1. Warm Up: You are the owner of an ice cream parlor. A class of 20 small,ravenous children storm your shop, each demanding an ice cream sundae. One sundae requires 50 mL of chocolate syrup, 2 scoops (1 cup) of vanilla ice cream, and 1 cherry. If you have 600 mL syrup, 25 cups of ice cream, and 20 cherries, how many sundaes will you be able to make? How is the recipe for making an ice cream sundae like a chemical equation? What type of reaction would this represent?

2. Ch. 9.1 Intro to Stoichiometry  Stoichiometry - branch of chemistry that involves calculating the amount of reactants consumed or products formed in a chemical reaction.  Before you can calculate quantities involved in a particular reaction, you must understand the significance of a chemical equation.  The coefficients can be interpreted 2 ways: (a) particle interpretation (b) mole interpretation

3.  Particle Interpretation: Coefficients represent the relative number of particles of each substance. Example: 2 H 2 (g) + O 2 (g) --> 2 H 2 O(l) 2 molecules of H 2 reacts with 1 molecule of O 2 to produce 2 molecules of H 2 O This is consistent with the law of conservation of mass.  Same number of each atom on both sides of the equation.

4.  Mole Interpretation: Coefficients can also represent the relative number of moles of each substance. Example: 2 H 2 (g) + O 2 (g) --> 2 H 2 O(l) 2 moles of H 2 reacts with 1 mole of O 2 to produce 2 moles of H 2 This is also consistent with the law of conservation of mass. 2 (2 g) + 32 g --> 2 (18 g) 36g --> 36 g

5.  However, the coefficients in an equation DO NOT represent a mass relationship. 2 H 2 (g) + O 2 (g) --> 2 H 2 O(l) 2 g + 1 g not equal to 2 g

6. Mole Ratio  A mole ratio is a conversion factor that relates the amounts in moles of any two substances involved in a chemical reaction Example: 2 Al 2 O 3 (l) --> 4Al(s) + 3O 2 (g) Molar conversion Video

7. What Do You Think?  Balance the following chemical equation and provide all the possible mole ratios that can be derived from this equation. (Hint: there are six) N 2 (g) + H 2 (g) --> NH 3 (g)

8. EOC Sample Question ___ N 2 + ___ O 2 --> 2 N 2 O 5 What quantities of nitrogen gas (N 2 ) and oxygen gas (O 2 ) will react completely to produce 2 moles of dinitrogen pentoxide (N 2 O 5 )? A. 4 moles of N 2 and 10 moles of O 2 B. 4 moles of N 2 and 5 moles of O 2 C. 2 moles of N 2 and 10 moles of O 2 D. 2 moles of N 2 and 5 moles of O 2

9.  The mole ratios can help us determine amount of reactants consumed or products formed in a particular chemical reaction.  Given moles of one substance in a reaction, we can use mole ratio to calculate the moles of another substance in the reaction.

10. Sample Problem In a spacecraft, the carbon dioxide exhaled by astronauts can be removed by its reaction with lithium hydroxide, LiOH, according to the following chemical equation. CO 2 (g) + 2 LiOH(s) --> Li 2 CO 3 (s) + H 2 O(l) How many moles of lithium hydroxide are required to react with 20 mol CO 2, the average amount exhaled by a person each day?

11. Your Turn  In the reaction: 4 NH 3 (g) + 6 NO (g) --> 5 N 2 (g) + 6 H 2 O (g) How many moles of NH 3 are needed to produce 12.4 mol H 2 O?

12. Reflection  What is the most important thing you learned today?  What is a question you would still liked answered?  What is a way what you learned today connects with what you knew before?