# Potentials Mechanically, a potential A(r) was the difference A(r2 )  –  A(r1) and equal to the work needed to go from r1 to r2. The decisive point was that A(r ) did not depend on the particular way chosen to go from r1 to r2 as long as the acting forces F (r) were given as the derivative of the potential A(r) with respect to the coordinates. We have
  = F( r) æ è ö ø These are the well known relations for mechanic (and electrostatic) potentials. If one knows the potential and the momentum of a massive (and charged) particle, one knows everything one can know and needs to know. The history, i.e. how the particle came to its present position r with the potential A( r) and momentum, is totally irrelevant. Potential and momentum together then define the state of the particle. We may first generalize the idea of a potential by allowing generalized coordinates, i.e. any variables (and not just space coordinates) that describe the state of a system. This allows to treat thermodynamic systems consisting of many particles, where individual coordinates loose significance and average values describing the system take precedence. Lets consider the free energy as a first example. It is a thermodynamic potential and at the same time a state function, i.e. it describes completely the state of systems with the generalized coordinates temperature T, volume V and particle numbers Ni. The mechanical potential by itself, in contrast, is not a state function (we would need the momentum, too, to describe the state of a mechanical system). A change of state thus necessarily demands a change in at least one of the three generalized coordinates from the above example. In formulas we write
F  =  thermodynamic
potential
=  F(V, T, N1, ... Ni) The Ni denote the number of particles of kind i. Is it that easy? Can we elevate all kinds of functions to the state of thermodynamic potentials and state functions? The answer, of course, is No! The statement that the function P(xi) is a potential with respect to the generalized coordinates xi is only true if a number of conditions are met. For the case of equilibrium (which requires that nothing changes and therefore that all P/xi = 0) those requirements are: The values of the generalized coordinates describe the state of the system completely (this means you have the right number and the right kinds of coordinates). The value of P(xi) for a set of values of the generalized coordinates is independent from the path chosen to arrive at the particular state and thus from the history of the system. In formulas:
DP  =      change in P between a state 1 and a state 2 2 ó õ 1 2 ó õ 1 2 ó õ 1 i.e. the difference depends only on the starting and end state. This can only be true if dP is a total differential of P, i.e.
dP  =  P
x1
· dx1   +  P
x2
· dx 2  +   .... i.e. the changes in the generalized coordinates describe unambiguously the total change in P. The numerical values of the partial derivatives of the thermodynamic potentials describe the "effort" it takes to change the potential by fiddling with the particular coordinate considered. This can be understood as a generalized force. If the derivative happens to be taken with respect to a space coordinate of the system, the generalized force is a real mechanical force - it describes the change of energy with space as it should. If the derivative happens to be taken with respect to a particle number, however, the resulting quantity is not called, e.g., "particle number changing force" (which would have been a perfectly good name), but chemical potential, which might be a bit confusing at times. How do we know if a given function is a thermodynamic potential and a state function? For a given function (in differential form), it is not necessarily obvious if it is a total differential. You have to resort to physical or mathematical reasoning to find out. Lets first look at an example of physical reasoning: The first law of thermodynamics was defined as follows:
d U  =  dQ  –  dW Are these three differential quantities total differentials and thus state function and thermodynamic potentials, or are they not? Physical reasoning tells us that dU must be a total differential because U must be a thermodynamic state function - otherwise we can construct a perpetuum mobile! Lets see why: If we start from some value U1, characterized by as many variables xi (= coordinates) as you like (e.g. pressure p1, volume V1 , temperature T1 ) and than move to a second value U2 by adding, for example, a heat quantity Q; we have described a path 1 to move from U1 to U2. If we return to the same values of the generalized coordinates by a different path; e.g. by now extracting some mechanical work, but have a value U1 ' that is not identical to U1, we are now in a position to construct a cycle between the states 1 and 2 as characterized by the generalized coordinates that allows us to extract work in every cycle - we have a perpetuum mobile. So dU must be a total differential - and this requires that dQ and dW are not total differentials! Because it is entirely possible to go from one state of U to another one by adding different amounts of Q and W - the path described by these circumstances must not matter! DQ = Q2Q1 or DW = W2W1 thus are not independent of the path, therefore they are not state functions and their differentials cannot be total differentials. This is essentially tied to the fact that the system entropy may change in these cases. Now lets turn to mathematical reasoning. Obviously, if a function P(xi) of several variables xi is given, it is always possible to calculate the total differential dP(xi ). But the reverse is not necessarily true: If P is given in differential form, it always can be written as
d P(x,y)  =  g(x,y ) · dx  +  f(x,y) · dy We used only two variables x and y for simplicities sake. The functions g(x,y) and f(x,y) are arbitrary functions - what ever you like is allowed. If dP is a total differential, we have necessarily
g(x,y)  =  P
x

f( x,y)  =  P
y On the other hand for all functions P( x,y) the following equalities must obtain
¶ ¶P ¶ x  =  ¶ ¶y ¶x æ ç è ö ÷ ø æ ç è ö ÷ ø This requires that

g(x,y)
y
=  f(x,y)
x Only if the above relation is fulfilled, is dP(x,y) = g(x,y)dx + f(x,y)dy a total differential. So we have a simple checking procedure for a given differential function (a mathematical rule) to find out if it is indeed a total differential. Internal Energy, Enthalpie, Entropy and Free Enthalpie The chemical potential Internal Energy, Enthalpie, Entropy and Free Enthalpie 2.4.2 Kröger-Vink Notation

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