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Journal articles on the topic 'First order reaction'

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Author: Grafiati

Published: 6 September 2023

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1

Ball, David. "Kinetics of Consecutive Reactions: First Reaction, First-Order; Second Reaction, Zeroth Order." Journal of Chemical Education 75, no. 7 (July 1998): 917. http://dx.doi.org/10.1021/ed075p917.

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2

Croce, A. E. "First-order parallel and consecutive reaction mechanisms — Isosbestic points criterium." Canadian Journal of Chemistry 86, no. 9 (September 1, 2008): 918–24. http://dx.doi.org/10.1139/v08-098.

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A criterium for the selection of reaction mechanism derived from a condition for isosbestic points occurrence is presented. Analytical relationships involving the molar absorption coefficients of the species, which participate in a mechanism of parallel first-order reactions and the corresponding rate coefficients, are also reported. A model system of four species that present overlapping absorption spectra may correspond to the reactant and products of a system of parallel or consecutive first-order reactions. In the first case, under experimental conditions in which the absorbances are additive, the presence of an isosbestic point in the spectrum of the reaction mixture at a given wavelength leads to a time-independent ratio of the degree of advancement of reaction variables. From this, relevant kinetic information may be extracted, namely, the ratio of the reaction rate coefficients. Moreover, the occurrence of isosbestic points allows discarding the second mechanism. This conclusion is independent of the number of absorbing species. Model calculated examples show the application of the equations here derived. The resolution for the general case of mechanisms of N first-order reactions is provided.Key words: chemical kinetics, time-resolved absorption spectra, reaction mechanism.

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3

Boeker, E. A. "Integrated rate equations for irreversible enzyme-catalysed first-order and second-order reactions." Biochemical Journal 226, no. 1 (February 15, 1985): 29–35. http://dx.doi.org/10.1042/bj2260029.

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Integrated rate equations are presented that describe irreversible enzyme-catalysed first-order and second-order reactions. The equations are independent of the detailed mechanism of the reaction, requiring only that it be hyperbolic and unbranched. The results should be directly applicable in the laboratory.

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4

Vinnett, Luis, and Kristian E. Waters. "Representation of Kinetics Models in Batch Flotation as Distributed First-Order Reactions." Minerals 10, no. 10 (October 15, 2020): 913. http://dx.doi.org/10.3390/min10100913.

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Four kinetic models are studied as first-order reactions with flotation rate distribution f(k): (i) deterministic nth-order reaction, (ii) second-order with Rectangular f(k), (iii) Rosin–Rammler, and (iv) Fractional kinetics. These models are studied because they are considered as alternatives to the first-order reactions. The first-order representation leads to the same recovery R(t) as in the original domain. The first-order R∞-f(k) are obtained by inspection of the R(t) formulae or by inverse Laplace Transforms. The reaction orders of model (i) are related to the shape parameters of first-order Gamma f(k)s. Higher reaction orders imply rate concentrations at k ≈ 0 in the first-order domain. Model (ii) shows reverse J-shaped first-order f(k)s. Model (iii) under stretched exponentials presents mounded first-order f(k)s, whereas model (iv) with derivative orders lower than 1 shows from reverse J-shaped to mounded first-order f(k)s. Kinetic descriptions that lead to the same R(t) cannot be differentiated between each other. However, the first-order f(k)s can be studied in a comparable domain.

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5

Strieder, William. "Chemoreceptor diffusion and reaction: first-order kinetics." Chemical Engineering Science 55, no. 14 (April 2000): 2579–84. http://dx.doi.org/10.1016/s0009-2509(99)00538-2.

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6

Riazi, Mohammad R., and Amir Faghri. "Solid dissolution with first-order chemical reaction." Chemical Engineering Science 40, no. 8 (1985): 1601–3. http://dx.doi.org/10.1016/0009-2509(85)80105-6.

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7

Wu, Xizun, Wenzhi Zhang, Shengmin Cai, and Degang Han. "A Method for Estimation of Kinetic Parameters; A Simple First-Order Reaction and Two Parallel First-Order Reactions Producing a Common Product." Collection of Czechoslovak Chemical Communications 57, no. 6 (1992): 1196–200. http://dx.doi.org/10.1135/cccc19921196.

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A method is proposed for the treatment of data from a kinetic system of a simple first-order reaction and two parallel first-order reactions, producing a common product. It is based on the solving of a contrary proposition for an ordinary differential equation.

