The effect of temperature on the aggregation kinetics of partially bare gold nanoparticles

Temperature dependent aggregation reaction of partially bare gold nanoparticles showed a first order kinetics and prevalence of reaction limited colloidal aggregation with an activation energy equal to 36.2 ± 3.0 kJ mol−1.

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The dissociation energy of the C-N bond in benzylamine

Proceedings of the Royal Society of London Series A - Mathematical and Physical Sciences ◽

10.1098/rspa.1949.0101 ◽

1949 ◽

Vol 198 (1053) ◽

pp. 285-292 ◽

Cited By ~ 13

Keyword(s):

Activation Energy ◽

Thermal Decomposition ◽

Dissociation Energy ◽

Heat Of Formation ◽

Molar Ratio ◽

Kcal Mole ◽

First Order ◽

First Order Kinetics ◽

Permanent Gases ◽

Kinetics Of

The kinetics of the thermal decomposition of benzylamine were studied by a flow method using toluene as a carrier gas. The decomposition produced NH 3 and dibenzyl in a molar ratio of 1:1, and small quantities of permanent gases consisting mainly of H 2 . Over a temperature range of 150° (650 to 800° C) the process was found to be a homogeneous gas reaction, following first-order kinetics, the rate constant being expressed by k = 6 x 10 12 exp (59,000/ RT ) sec. -1 . It was concluded, therefore, that the mechanism of the decomposition could be represented by the following equations: C 6 H 5 . CH 2 . NH 2 → C 6 H 5 . CH 2 • + NH 2 •, C 6 H 5 . CH 3 + NH 2 •→ C 6 H 5 . CH 2 • + NH 3 , 2C 6 H 5 . CH 2 •→ dibenzyl, and the experimentally determined activation energy of 59 ± 4 kcal./mole is equal to the dissociation energy of the C-N bond in benzylamine. Using the available thermochemical data we calculated on this basis the heat of formation of the NH 2 radical as 35.5 kcal./mole, in a fair agreement with the result obtained by the study of the pyrolysis of hydrazine. A review of the reactions of the NH 2 radicals is given.

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Temperature and pH effects on the kinetics of 2-aminophenol auto-oxidation in aqueous solution

Open Chemistry ◽

10.2478/bf02476226 ◽

2003 ◽

Vol 1 (3) ◽

pp. 233-241 ◽

Cited By ~ 3

Author(s):

Dumitru Oancea ◽

Mihaela Puiu

Keyword(s):

Experimental Data ◽

Activation Energy ◽

Aqueous Solution ◽

Ph Effects ◽

Influence Of Temperature ◽

First Order ◽

Incremental Methods ◽

First Order Kinetics ◽

Ph Range ◽

Kinetics Of

AbstractThe kinetics of the auto-oxidation of 2-aminophenol (OAP) to 2-amino-phenoxazin-3-one (APX) was followed in air-saturated aqueous solutions and the influence of temperature and pH on the auto-oxidation rate was studied. The kinetic analysis was based on a spectrophotometric method following the increase of the absorbance of APX. The process follows first order kinetics according to the rate law—d[OAP]/dt=k′[OAP]. The experimental data, within the pH range 4–9.85, were analyzed using both differential and incremental methods. The temperature variation of the overall rate constant was studied at pH=9.85 within the range 25–50°C and the corresponding activation energy was evaluated.

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Temperature Effects Associated with the Adsorption of Neodymium Ions onto Activated Charcoal

Adsorption Science & Technology ◽

10.1260/026361705774355432 ◽

2005 ◽

Vol 23 (5) ◽

pp. 399-406 ◽

Cited By ~ 1

Author(s):

Riaz Qadeer

Keyword(s):

Activation Energy ◽

Activated Charcoal ◽

Temperature Effects ◽

Adsorption Process ◽

First Order ◽

First Order Kinetics ◽

Charcoal Adsorption ◽

Increasing Temperature ◽

Kinetics Of ◽

Activated Charcoal Adsorption

The temperature dependence of the kinetics of the adsorption of neodymium ions from aqueous solution onto activated charcoal has been studied. The results obtained indicate that a form of equilibration appears to be attained after ca. 30 min although further very slow changes may occur over a much longer period. The adsorption process is controlled by the diffusion of neodymium ions into the pores of the activated charcoal. Adsorption follows first-order kinetics with an activation energy of 13.09 kJ/mol. Values of the equilibrium constant for the adsorption of neodymium ions onto activated charcoal increase with increasing temperature, thereby indicate the endothermic nature of the process.

