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As ammonium nitrate is a salt, both the cation, NH + 4, and the anion, NO − 3, may take part in chemical reactions. Solid ammonium nitrate decomposes on heating. At temperatures below around 300 °C, the decomposition mainly produces nitrous oxide and water: NH 4 NO 3 → N 2 O + 2 H 2 O. At higher temperatures, the following reaction ...
Fritz Haber, 1918. 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:
HNO 3 + 2 H 2 SO 4 ⇌ [NO 2] + + [H 3 O] + + 2 HSO − 4; Equilibrium constant: K ≈ 22. The nitronium ion, [NO 2] +, is the active reagent in aromatic nitration reactions. Since nitric acid has both acidic and basic properties, it can undergo an autoprotolysis reaction, similar to the self-ionization of water: 2 HNO 3 ⇌ [NO 2] + + NO − 3 ...
Nitric acid (HNO 3) is an acid because it donates a proton to the water molecule and its conjugate base is nitrate (NO − 3). The water molecule acts as a base because it receives the hydrogen cation (proton) and its conjugate acid is the hydronium ion (H 3 O +).
Nitrous oxide (N 2 O), better known as laughing gas, is made by thermal decomposition of molten ammonium nitrate at 250 °C. This is a redox reaction and thus nitric oxide and nitrogen are also produced as byproducts. It is mostly used as a propellant and aerating agent for sprayed canned whipped cream, and was formerly commonly used as an ...
The Ostwald process begins with burning ammonia.Ammonia burns in oxygen at temperature about 900 °C (1,650 °F) and pressure up to 8 standard atmospheres (810 kPa) [4] in the presence of a catalyst such as platinum gauze, alloyed with 10% rhodium to increase its strength and nitric oxide yield, platinum metal on fused silica wool, copper or nickel to form nitric oxide (nitrogen(II) oxide) and ...
The reaction is consistent with the Brønsted–Lowry definition because in reality the hydrogen ion exists as the hydronium ion, so that the neutralization reaction may be written as H 3 O + + OH − → H 2 O + H 2 O. When a strong acid is neutralized by a strong base there are no excess hydrogen ions left in the solution.
The ammonium nitrate making process is a neutralisation process consisting of a reaction between ammonia and nitric acid. Ammonia is vaporised and then sparged through a proportionate amount of nitric acid to make an 83% wt/wt ammonium nitrate solution. The solution is concentrated to a 99% melt by vaporising water using two evaporators in ...