| Journal Articles: 70 results |
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An Updated Equilibrium Machine Emeric Schultz
Describes a device that can demonstrate equilibrium and the Le Châtelier principle, as well as kinetic and thermodynamic concepts. The device consists of a leaf blower attached to a plastic container divided into two chambers by a barrier of variable size and form. Styrofoam balls can be exchanged across the barrier when various air pressures are applied by the blower.
Schultz, Emeric. J. Chem. Educ. 2008, 85, 1131.
Equilibrium |
Kinetics |
Thermodynamics
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An Experimental Approach to Teaching and Learning Elementary Statistical Mechanics Frank B. Ellis and David C. Ellis
This article details demonstrations that show how equilibrium changes with temperature, energy, and entropy and involve exothermic and endothermic reactions, the dynamic nature of equilibrium, and Le Châtelier's principle.
Ellis, Frank B.; Ellis, David C. J. Chem. Educ. 2008, 85, 78.
Equilibrium |
Kinetics |
Statistical Mechanics |
Thermodynamics
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Configurational Entropy Revisited Frank L. Lambert
Positional entropy should be eliminated from general chemistry instruction and replaced by emphasis on the motional energy of molecules as enabling entropy change.
Lambert, Frank L. J. Chem. Educ. 2007, 84, 1548.
Statistical Mechanics |
Thermodynamics
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Job's Analysis of the Range of the "Dalton Syringe Rocket" Natalie Barto, Brandon Henrie, and Ed Vitz
An apparatus for safely igniting fuel gas/oxygen mixtures in a syringe and measuring the distance that the syringe is propelled is presented. The distance (range) is analyzed by the method of continuous variation (Job's Method) to determine the stoichiometry of the reaction.
Barto, Natalie; Henrie, Brandon; Vitz, Ed. J. Chem. Educ. 2006, 83, 1505.
Gases |
Oxidation / Reduction |
Thermodynamics |
Stoichiometry
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New Highlights on Analyzing First-Order Kinetic Data of the Peroxodisulfate–Iodide System at Different Temperatures J. Yperman and W. J. Guedens
A pseudo-first order kinetic experiment examining the peroxodisulfateiodide system is executed at different temperatures, making it possible to calculate the activation energy of this reaction.
Yperman, J.; Guedens, W. J. J. Chem. Educ. 2006, 83, 641.
Kinetics |
Laboratory Computing / Interfacing |
Oxidation / Reduction |
Rate Law |
Thermodynamics
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E = mc2 for the Chemist: When Is Mass Conserved? Richard S. Treptow
Einstein's famous equation is frequently misunderstood in textbooks and popular science literature. Its correct interpretation is that mass and energy are different measures of a single quantity known as massenergy, which is conserved in all processes.
Treptow, Richard S. J. Chem. Educ. 2005, 82, 1636.
Atomic Properties / Structure |
Nuclear / Radiochemistry |
Theoretical Chemistry |
Thermodynamics
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Conceptual Considerations in Molecular Science Donald T. Sawyer
The undergraduate curriculum and associated textbooks include several significant misconceptions.
Sawyer, Donald T. J. Chem. Educ. 2005, 82, 985.
Catalysis |
Covalent Bonding |
Electrolytic / Galvanic Cells / Potentials |
Oxidation / Reduction |
Reactions |
Reactive Intermediates |
Thermodynamics |
Water / Water Chemistry
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The q/T Paradox: Which "Contains More Heat", a Cup of Coffee at 95°C or a Liter of Icewater? Ed Vitz and Michael J. Schuman
In this demonstration, heat is removed from 10 cm3 of water at ~95C and 42 cm3 of water at ~0C by adding each to a measured sample of liquid nitrogen. The heat removed from the water boils the N2(l), and the quantity of liquid nitrogen that is evaporated by boiling is determined. The quantity of heat that was absorbed is calculated from the heat of vaporization of liquid nitrogen and found to be about 10,000 J in the case of the hot water and 25,000 J in the case of the icewater.
