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This reaction may give rise to some non-negligible variations in the vapor pressure above the liquid because the nitrogen oxides produced dissolve partly or completely in the acid. The nitrogen dioxide (NO 2) and/or dinitrogen tetroxide (N 2 O 4) remains dissolved in the nitric acid coloring it yellow or even red at higher temperatures. While ...
Hydrated copper nitrate is prepared by treating copper metal or its oxide with nitric acid: [7] Cu + 4 HNO 3 → Cu(NO 3) 2 + 2 H 2 O + 2 NO 2. The same salts can be prepared treating copper metal with an aqueous solution of silver nitrate. That reaction illustrates the ability of copper metal to reduce silver ions.
The recovery and reuse of oxides of nitrogen was an important economic consideration in the operation of a chamber process plant. In the reaction chambers, nitric oxide reacts with oxygen to produce nitrogen dioxide. Liquid from the bottom of the chambers is diluted and pumped to the top of the chamber, and sprayed downward in a fine mist.
The redox reaction of nitrosonium and the metal can give rise to nitrogen oxide which forms strong metal nitrosyl complexes; nitronium ions (NO 2 +) are similarly observed. [16] In some cases, nitrate complexes are produced from the reaction of nitrogen dioxide with a metal dioxygen complex: [17]
The Haber process, [1] also called the Haber–Bosch process, is the main industrial procedure for the production of ammonia. [2] [3] It converts atmospheric nitrogen (N 2) to ammonia (NH 3) by a reaction with hydrogen (H 2) using finely divided iron metal as a catalyst:
A typical reaction with silver nitrate is to suspend a rod of copper in a solution of silver nitrate and leave it for a few hours. The silver nitrate reacts with copper to form hairlike crystals of silver metal and a blue solution of copper nitrate: 2 AgNO 3 + Cu → Cu(NO 3) 2 + 2 Ag. Silver nitrate decomposes when heated:
It is produced commercially by reaction of metallic lead with concentrated nitric acid in which it is sparingly soluble. [ 6 ] [ 7 ] It has been produced as a raw material for making pigments such as chrome yellow (lead(II) chromate, PbCrO 4 ) and chrome orange (basic lead(II) chromate, Pb 2 CrO 5 ) and Naples yellow .
It is a multi-step nitrogen fixation reaction that uses electrical arcs to react atmospheric nitrogen (N 2) with oxygen (O 2), ultimately producing nitric acid (HNO 3) with water. [1] The resultant nitric acid was then used as a source of nitrate (NO 3 − ) in the reaction HNO 3 + H 2 O H 3 O + + NO 3 − {\textstyle {\ce {HNO3 + H2O -> H3O ...