The relative formula mass of a compound is calculated by adding together the relative atomic mass values for all the atoms in its formula. Moles are units used to measure substance amount.

Chemists measure the amount of a substance in a unit called ‘the **mole**’. This is a convenient way of counting atoms. It allows chemists to make predictions about the masses of different substances that are involved in reactions.

One mole is the **Avogadro number of particles** (atoms, molecules, ions or electrons) **in a substance**.

One mole of atoms contains 6 x 10^{23} atoms, no matter what element it is. This is a very large number: it is 6 with 23 zeros after it. It is known as the **Avogadro number**.

This number is used in chemistry because if you could count out this many carbon atoms, the total mass of carbon you would have is 12 g. On the other hand, weighing out 12 g of carbon allows you to know how many atoms you have.

One mole of carbon atoms has a mass of exactly 12 g. Because magnesium atoms each have twice the mass of carbon atoms (^{24}Mg compared with ^{12}C), one mole of magnesium has a mass of 24 g. In fact, one mole of any element has a mass in grams that is equal to its **relative atomic mass**. One mole of iron has a mass of **56 g**.

A mole of a molecular compound contains 6 x 10^{23} molecules. It has a **mass that is equal to its** relative formula mass. So a mole of water (H_{2}O) has a mass of 18 g. A mole of carbon dioxide (CO_{2}) has a mass of 44 g. This also works for ionic compounds, so a mole of sodium chloride (NaCl) has a mass of 58.5 g.

This approach can also be used for elements that are made from molecules. For example, oxygen gas O_{2} is **diatomic** (each molecule contains two atoms) so its relative formula mass is 32. One mole of oxygen molecules would therefore have a mass of 32 g. One mole of oxygen **atoms** (if you could ever isolate them) would have a mass of 16 g.