Copper nitrate nitration with

The intermediate precipitate obtained by the reaction of copper nitrate with ammonium dichromate and ammonia has been shown to be Cu(0H)NH4Cr04,122 and the decomposition of the precipitate to give the catalyst to be formulated as in eq. 1.6, by an X-ray diffraction study by Stroupe, although the catalysts obtained by decomposition at sufficiently controlled low temperature (350°C) are amorphous.123 Catalysts previosly used in liquid-phase hydrogenation below 300°C often show crystalline cupric chromite to have been largely reduced to the cuprous chromite... 

The paper discusses two types of reaction involving metal complexes, and it is postulated that each proceeds by an initial free-radical step. In reactions between metal carbonyls and N2O4—NO2 mixtures, the nature of the product depends upon the phase in which the reaction is carried out. In the liquid phase, where the predominant equilibrium is N204 N0+ + NO3-, metal nitrates or carbonyl nitrates are formed in the gas phase, where the equilibrium is N2O4 2NO2/ nitrites or their derivatives are produced. Reactions of Mn2(CO) o Fe(CO)5, Co2(CO)3, and Ni(CO)4 are discussed. Anhydrous metal nitrates in which the nitrate group is covalently bonded to the metal have enhanced reactivity. This is believed to result from the dissociation M—O—N02 M—O + NO2 This can explain the solution properties of beryllium nitrates, and the vigorous (even explosive) reaction of anhydrous copper nitrate with diethyl ether. 

Reaction of Copper Nitrate with Dimethyl Ether. In sharp contrast to the behavior of diethyl ether, dimethyl ether shows little reactivity with copper nitrate. Dimethyl ether was condensed onto copper nitrate at —70° C. on warming to —20° C. ether evaporated to leave a pale blue solid which melted to a green oil at —12°. This oil was stable up to 50° C., and analysis showed it to be a molecular addition compound, Cu(N03)2.1.5 Me20 on treatment with water the dimethyl ether was evolved. Some decomposition of the addition compound does occur on long standing under vacuum (16),... 

Fe-Cu-Na catalysts were prepared by coprecipitation from the iron and copper nitrates with sodium hydroxide. Sodium contents were controlled by washing the precipitates. The composite catalysts were obtained by physical mixing of equal amounts of Fe-Cu-Na oxides and zeolites. After reducing the samples in a flow of 10% H2/N2 for 6 h at 350°C, the catalysts were kept at 250°C in a flow of reaction gas under 20 atm. The reactants and products were analyzed with an online gas chromatograph system. The XRD powder patterns of the catalysts before and after the reaction were obtained with C xKa radiation at 40 kV and 30 mA on a RIGAKU X-ray diffractometer. 

The most important cyclic phosphate is tetrametaphosphate, which can be prepared by heating copper nitrate with slightly more than an equimolar amount of phosphoric acid (75%) slowly to 400°. The sodium salt can be obtained by treating a solution of the copper salt with Na2S. Slow addition of P4O10 to ice water gives 75% of the P as tetrametaphosphate. 

Recently, Han and co-workers reported a modification of a classical synthesis of 3,6-disubstituted-l,2,4,5-tetrazines 1 from nitriles using an activated catalyst prepared from copper nitrate with excess zinc in the presence of hydrazine monohydrate. It is noteworthy that the corresponding 1,2-dihydrotetrazines 2 were formed as the primary products, which were then air-oxidized during workup to give the fully unsaturated compounds 1 in 20-90% yields (Scheme 10) <1995BKC374>. 

Field (1835) stated that olive lake (. v.) was prepared from ebony. However, Riffault et al. (1874) describe how ebony black was obtained from burning copper nitrate with peat. 

Mercuric halides, silver nitrate, and copper nitrates form stable complexes with bis-2.2 -thiazolylazo compounds (1591). for which the X-ray structure is not yet known. 

