|
1. |
Proceedings of the Chemical Society, Vol. 9, No. 125 |
|
Proceedings of the Chemical Society, London,
Volume 9,
Issue 125,
1893,
Page 141-160
Preview
|
PDF (1102KB)
|
|
摘要:
Issued 3/6/1893. PROCEEDINGS OF THE CHEMICAL SOCIETY. No. 125. Session 1893-94. May 18th, 1893. Dr. Armstrong, President, in the Chair. Mr. H. A. D. Jomett was formally admitted a Fellow of the Society. Certificates were read for the first time in favour of Messrs. S. W. M. Davy, Sharrow View, Sharrow, Sheffield; James John Howitt, Dunley, Toft Road, Knutsford ; John Walter Leather, 15, Bradgate Road, Catford, S.E.; K. P. McElroy, 1,412, Sixteenth Street, Washington, U.S.A. ; John Watson Napier, Minto House, Edinburgh ; Claude Theodore James Vautin, 10, Hanover Square, London ; Edward Augustus Warmington, 266, Castle Street, Dudley. Of the following papers those marked * were read :-“20. ‘‘Studies on the formation of ozone. 11.” By W. A. Shenstone and Martin Priest.The authors have submitted a known volume of oxygen confined in an ozone generator of the Brodie pattern to the influence of dis-charges produced by varying differences of potential, and hsve determined the amount of ozone produced by observing the change in volume by means of a mercury manometer. A full description is given of the contact breaker used, of the means adopted to measure the differences of potential, to prevent the ozone coming into contact with the mercury, &c.; in some of the experiments the discharge from an induction coil, in others that from an influence machine, mas used. The following conclusions are drawn :-1. It is possible to obtain very fairly concordant results. 2. Provided that the path of the discharge be not too short, at any 142 point in the generator, the maximum proportion of ozone that can be produced at a given temperature and pressure is nearly independent of the difference of potential employed, provided that this be between the limits of 33 and 69 C.G.S. (electrostatic) units.3. If the path of the discharge be very short at any point in the generator, the maximum proportion of ozone that can be obtained has an inverse relation to the differences of potential employed. 4. The rapidity with which oxygen is conrerted into ozone in a given ozone geuerator, and under given conditions of temperature and pressure, is greater when great than when small differences of potential are employed, or, in other words, a given percentage of ozone can be obtained moye quickly by employing a high difference of potential than by means of a lower one.5. The maximum proportion of ozone that is obtained in it given generator, at given temperature and pressure, is less when the number of discharges in unit of time is very great than when it is more moderate. 6. The highest proportions of ozone can be obtained (at given tem- perature and pressure, and if a given differeiice of potential be employed) by using a generator made of very thin glass and in which the inner tube fits into the outer tube rather closely, but such a generator acts very slowly if the mingling of its contents depend upon diffusion. 7. A greater proportion of oxygen can be converted into ozone in a given generator by means of a given difference of potential, the gas being maintained at a given temperature and pressure, by the action of an induction coil than by means of a "Wimshurst " or "Voss '' machine.The authors conclude from their results that the silent dis-charge acts by decomposing oxygen molecules into their atoms, which, subsequently re-combine to a greater or less cxtent (according to the temperature and pressure) to form the triatomic molecules of ozone; and that ozone is uot formed by the direct action of the discharge. DISCUSS~~N. Professor MCLEODreferred to the heating effect of tlie discharge, and asked wl~ether it had been noticed that a rise of temperatui-e took place in the inner vessel of the generator wliich might account for the decomposition.He drew attention to the possibility of producing ozone in considerable qua,ntity by subjecting oxygen under pressura to tlie influence of the discharge in a tube one end of which was at,a low temperature : unfortunately the tendency of ozone to explode when in the liquid condition appeared to be abarrier to the successful application of this method. Professor RAMSAYcommented on the fact that the authors had paid attention only to the influence of difference of potential, and had not taken into account what was probably of more importance, viz., the quantity of electricity in the discharge. Mi*.CROOBESconcurred in Professor Ramsay’s criticism, and mid that perhaps the difference observed in the case of the coil and influence machiue might be ascribable to this, as the coil would afford a larger quantity of electricity; and that a rapid discharge would also afford a smaller quantity of electricity than a slow one. Locally the temperature might be very high in such tubes.He then referred to the difficulty he