The Van der Waals equation can be obtained considering the atoms of a gas as hard spheres. In this case, in fact, the mean field has the form:
a parameter that in general can depend on
. In other words the particles are modelled as spheres of radius
: for large distances the potential is attractive, while for short distances it is repulsive and prevents the atoms from overlapping. Note also that this is a very rough first approximation: the potential, when attractive, does not depend on the distance between the atoms, and
is discontinuous. We will later see what happens when we make a more realistic approximation.
Therefore, we will have:
the volume that must be excluded because the particles are hard spheres (namely the volume occupied by all the other atoms) the configurational partition function will be:
The configurational part of the free energy is thus:
We can determine the state equation of this system as usual (we derive only the configurational part of
because the kinetic one does not contain terms depending on
is the attractive term between the particles we can suppose that it is proportional to the particle density (intuitively, if the system is dense the particles will be closer to each other and will interact strongly), and of course the excluded volume
will be proportional to the number of particles; therefore, setting:
which is exactly Van der Waals equation. Defining
we can rewrite it as:
Critical point of Van der Waals equation[edit | edit source]
The behaviour of the Van der Waals isotherms is the following:
Van der Waals isotherms for
As we can see this changes with the temperature and resembles that of real isotherms (see Phase transitions and phase diagrams); however, Van der Waals isotherms are always analytic and have a non physical behaviour in certain regions of plane, called spinodal curves, if : for some values of we have , which is physically impossible. This is a consequence of the roughness of the approximation we have made, since it can be shown that it doesn't ensure that the equilibrium state of the system globally minimizes the Gibbs free energy. As we will shortly see, however, this problem can be solved "by hand" with Maxwell's equal area rule, or Maxwell's Construction
Let us now see how to determine the critical point of a system obeying Van der Waals equation.
First of all, from the representation of the isotherms we can see that the critical point is a flex for the critical isotherm (i.e. the one with ); in other words, we can determine the critical point from the equations:
Equivalently, we can note that the equation is cubic in . In fact, we can rewrite the Van der Waals equation as:
this equation has one real solution and two imaginary ones, and for
three distinct real solutions; when
the three solutions of the equation coincide. This means that at the critical point this last equation must be written in the form:
Equating the coefficients we get:
from which we have:
We have found a very interesting result: in fact, if we can measure
at high temperatures then we are able to determine the critical point of the system.
This model has also an interesting property, since it predicts that:
which is a universal number
, independent of
and so of the particular fluid considered. Experimentally this ratio is approximately 0.29 for Argon, 0.23 for water and 0.31 for
. Therefore, even if it is very rough, this model leads to reasonable conclusions.
Law of corresponding states[edit | edit source]
We can also rewrite Van der Waals equation in a dimensionless form, rescaling the thermodynamic quantities of the system. In particular, defining:
Van der Waals equation becomes:
We have found another very interesting result: when rescaled by their critical thermodynamic properties, all fluids obey the same state equation
. This is the law of corresponding states
that we have already encountered in Critical exponents and universality
This is a form of universality, but substantially different from the one we have seen until now, which applies only in the neighbourhood of a critical point: in fact, the law of corresponding states applies everywhere
on the phase diagram. It can even be shown that this law is a consequence of dimensional analysis, and is more general than what might seem: experimentally the law of corresponding states is well satisfied also by fluids which do not obey Van der Waals equation.
As we have previously anticipated, Maxwell's equal area rule is a method to "manually" remove the unphysical regions of Van der Waals isotherms.
Maxwell's equal area rule
From Phase coexistence and general properties of phase transitions we know that at the coexistence of two phases the chemical potentials and the pressures of the two phases must be equal; furthermore, from Thermodynamic potentials we also know that the chemical potential is the Gibbs free energy per particle, namely , and in general we have also:
and subtracting this last equation we get:
Therefore, since along an isotherm
, we will have:
Looking also at the previous figure, we see that this means that the horizontal segment of the isotherm must be drawn so that regions
have the same area (from which the name of the method).
Let us now study the behaviour of systems obeying Van der Waals equations near the critical point, computing one of the critical exponents.
This exponent can be computed from the shape of the coexistence curve for ; this can be done using the law of corresponding states. In fact, defining:
we can expand the law of corresponding states near
, or equivalently
(namely in the neighbourhood of the critical point):
where the terms we have neglected are justified a posteriori (i.e. we will see that
; we could have not neglected them, but the result of the computation doesn't change).
The strategy we want to apply is the following: since we want to determine how
, we can determine the relation between the densities
in the gaseous and liquid phase from Maxwell's equal area rule. This way, from the expression of
we can determine the pressures in the two phases and express them in terms of
, and since
at the coexistence we can obtain from this equation the behaviour of
in terms of
Therefore, from Maxwell's equal area rule we have:
where we have used the definitions of
If we now set our system on an isotherm with
small (so that the expansion of
makes sense), the variation of
in terms of
We thus have
is small we can neglect it, and so:
we see that the only acceptable solution is
(since the volume of a gas is larger than that of a liquid).
at the phase coexistence, we have:
and excluding of course the case
, in the end:
which is what we could have expected from a mean field theory.
In fact, if we compute all the other critical exponent, we get exactly:
A more precise approximation[edit | edit source]
We have seen that the problem of Van der Waals equation comes from the rough approximation that we have made in .
A better formulation of Van der Waals mean field theory can be done using the potential:
is a parameter that determines the range of the potential.
In this case (we don't do the computations, we just state the result) after having computed the partition function, in the limit
the potential becomes infinitely ranged and weak. The interesting fact is that in this limit the theory becomes essentially the same that we have seen before, but with the exception that there are no unphysical regions and Maxwell's rule is no longer necessary, since this model naturally predicts the existence of the "plateaux" relative to the liquid-gaseous phase transition in
- ↑ Remember that by definition describes the behaviour of the order parameter in the neighbourhood of the critical temperature, so we will have .
- ↑ If we didn't neglected the term of the expansion of , we would have found:
Again, the terms linear in can be neglected since is small (and , are just numbers).