Question

assuming a 90.0% recovery what mass of iron in grams would actually be produced by 927g Fe2O3?

Answer 1

90.0% of 927g is?

Answer 2

834.3..?

Answer 3

Is the assumption for recovery is for the mass of iron?

Answer 4

\[Fe_2O_3 + 3 CO \rightarrow 2 Fe + 3 CO_2\]
Nevermind that, for every mole of \(Fe_2O_3\) we should get 2 moles of iron, Fe.

Answer 5

So, we should find the moles of iron itself first, by doing
\[927g Fe_2O_3 \times \frac{1~molFe_2O_3}{159.69~gFe_2O_3} \times \frac{2~mol Fe}{1~molFe_2O_3}=11.61~moles~of~Fe\]

Answer 6

Then use the 11.61moles of Fe multiplying it by the molar mass of Fe and you'd get the mass.
\[11.61molesFe \times \frac{55.85gFe}{1~molFe}=648.4gFe\]

Answer 7

Then it says you should be recovering 90% of the iron, so 90% of 648.4 grams of iron is
\[\frac{90 \%}{100 \%} \times 648.4g=583.6~\text{grams of iron recovered}\]

Answer 8

thanks!

Answer 9

yw :) make sure you're getting it