1. Modern Chemistry Chapter 9 Stoichiometry
Sections 1-3 Introduction to Stoichiometry Ideal Stoichiometric Calculations Limiting Reactant and Percent Yield

2. Chapter 9 Vocabulary Composition Stoichiometry Reaction Stoichiometry
Mole Ratio
Limiting Reactant
Excess Reactant
Actual Yield
Theoretical Yield
Percent Yield

3. Chapter 9 Section 1 Introduction to Stoichiometry
Chapter 9 Section 1 Intro. Stoichiometry pages

4. Chapter 9 Section 1 Intro. Stoichiometry pages 299-303
Definitions
Composition stoichiometry deals with the mass relationships of elements in compounds.
Reaction stoichiometry involves the mass relationships between reactants and products in a chemical reaction.
Chapter 9 Section 1 Intro. Stoichiometry pages

5. Stoichiometry Animation
Chapter 9 Section 1 Intro. Stoichiometry pages
p. xx

6. Chapter 9 Section 1 Intro. Stoichiometry pages 299-303
Definitions
A mole ratio is a conversion factor that relates the amounts in moles of any two substances involved in a chemical reaction
Example: 2Al2O3(l)  4Al(s) + 3O2(g)
Mole Ratios: 2 mol Al2O mol Al2O mol Al
4 mol Al 3 mol O mol O2
Chapter 9 Section 1 Intro. Stoichiometry pages

7. Chapter 9 Section 1 Intro. Stoichiometry pages 299-303
Using the Mole Ratio
Chapter 9 Section 1 Intro. Stoichiometry pages
p. xx

8. Mg(s) + 2HCl(aq)  MgCl2(aq) + H2(g)
Mole – Mole Examples
Mg(s) + 2HCl(aq)  MgCl2(aq) + H2(g)
If 2 mol of HCl react, how many moles of H2 are obtained?
How many moles of Mg will react with 2 mol of HCl?
If 4 mol of HCl react, how many mol of each product are produced?
How would you convert from moles of substances to masses?
Chapter 9 Section 1 Intro. Stoichiometry pages

9. Chapter 9 Section 1 Intro. Stoichiometry pages 299-303
Converting from gmol
Chapter 9 Section 1 Intro. Stoichiometry pages
p. xx

10. Chapter 9 Section 1 Intro. Stoichiometry pages 299-303
Section 1 Homework
Page 301 #1-4
Chapter 9 Section 1 Intro. Stoichiometry pages

11. Chapter 9 Section 2 Ideal Stoichiometric Calculations
Chapter 9 Section 2 Ideal Stoichiometry pages

12. Reactants  Products MASS OF SUBSTANCE GIVEN MASS OF SUBSTANCE WANTED
MOLAR MASS
MOLAR MASS
MOLES OF SUBSTANCE GIVEN
MOLES OF SUBSTANCE WANTED
MOLE RATIO
Chapter 9 Section 2 Ideal Stoichiometry pages

13. Chapter 9 Section 2 Ideal Stoichiometry pages 304-311
Tool Box
GRAMSmL
DENSITY
GRAMSMOLES
MOLAR MASS
MOLES MOLES
MOLE RATIO
MOLES PARTICLES
6.02x1023
1000 g = 1kg
1000 mL = 1L
1000 mg = 1g
Chapter 9 Section 2 Ideal Stoichiometry pages

14. Chapter 9 Section 2 Ideal Stoichiometry pages 304-311Kg L mg mL g
MOLES
MOLES g mg mL L Kg
Chapter 9 Section 2 Ideal Stoichiometry pages

15. Chapter 9 Section 2 Ideal Stoichiometry pages 304-311
Sample Problem
How many kilograms of ethane are required to react with excess oxygen to produce 8.70 L of carbon dioxide? The density of carbon dioxide gas at standard temperature is g/L. kg
Chapter 9 Section 2 Ideal Stoichiometry pages

16. Chapter 9 Section 2 Ideal Stoichiometry pages 304-311Kg L mg mL g
MOLES
MOLES g mg mL L Kg
Chapter 9 Section 2 Ideal Stoichiometry pages

17. Chapter 9 Section 2 Ideal Stoichiometry pages 304-311
L CO2
g CO2
mol CO2
mol C2H6
g C2H6
kg C2H6 x x x x x
L CO2
g CO2
mol CO2
mol C2H6
g C2H6 Kg g
MOLES
MOLES g L
Chapter 9 Section 2 Ideal Stoichiometry pages

18. C2H6 (g) + O2 (g)  CO2 (g) + H2O (g) + E
8.70L
? Kg g g
MOLES
MOLES
L CO2
g CO2
mol CO2
mol C2H6
g C2H6
kg C2H6 x x x x x
L CO2
g CO2
mol CO2
mol C2H6
g C2H6
Chapter 9 Section 2 Ideal Stoichiometry pages

