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Copper nitrate, in combination with acetic anhydride, is an effective reagent for nitration of aromatic compounds, known as the Menke nitration. [17] Hydrated copper nitrate adsorbed onto clay affords a reagent called "Claycop". The resulting blue-colored clay is used as a slurry, for example for the oxidation of thiols to disulfides.
The reaction is usually endothermic as heat is required to break chemical bonds in the compound undergoing decomposition. If decomposition is sufficiently exothermic, a positive feedback loop is created producing thermal runaway and possibly an explosion or other chemical reaction. Thermal decomposition is a chemical reaction where heat is a ...
Thus copper(II) nitrate readily dissociates in aqueous solution to give the aqua complex: Cu(NO 3) 2 + 6 H 2 O → [Cu(H 2 O) 6](NO 3) 2. Pyrolysis of metal nitrates yields oxides. [18] Ni(NO 3) 2 → NiO + NO 2 + 0.5 O 2. This reaction is used to impregnate oxide supports with nickel oxides. Nitrate reductase enzymes convert nitrate to
The resulting acid solution is the 68.5% azeotrope, and can be further concentrated (as in industry) with either sulfuric acid or magnesium nitrate. [36] Alternatively, thermal decomposition of copper(II) nitrate gives nitrogen dioxide and oxygen gases; these are then passed through water or hydrogen peroxide [38] as in the Ostwald process:
Oxygen likely affects denitrification in multiple ways—because most denitrifiers are facultative, oxygen can inhibit rates, but it can also stimulate denitrification by facilitating nitrification and the production of nitrate. In wetlands as well as deserts, [21] moisture is an environmental limitation to rates of denitrification.
For example, the thermal decomposition of some metal nitrates generates NO 2: [14] Pb(NO 3) 2 → PbO + 2 NO 2 + 1 ⁄ 2 O 2. Alternatively, dehydration of nitric acid produces nitronium nitrate... 2 HNO 3 → N 2 O 5 + H 2 O 6 HNO 3 + 1 ⁄ 2 P 4 O 10 → 3 N 2 O 5 + 2 H 3 PO 4...which subsequently undergoes thermal decomposition: N 2 O 5 → ...
It can be formed by heating copper in air at around 300–800 °C: 2 Cu + O 2 → 2 CuO. For laboratory uses, copper(II) oxide is conveniently prepared by pyrolysis of copper(II) nitrate or basic copper(II) carbonate: [4] 2 Cu(NO 3) 2 → 2 CuO + 4 NO 2 + O 2 (180°C) Cu 2 (OH) 2 CO 3 → 2 CuO + CO 2 + H 2 O. Dehydration of cupric hydroxide ...
In this type of decomposition reaction, a metal chloride and oxygen gas are the products. Here, again, M represents the metal: 2 MClO 3 → 2 MCl+ 3 O 2. A common decomposition of a chlorate is in the reaction of potassium chlorate where oxygen is the product. This can be written as: 2 KClO 3 → 2 KCl + 3 O 2