ABSTRACT
Some basic thermodynamic concepts that are applicable to thermitic reactions and thermites are explained. Four physical laws govern all thermodynamic interactions. Furthermore, any thermodynamic process we might imagine is reversible, irreversible, or impossible. Chemical reactions may be described as thermodynamic processes. Changes in entropy, enthalpy, and Gibbs energy characterize isothermal and isobaric transformations. A decrease in Gibbs energy indicates the maximum amount of nonexpansion work a chemical system could ever do at a constant pressure and temperature. The connections between thermodynamic work, Gibbs energy, and spontaneity are revealed. The concept of an adiabatic equilibrium state is described. Adiabatic reactions are shown to be combinations of hypothetical subprocesses. Some thermodynamic conventions concerning pure substances are explained. Oxide decomposition reactions are used to illustrate the key features of chemical decomposition equilibria and the effects of mixing interactions in the gas phase. The fundamental equation of chemical thermodynamics is shown to describe components, phases, and heterogeneous equilibria. It is also demonstrated that simplified phase diagrams can explain the basic features of adiabatic equilibrium temperature plots. In conclusion, the author notes that we are all involuntary participants in the inescapable approach to equilibrium that relentlessly continues in the aggregate.
