One of the reactions that occurs in a blast furnace (where iron core is converted into cast iron) is that iron

Question

One of the reactions that occurs in a blast furnace (where iron core is converted into cast iron) is that iron (III) is treated with carbon monoxide to produce elemental iron and carbon dioxide. Suppose that 1.64 x 10^3 kg of iron are obtained from a 2.62 x 10^3 kg of iron(III) oxide. Assuming that the reaction goes to completion (ie, no leftover iron(III) oxide) what is the percent purity of iron(III) oxide in the original sample?

Answer 1

The balanced equation is
Fe2O3 + 3 CO >> 2 Fe + 3 CO2
1.64 x 10^3 Kg = 1.64 x 10^6 g
Atomic weight Fe = 55.847 g/mol
1.64 x 10^6 / 55.847 = 2.94 x 10^4 moles Fe obtained
2.62 x 10^3 Kg = 2.62 x 10^6 g
Molecular weight Fe2O3 = 159.7 g/mol
2.62 x 10^6 g / 159.7 = 1.64 x 10^4 moles Fe2O3
The ratio between Fe2O3 and Fe is 1 : 2
1 : 2 = 1.64 x 10^4 : x
x = 3.28 x 10^4 moles Fe that we would get if the compound is pure
2.94 x 10^4 : 3.28 x 10^4 = x : 100
x = 89.6 % ( percent purity )

Answer 2

Fe2O3 + 3 CO -> 2Fe + 3 CO2

Mol. wt. of Fe2O3 = 160 g

So, moles of Fe = 1.64x10^3 / 56 kMol

Mass of Fe2O3 = 80*1640/56 x 10^3 kg

Answer 3

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