Determine the molecular mass of iron III oxide

Chemistry

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Answer

159.687 g/mol\text{159.687 g/mol}

Step-by-step solution

3 steps

  1. Determine the chemical formula for iron (III) oxide.

    Iron (III) indicates that iron has an oxidation state of +3+3 (Fe3+Fe^{3+}). Oxide indicates oxygen with an oxidation state of −2-2 (O2−O^{2-}). To balance the charges, we need two iron ions and three oxygen ions.
    The chemical formula is Fe2O3Fe_2O_3.

  2. List the atomic masses of the elements.

    From the periodic table:
    Atomic mass of Iron (Fe) ≈55.845 g/mol\approx 55.845 \text{ g/mol}
    Atomic mass of Oxygen (O) ≈15.999 g/mol\approx 15.999 \text{ g/mol}

  3. Calculate the molecular mass of Fe2O3Fe_2O_3.

    The molecular mass is the sum of the atomic masses of all atoms in the formula.

    Molecular mass of Fe2O3=(2×Atomic mass of Fe)+(3×Atomic mass of O)\text{Molecular mass of } Fe_2O_3 = (2 \times \text{Atomic mass of Fe}) + (3 \times \text{Atomic mass of O}) Molecular mass of Fe2O3=(2×55.845 g/mol)+(3×15.999 g/mol)\text{Molecular mass of } Fe_2O_3 = (2 \times 55.845 \text{ g/mol}) + (3 \times 15.999 \text{ g/mol}) Molecular mass of Fe2O3=111.690 g/mol+47.997 g/mol\text{Molecular mass of } Fe_2O_3 = 111.690 \text{ g/mol} + 47.997 \text{ g/mol} Molecular mass of Fe2O3=159.687 g/mol\text{Molecular mass of } Fe_2O_3 = 159.687 \text{ g/mol}

    The molecular mass of iron (III) oxide is 159.687 g/mol\text{159.687 g/mol}.

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