had frequently met with in causing a discharge to pass in “Tesla” tubes: a tube through which no discharge would pass during several minutes would suddenly become luminous, but only when charged dangerously near to the breaking point. Mr. G. N. HUNTLPasked whether MI*.Shenstone intended to study the effect of temperature on the yield of ozone ;as it was a sub- stance in the formation of which heat was absorbed, its stability should reach a maximum at a temperatare fixed by its physical constants, and either above or below this temperature the yield of ozone should fall off. In connection with this, the production of ozone at 1200-1300” C., observed by Troost and Hautefeuille, re- qui red confirmation.The PRESIDENTregretted that no electricians were present to dis- cnss the arrangements adopted by the authors. Professor J. .J Thomson, he knew, held the view tha.t the electric discharge in gases was of the natiire of chemical action. Personally he was not satisfied with the evidence adduced by Cundall and Shenstone that only oxygen was concerned in the production of ozone ; he was of opinion that it would eventually have to be admitted that the formation of ozone was the outcome of an electrolytic change, in which probably conducting moisture was concerned, somewhat as expressed by the symbols 0,OH2 03 H2Oc 02’OHz’O2 -0;&O.Mr. SHENSTOXE,in reply, said that the electricity does not flow directly from the induction coil, or machine, into the ozone geae- rator. It acts inductively; the ozone generator being a sort of condenser with a compound dielectric consisting of two layers of glass with a lajer of oxygen between them. The discharge inside the ozone generator depends on a surface electrification set up on thc glass. The “quantity ” of electricity which passes through thc oxygen in a given ozone geuerator at each discharge depeuds on the 144 difference of pste~~tialthus set up, and tbis in its turn depends on the difference of potential of the inducing charge at the two electrodes of the generator.Therefore when the difference of potential of the inducing charge is increased, the quantity of electricity which t,akes part in B discharge is increased, and aice versd, and we are in fact studying the effect of different “ quantities ” of electricity on the gas, and we know when we increase or decrease the quantity. With regard to the suggestion that the greater “quantity ” of the current of a coil may explain some of the phenomena, it would seem that this is not likely to influence the inductive effect of a charge at a given difference of potential. It would simply make it possible to bring up the charge to the desired difference of potential somewhat more quickly by means of a coil than by means of a machine. They had not observed any extra heating of the acid in the inner tube of the generator, but rather the contrary.Referring to Mr. Crookes’ remarks, he said that they had sometimes observed that the production of ozone did not set in until after some time, #21.“The relative strengths or ‘avidities ’ of some compounds of weak acid character.” By John Shields, D.Sc., Ph.D. The author has calculated the relative strengths of number of compounds of weak acid character from the rate at which salt solu-tions bydrolyse ethylic acetate (Phil.Mag. [5], 35,365). The comparison has been made in deci-normal solution, the “ dis-Rociation ratio ” being taken as the measure of relative strength or “avidity,” and in order to obtain a better idea of their relative strengths the compounds examined have been compared with some of the stronger acids taken from Ostwald’s tables.The results are contained in the following table, from which it will be seen that in deci-normal solution, hydrogen chloride, for example, is about 100,000 times stronger than phenol. Hydrogen chloride .............. 100 Trichloracetic acid .............. 68 Dichloracetic ................ 33 Monochloracetic acid ............ 4 *3 Acetic ................ 0.35 Biboric ................ 0.0057 Hydrogen cyanide.. .............. 0 -0026 Phenol ........................ 0.00094 Carbonic acid.................... 0 -00091 145 +22. “The boiling points of homologous compounds. Part 1.Simpleand mixed ethers.” By James Walker, Ph.D.,D.Sc. The author finds that the boiling points of many homologous series may be expressed by means of the relation T = aMb, where T is the boiling point on the absolute scale, M the molecular weight, and a and b constants which have values peculiar to each series. He applies the formula to the ethers prepared and investigated by Dobriner (Annulen, 243, 1)and Pinette (Annulen, 243, 33). The difference. between the calculated and observed values is generally considerably less than a degree. The following rule is a deductioii from the formula :-The logarithm of the ratio of the absolute boiling points of any two members of a homologous series, divided by the logarithm of the ratio of their molecular weights, is constant.23. “The