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When iron(III) oxide reacts with aluminum, aluminum oxide and iron are produced. The balanced equation for this reaction is:
Fe2O3 (s) + 2Al (s) --------> Al2O3 (s) + 2Fe (s)
If 6 moles of aluminum react:
i. The reaction consumes ________ moles of iron(III) oxide.
ii. The reaction produces _________ moles of aluminum oxide and ________ moles of iron.

Respuesta :

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 :

[tex]Fe_2O_3(s)+2Al(s)\rightarrow Al_2O_3(s)+2Fe(s)[/tex]

According to stoichiometry:

a) 2 moles of aluminium consume = 1 mole of [tex]Fe_2O_3[/tex]

6 moles of aluminium consume = [tex]\frac{1}{2}\times 6=3[/tex] moles of [tex]Fe_2O_3[/tex]

b) 2 moles of aluminium produce = 1 mole of [tex]Al_2O_3[/tex]

6 moles of aluminium consume = [tex]\frac{1}{2}\times 6=3[/tex] moles of [tex]Al_2O_3[/tex]

2 moles of aluminium produce = 2 moles of [tex]Fe[/tex]

6 moles of aluminium consume = [tex]\frac{2}{2}\times 6=6[/tex] moles of [tex]Fe[/tex]

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