Given the following:

4Al+ 3O2---> 2Al2O3

Which reactant is limiting if 0.32 mol Al and 0.26 mol O2 are available?

I got 0.24 mol Al and 0.35 mol O2 when I did my work. Therefore Al is limiting. Can you tell me if I am right.

I don't know what your statement about 0.24 mol Al and 0.35 mol O2 means. I don't believe Al is the limiting reagent. If you will post your work I'll find what's wrong.

To determine which reactant is limiting, we need to compare the moles of each reactant to the stoichiometric ratio given in the balanced chemical equation.

From the balanced equation, we can see that the stoichiometric ratio between Al and O2 is 4:3. This means that for every 4 moles of Al, we need 3 moles of O2 to react completely.

Let's calculate the moles of Al and O2 available:

Moles of Al = 0.32 mol
Moles of O2 = 0.26 mol

Now let's calculate the moles of Al and O2 required based on the stoichiometric ratio:

Moles of Al required = (Moles of O2 available) x (4 moles Al / 3 moles O2)
= 0.26 mol O2 x (4 mol Al / 3 mol O2)
= 0.3467 mol Al

Moles of O2 required = (Moles of Al available) x (3 moles O2 / 4 moles Al)
= 0.32 mol Al x (3 mol O2 / 4 mol Al)
= 0.24 mol O2

According to the calculations, 0.3467 moles of Al are required, but only 0.32 moles of Al are available. Therefore, Al is the limiting reactant. Your calculation of 0.24 mol Al and 0.35 mol O2 seems incorrect.