Primary Thermal Dissociation - Velocity Constants for Propane, n-Butane and Isobutane

Paul, R.; Marek, L. F.

doi:10.1021/ie50292a022

Cited by 26 publications

(10 citation statements)

References 2 publications

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“…The pioneers in this field were Pease (76), Marek and McCluer (58), Paul and Marek (75), Pease and Durgan (77), Rice (82), Frey and Hepp (27), Dintess and Frost (22)(23)(24), Steacie and Puddington (89), Hobbs and Hinshelwood (34), and Ingold et al (35). All of these studies were conducted in the low (25-400 °C) temperature ranges.…”

Section: A Study At Plant Levelmentioning

confidence: 99%

Survey of Propane Pyrolysis Literature

VOLKAN¹,

April²

1977

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

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Hydrocarbon pyrolyses have occupied a central role In the development of gas kinetics, first, because of their great economic potential, and secondly, because their relative molecular simplicity has been thought to offer the prospect of reasonably straightforward elucidation of the processes involved. Hydrocarbon pyrolyses to produce olefins, diolefins, and aromatics are the main processes of today's petrochemical industry. The purpose of this survey is to review a sub-set of this broad field of study-the thermal decomposition of propane. More than a decade ago it would have been relatively easy to review the entire hydrocarbon pyrolysis field, but the number of studies published in the past ten years restricts this review to the field of propane pyrolysis. A summary of recently reported data and results does not exist. Therefore, the intent of this review is to compile the propane pyrolysis data and to present the available knowledge to those interested in hydrocarbon pyrolysis studies and the positive impact that may occur within the petrochemical industry.

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Section: A Study At Plant Levelmentioning

confidence: 99%

Survey of Propane Pyrolysis Literature

VOLKAN¹,

April²

1977

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

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“…The values found were 0.55 and 0.57, as compared with predicted values of 0.91 and 1.04. Paul and Marek (139) repeated the investigation from the point of view of the kinetics of the processes. In the temperature range 550°to 610°C.…”

Section: Atomic and Photochemical Reactionsmentioning

confidence: 99%

“…2.6 X 10-8 Steacie and Puddington . (198a) [ (65,000) Pease and Durgan (147) iso-C4Hioi 4.8 X 10-8 Frey and Hepp (58) 1 14.89 66,040 1.5 X 10-8 7.1 X 10-8 Paul and Marek (139) ÍI-C5H12. .…”

Section: F Comparison Of the Para-fin Decompositionsmentioning

confidence: 99%

The Kinetics of Elementary Reactions of the Simple Hydrocarbons.

Steacie¹

1938

Chem. Rev.

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“…Pease (1928) and Pease and Durgan (1930) showed the reaction was first order and homogeneous. Paul and Marek (1934) found an activation energy of 66 kcal per mole at low conversions. Steacie and Puddington (1938) investigated the kinetics of this reaction thoroughly in a pressure range from 5 to 60 cm of Hg and at temperatures from 522°to 582°C.…”

mentioning

confidence: 99%

Thermal Cracking of Isobutane. Kinetics and Product Distributions

Buekens¹,

Froment²

1971

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

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The thermal cracking of isobutane was studied in a flow apparatus between 620°a nd 820°C and at atmospheric pressure. Product distributions were established and a reaction scheme was deduced. The order of the isobutane decomposition was determined by comparing experiments with different degrees of feed dilution and was close to one. Owing to inhibition the first-order rate coefficient decreases with increasing conversion. Therefore, the rate coefficient is considered a hyperbolic function of conversion.The activation energy of the first-order rate coefficient increases slightly with conversion.Finally, the radical nature of the process is discussed.

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Primary Thermal Dissociation - Velocity Constants for Propane, n-Butane and Isobutane

Cited by 26 publications

References 2 publications

Survey of Propane Pyrolysis Literature

Survey of Propane Pyrolysis Literature

The Kinetics of Elementary Reactions of the Simple Hydrocarbons.

Thermal Cracking of Isobutane. Kinetics and Product Distributions

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