Comparing Real and Ideal Gases (5.4.1) Flashcards
• Real gases do not always behave like ideal gases.
• Real gases do not always behave like ideal gases.
• The van der Waals equation more accurately predicts the behavior of real gases by accounting for the volume of the gas molecules and the attraction between the
molecules of the gas.
• The van der Waals equation more accurately predicts the behavior of real gases by accounting for the volume of the gas molecules and the attraction between the
molecules of the gas.
The ideal gas law is based on two assumptions:
there are no interactions between gas particles, and
the particles of the gas behave as if they have no
volume.
For low pressures, the measured pressure of a real
gas is often lower than that predicted by the ideal
gas law. This is due to intermolecular interactions
between molecules within the gas.
At higher pressures, the measured pressure is often
much higher than that predicted by the ideal gas
law. This is because the particles of the gas
actually do have a small volume.
The ideal gas law is based on two assumptions:
there are no interactions between gas particles, and
the particles of the gas behave as if they have no
volume.
For low pressures, the measured pressure of a real
gas is often lower than that predicted by the ideal
gas law. This is due to intermolecular interactions
between molecules within the gas.
At higher pressures, the measured pressure is often
much higher than that predicted by the ideal gas
law. This is because the particles of the gas
actually do have a small volume.
The van der Waals equation more accurately
predicts the behavior of real gases by accounting for
the volume of the gas molecules and the attraction
between the molecules of the gas.
The volume correction takes into account the
number of moles of gas particles (n) and the
volume of each of these particles (b).
The pressure correction takes into account the
attraction between gas particles. The attractive
forces will depend on the concentration of particles
about to hit the wall and the concentration of
particles neighboring these particles. This is
expressed as the concentration (n/V) squared times
the strength of the attractions (a).
The complete van der Waals equation can be used
to more accurately predict the pressure or volume of
a real gas.
The van der Waals equation more accurately
predicts the behavior of real gases by accounting for
the volume of the gas molecules and the attraction
between the molecules of the gas.
The volume correction takes into account the
number of moles of gas particles (n) and the
volume of each of these particles (b).
The pressure correction takes into account the
attraction between gas particles. The attractive
forces will depend on the concentration of particles
about to hit the wall and the concentration of
particles neighboring these particles. This is
expressed as the concentration (n/V) squared times
the strength of the attractions (a).
The complete van der Waals equation can be used
to more accurately predict the pressure or volume of
a real gas.
The values of a and b have been calculated for
many gases. Water (H2O) has a strong
intermolecular attraction (a), due to hydrogen
bonding. Carbon dioxide (CO2) has a relatively
high volume correction (b).
The values of a and b have been calculated for
many gases. Water (H2O) has a strong
intermolecular attraction (a), due to hydrogen
bonding. Carbon dioxide (CO2) has a relatively
high volume correction (b).
