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32 Cards in this Set
- Front
- Back
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the amount of gas in the system is expressed in
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terms of the number of moles
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the volume occupied by a gas at a specified temperature and pressure must depend on the
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number of gas particles
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the number of moles of gas is directly proportional to the
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number of particles
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moles must be directly proportional to
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volume
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PV/Tn shows
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that (PxV)(Txn) is a constant and holds for ideal gases
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a gas behaves ideally if it conforms to
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the gas laws
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has the value 8.31 (L x Kpa)/(K x mol)
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ideal gas constant (R)
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P x V = n x R x T
R = P x V / T x n |
ideal gas law
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what is an advantage of the ideal gas law over the combined gas law
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it permits you to solve for the number of moles of a contained gas when p,v, and t are known
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a gas that follows the gas laws at all conditions of pressure and temperature is
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a truly ideal gas
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the particles of a truly ideal gas would have
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no volume and could not be attracted to each other at all
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is there any gas that is a truly ideal gas
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no
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an ideal gas
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does not exist
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real gases can behave as
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ideal gases
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what is an important behavior of real gases that differs from that of a hypothetical ideal gas
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real gases can be liquefied and sometimes solidified by cooling and by applying pressure
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you can analyze how much a gas departs from ideal behavior by considering
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PVNRT
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according the ideal gas law, this ratio fr an ideal gas equal 1 by:
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dividing both sides of the ideal gas lawby nRT
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PVNRT plotted against pressure gives a _________ for an ideal gas because the ratio is constant
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horizontal line
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for real gases at high pressure, the ratio PVNRT may depart
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widely from the ideal constant value of 1
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the explanations for these departures of deviations rom the ideal is based on two factors:
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the attractions between molecules and the volume of gas molecules
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PVNRT may be greater or less than one
if positive - negative - |
above the line, below the line
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simple kinetic theory assumes that
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gas particles are not attracted to each other and that the paticles have no volume
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are the assumptions of the simple kinetic theory correct
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no, incorrect
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gases and vapors could not be liquefied if there were no
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attractions between molecules
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real gases are made up of
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actual physical particles, which do have volume
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the intermolecular forces that tend to hold the particles in a gas together effectively
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reduce the distance between particles
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the gas occupies less volume than is expected by the
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no-attractions assumption of the kinetic theory, which causes the ratio to tend to be less than 1
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the molecules occupy some volu,e thus contradicting the
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zero volume assuption of kinetic theory, which causes the ratio to be greater than 1
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in portion of the curves below the line,
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the intermolecular attractions dominate causing the total volume to be less than ideal
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in portions of the curves above the line,
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the effect of volume of the molecules dominates, causing the total value to be greater than ideal
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the ratio is nearly equal to 1 at
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lower pressure at the elevated temperature
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the ratio increases to greater than 1 only when
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the volume of the individual gas paritlces becomes important, as it does at high pressure
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