1. Gas Stoichiometry! Unless you are at STP you MUST convert between Liters  moles using the Ideal Gas Law PV = nRT The only other exception is this: If (and only IF) the compounds given to you in the problem on both sides of the equation are measured in liters, you can use the mole ratio conversion directly between them Problem: Using the equation: 2 H 2 + O 2  2 H 2 O How many liters of water can be made from 25 liters of oxygen?

2. Helpful Concept Map: This map might be helpful to you in solving problems, especially if you are a sequential problem solver:

3. Let’s Do Some Practice Problem: Given the equation: 2 H 2 + O 2  2 H 2 O Using electrochemistry, we can make liquid water from H 2 and O 2 gas. If I use 20.0 L of oxygen gas at a pressure of 1.0 atm and a temperature of - 35 0 C, how many grams of water will I make?

4. More Practice of Stoichiometry! Use the following reaction to answer the next couple of questions: 2 C 8 H 18(l) + 25 O 2(g) ----> 16 CO 2(g) + 18 H 2 O (g) The above reaction is the reaction between gasoline (octane) & oxygen that occurs inside car engines. If 4.00 moles of gasoline are burned, what volume of oxygen is needed if the pressure is 0.953 atm, and the temperature is 35.0°C? If you burned one gallon of gas (C8H18) (approximately 4000 grams), how many liters of CO 2 would be produced at a temperature of 21.0°C and a pressure of 1.00 atm?

5. Making of an Air Bag Lab You are going to be utilizing the Ideal Gas Law and Gas Law Stoichiometry to complete today’s lab! Please begin reading over the lab sheet to see what you will be doing today.

6. End of: Gas Law Stoichiometry HW for Next Class: Complete combined Ideal Gas Law Practice and Gas Law Stoichiometry Worksheet (Problems 6-9 turned in next class) AND Read pgs. 432-436 and take 5-10 bullet notes AND Complete Making Air Bag Lab activity if not finished already AND Complete any missing HW to use for upcoming HW Check next class