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32 Cards in this Set

  • Front
  • Back
the amount of gas in the system is expressed in
terms of the number of moles
the volume occupied by a gas at a specified temperature and pressure must depend on the
number of gas particles
the number of moles of gas is directly proportional to the
number of particles
moles must be directly proportional to
volume
PV/Tn shows
that (PxV)(Txn) is a constant and holds for ideal gases
a gas behaves ideally if it conforms to
the gas laws
has the value 8.31 (L x Kpa)/(K x mol)
ideal gas constant (R)
P x V = n x R x T

R = P x V / T x n
ideal gas law
what is an advantage of the ideal gas law over the combined gas law
it permits you to solve for the number of moles of a contained gas when p,v, and t are known
a gas that follows the gas laws at all conditions of pressure and temperature is
a truly ideal gas
the particles of a truly ideal gas would have
no volume and could not be attracted to each other at all
is there any gas that is a truly ideal gas
no
an ideal gas
does not exist
real gases can behave as
ideal gases
what is an important behavior of real gases that differs from that of a hypothetical ideal gas
real gases can be liquefied and sometimes solidified by cooling and by applying pressure
you can analyze how much a gas departs from ideal behavior by considering
PVNRT
according the ideal gas law, this ratio fr an ideal gas equal 1 by:
dividing both sides of the ideal gas lawby nRT
PVNRT plotted against pressure gives a _________ for an ideal gas because the ratio is constant
horizontal line
for real gases at high pressure, the ratio PVNRT may depart
widely from the ideal constant value of 1
the explanations for these departures of deviations rom the ideal is based on two factors:
the attractions between molecules and the volume of gas molecules
PVNRT may be greater or less than one
if positive -
negative -
above the line, below the line
simple kinetic theory assumes that
gas particles are not attracted to each other and that the paticles have no volume
are the assumptions of the simple kinetic theory correct
no, incorrect
gases and vapors could not be liquefied if there were no
attractions between molecules
real gases are made up of
actual physical particles, which do have volume
the intermolecular forces that tend to hold the particles in a gas together effectively
reduce the distance between particles
the gas occupies less volume than is expected by the
no-attractions assumption of the kinetic theory, which causes the ratio to tend to be less than 1
the molecules occupy some volu,e thus contradicting the
zero volume assuption of kinetic theory, which causes the ratio to be greater than 1
in portion of the curves below the line,
the intermolecular attractions dominate causing the total volume to be less than ideal
in portions of the curves above the line,
the effect of volume of the molecules dominates, causing the total value to be greater than ideal
the ratio is nearly equal to 1 at
lower pressure at the elevated temperature
the ratio increases to greater than 1 only when
the volume of the individual gas paritlces becomes important, as it does at high pressure