Thermal stability of tert-butyl peroxypivalate

Hordijk, A.C.; Verhoeff, J.; Groot, J. J. de

doi:10.1016/0040-6031(81)80130-x

Cited by 6 publications

(6 citation statements)

References 4 publications

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“…The adiabatic induction time to 0 = 5 at an initial temperature of 295.1 K can now be calculated with the aid of Eq. (1 8) as 59.7 h, in good agreement with the experimental value of 60.5 h. Calculation of the adiabatic induction time from the data of Hordijk et al [13] yields 72.9 h.…”

Section: Adiabatic Runaway Experimentssupporting

confidence: 75%

“…The thermal properties given in [13] are valid for an extended temperature range. Generally, self-heating properties can be described more accurately for a narrow temperature range.…”

Section: Adiabatic Runaway Experimentsmentioning

confidence: 99%

“…The adiabatic temperature rise can be calculated from the reported data as AT,, = 269 K and the specific heat capacity of the liquid is 2176 J/kg"C. The regression analysis of the data of the Arrhenius plot yields Qm = 1.18 x 10'' W/kg and EIR = 13753 K. Hordijk et al [13] mention different values of Qm and EIR for this diluted peroxide but the value of the parameter Qm exp( -E/RTo) is almost the same. The thermal properties given in [13] are valid for an extended temperature range.…”

Section: Adiabatic Runaway Experimentsmentioning

confidence: 99%

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Safe operation of a batch reactor: Safe storage of organic peroxides in supply vessels

Steensma

Westerterp

1991

Chem Eng & Technol

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In this study, we investigated the limits of safe operation for a cooled reactor, operated batchwise. As an example of a single-phase reaction, we studied the decomposition of t-butyl peroxypivalate, a well-known organic peroxide, undergoing self-heating at relatively low temperatures. If sufficiently diluted, it can be supplied to a polymerization process from large, cooled but unstirred vessels. We present a number of extensions to the existing homogeneous explosion theory, namely a practical definition of the critical condition, its calculation, and expressions for the available time before runaway in the case of a supercritical condition, taking into account the effects of natural convection inside the vessel and the reactant conversion. The extensions of the theory were confirmed by adiabatic and non-adiabatic runaway experiments on bench scale, and natural convection cooling experiments with liquids in various packages.

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Section: Adiabatic Runaway Experimentssupporting

confidence: 75%

“…The thermal properties given in [13] are valid for an extended temperature range. Generally, self-heating properties can be described more accurately for a narrow temperature range.…”

Section: Adiabatic Runaway Experimentsmentioning

confidence: 99%

Section: Adiabatic Runaway Experimentsmentioning

confidence: 99%

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Safe operation of a batch reactor: Safe storage of organic peroxides in supply vessels

Steensma

Westerterp

1991

Chem Eng & Technol

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“…The isothermal and adiabatic storage tests are the most sensitive, which means that reaction kinetic data are determined for the lowest possible temperature range. From investigating the thermal stability of tertiary butylperoxypivalate [12] the conclusion has been drawn that the test results of these methods agree surprisingly well for this substance in a rather broad concentration and temperature range. A similar, more extensive comparison is given here for tertiary butylperoxybenzoate.…”

Section: Decomposition Rates By Other Methodsmentioning

confidence: 94%

Thermal runaway in the thermal explosion of a liquid

Verhoeff

Berg

1984

Journal of Thermal Analysis

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To study the thermal explosion of liquids a low pressure autoclave has been built. The first stage of a thermal explosion, the thermal runaway, has been studied. Evaluation of the temperature-time history results in kinetic data. Comparison with other thermal methods shows that the reliability of the method is better than with DTA.Tertiary butylperoxybenzoate has been investigated in the temperature range of 330 K to 440 K. Decomposition starts with a short period of autocatalysis, up to a conversion of about 0.05. The subsequent deco#nposition can be described by a second order process in the first instance and by a first order process in the last resort. Induced decomposition occurs up to a conversion of about 0.95.The description of exploding liquids is usually based on detonation or deflagration. However, many liquids do not detonate when shocked by an explosive and do not deflagrate when ignited by a flame. Yet an explosion can occur after a prolonged period of heating. This is called thermal explosion and is characterized by a considerable degree of self-heating or thermal runaway of the liquid before the larger part of the explosion energy is released. Actually an explosion comparable to a deflagration or detonation does not occur until after a drastic change in the physical state of the liquid by the thermal runaway process.The theory of thermal explosion [1][2][3] is concerned with the competition between heat generation of the reacting system and heat dissipation by conduction, convection and radiation from the reacting mass to the outside. The tendency of the reacting system to rise above the ambient temperature due to self-heating is opposed by both the heat transfer to the surroundings and the heat consumption of the reactant. It is worth noting here that the thermal explosion theory tries to account for the onset of the explosive behaviour of energetic substances during storage or during batch-wise operation. Hence, a continuously stirred tank reactor is not considered.To evaluate the temperature-time history for a thermal explosion and to gather reaction kinetic data a low pressure autoclave has been built. Tertiary butyl peroxybenzoate (TBPB) has been chosen as a model substance [4].

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“…[7][8][9][10]) and of peroxycarboxylic esters in particular (e.g. [11][12][13][14][15]). Publications concerning heat production of synthesis are rare in the public literature.…”

Section: Introductionmentioning

confidence: 99%