Particles have LOTS of energy; moving all around Gases take on the shape and volume of their container. Gases will spread out evenly = diffusion Ruled by Gas Laws (Charles Law, Boyle’s Law) Examples: oxygen, carbon dioxide, “air”

 Pressure: amount of force on a unit of area. Can be measured in mm Hg, atm, Pascals  Formula for pressure: Pressure = Force/Area

Says: If you decrease the volume of a container of gas, the pressure will increase (temperature and # of particles must stay constant!) Deals with: volume and pressure. (NOT temperature!) Volume and pressure are INVERSELY related (one goes up, the other goes down) Thought examples: If I squeeze a balloon, the volume goes down, but the pressure goes up! Formula: P 1 V 1 = P 2 V 2

 66 Liter of a gas is at a pressure of 8 atm. What is the volume of the gas at 2 atm? P 1 V 1 = P 2 V 2 8 x 66 = 2 x V 2 528/2 = V liters

 4.00 L of a gas are under a pressure of 6.00 atm. What is the volume of the gas at 2.00 atm? P 1 V 1 = P 2 V 2 6 x 4 = 2 x V 2 24/2 = V 2 12 liters

Says: the volume of a gas increases as the temperature increases (pressure must stay constant) Deals with: volume and temperature (not pressure!) Thought example: If I heat up a balloon, it will get larger. If I put a balloon in the freezer, it will get smaller.

 mL of air is at 20.0 o C. What is the volume at 60 o C?  V 1 /T 1 = V 2 /T 2  600 /20 = V 2 /60  30 x 60 = (V 2 /60) 60  1800 mL = V 2

Says: the pressure of a gas is directly proportional to the temperature Deals with: Pressure and Temperature (volume is kept constant) Thought example: If I heat up a sealed container of gas, the pressure will increase inside the container