Question

Starting with the following equation, Fe₂O₃(s) + Al(s) → Fe(l) + Al₂O₃(s), calculate the moles of Fe₂O₃ that will be required to produce 645 grams of Fe.

a) 0.387 moles
b) 1.94 moles
c) 3.88 moles
d) 7.76 moles

Answer 1

To calculate the moles of Fe₂O₃ required to produce 645 grams of Fe, set up a proportion using the stoichiometry of the balanced chemical equation. Using the molar mass of Fe, you can convert the grams of Fe to moles. The answer is approximately 5.791 moles of Fe₂O₃.

Step-by-step explanation:

To calculate the moles of Fe₂O₃ required to produce 645 grams of Fe, we need to use the stoichiometry of the balanced chemical equation.

The balanced equation is Fe₂O₃(s) + Al(s) → Fe(l) + Al₂O₃(s).

From the balanced equation, we can see that the molar ratio between Fe₂O₃ and Fe is 1:2, meaning 1 mole of Fe₂O₃ produces 2 moles of Fe.

We can use this ratio to set up a proportion:

(moles of Fe₂O₃) = (moles of Fe) × (1 mole of Fe₂O₃/2 moles of Fe)

Using the molar mass of Fe (55.85 g/mol), we can convert the grams of Fe to moles:

(moles of Fe) = (grams of Fe)/(molar mass of Fe)

Substituting the given values, we get:

(moles of Fe₂O₃) = (645 g Fe)/(55.85 g/mol) × (1 mole of Fe₂O₃/2 moles of Fe) = 5.791 moles of Fe₂O₃

Therefore, the moles of Fe₂O₃ required to produce 645 grams of Fe is approximately 5.791 moles.