Question

How many moles of aluminum are needed to react completely with 1.2 mol of feo

Answer 1

Answer:

0.8 mol.

Explanation:

• The balanced equation for the reaction between Al and FeO is represented as:

2Al + 3FeO → 3Fe + Al₂O₃,

It is clear that 2 mol of Al react with 3 mol of FeO to produce 3 mol of Fe and 1 mol of Al₂O₃.

Using cross multiplication:

2 mol of Al needs → 3 mol of FeO, from stichiometry.

??? mol of Al needs → 1.2 mol of FeO.

∴ The no. of moles of Al are needed to react completely with 1.2 mol of FeO = (2 mol)(1.2 mol)/(3 mol) = 0.8 mol.

Answer 2

Considering the reaction stoichiometry, 0.8 moles of aluminum are needed to react completely with 1.2 moles of FeO.

The balanced reaction is:

2 Al + 3 FeO → 3 Fe + Al₂O₃

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

• Al: 2 moles  
• FeO: 3 moles
• Fe: 3 moles
• Al₂O₃: 1 mole

Then you can apply the following rule of three:  if by stoichiometry 3 moles of FeO react with 2 moles of Al, 1.2 moles of FeO react with how many moles of Al?

$amount of moles of Al= \frac{1.2 moles of FeOx2 moles of Al}{3 moles of FeO}$

amount of moles of Al= 0.8 moles

Finally, 0.8 moles of aluminum are needed to react completely with 1.2 moles of FeO.

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