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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 ...
The calcium nitrate mentioned before, can as said be worked up as calcium nitrate fertilizer but often it is converted into ammonium nitrate and calcium carbonate using carbon dioxide and ammonia. Ca ( NO 3 ) 2 + 2 NH 3 + CO 2 + H 2 O 2 NH 4 NO 3 + CaCO 3 {\displaystyle {\ce {Ca(NO3)2 + 2 NH3 + CO2 + H2O -> 2 NH4NO3 + CaCO3}}}
Dissolving ammonium nitrate in water is endothermic. The energy released by the solvation of the ammonium ions and nitrate ions is less than the energy absorbed in breaking up the ammonium nitrate ionic lattice and the attractions between water molecules.
For many substances, the formation reaction may be considered as the sum of a number of simpler reactions, either real or fictitious. The enthalpy of reaction can then be analyzed by applying Hess' law, which states that the sum of the enthalpy changes for a number of individual reaction steps equals the enthalpy change of the overall reaction.
Triammonium phosphate can be prepared in the laboratory by treating 85% phosphoric acid with 30% ammonia solution: [citation needed] H 3 PO 4 + 3 NH 3 → (NH 4) 3 PO 4 (NH 4) 3 PO 4 is a colorless, crystalline solid. The solid, which has the odor of ammonia, is readily soluble in water. The salt converts to diammonium hydrogen phosphate (NH 4 ...
The following chart shows the solubility of various ionic compounds in water at 1 atm pressure and room temperature (approx. 25 °C, 298.15 K). "Soluble" means the ionic compound doesn't precipitate, while "slightly soluble" and "insoluble" mean that a solid will precipitate; "slightly soluble" compounds like calcium sulfate may require heat to precipitate.
The decomposition of ammonium nitrate is also a common laboratory method for preparing the gas. Equivalently, it can be obtained by heating a mixture of sodium nitrate and ammonium sulfate: [53] 2 NaNO 3 + (NH 4) 2 SO 4 → Na 2 SO 4 + 2 N 2 O + 4 H 2 O. Another method involves the reaction of urea, nitric acid and sulfuric acid: [54]
The procedure involves first preparing a platinum nitrate which is then heated to expel nitrogen oxides. [3] H 2 PtCl 6 + 6 NaNO 3 → Pt(NO 3) 4 + 6 NaCl (aq) + 2 HNO 3 Pt(NO 3) 4 → PtO 2 + 4 NO 2 + O 2. The resulting brown cake is washed with water to free it from nitrates. The catalyst can either be used as is or dried and stored in a ...