Nitric Acid and Ammonia Concentrations as Factors Controlling the Thermal Decomposition of Ammonium Nitrate

Kołaczkowski, A.; Biskupski, A.

doi:10.1007/978-3-0348-6719-1_62

Cited by 5 publications

(4 citation statements)

References 2 publications

Supporting

Mentioning

Contrasting

Order By: Relevance

“…The use of the post-filtration liquor for obtaining the mixed sodium−ammonium nitrate is made difficult due to its explosiveness during the concentration process, especially in a presence of chloride ions. , Investigations of different additives to ammonium nitrate revealed that the presence of chloride ions accelerates 50 times its decomposition at 180 °C . The research on the mixed sodium−ammonium nitrate revealed that the presence of sodium nitrate does not affect significantly the mechanism of decomposition, compared to the pure ammonium nitrate, and the decomposition products of the mixed nitrate are the same as for ammonium nitrate: nitrous oxide, water, nitrogen and oxygen, and other nitrogen oxides, while NH 3 and HNO 3 are present only in small amounts.…”

Section: Introductionmentioning

confidence: 99%

Investigation of the Solubility in the NaVO₃−NaNO₃−H₂O System

and

Drużyński

2007

Ind. Eng. Chem. Res.

View full text Add to dashboard Cite

The solubility of sodium vanadate and sodium nitrate was investigated in the NaVO 3 -NaNO 3 -H 2 O system at the temperature range 293-323 K, with the method of isothermal saturation of a solution. The obtained results gave a basis for the plot of a fragment of the solubility isotherm for the investigated system. That system is a part of the five-component NH 4 NO 3 -NaVO 3 -NH 4 VO 3 -NaNO 3 -H 2 O system and is necessary for plotting the solubility isotherm in the projection according to Janecke method. Knowledge of the course of that isotherm for the five-component system is necessary for determination of the optimal conditions for utilization of the postfiltration liquor from the soda production from NaNO 3 by the Solvay method with the use of NaVO 3 .

show abstract

Section: Introductionmentioning

confidence: 99%

Investigation of the Solubility in the NaVO₃−NaNO₃−H₂O System

and

Drużyński

2007

Ind. Eng. Chem. Res.

View full text Add to dashboard Cite

show abstract

“…The authors of the SCS method assumed direct production of mixed fertilizer by crystallizing ammonium-sodium saltpeter. However, according to studies, − chloride ions accelerate thermal decomposition of ammonium nitrate(V) causing a real risk of explosion during the concentration, crystallization, and storage of ammonium-sodium saltpeter.…”

Section: Introductionmentioning

confidence: 99%

Equilibrium Study in the KNO₃ + NH₄NO₃ + H₂O System at Temperatures from 293.15 to 323.15 K

et al. 2019

View full text Add to dashboard Cite

A solid−liquid equilibrium (SLE) study was conducted in the ternary system KNO 3 + NH 4 NO 3 + H 2 O using the isothermal solution saturation method at temperatures of 293.15, 303.15, 313.15, and 323.15 K. The experimental data obtained were used to plot a section of the solubility polytherm of the investigated system and show the dependence of the densities of equilibrium solutions on their chemical compositions. It has been found that a complex salt of the formula K 0.25 (NH 4 ) 0.75 NO 3 is formed in the system at a temperature below 303.15 K.

show abstract

“…The transformation of that saltpeter into the nitrogenous fertilizer is difficult because of the presence of chloride ions and explosive properties of ammonium nitrate. Chloride ions catalyze the decomposition of ammonium nitrate, which causes the loss of nitrogen during the production and real risk of explosion during the processes of concentration, crystallization, and storage of the produced ammonium–sodium saltpeter. − …”

Section: Introductionmentioning

confidence: 99%

Solubility in the Reciprocal Quaternary NH₄⁺–Na⁺–NO₃^––VO₃^––H₂O System at (313 and 323) K

