| Journal Articles: 66 results |
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Teaching Avogadro's Hypothesis and Helping Students to See the World Differently Brett Criswell
This article uses a model from educational psychologyChi's theory of ontological misclassificationto explain the source of students' difficulties in understanding Avogadro's hypothesis and provide a method to successfully teach this fundamental concept.
Criswell, Brett. J. Chem. Educ. 2008, 85, 1372.
Atomic Properties / Structure |
Gases
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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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Effects of a Cooperative Learning Strategy on Teaching and Learning Phases of Matter and One-Component Phase Diagrams Kemal Doymus
Describes a study whose objective was to determine the effects of cooperative learning (using the jigsaw method) on students' achievement in a general chemistry course.
Doymus, Kemal. J. Chem. Educ. 2007, 84, 1857.
Gases |
Liquids |
Phases / Phase Transitions / Diagrams |
Solids
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Exception to the Le Châtelier Principle Thomas R. Herrinton
Disagreement regarding an apparent exception to the Le Chtelier principle involving the effects of nonideality on the direction in which the ammonia synthesis reaction shifts upon addition of infinitesimal and finite quantities of nitrogen at constant pressure and temperature.
Herrinton, Thomas R. J. Chem. Educ. 2007, 84, 1427.
Equilibrium |
Gases
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Exception to the Le Châtelier Principle Thomas R. Herrinton
Disagreement regarding an apparent exception to the Le Chatelier principle involving the effects of nonideality on the direction in which the ammonia synthesis reaction shifts upon addition of infinitesimal and finite quantities of nitrogen at constant pressure and temperature.
Herrinton, Thomas R. J. Chem. Educ. 2007, 84, 1427.
Equilibrium |
Gases
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Determining the Pressure inside an Unopened Carbonated Beverage Hans de Grys
Determining the pressure of carbon dioxide inside a sealed soft drink can represents a challenging student exercise. Several methods are discussed for solving the problem, including applying the ideal gas law, gas collection via water displacement, and Henry's law.
de Grys, Hans. J. Chem. Educ. 2007, 84, 1117.
Applications of Chemistry |
Aqueous Solution Chemistry |
Consumer Chemistry |
Food Science |
Gases |
Solutions / Solvents |
Student-Centered Learning
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Using Dalton's Law of Partial Pressures To Determine the Vapor Pressure of a Volatile Liquid Fred R. Hilgeman, Gary Bertrand, and Brent Wilson
This experiment, designed for a general chemistry laboratory, illustrates the use of Dalton's law of partial pressures to determine the vapor pressure of a volatile liquid.
Hilgeman, Fred R.; Bertrand, Gary; Wilson, Brent. J. Chem. Educ. 2007, 84, 469.
Gases |
Liquids |
Physical Properties |
Solutions / Solvents
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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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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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Theoretical Insights for Practical Handling of Pressurized Fluids Alfonso Aranda and María del Prado Rodríguez
Introduces the basic considerations for managing pressurized fluids, mainly liquefied and compressed gases.
Aranda, Alfonso; Rodríguez, María del Prado. J. Chem. Educ. 2006, 83, 93.
Applications of Chemistry |
Gases |
Phases / Phase Transitions / Diagrams |
Thermodynamics
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Gas Permeability of Polymers Jee-Yon Lee
Undergraduate students can learn what causes the helium-inflated balloon to fall in a few days through the proposed experiment.
Lee, Jee-Yon. J. Chem. Educ. 2005, 82, 1472.
Gases |
Transport Properties
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Gas Permeability of Polymers Bruno Lunelli
The recent article, Applying Chemical Potential and Partial Pressure Concepts To Understand the Spontaneous Mixing of Helium and Air in a Helium-Inflated Balloon, proposes a model of permeation untenable and in contradiction with correct statements present in the same text and consequently does not consider the material of which the investigated balloons are made.
Lunelli, Bruno. J. Chem. Educ. 2005, 82, 1471.
Gases |
Transport Properties
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Gas Permeability of Polymers Bruno Lunelli
By studying a number of soft drinks with color but with or without phosphoric acid, the authors have determined that the required 20-fold dilution required in the Determination of Phosphorus in Cola Drinks is not to dilute the color but merely to place the sample within the calibration range of the analysis.
Lunelli, Bruno. J. Chem. Educ. 2005, 82, 1471.
