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An iron ore sample contains Fe2O3 together with other substances. Reaction of the ore with CO produces iron metal:

αFe2O3(s)+βCO(g)→γFe(s)+δCO2(g)

A)Balance this equation.

B)Calculate the number of grams of CO that can react with 0.320 kg of Fe2O3.

C)Calculate the number of grams of Fe formed when 0.320 kg of Fe2O3 reacts.

D)Calculate the number of grams of CO2 formed when 0.320 kg of Fe2O3 reacts.

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  1. αFe2O3(s)+βCO(g)→γFe(s)+δCO2(g)

    A)Balance this equation.
    Fe2O3(s) + 3CO(g)→ 2Fe(s) + 3CO2(g)
    B)Calculate the number of grams of CO that can react with 0.320 kg of Fe2O3.
    mols Fe2O3 = g/molar mass = 320 g/approx 160 = approx 2
    How many mols CO exactly reacts?
    That's 2 mol Fe2O3 x (3 mols CO/1 mol Fe2O3) = 6 mols CO
    Then convert to grams; ie. g = mols x molar mass = ? g and convert to kg. (NOTE) Note that ANY number of grams you want of CO will react with Fe2O3. I'm sure the author of the problem meant it to be "exactly" react.


    C)Calculate the number of grams of Fe formed when 0.320 kg of Fe2O3 reacts.
    This is just another stoichiometry problem. Work it the same way I did for grams CO.

    D)Calculate the number of grams of CO2 formed when 0.320 kg of Fe2O3 reacts.
    Another stoichiometry problem Works the same was as above.

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