This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Step 1: Determine the chemical formula for iron (III) oxide. Iron (III) indicates that iron has an oxidation state of +3 (Fe^3+). Oxide indicates oxygen with an oxidation state of -2 (O^2-). To balance the charges, we need two iron ions and three oxygen ions. The chemical formula is Fe_2O_3. Step 2: List the atomic masses of the elements. From the periodic table: Atomic mass of Iron (Fe) ≈ 55.845 g/mol Atomic mass of Oxygen (O) ≈ 15.999 g/mol Step 3: Calculate the molecular mass of Fe_2O_3. The molecular mass is the sum of the atomic masses of all atoms in the formula. Molecular mass of Fe_2O_3 = (2 × Atomic mass of Fe) + (3 × Atomic mass of O) Molecular mass of Fe_2O_3 = (2 × 55.845 g/mol) + (3 × 15.999 g/mol) Molecular mass of Fe_2O_3 = 111.690 g/mol + 47.997 g/mol Molecular mass of Fe_2O_3 = 159.687 g/mol The molecular mass of iron (III) oxide is 159.687 g/mol. Last free one today — make it count tomorrow, or type /upgrade for unlimited.