How many moles of aluminum are needed to react completely with 2.4 mol of FeO?
To determine the number of moles of aluminum needed to react completely with 2.4 mol of FeO, we need to use the balanced chemical equation for the reaction between aluminum (Al) and iron(II) oxide (FeO).
The balanced chemical equation for this reaction is:
2Al + 3FeO -> 3Fe + Al2O3
From the balanced equation, we can see that 2 moles of aluminum react with 3 moles of FeO to produce 3 moles of iron (Fe) and 1 mole of aluminum oxide (Al2O3).
Using the mole ratio from the balanced equation, we can set up the following proportion:
2 mol Al / 3 mol FeO = x mol Al / 2.4 mol FeO
Solving this proportion, we can find the value of x (the number of moles of aluminum needed).
Cross-multiplying, we get:
(2 mol Al) * (2.4 mol FeO) = (3 mol FeO) * (x mol Al)
4.8 mol Al = 3x mol Al
Now, we can solve for x:
x = (4.8 mol Al) / (3 mol Al)
x = 1.6 mol Al
Therefore, 1.6 moles of aluminum are needed to react completely with 2.4 moles of FeO.