# AP Chemistry

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A 7.6 g sample of iron ore is treated as follows.
The iron in the sample is all converted by a
series of chemical reactions to Fe2O3. The
mass of Fe2O3 is measured to be 12.9 g. What
was the mass of iron in the sample of ore?

• AP Chemistry -

Didn't I do this for you (or one similar to it) a couple of days ago.

12.9g x (1 mol Fe2O3/molar mass Fe2O3) x (2 mols Fe/1 mol Fe2O3) x (atomic mass Fe/1 mol Fe) = ?

There is an easier way to do this but chemical factors are not taught in most schools now.
12.9 x (2*Fe/Fe2O3) = 12.9*2*55.85/159.7 = 9.02 g.
Check your post. There is a problem because the mass of Fe CAN'T be more than the 7.6g you started with.

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