epoxyethane, ethylene oxide, dimethylene oxide, oxacyclopropane, 1,2-Epoxy ethane
3D model (JSmol)
|Molar mass||44.052 g·mol−1|
|Melting point||−112.46 °C (−170.43 °F; 160.69 K)|
|Boiling point||10.4 °C (50.7 °F; 283.5 K)|
|Vapor pressure||1.46 atm (20 °C)|
Refractive index (nD)
|1.3597 (589 nm)|
Std enthalpy of
Gibbs free energy (ΔfG˚)
|Safety data sheet||ICSC 0155|
| F+ T
Carc. Cat. 1
|R-phrases (outdated)||R45, R46, R12, R23, R36/37/38|
|S-phrases (outdated)||S53, S45|
|Flash point||−20 °C (−4 °F; 253 K)|
|429 °C (804 °F; 702 K)|
|Explosive limits||3 to 100%|
|Lethal dose or concentration (LD, LC):|
LC50 (median concentration)
|836 ppm (mouse, 4 hr)
4000 ppm (rat, 4 hr)
800 ppm (rat, 4 hr)
819 ppm (guinea pig, 4 hr)
1460 ppm (rat, 4 hr)
835 ppm (mouse, 4 hr)
960 ppm (dog, 4 hr)
|US health exposure limits (NIOSH):|
|TWA 1 ppm 5 ppm [15-minute excursion]|
|Ca TWA <0.1 ppm (0.18 mg/m3) C 5 ppm (9 mg/m3) [10-min/day]|
IDLH (Immediate danger)
|Ca [800 ppm]|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is ?)(|
Ethylene oxide, called oxirane by IUPAC, is an organic compound with the formula C
4O. It is a cyclic ether and the simplest epoxide: a three-membered ring consisting of one oxygen atom and two carbon atoms. Ethylene oxide is a colorless and flammable gas with a faintly sweet odor. Because it is a strained ring, ethylene oxide easily participates in a number of addition reactions that result in ring-opening. Ethylene oxide is isomeric with acetaldehyde and with vinyl alcohol. Ethylene oxide is industrially produced by oxidation of ethylene in the presence of silver catalyst.
The reactivity that is responsible for many of ethylene oxide's hazards also make it useful. Although too dangerous for direct household use and generally unfamiliar to consumers, ethylene oxide is used for making many consumer products as well as non-consumer chemicals and intermediates. These products include detergents, thickeners, solvents, plastics, and various organic chemicals such as ethylene glycol, ethanolamines, simple and complex glycols, polyglycol ethers, and other compounds. Although it is a vital raw material with diverse applications, including the manufacture of products like polysorbate 20 and polyethylene glycol (PEG) that are often more effective and less toxic than alternative materials, ethylene oxide itself is a very hazardous substance. At room temperature it is a flammable, carcinogenic, mutagenic, irritating, and anaesthetic gas.
As a toxic gas that leaves no residue on items it contacts, ethylene oxide is a surface disinfectant that is widely used in hospitals and the medical equipment industry to replace steam in the sterilization of heat-sensitive tools and equipment, such as disposable plastic syringes. It is so flammable and extremely explosive that it is used as a main component of thermobaric weapons; therefore, it is commonly handled and shipped as a refrigerated liquid to control its hazardous nature.
- 1 History
- 2 Molecular structure and properties
- 3 Physical properties
- 4 Chemical properties
- 4.1 Addition of water and alcohols
- 4.2 Addition of carboxylic acids and their derivatives
- 4.3 Adding ammonia and amines
- 4.4 Halide addition
- 4.5 Metalorganic addition
- 4.6 Other addition reactions
- 4.7 Isomerization
- 4.8 Reduction reaction
- 4.9 Oxidation
- 4.10 Dimerization
- 4.11 Polymerization
- 4.12 Thermal decomposition
- 4.13 Other reactions
- 5 Laboratory synthesis
- 6 Industrial synthesis
- 7 Process overview
- 8 Applications
- 9 Non-industrial uses
- 10 Identification of ethylene oxide
- 11 Fire and explosion hazards
- 12 Physiological effects
- 13 Global demand
- 14 References
- 15 Cited sources
- 16 External links
- Cl–CH2CH2–OH + KOH → (CH2CH2)O + KCl + H2O
Wurtz measured the boiling point of ethylene oxide as 13.5 °C (56.3 °F), slightly higher than the present value, and discovered the ability of ethylene oxide to react with acids and salts of metals. Wurtz mistakenly assumed that ethylene oxide has the properties of an organic base. This misconception persisted until 1896 when Georg Bredig found that ethylene oxide is not an electrolyte. That it differed from other ethers — particularly by its propensity to engage in addition reactions, which are typical of unsaturated compounds — had long been a matter of debate. The heterocyclic triangular structure of ethylene oxide was proposed by 1868 or earlier.
Wurtz's 1859 synthesis long remained the only method of preparing ethylene oxide, despite numerous attempts, including by Wurtz himself, to produce ethylene oxide directly from ethylene. Only in 1931 did French chemist Theodore Lefort develop a method of direct oxidation of ethylene in the presence of silver catalyst. Since 1940, almost all industrial production of ethylene oxide has relied on this process. Sterilization by ethylene oxide for the preservation of spices was patented in 1938 by the American chemist Lloyd Hall. Ethylene oxide achieved industrial importance during World War I as a precursor to both the coolant ethylene glycol and the chemical weapon mustard gas.
Molecular structure and properties
The epoxy cycle of ethylene oxide is an almost regular triangle with bond angles of about 60° and a significant angular strain corresponding to the energy of 105 kJ/mol. For comparison, in alcohols the C–O–H angle is about 110°; in ethers, the C–O–C angle is 120°. The moment of inertia about each of the principal axes are IA = 32.921×10−40 g·cm2, IB = 37.926×10−40 g·cm2 and IC = 59.510×10−40 g·cm2.
The relative instability of the carbon-oxygen bonds in the molecule is revealed by the comparison in the table of the energy required to break two C–O bonds in the ethylene oxide or one C–O bond in ethanol and dimethyl ether:
|(C2H4)O → C2H4 + O (cleavage of two bonds)||354.38||Calculated, from atomic enthalpies|
|C2H5OH → C2H5 + OH (breaking one bond)||405.85||Electron impact|
|CH3OCH3 → CH3O + CH3 (breaking one bond)||334.72||Calculated using enthalpies of radicals formation|
This instability correlates with its high reactivity, explaining the ease of its ring-opening reactions (see Chemical properties).
Ethylene oxide is a colorless gas at 25 °C (77 °F) and is a mobile liquid at 0 °C (32 °F) – viscosity of liquid ethylene oxide at 0 °C is about 5.5 times lower than that of water. The gas has a characteristic sweet odor of ether, noticeable when its concentration in air exceeds 500 ppm. Ethylene oxide is readily soluble in water, ethanol, diethyl ether and many organic solvents.
Main thermodynamical constants are:
- The surface tension of liquid ethylene oxide, at the interface with its own vapor, is 35.8 mJ/m2 (0.00079 cal/sq ft) at −50.1 °C (−58.2 °F) and 27.6 mJ/m2 (0.00061 cal/sq ft) at −0.1 °C (31.8 °F).
- The boiling point increases with the vapor pressure as follows: 57.7 °C (135.9 °F) (2 atm (200 kPa; 29 psi)), 83.6 °C (182.5 °F) (5 atm (510 kPa; 73 psi)), and 114.0 °C (237.2 °F) (10 atm (1,000 kPa; 150 psi)).
- Viscosity decreases with temperature with the values of 0.577 kPa·s at −49.8 °C (−57.6 °F), 0.488 kPa·s at −38.2 °C (−36.8 °F), 0.394 kPa·s at −21.0 °C (−5.8 °F), and 0.320 kPa·s at 0 °C (32 °F).
Between −91 and 10.5 °C (−131.8 and 50.9 °F), vapor pressure p (in mmHg) varies with temperature (T in °C) as .
|Temperature, °C||Vapor pressure, kPa||Enthalpy of the liquid, J/g||Enthalpy of vaporization, J/g||Density, kg/L||Heat capacity, J/(kg·K)||Thermal conductivity, W/(m·K)|
*N/A – data not available.
|Temperature, K||Entropy, J/(mol·K)||Heat of formation, kJ/mol||Free energy of formation, kJ/mol||Viscosity, Pa·s||Thermal conductivity, W/(m·K)||Heat capacity, J/(mol·K)|
*N/A – data not available.