UV-Vis Spectroscopy |
Instrumental Methods |
Gases |
Transport Properties
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The Fizz-Keeper: A Useful Science Tool John P. Williams, Sandy Van Natta, and Rebecca Knipp
The Fizz-Keeper is well suited for a great variety of pressure-based activities.
Williams, John P.; Van Natta, Sandy; Knipp, Rebecca. J. Chem. Educ. 2005, 82, 1454.
Applications of Chemistry |
Colloids |
Gases
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A Note on Dalton's Law: Myths, Facts, and Implementation Ronald W. Missen and William R. Smith
The treatment of Dalton's law for gas mixtures commonly includes the improper designation "Dalton's law of partial pressures", rather than the correct "Dalton's law of additivity of (pure component) pressures". It also identifies the pure component pressure as the partial pressure, although these are only numerically equal for a mixture of ideal gases. The situation is clarified by examination of an appropriate statement of the law and definitions, eventually in operational form with reference to mixtures of nonideal gases.
Missen, Ronald Wi.; Smith, William R. J. Chem. Educ. 2005, 82, 1197.
Thermodynamics |
Gases
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Some Insights Regarding a Popular Introductory Gas Law Experiment Ed DePierro and Fred Garafalo
This paper alerts readers to a potential source of error in one approach to the Dumas method as it is often practiced in introductory chemistry laboratories. The room-temperature vapor pressures of volatile compounds that might be considered as unknowns for the experiment lead to determined molar masses that are too low. The greater the vapor pressure of the compound, the lower the determined molar mass will be, when compared to the accepted value.
DePierro, Ed; Garafalo, Fred. J. Chem. Educ. 2005, 82, 1194.
Gases |
Laboratory Equipment / Apparatus |
Phases / Phase Transitions / Diagrams |
Physical Properties
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Steel Wool and Oxygen: A Look at Kinetics James Gordon and Katherine Chancey
An experimental method is described to study the kinetics of the reaction of the iron in steel wool with molecular oxygen. A calculator-based data collection system is used with an oxygen gas sensor to determine the order of the reaction with respect to oxygen. Using the graphical method, students determine that the reaction follows first-order kinetics with respect to oxygen.
Gordon, James; Chancey, Katherine. J. Chem. Educ. 2005, 82, 1065.
Atmospheric Chemistry |
Gases |
Kinetics |
Oxidation / Reduction
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Applying Chemical Potential and Partial Pressure Concepts To Understand the Spontaneous Mixing of Helium and Air in a Helium-Inflated Balloon Jee-Yon Lee, Hee-Soo Yoo, Jong Sook Park, Kwang-Jin Hwang, and Jin Seog Kim
In developing this laboratory, our initial motivation for the analysis of gases in a balloon was to answer simple and basic questions, such as, Why does a helium-charged balloon left in the air always drop in a few days? Is leakage of helium the only cause of the drop? What is the composition of the gas in the balloon when it falls after deflation? Students were intrigued by these questions, too, as they analyzed the variation over time in the composition in a balloon inflated with helium. Using the concepts of partial pressure and chemical potential, the laboratory experiment described effectively investigates the diffusion process and the behavior of gas molecules for teaching these concepts in general and physical chemistry.
Lee, Jee-Yon; Yoo, Hee-Soo; Park, Jong Sook; Hwang, Kwang-Jin; Kim, Jin Seog. J. Chem. Educ. 2005, 82, 288.
Transport Properties |
Gases |
Mass Spectrometry |
Quantitative Analysis
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Water in the Atmosphere Joel M. Kauffman
None of eight college-level general chemistry texts gave a mean value for water in the atmosphere, despite its being the third most prevalent constituent at about 1.5% by mass as vapor and about 2% if clouds and ice crystals are included. The importance of water as a greenhouse gas was omitted or marginalized by five of the eight texts. An infrared spectrum of humid air was determined to demonstrate that water vapor, because of its higher concentration, was more absorptive than carbon dioxide. The cooling effect of clouds, or other influences on the Earth's albedo, were not mentioned in most of the texts. These pervasive errors should be corrected in new or future editions of textbooks.
Kauffman, Joel M. J. Chem. Educ. 2004, 81, 1229.
Atmospheric Chemistry |
Gases |
Green Chemistry |
IR Spectroscopy
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Chemistry and Song: A Novel Way To Educate and Entertain Cory C. Pye
In this article, a novel way of teaching chemistry is presented that uses contemporary music and chemical lyrics to educate.