Vitz, Ed; Schuman, Michael J. J. Chem. Educ. 2005, 82, 856.
Calorimetry / Thermochemistry |
Heat Capacity |
Phases / Phase Transitions / Diagrams |
Thermodynamics
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Teaching Entropy Analysis in the First-Year High School Course and Beyond Thomas H. Bindel
A 16-day teaching unit is presented that develops chemical thermodynamics at the introductory high school level and beyond from exclusively an entropy viewpoint referred to as entropy analysis. Many concepts are presented, such as: entropy, spontaneity, the second law of thermodynamics, qualitative and quantitative entropy analysis, extent of reaction, thermodynamic equilibrium, coupled equilibria, and Gibbs free energy. Entropy is presented in a nontraditional way, using energy dispersal.
Bindel, Thomas H. J. Chem. Educ. 2004, 81, 1585.
Thermodynamics
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Entropy and Constraint of Motion Frank L. Lambert
William Jensen's presentation of entropy increase as solely due to kinetic energy dispersion is stimulating.
Lambert, Frank L. J. Chem. Educ. 2004, 81, 640.
Thermodynamics
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Entropy and Constraint of Motion William B. Jensen
I would like to make several observations supplementing and supporting the article by Frank Lambert on entropy as energy dissipation, since this is an approach that I have also used for many years when teaching a qualitative version of the entropy concept to students of general and introductory inorganic chemistry.
Jensen, William B. J. Chem. Educ. 2004, 81, 639.
Thermodynamics
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Why Chemical Reactions Happen (James Keeler and Peter Wothers) John Krenos
By concentrating on a limited number of model reactions, this book presents chemistry as a cohesive whole by tying together the fundamentals of thermodynamics, chemical kinetics, and quantum chemistry, mainly through the use of molecular orbital interpretations.
Krenos, John. J. Chem. Educ. 2004, 81, 201.
Mechanisms of Reactions |
Thermodynamics |
Kinetics |
Quantum Chemistry |
MO Theory
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Another Variation on the "Whoosh Bottle" Theme Edward G. Senkbeil
Description of a similar demonstration and additional safety considerations.
Senkbeil, Edward G. J. Chem. Educ. 2004, 81, 31.
Thermodynamics |
Gases
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Entropy Is Simple, Qualitatively Frank L. Lambert
Explanation of entropy in terms of energy dispersal; includes considerations of fusion and vaporization, expanding gasses and mixing fluids, colligative properties, and the Gibbs function.
Lambert, Frank L. J. Chem. Educ. 2002, 79, 1241.
Thermodynamics |
Phases / Phase Transitions / Diagrams |
Gases
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Understanding of Elementary Concepts in Heat and Temperature among College Students and K–12 Teachers Paul G. Jasien and Graham E. Oberem
Report on a study of the understanding of elementary concepts related to heat and temperature (thermal equilibrium and energy transfer in the form of heat) in undergraduate and post-baccalaurate students as a function of their number of semesters of college-level physical science training.
Jasien, Paul G.; Oberem, Graham E. J. Chem. Educ. 2002, 79, 889.
Thermodynamics |
Equilibrium
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Experiencing and Visualizing the First Law of Thermodynamics: An In-Class Workshop Pamela Mills, William V. Sweeney, and Waldemar Cieniewicz
A handheld device that illustrates the concepts of heat, work, energy transfer, and thermodynamic path.
Mills, Pamela; Sweeney, William V.; Cieniewicz, Waldemar. J. Chem. Educ. 2001, 78, 1360.
Gases |
Thermodynamics |
Laboratory Equipment / Apparatus |
Laboratory Computing / Interfacing
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Stories to Make Thermodynamics and Related Subjects More Palatable Lawrence S. Bartell
Collection of anecdotes regarding the history and human side of chemistry.
Bartell, Lawrence S. J. Chem. Educ. 2001, 78, 1059.
