Chapter 6 Flashcards
properties of gas
- High kinetic energy
–Travel in straight lines until they collide
–There is a lot of empty space between the
particles
is the force exerted
per unit area
pressure
is an evacuated glass
tube, the tip of which is submerged in a
pool of mercury (Hg).
barometer
on the liquid
mercury’s surface forces the mercury
upward into the evacuated tube.Atmospheric pressure
Atmospheric pressure
on the liquid
mercury’s surface forces the mercury
upward into the evacuated tube.Atmospheric pressure
Atmospheric pressure
nc on slide 7
here is an inverse
relationship between
volume and pressure.
Boyle’s Law
The volume of a fixed amount of gas (n) at
a constant pressure (P) increases linearly
with increasing temperature (in kelvins).
Charles’ Law
If the lines are extrapolated back to a volume of “0,”
they all show the same temperature,
absolute zero
volume directly proportional to the
number of gas molecules when P
and T are constant
avogadro’s law
The simple gas laws can be combined into a
single law –
ideal gas law
gas constant.
R
is used to
compare the properties of different gases.
A standard set of conditions
are U-shaped tubes partially
filled with a liquid that is connected to the
gas sample on one side and open to
the air on the other.
manometers
measure of the gas pressure relative to
atmospheric pressure.
- The difference in the liquid levels
The pressure of a single gas in a mixture of
gases is called its
parial pressure
The sum of the partial pressures of all the gases
in the mixture equals the total pressure
Dalton’s Law of Partial Pressures
The pressure due to any individual
component in a gas mixture is its
partial
pressure (P n).
the partial pressure of the water vapor, c
vapor pressure
The simplest model that describes the
behavior of gases is the
kinetic molecular theory
The particles of the gas (either atoms or molecules) are
constantly moving.
The attraction between particles is
negligible
The average kinetic energy of the gas particles is
directly proportional to the Kelvin temperature.
Kinetic Molecular Theory (KMT)
The result of many particles in a gas sample
exerting forces on the surfaces around them
is a
constant pressure
the kinetic molecular theory is a
quantitative
model
the average distance
a molecule travels
between collisions is
called the
mean free path
The process of a collection of molecules
spreading out from high concentration to low
concentration is called
diffusion
The process by which a collection of
molecules escapes through a small hole into
a vacuum is called
effusion
The rates of diffusion and effusion of a gas are
both related to what
its rms velocity
often do not behave like ideal gases at
high pressure or low temperature.
Real gases
to account for the behavior of real gases at high pressure.
Johannes van der Waals
