Decomposes sentence example

decomposes
  • It slowly decomposes on exposure or on heating.
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  • Concentrated sulphuric acid also decomposes it: H 2 SO 4 +H 2 S = 2H 2 0 +S02+S.
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  • It decomposes water slowly in the cold, and more rapidly on heating.
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  • On fusion with solid potash at 250° C. it completely decomposes, giving potassium oxalate and hydrogen, C2H602-1-2KHO =K2C204+4H2.
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  • Long-continued heating with water also decomposes it slowly.
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  • A pentasulphide B2S5 is prepared, in an impure condition, by heating a solution of sulphur in carbon bisulphide with boron iodide, and forms a white crystalline powder which decomposes under the influence of water into sulphur, sulphuretted hydrogen and boric acid.
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  • It combines with many metals to form sulphides, and also decomposes many metallic salts with consequent production of sulphides, a property which renders it extremely useful in chemical analysis.
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  • It may be condensed and yields a solid which melts at - 55° C. Sulphuretted hydrogen decomposes it with formation of hydrofluoric acid and liberation of sulphur.
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  • Cadmium vapour decomposes water at a red heat, with liberation of hydrogen, and formation of the oxide of the metal.
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  • Water decomposes it violently with formation of hydrochloric and sulphurous acids.
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  • Water decomposes it into hydrochloric and sulphurous acids.
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  • Thiosulphuric acid, formerly called hyposulphurous acid, H2S203, cannot be preserved in the free state, since it gradually decomposes with evolution of sulphur dioxide and liberation of sulphur: H 2 S 2 O 3 = S+S0 2 +H 2 O.
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  • It also burns when heated in a current of steam, which it decomposes with the liberation of hydrogen and the formation of magnesia.
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  • It is unstable at ordinary temperatures and rapidly decomposes into its generators on warming.
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  • Water decomposes it with formation of sulphuric acid and oxygen: 25207 + 4H 2 0 = 4H 2 SO 4 + 02.
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  • Its aqueous solution gradually decomposes with evolution of oxygen, behaves as a strong oxidant, and liberates iodine from potassium iodide.
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  • This salt, on standing, decomposes into barium dithionate, BaS206, and diethyl disulphide, (C2H5)2S2, which points to the presence of the SH group in the molecule.
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  • It is only stable in dilute aqueous solution, for on concentration the acid decomposes with formation of sulphuric acid, sulphur dioxide and sulphur.
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  • The acid melts at 132° C., and at a higher temperature it rapidly decomposes into acetic acid and carbon dioxide.
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  • It melts at 70° C.and at higher temperatures decomposes, with evolution of carbon dioxide and formation of aceto-nitrile, CH 3 CN.
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  • A higher temperature decomposes this body into carbon dioxide and itaconic acid, C 5 H 6 0 4, which, again, by the expulsion of a molecule of water, yields citraconic anhydride, C 5 H 4 0 3.
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  • It is a strong acid, and dissolved in water decomposes carbonates and attacks iron and zinc.
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  • It is insoluble in acids and decomposes when heated to a sufficiently high temperature.
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  • It forms a golden yellow crystalline mass, which sublimes slowly in vacuo, and melts at 25.5° C. It blackens on exposure to moisture, and decomposes when exposed to light.
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  • It is insoluble in water, but gradually decomposes, forming a hydrated oxide, Ru 2 0 5 H 2 O.
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  • The per-ruthenate, KRuO 4, formed by the action of chlorine on the ruthenate, or of alkalis on the peroxide at 50° C., is a black crystalline solid which is stable in dry air but decomposes when heated strongly.
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  • On fusion with caustic potash it decomposes with formation of tetrahydroxy-benzophenone, which then breaks up into resorcin and hydroquinone.
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  • When nitric peroxide, N204, is converted into gas, it decomposes, and at about 180° C. its vapour entirely consists of molecules of the composition N02; while at temperatures between this and o C. it consists of a mixture in different proportions of the two kinds of molecules, N 2 O 4 and N02.
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  • This artifice is specially valuable when the substance decomposes or volatilizes in a warm current of carbon dioxide.
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  • It sublimes, but on rapid heating decomposes into carbon dioxide and phenol.
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  • When heated in air for many hours it decomposes, yielding carbon dioxide, phenol and xanthone.
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  • It decomposes slowly on standing, yielding water and nitrous oxide.
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  • The pure acid has not yet been obtained, since in the presence of water it decomposes with formation of nitric acid and liberation of nitric oxide: 3HN02 =HNO 3 +2N0+H20.
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  • It is a gas at ordinary temperature; when liquefied it boils at -63.5° C. and on solidification melts at -139° C. Water decomposes it into nitric and hydrofluoric acids.
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  • Boiling with dilute mineral acids, or baryta water, decomposes albumins into carbon dioxide, ammonia and fatty aminoand other acids.
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  • Thus the hydroxyl mentioned above decomposes into water and oxygen, and the chlorine produced by the electrolysis of a chloride may attack the metal of the anode.
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  • There is present in the seeds an enzyme which rapidly decomposes the oil if the seeds are crushed and kept, setting free a fatty acid and glycerin.
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  • With water it forms a hydrate, and ultimately decomposes into lead dioxide and hydrochloric acid.
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  • In the German Patent 1 57573 (1904) it is shown that by the action of at least two molecular proportions of an alkyl formate on two molecular proportions of a magnesium alkyl or aryl haloid, a complex addition compound is formed, which readily decomposes into a basic magnesium salt and an aldehyde, C H MgBr-f-H000R-RO�CH�C H.
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  • Nitromethane, CH 3 NO 2, is a colourless oil which boils at 101° C. Fuming sulphuric acid decomposes it into carbon monoxide and hydroxylamine.
