Final answer:
To react completely with 1.2 mol of FeO, 0.8 moles of aluminum are required as per the stoichiometric ratio from the balanced chemical equation.
Step-by-step explanation:
To determine how many moles of aluminum are needed to react completely with 1.2 mol of FeO, we can use stoichiometry based on the balanced chemical equation:
2 Al(s) + 3 FeO(s) → 3Fe(s) + Al2O3(s)
According to the balanced equation, 2 moles of aluminum (Al) react with 3 moles of iron oxide (FeO). Therefore, to find the moles of aluminum needed to react with 1.2 moles of FeO, we use the following ratio:
(moles of Al) = (moles of FeO) ×
mol Al/ mol FeO
Substituting the given values we get:
(moles of Al) = 1.2 mol FeO × 2 mol Al / 3 mol FeO
This simplifies to:
(moles of Al) = 0.8 mol Al
Thus, 0.8 moles of aluminum are required to react completely with 1.2 mol of FeO.