Figure 2 shows the chemical potential for the van der Waals model as a function of density at this same temperature. Rem

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Figure 2 Shows The Chemical Potential For The Van Der Waals Model As A Function Of Density At This Same Temperature Rem 1 (76.66 KiB) Viewed 43 times

Figure 2 shows the chemical potential for the van der Waals model as a function of density at this same temperature. Remember that the Gibbs free energy is un, so this is also the Gibbs free energy per molecule. Note that the van der Waals solution assumes that the system is filled with molecules at a uniform density p, not a mixture of liquid and gas.
-9.00 -9.02 -9.04 -9.06 Chemical potential (10^-13 erg/molecule) -9.08 -9.10 -9.12 -9.14 0.000 0.005 0.010 0.015 0.020 0.025 0.030 Density (moles/cm^3) Fig. 2 Chemical potential u vs. density p for the van der Waals model for H20 at T = 550K. (c) Sketch on a copy of Fig. 2 the free energy one would obtain by allowing for the separation of the water into coexisting liquid and gas. (Ignore the small contribution of surface tension.) If a system can be broken up into two weakly interacting subsystems, then the minimum free energy for the system in the limit of infinite size must be convex (see note 4 on page 322). (d) In your solution to part (c), what are the two weakly interacting subsystems? Why did we need to take the limit of infinite size to ignore surface tension? Is your answer convex?