|
1. |
Proceedings of the Chemical Society, Vol. 12, No. 159 |
|
Proceedings of the Chemical Society, London,
Volume 12,
Issue 159,
1896,
Page 1-24
Preview
|
PDF (1497KB)
|
|
摘要:
lssiied 3/2/l896. PROCEEDINGS OP TEE CHEMICAL SOCIETY. EDITED BY THE SECRETARIEX. January 16th, 1896. MY.A. G. Vernon Harcourt, President, in the chair. Messrs. A. J. Chapman, H. W. Dickinson, G. Goldfinch, E Grossma,n, and A. F. Theodosius mere formally admitted Fellows of t11e Society. Certificates were read for the first time in favour of Messrs. William Henry Bentley, B.Sc., 116, Yarburgh Street, Moss Side, Mancheater ; Joseph John Bowley, 34, Elm Park Road, Chelsea ; Daiiiel Bray, Broadmoor, Cinderford ; Hugh Charles Herbert Candy, B.A., B.Sc., 101, Gower Street, W.C.; Thomas Ewm, B.Sc., Ph.D., Yorkshire College, Leeds ; Charles James Pemeller Fuller, Mona House, Horwich, Lancs. ; William Harrington, 11, Edgehill, WhitehaTen ; Albert Howard, 17, Elthiron Road, Fulham, S.W.; Ernest Haynes Jeffers, 50, St. John’s Hill Grove, New Wandswortli. S.W. ; James Johnstone, Braehead, Pai-khill, Rutherglen ; Charles Edward Sage, 7, Oseney Crescent, N.W. OE the following papers those marked * were read :-“1. “The acetylene theory of luminosity.” By Vivian B. Lewes. The author points out that in 1882 Professors Dewar and Liveing (Proc. Boy. Soc., 34, 438) came to the conclusion that the “for-mation of acetylene in ordinary combustion seems to be the agent through which a very high local temperature is produced,” whilst Guequen (Trans. Socie‘f6 Techzique, 1884) claims to have put forward the acetylene theory of lumiiiosity in 1884. 2 The author considers that the critickm offered against the acetylene theory by Smithells (Trans., 1895,67,1049)in no way affects the considerations upon which the theory ie based, which are-1. That the unsaturated hydrocarbons in the inner regicii of the flame are largely converted into acetylene before luminosity com- mences.2. That acetylene develops luminosity when heated whilst flowing through a hard glass tube, no air being present). 3. That the temperature necessary to decompose acetylene with evolution of light does not raise to incandescence the carbon liberated by the decomposition. 4.That in luminous hydrocarbon flames of suficiently high tem-perature the luminosity varies directly with the amount of acetylene present at the point where luminosity commences. The objections raised by Smithells agaiost the determination of absolute temperatures in flames by means of the Le Chatelier thermo- couple are warmly endorsed by the author as far as those portions are concerned in which combustion is taking place, and these objec- tions were pointed out in his former paper (PYOC.Roy. Xoc., 57,452), but he contends that the results obtained in the inner non-luminous portion of a hSdrocarbon flame are probably fairly accurate, and the results obtained by Smithells fulIy confirm the statement that the temperature in the inner zone rises from a comparatively low tem-perature close to the burner to over 1000° at the apex of the zone.The author describes experiments showing that although the heat of combustion of acetylene is very high, so small a proportion has to be burnt in order to develop the remaining energy as light and radiant heat that it by no meana follows that the acetylene flame is hotter, or even as hot,, as a coal gas or ethylene flame of the same size.Smithells has come to the conclusion that the statement that cjsnogen could be made to undergo luminous combustion has arisen from a yellow ammonia flame having been mistaken for one contain- ing solid carbon ; the author shows that by surrounding the cganogen flame by nitric oxide, intense luminosity and a copious deposit of soot ca,n be obtained. The author contends that the flame is in reality divided into two zoces-1. The outer sheath of combustion, 2. The inner region of non-combustion, and that the latter consists of an internal portion in which radiant heat is converting the hjdrocarhous into acetylene : a luminous envelope which caps it, and in which more intense heat is decompos-ing the acetylene with emission of light, and the blue calyx at the bottom of the inner zone where the hydrocarbons are undergoing de- 3 composition by water vapour and carbon dioxide mithout previous separation of carbon.The author also contends that t,he incandescent carbon particles in the upper portion of the flame are acted upon by carbon dioxide and water vapour forming carbon monoxide and hydrogen, and that this action tends far more than combustion by the air to prevent their escape from the flame.DISCUSSION. Professor SMITHELLSsaid that he had always considered the acetylene theory ingenious, and feared indeed that its very attrac- tiveness had led Professor Lewes to a one-sided and, in many cases, an erroneous interpretation of evidence. The question was not whether the explaiiation of luniinosity afforded by the acetylene theory was conceivable, but whethcr the theory mas really in harmony with ascertained facts; and this question, he still thought, mas to be answered decidedly in the negative. As Professor Lewes had not read the whole paper, but had only drawn the attention of the meeting to certain points, he was unable to say to what extent Pro-fessor Lewes had dealt with the series of objections raised to the theory, 2nd his remarks must not, therefore, be regarded as pretending to be a complete reply.He wished that Professor Lewes would state explicitly what view he had as to the structure of an ordinary gas flame. Did lie, or did he not accept the old and generally accepted view, that the flame consisted of three distinct parts-a luminous region, a mantle, and a blue calyx at the base? Professor Idewes had attempted to define the parts of flame by reference to temperatures ; and wherms at one time he indicated the mantle as the region of lowest tem- perature, he now appeared to agree that it was the hottest part. Did he still maintain temperature measurements to be a reasonable basis for defining the anatomy of the flame ? He did not consider that' Professor Lewes had explained the extra- ordinary discrepancies that had been pointed out in his measuremefits of temperature ; and he should like to know whether Professor Lewes had used the thermo-couple, as shown in the apparatus before them, or whether he had not, as implied in his previous papers, inserted the twist of the thermo-couple in a manner now admitted to be improper.He still thought that