Hydrogen cyanide is a reactant in the production of acrylonitrile, methyl methacrylates (from acetone), adiponitrile, and sodium cyanide. It is also used to make oxamide, a long-lived fertilizer that releases nitrogen steadily over the vegetation period. Oxamide is produced by the reaction of hydrogen cyanide with water and oxygen using a copper nitrate catalyst at about 70°C and atmospheric pressure ... 

As a third oxidation-reduction example, suppose a strip of metallic zinc is placed in a solution of copper nitrate, Cu(N03)j. The strip becomes coated with reddish metallic copper and the bluish color of the solution disappears. The presence of zinc ion, Zn+2, among the products can be shown when the Cu+2 color is gone. Then if hydrogen sulfide gas is passed into the mixture, white zinc sulfide, ZnS, can be seen. The reaction between metallic zinc and the aqueous copper nitrate is... 

These reactions can be viewed as a competition between two kinds of atoms (or molecules) for electrons. Equilibrium is attained when this competition reaches a balance between opposing reactions. In the case of reaction (3), copper metal reacting with silver nitrate solution, the Cu(s) releases electrons and Ag+ accepts them so readily that equilibrium greatly favors the products, Cu+2 and Ag(s). Since randomness tends to favor neither reactants nor products, the equilibrium must favor products because the energy is lowered as the electrons are transferred. If we regard reaction (5) as a competition between silver and copper for electrons, stability favors silver over copper. 

Synthetic standard solution (for analysis of steel). Dissolve an appropriate weight of pure iron (Johnson Matthey) in a mixture of equal volumes of concentrated hydrochloric acid and concentrated nitric acid with this solution as base, add a suitable amount of copper nitrate solution containing 0.01 g copper per L. 

Attempts to brominate cyclopent[/>]azepine (10) with bromine failed, as did nitration with copper(II) nitrate in acetic anhydride 2 however, with one equivalent of A -bromosuccinimide in acetic acid a separable mixture of the unstable 8-bromo 11 and 6-bromo 12 derivatives, along with the stable 6,8-dibromo derivative 13, is formed. An excess of brominating agent yields the dibromo compound as the sole product. 

Copper nitrate reacts with sodamide and ammonia by forming explosive copper amides. The oxidising properties of this nitrate have led to violent detonations with ammonium hexacyanoferrates heated to 220 C in the presence of water traces, or dry at the same temperature, but in the presence of an excess of hexacyanoferrate. These accidents illustrate once more the incompatibility between compounds with a cyano group (or cyanide anion) and oxidants. An accident also occurred with a potassium hexacyanoferrate. 

Use of mixtures of metal nitrates with acetic anhydride as a nitrating agent may be hazardous, depending on the proportions of reactants and on the cation copper nitrate or sodium nitrate usually cause violent reactions [ 1], An improved procedure for the use of the anhydride-copper(II) nitration mixture [2] has been further modified [3] to improve safety aspects. 

Boron phosphide ignites in molten nitrates mixtures of the nitrate with copper(II) phosphide explode on heating, and that with copper monophosphide explodes on impact. 

Mixtures of the nitrate with powdered aluminium or its oxide (the latter seems unlikely) were reported to be explosive [1], and the performance characteristics of flares containing compressed mixtures of the metal and nitrate have been evaluated [2]. A violent explosion in a copper smelting works was caused mainly by reaction of aluminium with sodium nitrate [3],... 

FIGURE 6.11 Diagram of the processing technique used to prepare Cu-Ce02-YSZ anodes for direct oxidation of hydrocarbon fuels by preparing a porous preform of YSZ and then infiltrating it with cerium nitrates to form ceria and then with copper nitrates to form metallic copper [84]. Reprinted from [84] with permission from Elsevier. 

Mercuric oxide (5 g.) is dissolved for the most part in a still warm mixture of 110 c.c. of water and 50 c.c. of concentrated sulphuric acid. The mixture is brought into a large hydrogenation flask (Fig. 58, p. 377) and shaken for some time with acetylene prepared from calcium carbide, purified with acid solutions of dichromate and copper nitrate, and collected over saturated sodium chloride solution in a glass gas-holder (capacity 10-15 litres). Before shaking is begun the air present must be displaced by the hydrocarbon. 