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Hydrogenation Kinetics of N-Ethylcarbaozle as a Heteroaromatic Liquid Organic Hydrogen Carrier

Advanced Materials Research ◽

10.4028/www.scientific.net/amr.953-954.981 ◽

2014 ◽

Vol 953-954 ◽

pp. 981-984 ◽

Cited By ~ 6

Author(s):

Ming Yang ◽

Yuan Dong ◽

Han Song Cheng

Keyword(s):

Activation Energy ◽

High Temperature ◽

Hydrogen Pressure ◽

Reaction Rate ◽

Hydrogenation Reaction ◽

First Order ◽

First Order Kinetics ◽

Hydrogenation Kinetics ◽

Hydrogen Carrier ◽

Kinetics Of

The catalytic hydrogenation kinetics of N-ethylcarbazole over 5 wt% Ru/Al2O3 was investigated at various temperatures. The results shows that the hydrogenation reaction was exothermic and high temperature is unfavorable for the reaction rate. Fully hydrogenation was achieved within 1 hour under the best reaction temperature of 170 °C. The kinetics of N-ethylcarbazole follows the first-order kinetics in terms of the reactant concentration but independent of hydrogen pressure, which was maintained as a constant in the reaction process. The apparent activation energy of N-ethylcarbazole hydrogenation reaction at 150-180 °C was found to be 71.2 kJ/mol.

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An Experimental Study of the Coking Process

International Journal of Chemical Reactor Engineering ◽

10.2202/1542-6580.2001 ◽

2010 ◽

Vol 8 (1) ◽

Author(s):

Somayeh Ebrahimi ◽

Jafarsadegh Moghaddas

Keyword(s):

Activation Energy ◽

Coke Formation ◽

Nitrogen Atmosphere ◽

Fuel Oil ◽

Effective Parameters ◽

Pyrolysis Kinetics ◽

Exponential Factor ◽

First Order ◽

First Order Kinetics ◽

Kinetics Of

The coking process includes two dynamic and isothermal steps. In this process, some factors control the coke formation kinetics. In this research, effects of some important and effective parameters of feed on the quality of petroleum coke were studied. Two hydrocarbon residue feeds; Cracked Fuel Oil (CFO) and Styrene Monomer Tar (SMTAR) were used at 500°C with atmospheric pressure of nitrogen used as an inert gas. Rate of weight loss and gas evolution from these feeds were considered by data of thermal analysis TG (thermogravimetry) and DTG (derivative thermogravimetry). Based on the results, CFO was assigned as the better feed. After selecting better feed, simultaneous thermogravimetry-differential analysis (TG-DTA) was used to study the pyrolysis kinetics of CFO. Samples were heated in a TG-DTA apparatus in nitrogen atmosphere at a temperature range of 37-600°C. The activation energy (Ea) and pre-exponential factor (A) were calculated from the experimental results by using a three stage Arrhenius-type kinetic model and showed that CFO pyrolysis kinetics at temperature ranges 37-285, 320-450 and 467-600°C follows first, second and first order kinetics, respectively. Attentive to temperature increase and reaction progress, activation energy and pre-exponential factor indicated different values at each stage. Also, kinetics of the isothermal step of coke formation was studied during heating of CFO. Samples were reacted in a tube furnace at 450°C and with nitrogen atmosphere. The kinetics of coke formation for petroleum residue was followed by solvent extraction (insolubility in hexane (HI), toluene (TI)) and a development of TI approximate to apparent first order kinetics. The rate constant at this temperature was calculated and it was also observed that the coke formation had been started at a temperature below 450°C.

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Kinetics of the decomposition and the estimation of the stability of 10% aqueous and non-aqueous hydrogen peroxide solutions

Current Issues in Pharmacy and Medical Sciences ◽

10.1515/cipms-2015-0017 ◽

2014 ◽

Vol 27 (4) ◽

pp. 213-216 ◽

Cited By ~ 2

Author(s):

Maria Zun ◽

Dorota Dwornicka ◽

Katarzyna Wojciechowska ◽

Katarzyna Swiader ◽

Regina Kasperek ◽

...

Keyword(s):

Activation Energy ◽

Hydrogen Peroxide ◽

Decomposition Rate ◽

Aqueous Hydrogen Peroxide ◽

Decomposition Rate Constant ◽

First Order ◽

First Order Kinetics ◽

C 30 ◽

The Stability ◽

Kinetics Of

Abstract In this study, the stability of 10% hydrogen peroxide aqueous and non-aqueous solutions with the addition of 6% (w/w) of urea was evaluated. The solutions were stored at 20°C, 30°C and 40°C, and the decomposition of hydrogen peroxide proceeded according to first-order kinetics. With the addition of the urea in the solutions, the decomposition rate constant increased and the activation energy decreased. The temperature of storage also affected the decomposition of substance, however, 10% hydrogen peroxide solutions prepared in PEG-300, and stabilized with the addition of 6% (w/w) of urea had the best constancy.