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8

Vajda, S., and H. Rabitz. "Identifiability and distinguishability of first-order reaction systems." Journal of Physical Chemistry 92, no. 3 (February 1988): 701–7. http://dx.doi.org/10.1021/j100314a024.

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9

Tóbiás, Roland, László L. Stacho, and Gyula Tasi. "First-order chemical reaction networks I: theoretical considerations." Journal of Mathematical Chemistry 54, no. 9 (June 14, 2016): 1863–78. http://dx.doi.org/10.1007/s10910-016-0655-2.

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10

Chau, F. T., and K. W. Mok. "Multiwavelength analysis for a first-order consecutive reaction." Computers & Chemistry 16, no. 3 (July 1992): 239–42. http://dx.doi.org/10.1016/0097-8485(92)80009-o.

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11

GADGIL, C., C. LEE, and H. OTHMER. "A stochastic analysis of first-order reaction networks." Bulletin of Mathematical Biology 67, no. 5 (September 2005): 901–46. http://dx.doi.org/10.1016/j.bulm.2004.09.009.

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12

Robbins, D. J., A. J. Almquist, D. C. Timm, J. I. Brand, and R. E. Gilbert. "Experimental Evaluation of Nonisothermal, First-Order Reaction Kinetics." Macromolecules 28, no. 26 (December 1995): 8729–34. http://dx.doi.org/10.1021/ma00130a004.

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13

Vrentas, J. S., and C. M. Vrentas. "Unsteady diffusion with a first-order homogeneous reaction." AIChE Journal 33, no. 1 (January 1987): 167–68. http://dx.doi.org/10.1002/aic.690330122.

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14

Klump, H. H. "Energetics of order/order transitions in nucleic acids." Canadian Journal of Chemistry 66, no. 4 (April 1, 1988): 804–11. http://dx.doi.org/10.1139/v88-140.

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Besides the temperature induced canonical helix to random coil transition, which serves as a prototype of an order/disorder transition, there is a second group of conformational changes in helical polynucleotides, which will be termed order/order transitions. Depending on the environmental conditions and the sequence of the polynucleotides involved, there are four alternative reaction schemes: (i) The inversion of the helical handedness from a right-handed to a left-handed conformation, (ii) the disproportionation of a double helix into a single strand and a triple helix, (iii) the addition of a single strand to a double helix, and (iv) the single/double strand displacement reactions, that is, the displacement of one of the two strands of the helix by a matching single-stranded polynucleotide or the mutual exchange of one strand each between two helical structures. The first three reactions are considered reversible while the last reaction is irreversible; that is, one cannot regain the initial state by inversing the course of the change, here the change in temperature. Both ribo and deoxyribo polynucleotides can undergo these reactions. In the following paper at least one example is given for each of these reactions.

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15

Offurum, J. C., M. M. Chukwu, C. A. Mbadike, T. U. Nwaneri, and A. A. Nwakaudu. "JUSTIFICATION OF ORDER OF CORROSION INHIBITION KINETICS FOR ESTERS OF CASTOR AND RUBBER SEED OILS." JOURNAL OF THE NIGERIAN SOCIETY OF CHEMICAL ENGINEERS 37, no. 1 (April 1, 2022): 88–93. http://dx.doi.org/10.51975/22370108.som.

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The present study centres on the justification of order of corrosion inhibition kinetics for esters of castor and rubber seed oils. Inhibition of mildsteel corrosion was studied in the presence of sulphuric acid medium. The study was justified by the regular misprediction of order of chemical reactions (especially corrosion reaction), due to varying individual perceptions in this regard. While many researchers assume that corrosion reaction kinetics is of first order in most cases, others resolve that it is of zero or even second order. Experimental (gravimetric) data from the mildsteel corrosion inhibition process was used to generate the kinetic data at different experimental conditions of 10g/l (concentration), 40oC (temperature) and 50% stroke (pressure), at different times of 4, 8, 16, 24 and 32hours. Equations of the lines were generated, and coefficient of determination, R2 values for the different (derived) kinetic equations (zero, first and second orders) were obtained. While R2 values for zero order curves fall between 0.9250 – 0.9790, those of first order fall between 0.9740 – 0.9880, and those of second order fall between 0.7820 – 0.9520, which indicates that the R2 values of first order kinetics tend more towards unity than those of zero and second orders. This implies that the corrosion reaction, generally, is governed by the postulations of first order kinetics, followed by the zero order and, then, second order. The results, therefore, justify that kinetics of corrosion reactions is (always) of first order. Keywords: Corrosion inhibition, Justification, Kinetics, Order of reaction.

