Mole: Difference between revisions
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A | A mole is a measure of chemical mass which is defined by the unit 6.022x10<sup>23</sup> [[Atom|atoms]] of [[Carbon|carbon]]-12. This value is also known as [http://www.avogadro.co.uk/definitions/avogconst.htm Avagadro's Constant.] | ||
Moles are the units used to measure the concentration of a chemical in a solution. | Moles are the units used to measure the concentration of a chemical in a solution. | ||
A mole, in chemical terms, should not be confused with a small brown furry animal that can dig up your lawn. Nor with Molarity( denoted by M) which is a measure of concentration of a chemical species/substance in moles per unit volume, commonly per litre (Mol/L). | A mole, in chemical terms, should not be confused with a small brown furry animal that can dig up your lawn. Nor with [[Molarity|Molarity]] (denoted by M) which is a measure of concentration of a chemical species/substance in moles per unit volume, commonly per litre (Mol/L). | ||
The numbers of moles in a sample can be calculated as follows: | The numbers of moles in a sample can be calculated as follows: | ||
Number of Moles = Mass of the Sample (g) / Relative Formula (or Atomic) Mass | Number of Moles = Mass of the Sample (g) / Relative Formula (or [[Atomic_mass|Atomic]]) Mass | ||
For example, the mass of 1 mole of sodium chloride (NaCl) is 58.44g. | For example, the mass of 1 mole of sodium chloride (NaCl) is 58.44g. | ||
Latest revision as of 02:31, 12 November 2012
A mole is a measure of chemical mass which is defined by the unit 6.022x1023 atoms of carbon-12. This value is also known as Avagadro's Constant.
Moles are the units used to measure the concentration of a chemical in a solution.
A mole, in chemical terms, should not be confused with a small brown furry animal that can dig up your lawn. Nor with Molarity (denoted by M) which is a measure of concentration of a chemical species/substance in moles per unit volume, commonly per litre (Mol/L).
The numbers of moles in a sample can be calculated as follows:
Number of Moles = Mass of the Sample (g) / Relative Formula (or Atomic) Mass
For example, the mass of 1 mole of sodium chloride (NaCl) is 58.44g.