Kinetic analysis of thermogravimetric data, VI

Zsakó, J.

doi:10.1007/bf01950372

Cited by 117 publications

(17 citation statements)

References 18 publications

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“…Some of these results are listed in Table 4. 6 Horowitz and Metzger method [10] F n , (n = 0.71) 89. 6 Coats and Redfern method [12] F n , (n = 0.66) 95.…”

Section: Resultsmentioning

confidence: 99%

“…6 Horowitz and Metzger method [10] F n , (n = 0.71) 89. 6 Coats and Redfern method [12] F n , (n = 0.66) 95. 9 Horowitz and Metzger method [13] F 1 , (n = 1) 92.…”

Section: Resultsmentioning

confidence: 99%

“…The technology of TA has been widely used to reveal the thermal behavior and thermal character of solid-state reactions and the primary aim here is to establish the values of the apparent activation energy E, pre-exponential factor A in Arrhenius equation and choose the most probable mechanism function f(a) of a reaction [4,5]. The mathematical apparatus and calculation procedures used are rather versatile but all of them are related to the mathematical analysis of thermogravimetric curves [6][7][8]. The analysis of these curves allows establishing the mechanism of rate-controlled stage of the conversion and the values of the kinetic parameters characterizing it.…”

Section: Introductionmentioning

confidence: 99%

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A comparative study of non-isothermal kinetics of decomposition of calcium oxalate monohydrate

Vlaev

Nedelchev

Gyurova

et al. 2008

Journal of Analytical and Applied Pyrolysis

289

178

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“…Some of these results are listed in Table 4. 6 Horowitz and Metzger method [10] F n , (n = 0.71) 89. 6 Coats and Redfern method [12] F n , (n = 0.66) 95.…”

Section: Resultsmentioning

confidence: 99%

“…6 Horowitz and Metzger method [10] F n , (n = 0.71) 89. 6 Coats and Redfern method [12] F n , (n = 0.66) 95. 9 Horowitz and Metzger method [13] F 1 , (n = 1) 92.…”

Section: Resultsmentioning

confidence: 99%

Section: Introductionmentioning

confidence: 99%

See 1 more Smart Citation

A comparative study of non-isothermal kinetics of decomposition of calcium oxalate monohydrate

Vlaev

Nedelchev

Gyurova

et al. 2008

Journal of Analytical and Applied Pyrolysis

289

178

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“…A number of models have been developed for study the mechanism of solid state decomposition processes [5][6][7][8][9]. Method of Redfern and Coats was found to be the most convenient [10,11]. Thus the equations for determination of the E A and K are as follows:…”

Section: Methodsmentioning

confidence: 99%

Mechanism and Kinetic Parameters of the Thermal Decomposition of Gibbsite Al(OH)₃ by Thermogravimetric Analysis

et al. 2017

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In this study, the mechanism and the kinetic parameters of the thermal decomposition of gibbsite Al(OH)3 were studied by differential thermogravimetry technique under non-isothermal conditions, between room temperature and 1200 K at heating rates of 5, 10, 15 and 20The obtained differential thermogravimetry curves show clearly three distinct peaks. The first peak is due to the partial dehydroxylation of gibbsite. Among the 32 types of differential equations of non-isothermal kinetics, we have found that the most suitable mechanism is (A 3/2 :2/3 ) also called Avrami-Erofeev equation of order 2/3. The values of the activation energy EA and of the pre-exponential factor K are 157 kJ mol −1 and 7.58 × 10 15 s −1 , respectively. The second peak corresponds to the decomposition of gibbsite to boehmite. Decomposition is controlled by the rate of second-order reaction (F2: g(x) = (1 − x) −1 − 1), under the applied conditions. The activation energy EA and pre-exponential factor K correspond to 243 kJ mol −1 and 3.73 × 10 22 s −1 , respectively. The third peak is due to transformation of boehmite to alumina. However the mechanism for such transformation is better described by the 3/2 rate order reaction (F 3/2 : g(x) = (1 − x) −1/2 − 1). In addition, the values of EA and K were determined to be around 296 kJ mol −1 and 1.82 × 10 19 s −1 , respectively. The results of differential thermogravimetry were supplemented by the differential thermal analysis. X-ray powder diffraction analysis was carried out for samples of gibbsite treated at different temperatures between 200 and 1200• C in 200• C steps.

