the behavior of gases -...
TRANSCRIPT
The Behavior of gases Section 14.1: Properties of Gases
Why do soccer balls explode if you over pump them?
What is meant by the term compressibility? ● Compressibility is a measure of
how much the volume of matter decreases under pressure
● Example - airbags○ Airbags are much more compressible
than the dashboard○ The particles in the airbag are able to
move together, absorbing much of the impacts energy
● Under increased pressure, particles in a gas are forced together, or compressed
Modeling air at different pressuresWhich piston is at the higher pressure?
What variables are used to describe a gas?
● Pressure ○ Directly related to the number of
molecules (number of moles)○ More particles in container = more
pressure○ Used to make predictions as in, maximum
possible pressure○ If pressure in sealed container is lower
than atmospheric pressure air will rush
What variables are used to describe a gas?
● Volume○ Pressure can be increased by
decreasing the volume of the container
● Temperature○ Higher temperature means that
particles move faster, and therefore collide with side of object with more energy
The Gas LawsSection 14.2
How does a hot air balloon work?
Boyle’s lawThere is an inverse relationship between pressure and volume (assuming a constant temperature)
Practice problems - page 429
Charles’s lawThe volume of a gas is directly proportional to its kelvin temperature if pressure remains constant
Temperature must be in Kelvins!
Practice problems page 432
Guy - Lussac’s lawThe pressure of a gas is directly proportional to the Kelvin temperature, assuming that pressure remains constant
Knowing this, how could you fix this?
The combined gas lawAll three gas laws can be combined to determine what occurs when pressure, temperature and volume all vary
Ideal GasesSection 14.3
The amount of gas…...Whilst discussing the gas laws in section 14.2, we have not really spoken amount the 4th variable, the number of moles
The ideal gas law describes the physical behavior of an ideal gas - the relationship of pressure, volume, temperature and number of moles
The ideal gas constant is a set value of 8.31 (L.kPa/K.mol).
What is the difference between ideal and real gases? ● In reality ideal gases do not exist, BUT most gases sometimes can behave
like an ideal gas● In real gases, particles have a volume and can be attracted to each other
Question Ideal Gas Real Gas
Does it exist No Yes
Does it obey all gas laws? Yes Sometimes, mainly at High T and Low P
How big are the particles? So small they are insignificant
Small, but when compressed, size is important
Are there attractive forces between particles
No Yes, but due to particle speed often insignificant. Become important at lower temperatures
Gases: Mixtures and Movements
Section 14.4
What is meant by the term partial pressure?In a mixture of gases, the partial pressure is the contribution each gas makes to the total pressure
Dalton’s lawThis law states that the total pressure of a mixture of gases equals the sum of the partial pressure of the gases in the mixture
Essentially the number of particles is important for calculating pressure - the type of particle is not significant
This law assumes that volume and temperature are constant AND that each gas’s pressure is not affected by the pressures of other gases in the mixture
Percent composition and partial pressure
If you know the total pressure of a system, and the percent composition, you can calculate the partial pressure of a component gas
Diffusion vs EffusionDiffusion: The tendency for particles to move from areas of high concentration to areas of low concentration until the the concentration is uniform throughout
Effusion: The process that occurs when a gas escapes through a tiny hole in a container
How fast can particles diffuse or effuse?● The answer depends on the mass of the particle● The lower the molar mass, the faster the rate of diffusion or effusion -
Graham’s Law● This is based on the idea that if two objects with different masses have the
same kinetic energy, the lighter object will move faster● This explains why helium blimps must be airtight!