11. Johannes Diderik van der Waals
November 23, 1837
– March 8, 1923
Dutch
1910 Nobel Prize in
Physics
12. Van der Waals Equation
In 1873 Modified from ideal gas equation
Accounts for:
Non-zero volumes of gas particles
Attractive forces between gas particles
(attractive effect)
13. Van der Waals Equation
Attractive effect
Pressure = Force per unit area of container
exerted by gas molecules
Dependent on:
Frequency of collision
Force of each collision
Both factors affected by attractive forces
14. Van der Waals Equation
Hence pressure changed proportional to
(n/V)2
Letting a be the constant relating p and
(n/V)2…
Pressure term, p, in ideal gas equation
becomes [p+a(n/V)2]
15. Van der Waals Equation
Repulsive effect
Gas molecules behave like small,
impenetrable spheres
Actual volume available for gas smaller than
volume of container, V
Reduction in volume proportional to amount of
gas, n
16. Van der Waals Equation
Let another constant, b, relate amount of gas,
n, to reduction in volume
Volume term in ideal gas equation, V,
becomes (V-nb)
17. Van der Waals Equation
Combining both derivations…
We get the Van der Waals Equation
19. Virial Equations
•B(T), is a function of temperature and is
called the "second virial coefficient.
•C(T) is called the third virial coefficient,
and so on
20. Virial Equations
Most flexible form of state equation
Terms can be added when necessary
Accuracy can be increase by adding infinite
terms
21. Isothermal Equation of State
The simplest isothermal EOS for a solid is
the bulk modulus or incompressibility, K
K = -V (∂P/∂V)
This equation is only valid for P < K
for a linearly increasing K
K = K0 + K0' P
22. Murnaghan - 1937
The Murnaghan assumed that the bulk
modulus varies linearly with pressure
V = V0 (1+K'P/ K0)
Vinet EoS / 'Universal EoS' – 1986