If iron steel wool () is heated until it turns and is placed in a vial containing pure oxygen, iron reacts

If the iron and steel wool () is heated until it turns and is placed in a vial containing pure oxygen, the iron reacts dramatically to produce iron (III) oxide. Fe (s) + O2 (g) = Fe2O3 (s) If 1.25 g of iron is heated and placed in a vial containing 0.0213 mol of oxygen gas, the mass of iron oxide (III) product?

Mole ratio 4:3:2 mass Fe = 1.25 g = ENF MFE * molar mass of Fe = 1.25 g mol * 55.85 g / = 2.238137869 x 10 -2 mol = 0.0213 mol NO2 First, we find the limiting reagent. ENF = 0.0213 mol O2 needed * 4 mol / 3 mol O2 Fe = 2.84 x 10 ^ 2 mol Therefore, Fe is limiting reagent. Thus, we use the moles of Fe to continue the calculations. = 2.238137869 NFe2O3 x 10 -2 mol Fe mol Fe2O3 * 2 / 4 mol Fe = 1.119068935 x 10 -2 mol molar mass of Fe2O3 Fe2O3 = 159.70 g / mol made by 2 x 3 x 55.85 + 16.00] [g / mol Mass of N * Fe2O3 = Molar mass of Fe2O3 to Fe2O3 = 1.119068935 x 10 -2 mol * 159.70 g / mol = 1 g Fe2O3 787,153,088

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