Answer:
2.5 moles of aluminum oxide will form when all 5.0 moles of aluminum are used up.
Step-by-step explanation:
The balanced chemical equation for the reaction between aluminum (Al) and oxygen (O2) to form aluminum oxide (Al2O3) is:
4 Al + 3 O2 → 2 Al2O3
This equation shows that 4 moles of aluminum react with 3 moles of oxygen to form 2 moles of aluminum oxide.
According to the problem, we have 5.0 mol of aluminum, which is more than enough to react with the oxygen available, and the limiting reagent in this reaction will be aluminum. Therefore, we need to use the mole ratio from the balanced equation to find out how many moles of aluminum oxide will form when all 5.0 moles of aluminum are used up.
From the equation, we can see that for every 4 moles of aluminum, 2 moles of aluminum oxide will form. Therefore, the mole ratio of aluminum to aluminum oxide is 4:2, or simplified, 2:1.
Using this mole ratio, we can calculate the number of moles of aluminum oxide that will form when all 5.0 moles of aluminum react:
5.0 mol Al × (2 mol Al2O3/4 mol Al) = 2.5 mol Al2O3
Therefore, 2.5 moles of aluminum oxide will form when all 5.0 moles of aluminum are used up.