To determine the mass of an Fe3N2 sample based on the number of nitrogen atoms, we need to consider the molar mass and stoichiometry of Fe3N2.
The molar mass of Fe3N2 can be calculated by adding up the atomic masses of its constituents, which are iron (Fe) and nitrogen (N). The atomic mass of iron is approximately 55.85 grams per mole, and the atomic mass of nitrogen is approximately 14.01 grams per mole.
Fe3N2 contains three iron atoms (Fe) and two nitrogen atoms (N) in its formula. Therefore, the molar mass of Fe3N2 can be calculated as follows:
Molar mass of Fe3N2 = (3 × atomic mass of Fe) + (2 × atomic mass of N) = (3 × 55.85 g/mol) + (2 × 14.01 g/mol) = 167.55 g/mol + 28.02 g/mol = 195.57 g/mol
Now, we can calculate the mass of the Fe3N2 sample using the given number of nitrogen atoms (7.3x10^23):
Number of moles of nitrogen = (7.3x10^23) / (Avogadro's number) ≈ (7.3x10^23) / (6.022 × 10^23 mol^-1) ≈ 1.21 moles
Mass of Fe3N2 sample = (Number of moles of nitrogen) × (Molar mass of Fe3N2) ≈ 1.21 moles × 195.57 g/mol ≈ 236.45 grams
Therefore, the mass of the Fe3N2 sample containing 7.3x10^23 nitrogen atoms is approximately 236.45 grams.