# Lecture 4 Thermal Equilibrium_ Temperature_ and Entropy

Document Sample

```					Lecture 4
Thermal Equilibrium, Temperature, and
Entropy

Recall that, since the systems 1 and 2 are independent of each other, the total multiplicity
for ﬁxed (E, V, N ) is just:

Ω(E, V, N ) =                     Ω(E, V, N, α)
α

=                    Ω(E, V, N, E1 , V1 , N1 )              (4.1)
E1 ,V1 ,N1

=                    Ω1 (E1 , V1 , N1 )Ω2 (E2 , V2 , N2 )
E1 ,V1 ,N1

where the summations are performed over all possible macrostates of the combined system.
If we let N1 and V1 be ﬁxed, then what does the total multiplicity look like as a function of
E1 ?

Ω (E ) Ω (E )
1   1   1   1

0           E*               E
1                   1

Figure 4.1: Resultant multiplicity for two systems brought in contact which achieve thermal
∗
equlibrium at E1

• Note that this is a “sharp” function for large systems (refer to Prob. 2.21 in Tutorial
1) and only a small number of macrostates dominate the statistics of the combined
system.
∗
• The most probable macrostate (conﬁguration) occurs at E1 which corresponds to ther-
mal equilibrium. This is the macrostate which has the greatest multiplicity.

• Since the ﬂuctuations are small, we can replace our averages, X over all macrostates
by that of an average only over the most probable conﬁguration. This replacement
should have minimal error.

4.1      Thermal Equilibrium
Let us return to Eq. 4.1 but, as mentioned above, ﬁx N1 , V1 and, since E, V, N, V2 , N2 were
also ﬁxed, thus E1 is the only independent variable. Thus, we have

Ω(E) =           Ω1 (E1 )Ω2 (E2 ) =                  Ω1 (E1 )Ω2 (E − E1 )             (4.2)
E1                                  E1

∗
By our Third Postulate, we expect that the most probable macrostate corresponding to E1
is such that,
dΩ(E)              ∂Ω1                       dE1               ∂Ω2              dE2
=                         Ω2        + Ω1                               = 01
dE      ∗
E1         ∂E1        V1 ,N1         dE1               ∂E2     V2 ,N2   dE1
dE2
Recall that E2 = E − E1 and, thus,             dE1
= −1, therefore, dividing by Ω1 Ω2 we ﬁnd,

1        ∂Ω1                      1      ∂Ω2
=
Ω1       ∂E1       V1 ,N1         Ω2     ∂E2       V2 ,N2
∂ ln Ω1                       ∂ ln Ω2
=
∂E1        V1 ,N1             ∂E2          V2 ,N2

We deﬁne a quantity σ, called the entropy as: the measure of the disorder of a system in a given macrosta

σ(E, V, N ) ≡ ln Ω(E, V, N )                                         (4.3)

which is just a pure number (dimensionless). Using this deﬁnition, we arrive at the funda-
mental condition for thermal equilibrium for two systems in thermal contact,

∂σ1                       ∂σ2
=                                             (4.4)
∂E1       V1 ,N1          ∂E2       V2 ,N2

• At thermal equilibrium, there is no substantial heat transfer (although there will be
small temperature ﬂuctuations).
1
When performing thermodynamic derivatives, such as these, we must be careful to clearly label the
macrostate parameters, such as N1 , V1 , which are held ﬁxed while diﬀerentiating
• If there is no heat transfer, then the two systems must be at the same temperature,
i.e.,
τ1 = τ2 .

• From Eq. 4.4, this implies that τ is a function of ∂σ/∂E. In particular, we deﬁne the
fundamental temperautre, τ , as

1       ∂σ
=                .                         (4.5)
τ       ∂E   V,N

• Now the “standard” entropy S, which you are most likely familiar with, is Bolzmann’s
Deﬁnitions,

S = kB σ = kB ln Ω(E, V, N )                        (4.6)

where kB = 1.381 × 10−23 J/K is Boltzmann’s contant.

