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kinetically treated as a gas–solid reaction to study the reduction behavior using model based and model-free methods. In model based methods, a single run data is used to calculate the Arrhenius activation energy values whereas model-free methods involve

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the reaction mechanism, and k is the specific rate constant given by the Arrhenius equation: where A is the pre-exponential factor in min −1 , E is the activation energy (kJ/mol), R is the universal gas constant (J/mol/K), and T is the

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Reaction Kinetics, Mechanisms and Catalysis
Authors: Alexander Khassin, Georgiy Filonenko, Tatyana Minyukova, Irina Molina, Lyudmila Plyasova, Tatyana Larina, and Vladimir Anufrienko

observed for reduction of the JC sample, while the exothermic peaks of the reduction of the AE sample are wider and shifted to higher temperatures. Pre-calcined sample reduction is characterized by effective activation energy, E a = 19 kJ/mol, which only

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assumed to have Arrhenius dependence with temperature: (19) where E is the activation energy, R is the universal gas constant and k 0 is a pre-exponential factor. After the estimation of each kinetic constant, its activation energy and pre

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Catalyst Rate constant k (h −1 ) Activation energy (E a ) (kJ/mol) Pre-exponential factor (A) (mol −1 h −1 ) Enthalpy (ΔH # ) (kJ mol −1

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HPMo ( 1 ), HPVMo ( 2 ), (NH 4 ) 3 PMo ( 3 ), (NH 4 ) 3 HPVMo ( 4 ), (NH 4 ) 2 KHPVMo ( 5 ), (NH 4 ) 1,5 CsH 1,5 PVMo ( 6 ), Cs 3 HPVMo ( 7 ) By means of the well-known Arrhenius equation, the values of apparent activation energy were determined

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isopropyl alcohol conversion. The activation energies and selectivities of parallel dehydration and dehydrogenation reactions were obtained. The results were correlated with the data concerning the polarity of the bond between the central atom and oxygen in

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by the Arrhenius equation: where the activation energy E A,i can be calculated from the slope of ln k i versus 1/ T in the Arrhenius diagram. In order to study the effect of temperature on the reaction, experiments were carried out

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activation; the hydrogen generation rate was constant with time in a batch reactor. The reaction rate equation can be written as follows: (1) where k 0 is the rate constant (ml min −1 g −1 ), E a is the activation energy for the reaction (kJ mol −1 ), R

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Reaction Kinetics, Mechanisms and Catalysis
Authors: Saet Byul Kim, Mi Ran Lee, Eun Duck Park, Sang Min Lee, HyoKyu Lee, Ki Hyun Park, and Myung-June Park

correlation between pre-exponential factor and activation energy leads to a highly nonlinear problem, and thus the following form is used in the estimation to reduce correlation: The objective function, Eq. 10 , was minimized using the lsqcurvefit

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