This is true for all atoms of carbon-12 in the universe. For example, the atomic mass of carbon-12 is 12В u. The atomic mass is constant for a particular isotopic element. The existence of isotopes is accounted for since it is a bulk property.

GВ mol в€’1 is the standard unit for the molar mass. It has a unit of the unified mass unit (u) or the atomic mass unit (amu). The atomic mass is the sum of the mass of protons, neutrons, and electrons. Table 1: Difference between Atomic Mass and Molar Mass Atomic Mass

The table below describes the differences between the two. But they are two different quantities with a definition. The atomic mass and the molar mass are confused with one another.

It is used to convert the mass of a substance to its mole and vice versa.

Thus, it can vary with a terrestrial location.

It is dependents on percentages of consistents of a sample.

So, it does not vary with the size of a sample.

It is a bulk property, not atomic property, of a substance.

Some of the important points regarding the molar mass are as follows: Figure 1: One mole of sodium chloride NaCl weighs 58.44В g Hence, we have one mole of NaCl measured. So, we measure 58.44В g of NaCl with a weight scale, which is equivalent to one of 58.44В g. But we know 58.44В g of sodium chloride is equivalent to one mole of it. If we have to measure one mole of sodium chloride, there is no instrument that can directly measures it. The molar mass of sodium chloride is known it is 58.44В gВ mol в€’1. Let me make it more clear with an example of sodium chloride. Thus, by knowing the molar mass, we can determine the number of moles contained in a given mass of a sample.

The molar mass links the mass of a substance to its moles. Although there is no direct way to measure the number of moles of any substance, the number of moles can be calculated by knowing the molar mass of the substance. Calculations often include quantities like molarity, molality, mole fraction, molar volume. In chemistry, calculations are related to chemical reactions and stoichiometry. When we say the molar mass of carbon is 12.0В gВ mol в€’1, it means one mole of carbon weighs 12.01В g. Thus, one mole of carbon contains 6.022В Г—В 10 23 atoms of carbon. This number (aka AvogadroвЂ™s constant) is mostly approximated to 6.022В Г—В 10 23. We know that one mole of a substance consists of 6.022вЂЇ140вЂЇ76В Г—В 10 23 elementary particles. The SI unit is kgВ mol в€’1, however, it is very uncommon. In other words, it is the mass per mole of a substance. The molar mass of a given substance is defined as the mass of a sample divided by the moles of that substance in the sample. It measures the mass of a mole of a given substance. In chemistry, the molar mass is an important quantity.

Helium molar mass