The relationship between molar mass, average atomic mass, and relative molecular mass is as follows:
Molar Mass: Molar mass is the mass of one mole of a substance and is expressed in grams per mole (g/mol). It is numerically equal to the average atomic mass or relative molecular mass of the substance. For example, the molar mass of carbon (C) is approximately 12.01 g/mol, which is the average atomic mass of carbon.
Average Atomic Mass: The average atomic mass is the weighted average of the masses of all naturally occurring isotopes of an element. It is usually expressed in atomic mass units (amu) or unified atomic mass units (u). The average atomic mass is numerically equal to the molar mass of the element. For example, the average atomic mass of carbon is approximately 12.01 amu, which is the molar mass of carbon.
Relative Molecular Mass: The relative molecular mass, also known as the molecular weight, is the sum of the atomic masses of all the atoms in a molecule. It is calculated by adding up the average atomic masses of all the elements present in the molecule. The relative molecular mass is numerically equal to the molar mass of the compound. For example, the relative molecular mass of water (H2O) is approximately 18.02 g/mol, which is the molar mass of water.
In summary, molar mass, average atomic mass, and relative molecular mass are numerically equal and represent the mass of one mole of a substance, whether it is an element or a compound. The units used to express these masses may differ (grams per mole for molar mass, atomic mass units for average atomic mass, and unified atomic mass units or grams per mole for relative molecular mass), but the numerical values are the same.