| Journal Articles: 58 results |
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Does the Addition of Inert Gases at Constant Volume and Temperature Affect Chemical Equilibrium? João C. M. Paiva, Jorge Gonçalves, and Susana Fonseca
This article examines three approaches, leading to different conclusions, for answering the question "Does the addition of inert gases at constant volume and temperature modify the state of equilibrium?"
Paiva, João C. M.; Gonçalves, Jorge; Fonseca, Susana. J. Chem. Educ. 2008, 85, 1133.
Equilibrium |
Gases |
Thermodynamics
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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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EQVAPSIM: A Vapor–Liquid Equilibria of Binary Systems Computer Simulation by LabVIEW A. Belletti, R. Borromei, and G. Ingletto
Reports the results of a program using LabVIEW software to simulate the construction of a phase diagram representing a liquidvapor equilibrium. The program models work in a real laboratory, including mistakes commonly made in this context.
Belletti, A.; Borromei, R.; Ingletto, G. J. Chem. Educ. 2008, 85, 879.
Equilibrium |
Thermodynamics |
Student-Centered Learning
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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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The Use of Limits in an Advanced Placement Chemistry Course Paul S. Matsumoto, Jonathan Ring, and Jia Li (Lily) Zhu
This article describes the use of limits in topics usually covered in advanced placement or first-year college chemistry. This approach supplements the interpretation of the graph of an equation since it is usually easier to evaluate the limit of a function than to generate its graph.
Matsumoto, Paul S.; Ring, Jonathan; Zhu, Jia Li (Lily). J. Chem. Educ. 2007, 84, 1655.
Acids / Bases |
Equilibrium |
Gases |
Mathematics / Symbolic Mathematics |
Thermodynamics
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Peer-Developed and Peer-Led Labs in General Chemistry Lorena Tribe and Kim Kostka
Describes a student-developed and led laboratory curriculum as a model for producing a more student-centered and rich laboratory experience in general chemistry laboratories.
Tribe, Lorena; Kostka, Kim. J. Chem. Educ. 2007, 84, 1031.
Acids / Bases |
Electrochemistry |
Equilibrium |
Kinetics |
Laboratory Management |
Thermodynamics |
Student-Centered Learning
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Flame Emission Spectrometry in General Chemistry Labs: Solubility Product (Ksp) of Potassium Hydrogen Phthalate Frazier W. Nyasulu, William Cusworth III, David Lindquist, and John Mackin
In this general chemistry laboratory, flame emission spectrometry is used to determine the potassium ion concentration in saturated solutions of potassium hydrogen phthalate. From these data the solubility products, the Gibbs free energies of solution, the standard enthalpy of solution, and the standard entropy of solution are calculated.
Nyasulu, Frazier W.; Cusworth, William, III; Lindquist, David; Mackin, John. J. Chem. Educ. 2007, 84, 456.
Acids / Bases |
Atomic Properties / Structure |
Spectroscopy |
Equilibrium |
Quantitative Analysis |
Thermodynamics |
Titration / Volumetric Analysis |
Solutions / Solvents |
Aqueous Solution Chemistry |
Atomic Spectroscopy
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Discovering the Thermodynamics of Simultaneous Equilibria. An Entropy Analysis Activity Involving Consecutive Equilibria Thomas H. Bindel
This activity explores the thermodynamics of simultaneous, consecutive equilibria and is appropriate for second-year high school or AP chemistry. Students discover that a reactant-favored (entropy-diminishing) reaction can be caused to happen if it is coupled with a product-favored reaction of sufficient entropy production.
Bindel, Thomas H. J. Chem. Educ. 2007, 84, 449.
Acids / Bases |
Equilibrium |
Thermodynamics
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Teaching Physical Chemistry Experiments with a Computer Simulation by LabVIEW A. Belletti, R. Borromei, and G. Ingletto
This article reports on a computer simulation developed with the software LabVIEW of the physical chemistry experiment regarding the vapor pressure measurements of a pure liquid as a function of temperature, as well as a system of data collecting that emphasizes the similarities between the virtual and real experiment.
