1. Single Replacement Reactions
1.) There are 5 major types of chemical reactions
A. Combustion: burns, explodes
B. Synthesis: to make something new
C. Decomposition: break down
D. Double Replacement: 2 elements change
E. Single Replacement: 1 element changes

2. Single Replacement Reactions
2.) In a single replacement reaction, 1 element replaces another element in a compound.

3. Replacement Reactions
3.) Not all metals can be replaced, we use the reactivity series of metals list to predict changes. 4.) The higher an element is on the list, the more likely it is to replace another element.

4. Replacement Reactions

5. Single Replacement Reactions
Example 1 : Zn + Ag(NO3)  Zn (No3) + Ag - Zinc is higher on the list than Silver, therefore it can switch places.

6. Single Replacement Reactions
Example 2 : Au + Ni(SO4)  No reaction - Gold is NOT higher on the list than Nickel, therefore it cannot switch places.

7. Single Replacement Reactions
Example 3: Zn + NiCl2  ZnCl2 + Ni Why was Zn able to switch places with Ni?

8. Single Replacement Reactions
Example 4: Fe + MgCl2  No reaction Why did the reaction not occur?

9. Notes. Advanced Stoichiometry with Moles

10. Advanced Stoichiometry with Moles
Stoichiometry looks at the relationship between the coefficients in a chemical reaction.
Stoichiometry uses dimensional analysis and balancing equations to solve a problem.
In these multi-step t-chart problems we will use what is called a “mole ratio” in the middle of the problem.

11. Advanced Stoichiometry with Moles
Now that we know to convert between moles, atoms, atoms to moles, molecules to moles, moles to grams and grams to moles it’s time to put our knowledge to work and apply it to some advance chemistry problems involving Stoichiometry and dimensional analysis.

12. Advanced Stoichiometry and Moles
Example One:
The reaction between nitrogen monoxide (NO) and oxygen to form nitrogen dioxide (NO2) is a key step in photochemical smog formation.
Question: How many moles of NO2 are formed by the complete reaction of moles of O2?

13. Advanced Stoichiometry and Moles
Example 1: Question: How many moles of NO2 are formed by the complete reaction of moles of O2? Answer: In order to start solving these types of equations we are going to start at the beginning and determine what information we already know about this problem.

14. Advanced Stoichiometry and Moles
Example 1:
Step One-
What do we already know?
- We are starting with moles of O2
- We know that 1 mole of O2= molecules of O2
- We know that the molar mass of O2 is= grams.
- We know that according to the chemical equation shown above moles of NO are needed to react with mole of O2 in order to form moles of NO2.
What do we want to know?
- We want to find out how many moles of are formed.

15. Advanced Stoichiometry and Moles
Example 1: Step Two- Set-up the Dimensional Analysis Problem using the steps we have discussed before:

16. Advanced Stoichiometry and Moles
Example 2: Ammonia (NH3) can be formed from the elements N2 and H2, as shown below. N2 + 3H2  2NH3 Question: How many moles of ammonia can be made from .7 moles of H2? Answer: In order to start solving these types of equations we are going to start at the beginning and determine what information we already know about this problem.

17. Advanced Stoichiometry and Moles
Example 2:
Step One-
What do we already know?
- We are starting with moles of H2
- We know that 1 mole of H2= molecules of H2
- We know that the molar mass of H2 is= grams.
- We know that according to the chemical equation shown above moles of N2 are needed to react with mole of H2 in order to form moles of NH3.
What do we want to know?
- We want to find out how many moles of are formed.

18. Advanced Stoichiometry and Moles
Example 2: Step Two- Set-up the Dimensional Analysis Problem using the steps we have discussed before:

19. Advanced Stoichiometry and Moles
Example 3: The reaction between nitrogen monoxide (NO) and oxygen combine to form nitrogen dioxide (NO2) is a key step in photochemical smog formation. 2 NO + O2 2NO2 Question: How many grams of NO2 are formed by the reaction of 1.44 grams of NO with excess O2? Answer: In order to start solving these types of equations we are going to start at the beginning and determine what information we already know about this problem.

20. Advanced Stoichiometry and Moles
Example 3:
Step One-
What do we already know?
- We are starting with moles of NO
- We know that 1 mole of NO= molecules of NO
- We know that the molar mass of NO is= grams.
- We know that according to the chemical equation shown above moles of NO are needed to react with mole of O2 in order to form moles of NO2.
What do we want to know?
- We want to find out how many of NO2 are formed.

21. Advanced Stoichiometry and Moles
Example 3: Step Two- Set-up the Dimensional Analysis Problem using the steps we have discussed before:

22. Advanced Stoichiometry and Moles
Example 4: Use the reaction below to answer the following question. CH4 + 2 O2  CO2 + H2O Question: How many grams of H2O are formed by the reaction of 5.78 grams of CH4 with excess O2? Answer: In order to start solving these types of equations we are going to start at the beginning and determine what information we already know about this problem.

