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18 Cards in this Set

  • Front
  • Back
assumptions of kienetic molecular theory of gases

(ideal gas)
1. particles with negligible volume

2. no intermolecular attractions or repulsions

3. continuous, random motion (gas molecule collide with each other and wall of their container in a random continuous motion)

4. elastic collisions, conservation of kinetic energy (nogain or loss of energy)

5. avg kinetic energy of gas particles proportional to the absolute temp
at high T and low P real gas is like???
ideal gas
ideal gas equation

P = 1atm = 760mmHg =760 torr
V = in L or mL
T= T(K)=T(C)+273.15
273.15K(0 C) and 1atm
volume of 1 mole of any gas at STP
22.4 L
molar mass

(divide weight by volume then multiply by 22.4L/mol)
Boyle's law
constant temp (isothermal condition)

isothermal condition
constant temp
Dalton's law of partial pressure
when two or more ideal gases are in one vessle withon chem interacton

Mole fraction
the mole fraction of gas A

Xa = number of moles of a /total number of moles of gases
partial pressure
Ppartial of a = Ptotal Xa
charles's law
constant pressure

V1/T1 = V2/T2
Avagadro's principle
for all gases at constant T,P

n1/v1 = n2/v2

thus all gases have the same number of moles in the same volume.
the flow of gas particles under pressure from one compartment to another through small opening

gives ration of the rates of two process how fast either occurs and relate to gas's molar masses.

r1/r2 = SQR M2/M1

r = rate of effusion

M = density
heavier the gas
slow it to diffuse or effuse
how quickly gas travel in open air( how gas expends)

more massive slow it moves and thus diffuse and effuse slowly)

diffusion equation is same as effusion
maxwell-boltzmann distribution curve
shows the distribution of speeds of all the gas particle in a sample at a gien temperature

bell curve

flattening means
at T inc, gas travel greate range speed
thus small porporton of the movlecule will move at exactly the new average speed