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  • The silver salt, obtained by shaking an ether solution of nitroform with freshly prepared, slightly moist silver oxide, reacts with methyl iodide to form trinitroethane, a crystalline solid which melts at 56° C. Concentrated caustic potash decomposes the latter compound, forming the potassium salt of dinitroethane, CH3 C(N02)2K.
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  • Hantzsch, Ber., 1906, 39, p. 139): Ordinary temperature Cyamelide (CNOH) 3 Cyanic acid CNOH HO ions 1 High Cyanuric acid Decomposes with temperature
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  • The powdery metal when heated in air to 150° or 170° C. catches fire and burns brilliantly into U 3 0 8; it decomposes water slowly at ordinary temperatures, but rapidly when boiling.
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  • Alcoholic potash decomposes it into piperidine, C5H,1N, and piperic acid, C 12 H 10 O 4.
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  • It decomposes ammonia at a red heat, liberating hydrogen and yielding a compound containing silicon and nitrogen.
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  • It decomposes solutions of silver nitrate and copper sulphate.
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  • Water decomposes it into silicofluoric acid and silicic acid: 3SiF 4 +3H 2 0 =2H2SiF6+ H 2 SiO 3.
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  • The solution on evaporation deposits a hydrated form, H 2 SiF 6.2H 2 O, which decomposes when heated.
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  • The anhydrous acid is not known, since on evaporating the aqueous solution it gradually decomposes into silicon fluoride and hydrofluoric acid.
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  • Water decomposes it into hydrochloric and silicic acids.
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  • It is a colourless liquid which boils at 210° C. Water decomposes it with the formation of silico-mesoxalic acid, HOOSi Si(OH) 2 SiOOH.
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  • It is a colourless, strongly refracting liquid, which boils at about 220° C., slight decomposition setting in above 150° C. Water decomposes it with production of leucone.
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  • It is readily decomposed by water: Si(NH 2) 4 +2H 2 O=4NH 3 +S10 2 Above o° C. it decomposes thus: Si(NH 2) 4 =2HN3-}-Si(NH)2.
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  • It decomposes water at ordinary temperature with evolution of hydrogen but without production of silicon hydride, whilst cold hydrochloric acid attacks it vigorously with evolution of hydrogen and spontaneously inflammable silicon hydride.
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  • OH, formed by the action of moist air on silicon octochloride at o° C., is very unstable, and hot water decomposes it with evolution of hydrogen and formation of silicic acid (L.
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  • The ultimate chlorination product of copper, CuC1 2, when heated to redness, decomposes into the lower chloride, CuCI, and chlorine.
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  • At a red heat it evolves oxygen with the formation of potassium nitrite, which, in turn, decomposes at a higher temperature.
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  • Titanium dichloride, TiC1 21 obtained by passing hydrogen over the trichloride at a dull red heat, is a very hygroscopic brown powder which inflames when exposed to air, and energetically decomposes water.
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  • With dry ammonia at 60° the metal forms strontium ammonium, which slowly decomposes in a vacuum at 20° giving Sr(NH 3) 2; with carbon monoxide it gives Sr(CO) 2; with oxygen it forms the monoxide and peroxide, and with nitric oxide it gives the hyponitrite (Roederer, Bull.
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  • It is a white solid, which readily decomposes water in the cold and behaves as a strong reducing agent.
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  • It is a white solid, which combines with gaseous ammonia to form SrC1 2.8NH 3, and when heated in superheated steam it decomposes with evolution of hydrochloric acid.
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  • Phosphorus pentachloride decomposes it into carbon monoxide and dioxide, the reaction being the one generally applied for the purpose of preparing phosphorus oxychloride.
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  • The silver salt decomposes with explosive violence, leaving a residue of the metal.
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  • It begins to decompose into gold and chlorine at 185°, the decomposition being complete at 230°; water decomposes it into gold and auric chloride.
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  • Water decomposes it into gold and auric chloride.
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  • Aurous iodide, Aul, is a light-yellow, sparingly soluble powder obtained, together with free iodine, by adding potassium iodide to auric chloride; auric iodide, Au13, is formed as a dark-green powder at the same time, but it readily decomposes to aurous iodide and iodine.
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  • Treated with sodammonium it yields a bluish-black mass, BiNa 3, which takes fire in the air and decomposes water.
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  • Water decomposes it to metallic bismuth and the oxychloride, BiOC1.
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  • Water decomposes it, giving a basic salt, Bi 2 (SO 4)(OH) i which on heating gives (BiO) 2 SO 4.
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  • It is soluble in water, the solution gradually decomposing with deposition of tellurium; it also decomposes on exposure to light.
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  • It melts at 224° C. and is exceedingly hygroscopic. Water decomposes it with formation of tellurous acid and other products.
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  • They found that if liquid acetylene in a steel bottle be heated at one point by a platinum wire raised to a red heat, the whole mass decomposes and gives rise to such tremendous pressures that no cylinder would be able to withstand them.
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  • It is insoluble in acids and exists in several hydrated forms. The osmiates, corresponding to the unknown trioxide 0503, are red or green coloured salts; the solutions are only stable in the presence of excess of caustic alkali; on boiling an aqueous solution of the potassium salt it decomposes readily, forming a black precipitate of osmic acid, H20s04.
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  • It is stable in dry air, but in moist air rapidly decomposes.
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  • It is soluble in water, but the dilute solution readily decomposes on standing.
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  • The aqueous solution decomposes rapidly on boiling.
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  • In chemistry the term is given to chemical reactions in which a substance decomposes into two or more substances, and particularly to cases in which associated molecules break down into simpler molecules.
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  • As the current flows it decomposes the liquid and liberates oxygen and hydrogen gases, which escape.
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  • Water decomposes it to give hydrogen free from ammonia and acetylene, i gram yielding about loo ccs.
