1. CHAPTER 5 Explosions

2. Caused when a chemical reaction releases a large amount of gas and energy very quickly Explosion sends a pressure wave through surrounding materials Usually oxidation or decomposition rxn Oxidation – combo of 2 substances making one Decomp – one compound is broken down into 2+

3. Properties of gases Kinetic molecular theory – gas behavior Many particles moving rapidly & randomly Particles in gas are smaller than the space b/t them – most of Vol = empty space When particles collide, no net loss of energy As temp increases, so does average kinetic energy of its particles No force of attraction b/t particles and other things

4. Relationship b/t Temp, Pressure, & Volume Gas expands to fill space/container Vol, pressure IfAndThen Temp increasesVol is constantPressure increases Temp increasesPressure is constantVol increases Temp is constantPressure decreases Vol increasesPressure is constantTemp increases Pressure increasesTemp is constantVol decreases Pressure increasesVol is constantTemp increases

5. Combined Gas Law P = Pressure (kPa) (= kiloPascals) V = Volume (L) (= liters) T = Temperature (K) (= Kelvin) Predict how Temp, Vol, or Press will change when conditions change

6. Under certain conditions, pressure increases until container can no longer hold gas Container explodes

7. Problem The volume of a gas-filled balloon is 30.0 L at 313 K and 153 kPa pressure. What would the volume be at standard temperature and pressure (STP)? Knowns : V 1 = 30.0 L T 1 = 313 K P 1 = 153 kPa T 2 = 273 K (standard temp) P 2 = 101.3 kPa (standard pressure)