Alkenes are used for artificial ripening of fruits, as a general anesthetic, for making poisonous mustard gas (War gas) and ethylene-oxygen flame.
1. Making plastics by polymerisation
2. Making ethylene glycol
3. Making industrial ethanol and further oxidation to ethanoic acid
4. Making Halogenoalkanes important industrial solvents
5. catalytic reforming to form benzene and other aryl compounds
From alkenes
In hydrohalogenation, an alkene reacts with a dry hydrogen halide (HX) like hydrogen chloride (HCl) or hydrogen bromide (HBr) to form a haloalkane. The double bond of the alkene is replaced by two new bonds, one with the halogen and one with the hydrogen atom of the hydrohalic acid. Markovnikov's rule states that in this reaction, the halogen is more likely to become attached to the more substituted carbon. This is a electrophilic addition reaction. Water must be absent otherwise there will be a side product(water). The reaction is necessarily to be carried out in a dry inert solvent such as CCl4 or directly in the gaseous phase.
Alkenes also react with halogens (X2) to form haloalkanes with two neighboring halogen atoms in a halogen addition reaction. This is sometimes known as "decolorizing" the halogen, since the reagent X2 is colored and the product is usually colorless.
Ethylene glycol is produced from ethylene, via the intermediate ethylene oxide. Ethylene oxide reacts with water to produce ethylene glycol according to the chemical equation
C2H4O + H2O → HOCH2CH2OH
This reaction can be catalyzed by either acids or bases, or can occur at neutral pH under elevated temperatures. The highest yields of ethylene glycol occur at acidic or neutral pH with a large excess of water. Under these conditions, ethylene glycol yields of 90% can be achieved. The major byproducts are the ethylene glycol oligomers diethylene glycol, triethylene glycol, and tetraethylene glycol.
Ethanol for use as industrial feedstock is most often made from petrochemical feed stocks, typically by the acid-catalyzed hydration of ethylene, represented by the chemical equation
C2H4(g) + H2O(g) → CH3CH2OH(l).
The catalyst is most commonly phosphoric acid,[17] adsorbed onto a porous support such as diatomaceous earth or charcoal. This catalyst was first used for large-scale ethanol production by the Shell Oil Company in 1947.[18] The reaction is carried out with an excess of high pressure steam at 300°C.
2. Alkenes are compounds containing a Carbon-Carbon double bond. This gives them the ability to undergo addition polymerisation to form polymers (plastics). The simplest example of this is the polymerisation of ethene (also known as ethylene) monomers (H2C=CH2) by breaking their double bonds and forming single bonds between them, resulting in polyethene, more commonly known as polythene, a long repeated chain of -CH2-. There are a huge variety of polymers formed from alkenes in this way. Alkenes are also an important starting material in organic synthesis as they are able to undergo a large variety of addition reactions across the double bond, forming products such as halogenoalkanes, alcohols or amines.
Alkenes are used for artificial ripening of fruits, as a general anesthetic, for making poisonous mustard gas (War gas) and ethylene-oxygen flame.
1. Making plastics by polymerisation
2. Making ethylene glycol
3. Making industrial ethanol and further oxidation to ethanoic acid
4. Making Halogenoalkanes important industrial solvents
5. catalytic reforming to form benzene and other aryl compounds
From alkenes
In hydrohalogenation, an alkene reacts with a dry hydrogen halide (HX) like hydrogen chloride (HCl) or hydrogen bromide (HBr) to form a haloalkane. The double bond of the alkene is replaced by two new bonds, one with the halogen and one with the hydrogen atom of the hydrohalic acid. Markovnikov's rule states that in this reaction, the halogen is more likely to become attached to the more substituted carbon. This is a electrophilic addition reaction. Water must be absent otherwise there will be a side product(water). The reaction is necessarily to be carried out in a dry inert solvent such as CCl4 or directly in the gaseous phase.