conditions determinative of chemical change.” By HenryE. Armstrong. Notwithstanding the large amount of evidence now placed on record that substances commonly supposed to be capable of directly interacting do so only in the presence of at least one other substance, chemists do not appear to have arrived at any clear and consistent understanding of the conditions determinative of chemical change : as each fresh case is recorded, we continue to express surprise, over- looking the fact that Faraday, in his early “ Experimental Researches in Electricity,” cleai-ly foresaw what the conditions were, and that but a slight extension of his generalisations is needed to frame a comprehensive theory.The subject is of such importance that it appears to me desirable to discuss the bearing of recent observations, especially as they to some extent necessitate the modification of views that I have expressed elsewhere, and in order to attract the attention of physicists, fo whom we must now Iook for guidanee in these matters, Eight years ago, in the course of the discussion on Mlr. H. B. Baker’s communication on (‘Combustion in dried gases ” (these Proceedings, 1885,40), I defined chemical action as reversed electro- lysis .-in ot’her words, in order that chemical action may take place, it is essential that the system operated on comprise an electrolyte. then pointed out that as neither hydrogen nor oxygen was an electro-lyte, a mixture of only these two gases should not be explosive ; and, moreover, that as water was not an electrolyte, and it was scarcely proba.ble that water and oxygen or hydrogen would form an electro- lyte, it was difficult to understand how the presence of water pure and simple should be of influence in the case of it mixture of hydrogen and oxygen.This forecast has since been verified, the remarkable series of experiments carried out by V. Meyer in conjunction with Kranse and Askenasy having clearly denionstrated that the forma- tion of water from hydrogen and oxygen takes place at an irregular rate, and is, therefore, dcpendent on the presence of a something ofher than water-I imagine an acid impurity.But this is a con-sideration which has not yet received the proper attention, and it is, therefore, desirable to emphasise its importance by reference to other cases. Mr. Baker’s recent preliminary note on the influence of moisture in promoting chemical action (ante, p. 229) affords several interesting examples :-Thus, he states that neither does hydrogen chloride combine with ammonia nor is nitric oxide oxidised by oxygen if moisture be excluded. In the former case, the addition of water should suf3ce to determine the combination, as water and hydrogen chloride together form a “composite electrolyte ” (cf. Roy. 8oc. Proc., 1886, No. 243, p. 268) ; as neit.her nitric oxide nor oxygen, however, forms a composite electrolyte with wat er, in this case water alone should not determine the occurrence of change ; but if by the introduction of a trace of “impurity ” in addition to water the pre- sence of a composite electrolyte were secured (however high its resist-ance, owing to the smallness of the amount of “impurity ”), act.ion would set in, and when once commenced wdd proceed at an increrts- ing rate, as nit.ric acid would be formed and the resistance of the electrolyte would consequently diminish.011 this account it will be a task of exceeding diflicul ty to experimentally demonstrate that nitric oxide and oxygen are inactive in presence of water alone ; but there can be no doubt that such must eventually be admitted to be the case, provided always that it is permissible to extrapolate Kohlrausch’s observations and to conclude from them that pttre water is a dielectric.The gradual increase in the rate of change here contemplated corresponds to the period of induction observed by Bunsen and Roscoe in their observations on the interaction of chlorine and hydrogen ; the statement recently made by Bodenstein and V. Meyer (Berichte, 1893, 1146) that a mixture of chlorine and hydrogen behaves irregularly on exposure to light is a valuable con- firmation of Pringsheim’s observations, and there is now no room for doubt that pure chlorine and hydrogen would be incapable of interacting. That no such irregnlarity is ohserved on heating iodine with hydrogen is not surprising, as hydrogen iodide would be formed from the very outset and the electrolyte present would exert n minimum. resistance almost at once.There is, however, a significant difference in the behaviour of the two mixtures, as hydrogen ch1oi.