Real Gases. The ideal gas equation of state is not sufficient to describe the P,V, and T behaviour...
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Transcript of Real Gases. The ideal gas equation of state is not sufficient to describe the P,V, and T behaviour...
![Page 1: Real Gases. The ideal gas equation of state is not sufficient to describe the P,V, and T behaviour of most real gases. Most real gases depart from ideal.](https://reader035.fdocuments.us/reader035/viewer/2022062722/56649f305503460f94c4b817/html5/thumbnails/1.jpg)
Real Gases
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The ideal gas equation of state is not sufficient to describe the P,V, and T behaviour of most real gases.
Most real gases depart from ideal behaviour at deviation from • low temperature
• high pressure
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Low Temperatures
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The variation of the potential energy of two molecules on their separation.
High positive potential energy (little separation)• Repulsive interactions
Intermediate separations• attractive interactions dominate
Large separations (on the right) • the potential energy is zero and there is
no interaction between the molecules.
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High Pressures
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Real gas molecules do attract one another
(Pid = Pobs + constant) Real gas molecules are not point
masses
(Vid = Vobs - const.)
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Vid = Vobs - nb
• b is a constant for different gases
Pid = Pobs + a (n / V)2
• a is also different for different gases
Ideal gas Law Pid Vid = nRT
2
2
mmobs
obs
V
abV
RTP
nRTnbVVn
aP
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The compressibility factor
PVZ
nRT
The deviation from ideal behaviour can be measured in terms of compressibility factor, Z.
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For ideal gas Z = 1 at all temperatures and pressures as pV = nRT. For ideal gas Z = 1 at all temperatures and pressures as pV = nRT.
The graph of Z vs p will be a straight line parallel to pressure axis.
For gases which deviate from ideality, value of Z deviates from unity.
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PVZ
nRT
Gases show ideal behaviour when the volume occupied is large so that the volume of the molecules can be neglected in comparison to it.
The behaviour of the gas becomes more ideal when pressure is very low.
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For a perfect gas, the slope is zero
The temperature at which a real gas obeys ideal gas law over an appreciable range of pressure is called Boyle temperature or Boyle point.
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Boyle temperature - for a van der Waals gas, the Boyle temperature (TB) is written
Rba
TB
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Critical temperature (Tc) - the temperature above which a gas cannot be liquefied.
Critical pressure (Pc) – the minimum pressure that needs to be applied at Tc to bring about liquefaction.
Critical volume (Vc) – volume of one mole of the gas at critical temperature.
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At the critical point
375.0Z ;27
8a
27
aP ;3
c
2c
c
ccc
c
RTVP
RbT
bbV