The molar mass of an element is indeed equal to the product of Avogadro's number (6.022 × 10^23) and the atomic mass of the element. However, it is important to note that the atomic mass of an element is typically given in atomic mass units (u) or Daltons (Da), while the molar mass is expressed in grams per mole (g/mol).
The atomic mass of an element represents the average mass of the naturally occurring isotopes of that element, taking into account their relative abundances. Atomic mass units (u) are defined based on the carbon-12 isotope, which is assigned a mass of exactly 12 atomic mass units.
On the other hand, the molar mass of an element is the mass of one mole of that element. One mole of any substance contains Avogadro's number of particles (6.022 × 10^23). Therefore, when you multiply the atomic mass (in atomic mass units) by Avogadro's number, the units cancel out, resulting in the molar mass expressed in grams per mole.
For example, let's consider carbon. The atomic mass of carbon is approximately 12.01 atomic mass units. When we multiply this value by Avogadro's number (6.022 × 10^23), the units cancel out, and we obtain the molar mass of carbon, which is approximately 12.01 grams per mole.
So, the atomic mass and the molar mass of an element have the same numerical value when expressed in different units, but they represent different concepts. The atomic mass refers to the mass of individual atoms, while the molar mass represents the mass of one mole of a substance.