Alkenes also react with halogens (X2) to form haloalkanes with two neighboring halogen atoms in a halogen addition reaction. This is sometimes known as "decolorizing" the halogen, since the reagent X2 is colored and the product is usually colorless.
Ethylene glycol is produced from ethylene, via the intermediate ethylene oxide. Ethylene oxide reacts with water to produce ethylene glycol according to the chemical equation
C2H4O + H2O → HOCH2CH2OH
This reaction can be catalyzed by either acids or bases, or can occur at neutral pH under elevated temperatures. The highest yields of ethylene glycol occur at acidic or neutral pH with a large excess of water. Under these conditions, ethylene glycol yields of 90% can be achieved. The major byproducts are the ethylene glycol oligomers diethylene glycol, triethylene glycol, and tetraethylene glycol.
Ethanol for use as industrial feedstock is most often made from petrochemical feed stocks, typically by the acid-catalyzed hydration of ethylene, represented by the chemical equation
C2H4(g) + H2O(g) → CH3CH2OH(l).
The catalyst is most commonly phosphoric acid,[17] adsorbed onto a porous support such as diatomaceous earth or charcoal. This catalyst was first used for large-scale ethanol production by the Shell Oil Company in 1947.[18] The reaction is carried out with an excess of high pressure steam at 300°C.
2. Alkenes are compounds containing a Carbon-Carbon double bond. This gives them the ability to undergo addition polymerisation to form polymers (plastics). The simplest example of this is the polymerisation of ethene (also known as ethylene) monomers (H2C=CH2) by breaking their double bonds and forming single bonds between them, resulting in polyethene, more commonly known as polythene, a long repeated chain of -CH2-. There are a huge variety of polymers formed from alkenes in this way. Alkenes are also an important starting material in organic synthesis as they are able to undergo a large variety of addition reactions across the double bond, forming products such as halogenoalkanes, alcohols or amines.
they can be used in manufactures to make plastic.
Pt and Pd can be used as catalyst in the hydrogenation of alkenes or (de)hydrogenation of hydrocarbons (cracking in petrol industry)
Zoe alkenes found alkenes
Alkenes are very important as: 1. They are used in the manufacture of polythene, Mustard gas(beta-beta dichloro ethyl sulphide) 2. Ethene, one of the alkenes, is used as a general anaesthetic and for artificial ripening of fruits. 3. Alkenes are used as a starting material for a large number of chemicals of industrial use such as glycols(antifreeze) , ethyl halide and ethyl alcohol.
A carbon-carbon double bond.
alkenes
Pt and Pd can be used as catalyst in the hydrogenation of alkenes or (de)hydrogenation of hydrocarbons (cracking in petrol industry)
alkenes are used to make polycarbonates such as polyethene which is used in making rope, plastics, etc.
Since alcohols are obtained by hydration of alkenes, it is meaningless to manufacture alkenes from alkanes. Moreover, cracking hydrocarbons is a more effective and economical to make alkenes. Shawkat
Zoe alkenes found alkenes
Petrochemical Industries
Alkenes are very important as: 1. They are used in the manufacture of polythene, Mustard gas(beta-beta dichloro ethyl sulphide) 2. Ethene, one of the alkenes, is used as a general anaesthetic and for artificial ripening of fruits. 3. Alkenes are used as a starting material for a large number of chemicals of industrial use such as glycols(antifreeze) , ethyl halide and ethyl alcohol.
True
No. The lower alkenes are gases. As the number of carbon atom increases, liquid and solid alkenes are known.
Smaller alkanes and alkenes
Yes, Alkenes are used for fuels - as they are one of our organic compounds in society. For example, fuel can be used for cooking and petrol.
they contain unreactive atoms
Alkenes are defined as any of the series of unsaturated hydrocarbons containing a double bond, including ethylene and propylene. Disadvantages include that many alkenes are insoluble in aqueous acid and side reactions are possible.