1
mol
6.022
x10^23
1
mol
6.022
x10^23
The Mole Calculator converts between mass and moles using the fundamental relationship n = m/M. The mole is the SI unit for the amount of substance, defined as exactly 6.02214076 x 1023 elementary entities (atoms, molecules, ions, etc.). This number, known as Avogadro's number, bridges the macroscopic world of grams and the microscopic world of atoms. The mole concept is arguably the most important quantitative tool in chemistry, essential for stoichiometry, solution preparation, reaction yield calculations, and chemical analysis. Simply enter the mass of your substance and its molar mass (from the periodic table), and the calculator returns the number of moles and the corresponding number of particles.
The mole calculation uses the fundamental equation:
n = m / M
Where:
To find the molar mass, add up the atomic masses of all atoms in the chemical formula. For example:
Once you have the number of moles, multiply by Avogadro's number to get the number of particles:
N = n x NA = n x 6.022 x 1023
The reverse calculation is equally important: if you know the moles needed (from stoichiometry), multiply by molar mass to find the required mass: m = n x M.
One mole of any substance contains exactly 6.022 x 1023 particles and has a mass in grams numerically equal to its molar mass. So 1 mole of water weighs 18.015 g, 1 mole of NaCl weighs 58.44 g, and 1 mole of iron weighs 55.85 g. The output shows both the number of moles and the equivalent number of particles, making it easy to work with either quantity in subsequent calculations.
Inputs
Results
n = 100 / 18.015 = 5.551 mol. Number of molecules = 5.551 x 6.022 x 10^23 = 3.343 x 10^24 = 33.43 x 10^23 molecules of water.
Inputs
Results
n = 10 / 58.44 = 0.1711 mol. Number of formula units = 0.1711 x 6.022 x 10^23 = 1.030 x 10^23 formula units of NaCl.
A mole is the SI unit for amount of substance. It is defined as exactly 6.02214076 x 10^23 elementary entities. One mole of any substance contains this many atoms, molecules, ions, or formula units, depending on the substance.
Add up the atomic masses of all atoms in the chemical formula using values from the periodic table. For example, H2SO4: 2(1.008) + 32.07 + 4(16.00) = 98.08 g/mol. Most periodic tables list atomic masses to 2-4 decimal places.
They are numerically equal but have different units. Molecular weight (or molecular mass) is expressed in atomic mass units (amu or u) and refers to a single molecule. Molar mass is expressed in g/mol and refers to one mole of molecules.
Yes. For ionic compounds like NaCl, use the formula mass (sum of all atomic masses in the formula unit) as the molar mass. The result gives moles of formula units, not individual ions.
The mole allows chemists to count atoms and molecules by weighing them. Since individual atoms are far too small to count, the mole bridges the gap between the atomic scale and the laboratory scale, making stoichiometric calculations possible.
Historically, methods include Millikan's oil drop experiment, X-ray crystallography of silicon crystals, and Brownian motion analysis. Since 2019, Avogadro's number is defined exactly as 6.02214076 x 10^23 mol^-1 as part of the SI unit redefinition.
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