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Abstracts of the Proceedings of the Chemical Society, Vol. 2, No. 24 |
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Proceedings of the Chemical Society, London,
Volume 2,
Issue 24,
1886,
Page 197-208
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摘要:
ABSTRACTS OF THE PROCEEDINGS OF THE CHEMICAL SOCIETY. No. 24. Session 1885-86. May 20th, 1886. Dr. Hugo Muller, F.R.S., President, in the Chair. Certificates were read for the first time in favour of Messrs. Thomas Akitt, 25, Gascoyne Road, South Hackney, London; Alfred C. A. W. H. Chapman, 2, Quecn Anne’s Avenue, High Road, South Tottenham ; Charles Alexr. Kohn, Redcliffe Villa, Redcliffe Road, Nottingham ; John Temple Leon, 26, Belsize Park Gardens, N.W. ; William Ray, Spenceley House, Victoria Road, Leeds ; William Richards, 185, Islcdon Road, Pinsbary Park, London, N. ; Joseph Price Remington, 1233, Walnut Street, Philadelphia, U.S. ; William Saunders, London, Ontario, Canada,; Charles A. Smith, The Laboratory, 8, Loftus Street, Sydney. The following were duly elected Fellows of the Society :-3Iessrs.Edward Jenniiigs Ball, Ph.D., Holland Crompton, Parvati Nath Datta, Robert Elliott Doran, Richard Dormer, Witham Dobin- son Halliburton, George William Saul Howson, John Tysilio Johnson, A. Wentworth Jones, William Henry Pendlebury, William Selby Simpson, Henry H. Walker. The President exhibited a specimen of the mineral Argyrodite-a sulphogermaniate of silver ; also a number of specimens which he had recently received from Prof. Winkler of the new element Ger- manium (ante, p. 161) and its derivatives. He said that, according to the information given to him, germanium was a silver-white, brittle, volatile metalloid of the relative density 5.46 ; its atomic weight is 72.75.It appears to be identical with Mendelejeff’s E’lt.asiZicium,for which the atomic weight predicted was 72 and the relative density 5.5. Germanium forms two sulphides, a yellow monosulphide, soluble in alkali, which readily volatilises, subliming in well-formed crystals somewhat like those of iodine in colour; and it white 198 disulphide. It furnishes corresponding oxides : a liquid tetrachloride, boiling at 88" ; and an orange-red, crystalline, volatile tetriodide. Mr. Newlands called attention to the fact that in 1864 he had predicted the existence of an element having the atomic weight 73,and belonging to the carbon-silicon group. Dr. Sprengel exhibited a series of specimens illustrating the effect produced on leaden cylinders by the explosion of equal weights (15 grams) of nitroglycerine and of mixtures of half nitric peroxide and half (a) CS2, (b) benzene, (c) nitrobenzene, (a) nitrotoluene. The effect produced by the nitroglycerine was very much less marked than that produced by any of the other explosives, of which those containing nitrobenzene and nitrotoluene were by far the most powerful, The following papers were read :-46.'(Sources of Error in the Calorimetric Study of Salts." ByProf. W. A. Tilden, F.R.S. Mr. Pickering has recently published in the Transactions of the Chemical Society a paper containing very numerous esiimations of the heat of dissolution of various salts at temperatures ranging from near zero to about 25" C., and in the Phil. Mag. for March and April he has given an account of the precautions he has taken to avoid experi- mental error or to make allowance for it.In his principal paper (Chem. SOC.Trans.,May, 1886) he arrives at such extraordinary conclusions in regard to the behaviour of salts in act of dissolution in water, and at the same time protests so emphati-cally against the suspicion that the irregularities he has observed are due to experimental error, that having been myself occupied with experiments in the same direction, I have been led to examine Mr. Pickering's paper very carefully. The process of dissolving a solid in water in such a manner as to allow of the determination of the heat evolved or absorbed is one which is beset with difficulties. But these are not all of equalimport-ance, some being so small as to produce little or no appreciable effect on the result, others, however, being of such a formidable character as to render such determinations extremely difficult and uncertain.Mr. Pickering claims that his results exhibit an extremely high and altogether exceptional degree of accuracy. Without this exceptional accuracy the conclusion which he deduces cannot be maintained. A critical examination of the numbers recorded in his tables of results shows that his experiments, though