11. Calculate the energy in KJ produced by the reaction of 10.0 g of hydrogen with excess oxygen. 2H2 + O2 2H2O + 213 KJ → 10.0 g H2 x 1 mole x 213 KJ = 527 KJ 2.02 g 2 mole 12. Calculate the theoretical yield in grams of Fe produced by the reaction of 5.67 g of iron III oxide. If the actual yield is 2.00 g calculate the percentage yield. 2Fe2O3 + 3C 4Fe +3CO2 → 5.67 g x 1 mole x 4 mole Fe x 55.8 g = 3.96 g Fe 159.6 g 2 mole Fe2O3 1 mole % = 2.00 g x 100 % = 50.4 % 3.96 g 13. Calculate the amount of CO2 produced by the reaction of 8.45 g of iron III oxide. If the percentage yield is 75 %, calculate the actual yield. 2Fe2O3 + 3C 4Fe +3CO2 → 8.45 g Fe2O3 x 1 mole x 3 mole CO2 x 44.0 g = 3.49 g CO2 x 0.75 = 2.6 g CO2 159.6 g 2 mole 1 mole 14. Calculate the number of moles CO2 produced by the reaction of 8.45 g of C. 2Fe2O3 + 3C 4Fe +3CO2 → 8.45 g C x 1mole x 3 mole CO2 = 0.704 mole CO2 12.0 g 3 mole C
11. Calculate the energy in KJ produced by the reaction of 10.0 g of hydrogen with excess oxygen. 2H2 + O2 → 2H2O + 213 KJ 10.0 g H2 x 1 mole x 213 KJ = 527 KJ 2.02 g 2 mole 12. Calculate the theoretical yield in grams of Fe produced by the reaction of 5.67 g of iron III oxide. If the actual yield is 2.00 g calculate the percentage yield. 2Fe2O3 + 3C → 4Fe +3CO2 5.67 g x 1 mole x 4 mole Fe x 55.8 g = 3.96 g Fe 159.6 g 2 mole Fe2O3 1 mole % = 2.00 g x 100 % = 50.4 % 3.96 g 13. Calculate the amount of CO2 produced by the reaction of 8.45 g of iron III oxide. If the percentage yield is 75 %, calculate the actual yield. 2Fe2O3 + 3C → 4Fe +3CO2 8.45 g Fe2O3 x 1 mole x 3 mole CO2 x 44.0 g = 3.49 g CO2 x 0.75 = 2.6 g CO2 159.6 g 2 mole 1 mole 14. Calculate the number of moles CO2 produced by the reaction of 8.45 g of C. 2Fe2O3 + 3C → 4Fe +3CO2 8.45 g C x 1mole x 3 mole CO2 = 0.704 mole CO2 12.0 g 3 mole C
unit_5_workbook_answers.docx