Belletti, A.; Borromei, R.; Ingletto, G. J. Chem. Educ. 2006, 83, 1353.
Equilibrium |
Laboratory Computing / Interfacing |
Liquids |
Thermodynamics |
Gases |
Student-Centered Learning
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Achieving Chemical Equilibrium: The Role of Imposed Conditions in the Ammonia Formation Reaction Joel Tellinghuisen
The conditions under which chemical reactions occur determine which thermodynamic functions are minimized or maximized. This point is illustrated for the formation of ammonia in the ideal gas approximation using a numerical exercise.
Tellinghuisen, Joel. J. Chem. Educ. 2006, 83, 1090.
Gases |
Equilibrium |
Thermodynamics
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Give Them Money: The Boltzmann Game, a Classroom or Laboratory Activity Modeling Entropy Changes and the Distribution of Energy in Chemical Systems Robert M. Hanson and Bridget Michalek
Described here is a short, simple activity that can be used in any high school or college chemistry classroom or lab to explore the way energy is distributed in real chemical systems and as an entry into discussions of the probabilistic nature of entropy.
Hanson, Robert M.; Michalek, Bridget. J. Chem. Educ. 2006, 83, 581.
Equilibrium |
Statistical Mechanics |
Thermodynamics
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Computer Simulations of Salt Solubility Victor M. S. Gil and João C. M. Paiva
Computer Simulations of Salt Solubility provides an animated, visual interpretation of the different solubilities of related salts based on simple entropy changes associated with dissolution: configurational disorder and thermal disorder.
Gil, Victor M. S.; Paiva, João C. M. J. Chem. Educ. 2006, 83, 173.
Thermodynamics |
Equilibrium |
Solutions / Solvents |
Precipitation / Solubility |
Computational Chemistry
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A New Java Animation in Peer-Reviewed JCE WebWare William F. Coleman and Edward W. Fedosky
Just added to JCE WebWare, Computer Simulations of Salt Solubility uses a Java applet and Web browser to present an animated illustration of differences in the solubility of salts due to differences in the entropy of solvation.
Coleman, William F.; Fedosky, Edward W. J. Chem. Educ. 2006, 83, 173.
Computational Chemistry |
Equilibrium |
Thermodynamics |
Solutions / Solvents |
Precipitation / Solubility
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Using Computer Simulations To Teach Salt Solubility. The Role of Entropy in Solubility Equilibrium Victor M. S. Gil and João C. M. Paiva
Pairs of salts are discussed to illustrate the interpretation of their different behavior in water in terms of the fundamental concept of entropy. The ability of computer simulations to help improve students' understanding of these chemistry concepts is also examined.
Gil, Victor M. S.; Paiva, João C. M. J. Chem. Educ. 2006, 83, 170.
Computational Chemistry |
Equilibrium |
Thermodynamics |
Solutions / Solvents |
Precipitation / Solubility
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Equilibria That Shift Left upon Addition of More Reactant Jeffrey E. Lacy
Most textbook presentations of Le Chtelier's principle in general and physical chemistry do not include a discussion of constant pressure conditions for which addition of a reactant can shift the equilibrium to the left. We propose presentations of isothermal, open systems at constant pressure for both levels of study by using concepts and skills that the respective students already possess. In addition, we derive novel criteria based on the stoichiometry of the reaction that can be used to identify those equilibria that will shift left upon addition of more reactant.
Lacy, Jeffrey E. J. Chem. Educ. 2005, 82, 1192.
Equilibrium |
Mathematics / Symbolic Mathematics |
Thermodynamics
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Microscopic Description of Le Châtelier's Principle Igor Novak
The analysis based on microscopic descriptors (energy levels and their populations) is given that provides visualization of free energies and conceptual rationalization of Le Châtelier's principle. The misconception "nature favors equilibrium" is highlighted.