undoubtedly conducted with great care and skill, have not led to results of any very unusual accuracy, and in fact that there are in many cases great discrepancies in the results of duplicate experiments. Some of these discrepancies I attribute to a want of discrimination between the several sources of error in respect to their influence on the result, Mr.Pickering has given great attention to the calibration and observation of his thermometers, even using instruments said to be capable of reading to aGbath of a degree C., but he has given no detailed account of his method of correcting for the cooling or heating by radiation or conduction of the calorimeter during the progress of the experiment, although this latter, as he admits, is by far the most serious source of error, and might lead to a difference a hundred times greater than that arising from ordinary errors .in calibration or reading of thermometers. Again, it would doubt- less be impossible in such experiments to ensure the accomplish-ment of the act of dissolution in the several experiments at any given temperature in equal times; and yet if this is not done an error is introduced which it is impossible to estimate by observation of the rate of cooling before or after the experiment.However, it is not suggested that Mr. Pickering's results are less than usually accurate, but only that they do not reach that unassail- able standard which alone would justify the conclusions he draws from them. The supposition that the heat of dissolution of a given salt in water at successively higher temperatures is represented by a succession of irregular curves is not supported by Mr. Pickering's own experimental numbers, but results from the unjustifiable employ- ment of arithmetical means.When aZZ the numbers given in the tables are plotted on curve paper the remarkable sinuosities pointed out by Mr. Pickering for the most part disappear. One does perceive, however, that the discrepancies among the individual results are so great as to preclude the possibility of drawing from them any con- clusion whatever as to the exact form of the curve in the several cases. DISCUSSION. Mr. PICKERINGsaid that no one could be more fully aware than he was himself that the irregularities which he had observed depended on differences but little larger than those due to experimental error. The whole difficulty of the investigation lay in this very fact. No one could have laboured more energetically than he himself had done to disprove these irregularities, and he only accepted them when their existence became undeniable.In his opinion it was distinctly a case in which the means from a large number of experiments, and not each individual determination, should be considered. Taking the instances selected by Dr. Tilden, he contended that the irregularities could not be regarded as experimental emors. In the case of potassium sulphate the heat of dissolution from 26.5"to 17" is represented by a straight 200 line; from 11" down to 3' it is represented by another line at a different inclination from the first, but scarcely less straight. If the point at 14"is to lie in the first line the heat of dissolution there would be 6870 cals., if in the second line 6820 cals.Now of the eight determinations on which the observed depression at this point was based, the lowest was only 6908 cals. ;the mean of four determinations with one thermometer gave 6941 cds., and of four other determina- tions with another thermometer 6963. By no possibility could Dr. Tilden manipulate those numbers so as to lower them even to 6870, and fhus obliterate the depression which they represent. The only other means by which this could be done would be to admit an error of at least 82 cals. in the geneml results of all the other experiments -70 in number-at the other temperatures; a proposition quite inadmissible. Mr. Pickering professed himself ready to discuss in the same way the irregularities in any of the other curves.Dr. Tilden had specially alluded to the depression in the curve of CUE:,(SO~)~*~H~O,which was the one salt least fully examined of all ; as Mr. Pickering had mentioned in his paper (p. 282), he would have paid but little attention to this depression were it not that there was subsidiary evidence that the point at which it occurs (14") was a temperature at which the salt experienced some marked alteration. Looking at the curve representing the heat of combination of the salt with its water of crystallisation, it would be seen that this heat is represented by a straight line from 2" to 12" showing