A 3.6 g sample of iron (III) oxide reacts with sufficient aluminum to be entirely used up. How much iron is produced?

0.046 mol

Explanation:

Step 1: Write the balanced equation

Fe₂O₃ + 2 Al ⇒ 2 Fe + Al₂O₃

Step 2: Calculate the moles corresponding to 3.6 g of Fe₂O₃

The molar mass of Fe₂O₃ is 159.69 g/mol.

3.6 g × 1 mol/159.69 g = 0.023 mol

Step 3: Calculate the moles of Fe produced from 0.023 moles of Fe₂O₃

The molar ratio of Fe₂O₃ to Fe is 1:2.

0.023 mol  Fe₂O₃ × 2 mol Fe/1 mol Fe₂O₃ = 0.046 mol Fe

there all right good

explanation: