Wilson / Newcombe / Denaro Experiments in Physical Chemistry

2. Auflage 2013
ISBN: 978-1-4831-8619-1
Verlag: Elsevier Science & Techn.
Format: PDF
Kopierschutz: 1 - PDF Watermark

E-Book, Englisch, 408 Seiten, Web PDF

Experiments in Physical Chemistry, Second Edition provides a compilation of experiments concerning physical chemistry. This book illustrates the link between the theory and practice of physical chemistry. Organized into three parts, this edition begins with an overview of those experiments that generally have a simple theoretical background. Part II contains experiments that are associated with more advanced theory or more developed techniques, or which require a greater degree of experimental skill. Part III consists of experiments that are in the nature of investigations wherein these investigations may be regarded as minor research project suitable for final-year students. This book is intended to be suitable for university students who are majoring in Chemistry.

Autoren/Hrsg.

Wilson, J. M.

Newcombe, R. J.

Denaro, A. R.

Inhaltsverzeichnis

1;Front Cover;1
2;Experiments in Physical Chemistry;4
3;Copyright Page;5
4;Table of Contents;6
5;Preface;10
6;List of Symbols;12
7;PART I;14
7.1;Experiments;16
7.2;Physical Properties and Molecular Structure;16
7.2.1;1. Molecular Weight using van der Waals' Equation;16
7.2.2;2. The Density of a Liquid as a Function of Temperature;18
7.2.3;3. Molar Refraction;21
7.2.4;4. Viscosity as a Function of Temperature;23
7.3;Thermodynamics;25
7.3.1;5. The Ratio of the Heat Capacities of a Gas (Clément and Desormes Method);25
7.3.2;6. The Ratio of the Heat Capacities of a Gas (Lummer and Pringsheim Method);28
7.3.3;7. Molecular Weight by Ebullioscopy (Landsberger's Method);31
7.3.4;8. Molecular Weight by Ebullioscopy (Cottrell's Method);34
7.3.5;9. Molecular Weight by Cryoscopy;36
7.3.6;10. Molecular Weight by Rast's Method;39
7.3.7;11. Heat of Neutralization by Calorimetry;40
7.3.8;12. Heat of Transition by Calorimetry;43
7.3.9;13. Heat of Vaporization by Calorimetry;44
7.3.10;14. The Vapour Pressure of a Liquid as a Function of Temperature;46
7.3.11;15. Heat of Solution from Solubility;48
7.3.12;16. Heat of Combustion by Bomb Calorimetry;50
7.3.13;17. An Equilibrium Constant by the Distribution Method;54
7.4;Phase Equilibria;56
7.4.1;18. Distillation of an Azeotropic Mixture with a Minimum Boiling Point;56
7.4.2;19. Molecular Weight of a Liquid by Steam Distillation;59
7.4.3;20. Phase Diagram for a Binary System;61
7.4.4;21. The Variation of Miscibility with Temperature;62
7.4.5;22. A Study of the Ternary System: Benzene-Acetic Acid-Water;64
7.4.6;23. The Thermal Analysis of a Hydrate by the Differential Couple Method;67
7.4.7;24. A Transition Temperature by a Solubility Method;70
7.5;Light and Spectra;72
7.5.1;25. Verification of the Lambert-Beer Law;72
7.5.2;26. Composition of a Complex Ion in Solution;74
7.5.3;Chemical kinetics;74
7.5.4;27. A Velocity Constant by a Titration Method;76
7.5.5;28. Variation of a Velocity Constant with Catalyst Concentration by a Polarimetric Method;79
7.5.6;29. A Velocity Constant by a Gas Evolution Method;82
7.5.7;30. A Velocity Constant by a Conductimetric Method;85
7.5.8;31. The Effect of Change of Temperature on the Rate of a Reaction;87
