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Could someone do this chemistry question on limiting reactants please?

A mixture contains 1.00 kg of aluminium and 3.00 kg of iron oxide.
The equation for the reaction is:
2 Al + Fe2O3 → 2 Fe + Al2O3
Show that aluminium is the limiting reactant.
Relative atomic masses (Ar): O = 16 Al = 27 Fe = 56
What have you done so far?
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Polp
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Original post by GabiAbi84
What have you done so far?

I wasn't sure on how to approach the question but I tried figuring out the moles.
(edited 2 years ago)
Original post by Polp
I wasn't sure on how to approach the question but I tried figuring out the moles.


That’s the correct approach.
So what have you figured out?
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Polp
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Original post by GabiAbi84
That’s the correct approach.
So what have you figured out?

So I got 18.5 mols for the mixture that contains 1kg of aluminum and I got 18.75 mols for the iron oxide. Im not sure what to do to prove that aluminum is a limiting reactant and im not sure if my mole calculations are correct for the mixture.
Original post by Polp
So I got 18.5 mols for the mixture that contains 1kg of aluminum and I got 18.75 mols for the iron oxide. Im not sure what to do to prove that aluminum is a limiting reactant and im not sure if my mole calculations are correct for the mixture.

It’s just the fact aluminium has fewer moles so is the limiting reagent

Plus it’s a 2:1 ratio so 18.5 moles aluminium reacts with 9.25 moles iron oxide
(edited 2 years ago)
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Polp
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Original post by Hellllpppp
It’s just the fact aluminium has fewer moles so is the limiting reagent

ight thx
Original post by Hellllpppp
It’s just the fact aluminium has fewer moles so is the limiting reagent

thanks what a coincident i was stuck on this question too thanks

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