Carbonyl bromide

Carbonyl bromide[1]
Names
Other names
Bromophosgene, carbonic dibromide, carbonyl dibromide
Identifiers
593-95-3 YesY=
ChemSpider 71389 YesY
Jmol interactive 3D Image
PubChem 79057
Properties
COBr2
Molar mass 187.818 g/mol
Appearance colorless liquid
Density 2.52 g/ml at 15°C
Boiling point 64.5 °C (148.1 °F; 337.6 K) decomposes
reacts
Thermochemistry
61.8 J·mol−1·K−1 (gas)
309.1 J·mol−1·K−1 (gas)
-127.2 or -145.2 kJ·mol−1 (liquid)
-96.2 or -114 kJ·mol−1 (gas)
Hazards
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 4: Very short exposure could cause death or major residual injury. E.g., VX gas Reactivity code 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g., calcium Special hazards (white): no codeNFPA 704 four-colored diamond
0
4
1
Related compounds
Related compounds
 Carbonyl fluoride
Phosgene
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
YesY verify (what is YesYN ?)
Infobox references

Carbonyl bromide, also known as bromophosgene by analogy to phosgene, is an organic chemical compound. It is a decomposition product of halon compounds used in fire extinguishers.[2]

Reactions

Carbonyl bromide is formed when carbon tetrabromide is melted and concentrated sulfuric acid is added.

In contrast to phosgene, carbonyl bromide cannot be produced efficiently from carbon monoxide and bromine. A complete conversion is not possible due to thermodynamic reasons. Additionally, the reaction

CO + Br2 <-> COBr2

processes slowly at room temperature. Increasing temperature, in order to increase the reaction rate, results in a further shift of the chemical equilibrium towards the educts (since ΔRH < 0 and ΔRS < 0).[3]

On the other hand, carbonyl bromide slowly decomposes to carbon monoxide and elemental bromine even at low temperatures.[4] It is also sensitive to hydrolysis.

References

  1. ↑ Lide, David R. (1998), Handbook of Chemistry and Physics (87 ed.), Boca Raton, FL: CRC Press, pp. 3–96, 4–50, 5–26, ISBN 0-8493-0594-2
  2. ↑ US Occupational Safety and Health Administration (May 1996). "Common Fire Extinguishing Agents". Retrieved 2009-11-21.
  3. ↑ https://books.google.de/books?id=fM43Ny2eFS8C&pg=PA900&lpg=PA900&dq=carbonyl+bromide+enthalpy+of+formation&source=bl&ots=-ny9U7I-bx&sig=4XDedlqIFEK2OtXizrJaUfkBdzI&hl=de&sa=X&ei=UEgoVYCmI86uabvrgLAK&ved=0CDwQ6AEwAw#v=onepage&q=carbonyl%20bromide%20enthalpy%20of%20formation&f=false, pp. 669-671, retrieved 2015-04-11
  4. ↑ Katrizsky, Alan R.; Meth-Cohn, Otto; Wees, Charles W. (1995), Organic Functional Group Transformations 6, Elsevier, pp. 417–8, ISBN 978-0-08-042704-1, retrieved 2009-11-23
This article is issued from Wikipedia - version of the Wednesday, July 15, 2015. The text is available under the Creative Commons Attribution/Share Alike but additional terms may apply for the media files.