Question

When iron(III) oxide reacts with aluminum, aluminum oxide and iron are produced. The balanced equation for this reaction is:

Answer 1

Answer: i. The reaction consumes 3 moles of iron(III) oxide.

ii. The reaction produces 3 moles of aluminum oxide and 6 moles of iron.

Explanation:

The balanced reaction is :

$Fe_2O_3(s)+2Al(s)\rightarrow Al_2O_3(s)+2Fe(s)$

According to stoichiometry:

a) 2 moles of aluminium consume = 1 mole of $Fe_2O_3$

6 moles of aluminium consume = $\frac{1}{2}\times 6=3$ moles of $Fe_2O_3$

b) 2 moles of aluminium produce = 1 mole of $Al_2O_3$

6 moles of aluminium consume = $\frac{1}{2}\times 6=3$ moles of $Al_2O_3$

2 moles of aluminium produce = 2 moles of $Fe$

6 moles of aluminium consume = $\frac{2}{2}\times 6=6$ moles of $Fe$