Gases n Properties n Kinetic Molecular Theory n Variables n The Atmosphere n Gas Laws
Properties of a Gas n No definite shape or volume n Gases expand to fill any container n Thus they take the shape of the container, as well as the volume n Low Density n Most of the volume of a gas is empty spacesince the gas particles want to be as far from all like particles as possible n As a result, gases are compressible
Properties of a Gas n Fluid n can flow like a liquid
The Atmosphere Composed of a mixture of gases -Approx. 80% N 2 and 20% O 2 Provides conditions for life, protects from UV radiation, traps heat Please read about the Greenhouse Effect and the Ozone Layer in your text books you will be responsible for that information...
The Kinetic Molecular Theory n Explains the behavior of gases at the molecular level n Based on assumptions about a theoretical gas referred to as the Ideal Gas.
The Kinetic Molecular Theory 1) Volume of gas particles is essentially zero (Point Masses) 2) Particles are in constant, random motion 3) No attractive forces betw. particles and collisions are perfectly elastic n No energy is lost by the particles during collisions
The Kinetic Molecular Theory 4) The temperature of a gas is directly proportional to the average kinetic energy associated with the particles, thus the higher the temperature, the faster the particles are moving... n K.E. = 1/2 mv 2
Ideal vs. Real Gas Ideal Gas n Has mass but no volume n Has no attractive forces between molecules Real Gas n Molecules do have volume n Molecules exert an attractive force on each other when very close.
Ideal vs. Real Gas n At normal temps. & pressures, real gases behave like ideal gases
Four variables that describe a gas... 1) Temperature - the measure of the avg. kinetic energy n gases at the same temp. must have the same avg. kinetic energy n Must be in Kelvin T K = T C + 273
Four variables that describe a gas... 2) Volume - The amount of space occupied by the particles, measured in liters, ml, cm 3, m 3, etc.
Four variables that describe a gas... 3) Pressure - The force exerted by the gas per unit of area n In gases - meas. of total force exerted by the particles colliding w/ the walls of their container. n - proportional to the number of collisions -Incr. temp, incr. press. - Incr. # of particles, incr. press. n usually measured in: atmospheres (atm), kpa (kilo-pascals), N/m 2 n Pascal - SI unit of pressure = to 1 N/m 2 very small press. - usually use kilopascals
Four variables that describe a gas... 4) Number of particles Equal volumes of gases under the same conditions have equal numbers of particles...
Avogadro s Principle The volume of a gas at a given temperature and pressure is directly proportional to the number of moles of that gas n ie equal volumes of gases under the same conditions contain the same number of particles. Molar Volume is the volume of 1 mole of any gas at STP
Standard Conditions STP Standard Temperature is 273 K Standard Pressure is 1.0000 atm 101.325 kpa 760.0 mm Hg 760.0 torr Note: you can use any pressure units but you can only use Kelvin temperature units
The Gas Laws Boyle s Law - the volume of a gas at constant temp. is inversely proportional to the pressure P 1 V 1 = P 2 V 2 Read Ch. 12 Section 2
The Gas Laws Charles Law - the volume of a gas at constant press. is directly proportional to the absolute (Kelvin) temp. V 1 / T 1 = V 2 / T 2
The Gas Laws Combined Gas Law - Combines Boyle s & Charles Law P 1 V 1 / T 1 = P 2 V 2 / T 2 Read Ch. 12 Section 2
The Gas Laws Ideal Gas Law PV = n R T n = # of moles R = 8.31 L kpa / mol K Or 0.0821 L atm / mol K Read Ch. 12 Section 2