Ethylene oxide readily reacts with diverse compounds with opening of the ring. Its typical reactions are with nucleophiles which proceed via the SN2 mechanism both in acidic (weak nucleophiles: water, alcohols) and alkaline media (strong nucleophiles: OH−, RO−, NH3, RNH2, RR'NH, etc.). The general reaction scheme is
and more specific reactions are described below.
Addition of water and alcohols
Aqueous solutions of ethylene oxide are rather stable and can exist for a long time without any noticeable chemical reaction, but adding a small amount of acid, such as strongly diluted sulfuric acid, immediately leads to the formation of ethylene glycol, even at room temperature:
- (CH2CH2)O + H2O → HO–CH2CH2–OH
The reaction is usually carried out at about 60 °C (140 °F) with a large excess of water, in order to prevent the reaction of the formed ethylene glycol with ethylene oxide that would form di- and triethylene glycol:
- 2 (CH2CH2)O + H2O → HO–CH2CH2–O–CH2CH2–OH
- 3 (CH2CH2)O + H2O → HO–CH2CH2–O–CH2CH2–O–CH2CH2–OH
The use of alkaline catalysts may lead to the formation of polyethylene glycol:
- n (CH2CH2)O + H2O → HO–(–CH2CH2–O–)n–H
Reactions with alcohols proceed similarly yielding ethylene glycol ethers:
- (CH2CH2)O + C2H5OH → HO–CH2CH2–OC2H5
- 2 (CH2CH2)O + C2H5OH → HO–CH2CH2–O–CH2CH2–OC2H5
Reactions with lower alcohols occur less actively than with water and require more severe conditions, such as heating to 160 °C (320 °F) and pressurizing to 3 MPa (440 psi) and adding an acid or alkali catalyst.
Addition of carboxylic acids and their derivatives
Reactions of ethylene oxide with carboxylic acids in the presence of a catalyst results in glycol mono- and diesters:
- (CH2CH2)O + CH3CO2H → HOCH2CH2–O2CCH3
- (CH2CH2)O + (CH3CO)2O → CH3CO2CH2CH2O2CCH3
The addition of acid amides proceeds similarly:
- (CH2CH2)O + CH3CONH2 → HOCH2CH2NHC(O)CH3
Addition of ethylene oxide to higher carboxylic acids is carried out at elevated temperatures (typically 140–180 °C (284–356 °F)) and pressure (0.3–0.5 MPa (44–73 psi)) in an inert atmosphere, in presence of an alkaline catalyst (concentration 0.01–2%), such as hydroxide or carbonate of sodium or potassium. The carboxylate ion acts as nucleophile in the reaction:
- (CH2CH2)O + RCO2− → RCO2CH2CH2O−
- RCO2CH2CH2O− + RCO2H → RCO2CH2CH2OH + RCO2−
Adding ammonia and amines
- (CH2CH2)O + NH3 → HO–CH2CH2–NH2
- 2 (CH2CH2)O + NH3 → (HO–CH2CH2)2NH
- 3 (CH2CH2)O + NH3 → (HO–CH2CH2)3N
Similarly proceed the reactions with primary and secondary amines:
- (CH2CH2)O + RNH2 → HO–CH2CH2–NHR
Dialkylamino ethanols can further react with ethylene oxide, forming amino polyethylene glycols:
- n (CH2CH2)O + R2NCH2CH2OH → R2NCH2CH2O–(–CH2CH2O–)n–H
- (CH2CH2)O + (CH3)3N + H2O → [HOCH2CH2N (CH3)3]+OH−
Aromatic primary and secondary amines also react with ethylene oxide, forming the corresponding arylamino alcohols.
- (CH2CH2)O + HCl → HO–CH2CH2–Cl
The reaction with these acids competes with the acid-catalyzed hydration of ethylene oxide; therefore, there is always a by-product of ethylene glycol with an admixture of diethylene glycol. For a cleaner product, the reaction is conducted in the gas phase or in an organic solvent.
Ethylene fluorohydrin is obtained differently, by boiling hydrogen fluoride with a 5–6% solution of ethylene oxide in diethyl ether. The ether normally has a water content of 1.5–2%; in absence of water, ethylene oxide polymerizes.
Halohydrins can also be obtained by passing ethylene oxide through aqueous solutions of metal halides:
- 2 (CH2CH2)O + CuCl2 + 2 H2O → 2 HO–CH2CH2–Cl + Cu(OH)2↓
Interaction of ethylene oxide with organomagnesium compounds, which are Grignard reagents, can be regarded as nucleophilic substitution influenced by carbanion organometallic compounds. The final product of the reaction is a primary alcohol:
Similar mechanism is valid for other organometallic compounds, such as alkyl lithium:
Other addition reactions
Addition of hydrogen cyanide
Ethylene oxide easily reacts with the hydrogen cyanide forming ethylene cyanohydrin:
- (CH2CH2)O + HCN → HO–CH2CH2–CN
- 2 (CH2CH2)O + Ca(CN)2 + 2 H2O → 2 HO–CH2CH2–CN + Ca(OH)2
Ethylene cyanohydrin easily loses water, producing acrylonitrile:
- HO–CH2CH2–CN → CH2=CH–CN + H2O
Addition of hydrogen sulfide and mercaptans
When reacting with the hydrogen sulfide, ethylene oxide forms 2-mercaptoethanol and thiodiglycol, and with alkylmercaptans it produces 2-alkyl mercaptoetanol:
- (CH2CH2)O + H2S → HO–CH2CH2–HS
- 2 (CH2CH2)O + H2S → (HO–CH2CH2)2S
- (CH2CH2)O + RHS → HO–CH2CH2–SR
The excess of ethylene oxide with an aqueous solution of hydrogen sulfide leads to the tris-(hydroxyethyl) sulfonyl hydroxide:
- 3 (CH2CH2)O + H2S → [(HO–CH2CH2)3S+]OH−
Addition of nitrous and nitric acids
- 2 (CH2CH2)O + Ca(NO2)2 + 2 H2O → 2 HO–CH2CH2–NO2 + Ca(OH)2
Reaction with compounds containing active methylene groups
Alkylation of aromatic compounds
Styrene can be obtained in one stage if this reaction is conducted at elevated temperatures (315–440 °C (599–824 °F)) and pressures (0.35–0.7 MPa (51–102 psi)), in presence of an aluminosilicate catalyst.
Synthesis of crown ethers
A series of polynomial heterocyclic compounds, known as crown ethers, can be synthesized with ethylene oxide. One method is the cationic cyclopolymerization of ethylene oxide, limiting the size of the formed cycle:
- n (CH2CH2)O → (–CH2CH2–O–)n
To suppress the formation of other linear polymers the reaction is carried out in a highly dilute solution.
The radical mechanism was proposed to explain this reaction in the gas phase; it comprises the following stages:
(CH2CH2)O ↔ •CH2CH2O• → CH3CHO*
CH3CHO* → CH3• + CHO•
CH3CHO* + M → CH3CHO + M*
In reaction (3), M refers to the wall of the reaction vessel or to a heterogeneous catalyst. The moiety CH3CHO* represents a short-lived (lifetime of 10−8.5 seconds), activated molecule of acetaldehyde. Its excess energy is about 355.6 kJ/mol, which exceeds by 29.3 kJ/mol the binding energy of the C-C bond in acetaldehyde.
Conversely, with some other catalysts, ethylene oxide may be reduced by hydrogen to ethylene with the yield up to 70%. The reduction catalysts include mixtures of zinc dust and acetic acid, of lithium aluminium hydride with titanium trichloride (the reducing agent is actually titanium dichloride, formed by the reaction between LiAlH4 and TiCl3) and of iron(III) chloride with butyllithium in tetrahydrofuran.
Deep gas-phase reactor oxidation of ethylene oxide at 800–1,000 K (527–727 °C; 980–1,340 °F) and a pressure of 0.1–1 MPa (15–145 psi) yields a complex mixture of products containing O2, H2, CO, CO2, CH4, C2H2, C2H4, C2H6, C3H6, C3H8 and CH3CHO.
In the presence of acid catalysts, ethylene oxide dimerizes to afford dioxane:
The reaction mechanism is as follows:
The dimerization reaction is unselective. By-products include acetaldehyde (due to isomerization). The selectivity and speed of dimerization can be increased by adding a catalyst, such as platinum, platinum-palladium, or iodine with sulfolane. 2-methyl-1,3-dioxolane is formed as a side product in the last case.