Novak, Igor. J. Chem. Educ. 2005, 82, 1190.
Equilibrium |
Thermodynamics
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The Reaction Quotient Is Unnecessary To Solve Equilibrium Problems: The Reaction Quotient (Q) IS Useful After All Todd P. Silverstein
Paul Matsumoto was absolutely correct in writing The Reaction Quotient Is Unnecessary To Solve Equilibrium Problems.
Silverstein, Todd P. J. Chem. Educ. 2005, 82, 1149.
Equilibrium |
Thermodynamics
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The Reaction Quotient Is Unnecessary To Solve Equilibrium Problems: The Reaction Quotient (Q) IS Useful After All Todd P. Silverstein
Paul Matsumoto was absolutely correct in writing The Reaction Quotient Is Unnecessary To Solve Equilibrium Problems.
Silverstein, Todd P. J. Chem. Educ. 2005, 82, 1149.
Equilibrium |
Thermodynamics
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JavaScript Programs To Calculate Thermodynamic Properties Using Cubic Equations of State
Cubic equations of state are widely used by chemists and chemical engineers to predict the thermodynamic properties of both pure substances and mixtures. In particular, these equations enable predictions concerning the temperature and pressure at which vaporliquid equilibrium occurs. These two educational JavaScript programs perform calculations using cubic equations of state and, equally importantly, explain how the calculations are performed.
J. Chem. Educ. 2005, 82, 960.
Enrichment / Review Materials |
Equilibrium |
Thermodynamics
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JavaScript Programs To Calculate Thermodynamic Properties Using Cubic Equations of State Patrick J. Barrie
In this article, two JavaScript programs are described. The first program gives students the choice of five different cubic equations of state and performs calculations for pure substances. The second program predicts vaporliquid equilibrium for binary mixtures using a choice of three modern equations of state and the van der Waals mixing rules.
Barrie, Patrick J. J. Chem. Educ. 2005, 82, 958.
Enrichment / Review Materials |
Thermodynamics |
Equilibrium
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Procedure for Decomposing a Redox Reaction into Half-Reactions Ilie Fishtik and Ladislav H. Berka
The principle of stoichiometric uniqueness provides a simple algorithm to check whether a simple redox reaction may be uniquely decomposed into half-reactions in a single way. For complex redox reactions the approach permits a complete enumeration of a finite and unique number of ways a redox reaction may be decomposed into half-reactions. Several examples are given.
Fishtik, Ilie; Berka, Ladislav H. J. Chem. Educ. 2005, 82, 553.
Stoichiometry |
Equilibrium |
Electrochemistry |
Oxidation / Reduction |
Reactions |
Thermodynamics
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Playing Card Equilibrium Frank L. Lambert
From experience, I am hypersensitive to the misconceptions of students and instructors that can be caused when playing cards are used in teaching chemistry. The root of such errors lies in overlooking the non-mobile, non-energetically-interacting nature of pieces of cardboard. Only if they are being shuffled can cards serve as some sort of analogy to molecular behavior in chemistry.
Lambert, Frank L. J. Chem. Educ. 2004, 81, 1569.
Equilibrium |
Statistical Mechanics |
Thermodynamics
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Playing-Card Equilibrium Robert M. Hanson
A simple hands-on simulation suitable for either classroom use or laboratory investigation involves using a standard deck of playing cards to explore the statistical aspects of equilibrium. Concepts that can be easily demonstrated include fluctuation around a most probable distribution, Le Chtelier's principle, the equilibrium constant, prediction of the equilibrium constant based on probability, and the effect of sample size on equilibrium fluctuations.
Hanson, Robert M. J. Chem. Educ. 2003, 80, 1271.
Equilibrium |
Statistical Mechanics |
Thermodynamics
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Rubber Bands, Free Energy, and Le Châtelier's Principle Warren Hirsch
Using a rubber band to illustrate Gibbs free energy, entropy, and enthalpy.
