Carbon has an atomic mass of 12.0 amu. A carbon sample with a mass of 12.0 g contains 6.02 × 1023 of carbon.

The statement you provided is not a question, but it seems to be leading towards a discussion about Avogadro's number and the concept of a mole in chemistry.

Avogadro's number (6.02 x 10^23) is the number of atoms in one mole of any substance. In this case, it's being applied to carbon.

The atomic mass unit (amu) is a standard unit of mass that quantifies mass on an atomic or molecular scale. The atomic mass of carbon is 12.0 amu.

The statement says that a 12.0 g sample of carbon contains 6.02 x 10^23 atoms of carbon. This is because the molar mass of carbon (12.0 g/mole) is numerically equal to carbon's atomic mass (12.0 amu), and one mole of any substance contains Avogadro's number of atoms or molecules (6.02 x 10^23).

So, in summary, the statement is illustrating that a 12.0 g sample of carbon (which is one mole of carbon because the molar mass of carbon is 12.0 g/mole) contains 6.02 x 10^23 atoms of carbon (because one mole of any substance contains 6.02 x 10^23 atoms or molecules).