Using Resources Use resources such as the CRC Handbook of Chemistry and Physics, the Merck Index, or the Internet to determine the colors of silver metal and copper nitrate in water. Compare this information with your observations of the reactants and products in step 6. 

Peng, Y. and Q. Chen, Fabrication of copper/multi-walled carbon nanotube hybrid nanowires using electroless copper deposition activated with silver nitrate. Journal of The Electrochemical Society, 2012.159(2) p. D72-D76. 

The first three components suggest regional sources of acidic anthropogenic aerosol, the marker elements of a copper smelter, and seasalt, respectively. The fourth component or the ammonium In component three do not provide a ready Interpretation of a known emission or meteorological source of variability. The negative correlation of nitrate with component two Is consistent with separate Influences of the copper smelter and automobile emissions. 

Benzaldehyde. There are many ways to make many types of benzaldehydes. Different benzal-dehydes give different products. I am giving the formula to the basic type. It can be modified to give a specific type of benzaldehyde. 50 g of benzyl chloride and 50 g of copper nitrate in 300 cc of water are refluxed together, in a current of carbon dioxide for 8Vi hours or until a sample tested contains very little chlorine. Extract the mixture with ether, remove the ether on a water bath, and stir or shake the remaining oil for 1 hour (shaking is best) with a saturated solution of sodium bisulfite. Let stand for 2 hours, filter with vacuo and wash with a little cold alcohol, then with cold ether. The washings are warmed with an excess of 10% sulfuric acid. The aldehyde... 

The efficient At-nitration of secondary amines has been achieved by transfer nitration with 4-chloro-5-methoxy-2-nitropyridazin-3-one, a reagent prepared from the nitration of the parent 4-chloro-5-methoxypyridazin-3-one with copper nitrate trihydrate in acetic anhydride. Reactions have been conducted in methylene chloride, ethyl acetate, acetonitrile and diethyl ether where yields of secondary nitramine are generally high. Homopiperazine is selectively nitrated to At-nitrohomopiperazine or At, At -dinitrohomopiperazine depending on the reaction stoichiometry. At-Nitration of primary amines or aromatic secondary amines is not achievable with this reagent. 

Nitrotetrazole is readily prepared from the diazotization of 5-aminotetrazole in the presence of excess sodium nitrite and is best isolated as the copper salt complex with ethylenediamine. The salts of 5-nitrotetrazole have attracted interest for their initiating properties. The mercury salt is a detonating primary explosive. The amine salts of 5-nitrotetrazole are reported to form useful eutectics with ammonium nitrate. ... 

Catalysts suitable specifically for reduction of carbon-oxygen bonds are based on oxides of copper, zinc and chromium Adkins catalysts). The so-called copper chromite (which is not necessarily a stoichiometric compound) is prepared by thermal decomposition of ammonium chromate and copper nitrate [50]. Its activity and stability is improved if barium nitrate is added before the thermal decomposition [57]. Similarly prepared zinc chromite is suitable for reductions of unsaturated acids and esters to unsaturated alcohols [52]. These catalysts are used specifically for reduction of carbonyl- and carboxyl-containing compounds to alcohols. Aldehydes and ketones are reduced at 150-200° and 100-150 atm, whereas esters and acids require temperatures up to 300° and pressures up to 350 atm. Because such conditions require special equipment and because all reductions achievable with copper chromite catalysts can be accomplished by hydrides and complex hydrides the use of Adkins catalyst in the laboratory is very limited. 

Copper(ll) nitrate is made by action of copper or copper(II) oxide with nitric acid. The solution is evaporated and the product is obtained by crystallization... 

Copper oxide reacts with dilute sulfuric and nitric acids forming copper(II) sulfate and copper(II) nitrate, respectively, and precipitating metallic copper ... 

When heated with nitric acid, copper(l) sulfide decomposes forming copper nitrate and hydrogen sulfide. The compound dissolves in aqueous solutions containing cyanide ions forming soluble copper-cyanide complexes. 

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