it was misleading to speak of' 80 per cent. of the unsaturated hydrocarbons as being converted in to acetylene within the flame. If acetylene were the source of light, and if the light depended on the almost explosive character of its decomposi- tion, there surely was some reason to ask for evidence that a mixture of gases containing 1.4 per cent.of acetylene, 0.5 per cent. of other unsaturated hydrocarbons and 9s per cent. of other gases (four-fifths of which were incombustible) could afford light in the manner stated. He considered that such a doctrine was incredible. The evidence now adduced by ProEessor Lewes to show not. that, the acetylene flame was comparatively cool, but that, conceivitbIy it might be so if the fact were not otherwise, was very remarkable. He could not exactly s%y what was the mechanical equivalent of light, but his recollection was that it was extremely small, and he advised Professor Lewes to look into what was known on this subject before committing himself to the view that the acetylene flame lost so large a fractioii of its total energy in the form of light.However, this seemed to be it matter of lihtle consequence, for there was no getting over the fact that the acetylene flame was surrounded by a, mantle of extremely high temperature, and that a platinum wire introduced into it glowed at least as brightly as the carbon within the flame. That being the case, there was no occasion to exp!ain that, hypo- thetically, the flame might be cool. With regard to the cyanogen flame, be had nothing to withdraw from what he had said on a previous occasion, though he gladly con- gratulated Professor Lewes on having now made a new and interest- ing observation. He had entirely failed to obtain evidence of carbon being separated in a cyanogen flame surrounded by burning hydro- gen, and Professor Lewes had not shown that it was separated.The use of nitric oxide (which would in its luminous result remind them of the behaviour of that gas towards carbon disulphide) un-doubtedly led to the separatioii of carbon, and supplied a piece of evidence which Professor Lewes was now entitled to claim. Much circumstantial evidence, believed by Professor Lewes to favour the acetylene theory, had been adduced. Among it was a calculation which, having a striking practical aspect, might have considerable influence on some minds, and he desired to ask Professor Lewes to explain and justify it. It was intended to give the theoretical illuminating value of ethane, ethylene, and acetylene respectively, on the supposition that in giving light after passing through the state of acetylene they were resolved into carbon and hydrogen, and this calculation gave results in tolerable agreement with the illuminating value of the gases as determined by the photo- meter.The calculation was, he thought, unintelligible from a scien-tific point of view, but, even if the principle were admitted, seemed not, only incorrectly made, but capable of affording a set of numbers entirely at variance with practical measurements, just as easily as num-bers in harmony with them. He thought some explanation of this was due from Professor Lewes. He would only-, in conclusion, say again 5 that his remarks must not be taken at all as his complete answer to Professor Lewes, whose manner of presenting his paper had rendered this impossible.Professor R~~CKERthought that the use of a thermo-couple in a flame above the melting point of one of the metals was open to grave objection, on account of the uncertainty as to the temperature which the junction actually attained. The validity of Professor Lewes’ experiment on the thermal value of the luminous radiation depended on whether the whole of the non-luminous radiation had been absorbed in the comparison experiment. This in turn depended in part OLI the dimensions of the apparatus. By the solution of a small quantity of an iron salt the absorptive power of the water would have been increased, while the light would not have been very largely diminished. Professor THORPEremarked that a possible fallacy might underlie the deductions as to temperature drawn from the hehaviour of a platinum wire in a flame containing free carbon and carbonic oxide, on account of the specific chemical action which those substances might exeyt on the metal.The fact that a platinum wire would melt even in an ordinary candle flame, which is not particularly hot, was known to Smithson Tennant, and is referred to by Davy in his well- known paper. Davy also found that a filament of platinum could be fused by a flame of cpnogen in air, whereas the same wire was not melted by a hydrogen flame. Mr. GROVESdrew attention to Professor Lewes’ statement that the yellow light emitted by a jet of cyanogen when surrounded by a hydrogen flame was due to carbon liberated by the decomposition of the cyanogen, and suggested that if the image of the sun were thrown on to this flame by means of a lens, and the reflected light examined by methods familiar to physicists, it would be easy to ascertain whether the flame contained solid particles.In that asp, not only would the light be found to be polarised, but,, if examined spectroscopically, would exhibit the k’raunhofer lines. If the flame contained no solid particles, then the luminosity could not be due to liberated carbon ; on the other hand, even if it were found to con- tain solid particles, it would not necessarily follow that these were carbon. The PRESIDENTr&rred to a suggestion of Professor Lewes that the great output of light from the acetylene flame inay leave the flame itself comparatively cool.He thought that of the energy made kinetic by chemical changes within the flame only a small part radiated out in waves of such a length as to be light. The small carbon particles in the flame lost much heat by radiation, and would thus be cooler than the non-radiating gases in which they floated. It was agreed that the outside of a flame was the hottest part. One of the causes of the splendour of the flame of pure acetylene wap, no doubt, the high temperature to which the separa- tion, as well as the oxidation, of the carbon and hydrogen contributed ; but a suitable burner was necessary: the flame must have a large outer surface, and close within this must be spread over the whole frontier, the little particles of carbon which glow for an instant and disappear.Among the causes which make the flame oE one gas brighter than that of another might be a difference in the size and numbcr