STUDIES ON THE RATE OF OXIDATION OF NITRIC OXIDE<sup>1</sup> II. THE VELOCITY OF THE REACTION BETWEEN NITRIC OXIDE AND OXYGEN AT 0° AND 30°

Hasche, R. Leonard; Patrick, Walter A.

doi:10.1021/ja01682a002

Cited by 15 publications

(16 citation statements)

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“…In Equation (2), r NO represents the rate of nitric oxide oxidation. The majority of the published papers 1–21 are in agreement with Equation (2). The data obtained by these authors on the rate constant k 1 are summarized in Table 1.…”

Section: Literature Reviewsupporting

confidence: 63%

“…However, some authors 2,3,6–9,12,13 use a two‐step mechanism to describe their experimental results when they are derived from Equation (2). A literature review from Heicklen and Cohen 26 summarizes most of these studies, and the two main mechanisms are a first mechanism (M‐I) with a dimer of NO as an intermediate:

N {normalO}_{((), g)} + E ⇆_{k_{- 2}}^{k_{2}} {((), NO)}_{2 (normalg)}

{((), NO)}_{2 (normalg)} + {normalO}_{2 (normalg)} \overset{k_{3}}{\to} 2 N {normalO}_{2 (normalg)}

r_{normalNO} = \frac{k_{2} * k_{3} * {([], NO)}^{2} * [O_{2}]}{k_{- 2} + k_{3} * [O_{2}]}

and a second mechanism (M‐II) with NO 3 as an intermediate:

N {normalO}_{((), g)} + {normalO}_{2 (normalg)} ⇆_{k_{- 4}}^{k_{4}} N {normalO}_{3 (normalg)}

N {normalO}_{3 (normalg)} + N {normalO}_{((), g)} \overset{k}{\to}

…”

Section: Literature Reviewmentioning

confidence: 99%

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Kinetic study of the nitric oxide oxidation between 288 and 323 K, under pressure, focus on the oxygen influence on the reaction rate constant

Neyrolles

Cruz

Bassil

et al. 2020

Int J of Chemical Kinetics

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The sequestration of carbon dioxide fumes from oxyfuel combustion is used to reduce significantly the carbon dioxide emissions from coal‐fired power plants. Impurities like nitric oxide, present in the fumes, can cause technical difficulties during the capture, the treatment, the transport, and the storage steps of the CO2 fumes. The purpose of this study is to better understand the oxidation of nitric oxide under pressure in the presence of carbon dioxide and in the experimental condition of flue gas treatment. This reaction is known to be a third‐order reaction, two order in nitric oxide and first order in oxygen. To examine the effect of the temperature, the pressure and the volume fraction of oxygen on the rate constant of oxidation, k1, an autoclave is used. The first experiment studies the influence of the temperature between 288 and 323 K. The results found are in the form of an Arrhenius‐type equation: k1 = 810 exp(620/T) and are in agreement with the literature. Carbon dioxide does not seem to have an influence on the rate constant, whereas our experimental measurements indicate an influence of the volume fraction of oxygen. The rate constant decreases when the oxygen volume fraction increases by up to 10%. Then the rate constant remains constant. This observation allows us to conclude that the mechanism involving the mechanism with a dimer of NO as an intermediate is more likely to be the mechanism involved in the nitric oxide oxidation in our experimental conditions: high pressure and ambient temperature. The rate constant k2, k–2, and k3 were also estimated in these conditions.

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Section: Literature Reviewsupporting

confidence: 63%

N {normalO}_{((), g)} + E ⇆_{k_{- 2}}^{k_{2}} {((), NO)}_{2 (normalg)}

{((), NO)}_{2 (normalg)} + {normalO}_{2 (normalg)} \overset{k_{3}}{\to} 2 N {normalO}_{2 (normalg)}

r_{normalNO} = \frac{k_{2} * k_{3} * {([], NO)}^{2} * [O_{2}]}{k_{- 2} + k_{3} * [O_{2}]}

and a second mechanism (M‐II) with NO 3 as an intermediate:

N {normalO}_{((), g)} + {normalO}_{2 (normalg)} ⇆_{k_{- 4}}^{k_{4}} N {normalO}_{3 (normalg)}

N {normalO}_{3 (normalg)} + N {normalO}_{((), g)} \overset{k}{\to}

…”

Section: Literature Reviewmentioning

confidence: 99%

Kinetic study of the nitric oxide oxidation between 288 and 323 K, under pressure, focus on the oxygen influence on the reaction rate constant

Neyrolles

Cruz

Bassil

et al. 2020

Int J of Chemical Kinetics

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“…Oxidation of gaseous NO occurs as an overall third-order gas-phase reaction (Ashmore et al, 1962;Bodenstein, 1918;Greig and Hall, 1967;Hasche and Patrick, 1925;Morrison et al, 1966;Treacy and Daniels, 1955).…”

Section: Theoreticalmentioning

confidence: 99%

Gaseous Nitrogen Oxide Absorption in a Sieve-Plate Column

Counce¹,

Perona²

1979

Ind. Eng. Chem. Fund.

