C6H6O3 + 6O2 --> 6 CO2 + 3 H2O 40.8 g of C6H6O3 g reacts and 11.8 g of H2O are produced. What is the % yield of H2O?

Answer 1

1. We would have to convert grams of C6H6O3 to Mols of C6H6O3. We do this by using the molar mass found in the periodic table of elements (these may vary slightly depending on your source).
2. Carbon- 12.011g/mol. 6*12.011g/mol= 72.066g/mol
3. Hydrogen- 1.008g/mol. 6*1.008g/mol= 6.048g/mol
4. Oxygen- 15.999g/mol. 3*15.999g/mol= 47.997g/mol
5. 72.066g/mol+6.048g/mol+47.997g/mol= 126.111g/mol
6. C6H6O3 molecular mass= 126.111g/mol
7. Divide grams of C6H6O3 by the molecular mass to get mols of C6H6O3. 40.8g/126.111g/mol= 0.324 mols
8. According to the chemical equation, for every 1 mol of C6H6O3, the chemical reaction produces 3 mols of H2O. Now we have to multiply the mols of C6H6O3 by 3 to get the mols of H2O.
9. 3*0.324 mols of C6H6O3=0.972mols of H2O
10. We now have to convert mols of H2O into grams of H2O. We do this by using the molar mass found in the periodic table of elements (these may vary slightly depending on your source).
11. Hydrogen- 1.008g/mol. 3*1.008g/mol= 3.024g/mol
12. Oxygen- 15.999g/mol. 1*15.999g/mol= 15.999g/mol
13. 3.024g/mol+15.999g/mol= 19.023g/mol
14. H2O Molecular mass=19.023g/mol
15. 0.972mols H2O*19.023g/mol (molecular mass)= 18.490g which is our theoretical yield.
16. We now have to take our actual yield and divide it by our theoretical yield and then multiply by 100 to get our %yield. *Theoretical yield was rounded to 18.5g*
17. (11.8g/18.5g)*100= 63.8% yield.