[student2007]

Hello,

The following problem was given as a take home homework assignment. I believe that I have this figured out correctly but would like anexperts opinion:

The reaction is:
Fe2O3 (s) + 3CO(g) --> 2Fe (s) + 3CO2 (g)

How many grams of iron can be produced from 4.50 Kg Fe2O3?

My solution:

Step 1:
4.50kg Fe2O3 x 1000g / 1kg = 4500 g Fe2O3

Step 2:
4500g Fe2O3 x 1 mole / 159.7 Fe2O3 = 28.18 moles Fe2O3

Step 3:
28.18 moles Fe2O3 x 2moles Fe2 / 1 mole Fe2O3 = 56.36 moles Fe2

Step 4 Final answer:
56.36 moles Fe2 x 111.7 g Fe2 / 1 mole Fe2 = 6295 g Fe2

I would like to verify that this is indeed correct. If not could someone guide me onto the right path without providing the answer (I can't learn that way).

Thanks,

[Yggdrasil]

Very good work.  Both your method and your answer is correct.  One minor detail is that you may want to pay attention to significant figures.  Since the starting amount is given to three significant figures, you should report only three significant figures in your answer.