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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 ...
NH4NO3. Add languages. ... Download as PDF; Printable version; ... Ammonium nitrate; From a chemical formula: This is a redirect from a chemical/molecular formula to ...
Ammonium nitrate decomposes in temperatures above 169 °C (336 °F). Pure AN is stable and will stop decomposing once the heat source is removed, but when catalysts are present, the reaction can become self-sustaining (known as self-sustaining decomposition, or SSD).
Enthalpy is the transfer of energy in a reaction (for chemical reactions, it is in the form of heat) and is the change in enthalpy. Δ H {\displaystyle \Delta H} is a state function, meaning that Δ H {\displaystyle \Delta H} is independent of processes occurring between initial and final states.
Ammonium nitrite is a chemical compound with the chemical formula [NH 4]NO 2. It is the ammonium salt of nitrous acid. It is composed of ammonium cations [NH 4] + and nitrite anions NO − 2. It is not used in pure isolated form since it is highly unstable and decomposes into water and nitrogen, even at room temperature.
The chemistry of ANFO detonation is the reaction of ammonium nitrate with a long-chain alkane (C n H 2n+2) to form nitrogen, carbon dioxide, and water.In an ideal stoichiometrically balanced reaction, ANFO is composed of about 94.5% AN and 5.5% FO by weight.
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In thermochemistry, the heat of dilution, or enthalpy of dilution, refers to the enthalpy change associated with the dilution process of a component in a solution at a constant pressure. If the initial state of the component is a pure liquid (presuming the solution is liquid), the dilution process is equal to its dissolution process and the ...