Please show work. I am in desperate need of help.An iron ore sample contains Fe2O3 plus other impurities. A 752g sample of impure iron ore is heated with excess carbon, producing 453g of pure iron by the following reaction:Fe2O3 + 3C ---gt; 2Fe + 3COWhat 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.
well, you can, but the labor to do it would be difficult. its only limited to any custom modifications to the parts you're willing to make.
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% by capacity of mass of Fe2O3 (mass of organic Fe2O3 / mass of iron ore) x a hundred% mass of Fe2O3 (organic) (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 fifty 5.80 5 stoichiometric mole ratio of Fe2O3/Fe a million/2 MW of Fe2O3 159.7 mass of organic Fe2O3 (453/fifty 5.80 5) x (a million/2) x 159.7 mass of organic Fe2O3 647.66 grams %by capacity of mass of Fe2O3 (647.66 / 752) x a hundred 86.13 %
Assume that the 752 grams was pure iron (III) oxide, so how many moles does that account for? Now, you know that for every mole of iron (III) oxide, you get 2 moles of iron, and you got 453 grams. So how many moles is that? Knowing how many moles of iron you got, and relating that to what you could have gotten, you can do the arithmetic and get the answer.