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  • By the addition of sodium amalgam to a concentrated solution of ammonium chloride, the so-called ammonium amalgam is obtained as a spongy mass which floats on the surface of the liquid; it decomposes readily at ordinary temperatures into ammonia and hydrogen; it does not reduce silver and gold salts, a behaviour which distinguishes it from the amalgams of the alkali metals, and for this reason it is regarded by some chemists as being merely mercury inflated by gaseous ammonia and hydrogen.
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  • It decomposes silicates on being heated with them.
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  • At 200° C. this salt decomposes, giving off hydrofluoric acid, and between 230-250° C. fluorine is liberated.
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  • When anhydrous it is a colourless opaque solid which melts at 310 °, and decomposes at about 110o°.
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  • Water decomposes it, giving oxygen and the dioxide.
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  • Under these conditions the lactose decomposes into dark-brown fission products, the fat loses its emulsified condition and separates out as cream which cannot be made to diffuse again even by shaking, and the albuminoids are converted into a form very difficult of digestion.
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  • In this method of preparation it is found that the secondary alcohols decompose more readily that the primary alcohols of the series, and when sulphuric acid is used, two phases are present in the reaction, the first being the building up of an intermediate sulphuric acid ester, which then decomposes into sulphuric acid and hydrocarbon: C2H 5 OH->C 2 H 5 HSO 4 ->C 2 H 4 +-H 2 SO 4.
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  • Water decomposes it violently, with formation of carbon dioxide and hydrochloric acid.
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  • It Is Soluble In Water; The Aqueous Solution Gradually Decomposes On Standing, Forming Carbon Dioxide And Sulphuretted Hydrogen.
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  • On boiling with water it decomposes into quinone and hydroquinone.
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  • This salt is very deliquescent; it melts at 45°, and at 100° decomposes into iodine and potassium iodide.
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  • When the dry salt is heated to 190° it decomposes into normal carbonate, carbon dioxide and water.
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  • The solution is strongly caustic. It turns yellow on exposure to air, absorbing oxygen and carbon dioxide and forming thiosulphate and potassium carbonate and liberating sulphuretted hydrogen, which decomposes into water and sulphur, the latter combining with the monosulphide to form higher salts.
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  • The solution also decomposes on boiling.
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  • It decomposes in moist air, or with water, giving caustic potash and ammonia, in the latter case with considerable evolution of heat.
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  • Potash fusion decomposes it into benzoic and acetic acids.
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  • Strong heating decomposes the majority of the iodides.
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  • It crystallizes in long yellow needles and decomposes readily on heating into the monochloride and chlorine.
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  • It is readily soluble in water, but excess of water decomposes it.
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  • and is readily soluble in water, but the solution is unstable and decomposes on standing, giving amorphous insoluble substances, and ammonium formate, oxalic acid, &c. An aqueous solution of hydrogen peroxide converts it into oxamide, (CONH 2) 2, and reduction by zinc and hydrochloric acid gives methylamine.
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  • 7764 (1890)] decomposes sulphocyanides by fusing with zinc: the zinc is heated with a small quantity of carbon and when completely fused potassium sulphocyanide is added, the mass being well stirred and heated until it thickens and begins to turn red; finally it is allowed to cool out of contact with air, lixiviated with water, the solution decanted, and evaporated to a paste in vacuo.
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  • It is a tetrabasic acid, of markedly acid character, and readily decomposes carbonates and acetates.
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  • The solution decomposes on standing, and in the presence of an alkali acts as an oxidizing agent: 2K 3 Fe(NC) 6 +2KHO = 2K4Fe(NC)6+H20+0.
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  • When heated with zinc dust, tac: acid decomposes into carbon monoxide and hydrogen.
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  • The hydrated salt loses water on heating, and partially decomposes into hydrochloric acid and magnesium oxychlorides.
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  • Water decomposes it with liberation of ammonia and formation of magnesium hydroxide.
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  • It slowly decomposes in moist air, liberating sulphuretted hydrogen, and with water it gives a yellow solution which becomes colourless on exposure.
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  • On the other hand, if the concrete is rough and porous the sea-water will gradually eat into the heart of the structure, especially in a case like a dam, where the water, being higher on one side than the other, constantly forces its way through the rough material, and decomposes the Portland cement it contains.
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  • It has been found, however, that molten cryolite and the analogous double fluoride represented by the formula Al 2 F 6.2NaF are very efficient solvents of alumina, and that these solutions can be easily electrolysed at about 800° C. by means of a current that completely decomposes the oxide but leaves the haloid salts unaffected.
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  • The metal in mass is not affected by hot or cold water, the foil is very slowly oxidized, while the amalgam decomposes rapidly.
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  • At elevated temperatures the metal decomposes nearly all other metallic oxides, wherefore it is most serviceable as a metallurgical reagent.
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  • Nickel and manganese lower these critical points, so that with 25% of nickel Ar lies below the common temperature 20° C. With 13% of manganese Ar is very low, and the austenite decomposes so slowly that it is preserved practically intact by sudden cooling.
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  • Hantzsch explains the characteristic reactions of the diazonium compounds ky the assumption that an addition compound is first formed, which breaks down with the elimination of the hydride of the acid radical, and the formation of an unstable syn-diazo compound, which, in its turn, decomposes with evolution of nitrogen (Ber., 18 97, 30, p. 2 54 8; 1898, 31, p. 2053).
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  • Concentrated hydrochloric acid decomposes it with formation of C6H 6 N OH HO'N'H chloranilines and elimination of nitrogen, whilst on boiling with sulphuric acid it is converted into aminophenols.
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  • It is a yellowish oil which melts at - 24° C.; it boils at 143-144° C., but cannot be distilled safely as it decomposes violently, giving nitrogen and ethyl fumarate.
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  • soc. chim., 1902, 27, p. 1141) has shown that potassium hydride decomposes cold water, with evolution of hydrogen, KH+H 2 0 = KOH+ H2.
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  • Calcium hydride or hydrolite, prepared by passing hydrogen over heated calcium, decomposes water similarly, r gram giving 1 litre of gas; it has been proposed as a commercial source (Prats Aymerich, Abst.
