![]() Iron (Fe) reacts with nitric acid (HNO 3) to produce iron nitrate (Fe(NO 3) 3), nitrogen monoxide (NO), and water (H 2O). The balanced chemical equation for this reaction is: This reaction gives off heat, making it an exothermic process. Iron nitrate is produced industrially through a reaction involving iron, nitric acid, and water. Molar mass: 404.0 g/mol (for nonahydrate) ![]() It has a melting point of 47.2 degrees Celsius and decomposes when heated above 125 degrees Celsius. The molar mass of iron nitrate nonahydrate is approximately 404.0 g/mol, and it possesses a density of about 1.68 g/cm 3. On exposure to high temperatures, it decomposes into nitrogen dioxide, oxygen, and iron oxide. ![]() Iron nitrate nonahydrate is highly soluble in water and ethanol. It’s a deliquescent solid, meaning it can absorb moisture from the air and dissolve in it, turning into a liquid. Iron nitrate is characterized by its bright violet color in the nonahydrate form. This versatile compound boasts various applications spanning multiple industries, including pharmaceutical, manufacturing, and even art. ![]() It primarily exists in two forms: nonahydrate (9 molecules of water) and nona- and hexa-hydrate. Iron nitrate, chemically denoted as Fe(NO 3) 3, is an inorganic compound and a key member of the nitrate family of chemicals. Explore the chemical compound iron nitrate, its properties, production, applications, safety measures, and environmental impact. ![]()
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