of these solid particles. As one salt gave a large-grained and another a sma'l-grained precipitate, so it might be with decomposing hydro- cirbons; and as a given quantity of platinum wire coiled into a spiral and held in a Bunsen flamr: mould give more light the smaller the gauge, SO the finer dust of carbon might make the brighter flame. Some ides of the proportion between the surface of the flame and the actual surface of the glowing particles to which its light is due might be gained from a comparison with the filament of an electric glow-lamp.The radiating substance was similar in the two cases, and when the filament and current were such that the glow-lamp gave light of the same amount and colour as the gas-flnme, it was likely that the glowing surfacea had a similar area. Professor LEW-ES,in reply, said that he extremely regretted not having read his paper i12 eztenso, as it contained answers to most of the objections advanced by Professor Smithells. His views as to the structure of an ordinary gns flame were that it caatained four parts, but that three of these, namely, the non-]uzr,inous inner zone, the luminous sheath, and the blue caIyx wcre portions of the region in which no combustion, in the ordinayy acceptance of the term, took place; whilst the outer mantle of tlie flame was the region of intense combustion, and is undoubtedly the hottest part of the flame.In a paper read in 1892, he had given a description of the structure of a gas flame, buh, in criticising this, Pl-ofessor Smithells had evidently overlooked the fact that the portion of the paper following the description was devoted to an investigatioii as to the causes which led to the non-luminosity of hydrocarbon flames, which showed that the outer envelopc mwt be the hottest portion of the flame, but it is also manifest that the outer side of this mantle must be rapidly cooled by admixture with air and products of combustion, so that the maximum temperature will be near the inner side of this region, and it was the extreme outer portion of this zone which he had described in the words criticised by Professor Smi t hells.7 He thoroughly agreed in condemning any temperature measure-ments cf those portions of the flame in which active combustion was going on, but still believed in the measurements obtained in the area of non-combustion. Professor Smithells had pointed out that serious discrepancies existed between the temperatures recorded in a flat flame in the 1892 paper and in the 1895 paper, but as the one was from a No. 6 Bray, whilst the other was given by a 0000 Bray, it was difficult to understand 011 what grounds it could be expected that they would show any agreement, as the temperatures Val-ied for every alteration in the size of the burner, and for every variation in the pressure at which the gas was burnt.Oue of Professor Smithells’ strongest points mas that it was mis- leading to speak of 80 per cent. of the unsaturated hydrocarbons being converted into acetylene within the flame-the statement he had made was that 80 per cent. of the unsaturated hydrocarbons at the point just before luminosity commenced consisted of acetylene. If a mixture of 1.5 per cent. of acetylene and any gas which had a non-luminous fianie was burnt, no luminosity would be generated, and no trace of acetylene would be detected at; the top of the inner zone, it having been consumed before the temperature necessary for its decomposition wa3 reached ; but if 1.5 per cent. of acet,ylene was led into the top of the inner zone of a flame of coal gas, from which the unsaturated hydrocarbons bad been absorbed, then this addition would make the flame as luminous as if the unsaturated hydrocarbons had not been withdrawn, and be thought that Professor Smithells’ doubt as to the truth of the acetylene theory was based largely on a misconception of this point. As regards the experiment8 to show that a flame radiates a con- siderable amount of energy when emitting light, he was perfectly in accord with those who pointed out that the amount of energy COII-verted into light was but small; there was also a large amount, of heat radiated, and the experiment with the blackened bulb would give the total radiation cut off by the opaque coating, which when the flame was radiating freely would be lost to the flame. It would be preposterous to lay any great stress on this experiment, as the products of combustion were practically escaping uncooled.He had made in a former paper a calculation to show that a ratio existed between the heat of formation of a hydrocarbon and its illu-minating value, but he had been careful to point out that in our present absence of knowledge as to the heat relations existing at high temperatures, any such calculations were valueless except as showing that the greater the endothermic value of a compound the higher was its illuminating value. Professor Smithells concludes that because a platinum wire held in 8 the onter shield of a flame glows with the same incandescence as the carbon particles in the flame itself, therefore there is no need to assume any other source of heat than that given by the combustion going on in the flame walls.He thought that this conclusion was based upon at least two fallacies. In the first place Professor Smithells had himself clearly pointed out that there is a temperature gradient on the horizontal plane in which there is an abrupt rise in temperature from the lumi- nous sheath to the point of maximum combustion in the external envelope, and it therefore follows that the platinum wire held iu the external envelope must be heated to a higher temperature than tlie carbon particles in the 1uminous sheath. Secondly, the conclusion is based upon the assumptioii that the emissive power for light of carbon and platinum is the same, which is highly improbable.It has been shown that metals at high temperatures reflect light, and he thought it quite possible that some of the apparent brightness of the platinum wire might be due to light reflected from the Inminous veil in front of which the wire was placed. 2. “The action of sodium alcoholate on certain aromatic amides,” By J. B. Cohen, Ph.D., and W. H.Archdeacon, B.Sc. If acetanilide is dissolved in ether, and sodium methylate added, a crystalline addition compound of the formula Ph*NH*Ac,CH,-ONa is formed. Similar compounds with sodium methylate and ethylate have been prepared from ortho- and para-acetoluide, a-and /?