- ide should behave as hydrogen iodide, so that the problem is but, incompletely solved: it may be that t,he one mixture was more nearly 147 pare than the other, or it may be that the formntion cf hydrogen chloride from hydrogen and chlorine, under the influence of light, is dependent on the presence of some part’icular substance, together with water, and does not take place under the influence of any sub- stance capable of forming a composite electrolyte with water ; prob-ably, however, the difference observed is chiefly due to the fact that only one of the actions is reversible under the conditions prevailing in the experiments.Lastly, attention may be directed to the formation of sulphuric oxide from sulphurous oxide and oxygen, which is readily effected in presence of a catalyst, such as finely divided platinum; it cannot be supposed that the mere presence of platinum would condition the occurrence of change, and doubtleas moisture is also necessary, the platinum or other catalyst but serving to promote the oxidation of the sulphurous oxide at a temperature considerably below that at which snlphuric oxide decomposes when heated. The action of surfaces generally may me11 be of this character, and the converse influence they so frequently exercise is probably an effect of the same order.I have elsewhere raised the question whether there may not be a difference between actions taking place under the influence of low and. of high electromotive forces-whether water, per se, may not be an electrolyte towards high, although not towards low, forces in the, case of high temperature changes, or those brought about under the influence of the electric spark, for example. Mnore attentive con-sideration of the subject has led me to think that this is not the case, and that we must treat high temperature changes such as occur and are involved in gaseous explosious in the same way as those occur- ring under ordinary conditions and at low temperatures. From this point of view, Mr.Baker’s statement that ammonia and hydrogen chloride do not combine is of extreme importance ; the formation of ammonium chloride from these two compounds apparently involves no interchange, bnt a mere combination of two substances each endowed with considerable ‘‘residual affinity,” and there is no reason wliy a distinction should be drawn between such a case and that afforded by, say, atoms of hydrogen and oxygen, the difference being, it would seem, one of degree only: in fact, I am no longer inclined to believe that atoms are capable of directly uniting. In all cases at least one function of the (composite) electxolyte would appear to be that of providing the necessary “mechanism ” whereby the degradation or discharge of the energy is eEected.If this argument be sound, its logical extension involves the conclusion that pure gases should be dielectrics, ie., that the passage of an electric discharge through a gas like that of an explosive wave through, say, a mixture of hydro- 148 gen and oxygen, can only take place if an electrolyte be present. Hitherto but little attention has been paid to the electric discharge in gases which have been highly purified. The peculiar behaviour of Tesla tubes referred to by Mr. Crookes in the discussion on Mr. Shenstone’s paper on the formation of ozone is, perhaps, explicable from this point of view-it may be that the atmosphere within the tube does not become conducting until sufficient moisture and “impurity” have been projected from its sides.It is conceivable that a similar explanation may hold good in the case of Professor Schuster’s observation, that it is possible to urge a current of low electromotive force across a gas subjected to a high electromotive force in itself insufficient to cause a discharge in the gas ; the atomic dissociation hypothesis put forward in explanation of the phenomenon does not appear to me to be sufficient. Finally, the question arises, Can no line be drawn; are no two pure substances capable of combining or interacting :-For example, water and sulphuric anhydride? There is little to guide us here, but it seems not unlikely that water has special properties which enable it to act directly ; moreover-perhaps because-in such cases composite electrolytes would result.Ammonium chloride, so long as it remains solid, is clearly a compound of a different order, and it may well be that compounds of this type are in no case directly obtainable from their constituents, because, under the conditions under which they are formed, they cannot behave as electrolytes. Apparently, in all cases in which molecular aggregates are formed -as in the case of solutions-we are dealing with dissociable and dissociating systems, and it is not improbable that we may ultimately find an explanation of the mechanism of such changes in this fact. At present there is no information forthcoming whether simple electrolytes, such as fused silver chloride, for example, will conditioii chemical change in the way that water does-whether, for instance, silver chloride will condition the formation of hydrogen chloride from chlorine and hydrogen, so that a gas battery might be constructed of these three substances.24. “The nature of depolarisers.” By Henry E.Armstrong. When an electric current is passed between plates of platinum through a solution of sulphuric acid, the hydrogen