Statistical Mechanics - Physics at Oregon State University
Statistical Mechanics - Physics at Oregon State University
Statistical Mechanics - Physics at Oregon State University
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3.5. OVERVIEW OF CALCULATION METHODS. 55<br />
occur easily, it is also easy to induce a change in the average by external means,<br />
e.g. changing µ. Finally, the fluctu<strong>at</strong>ions ∆N are proportional to √ N. In the<br />
thermodynamic limit the fluctu<strong>at</strong>ions in the number of particles are infinitely<br />
large, but the fluctu<strong>at</strong>ions per particle become infinitesimally small.<br />
3.5 Overview of calcul<strong>at</strong>ion methods.<br />
The development of the ideas used in st<strong>at</strong>istical mechanics starts with the discussion<br />
of a closed system, with extensive parameters V, U, and N (and possibly<br />
more), which can be set <strong>at</strong> specified values. These extensive parameters are the<br />
independent parameters describing the system. The link between the microscopic<br />
world and thermodynamics is obtained by calcul<strong>at</strong>ing the entropy. There<br />
are several ways of doing so (more about th<strong>at</strong> in a l<strong>at</strong>er chapter), but here we<br />
start with the multiplicity function, g(U, V, N). This function gives the number<br />
of microscopic st<strong>at</strong>es available to the system <strong>at</strong> given U, V, and N. Next, we<br />
define the entropy analogue by S(U, V, N) = kB log(g(U, V, N)). We then take<br />
the thermodynamic limit, making the system infinite, and all variables become<br />
continuous. The thermodynamic limit is always needed, no m<strong>at</strong>ter which formul<strong>at</strong>ion<br />
of st<strong>at</strong>istical mechanics one is using. Sometimes people try to hide it, and<br />
calcul<strong>at</strong>e st<strong>at</strong>istical mechanical functions for small systems. But those results<br />
are suspect, because only in the thermodynamic limit can we prove th<strong>at</strong> the<br />
entropy analogue defined above is equivalent to the entropy defined in thermodynamics.<br />
Once we have shown th<strong>at</strong> the entropy analogue is indeed equivalent<br />
to the thermodynamical entropy, we can use all results from thermodynamics,<br />
and we are in business.<br />
The p<strong>at</strong>h followed above is a good p<strong>at</strong>h for theoretical development, but<br />
often not a good way for practical calcul<strong>at</strong>ions. Using the temper<strong>at</strong>ure T as an<br />
independent variable makes life much easier (most of the time). In our model<br />
system we can now choose the following combin<strong>at</strong>ions of independent variables:<br />
(T, V, N), (T, V, µ) , and (T, p, N). Note th<strong>at</strong> we need <strong>at</strong> least one extensive<br />
variable. Other combin<strong>at</strong>ions are possible to, but do not lead to useful free<br />
energies (see thermodynamics). Next, we construct the Hilbert space of all<br />
possible quantum st<strong>at</strong>es which are consistent with the values of the extensive<br />
parameters in the combin<strong>at</strong>ion. This space is, for the three cases above, S(V, N)<br />
, S(V ) , and S(N), respectively. Next, we calcul<strong>at</strong>e the partition sum for these<br />
situ<strong>at</strong>ions:<br />
Z(T, V, N) = <br />
Z(T, V, µ) = <br />
s∈S(V,N)<br />
s∈S(V )<br />
ζ(T, p, N) = <br />
s∈S(N)<br />
e −βɛs (3.62)<br />
e −β(ɛs−µns)<br />
e −β(ɛs+pvs)<br />
(3.63)<br />
(3.64)