The Dissociation Pressure and Free Energy of Formation of Ammonium Nitrate

Feick, George

doi:10.1021/ja01651a095

Cited by 44 publications

(29 citation statements)

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“…The stability of ammonium nitrate has been the object of several studies [127,128]. NH4NO3 does not start its well-known rapid, self-accelerating decomposition to N2O and water until heated to 260-280 °C.…”

Section: Atmospheric Reaction Of Ammonia and Nitric Acidmentioning

confidence: 99%

Fate of ammonia in the atmosphere?a review for applicability to hazardous releases

Renard

Calidonna

Henley³

2004

Journal of Hazardous Materials

138

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Section: Atmospheric Reaction Of Ammonia and Nitric Acidmentioning

confidence: 99%

Fate of ammonia in the atmosphere?a review for applicability to hazardous releases

Renard

Calidonna

Henley³

2004

Journal of Hazardous Materials

138

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“…For the calculations presented here, I will use the data of Nagatani et al (1967) since it extends to the highest temperature, 410 K, and appears to be the most thorough study. For calculations above 410 K, I have extrapolated Nagatani et al's (1967) heat capacity data for crystalline phase I to the melting point at 442.75 K (Dellien, 1982), used the value of the heat of fusion of 6.20+0.20 kJ mol-i reported by Dellien (1982), and used the liquid phase heat capacity (0.191 J mol-1 K-1 ) measured by Feick (1954). Data for NHa(g) were taken from Haar (1968) while data for HNO3(g) were taken from the JANAF tables (Chase et al, 1985).…”

Section: Extrapolation Of Vapour Pressure Measurementsmentioning

confidence: 99%

“…The standard free energy of dissociation was determined from two sets of vapour pressure measurements; those of Feick (1954) over the liquid at 442.8-522.3 K and those of Brandner et al (1962) over the solid at 349.2-438.2 K and over the liquid at 443.2-513.2 K. Each reported vapour pressure was used to determine the dissociation constant at that temperature from the formula Kp=(Pvav/2) 2. These were then used to compute AG~i.…”

Section: Extrapolation Of Vapour Pressure Measurementsmentioning

confidence: 99%

“…Values of AG,~iss and Kp(298), derived from several independent sets of measurements, are summarized in Table 1 and discussed individually in the following. Feick (1954) has measured the vapour pressure of liquid NH4NO3 and Brandner et al (1962) have measured the vapour pressure of solid and liquid NH4NO3 at elevated temperatures. Jaffe (1988) has criticized the extrapolation of this data to lower temperatures, largely because of the sensitivity of the extrapolation to small changes in the slope or intercept.…”

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confidence: 99%

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The dissociation constant of ammonium nitrate and its dependence on temperature, relative humidity and particle size

Mozurkewich

1993

Atmospheric Environment. Part A. General Topics

297

151

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“…HN 03 (g) Equilibria involving HNO 3 were measured by Jones [75], Feick [76], and Abel, et al [77], yielding AHf = -32.06, -32.02, and -32.09 kcal. Becker and Roth [78] and Thomsen [59] measured the heat of neutralization of HN 03 (aq) with NH 3 ; combining these values with the data for NH 4 NO 3 yields AHf = -32.27 and -32.07 kcal.…”

Section: N2®4(g)mentioning

confidence: 99%

Preliminary report on the thermodynamic properties of selected light-element and some related compounds:

1962

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This is the seventh semi-annual report on the current experimental, theoretical, and evaluative program, at the National Bureau of Standards, on the thermodynamic properties of selected light-element compounds of primary interest in high-temperature research. In this connection the chemical elements principally involved are H, Li, Be, B, C, N, 0, F, At, Cl, and Zr, with more secondary interest in the compounds of Mg, Si, K, Ti, Br, I, W, Hg, and Pb. The emphasis in the NBS work has been on the simpler compounds of these elements.This report includes some recent NBS measurements under the program: The heat of formation of nitronium perchlorate, and the high-temperature heat capacity of aluminum carbide. As discussed in the report, precise measurements are essentially completed on the heat of combustion of aluminum in fluorine and on the low-temperature heat capacities and absolute entropies of LiH, and LiAlH^; however, these data are not yet presented, pending the resolution of small discrepancies needed to put the results on a final basis. Tables of thermodynamic functions are given for four gases omitted from earlier reports (H 2 > 02> H , and electron gas), and, on the basis of improved data, for the condensed phases of two substances (BeF 2 and At^C^) . A contribution from those areas in which elaborate apparatus development is still progressing is a description in the report of a new fast-opening large-aperture shutter for high-speed photography. This development will be important in the study of combustions at very high temperatures and pressures.Also included are several up-to-date literature surveys in the field.One describes recent additions to the literature on the chemistry of numerous light-element compounds. A second describes alloys and intermetallic compounds of aluminum and beryllium with titajaium and zirconium; while a third survey covers low-temperature heat capacities aud entropies of various substances, particularly the oxides of eight light elements. The fourth report is a comprehensive and critical assembly of the available values for the heats of formation of a large number of compounds. IntroductionNitronium perchlorate is a v;hite, crystalline material, stable at temperatures up to 120°C. It is extremely hygroscopic, reacting rapidly with water to form nitric and perchloric acids. Aqueous solutions of potassium hydroxide were used in this investigation, as the potassium salts of the acids provided more suitable reference substances. The heats of solution of KN0_(c) and KClO/c) in KOH(aq) were also determined. Constants and Conversion FactorsThe results of this investigation are given in joules and calories, with 1 cal = 4*1840 joules. All weights are corrected to vacuum. The molecular weights are calculated from the 1957 International Table of Atomic Weights [l]. For N02C10/(c) an estimated heat capacity of 36 cal/deg mole was used; other auxiliary data were taken where possible from [2].3. MaterialsThe KNO^(c) and KC10/(c) were reagent-grade materials, dried at 120°...

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The Dissociation Pressure and Free Energy of Formation of Ammonium Nitrate

Cited by 44 publications

References 1 publication

Fate of ammonia in the atmosphere?a review for applicability to hazardous releases

Fate of ammonia in the atmosphere?a review for applicability to hazardous releases

The dissociation constant of ammonium nitrate and its dependence on temperature, relative humidity and particle size

Preliminary report on the thermodynamic properties of selected light-element and some related compounds:

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