the rapid increase of 130 cals. per degree, while from 16" to 23" the heat of combination remains constant.On the strength of there being but one determination with K2SO* at 12-36', Dr. Tilden accused him of having repeated experiments at the debatable points without having examined the points in its vicinity. This charge Mr. Pickering entirely denied. In the case in point Dr. Tilden would find on a more careful examination that within about 3" of the temperature where the depression was noticed (14", there being eight experiments here) he had made no less than 19 determinations. Again, the lowest point (13.14") in the MgS04*7H20curve, at which there were seven determinations, was accompanied by nine determinations at other temperatures within 1.5" of it. It was certainly natural, and indeed indispensable, that any point at which an anomaly was noticed should be more fully examined than other normal points, but the repetition of such experiments was generally accompanied by the repetition of other experiments at points above and below it, though not necessarily very near to it, and as a further precaution these experiments at different temperatures were in many cases, and at the expense of immense labour, per- formed on the same day (p.281). 201 Dr. Tilden suggested that Mr. Pickering, while fully alive to the less important errors introduced by defects in the thermometers, might have overlooked the greater errors involved in determining the rate of cooling, and in the manipulation generally. Dr. Tilde11 Would, however, find that in a paper read before the Physical Society (P7d.Mag., 1886, p.324) he had discussed not the errors inherent in thermometers, as he did in two other papers (ibid.,180,330), but the errors of calorimetric work as illustrated by the actual results obtained in these very experiments themselves, results which had been influenced by and would therefore afford a criterion of the accu- mulated errors from all sources. Mr. Pickering then described his method of operation, and ex-plained that the determination of the rate of cooling was far more simple in his experiments than those of Dr. Tilden; for the tern- perature of the air is always the same as that of the calorimeter, and the rate of cooling was thus reduced SO far as to be constant for the whole duration of the experiment. Mr.Pickering had found that even where the dissolution of a salt was not completed within five minutes or more, the final temperature of the calorimetric water was practically attained within about half a minute; it was during this short space of one half minute only that the temperature and there- fore the cooling correction was uncertain. Dr. WRIGHT remarked that according to his experience the experi- mental error was much greater if the substances to be mixed were at the temperature of the air ; the error due to radiation was much less if the temperature initially was as much below as it was finally above atmospheric temperature. Prof. TILDEN, in reply, said that he thought that Mr. Pickering had failed to explain the discrepancies which he had pointed out.47. "On the Action of Aldehydes and Ammonia on Benzil." By Francis R. Japp, F.R.S., and W. Palmer Wynne, B.Sc. The compounds obtained with acetaldehyde and isovaleraldehyde are the glyoxalines- C6H5*C-NH CsH,*C-NH11 \C*CH, and II \C*CH~.CH(CH~)~.CsH5.C--N/ C~H~~C-N/ Methyldiphenylglyoxaline(m. p. 235"). Isobutyldiphenylglyoxaline(m. p. 223"). With cinnnmaldehyde, benzil and ammonia, two reactions occur, two distinct compounds being formed, one of which is practicztlly insoluble, the other moderately soluble, in boiling alcohol. The insoluble compound has the formula C32Hz8Nz02,and is an analogue 202 of that obtained by Japp and Hooker from salicylaldehyde, benzil and ammonia.It has the constitution- C6H5*CH:CH*CH*NH*CO.CsH,I CsH5CH :CH*CHoNH*CO*C6H5 Dibenzoyldicinnylenediamine (m.p. 264'). Heated with a solution of potash in methyl alcohol, it yields benzoic acid and the compound- C6H5*CH:CH*CH-NHI 'C*C6H5. C6H5*CH:cH*cH-N' Benzenyldicinnylenediamine(m. p. 207"). The soluble compound melts at 188". It has the formula C37H30N203= 2C14Hlo02+ C9H,0 + 2NH3 -H20. As this com-pound may be regarded as imabenzil in the formation of which 1 mol. of cinnamaldehyde has taken the place of 1mol. of benxaldehyde, it is proposed to name it cinnirnabensil. This is the fourth of the distinct rea>ctions in which diketones, aldehydes and ammonia react jointly to form condensation products (comp. this Journal, 1884, Trans., 672).By treatment in the cold with a solution of potash in methyl alcohol, the compound C37H30N203is decomposed into benzoate and the compound C30H26N20,(m. p. 283'). 