calculate the molar mass of Fe2O3 to one decimal point
The correct answer and explanation is:
The molar mass of iron(III) oxide (Fe2O3\text{Fe}_2\text{O}_3) is calculated as follows:
- Iron (Fe): Atomic mass = 55.8 g/mol
Since there are 2 Fe atoms, the total mass contribution from Fe is: 2×55.8=111.6 g/mol2 \times 55.8 = 111.6 \text{ g/mol} - Oxygen (O): Atomic mass = 16.0 g/mol
Since there are 3 O atoms, the total mass contribution from O is: 3×16.0=48.0 g/mol3 \times 16.0 = 48.0 \text{ g/mol} - Total Molar Mass: 111.6+48.0=159.6 g/mol111.6 + 48.0 = 159.6 \text{ g/mol}
Final Answer: 159.6 g/mol
Explanation (300 words)
Iron(III) oxide (Fe2O3\text{Fe}_2\text{O}_3) is a chemical compound consisting of iron and oxygen. It is commonly found in nature as hematite, an important iron ore. The molar mass of a compound is the sum of the atomic masses of all the atoms present in its molecular formula, expressed in grams per mole (g/mol).
To determine the molar mass of Fe2_2O3_3, we first look at the periodic table to find the atomic masses of iron (Fe) and oxygen (O). The atomic mass of iron is 55.8 g/mol, and the atomic mass of oxygen is 16.0 g/mol.
Since the formula Fe2_2O3_3 contains two Fe atoms and three O atoms, we calculate their contributions separately:
- Iron Contribution: 2×55.8=111.62 \times 55.8 = 111.6 g/mol
- Oxygen Contribution: 3×16.0=48.03 \times 16.0 = 48.0 g/mol
Adding these together, we get the total molar mass: 159.6 g/mol159.6 \text{ g/mol}
Understanding molar mass is essential in chemistry for stoichiometric calculations, which help in determining the amounts of reactants and products in a chemical reaction. Fe2_2O3_3 is widely used in industries, including steel manufacturing and pigments. Its correct molar mass calculation is crucial for precise formulation and reaction balancing.