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Kinetics of Desulfuration Product Sulphoaluminate Calcium

Advanced Materials Research ◽

10.4028/www.scientific.net/amr.113-116.1814 ◽

2010 ◽

Vol 113-116 ◽

pp. 1814-1817 ◽

Cited By ~ 2

Author(s):

Hui Ling Guo ◽

Jun Lin Xie

Keyword(s):

Activation Energy ◽

High Temperature ◽

Formation Rate ◽

Experimental Investigations ◽

Exponential Factor ◽

First Order ◽

First Order Kinetics ◽

Formation Kinetics ◽

Competitive Reactions ◽

Kinetics Of

The formation kinetics of sulphoaluminate calcium was studied by variations of sulfur release with time from SC-132 based on competitive reactions, the generation of sulphoaluminate calcium and the decomposition of CaSO4. Experimental investigations and theoretical derivations show that the formation rate of sulphoaluminate calcium can be described as first-order kinetics at high temperature, and it belongs to the mechanism of random nucleus growth. The apparent activation energy is 456.37 KJ•mol-1 and pre-exponential factor is 1.545×1012.

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QUANTITATIVE STUDIES ON THE PROPERDIN-COMPLEMENT SYSTEM

Journal of Experimental Medicine ◽

10.1084/jem.103.3.285 ◽

1956 ◽

Vol 103 (3) ◽

pp. 285-293 ◽

Cited By ~ 32

Author(s):

Myron A. Leon ◽

Keyword(s):

Activation Energy ◽

Complement System ◽

Quantitative Methods ◽

Reaction Rate ◽

First Order ◽

First Order Kinetics ◽

Quantitative Studies ◽

Kinetics Of

Quantitative methods have been developed for the estimation of C'3 and properdin. With these methods, the kinetics of the over-all reaction between properdin, zymosan, and C'3 were investigated. The reaction followed first order kinetics, provided zymosan was in excess, and the serum not diluted beyond 1/4. The reaction rate was proportional to the temperature, and an activation energy of 20,500 calories/mole was found. The distinction between total properdin and available serum properdin is discussed.

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Ethylene exchange in PtCl(C5H7O2)(π-C2H4)

Canadian Journal of Chemistry ◽

10.1139/v70-642 ◽

1970 ◽

Vol 48 (24) ◽

pp. 3802-3806 ◽

Cited By ~ 7

Author(s):

C. E. Holloway ◽

J. Fogelman

Keyword(s):

Activation Energy ◽

Magnetic Resonance ◽

Proton Magnetic Resonance ◽

Kcal Mole ◽

First Order ◽

First Order Kinetics ◽

Solvent Dependence ◽

Kinetics Of

The kinetics of exchange of free with complexed ethylene in the system PtCl(acac)(π-C2H4) have been investigated over a temperature and concentration range by proton magnetic resonance. First order kinetics are observed with respect to each component with no solvent dependence of rate. The activation energy and entropy are 2.7 kcal mole−1 and −36 cal deg−1 mole−1, respectively. A five coordinate intermediate is suggested, with complete retention of configuration at the platinum.

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Comparison of H2 Desorption Kinetics from Si(111)7×7 and Si(100)2×l

MRS Proceedings ◽

10.1557/proc-204-319 ◽

1990 ◽

Vol 204 ◽

Cited By ~ 10

Author(s):

M. L. Wise ◽

B. G. Koehler ◽

P. Gupta ◽

P. A. Coon ◽

S. M. George

Keyword(s):

Activation Energy ◽

Preexponential Factor ◽

Desorption Kinetics ◽

Bond Energies ◽

First Order ◽

First Order Kinetics ◽

Upper Limits ◽

Desorption Activation Energy ◽

Temperature Programmed ◽

Kinetics Of

ABSTRACTThe desorption kinetics of hydrogen from the β1 H2 -TPD state on Si(111)7×7 and Si(100)2×l were studied using laser-induced thermal desorption (LITD) and temperature programmed desorption (TPD) techniques. Isothermal LITD studies of H2 desorption from Si(111)7×7 revealed second-order kinetics with a desorption activation energy of Ed = 62 ±4 kcal/mol and a preexponential factor of Vd = 92 ±10 cm2 /s. In contrast, H2 desorption from Si(100)2×l revealed first-order kinetics with an activation energy of Ed = 58 ±2 kcal/mol and a preexponential factor of Vd = 5.5 ±0.5 × 1015 s−1. The desorption kinetics yield similar upper limits for the Si-H bond energies but different desorption mechanisms on Si(lll)7×7 and Si(100)2×l.

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