48. '(On Imabenxil." By the same. In repeating the work of Laurent on the action of ammonia upon benzil, Henius arrived at the conclusion that the three compounds described by Laurent possessed the following formulae :-Imabenzil.. ...... C42H32N204. Benzilimide.. .... C42H32N204n Benzilam.. ...... C42HXN202. In a preliminary note on the same subject (Bey., 16,2636), Dr. Japp showed that benzilam has the formula CZ1Hl5NO,and that benzilimide, from which it may be obtained by the abstraction of the elements of water, is C21H17N02.He ascribed to these compounds the constitution- c&&,*c-o,11 //c*c6&CeH5*C-N Cf3H5*C--0]ICGH5.C-NH >C(OH) *CJ35.Benzilam. Benzilimide. 203 These formulae have since been accepted by Henius (Ann., 228,339). In the note above referred to, Dr. Japp further admitted that the formula assigned by Henius to imabenzil was probably correct, basing this opinion upon an examination of amorphou,s imabenzil prepared by the method of Henius. The authors have now prepared crystaZZised imabenzil, and have been able to rectify its formula, which they find to be C35H28N203.It is formed from benzil and ammonia according to the equation- 3ClaH10Oz+ 2NH3 = C35H~8N203+ C,H,*COOH+ H20. Irnabenzil as prepared by Henius contains unaltered henzil. Contrary to the statement of Henius, imabenzil can be readily recrystallised; methyl alcohol was found to give the best results.The crystals have been measured by Mr. L. Fletcher, and found to agree with the description and approximate figure given by Laurent,. The melting point was found at 194". 49. "On Ammonia-derivatives of Benzoin." By Francis R. Japp, F.R.S., and W. H. Wilson, Ph.D. The action of alcoholic ammonia upon benzoyn was studied by Laurent and later by Erdmann. Both these chemists obtained a substance of the formula C2,H2,N20,to which Laurent gave the name benzoznam. Erdmann further isolated a substance which he called henzohimide, assigning to it the formula ClaH,N. The authors confirm the formula of Laui-ent and Erdmann for benzoham.Their analyses of benzoinimide, however, lead to the formula C28HzoNZ. They regard it as an analogue of diphenanthrylene-azotide, C2SH16N2, and as it can no longer be classed as an imide, they propose to call it ditoZane-azotide. It is most readily obtained free from the other compounds formed from benzo'in and ammonia, by heating benzoin with fused ammonium acetate over a flame until the whole of the ammonium salt is volatilised. A third compound, not described by the foregoing investigators, was obtained. It is formed in largest quantity when benzo'in is allowed to stand with alcoholic ammonia for several weeks in tbe cold. It crystalliscs from alcohol in minute oblique tables or prisms melting at 199". The analyses agreed best with the formula C?8H23N02.The equation for its formation would be 2C14H1202+ NH, = C&2,N02 + 2Hz0. As nothing is known concerning its constitution, it may be named, for the sake of distinction, benzoinidam. 50. "On Compounds from Benzil and Renzo'in and Alcohols." By Francis R. Japp, F.R.S., and Julius Raschen. 204 The authors have made experiments to ascertain whether other alcohols besides ethyl alcohol form condensation compounds with benzil in presence of a small quantity of caustic potash in the cold (comp. Trans., 1885, 90). Of the various alcohols employed only isopropyl alcohol yielded a result. A compound of the formula C,lH,,Oa was obtained, which is deposited from alcohol in small lustrous faintly yellow cryshals, of rhombohedra1 habit, melting at 147-148'.The benzil and isopropyl alcohol react according to the equation : 2C14H1002+ CsH,O = C31H2@4 + 0, and the compound is therefore formed by a process of reduction, and is not analogous to the compound C30H2504, which, as was shown by Owens and Japp (Zoc. cit.), is formed from ethyl alcohol and benzil merely by elimina- tion of water. The action of a small quantity of potash at ordinary temperatures upon benzo'in dissolved in various alcohols was also tried, but only in the case of ethyl alcohol was a definite result obtained. Air must be carefully excluded during the reaction otherwise the benzoin is oxidised to benzil. Benzoin slowly reacts with ethyl alcohol, in pre- sence of a small quantity of potash : 3Cl4H1202 + 2C2H60= C46H4004 + 4H20 ; the compound C46H4004thus obtained corresponds with the compound Ca6H3404formed by the interaction of the same molecular proportions of benzil and ethyl alcohol (Zoc.cit.). The benzoin compound, C4cH4004,melts at 249-250". 