Hirsch, Warren. J. Chem. Educ. 2002, 79, 200A.
Noncovalent Interactions |
Thermodynamics |
Equilibrium
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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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Determination of Ksp, ΔG0, ΔH0, and ΔS0 for the Dissolution of Calcium Hydroxide in Water: A General Chemistry Experiment William B. Euler, Louis J. Kirschenbaum, and Ben Ruekberg
This exercise utilizes low-cost, relatively nonhazardous materials presenting few disposal problems. It reinforces the students' understanding of the interrelationship of solubility, Ksp, ΔG0, ΔH0, and ΔS0.
Euler, William B.; Kirschenbaum, Louis J.; Ruekberg, Ben. J. Chem. Educ. 2000, 77, 1039.
Equilibrium |
Thermodynamics |
Titration / Volumetric Analysis
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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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Chemical Equilibrium (the author replies) Banerjee, Anil
Item 7 deserves a fuller answer than was provided.
Banerjee, Anil J. Chem. Educ. 1996, 73, A262.
Equilibrium |
Thermodynamics
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Chemical Equilibrium Logan, S. R.
Item 7 deserves a fuller answer than was provided.
Logan, S. R. J. Chem. Educ. 1996, 73, A261.
Equilibrium |
Thermodynamics
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Thermodynamics and Spontaneity Raymond S. Ochs
Despite the importance of thermodynamics as the foundation of chemistry, most students emerge from introductory courses with only a dim understanding of this subject.
Ochs, Raymond S. J. Chem. Educ. 1996, 73, 952.
Thermodynamics |
Learning Theories |
Equilibrium
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SIRS: Simulations and Interactive Resources, III Martin, John S.
Simulations and Interactive Resources (SIRs) are designed to support interactive lectures in introductory chemistry. This third issue of SIRs includes five new SIRs as well as updated and final versions of all previously published SIRs.
Martin, John S. J. Chem. Educ. 1996, 73, 722.
Periodicity / Periodic Table |
Equilibrium |
Gases |
Thermodynamics |
Reactions |
Electrochemistry |
Kinetics
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An Approach to Reaction Thermodynamics through Enthalpies, Entropies, and Free Energies of Atomization James N. Spencer, Richard S. Moog, and Ronald J. Gillespie
An alternative to the conventional method of calculating enthalpies of reaction is presented, using enthalpies of atomization in place of enthalpies of formation. This allows the student to see directly that the reaction enthalpies are determined by the difference in bond strengths in the reactants and products.
James N. Spencer, Richard S. Moog, and Ronald J. Gillespie. J. Chem. Educ. 1996, 73, 631.
Calorimetry / Thermochemistry |
Thermodynamics |
Equilibrium |
Reactions |
Atomic Properties / Structure |
Stoichiometry
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Solubility and Thermodynamics: An Introductory Experiment Robert G. Silberman
This article describes a laboratory experiment suitable for high school or freshman chemistry students in which the solubility of potassium nitrate is determined at several different temperatures.
Silberman, Robert G. J. Chem. Educ. 1996, 73, 426.
Precipitation / Solubility |
Thermodynamics |
Equilibrium
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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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REACT: Exploring Practical Thermodynamic and Equilibrium Calculations Ramette, Richard W.
Description of REACT software to balance complicated equations; determine thermodynamic data for all reactants and products; calculate changes in free energy, enthalpy, and entropy for a reaction; and find equilibrium conditions for the a reaction.
Ramette, Richard W. J. Chem. Educ. 1995, 72, 240.
Stoichiometry |
Equilibrium |
Thermodynamics |
Chemometrics
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Chemical equilibrium: I. The thermodynamic equilibrium constant Gordus, Adon A.
This is the first article in a series of eight that investigates the various assumptions that result in the simplified equilibrium equations found in most introductory texts. In this first article, the author considers the general nature of the constant K, Le Chatelier's principle, and the effect of the temperature on K.
Gordus, Adon A. J. Chem. Educ. 1991, 68, 138.