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  • p. 543), as has also aluminium turnings moistened with potassium cyanide and mercuric chloride, which decomposes water regularly at 70°, i gram giving 1.3 litres of gas (Mauricheau-Beaupre, Comptes rendus, 1908, 147, p. 310).
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  • It is sought to explain these oxidation processes by assuming that the hydrogen peroxide unites with the compound undergoing oxidation to form an addition compound, which subsequently decomposes (J.
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  • It is a colourless oily liquid of strongly acid reaction; its aqueous solution decomposes on standing and on heating it forms diethyl sulphate and sulphuric acid.
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  • It decomposes cold water slowly, but hot water violently.
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  • It decomposes ammonium salts.
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  • This consists in the use of emetics or the stomach-pump, with lime-water, which decomposes the alkaloid.
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  • Bokorny, moreover, it appears that such filaments will yield :starch from formaldehyde when they are supplied with sodium -oxymethyl sulphonate, a salt which readily decomposes into formaldehyde and hydrogen sodium sulphite, an observation which has been taken to mean that formaldehyde is always a stage in the synthesis of starch.
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  • It decomposes water at a red heat, liberating hydrogen and being itself converted into the hydrate.
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  • It melts at 720° and decomposes rapidly above 800°, giving oxygen and thallous oxide.
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  • The sulphate decomposes into sulphuric acid and the trioxide on warming with water, and differs from aluminium sulphate in not forming alums.
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  • Dry chlorine gas passed into melted urea decomposes it with formation of cyanuric acid and ammonium chloride, nitrogen and ammonia being simultaneously liberated.
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  • Riegler (ibid., 18 94, 33, p. 49) decomposes urea solutions by means of mercury dissolved in nitric acid, and measures the evolved gas.
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  • Lachmann, Ann., 1895, 288, p. 281), is a crystalline powder, soluble in water, and which decomposes on heating.
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  • Hydrolysis by alkalis decomposes them into carbon dioxide, amines and ammonia.
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  • Acetyl urea, NH 2 CO NH 000H 31 formed by the action of acetic anhydride on urea, crystallizes in needles which melt at 212° C. and, on heating, strongly decomposes into acetamide and cyanuric acid.
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  • Hydrochloric acid at 200° C. decomposes into oxalic acid, carbon dioxide and methylamine, whilst an alcoholic solution of a caustic alkali gives dimethyl urea and oxalic acid.
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  • Above 50° C. it decomposes into the dioxide and oxygen.
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  • It decomposes violently on heating, and explodes in contact with hydrogen, sulphur, phosphorus, &c. It dissolves in water to form a deep red solution which contains permanganic acid, HMnO 4.
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  • This solution is of a deep violetred colour, and is somewhat fluorescent; it decomposes on exposure to light, or when heated.
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  • The excess of acid is removed by spreading the mass on a porous plate, the residue stirred for some hours with nitric acid, again spread on a porous plate, and finally dried quickly at about 130° C. It is a dark green deliquescent powder which decomposes on heating or on exposure to moist air.
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  • It completely decomposes hydrogen peroxide in sulphuric acid solution 2KMn04+5H202-I-3H2S04 = K2S04+2MnS04+8H20+502.
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  • It decomposes when heated to 200° - 240°C.: 2KMn04=K2Mn04+Mn02+02; and when warmed with hydrochloric acid it yields chlorine: 2 KM nO 4 + 16HC1= 2KC1 +2 MnC1 2 +8H 2 0 +5C12.
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  • Ammonium Permanganate, NH 4 Mn0 4, explodes violently on rubbing, and its aqueous solution decomposes on boiling (W.
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  • This amidoguanidine decomposes on hydrolysis with the formation of semicarbazide, NH 2 CO NH NH 21 which, in its turn, breaks down into carbon dioxide, ammonia and hydrazine.
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  • By heating gallium in a regulated stream of chlorine the dichloride GaC1 2 is obtained as a crystalline mass, which melts at 164° C. and readily decomposes on exposure to moist air.
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  • 18 95, p. 945) has obtained metallic nickel from the Canadian mattes by first roasting them and then eliminating copper by the action of sulphuric acid, the product so obtained being then exposed to the reducing action of producer gas at about 350° C. The reduced metal is then passed into a "volatilizer" and exposed to the action of carbon monoxide at about 80° C., the nickel carbonyl so formed being received in a chamber heated to 180-200° C., where it decomposes, the nickel being deposited and the carbon monoxide returned to the volatilizer.
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  • It decomposes water at a red heat.
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  • It decomposes with explosive violence when heated rapidly.
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  • It oxidizes rapidly on exposure to air, and decomposes cold water very rapidly.
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  • Ammonia does not react with tungsten or the dioxide, but with trioxide at a red heat a substance of the formula W 5 H 6 N 3 0 5 is obtained, which is insoluble in acids and alkalis and on ignition decomposes, evolving nitrogen, hydrogen and ammonia.
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  • On the addition of iodine to this oxide, chlorine is liberated and a white substance is produced, which decomposes, on heating to 380° C., into iodine and oxygen; bromine is without action (see A.
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  • The crystalline hydrate melts at 50° C. The pure acid decomposes slowly on standing, but is stable in dilute aqueous solution.
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  • Ferrous chloride decomposes the copper oxide and carbonate with the formation of cuprous and cupric chlorides (which remain in solution), and the precipitation of ferrous oxide, carbon dioxide being simultaneously liberated from the carbonate.
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  • When moist, it decomposes at about 6° C., but the dry substance must be heated to about 180°, before decomposition sets in (see L.
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  • Merrill, it decomposes when heated, and gives cupric hydride, CuH 21 as a reddish-brown spongy mass, which turns to a chocolate colour on exposure.
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  • It decomposes when heated to 900; with water it gives nitric oxide and cupric nitrate and nitrite.