Liquid ethylene oxide can form polyethyleneglycols. The polymerization can proceed via radical and ionic mechanisms, but only the latter has a wide practical application. Cationic polymerization of ethylene oxide is assisted by protonic acids (HClO4, HCl), Lewis acids (SnCl4, BF3, etc.), organometallic compounds or more complex reagents:
The reaction mechanism is as follows. At the first stage, the catalyst (MXm) is initiated by alkyl-or acylhalogen or by compounds with active hydrogen atoms, usually water, alcohol or glycol:
- MXm + ROH → MXmRO−H+
The resulting active complex reacts with ethylene oxide via the SN2 mechanism:
- (CH2CH2)O + MXmRO−H+ → (CH2CH2)O•••H+O−RMXm
- (CH2CH2)O•••H+ O−RMXm → HO–CH2CH2+ + MXmRO−2
- HO–CH2CH2+ + n (CH2CH2)O → HO–CH2CH2–(O–CH2CH2)n+
The chain breaks as
- HO–CH2CH2–(O–CH2CH2)n+ + MXmRO− → HO–CH2CH2–(O–CH2CH2)n–OR + MXm
- H(O–CH2CH2)n–O–CH2–CH2+ + MXmRO− → H(O–CH2CH2)n–O–CH=CH2 + MXm + ROH
Anionic polymerization of ethylene oxide is assisted by bases, such as alkoxides, hydroxides, carbonates or other compounds of alkali or alkaline earth metals. The reaction mechanism is as follows:
- (CH2CH2)O + RONa → RO–CH2CH2–O−Na+
- RO–CH2CH2–O−Na+ + n (CH2CH2)O → RO–(CH2CH2–O)n–CH2CH2–O−Na+
- RO–(CH2CH2–O)n–CH2CH2–O−Na+ → RO–(CH2CH2–O)n–CH=CH2 + NaOH
- RO–(CH2CH2–O)n–CH2CH2–O−Na+ + H2O → RO–(CH2CH2–O)(n+1)OH + NaOH
Ethylene oxide is relatively stable to heating – in the absence of a catalyst, it does not dissociate up to 300 °C (572 °F), and only above 570 °C (1,058 °F) there is a major exothermic decomposition, which proceeds through the radical mechanism. The first stage involves isomerization, however high temperature accelerates the radical processes. They result in a gas mixture containing acetaldehyde, ethane, ethyl, methane, hydrogen, carbon dioxide, ketene and formaldehyde. High-temperature pyrolysis (830–1,200 K (557–927 °C; 1,034–1,700 °F)) at elevated pressure in an inert atmosphere leads to a more complex composition of the gas mixture, which also contains acetylene and propane. Contrary to the isomerization, initiation of the chain occurs mainly as follows:
- (CH2CH2)O → •CH2CH2O• → CH2O + CH2:
When carrying the thermal decomposition of ethylene oxide in the presence of transition metal compounds as catalysts, it is possible not only to reduce its temperature, but also to have ethyl as the main product, that is to reverse the ethylene oxide synthesis reaction.
- (CH2CH2)O + (NH2)2C=S → (CH2CH2)S + (NH2)2C=O
- (CH2CH2)O + PCl5 → Cl–CH2CH2–Cl + POCl3
- (CH2CH2)O + PCl3 → Cl–CH2CH2–OPCl2
- 2 (CH2CH2)O + PCl3 → (Cl–CH2CH2–O)2PCl
- 3 (CH2CH2)O + PCl3 → Cl–CH2CH2–O)3P
- (CH2CH2)O + RCOCl + NaI → RC(O)–OCH2CH2–I + NaCl
In industry, a similar reaction is carried out at high pressure and temperature in the presence of quaternary ammonium or phosphonium salts as a catalyst.
Substituting formaldehyde by other aldehydes or ketones results in a 2-substituted 1,3-dioxolane (yield: 70–85%, catalyst: tetraethylammonium bromide).
Dehydrochlorination of ethylene and its derivatives
Dehydrochlorination of 2-chloroethanol, developed by Wurtz back in 1859, remains a common laboratory route to ethylene oxide:
- Cl–CH2CH2–OH + NaOH → (CH2CH2)O + NaCl + H2O
The reaction is carried out at elevated temperature, and beside sodium hydroxide or potassium hydroxide, calcium hydroxide, barium hydroxide, magnesium hydroxide or carbonates of alkali or alkaline earth metals can be used.
- 2 CH3CH2–OCl + CaO → 2 (CH2CH2)O + CaCl2 + H2O
Direct oxidation of ethylene by peroxy acids
Oxidation by peroxy acids is efficient for higher alkenes, but not for ethylene. The above reaction is slow and has low yield, therefore it is not used in the industry.
Other preparative methods
and decomposition of ethylene carbonate at 200–210 °C (392–410 °F) in the presence of hexachloroethane:
Commercial production of ethylene oxide dates back to 1914 when BASF built the first factory which used the chlorohydrin process (reaction of ethylene chlorohydrin with calcium hydroxide). The chlorohydrin process was unattractive for several reasons, including low efficiency and loss of valuable chlorine into calcium chloride. More efficient direct oxidation of ethylene by air was invented by Lefort in 1931 and in 1937 Union Carbide opened the first plant using this process. It was further improved in 1958 by Shell Oil Co. by replacing air with oxygen and using elevated temperature of 200–300 °C (390–570 °F) and pressure (1–3 MPa (150–440 psi)). This more efficient routine accounted for about half of ethylene oxide production in the 1950s in the US, and after 1975 it completely replaced the previous methods. The production of ethylene oxide accounts for approximately 11% of worldwide ethylene demand.
Chlorohydrin process of production of ethylene oxide
Although the chlorohydrin process is almost entirely superseded in the industry by the direct oxidation of ethylene, the knowledge of this method is still important for educational reasons and because it is still used in the production of propylene oxide. The process consists of three major steps: synthesis of ethylene chlorohydrin, dehydrochlorination of ethylene chlorohydrin to ethylene oxide and purification of ethylene oxide. Those steps are carried continuously. In the first column, hypochlorination of ethylene is carried out as follows:
- Cl2 + H2O → HOCl + HCl
- CH2=CH2 + HOCl → OH–CH2CH2–Cl
- CH2=CH2 + Cl2 → Cl–CH2CH2–Cl
To suppress the conversion of ethylene into the ethylene dichloride (the last reaction), the concentration of ethylene is maintained at about 4–6%, and the solution is heated by steam to the boiling point.
Next, aqueous solution of ethylene chlorohydrin enters the second column, where it reacts with a 30% solution of calcium hydroxide at 100 °C (212 °F):
- 2 OH–CH2CH2–Cl + Ca(OH)2 → 2 (CH2CH2)O + CaCl2 + 2H2O
The produced ethylene oxide is purified by rectification. The chlorohydrin process allows to reach 95% conversion of ethylene chlorohydrin. The yield of ethylene oxide is about 80% of the theoretical value; for 1 tonne (0.98 long tons; 1.1 short tons) of ethylene oxide, about 200 kg (440 lb) of ethylene dichloride is produced. But, the major drawbacks of this process are high chlorine consumption and effluent load. This process is now obsolete.
Direct oxidation of ethylene
Usage in global industry
Direct oxidation of ethylene was patented by Lefort in 1931. This method was repeatedly modified for industrial use, and at least four major variations are known. They all use oxidation by oxygen or air and a silver-based catalyst, but differ in the technological details and hardware implementations.
A similar production method was developed by Scientific Design Co., but it received wider use because of the licensing system – it accounts for 25% of the world's production and for 75% of world's licensed production of ethylene oxide. A proprietary variation of this method is used by Japan Catalytic Chemical Co., which adapted synthesis of both ethylene oxide and ethylene glycol in a single industrial complex.
A different modification was developed Shell International Chemicals BV. Their method is rather flexible with regard to the specific requirements of specific industries; it is characterized by high selectivity with respect to the ethylene oxide product and long lifetime of the catalyst (3 years). It accounts for about 40% of global production.
Older factories typically use air for oxidation whereas newer plants and processes, such as METEOR and Japan Catalytic, favor oxygen.
