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Ethylene oxide



Name Ethylene oxide
Chemical formula C2H4O
Appearance Colorless gas


Formula weight 44.1 amu
Melting point 161 K (-112 °C)
Boiling point 284 K (11 °C)
Density 0.82 ×103 kg/m3 (liquid)
Solubility miscible with water


ΔfH0gas ? kJ/mol
ΔfH0liquid ? kJ/mol
ΔfH0solid ? kJ/mol
S0gas, 1 bar ? J/mol·K
S0liquid, 1 bar ? J/mol·K
S0solid ? J/mol·K


Ingestion May cause nausea, vomiting.
Inhalation Usually irritates mucous membranes. Delayed pulmonary edema or pneumonia possible.
Skin May cause skin irritation, frostbite. Can be absorbed through skin, with harmful or fatal results.
Eyes May cause severe irritation or injury, frostbite.
More info Hazardous Chemical Database
SI units were used where possible. Unless otherwise stated, standard conditions were used.

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 sterliant for foodstuffs and medical supplies. It is a colorless flammable gas or refrigerated liquid with a faintly sweet odor.

Its IUPAC name is 1,2-epoxyethane. Other names for it include oxirane and dimethylene oxide.

Table of contents
1 History
2 Production
3 Uses
4 Health effects


Ethylene oxide was first prepared in 1859 by the French chemist Charles 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 and oxygen react on a silver catalyst at 200-300°C. The chemical equation for this reaction is

CH2=CH2 + ½ O2 → C2H4O

The typical yield for this reaction is 70-80%, the major side reaction being combustion of ethylene to produce carbon dioxide. Several methods to produce ethylene oxide more selectively have been proposed, but none have achieved industrial importance.


Ethylene oxide gas kills bacteria, 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.

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, which is widely used as an automotive coolant and antifreeze, and is also used to produce polyester polymers.

Ethylene oxide itself can be polymerized to form polyethylene glycol or polyethylene oxide, which are useful as non-toxic, water-soluble polymers. Ethylene oxide is also important in the manufacture of surfactants and otherdetergents.

One class of ethylene oxide derivatives that has attracted much scientific attention are 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.

Health effects

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.