• The zeroth law defines the concept of temperature. Temperature is an intensive thermodynamic state variable.1

• The first law quantifies conservation of energy; it is entirely bookkeeping – keeping track of the types and amounts of energy stored in a system and transferred into or from it.

• The second law restricts the possible changes of forms of energy. In a nutshell, changes of energy from organized to disorganized are unconstrained, but transfers of energy from disorganized to organized are severely limited2 and are quantified by the thermodynamic efficiency; see Appendix E.11. An unavoidable consequence of the second law is the degradation of the kinetic energy of a flowing fluid to heat due to the action of viscous forces.

• E.1: a discussion of storage and transfers of energy;

• E.2: an introduction to the mole, which is a way to count atoms or molecules;

• E.3: an introduction to the first law of thermodynamics;

• E.4: a discussion and categorization of thermodynamic potentials, variables and parameters;

• E.5: the equations of state for density and entropy, including an alternate form for the first law and the equation of state for sea water;

• E.6: an introduction to ideal mixtures;

• E.7: development of the energy equation;

• E.8: a brief introduction to the thermodynamic behavior of ideal gases;

• E.9: a summary of the thermodynamics of the atmosphere;

• E.10: a discussion of phase equilibrium; and

• E.11: quantification of thermodynamic efficiency.