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“…In Table 2 are also given the rate constants k which were calculated in terms of the appropriate functions, A1.4 and R3.4. Table 3 According to the CR method [16,17], the D1 law was estimated as appropriate, yielding E=220-266 kJ/mol and log A=17-20 I/s, depending on the heating Table 4 were obtained. It is noted here that the Arrhenius parameters do not decrease with the increasing heating rate.…”

Section: Kinetics Of the Thermal Decomposition Of Synthetic Malachitementioning

confidence: 99%

Preparation and thermal analysis of synthetic malachite CuCO3·Cu(OH)2

Tanaka

Yamane

1992

Journal of Thermal Analysis

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The synthesis of malachite CuCO3"Cu(OH)2 or Cu2CO3(OH)2 was studied through titrations of copper(II) salt solutions with a solution of sodium carbonate at different temperatures. The precipitates were characterized by TG, IR and chemical analysis. The composition varies depending on the pH of the solution and the temperature. Purer malachite was synthesized by simple mixing of a solution of copper(II) nitrate or sulfate with a solution of sodium carbonate at 50~The kinetics of the thermal decomposition of synthetic malachite was described by either R3 or A~(m=l.2-1.4) law, according to TG analysis, both isothermal and nonisothermal. The Arrhenius parameters determined using three different integral methods showed the kinetic compensation effect, which is correlated to the working temperature interval analyzed. Keywords: kinetics of thermal decomposition, synthetic malachite In~oducfionPure CuCO3-Cu(OH)2 is synthesized by mixing 0.1 M copper(II) salt solution with 0.1 M-Na2CO3 solution at 50~ in a mole ratio of 1.0 or with a little excess of Na2CO3. Formation of synthetic malachite was examined comprehensively through titrations, normal and reverse, under various experimental conditions. Kinetic analysis by thermogravimetry, both isothermal and nonisothermal, revealed that the decomposition of synthetic malachite is regulated by either Rn(n=3) or Am(m--1.2-1.4) law. The Arrhenius parameters determined using three different methods showed the kinetic compensation effect, which is rationalized in view of the working temperature interval analyzed.It is known that copper(II) carbonate hydroxide, or synthetic malachite is obtained by reacting a solution of copper(II) nitrate with a solution containing the equivalent amount of sodium carbonate at room temperature [1]. However, little John Wiley & Sons, Limited, Chichester Akad~miai Kiad6, Budapest

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Kinetic analysis of thermogravimetric data, VI

Cited by 117 publications

References 18 publications

A comparative study of non-isothermal kinetics of decomposition of calcium oxalate monohydrate

A comparative study of non-isothermal kinetics of decomposition of calcium oxalate monohydrate

Mechanism and Kinetic Parameters of the Thermal Decomposition of Gibbsite Al(OH)₃ by Thermogravimetric Analysis

Preparation and thermal analysis of synthetic malachite CuCO3·Cu(OH)2

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Kinetic analysis of thermogravimetric data, VI

Cited by 117 publications

References 18 publications

A comparative study of non-isothermal kinetics of decomposition of calcium oxalate monohydrate

A comparative study of non-isothermal kinetics of decomposition of calcium oxalate monohydrate

Mechanism and Kinetic Parameters of the Thermal Decomposition of Gibbsite Al(OH)3 by Thermogravimetric Analysis

Preparation and thermal analysis of synthetic malachite CuCO3·Cu(OH)2

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Product

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Mechanism and Kinetic Parameters of the Thermal Decomposition of Gibbsite Al(OH)₃ by Thermogravimetric Analysis