Pye, Cory C. J. Chem. Educ. 2004, 81, 507.
Gases
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Just Breathe: The Oxygen Content of Air JCE Editorial Staff
Students estimate the percent oxygen (volume) in air using steel wool in a test tube that is inverted in a beaker of water. Oxygen in the trapped air reacts with iron to form rust, and the water level rises inside the test tube; within 30-45 minutes, the majority of oxygen is consumed.
JCE Editorial Staff. J. Chem. Educ. 2001, 78, 512A.
Electrochemistry |
Gases |
Oxidation / Reduction
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On Concepts of Partial Volume and Law of Partial Volume (re J. Chem. Educ. 2001, 78, 238-240) Myung-Hoon Kim
Supplementing the law of partial pressures with a law of partial volumes.
Kim, Myung-Hoon. J. Chem. Educ. 2001, 78, 1594.
Gases |
Chemometrics |
Physical Properties
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On Concepts of Partial Volume and Law of Partial Volume (re J. Chem. Educ. 2001, 78, 238-240) David W. Miller
Supplementing the law of partial pressures with a law of partial volumes.
Miller, David W. J. Chem. Educ. 2001, 78, 1594.
Gases |
Chemometrics |
Physical Properties
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On the Importance of Ideality Rubin Battino, Scott E. Wood, and Arthur G. Williamson
Analysis of the utility of ideality in gaseous phenomena, solutions, and the thermodynamic concept of reversibility.
Battino, Rubin; Wood, Scott E.; Williamson, Arthur G. J. Chem. Educ. 2001, 78, 1364.
Thermodynamics |
Gases |
Solutions / Solvents
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Determination of the Universal Gas Constant, R. A Discovery Laboratory David B. Moss and Kathleen Cornely
Discovery laboratory in which groups of students collect oxygen, hydrogen, and nitrogen gas over water and determine the value of the universal gas constant, R, using the ideal gas law.
Moss, David B.; Cornely, Kathleen. J. Chem. Educ. 2001, 78, 1260.
Gases
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A Simple Laboratory Experiment for the Determination of Absolute Zero Myung-Hoon Kim, Michelle Song Kim, and Suw-Young Ly
A novel method that employs a remarkably simple and inexpensive apparatus and is based on the extrapolation of the volume of a given amount of dry air to zero volume after a volume of air trapped inside a 10-mL graduated cylinder is measured at various temperatures.
Kim, Myung-Hoon; Kim, Michelle Song; Ly, Suw-Young. J. Chem. Educ. 2001, 78, 238.
Gases |
Physical Properties |
Chemometrics
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Potentiometric Determination of CO2 Concentration in the Gaseous Phase: Applications in Different Laboratory Activities Eduardo Cortón, Santiago Kocmur, Liliana Haim, and Lydia Galagovsky
The first lab comprises the calibration of a CO2 potentiometric detector with gas mixtures. The CO2 and CO2-free air required for the gaseous samples are produced in the lab by an inexpensive and simple apparatus. In the second lab, the CO2 potentiometric device is used to measure CO2 uptake and release during different metabolic processes.
Cortón, Eduardo; Kocmur, Santiago; Haim, Liliana; Galagovsky, Lydia. J. Chem. Educ. 2000, 77, 1188.
Electrochemistry |
Gases |
Quantitative Analysis |
Metabolism
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Paradoxes, Puzzles, and Pitfalls of Incomplete Combustion Demonstrations Ed Vitz
Paper is burned in a closed container containing sufficient oxygen to consume all the paper. Paradoxically, the flame expires while half of the paper remains. This demonstrates that thermodynamics or stoichiometry is insufficient to explain everyday chemical processes, and that kinetics is often necessary. The gases in the container are analyzed by GC before and after combustion, and the results are examined in detail.
Vitz, Ed. J. Chem. Educ. 2000, 77, 1011.
Gases |
Kinetics |
Stoichiometry
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Letters
Points out that solid NaHSO3 does not exist.
Tudela, David. J. Chem. Educ. 2000, 77, 830.
Gases |
Oxidation / Reduction |
Carbohydrates
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The Fizz Keeper, a Case Study in Chemical Education, Equilibrium, and Kinetics Reed Howald
The chemistry of the loss of carbonation from carbonated beverages on storage is considered. Increasing the pressure of CO2(g) will restore carbonation, but an increase in pressure adding air should not affect the equilibria. It can and does, however, affect the kinetics-the rate at which a new equilibrium is established. Thus the Fizz Keeper is effective for storage of resealed pop containers for hours, but not for periods of weeks or months.
