Presentation is loading. Please wait.

Presentation is loading. Please wait.

Stoichiometry Chap. 12. I.What is stoichiometry? Study of quantitative relationships between amounts of reactants and products.

Similar presentations


Presentation on theme: "Stoichiometry Chap. 12. I.What is stoichiometry? Study of quantitative relationships between amounts of reactants and products."— Presentation transcript:

1 Stoichiometry Chap. 12

2 I.What is stoichiometry? Study of quantitative relationships between amounts of reactants and products

3 I.What is stoichiometry? Mass is conserved during a chemical reaction. A.Stoichiometry is based on Lavoisier’s Law

4 I.What is stoichiometry? Coefficients give an important information for calculation A.Stoichiometry is based on Lavoisier’s Law B.Uses a balanced equation

5 Al 2 O 3 + C Al + CO 2 Coefficients in Equation

6 Al 2 O 3 + C Al + CO 2 Coefficients in Equation 2334

7 Al 2 O 3 + C Al + CO 2 Coefficients in Equation formula units 3 atoms 4 atoms 3 molecules

8 Al 2 O 3 + C Al + CO 2 Coefficients in Equation moles 3 moles 4 moles 3 moles

9 I.What is stoichiometry? A.Stoichiometry is based on Lavoisier’s Law B.Uses a balanced equation C.Involves mole conversions

10 I.What is stoichiometry? A.Stoichiometry is based on Lavoisier’s Law B.Uses a balanced equation C.Involves mole conversions 1.grams moles

11 I.What is stoichiometry? A.Stoichiometry is based on Lavoisier’s Law B.Uses a balanced equation C.Involves mole conversions 1.grams moles 2.particles moles

12 I.What is stoichiometry? A.Stoichiometry is based on Lavoisier’s Law B.Uses a balanced equation C.Involves mole conversions 1.grams moles 2.particles moles 3.liters moles

13 II. Mole to Mole ratio

14 A.Comes from equation

15 H 2 + O 2 H 2 O Coefficients in Equation

16 H 2 + O 2 H 2 O Coefficients in Equation moles 1 mole2 moles

17 H 2 + O 2 H 2 O Coefficients in Equation moles 1 mole2 moles 2 mol H 2 1 mol O 2 2 mol H 2 2 mol H 2 O 1 mol O 2 2 mol H 2 O some mole ratios from this equation:

18 II. Mole to Mole ratio A.Comes from equation B.Calculations

19 Self Check – Ex. 1 2C + O 2 2CO How many moles of oxygen are required to react with 4.2 moles of carbon?

20 Self Check – Ex. 2 2C + O 2 2CO How many moles of carbon monoxide can be formed when 3 moles of oxygen react?

21 III. Stoichiometry Calculations

22 A.Gram to grams

23 Self Check – Ex. 3 2C + O 2 2CO How many grams of carbon monoxide can be formed when 96 grams of oxygen react?

24 III. Stoichiometry Calculations A.Gram to grams B.Grams to molecules

25 Self Check – Ex. 4 CaCl AgNO 3 Ca(NO 3 ) 2 + 2AgCl How many formula units of silver chloride are formed when 111 g of calcium chloride react?

26 III. Stoichiometry Calculations A.Gram to grams B.Grams to molecules C.Grams to liters

27 Self Check – Ex. 5 Zn + HNO 3 H 2 + Zn(NO 3 ) 2 How many liters of hydrogen gas at STP could be formed when 6.00 g of zinc reacts with nitric acid?

28 IV. Limiting Reactants How do you ‘turn off’ a chemical reaction?

29 IV. Limiting Reactants A.Terms

30 IV. Limiting Reactants A.Terms 1.Limiting reactant Substance that runs out first in a chemical reaction, thus limits the amount of product.

31 IV. Limiting Reactants A.Terms 1.Limiting reactant 2.Excess reactant Reactant that is present in excess, thus is left over when a reaction stops.

32 IV. Limiting Reactants A.Terms B.An analogy

33 The following parts are used to make trikes: WheelsFramePedals Symbol: W Requirement: 3 Symbol: F Requirement: 1 Symbol: P Requirement: 2

34 What is the ‘chemical formula’ for this trike?

35 W 3 FP 2

36 Write the ‘balanced equation’ for trike-making.

37 3 W + 1 F + 2 P W 3 FP 2 ++

38 How much product (trikes) could you make with: Supplies 24 wheels 10 frames 14 pedals

39 IV. Limiting Reactants A.Terms B.An analogy C.A chemical example

40 How many grams of product can you make with: Supplies 28 g N 2 18 g H 2 N 2 + 3H 2 2 NH 3

41 Recognizing a limiting reactant problem:

42 There are two ‘givens’

43 Solving a limiting reactant problem:

44 Do two calculations, and pick the reactant that makes the smaller amount of product.

45 Self Check – Ex. 6 2Na + 1H 2 O 2NaOH + 2H 2 If 23.0 g of sodium reacts with 9.0 g of water, what mass of hydrogen gas is formed?

46 Self Check – Ex. 7 1Fe 2 O 3 + 3H 2 2Fe + 3H 2 O If 85.5 g of iron (III) oxide reacts with 15.7 g of hydrogen, what mass of iron is formed? What is the limiting reactant?

47 V. Percent Yield A value that tells how ‘successful’ a reaction is at making product.

48 V. Percent Yield A.Theoretical yield The mass of product that can be formed in a reaction (calculated value)

49 V. Percent Yield A.Theoretical yield B.Actual yield The mass of product that is produced in a reaction (measured by experiment)

50 V. Percent Yield A.Theoretical yield B.Actual yield C.Percent Yield Actual yield Theoretical yield x 100 Percent yield =

51 V. Percent Yield C.An analogy

52 V. Percent Yield C.An analogy What is the percent yield? 30 kernels

53 What is the percent yield? 30 kernels Actual yield Percent yield = Theoretical yield

54 What is the percent yield? 30 kernels Actual yield Percent yield = Theoretical yield = 30

55 What is the percent yield? 30 kernels Actual yield = 24 Percent yield = Theoretical yield = popped corn

56 What is the percent yield? 30 kernels Actual yield = 24 Percent yield = Theoretical yield = popped corn = 75%

57 V. Percent Yield A.Theoretical yield B.Actual yield C.Percent Yield D.An analogy E.Examples

58 Self Check – Ex. 8 2Ca + 2H 2 O 2Ca(OH) 2 + 1H 2 When 10.0 g of calcium reacts with excess water, 15.0 g of calcium hydroxide is recovered. What is the percent yield?

59 The end.


Download ppt "Stoichiometry Chap. 12. I.What is stoichiometry? Study of quantitative relationships between amounts of reactants and products."

Similar presentations


Ads by Google