The foundation of science, and of thermodynamics in particular, can be developed cogently and without arbitrariness. The goal of science, description of nature, is externally given; it requires a set of basic concepts as indispensable tools. Mathematics has no similar externally given goal. (Author/TS)

Describes basic characteristics of the electrochemical cell. Also describes basic principles of electrochemical procedures and use of these concepts to explain use of the term "primarily" in discussions of methods primarily responsive to equilibrium cell potential, bulk ohmic resistance, and the Faradaic impedance. (JN)

Provides an alternative derivation of the Boltzmann distribution based on the minimization of the Helmholtz free energy. (CS)

Provides information concerning the Boltzmann distribution mentioning partition functions, spectroscopy, basic mathematics, and its relation to temperature distribution. (CS)

Suggests a testing format suitable for thermodynamics, including questions and correct answers. Also offers a test question and an acceptable solution focusing on the elimination of certain steps in the glycolytic pathway. (SK)

Describes how Gibbs valley graphs can clarify the relation between the Gibbs function and chemical equilibrium. Gives examples from gas phase equilibria. (CS)

Describes the specifics of instruction in thermodynamics using a problem-solving technique introduced in a previous issue of this journal. (CS)

Discusses a special topics biochemistry course that uses membrance phenomena to illustrate the interplay of many physical chemistry principles. (MLH)

Describes a laboratory experiment that uses a programmable calculator and the concepts of activity and activity coefficients to examine the effect of ionic strength on equilibrium constants. (LH)

Describes an experiment that illustrates the role of hydrogen bond formation in producing a heat of reaction when ethanol and water are mixed. (MLH)

Discusses an equation that describes the variation with temperature of acid dissociation constants. (MLH)

Describes a new demonstration that uses an apparatus like the ammonia-fountain apparatus but with modifications designed to produce ammonium-chloride smoke. This demonstration is easy to perform, interesting to observe, and allows demonstration of the solubility of ammonia in water, the basic nature of ammonia, the acidic nature of hydrogen…

Presents an alternative approach to teaching reaction thermodynamics in introductory chemistry courses using calculations of enthalpies, entropies, and free energies of atomization. Uses a consistent concept, that of decomposition of a compound to its gaseous atoms, to discuss not only thermodynamic parameters but also equilibrium and…

Describes an experiment that involves the determination of the enthalpy change for a single reaction of the decomposition of aqueous hydrogen peroxide. (CCM)

Introduces a demonstration that can be used to explain elementary chemical thermodynamics of heating and boiling. (YDS)