Howald, Reed. J. Chem. Educ. 1999, 76, 208.
Transport Properties |
Equilibrium |
Gases |
Kinetics |
Aqueous Solution Chemistry |
Consumer Chemistry |
Applications of Chemistry
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A Precise Method for Determining the CO2 Content of Carbonate Materials Donald L. Pile, Alana S. Benjamin, Klaus S. Lackner, Christopher H. Wendt, and Darryl P. Butt
The design and use of a buret apparatus for CO2 gas capture and mass determination are described. The derivation of a comprehensive equation to determine the CO2 mass and percent carbonation of the material is outlined. Experimental factors such as temperature and pressure, including elevation effects, and apparatus parameters are discussed and incorporated into one general equation.
Pile, Donald L.; Benjamin, Alana S.; Lackner, Klaus S.; Wendt, Christopher H.; Butt, Darryl P. J. Chem. Educ. 1998, 75, 1610.
Laboratory Equipment / Apparatus |
Gases |
Quantitative Analysis
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Thermal Physics (and Some Chemistry) of the Atmosphere Stephen K. Lower
An exploration of how the temperature of the atmosphere varies with altitude can serve as a useful means of illustrating some important principles relating to the behavior of gases and to the absorption and transformation of radiant energy.
Lower, Stephen K. J. Chem. Educ. 1998, 75, 837.
Atmospheric Chemistry |
Gases
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Small-Scale Experiments Involving Gas Evolution Brouwer, H.
Apparatus for measuring very small volume changes of gases and several experimental procedures involving the evolution of gases.
Brouwer, H. J. Chem. Educ. 1995, 72, A100.
Gases |
Laboratory Equipment / Apparatus |
Stoichiometry |
Acids / Bases |
Reactions |
Mechanisms of Reactions |
Microscale Lab
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Simple analogies in general chemistry. McCullough, Thomas.
Great Plains Indians and Dalton's Law; bullets, BB's, and the photoelectric effect; and high velocity bullets and high frequency light.
McCullough, Thomas. J. Chem. Educ. 1992, 69, 543.
Gases |
Photochemistry
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Does a one-molecule gas obey Boyle's law? Rhodes, Gail
Because the kinetic molecular theory provides a plausible explanation for the lawful behavior of gases, it should be treated in enough depth to show students that the theory accounts for all of the important aspects of ideal gas behavior.
Rhodes, Gail J. Chem. Educ. 1992, 69, 16.
Gases |
Kinetic-Molecular Theory
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Le Châtelier's Principle Knox, Kerro
Question involving effect of increasing the pressure on the N2 + 3H2 <=> 2NH3 system.
Knox, Kerro J. Chem. Educ. 1985, 62, 863.
Equilibrium |
Gases
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Why teach the gas laws? Davenport, Derek A.
Justification for teaching the gas laws.
Davenport, Derek A. J. Chem. Educ. 1985, 62, 505.
Gases |
Stoichiometry
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Why do we teach gas laws? Roe, Robert, Jr.
Justification for teaching the gas laws.
Roe, Robert, Jr. J. Chem. Educ. 1985, 62, 505.
Gases |
Kinetic-Molecular Theory
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NH4HC03: a stimulant for learning Richards, R. Ronald
Students, professors, and the literature have all been confused by the unusual dissociation equilibrium of NH4HCO3.
Richards, R. Ronald J. Chem. Educ. 1983, 60, 555.
Equilibrium |
Amines / Ammonium Compounds |
Gases
|
An effective demonstration of some properties of real vapors Metsger, D. Scott
The apparatus described in this article has been found by the authors to be the most effective in vividly illustrating the behavior of a nearly ideal gas to first year chemistry students.
Metsger, D. Scott J. Chem. Educ. 1983, 60, 67.
Laboratory Equipment / Apparatus |
Gases |
Physical Properties |
Solids
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A simple experiment for determining vapor pressure and enthalpy of vaporization of water Levinson, Gerald S.
It is possible to determine the vapor pressure of water using only a tall beaker, a graduated cylinder, and a thermometer.
Levinson, Gerald S. J. Chem. Educ. 1982, 59, 337.