19. C2H6 (g) + O2 (g)  CO2 (g) + H2O (g) + E
8.70L
? Kg g g
1000g=1Kg
MOLAR
MASS
MOLAR
MASS
MOLAR
RATIO
MOLES
MOLES
DENSITY
L CO2
g CO2
mol CO2
mol C2H6
g C2H6
kg C2H6 x x x x x
L CO2
g CO2
mol CO2
mol C2H6
g C2H6
Chapter 9 Section 2 Ideal Stoichiometry pages

20. Chapter 9 Section 2 Ideal Stoichiometry pages 304-311
Sample Problem p. 306
In photosynthesis, plants use energy from the sun to produce glucose, C6H12O6, and oxygen from the reaction of carbon dioxide and water.
What mass, in grams, of glucose is produced when 3.00 mol of water react with carbon dioxide?
90.1 g C6H12O6
Chapter 9 Section 2 Ideal Stoichiometry pages
mol-mass

21. Chapter 9 Section 2 Ideal Stoichiometry pages 304-311
Sample Problem p. 310
Tin (II) fluoride, SnF2, is used in some toothpastes. It is made by the reaction of tin with hydrogen fluoride according to the following equation.
Sn(s) + 2HF(g)  SnF2(s) + H2(g)
How many grams of SnF2 are produced from the reaction of g HF with Sn?
117.5 g SnF2
Chapter 9 Section 2 Ideal Stoichiometry pages
mass-mass.

22. Chapter 9 Section 2 Ideal Stoichiometry pages 304-311
Sample Problem p. 305
In a spacecraft, the carbon dioxide exhaled by astronauts can be removed by its reaction with lithium hydroxide, LiOH, according to the following chemical equation.
CO2(g) + 2LiOH(s)  Li2CO3(s) + H2O(l)
How many moles of lithium hydroxide are required to react with 20 mol CO2, the average amount exhaled by a person each day?
40 mol LiOH
Chapter 9 Section 2 Ideal Stoichiometry pages
mol-mol

23. Chapter 9 Section 2 Ideal Stoichiometry pages 304-311
Sample Problem p. 309
The first step in the industrial manufacture of nitric acid is the catalytic oxidation of ammonia.
NH3(g) + O2(g)  NO(g) + H2O(g) (unbalanced)
The reaction is run using 824 g NH3 and excess oxygen.
a. How many moles of NO are formed?
b. How many moles of H2O are formed?
48.4mol NO; mol H2O
Chapter 9 Section 2 Ideal Stoichiometry pages
mass-mol

24. Chapter 9 Section 2 Ideal Stoichiometry pages 304-311
Problem
Magnesium burns in oxygen to produce magnesium oxide. How many grams magnesium will burn in the presence of 189 mL of oxygen? The density of oxygen is 1.429g/L.
0.410 g Mg
Chapter 9 Section 2 Ideal Stoichiometry pages
mL-g

25. Chapter 9 Section 2 Ideal Stoichiometry pages 304-311
Problem
Limestone, CaCO3, can be decomposed with heat to form lime, CaO, and carbon dioxide. How many moles of lime would be formed from the decomposition of 20.1 kilograms of limestone?
201 moles CaO
Chapter 9 Section 2 Ideal Stoichiometry pages
Kg-mol.

26. Chapter 9 Section 2 Ideal Stoichiometry pages 304-311
Section 2 Homework
Page 311 #1-5
Chapter 9 Section 2 Ideal Stoichiometry pages

27. Section 2 Homework Problem Bank
Page #176, 177, 179, 180, 184, 187, 190, 191, 192, 194, 196
Chapter 9 Section 2 Ideal Stoichiometry pages

28. Chapter 9 Section 3 Limiting Reactant and Percent Yield
Chapter 9 Section 3 Limiting Reactant pages

29. Chapter 9 Section 3 Limiting Reactant pages 312-318
Definitions
The limiting reactant is the reactant that limits the amount of the other reactant that can combine and the amount of product that can form in a chemical reaction.
The excess reactant is the substance that is not used up completely in a reaction.
Chapter 9 Section 3 Limiting Reactant pages

30. Chapter 9 Section 3 Limiting Reactant pages 312-318
S’mores
Given the bag o’ reactants find the number of s’mores you could produce if the balanced equation is
2 Tg + 1 Mm  1 Sm
Tg = Teddy Graham
Mm = Minimarshmallow
Sm = S’more
Chapter 9 Section 3 Limiting Reactant pages

31. Chapter 9 Section 3 Limiting Reactant pages 312-318
S’mores
What is the limiting reactant?
What is the reactant in excess?
What is the amount in excess ?
What is the theoretical yield?
What is the actual yield?
What is the percent yield?
Chapter 9 Section 3 Limiting Reactant pages

