Can someone please help me with stoichiometry

(Part 1 of 2)

The solid fuel in the booster stage of the space shuttle is a mixture of ammonium perchlorate
and aluminum powder. On ignition, the reaction that takes place is
6NH4ClO4(s) + 10Al(s) --> 5Al2O3(s) + 3N2(g) + 6HCl(g) + 9H2O(g) .
What mass of aluminum is required to react with 1.696 kg of NH4ClO4 for this reaction?
Answer in units of g.

(Part 2 of 2)

What mass of Al2O3 (alumina, a finely divided white powder that is produced as billows of white smoke) is formed in the reaction of 1100 kg of aluminum?
Answer in units of kg.

Ok, so the molar mass of NH4ClO4 is 117.45 g/mol
1.696 kg is 1696 grams, so 1696 / 117.45 is 14.44 moles NH4ClO4.

Then, using the mol ratios, for every 6 moles NH4ClO4 used, 10 moles Aluminum is used. multiply 14.44 by 10/6 and that's the amount of moles which is 24.1.

then, the molar mass of aluminum is 26.98, so multiply 24.1 by that, and it's 649.31 grams aluminum.

Use mole ratios again to find the white powder (dont forget to convert to kg)

10 to 6 relation

divide 1.696kg by the molar mass of NH4ClO4 to find moles

then times answer by (10/6) to find moles Al

times moles Al by molar mass of Al

then you'll get the answer