What is a Mole?
- One mole of helium gas is equal to 02×1023atoms.
- One mole of oxygen is equal to has 02×1023 molecules.
- One mole of NaCl has 02×1023Na and 6.02×1023 Cl ions.
How to calculate moles?
![Color by number the mole Color by number the mole](/uploads/1/1/0/2/110257189/665756730.jpg)
FAQs
How many grams are in a mole?
How many molecules in a mole?
How many atoms in a gram?
Are molar mass and molecular mass the same?
References:
- Mole | Definition, Number, & Facts. Encyclopedia Britannica.
- What Is a Mole and Why Is It Used in Chemistry?. ThoughtCo.
- The Mole. Chemistry.bd.psu.edu.
Note: this document will print in an appropriately modified format (6 pages)
Owing to their tiny size, atoms and molecules cannot be counted by direct observation. But much as we do when 'counting' beans in a jar, we can estimate the number of particles in a sample of an element or compound if we have some idea of the volume occupied by each particle and the volume of the container.
Once this has been done, we know the number of formula units (to use the most general term for any combination of atoms we wish to define) in any arbitrary weight of the substance. The number will of course depend both on the formula of the substance and on the weight of the sample. But if we consider a weight of substance that is the same as its formula (molecular) weight expressed in grams, we have only one number to know: Avogadro's number, 6.022141527 × 1023, usually designated by NA.
Avogadro only originated the concept of this number, whose actual value was first estimated by Josef Loschmidt, an Austrian chemistry teacher, in 1895.
You should know it to three significant figures:
NA = 6.02 × 1023
6.02 × 1023 of what? Well, of anything you like: apples, stars in the sky, burritos. But the only practical use for NA is to have a more convenient way of expressing the huge numbers of the tiny particles such as atoms or molecules that we deal with in chemistry. Avogadro's number is a collective number, just like a dozen.
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Before we get into the use of Avogadro's number in problems, take a moment to convince yourself of the reasoning embodied in the following examples.
or 12 × 1.6605 × 10–27 g = 19.9 × 10–27 kg. The mass of the oxygen atom will be 4/3 greater, or 2.66 × 10–26 kg.
4/3 × 12 g = 16.0 g.
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Things to understand about Avogadro's number NA
The Mole Number Of Particles Relationship
Wikipedia has a good discussion of Avogadro's number
The mole (abbreviated mol) is the the SI measure of quantity of a 'chemical entity', which can be an atom, molecule, formula unit, electron or photon. One mol of anything is just Avogadro's number of that something. Or, if you think like a lawyer, you might prefer the official SI definition: