To determine the limiting reactant and the mass of iron oxide produced, we first need to write the balanced chemical equation for the reaction:4 Fe + 3 O2 2 Fe2O3Now, we'll calculate the moles of each reactant:Moles of iron Fe = mass / molar massMoles of Fe = 10 g / 55.85 g/mol 0.179 molesMoles of oxygen O2 = mass / molar massMoles of O2 = 15 g / 32.00 g/mol 0.469 molesNext, we'll determine the mole ratio of iron to oxygen in the balanced equation:Mole ratio Fe:O2 = 4:3Now, we'll divide the moles of each reactant by their respective coefficients in the balanced equation to find which reactant is limiting:Fe: 0.179 moles / 4 0.045O2: 0.469 moles / 3 0.156Since the value for iron Fe is smaller, it is the limiting reactant.Now, we'll use the stoichiometry of the balanced equation to determine the moles of iron oxide Fe2O3 produced:Moles of Fe2O3 = moles of limiting reactant * coefficient of Fe2O3 / coefficient of limiting reactant Moles of Fe2O3 = 0.179 moles * 2 / 4 0.0895 molesFinally, we'll convert the moles of iron oxide to grams:Mass of Fe2O3 = moles * molar massMass of Fe2O3 = 0.0895 moles * 159.69 g/mol 14.3 gSo, the limiting reactant is iron Fe , and the mass of iron oxide Fe2O3 produced is approximately 14.3 grams.