How many grams of iron can be produced from 14.0g of Al and excess Fe3O4?

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SUMMARY

The discussion focuses on calculating the grams of iron produced from 14.0g of aluminum (Al) when reacted with excess iron(II,III) oxide (Fe3O4). The balanced chemical equation is 8Al(s) + 3Fe3O4 = 9Fe(s) + 4Al2O3(s). Using stoichiometry, participants emphasize the need to convert grams of Al to moles and apply the mole ratio from the balanced equation to find the mass of iron produced. The correct approach involves determining the moles of Al and using the stoichiometric coefficients to calculate the resultant iron mass.

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Homework Statement


Al(s) + Fe3 O4 = Fe (s) + Al2 O3(s)
calculate how many grams of iron can be produced when 14.0g of Al are combined with excess FeO4.


Homework Equations





The Attempt at a Solution



I know that I need to balance the solution which is:
8Al(s) + 3Fe3 O4 = 9Fe (s) + 4Al2 O3(s)

net/ionic eq

8al + 3fe3o4 = 9fe + 4al2 o3

can someone please help me on this I can't get any further on finding the excess on using the net or balance ionic equation. I can't really cancel any out that are the same on both side. please help.
 
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Start with the number of MOLES of Aluminum. Find the other necessary ratios from your balanced reaction.
 
There is no net ionic reaction here (it is not happening in the solution and neither of the substances is dissociated) and the one you have is properly balanced.

Simple stoichiometry now - how many moles of Al? How many moles of iron produced per mole of Al?

--
 

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