Chemistry and kinetics of the direct oxidation process
Formally, the direct oxidation process is expressed by the following equation:
- , ΔH = −105 kJ/mol
However, significant yield of carbon dioxide and water is observed in practice, which can be explained by the complete oxidation of ethylene or ethylene oxide:
- CH2=CH2 + 3 O2 → 2 CO2 + 2 H2O, ΔH = −1327 kJ/mol
- (CH2CH2)O + 2.5 O2 → 2 CO2 + 2 H2O, ΔH = −1223 kJ/mol
The process of heterogeneous catalytic oxidation of ethylene was studied by P. A. Kilty and W. M. H. Sachtler, who suggested the following mechanism:
- O2 + 4 Ag(adj) → 4 Ag + 2 O2−(ads)
- O2 + Ag → Ag+ + O2−
- O2−(ads) + CH2=CH2 → (CH2CH2)O + O(ads)
- 6 O (ads) + CH2=CH2 → 2 CO2 + 2 H2O
Here (ads) refers to particles adsorbed on the catalyst surface and (adj) to particles of silver, directly adjacent to the oxygen atoms. In this process, 1,2-dichloroethane, vinyl chloride are used as inhibitors so as to prevent further oxidation of ethylene oxide to CO2 and H2O. Here, the chemisorbed chlorine hinders dissociative chemisorption of atomic oxygen.
Thus the overall reaction is expressed as
- 7 CH2=CH2 + 6 O2 → 6 (CH2CH2)O + 2 CO2 + 2 H2O
and the maximum degree of conversion of ethylene to ethylene oxide is 6/7 or 85.7%.
The catalyst for the reaction is metallic silver deposited on various matrixes, including pumice, silica gel, various silicates and aluminosilicates, alumina and silicon carbide, and activated by certain additives (antimony, bismuth, barium peroxide, etc.). The process temperature was optimized as 220–280 °C (430–540 °F). Lower temperatures reduce the activity of the catalyst, and higher temperatures promote the complete oxidation of ethylene thereby reducing the yield of ethylene oxide. Elevated pressure of 1–3 MPa (150–440 psi) increases the productivity of the catalyst and facilitates absorption of ethylene oxide from the reacting gases.
Whereas oxidation by air is still being used, oxygen (> 95% purity) is preferred for several reasons, such as higher molar yield of ethylene oxide (75–82% for oxygen vs. 63–75% for air), higher reaction rate (no gas dilution) and no need of separating nitrogen in the reaction products.
The production of ethylene oxide on a commercial scale is attained with the unification of the following unit processes:
- Main reactor
- Ethylene oxide scrubber
- Ethylene oxide de-sorber
- Stripping and distillation column
- CO2 scrubber and CO2 de-scrubber
Main Reactor: The main reactor consists of thousands of catalyst tubes in bundles. These tubes are generally 6 to 15 m (20 to 50 ft) long with an inner diameter of 20 to 50 mm (0.8 to 2.0 in). The catalyst packed in these tubes is in the form of spheres or rings of diameter 3 to 10 mm (0.12 to 0.39 in). The operating conditions of 200–300 °C (390–570 °F) with a pressure of 1–3 MPa (150–440 psi) prevail in the reactor. To maintain this temperature, the cooling system of the reactor plays a vital role. With the aging of the catalyst, its selectivity decreases and it produces more exothermic side products of CO2.
Ethylene oxide scrubber: After the gaseous stream from the main reactor, containing ethylene oxide (1–2%) and CO2 (5%), is cooled, it is then passed to the ethylene oxide scrubber. Here, water is used as the scrubbing media which scrubs away majority of ethylene oxide along with some amounts of CO2, N2, CH2=CH2, CH4 and aldehydes (introduced by the recycle stream). Also, a small proportion of the gas leaving the ethylene oxide scrubber (0.1–0.2%) is removed continuously (combusted) to prevent the buildup of inert compounds (N2, Ar, and C2H6), which are introduced as impurities with the reactants.
Ethylene oxide de-sorber: The aqueous stream resulting from the above scrubbing process is then sent to the ethylene oxide de-sorber. Here, ethylene oxide is obtained as the overhead product, whereas the bottom product obtained is known as the glycol bleed. When ethylene oxide is scrubbed from the recycle gas with an aqueous solution, ethylene glycols (viz. mono-ethylene glycol, di-ethylene glycol and other poly-ethylene glycols) get unavoidably produced. Thus, in-order to prevent them from building up in the system, they are continuously bled off.
Stripping and distillation column: Here, the ethylene oxide stream is stripped off its low boiling components and then distilled in-order to separate it into water and ethylene oxide.
CO2 scrubber: The recycle stream obtained from the ethylene oxide scrubber is compressed and a side-stream is fed to the CO2 scrubber. Here, CO2 gets dissolved into the hot aqueous solution of potassium carbonate (i.e., the scrubbing media). The dissolution of CO2 is not only a physical phenomenon, but a chemical phenomenon as well, for, the CO2 reacts with potassium carbonate to produce potassium hydrogen carbonate.
- K2CO3 + CO2 + H2O → 2 KHCO3
CO2 de-scrubber: The above potassium carbonate solution (enriched with CO2) is then sent to the CO2 de-scrubber where CO2 is de-scrubbed by stepwise (usually two steps) flashing. The first step is done to remove the hydrocarbon gases, and the second step is employed to strip off CO2.
World production of ethylene oxide
The world production of ethylene oxide was 20 million tonnes (22 million short tons; 20 million long tons) in 2009, 19 million tonnes (21 million short tons; 19 million long tons) in 2008 and 18 million tonnes (20 million short tons; 18 million long tons) in 2007. This places ethylene oxide 14th most produced organic chemical, whereas the most produced one was ethylene with 113 million tonnes (125 million short tons; 111 million long tons). SRI Consulting forecasted the growth of consumption of ethylene oxide of 4.4% per year during 2008–2013 and 3% from 2013 to 2018.
In 2004, the global production of ethylene oxide by region was as follows:
|Region||Number of major producers||Production, thousand tonnes|
The world's largest producers of ethylene oxide are Dow Chemical Company (3–3.5 million tonnes (3.3–3.9 million short tons; 3.0–3.4 million long tons) in 2006), Saudi Basic Industries (2,000–2,500 tonnes (2,200–2,800 short tons; 2,000–2,500 long tons) in 2006), Royal Dutch Shell (1.328 million tonnes (1.464 million short tons; 1.307 million long tons) in 2008–2009), BASF (1.175 million tonnes (1.295 million short tons; 1.156 million long tons) in 2008–2009), China Petrochemical Corporation (~1 million tonnes (1.1 million short tons; 0.98 million long tons) in 2006), Formosa Plastics (~1 million tonnes (1.1 million short tons; 0.98 million long tons) in 2006) and Ineos (0.92 million tonnes (1.01 million short tons; 0.91 million long tons) in 2008–2009).
Ethylene oxide is one of the most important raw materials used in large-scale chemical production. Most ethylene oxide is used for synthesis of ethylene glycols, including diethylene glycol and triethylene glycol, that accounts for up to 75% of global consumption. Other important products include ethylene glycol ethers, ethanolamines and ethoxylates. Among glycols, ethylene glycol is used as antifreeze, in the production of polyester and polyethylene terephthalate (PET – raw material for plastic bottles), liquid coolants and solvents.
|Sector||Demand share (%)|
|Total ||5.2 Mt|
Polyethyleneglycols are used in perfumes, cosmetics, pharmaceuticals, lubricants, paint thinners and plasticizers. Ethylene glycol ethers are part of brake fluids, detergents, solvents, lacquers and paints. Other products of ethylene oxide. Ethanolamines are used in the manufacture of soap and detergents and for purification of natural gas. Ethoxylates are reaction products of ethylene oxide with higher alcohols, acids or amines. They are used in the manufacture of detergents, surfactants, emulsifiers and dispersants.
Whereas synthesis of ethylene glycols is the major application of ethylene oxide, its percentage varies greatly depending on the region: from 44% in the Western Europe, 63% in Japan and 73% in North America to 90% in the rest of Asia and 99% in Africa.
Production of ethylene glycol
Ethylene glycol is industrially produced by non-catalytic hydration of ethylene oxide at a temperature of 200 °C (392 °F) and a pressure of 1.5–2 MPa (220–290 psi):
- (CH2CH2)O + H2O → HOCH2CH2OH
By-products of the reaction are diethylene glycol, triethylene glycol and polyglycols with the total of about 10%, which are separated from the ethylene glycol by distillation at reduced pressure.
Another synthesis method is the reaction of ethylene oxide and CO2 (temperature 80–120 °C (176–248 °F) and pressure of 5.2 MPa (750 psi)) yielding ethylene carbonate and its subsequent hydrolysis with decarboxylation:
Modern technologies of production of ethylene glycol include the following. Shell OMEGA technology (Only Mono-Ethylene Glycol Advantage) is a two-step synthesis of ethylene carbonate using a phosphonium halide as a catalyst. The glycol yield is 99–99.5%, with other glycols practically absent. The main advantage of the process is production of pure ethylene glycol without the need for further purification. The first commercial plant which uses this method was opened in 2008 in South Korea. Dow METEOR (Most Effective Technology for Ethylene Oxide Reactions) is an integrated technology for producing ethylene oxide and its subsequent hydrolysis into ethylene glycol. The glycol yield is 90–93%. The main advantage of the process is relative simplicity, using fewer stages and less equipment.