and oxygen are partly retained at the surfaces-and apparently also within the plates-and under these conditions are capable of interacting, as in the well-known Grove gas battery : so that in so far as the “gases” thus circumstanced are concerned the change may be expressed by a reversible equation. This reversal constitutes the well known phe-nomenon termed polarisation by physicists.149 Reversal owing to the retention of hydrogen in circuit is promoted to different extents by different metals-hence apparently thc vary- ing electromotive forces of single fluid cells containing different negative plates; and when the pressure is sufficient to retain the whole of the hydrogen at the plate, it becomes total-hence it is, for example, that zinc does not dissolve in snlphuric acid under great pressure. Various substances known generally as depolarisers are used to prevent the accumulation of products of electrolysis and the conse- quent reversal of the action-such as copper sulphnte in the case of the Daniel1 cell and “nitric acid” in the case of the Grove and Bunsen cells ; but whereas the action of copper sulphate is easy to uuderstand, that of LL nitric acid ” offers many difficulties. As the heatl of dissolution of copper in dilute sulphuric acid is a negative value (about 12,000 units) the displacement of copper by hydrogen--i.e., the heat of dissolution of hjdrogen in copper sulphate-is a positive value, so that not only does the presence of the copper sulphate prevent the accumulation of hydrogen, but in removing hydrogen it also serves to increase the electromotive force of the cell from about 37/46ths to about 50/46ths of a volt.The principle underlying this is extensible even to cases in which one part of the cumulative effect of the cycle of change is a negative value. Thus,although copper has a negative heat of dissolution, it will readily dissolve in dilute sulph- uric acid if it be used in place of zinc in a Grove cell, the negative heat of dissolution of copper being more than compensated for by the positive heat of dissolution of hydrogen in ‘‘nitric acid” ; and it is well known that copper dissolves in many weak acids in presence of oxygen.It is easy to understand how oxygen acts in such case8, but the facts show that the effect produced by “ nitric acid ” is not so readily interpreted, and their consideration raises important ques- tions of general application. Rassell and Lapraik have shown that when “ nitric acid ” is freed from nitrous compounds it does not dissolve silver, but that action sets in when a trace of nitric oxide is introduced, and continues with increasing rnpidi ty as the quantity of the nitrous compound--a necessary product of the action-increases ; Veley’s later experiments have shown that the same is true of copper, without, however, affording any further explanation of the phenomena.Alt,hough it is not to be expected that such metals would dissolve in nitric acid even when coupled with a relatively electronegative conductor, as they have negative heats of dissolution, yet if the acid also acted as depolariser a cycle might be formed in which sufficient energy would be developed to condition change: it therefore follows that in such cases nitric acid does not act as the depolariser in accordance with 150 hhe equation: 2Ag + 211u'O,H + ONO,H = BSgNO, + H,O + N02H7and that in point of fact the nitrous compouiid is the de- polariser, although the nitric acid is the actual solvent of the metal, the hydrogen of the acid being virtually directly displaced by the metal with the assistance, however, of the current energy derived from its own oxidation by the nitrous compound.But what interpretation is to be given of the behavioar of more active metals, such as zinc, magnesium, &c., which have positive heats of dissolution, and, therefore, are capable of dissolving in the pure dilute acid if coupled with a relatively negative conductor; does nitric acid in their case directly act, as depolariser ? If it be capable of thus acting, such metals even when uncoupled should dissolve in the pure diluted acid.It is noteworthy that when such metals are dissolved in nitric acid hydrogen is sometimes evolved. It has been suggested that this hydrogen is derived from the int,eraction of the metal and water, but I cannot now regard this as a probable explanation ; itls production serves rather to suggest a deficiency of the depolarising agent, which cannot well occur if nitric acid be the depolariser. Indeed, if nitric acid be regarded as directly active, it is remarkable that in presence of the large excess of the acid which is always present any hydrogen should escape ; and also that the re-duction should extend so far at it often does, and not extend merely to the formation of nitrous acid. If, however, the acid be incapable oC directly acting as depolariser, and a nitrous compound be the initially active depolarising agent, it is no longer surprising that owing to the