-acetnaph thalide, henzanilide, and formanilide.With f orrnylphenylhydrazide, disodium formylpheiiylhydrazi.de is obtained. Benzamide yields a sodium compound of indefinite com-position. With propionanilide and bntyranilide compounds similar to acet-anilide sodium alcoholate appear to be formed in solution, but they codd no: be isolated, Sodium alcoholate does not react with di- phenylacetaiiiide and ethylacetanilide. 3. Note on the electro!ytic conductivity of formanilide and thioform- anaide.” By Thomas Ewan,B.Sc., Ph.D. The majority of the amides are too little soluble in water to allow of measurements of electrolytic conductivity being made. Others, again, are decomposed by water too rapidly into acid and amine. The conductivity of formanilide shows that it possesses feebly acidic properties.In aqueous solution the sodium compound of formanilide is completely decomposed. In the case of thioformani-lide, the sodium compound appears to exist in aqueous solution. 4. "The action of sugar on ammoniacal silver nitrate." By J. Henderson, B.Sc. The author has investigated the reducing powers of the €ollowiag substances on ammoniacal silver nitrate, viz., glucose, laevulose, galactose, cane-sugar, starch, dextrin, lactose, and maltose. The results obtained may be ths sumniarised :-(1) When glucose, hvulose, and galactose are heated with ani-moniacnl silver nitrate under the given conditions, a definite factor can be found in each case. (2) Cane-sugar, starch, and dextrin, when heated under the same conditions, exert no reducing action on ammoniacal silver nitrate.(3) In the case of lactose and maltose a definite factor cannot be obfained, owing to the gradual hydrolysis of the disaccharide by the ammonia. 5. LLSolution and diffusion of certain metals in ~iercury.~'By W. J. Humphreys. The author has examined quantitatively the solution and diffusion of tin, lead, bismuth, zinc, coppei*, and silver in mercury with a view to determining the extent to which these pheiioinenn differ, if at all, from the solution and diffusion of non-metallic solids in liquids. Pieces of metal were placed on the upper surface of a column of pure mercury, and samples of the liquid were taken at definite depths below the surface, and the amount of foreign metal estimated. As far as the experiments go, the author concludes that the solutionand diffusion of metals in mercury do not essentially differ from those of non-metallic solids in liquids.Copper and silver dissolve in mercury to a very small extent at ordinary temperatures, but diffuse very rapidly. 6. 'I On some of the ethereal salts of active and inactive monobenzoyl, dibenzoyl, diphenylacetyl, and dipropionyl-glyceric acids." ByPercy Frankland, Ph.D., F.R.S., and John MacGregor, M.A. The following compounds have been prepared by the authors :-Methyl dibenzoylglycerate (active). Long radiating needles me1 t-ing at 58-59'. [aIDat 183" = +8.55'; d 1S3O/-i0 = 1.0951. ,, 59.5' = +22.13"; d 59.5'/4" = 1.1877. ,, 15' (calculated) = +26*ScJ".Methyl dibenzoylglycerate (inactive). Long radiating needles melting at 44-46'. Ethyl dibenzoylglycerete (active). Radiating needles melting at 25". 10 [a]Dat 183' = 3-8.62"; d 183"/4" = 1.0599. ,, 16.5" (superfusion) = +26*28'; d 16.5'/4' = 1-1996. ,, 15" (calculated) = +26.58'. Propyldibenzoylglycerate (active). Liquid boiling at 26 7-269" under 11mm. pressure. [a], at 87" = +15*34'; d 873/40 = 1*1175, ,, 19.5' = +20w; a i9.50/40= 1.1771. ,, 15' (calculated) = +21.00". Methyl diphenylacetylglycerate (active). Liquid boiling at 266--270" under 17 mm. [a]=at 77.5" = -114.10" ; d 77.Eio/4" = 1.1427. ,, 14.5' = -16.06"; d 14.5"/4" = 1.1972. Methyl monobenzoylglycerate (active). A dextro-rotatory liquid which, on distillation, yielded a more dextro-rotatory distillate.It is probable that the original liquid consisted of the a-and p-isomeric monobenzoylglycerates, of which the a-compound would have the lower boiling point, and that this a-compound is more dextro-rotatory than tlie p-compound. Methyl monobenzoylglycerate (inactive). Crystnllises in small, worty groups melting at, 92.5-93'. It is probable that this is the /3-compound, the a-compound being liquid. Ethy1 monobenzoylglycerate (active). Radiating needles melting at 63". This is probably the p-compound ; it is laworotatory, whilst the liquid from which it crystallised, and which would contain the a-compound, was dextro-rotatory. This solid ethyl monobenzoylgly- cerate is remarkable for its almost complete insensitiveness to tem- perature, thus- at 136.5' = -9.47"; cl 136.5'/4' = 1.0886.,, 67" =: -9.80"; d 6i0/4" = 1.1547. Methyl dipropionylglycerate (active). Liquid. [a]=at 15' = -10.9'7"; d 15'/4" = 1.1349. The relationship between the rotatory power and the chemical constitution of these and other derivatives of glyceric acid is dis-cussed, attention being again directed to tho manner in which the rotation is more powerfully influenced by the qualitative character than by the mere mass of the groups attached to the asymmetric carbon atom. It is also pointed out that the reaction is more influ-enced by an element or group of elements introduced in the vicinity than by the same at a distance from the asymmetric carbon atom.11 7. “On the rotation of optically active compounds in organic solvents.” By Percy Frankland, Ph.D., F.R.S., and R. H. Pickard, B.Sc. The authors have investigated the variation in the value of [Z]D for methyl dibenzoylglycerate when dissolved in benzene, nitroben- zene, ethylene dibromide, and acetic acid respectively, employing a number of different concentrations in the case of each solvent. T’he molecular weight was also cryoscopically determined for a series of similar concentrations with each solvent. The cryoscopic determinations showed that inactive methyl diben- zoylglycerate does not exist as a “racemised” molecule in these solvents, practically the same values for t,he molecular weight baing obtained as with the active compound under the same conditions.The cryoscopic values were, with all the concentrations employed, below the theoretical ones in benzene; in ethylene dibromide and nitrobenzene they were below the theory with dilute, and above the theory with strong solutions. In the case of acetic acid, the cryoscopic- values were with all concentrat,ions sometimes above, and sometimes below, the theoretical value. The values of [z]D in the benzene solutions were much in excess, whilst in the nitrobenzene and ethylene dibromide solutions they mere much below the value for [aJDexhibited by the pure