Production of glycol ethers
The major industrial esters of mono-, di- and triethylene glycols are methyl, ethyl and normal butyl ethers, as well as their acetates and phthalates. The synthesis involves reaction of the appropriate alcohol with ethylene oxide:
- (CH2CH2)O + ROH → HOCH2CH2OR
- (CH2CH2)O + HOCH2CH2OR → HOCH2CH2OCH2CH2OR
- (CH2CH2)O + HOCH2CH2OCH2CH2OR → HOCH2CH2OCH2CH2OCH2CH2OR
The reaction of monoesters with an acid or its anhydride leads to the formation of the esters:
- CH3CO2H + HOCH2CH2OR → ROCH2CH2OCOCH3 + H2O
Production of ethanolamines
In the industry, ethanolamines (mono-, di- and triethanolamines) are produced by reacting ammonia and ethylene oxide in anhydrous medium at a temperature of 40–70 °C (100–160 °F) and pressure of 1.5–3.5 MPa (220–510 psi) MPa:
- (CH2CH2)O + NH3 → HOCH2CH2NH2
- 2 (CH2CH2)O + NH3 → (HOCH2CH2)2NH
- 3 (CH2CH2)O + NH3 → (HOCH2CH2)3N
All three ethanolamines are produced in the process, while ammonia and part of methylamine are recycled. The final products are separated by vacuum distillation. Hydroxyalkylamines are produced in a similar process:
- (CH2CH2)O + RNH2 → HOCH2CH2NHR
- 2 (CH2CH2)O + RNH2 → (HOCH2CH2)2NR
Monosubstituted products are formed by reacting a large excess of amine with ethylene oxide in presence of water and at a temperature below 100 °C (212 °F). Disubstituted products are obtained with a small excess of ethylene oxide, at a temperature of 120–140 °C (250–280 °F) and a pressure of 0.3–0.5 MPa (45–75 psi).
Production of ethoxylates
Industrial production of ethoxylates is realized by a direct reaction of higher alcohols, acids or amines with ethylene oxide in the presence of an alkaline catalyst at a temperature of 120–180 °C (250–360 °F). Modern plants producing ethoxylates are usually based on the BUSS LOOP reactors technology, which is based on a three-stage continuous process. In the first stage, the initiator or catalyst of the reaction and the feedstock are fed into the container, where they are mixed, heated and vacuum dried. Then reaction is carried out in a special insulated reactor in an inert atmosphere (nitrogen) to prevent a possible explosion of ethylene oxide. Finally, the reaction mixture is neutralized, degassed and purified.
Production of acrylonitrile
Currently, most acrylonitrile (90% in 2008) is produced by the SOHIO method, which is based on the catalytic oxidation of propylene in the presence of ammonia and bismuth phosphomolybdate. However, until 1960 a key production process was addition of hydrogen cyanide to ethylene oxide, followed by dehydration of the resulting cyanohydrin: 
Addition of hydrocyanic acid to ethylene oxide is carried out in the presence of a catalyst (sodium hydroxide and diethylamine), and dehydration of cyanohydrin occurs in the gas phase upon the catalytic action of aluminium oxide.
The direct use of ethylene oxide accounts for only 0.05% (2004 data) of its global production. Ethylene oxide is used as a sterilizing agent, disinfecting agent and fumigant as a mixture with carbon dioxide (8.5–80% of ethylene oxide), nitrogen or dichlorodifluoromethane (12% ethylene oxide). It is applied for gas-phase sterilization of medical equipment and instruments, packaging materials and clothing, surgical and scientific equipment; for processing of storage facilities (tobacco, packages of grain, sacks of rice, etc.), clothing, furs and valuable documents.
Ethylene oxide is one of the most commonly used sterilization methods in the healthcare industry because of its non-damaging effects for delicate instruments and devices that require sterilization, and for its wide range of material compatibility. It is used for instruments that cannot tolerate heat, moisture or abrasive chemicals, such as electronics, optical equipment, paper, rubber and plastics. It was developed in the 1940s as a sterilant by the US military, and its use as a medical sterilant dates to the late 1950s, when the McDonald process was patented for medical devices. The Anprolene system was patented in the 1960s by Andersen Products, and it remains the most commonly used system in several niche markets, notably the veterinary market and some international markets. It relies on the use of a flexible sterilization chamber and an EtO cartridge for small volume sterilization, and where environmental and/or portability considerations dictate the use of a low dose. It is therefore referred to as the "flexible chamber sterilization" method, or the "gas diffusion sterilization" method.
Identification of ethylene oxide
An inexpensive test for ethylene oxide exploits its precipitation of solids hydroxides of metals when it is passed through aqueous solutions of their salts:
- 2 (CH2CH2)O + MnCl2 + 2 H2O → 2 HO–CH2CH2–Cl + Mn(OH)2↓
Similarly, ethylene oxide is detected by the bright pink color of the indicator when passing air through aqueous solutions of some salts of sodium or potassium (chlorides, iodides, thiosulfates, etc.) with the addition of phenolphthalein:
- (CH2CH2)O + NaCl + H2O → HO–CH2CH2–Cl + NaOH
Other methods of ethylene oxide detection are color reactions with pyridine derivatives and hydrolysis of ethylene glycol with periodic acid. The produced iodic acid is detected with silver nitrate.
Fire and explosion hazards
Ethylene oxide is extremely flammable, and its mixtures with air are explosive. When heated it may rapidly expand, causing fire and explosion. The Autoignition temperature is 429 °C (804 °F), decomposition temperature of 571 °C (1,060 °F) at 101.3 kPa (14.69 psi), minimum inflammable content in the air is 2.7%, and maximum limit is 100%. The NFPA rating is NFPA 704. Ethylene oxide in presence of water can hydrolyze to ethylene glycol and form poly ethylene oxide which then eventually gets oxidized by air and leads to hotspots that can trigger to explosive decomposition.
Fires caused by ethylene oxide are extinguished by traditional media, including foam, carbon dioxide or water. Suppression of this activity can be done by blanketing with an inert gas until total pressure reaches non explosive range. Extinguishing of burning ethylene oxide is complicated by that it can continue burning in an inert atmosphere and in water solutions. Fire suppression is reached only upon dilution with water above 22:1.
Accidents involving ethylene oxide explosion
An Ethylene oxide explosion on August 19, 2004 in Sterigenics International Inc. in Ontario, California, USA injured four employees and severely damaged the medical products sterilization facility. It was caused by workers skipping a crucial step in removing ethylene oxide from a sterilization chamber. 
Effect on microorganisms
Exposure to ethylene oxide gas causes alkylation to microorganisms at a nuclear level. The disinfectant effect of ethylene oxide is similar to that of sterilization by heat, but because of limited penetration, it affects only the surface. ETO sterilization can take up to 12 hours due to its slow action upon microorganisms, and lengthy processing and aeration time.
Effects on humans and animals
Ethylene oxide is an alkylating agent; it has irritating, sensitizing and narcotic effects. Chronic exposure to ethylene oxide is also mutagenic. The International Agency for Research on Cancer classifies ethylene oxide into group 1, meaning it is a proven carcinogen. Ethylene oxide is classified as a class 2 carcinogen by the German MAK commission and as a class A2 carcinogen by the ACGIH. A 2003 study of 7,576 women exposed while at work in commercial sterilization facilities in the US suggests ethylene oxide is associated with breast cancer incidence. A 2004 follow up study analyzing 18,235 men and women workers exposed to ethylene oxide from 1987 to 1998 concluded "There was little evidence of any excess cancer mortality for the cohort as a whole, with the exception of bone cancer based on small numbers. Positive exposure-response trends for lymphoid tumors were found for males only. Reasons for the sex specificity of this effect are not known. There was also some evidence of a positive exposure-response for breast cancer mortality." An increased incidence of brain tumors and mononuclear cell leukemia was found in rats that had inhaled ethylene oxide at concentrations of 10, 33 or 100 mL/m3 (0.0100, 0.0329 or 0.0997 imp fl oz/cu ft) over a period of two years. An increased incidence of peritoneal mesotheliomas was also observed in the animals exposed to concentrations of 33 and 100 mL/m3 (0.0329 and 0.0997 imp fl oz/cu ft). Results of human epidemiological studies on workers exposed to ethylene oxide differ. There is evidence from both human and animal studies that inhalation exposure to ethylene oxide can result in a wide range of carcinogenic effects.
