chloride is difficult to work with as a solvent, because its boiling point is low, it has a small liquid range, its dielectric constant is low and it does not dissociate appreciably into H 2 Cl + and HCl − 2 ions – the latter, in any case, are much less stable than the bifluoride ions (HF −
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