51. "On the Action of Phosphoric Sulphide on Renzophenone." By the same. By heating benzophenone with phosphoric sulphide for two days at 100" the authors obtained a compound C26H,S2, melting at 152", previously described by Engler, who prepared it both by the action of alkaline hydrosulphides upon benzophenonidene dichloride, (CcH5)CCl,, and by heating benzhydrol with phosphoric sulphide. At a temperature of 140-150" benzophenone and phosphoric sulphide yielded a compound of the formula C26HzoP2S5.It 'crystal-lised from hot benzene in colourless microscopic plates melting at 226-227".It decomposes in melting, assuming a, deep-blue colonr. It may be regarded as an ethereal thio-salt €ormed by the union of 2 mols. of thiobenzophenone, (c&)&s, with 1 mol. of phosphorous sulphide, P2S3.Its constitution may be expressed by the formula- It would thus be a bensophenonidenepyrothiophosphite. On oxidation with a solution of chromic anhydride in glacial acetic acid, it yields benzophenone. 52. “The Separation and Estimation of Zirconium by means of Hydrogen Peroxide.” By G. H. Bailey, D.Sc., Ph.D. The author has determined zirconium by means of hydrogen peroxide in a number of mixtures containing also iron, titanium and niobium, and finds that even when the zirconium forms only 2.3 per cent.of the mixture the method of separation which he has pre- viously described (Trans., 1886, 149) is applicable and the results obtained are accurate. The zirconia precipitated in presence of a large excess of iron or of titanium does not contain a trace of these elements. The oxide generally obtained by means of hydrogen peroxide is the pentoxide, but he has also obtained a higher oxide, ZrO,, apparently identical with that described by C16ve. The dried oxides have a composition approximating to Zr206*4Hz0 and ZrO3*5H,O, though oxygen is lost at loo”, and the product remaining is not definite in composition. Dried at 15”,however, the higher oxide retains the whole of its oxygen, and is evidently more stable than the pentoxide.Dilute mineral acids and acetic acid, which dissolves freshly precipitated zirconia quite readily, fail to act on these oxides except on prolonged heating. 53. “An Apparatus for the Determination of the Temperature of Decomposition of Salts.” By G. H. Bailey, D.Sc., Ph.D. The apparatus is for the purpose of maintaining a substance at a given temperature for a proionged period, and permits of the tempe- rature attained being determined, while any change taking place in the substance can be observed. The author proposes to apply it in the first instance to the study of sulphates used in atomic weight determinations. The bulb of an air-thermometer and a narrow tube into which a boat containing the salt to be heated can be introduced are fixed side by side in a hard glass jacket tube, in shape like a test- tube, which can be heated in an iron tube furnace; the capillary stem of the air thermometer is bent at a right angle and its end is connected by a ground joint to the one limb of a U-tube, charged with mercury, fixed in front of a graduated scale ; the other limb of the tube is arranged to act as a gas regulator.The position of the mercury at various temperatures having been once for all determined, it is easy to observe the temperature within the tube to which the substance is subjected ; the temperature can be maintained constant to within a degree or two even at high temperatures; and the substance may be withdrawn for examination whenever necessary, or products of decomposition may be sucked out from the tube.54. "The Retention of Lead Salts by Filter-paper." By L. Trant 0'Shea. The absorption effect of filter-paper on dilute solutions of metallic salts has not, so far as the author has been able to ascertain, been studied. His attention was drawn to the subject whilst estimating small quantities of lead in water acidulated with sulphuric acid: although the water was perfectly clear, there was a considerable excess of lead in the unfiltered water over that in the water filtered through a single fluted filter-paper. To test the generality of the phenomenon, various kinds of filter-paper were used. In all the experiments a solution of lead acetate containing 6 mgrm.lead per litre (0.42 grain per gal.) was used, and in each case 50 C.C. (= 0.3 mgrm. Pb) was passed through the filter- paper folded in the ordinary conical form. Mgrm. Pb in 50 C.C. sol. after filtering through Pilter-paper. One filter-paper, Two filter-paper a,7 cm. diam. 7 C.C. diam. Schleicher u. Schiill ............ 