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gases in the atmosphere include
O2 - 21%
N2 - 78%
O3, Ar, CO2 and water vapor
gas consists of small particles that
move in straight lines, no attractive forces, have small volumes and their kinetic energies increase with a temperature increase
describing gases through properties
pressure, volume, temperature, amount
volume
same volume as the container it occupies
measured in Liters or milliliters
increases with an increase in temperature at a constant pressure
temperature
measured in kelvin
relates to the kinetic energy of the molecules
temp decreases: few collisions between molecules
temp increases: more collisions between molecules
pressure
measure of the gas particle collisions with the sides of the ocntainer
measured in mmHg, torr, or atm
atmospheric pressure
pressure exerted by air from the top of the atmosphere to the surface of the earth
ex: gas particles in the air exert pressure on us
is 1 atm at sea level
decreases as height increases
sum of the partial pressures of all the gases in the air
barometer
measures pressure
shows the amount of pressure as a column with no air (vacuum) fills up with mercury
at 1 atm the barometer tube is 760 mm high
1 atm is the same as
760 mmHg and 760 torr (Evangelista torricelli)
atmospheric pressure changes
a hot day: mercury column rises meaning a higher atmospheric pressure
a rainy day: mercury column falls meaning less exerting of atmosphere and less pressure
boyles law
relationship between volume and pressure of a gas
boyles law: when volume increases
pressure decreases
anglo- irish
1st modern chemist and made boyles law
boyles law: when we inhale
lungs expand, pressure decreases, air flows towards the lower pressure in the lungs
boyles law: when we exhale
lung volume decreases and pressure increases. air flows from the highter pressure in the lungs to the outside
charles law
relationship between temperature and volume
charles law: if we increase the temperature of gas
volume of the container increases due to knetic energy
charles
balloonist
gay-lussacs law
relationship between temperature and pressure
gay-lussacs law: when temperature rises
pressure also rises
combined gas law
uses the pressure, volume and temperature relationship.
avogadros law
relationship between amount of gas and volume of gas
avogadros law: when amount of gas increases
volume increases
where do the combined gas laws come from
ideal gas law
ultra combined gas law
volume of gases can be compared at
STP (standard, temperature and pressure)
both conditions must be met
STP - standard temperature
0 degree celcius or 273 K
STP - standard pressure
1 atm or 760mmHg
STP - molar volume
1 mole of gas = 22.4 L
stp molar volume for gas is same as volume of 3 basketballs
partial pressure
pressure that each gas in a mixture would have if it were by itself in the container
daltons law
partial pressure
pressure depends on total number of gas particles not the type of particles
total pressure exerted by gases in a mixture is the sum of partial pressures of those gases
finding partial pressure
P(total) = P1 + P2 + P3…
the air we breath is mostly made up of
N2 and O2
solubility relationship with temp
solids increase in solubility as temp increases
gases decreases in solubility as temper increases
why cant gases dissolve at high temps?
for them to dissolve (convert to liquid) they have to get closer
high temp = molecules move fast and are far apart
diffusion
movement of a substance from a high concentration to a low one
gases move faster
rate of diffusion depends on
gas density or grahams law
boyles law examples
syringes, lungs, bicycle pump, outer space, air bubbles
charles law examples
deoderant/ soda can in the heat, basketball outside
guy-lussacs law example
pressure cooker, fire extinguisher, tire bursting, firing a bullet
avogadros law examples
blowing up a basket ball or a ballon with air molecules
