High Temperature Properties and Decomposition of Inorganic Salts Part 3, Nitrates and Nitrites

Stern, Kurt H.

doi:10.1063/1.3253104

Cited by 266 publications

(110 citation statements)

References 38 publications

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“…In agreement with published literature [39][40] , it was found that the decomposition does not occur at standard conditions because the reaction requires a Gibbs free energy (G) of 71.9…”

Section: Decomposition Of Pure Nano2supporting

confidence: 75%

Theoretical and Experimental Study of the Reaction between Ammonium Nitrate and Sodium Salts

Cagnina

Rotureau

Singh

et al. 2016

Ind. Eng. Chem. Res.

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Hazards posed by chemical incompatibility, especially in a large-scale industrial environment, warrant a deeper understanding of the mechanisms of the reactions involved in these phenomena. In this study, reactions between ammonium nitrate and two sodium salts, namely, sodium nitrate and sodium nitrite, have been studied by ab initio calculations (with density functional theory, DFT) and experimental calorimetric methods (with differential scanning calorimetry, DSC, and heat flux calorimetry, HFC). The agreement between theoretical and experimental results allows an understanding of the thermal decomposition behaviors of the two sodium salts when exposed to ammonium nitrate. Moreover, this study highlighted the critical role of the water that appears to promote the incompatibility between ammonium nitrate and sodium nitrite.

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Section: Decomposition Of Pure Nano2supporting

confidence: 75%

Theoretical and Experimental Study of the Reaction between Ammonium Nitrate and Sodium Salts

Cagnina

Rotureau

Singh

et al. 2016

Ind. Eng. Chem. Res.

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“…In contrast, nitrate has a better affinity for lithium and decomposes at a higher temperature [37,38]. Thus, we can assume that the higher concentration of lithium in the mesopores and the elevated temperature at the start of the metathesis reaction favourably induced the formation of a surface seed crystals (heterogeneous crystallisation), which grew during the second stage of the stabilisation at 500°C for 5 h. This implies that the surface area and pore volume had a direct impact on the formation of this seed crystal, which could explain why higher water content accelerated crystallisation.…”

Section: Crystallisation Behaviour Upon Thermal Stabilisationmentioning

confidence: 99%

Lithium-silicate sol–gel bioactive glass and the effect of lithium precursor on structure–property relationships

Maçon

Jacquemin

Page

et al. 2016

J Sol-Gel Sci Technol

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This work reports the synthesis of lithium-silicate glass, containing 10 mol% of Li 2 O by the sol-gel process, intended for the regeneration of cartilage. Lithium citrate and lithium nitrate were selected as lithium precursors. The effects of the lithium precursor on the sol-gel process, and the resulting glass structure, morphology, dissolution behaviour, chondrocyte viability and proliferation, were investigated. When lithium citrate was used, mesoporous glass containing lithium as a network modifier was obtained, whereas the use of lithium nitrate produced relatively dense glass-ceramic with the presence of lithium metasilicate, as shown by X-ray diffraction, 29 Si and 7 Li MAS NMR and nitrogen sorption data. Nitrate has a better affinity for lithium than citrate, leading to heterogeneous crystallisation from the mesopores, where lithium salts precipitated during drying. Citrate decomposed at a lower temperature, where the crystallisation of lithium-silicate crystal is not thermodynamically favourable. Upon decomposition of the citrate, a solid-state salt metathesis reaction between citrate and silanol occurred, followed by the diffusion of lithium within the structure of the glass. Both glass and glass-ceramic released silica and lithium ions in culture media, but release rate was lower for the glass-ceramic. Both samples did not affect chondrocyte viability and proliferation.Graphical Abstract

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“…No solid transitions are reported. It begins to decompose at about 600 K to give N 3 0 , NO, and NO, (Stern 1972). NO reoxidizes the nitrite to nitrate, producing N2.…”

Section: Thermal Data For Compoundsmentioning

confidence: 99%

Calculation of reaction energies and adiabatic temperatures for waste tank reactions

Burger¹

1993

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SummaryContinual concern has been expressed over potentially hazardous exothermic reactions that might occur in Hanford Site underground waste storage tanks. These tanks contain many different oxidizable compounds covering a wide range of concentrations. Several compounds may be in concentrations and quantities great enough to be considered a hazard in that they could undergo rapid and energetic chemical reactions with nitrate and nitrite salts that are present it heated to the initiating or critical temperature. The chemical hazards are a function of several interrelated factors, including the amount of energy (heat) produced, how fast it is produced, and the thermal absorption and heat transfer properties of the system. The reaction path(s) will determine the amount of energy produced and kinetics will determine the rate that it is produced. The tanks also contain many inorganic compounds inert to oxidation. These compounds act as diluents and can inhibit exothermic reactions because of their heat capacity and thus, in contrast to the oxidizable compounds, provide mitigation of hazardous reactions.In this report the energy that may be released when various organic and inorganic compounds react is computed as a function of the reaction-mix composition and the temperature. The enthalpy, or integrated heat capacity, of these compounds and various reaction products is presented as a function of temperature; the enthalpy of a given mixture can then be equated to the energy release from various reactions to predict the maximum temperature which may be reached. This is estimated for several different compositions. Alternatively, the amounts of various diluents required to prevent the temperature from reaching a critical value can be estimated. Reactions W i g different paths, forming different products such as N20 in place of N2 are also considered, as are reactions where an excess of caustic is present. Oxidants other than nitrate and nitrite are considered briefly.The relative available energy per unit mass of the various oxidizable compounds, or "fuels," that may be present ranges from 1 to about 25. Stoichiometric mixes with oxidant, e.g., fuel plus the required amount of sodium nitrate (NaNO,) for a complete reaction, compared on a mass basis, also show large differences. This "energy density" covers a range of 1 to about 5.A consequence of different stoichiometries for different fuels is that an excess of sodium nitrate or nitrite for one reactant may be a deficiency for another. This is significant since excess nitrate or nitrite is an excellent heat sink, especially at elevated temperatures.The efficiency of various compounds as heat sinks, i.e., their enthalpies, vary greatly. In the wastes water is the most significant material at temperatures up to slightly above 100°C. From 100°C to about 300°C the greatest effect is probably from hydrated salts, with some contribution from concentrated caustic solutions. The loss of water from these materials requires a large energy input, some 50% to 100% greater than f...

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High Temperature Properties and Decomposition of Inorganic Salts Part 3, Nitrates and Nitrites

Cited by 266 publications

References 38 publications

Theoretical and Experimental Study of the Reaction between Ammonium Nitrate and Sodium Salts

Theoretical and Experimental Study of the Reaction between Ammonium Nitrate and Sodium Salts

Lithium-silicate sol–gel bioactive glass and the effect of lithium precursor on structure–property relationships

Calculation of reaction energies and adiabatic temperatures for waste tank reactions

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