If 12.8 grams of iron (III) oxide reacts with 11.5 grams of carbon monoxide to produce 6.10 g of pure iron, what are the theoretical yield and percent yield of this reaction? Be sure to show the work that you did to solve this problem. (4 points)

unbalanced equation: Fe2O3 + CO yields Fe + CO2

Question

If 12.8 grams of iron (III) oxide reacts with 11.5 grams of carbon monoxide to produce 6.10 g of pure iron, what are the theoretical yield and percent yield of this reaction? Be sure to show the work that you did to solve this problem. (4 points)

unbalanced equation: Fe2O3 + CO yields Fe + CO2

anonymous · Answer

@abb0t helppp! please :)

abb0t · Answer

$\sf \color{}{Fe_2O_3 + CO \rightarrow Fe + CO_2}$ now, you need to start by balancing this. Do you know how to balance?

anonymous · Answer

Fe2O3 + 3 CO = 2 Fe + 3 CO2 

is that correct?

abb0t · Answer

Yes, that is correct. Good job.

anonymous · Answer

Cool :)

abb0t · Answer

Now find the mass of each and convert to the products, which is CO$_2$. you are essentially trying to find out how much of each you would theoretically produce with the given amounts

abb0t · Answer

So, convert 12.8 grams of Fe$_2$O$_3$ and 11.5 grams of CO to Fe and CO$_2$.

abb0t · Answer

aRE You familiar with how to convert to iron and carbon dioxide? Meaning, use of dimensional analysis.

anonymous · Answer

Fe2O3 = 12.8 g / 159.694 g / mol = 0.0802

anonymous · Answer

No.. This is not a practice exam. This is a module quiz from FLVS so using this answer will be an academic integrity violation. Plus it has a obvious mistake in it. 

Mr. Carlyle 
FLVS Chemistry Instructor 

This question is a violation of the OpenStudy Guidelines. The question is from an online school plus a violation by solicitation for members to unknowingly assist them cheating on an exam. 30653065chem30653065