There are so many uses of carbon in industries. We can conclude that, carbon are very important to our industries. Here, we attached some application of carbon.Thursday, 9 May 2013
Application of Carbon in Industries
There are so many uses of carbon in industries. We can conclude that, carbon are very important to our industries. Here, we attached some application of carbon.
Application of Carbon In Daily Life
There are so many thing that applied carbon in our daily life. The most closure to us is pencil. Carbon is used in pencil lead.
If you are wearing a diamond ring that is also carbon.
Also graphite powder is used as a lubricant.
Carbon as a semiconducting material is used in electrical resistors, and spark plug wires. Carbon is added (in specific quantities) to steel to give it a desired hardness.
- Carbon is used as a base for the ink in inkjet printers.
- Carbon, in the form of carbon dioxide, is used in the manufacture of many fizzy and carbonated drinks. It is also used in fire extinguishers.
- Dry ice, which is the solid form of carbon dioxide, is used as a cooling agent.
- Freon, is used in cooling systems and devices like refrigerators and air conditioners.
- Carbon is also used to manufacture many heat resistant devices and tools and metal cutters.
- It is used as a decorative tool in many jewelry items.
- Carbon monoxide, extracted through metallurgical process, is used as a reducing agent to obtain many elements and compounds.
- Vegetal carbon, which is an amorphous form of carbon, is utilized as a bleaching agent and a gas absorbent.
- Carbon is used in the rim of automobiles as a black fume pigment.
- Calcium carbide is used as a welding agent for cutting metals, in the preparation of acetylene and other organic compounds.
Overall Notes
Here are few notes of overall chapter Carbon Compound provided for your references. We are glad to help you my dear students.
Wednesday, 8 May 2013
10 CARBON FACTS
Carbon - The Chemical Basis for Life
By Anne Marie Helmenstine, Ph.D.,
1. Carbon is the basis for organic chemistry, as it occurs in all living organisms.
2. Carbon is a nonmetal that can bond with itself and many other chemical elements, forming nearly ten million compounds.
3. Elemental carbon can take the form of one of the hardest substances (diamond) or one of the softest (graphite).
4. Carbon is made in the interiors of stars, though it was not produced in the Big Bang.
5. Carbon compounds have limitless uses. In its elemental form, diamond is a gemstone and used for drilling/cutting; graphite is used in pencils, as a lubricant, and to protect against rust; while charcoal is used to remove toxins, tastes, and odors. The isotope Carbon-14 is used in radiocarbon dating.
6. Carbon has the highest melting/sublimation point of the elements. The melting point of diamond is ~3550°C, with the sublimation point of carbon around 3800°C.
7. Pure carbon exists free in nature and has been known since prehistoric time.
8. The origin of the name 'carbon' comes from the Latin word carbo, for charcoal. The German and French words for charoal are similar.
9. Pure carbon is considered non-toxic, although inhalation of fine particles, such as soot, can damage lung tissue.
10. Carbon is the fourth most abundant element in the universe (hydrogen, helium, and oxygen are found in higher amounts, by mass).
CARBOXYLIC ACIDS
1. Carboxylic acids are organic compounds which form an homologous series with the general
formula of CnH2n+1COOH.
2. Carboxylic acids are compounds which contain a -COOH functional group.
3. Carboxylic acids are weak acid which ionize partially in water to produce lower concentration of
hydrogen ions compare to strong acid. Ethanoic acid turns moist blue litmus paper red.
CH3COOH <–> CH3COO- + H+
4. Physical properties of carboxylic acid
| Name | Molecularformula | Boiling point (°C) |
| Methanoic acid(Formic acid) | HCOOH | 101 |
| Ethanoic acid(Acetic acid) | CH3COOH | 118 |
| Propanoic acid | C2H5COOH | 141 |
| Butanoic acid | C3H7COH | 164 |
- Solubility in water – generally in carboxylic acid (the less than four carbon atoms) are very soluble in water and ionise partially to form weak .
- Density of carboxylic acid – density of carboxylic acid increases due to the increases in the number of carbon atoms in a molecule.
