Reaction of nitric oxide and oxygen

Ashmore, P. G.; Burnett, Michael G.; Tyler, Bonnie J.

doi:10.1039/tf9625800685

Cited by 38 publications

(22 citation statements)

References 2 publications

Supporting

Mentioning

Contrasting

Order By: Relevance

“…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%

“…Rate constant k 1 according to the temperature: ‐ . ‐, Bodenstein 1 ; … , Hasche and Patrick 2 ; – – –, Tipper and Williams 7 ; —, Ashmore et al 8 ; – ‐ ‐, Greig and Hall 13 ; , Hisatsune and Zafonte 14 ; , Mahenc et al 15 ; , Baulch et al 25 ; , England and Corcoran 17 ; , Olbregts 19 ; , this study [Color figure can be viewed at wileyonlinelibrary.com]…”

Section: Resultsmentioning

confidence: 62%

“…Ashmore et al 8 , Glasson and Tuesday, 9 and Greig and Hall 13 observe that the reaction is second order with respect to nitric oxide and first order with respect to oxygen. They also suggest the mechanism (M‐II) to describe the oxidation of nitric oxide rather than the mechanism (M‐I) because NO 3 has been identified spectroscopically 28 …”

Section: Literature Reviewmentioning

confidence: 98%

“…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%

“…The presence of nitrogen as an inert gas has been studied by several authors 5,8,9,[13][14][15][16] . None of them have reported any influence of the nitrogen on the oxidation.…”

Section: Pressure Influencementioning

confidence: 99%

See 4 more Smart Citations

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

View full text Add to dashboard Cite

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.

show abstract

Section: Literature Reviewsupporting

confidence: 63%

Section: Resultsmentioning

confidence: 62%

Section: Literature Reviewmentioning

confidence: 98%

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%

“…The presence of nitrogen as an inert gas has been studied by several authors 5,8,9,[13][14][15][16] . None of them have reported any influence of the nitrogen on the oxidation.…”

Section: Pressure Influencementioning

confidence: 99%

See 3 more Smart Citations

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

View full text Add to dashboard Cite

show abstract

The Role of Nitric Oxide in Photochemistry

Heicklen¹,

Cohen²

1968

Advances in Photochemistry

View full text Add to dashboard Cite

Nitric oxide gas absorption in a limestone packed column

Myerson

Sandy

1981

AIChE Journal

View full text Add to dashboard Cite

then he drawn through these localized K-values to cover the entire TBP range. The calculations also indicate that the variation of the liquid concentrations of the heavy components contribute much less to the error in the K-values from the pseudocomponent treatment than the variation in the y value across the same cut. For example for the 533.15-560.95K fraction, at 533.15K and 10.335 MPa, the x-value of the heavy component varies from 0.8483 to 0.8473 while the y-value varies from 0.003834 to 0.007884.Once the basic data for the equilibrium liquid and vapor compositions of acceptable accuracy have been obtained to represent the K-values as a function of pressure, temperature and composition, the latter assigned along the true boiling point cut, then the calculations can he conducted using size of cuts more consistent with the new experimental accuracy, hopefully, much smaller than are inherent in the present treatment. NOTATION LV%WV P, = critical pressure T, = critical temperature y = volume percent of liquid boil off = liquid to vapor molar ratio X = mole fraction in the liquid phase = mole fraction in the vapor phase Greek Letters y Y O 4 o = acentric factor = activity coefficient in the liquid phase = fugacity coefficient in the liquid phase = fugacity coefficient in the vapor phase

show abstract

Reaction of nitric oxide and oxygen

Cited by 38 publications

References 2 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

The Role of Nitric Oxide in Photochemistry

Nitric oxide gas absorption in a limestone packed column

Contact Info

Product

Resources

About