Here‘s the question:An iron ore sample 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 that Fe2O3 is the only source of iron and that the reaction is 100% efficient. The answer at the back of the book says 86.2% but I do not know how they got that. Can anyone show me the steps to get to the answer please. Thanks!
