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Lesson 3 Percentage Yield and Energy

Lesson 3 Percentage Yield and Energy. Sometimes reactions do not go to completion. Reaction can have yields from 1% to 100%. 1. How many grams of Fe are produced by the reaction of 100. g of Fe 2 O 3, if the percentage yield is 75.0%? 2Fe 2 O 3 + 3C  4Fe + 3CO 2 100. g ? g

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Lesson 3 Percentage Yield and Energy

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  1. Lesson 3 Percentage Yield and Energy

  2. Sometimes reactions do not go to completion.Reaction can have yields from 1% to 100%. 1. How many grams of Fe are produced by the reaction of 100. g of Fe2O3, if the percentage yield is 75.0%? 2Fe2O3 + 3C  4Fe + 3CO2 100. g ? g 100. g Fe2O3

  3. Sometimes reactions do not go to completion.Reaction can have yields from 1% to 100%. 1. How many grams of Fe are produced by the reaction of 100. g of Fe2O3, if the percentage yield is 75.0%? 2Fe2O3 + 3C  4Fe + 3CO2 100. g ? g 100. g Fe2O3 x 1 mole 159.6 g

  4. Sometimes reactions do not go to completion.Reaction can have yields from 1% to 100%. 1. How many grams of Fe are produced by the reaction of 100. g of Fe2O3, if the percentage yield is 75.0%? 2Fe2O3 + 3C  4Fe + 3CO2 100. g ? g 100. g Fe2O3 x 1 mole x 4 mole Fe 159.6 g 2 mole Fe2O3

  5. Sometimes reactions do not go to completion.Reaction can have yields from 1% to 100%. 1. How many grams of Fe are produced by the reaction of 100. g of Fe2O3, if the percentage yield is 75.0%? 2Fe2O3 + 3C  4Fe + 3CO2 100. g ? g 100. g Fe2O3 x 1 mole x 4 mole Fe x 55.8 g 159.6 g 2 mole Fe2O3 1 mole

  6. Sometimes reactions do not go to completion.Reaction can have yields from 1% to 100%. 1. How many grams of Fe are produced by the reaction of 100. g of Fe2O3, if the percentage yield is 75.0%? 2Fe2O3 + 3C  4Fe + 3CO2 100. g ? g 100. g Fe2O3 x 1 mole x 4 mole Fe x 55.8 g x 0.750 = 52.4 g 159.6 g 2 mole Fe2O3 1 mole

  7. Percentage Yield = Actual Yield x 100% Theorectical Yield Actual Yield is what is experimentally measured. Theoretical Yield is what is calculated using stoichiometry.

  8. 2. In an experiment 152. g of AgNO3 is used to make 75.1 g of Ag2SO4(s). Calculate the percentage yield. 75.1 g actual yield 2AgNO3(aq) + Na2SO4(aq) Ag2SO4(s) + 2NaNO3(aq) 152 g ? g 152. g AgNO3 x 1 mole 169.9 g

  9. 2. In an experiment 152. g of AgNO3 is used to make 75.1 g of Ag2SO4(s). Calculate the percentage yield. 75.1 g actual yield 2AgNO3(aq) + Na2SO4(aq) Ag2SO4(s) + 2NaNO3(aq) 152 g ? g 152. g AgNO3 x 1 mole x 1 Ag2SO4 169.9 g 2 mole AgNO3

  10. 2. In an experiment 152. g of AgNO3 is used to make 75.1 g of Ag2SO4(s). Calculate the percentage yield. 75.1 g actual yield 2AgNO3(aq) + Na2SO4(aq) Ag2SO4(s) + 2NaNO3(aq) 152 g ? g 152. g AgNO3 x 1 mole x 1 Ag2SO4 x 311.9 g = 139.5 g 169.9 g 2 mole AgNO3 1 mole

  11. 2. In an experiment 152. g of AgNO3 is used to make 75.1 g of Ag2SO4(s). Calculate the percentage yield. 75.1 g actual yield 2AgNO3(aq) + Na2SO4(aq) Ag2SO4(s) + 2NaNO3(aq) 152 g ? g 152. g AgNO3 x 1 mole x 1 Ag2SO4 x 311.9 g = 139.5 g 169.9 g 2 mole AgNO3 1 mole % yield = 75.1 x 100 %

