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35 Cards in this Set

  • Front
  • Back
phases
solid liquid gas
gases and liquids are defined as _____
fluids
they both can 'flow'
gas particles have ___ intermolecular forces between them
weak
both gases/liquids can take the shape of the container
know this
gases are ______, unlike solids and liquids
compressible
define gas based on 4 variables
pressure
temperature
moles
volume
1 atm =
760mm Hg = 760torr = 100kPa
gases occur under STP
273K and 1 atm
ideal gases have
1. no intermolecular forces/interactions
2. occupy no volume
3. low pressure
4. high temperature
non ideal gas situation?
high pressure and low temperature
kinetic molecular theory
all gases show similar physical characteristics and behavior irrespective of their chemical identity
rules of kinetic molecular theory
1. gases are made up of particles whose volumes are ____ compared to volume of container
1. negligible
2. gas atoms/molecules exhibit no ________ or _______
2. intermolecular attractions or repulsions
3. gas particles are in continuous ____ motion
3. random
4. collisions between molecules are _____ meaning conservation of momentum and KE
4. elastic
5. the average KE is ____ to the temperature
proportional
6.the KE is ____ of all gases at a given temperature, regardless of chemical identity or mass
6. identical
average molecular speeds =
KE = 1/2mv^2 = (3/2kT)
know this
speed = (3RT/MM)^1/2

trend?
speed is inversely proportional to molecular mass...hence the heavier an atom is, the slower it will move
as temperature increases, the average speed of molecules ____
increase
diffusion = effusion =

r1/r2 = (MM2/MM1)^1/2
r = rates (proportion)
MM = molecular mass
all gas particles have the ____ KE at the same temperature
same
effusion =
flow of a gas particles under pressure from one compartment to another through a small opening
avogadro's principle with constant pressure and temperature
equal amts of all gases at the same temperature and pressure will occupy equal volumes
volume at STP
22.4L/mol
n1/V1 = n2/V2 = k
proportional moles to volumes
ideal gas law EQ
PV = nRT

R = 8.314J or .0821atm
density
mass/volume = g/L

OR

[P(MM)] / RT
PV/T =P2V2 / T2
know this
Boyle's Law
PV =PV
Charles' Law
V/T = V/T
partial pressures
P(A) = P(T)*X(A)

P(T) = total pressure
X = moles
real gases deviate with
pressure
temperature
real gases and pressure
as pressure increases, take up LARGER volume than predicted
real gases and temperature
as the temperature is decreased, the particles have a SMALLER volume than predicted