1. Chemistry: Chapter 11 Note Packet

2. Converting Limiting Reactants % Yield
Basic (g A, L A, mol A, particles A)
Using mole A  mole B (entire mole map)
Limiting Reactants
Finding LR and ER
Finding Theoretical Yield
% Yield
Solving for Actual Yield, Theoretical Yield or % when given two of the three
Finding Theoretical Yield using LR questions then solving for actual yield or %

4. Review Composition Stoichiometry 0.15 mol NaOH to grams
Stoichiometry-The study of the quantitative relationships between chemical formulas, reactions, and equations
Review Composition Stoichiometry
0.15 mol NaOH to grams
9.00 g MgCl2 convert to molecules of MgCl2
0.15 mol NaOH x 40.0 g NaOH = 6.0 g NaOH
1 mol NaOH
9.00 g MgCl2 x 1mol MgCl2 x 6.02x1023 =
95.3g MgCl mol MgCl2

5. Ex: Combustion of Propane __C3H8 + __O2  __CO2 + __H20
In this chapter, we do reaction stoichiometry. The book says there are many different types of problems. However, we are going to condense the problems to one type. They are all gram, mole, atom, liter conversion problems tied into equations. Stoichiometry will be used to perform our equations.
Ex: Combustion of Propane
__C3H8 + __O2  __CO2 + __H20
C3H8 + 5 O2 3CO2 + 4H2O
Thus, for every 1 mole propane 5 moles oxygen are required to produce 3 moles of carbon dioxide and 4 moles of water.

6. What equalities can you get from the equation? (6)
C3H8 + 5 O2 3CO2 + 4H2O

7. Use the equalities Ex1: 3 moles propane to moles of water
Ex2: 6 moles of oxygen to moles of water
Ex3: 20 moles of carbon dioxide to moles of propane

8. Mole to mole wks

9. New Mole Map

11. Synthesis of Hydrogen and Oxygen…..
Three Core Steps:
1. Go to moles of “A” (A is whatever substance you start with)
2. Mole to Mole (Change from “A” to “B”)(B is new substance)
3. Go away from moles of “B”
Note: Step 2 is always present!! A ____________ chemical equation is necessary!
Synthesis of Hydrogen and Oxygen…..
Ex 1: How many moles of water vapor are created from 2 moles of hydrogen?

12. Ex2: How many grams of water vapor are created from 64
Ex2: How many grams of water vapor are created from 64.0 grams of Oxygen?
Ex3: How many liters of H2O are made from L of Oxygen

13. Avagadro’s hypothesis makes it easier - “Equal volumes of gases at equal pressures and equal temperatures have equal # of particles.”
So... two gases at 20 C, 1 atm, and 22.4 L each have 6.02 x 1023 molecules.
Combustion of C5H12
Ex4: How many Liters of Oxygen are needed to react with g C5H12?

14. Lithium hydroxide reacts with carbon dioxide to produce Lithium carbonate and water Ex5: How many grams of solid lithium hydroxide are needed to react with 8.50 grams of carbon dioxide gas? Ex6: How many grams of water are produced from 2.00 moles of carbon dioxide and excess amount of lithium hydroxide Ex7: How many moles of lithium carbonate are produce from 152 grams of carbon dioxide and an excess amount of lithium hydroxide?

15. How many sandwiches can we make?
What is left over?
Problem: We want to make ten ham, egg, and cheese sandwiches. Each sandwich will be composed of two slices of bread, three slices of cheese, one egg, and one slice of ham. We have the following items:
10 slices of bread
25 slices of cheese
12 eggs
10 slices of ham

16. How many sandwiches can we make with what we are given?
1)What limits us in making ten sandwiches?
2) How much of the excess reactants do we have?

17. When one of the reactants runs out the reaction is over
Limiting Reactant –
A) the reactant that runs out first
B) determines the amount of product that can be formed by a reaction.
Excess reactant – not completely used up during a reaction (i.e. left over)

18. How to determine which reactant is the limiting reactant
How did you do it with the sandwiches?
Determine how many sandwiches you could make with each of the ingredients
Lowest # of sandwiches produced was a result of the limiting reactant

19. 9.3 Limiting Reactant Problems and % Yield...
Ex1: How many grams of Magnesium Chloride can be made from 3.64 g of magnesium and 7.10 g of Chlorine gas? (It’s a synthesis reaction)
Ex1a: What is the Limiting Reactant?

20. 9.3 Limiting Reactant Problems and % Yield...
Ex2: How many moles of CO2 can be made from 2.70 moles of Ethene (C2H4) and 6.30 mole of oxygen? (It’s a combustion reaction)
Ex2a: What is the Limiting Reactant?

21. % yield = actual yield x 100 theoretical yield
Ex1: What is the percent yield if a reaction produces only 75 moles of carbon dioxide when the theoretical yield was 95 moles of carbon dioxide?
1a- limiting reactant?
Ex2: If a reaction produces a 70% yield and the reaction should have produced 85g of methane, how much methane was actually produced?
2a- limiting reactant?

22. Put it all together
Ex3: Reacting 4.20 grams of Nitrogen with g of Hydrogen produces______g of NH3 if there is a 75.5 % yield?
A) What is the theoretical yield? _________ grams of NH3.
B) What is the limiting reactant?
C)What is the actual yield given a 75.5% yield?

23. Put it all together
Ex4: How much hydrogen gas is produced when 6g of HCl and 5g of Mg react? What is the LR? If 2.4 moles should be produced by this reaction what is the % Yield? (hint: single replacement reaction)