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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.

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Presentation on theme: "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."— Presentation transcript:

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 Fe 2 O 3, if the percentage yield is 75.0%? 2Fe 2 O 3 +3C  4Fe+3CO 2 100. g? g 100. g Fe 2 O 3

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 Fe 2 O 3, if the percentage yield is 75.0%? 2Fe 2 O 3 +3C  4Fe+3CO 2 100. g? g 100. g Fe 2 O 3 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 Fe 2 O 3, if the percentage yield is 75.0%? 2Fe 2 O 3 +3C  4Fe+3CO 2 100. g? g 100. g Fe 2 O 3 x 1 mole x 4 mole Fe 159.6 g 2 mole Fe 2 O 3

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 Fe 2 O 3, if the percentage yield is 75.0%? 2Fe 2 O 3 +3C  4Fe+3CO 2 100. g? g 100. g Fe 2 O 3 x 1 mole x 4 mole Fe x 55.8 g 159.6 g 2 mole Fe 2 O 3 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 Fe 2 O 3, if the percentage yield is 75.0%? 2Fe 2 O 3 +3C  4Fe+3CO 2 100. g? g 100. g Fe 2 O 3 x 1 mole x 4 mole Fe x 55.8 g x 0.750 = 52.4 g 159.6 g 2 mole Fe 2 O 3 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.

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9 2.In an experiment 152. g of AgNO 3 is used to make 75.1 g of Ag 2 SO 4(s). Calculate the percentage yield. 75.1 g actual yield 2AgNO 3(aq) + Na 2 SO 4(aq)  Ag 2 SO 4(s) + 2NaNO 3(aq) 152 g ? g 152. g AgNO 3 x 1 mole 169.9 g

10 2.In an experiment 152. g of AgNO 3 is used to make 75.1 g of Ag 2 SO 4(s). Calculate the percentage yield. 75.1 g actual yield 2AgNO 3(aq) + Na 2 SO 4(aq)  Ag 2 SO 4(s) + 2NaNO 3(aq) 152 g ? g 152. g AgNO 3 x 1 mole x 1 Ag 2 SO 4 169.9 g 2 mole AgNO 3

11 2.In an experiment 152. g of AgNO 3 is used to make 75.1 g of Ag 2 SO 4(s). Calculate the percentage yield. 75.1 g actual yield 2AgNO 3(aq) + Na 2 SO 4(aq)  Ag 2 SO 4(s) + 2NaNO 3(aq) 152 g ? g 152. g AgNO 3 x 1 mole x 1 Ag 2 SO 4 x 311.9 g = 139.5 g 169.9 g 2 mole AgNO 3 1 mole

12 2.In an experiment 152. g of AgNO 3 is used to make 75.1 g of Ag 2 SO 4(s). Calculate the percentage yield. 75.1 g actual yield 2AgNO 3(aq) + Na 2 SO 4(aq)  Ag 2 SO 4(s) + 2NaNO 3(aq) 152 g ? g 152. g AgNO 3 x 1 mole x 1 Ag 2 SO 4 x 311.9 g = 139.5 g 169.9 g 2 mole AgNO 3 1 mole % yield = 75.1 x 100 %

13 2.In an experiment 152. g of AgNO 3 is used to make 75.1 g of Ag 2 SO 4(s). Calculate the percentage yield. 75.1 g actual yield 2AgNO 3(aq) + Na 2 SO 4(aq)  Ag 2 SO 4(s) + 2NaNO 3(aq) 152 g ? g 152. g AgNO 3 x 1 mole x 1 Ag 2 SO 4 x 311.9 g = 139.5 g 169.9 g 2 mole AgNO 3 1 mole % yield = 75.1 x 100 %=53.8 % 139.5

14 Energy Calculations The energy term in a balanced equation can be used to calculate the amount of energy consumed or produced in an endothermic or exothermic reaction. 3.How much energy is required to produce 25.4 g of H 2 ? 213 kJ +2H 2 O  2H 2 +O 2 ? kJ25.4 g

15 Energy Calculations The energy term in a balanced equation can be used to calculate the amount of energy consumed or produced in an endothermic or exothermic reaction. 3.How much energy is required to produce 25.4 g of H 2 ? 213 kJ +2H 2 O  2H 2 +O 2 ? kJ25.4 g 25.4 g H 2

16 Energy Calculations The energy term in a balanced equation can be used to calculate the amount of energy consumed or produced in an endothermic or exothermic reaction. 3.How much energy is required to produce 25.4 g of H 2 ? 213 kJ +2H 2 O  2H 2 +O 2 ? kJ25.4 g 25.4 g H 2 x 1 mole 2.02 g

17 Energy Calculations The energy term in a balanced equation can be used to calculate the amount of energy consumed or produced in an endothermic or exothermic reaction. 3.How much energy is required to produce 25.4 g of H 2 ? 213 kJ +2H 2 O  2H 2 +O 2 ? kJ25.4 g 25.4 g H 2 x 1 mole x 213 kJ 2.02 g2 mole H 2

18 Energy Calculations The energy term in a balanced equation can be used to calculate the amount of energy consumed or produced in an endothermic or exothermic reaction. 3.How much energy is required to produce 25.4 g of H 2 ? 213 kJ +2H 2 O  2H 2 +O 2 ? kJ25.4 g 25.4 g H 2 x 1 mole x 213 kJ = 1.34 x 10 3 kJ 2.02 g2 mole H 2

19 4.How many molecules of H 2 can be produced when 452 kJ of energy if consumed? 2H 2 +O 2  2H 2 O +213 kJ ? Molecules452 kJ 452 kJ

20 4.How many molecules of H 2 can be produced when 452 kJ of energy if consumed? 2H 2 +O 2  2H 2 O +213 kJ ? Molecules452 kJ 452 kJ x 2 moles H 2 213 kJ

21 4.How many molecules of H 2 can be produced when 452 kJ of energy if consumed? 2H 2 +O 2  2H 2 O +213 kJ ? Molecules452 kJ 452 kJ x 2 moles H 2 x 6.02 x 10 23 molecules 213 kJ 1 mole

22 4.How many molecules of H 2 can be produced when 452 kJ of energy if consumed? 2H 2 +O 2  2H 2 O +213 kJ ? Molecules452 kJ 452 kJ x 2 moles H 2 x 6.02 x 10 23 molecules = 2.55 x 10 24 molecs 213 kJ 1 mole

23 4.How many molecules of H 2 can be produced when 452 kJ of energy if consumed? 2H 2 +O 2  2H 2 O +213 kJ ? Molecules452 kJ 452 kJ x 2 moles H 2 x 6.02 x 10 23 molecules = 2.55 x 10 24 molecs 213 kJ 1 mole

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

25 5.How much energy is produced by an explosion of a 5.2 L balloon full of hydrogen at STP? 2H 2 +O 2  2H 2 O +213 kJ 5.2 L? kJ 5.2 L

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

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

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

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