Disulfuryl chloride

Disulfuryl chloride
Names
Other names
  • Pyrosulfuryl chloride
  • Disulfur pentoxydichloride
  • Sulfur pentoxydichloride
Identifiers
3D model (JSmol)
ChemSpider
UNII
UN number 1817 (PYROSULFURYL CHLORIDE)
  • InChI=1S/Cl2O5S2/c1-8(3,4)7-9(2,5)6
    Key: NNTJKSMVNWGFTB-UHFFFAOYSA-N
  • O=S(=O)(OS(=O)(=O)Cl)Cl
Properties
Cl2O5S2
Molar mass 215.02 g·mol−1
Appearance colorless liquid
Density 1.84 g/cm3
Melting point –37 °C
Boiling point 152.5 °C
reacts with water
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Disulfuryl chloride is an inorganic compound of sulfur, chlorine, and oxygen with the chemical formula S2O5Cl2.[1] This is the anhydride of chlorosulfuric acid.

Synthesis

Careful heating of sulfur trioxide and carbon tetrachloride:[2]

2SO3 + CCl4 → S2O5Cl2 + COCl2

There are also other known methods that do not produce phosgene as a by-product, for example mixing sulfur trioxide and sulfuryl chloride:

SO3 + SO2Cl2 → S2O5Cl2

Physical properties

The compound appears as a dense, very refractive, colorless liquid with a pungent odor, insoluble in cold water, and prone to hydrolysis.[3][4] Its tendency to smoke in air is low when the compound is pure, while the smoke increases with the presence of chlorosulfuric acid impurities, which are more prone to hydrolysis.

Chemical properties

It slowly drools on contact with water:[5]

S2O5Cl2 + 3H2O → 2H2SO4 + 2HCl↑

Prolonged boiling or heating to 250 °C results in dissociation into sulfur trioxide, sulfur dioxide, and chlorine.[2]

Uses

The compound is used in organic synthesis and as a chlorinating agent.[5]

See also

References

  1. ^ Bünzli-Trepp, Ursula (1 January 2007). Systematic Nomenclature of Organic, Organometallic and Coordination Chemistry: Chemical-Abstracts Guidelines with IUPAC Recommendations and Many Trivial Names. EPFL Press. p. 290. ISBN 978-1-4200-4615-1. Retrieved 17 August 2025.
  2. ^ a b Brauer, Georg (1975). Handbuch der Präparativen Anorganischen Chemie (in German) (3., umgearb. Aufl ed.). Stuttgart: Enke. p. 389. ISBN 3-432-02328-6. Retrieved 17 August 2025.
  3. ^ Lewis, Robert A. (31 May 2016). Hawley's Condensed Chemical Dictionary. John Wiley & Sons. p. 1156. ISBN 978-1-118-13515-0. Retrieved 17 August 2025.
  4. ^ Craig, Bruce D.; Anderson, David S. (31 December 1994). Handbook of Corrosion Data. ASM International. p. 328. ISBN 978-0-87170-518-1. Retrieved 17 August 2025.
  5. ^ a b Macintyre, Jane E. (23 July 1992). Dictionary of Inorganic Compounds. CRC Press. p. 2896. ISBN 978-0-412-30120-9. Retrieved 17 August 2025.
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