Ethylene oxide is toxic by inhalation, with a US OSHA permissible exposure limit calculated as a TWA (time weighted average) over 8 hours of 1 ppm, and a short term exposure limit (excursion limit) calculated as a TWA over 15 minutes of 5 ppm. At concentrations in the air about 200 parts per million, ethylene oxide irritates mucous membranes of the nose and throat; higher contents cause damage to the trachea and bronchi, progressing into the partial collapse of the lungs. High concentrations can cause pulmonary edema and damage the cardiovascular system; the damaging effect of ethylene oxide may occur only after 72 hours after exposure. The maximum content of ethylene oxide in the air according to the US standards (ACGIH) is 1.8 mg/m3 (0.00079 gr/cu ft). NIOSH has determined that the Immediately Dangerous to Life and Health level (IDLH) is 800 ppm.
Because the odor threshold for ethylene oxide varies between 250 and 700 ppm, the gas is already at toxic concentrations when it can be smelled. Even then, the odor of ethylene oxide is sweet, aromatic, and can easily be mistaken for the pleasant aroma of diethyl ether, a common laboratory solvent of very low toxicity. In view of these insidious warning properties, continuous electrochemical monitors are standard practice, and it is forbidden to use ethylene oxide to fumigate building interiors in the EU and some other jurisdictions.
Ethylene oxide causes acute poisoning, accompanied by a variety of symptoms. Central nervous system effects are frequently associated with human exposure to ethylene oxide in occupational settings. Headache, nausea, and vomiting have been reported.[clarification needed] Peripheral neuropathy, impaired hand-eye coordination and memory loss have been reported in more recent case studies of chronically-exposed workers at estimated average exposure levels as low as 3 ppm (with possible short-term peaks as high as 700 ppm). The metabolism of ethylene oxide is not completely known. Data from animal studies indicate two possible pathways for the metabolism of ethylene oxide: hydrolysis to ethylene glycol and glutathione conjugation to form mercapturic acid and meththio-metabolites.
Toxicity data for ethylene oxide are as follows:
- Eye exposure: 18 mg (0.28 gr)/6 hours (rabbit)
- Oral: 72 mg/kg (0.00115 oz/lb) (rat, LD50), 1,186 mg/kg (0.01898 oz/lb) (rat, TDLo), 5,112 mg/kg (0.08179 oz/lb) (rat, TD)
- Inhalation: 12,500 ppm (human, TCLo), 960 ppm/4 hours (dog, LC50) 33–50 ppm (rat or mouse, TC), 800 ppm/4 hours (rat or mouse, LC50)
- Subcutaneous injection: 100 mg/kg (0.0016 oz/lb) (cat, LDLo), 292 mg/kg (0.00467 oz/lb) (mouse, TDLo) 900–2,600 mg/kg (0.014–0.042 oz/lb) (mouse, TD), 187 mg/kg (0.00299 oz/lb) (rat, LD50).
- Intraperitoneal injection: 750 mg/kg (0.0120 oz/lb) (mouse, TDLo), 175 mg/kg (0.00280 oz/lb) (mouse, LD50)
- Intravenous injection: 175 mg/kg (0.00280 oz/lb) (rabbit, LD50), 290 mg/kg (0.0046 oz/lb) (mouse, LD50)
- The US Environmental Protection Agency (USEPA) estimated in 2016 that for low doses, the inhalation of ethylene oxide for a lifetime could increase an individual's lifetime cancer risk by as much as 3.0 × 10−3 per μg/m3 (without considering that early-life exposures are likely more potent). The USEPA estimated the slope of the dose-response declines at higher doses, and extra cancer risk estimates for several occupational exposure scenarios are calculated.
Global EO demand has expanded from 16.6 Mt (18.3 million short tons; 16.3 million long tons) in 2004 to 20 Mt (22 million short tons; 20 million long tons) in 2009, while demand for refined EO expanded from 4.64 Mt (5.11 million short tons; 4.57 million long tons) in 2004 to 5.6 Mt (6.2 million short tons; 5.5 million long tons) in 2008. In 2009, demand is estimated to have declined to about 5.2 Mt (5.7 million short tons; 5.1 million long tons). Total EO demand registered a growth rate of 5.6% per annum during the period 2005 to 2009 and is projected to grow at 5.7% per annum during 2009 to 2013.
- Oxirane | C2H4O – PubChem. Pubchem.ncbi.nlm.nih.gov. Retrieved on 2017-05-08.
- Haynes, p. 3.430
- "NIOSH Pocket Guide to Chemical Hazards #0275". National Institute for Occupational Safety and Health (NIOSH).
- Haynes, p. 3.576
- Haynes, p. 15.20
- Haynes, p. 5.22
- "Ethylene oxide". Immediately Dangerous to Life and Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
- Rebsdat, Siegfried and Mayer, Dieter (2005) "Ethylene Oxide" in Ullmann's Encyclopedia of Industrial Chemistry. Wiley-VCH, Weinheim. doi:10.1002/14356007.a10_117.
- McKetta, John J.; Cunningham, William A. (1984). Encyclopedia of Chemical Processing and Design. 20. CRC Press. p. 309. ISBN 0-8247-2470-4.
- Croddy, Eric; Wirtz, James J. (2005). Weapons of mass destruction: an encyclopedia of worldwide policy, technology, and history, Volume 2. ABC-CLIO. p. 136. ISBN 1-85109-490-3.
- Meyer, Rudolf; Köhler, Josef; Homburg, Axel (2007). Explosives. Wiley-VCH. p. 142. ISBN 3-527-31656-6.
- Wurtz, A. (1859). "Sur l'oxyde d'éthylène". Comptes rendus. 48: 101–105.
- Zimakov, P.V.; Dyment, O. H., eds. (1967). "Part I. Structure and properties of ethylene oxide. Features of the reactivity of ethylene oxide and the structure of its molecules". Ethylene oxide. Khimiya. pp. 15–17.
- Bredig, G.; Usoff, A. (1896). "Ist Acetylen ein Elektrolyt?" [Is acetylene an electrolyte?]. Zeitschrift für Elektrochemie. 3: 116–117.
- Eugen F. von Gorup-Besanez, ed., Lehrbuch der organischen Chemie für den Unterricht auf Universitäten … [Textbook of Organic Chemistry for Instruction at Universities … ], 3rd ed. (Braunschweig, Germany: Friedrich Vieweg und Sohn, 1868), vol. 2, p. 286.
See also p. 253 of the 1876 edition: Eugen F. von Gorup-Besanez, ed., Lehrbuch der organischen Chemie für den Unterricht auf Universitäten …, 5th ed. (Braunschweig, Germany: Friedrich Vieweg und Sohn, 1876), vol. 2.
- "Ethylene Oxide". Kirk-Othmer Encyclopedia of Chemical Technology. Elastomers, synthetic to Expert Systems. 9 (4 ed.). New York: John Wiley & Sons. 1994. pp. 450–466.
- Lefort, T.E. (23 April 1935) "Process for the production of ethylene oxide". U.S. Patent 1,998,878
- McClellan, P. P. (1950). "Manufacture and Uses of Ethylene Oxide and Ethylene Glycol". Ind. Eng. Chem. 42 (12): 2402–2407. doi:10.1021/ie50492a013.
- Knunyants, I. L., ed. (1988). "Voltage molecules". Chemical Encyclopedia. 3. "Soviet encyclopedia". pp. 330–334.
- Traven VF (2004). VFTraven, ed. Organic chemistry: textbook for schools. 2. ECC "Academkniga". pp. 102–106. ISBN 5-94628-172-0.
- Cunningham G. L.; Levan W. I.; Gwinn W. D. (1948). "The Rotational Spectrum of Ethylene Oxide". Phys. Rev. 74 (10): 1537. Bibcode:1948PhRv...74.1537C. doi:10.1103/PhysRev.74.1537.
- Kondrat'ev, VN, ed. (1974). Energy of chemical bonds. Ionization potentials and electron affinity. Nauka. pp. 77–78.
- "Medical Management Guidelines for Ethylene Oxide". Medical Management Guidelines (MMGs). Agency for Toxic Substances and Disease Registry. Retrieved 29 September 2009.
