1 mole is equal to avogadro number of molecules
Mole ConceptTerm mole was suggested by Ostwald (Latin word mole = heap)A mole is defined as the amount of substance which contains same number of elementary particles (atoms, molecules or ions) as the number of atoms present in 12 g of carbon (C-12).1 mol = 6.023 * 1023\xa0atoms = one gram-atom = gram atomic mass1 mol = 6.023 * 1023\xa0molecules = gram molecular massIn gaseous state at STP (T = 273 K, p = 1 atm)Gram molecular mass = 1 mol= 22.4 L = 6.022 * 1023\xa0molecules

The mole is the unit of measurement for amount of substance in the International System of Units
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Mole ConceptTerm mole was suggested by Ostwald (Latin word mole = heap)A mole is defined as the amount of substance which contains same number of elementary particles (atoms, molecules or ions) as the number of atoms present in 12 g of carbon (C-12).1 mol = 6.023 * 1023\xa0atoms = one gram-atom = gram atomic mass1 mol = 6.023 * 1023\xa0molecules = gram molecular massIn gaseous state at STP (T = 273 K, p = 1 atm)Gram molecular mass = 1 mol= 22.4 L = 6.022 * 1023\xa0moleculesStandard number 6.023x 1023\xa0is called Avogadro number in honour of Avogadro (he did not give this number) and is denoted by NA.The volume occupied by one mole molecules of a gaseous substance is called molar volume or gram molecular volume.Number of moles = amount of substance (in gram) / molar mass

The mole is the unit of amount in chemistry. A mole of a substance is defined as: The mass of substance containing the same number of fundamental units as there are atoms in exactly 12.000 g of 12C. Fundamental units may be atoms, molecules, or formula units, depending on the substance concerned.

Given mass / atomic mass
Counting unit for atoms molecules or ions a