7.5.9;32. Determination of the Order of a Reaction;90
7.5.10;Surface Ohemistry and Colloids;92
7.5.11;33. Surface Tension using a Traube Stalagmometer;92
7.5.12;34. Interfacial Tension (Micrometer Syringe Method);95
7.5.13;35. Variation of the Surface Tension of a Liquid with Temperature;97
7.5.14;36. Adsorption Isotherm;100
7.6;Oonductance and Transference;103
7.6.1;37. Variation of Conductance with Concentration (Strong and Weak Electrolytes);103
7.6.2;38. Conductimetric Titration of an Acid Mixturo;106
7.6.3;39. Solubility by a Conductimetric Method;108
7.6.4;40. Transport Numbers (Hittorf's Method);110
7.7;Ionic EquiUbria;113
7.7.1;41. Dissociation Constant of a Weak Acid (Approximate e.m.f, Method);113
7.7.2;42. Dissociation Constant of a Weak Acid (Conductimetric Method);117
7.7.3;43. Hydrolysis Constant by a Conductimetric Method;119
7.8;Electrode Potential and Electrode Processes;121
7.8.1;44. The Standard Electrode Potentials of Zinc and Copper;121
7.8.2;45. Concentration Cells;125
7.8.3;46. Solubility Product from e.m.f, Measurements;127
7.8.4;47. The Quinhydrone Reference Electrode;129
7.8.5;48. pH Titration Curve;131
7.8.6;49. Study of Potentiometric and Indicator End Points;134
7.8.7;50. Potentiometric Titration-Verification of the Nernst Equation;136
7.8.8;51. Thermodynamics of Cells;138
8;PART II;142
8.1;Experiments;144
8.2;Physical Properties and Molecular Structure;144
8.2.1;52. The Radius of a Molecule from Viscosity Measurements;144
8.2.2;53. Dipole Moment of a Polar Molecule;146
8.2.3;54. The Additivity of Group Moments in Aromatic Compounds Thermodynamics;150
8.2.4;55. The Joule-Thomson Coefficient;152
8.2.5;56. The Partition Coefficient in Gas Chromatography;157
8.2.6;57. The Raoult Law Factor in Gas Chromatography;161
8.2.7;58. Activity of a Non-electrolyte by Cryoscopy;164
8.2.8;59. Activity of an Electrolyte by Cryoscopy;167
8.2.9;60. Activity Coefficient by an e.m.f, Method;175
8.2.10;61. The Partial Molal Volumes of a Binary Solution;179
8.3;Phase Equilibria;182
8.3.1;62. A Ternary Phase Diagram for a System of Two Solids and a Liquid;182
8.4;Light and Spectra;186
8.4.1;63. Emission Spectra Study of Atomic Hydrogen;186
8.4.2;64. The Ultra-violet Absorption Spectra of Geometrical Isomers;189
8.4.3;65. Force Constants from Vibrational Frequencies;192
8.4.4;66. Infra-red Spectra of Carbonyl Compounds;194
8.5;Chemical Kinetics;196
8.5.1;67. Variation of Velocity Constant with Catalyst Concentration by a Dilatometer Method;196
8.5.2;68. A Velocity Constant by an Amperometric Method;199
8.5.3;69. A Velocity Constant by a Potentiometric Method;202
8.5.4;70. A Velocity Constant by a Polarimetrie Method;204
8.5.5;71. A Velocity Constant for an Anionotropic Rearrangement (Spectrophotometric Method);208
8.6;Surface Chemistry and Colloids;210
8.6.1;72. Gas Adsorption (McBain-Bakr Balance);210
8.6.2;73. Surface Tension-Concentration Relationship for Solutions (Gibbs Equation);213
8.6.3;74. Molecular Weight of a Polymer from Viscosity Measurements;215
8.6.4;75. Electrophoresis;217
8.6.5;Conductance and Transference;220
8.6.6;76. Variation of Conductance with Concentration;220
8.6.7;77. Transport Numbers (Moving Boundary Method);222
8.6.8;78. Transport Numbers (e.m.f. Method);225
8.7;Ionic Equilibria;228
8.7.1;79. The Absorption Curve of an Indicator as a Function of pH;228