Thermodynamics |
Equilibrium
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A simple explanation of the salt water oscillator Noyes, Richard M.
Yoshikawa et al. have described a simple device that undergoes repeated oscillations and that can also illustrate some of the principles essential to the oscillators driven by chemical reactions.
Noyes, Richard M. J. Chem. Educ. 1989, 66, 207.
Laboratory Equipment / Apparatus |
Thermodynamics |
Equilibrium
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Amusement with a salt-water oscillator Yoshikawa, Kenichi; Nakata, Satoshi; Yamanaka, Masahiro; Waki, Takeshi
Rhythmic oscillations of water flow are generated when a vertically oriented hypodermic syringe, with the plunger removed, is filled with salt water and partially submerged in a beaker of pure water.
Yoshikawa, Kenichi; Nakata, Satoshi; Yamanaka, Masahiro; Waki, Takeshi J. Chem. Educ. 1989, 66, 205.
Thermodynamics |
Equilibrium |
Laboratory Equipment / Apparatus
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Correct equilibrium constants for water (the authors reply) Starkey, Ronald; Norman, Jack; Hinitze, Mark
Water and hydronium ion Ka values are special cases.
Starkey, Ronald; Norman, Jack; Hinitze, Mark J. Chem. Educ. 1987, 64, 1068.
Equilibrium |
Water / Water Chemistry |
Aqueous Solution Chemistry |
Acids / Bases |
Thermodynamics
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Thermodynamics of the rhodamine B lactone zwitterion equilibrium: An undergraduate laboratory experiment Hinckley, Daniel A.; Seybold, Paul G.
An experiment to derive thermodynamic values from a thermochromic equilibrium that uses a commercially available dye, attains equilibrium rapidly, and employs a simple, single-beam spectrophotometer.
Hinckley, Daniel A.; Seybold, Paul G. J. Chem. Educ. 1987, 64, 362.
Thermodynamics |
Dyes / Pigments |
Spectroscopy |
Equilibrium
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Le Châtelier's principle, temperature effects, and entropy Campbell, J. Arthur
A useful extension of Le Chatelier's Principle to predict concentration, pressure, and temperature effects solely from the equation for the net reaction.
Campbell, J. Arthur J. Chem. Educ. 1985, 62, 231.
Equilibrium |
Thermodynamics
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Thermodynamic changes, kinetics, equilibrium, and LeChatelier's principle Hansen, Robert C.
A series of demonstrations in which water in beakers and the flow of water between beakers is used to represent the components of an exothermic chemical reaction and the flow and quantity of thermal energy involved in chemical changes.
Hansen, Robert C. J. Chem. Educ. 1984, 61, 804.
Equilibrium |
Kinetics |
Thermodynamics
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Le Châtelier's principle: the effect of temperature on the solubility of solids in liquids Brice, L. K.
The purpose of this article is to provide a rigorous but straightforward thermodynamic treatment of the temperature dependence of solubility of solids in liquids that is suitable for presentation at the undergraduate level. The present discussion may suggest how to approach the qualitative aspects of the subject for freshman.
Brice, L. K. J. Chem. Educ. 1983, 60, 387.
Thermodynamics |
Liquids |
Solids |
Chemometrics |
Equilibrium
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An apparent contradiction in the application of the principle of Le Chtelier Mellon, E. K.
Unless some care is exercised, the application of free energy concepts in situations where marked temperature changes occur can lead to apparent contradictions like the one described in this paper.
Mellon, E. K. J. Chem. Educ. 1979, 56, 380.
Equilibrium |
Thermodynamics
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Le Chtelier's principle demonstrated with a rubber band Smith, Douglas D.
Heating a rubber band causes it to contract and stretching it causes it to become warmer.
Smith, Douglas D. J. Chem. Educ. 1977, 54, 701.
Equilibrium |
Thermodynamics
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Physical chemistry of the drinking duck Plumb, Robert C.; Wagner, Robert E.