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  • It decomposes steam at a red heat, and burns (especially when finely powdered) in chlorine.
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  • On heating in absence of air, it decomposes into the trisulphide and sulphur.
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  • It is easily soluble in water and decomposes when heated to zoo° C.
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  • Potassium permanganate decomposes morphine by oxidation, the action being facilitated by the addition of a small quantity of mineral acid to the solution.
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  • In amalgamating without the use of chemicals, finely divided iron, worn from the shoes and dies in the stamp-mill and the pan, decomposes cerargyrite and argentite, and the liberated silver is taken up by the quicksilver; the process is hastened by adding salt.
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  • This salt, insoluble in water but soluble in brine, also acts upon argentite (Ag 2 S-+-Cu 2 C1 2 =2AgC1±-CuS±-Cu) and pyrargyrite (2Ag 3 SbS 3 -I-Cu 2 C12 = 2AgC1 +Ag 2 S +2Ag +2CuS +Sb2S3), and would give with silver sulphide in the presence of quicksilver, the Patioreaction; metallic silver, cupric sulphide, and mercurous chloride (2Ag 2 S+Cu 2 C1 2 +2Hg=4Ag+2CuS+Hg 2 C1 2), but the iron decomposes the quicksilver salt, setting free the quicksilver.
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  • It readily decomposes into silver and oxygen.
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  • It decomposes when strongly heated.
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  • It decomposes when heated above 35° C., and also in the presence of water.
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  • It decomposes water at ordinary temperature, liberating hydrogen and forming lithium hydroxide.
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  • They are decomposed by chlorine, with liberation of bromine and formation of metallic chlorides; concentrated sulphuric acid also decomposes them, with formation of a metallic sulphate and liberation of bromine and sulphur dioxide.
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  • Hydrobromic acid decomposes it according to the equation HBrO, 5HBr=3H20 3Br2.
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  • It forms a colourless syrup, of specific gravity 1.2485 (1 5°/4°), and decomposes on distillation under ordinary atmospheric pressure; but at very low pressures (about i mm.) it distils at about 85° C., and then sets to a crystalline solid, which melts at about 18° C. It possesses the properties both of an acid and of an alcohol.
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  • When finely divided it decomposes water giving hydrogen phosphide; it also reduces sulphurous and sulphuric' acids, and when boiled with water gives phosphine and hypophosphorous acid; when slowly oxidized under water it yields, hypophosphoric acid.
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  • It decomposes when heated, hydrogen and red phosphorus being formed.
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  • It decomposes on heating into phosphine and phosphoric acid.
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  • Deliquescent, rectangular tablets of H 4 P 2062H 2 O separate out on concentrating a solution in a vacuum, which on drying further give the acid, which melts at 55°, and decomposes suddenly when heated to 70° into phosphorous and metaphosphoric acids with a certain amount of hydrogen phosphide.
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  • It decomposes slowly at ordinary temperatures.
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  • The bromochloride, PC1 3 Br 21 is an orange-coloured solid formed from bromine and the trichloride, into which components it decomposes at 35°.
    0
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  • It is a white, infusible, very stable solid, which decomposes water on heating, giving ammonia and metaphosphoric acid, whilst alkalis give an analogous reaction.
    0
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  • The diamide, PN 2 H 4, was obtained by Hugot (ibid., 1905, 141, p. 1235) by acting with ammonia gas on phosphorus tribromide or tri-iodide at -70 0; it is very unstable, and decomposes at -25°.
    0
    0
  • Carbon decomposes hot strong sulphuric acid on long continued boiling, with the formation of carbon dioxide and sulphur dioxide.
    0
    0
  • Sedanolic acid readily decomposes into water and its lactone sedanolid, C 12 H 18 0 2, the odorous constituent of celery oil.
    0
    0
  • With bromine it forms a dibromide, which then heated to 110° C. decomposes into hydrobromic acid and benzyl bromide.
    0
    0
  • The ammonium hydroxide on distillation decomposes into trimethylamine, water and cyclo-octadiene 1.3.
    0
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  • Ethane, when heated to this degree, splits up into ethylene and hydrogen, whilst ethylene decomposes to methane and acetylene, and the acetylene at once polymerizes to benzene, styrolene, retene, &c. A portion also condenses, and at the same time loses some hydrogen, becoming naphthalene; and the compounds so formed by interactions amongst themselves build up the remainder of the hydrocarbons present in the coal tar, whilst the organic substances containing oxygen in the coal break down, and cause the formation of the phenols in the tar.
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  • It will be noticed that in the earlier stages the quantity of sulphur impurities is actually increased between the purifiers - in fact, the greater amount of sulphiding procures the ready removal of the carbon disulphide, - but it is the carbon dioxide in the gas that is the disturbing element, inasmuch as it decomposes the combinations of sulphur and calcium; consequently it is a paramount object in this system to prevent this latter impurity finding its way through the first box of the series.
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  • The dinitroso acid slowly decomposes into sulphuretted hydrogen, nitrogen, nitrous oxide, and the heptanitroso acid.
    0
    0
  • The halogens give ferrous and ferric haloids and carbon monoxide; hydrochloric and hydrobromic acids have no action, but hydriodic decomposes it.
    0
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  • By reacting with a zinc alkyl (methyl or ethyl) on an acid chloride, an addition compound is first formed, which decomposes with water to give a ketone.
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  • Arsenic tribromide, AsBr3, is formed by the direct union of arsenic and bromine, and subsequent distillation from the excess of arsenic; it forms colourless deliquescent prisms which melt at 20 0 -25° C., and boil at 220° C. Water decomposes it, a small quantity of water leading to the formation of the oxybromide, AsOBr, whilst a large excess of water gives arsenious oxide, As4O6.
