Given the reaction 2Al + 3FeO → Al2O3 + 3Fe, how many moles of aluminum (Al) are needed to react completely with 1.2 mol of iron(II) oxide (FeO)?

• A. 1.2 mol
• B. 0.80 mol
• C. 0.60 mol
• D. 0.80 mol

Answer: (D)

Verified step by step guidance

1. Identify the balanced chemical equation: \$2Al + 3FeO \rightarrow Al_2O_3 + 3Fe$.
2. Determine the mole ratio between aluminum (Al) and iron(II) oxide (FeO) from the balanced equation. For every 3 moles of FeO, 2 moles of Al are required.
3. Set up a proportion to find the moles of Al needed for 1.2 moles of FeO using the mole ratio: \(\frac{2\ \text{mol Al}}{3\ \text{mol FeO}} = \frac{x\ \text{mol Al}}{1.2\ \text{mol FeO}}\).
4. Solve for \(x\) (moles of Al) by cross-multiplying and dividing: \(x = \frac{2}{3} \times 1.2\).
5. Interpret the result as the number of moles of aluminum required to completely react with 1.2 moles of iron(II) oxide.