Introduction to Gases Chemistry—2 nd semester
Mar 31, 2015
Introduction to GasesChemistry—2nd semester
PropertiesAll gases share some physical properties:
Pressure (P)Volume (V)Temperature (T)Number of moles (n)
These properties combine to describe the behavior of gases using the “gas laws”
PressurePressure is the amount of force per given amount of area (P=F/area)
Greater forces exert greater pressure
When the area over which the pressure is exerted is decreased, the pressure is increased
Pressure Cont.Pressure is the result of
collisions of gas molecules and the sides of a container
ApplicationsWhy is there more pressure on
you the deeper you move in a body of water?
Why is it harder to breathe when you’re up in a mountain?
ApplicationsWhy is there more pressure on
you the deeper you move in a body of water?◦There is more water pushing down
on you. Greater force means greater pressure
Why is it harder to breathe when you’re up in a mountain?◦The air is “thinner” which means
there is less atmospheric pressure because there is less air pushing down on you
Atmospheric PressureThe pressure exerted by the
atmosphere on the earthDecreases as you move upAbout 15 psi (pounds per square
inch) at sea level
Standard Pressure“normal” atmospheric pressure
at sea levelStandard Pressure:
◦1.00 atm (atmospheres)◦101.3 kPa (kilopascals)◦760 mmHg (millimeters of mercury)◦760 torr
Standard temperatureAbsolute temperature is
measured in Kelvin (K)0 K is absolute zero
K = °C + 273°C = K – 273
Standard temperature: 273 K
Ways to measure pressureBarometer
Ways to measure pressureManometer
Kinetic Theory of GasesA set of ideas (5 points) used to
describe and explain the behavior of gases
Any gas that behaves exactly in this manner is called an “ideal gas”
There are not any “ideal gases” in real life. Real gases behave much like “ideal” gases unless they are under high pressure and temp.
Point OneGases are composed of tiny
particles called moleculesMolecules are so far apart that
gases are mostly empty spaceBecause of this, gases can be
easily compressed and mixed
Point TwoGas molecules posses kinetic
energy (KE=1/2mv2)Gas molecules are in constant,
random, straight line motion
Point ThreeCollisions between gas molecules
and each other or the container are elastic◦No kinetic energy is changed into
another form of energy (like heat)The pressure of an enclosed gas
will NOT change unless its temperature or volume changes
Point FourMolecules of a gas are not
attracted to or repulsed by each other
They move independently of each other
Point FiveIndividual molecules of a gas are
moving at different speeds because they have different kinetic energies
The average kinetic energy (speed) is directly proportional to the temperature of a gas
Dalton’s Law of Partial Pressure• The total pressure of a mixture of
gases is the sum of the partial pressures of the individual gases
• PT = P1 + P2 + P3 + .......
Effusion
• Effusion is the movement of gas molecules through an extremely tiny opening into a region of lower pressure•helium escaping a balloon•air leaking from a tire
Diffusion
•Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout the system•mixing of gases
Graham’s Law of Effusion
•Molecules of lower molar mass diffuse and effuse faster.