nitrous compound suffering further reduction it should be deficient parts of the circuit, and that consequently hydrogeii should escape. Why the reduction should extend so much further when metals having positive heats of dissolution are used, however, still requires elucidation.In the case of sulphuric acid, whatever metals be dissolved in the diEuted acid, no reduction takes place ; and it is only when the con- centrated and mcire or less heated acid is used that sulphurous oxide and dther reduction products are obtained. It appears not, improb-able that reduction only takes place under conditions under which the presence of sulphuric oxide is possible, i.e., that depolarisation is effected by sulphuric oxide and never by sulphui-ic acid, although this latter may be regarded as the actual solvent of the metal.There is at present no evidence forthcoming to show that nitric acid can dissociate into the anhydride and water, and even if such a change took place in concentrated solutions, there is no reason to assume that it can also take pIace in dilute solutions, and that this is the explanation of the difl'erence between nitric and sulphuric acids. It is well known, however, that nitric acid is resolved with extreme 151 facility into nitrogen dioxide, water and oxygen, and that it is excessively sensitive to the action of nitric oxide-a trace of nitric acid would therefore exercise a fermentative action and condition, the formation, it may be, of nitrous acid, or-as there is no evidence compelling us to suppose that the compound represented by the formula HNO, exists-it may be of nitrogen dioxide.In this latter case, solutions of nitric acid would resemble concentrated sulphuric acid in containing a reducible oxide, and it may be that their de-polarising action is initially exerted through such an oxide alone. To arrive at a clear conception of the function of acids in dissolving metals, and of the nature of depolarising agents, it would, therefore, appear to be necessary to take into account many circumstances to which hitherto but little attention has been paid.RESEARCH FUND. ,4 meeting of the Research Fund Committee will be held iu. Jone. Fellows desiring grants are requested to make application before June 10th. NOTICE TO AUTHORS OF PAPERS. Authors are particularly requested to send their papers to the Secretaries, at Burlington House, not later than the Monday previous to the meetilzg at which they are to be read. In all caaes an abRtract of each paper should be supplied for inser-tion in the “ Proceedings.” CERTIFICATES OF CANDIDATES FOR ELECTION AT THE NEXT BALLOT. N.13.-The names of those who sign from (‘General Knowledge ” are printed in itulics. The following Candidates will be balloted for on 25th June, 1893:-Bailey, Henry, 18, Lavender Sweep, London, S.W. Analytical Chemist and Assayer.Four years Assistant to the Public Analyst, of Cornwall. Assisted in the experimental work for the Messrs. Beringer’s book on “ Assaying,” as mentioned in preface. Some time Lecturer on Chemistry and Metallurgy at Penzance Science School. At present Chemist to the Rio Tinto Copper Co., Ltd. C. Beringer, J. J. Be ringer. John Gill. P. Gerald Sanford. William Bate, Bateman, John, Saltney, near Chester. Manager of Candle Works and Paraffin Refinery, Sulphuric, Nitric and Nitro-naphthalene Works. 20 years’ experience in manufacture of Candles and Paraffin refining. “ Sulphnric acid Works Chemist.” Honours, South Kensington S. & A,, ‘Inorganic and Organic. W. F. Love. John Bairstow. G. Watenny W.Webster. A. J. Creenaway. J. Curter Bell. Berridge, Douglas S. P., B.A. Oxon., Malverri College. Schoolmaster. Studied Science at Technical Schools, Link t ed. and at University of Oxford, took 2nd clhss Honours degree in Natural Science at latter ; at present Science Master, Malvern College ; engaged now, as for some time past, in studying Action of Light 0x1 Metallic Iodides. W. W. Fisher. V. H. Veley. J. E. Marsh. John Watts. H. Brereton Baker. Cahill, Robert S., 90, Park Lane, Norwich. Science Master of the Duke Street Higher Grade Organised Science School. I have at, present over 180 students in Theoretical and Practical Chemistry, including Advanced and Honours pupils, and have taught science work for 10 years.Francis Sutton. Edward J. Caley. F. Kapier Sutton. John R. 8:kelto)L. Williaiit Jago. John J. Pilley. Coste, John Henry, 69, Goswell Road, E.C. AnalStical Chemist. Joint author (Meldola aiid Coste : “Benzyl Derivatives of the Phenylenediamines,” J. Chem. Xoc., 1889, 590), 1at.e Student and Senior Student Chemical Department, Finshury Technical College, Assistant in Laboratory of Royal Agricultural Society of England. J. Augustue Voelcker. E.W. Voelcker. R. Meldola. Fsredk. J.Lloyd. Bernard Dyt~. Davy, S.W. M., Shsrrow View, Sliarrow, XhefEeld. Chemist and Gas Examiner to the SheEeld Gas Company. Ap-prentice with the South Down Metal Chemical Co., Ltd., 1879-82. Chemist at the Manchester Corporation Gas Works, 1882-88. Head Chemist to the Slie5eld United Gas Light Co.