- "Этилена окись (Ethylene oxide)" (in Russian). Great Soviet Encyclopedia. Retrieved 25 September 2009.
- "Термодинамические показатели органических соединений". ChemAnalitica.com. 1 April 2009. Retrieved 21 September 2009.
- "Surface tension of liquefied gas at the border with its own steam". ChemAnalitica.com. 1 April 2009. Retrieved 21 September 2009.
- "Boiling point or sublimation (°C) organic matter in the vapor pressure above 101.3 kPa". ChemAnalitica.com. 1 April 2009. Retrieved 21 September 2009.
- "Viscosity of organic compounds". ChemAnalitica.com. 1 April 2009. Retrieved 21 September 2009.
- "Vapor pressure of organic compounds". ChemAnalitica.com. 1 April 2009. Retrieved 21 September 2009.
- Zimakov, P.V.; Dyment, O. H., eds. (1967). "Chapter III. Review of the individual reactions of ethylene oxide". Ethylene oxide. M.: Khimiya. pp. 90–120.
- "Epoxyethane (Ethylene Oxide)". Alkenes menu. Chemguide. Retrieved 5 October 2009.
- van Os; N. M., eds. (1998). Nonionic surfactants: organic chemistry. CRC Press. pp. 129–131. ISBN 978-0-8247-9997-7.
- Petrov, AA; Balian HV; Troshchenko AT (2002). "Chapter 12. Amino alcohol". In Stadnichuk. Organic chemistry (5 ed.). St. Petersburg. p. 286. ISBN 5-8194-0067-4.
- Sheppard, William A.; Sharts, Clay M. (1969). Organic Fluorine Chemistry. W.A. Benjamin. p. 98. ISBN 0-8053-8790-0.
- Kendall, E. C. and McKenzie, B. (1923). "o-Chloromercuriphenol". Organic Syntheses. 3: 57.
- Noland, Wayland E. (1973). "2-Nitroethanol". Organic Syntheses. 5: 833.
- Orlova, EY (1981). Chemistry and technology of high explosives: Textbook for high schools (3 ed.). Khimiya. p. 278.
- Vogel, A.I. (1989). Vogel's Textbook of practical organic chemistry (5 ed.). UK: Longman Scientific & Technical. p. 1088. ISBN 0-582-46236-3.
- Watson, James M. and Forward, Cleve (17 April 1984) U.S. Patent 4,443,643. "Reaction of benzene with ethylene oxide to produce styrene"
- Hiraoka M. (1982). Crown Compounds. Their Characteristics and Applications. Kodansha. pp. 33–34. ISBN 4-06-139444-4.
- Roesky H. W.; Schmidt H. G. (1985). "Reaction of Ethylene Oxide with Sulfur Dioxide in the Presence of Cesium Ions: Synthesis of 1,3,6,9,2 λ 4-Tetraoxathia-2-cycloundecanone". Angewandte Chemie International Edition. 24 (8): 695. doi:10.1002/anie.198506951.
- Petrov, AA; Balian HV; Troshchenko AT (2002). "Chapter 4. Ethers". Organic chemistry (5 ed.). St. Petersburg. pp. 159–160. ISBN 5-8194-0067-4.
- Benson S. W. (1964). "Pyrolysis of Ethylene Oxide. A Hot Molecule Reaction". The Journal of Chemical Physics. 40: 105. Bibcode:1964JChPh..40..105B. doi:10.1063/1.1729851.
- Zimakov, P.V.; Dyment, O. H., eds. (1967). "Chapter II. Chemical properties of ethylene oxide". Ethylene oxide. Khimiya. pp. 57–85.
- Hudlický M. (1984). Reductions in Organic Chemistry. Chichester: Ellis Horwood Limited. p. 83. ISBN 0-85312-345-4.
- Dagaut P.; Voisin D.; Cathonnet M.; Mcguinness M.; Simmie J. M. (1996). "The oxidation of ethylene oxide in a jet-stirred reactor and its ignition in shock waves". Combustion and Flame. 156: 62–68. doi:10.1016/0010-2180(95)00229-4.
- Stapp, Paul R. (21 December 1976) U.S. Patent 3,998,848 "Cyclodimerization of ethylene oxide"
- Dyment, ON; Kazanskii, KS; Miroshnikov AM (1976). Dyment, ON, ed. Гликоли и другие производные окисей этилена и пропилена [Glycols and other derivatives of ethylene oxide and propylene]. Khimiya. pp. 214–217.
- Salamone, Joseph C., ed. (1996). Polymeric materials encyclopedia. 8. CRC Press. pp. 6036–6037. ISBN 978-0-8493-2470-3.
- Neufeld L.M.; Blades A.T. (1963). "The Kinetics of the Thermal Reactions of Ethylene Oxide". Canadian Journal of Chemistry. 41 (12): 2956–2961. doi:10.1139/v63-434.
- Lifshitz A.; Ben-Hamou H. (1983). "Thermal reactions of cyclic ethers at high temperatures. 1. Pyrolysis of ethylene oxide behind reflected shocks". The Journal of Physical Chemistry. 87 (10): 1782–1787. doi:10.1021/j100233a026.
- Gilchrist T. (1985). Heterocyclic Chemistry. Pearson Education. pp. 411–412. ISBN 81-317-0793-8.
- Smith, Michael B.; March, Jerry (2007). Advanced organic chemistry. Reactions, Mechanisms and Structure. Wiley-Interscience. ISBN 0-471-72091-7.
- Fieser, L.; Fieser, M. (1979). Reagents for Organic Synthesis. 7. Wiley. p. 545. ISBN 978-0-471-02918-2.
- Sheldon RA (1983). Chemicals from synthesis gas: catalytic reactions of CO and, Volume 2. Springer. p. 193. ISBN 90-277-1489-4.
- Fieser, L.; Fieser, M. (1977). Reagents for Organic Synthesis. 6. Wiley. p. 197. ISBN 978-0-471-25873-5.
- Han, Yuan-Zhang and Viswanathan, Krishnan (13 February 2003) U.S. Patent 20,030,032,845 "Hydroformylation of ethylene oxide"
- Zimakov, P.V.; Dyment, O. H., eds. (1967). "Chapter V. Producing ethylene oxide through ethylene". Ethylene oxide. Khimiya. pp. 155–182.
- Zimakov, P.V.; Dyment, O. H., eds. (1967). "Part II. Synthesis of ethylene oxide. Overview of reactions of formation of ethylene oxide and other α-oxides". Ethylene oxide. Khimiya. pp. 145–153.
- McMurry J. (2008). Organic chemistry (7 ed.). Thomson. p. 661. ISBN 0-495-11258-5.
- Norris, J.F. (1919). "The Manufacture of War Gases in Germany". Journal of Industrial and Engineering Chemistry. 11 (9): 817–829. doi:10.1021/ie50117a002.
- Weissermel K.; Arpe H-J. (2003). Industrial organic chemistry (4 ed.). Weinheim: Wiley-VCH. pp. 145–148. ISBN 978-3-527-30578-0.
- Market Study: Ethylene. Ceresana.com (December 2010). Retrieved on 2017-05-08.
- "Process Economics Program Report 2D". PEP Report. SRI Consulting. February 1985. Retrieved 19 November 2009.
- Yukelson I.I. (1968). The technology of basic organic synthesis. Khimiya. pp. 554–559.
- Eley, D.D.; Pines, H.; Weisz, P.B., eds. (1967). "Catalitic Oxidation of Olefins". Advances in catalysis and related subjects. 17. New York: Academic Press Inc. pp. 156–157.
- Bloch H. P.; Godse A. (2006). Compressors and modern process applications. John Wiley and Sons. pp. 295–296. ISBN 978-0-471-72792-7.
- "Ethylene Oxide/Ethylene Glycol Process". Process Licensing and Engineering. Scientific Design Company. Archived from the original on 16 July 2011. Retrieved 3 October 2009.
- Chauvel A.; Lefebvre G. (1989). Petrochemical processes 2. Major Oxygenated, Chlorinated and Nitrated Derivatives. 2 (2 ed.). Paris: Editions Technip. p. 4. ISBN 2-7108-0563-4.
- Kilty P. A.; Sachtler W. M. H. (1974). "The mechanism of the selective oxidation of ethylene to ethylene oxide". Catalysis Reviews: Science and Engineering. 10: 1–16. doi:10.1080/01614947408079624.
- Lebedev, N.N. Chemistry and technology of basic organic and petrochemical synthesis (4 ed.). Khimiya. pp. 420–424. ISBN 5-7245-0008-6.
