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In an experiment, iron was heated in the presence of excess oxygen and the following data was obtained.
Mass of empty crucible = 10.98 g
Mass of crucible + iron before reaction = 12.66 g
Mass of crucible + iron after heating = 13.30 g
Calculate the empirical formula of the oxide of iron. (Fe =56, O = 16)

Answer Text:
Mass Fe = 12.66 – 10.98 = 1.68
Mass of O = 13.30 – 12.66 = 0.64
Moles Fe = #1.68/56# = 0.03
Moles O = #0.64/16#= 0.04
Mole ratio Fe:O = 3:4
E.F = #Fe_3O_4#