The Experimental Basis of Chemistry suggestions for a series of experiments illustrative of the fundamental principles of chemistryCUP Archive, 1920 - 408 ページ |
目次
INTRODUCTORY | 1 |
Fundamental differences between students illustrative experiments | 9 |
Error of experimental measurements 24 1 Nature and evaluation | 24 |
CHAPTER I | 48 |
Nature of chemical change 53 1 Typical cases to show the existence | 58 |
Criteria for the occurrence of a chemical change 59 1 Theoretical | 65 |
Historically interesting and debatable cases 76 1 Classical | 77 |
THE CLASSIFICATION OF SUBSTANCES INTO COMPLEX | 82 |
CHAPTER V | 192 |
Students Illustrative Experiments 206 1 A reaction is made | 206 |
CHAPTER VI | 225 |
substancesinteracting in solution are independent of the concentra | 235 |
The composition of the compound is independent of the relative | 245 |
CHAPTER VII | 253 |
and B present in the different compounds C1 C2 | 267 |
CHAPTER VIII | 284 |
The results of the quantitative aspect of chemical change used | 103 |
Classical researches in this province 108 1 The isolation of elements | 109 |
Method followed and practical work required in recognising | 123 |
Classical researches undertaken with the object of recognising | 132 |
Recent developments in the technique of the purification of gases | 139 |
Historical 142 1 Sequence in the discovery and the establishment | 149 |
Interpretation of the various phenomena observed in the study | 177 |
discovery and establishment of the law 288 1 Cavendish | 292 |
COMBINING OR EQUIVALENT WEIGHTS | 314 |
The experimental determination of the Combining or Equivalent | 324 |
Students Illustrative Experiments 340 1 Utilisation for the purpose | 348 |
Atomic Weight | 360 |
THE LAW OF COMBINING VOLUMES | 380 |
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accuracy action addition amount analysis apparatus atomic weight calculation carbon dioxide Chapter chemical Chemistry chlorate chloride closed collected combining weight complete composition compounds conservation of mass considerable considered constituents containing copper course density determination effect elements equal error experiment experimental fact flask gases give given glass grams heating hence hydrochloric acid hydrogen hydrogen chloride identical importance increase involved iodine iron known lead liquid matter means measurement metal method nature nitric nitrogen obtained occur original oxide oxygen phosphorus possible potash potassium practical precipitate prepared present pressure principle produced properties pure quantities ratio reaction removed represented residual salt separation shown silver nitrate simple sodium solid soluble solution standard substance suitable sulphuric acid taken temperature tube various vessel volume whole