• With this deﬁnition, we can express the “standard” temperature as,

1      ∂S
=                                         (4.7)
T      ∂E    V,N

1. Entropy is additive, which can be seen from the deﬁnition of the total multiplicity for
two systems in contact,

Ω(E, V, N ) = Ω1 (E1 , V1 , N1 )Ω2 (E2 , V2 , N2 )
∴, S(E, V, N ) = S1 (E1 , V1 , N1 ) + S2 (E2 , V2 , N2 ).

This implies that entropy is an extensive quantity.
Deﬁnitions:
Extensive Quantity: proportional to the size of the system → double the size, double
the quantity. Intensive Quantity: independent of the size of the system e.g. tem-
perature, pressure.

2. Entropy is increased when constraints are removed:

↓ Constraints →↑ no. of accessible microstates of the system →↑ no. of degrees of freedom →↑ S
(a)                   (b)

Figure 4.2: By removing the partition, a signiﬁcant constraint on the system is lifted allowing
for a greater number of accessible microstates and, hence, an increase in entropy

Picture: Note: Even though we said at the beginning of the course that a conﬁguration like
(a) (but without the barrier) was not impossible to observe, although highly improbable,
we would never see the system go from this maximum probable conﬁguration (b) to the
initial one (a) (without the barrier). That is, this is an irreversible process, even though the
equations of motion are reversible in time.
The Second Law of Thermodynamics or The Law of Increase of Entropy (Mul-
tiplicity): The entropy of a closed system either remains constant or increases when a
constraint is removed.
Consider our two systems in thermal contact and evaluate the “rate of change of entropy”:
dS   ∂S dE1   ∂S dE2
=        +
dt   ∂E1 dt   ∂E2 dt
or
Clausius’ Principle:

dS      1   1      dE1
=      −            >0                                (4.8)
dt      T1 T2       dt

If T1 < T2 , dE1 > 0, since heat ﬂows from the subsystem at higher temperature to that at
dt
lower temperature.
Picture:
T1 < T2

1                          2

Heat Flow
E1                E2

E                                S(E)

Entropy
Energy
E2

E1

t                    t

Figure 4.3: A demonstration of Clausius’ Principle: since T1 < T2 , heat will ﬂow from 2 → 1
and the entropy will increase until the two systems are at the same temperature and the
entropy reaches a constant value (maximum threshold for a given total energy E)

Let us apply these to a system composed of two Einstein solids in thermal contact.

Example 4.1 Two Einstein Solids in Thermal Contact

• Consider two Einstein solids, A and B, where NA = 4 and NB = 5 and they contain a
total of 10 units of energy, qtotal = qA + qB = 10.

• When brought into thermal contact, the two systems will exchange energy until they
reach thermal equilibrium → which corresponds to the macrostate (of the combined sys-
tem) which has the greatest multiplicity and, hence, the greatest probability of occuring

• Calculate the multiplicities for all of the possible macrostates of the combined system?
Which macrostate has the greatest probability of occuring?
Table 4.1: Diﬀerent possible macrostates and multiplicities for a system of two Einstein solids,
one containing four oscillators, the other having ﬁve oscillators, and both sharing a total of ten
units of energy

qA                ΩA        qB    ΩB      Ωtotal = ΩA ΩB
0                 1        10   1001           1001
1                 4         9   715            2860
2                10         8   495            4950
3                20         7   330            6600
4                35         6   210            7350
5                56         5   126            7056
6                84         4    70            5880
7                120        3    35            4200
8                165        2    15            2475
9                220        1     5            1100
10                286        0     1             286

8000

6000
Ωtot

4000

2000

0
0         2        4        6     8     10
qA

Figure 4.4: Resultant multiplicity for two Einstein solids brought in contact which achieve
thermal equlibrium at qA = 4

```
DOCUMENT INFO
Shared By:
Categories:
Stats:
 views: 9 posted: 3/22/2010 language: English pages: 6