how many moles of aluminum are needed to react completly with 1.2 mol of FeO
2Al(s)+3FeO(s)=3Fe(s)+ Al2O3(s)
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from the equation, 2 moles of AL are need for each 3 moles Fe.
So, 2/3 * 1.2 = 0.8 moles of Al react with 1.2 moles Fe
To determine the number of moles of aluminum needed to react completely with 1.2 mol of FeO, we must use the stoichiometry of the balanced chemical equation.
The balanced equation is as follows:
2Al(s) + 3FeO(s) -> 3Fe(s) + Al2O3(s)
From the equation, we can see that for every 2 moles of aluminum, 3 moles of FeO are required.
So the molar ratio of aluminum to FeO is 2:3.
To find the number of moles of aluminum needed, we can set up a proportion:
2 mol Al / 3 mol FeO = x mol Al / 1.2 mol FeO
By cross-multiplication, we have:
2 mol Al * 1.2 mol FeO = 3 mol FeO * x mol Al
2.4 mol Al = 3 mol FeO * x mol Al
Divide both sides of the equation by 3 to solve for x:
x mol Al = 2.4 mol Al / 3
x mol Al ≈ 0.8 mol Al
Therefore, approximately 0.8 moles of aluminum are needed to react completely with 1.2 moles of FeO.
To determine the number of moles of aluminum needed to react completely with 1.2 moles of FeO, we need to use the balanced chemical equation.
The balanced equation is:
2Al(s) + 3FeO(s) → 3Fe(s) + Al2O3(s)
From the equation, we can see that 2 moles of aluminum react with 3 moles of FeO. This means that the mole ratio between aluminum and FeO is 2:3.
To find out how many moles of aluminum are needed, we can set up a proportion using the mole ratio:
(2 moles of Al) / (3 moles of FeO) = (x moles of Al) / (1.2 moles of FeO)
Now, we can solve for x:
x = (2 moles of Al) / (3 moles of FeO) * (1.2 moles of FeO)
x = 0.8 moles of Al
Therefore, 0.8 moles of aluminum are needed to react completely with 1.2 moles of FeO.