Answer:
The molecular formula is SO2F2
Explanation:
Step 1: Data given
Suppose the mass of compound = 100 grams
The compound contains:
31.42 % S = 31.42 grams S
31.35 % O = 31.35 grams O
100 - 31.42 - 31.35 = 37.23 F
Molar mass of S = 32.065 g/mol
Molar mass F = 19.00 g/mol
Molar mass O = 16.00 g/mol
Step 2: Calculate moles
Moles = mass / molar mass
Moles S = 31.42 grams / 32.065 g/mol
Moles S = 0.9799 moles
Moles 0 = 31.35 grams / 16.00 g/mol
Moles 0 = 1.959 moles
Moles F = 37.23 grams / 19.00 g/mol
Moles F = 1.959 moles
Step 3: Calculate mol ratio
We divide by the smallest amount of moles
S: 0.9799 / 0.9799 = 1
F: 1.959/ 0.9799 = 2
O : 1.959 / 0.9799 = 2
The empirical formula is SO2F2
This formula has a molecular mass of 102.06 g/mol
This means the empirical formula is also the molecular formula : SO2F2
