The mass percentage of **pure** **Fe**_{2}**O**** _{3}** can be computed using the equation:

Since the reaction is __100% efficient__ this means that **all Fe**_{2}**O**_{3}** in the iron ore reacted** to form pure Fe.

The **mass of impure Fe_{2}O_{3 }**or the

But, the **mass of pure Fe**_{2}**O**** _{3 }**needs to be calculated based on the

We can solve for the Mass of Fe_{2}O_{3} through the following steps:

- a
calculation (converting mass of Fe to moles)__mass to mole__ - a
calculation (moles Fe to moles Fe__mole to mole___{2}O3 ) - a
calculation (converting moles to mass of Fe__mole to mass___{2}O3)

An iron ore sample contains Fe_{2}O_{3} plus other impurities. A 752-g sample of impure iron ore is heated with excess carbon, producing 453 g of pure iron by the following reaction:

Fe_{2}O_{3} _{(s)} + 3 C _{(s)} → 2 Fe _{(s)} + 3 CO (g)

What is the mass percent of Fe _{2}O_{3} in the impure iron ore sample? Assume that Fe _{2}O_{3} is the only source of iron and that the reaction is 100% efficient.

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