  12. 2. In an experiment 152. g of AgNO3 is used to make 75.1 g of Ag2SO4(s). Calculate the percentage yield. 75.1 g actual yield 2AgNO3(aq) + Na2SO4(aq) Ag2SO4(s) + 2NaNO3(aq) 152 g ? g 152. g AgNO3 x 1 mole x 1 Ag2SO4 x 311.9 g = 139.5 g 169.9 g 2 mole AgNO3 1 mole % yield = 75.1 x 100 % = 53.8 % 139.5

  13. Energy Calculations The energy term in a balanced equation can be used to calculate the amount of energyconsumed or produced in an endothermic or exothermic reaction. 3. How much energy is required to produce 25.4 g of H2? 213 kJ + 2H2O 2H2 + O2 ? kJ 25.4 g

  14. Energy Calculations The energy term in a balanced equation can be used to calculate the amount of energyconsumed or produced in an endothermic or exothermic reaction. 3. How much energy is required to produce 25.4 g of H2? 213 kJ + 2H2O 2H2 + O2 ? kJ 25.4 g 25.4 g H2

  15. Energy Calculations The energy term in a balanced equation can be used to calculate the amount of energyconsumed or produced in an endothermic or exothermic reaction. 3. How much energy is required to produce 25.4 g of H2? 213 kJ + 2H2O 2H2 + O2 ? kJ 25.4 g 25.4 g H2 x 1 mole 2.02 g

  16. Energy Calculations The energy term in a balanced equation can be used to calculate the amount of energyconsumed or produced in an endothermic or exothermic reaction. 3. How much energy is required to produce 25.4 g of H2? 213 kJ + 2H2O 2H2 + O2 ? kJ 25.4 g 25.4 g H2 x 1 mole x 213 kJ 2.02 g 2 mole H2

  17. Energy Calculations The energy term in a balanced equation can be used to calculate the amount of energyconsumed or produced in an endothermic or exothermic reaction. 3. How much energy is required to produce 25.4 g of H2? 213 kJ + 2H2O 2H2 + O2 ? kJ 25.4 g 25.4 g H2 x 1 mole x 213 kJ = 1.34 x 103 kJ 2.02 g 2 mole H2

  18. 4. How many molecules of H2 can be produced when 452 kJ of energy if consumed? 2H2 + O2 2H2O + 213 kJ ? Molecules 452 kJ 452 kJ

  19. 4. How many molecules of H2 can be produced when 452 kJ of energy if consumed? 2H2 + O2 2H2O + 213 kJ ? Molecules 452 kJ 452 kJ x 2 moles H2 213 kJ

  20. 4. How many molecules of H2 can be produced when 452 kJ of energy if consumed? 2H2 + O2 2H2O + 213 kJ ? Molecules 452 kJ 452 kJ x 2 moles H2 x 6.02 x 1023 molecules 213 kJ 1 mole

  21. 4. How many molecules of H2 can be produced when 452 kJ of energy if consumed? 2H2 + O2 2H2O + 213 kJ ? Molecules 452 kJ 452 kJ x 2 moles H2 x 6.02 x 1023 molecules = 2.55 x 1024 molecs 213 kJ 1 mole

  22. 4. How many molecules of H2 can be produced when 452 kJ of energy if consumed? 2H2 + O2 2H2O + 213 kJ ? Molecules 452 kJ 452 kJ x 2 moles H2 x 6.02 x 1023 molecules = 2.55 x 1024 molecs 213 kJ 1 mole

  23. 5. How much energy is produced by an explosion of a 5.2 L balloon full of hydrogen at STP? 2H2 + O22H2O + 213 kJ 5.2 L ? kJ

  24. 5. How much energy is produced by an explosion of a 5.2 L balloon full of hydrogen at STP? 2H2 + O22H2O + 213 kJ 5.2 L ? kJ 5.2 L

  25. 5. How much energy is produced by an explosion of a 5.2 L balloon full of hydrogen at STP? 2H2 + O22H2O + 213 kJ 5.2 L ? kJ 5.2 L x 1 mole 22.4 L

  26. 5. How much energy is produced by an explosion of a 5.2 L balloon full of hydrogen at STP? 2H2 + O22H2O + 213 kJ 5.2 L ? kJ 5.2 L x 1 mole x 213 kJ 22.4 L 2 moles H2

  27. 5. How much energy is produced by an explosion of a 5.2 L balloon full of hydrogen at STP? 2H2 + O22H2O + 213 kJ 5.2 L ? kJ 5.2 L x 1 mole x 213 kJ= 25 kJ 22.4 L 2 moles H2 Home work Worksheet # 3 page 131

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