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Question

What is a mol, how much is a mol and where did it come from?

Answer 1

The mole (symbol: mol) is the SI base unit that measures an amount of substance. One mole contains Avogadro's number (approximately 6.022×1023) entities. A mole is much like a dozen in that both units can describe any set of elementary objects, although the mole's use is usually limited to measurement of subatomic, atomic, and molecular structures, as a mole represents an exceedingly large number of entities.

Answer 2

The mole (symbol: mol) is the SI base unit that measures an amount of substance. One mole contains Avogadro's number (approximately 6.022×1023) entities. A mole is much like a dozen in that both units can describe any set of elementary objects, although the mole's use is usually limited to measurement of subatomic, atomic, and molecular structures, as a mole represents an exceedingly large number of entities.

Answer 3

The mole (symbol: mol) is the SI base unit that measures an amount of substance. One mole contains Avogadro's number (approximately 6.022×1023) entities. A mole is much like a dozen in that both units can describe any set of elementary objects, although the mole's use is usually limited to measurement of subatomic, atomic, and molecular structures, as a mole represents an exceedingly large number of entities.

A mole is the amount of substance of a system which contains as many elementary entities as there are atoms in 0.012 kilogram of carbon-12, where the carbon-12 atoms are unbound, at rest and in their ground state.[1] The number of atoms in 0.012 kilogram of carbon-12 is known as Avogadro's number, and is determined empirically. The currently accepted value is 6.0221415(10)×1023 mol-1 (2002 CODATA).

According to the SI, the mole is not dimensionless, but has its very own dimensions, namely "amount of substance", comparable to other dimensions such as mass and luminous intensity. (By contrast, the SI specifically defines the radian and the steradian as special names for the dimensionless unit one[1].) The SI additionally defines Avogadro's number as having the unit reciprocal mole, as it is the ratio of a dimensionless quantity and a quantity with the unit mole [2]. However, if in the future the kilogram is redefined in terms of a specific number of carbon-12 atoms (see below), then the value of Avogadro's number will be defined rather than measured, and the mole will cease to be a unit of physical significance.[2

The name mole (German Mol) is attributed to Wilhelm Ostwald who introduced the concept in the year 1902. It is an abbreviation for molecule (German Molekül), which is in turn derived from Latin moles "mass, massive structure". He used it to express the gram molecular weight of a substance. So, for example, 1 mole of hydrochloric acid (HCl) has a mass of 36.5 grams (atomic weights Cl: 35.5 u, H: 1.0 u).

Prior to 1959 both the IUPAP and IUPAC used oxygen to define the mole, the chemists defining the mole as the number of atoms of oxygen which had mass 16 g, the physicists using a similar definition but with the oxygen-16 isotope only. The two organizations agreed in 1959/1960 to define the mole as such:

The mole is the amount of substance of a system which contains as many elementary entities as there are atoms in 0.012 kilogram of carbon-12; its symbol is "mol."
This was adopted by the CIPM (International Committee for Weights and Measures) in 1967, and in 1971 it was adopted by the 14th CGPM (General Conference on Weights and Measures)

In 1980 the CIPM clarified the above definition, defining that the carbon-12 atoms are unbound and in their ground state.

The mole is useful in chemistry because it allows different substances to be measured in a comparable way. Using the same number of moles of two substances, both amounts have the same number of molecules or atoms. The mole makes it easier to interpret chemical equations in practical terms.

Answer 4

To make it a little simpler, a mole of anything is the number of grams of that something equal to its molecular weight.
Ex: 1 mole of oxygen = 32 g because the molecular weight of O2 is 2*16=32.

A side note is that 1 mole of anything will contain 6.02E23 molecules.

Answer 5

I agree with the first answer. 6.022 x 10^23.