1. Stoichiometry
Easy as 1,2,3!!! 

2. Stoichiometry
The study of the relationships or ratios between two or more substances undergoing chemical reactions
***Must balance reaction 1st before solving***

3. Mole Ratio
In a balanced equation you can create ratios from one compound to another creating a bridge conversion factor
__ Mg + __ O2  __ MgO

4. Mass to mass

5. Diving In (Practice)
If you have 6.85 g of phosphorus how much oxygen gas (in grams) do you need to combine with it?
__ P + __ O2  __ P4O10

6. Practice
If you begin with 200 g of sodium hydroxide how many grams of sodium sulfate will be produced?
NaOH + H2SO4  H2O + Na2SO4

7. Practice
If you are give 8 g of oxygen gas how many grams of product can be produced?
__ P + __ O2  __ P4O10

8. Practice
If you produce 250 g of Li2SO4 how many grams of LiNO3 did you begin with?
Pb(SO4)2 + LiNO3  Pb(NO3) 4 + Li2SO4

9. Practice
If you create 7.46 g of P4O10 how many grams of phosphorus would you need to start with?
__ P + __ O2  __ P4O10

10. Mass to volume

11. Practice
In the following reaction 13.5 L of Oxygen reacted with the mercury. How many grams of Mercury (I) Oxide were formed?
Hg + O2  Hg2O

12. Practice
In the following reaction you react 48 grams of Oxygen with an unknown volume of hydrogen to form water. How many liters of hydrogen were used? O2 + H2  H2O

13. Volume to volume

14. Practice
Nitric Oxide (NO) reacts instantly with oxygen gas to give Nitrogen Dioxide, a dark brown gas. If you finished with 65.2 liters of Nitrogen Dioxide, how many liters of Oxygen were used?
NO + O2  NO2

15. Percent Yield

16. Formula
Actual x 100 Theoretical

17. Percent Yield
In the following reaction, you started off with 35 grams of Hydrogen. When BT did the experiment, they produced grams of Dihydrogen Monoxide. What is their percent yield? H2 + O2  H2O

18. Percent Yield
In the following reaction, you started off with 2000 grams of Rubidium. When BT did the experiment, they produced 1500 grams of Rubidium Sulfide. What is their percent yield?
Rb + S8  Rb2S

19. Limiting and Excess reactants

20. Practice
If 5.00 grams of copper metal react with a solution containing 20.0 grams of AgNO3, which reactant is limiting? What is in excess and how much of it is left over?
Cu + AgNO3  Cu(NO3)2 + Ag

21. Practice
What reactant is limiting if 3 liters of Cl2 react with a solution containing 25.0 grams of NaBr? What is in excess and how much of it is left over? NaBr + Cl2  NaCl + Br2

22. Practice
Suppose in the reaction below you had 45 g of Na and 80 g of Cl2. What is the limiting reactant? What is in excess and how much? Na + Cl2  NaCl

23. Practice
Suppose in the following reaction you had 32 g of Mg and 40 g of Oxygen. What is the limiting reactant, what is in excess, and how much?
Mg + O2  MgO