1. Phase Transitions The above picture shows a block of solid Ar melting and subliming after exposur to aire at roughly room temperature. http://en.wikipedia.org/wiki/Phase_transition

2. Phase Diagram of H2O http://people.virginia.edu/~lz2n/mse209/Chapter9-p1.pdf See also: http://www1.lsbu.ac.uk/water/phase.html

3. Examples Chapter 12 • 4.) A system consists of 1024 molecules of water. The initial state is pure vapor at 373 K and atmospheric pressure. The water is heater at constant pressure to T=700K, subsequently compressed isothermally to a pressure of 230 atm, cooled to 373 K a this constant pressure, and finally allowed to expand isothermally to atmospheric pressure. The final state is pure liquid. • What is the net change in the system’s internal energy? • What is the net change in the system’s chemical potential? • 5). The top of Mt. Everest is 8,854 meters above sea level. Calculate the temperature at which water boils at the summit. • 7). The vapor-pressure curves at the triple point display a cusp (if you look carefully enough, and if the person drawing the diagram was careful enough). Explain why this must be the case. • a). Specifically, near the triple point for water vg/vl=2.06x105vs/vl=1.09 and the latent heats are 0.47, 0.53 and 0.062 eV/molecule (for vaporization, sublimation and melting respectively).

5. From J.R. Waldram “The Theory of Thermodynamics”

6. Alloy phase diagram of Cu-Ni http://people.virginia.edu/~lz2n/mse209/Chapter9-p1.pdf

7. Eutectic Phase Diagram NOTE: at a given overall composition (say: X), both the relative amounts of the two phases (a,b or c,d) AND the composition of one (or possibly both) depend on the temperature http://www.tulane.edu/~sanelson/geol212/2compphasdiag.html