Surface Science |
Thermodynamics |
Kinetic-Molecular Theory |
Applications of Chemistry
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Melting Point, Density, and Reactivity of Metals Michael Laing
Using melting points and densities to the predict the relative reactivities of metals.
Laing, Michael. J. Chem. Educ. 2001, 78, 1054.
Descriptive Chemistry |
Metals |
Periodicity / Periodic Table |
Physical Properties |
Reactions |
Thermodynamics |
Calorimetry / Thermochemistry |
Electrochemistry
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Interpretation of Second Virial Coefficient Vivek Utgikar
Identifying the gel point of a polymer using a multimeter.
Utgikar, Vivek. J. Chem. Educ. 2000, 77, 1409.
Kinetics |
Lasers |
Spectroscopy |
Gases |
Thermodynamics
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A Closer Look at Phase Diagrams for the General Chemistry Course Stephen A. Gramsch
The information provided by the high-pressure phase diagrams of some simple systems (carbon dioxide, water, hydrogen, and iron) can provide a useful extension to the traditional discussion of phase diagrams in the general chemistry course. At the same time, it can prepare students for a more illuminating presentation of the concept of equilibrium than is possible through the discussion of gas phase, acid-base, and solubility product equilibria alone.
Gramsch, Stephen A. J. Chem. Educ. 2000, 77, 718.
Equilibrium |
Phases / Phase Transitions / Diagrams |
Thermodynamics |
Geochemistry
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Illustrating Thermodynamic Concepts Using a Hero's Engine Pedro L. Muiño and James R. Hodgson
A modified Hero's engine is used to illustrate concepts of thermodynamics and engineering design suitable for introductory chemistry courses and more advanced physical chemistry courses. This demonstration is suitable to illustrate concepts like gas expansion, gas cooling through expansion, conversion of heat to work, interconversion between kinetic energy and potential energy, and feedback mechanisms.
Muio, Pedro L.; Hodgson, James R. J. Chem. Educ. 2000, 77, 615.
Gases |
Thermodynamics |
Phases / Phase Transitions / Diagrams
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Boerhaave on Fire Damon Diemente
This article offers a selection of passages from Boerhaave's chapter on fire. Boerhaave offers demonstrations and experiments that can be instructively performed today, quantitative data that can be checked against modern equations, and much theory and hypothesis that can be assessed in light of modern chemical ideas.
Diemente, Damon. J. Chem. Educ. 2000, 77, 42.
Calorimetry / Thermochemistry |
Thermodynamics
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Entropy, Disorder, and Freezing Brian B. Laird
It is argued that the usual view that entropy is a measure of "disorder" is problematic and that there exist systems at high density, for which packing considerations dominate, where a spatially ordered state has a higher entropy than a disordered one.
Laird, Brian B. J. Chem. Educ. 1999, 76, 1388.
Phases / Phase Transitions / Diagrams |
Thermodynamics |
Statistical Mechanics
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Why Don't Things Go Wrong More Often? Activation Energies: Maxwell's Angels, Obstacles to Murphy's Law Frank L. Lambert
The micro-complexity of fracturing utilitarian or beautiful objects prevents assigning a characteristic activation energy even to chemically identical artifacts. Nevertheless, a qualitative EACT SOLID can be developed. Its surmounting is correlated with the radical drop in human valuation of an object when it is broken.
Lambert, Frank L. J. Chem. Educ. 1997, 74, 947.
Kinetics |
Nonmajor Courses |
Thermodynamics
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In Defense of Thermodynamics - An Animate Analogy Sture Nordholm
In order to illustrate the deepest roots of thermodynamics and its great power and generality, it is applied by way of analogy to human behavior from an economic point of view.
Nordholm, Sture. J. Chem. Educ. 1997, 74, 273.
Thermodynamics
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Teaching Chemical Equilibrium and Thermodynamics in Undergraduate General Chemistry Classes Anil C. Banerjee
Discussion of the conceptual difficulties experienced by undergraduates when dealing with equilibrium and thermodynamics, along with teaching strategies for dealing with these difficulties.