substance ; in acetic acid the values for [alDmost closely approximated to that of the pure substance. Low cryoscopic values for the molecular weight of methyl dibenzoylglycerate were accompanied by high ralues for [a;],, and ziice versci.This relationship between [a]Dand indicated molecular weight is borne out by the behaviour of ethyl diacet’ylglycerate in benzerie and acetic acid solutions respectively, only that in this case the low mole-cular weights and high specific rotations were obtained in acetic acid, the high molecular weights and low rotations in benzene solu-tion. The real value of [aIDfor an active body cannot be directly calcu- lated from the rotation of its solution, even when the cryoscopic examination of that solution shows the molecular weight to be normal, and even R moderately accurate estimate of the real value of [a]=can only be arrived at by the study of solutions giving normal molecular weights and extrapolating for infinite concentration on their rotstion curves.The explanation of these phenomena on the assumption of disso-ciation and association processes taking place in the several solutkms, as has been suggested by Preundler, is discussed. The dissocia- tion indicated by the low cryoscopic values obtained with methyl dibenzoylglycerate in benzene, and with ethjl diacetylglycerate 12 in acetic acid solution, appears to be in h,zrmony with the rotation phenomena only if the dissociation consists in the splitting off of the inethyl and ethyl g:*oups respectively, the active ion rataining in each case the acid radicles (benzoyl and acetgl). This conclusion is opposed to that arrived at by Preundler in the case of the diacidjl tartrates.8. “Note on the action of hydrogen chloride on ethyl alcohol.” By J. C. Cain, B.Sc., Ph.D. The author refera to tlie statement recently made by Dr. Armstroug, in his Presidential Address to the Society, that ‘(Perkin has estab- lished the incorrectness of tlie supposition that until recently has a1ways“been made, that hydrogen chloride, wheii dissolved in alcohol, acts fairly readily on it,” and points out that this supposition has been known to be incorrect for a considerable time. Berthelot, in 18S0, fonnd that no reaction takes place on making the solution, and Villiers found a reaction at 10--25° only after some months. The author examined the action of hydrogen chloride on ethyl alcohol in 1893, and found that hydrogen chloride had no action on ethyl alcohol after acting for 17 days at 0” C., or for 15 days at 15’ C.The reaction probably begins at 20-25’ C. A saturated solution of hydrogen chloride in alcohol contains 39.06 per cent. HCI, at 10°C. This is near the number found by Dr. W. H. Perkin, sen. (38.45per cent.). The temperature at which the experiment was made is not given, and was therefore probably higher than 10”C. 9. Transformation of the alkylammonium cyanates into the corre- sponding ureas.” By J. Walker and J. R. Appleyard. A comparison has been made of the rates of transformation of the alkylammoniurn cyanates into ureas, and of the reverse transforma- tion of the ureas into cyanates.In every case the results agree with the assumption that the cyanates are present in tbe aqueous solution in the form of two independent ions. In some instances the reverse transformation is well developed ;for example, equilibrium is reached in a 1/15 normal solution of tertiary amyl ammonium cyanate when half of the cyanate has been transformed into tertiary amyl urea, no production of the nren beyond that amount taking place. x70 defi-nite relation between the values of the constants and the nature and number of the replacing alkyl groups was observed. 10. ‘I On certain phenylthiocarbamates.” By H. Lloyd Snape, D.Sc., Ph.D. The author has examined the action of phenylthiocarbimide upon phenol, resorcinol, quinol, and glycol. A.E. Dixon (Trans,, 57, 13 268) had already shown that interaction takes place between the above-named thiocarbimide and phenol ; but his paper had been overlooked by the writer, who claims, in the course of the experi-ments he independently carried out, to have obtained the phenyl salt of pheriylthiocarbamic acid in purer coiidition and in larger quantity. He found, in opposition to Dixon's experience, that the higher the temperature (below 280") and the longer the duration of the experiment, the better was the yield, and in one experiment found this to amount to 25 per cent. of the theoretical, whereas Dixon, working at lower temperatures and for a shorter time, only obtained 7 per cent. By crystallisation from absolute alcohol, the crystals obtained melted sharply at 148" (149-151°, Dixon).So much difficulty having been experienced in effecting combina- tion between phenylthiocarbimide aud phenol, it was to be antici- pated that reaction between the former substance and dihydroxy- compounds would be even more diEcult to carry out ; and no thio-carbamate could be obtained from resorcinol, quinol, or glycol. The \niter, however, succeeded in obtaining, by the action of phenyl cynnate upon dithioresorcinol and dithioquiuol respectively, the iso- merides of the tliiocarbamates he had hoped to prepare by the fore- going method. m-Phenyleize Salt of Pl~enyleiiethiocal-7,amicacid.-Phenylcyanate and dithioresorcinol, in the theoretical proportions, were heated in a bath containing a solution of common salt for half an hour.Crystals rapidly separated. After washing with cold alcohol and recr~stallisa- tion from glacial acetic acid, large white needles were obtained melting at 178-179". The reaction is expressed thus C,Hi*(SH), + 2CCHjNCO = C,H*(S.CO*NH*C,H,),. p-Phenylene Salt of Pheizyleiiethiocarbanzic acid.-Phenylcyanate and dithioquinol was heated in a water bath. Again combination readily occurred. The crystals obtained by recrystallisation from glacial acetic acid were smaller than in the preceding case, and melted at 200-2@2°. 