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Glycerine" and "Glycerin" redirect here. For the Bush song, see Glycerine (song).
Ball-and-stick model of glycerol Space-filling model of glycerol
Sample of glycerine
CAS number 56-81-5 YesY
PubChem 753
ChemSpider 733 YesY
DrugBank DB04077
KEGG D00028 YesY
ChEBI CHEBI:17522 YesY
ATC code A06AG04,A06AX01, QA16QA03
Jmol-3D images Image 1
Molecular formula C3H8O3
Molar mass 92.09 g mol−1
Appearance colorless liquid
Odor odorless
Density 1.261 g/cm3
Melting point 17.8 °C (64.0 °F; 290.9 K)
Boiling point 290 °C (554 °F; 563 K)[2]
Refractive index (nD) 1.4746
Viscosity 1.412 Pa·s[1]
MSDS External MSDS
NFPA 704
Flammability code 1: Must be pre-heated before ignition can occur. Flash point over 93 °C (200 °F). E.g., canola oil Health code 1: Exposure would cause irritation but only minor residual injury. E.g., turpentine Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazards (white): no codeNFPA 704 four-colored diamond
Flash point 160 °C (320 °F; 433 K) (closed cup)
176 °C (349 °F; 449 K) (open cup)
Supplementary data page
Structure and
n, εr, etc.
Phase behaviour
Solid, liquid, gas
Spectral data UV, IR, NMR, MS
Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
YesY (verify) (what is: YesY/N?)
Infobox references

Glycerol (or glycerine, glycerin) is a simple polyol (sugar alcohol) compound. It is a colorless, odorless, viscous liquid that is widely used in pharmaceutical formulations. Glycerol has three hydroxyl groups that are responsible for its solubility in water and its hygroscopic nature. The glycerol backbone is central to all lipids known as triglycerides. Glycerol is sweet-tasting and generally considered non-toxic.

น้ำมันก๊าด (Kerosene)article


From Wikipedia, the free encyclopedia
Jump to: navigation, search
For other uses, see Kerosene (disambiguation).
An Australian kerosene bottle, containing blue-dyed kerosene

Kerosene, also known as lamp oil, is a combustible hydrocarbon liquid widely used as a fuel in industry and households. Its name derives from Greek: κηρός (keros) meaning wax, and was registered as a trademark by Abraham Gesner in 1854 before evolving into a genericized trademar. It is sometimes spelled kerosine in scientific and industrial usage.[1] The term "kerosene" is common in much of India, Canada, the United States, Argentina, Australia and New Zealand.[2][3]

Kerosene is usually called paraffin in the United Kingdom, Southeast Asia, East Africa and South Africa.[4] A more viscous paraffin oil is used as a laxative. A waxy solid extracted from petroleum is called paraffin wax.

Kerosene is widely used to power jet engines of aircraft (jet fuel) and some rocket engines, and is also commonly used as a cooking and lighting fuel and for fire toys such as poi. In parts of Asia, where the price of kerosene is subsidized, it fuels outboard motors on small fishing boats.[5] World total kerosene consumption for all purposes is equivalent to about 1.2 million barrels per day.[6]

To prevent confusion between kerosene and the much more flammable and volatile gasoline, some jurisdictions regulate markings or colorings for containers used to store or dispense kerosene. For example, in the United States, the Commonwealth of Pennsylvania requires that portable containers used at retail service stations be colored blue, as opposed to red (for gasoline) or yellow (for Diesel fuel).[



