Thus, the formula mass of calcium hydrogen carbonate is 117.10 amu and the molar mass of calcium hydrogen carbonate is 117.10 grams per mole (g/mol). Multiplying the molar mass of each atom by the number of atoms of that type in bilirubin’s formula and adding the results, we get. Our PTE App is the ultimate tool for every friend of chemistry - whether pupil or teacher, student or professor, amateur or expert, hobbyist or technician. Solutions to Example 6.2.2, Summing the molar masses of the atoms in the NaCl formula unit gives. However when talking about a mole of an ionic compound we will still use the term molar mass. Immediately find any imaginable information about an element, calculate molar masses of any compounds you like, facilitate your overview with infographics and much more. This is because there are no individual molecules in ionic compounds. For compounds that are not molecular (ionic compounds), it is improper to use the term “molecular mass” and “ formula mass” is generally substituted. The molar mass of the N 2 molecule is therefore 28.02 g/mol. This is referred to as the molecular mass and the molecular mass of any molecule is simply the sum of the atomic masses of all of the elements in that molecule. For nitrogen, the mass of the N 2 molecule is simply (14.01 + 14.01) = 28.02 amu. For a molecule (for example, nitrogen, N 2) the mass of molecule is the sum of the atomic masses of the two nitrogen atoms.

The concept of molar mass can also be applied to compounds. Further, if you have 16.00 grams of oxygen atoms, you know from the definition of a mole that your sample contains 6.022 x 10 23 oxygen atoms. For example, the atomic mass of an oxygen atom is 16.00 amu that means the molar mass of an oxygen atom is 16.00 g/mol. Generalizing this definition, the molar mass of any substance in grams per mole is numerically equal to the mass of that substance expressed in atomic mass units. By definition, the molar mass of carbon-12 is numerically the same, and is therefore exactly 12 grams. We have defined a mole based on the isotopic atomic mass of carbon-12. The atomic mass of an element is the relative average of all of the naturally occurring isotopes of that element and atomic mass is the number that appears in the periodic table. ) a carbon atom with six proton and six neutrons in its’ nucleus, surrounded by six electrons.

Molar mass table of elements