Water / Water Chemistry |
Gases |
Phases / Phase Transitions / Diagrams
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Gases and their behavior Schmuckler, Joseph S.
Schmuckler, Joseph S. J. Chem. Educ. 1980, 57, 885.
Gases
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A "road map" problem for freshman chemistry students Burness, James H.
Question suitable for a take-home type of exam.
Burness, James H. J. Chem. Educ. 1980, 57, 647.
Gases |
Solutions / Solvents |
Stoichiometry |
Nomenclature / Units / Symbols |
Chemometrics
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Bicarbonate in Alka-Seltzer: A general chemistry experiment Peck, Larry; Irgolic, Kurt; O'Connor, Rod
Determining the percentage bicarbonate ion by mass in Alka-Seltzer.
Peck, Larry; Irgolic, Kurt; O'Connor, Rod J. Chem. Educ. 1980, 57, 517.
Quantitative Analysis |
Gases |
Stoichiometry |
Acids / Bases
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The gases of life J. Chem. Educ. Staff
Considers the topics of diffusion, oxygen transport through the lungs, oxygen in arterial blood, and CO2 transfer.
J. Chem. Educ. Staff J. Chem. Educ. 1979, 56, 748.
Gases |
Transport Properties |
Equilibrium
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Participatory lecture demonstrations Battino, Rubin
Examples of participatory lecture demonstrations in chromatography, chemical kinetics, balancing equations, the gas laws, the kinetic-molecular theory, Henry's law, electronic energy levels in atoms, translational, vibrational, and rotational energies of molecules, and organic chemistry.
Battino, Rubin J. Chem. Educ. 1979, 56, 39.
Chromatography |
Kinetic-Molecular Theory |
Kinetics |
Stoichiometry |
Gases |
Atomic Properties / Structure |
Molecular Properties / Structure
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A discovery experiment. CO2 soap bubble dynamics Millikan, Roger C.
Students often make a choice of major based upon the view of a subject that they derive from the beginning course. Rare are the chemistry courses that provide the excitement and chance for discovery, while providing a basic understanding of chemistry. This article describes an experiment that does provide such an opportunity.
Millikan, Roger C. J. Chem. Educ. 1978, 55, 807.
Gases |
Physical Properties |
Surface Science
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An Exercise with Boyle's law Moeller, Michael B.
A procedure for doing a demonstration of Boyles' law.
Moeller, Michael B. J. Chem. Educ. 1978, 55, 584.
Gases
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Gasoline vapor: An invisible pollutant Stephens, Edgar R.
An apparatus and procedure to demonstrate the substantial contribution vaporized gasoline makes to hydrocarbon pollution.
Stephens, Edgar R. J. Chem. Educ. 1977, 54, 682.
Physical Properties |
Gases |
Atmospheric Chemistry
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Questions [and] Answers Campbell, J. A.
309-314. Six questions involving practical applications of chemistry.
Campbell, J. A. J. Chem. Educ. 1977, 54, 437.
Enrichment / Review Materials |
Toxicology |
Alcohols |
Gases |
Natural Products
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Questions [and] Answers Campbell, J. A.
188-192. Five biochemistry related questions and their answers.
Campbell, J. A. J. Chem. Educ. 1975, 52, 390.
Enrichment / Review Materials |
Nuclear / Radiochemistry |
Chromatography |
Gases |
Nutrition
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A Dalton's law experiment for students in the health sciences Feigl, Dorothy M.
The number of students who take an introductory chemistry course in preparation for the health sciences is increasing. This note is an illustration of Dalton's law of partial pressures adapted to demonstrate the ability of the lungs to effect the removal of excess dioxide from the body.
Feigl, Dorothy M. J. Chem. Educ. 1974, 51, 273.
Gases |
Biophysical Chemistry
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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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Dissolved oxygen. A relevant experiment for the introductory laboratory Stagg, William R.
Students measure the dissolved oxygen content of water from several natural sources as well as the change in solubility with temperature.
Stagg, William R. J. Chem. Educ. 1972, 49, 427.
Water / Water Chemistry |
Oxidation / Reduction |
Quantitative Analysis |
Solutions / Solvents |
Precipitation / Solubility |
Gases
|
Prolonging death (in apples) Plumb, Robert C.
Using controlled atmosphere storage to prolong the freshness of vegetables and fruits after they have been harvested.
