General Chemistry/Formulas and Numbers
Calculating Formula Masses[edit | edit source]
The calculation of a compound's formula mass (the mass of its molecule or formula unit) is straightforward. Simply add the individual mass of each atom in the compound (found on the periodic table). For example, the formula mass of glucose (C6H12O6) is 180 amu.
Molar masses are just as easy to calculate. The molar mass is equal to the formula mass, except that the unit is grams per mole instead of amu.
Calculating Percentage Composition[edit | edit source]
Percentage composition is the relative mass of one substance in a compound compared to the whole. For example, in methane (CH4), the percentage mass of hydrogen is 25% because hydrogen makes up a total of 4 amu out of 16 amu overall.
Using Percentage Composition[edit | edit source]
Percentage composition can be used to find the empirical formula of a compound, which shows the ratios of elements in the compound. However, this is not the same as the molecular formula. For example, many sugars have the empirical formula CH2O, which could correspond to a molecular formula of CH2O, C2H4O2, C6H12O6, etc.
For example, a compound is composed of 75% carbon and 25% hydrogen by mass. Find the empirical formula.
- 75g C / (12 g/mol C) = 6.25 mol C
- 25g H / (1 g/mol H) = 25 mol H
- 6.25 mol C / 6.25 = 1 mol C
- 25 mol H / 6.25 = 4 mol H
Thus the empirical formula is CH4.
Calculating Molecular Formula[edit | edit source]
If you find the empirical formula of a compound and its molar/molecular mass, then you can find its exact molecular formula. Remember that the molecular formula is always a whole-number multiple of the empirical formula. For example, a compound with the empirical formula HO has a molecular mass of 34.0 amu. Since HO would only be 17.0 amu, which is half of 34.0, the molecular formula must be H2O2.