OpenStudy (faith123):

If 7.65 grams of iron (III) oxide reacts with 6.85 grams of carbon monoxide to produce 5.10 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. unbalanced equation: Fe2O3 + CO “yields”/ Fe + CO2

4 years ago
OpenStudy (anonymous):

this would be your balanced equation...FE2O3 + 3CO=2Fe +3CO2

4 years ago
OpenStudy (anonymous):

you always start with what you are given which is the 7.63

4 years ago
OpenStudy (anonymous):

7.65 my fault, sorry i have a new computer keyboard and i'm getting used to it

4 years ago
OpenStudy (anonymous):

7.65 (1mol/156.694g)=0.04882 you get the 156.694 by adding together the elements atomic mass that you have

4 years ago
OpenStudy (anonymous):

you have 1 Fe2O3 and 3 CO so you have a ratio of 1:3

4 years ago
OpenStudy (anonymous):

0.04882 times 2 =0.9764

4 years ago
OpenStudy (anonymous):

the other one is 6.85g(1mol/28.01g/mol)=0.245CO

4 years ago
OpenStudy (anonymous):

your limiting reactant is your Fe2O3 because it is less than you co you take your moles of fe and multiply by 2 which is your 0.9764 above and you take that 0.9764 and mulitply it by 55.847g/mol which is all the atomic mass added together=5.35g

4 years ago
OpenStudy (anonymous):

since you need the percent yield i think that's the easiest part. it's actual/theoretical multiplied by 100%

4 years ago