No Slide Title

1Gas LawsSTP2Standard Temperature and Pressure0C and 1 atmBoyles LawAt a constant temperature pressure and volume are inversely related.As one goes up the other goes downP x V = K(K is some constant)Easier to use P1 V1=P2 V23Page #PV4Page #ExamplesA balloon is filled with 25 L of air at 1.0 atm pressure. If the pressure is change to 1.5 atm what is the new volume?5Page #Charles LawThe volume of a gas is directly proportional to the Kelvin temperature if the pressure is held constant.V/T= K (K is some constant)V1/T1= V2/T26Page #VT7Page #Absolute Zero8If data of T and V is extrapolated to the temp where volume is zero, the temp is 273.15CThis temp is where volume collapses all atomic and subatomic motion stopsExamplesWhat is the temperature of a gas that is expanded from 2.5 L at 25C to 4.1L at constant pressure.9Page #Gay Lussacs LawThe temperature and the pressure of a gas are directly related at constant volume.P/T = K (K is some constant)P1/T1= P2/T210Page #PT11Page #ExamplesWhat is the pressure inside a can of deodorant that starts at 25C and 1.2 atm if the temperature is raised to 100C?

12Page #Putting the pieces togetherThe Combined Gas Law Deals with the situation where only the number of molecules stays constant. (P1 x V1)/T1= (P2 x V2)/T2.13Page #ExamplesIf 6.2 L of gas at 723 mm Hg at 21C is compressed to 2.2 L at 4117 mm Hg, what is the temperature of the gas?14Page #Avogadros Law15The volume of a gas is directly proportional to the number of moles (n) V1/n1= V2/n2Example: A 12.2 L sample containing 0.50 mole of oxygen gas (O2) is converted to ozone (O3) at the same temperature and pressure. What is the volume of the ozone gas?

The Ideal Gas LawP V = n R TPressure times Volume equals the number of moles times the Ideal Gas Constant (R) times the temperature in Kelvin.This time R does not depend on anything, it is really constant R = 0.0821 (L atm)/(mol K)16Page #Example17What mass of hydrogen gas will occupy a volume of 2.50 L at a pressure of 755 mmHg and a temperature of 28oC?