What mass of iron oxide is produced when 11.2g of Iron burns? Could you please check my working and answer?

Question

Fe(s) + 3O2(s) = 2Fe2 O3(s)

There is 1 mole of Fe and 2 moles of 2Fe2 O3.

1 mole of Fe is 56g and 2 moles of 2Fe2 O3 is 320g.

(56/56)*11.2g gives you 11.2g of iron, as asked for in the question, so we must do the same calculation for 2Fe2 O3.

so, (320/56)*11.2g = 64g

Therefore, 64g of iron oxide is produced.

Answer 1

Answer's wrong pal!
First balance the reaction :
4Fe(s) + 3O2(s) = 2Fe2 O3(s)

4 mol of Fe(s) = 2 mol of Fe2 O3(s)
2 mol of Fe(s) = 1 mol of Fe2 O3(s)

2 mol of Fe is 112g and 1 mol of Fe2 O3 is 160 g

11.2 g Fe(s) = 0.2 mol of Fe(s)
That gives on oxidation 0.1 mol Fe2 O3(s) = 16 g

Therefore, 16 g of iron oxide is produced.

Answer 2

15605gm