Role of nitrous acid decomposition in absorber and bleacher in nitric acid plant

Ingale, Nilesh; Chatterjee, I.B.; Joshi, Jyeshtharaj B.

doi:10.1016/j.cej.2009.09.017

Cited by 9 publications

(1 citation statement)

References 20 publications

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“…Motivation for the study of nitrous acid decomposition is diverse, with the reactions playing important roles in many industrial and environmental processes. Industrially, decomposition of nitrous acid is a significant process occurring in the manufacture of nitric acid, wherein a gaseous NO x stream is absorbed in water, , and in synthesis reactions involving nitrous acid (i.e., nitrosation reactions) where the NO x side products pose a toxicity hazard. , In atmospheric chemistry, reactions of nitrous acid and NO x have received attention owing to their importance in acid deposition on the earth’s surface and their role in smog formation, while the reactions may be of biological importance under certain conditions where nitrous acid decomposition could contribute to NO production in the body . Decomposition of nitrous acid can be employed as a source of NO in the laboratory and has been implicated in the release of nitrogen oxides from plants .…”

Section: Introductionmentioning

confidence: 99%

Accurate Rate Constants for Decomposition of Aqueous Nitrous Acid

et al. 2012

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Decomposition of nitrous acid in aqueous solution has been studied by stopped flow spectrophotometry to resolve discrepancies in literature values for the rate constants of the decomposition reactions. Under the conditions employed, the rate-limiting reaction step comprises the hydrolysis of NO(2). A simplified rate law based on the known elementary reaction mechanism provides an excellent fit to the experimental data. The rate constant, 1.34 × 10(-6) M(-1) s(-1), is thought to be of higher accuracy than those in the literature as it does not depend on the rate of parallel reaction pathways or on the rate of interphase mass transfer of gaseous reaction products. The activation energy for the simplified rate law was established to be 107 kJ mol(-1). Quantum chemistry calculations indicate that the majority of the large activation energy results from the endothermic nature of the equilibrium 2HNO(2) ⇆ NO + NO(2) + H(2)O. The rate constant for the reaction between nitrate ions and nitrous acid, which inhibits HNO(2) decomposition, was also determined.

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Section: Introductionmentioning

confidence: 99%

Accurate Rate Constants for Decomposition of Aqueous Nitrous Acid

et al. 2012

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Nitric Acid

Groves¹

2020

Kirk-Othmer Encyclopedia of Chemical Technology

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Nitric acid is a key chemical for many industries. Some 60 million tons are produced annually, of which 80% goes into nitrate production for fertilizers and explosives, the latter principally for mining. Other significant uses include the manufacture of intermediates for polyurethane and polyamide production. This article covers the birth and development of the Ostwald nitric acid manufacturing process and describes the modern commercial production methods for both “weak” (≤68 wt%) and “strong” (∼69–99 wt%) nitric acid. An overview of the present state of knowledge is given about the main chemical process steps of ammonia oxidation and nitrogen oxide absorption. Nitric acid plants are emitters of NO x and N 2 O, and the currently available technologies to limit these to their permitted levels are discussed. Further information includes health and safety aspects, shipping and handling regulations, and economics. The article concludes with a description of alternative production technologies and a brief outlook on the future of nitric acid.

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