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pino40

24.05.2021

Chemistry

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

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

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