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16

Balogh, Ágnes, Gábor Lente, József Kalmár, and István Fábián. "Reaction Schemes That Are Easily Confused with a Reversible First-Order Reaction." International Journal of Chemical Kinetics 47, no. 12 (October 23, 2015): 773–82. http://dx.doi.org/10.1002/kin.20960.

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17

Evans, J. W., and M. S. Miesch. "Catalytic reaction kinetics near a first-order poisoning transition." Surface Science 245, no. 3 (April 1991): 401–10. http://dx.doi.org/10.1016/0039-6028(91)90042-q.

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18

Evans, J. W., and M. S. Miesch. "Catalytic reaction kinetics near a first-order poisoning transition." Surface Science Letters 245, no. 3 (April 1991): A146. http://dx.doi.org/10.1016/0167-2584(91)90784-o.

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19

Yih, Siu-Ming. "Comments on solid dissolution with first-order chemical reaction." Chemical Engineering Science 42, no. 5 (1987): 1269. http://dx.doi.org/10.1016/0009-2509(87)80086-6.

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20

Chrastil, Joseph. "Determination of the first-order consecutive reversible reaction kinetics." Computers & Chemistry 17, no. 1 (March 1993): 103–6. http://dx.doi.org/10.1016/0097-8485(93)80035-c.

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21

Obrazovskiĭ, E. G. "Diffusion-controlled first-order surface reaction in turbulent flow." Journal of Experimental and Theoretical Physics 103, no. 1 (July 2006): 119–25. http://dx.doi.org/10.1134/s1063776106070132.

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22

Giona, Massimiliano. "First-order reaction—diffusion kinetics in complex fractal media." Chemical Engineering Science 47, no. 6 (1992): 1503–15. http://dx.doi.org/10.1016/0009-2509(92)80295-n.

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23

Kiss, Virág, and Katalin Ősz. "Double Exponential Evaluation under Non-Pseudo-First-Order Conditions: A Mixed Second-Order Process Followed by a First-Order Reaction." International Journal of Chemical Kinetics 49, no. 8 (June 12, 2017): 602–10. http://dx.doi.org/10.1002/kin.21100.

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24

Katritzky, Alan R., and Bogumil Brycki. "Kinetics and mechanism of nucleophilic displacements with heterocycles as leaving groups. Part 23. Studies at the borderlines between reactions proceeding (i) via free carbocations, (ii) via rate-determining formation of ion–molecule pairs, and (iii) via rate-determining nucleophilic attack on ion–molecule pairs." Canadian Journal of Chemistry 64, no. 6 (June 1, 1986): 1161–69. http://dx.doi.org/10.1139/v86-192.

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Evidence is presented to demonstrate that at the borderline between first-order reaction via nucleophilic trapping of intimate ion–molecule pairs and first-order reaction via the formation of free carbocations, both mechanisms proceed independently, without merging. Similarly at the borderline between first-order (rate-determining formation) and second-order (rate-determining nucleophilic attack) reactions of intimate ion–molecule pairs, both reactions again proceed independently.

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25

Hutchinson, Claire V., and Tim Ledgeway. "Temporal frequency modulates reaction time responses to first-order and second-order motion." Journal of Experimental Psychology: Human Perception and Performance 36, no. 5 (2010): 1325–32. http://dx.doi.org/10.1037/a0019250.

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26

Šolc, Milan. "The first passage time to the equilibrium state of a first order reaction." Collection of Czechoslovak Chemical Communications 52, no. 1 (1987): 1–5. http://dx.doi.org/10.1135/cccc19870001.

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The first passage time to the state of exact equilibrium (the most probable stationary state) for a first order reaction is described in terms of the probability density and the first and second moments. For large systems, the first moment is proportional to the logarithm of the number of particles in the system, while the dispersion is independent of the size of the system.

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27

YUANQING, ZHANG, ZENG XIANCHENG, CHENG SIQING, YU XIAOQI, and TIAN ANMING. "MICELLAR CATALYSIS OF COMPOSITE REACTIONS I MICELLAR EFFECT ON THE CONSECUTIVE FIRST ORDER REACTION." Journal of Dispersion Science and Technology 20, no. 3 (April 1999): 1009–24. http://dx.doi.org/10.1080/01932699908943831.

