Fe2O3(s) + 3CO(g) 2Fe(s) +3CO2(g) How many grams of iron can be produced from 1.00 kg Fe2O3?

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    ##699 g##
    The idea here is that you need to use the that exists between ferric oxide ##Fe_2O_3## and iron metal ##Fe## to determine how many moles of the latter will be produced when all the given mass of the ferric oxide reacts.
    ##Fe_2O_text(3(s]) + 3CO_text((g]) -> color(purple)(2)Fe_text((s]) + 3CO_text(2(g])##
    Notice that every mole of ferric oxide will produce ##color(purple)(2)## moles of iron metal.
    To determine how many mole of ferric oxide you get in ##1.00 kg## of the compound use its molar mass
    ##1.00color(red)(cancel(color(black)(kg))) * (1000color(red)(cancel(color(black)(g))))/(1color(red)(cancel(color(black)(kg)))) * (1 mole Fe_2O_3)/(159.69color(red)(cancel(color(black)(g)))) = 6.262 moles Fe_2O_3##
    Now use the ##1:color(purple(2)## mole ratio to find how many moles of iron metal will be produced by the reaction
    ##6.262color(red)(cancel(color(black)(moles Fe_2O_3))) * (color(purple)(2) moles Fe)/(1color(red)(cancel(color(black)(mole Fe_2O_3)))) = 12.524 moles Fe##
    Finally use iron’s molar mass to find how many grams will contain this many moles of iron
    ##12.524color(red)(cancel(color(black)(moles))) * 55.845 g/(1color(red)(cancel(color(black)(mole)))) = 699.4 g Fe##
    Rounded to three the answer will be
    ##m_Fe = color(green)(699 g)##

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