8.7.2;80. Dissociation Constant of an Acid (Accurate e.m.f. Method);231
8.7.3;81. Dissociation Constant of an Acid (Spectrophotometric Method);236
8.7.4;82. Dissociation Constant of a Weak Acid (Accurate Conductimetric Method);239
8.8;Electrode Potential and Electrode Processes;242
8.8.1;83. Dead-stop End Point Titration Technique;242
8.8.2;84. Potentiometric Titration-Solubility of Silver Halides;244
8.8.3;85. The Polarographic Method of Analysis;246
8.8.4;86. The Polarographic Method of Analysis—Wave Separation;249
8.8.5;87. Polarographic Study of Acetaldehyde;251
8.9;Radiochemistry;254
8.10;Safety Precautions;254
8.10.1;88. Separation of Radioelements by Ion Exchange;254
8.10.2;89. Distribution Constant by a Radioactive Tracer Technique;257
9;PART III;262
9.1;Investigations;264
9.2;Physical Properties and Molecular Structure;264
9.2.1;90. A Chromatographie Study of the Effects of Substitution on Acetophenone;264
9.2.2;91. A Chromatographie Study of the Relationship between Heats of Solution and Molecular Structure;268
9.2.3;92. Steric Effects and Resonance;270
9.2.4;93. Dipole Moments of Polar Compounds (Guggenheim's Method);272
9.2.5;94. Diffusion of Solvent Molecules through High Polymers;275
9.2.6;95. Interpretation of X-ray Powder Photographs;279
9.2.7;96. Delocalization Energies of ? Molecular Orbital Systems;284
9.3;Thermodynamics;291
9.3.1;97. Thermodynamic Equilibrium Constant of a Molecular Charge Transfer Complex;291
9.3.2;98. Thermodynamic Functions for Acid-Base Equilibria;295
9.4;Phase Equilibria;297
9.4.1;99. A Comparison of the Efficiency of Laboratory Fractionating Columns;297
9.5;Light and Spectra;301
9.5.1;100. The Angle of Twist around an Essential C—C Single Bond for a Series of Substituted Carbonyl Compounds;301
9.5.2;101. Relative Strengths of Hydrogen Bonds by a Spectrophotometric Method;306
9.5.3;102. The Evaluation of the Bond Angle, Force Constants and Heat Capacity of Sulphur Dioxide from its Vibrational Spectrum;309
9.5.4;103. The Internuclear Distance of Hydrogen Chloride from its Vibration- Rotation Spectrum;314
9.5.5;104. The Dissociation Energy of Iodine from its Absorption Spectrum;318
9.5.6;105. The Interpretation of Nuclear Magnetic Resonance Spectra;322
9.5.7;Chemical Kinetics;340
9.5.8;106. Explosion Limits of the Hydrogen-Oxygen Reaction;340
9.5.9;107. Mechanism of the Reaction between Hydrogen Iodide and Hydrogen Peroxide;344
9.5.10;108. The Bronsted Primary Salt Effect;347
9.5.11;109. The Variation of Rate Constant with Catalyst Concentration by a Polarimetrie Method;350
9.6;Surface Chemistry and Colloids;352
9.6.1;110. The Measurement of Surface Area by the B.E.T. Method;352
9.6.2;111. Critical Micelle Concentration;358
9.7;Ionic Equilibria;360
9.7.1;112. The Protonation of Aldehydes and Ketones in Sulphuric Acid Media;360
9.8;Electrode Potential and Electrode Processes;364
9.8.1;113. The Anodic Behaviour of Metals;364
9.8.2;114. The Polarograph: A Study of the Variables when Interpreting Polarograms;366
9.8.3;115. Differential Potentiometric Titrations;368
10;APPENDIX I: Statistical Treatment of Experimental Data;371
11;APPENDIX II: List of Textbooks;392
12;APPENDIX III: List of Instruments and Manufacturers;394
13;LOGARITHMS OF NUMBERS;399
14;ANTILOGARITHMS;401
15;INDEX;404