0-18 0 '13 0.06 0.05 English ...................... 0 -10 0-09 0-03 0.05 French, white.. ................ 0.11 0'11 0'05 0.04), grep .................. 0 -15 0 -17 0.06 0.03 German thin (595) ............ 0 -17 0.15 0.02 0'02.. thick (597) ............ 0 -15 0'10 0.00 -)) thickest ............... 0-15 0-13 0.04 0'06 Though illustrating the phenomenon, these results are not strictly comparable, since the filter-paper was not kept constantly full ; consequently larger filter-papers were used which when folded would hold 50 C.C.and the time of filtration was noted. English Fi1ter-paper. Time in min.. .......... 1.5 1.7 2.25 2.5 2.75 3 Mgrm. Pb in 50 C.C. filtered solution ............. 0.2 0.23 0.17 0.15 0.11 0.0s Fq*enck,white. Time in min. .................. 3 4 4.2 7 Mgrm. Pb in ti0 C.C. filtered sol.. . 0.22 0.19 0.09 0.05 207 Fwnch, grey. Time in min. .................. 3 3 3.5 7 Mgrm. Pb int50 C.G. filtered sol.. . 0.14 0.18 0.1 0.07 Washing the filter-paper with water after filtration does not effect the removal of the absorbed salt.A Schleicher and Schiill filter- paper, No. 589, absorbsd during one filtration of 50 C.C. of solution a quantity of salt equivalent to 0.12 mgrm. lead ; it then was washed twice with 50 C.C. water :-1st washing contained.. .... 0.02 mgrm. Pb, 2nd 7, 7, ...... 0.00 ,, On filtering the same solution twice through the same filter-paper, a quantity of salt equivalent to 0.24 mgrm. Pb was absorbed, and on treating with 50 C.C. water nothing was washed out. Not only does the absorption take place during filtration, but also when the paper is immersed in the lead solution although at a much slower rate ; the amounts of lead remaining after immersing a paper 7 cm. in diameter in 50 C.C. solution (= 0.3 mgrm. Pb) were as follows :-1 1Time in hours.......... 1. 2. 5. 14. I English.. ...................... 0.03 0*23 0'23 0.05 French, white .................. 0.25 0'12 0 -05 0.00.. grey.. .................. 0 -27 0.17 0'15 0 *04 German, thin (595).. ............ 0-25 0-18 0'19 0'03.. thick (597) ............ 0-25 0.24 0.19 0'00.. thickest ............... 0-25 0.20 0.18 0'00 ADDITIONS TO THE LIBRARY. I. Donations. A Manual of Jurisprudence : by A. S. Taylor. Eleventh edition. Edited by T. Stevenson : London, 1886 : from the Editor. A Practical Essay on the Analysis of Minerals : by F. Accum : London, 1804 : from R. R. Steele, Esq. Chemical Amusement, comprising a series of curious and instructive Experiments in Chemistry : by F. Accnm : London, 1817 : by R. R. Steele, Esq.Pamphlets : Experiments on Ensilage, conducted at Rothamsted : Season 1884-5: by J.B. Lawes and J. H. Gilbert: London, 1886. 208 On the Valuation of Unexhausted Manures : by J. B. Lawes and J. H. Gilbert: London, 1886. Report of Experiments on the Growth of Wheat for the second period of twenty years in succession on the same ground: by J. B, Lawes and J. H. Gilbert : London, 1885. On Agricultural Investigation : a Lecture delivered October 27, 1884, at Rutzer’s College, New Brunswick, N.J. : by J. H. Gilbert: 1885. Note on some Conditions of the Development and the Activity of Chlorophyll: by J. H. Gilbert : London, 1885 : from the Authors, The Hell-Gate Explosion near New York, and so-called ‘‘ Racka-rock,” with a few words on so-called (( Panclastite :” by H.Sprengel : London, 1886 : from the Author, New Experiments on Electricity : by A. Bennet: Derby, 1879. from J. M. Stocks, Esq. Practical Blowpipe Assaying : by G. Attwood : London, 1880. from the Author. The Sale of Food and Drugs Acts, 1875 and 1879: with Notes and Cases : by W. J. Bell : London, 1886. from the Author. Elements of Chemistry in a, New Systematic Order : by Lavoisier : translated by R. Kerr : fifth edition : Edinburgh, 1802. 11. By Parchase. Elements of Chemical Physics : by J. P. Cooke, junr. : London, 1886. Trait6 Qlhmentaire de Chsmie, fondke sur les principes de la Thermochemie : par A. Ditte : Paris, 1884. RESEARCH FUND. A meeting of the Research Fund Committee will be held in June. Fellows desiring grants are requested to make application before June 10th. At the next meeting, on June 3rd, the following papers will be read :-‘‘ The Effect of Remelting on the Properties of Iron. Notes on Sir Wm. Fairbairn’s 1853 Experiments.” By Thomas Turner. “ Some Ammonium compounds and other derivatives of (al’)Hy-droxyquinoline.” By C. A. Kohn, B.Sc., Ph.D. HARRISON AND SONS, PRINTERSIN ORDINARY TO HER MAJESTY, ST. MARTIE’S LANK.
ISSN:0369-8718
DOI:10.1039/PL8860200197
出版商:RSC
年代:1886
数据来源: RSC
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