11. "The availabIe potash in soils." By T. B. Wood, M.A. The author has had under his care a number of experimental plots in Norfolk and Suffolk, and in this paper he tests the practicability ofDr.Bernard Dyer's method of estimating available potash in soils (Trans., 1894, 115-167), by comparing the analytical numbers obtained by Dr. Dyer's method with the results obtained in actual field experiment. The soils experimented upon may be divided into two classes, viz., (I) those rich in available potash and (11)those pool9 in this sub- 14 stancc.. The former soils gave no marked crop increase (barley) when treated with pot,ash manures, the latter gave a very large increase. The former soils gave by Dr. Dyer’s method on an average 0.0147 per cent. of available potash (sol. in 1 per cent. citric acid). the latter only 0.0073 per cent., whereas the potash soluble in strong hydrochloric acid (0.178 and 0.137) was much more nearly equal in each case.The author concludes that Dr. Dyer’s method is likely to be of technical value to the agriculturist; since, in the cases examined, laboratory experiments lead to the same conclusions as the more tedious and expensive field experiments. The modification of the method mentioned at the end of Dr. Dyer’s paper for use in the case of soils containing much chalk gives far less satisfactory result;; tlian t>he unmodified analytical process. ADDITIONS TO THE LIBRARY. I. Donations. Thorpe, T. E. A Manual of Inorganic Chemistry. Vol. I. The Non-metals. 511 pp. with 126 illustrations. Vol. XI. The Metals. 430 pp. with 183 illustrations. London 1896. 81-0. Prom the Author. Thorpe, T. E. Quantitative Chemical Analysis.Tenth Editlion. xiv + 389 pp. with 88 illustrations. London 1893. 8vo. (Text-books of Science.) From the Author. Sadtler, S. P. A Handbook of Industrial Organic Chemistry adapted for the use of Manufacturers, Chemists, and all interested in the ntilisation of Organic Materials in the Industrial Arts. Second re- vised and enlarged edition. xvi + 537 pp. with 127 illustrations. Philadelphia 1895. 8vo. From the Publishers. Guttman, Oscar. The Manufacture of Explosives : a theoretical and practical treatise on the History, the Physical and Chemical Properties, and the Manufacture of Explosives. Vol. I. viii + 348 pp. with 147 illustrations. Vol. 11. xiv+444 pp. with 181 illustra-tions. London 1895. 8vo. From the Author. Pharmaceuiical Society.The Calendar of the Pharmaceutical Societ’yof Great Britain, 1896. 507 pp. London 1896. Svo. From the Society, Lmdauer, John. Die Spectralanalyse: mit 44! in den Text ein- gedruckten Holzstichen nnd einer Spectraltafel. viii + 174 pp. Braunschweig 1896. 8vo. From the Publishers. 15 Roscoe, H. E., and Harden, Arthur. A new view of the Origin of Dalton’s Atomic Theory : a contribution to Chemical History ; together with lett’ers and documentas concerning the Life and Labours of John Dalton, now for the first time published from MS. in the possession of the Literary and Philosophical Society of Manchester. x+192 pp. with portrait. London 1896. 8vo. From the Authors. 11. By Puychase. MBmorial des Pondres et Saltphes.Publie par les soins du Service des Poudres et Saltp6tres avec l’approbation du Ministre de la, Guerre. Tome VII. 233+154pp. Paris 1894. Svo. Bobinson, H. If,,and Cribb, C. H. The Law and Chemistry of pp.Food and Thugs. ~~$499 London 1895. 8vo. Pamphlets. The Discovery of Oxygen, and its immediate results, including the overthrow of the Phlogiston Theory. A concise account of the labours of Priestley, Scheele, Cayendish, and Lavoisier. 60 pp. London 1895. Svo. From the Author. Seaman, TV. H. On the relations of Cheniistry to Education. Address of the retiring President before the Chemical Society of Washington, February 14, 1895. 45-63 pp. with a folding sheet. Washington 1895. 8vo. (Reprint from Eull. No. 9 of the Chemical Society of Washington.) From the Author.Maiden, J. H., and Smith, H. G. Preliminary Notes on the Bark of Cahsa ozrata, R. Br. Far. Stolonifern, Bail. (Reprint from Proc. Australian Association. Brisbane 1895.) From the Author. At the next meeting, on Thursday, February 6th, the following papers will be read :-“ The molecular weight and formuIa of phosphoric anhydride and of metaphosphoric acid.” By Professor Tilden, F.R S., and R. E. B arne tt. “ Lead tptracetate and the plumbic salts.’’ By Dr. A. Hutchinson and W. Pollnrd. “ An improved method of determining urea by the hypobromite process.’’ By Alfred H. Allen. CERTIFICATES OF CANDIDATES FOR ELECTION AT THE NEXT BALLOT, N.B.-The names of those who sign from " General Knowledge '' are printed in itulics.The following Candidates will be balloted for on Thursday, February 20, 1896 :-Allan, John, 242, Moss Lane East, Manchester. Analytical Chemist and Science Teacher. Seven years' experi- ence in laboratory of Public Analyst. Six years Chemist in sugar refinery. Six years Teacher and Lecturer in Practical and Theo- rhea1 Ghemistry. John Wm. Biggart. Angus Smith, F.I.C. A. Hxmboldt Sexton. Jas. Grant. T.L. Pattemon. a. G. Hendemm. Barker, William Henry, 26, Belgrave Road, Longton, Staffs. Lecturer in Chemistry, Technical Inslruction, Endowed School, Longton, Staffs. B.Sc. London. Fourth in Honours Chemistry. Formerly Student at University College, Aberystwyth, and Oweas, Manchester. Lecturer in Chemistry, Longton, Staffs.H. B. Dixon. W. H. Perkin, jun. Arthur Harden. P. J. Hartog. Bevan Lean. William A. Bone. Bentley, William Henry, 110,Yarburgh Street, Moss Side, Manchestel*. Fellow of the Victoria University. Three years as Student in the Chemistry Department of Owens College. First Class Honours in Chemistry. B.Sc. Victoria. University Scholar and Dalton Scholar. Author of (1)"~~-Methy1ethylpropionicAcid " (J.Chem. Xoc., 1895) ; (2) ''Methylisobutylacetic Acid " (J. Chem. Xoc., 1895). Harold B. Dixon. W. H. Perkin, jun. J. P. Thorpe. G. H. Bailey. A. Harden. Win. A. Bone. E. Haworth. 17 Blood, Maurice, 15, Clyde Road, Bristol. Has taught am4 lectured in Chemistry and Mat>hematica during four terms at Northampton and County Modern and Technical School.Recently appointed to teach Chemistry and Physics at Kingston Endowed Schools. B.A. Oxford. Open Scholarship at Merton College, Oxford. During five years’ residence obtained :-Second Class iii Honour Mathematical Moderations. Second Class in Alnthem%tics arid Yhj-sics, Final Honour School. Second Clabs in Chemistry, Final Honour Scl~ool. R!. Elliot Sttiel. J. A. Gnrdner. W. W. Pisliw. J. E. Marsh. H. 0. Halc. Blyde, Joseph Edwin Alger, Net’her House, Ranmoor, Sheffield, Steel Maker and Tester in the firm of Blyde, Ledingham and Cornpauy, tho Wn1l:ice Steel Works, Sheffield, and Senior Partner in above firm, Makcr of crucible steel and Member of Shefield llctdliirgical Snciet’y and Science Section of the Literary and Philw sophical Society, I;.Arc11 butt.Alfkd H, Allen, (3, 1’.W. Newslioline, 1C’m T.l.il?d. m.’iLEiitnh Id, Oates. Bowley, Joseph John, 34. Elm Pork Road, Chelsea. Varnish and Colc;ur bfmufacturer, Wellington Work?, Battersea, lhuf ac+urer. Willm. Thorp, Eoverton Redwood, John