Banerjee, Anil C. J. Chem. Educ. 1995, 72, 879.
Equilibrium |
Thermodynamics
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Kinetics in Thermodynamic Clothing: Fun with Cooling Curves: A First-Year Undergraduate Chemistry Experiment Casadonte, Dominick J., Jr.
A series of experiments examining the phenomenon of cooling by producing part of the cooling curve for water at different initial temperatures, focussing on the fact that the curve is nonlinear (unlike the information presented in many texts).
Casadonte, Dominick J., Jr. J. Chem. Educ. 1995, 72, 346.
Thermodynamics |
Phases / Phase Transitions / Diagrams |
Kinetics
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Probing Student Misconceptions in Thermodynamics with In-Class Writing Beall, Herbert
Examples of the use of in-class writing assignments in the teaching of thermodynamics in general chemistry are presented.
Beall, Herbert J. Chem. Educ. 1994, 71, 1056.
Thermodynamics
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Cryophori, Hot Molecules, and Frozen Nitrogen Hunter, Paul W. W.; Knoespel, Sheldon L.
Freezing water and nitrogen at low atmospheric pressure.
Hunter, Paul W. W.; Knoespel, Sheldon L. J. Chem. Educ. 1994, 71, 67.
Thermodynamics |
Phases / Phase Transitions / Diagrams
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Photon-initiated hydrogen-chlorine reaction: A student experiment at the microscale level Egolf, Leanne M.; Keiser, Joseph T.
This lab offers a way to integrate the principles of thermodynamics and kinetics as well as other valuable instrumental methods.
Egolf, Leanne M.; Keiser, Joseph T. J. Chem. Educ. 1993, 70, A208.
Covalent Bonding |
Ionic Bonding |
Electrochemistry |
Free Radicals |
Microscale Lab |
Thermodynamics |
Kinetics
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Applications of Maxwell-Boltzmann distribution diagrams. Peckham, Gavin D.; McNaught, Ian J.
Although Maxwell-Boltzmann distribution diagrams are intuitively appealing, care must be taken to avoid several common errors and misconceptions.
Peckham, Gavin D.; McNaught, Ian J. J. Chem. Educ. 1992, 69, 554.
Thermodynamics |
Rate Law |
Catalysis
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Thermodynamics should be built on energy-not on heat and work Barrow, Gordon M.
This author looks closely at the concepts of heat, work, energy, and the laws of thermodynamics to back up his title argument.
Barrow, Gordon M. J. Chem. Educ. 1988, 65, 122.
Thermodynamics
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Thermodynamics and reactions in the dry way Tykodi, Ralph J.
In dealing with reactions in the dry way, we can actually "see" in detail the workings of the thermodynamic machinery responsible for moving the reaction in the spontaneous direction. This note presents ideas at the general chemistry level.
Tykodi, Ralph J. J. Chem. Educ. 1986, 63, 107.
Thermodynamics |
Oxidation / Reduction
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Constant properties of systems: A rationale for the inclusion of thermodynamics in a high school chemistry course Schultz, Ethel L.
Using the zinc / copper system to illustrate how the thermodynamic functions can be introduced gradually and naturally into a course of study.
Schultz, Ethel L. J. Chem. Educ. 1985, 62, 228.
Thermodynamics
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A gas kinetic explanation of simple thermodynamic processes Waite, Boyd A.
Proposes a simplified, semi-quantitative description of heat, work, and internal energy from the viewpoint of gas kinetic theory; both heat and work should not be considered as forms of energy but rather as different mechanisms by which internal energy is transferred from system to surroundings.
Waite, Boyd A. J. Chem. Educ. 1985, 62, 224.
Gases |
Kinetic-Molecular Theory |
Thermodynamics
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Further reflections on heat Hornack, Frederick M.
Confusion regarding the nature of heat and thermodynamics.