Trypuć

Drużyński

2011

J. Chem. Eng. Data

View full text Add to dashboard Cite

The equilibrium solubility studies of the NH 4 NO 3 þ NaVO 3 þ H 2 O system at (313 and 323) K have been performed. On the basis of the results, the equilibrium plots for the system in a planar projection have been obtained according to the J€ anecke method. The plots enable the determination of the optimal conditions for the conversion reaction of ammonium nitrate into sodium nitrate with the use of sodium metavanadate. The source of ammonium nitrate is the postfiltration lye from the soda production with the sodaÀchlorineÀsaltpeter (SCS) method. The conversion of NH 4 NO 3 from the postfiltration lye into NaNO 3 cancels the risk of explosion during the process of production of ammoniumÀsodium saltpeter. ' INTRODUCTIONSodium carbonate is one of the basic products of the inorganic industry. That compound is used among others as a flux agent in a process of glass production or as a substrate for production of water glass. 1,2 The production of sodium carbonate reaches ca. 50 million ton per year, and about 50 % of that is produced with the Solvay method. That method is based on the easily available raw materials such as halite, limestone, carbon, and ammonia. 3,4 That technology is characterized by the significant noxiousness for the natural environment, mainly due to the emission of large amounts of the liquid waste (CaCl 2 and NaCl solution) and solid waste (CaCO 3 , Ca(OH) 2 , ashes). 3,4 An alternative method of sodium carbonate production which relies on the same raw materials is the wasteless sodaÀchlorineÀ saltpeter (SCS) method. The difference between SCS and the Solvay method is that during the carbonization process (eq 1) the sodium nitrate brine is used instead of sodium chloride. Sodium nitrate is obtained in the process of oxidation of solid sodium chloride with the nitric acid in the presence of air. The second valuable product in that process is chlorine. 4,5The solution obtained after filtration of sodium bicarbonate contains mainly ammonium nitrate, unreacted sodium nitrate, and a small amount of sodium chloride. The obtained lye is used in the production of mixed ammoniumÀsodium saltpeter, which is further used as a fertilizer. The transformation of that saltpeter into the nitrogenous fertilizer is difficult because of the presence of chloride ions and explosive properties of ammonium nitrate. Chloride ions catalyze the decomposition of ammonium nitrate, which causes the loss of nitrogen during the production and real risk of explosion during the processes of concentration, crystallization, and storage of the produced ammoniumÀsodium saltpeter. 5À7 This phenomenon can be eliminated by modification of the SCS method based on the conversion of ammonium nitrate into sodium nitrate with sodium metavanadate (eq 2). The solution of sodium nitrate obtained in that process does not cause any risk of explosion during the production of sodium saltpeter. 8,9 NH 4 The precipitated ammonium metavanadate is subjected to calcination (eq 3), to recover ammonia and vanadium(V) oxide, which in turn is used ...

show abstract

Nitric Acid and Ammonia Concentrations as Factors Controlling the Thermal Decomposition of Ammonium Nitrate

Cited by 5 publications

References 2 publications

Investigation of the Solubility in the NaVO₃−NaNO₃−H₂O System

Investigation of the Solubility in the NaVO₃−NaNO₃−H₂O System

Equilibrium Study in the KNO₃ + NH₄NO₃ + H₂O System at Temperatures from 293.15 to 323.15 K

Solubility in the Reciprocal Quaternary NH₄⁺–Na⁺–NO₃^––VO₃^––H₂O System at (313 and 323) K

Contact Info

Product

Resources

About

Nitric Acid and Ammonia Concentrations as Factors Controlling the Thermal Decomposition of Ammonium Nitrate

Cited by 5 publications

References 2 publications

Investigation of the Solubility in the NaVO3−NaNO3−H2O System

Investigation of the Solubility in the NaVO3−NaNO3−H2O System

Equilibrium Study in the KNO3 + NH4NO3 + H2O System at Temperatures from 293.15 to 323.15 K

Solubility in the Reciprocal Quaternary NH4+–Na+–NO3––VO3––H2O System at (313 and 323) K

Contact Info

Product

Resources

About

Investigation of the Solubility in the NaVO₃−NaNO₃−H₂O System

Investigation of the Solubility in the NaVO₃−NaNO₃−H₂O System

Equilibrium Study in the KNO₃ + NH₄NO₃ + H₂O System at Temperatures from 293.15 to 323.15 K

Solubility in the Reciprocal Quaternary NH₄⁺–Na⁺–NO₃^––VO₃^––H₂O System at (313 and 323) K