32. Chapter 9 Section 2 Ideal Stoichiometry pages 304-311
Sample Problem p. 313
Silicon dioxide (quartz) is usually quite unreactive but reacts readily with hydrogen fluoride according to the following equation.
SiO2(s) + 4HF(g)  SiF4(g) + 2H2O(l)
If 6.0 mol HF is added to 4.5 mol SiO2, which is the limiting reactant? HF
Chapter 9 Section 2 Ideal Stoichiometry pages
mol & mol limiting

33. Chapter 9 Section 3 Limiting Reactant pages 312-318
Problem
I need a problem that requires them to answer these questions
a. Which compound is the limiting reactant?
b. What is the theoretical yield of product?
c. What is the reactant in excess, and how much remains after the reaction is completed?
8.940 x 1023 molecules
Chapter 9 Section 3 Limiting Reactant pages
mass & mass, limiting, actual

34. Chapter 9 Section 3 Limiting Reactant pages 312-318
Problem
I need another problem that requires them to answer these questions
a. Which compound is the limiting reactant?
b. What is the theoretical yield of product?
c. What is the reactant in excess, and how much remains after the reaction is completed?
8.940 x 1023 molecules
Chapter 9 Section 3 Limiting Reactant pages
mass & mass, limiting, actual

35. Chapter 9 Section 3 Limiting Reactant pages 312-318
p. xx

36. Chapter 9 Section 3 Limiting Reactant pages 312-318
Section 3 Homework
Page 318 #1 & 2
Chapter 9 Section 3 Limiting Reactant pages

37. Chapter 9 Section 3 Limiting Reactant pages 312-318
Definitions
The theoretical yield is the maximum amount of product that can be produced from a give amount of reactant.
The actual yield is the measured amount of product obtained from a reaction.
The percentage yield is the ratio of the actual yield to the theoretical yield, multiplied by 100.
Chapter 9 Section 3 Limiting Reactant pages

38. Chapter 9 Section 3 Limiting Reactant pages 312-318
Percent Yield
Chapter 9 Section 3 Limiting Reactant pages
p. xx

39. Chapter 9 Section 2 Ideal Stoichiometry pages 304-311
Sample Problem p. 317
Chlorobenzene, C6H5Cl, is used in the production of many important chemicals, such as aspirin, dyes, and disinfectants. One industrial method of preparing chlorobenzene is to react benzene, C6H6, with chlorine, as represented by the following equation.
C6H6 (l) + Cl2 (g)  C6H5Cl (l) + HCl (g)
When 36.8 g C6H6 react with an excess of Cl2, the actual yield of C6H5Cl is 38.8 g.
What is the percentage yield of C6H5Cl?
73.2%
Chapter 9 Section 2 Ideal Stoichiometry pages
mass-mass percent

40. Chapter 9 Section 3 Limiting Reactant pages 312-318
Problem
Hydrogen sulfide gas can be formed by the action of HCl and FeS, forming FeCl2 as product. What is the theoretical yield in molecules of hydrogen sulfide if g of FeS are mixed with g of HCl? If the percent yield in the lab is 93.6% what is the actual yield?
8.940 x 1023 molecules
Chapter 9 Section 3 Limiting Reactant pages
mass & mass, limiting, actual

41. Chapter 9 Section 2 Ideal Stoichiometry pages 304-311
Problem
Benzene, C6H6, is reacted with bromine, Br2, to produce bromobenzene, C6H5Br, and hydrogen bromide, HBr, as shown below. When 40.0 g of benzene are reacted with 95.0 g of bromine, 65.0 g of bromobenzene is produced.
C6H6 + Br2  C6H5Br + HBr
a. Which compound is the limiting reactant?
b. What is the theoretical yield of bromobenzene?
c. What is the reactant in excess, and how much remains after the reaction is completed?
d. What is the percentage yield?
Benzene, 80.4g, Br2 13.2g, 80.8%
Chapter 9 Section 2 Ideal Stoichiometry pages

42. Chapter 9 Section 3 Limiting Reactant pages 312-318
Molarity
Molarity measures the concentration of solutions. (aq)
Molarity = moles / liter
3 mol
3M =
1 L
Chapter 9 Section 3 Limiting Reactant pages

43. Chapter 9 Section 3 Limiting Reactant pages 312-318
Problem
When 20.0 mL of 0.90M solution of lithium nitrate and 15.0 mL of 0.40M solution of calcium phosphate react, a precipitate is formed. The mass of the precipitate produced in the lab is 0.66 grams. What is the reactant in excess, the limiting reactant, the amount in excess, the theoretical yield and the percent yield.
0.69 grams theo.
Chapter 9 Section 3 Limiting Reactant pages

44. Section 3 Homework Problem Bank
Page #201, 208, 214, 217, 219, 223, 226, 229, 232
Chapter 9 Section 3 Limiting Reactant pages