- Boiling points – all carboxylic acid in general have relatively high boiling points than the corresponding alkanes. This is due to the presence of carboxyl group in carboxylic acid.
- Smell – carboxylic acid (< 10 carbon) are colourless and pungent smell. Carboxylic acid (>10 carbons) are wax-like solids.
| Formula | Common Name | Source | IUPAC Name | ||
|---|---|---|---|---|---|
| HCO2H | formic acid | ants (L. formica) | methanoic acid | ||
| CH3CO2H | acetic acid | vinegar (L. acetum) | ethanoic acid | ||
| CH3CH2CO2H | propionic acid | milk (Gk. protus prion) | propanoic acid | ||
| CH3(CH2)2CO2H | butyric acid | butter (L. butyrum) | butanoic acid | ||
| CH3(CH2)3CO2H | valeric acid | valerian root | pentanoic acid | ||
| CH3(CH2)4CO2H | caproic acid | goats (L. caper) | hexanoic acid | ||
| CH3(CH2)5CO2H | enanthic acid | vines (Gk. oenanthe) | heptanoic acid | ||
| CH3(CH2)6CO2H | caprylic acid | goats (L. caper) | octanoic acid | ||
| CH3(CH2)7CO2H | pelargonic acid | pelargonium (an herb) | nonanoic acid | ||
| CH3(CH2)8CO2H | capric acid | goats (L. caper) | decanoic a |
5. Preparation of carboxylic acid
Oxidation of an alcohol
-
The oxidation of ethanol is used to prepare ethanoic acid.
C2H5OH + 2[O] –> CH3COOH + H2O
Carried out by refluxing* ethanol with an oxidising agent
[acidified potassium dichromate(VI) solution – orange colour turns to green /
acidified potassium manganate(VII) solution – purple colour turns to colourless]
6. Chemical properties of carboxylic acid
- Reaction with metals
- Ethanoic acid reacts with reactive metals (copper and metals below it in the reactivity series cannot react with ethanoic acid).
- (K, Na, Mg, Al, Zn, Fe, Sn, Pb, Cu, Hg, Au)
- Reaction with bases acid neutralises alkalis (sodium hydroxide).
CH3COOH + NaOH –> CH3COONa + H2O
In this reaction, a salt (sodium ethanoate) and water are formed.
- Reaction with carbonates
Ethanoic acid reacts with metal carbonates (calcium carbonate, magnesium carbonate, zinc carbonate).
2CH3COOH + CaCO3 –> Ca(CH3COO)2 + CO2 + H2O
In this reaction, a salt (calcium ethanoate), carbon dioxide and water are formed.
- Reaction with alcohols (Esterification)
Ethanoic acid reacts with alcohol (ethanol, propanol, butanol)
CH3CO-OH + H-OC4H9 –> CH3COOC4H9 + H2O (Concentrated H2SO4 is a catalyst)
In this reaction, an ester (colourless sweet-smelling liquid) (butyl ethanoate) and water are formed.
7. Uses of Carboxylic Acid
 |
| soap |
 |
| vinegar |
| aspirin |
| coagulant |
 |
| dye |
ALCOHOL
1. General formula: CnH2n + 1OH
- Where n = 1, 2, 3 … (n = number of carbon)
hydroxyl functional group (-O H) is
bound to a carbon atom. In particular, this carbon
center should be saturated, having
single bonds to three other atoms.
3. The functional group in alcohols is hydroxyl group, – OH.
| Name of alcohol | Molecular formula of alcohol |
| Methanol | CH3OH |
| Ethanol | C2H5OH |
| Propanol / Propan-1-ol | C3H7OH |
| Butanol / Butan-1-ol | C4H9OH |
| Pentanol / Pentan-1-ol | C5H11OH |
| Hexanol / Hexan-1-ol | C6H13OH |
| Heptanol / Heptan-1-ol | C7H15OH |
| Octanol / Octan-1-ol | C8H17OH |
| Nonanol / Nonan-1-ol | C9H19OH |
| Decanol / Decan-1-ol | C10H21OH |
4. Physical properties of alcohol
| Name | Molecular formula | Melting point (°C) | Boiling point (°C) | Physical state at 25°C |
| Methanol | CH3OH | -97 | 65 | Liquid |
| Ethanol | C2H3OH | -117 | 78 | Liquid |
| Propanol | C3H5OH | -127 | 97 | Liquid |
| Butanol | C4H7OH | -90 | 118 | Liquid |
| Pentanol | C5H9OH | -79 | 138 | Liquid |
- Solubility in water – all members in alcohol are very soluble in water (miscible with water).
