Achemist found that 4.69 g of sulfur combined with fluorine to produce 15.81 g of a gas. what is the empirical formula of the gas? 1. s2f6 2. s3f2 3. sf4 4. sf7 5. sf5 6. s4f

Mass of sulfur combined - 4.69 g
Mass of gas produced is 15.81 g, therefore mass of fluorine is (15.81-4.69) = 11.12 g
Number of sulfur moles - 4.69 g/32 g/mol = 0.15 mol
Number of fluorine moles - 11.12 g/ 19 g/mol = 0.585 mol
divide both by least number of moles 
S - 0.15/0.15 = 1
F - 0.585/0.15 = 3.9 rounded off is 4
ratio of S to F = 1:4Therefore formula of the gas is SF₄

10.063g / 10.00 ml = 1.0063 g/ml which rounds off to 4 sig figs as: 1.006 g/ml