Hornack, Frederick M. J. Chem. Educ. 1984, 61, 869.
Kinetic-Molecular Theory |
Thermodynamics |
Calorimetry / Thermochemistry
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Paradigms and paradoxes Campbell, J. A.
Examines the commonly held tenets "systems tend to a minimum potential energy," "the entropy of a shuffled deck of cards is greater than that of a new deck," and "energy is the ability to do work."
Campbell, J. A. J. Chem. Educ. 1980, 57, 41.
Thermodynamics
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Corrosion: A Waste of energy J. Chem. Educ. Staff
Thermodynamics and electrochemical aspects of corrosion, and inhibition of the corrosion process.
J. Chem. Educ. Staff J. Chem. Educ. 1979, 56, 673.
Oxidation / Reduction |
Applications of Chemistry |
Metals |
Thermodynamics |
Electrochemistry
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Compact Compacts Huebner, Jay S.; Shiflett, R. B.; Blanck, Harvey F.
A collection of three suggestions regarding demonstrating the oxidation of hydrocarbons and the primary, secondary, and tertiary structure of proteins and the first law of thermodynamics as applied to air conditioning.
Huebner, Jay S.; Shiflett, R. B.; Blanck, Harvey F. J. Chem. Educ. 1979, 56, 389.
Oxidation / Reduction |
Alkanes / Cycloalkanes |
Molecular Properties / Structure |
Proteins / Peptides |
Thermodynamics
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I. How much work can a person do? Bent, Henry A.
This article relates concepts of work and energy by walking through a calculation of how much work is produced during exercise. [Debut]
Bent, Henry A. J. Chem. Educ. 1978, 55, 456.
Thermodynamics |
Biophysical Chemistry
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Using oxidation state diagrams to teach thermodynamics and inorganic chemistry Friedel, A.; Murray, R.
Using oxidation state diagrams is suggested as a means of solving some of the problems associated with the teaching of thermodynamics and inorganic group chemistry.
Friedel, A.; Murray, R. J. Chem. Educ. 1977, 54, 485.
Thermodynamics |
Oxidation State
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Free energy surfaces and transition state theory Cruickshank, F. R.; Hyde, A. J.; Pugh, D.
130/131. Unless free energy diagrams are very precisely labeled and explained they are seriously misleading and often incorporate a major error of principle. [Note: This should be #130 in the series, as shown in the table of contents. But p. 288 shows #131. The error was not caught, so the next one in the series is #132. The present article is both #130 and #131.]
Cruickshank, F. R.; Hyde, A. J.; Pugh, D. J. Chem. Educ. 1977, 54, 288.
Thermodynamics
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Freezing ice cream and making caramel topping Plumb, Robert C.; Olson, John Otto; Bowman, Leo H.
The obscurity of "colligative properties" can be dispelled by this ice cream example.
Plumb, Robert C.; Olson, John Otto; Bowman, Leo H. J. Chem. Educ. 1976, 53, 49.
Phases / Phase Transitions / Diagrams |
Physical Properties |
Thermodynamics |
Applications of Chemistry
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Brief introduction to the three laws of thermodynamics Stevenson, Kenneth L.
Brief descriptions of the three laws of thermodynamics.
Stevenson, Kenneth L. J. Chem. Educ. 1975, 52, 330.
Thermodynamics
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Scuba diving and the gas laws Cooke, E. D.; Baranowski, Conrad
Three illustrations of physical-chemical principles drawn from scuba diving.
Cooke, E. D.; Baranowski, Conrad J. Chem. Educ. 1973, 50, 425.
Gases |
Applications of Chemistry |
Thermodynamics
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Footnote to the house heating exemplum Plumb, Robert C.; Campbell, J. A.
Offers a simple proof regarding an earlier column.
Plumb, Robert C.; Campbell, J. A. J. Chem. Educ. 1973, 50, 365.
Thermodynamics |
Gases
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When You Heat Your House Does the Thermal Energy Content Increase? Bilkadi, Zayn; Bridgman, Wilbur B.
