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Calculating percent purity from a reaction
One of the reactions that occurs in a blast furnace, where iron ore is converted to cast iron is Fe2O3 + CO = Fe + CO2.

Suppose that 1750 kg of Fe is obtained from a 2780 kg sample of Fe2O3. Assuming that the reaction goes to completion, what is he percent purity of Fe2O3 in the original sample?
I balanced the equation to get Fe2O3 +3CO= 2Fe + 3CO2. Then I calculated the moles of Fe obtained to compare to moles of Fe2O3, getting:

1750 kg of Fe X 1 mole Fe/56 g Fe = 31250 mol Fe

2780 kg of Fe2O3 X 1 mole Fe2O3/160 g Fe2O3 =17.38 g Fe2O3

So now I'm not exactly sure what the problem is asking for in asking for percent purity of Fe2O3- is it asking what the percent of Fe is in

Fe2O3? It has to be set up as a ratio, but I just don't know where to go from here 31250 mol Fe X (1 mol Fe2O3/2 mol Fe) X(17.38 g Fe2O3/ 1 mole Fe2O3)=???? huge

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