23. Advanced Stoichiometry and Moles
Example 3:
Step One-
What do we already know?
- We are starting with grams of CH4
- We know that 1 mole of CH4= molecules of CH4
- We know that the molar mass of CH4 is= grams.
- We know that according to the chemical equation shown above moles of CH4 are needed to react with mole of O2 in order to form moles of H2O.
What do we want to know?
- We want to find out how many of H2O are formed.

24. Advanced Stoichiometry and Moles
Example 4: Step Two- Set-up the Dimensional Analysis Problem using the steps we have discussed before:

25. Stoichiometry
Ex. 5 How many grams of H2O are produced if you begin with 98.4 g of O2?
H O2  H2O

26. Stoichiometry
Ex. 6 How many grams of Cl2 are needed to make 209g of NaCl? Na + Cl2  NaCl

27. Stoichiometry
Ex. 7 How many grams of CO2 are produced from 318g of O2? CO + O2  CO2

28. Notes. Limiting Reagent

29. Limiting Reagents
What is a limiting reagent?

30. Limiting Reagents
1.) A limiting reagent/ reactant is a substance needed to start a chemical reaction that we run out of and prevents us from doing the equation again.

31. Limiting Reagents
Baking or cooking recipes are good examples of limiting reactants because eventually you will run out of one of the ingredients you need Example: Let’s say you want to bake a batch of cookies. First ,you google a sugar cookie recipe and find the recipe with the following ingredients (3 eggs, ½ cup milk, 1 cup flour, 2 cups sugar). Second, you find the needed ingredients and determine how many batches you can make given the ingredient amounts below.

32. Limiting Reagents 2.) Which ingredient will you run out of first?
3.) Which ingredients on hand were in excess for the recipe?
Recipe
Ingredients You Have
3 eggs
12 eggs
½ cup milk
2 cups milk
1 cup flour
4 cups flour
2 cups sugar
6 cups sugar

33. Limiting Reagents
4.) You have 100 bolts, 150 nuts and 150 washers. You assemble a nut/bolt/washer set using the following recipe or equation.
2 washers + 1 bolt + 1 nut = 1 set
How many sets can you assemble from your supplies?
Which is the limiting component?

34. Limiting Reagents
We can use this same logic used above in our hotdog, cookie and nuts/bolts/washer example and apply it to chemical reactions. When dealing with a chemical equation, the chemical of which there are fewer moles than the reaction requires is the limiting reagent. In order to solve limiting reagent problems we need to follow 3 main steps.

35. Limiting Reagents
Steps to Solving Limiting Reagent Problems 1.) Balance the equation 2.) Convert all numbers to moles. 3.) Compare number of moles you have available to the number of moles you need in a balanced equation.

36. Limiting Reagents
Example 1: If 6 moles of H2 and 4 moles of O2 are mixed and reacted, which is the limiting reagent?
Step 1: Balance the chemical equation
H2 + O2  H2O 
Step 2: Convert all numbers to moles. 
Step 3: Compare number of moles you have available to the number of moles you need in the balanced equation.

37. Limiting Reagents H2 + O2  H2O What is the limiting reactant?
Example 1: If 6 moles of H2 and 4 moles of O2 are mixed and reacted, which is the limiting reagent?
H2 + O2  H2O 
What is the limiting reactant?
How many moles of water would be produced?

38. Limiting Reagents
Example 2: 200 g of Na react with 200g Cl2. What is the limiting reactant?
Step 1: Balance the equation
Na + Cl2  Na Cl 
Step 2: Convert all numbers to moles.
Step 3: Compare number of moles you have available to the number of moles you need in the balanced equation.
What is the limiting reactant?

39. Limiting Reagents
Example 3: If you had 17.3 g of Hydrogen and 8.91g of oxygen, which is the limiting reagent, and how many grams of water could you produce?

40. Limiting Reagents
Example 4: Solid sodium and iron (III) oxide are involved in a reaction that is one of many reactions responsible for inflating a car airbag. If g Na and g Fe2O3 are used, determine:
6 Na + Fe2O3  3 Na2O + 2Fe
a.) Limiting reactant
b.) Excess reactant
c.) Mass of solid iron produced
d.) Mass of excess reactant left over

41. Limiting Reagents In order to solve this problem we will need to:
a.) Start with one reactant and turn it into the other reactant (either one is fine to start with). Compare the answer with the given amount in the problem to determine if you have more of less of what is given. From this information, the limiting reactants can be determined.
b.) Using information in A, determine the excess reactant.
c.) Determine how many grams of the product, Iron, can be formed, starting with the limiting reactant.
d.) Determine how much of your excess reactant is left over.

42. Limiting Reagents
Example 4: Solid sodium and iron (III) oxide are involved in a reaction that is one of many reactions responsible for inflating a car airbag. If g Na and g Fe2O3 are used, determine:
6 Na + Fe2O3  3 Na2O + 2Fe