To determine the number of fluorine atoms in 24.24 grams of sulfur hexafluoride (SF6), we need to use the molar mass of SF6 and Avogadro's number.
The molar mass of SF6 can be calculated by adding up the atomic masses of sulfur (S) and six fluorine (F) atoms: Molar mass of S = 32.06 g/mol Molar mass of F = 18.998 g/mol
Molar mass of SF6 = (1 × Molar mass of S) + (6 × Molar mass of F) = (1 × 32.06 g/mol) + (6 × 18.998 g/mol) = 32.06 g/mol + 113.988 g/mol = 146.046 g/mol
Now we can use the molar mass to calculate the number of moles of SF6: Number of moles = Mass / Molar mass = 24.24 g / 146.046 g/mol ≈ 0.166 moles
Since there are six fluorine atoms in one SF6 molecule, the number of fluorine atoms can be calculated by multiplying the number of moles by Avogadro's number (6.022 × 10^23 atoms/mol): Number of fluorine atoms = Number of moles × Avogadro's number = 0.166 moles × (6.022 × 10^23 atoms/mol) ≈ 9.987 × 10^22 fluorine atoms
Therefore, there are approximately 9.987 × 10^22 fluorine atoms in 24.24 grams of sulfur hexafluoride.