Whether or not the total energy content of the air increases or decreases cannot be answered unambiguously.
Bilkadi, Zayn; Bridgman, Wilbur B. J. Chem. Educ. 1972, 49, 493.
Thermodynamics
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Entropy Makes Water Run Uphill - in Trees Stevenson, Philip E.
Explains how Sequoias over 300 feet tall can draw water up to their topmost leaves.
Stevenson, Philip E. J. Chem. Educ. 1971, 48, 837.
Applications of Chemistry |
Thermodynamics |
Plant Chemistry |
Membranes |
Transport Properties |
Solutions / Solvents
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Tire Inflation Thermodynamics Plumb, Robert C.; Connors, John J.
Explains why inflating a tire with a hand pump heats the air being pumped into the tire.
Plumb, Robert C.; Connors, John J. J. Chem. Educ. 1971, 48, 837.
Gases |
Thermodynamics |
Applications of Chemistry
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An alternative to free energy for undergraduate instruction Strong, Laurence E.; Halliwell, H. Frank
It is the purpose of this paper to question the usefulness of the Gibbs function for the student and to propose an alternative based on the use of entropy functions that help the student to focus more sharply on the features of a system that relate to its capacity to change.
Strong, Laurence E.; Halliwell, H. Frank J. Chem. Educ. 1970, 47, 347.
Thermodynamics
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Our freshmen like the second law Craig, Norman C.
The author affirms the place of thermodynamics in the introductory chemistry course and outlines a presentation that has been used with students at this level.
Craig, Norman C. J. Chem. Educ. 1970, 47, 342.
Thermodynamics
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Sealed tube experiments Campbell, J. A.
Lists and briefly describes a large set of "sealed tube experiments," each of which requires less than five minutes to set-up and clean-up, requires less than five minutes to run, provides dramatic results observable by a large class, and illustrates important chemical concepts.
Campbell, J. A. J. Chem. Educ. 1970, 47, 273.
Thermodynamics |
Crystals / Crystallography |
Solids |
Liquids |
Gases |
Rate Law |
Equilibrium
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Cloud Caps on High Mountains Stevenson, Philip E.
The formation of cloud caps on high mountains illustrates cooling in an adiabatic expansion and the change in vapor pressure of a liquid with temperature.
Stevenson, Philip E. J. Chem. Educ. 1970, 47, 272.
Atmospheric Chemistry |
Gases |
Applications of Chemistry |
Phases / Phase Transitions / Diagrams |
Thermodynamics
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The Methanol Lighter Bailar, John C., Jr.
The methanol lighter illustrates the roles that thermodynamics, kinetics, and catalysis play in determining if a reaction will take place.
Bailar, John C., Jr. J. Chem. Educ. 1970, 47, 272.
Thermodynamics |
Kinetics |
Catalysis |
Consumer Chemistry |
Applications of Chemistry
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The snowmaking machines Plumb, Robert C.
Illustrating principles of thermodynamics in gas expansions and phase changes.
Plumb, Robert C. J. Chem. Educ. 1970, 47, 176.
Gases |
Thermodynamics |
Phases / Phase Transitions / Diagrams
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Chemical principles exemplified Plumb, Robert C.
Introduction to a new series, containing "exempla" (brief anecdotes about materials and phenomena which exemplify chemical principles). [Debut]
Plumb, Robert C. J. Chem. Educ. 1970, 47, 175.
Gases |
Kinetic-Molecular Theory |
Phases / Phase Transitions / Diagrams |
Thermodynamics |
Equilibrium |
Photochemistry |
Applications of Chemistry
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Quantities of work in thermodynamic equations Wright, P. G.
Examines distinctions to be made between work done by forces exerted by external bodies and acting on a system with work done by forces exerted by the system on external bodies.
Wright, P. G. J. Chem. Educ. 1969, 46, 380.
Thermodynamics
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Chemical queries. Especially for introductory chemistry teachers Young, J. A.; Malik, J. G.