Plumb, Robert C. J. Chem. Educ. 1970, 47, 518.
Equilibrium |
Kinetics |
Agricultural Chemistry |
Applications of Chemistry |
Gases
|
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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Baby bottles and elementary chemistry Davenport, D. A.
Presents several experiments that rely on baby bottles, including Charles' Law expansion, vapor pressure of volatile liquids, molecular weights of volatile liquids, and closed-atmosphere experiments.
Davenport, D. A. J. Chem. Educ. 1969, 46, 878.
Laboratory Equipment / Apparatus |
Laboratory Management |
Gases |
Liquids |
Oxidation / Reduction
|
An inexpensive vacuum and gas handling system for the freshman laboratory Zuehlke, R. W.; Cartier, P. G.
Presents an inexpensive vacuum and gas handling system for the freshman laboratory.
Zuehlke, R. W.; Cartier, P. G. J. Chem. Educ. 1969, 46, 874.
Laboratory Equipment / Apparatus |
Laboratory Management |
Gases
|
The range of validity of Graham's Laws Kirk, A. D.
It is the purpose of this article to discuss effusion, diffusion, and some related processes and to outline the range of validity of Graham's law.
Kirk, A. D. J. Chem. Educ. 1967, 44, 745.
Gases |
Transport Properties
|
Capillary tube experiments for introductory chemistry laboratory Gesser, H. D.; Lithown, Caroline; Brattston, D.; Thompson, Ian
Describes the use of a capillary tube to determine how vapor changes with temperature.
Gesser, H. D.; Lithown, Caroline; Brattston, D.; Thompson, Ian J. Chem. Educ. 1967, 44, 387.
Gases |
Phases / Phase Transitions / Diagrams
|
Manometric apparatus for vapor and solution studies Taha, Ahmed A.; Grigsby, Ronald D.; Johnson, James R.; Christian, Sherril D.; Affsprung, Harold E.
Presents a device that can be sued to obtain vapor density and PVT measurements, vapor pressures of solutions and liquids, dew-point pressures and compositions, solubilities of gases in liquids, solubilities of slightly-miscible liquids, equilibrium constants for association reactions in solutions, interactions of vapors and gases with solids, and gas and vapor viscosities.
Taha, Ahmed A.; Grigsby, Ronald D.; Johnson, James R.; Christian, Sherril D.; Affsprung, Harold E. J. Chem. Educ. 1966, 43, 432.
Laboratory Equipment / Apparatus |
Physical Properties |
Solutions / Solvents |
Gases |
Liquids |
Solids
|
The relationship between Avogadro's Principle and the Law of Gay-Lussac Feifer, Nathan
Teaching Avogadro's Principle as an explanation of the phenomena described by Gay-Lussac's Law gives the instructor an opportunity to stress some of the basic assumptions in chemistry and to highlight the logic implicit in Avogadro's reasoning.
Feifer, Nathan J. Chem. Educ. 1966, 43, 411.
Stoichiometry |
Gases
|
Hypodermic syringes in quantitative elementary chemistry experiments. Part 2. General chemistry experiments Davenport, Derek A.; Saba, Afif N.
Presents a variety of experiments that make use of hypodermic syringes in quantitative elementary chemistry.
Davenport, Derek A.; Saba, Afif N. J. Chem. Educ. 1962, 39, 617.
Laboratory Equipment / Apparatus |
Gases |
Liquids |
Reactions |
Equilibrium |
Stoichiometry
|
Dalton's law of partial pressures Dutton, Frederic B.
Demonstrates that breaking a sealed ampule of ether in a closed system increases the pressure inside that system.
Dutton, Frederic B. J. Chem. Educ. 1961, 38, A545.
Gases |
Ethers
|
Textbook errors: XX. Miscellanea No. 2 Mysels, Karol J.
Subjects considered include the meaning of "element," the solubility of phenol in carbonate solutions, and the change of vapor pressure with temperature.
Mysels, Karol J. J. Chem. Educ. 1958, 35, 568.
Precipitation / Solubility |
Phenols |
Gases |
Liquids
|
Textbook errors: III. The solubility of gases in liquids Mysels, Karol J.
Rising temperature is generally said to reduce the solubility of gases in liquids, yet the facts disagree with any such generalization.
Mysels, Karol J. J. Chem. Educ. 1955, 32, 399.
Gases |
Liquids |
Precipitation / Solubility |
Solutions / Solvents
|
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