HOW TO SOLVE THIS....

I think I'm right, but I when it comes to stoichiometry i doub it,

The problem is:
Calculate the amounts requested if 3.30 mol of Fe2O3 completely react according to the following equation:
Fe2O3 +2Al ---> 2Fe + Al2 O3

a) moles of Al needed
b) moles of iron formed
c) moles of aluminum oxide formed

For a) I got 6.6 mol of Al because I did:
3.30 mol Fe2O3 X 2 mol Al/1 mol Fe2O3 = 6.6 mol Al

Is this wrong or right? Anyone explain please?

It is correct - the equation shows that for every mole of Fe2O3, you need 2 moles of Al, just as you calculated. You do need to watch significant figures though - the full answer is 6.60 moles

The correct answer for b will also be 6.60

The correct answer for c will be 3.30

yes it is absolutely right.Since the mole ratio in the given equation is 1:2.every 1 mole of Fe2O3 requires two moles of Al.so u just have to multiply.

I think it should be 6.60 because of significant figures. Other than that, it's the right answer :)