The average kinetic energy of a collection of gas particles is
6/6/1166Chapter 5Gases and the Kinetic-molecular TheoryGas Pressure Pressure = Atmospheric pressure: Barometer: Units of pressure: 1 atm = 760 mm Hg=760 Torr= 14.7 lb/in2= 29.9 in Hg = 1.01325 x 105Pascals (Pa) 1 Pa = 1 N/m2
6/6/1177Chapter 5Gases and the Kinetic-molecular TheoryRelationships Between Gas Pressure, Volume and Temperature Pressure vs. Volume:Boyle's Law: At constant temperature, the volume of a fixed mass of gas is to the pressure.
6/6/1188Chapter 5Gases and the Kinetic-molecular TheoryVolume vs. Temperature: Charles' Law:At constant pressure, the volume of a fixed mass of gas is to the Kelvin temperature.
6/6/1199Chapter 5Gases and the Kinetic-molecular TheoryPressure vs. Temperature: Amonton's Law: At constant volume, the pressure of a fixed amount of gas is to the Kelvin temperature. Avogadro's Law: Equal volumes of different gases as the same temperature and pressure contain
6/6/111010Chapter 5Gases and the Kinetic-molecular TheoryIdeal Gas Equation Combine these laws: Boyle's Law: PV = k Charles' Law: V αT or V = kT Amonton's Law: P αT or P = kT Avogadro's Law: V αn P = pressure in V = volume in n = number of moles T = temperature in R = Ideal Gas constant:
1111Chapter 5Gases and the Kinetic-molecular TheoryCalculations with the Ideal Gas Law:Example Problem; What volume will 2.5 L of a gas occupy if the pressure is changed from 760 mm Hg to 630 mm Hg? Example Problem: 3.0 L of H2at -20oC are allowed to warm to a room temperature of 27oC. What is the volume then if the pressure remains constant?