- Volatility – all alcohols are highly volatile.
- Colour and Smell – alcohols are colourless liquid and have sharp smell.
- Boiling and melting points – all alcohols in general have low boiling points (78°C).
- Combustion of alcohol
C2H5OH + 3O2 –> 2CO2 + 3H2O
(Alcohol burns with clean blue flames. Alcohol burns plenty of oxygen to produce
carbon dioxide and water. This reaction releases a lot of heat. Therefore, it is a clean
fuel as it does not pollute the air.)
- Oxidation of ethanol
Two common oxidising agents are used for the oxidation of ethanol.
1. Acidified potassium dichromate(VI) solution (orange to green)
2. Acidified potassium manganate(VII) solution (purple to colourless).
C2H5OH + 2[O] –> CH3COOH + H2O
- Removal of water (Dehydration)
It results in the formation of a C=C double bond.
CnH2n+1OH –> CnH2n + H2O C2H5OH –> C2H4 + H2O
Two methods are being used to carry out a dehydration in the laboratory.
a) Ethanol vapour is passed over a heated catalyst such as aluminium oxide, unglazed
porcelain chips, pumice stone or porous pot.
b) Ethanol is heated under reflux at 180°C with excess concentrated sulphuric acid,
H2SO4.
C3H7OH –> C3H6 + H2O
6. Uses of Alcohol
- Alcohol as a solvent (cosmetics, toiletries, thinners, varnishes, perfumes).
 |
| cosmetic |
- Alcohol as a fuel (fuel for racing car, clean fuel, alternative fuel).
 |
| clean fuel |
| vinegar |
- Alcohol as a source of chemicals (polymer, explosives, vinegar, fiber).
 |
| Mouth wash |
- Alcohol as a source of medical product (antiseptics for skin disinfection, rubbing alcohol).
Manufacture of Ethanol (Hydration)
Ethanol is manufactured by reacting ethene with steam. The reaction is reversible, and the formation of the ethanol is exothermic.
An experiment can be done in laboratory to obtained ethene.
 |
| Method to Obtain Ethene |
ISOMERISME
ISOMERISM
Existence of different compounds with the same molecular formula but different structural formular. Depend to branching of carbon and location of functional group.
ISOMERS
Different compounds that have same molecular formula
There are two types of isomers;
1. Chain Isomer -
different arrangement in carbon atoms leading to linear and branched chain
different arrangement in carbon atoms leading to linear and branched chain
2. Positional Isomer -
the basic carbon skeleton remains unchanged, but the functional groups are moved around on that skeleton.
Isomerism in alkanes
Isomerism in alkenes
the basic carbon skeleton remains unchanged, but the functional groups are moved around on that skeleton.
Isomerism in alkanes
| Molecular formula | Number of isomers | Structure name |
| CH4 | (no isomer) | Methane |
| C2H6 | (no isomer) | Ethane |
| C3H8 | (no isomer) | Propane |
| C4H10 | 2 | Butane 2-methylpropane |
| C5H12 | 3 |
Pentane
2-methylbutane
2,2-dimethylpropane
|
Isomerism in alkenes
| Molecular formula | Number of isomers | Structure name |
| C2H4 | (no isomer) | Ethene |
| C3H6 | (no isomer) | Propene |
C4H8
|
3
|
But-1-ene
But-2-ene
2-methylpropene
|
C5H10
|
5
|
Pent-1-ene
Pent-2-ene
2-methylbut-1-ene
3-methylbut-1-ene
2-methylbut-2-ene
|
FUNCTIONAL GROUP
Functional groups are groups of atoms found within molecules that are involved in the chemical reactions characteristic of those molecules
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