1. Chapter 9 “Stoichiometry” Chemistry Charles Page High School Stephen L. Cotton

2. Stoichiometry is… u Greek for “measuring elements” Pronounced “stoy kee ahm uh tree” u Defined as: calculations of the quantities in chemical reactions, based on a balanced equation. u There are 4 ways to interpret a balanced chemical equation

3. #1. In terms of Particles u Element= made of atoms u Molecular compound (made of only nonmetals) = molecules u Ionic Compounds (made of a metal and nonmetal parts) = formula units (ions)

4. 2H 2 + O 2   2H 2 O u Two molecules of hydrogen and one molecule of oxygen form two molecules of water.  2 Al 2 O 3  Al + 3O 2 2formula unitsAl 2 O 3 form4 atoms Al and3moleculesO2O2 Now try this: 2Na + 2H 2 O  2NaOH + H 2

5. #2. In terms of Moles  2 Al 2 O 3  Al + 3O 2  2Na + 2H 2 O  2NaOH + H 2 u The coefficients tell us how many moles of each substance u A balanced equation is a Molar Ratio

6. Chemical Calculations u OBJECTIVES: Construct mole ratios from balanced chemical equations, and apply these ratios in mole-mole stoichiometric calculations.

7. Chemical Calculations u OBJECTIVES: Calculate stoichiometric quantities from balanced chemical equations using units of moles, mass, representative particles, and volumes of gases at STP.

8. Mole to Mole conversions  2 Al 2 O 3  Al + 3O 2 each time we use 2 moles of Al 2 O 3 we will also make 3 moles of O 2 2 moles Al 2 O 3 3 mole O 2 or 2 moles Al 2 O 3 3 mole O 2 These are the two possible conversion factors

9. Calculating Stoichiometric Problems 1. Balance the equation. 2. Convert mass in grams to moles. 3. Set up mole ratios. 4. Use mole ratios to calculate moles of desired chemical. 5. Convert moles back into grams, if necessary.

10. Avogadro told us: u Equal volumes of gas, at the same temperature and pressure contain the same number of particles. u Moles are numbers of particles u You can treat reactions as if they happen liters at a time, as long as you keep the temperature and pressure the same. 1 mole = 22.4 L @ STP

11. Shortcut for Volume-Volume: u How many liters of CH 4 at STP are required to completely react with 17.5 L of O 2 ?  CH 4 + 2O 2  CO 2 + 2H 2 O 17.5 L O2O2 2 L O 2 1 L CH 4 = 8.75 L CH 4 Note: This only works for Volume-Volume problems.

12. Limiting Reagent & Percent Yield u OBJECTIVES: Identify the limiting reagent in a reaction.

13. Limiting Reagent & Percent Yield u OBJECTIVES: Calculate theoretical yield, percent yield, and the amount of excess reagent that remains unreacted given appropriate information.

14. “Limiting” Reagent u If you are given one dozen loaves of bread, a gallon of mustard, and three pieces of salami, how many salami sandwiches can you make? u The limiting reagent is the reactant you run out of first. u The excess reagent is the one you have left over. u The limiting reagent determines how much product you can make

15. Limiting Reagents - Combustion

16. How do you find out which is limited? u Do two stoichiometry problems. u The one that makes the least amount of product is the limiting reagent.

17. The Concept of: A little different type of yield than you had in Driver’s Education class.

18. What is Yield? u The amount of product made in a chemical reaction. u There are three types: 1. Actual yield- what you get in the lab when the chemicals are mixed 2. Theoretical yield- what the balanced equation tells should be made 3. Percent yield 3. Percent yield = Actual Theoretical x 100

19. Details on Yield: u Percent yield tells us how “efficient” a reaction is. u Percent yield can not be bigger than 100 %. u Theoretical yield will always be larger than actual yield! Due to impure reactants; competing side reactions; loss of product in filtering or transferring between containers; measuring