The operation of the drinking bird is easily understood in terms of a few elementary physical chemistry principles.
Plumb, Robert C.; Wagner, Robert E. J. Chem. Educ. 1973, 50, 213.
Thermodynamics |
Phases / Phase Transitions / Diagrams |
Equilibrium
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LeChatelier's principle and a rubber band DeLorenzo, Ronald
The cited demonstration can also be sued to illustrate LeChatelier's principle .
DeLorenzo, Ronald J. Chem. Educ. 1973, 50, 124.
Equilibrium |
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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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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A distribution experiment Campbell, J. A.; Nelson, Douglas; Rudesill, John
An experiment to determine the distribution coefficient of an acid between an aqueous and nonaqueous phase.
Campbell, J. A.; Nelson, Douglas; Rudesill, John J. Chem. Educ. 1969, 46, 454.
Acids / Bases |
Aqueous Solution Chemistry |
Thermodynamics |
Equilibrium |
Titration / Volumetric Analysis
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A computer program for the analysis of the N2O4 dissociation equilibrium Erickson, Luther E.
Describes a Fortran IV program for the analysis of empirical data collected for the N2O4 dissociation equilibrium.
Erickson, Luther E. J. Chem. Educ. 1969, 46, 383.
Equilibrium |
Thermodynamics
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A simple analogy of the relationship of ?G to the position of equilibrium Marks, D. J.
This short note describes a simple demonstration to serve as an analogy of the relationship of ?G to the position of equilibrium.
Marks, D. J. J. Chem. Educ. 1967, 44, 402.
Thermodynamics |
Equilibrium
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Concerning equilibrium, free energy changes, LeChatelier's Principle. III. Halide-halate equilibria Eberhardt, William H.
Compares four equilibria: KI + KIO3, KI + KBrO3, KBR + KBrO3, and KBr + KIO3.
Eberhardt, William H. J. Chem. Educ. 1964, 41, A883.
Equilibrium |
Aqueous Solution Chemistry |
Thermodynamics
|
Concerning equilibrium, free energy changes, Le Châtelier's principle II Eberhardt, William H.
This demonstration involves a reversible, temperature-based transformation from blue tetrahedrally coordinated Co2+ to pink sixfold coordinated Co2+.
Eberhardt, William H. J. Chem. Educ. 1964, 41, A591.
Equilibrium |
Thermodynamics |
Aqueous Solution Chemistry |
Coordination Compounds
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Concerning equilibrium, free energy changes, Le Chtelier's principle Eberhardt, William H.
Aqueous KI is added to a solution of CuSO4 in a separatory funnel; adding more CuSO4 demonstrates an equilibrium sift.
Eberhardt, William H. J. Chem. Educ. 1964, 41, A477.
Equilibrium |
Thermodynamics |
Reactions
|
Temperature dependence of equilibrium: A first experiment in general chemistry Mahan, Bruce H.
This experiment uses cooling curves to derive the expression for the temperature dependence of the equilibrium constant.
Mahan, Bruce H. J. Chem. Educ. 1963, 40, 293.
Equilibrium |
Thermodynamics
|
Praseodymium tetrafluoride Perros, Theodore P.; Munson, Thomas R.; Naeser, Charles R.
In spite of the experimental failures to prepare praseodymium tetrafluoride, there is strong evidence for its possible formation to be found by calculating the equilibrium constants for some of the reactions by which this compound might be prepared.
Perros, Theodore P.; Munson, Thomas R.; Naeser, Charles R. J. Chem. Educ. 1953, 30, 402.
Oxidation State |
Equilibrium |
Thermodynamics
|
A temperature-equilibrium demonstration Brown, John A.
This demonstration makes use of the colored cobaltous complexes in a mixed solvent to show the dependence of some equilibria on temperature.
Brown, John A. J. Chem. Educ. 1951, 28, 640.
Equilibrium |
Calorimetry / Thermochemistry |
Thermodynamics |
Coordination Compounds
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