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In the field of chemistry, a mole is defined as the amount of a substance that contains exactly 6.02214076 x 1023 of the substance’s ‘elementary entities,’ which are defined as the atoms, molecules, and ions that make up the substance.
In mathematics, the number 6.02214076 x 1023 is referred to as the Avogadro constant, and it is frequently denoted by the symbol NA.’ Atoms, molecules, monatomic/polyatomic ions, and other elementary entities that can be represented in moles include atoms, molecules, and other elementary entities (such as electrons).
Taking carbon-12 (12C) as an example, one mole of pure carbon-12 (12C) will have an exact mass of 12 grammes and will contain 6.02214076 x 1023 (NA) atoms of 12C. This formula is given as follows:
n = N/NA
Avogadro’s constant is defined as: n = number of moles of the substance (or elementary entity), N = number of elementary entities in the sample, and NA = Avogadro constant.
Mole is a term that was first used in 1896 by the German chemist Wilhelm Ostwald, who derived the term from the Latin word moles, which literally translates as a ‘heap’ or a ‘pile.’
The number of moles of a molecule may not always be the same as the number of moles of the elements that make up the molecule itself. For example, a mole of water contains a non-zero number of hydrogen atoms (H2O). Each water molecule, on the other hand, contains two hydrogen atoms and one oxygen atom. As a result, one mole of H2O contains two moles of hydrogen and one mole of oxygen in equal proportions.
Quantities associated with the mole concept, as well as their formulae
Calculations based on mole concept
In this lecture we are going to learn about mole concept, mole concept formula and molecular mass