From Wikipedia, the free encyclopedia
Jump to: navigation, search
IUPAC name
Other names
108-88-3 YesY
Abbreviations PhMe
ChemSpider 1108 YesY
DrugBank DB01900 N
Jmol interactive 3D Image
KEGG C01455 YesY
PubChem 1140
RTECS number XS5250000
Molar mass 92.14 g·mol−1
Appearance Colorless liquid[1]
Odor sweet, pungent, benzene-like[2]
Density 0.87 g/mL (20 °C)[1]
Melting point −95 °C (−139 °F; 178 K)[1]
Boiling point 111 °C (232 °F; 384 K)[1]
0.52 g/L (20 °C)[1]
Vapor pressure 21 mmHg (20°C)[2]
1.497 (20 °C)
Viscosity 0.590 cP (20 °C)
0.36 D
Main hazards highly flammable
Safety data sheet See: data page
R-phrases R11, R38, R48/20, R63, R65, R67
S-phrases (S2), S36/37, S29, S46, S62
NFPA 704
Flammability code 3: Liquids and solids that can be ignited under almost all ambient temperature conditions. Flash point between 23 and 38 °C (73 and 100 °F). E.g., gasoline) Health code 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g., chloroform Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazards (white): no codeNFPA 704 four-colored diamond
Flash point 6 °C (43 °F; 279 K)[1]
Explosive limits 1.1%-7.1%[2]
50 mL m−3, 190 mg m−3
Lethal dose or concentration (LD, LC):
>26700 ppm (rat, 1 hr)
400 ppm (mouse, 24 hr)[3]
55,000 ppm (rabbit, 40 min)[3]
US health exposure limits (NIOSH):
TWA 200 ppm C 300 ppm 500 ppm (10-minute maximum peak)[2]
TWA 100 ppm (375 mg/m3) ST 150 ppm (560 mg/m3)[2]
500 ppm[2]
Related compounds
Related compounds
Supplementary data page
Refractive index (n),
Dielectric constantr), etc.
Phase behaviour
N verify (what is YesYN ?)
Infobox references

Toluene /ˈtɒljn/, formerly known as toluol /ˈtɒljɒl/, is a colorless, water-insoluble liquid with the smell associated with paint thinners. It is a mono-substituted benzene derivative, consisting of a CH3 group attached to a phenyl group. As such, its IUPAC systematic name is methylbenzene. It is an aromatic hydrocarbon.

Toluene is widely used as an industrial feedstock and as a solvent. Like other solvents, toluene is sometimes also used as an inhalant drug for its intoxicating properties; however, inhaling toluene has potential to cause severe neurological harm.[5][6] Toluene is an important organic solvent.[7] Its economic significance is considerable: In 2013, worldwide about 24.5 billion US-dollars were generated with the sale of toluene.[8]




The compound was first isolated in 1837 through a distillation of pine oil by a Polish chemist named Filip Walter, who named it rétinnaphte.[9] In 1841, French chemist Henri Étienne Sainte-Claire Deville isolated a hydrocarbon from balsam of Tolu (an aromatic extract from the tropical Colombian tree Myroxylon balsamum), which Deville recognized as similar to Walter's rétinnaphte and to benzene; hence he called the new hydrocarbon benzoène.[10] In 1843, Jöns Jacob Berzelius recommended the name toluin.[11] In 1850, French chemist Auguste Cahours isolated from a distillate of wood a hydrocarbon which he recognized as similar to Deville's benzoène and which Cahours named toluène.[12]

Chemical properties[edit]

Toluene reacts as a normal aromatic hydrocarbon towards electrophilic aromatic substitution.[13][14][15] Owing to greater electron-releasing properties of the methyl group vs hydrogen, toluene is more reactive than benzene to electrophiles. It undergoes sulfonation to give p-toluenesulfonic acid, and chlorination by Cl2 in the presence of FeCl3 to give ortho and para isomers of chlorotoluene.

Importantly the methyl side chain in toluene is susceptible to oxidation. Potassium permanganate converts toluene to benzoic acid, whereas chromyl chloride leads to benzaldehyde (Étard reaction). The methyl group undergoes halogenation can be performed under free radical conditions. For example, N-bromosuccinimide (NBS) heated with toluene in the presence of AIBN leads to benzyl bromide. The same conversion can be effected with elemental bromine in the presence of UV light or even sunlight. Toluene may also be brominated by treating it with HBr and H2O2 in the presence of light.[16]

C6H5CH3 + Br2 → C6H5CH2Br + HBr
C6H5CH2Br + Br2 → C6H5CHBr2 + HBr

The methyl group in toluene undergoes deprotonation only with very strong bases, its pKa is estimated to be approximately 41.[17] Catalytic hydrogenation of toluene gives methylcyclohexane. The reaction requires a high pressure of hydrogen and a catalyst.


Toluene occurs naturally at low levels in crude oil and is usually produced in the production of gasoline via a catalytic reformer, in an ethylene cracker, or the production of coke from coal. Final separation, either via distillation or solvent extraction, takes place in one of the many available processes for extraction of the BTX aromatics (benzene, toluene, and xylene isomers).