Spiller. Thos. Tyrer. Frederic Jns. 31, Page. Napiw Sotton.El. D(“id HXC nrd* J. P. J’oriwy. Bowman, Herbert Lister, 13, SheHicld Gardens, Kcusiiigton: W, Student in the University Tlaboratories, Oxforrl. R.A. Oxon. Honours in the Final :C;clioolof Natural Science (Cheniistr~). ITT. W.Fishel., JTaH. Vcley. ;To1111 \VR it s , W i1I inin 0d1ing, n. u. N;Ig.el* T.CAPortel-, J, E, Xawii, 18 Bray, Daniel, Broadmoor, Cind erf ord, Glos.Manager and Chemist of the Broadmwr Chcmicczl Works, Cinder-fwd. Articled Pupil for three years to DY.Wm. Morgan, P.I.C.,late Public Analyst for County Borough of Swanwa, $c. For two nn'i three-quarter years Chemical Superin tendent of the Wet Process for extraotion of nickel and cobalt at H. H. Vivian and Co., Hafod Isha Works, Swnnsea. Now Manager of the Broadmoor Cliernical Works, Cinderford, Glos. Rhys P. Charles. Arthur Lutg. Sydney W. Harris. W. Terrill. E. Chant Hooper. R. Bnvmiskey. Wm. Ewrk;7tess. H. J. IItdm. Burbridge, fames Kerry, A.I.C., Moor's Len, Winchmore Hill, N. Works' Chemist. Studied at the Univemitg of Bonn for two Sessions, under Professors Kekul6, AnschutE, and Klinger.From 1890 to 1894 at King's College, London, in the hilnthc~mntical, Phybi- cal, and Chouiical Departments. Have passed t,hc Examjnation of' the Institute of Chemistq, July, 1895. Have been engaged in chemiw.1 work connected with the manufacture of india-rubber goods during 1895. John M. Thomsm. Herbert Jacbon. Patrick H. Kirkaldy. Chas. A. Fnwsitt. R. S. Yoiing. Duvid II@U'lZ7.d. Oandy, Hugh Charles Berbert, 101, Gower Street, London, W.C. Lecturer on Organic Chemistry at the London Hospital Medical School. Graduated B.A., Lond., 1883, and B.Sc., Lond,, 1888, Student of Chemistry in Dr. Frankland's laboratory at the Normal School of Science, South Kensington, October, 18131-3far~h, 3882, and of Chemistry and Physics, at University College, Loiidon, in 1883,and at intervals since.E. Frankland. Hy. Forster Morleg. Percy P,Frankland. W. Palmer Wynnc. Frederic Jas. 34. Page, Percy A.. E. Richards. nary College, GlaPgow, now Lecturer on Chemistry under Glasgow School Board, at Grove Street School. G. G. lieiidcrson. A. Rnniboldt Sext011. Percy P.3'i~nnkl;tiid. John E'eig iisoii. Id. B. Il%tlock. IIowtio Udluutyne. X712G. c. Stuc?Lfur17. Dixon, Frank, 73, King Edward Road, S. Hackney, N.E. Science Teacher. Royal College of Science, 1st Class Chem. Certificate, 1889. London University ; Inter. B.Sc., 1894. Have taught Chemistry since 1890, and am at present teaching Chem. and Physics at Lenian Street Foundatioii School. Percy F. Fi-an2land.Samuel Jackson. Lioriel 11.Joiies. Frederic Wm. Richardson. A. E. Tuttun. Eiloart, Arnold, 2, Lansdowne Road, East Croydon. Chemist;. Assistant in Chemist8ry, Royal College of Science, South Kensington, formerly Instructor in Chemistry, Cornell University. Author of A Guide to S!ereocheinistry, &c. Wiliiam A. Tilden. Johli &I. Thomson. Herbort Jackson. Chap man Jones. William Tate. Ewan, Thomas, The Yorksliire College, Leeds. Demonstrator of Chemistry. B.Sc. (Vict.), Ph.D. (Munich), De-monstrator of Chemistry at the k'ot~kshii~e College, formerly 1851 Exhibition Scholar at Owens College. Author of a number of papers on Organic and Physical Chemistry, published in the l'mnsactions of the Cfiernicnl Society, 1889 and 1892 ; PhiEosoplLical Jlagnzinc, 1892 and 1894 ; Proceedings of the Royal Suciety, 1895; Liebig's Annalen, 1895 ; Zeitschvift fiir Yl~ysilialische Cheinie, 1S94 and 1895 ; and elsewhere.Arthur Smithells. Harold €3. Dixon. W. H. Perkin, jun. P. J. Hartog. Herbert Ingle. Julius B. Cohen. G. 13. Bailey. Fuller, Charles James Pemeller, Mona House, ILorwich, Lancayhire. Analytical and Consultiiig Chemist. Have been engaged in An:JjticiLl Cheniist,i*y for tlie past 15 yeam, the last eight of \vliich I 20 hare been Cllief Chcmist at the Laiicashire an(l Yurksliire Ritiliyay Company’s Works at Horwich. Also Teacher of Inorganic Chemistry at the Horwich Technical School. Edwd. Riley. Jim. Ir. Whiteside. E. H. Saniter. B. Boutledye. J~Lo.T.Brierley. Grice, Walter Thomas, 9, Da1hous;e Square, Calcutta. Chemist to Messrs. Smith, Stainstreet,, and Co., Manufacturing and Analytical Chemists. I hare been enffaged during the last six years in the annljsis of raw materials, mineral products, and foods and drugs of this country, including :-Indigo, shellac, beeswax, cutcli, bone dust, nitre, gold, lead, copper and tin oreb, waters, milk, glue, butter, &c. Previous to this I was Assistant Chemist to Messrs. 1’. Harris, and Co., and afterwards in the laboratory of Mr. A. Robinson, F.C.S., in Birmingham. Kanny Loll Dey. Preo Loll Dey. F. H. AlcocB. H. J. Shorthouse. C’. J. €1. TKiden, 3I.D. Harrington, William, 11, Edgehi 1I , IV 11itehavm. Chemist. Analyst. For four years Assistant to A.Kitchin, F.I.C. Have been for two years Teacher of Chemistry for the County Council of Cumberland, under the Whiteliaven Teclinical Instruction Committee. , Archd. Kitchin. Robert Hellon. George Dixon. D. A. Sutherland. J. E. Rrockbank. Helps, James William, 3, Tai-istock Road, Croydon. Engineer and Manager to the Croydon Gas Company. Assoc. Mem. Inst. Civil Engineers. Studied Cheniistry 1871-75, nndw Ah. J. W. Gatehouse, City Analyst, Bath. Carried out all chemical work for the Gas Department of the Leeds Corporation, 1876-1880, and since then for the Wcston-~uper-Mai.e and Croydori Gas Com-panies, in my position as Engineer and Manager. When in Leeds I studied chemistry in Dr. Thorpe’s ereuiilg classes, at the Yorkshire College of Science.Have designed and erected works for the manu- facture of Sulphate of Ammonia, and 11ai.e contributed papers on Gus Purification and Aniline Colours to several Associations. Gerald T. Moody. Thomas G. Nicliolson. William J. Pope. H. Macan. Herwy E. Arwutrowg. 