Benzene
Benzene is an organic chemical compound with the molecular formula C6H6. It is the simplest aromatic hydrocarbon.
Contents
Properties
Chemical
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).
The nitration of benzene occurs with a solution of concentrated sulfuric acid and nitric acid.
Physical
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.
Availability
Benzene is available at organic chemical suppliers, but because of its environmental hazards it tends to be somewhat overpriced. In most countries it has been phased out from most products and it's also hard to find as a pure reagent.
Preparation
Benzene can be prepared from the decarboxylation of sodium benzoate with sodium hydroxide, by heating the mixture and condensing the resulting benzene. You can also use calcium oxide and benzoic acid. The decarboxylation method tends to produce biphenyl as well, giving the condensate a reddish color. Distillation will remove any impurities.
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]
CHROMIUM has published a pdf on Sciencemadness library about many methods of synthesizing benzene, gathered from various members.[2]
Projects
- Napalm
- Toluene synthesis
- Chlorobenzene synthesis
- Nitrobenzene synthesis
- Sulfur extraction
Handling
Safety
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.
Storage
Benzene must be stored in closed bottles, away from any source of heat.
Disposal
Benzene can 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.
Benzene can also be burned, but this will give off lots of soot, carbon monoxide, other aromatics and unburnt benzene vapors, unless it's done in a waste incinerator. If you really want to do this, do it outside, away from people.
References
- ↑ http://www.youtube.com/watch?v=JhUxaNesnxs
- ↑ http://www.sciencemadness.org/member_publications/benzene_production.pdf
