Introduction To Statistical Thermodynamics -1
고려대학교 화공생명공학과
강정원
Statistical Thermodynamics ?
Link between microscopic properties and bulk properties
Microscopic Properties
T,P
U,H,A,G,S μ,Cp,…
Microscopic Properties
Statistical Thermodynamics
Molecular Properties Thermodynamic Properties
uij
r
) 1 ( +
=hcBJ J
EJ Eν=(v+21)hcv~
2 2 2
8mX h En = n
Potential Energy
Kinetic Energy
Two Types of Approach for Microscopic View
Classical Mechanics
– Based on Newton’s Law of Motion
Quantum Mechanics
– Based on Quantum Theory
) ,...,
,
2 ( 1 2 N
i i
i U
m
H =
p + r r r
∇ Ψ + Ψ = Ψ−
i
i i
E m U
h 2
2 2
8π
Hamiltonian
Schrodinger’s Wave Equation
Solutions
Using classical mechanics, values of
position and momentum can be found as a function of time.
Using quantum mechanics, values of
allowed energy levels can be found. (For simple cases)
Purpose of statistical thermodynamics
Assume that energies of individual molecules can be calculated.
How can we calculate overall properties (energy, pressure,…) of the whole system ?
Statistical Distribution
n : number of object
b : a property (can have 1,2,3,4, … discrete values)
b ni
1 2 3 4 5 6
if we know “Distribution”
then we can calculate the average value of b
Normalized Distribution Function
Probability Function
>=
<
>=
<
i
i i i
i i
P b
F b
F
P b b
) ( )
b (
Pi
b1 b2 b3 b4 b5 b6
=
=
=
i
i i
i
i i
i i i
i i
i
b P
b n
b n n
b b n
P
1 )
(
) (
) ( )
) (
b : energies of individual molecule,… (
F(b) : internal energy, entropy, …
Finding probability (distribution) function is the main task in statistical thermodynamics
The distribution of molecular states
Quantum theory says ,
– Each molecules can have only discrete values of energies
Evidence
– Black-body radiation – Planck distribution – Heat capacities
– Atomic and molecular spectra – Wave-Particle duality
Configurations…
Instantaneous configuration
– At any instance, there may be no molecules at ε0 , n1 molecules at ε1 , n2 molecules at ε2 ,
… {n0 , n1 , n2 …} configuration
ε
0
ε2 ε
1
ε3 ε4 ε
5
{ 3,2,2,1,0,0}
Weight ….
Each configuration can be achieved in different ways …
Example1 : {3,0} configuration 1
Example2 : {2,1} configuration 3
ε
0
ε
1
ε
0
ε
1 ε
0
ε
1 ε
0
ε
1
Weight …
Weight (W) : number of ways that a
configuration can be achieved in different ways
General formula for the weight of {n0 , n1 , n2 …} configuration
=
∏
=
i
ni
N n
n n W N
!
!
!...
!
!
!
3 2
1
Example1
{1,0,3,5,10,1} of 20 objects W = 9.31E8
Example 2
{0,1,5,0,8,0,3,2,1} of 20 objects W = 4.19 E10
Principle of equal a priori probability
All distributions of energy are equally probable
If E = 5 and N = 5 then
0 1 2 3 4 5
0 1 2 3 4 5
0 1 2 3 4 5
All configurations have equal probability, but possible number of way (weight) is different.
The dominating configuration
For large number of molecules and large number of energy levels, there is a dominating configuration.
The weight of the dominating configuration is much more larger than the other configurations.
Configurations Wi
{ni}
The dominating configuration
0 1 2 3 4 5
0 1 2 3 4 5
0 1 2 3 4 5
W = 1 (5!/5!) W = 20 (5!/3!) W = 5 (5!/4!)
Difference in W becomes larger when N is increased !
Stirling’s Approximation
A useful formula when dealing with factorials of numbers.
N N
N
N ! = ln − ln
i i
i
i i i
i i
i
i
n n
N N
n n
n N
N N
n n N
n n W N
−
=
+
−
−
=
−
=
=
ln ln
ln ln
! ln
!
!... ln
!
! ln ! ln
3 2 1
The Boltzmann Distribution
Task : Find the dominating configuration for given N and total energy E.
Find Max. W which satisfies ;
=
=
i
i i i
i
n E
n N
ε 0
0
=
=
i
i i i
i
dn dn ε
Method of Undetermined Multiplier
Maximum weight , W
Recall the method to find min, max of a function…
Method of undetermined multiplier :
– Constraints should be multiplied by a constant and added to the main variation equation.
ln 0
0 ln
=
∂
= dni
W W d
Method of undetermined multipliers
ln 0 ln ln
=
+ −
= ∂
−
+
= ∂
i
i i
i
i
i i i
i i
i i
dn dn W
dn dn
dn dn W W
d
βε α
ε β
α
ln 0
=
−
+
∂
i
dni
W α βε
∂
− ∂
∂
= ∂
∂
∂
−
=
j i
j j
i i
i i
n n n
n N N
n W
n n
N N
W
) ln ln (
ln
ln ln
ln
1 1 ln
ln ln
+
=
∂
× ∂
+
∂
= ∂
∂
∂ N
n N N N
n N N n
N N
i i
i
= +
∂
× ∂
+
∂
= ∂
∂
∂
j
i i
j j
j j
i j
j i
j
j n
n n n n
n n n n
n
n 1 ln 1
) ln ln
(
N N n
n n
W i
i i
ln )
1 (ln
) 1 ln (ln
−
= +
+ +
−
∂ =
∂
0
ln + + =
− i
i
N
n α βε
e i
N
ni α−βε
=
−
−
=
=
=
j
j j
j
j
j
e e
e Ne
n N
α βε
α βε
1
−= −
=
j i
i j
i
e e N
P n βε
βε
Boltzmann Distribution (Probability function for
energy distribution)
The Molecular Partition Function ( 분자 분배 함수 )
Boltzmann Distribution
Molecular Partition Function
Degeneracies : Same energy value but different states (gj-fold degenerate)
q e e
e N
p n
i
j i
j i
i
βε βε
βε −
−
− =
=
=
−
=
j
e j
q βε
−
=
j levels
j
e j
g
q βε
An Interpretation of The Partition Function
Assumption :
T 0 then q 1
T infinity then q infinity
The molecular partition function gives an indication of the average number of states that are thermally accessible to a molecule at T.
kT /
= 1
β
An example : Two level system
Energy level can be 0 or ε
e kT
e
q =1+ −βε =1+ −ε/
Example
Energy levels : ε, 2ε, 3ε , ….
βε βε
βε
−
−
−
= − +
+ +
= e e e
q 1
... 1
1 2