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Journal Articles: 22 results
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
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
Popcorn—What's in the Bag?  Marissa B. Sherman and Thomas A. Evans
Three independent activities explore microwave popcorn, the nature of the packaging, and the popcorn produced.
Sherman, Marissa B.; Evans, Thomas A. J. Chem. Educ. 2006, 83, 416A.
Carbohydrates |
Nutrition |
Physical Properties |
Solutions / Solvents |
Water / Water Chemistry
Introduction of Differential Scanning Calorimetry in a General Chemistry Laboratory Course: Determination of Molar Mass by Freezing Point Depression  Ronald P. D'Amelia, Thomas Franks, and William F. Nirode
The work described herein uses differential scanning calorimetry to determine the molar mass of three unknowns (nonvolatile organic hydrocarbons) by freezing point depression.
D'Amelia, Ronald P.; Franks, Thomas; Nirode, William F. J. Chem. Educ. 2006, 83, 1537.
Calorimetry / Thermochemistry |
Instrumental Methods |
Thermal Analysis |
Solutions / Solvents
The Ultrasonic Soda Fountain: A Dramatic Demonstration of Gas Solubility in Aqueous Solutions  John E. Baur and Melinda B. Baur
An ultrasonic bath is used to accelerate the rate at which carbonated beverages equilibrate with the atmosphere. The resulting fountain, which can reach heights in excess of 3 meters, is a dramatic demonstration of the solubility of gases in liquids.
Baur, John E.; Baur, Melinda B. J. Chem. Educ. 2006, 83, 577.
Aqueous Solution Chemistry |
Kinetics |
Physical Properties |
Solutions / Solvents |
Precipitation / Solubility
Toys in the Classroom  Jerry L. Sarquis and Arlyne. M. (Mickey) Sarquis
The chemical principles behind Shrinky Dinks, Happy Birds, and Hand Boilers are described and suggestions for hands-on activities for students are given.
Sarquis, Jerry L.; Sarquis, Arlyne. M. (Mickey). J. Chem. Educ. 2005, 82, 1450.
Solutions / Solvents
Students' Understanding of Solution Chemistry Concepts  Tacettin Pinarbasi and Nurtaç Canpolat
This study examines undergraduates' understanding of some concepts in solution chemistry such as unsaturated, saturated, and supersaturated solutions; physical properties of solutions; and gas solubility. We suggest that the results can be utilized in research that develops teaching strategies to overcome students' misunderstanding.
Pinarbasi, Tacettin; Canpolat, Nurtaç . J. Chem. Educ. 2003, 80, 1328.
Solutions / Solvents |
Aqueous Solution Chemistry |
Precipitation / Solubility
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
Are Fizzing Drinks Boiling? A Chemical Insight from Chemical Education Research  Alan Goodwin
The suggestion that fizzing drinks are examples of liquids boiling at room temperature has proved to be controversial among both chemists and chemical educators. This paper presents a case for believing this everyday system to be a good example of a boiling solution and the consequent separation of carbon dioxide from the solution to exemplify fractional distillation.
Goodwin, Alan. J. Chem. Educ. 2001, 78, 385.
Aqueous Solution Chemistry |
Kinetic-Molecular Theory |
Equilibrium |
Gases |
Solutions / Solvents |
Phases / Phase Transitions / Diagrams
Ammonia Can Crush  Ed Vitz
When a 12-oz aluminum soft drink can filled with ammonia or hydrogen chloride gas is inverted and dipped into water, the rapidly dissolving gas evacuates the can and the can is crushed before water can be drawn into it. This demonstrates, among other things, the remarkable strength of hydrogen bonds.
Vitz, Ed. J. Chem. Educ. 1999, 76, 932.
Noncovalent Interactions |
Gases |
Solutions / Solvents |
Hydrogen Bonding
Integrating Computers into the First-Year Chemistry Laboratory: Application of Raoult's Law to a Two-Component System  R. Viswanathan and G. Horowitz
First-year chemistry students are introduced to a spreadsheet program to calculate the boiling points of a two-component solution containing a volatile solute. The boiling points are predicted by combining the Clausius-Clapeyron equation and Raoult's law. A simple experimental setup is used to measure the boiling points of solutions of varying compositions.
Viswanathan, Raji; Horowitz, Gail. J. Chem. Educ. 1998, 75, 1124.
