Standard enthalpy of solution of ammonium nitrate in water at 298 K

Медведев, В. А.; Efimov, M.E.; Cerutti, Paul J.; McKay, R. Michael L.; Johnson, L. H.; Hepler, Loren G.

doi:10.1016/0040-6031(78)85113-2

Cited by 7 publications

(6 citation statements)

References 2 publications

Supporting

Mentioning

Contrasting

Order By: Relevance

“…As a result, they must be roughly estimated from the formation enthalpies of the constitutive compounds, assuming the mixtures to be ideal. Test calculations indicate that u G values decrease by 2-3% as a value of 6 kcal=mol is assumed for the dissolution enthalpy of AN in the mixture, similar to the value reported for dissolving this salt in water [30]. ANFO is a 94=6 mixture of ammonium nitrate (AN) and gazole.…”

Section: Test Set 2008mentioning

confidence: 98%

Prediction of Gurney Parameters Based on an Analytic Description of the Expanding Products

Mathieu

2014

Journal of Energetic Materials

View full text Add to dashboard Cite

A new analytic model is introduced to predict Gurney parameters of explosives from their empirical formula, density, and formation enthalpy. It involves the H 2 O-CO 2 arbitrary, the assumption of a constant polytropic coefficient, and two empirical parameters. It is more physically grounded than previous models and proves twice more reliable, hence demonstrating that combining an analytic description of purely academic interest for hot gases with a small number of empirical parameters making up for its deficiencies proves superior to straightforward Quantitative Structure-Property Relationships (QSPR) approaches.

show abstract

Section: Test Set 2008mentioning

confidence: 98%

Prediction of Gurney Parameters Based on an Analytic Description of the Expanding Products

Mathieu

2014

Journal of Energetic Materials

View full text Add to dashboard Cite

show abstract

“…It is worth noting that the dissolution of ammonium nitrate (NH 4 NO 3 ) can exhibit a good dissolution endothermic effect (the standard enthalpy change, Δ H = 25.4 kJ/mol); therefore, it was widely used in middle school chemistry class demonstrations for absorbing heat with significant temperature decrease performance. Considering this principle, we attempted to build an enhanced thermometric assay, by superimposing the dual temperature signals of exothermic and endothermic reaction.…”

Section: Resultsmentioning

confidence: 99%

“…The sensing principle relies on the fact that CoOOH nanoflakes, as an effective catalyst, can catalyze the decomposition of H 2 O 2 into O 2 and H 2 O, accompanied by a significant increase of pressure of the sealed reaction vessel, as well as an obvious temperature enhancement because of this exothermic reaction process (Δ H = −98.2 kJ/mol) . Then the increased pressure further leads to the overflowing of a certain amount of H 2 O from the drainage device into another vessel, and finally leads to a significant temperature decrease due the preloaded ammonium nitrate (NH 4 NO 3 ) and its good dissolution endothermic effect (Δ H = 25.4 kJ/mol) . In the presence of target As(V), it can specifically interact with CoOOH nanoflakes via the electrostatic attraction and As–O covalent-type interaction.…”

mentioning

confidence: 99%

“…46 Then the increased pressure further leads to the overflowing of a certain amount of H 2 O from the drainage device into another vessel, and finally leads to a significant temperature decrease due the preloaded ammonium nitrate (NH 4 NO 3 ) and its good dissolution endothermic effect (ΔH = 25.4 kJ/mol). 47 In the presence of target As(V), it can specifically interact with CoOOH nanoflakes via the electrostatic attraction and As−O covalent-type interaction. Then the catalytic activity of CoOOH nanoflakes for H 2 O 2 decomposition can be significantly attenuated, leading to a dramatic decrease of pressure and temperature enhancement of the O 2 -generation system, as well as the decrease of temperature reduction of the NH 4 NO 3 -dissolution system.…”

mentioning

confidence: 99%

See 1 more Smart Citation

Enhanced Thermometric Sensor for Arsenate Analysis Based on Dual Temperature Readout Signaling Strategy

et al. 2020

View full text Add to dashboard Cite

New methods for portable detection of arsenate are still in urgent need. Herein, we explored a simple but sensitive thermometric strategy for arsenate determination without complex instruments and skilled technicians. Cobalt oxyhydroxide (CoOOH) nanoflakes, can ingeniously decompose hydrogen peroxide into oxygen in a sealed reaction vessel, accompanied by marked pressure and significant temperature increase due to the exothermic reaction effect (ΔH = −98.2 kJ/mol). The increased pressure then compelled a certain amount of H2O overflowing from the drainage device into another vessel, leading to a significant temperature decrease due to the preloaded ammonium nitrate (NH4NO3) and its good dissolution endothermic effect (ΔH = 25.4 kJ/mol). In the presence of arsenate, the catalytic activity of CoOOH nanoflakes for H2O2 decomposition was inhibited dramatically, resulting in an obvious decrease of the pressure, weighting water and temperature response. The two temperature responses with increasing and decreasing feature were easily measured through a common thermometer, and exhibited an effective signaling amplification via coupling both “signal-on” and “signal-off” temperature readout elements. The obtained dual superimposing temperature readout exhibits a good linear with the concentration of arsenate with a lower detection limit (51 nM, 3.8 ppb). Compared to the inductively coupled plasma mass spectrometry, this enhanced thermometric strategy provides a simple, rapid, convenient, low cost, and portable platform for sensing arsenate in real environmental water.

show abstract

“…The more endothermic a salt is while dissolving, the lower the vapor pressure and the higher the hygroscopicity. Enthalpy of solution (kJ g −1 ) for the compounds tested is +0.32 for ammonium nitrate, +0.14 for calcium nitrate, and +0.08 for CAN fertilizer (Grishchenko, Druzhinina, Tiflova, & Monayenkova, 2018; Laue, Thiemann, Scheibler, & Wiegand, 2000; Medvedev et al., 1978). Our findings were in accordance with these values, and the relatively weak endothermic properties of CAN could, together with the presence of coating, explain its lower hygroscopicity.…”

Section: Resultsmentioning

confidence: 99%

Laboratory studies on dissolution of nitrogen fertilizers by humidity and precipitation

Sigtryggsson

Hamnér

Kirchmann

2020

Agricultural & Env Letters

View full text Add to dashboard Cite

Aiming at improving fertilizer management by assessing fertilizer dissolution, we compared the hygroscopicity of calcium ammonium nitrate (CAN), ammonium nitrate (NS 27‐4), and nitrate compounds (laboratory grade). Dissolution of N fertilizers was also studied under simulated rain conditions. All compounds were highly hygroscopic, dissolving within 24 h at 90–99% relative humidity and 25 °C. Addition of 2 mm rain to fertilizer granules (3–4.5 mm diam.) was sufficient to dissolve 50% of the compounds. Dissolution rates by humidity or rain were not the limiting step for plant availability.

show abstract

Standard enthalpy of solution of ammonium nitrate in water at 298 K

Cited by 7 publications

References 2 publications

Prediction of Gurney Parameters Based on an Analytic Description of the Expanding Products

Prediction of Gurney Parameters Based on an Analytic Description of the Expanding Products

Enhanced Thermometric Sensor for Arsenate Analysis Based on Dual Temperature Readout Signaling Strategy

Laboratory studies on dissolution of nitrogen fertilizers by humidity and precipitation

Contact Info

Product

Resources

About