Relative atomic mass, also known as atomic weight, is a dimensionless quantity that represents the average mass of an atom of an element relative to 1/12th the mass of a carbon-12 atom. It is a weighted average of the masses of all the naturally occurring isotopes of an element, taking into account their abundances.
The relative atomic mass is often expressed in atomic mass units (u) or Daltons (Da). One atomic mass unit is defined as 1/12th the mass of a carbon-12 atom. So, a relative atomic mass of 12 u is equivalent to the mass of one carbon-12 atom.
The relationship between relative atomic mass and grams is based on the concept of the mole. The mole is a unit of measurement that allows scientists to count atoms or molecules on a macroscopic scale. One mole of any substance contains Avogadro's number of particles, which is approximately 6.022 × 10^23.
Since relative atomic mass is expressed in atomic mass units, the mass of one mole of atoms in grams is numerically equal to the relative atomic mass. For example, if the relative atomic mass of an element is 56 u, then one mole of that element will have a mass of 56 grams.
This relationship allows scientists to convert between the mass of an element in grams and the number of atoms or molecules using Avogadro's number. It is a fundamental concept in chemistry and is used extensively in calculations involving stoichiometry, molar mass, and chemical equations.