This page uses content from Wikipedia and is licensed under CC BY-SA.
|Preferred IUPAC name
3D model (JSmol)
|Molar mass||197.82 g/mol|
|Appearance||liquid at room temperature|
|Melting point||−57 °C (−71 °F; 216 K)|
|Boiling point||128 °C (262 °F; 401 K)|
|GHS signal word||Danger|
|H300, H314, H330|
|P260, P264, P270, P271, P280, P284, P301+310, P301+330+331, P303+361+353, P304+340, P305+351+338, P310, P320, P321, P330, P363, P403+233, P405, P501|
|Flash point||32 °C (90 °F; 305 K)|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is ?)(|
Diphosgene is a chemical compound with the formula ClCO2CCl3. This colorless liquid is a valuable reagent in the synthesis of organic compounds. Diphosgene is related to phosgene and has comparable toxicity, but is more conveniently handled because it is a liquid, whereas phosgene is a gas.
Another method is the radical chlorination of methyl formate:
Diphosgene converts to phosgene upon heating or upon catalysis with charcoal. It is thus useful for reactions traditionally relying on phosgene. For example, it convert amines into isocyanates, secondary amines into carbamoyl chlorides, carboxylic acids into acid chlorides, and formamides into isocyanides. Diphosgene serves as a source of two equivalents of phosgene:
It hydrolyzes to release HCl in humid air.
Diphosgene is used in some laboratory preparations because it is easier to handle than phosgene.
Diphosgene was originally developed as a pulmonary agent for chemical warfare, a few months after the first use of phosgene. It was used as a poison gas in artillery shells by Germany during World War I. The first recorded battlefield use was in May 1916. Diphosgene was developed because the vapors could destroy the filters in gas masks in use at the time.
Diphosgene has a relatively high vapor pressure of 10 mm Hg (1.3 kPa) at 20 °C and decomposes to phosgene around 300 °C. Exposure to diphosgene is similar in hazard to phosgene and the MSDS should be consulted.