    0
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  • Arsenic trichloride, AsCl3, is prepared by distilling white arsenic with concentrated sulphuric acid and common salt, or by the direct union of arsenic with chlorine, or from the action of phosphorus pentachloride on white arsenic. It is a colourless oily heavy liquid of specific gravity 2.205 (o° C.), which, when pure and free from chlorine, solidifies at - 18°C., and boils at 132 °C. It is very poisonous and decomposes in moist air with evolution of white fumes.
    0
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  • Water decomposes it into arsenious oxide and ammonia, and when heated to 60° it loses ammonia and forms arsenimide, As2(NH)3 (C. Hugot, Compt.
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  • This substance dissolves slowly in water, forming arsenic acid; by heating to redness it decomposes into arsenic and oxygen.
    0
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  • When heated with alcohol to 190° C. it decomposes into mercury and ethyldisulphide.
    0
    0
  • Its tetrazo compound on reduction gives a hydrazine which, on warming with hydrochloric acid at 150° C., decomposes into ammonium N = N chloride and phenazone, - (C 12 H 8 N 2).
    0
    0
  • The felspar decomposes into kaolin and quartz; its alkalis are for the most part set free and removed in solution, but are partly retained in the white mica which is constantly found in crude china-clays.
    0
    0
  • On heating strongly, the white solid ammonium chloride, decomposes into a mixture of two colorless gases - ammonia and hydrogen chloride.
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  • Also the temperature range within which austenite decomposes to form ferrite and carbide on cooling.
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  • Bacillus amylobacter usually accompanies the lactic acid organism, and decomposes lactic and other higher acids with formation of butyric acid.
    0
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  • It dissolves readily in water and the aqueous solution decomposes on standing; a dark-brown flocculent precipitate of azulmic acid, C 4 H 5 N 5 0, separating whilst ammonium oxalate, urea and hydrocyanic acid are found in the solution.
    0
    0
  • decomposes them, with elimination of nitrogen and the formation of the corresponding acid, RCO�NH 2 +[[Onoh = R�Cooh]]+N2-f-H20.
    0
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  • It is insoluble in water and unaffected by most reagents, but when heated in a current of steam or boiled for some time with a caustic alkali, slowly decomposes with evolution of ammonia and the formation of boron trioxide or an alkaline borate; it dissolves slowly in hydrofluoric acid.
    0
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  • Borimide B 2 (NH) 3 is obtained on long heating of the compound B 2 S 3.6NH 3 in a stream of hydrogen, or ammonia gas at 115-120° C. It is a white solid which decomposes on heating into boron nitride and ammonia.
    0
    0
  • On fusion with solid potash at 250° C. it completely decomposes, giving potassium oxalate and hydrogen, C2H602-1-2KHO =K2C204+4H2.
    0
    0
  • It may be condensed and yields a solid which melts at - 55° C. Sulphuretted hydrogen decomposes it with formation of hydrofluoric acid and liberation of sulphur.
    0
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  • It is a colourless fuming liquid which boils at 152-153° C. When heated under pressure it decomposes, forming sulphuric acid, sulphuryl chloride, &c. (Ruff, Ber., 1901, 34, p. 35 0 9).
    0
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  • r 265 at 15° C., possessing a somewhat sweet taste; below o° C. it solidifies to a white crystalline mass, which melts at 17° C. When heated alone it partially volatilizes, but the greater part decomposes; under a pressure of 12 mm.
    0
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  • The acid melts at 132° C., and at a higher temperature it rapidly decomposes into acetic acid and carbon dioxide.
    0
    0
  • It melts at 70° C.and at higher temperatures decomposes, with evolution of carbon dioxide and formation of aceto-nitrile, CH 3 CN.
    0
    0
  • It forms a golden yellow crystalline mass, which sublimes slowly in vacuo, and melts at 25.5° C. It blackens on exposure to moisture, and decomposes when exposed to light.
    0
    0
  • The per-ruthenate, KRuO 4, formed by the action of chlorine on the ruthenate, or of alkalis on the peroxide at 50° C., is a black crystalline solid which is stable in dry air but decomposes when heated strongly.
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  • When nitric peroxide, N204, is converted into gas, it decomposes, and at about 180° C. its vapour entirely consists of molecules of the composition N02; while at temperatures between this and o C. it consists of a mixture in different proportions of the two kinds of molecules, N 2 O 4 and N02.
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  • It is a gas at ordinary temperature; when liquefied it boils at -63.5° C. and on solidification melts at -139° C. Water decomposes it into nitric and hydrofluoric acids.
    0
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  • Again, with the solution of a salt such as sodium chloride, the sodium, which is primarily liberated at the cathode, decomposes the water and evolves hydrogen, while the chlorine may be evolved as such, may dissolve the anode, or may liberate oxygen from the water, according to the nature of the plate and the concentration of the solution.
    0
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  • In the German Patent 1 57573 (1904) it is shown that by the action of at least two molecular proportions of an alkyl formate on two molecular proportions of a magnesium alkyl or aryl haloid, a complex addition compound is formed, which readily decomposes into a basic magnesium salt and an aldehyde, C H MgBr-f-H000R-RO�CH�C H.
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  • Nitromethane, CH 3 NO 2, is a colourless oil which boils at 101° C. Fuming sulphuric acid decomposes it into carbon monoxide and hydroxylamine.
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  • The silver salt, obtained by shaking an ether solution of nitroform with freshly prepared, slightly moist silver oxide, reacts with methyl iodide to form trinitroethane, a crystalline solid which melts at 56° C. Concentrated caustic potash decomposes the latter compound, forming the potassium salt of dinitroethane, CH3 C(N02)2K.
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  • The powdery metal when heated in air to 150° or 170° C. catches fire and burns brilliantly into U 3 0 8; it decomposes water slowly at ordinary temperatures, but rapidly when boiling.
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    0
  • It is a colourless liquid which boils at 210° C. Water decomposes it with the formation of silico-mesoxalic acid, HOOSi Si(OH) 2 SiOOH.
