Final answer:
In 15 g of SF6, there are 3.71 x 10^23 atoms of fluorine. The calculation involves finding the molar mass of SF6, converting grams to moles, and then using Avogadro's number to determine the number of atoms.
Step-by-step explanation:
To calculate the number of fluorine atoms in 15 g of sulfur hexafluoride (SF6), we must first determine the molar mass of SF6 and then use Avogadro's number to convert moles to atoms.
The molar mass of SF6 can be calculated by adding the atomic masses of sulfur (S) and six fluorine (F) atoms: Molar mass of S = 32.07 g/mol, and Molar mass of F = 19.00 g/mol (per atom).
Molar mass of SF6 = (1 x 32.07 g/mol) + (6 x 19.00 g/mol) = 32.07 g/mol + 114.00 g/mol = 146.07 g/mol.
Next, we convert 15 g of SF6 to moles: Moles of SF6 = 15 g / 146.07 g/mol = 0.1027 mol.
Since each molecule of SF6 has six fluorine atoms, we multiply the moles of SF6 by Avogadro's number and then by 6 to find the number of fluorine atoms:
Number of F atoms = 0.1027 mol x 6.022 x 1023 atoms/mol x 6 = 3.71 x 1023 atoms.
Thus, the answer is (c) 3.71 x 1023 atoms of fluorine.