Laboratory Computing / Interfacing |
Physical Properties |
Solutions / Solvents |
Phases / Phase Transitions / Diagrams
Vapor Pressure Lowering by Nonvolatile Solutes  Gavin D. Peckham
This short article highlights a fundamental error that is entrenched in introductory chemistry textbooks. It is true that the addition of a nonvolatile solute causes a lowering in the vapor pressure of a solution. The error lies in attributing this vapor pressure lowering to the "blocking" of surface sites by nonvolatile particles. This is a totally fallacious argument for a number of reasons and the true explanation is to be found in the entropy changes that occur as a nonvolatile solute is added to a solution.
Peckham, Gavin D. J. Chem. Educ. 1998, 75, 787.
Gases |
Solutions / Solvents |
Thermodynamics
Experiments for Modern Introductory Chemistry: Intermolecular Forces and Raoult's Law  Berka, Ladislav H.; Kildahl, Nicholas
Procedure that illustrates the liquid-vapor phase equilibrium of ideal and nonideal solutions.
Berka, Ladislav H.; Kildahl, Nicholas J. Chem. Educ. 1994, 71, 613.
Noncovalent Interactions |
Gas Chromatography |
Gases |
Liquids |
Equilibrium |
Solutions / Solvents
An Ace reducing adapter for screw vials.  Canela, Ramon; Balcells, Merce.
Using this device, solvents contained in vials can be evaporated quickly without problems.
Canela, Ramon; Balcells, Merce. J. Chem. Educ. 1992, 69, 244.
Laboratory Equipment / Apparatus |
Solutions / Solvents |
Phases / Phase Transitions / Diagrams
Demonstrations of interfacial phenomena   Prall, Bruce R.
Overhead projector demonstrations that illustrate the interfacial interactions of the following systems: 1) water and carbon tetrachloride, 2) copper wire and water, 3) 1-Octanol and water.
Prall, Bruce R. J. Chem. Educ. 1991, 68, 592.
Surface Science |
Liquids |
Water / Water Chemistry |
Solutions / Solvents
A convenient method to recover the solvent from halogen-CCl4 mixtures  Sabol, Joseph E.; Kurtz, David W.
An alternative to disposal and distillation which is easy to perform, allowing the solvent to be recovered and stored within one hour after the completion of the experiment is presented here.
Sabol, Joseph E.; Kurtz, David W. J. Chem. Educ. 1990, 67, 532.
Solutions / Solvents |
Separation Science |
Laboratory Management
Molecular size and Raoult's Law  Kovac, Jeffrey
An additional cause for deviations from Raoult's Law that is rarely, if ever, mentioned in freshman chemistry texts.
Kovac, Jeffrey J. Chem. Educ. 1985, 62, 1090.
Molecular Properties / Structure |
Physical Properties |
Solutions / Solvents |
Gases
Experiments for display (Corridor demonstration)  Letcher, T. M.; Orchard, S. W.
The effect of heat on the color of cobalt(II) chloride water-alcohol solution. Refluxing solutions of different compositions.
Letcher, T. M.; Orchard, S. W. J. Chem. Educ. 1980, 57, 667.
Solutions / Solvents |
Aqueous Solution Chemistry
The precipitation of ferrous hydroxide: A lecture demonstration  Lau, O. W.
This demonstration can illustrate such topics as the solubility of ionic compounds, electrode potentials of transition elements and their modification by formation of either an insoluble compound of a complex ion, and mixed valence compounds.
Lau, O. W. J. Chem. Educ. 1979, 56, 474.
Precipitation / Solubility |
Solutions / Solvents |
Aqueous Solution Chemistry |
Transition Elements |
Metals |
Oxidation / Reduction |
Oxidation State
Miscellanea No. 6  Eberhardt, W. H.
A collection of clarified, underemphasized, and misunderstood topics, including cell electromotive force and disproportionate reactions; partially miscible liquids and upper consolute temperatures; enthalpy and free energy of formation; and magnetic moment.
Eberhardt, W. H. J. Chem. Educ. 1971, 48, 829.
Electrochemistry |
Solutions / Solvents |
Thermodynamics |
Magnetic Properties
Polywater. A lesson and opportunity in science  Christian, P. A.; Berka, L. H.
The authors present an intriguing observation and offer outlines of some possible studies that can be undertaken in any adequately equipped high school or college chemistry laboratory.
Christian, P. A.; Berka, L. H. J. Chem. Educ. 1971, 48, 667.
Water / Water Chemistry |
Solutions / Solvents
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