(appointed 1888). Henry Bird. C. Kilpatrick. R. L. Taylor. Francis Jones. Thornton Charles Lamb. Pemeval Babington. Cilbert J.Fowler. Arthur W. Crossley. Green, Arthur Henry, 176, Lloyd Street, Greenheys, Manchester. Analytical Chemist. I studied Chemistry under Mr. Francis Jones, Physics iiiider Mr. John Angell, F.T.C., and Mathematics nnder Messrs. Holme, Buohheirn, and Start at the Manchestel* Grammar School during 2 years (1384 to 1886). Then studied Chemistry during 5 years with Messrs. Crace-Cal yert aiid Thomson at the Royal Institution Laboratory at Manchester, 3 years as pupil and 2 as assistant (1886 to 1891). I attended evening classes at Owens College under Dr. Bailey and Dr. Harden (1885 to 1SSS).I 155 am now engaged in chemical investigation and analytical work at my own Laboratory. William Thomson. M. W. Jones., Arthur Harden. G. H. Bailey. John Angell. Francis Jones. George H. Eurst. Otto Eehner. Chades E.Cassal. Howitt, James John, Dimley, Toft Road, Knutsford, Cheshire. General Manager and Engineer of Chemical Works. I am a Cheniical Engineer, also a Chemical Student ; and Works General Manager (Chemical), and for many years been connected wit11 Manufacturing Chemistry, and still eugaged so. Francis Henry Tate. John Knowles. J. Caster Bell. Fredc. H. Bowman. Watson hith. Vieian B. Lewes. Leather, John Walter, 15, Bradgnte Ro;td, Catford, S.E. Agricultural Chemist. Doctor of Philosophy.Dissertation :-“ Die Pipizkiirnsaure.” Fellow of the Institute of Chemistry of Great Britain and Ireland. 5 years Senior A;isista.nt to Ur.Voelcker in the Laboratory of the Royal Agricultmd Society of England. J. Augustns Voelcker. E. W. Voelcker. J. H. Gilbert. P. Vieth. Bernard Dyer. Edward Kinch. Charles E. Groves. Henry E. Armstrong. Lloyd, William Howard, 5, Belmont Villas, New Walk, Leicester. Wholesale Jlanufacturing Chemist. Educated at the Wyggestoll Hospital School or Leicester Grammar School. For two years head Assistant in the manufacturing Laboratory of Messrs. Richardson & Co., of this town, and since then 4 years’ experience in manu-facturing, pharnracentical, and analytical work. Holder of the Assistant’s Certificate of Apothecaries’ Society and Associate of Pharmaceutical Society, and now of the firm of J.Howard, Lloyd, & Co., Manufacturing Chemists, Leicester. WiI liam Hzlsli nes s. Mamuel B’rancis Burford. John Hodgkin. J.Eell. H. J.Eeh. C. il’roctor. J. Tt’ood WLUTLE. 156 MoElroy, R.P., 1412, Sixteenth Street, Washington, D.C., U.S.A. Chemist. Second Assistant Chemist, United States Department of Agriculture ; Vice-president (1893), Washington Chemical Society. Edgar Richards. C1 ifford Richardson. Edw. Gudeman. Charles E. Mnnroe. C. F. Chandler. Elwyn Waller. H. T. Vulte’. McHerrow, Charles Alexander, 41, Eccles Old Road, Pendleton, near Manchester. Colorist and Chemist at the Clayton Aniline Co.’s works, Clayton, near Manchester.Author of “ The Bleaching, Dyeing, and Finishing uf Linen and Linen Goods,” in course of publication in The Textile Manufacturer. Formerly day Student at Owens College, Manchester, and at the laboratories of Carter Bell, Esq. Harold €3. Dixon. Julius B. Cohen. Francis Jones. Arthur Harden. J. Carter Bell. Arthur Smithells. William Thomson. H. E. Boscoe. Mills, Charles, Hazeldean, Fulham Palace Gardens, S.W. Student in Chemistry, Central Institution, Exhibition Road, S.W. Associate of the City and Guilds Institute. Joint Author with Professor Armstrong of “ The Action of Bromine on Aeobenzene,” cj. this Society’s Proceedings, December 1, 1892. Henry E. Armstrong. W. Palmer Wynne. F. Stanley Ripping. W. J. Pope. Arthur R.Ling. Martin, Alexander Mitohell, Douglas Villa, Dunbeth Road, Coatbridge. Analytical Chemist and Metallurgist. G-artsherrie Iron Works {Messrs. William Baird and Co.). I have been for the past 6 years in charge of Laboratory of above iron smelting work, where also the bye-products are recovered from the furnace gases, with 4 years’ pre- vious training in Chemistry and allied Sciences in theory and practice. R. R. Tatlock. Horat.io Bnllantyne. Edmnnd J. Mills. A. Humboldt Sexton, James G. Hardy. 157 Napier, John Watson, Minto House, Edinburgh. Analytical Chemist. Assistant for 4 years in the Laboratory of Mr. J. Falconer King, City Analyst, Edinburgh. Attended Lectures on Chemistry under Professor W. H. Perkin, jun., for three sessions.J. Falconer King. John Hunter. W. H. Perkin, jun, Hugh Marshall. G. H. Gemmell. Orndofl, William Ridgely, Ithaca, N.Y., U.S.A. Assistant Professor of Chemistry in Cornell University, A.B. and Ph.D. Johns Hopkins University, Baltimore, M.D. Have published the following papers :-“ Decomposition of Diazo-compounds with Alcohol ” (8mer. Ohem. J.,9, 387 ; 12,153 ; 14, 45) ; “ Decomposi-tion of Acetone with Bleaching Powder ” (Amer. Chem. J.,10,363) ; “Metmapropionic and Parapmpionio Aldehydes ” (Amer. Chem. J., 12, 352), and severs1 