A compound containing selenium and fluorine is decomposed in the laboratory and produces 2.231 g of selenium and 3.221 g of fluorine. Calculate the empirical formula of the compound.
The atomic weight of Se = 78.96 g/mol. The amount of Se produced = 2.231g
mole = 2.231g / 78.96g/mol
mole = 0.028254812
Atomic weight of F = 19.00g/mol . The amount of F produced = 3.221g
mole = 3.221g / 19.00g/mol
mole = 0.169526315
Divide both values by the lower value: 0.028254812 .
Se: 0.028254812 / 0.028254812 = 1
F: 0.169526315 / 0.028254812 = 6
Empirical formula: SeF₆ (Answer)