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Benzene distilled by NileRed.jpg
Freshly distilled benzene
Benzene structure.png
Structure of benzene
IUPAC name
Preferred IUPAC name
Systematic IUPAC name
Other names
Phenyl hydride
Molar mass 78.11 g/mol
Appearance Colorless liquid
Odor Sweet, aromatic
Density 0.8765(20) g/cm3
Melting point 5.53 °C (41.95 °F; 278.68 K)
Boiling point 80.1 °C (176.2 °F; 353.2 K)
1.53 g/L (0 °C)
1.81 g/L (9 °C)
1.79 g/L (15 °C)
1.84 g/L (30 °C)
2.26 g/L (61 °C)
3.94 g/L (100 °C)
21.7 g/kg (200 °C, 6.5 MPa)
17.8 g/kg (200 °C, 40 MPa)
Solubility Miscible with glacial acetic acid, acetone, carbon disulfide, CCl4, chloroform, diethyl ether, toluene, xylene
Immiscible with cyclohexane, heptane, hexane, pentane
Solubility in diethylene glycol 52 g/100 g (20 °C)
Solubility in ethylene glycol 5.83 g/100 g (20 °C)
6.61 g/100 g (40 °C)
7.61 g/100 g (60 °C)
Vapor pressure 12.7 kPa (25 °C)
24.4 kPa (40 °C)
181 kPa (100 °C)
173.26 J·mol-1·K-1
48.7 kJ/mol
Safety data sheet Sigma-Aldrich
Flash point −11.63 °C (11.07 °F; 261.52 K)
Lethal dose or concentration (LD, LC):
930 mg/kg (rat, oral)
Related compounds
Related compounds
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Benzene is an organic chemical compound with the molecular formula C6H6. It is the simplest aromatic hydrocarbon.



Benzene's aromatic ring is involved in complex reactions. At standard conditions, benzene is not very reactive, but it can react with halogens, alkenes, haloalkenes, organic acid anhydrides in the presence of a Lewis acid, (anhydrous aluminium chloride, iron(III) chloride), process known as Friedel–Crafts reaction.

The nitration of benzene occurs with a solution of concentrated sulfuric acid and nitric acid, giving nitrobenzene.

Benzene is flammable and will burn in air, releasing copious amounts of soot.


Benzene is a colorless and highly flammable liquid with a sweet smell. It is not miscible in water, but it is in many other organic solvents, such as haloalkanes, ethers, ethanol. Benzene will dissolve certain plastic materials, such as polystyrene. It is also a good solvent for sulfur.


Benzene is available at organic chemical suppliers, but because of its environmental hazards it tends to be somewhat overpriced when available. In most countries it has been phased out from most products and it's also hard to find as a pure reagent, as most suppliers will only sell it to companies, especially in most EU countries.


Benzene can be readily prepared from the decarboxylation of sodium benzoate with sodium hydroxide, by heating the mixture and condensing the resulting benzene.

C6H5COONa + NaOH → C6H6 + Na2CO3

The same result can be achieved using calcium oxide and benzoic acid. The decarboxylation method tends to produce biphenyl, biphenylene, benzophenone (which is produced as the major product if the calcium salt is used) and other side products, giving the condensate an orange or orange-reddish color. This can be removed with a simple distillation, giving crystal clear benzene, though some traces of water may still exist.

Benzene can also be produced by the pyrolysis of plastic (usually polyethylene) and sodium hydroxide. This method produces benzene along with other hydrocarbons, so fractional distillation might be required.[1]

Best plastic material however is polyethylene terephtalate (PET), which is readily available. You will first need to hydrolyze it with sodium hydroxide in a high boiling point solvent, such as in ethylene glycol, which gives sodium terephtalate, which can be decarboxylated to benzene using sodium hydroxide. The resulting product is an orange-reddish liquid with lots of basic water, which can be separated by using a separatory funnel, followed by distillation. The yield from this reaction however, is lower than that from sodium benzoate (~15% compared to 45-60%), and plenty of terephtalate can get charred if the temperature is too high. Lots of side products are produced, which may clog the distillation apparatus.[2][3][4]

CHROMIUM has published a pdf on Sciencemadness library about many methods of synthesizing benzene, gathered from various members.[5]




Benzene is a strong carcinogen, so work must be performed in a fume hood or outside. Protection gear is required, as it can penetrate skin. If possible, use toluene or xylene, which are cheaper, safer and more widely available.


Benzene must be stored in glass bottles with a good plastic lid and a clear label with a hazard symbol, away from any open flame sources.


Benzene can be destroyed by burning it, but this will give off lots of soot, carbon monoxide, other aromatics and unburnt benzene vapors, unless it's done in a special waste incinerator. If you really want to neutralize benzene via burning, a good idea would be to dilute it in alcohol first, as the flame will produce less soot. Do it outside, away from people.

Benzene can also be destroyed using Fenton's reagent. If the oxidation is incomplete, phenol and biphenyl will result. If too much benzene is added, the resulting gasses will aerosolize some of the benzene, which is dangerous in an enclosed area, carrying both a fire/explosion hazard as well as inhaling dangerous and carcinogenic benzene fumes. This inconvenience can be reduced by adding the benzene dropwise or bubbling (non-flammable) gas-carried benzene through a gas diffusing stone through the Fenton solution to limit vapor escape. Either perform the neutralization in a fumehood, or outside, preferably the latter. Photochemical neutralization, with the aid of a UV lamp will improve the yield of the oxidation process.




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