One gram contains approximately 6.022 x 1023 atomic mass units (amu). This value derives from Avogadro’s number, which indicates the number of atoms in a mole of a given substance. Since one mole of atoms is defined to have a mass equal to its atomic or molecular weight in grams, the relationship between grams and atomic mass units becomes clear.
To further illustrate, let’s break it down:
- The atomic mass unit is defined as one twelfth of the mass of a carbon-12 atom.
- One mole of any substance has a mass in grams equal to its molecular weight in amu.
- Thus, if you have one gram of a substance, you essentially have a collection of atoms that, when combined, correspond to about 6.022 x 1023 atoms, and each of these contributes to the overall atomic mass measured in amu.
In summary, the conversion between grams and atomic mass units is anchored in the concept of the mole, making it a fundamental component of chemistry.