1. New Section in Table of Contents
Stoichiometry Notes
New Section in Table of Contents

2. Real Life Application Ingredients 2 1/4 cups all-purpose flour
1 teaspoon baking soda
1 teaspoon salt
1 cup (2 sticks) butter, softened
3/4 cup granulated sugar
3/4 cup packed brown sugar
1 teaspoon vanilla extract
2 large eggs
2 cups (12-oz. pkg.) NESTLÉ® TOLL HOUSE® Semi-Sweet Chocolate Morsels
1 cup chopped nuts

3. Real Life Application
We cannot forget about the law of conservation of mass.
The mass of what we put in must be equal to what we get out.
KC 1: The excess reactants are all the leftover unused reactants. (The reactant that’s leftover).

4. Particle and Mole Relationships
Chemical reactions stop when one of the reactants is used up
KC 2: Stoichiometry is the study of quantitative relationships between the amounts of reactants used and amounts of products formed by a chemical reaction
So based on how much reactant you put in you can calculate how much product you will get out
Quick demo of baking soda.

5. Particle and Mole Relationships

6. Particle and Mole Relationships
KC 3: A mole ratio is a ratio between the numbers of moles of any 2 substances in a balanced equation
This can only be determined from a balanced chemical equation

7. Particle and Mole Relationships
Let practice: What is the mole-to-mole ratio for…
10C2H4O + 15O2  20CO2 + 2H2O
CH4 + 2O2  CO2 + 2H2O
H2 + O2  H2O

8. Using Stoichiometry
Mol CH4
Mole H2O
CH4 + 2O2  CO2 + 2H2O

9. Using Stoichiometry
Key Concept 4: How many moles of SO3 are formed if you start with 5 moles of Sulfur and have excess Oxygen? ____S + ____O2  ____SO3
2nd Hour

10. Using Stoichiometry 4Fe(s) + 3O2(g)  2Fe2O3(s) Mol Fe Mole Fe2O3

11. Using Stoichiometry
How many grams of Fe2O3 are formed when g of iron reacts with excess oxygen using the balanced chemical equation below:
4Fe(s) + 3O2(g)  2Fe2O3(s)

12. Using Stoichiometry
Key Concept 5:
How many grams of lithium nitrate will be needed to make 250 grams of lithium sulfate, assuming that you have an adequate amount of lead (IV) sulfate to do the reaction?
____Pb(SO4)2 + ____LiNO3  ____Pb(NO3)4 + ____Li2SO4

13. Using Stoichiometry ____NaOH + ____H2SO4  ____H2O + ____Na2SO4
Key Concept 6:
How many grams of sodium sulfate will be formed if you start with 200 grams of sodium hydroxide and you have an excess of sulfuric acid?
____NaOH + ____H2SO4  ____H2O + ____Na2SO4
1st hour

14. Using Stoichiometry New Conversion Factor:
1 mol of gas = 22.4L (at STP = standard temperature and pressure)
How many moles of sodium chloride are in 3.87 L?
How many grams of sodium chloride are in 3.87L?

15. Using Stoichiometry 4Fe(s) + 3O2(g)  2Fe2O3(s) Mol Fe Mole Fe2O3
L Fe2O3

16. Using Stoichiometry ____NaOH + ____H2SO4  ____H2O + ____Na2SO4
Key Concept 7:
How many liters of sodium sulfate will be formed if you start with 200 grams of sodium hydroxide and you have an excess of sulfuric acid?
____NaOH + ____H2SO4  ____H2O + ____Na2SO4

17. Practice
How many grams of water are formed when .25L of propane (C3H8) burns at STP with excess oxygen according to the reaction below:
_____C3H8 + ______O2 → ______CO2 + _______H2O

18. Practice
How many grams of CaCl2 are formed when 21.3g of Ca(OH)2 reacts with excess HCl?
_____Ca(OH)2 + _____HCl  ______CaCl2 + ______H2O

19. Practice
How many grams of BaCl2 are formed from moles of Ba(ClO3)2?
_______Ba(ClO3)2 → _______BaCl2 + _____O2

20. Practice
Iron(III) oxide, Fe2O3, can be reduced to iron by passing carbon monoxide, CO, over the heated oxide. How many moles of iron can be produced from moles of iron (III) oxide and excess carbon monoxide?
______Fe2O3(s) + _____CO(g)  _____Fe(s)­ + _____CO2(g)

21. Practice
Butyne, C4H6, burns in the presence of oxygen in air to produce carbon dioxide, CO2, and water H2O. How many moles of oxygen will be required to produce moles of carbon dioxide?
______C4H6 + ______O2  ______CO2 + ______H2O

23. Limiting and Excess Reactants
KC 8: If you have 2 givens in your problem, it is a limiting reactant problem
KC 9: The reactant that produces the smallest amount of a product is the limiting reactant. This is the reactant that will be used up first in the reaction.

24. Example
How many grams of Cu can be formed when g of Fe reacts with g of CuCl2?
2 Fe CuCl2  3 Cu + 2FeCl3

25. Steps for solving LR problems
KC 10:
Write down the givens
Use molar mass to convert to moles
Use mole ratio from the balanced equation
Convert to desired unit
The correct answer is the smallest answer as the reaction will stop once one reactant is gone

26. Limiting and Excess Reactant
KC 11: 80.0g Cu reacts with 25.0g S. Determine which is the limiting reactant and calculate how much Cu2S is formed in grams?
2Cu(s) + S(s) → Cu2S(s)

27. Limiting and Excess Reactant
KC 12: What is the limiting reactant if 65g of each reactant is present?
___Zn + ___HCl → ___ZnCl2 + ___H2

28. Excess and Percent Yield
KC 13: To find how much excess you have you must take the limiting reactant and solve for the excess reactant. You need to look at what you are given versus what you need.

29. Excess Reactant - Example
How many grams of Cu can be formed when g of Fe reacts with g of CuCl2?
2 Fe CuCl2  3 Cu + 2FeCl3
CuCl2 – limiting reactant
188.5g Cu is formed
How many grams of excess is left over?

31. Percent Yield KC 14: % yield = actual yield x 100 theoretical yield
KC 15: Actual yield must be found experimentally. It is recognized by words like “produced” and “formed”
KC 16: Theoretical yield is done using stoichiometry. It is a prediction and will always be done using math.

32. Percent Yield
KC 17: A student calculated she should obtain 28g of a substance. In the experiment, 25g was produced. What is the percent yield of the experiment?

33. Percent Yield - Example
167.4 g of Fe reacts with g of CuCl2 to form g of copper. What is the percent yield of copper?
2 Fe CuCl2  3 Cu + 2FeCl3

34. Practice
KC 18: 11.2g of nickel (II) sulfide reacts with 5.43g of oxygen producing 4.97g of nickel (II) oxide. What is the percent yield of this reaction?
_____NiS2 + _____O2 → _____NiO + _____SO2

35. Practice
KC 19: You are given 0.45g of Al(OH)3 and 0.55g of H2SO4. The reaction produces 0.15g of water. What is the percent yield of this reaction?
____Al(OH)3 + _____H2SO4 → _____Al2(SO4)3 + _____H2O

36. Practice
KC 20: You are given 3 moles of lithium and 3 moles of nitrogen. The reaction produces .5 moles of lithium nitride. What is the percent yield of this reaction?
____Li + _____N2 → _____Li3N