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Nitrogen oxides were absorbed into dilute nitric acid in a three-stage sieve-plate column. The variables investigated were liquid flow rate, total gas flow rate, partial pressure of nitrogen oxide in the feed gas, acid molarity, and condensable gas (steam) flow rate. The results of the study indicate the importance of three mechanisms in the absorption of gaseous NO, compounds: (1) the absorption of N204, which results in the production of liquid "OB and "0,; (2) the dissociation of the liquid HNO, into HNO, and gaseous NO; and (3) the gas-phase oxidation of NO to NO2. An interesting aspect of this study was the detrimental effect that liquid nitrous acid has on nitrogen oxide removal efficiency. The removal efficiencies varied between 75 and 90%.

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“…Through a parameter‐fitting process using the Eyring's transition state theory with the molecular properties, Gershinowitz and Eyring 9 justified a transition state in which each O atom in an O 2 molecule is partially bonded to N atom of each of the two NO molecules. Instead, two of the three molecules first form a complex which then reacts with the third molecule, reaction (a) would not be termed truly termolecular. Pre‐equilibrium mechanism with dimer of NO as an intermediate 10,11: In the solid and liquid states, NO exists as (NO) 2 . Pre‐equilibrium mechanism with NO 3 as an intermediate: …”

Section: Introductionmentioning

confidence: 99%

“…Pre‐equilibrium mechanism with dimer of NO as an intermediate 10,11: In the solid and liquid states, NO exists as (NO) 2 .…”

Section: Introductionmentioning

confidence: 99%

Effects of NO₂, CO, O₂, and SO₂ on oxidation kinetics of NO over Pt‐WO₃/TiO₂ catalyst for fast selective catalytic reduction process

Irfan

Goo

Kim

2006

Int J of Chemical Kinetics

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The selective catalytic reduction rate of NO with N-containing reducing agents can be enhanced considerably by converting a part of NO into NO 2 . The enhanced reaction rate is more pronounced at lower temperatures by using an equimolar mixture of NO and NO 2 . The kinetics of NO oxidation over Pt-WO 3 /TiO 2 catalyst has been determined in a fixed-bed reactor with different concentrations of oxygen, nitric oxide, and nitrogen dioxide in the presence of 8% water. It has been found that the reaction is second order with respect to nitric oxide, first order for oxygen with a third-order rate constant. Also, it is found that there is no effect on the reaction order with an addition of NO 2 , CO, or SO 2 . It follows the same second order but the reaction rate is found to be changed. It is observed that in the case of NO 2 and SO 2 , the reaction rate tends to decrease, but it increases with the addition of CO into the feed. C 2006

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STUDIES ON THE RATE OF OXIDATION OF NITRIC OXIDE¹ II. THE VELOCITY OF THE REACTION BETWEEN NITRIC OXIDE AND OXYGEN AT 0° AND 30°

Cited by 15 publications

References 0 publications

Kinetic study of the nitric oxide oxidation between 288 and 323 K, under pressure, focus on the oxygen influence on the reaction rate constant

Kinetic study of the nitric oxide oxidation between 288 and 323 K, under pressure, focus on the oxygen influence on the reaction rate constant

Gaseous Nitrogen Oxide Absorption in a Sieve-Plate Column

Effects of NO₂, CO, O₂, and SO₂ on oxidation kinetics of NO over Pt‐WO₃/TiO₂ catalyst for fast selective catalytic reduction process

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STUDIES ON THE RATE OF OXIDATION OF NITRIC OXIDE1 II. THE VELOCITY OF THE REACTION BETWEEN NITRIC OXIDE AND OXYGEN AT 0° AND 30°

Cited by 15 publications

References 0 publications

Kinetic study of the nitric oxide oxidation between 288 and 323 K, under pressure, focus on the oxygen influence on the reaction rate constant

Kinetic study of the nitric oxide oxidation between 288 and 323 K, under pressure, focus on the oxygen influence on the reaction rate constant

Gaseous Nitrogen Oxide Absorption in a Sieve-Plate Column

Effects of NO2, CO, O2, and SO2 on oxidation kinetics of NO over Pt‐WO3/TiO2 catalyst for fast selective catalytic reduction process

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STUDIES ON THE RATE OF OXIDATION OF NITRIC OXIDE¹ II. THE VELOCITY OF THE REACTION BETWEEN NITRIC OXIDE AND OXYGEN AT 0° AND 30°

Effects of NO₂, CO, O₂, and SO₂ on oxidation kinetics of NO over Pt‐WO₃/TiO₂ catalyst for fast selective catalytic reduction process