What is the mass percent of Fe2O3 in the iron ore sample?An iron ore samp;le contains Fe2O3 plus other impurities. A 752-g sample of impure iron ore is heated with excess carbon, producing 453 g of pure iron by the following reaction: Fe2O3 (s) + 3C(s) ----gt;2Fe (s) + 3CO(g). what is the mass percent of Fe2O3 in the impure iron ore sample? Assume Fe2O3 is the only source of iron and that the reaction is 100% efficient.
That is actually a good question
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Hi friend! Consider the balanced chemical reaction you gave. 111.6g of iron is produced from 159.6g of Fe2O3. calculate how much Fe2O3 is require to produce 453g of iron. 453 X 159.6 / 111.6 647.8g Percentage purity is 647.8 X 100 / 752 86.1 Your sample is 86% pure :-)
% by mass of Fe2O3 (mass of pure Fe2O3 / mass of iron ore) x 100% mass of Fe2O3 (pure) (mass of iron produced / MW of iron) x ( stoichiometric mole ratio of Fe2O3 over Fe based on the given chemical reaction x MW of Fe2O3 mass of iron produced 453 g MW of Fe 55.85 stoichiometric mole ratio of Fe2O3/Fe 1/2 MW of Fe2O3 159.7 mass of pure Fe2O3 (453/55.85) x (1/2) x 159.7 mass of pure Fe2O3 647.66 grams %by mass of Fe2O3 (647.66 / 752) x 100 86.13 %
