The mass in grams of 6.022 x 10^23 atoms of carbon (C) can be determined by using the molar mass of carbon, which is approximately 12.01 grams per mole.
One mole of any substance contains Avogadro's number (6.022 x 10^23) of particles, in this case, carbon atoms. Therefore, the molar mass of carbon (12.01 g/mol) is equal to the mass of 6.022 x 10^23 carbon atoms.
To calculate the mass of 6.022 x 10^23 carbon atoms, we can set up a proportion:
(12.01 g) / (1 mol) = (x g) / (6.022 x 10^23 atoms)
Cross-multiplying gives:
12.01 g * (6.022 x 10^23 atoms) = (1 mol) * (x g)
Simplifying further:
x g = (12.01 g) * (6.022 x 10^23 atoms)
Calculating this expression:
x g ≈ 72.32 x 10^23 g
So, the mass of 6.022 x 10^23 atoms of carbon is approximately 72.32 grams.