(1) Is there such a thing as a negative pH value? Or one above 14? (2) What is entropy, in terms a beginner may understand? (3) On calculating the molecular weight of a solute from concentration and freezing point depression.
Young, J. A.; Malik, J. G. J. Chem. Educ. 1969, 46, 36.
Acids / Bases |
Aqueous Solution Chemistry |
pH |
Thermodynamics |
Molecular Properties / Structure
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Chemical dynamics for college freshmen Hammond, George S.; Gray, Harry B.
Suggestions for topics regarding chemical dynamics to be considered in freshman chemistry.
Hammond, George S.; Gray, Harry B. J. Chem. Educ. 1968, 45, 354.
Thermodynamics |
Kinetics |
Reactions |
Mechanisms of Reactions |
Rate Law
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Biological oxidations and energy conservation Kirschbaum, Joel
Examines the oxidative steps leading to the synthesis of ATP in living organisms and their metabolic control.
Kirschbaum, Joel J. Chem. Educ. 1968, 45, 28.
Bioenergetics |
Oxidation / Reduction |
Thermodynamics |
Metabolism
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Demonstrations of spontaneous endothermic reactions Matthews, G. W. J.
The reaction between hydrated metal chlorides and thionyl chloride provides a series of valuable experiments that can be used to demonstrate spontaneous endothermic reactions.
Matthews, G. W. J. J. Chem. Educ. 1966, 43, 476.
Reactions |
Thermodynamics |
Calorimetry / Thermochemistry
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Maximum work revisited (Letters) Mysels, Karol J.
Comments on an earlier "Textbook Error" article that considers at length errors in the calculation of work done in compression or expansion of an ideal gas.
Mysels, Karol J. J. Chem. Educ. 1964, 41, 677.
Thermodynamics |
Gases
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Maximum work revisited (Letters) Bauman, Robert
Comments on an earlier "Textbook Error" article that considers at length errors in the calculation of work done in compression or expansion of an ideal gas.
Bauman, Robert J. Chem. Educ. 1964, 41, 676.
Thermodynamics |
Gases
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Maximum work revisited (Letters) Kokes, Richard J.
Comments on an earlier "Textbook Error" article that considers at length errors in the calculation of work done in compression or expansion of an ideal gas.
Kokes, Richard J. J. Chem. Educ. 1964, 41, 675.
Thermodynamics |
Gases
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Maximum work revisited (Letters) Bauman, Robert
Comments on an earlier "Textbook Error" article that considers at length errors in the calculation of work done in compression or expansion of an ideal gas.
Bauman, Robert J. Chem. Educ. 1964, 41, 675.
Thermodynamics |
Gases
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Teaching the entropy concept Plumb, Robert C.
Presents a macroscopic lecture demonstration illustrating both potential energy and entropy driving forces and showing their interrelationship.
Plumb, Robert C. J. Chem. Educ. 1964, 41, 254.
Thermodynamics |
Statistical Mechanics
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Work of compressing an ideal gas Bauman, Robert P.
In formulating examples of compression problems there should be an explicit statement that the process is reversible, or at least slow.
Bauman, Robert P. J. Chem. Educ. 1964, 41, 102.
Thermodynamics |
Gases
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A second lecture in thermodynamics Burton, Milton
Outlines an introduction for the three laws of thermodynamics
Burton, Milton J. Chem. Educ. 1962, 39, 500.
Thermodynamics
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How can you tell whether a reaction will occur? MacWood, George E.; Verhoek, Frank H.
This paper attempts to answer the title question in a clear and direct fashion.
MacWood, George E.; Verhoek, Frank H. J. Chem. Educ. 1961, 38, 334.
Thermodynamics
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A heat engine run by rubber Cox, E. G.
Describes a rotating wheel powered by the alternate heating and cooling of rubber bands.
Cox, E. G. J. Chem. Educ. 1954, 31, 307.
Thermodynamics
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