|Other names||ethylene oxide, dimethylene oxide, oxirane, oxacyclopropane|
3D model (JSmol)
|ECHA InfoCard||Lua error in Module:Wikidata at line 879: attempt to index field 'wikibase' (a nil value). Lua error in Module:Wikidata at line 879: attempt to index field 'wikibase' (a nil value).|
|Molar mass||44.05 g mol−1|
|Std enthalpy of
|−52.6 kJ mol−1|
|243 J mol−1 K−1|
|Explosive limits||3 to 100%|
|Except where noted otherwise, data are given for|
materials in their standard state
(at 25 °C, 100 kPa)
Infobox disclaimer and references
The chemical compound ethylene oxide is an important industrial chemical used as an intermediate in the production of ethylene glycol and other chemicals, and as a sterilant for foods and medical supplies. It is a colorless flammable gas or refrigerated liquid with a faintly sweet odor. It is the simplest example of an epoxide.
Its IUPAC name is epoxyethane. Other names for it include oxirane and dimethylene oxide.
Ethylene oxide was first prepared in 1859 by the French chemist Charles-Adolphe Wurtz, who prepared it by treating 2-chloroethanol with a base. It achieved industrial importance during World War I as a precursor to both the coolant ethylene glycol and the chemical weapon mustard gas. In 1931, Theodore Lefort, another French chemist, discovered a means to prepare ethylene oxide directly from ethylene and oxygen, using silver as a catalyst. Since 1940, almost all ethylene oxide produced industrially has been made using this method.
Industrially, ethylene oxide is produced when ethylene (CH2=CH2) and oxygen (O2) react on a silver catalyst at 200–300 °C showing large Ag nanoparticles supported on Alumina. Typically, chemical modifiers such as chlorine are also included. Pressures used are in the region of 1-2MPa. The chemical equation for this reaction is:
- CH2=CH2 + ½ O2 → C2H4O
The typical yield for this reaction under industrial conditions is 70-80%. In the reaction scheme above, an intermediate (oxametallacycle) is formed. Two different reaction pathways can then occur.
Ethylene oxide formation:
- CH2=CH2 + O → C2H4O
- CH2=CH2 + O → CH3CHO
- CH3CHO +5/2 O2 → 2CO2 + 2H2O
Several methods to produce ethylene oxide more selectively have been proposed, but none have achieved industrial importance.
Ethylene oxide gas kills bacteria (and their endospores), mold, and fungi, and can therefore be used to sterilize substances that would be damaged by sterilizing techniques such as pasteurization that rely on heat. Ethylene oxide sterilization for the preservation of spices was patented in 1938 by the American chemist Lloyd Hall, and it is still used in that role. Additionally, ethylene oxide is widely used to sterilize medical supplies such as bandages, sutures, and surgical implements. The overwhelming majority of medical items are sterilized with ethylene oxide. Preferred methods have been the traditional chamber sterilization method, where a chamber is flooded with a mix of ethylene oxide and other gases which are later aerated, and the more recent gas diffusion method which relies on a bag that wraps the elements to be sterilized and acts a a mini-chamber in order to minimize gas consumption and make the process economically feasible for small loads.
Most ethylene oxide, however, is used as an intermediate in the production of other chemicals. The major use of ethylene oxide is in the production of ethylene glycol. The primary end use for ethylene glycol is in the production of polyester polymers. Ethylene glycol is more commonly known for its use as an automotive coolant and antifreeze.
Because of its high flammability and wide explosive concentration range in air, ethylene oxide is sometimes used as the fuel component of a fuel-air explosive.
Most reactions are ring openings by nucleophiles.
C2H4O + H2O → HOCH2CH2OH
Despite the large excess of water, various types of polyethylene glycol (PEG) or polyethylene oxide (PEO) are still formed as secondary products. The degree of polymerization increases as a smaller proportion of water is used:
n(CH2CH2O) + H2O → HO(CH2CH2O)nH
One class of ethylene oxide derivatives that has attracted much scientific attention is the crown ethers, which are cyclic oligomers of ethylene oxide. These compounds have the ability to make ionic compounds such as salts soluble in nonpolar solvents which they otherwise could not dissolve in. However, the high cost of these compounds has largely confined their use to the laboratory rather than industrial practice.
Ethylene oxide is toxic by inhalation. Symptoms of overexposure include headache and dizziness, progressing with increasing exposure to convulsions, seizure and coma. It is also an irritant to skin and the respiratory tract, and inhaling the vapors may cause the lungs to fill with fluid several hours after exposure.
Ethylene oxide is usually stored as a pressurized or refrigerated liquid. At room temperature and pressure, it rapidly evaporates, potentially causing frostbite in cases of skin exposure.
Laboratory animals exposed to ethylene oxide for their entire lives have had a higher incidence of liver cancer. However, studies on human beings who have worked with ethylene oxide for extended periods and may have experienced low doses during that time have found no increase in cancer risk. Chronic ethylene oxide exposure may increase the risk of cataracts in humans.
In animals, ethylene oxide can cause numerous reproductive effects, including mutations and a higher rate of miscarriages. Its reproductive effects on humans have not been well studied, but it is considered probable that ethylene oxide exposure has similar effects on human reproduction.
Ethylene oxide is classified as carcinogenic to humans by the International Agency for Research on Cancer (IARC).
- National Pollutant Inventory - Ethylene oxide fact sheet
- Ethylene Oxide User's Guide
- Ethylene Oxide MSDS (Material Safety Data Sheet).
- Wurtz, A. (1859). Compt. rend. 48: 101–104. Missing or empty
- P. P. McClellan (1950). "Manufacture and Uses of Ethylene Oxide and Ethylene Glycol". Ind. Eng. Chem. 42: 2402–2407. doi:10.1021/ie50492a013.