Molar mass can be measured by a number of experimental methods, many of which will be introduced later. Molecular formulas are derived by comparing the compound’s molecular or molar mass to its empirical formula mass. As the name suggests, an empirical formula mass is the sum of the average atomic masses of all the atoms represented in an
Relative atomic mass/ atomic weight is the ratio between the atomic mass of an atom and 1/12th of the atomic mass of a C-12 atom and similarly, relative molecular mass/molecular weight is the ratio of the molecular mass of a molecule and 1/12th of the atomic mass of a C-12 atom. Both R.A.M. and R.M.M are unitless since they are the ratio of two
Find the molar mass of each element using the periodic table of elements. Make sure that you count the atoms for each element and calculate the molar mass of each of the atoms. Example problem: Molar mass of K = 39.1 g; Molar mass of Mn = 54.9 g; Molar mass of O = 16.0 g (The solute contains 4 O atoms, so count the 16g 4 times.) .