## Chemistry and Chemical Reactivity (9th Edition)

Empirical formula: $ICl_3$ Molecular formula: $I_2Cl_6$
Atomic weights (g/mol): $Cl: 35.45, \ I: 126.904$ Number of moles consumed: I: $0.678\ g\div126.904=5.34\times10^{-3}\ mol\ of\ I$ Cl: $(1.246-0.678)\ g\div35.45=1.602\times10^{-2}\ mol\ of\ Cl$ Dividing by the smallest number of moles: Cl: $1.602\times10^{-2}\div5.34\times10^{-3}=3.00$ Empirical formula: $ICl_3$ Molar mass of the empirical formula: $228.11\ g/mol$ Molar mass of the compound: $467\ g/mol$ Ratio of the two: $2.0$ Molecular formula: $I_2Cl_6$