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Iron is obtained commercially by the reaction of hematite (Fe2O3) with carbon monoxide. How many grams of iron is produced when 35.0 moles of hematite react with 41.5 moles of carbon monoxide?
Fe2O3(s) + 3 CO(g) 2 Fe(s) + 3 CO2(g)

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  1. This is a limiting reagent (LR) problem and you know that because amounts are given for BOTH reactants. You may want to locate the arrow keys on your computer and use them.

    Fe2O3(s) + 3CO(g)--> 2Fe(s) + 3CO2(g)

    mols Fe2O3 = 35.0
    mols CO = 41.5

    Use the coefficients in the balanced equation, convert mols Fe2o3 to mols Fe.
    Do the same for mols CO to mols Fe.
    It is likely that the two values will not agree so one must be wrong; the correct value in LR problems is ALWAYS the smaller value and the reagent producing that value is the LR.

    Using the smaller value convert mols Fe to grams. g = mols x molar mass.
    Post your work if you get stuck.

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