1. Warm-up
If I have 4.00 moles of a gas at a pressure of 5.60 atm and a volume of 12.0 liters, what is the temperature in kelvin?

2. Gas Stoichiometry

3. Gas Stoichiometry To find the volume of gas necessary (if not at STP):
Use dimensional analysis to find the moles of gas needed in the reaction.
Use the Ideal Gas Law to determine the volume that amount of moles of the gas will take up.
If you’re given a volume of gas (not at STP), follow these steps:
Use the Ideal Gas Law to determine the number of moles of gas that you have.
Use dimensional analysis to solve the rest of the problems.

4. Gas Stoichiometry
1) When calcium carbonate is heated strongly, carbon dioxide gas is released according to the following equation: CaCO3 (s)  CaO (s) + CO2 (g)
What volume of CO2, measured at STP, is produced if 15.2 grams of CaCO3 is heated?

5. Gas Stoichiometry
2 C8H18 (l) + 25 O2 (g)  16 CO2 (g) + 18 H2O (g) 3a) If 4.00 moles of gasoline are burned, what volume of oxygen is needed if the pressure is atm and the temperature is 35oC?

6. Gas Stoichiometry
2 C8H18 (l) + 25 O2 (g)  16 CO2 (g) + 18 H2O (g) 3b) How many grams of water would be produced if 20.0 L of oxygen were burned at a temperature of -10.0oC and a pressure of 1.3 atm?