Question

0.329 g of fe3o4 and 0.812 g of al are available for the following reaction.
3fe3o4 + 8al ----> 4al2o3 + 9fe

a. what reactant is the limiting reagent and which reactant is in the excess
b. how many grams of iron(fe) would be formed.

I need solution, thanks

Answer 1

Please keep in mind the intention of this site is to teach rather than to give away answers.

For part a) use stoichiometry to determine how much product each reactant can make. Starting with the equation, we check to see if it is balanced. It is, so we can move on to the next step.

Using 0.329g Fe3O4, divide by the molar mass of Fe3O4 to get to moles Fe3O4. Then use the balanced equation ratios to convert moles Fe3O4 to moles product (it asks about Fe in part b so let’s use Fe as our product).

The balanced equation tells us that 3 moles Fe3O4 makes 9 moles Fe, so you’d divide moles Fe3O4 by 3 and then multiply by 9 to get moles Fe.

Repeat this process with the other reactant.

Finally, compare the two reactants. Which one made less Fe? Whichever one it is is your limiting reactant.

Answer 2

For part b, whichever limiting reactant you got from part a, use the moles Fe you got from that. That’s how many moles of Fe your reaction makes. From there, multiply by the molar mass of Fe to get grams Fe.

Answer 3

thank you , another question summarize answers in a table?

Answer 4

I’m not sure what you mean. Once you have your solutions, organize them in a table?

Answer 5

something like that