6.18 (general formula for average values).5.130 (Saha equation for ionization of hydrogen).5.102 (equilibrium condition in terms of chemical potentials).5.90 (shift in boiling temperature of a dilute solution).5.86 (Raoult's law for the vapor pressure of a dilute solution).5.78 (van't Hoff's formula for osmotic pressure).5.72 (chemical potential of a dilute solute).5.69 (chemical potential of solvent in a dilute solution).5.61 (Gibbs free energy of an ideal mixture).5.47 (Clausius-Clapeyron relation, in terms of latent heat).5.46 (Clausius-Clapeyron relation, in terms of entropy).5.40 (chemical potential of an ideal gas in terms of pressure).5.37 (generalization of 5.35 to mixtures).5.35 (G related directly to chemical potential).5.8 (change in G related to other work).3.58 (generalized thermodynamic identity).3.55 (definition of chemical potential).3.48 (change in entropy in terms of heat).
3.5 (theoretical definition of temperature).2.40 (multiplicity of a monatomic ideal gas).2.16 (Stirling's less accurate approximation for ln N!).2.9 (multiplicity of an Einstein solid).2.6 (multiplicity of a two-state system).1.69 (shear stress in terms of viscosity).1.56 (heat capacity at constant pressure).1.44 (heat capacity at constant volume).Please don't accept this list uncritically instead,think about whether you believe each of these equations is reallyimportant, and consider whether other equations should be includedon your personal list. Of course, different readers will have differentopinions on which are the most important equations. Schroeder, Department ofPhysics, Weber State UniversityĪ reviewer has pointed out that the most important equations in the textshould be highlighted. Thermal Physics: Important Equations Important equations in An Introduction toThermal Physicsīy Daniel V.
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