Filling the Oxford Chair of Ecclesiastical History, 1866: the Nomination of H. L. Mansel

Knox, Bruce

doi:10.1111/j.1467-9809.1968.tb00300.x

Cited by 3 publications

(5 citation statements)

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“…Several postulates have been proposed Reid, 1954, 1961;Semenov, 1958;Knox, 1968; Baldwin et al, 1970;Euker and Leinroth, 1970) that explain relatively well certain results obtained over rather limited experimental conditions, but no postulate proposed to date explains results obtained over wide ranges of conditions. A proposed mechanism should explain both the kinetics'and composition of products obtained.…”

mentioning

confidence: 89%

“…Numerous previous investigators have presented experi-mental information that indicates partial oxidation results often vary significantly in reactors with different materials of construction or with different pretreatments of the inner surfaces. Several postulates have been proposed Reid, 1954, 1961;Semenov, 1958;Knox, 1968;Baldwin et al,, 1970;Euker and Leinroth, 1970) that explain relatively well certain results obtained over rather limited experimental conditions, but no postulate proposed to date explains results obtained over wide ranges of conditions. A proposed mechanism should explain both the kinetics'and composition of products obtained. In a steel reactor operated at atmospheric pressure, a relatively constant rate of oxidation of propane occurred over the entire range of oxygen conversion from essentially 0 to 100% (Kao, 1969).…”

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confidence: 99%

“…(3) Destruction or reactions of certain gaseous products. Knox (1968) indicated that hydroperoxides decompose at the surface. Euker and Leinroth (1970) reported that olefins are formed in part heterogeneously; no details of the actual reactions were given however.…”

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confidence: 99%

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Partial Oxidation of Light Hydrocarbons. 1. Major Differences Noted in Various Tubular Reactors

Mahajan¹,

Menzies²,

Albright³

1977

Ind. Eng. Chem. Proc. Des. Dev.

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Although the material of construction of the reactor used for the partial oxidation of light paraffins has a major effect on both the composition of the product obtained and on the kinetics of oxidation, the present investigation is the first one to investigate several reactors systematically over a wide range of operating conditions. Glass, aluminum, steel, and copper reactors were employed in the present investigation for partial oxidation of both methane and propane. Postulates proposed earlier to explain the role of the surface do not explain all results. The reactor surfaces were found in many cases to catalyze surface reactions.Numerous previous investigators have presented experimental information that indicates partial oxidation results often vary significantly in reactors with different materials of construction or with different pretreatments of the inner surfaces. Several postulates have been proposed Reid, 1954, 1961;Semenov, 1958;Knox, 1968; Baldwin et al., 1970;Euker and Leinroth, 1970) that explain relatively well certain results obtained over rather limited experimental conditions, but no postulate proposed to date explains results obtained over wide ranges of conditions. A proposed mechanism should explain both the kinetics'and composition of products obtained.In a steel reactor operated at atmospheric pressure, a relatively constant rate of oxidation of propane occurred over the entire range of oxygen conversion from essentially 0 to 100%

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Partial Oxidation of Light Hydrocarbons. 1. Major Differences Noted in Various Tubular Reactors

Mahajan¹,

Menzies²,

Albright³

1977

Ind. Eng. Chem. Proc. Des. Dev.

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“…The gen abstractions by a polyatomic, non-linear, free radical (12,25).3 Possibly they are in error because of systematic errors in the correction factor (see above). On the other hand, if they are correct they will explain an apparent anomaly in the E, values for saturated hydrocarbons calculated from gas phase and from liquid phase autoxidations that has been pointed out by Benson (26).…”

Section: Pre-exponential Factorsmentioning

confidence: 99%

Absolute Rate Constants for Hydrocarbon Autoxidation. XXI. Activation Energies for Propagation and the Correlation of Propagation Rate Constants with Carbon–Hydrogen Bond Strengths

Korček¹,

Chenier²,

Howard³

et al. 1972

Can. J. Chem.

251

130

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The rate constants, k,, for the abstraction of a hydrogen atom from a wide variety of organic substrates at 30" have been correlated with the strengths of the C-H bond that are broken, D[R-HI (in units of kcal/mol). Two empirical relations have been derived, one for tertiary peroxy radicals,and one for secondary peroxy radicals,These equations hold extremely well for hydrocarbons and reasonably well for substrates containing heteroatoms. The activation energies and pre-exponential factors for the oxidation of some hydrocarbons by I-butylperoxy radicals have been measured and the empirical relation derived. If D[I-ROO-H] is taken as 88 kcal/mol, this yields the Polanyi equation,where AH is the heat of the hydrogen abstraction reaction. These empirical equations permit the calculation of the rate constants for chain propagation in the autoxidation of many organic substrates at 30' and also at other temperatures.

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“…Medley and Cooley (1960) and Robertson (1955) reviewed the products and mechanisms of isobutane (2-methylpropane) oxidation. Knox (1968) presented mechanistic schemes for its oxidation at 300°and 500°t o 600°C ., while Aliara et al (1968) discussed its oxidation at 100°to 155°C. Mitchell (1956), Jones et al (1961), andFenske (1959) using the raining solids technique reported preliminary results on the oxidation products of re-butane and isobutane.…”

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confidence: 99%

Solids Effects on Butane and Butene Oxidation

Jones¹,

Daubert²,

Fenske³

et al. 1970

Ind. Eng. Chem. Proc. Des. Dev.

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Filling the Oxford Chair of Ecclesiastical History, 1866: the Nomination of H. L. Mansel

Cited by 3 publications

References 0 publications

Partial Oxidation of Light Hydrocarbons. 1. Major Differences Noted in Various Tubular Reactors

Partial Oxidation of Light Hydrocarbons. 1. Major Differences Noted in Various Tubular Reactors

Absolute Rate Constants for Hydrocarbon Autoxidation. XXI. Activation Energies for Propagation and the Correlation of Propagation Rate Constants with Carbon–Hydrogen Bond Strengths

Solids Effects on Butane and Butene Oxidation

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