Question

Using the equation, 4Fe + 3O2 Imported Asset 2Fe2O3, if 111.6 g of iron react, what mass of oxygen was consumed?

Answer 1

Answer: 48.0 g

Explanation:

According to avogadro's law, 1 mole of every substance occupies 22.4 L at STP and contains avogadro's number $6.023\times 10^{23}$ of particles.

To calculate the number of moles, we use the equation:

$\text{Number of moles of}Fe=\frac{\text{Given mass}}{\text{Molar mass}}=\frac{111.6g}{55.85g/mol}=2moles$

$4Fe+3O_2\rightarrow 2Fe_2O_3$

According to stoichiometry:

4 moles of iron react with 3 moles of oxygen

thus 2 moles of iron will react with =$\frac{3}{4}\times 2=1.5$ moles of oxygen

Mass of oxygen=$moles\times {\text {molar mass}}=1.5\times 32g/mol=48g$

Thus 48 g of oxygen were consumed.

Answer 2

Youll need a periodic table to get the masses