Question

Iron is obtained by reaction of hematite (Fe2O3) with carbon monoxide. From the balanced reaction below, how many grams of iron is produced when 24.6 mol of hematite is used up in the reaction?
Fe2O3 + 3CO ® 2Fe + 3CO2

Answer 1

Answer: 2755.2 g of $Fe$ will be produced from 24.6 mol of haematite.

Explanation:

The balanced chemical equation is:

$Fe_2O_3+3CO\rightarrow 2Fe+3CO_2$  

According to stoichiometry :

1 mole of $Fe_2O_3$ produce = 2 moles of $Fe$

Thus 24.6 moles of $Fe_2O_3$ will produce=$\frac{2}{1}\times 24.6=49.2moles$  of $Fe$  

Mass of $Fe=moles\times {\text {Molar mass}}=49.2moles\times 56g/mol=2755.2g$

Thus 2755.2 g of $Fe$ will be produced from 24.6 mol of haematite.