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    0
  • It is a colourless, strongly refracting liquid, which boils at about 220° C., slight decomposition setting in above 150° C. Water decomposes it with production of leucone.
    0
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  • It is readily decomposed by water: Si(NH 2) 4 +2H 2 O=4NH 3 +S10 2 Above o° C. it decomposes thus: Si(NH 2) 4 =2HN3-}-Si(NH)2.
    0
    0
  • OH, formed by the action of moist air on silicon octochloride at o° C., is very unstable, and hot water decomposes it with evolution of hydrogen and formation of silicic acid (L.
    0
    0
  • When it is heated to 120° C. with sodium ethylate it decomposes into ethyl ether and sodium ethyl carbonate (A.
    0
    0
  • With dry ammonia at 60° the metal forms strontium ammonium, which slowly decomposes in a vacuum at 20° giving Sr(NH 3) 2; with carbon monoxide it gives Sr(CO) 2; with oxygen it forms the monoxide and peroxide, and with nitric oxide it gives the hyponitrite (Roederer, Bull.
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  • It loses its water of crystallization at loo C., and begins to sublime at about 150160° C., whilst on heating to a still higher temperature it partially decomposes into carbon dioxide and formic acid, or into carbon dioxide, carbon monoxide and water; the latter decomposition being also brought about by heating oxalic acid with concentrated sulphuric acid.
    0
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  • It begins to decompose into gold and chlorine at 185°, the decomposition being complete at 230°; water decomposes it into gold and auric chloride.
    0
    0
  • It melts at 224° C. and is exceedingly hygroscopic. Water decomposes it with formation of tellurous acid and other products.
    0
    0
  • Calcium nitride, Ca 3 N 2, is a greyish-yellow powder formed by heating calcium in air or nitrogen; water decomposes it with evolution of ammonia (see H.
    0
    0
  • Water decomposes it with the evolution of spontaneously inflammable hydrogen phosphide; hence its use as a marine signal fire ("Holmes lights"), (see L.
    0
    0
  • At 200° C. this salt decomposes, giving off hydrofluoric acid, and between 230-250° C. fluorine is liberated.
    0
    0
  • When anhydrous it is a colourless opaque solid which melts at 310 °, and decomposes at about 110o°.
    0
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  • This salt is very deliquescent; it melts at 45°, and at 100° decomposes into iodine and potassium iodide.
    0
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  • When the dry salt is heated to 190° it decomposes into normal carbonate, carbon dioxide and water.
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  • It has been found, however, that molten cryolite and the analogous double fluoride represented by the formula Al 2 F 6.2NaF are very efficient solvents of alumina, and that these solutions can be easily electrolysed at about 800° C. by means of a current that completely decomposes the oxide but leaves the haloid salts unaffected.
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  • Aronheim, Ann., 1874, 171, p. 219); and by the action of ortho-xylylene bromide on sodium ethane tetracarboxylic ester, the resulting tetra-hydronaphthalene tetracarboxylic ester being hydrolysed and heated, when it yields hydronaphthalene dicarboxylic acid, the silver salt of which decomposes on distillation into naphthalene and other products (A.
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  • Nickel and manganese lower these critical points, so that with 25% of nickel Ar lies below the common temperature 20° C. With 13% of manganese Ar is very low, and the austenite decomposes so slowly that it is preserved practically intact by sudden cooling.
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  • It is a yellowish oil which melts at - 24° C.; it boils at 143-144° C., but cannot be distilled safely as it decomposes violently, giving nitrogen and ethyl fumarate.
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  • p. 543), as has also aluminium turnings moistened with potassium cyanide and mercuric chloride, which decomposes water regularly at 70°, i gram giving 1.3 litres of gas (Mauricheau-Beaupre, Comptes rendus, 1908, 147, p. 310).
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  • It melts at 720° and decomposes rapidly above 800°, giving oxygen and thallous oxide.
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  • Acetyl urea, NH 2 CO NH 000H 31 formed by the action of acetic anhydride on urea, crystallizes in needles which melt at 212° C. and, on heating, strongly decomposes into acetamide and cyanuric acid.
    0
    0
  • Hydrochloric acid at 200° C. decomposes into oxalic acid, carbon dioxide and methylamine, whilst an alcoholic solution of a caustic alkali gives dimethyl urea and oxalic acid.
    0
    0
  • Above 50° C. it decomposes into the dioxide and oxygen.
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    0
  • The excess of acid is removed by spreading the mass on a porous plate, the residue stirred for some hours with nitric acid, again spread on a porous plate, and finally dried quickly at about 130° C. It is a dark green deliquescent powder which decomposes on heating or on exposure to moist air.
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  • Water decomposes it, giving methane and hydrogen (H.
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    0
  • It decomposes when heated to 200° - 240°C.: 2KMn04=K2Mn04+Mn02+02; and when warmed with hydrochloric acid it yields chlorine: 2 KM nO 4 + 16HC1= 2KC1 +2 MnC1 2 +8H 2 0 +5C12.
    0
    0
  • By heating gallium in a regulated stream of chlorine the dichloride GaC1 2 is obtained as a crystalline mass, which melts at 164° C. and readily decomposes on exposure to moist air.
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  • 18 95, p. 945) has obtained metallic nickel from the Canadian mattes by first roasting them and then eliminating copper by the action of sulphuric acid, the product so obtained being then exposed to the reducing action of producer gas at about 350° C. The reduced metal is then passed into a "volatilizer" and exposed to the action of carbon monoxide at about 80° C., the nickel carbonyl so formed being received in a chamber heated to 180-200° C., where it decomposes, the nickel being deposited and the carbon monoxide returned to the volatilizer.
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    0
  • On the addition of iodine to this oxide, chlorine is liberated and a white substance is produced, which decomposes, on heating to 380° C., into iodine and oxygen; bromine is without action (see A.