Laboratory preparation[edit]

Toluene is so inexpensively produced industrially that it is not prepared in the laboratory. In principle it could be prepared by a variety of methods. For example, although only of didactical interest, benzene reacts with methyl chloride in presence of a Lewis acid such as aluminium chloride to give toluene:

C6H5H + CH3Cl → C6H5CH3 + HCl

Such reactions are complicated by polymethylation because toluene is more susceptible to alkylation than is benzene.


Toluene is mainly used as a precursor to benzene. The process involves hydrodealkylation:

C6H5CH3 + H2 → C6H6 + CH4

The second ranked application involves its disproportionation to a mixture of benzene and xylene. When oxidized it yields benzaldehyde and benzoic acid, two important intermediates in chemistry.[18]

Precursor to other chemicals[edit]

Aside from being converted to benzene and xylene, toluene is a raw material for toluene diisocyanate (used in the manufacture of polyurethane foam) and TNT. Also an important precursor in the production of synthetic drugs.


Toluene is a common solvent, e.g. for paints, paint thinners, silicone sealants,[19] many chemical reactants, rubber, printing ink, adhesives (glues), lacquers, leather tanners, and disinfectants.


Toluene can be used as an octane booster in gasoline fuels used in internal combustion engines. Toluene at 86% by volume fueled all the turbo Formula One teams in the 1980s, first pioneered by the Honda team. The remaining 14% was a "filler" of n-heptane, to reduce the octane to meet Formula One fuel restrictions. Toluene at 100% can be used as a fuel for both two-stroke and four-stroke engines; however, due to the density of the fuel and other factors, the fuel does not vaporize easily unless preheated to 70 °C (158 °F) (Honda accomplished this in their Formula One cars by routing the fuel lines through the exhaust system to heat the fuel).

In Australia, in 2003, toluene was found to have been illegally combined with petrol in fuel outlets for sale as standard vehicular fuel. Toluene attracts no fuel excise, whereas other fuels are taxed at over 40%, so fuel suppliers are able to profit from substituting the cheaper toluene for petrol. The extent of toluene substitution has not been determined.[20][21]

Toluene is another in a group of fuels that have recently been used as components for jet fuel surrogate blends.[22] Toluene is used as a jet fuel surrogate for its content of aromatic compounds.

Niche applications[edit]

In the laboratory, toluene is used as a solvent for carbon nanomaterials, including nanotubes and fullerenes, and it can also be used as a fullerene indicator. The color of the toluene solution of C60 is bright purple.

Toluene is used as a cement for fine polystyrene kits (by dissolving and then fusing surfaces) as it can be applied very precisely by brush and contains none of the bulk of an adhesive.

Toluene can be used to break open red blood cells in order to extract hemoglobin in biochemistry experiments.

Toluene has also been used as a coolant for its good heat transfer capabilities in sodium cold traps used in nuclear reactor system loops.

Toluene had also been used in the process of removing the cocaine from coca leaves in the production of Coca-Cola syrup.[23]

Toxicology and metabolism[edit]

Main article: Toluene (toxicology)

Inhalation of toluene in low to moderate levels can cause tiredness, confusion, weakness, drunken-type actions, memory loss, nausea, loss of appetite, and hearing and color vision loss. These symptoms usually disappear when exposure is stopped. Inhaling high levels of toluene in a short time may cause light-headedness, nausea, or sleepiness, unconsciousness - and even death.[24][25] Toluene is, however, much less toxic than benzene, and has, as a consequence, largely replaced it as an aromatic solvent in chemical preparation. The EPA considers that there is inadequate information to assess the carcinogenic potential of toluene.[26]

Similar to many other solvents such as 1,1,1-trichloroethane and some alkylbenzenes, toluene has been shown to act as a non-competitive NMDA receptor antagonist and GABAA receptor positive allosteric modulator.[27] Additionally, toluene has been shown to display antidepressant-like effects in rodents in the forced swim test (FST) and the tail suspension test (TST).[27]

It is sometimes used as an inhalant, likely on account of its euphoric and dissociative effects.[27]


Several types of fungi including Cladophialophora, Exophiala, Leptodontium, Pseudeurotium zonatum, and Cladosporium sphaerospermum, and certain species of bacteria can degrade toluene using it as a source of carbon and energy.

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