Question

One of the reactions that occurs in a blast furnace, in which iron ore is converted to cast iron, is

Fe2O3 + 3CO → 2Fe + 3CO2

Suppose that 1.59 × 103 kg of Fe is obtained from a 2.54 × 103 kg sample of Fe2O3. Assuming that the reaction goes to completion, what is the percent purity of Fe2O3 in the original sample?
There are easier ways to do this but I think this is the best way to go about it. I would change the kg to grams.
mols Fe = grams Fe/atomic mass Fe = ?
Using the coefficients in the balanced equation, convert mols Fe to mols Fe2O3. That is mols Fe x (1 mol Fe2O3/2 mols Fe) = ?
Now convert mols Fe2O3 to grams Fe2O3.
g Fe2O3 = mols Fe2O3 x molar mass Fe2O3 = ?
Finally, %Fe2O3 = %purity = (g Fe2O3/

%Fe = (mass Fe/mass sample)*100 = ?
Substitute and solve for %Fe which is the percent purity.
Can you put the figures into the equation for me, because I do not quite understand this?

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