Lt 2 Flashcards
The kinetic-molecular theory describes the
behavior of matter
in terms of particles in motion
. It is a relative model that
explains the
behavior of gases.
This theory was the work of three famous scientists
s: Rudolf
Clasius (1822-1888), James Clerk Maxwell (1831-1879), and
Ludwig Boltzmann (1844-1906
The postulates of this model are made only for
ideal gases
(theoretical gases).
They cannot all be thoroughly related to
Real gases
but can be used to
explain their observed behaviors:
qualitatively
the volume
occupied by a gas is assumed to be
mostly empty space.
- There is ? force of attraction between
and among gas molecules.
- There is no force of attraction between
and among gas molecules.
Gas molecules are in? Motion
constant, random,
and straight-line
They collide
frequently with one another and with the
walls of the container. ?? energy is lost
during collisions
No
The average kinetic energy for molecules
is the same for all gases at the same
temperature, and its value is ?
proportional to the ?
directly, Kelvin temperature
he three-dimensional space enclosed by the
container walls.
Vol
? gases uniformly fill up a container.
All
the measure of the average kinetic energy of
the particles in a sample of matter
Temp
? aka Lord Kelvin
William Thomson
K=
C + 273.15
Gas molecules create pressure as the particles
hit the
walls of the container.
P=
F/A
• Units of Pressure:
N/m2 (SI Unit), Pa (Pascal), mm Hg, torr
Torr
760
Mm of mercury
760
In of mercury
29.9hg
Lb per sq in
14.7 psi
Pascals
1.013x10^5 pa
Kilo pascals
101.3 pa
Bars
1.013 bars
Boyles law name
Robert boyle
Boyles law
pressure is
inversely proportional to voluume
Boyles law formula
P1V1=P2V2
Charles lawnam
Jean Jacques Charles
Charles law
The volume of a given amount of gas is directly proportional
to its Kelvin temperature at constant pressure
Charles law formulation .
.
V1T2 = T1V2
Gay-Lussac’s Law name
• Joseph Louis Gay-Lussac
Gay-Lussac ‘s law
The amount of gas varies directly with the Kelvin temperature
when the volume remains constant.
Gay lussacs Law formula
P1T2 = T1P2
Boyle’s, Charles’, and Gay-Lussac’s laws can be combined
into a single law which described the relationship among the
pressure, volume and temperature.
P1V1T2 = P
Combined Gas Law formula
P1V1T2 = P2V2T1
Graham’s Law
I’m the rate of effusion of a gas, which is the
amount of gas that moves through a hole in a given amount of
time, is inversely proportional to the square root of its molar mass.
process by which gas molecules pass through a very small
opening from a container at higher pressure to one at a lower
pressure
Effusion
ability of two or more gases to mix spontaneously until
they form a uniform mixture.
Diffusion
Thgrahams law of effusion
The rates of effusion (v) of two
gases at the same temperature
and pressure are inversely
proportional to the square root of
their densities (P) or molar mass
(M).