other papers and reports ia the same Journal. John A. Miller, Ph.D. W. H. Chandler. C. F. Chandler. Elwyn Waller. H. 1.Vulte’. Orr, Alexander, 109, Pitt Street, Sydney, Australia. Analytical Chemist.Assayer and Metallurgist. Inventor of the Orr White Lead Process-works now erecting in Belgium. Iu England, company is being formed by “Alliance Pure White Lead Syndicate.” Robert R. Tatlock. John Clark. Edw. C. Stanford. John Hargreaves. John W. Towers. Pring, Charles Herbert, The Ferns, Longfield Road, Bristol. Student. Student iu Chemical Laboratory Merchant Venturers’ School, Bristol, for two years, and still there engaged in Analytical work. Pharmaceutical ‘‘ Minor ” qualification. Two years Principal of Laboratory at Messrs. Clements & Co., Manufacturing Chemists, Bristol. At present engaged in Research, Repurification of Crude Animal Oils, &c. Ernest H. Cook. James Leicester. Thos. Coomber. Henry J.Palmer. T. W. G. Blyth. J. Wertheimer. 158 Ritchie, George, 8, Bucha’nan Gardens, Mount Vernon, N.B. Analytical Chemist. Chief Chemist at Parkhead Forge, Glasgow. Studied at City Analyst’s Laboratory under Robt. Tatlock, Esq. For past ten yea,rs have been engaged in the study and practice of Analytical Chemistry. Author of ‘‘Gaseous Fuel and its Production.” Robert It. Tatlock. John Clark. A. Humboldt Sexton. Horatio Ballantyne. T. F. Barbour. J. E.Stead. Jas. G.Hardy. Sessions, Wilfred, Russell House, Gloucester (at present Leigh ton Park, Reading). Schoolmaster. Science Master at Leighton Park School. Have taught Science for one year at Sidcot School. London Bachelor of Science. Three years’ Student in Owens College Laboratories.Harold B. Dixon. G. H. Bailey. Arthur Harden. Gilbert J. Fowler. P. J. Hartog, W,H. Perkin, jun. Sorrell, Henry Tho., Holly Lodge, Hill, Southampton West. Chemical Lecturer. Milldown Laboratory, Blandford. Late Braver at the Shirley Brewery, Croydon, and at the Hatcham Brewery, New Cross. Late Science Master at High School, Heaton Chapel, Manchester. Honours Inorganic Chemistry and 1st Class Organic Science and Art Department. Chapman Jones. Henry P. Harris. John M. H. Munro. W. Palmer Wynne. Wm. Tate. Thompson,Frank Ernest, 97, Murdoch Road, Handsworth, Birmingham. Teacher of Chemistry. (1) An Associate of the Royal College of Science, London, in the division of Chemistry. (2) Hold three Honours Chemistry (Science and Art Examinations) : 1st class Honours Practical Inorganic Chemistry ; 1st class Honours Practical Organic Chemistry (1st bracket) ; 2nd class Honours Theoretical Inorganic Chemistry.(3) Engaged as Teacher of Chemistry at the Waverley Road Technical School, Small Heath, Birmingham, and at the Dudley Institute. Chapman Jones. Alfred E. Tntton. William Tate. F. R. Japp. E. J. COG. 159 Vautin, Claude Theodore James, 10, Hanover Square, London. Metallurgist. Have been engaged in Metallurgical Cheizlistry during the past 18 years. Have devised successful process for refining metallic copper (at work, New South Wales). Co-inventor of Newbery-Vautin gold-extraction process. Devised process for extracting gold from tin (at work, Chiltern, Victoria).Introduced Matte smelting in Victoria at Bethanga. Devised plant from “ Bessemering ” copper and iron sulphides (Cobar, New South Wales), &c. At present investigating Aluminium Salts and the production of the metal, also in Electrolytical separations. William Ramsay. D. A. Louis. Edward Bevan. Chas. Fred. Cross. William Crookes. Warmington, Edward Augustus, 266, Castle Street, Dudley. Chemist. I have studied Chemistry for the last seven years, first at Mason College, Birmingham, under Professor Tilden, and then in Leipzig. In 1892 I obtained the degree of Doctor of Philosophy of Leipzig. I have contributed to Chemical Science a paper “Ueber Phenyluracil u. analoge Verbindungon,” published in the Journ,aZ fiir Praktische Chernie, 47, 201.William A. Tilden. W. W. J. Nicol. Thomas Turner. Credacre G. Moor. William Ramsay. Whittaker, Thomas, 76, Arden Terrace, Accrington. Chemical and Mechanical Engineer. Lecturer on Chemistry, Accrington Technical School. Past student Normal School of Science. Analyst to the Doury Iron Works, Accrington. Percy F. Frankland. John Wrightson. Conrad Gerland. Chapman Jones. &I.W. Jones. Wholly, Sydney, 38, Savelock Street, Canterbury. Science Master. Associate (in Chemistry) of the Royal College of Science, London. Science Master, Simon Langton Schools, Canter- bury. W. Palnier Wynne. Chapman Jones. Alfred E. Tutton. William Tate. Lionel M. Jones. J. W. Rodger. 160 The following Certificate is recommended by the Council under Bye-law I (par. 3) :-Hancock, Ernest Albert, Basseterre, St. Kitts, Leeward Islands. Analyst. Government Analytical Chemist for the Presidency of St. Christopher- Nevis . Francis Watts. John R. Bovell. Hewry E,drnzstroizg. HARRISON AND SONS,PRINTERS IN ORDINARY TO HER MAJESTY, ST.MARTIN’S LANE.
ISSN:0369-8718
DOI:10.1039/PL8930900141
出版商:RSC
年代:1893
数据来源: RSC
|
|