3’.Stadey Kippi7 by. Na1,lin 0. E’0st.r. 3:. Howard, Albert, 17, EltLiron Road, Fulham, S W. Student of Chemistry in the Rojal College of Science, London. First Class Honours in Chemistry at the Intermediate Science Exami-nation of London University, and at the May Examinations of tho Science and Art Departmeiit. At present taking the advanced coui*so in Chemistry in the Royal Collcge of Science, London. William A. Tilden. T. E. Thorpe.IT.Palmer Wynne. Cfiapnian Jones. A. E. Tutton. J. 1’.Hewit,t. J. W. Rodger. I’JLOS. P. Blunt. Jeffirs, Ernest Haynes, 50, St. John’s Hill Grove, New Wandsworth, S.W. Assistant Chemist at Messrs. Garton, Hill and Company’s Wadis, nnt,tersea. Two years at evening classes in Chemistry, atl People’s Palace. Two Sears in Laboratory of Messi-s. Gillriian and Spcnc.ti*. Otie and a half year’s student in Chemistry at Rojd Collqe of Science, South Kensington. Leonard Temple Thorne. TV. Palnicr Wj-line. William A. Tilden. J. W. Rodger. F. E.XatflLezcs. Johnstone, James, Braehead, Parkhill, Rut herglen. Cheiziist. Fellow of the Institute of Chemistry. Chemist to Messrs. John and James White, Maiiufacturitig Chemists, Shar.sficld, Rntliei-glen, for 12 years. Previously Stndent and Assistatit with Messrs.Wallace, Tntlock, and Clark, Public Analysts, Glasgow. W. J. Chiystal. Horntio rialInntync. John Clark. w. T. Cu1*phey. George Watson. Mathieson, Lzurence W., 104, Grove Road, BGW,E. Teacher and Demonstrator of Chemistry in the Peaple’s Palace Trchuical Schoo!~, E. Two semiofis Junior Demonstrator in Cliemistry to Professor Sexton, Glasgo N, and West of Scotland Technical College, Glasgotv. Two sessions Teacher of Chemistry in People’s Pdace Technical Schools, E. Honours (Practical nncl Theoretical) Science arid Art Depart>ment,1888and 18W Chemistrg, Part I, 1st Class, Royal College of Scicnce, London. J. Theo. Hewitt. T. E. Thorpe. A. Humboldt Sexton. P. Hope Gmd.lCldglry S.Bttl*yalt’t. Morrison, Joseph Edward, Montreal.; Clmnist. Chemist in clim.gc of Lalooratoiy of Messrs. Lyiiiaii, Soils and Go., Alaaufacturing Chemists. Editor Moitlr~aIYlmrmu-cczitirdl Jaumal. llntc Examiner in Chemistry for the Pliarmaceutical Associatioil of tlie Province of Quebec. Member Executive Board of the Montreal College of Pharmacy. Alfred By. Maso~1. Thomas Tyrer. Joseph P. Remington. Peter T.Azisten. J.E. Wai.nw?.ight. C. 3’.Chmdler. Robert L. Moizd. EOJ. Millard. Rostron, Harold, 70, Davenport Street, Bolton. Assistant Schoolmaster. Bachelor of Science (Victoria), Chemistry and Physics. For four years a student of the Owens College, Man-Chester ; in the Chemical (and Plipical) Laboratories three Sears.H. B. Dixon. W. H. Pcrkin, jun. P. J. Hartog. TNm. A. Bone. E. Haworth. G. H. Bailey. Gilbert J, Fowler. Rutter, Thomas Francis, The Huish School, Taunton. Science Teacher. Scholar and Medallist of UIiiversity Coll~g~, London, Bachelor of Science, London University. Science Master, the Huish School, Taunton. William Ramsay. Morris W. Travers. J. Norman Collie. R. T. Plimpton. H. R. Le Sueur. Sage, Charles Edward, 7, Oseney Crescent, N.W. Chemist in Manufacturing Laboratory. For 2; years Assistant Analyst, for If years Ch’ef Analyst, Works LiLbol~ato~y. Pupil aitd Assistant for five years to Mr. T. A. Ellwood, F.I.C. Passed major examination of Phnrniaceutical Society. Author of vnribus pnpers on technical and analytical chemistry appearing under my name in Yharmrrceut#.GalJoumal and other papers.T. A. Ellwood. Edward D. Gravill. E. F.Harrisoii. Hy. George E’. Stacey. G. Matthey. Joh S. Sclion. Salt, Arthur Philip, ‘‘ Sunn-jside,” Pinner Road, Harrow, Xiddlesex. Analytical Chemjst. For two years student, and Nedallist in Che-mistry (practical and theoretical) at the Polytechnic, London. Then for three years pupil, and now Assistant and Demonstrator to Professor J. Bajne, Annljticwl Chemist and Professor of Chemistry and Toxico- logy, Royal Veterinary College, Landon, N.W. Au Member of Society of Chemical Industry. James Bayne. Hubert E. Lindley. Percy A. E. Richards. Crestes V. Pisani. Chrcdes Illarch Caitios. Bernard Dyer. Scotland, Peter B., 30, Stirling Street,, Airdrie, N.S.Science l\lastcr, Secondary School, and Lecturer on Chemistry, Science tind Art School, Airdrie. Three years pupil assistant nnder Professop J R. Watson, ISLA., Anderson’s College, Glnsgom. Fou~ years as Demonstrator in Chemical Department, Coatbridge Tech-nical School and Mining College. Two summer sessions at Royal College of Science. First Class Houours in Chemistry, Scimce niici Art Department. Research on the k’errocynnides mid E’erricyanidea sensitive to light. W. Palmer Wjnne. WilIiam Tate. A. Humboldt Sex1on. William A. Tildelo. CI. CT. Hende~so~~ Simpson, Aitken Migget, 4,Kitto Road, St. Catherine’s Pai-k, S.E. Laboratory Chemist. Twelve years Chemist in Laboratory at MesSrs.Barrox, Harvey, arid Co., 6, Gi’lapur Street, E,C., manufacturing and- analytical work, Study : Two years School of Artsg Edinbfirgli ; certificates in Organic and Inorganic Chemistry ; six Sears E‘iusbury Technical Culleg:, Evening Classes ; certifiohe, Inorganic Chc-mistry. R. Meltlola. Arthur Roes. J. HARobbing. It. T. Marshall. R. @. T.Ecans. $ircar, Amrita Lal, E.M.S., Calcutta UniVersity, 61, Sanksrit01 a,, Ca1CII tta. Medicnl Pmctitionei-. Lecturer on Physics and CIieniist~y, Cal-cut ta Boys’ Scliool, College Depnrtirlcnt, 13trnoi’nry Assistant Secre-tory to the Indian AmociRtion for the Cultivation of Science. C. 3’. H. Warder), M.D. Tampu snuna Roy. Kanriy Loll Ik*j, I’IVO TI011 Dt.J. 1h I !I c;; ;W IG~D utta, 24 Smith, Henry George, Technological Museum, Sydney, New South Wales. Research Assistant, and in charge of the Mineralogical and Geolo-gical Collections of the Technological Museurn.Original papers bsfore the Royal Society of New South Wales on Chemical and Mineralogical Sabjects. Joint author with Mr. Maiden, the Super- intendent of three resoarches in th9 domain of Organic Chemistry. Assistant in t,h.: investig‘ation of very many products indigenous to the Colony, a4 Publislled in tho Proceedinqs of various Societius. J. I€. Maiden. A. Tivcrsidgc. William hl. Hamlet. 3A7:lzcnrdLL. Bewie. Johri C. H. Miw~ciye. Turner, Benjamin Bernard, 28, Lady Somerset Road, N.W. Teacher of Chemistry. Associate of City and Guilds of London InshitUte. Bachelor of Science, London University (1st cl;tss Hononrs, @l:ernisti*g).Teacher of Chemistry at tlic Dorough 1’01s-&ccIiiiic institute, 8.H. Hwry E:. ArmsCrong. W. Mnyho~cHd!cr, Gcruid T.Moody. 1101ln1d Ga.0ulptoll. b’. Sta8!iloyKipping. Approved by Coulj.uil undcr Bje-law I (:I). Kennicott, CassE., 4,050, Fllis Averiiic, Chicago, Ill., U.F.A. hna1gtic;tl Cl!emist, Dcpartmen t of Healt 11. Assistant D ircctor, M nil jcipnl lj‘iboratory, SiigteriritendeiiC Milk Inspectioii. Sccrctary, Section of C tieiizistry, Cliicttgo Acadciity of Scielices. A Member of the Anier.icxii Chemical Society. Anthor uf hperc~;on ‘‘ Dust Explo-sioiis,” “ C1;ern;stry Applied to hIoat Packing, &c,” Metlaoda of Water A~dysisand ALethocis of Milk Analysis, Reprt Chicago Departtneuf of Health, 1894. 11. H. lraclic r,stccn. Walter S. Hairiris.
ISSN:0369-8718
DOI:10.1039/PL8961200001
出版商:RSC
年代:1896
数据来源: RSC
|
|