# Chapter 2 Atoms, Molecules, and Ions - Study Questions - Page 95e: 94

6

#### Work Step by Step

Atomic weights (g/mol): $S: 32.06,\ F: 18.998$ Molar mass $F_2$: 38.00 g/mol Mass of S: 1.256 g Mass of the product: 5.722 g Mass of fluorine $F_2$: 5.722 - 1.256 = 4.466 g Number of moles: S: $1.256/32.06=3.92\times10^{-2}\ mol$ $F_2$: $4.466/38.00=0.118\ mol\ F_2 = 0.235\ mol\ F$ Normalizing by the smallest amount of moles: S: 1.0 F: 6.0 Empirical formula of the product: $SF_6$ Value of x: 6

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