Question

Please explain as much as possible

Consider gases described by the following two equations of state: RT RT b) p a) Perfect: p m 2 Vm -b as ) Use Maxwell Equation to derive an expression for for each equation of state т ii) for an isothermal expansion, compare the change in entropy expected for a perfect gas and for a gas obeying the Van der Waals equation of state (Equations a and b) ii Which has the greatest change in entropy and how can this conclusion be rationalized?

Answer 1

b) Real (Vander waal's RT and Vm P=RT a Vm-b Manvell quation for de, or Now we have o eualuat /P and b a For fedfet gon 2 (RT T Vm Vm for Vandernal's 2(RT T Vm-b Vm

-Constant T 3 sothema espusion Tanpeakine aud Volume inenasu fom Vm m, Constaud Chanys ( Vm Vm Integrat botih sic Vm S-Si Vm Vn As. Rlu Vn ASER Vm Caial

Real R Jutegrating bot sidu R dv Vm-b m S,-S vm-b Vm Rufe- R mVm-b A S Vm AsdeaRlVm aud ASeal Rl (Vm-b) we know b>o Vm-b Vm, Vm2- b Vm-b (> Asreal<ASded Vm,-b ferfat ga ha uster chag eary