When FeO reacts with 1 mole of O_2 to form Fe_3O_4, how many moles of Fe_3O_4 can be produced, assuming excess FeO is present? (Reaction: 6 FeO + O_2 → 2 Fe_3O_4)

• A. 2 moles
• B. 1 mole
• C. 0.5 moles
• D. 3 moles

Answer: (A)

Verified step by step guidance

1. Write down the balanced chemical equation: \$6\ FeO + O_2 \rightarrow 2\ Fe_3O_4$.
2. Identify the mole ratio between \(O_2\) and \(Fe_3O_4\) from the balanced equation. For every 1 mole of \(O_2\), 2 moles of \(Fe_3O_4\) are produced.
3. Since the problem states that 1 mole of \(O_2\) is reacting and there is excess \(FeO\), use the mole ratio to find the moles of \(Fe_3O_4\) produced.
4. Set up the proportion: \$1\ mole\ O_2 \times \frac{2\ moles\ Fe_3O_4}{1\ mole\ O_2} = 2\ moles\ Fe_3O_4$.
5. Conclude that 2 moles of \(Fe_3O_4\) can be produced from 1 mole of \(O_2\) when \(FeO\) is in excess.