Ethylene - C2H4

What is Ethylene?

Ethylene is an unsaturated organic compound with the chemical formula C2H4. It has one double bond and is the simplest member of the alkene class of hydrocarbons.

C2H4 is a simplest alkene with chemical name Ethylene. It is also called Ethene or Polyethylene or Etileno. It is widely used as a plant hormone, as a refrigerant, and as a food additive.

Polyethylene is a colorless gas which has a sweet odor and taste. It is flammable and lighter when compared to air. When exposed to heat or fire for a long duration, the containers can explode.

Properties of Ethylene – C2H4

C2H4 Ethylene
Molecular weight of C2H4 28.054 g/mol
Density of Ethylene 1.178 kg/m3
Boiling point of Ethylene −103.7 °C
Melting point of Ethylene −169.2 °C

Ethylene structure – C2H4

Structure of Ethylene

C2H4 Uses (Ethylene)

  • Ethylene is used in the manufacturing of alcohol.
  • Used in the manufacturing of polystyrene.
  • Used in promoting senescence.
  • Used to produce fabricated plastics.
  • Used as an herbicide.
  • Used as a curing agent for tobacco.
  • Used as a refrigerant.
  • Used as an anesthetic.
  • Used to accelerate the ripening of fruits commercially.
  • Used in welding metals.

Production of Ethylene

During the year 2013 Etileno was produced by approximately 117 companies from 32 countries.

Petrochemical industry – A predominant method of producing ethylene is by steam cracking. Hydrocarbons along with steam are heated to a temperature range of 750–950 °C. It converts large hydrocarbons into smaller hydrocarbons and initiates unsaturation. When feedstock is ethane then the product is ethylene. Polyethylene is separated from the obtained mixture mixture by repetitive compression and process of distillation. Other methods to produce ethylene include, Fischer-Tropsch synthesis, catalytic dehydrogenation, oxidative coupling of methane, and methanol-to-olefins (MTO).

Laboratory method – It is rarely prepared in the laboratories and is usually purchased. It can be synthesized by dehydrating ethanol with H2SO4 (sulfuric acid) or with aluminium oxide in the gas phase.

Health Hazards

Average concentration in air can cause drowsiness, unconsciousness, and dizziness. Overexposure may lead to headache, muscular weakness, and drowsiness. Also, the vapours of this compound can cause asphyxiation. When ethylene is touched in its liquid form, it causes burns, and severe injury. On heating, the fire liberates irritating and toxic gases.

FAQs

1. Who discovered ethylene?
A Russian scientist named Dimitry Neljubow demonstrated in 1901, that the active component was ethylene. Doubt discovered that in 1917 ethylene spurred abscission. Not until 1934 did Gane announce the plants synthesize ethylene

2. How is ethylene produced?
Ethylene is commercially developed by the steam cracking of a wide range of hydrocarbon feedstocks. Processes of olefin cracking and inter conversion are being built to improve efficiency of light olephins. They will usually transform C4-C8 olephins and light gasoline pyrolysis into ethylene and propylene.

3. Is ethylene heavier than air?
Ethylene has the appearance of a colorless gas with a light smell and taste. It is lighter than atmosphere.

4. Is ethylene polar or nonpolar?
Ethylene is a substance of a nonpolar nature. This is because they have an equal distribution of electrical charges, unlike a polar molecule.

5. What are the functions of ethylene?
In plants, ethylene acts as a hormone. It functions at trace rates during the plant’s life by stimulating or controlling fruit maturation, flowers opening and leaves abscission (or shedding).

Learn more about the Structure, physical and chemical properties of C2H4 from the experts at BYJU’S.

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