    0
    0
  • The crystalline hydrate melts at 50° C. The pure acid decomposes slowly on standing, but is stable in dilute aqueous solution.
    0
    0
  • When moist, it decomposes at about 6° C., but the dry substance must be heated to about 180°, before decomposition sets in (see L.
    0
    0
  • It is easily soluble in water and decomposes when heated to zoo° C.
    0
    0
  • It decomposes when heated above 35° C., and also in the presence of water.
    0
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  • It forms a colourless syrup, of specific gravity 1.2485 (1 5°/4°), and decomposes on distillation under ordinary atmospheric pressure; but at very low pressures (about i mm.) it distils at about 85° C., and then sets to a crystalline solid, which melts at about 18° C. It possesses the properties both of an acid and of an alcohol.
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  • Deliquescent, rectangular tablets of H 4 P 2062H 2 O separate out on concentrating a solution in a vacuum, which on drying further give the acid, which melts at 55°, and decomposes suddenly when heated to 70° into phosphorous and metaphosphoric acids with a certain amount of hydrogen phosphide.
    0
    0
  • The bromochloride, PC1 3 Br 21 is an orange-coloured solid formed from bromine and the trichloride, into which components it decomposes at 35°.
    0
    0
  • The diamide, PN 2 H 4, was obtained by Hugot (ibid., 1905, 141, p. 1235) by acting with ammonia gas on phosphorus tribromide or tri-iodide at -70 0; it is very unstable, and decomposes at -25°.
    0
    0
  • With bromine it forms a dibromide, which then heated to 110° C. decomposes into hydrobromic acid and benzyl bromide.
    0
    0
  • Arsenic tribromide, AsBr3, is formed by the direct union of arsenic and bromine, and subsequent distillation from the excess of arsenic; it forms colourless deliquescent prisms which melt at 20 0 -25° C., and boil at 220° C. Water decomposes it, a small quantity of water leading to the formation of the oxybromide, AsOBr, whilst a large excess of water gives arsenious oxide, As4O6.
    0
    0
  • Arsenic trichloride, AsCl3, is prepared by distilling white arsenic with concentrated sulphuric acid and common salt, or by the direct union of arsenic with chlorine, or from the action of phosphorus pentachloride on white arsenic. It is a colourless oily heavy liquid of specific gravity 2.205 (o° C.), which, when pure and free from chlorine, solidifies at - 18°C., and boils at 132 °C. It is very poisonous and decomposes in moist air with evolution of white fumes.
    0
    0
  • Water decomposes it into arsenious oxide and ammonia, and when heated to 60° it loses ammonia and forms arsenimide, As2(NH)3 (C. Hugot, Compt.
    0
    0
  • When heated with alcohol to 190° C. it decomposes into mercury and ethyldisulphide.
    0
    0
  • Jour., 1904, 3 2, p. 503) show that if metallic potassium be added to an ethereal solution of the blue compound at -20° C., hydrogen is liberated and a purple black precipitate of the perchromate, of composition KCrO 4 or K2Cr203, is produced; this compound is very unstable, and readily decomposes into oxygen and potassium bichromate.
    0
    0
  • Its tetrazo compound on reduction gives a hydrazine which, on warming with hydrochloric acid at 150° C., decomposes into ammonium N = N chloride and phenazone, - (C 12 H 8 N 2).
    0
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  • The historian evidently decomposes Alexander's power into the components: Talleyrand, Chateaubriand, and the rest--but the sum of the components, that is, the interactions of Chateaubriand, Talleyrand, Madame de Stael, and the others, evidently does not equal the resultant, namely the phenomenon of millions of Frenchmen submitting to the Bourbons.
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  • Bark, chips and cocoa hull mulch also breaks down or decomposes over time, adding nutrients to the soil.
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  • Although rubber mulch may go through many treatment processes to remove any residues, many people aren't convinced that the rubber itself won't poison the earth in which it decomposes.
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  • This enzyme decomposes organic matter and uses it as food.
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    0
  • It is a bluish-black powder which at high temperatures decomposes into the metal, dioxide and oxygen.
    0
    1
  • It decomposes steam at a red heat, and slowly dissolves in dilute hydrochloric and sulphuric acids, but more readily in nitric acid.
    0
    1
  • Hot concentrated sulphuric acid also decomposes allantoin, with production of ammonia, and carbon monoxide and dioxide.
    0
    1
  • This body is being continually formed in the yeast cell, and decomposes the sugar which has diffused into the cell.
    0
    1
  • The Bacterium acidi lacti described by Pasteur decomposes milk sugar into lactic acid.
    0
    1
  • It reduces many metallic oxides, such as lead monoxide and cupric oxide, and decomposes water at a red heat.
    0
    1
  • A saturated solution of the gas, in water, is a colourless, oily, strongly fuming liquid which after a time decomposes, with separation of metaboric acid, leaving hydrofluoboric acid HF BF3 in solution.
    0
    1
  • Borimide B 2 (NH) 3 is obtained on long heating of the compound B 2 S 3.6NH 3 in a stream of hydrogen, or ammonia gas at 115-120° C. It is a white solid which decomposes on heating into boron nitride and ammonia.
    0
    1
  • It is a colourless fuming liquid which boils at 152-153° C. When heated under pressure it decomposes, forming sulphuric acid, sulphuryl chloride, &c. (Ruff, Ber., 1901, 34, p. 35 0 9).
    0
    1
  • The salts are unstable; and a solution of the free acid (obtained by the addition of hydrofluosilicic acid to the potassium salt) on concentration in vacuo decomposes rapidly: H 2 S 3 0 6 = H 2 SO 4 -{- S S02.
    0
    1
  • r 265 at 15° C., possessing a somewhat sweet taste; below o° C. it solidifies to a white crystalline mass, which melts at 17° C. When heated alone it partially volatilizes, but the greater part decomposes; under a pressure of 12 mm.
    0
    1