- Gunardson H. (1998). Industrial gases in petrochemical processing. New York: Marcel Dekker, Inc. pp. 131–132. ISBN 0-8247-9908-9.
- Chemical Weekly, 26 January 2010
- "Ethylene Oxide". WP Report. SRI Consulting. January 2009. Retrieved 29 September 2009.
- "Ethylene". WP Report. SRI Consulting. January 2009. Retrieved 29 September 2009.
- "Vol. 97. 1,3-Butadiene, Ethylene Oxide and Vinyl Halides (Vinyl Fluoride, Vinyl Chloride and Vinyl Bromide)". IARC Monographs on the Evaluation of Carcinogenic Risks to Humans. Lyon: International Agency for Research on Cancer. 2008. pp. 185–287. ISBN 978-92-832-1297-3.
- Devanney M. T. (April 2007). "Ethylene Oxide". SEH Peport. SRI Consulting. Retrieved 19 November 2009.
- "Overview". Mitsubishi Chemical Corporation. Archived from the original on 25 February 2017. Retrieved 12 October 2009.
- "Shell Chemical LP – Geismar, United States of America". Manufacturing locations. Shell Chemicals. Archived from the original on 18 October 2010. Retrieved 12 October 2009.
- "Shell Nederland Chemie BV – Moerdijk, Netherlands". Manufacturing locations. Shell Chemicals. Archived from the original on 18 October 2010. Retrieved 12 October 2009.
- "Plants/Facilities and Capacity". CNOOC and Shell Petrochemicals Company Limited. Retrieved 12 October 2009.[permanent dead link]
- "Segment Chemicals – Products". BASF. Retrieved 12 October 2009.
- "Ethylene Oxide (EO)". Ineos Oxide. Archived from the original on 8 June 2013. Retrieved 12 October 2009.
- "Ethylene oxide product overview". Ethylene oxide. Shell Chemicals. Archived from the original on 11 December 2012. Retrieved 8 October 2009.
- "Ethylene Oxide (EO) Uses and Market Data". Chemical Intelligence. Chemical Industry News & Intelligence (ICIS.com). Retrieved 8 October 2009.
- Knunyants, I. L., ed. (1988). "Ethylene". Chemical Encyclopedia. 5. "Soviet encyclopedia". pp. 984–985.
- Zoller, Uri; Sosis, Paul, eds. (2008). Handbook of Detergents, Part F: Production. CRC Press. pp. 518–521. ISBN 978-0-8247-0349-3.
- Naqvi, Syed (September 2009). "Process Economics Program Report 2I". PEP Peport. SRI Consulting. Retrieved 20 October 2009.
- OMEGA delivers for ethylene glycol makers, Shell (October 2008).
- McKetta, John J.; Cunningham, William A., eds. (1984). Encyclopedia of chemical processing and design. 20. New York: Marcel Dekker, Inc. pp. 259–260. ISBN 0-8247-2470-4.
- "Technology of ethanolamine". Technology. Himtek Engineering. Archived from the original on 2 March 2005. Retrieved 22 October 2009.
- Chekalin MA, Passet BV, Ioffe BA (1980). The technology of organic dyes and intermediate products: A manual for technical (2 ed.). Khimiya. p. 185.
- NIOSH Workplace Safety and Health Topic. Retrieved 15 October 2012.
- Farn, R. J., ed. (2006). Chemistry and technology of surfactants. Blackwell Publishing. p. 133. ISBN 1-4051-2696-5.
- "Alkoxylation". BUSS LOOP Reactor. Buss ChemTech AG. Archived from the original on 8 March 2012. Retrieved 21 October 2009.
- "The Sohio Acrylonitrile Process". National Historic Chemical Landmarks. American Chemical Society. Archived from the original on 23 February 2013. Retrieved 25 June 2012.
- "184.108.40.206. Oxidative ammonolysis of hydrocarbons". ChemAnalitica.com. 1 April 2009. Retrieved 22 October 2009.
- Andreas, F.; Grabe, K. (1969). Propylenchemie. Akademie-Verlag. pp. 117–118.
- "Ethylene oxide". Chemical Backgrounders Index. The Environment Writer. Archived from the original on 28 August 2006. Retrieved 29 September 2009.
- "Ethylene Oxide Sterilization". Isometrix. Archived from the original on 2 April 2016.
- "3M on EtO sterilizers and EtO sterilization process". Retrieved 21 March 2013.
- "History of Ethylene Oxide". Isometrix. Archived from the original on 2 April 2016.
- "Dr. H.W. Andersen's patent of Ethylene Oxide flexible chamber system." Retrieved 21 March 2013.
- "Andersen Products". Retrieved 21 March 2013.
- "University of Pennsylvania, EtO uses in veterinarian practices". Archived from the original on 9 November 2013. Retrieved 21 March 2013.
- "EPA on EtO regulation" (PDF). Retrieved 21 March 2013.
- Hardy, Periam B.; Gay, Lewis L. and Husler, Edward L. (2 January 1979) U.S. Patent 4,132,170 "Fuel-air type bomb"
- Harris O.; et al. (August 1998). Toxicological Profile for 2-Butoxyethanol and 2-butoxyethanol acetate. US Dept of Health and Human Services.
- Zimakov, P.V.; Dyment, O. H., eds. (1967). "Chapter IV Methods of analysis of ethylene oxide". Ethylene oxide. Khimiya. pp. 128–140.
- "Ethylene oxide". ICSC/International Chemical Safety Cards. Institute of Industrial Safety, Labour Protection and Social Partnership. Archived from the original on 28 December 2005. Retrieved 21 September 2009.
- "Ethylene Oxide". Health and Safety Guide. International Programme on Chemical Safety (IPCS) INCHEM. 1988. Retrieved 23 September 2009.
- "Informational Bulletin NFPA-04N 2009" (PDF). Department of Emergency Services, County of Sonoma. 10 January 2009. Archived from the original (PDF) on 4 August 2009. Retrieved 23 October 2009.
- "Ethylene Oxide Safety Literature" (PDF). Shell Chemicals. Retrieved 23 October 2009.
- "Ethylene Oxide Sterilization". NASPCO. Retrieved 2017-02-10.
- "Ethylene Oxide (ETO): Properties, Mode of Action and Uses". Microbe Online. Retrieved 2017-02-10.
- "Harmful substances. Section 4. Heterocyclic compounds. Triplex heterocyclic compounds". ChemAnalitica.com. 1 April 2009. Retrieved 21 September 2009.
- Collins J. L. "Epoxy compounds". Encyclopedia of the ILO. Institute of Industrial Safety, Labour Protection and Social Partnership. Retrieved 25 September 2009.
- "Vol. 60. Some Industrial Chemicals". IARC Monographs on the Evaluation of Carcinogenic Risks to Humans. Lyon: International Agency for Research on Cancer. 1999. ISBN 978-92-832-1297-3.
- Steenland, K.; Whelan, E.; Deddens, J.; Stayner, L.; Ward, E. (2003). "Ethylene oxide and breast cancer incidence in a cohort study of 7576 women (United States)". Cancer Causes and Control. 14 (6): 531–9. doi:10.1023/A:1024891529592. PMID 12948284.
- Steenland, K; Stayner, L; Deddens, J (2004). "Mortality analyses in a cohort of 18 235 ethylene oxide exposed workers: Follow up extended from 1987 to 1998". Occupational and Environmental Medicine. 61 (1): 2–7. PMC . PMID 14691266.
- Toxicological Profile For Ethylene Oxide. Agency for Toxic Substances and Disease Registry, US Public Health Services
- Simmons, H. Leslie (1997). Building Materials: Dangerous Properties of Products in MasterFormat Divisions 7 and 9. John Wiley & Sons. p. 146. ISBN 978-0-442-02289-1. Codes.
- Carson P.A.; Mumford C.J. (1994). Hazardous Chemicals Handbooks. Oxford: Butterworth-Heinemann Ltd. p. 85. ISBN 0-7506-0278-3.
- Immediately Dangerous To Life or Health (IDLH) Values. Cdc.gov. Retrieved on 2017-05-08.
- Chemicals Regulation Directorate. "Banned and Non-Authorised Pesticides in the United Kingdom". Retrieved 1 December 2009.
- Evaluation of the Inhalation Carcinogenicity of Ethylene Oxide (PDF). US Environmental Protection Agency. 2016.
- Dutia, Pankaj (26 January 2010). "Ethylene Oxide: A Techno-Commercial Profile" (PDF). Chemical Weekly.
- Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. ISBN 1439855110.