TIGER

Journal Articles: 18 results
The Isothermal Heat Conduction Calorimeter: A Versatile Instrument for Studying Processes in Physics, Chemistry, and Biology  Lars Wadsö, Allan L. Smith, Hamid Shirazi, S. Rose Mulligan, and Thomas Hofelich
A simple but sensitive isothermal heat-conduction calorimeter and five experiments for students to illustrate its use (heat capacity of solids, acid-base titration, enthalpy of vaporization of solvents, cement hydration, and insect metabolism).
Wadsö, Lars; Smith, Allan L.; Shirazi, Hamid; Mulligan, S. Rose; Hofelich, Thomas. J. Chem. Educ. 2001, 78, 1080.
Calorimetry / Thermochemistry |
Laboratory Equipment / Apparatus |
Thermal Analysis |
Thermodynamics
A Simple Method for Determining the Temperature Coefficient of Voltaic Cell Voltage  Alfred E. Saieed, Keith M. Davies
This article describes a relatively simple method for preparing voltaic cells, and through their temperature coefficient, ?E/?T, it explores relationships between ?G, ?H,and ?S for the cell reactions involved.
Saieed, Alfred E.; Davies, Keith M. J. Chem. Educ. 1996, 73, 959.
Electrochemistry |
Calorimetry / Thermochemistry |
Thermodynamics |
Electrolytic / Galvanic Cells / Potentials |
Laboratory Equipment / Apparatus |
Laboratory Management |
Oxidation / Reduction
Synthesis and Decomposition of Zinc Iodide: Model Reactions for Investigating Chemical Change in the Introductory Laboratory  Stephen DeMeo
Procedure for synthesizing and then decomposing zinc iodide in introductory chemistry that offers advantages over traditional synthesis/decomposition species (e.g. copper sulfide and magnesium oxide).
DeMeo, Stephen. J. Chem. Educ. 1995, 72, 836.
Synthesis |
Thermodynamics |
Reactions
An Oscillating Reaction as a Demonstration of Principles Applied in Chemistry and Chemical Engineering  Weimer, Jeffrey J.
Platinum catalyzed decomposition of methanol.
Weimer, Jeffrey J. J. Chem. Educ. 1994, 71, 325.
Thermodynamics |
Catalysis |
Transport Properties |
Kinetics |
Reactions
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
Experiments with "Calo-pH Meter"   Paris, Michel R.; Aymes, Daniel J.

Paris, Michel R.; Aymes, Daniel J. J. Chem. Educ. 1990, 67, 510.
Laboratory Equipment / Apparatus |
Thermodynamics |
Calorimetry / Thermochemistry
The entropy of dissolution of urea  Pickering, Miles
This experiment combines colorimetric techniques, thermochemical techniques, some volumetric work, and actual measurements of entropy.
Pickering, Miles J. Chem. Educ. 1987, 64, 723.
Thermodynamics
Enthalpy and Hot Wheels: An analogy  Bonneau, Marcia C.
Demonstrating the relationship between activation energy and the heat of a reaction using a "Hot Wheels" track and car to simulate a potential energy diagram.
Bonneau, Marcia C. J. Chem. Educ. 1987, 64, 486.
Kinetics |
Calorimetry / Thermochemistry |
Thermodynamics
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
Teaching about "why do chemical reactions occur": Gibbs free energy  Vamvakis, Steven N.; Schmuckler, Joseph S.
Approaching the topic of Gibbs free energy from the student's prior experience in algebra and geometry, it is possible to construct a proof that should enable students to explain the derivation of G = H - TS.
Vamvakis, Steven N.; Schmuckler, Joseph S. J. Chem. Educ. 1977, 54, 757.
Thermodynamics |
Reactions
Questions [and] Answers  Campbell, J. A.
203-205. Three chemistry questions and their answers.
Campbell, J. A. J. Chem. Educ. 1975, 52, 587.
Enrichment / Review Materials |
Thermodynamics |
Calorimetry / Thermochemistry
The first law. For scientists, citizens, poets and philosophers  Bent, Henry A.
Practical experiences and phenomena that serve to illustrate the first law of thermodynamics.
Bent, Henry A. J. Chem. Educ. 1973, 50, 323.
Thermodynamics
So-called zeroth law of thermodynamics  Redlich, Otto
The "zeroth law of thermodynamics" elucidates the difference between the axiomatic and the epistemological method; it is neither a law nor a statement of fact but a guideline for checking our description of nature.
Redlich, Otto J. Chem. Educ. 1970, 47, 740.
Thermodynamics
Thermochemistry of hypochlorite oxidations  Bigelow, M. Jerome
Students mix various proportions of aqueous sodium hypochlorite and sodium sulfite and plot the change in temperature to determine the stoichiometry of the reaction.
Bigelow, M. Jerome J. Chem. Educ. 1969, 46, 378.
Calorimetry / Thermochemistry |
Oxidation / Reduction |
Aqueous Solution Chemistry |
Stoichiometry |
Thermodynamics |
Mechanisms of Reactions
Why does methane burn?  Sanderson, R. T.
A thermodynamic explanation for why methane burns.
Sanderson, R. T. J. Chem. Educ. 1968, 45, 423.
Thermodynamics |
Reactions |
Oxidation / Reduction |
Calorimetry / Thermochemistry |
Covalent Bonding |
Ionic Bonding
Energy cycles  Haight, G. P., Jr.
Points out limitations and potential pitfalls associated with the use energy cycles to show the atomic and molecular energy factors that may influence an observable chemical property.
Haight, G. P., Jr. J. Chem. Educ. 1968, 45, 420.
Thermodynamics
Principles of chemical reaction  Sanderson, R. T.
The purpose of this paper is to examine the nature of chemical change in the hope of recognizing and setting forth the basic principles that help us to understand why they occur.
Sanderson, R. T. J. Chem. Educ. 1964, 41, 13.
Reactions |
Thermodynamics |
Mechanisms of Reactions |
Kinetics |
Synthesis |
Covalent Bonding |
Ionic Bonding |
Metallic Bonding
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