1. Introduction to Thermodynamics

3. U = internal energy

9. Entropy P
P / 2

15. (Craig Counterman)

16. J g-1 K-1 at 300 K
atomic number
(Craig Counterman)

18. Allotropic Transition

19. Q Why is Gibbs free energy called ‘free’?
A Because it is that part of the energy which is
in principle obtainable as mechanical work.
N. K. Adam, Physical Chemistry,
Clarendon Press, Oxford (1956) page 263.

21. Allotropic Transition in Pure Iron

22. Mechanical Mixture Gibbs free energy per mole Concentration x of B m
free energy of
mechanical m o
mixture B G* m o
Gibbs free energy per mole A x
1-x A B
Concentration x of B

23. entropy is a capacity property, like mass, energy etc
entropy is a capacity property, like mass, energy etc. Different entropies can be added: S1+S2=S3
How does this fit with the probability picture?

24. Entropy
w=1 P
w=very large
P / 2

25. w is not a capacity property of the system.
For example, the chance of throwing two sixes with dice is (1/6)2, not 1/6+1/6.
Boltzmann realised that we should use ln{w} and not w to meaure disorder.

27. Gibbs free energy per mole
free energy of
mechanical m o
mixture B G*
Gibbs free energy per mole m o A ∆G M
G{x}
free energy
of solution A B x
Composition

28. Gibbs free energy per moleA
m { }
1-x A
m { } x B
G{x} A B x
Composition

35. Binary solution

46. Irreversible Processes: Steady State

47. dissipating free energy

48. Process whose direction can be changed by an infinitesimal change in external conditions is reversible.

50. Process which dissipates energy is irreversible to an infinitesimal change in external conditions.