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28

Filimonov, Valeriy Yu. "Critical ignition conditions in exothermically reacting systems: first-order reactions." Proceedings of the Royal Society A: Mathematical, Physical and Engineering Sciences 473, no. 2206 (October 2017): 20170145. http://dx.doi.org/10.1098/rspa.2017.0145.

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In this paper, the comparative analysis of the thermal explosion (TE) critical conditions on the planes temperature–conversion degree and temperature–time was conducted. It was established that the ignition criteria are almost identical only at relatively small values of Todes parameter. Otherwise, the results of critical conditions analysis on the plane temperature–conversion degree may be wrong. The asymptotic method of critical conditions calculation for the first-order reactions was proposed (taking into account the reactant consumption). The degeneration conditions of TE were determined. The calculation of critical conditions for specific first-order reaction was made. The comparison of the analytical results obtained with the results of numerical calculations and experimental data showed that they are in good agreement.

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29

Higham, Desmond J., and Raya Khanin. "Chemical Master versus Chemical Langevin for First-Order Reaction Networks." Open Applied Mathematics Journal 2, no. 1 (June 3, 2008): 59–79. http://dx.doi.org/10.2174/1874114200802010059.

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30

Rademacher, Jens D. M. "First and Second Order Semistrong Interaction in Reaction-Diffusion Systems." SIAM Journal on Applied Dynamical Systems 12, no. 1 (January 2013): 175–203. http://dx.doi.org/10.1137/110850165.

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31

Darowicki, K., and P. Ślepski. "Dynamic electrochemical impedance spectroscopy of the first order electrode reaction." Journal of Electroanalytical Chemistry 547, no. 1 (April 2003): 1–8. http://dx.doi.org/10.1016/s0022-0728(03)00154-2.

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32

Sheplev, V. S., S. A. Treskov, and E. P. Volokitin. "Dynamics of a stirred tank reactor with first-order reaction." Chemical Engineering Science 53, no. 21 (November 1998): 3719–28. http://dx.doi.org/10.1016/s0009-2509(98)00164-x.

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33

Amo-Salas, Mariano, Raúl Martín-Martín, and Licesio J. Rodríguez-Aragón. "Design of experiments for zeroth and first-order reaction rates." Biometrical Journal 56, no. 5 (May 19, 2014): 792–807. http://dx.doi.org/10.1002/bimj.201300210.

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34

Gitterman, Moshe, and George H. Weiss. "A class of exactly solvable reaction-diffusion equations with first-order distributed reaction rates." Chemical Physics Letters 193, no. 6 (June 1992): 469–72. http://dx.doi.org/10.1016/0009-2614(92)85833-v.

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35

Coppens, Marc-Olivier, and Gilbert F. Froment. "Diffusion and reaction in a fractal catalyst pore—II. Diffusion and first-order reaction." Chemical Engineering Science 50, no. 6 (March 1995): 1027–39. http://dx.doi.org/10.1016/0009-2509(94)00479-b.

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36

Selimović, Enisa, and Tanja Soldatović. "Study on the reactions between dichlorido[2,2′:6′,2″-terpyridine] zinc(II) and biologically relevant nucleophiles in aqueous solution." Progress in Reaction Kinetics and Mechanism 44, no. 2 (April 22, 2019): 105–13. http://dx.doi.org/10.1177/1468678319825724.

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Substitution reactions of square-pyramidal [ZnCl2(terpy)] complex (terpy = 2,2′:6′,2″-terpyridine) with biologically relevant nucleophiles such as imidazole, glutathione, 1,2,4-triazole, and pyrazine were investigated at pH 7.0 as a function of nucleophile concentration. The reactions were followed under pseudo first-order conditions by UV-Vis spectrophotometry. The substitution reactions comprised two steps of consecutive displacement of chlorido ligands. Different reaction pathways for the first reaction step of nucleophilic substitution were defined. The order of reactivity of the investigated nucleophiles for the first reaction was imidazole > glutathione > pyrazine > 1,2,4-triazole, while for the second reaction step it was pyrazine > 1,2,4-triazole > imidazole > glutathione.

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37

Fellner, Klemens, Wolfang Prager, and Bao Q. Tang. "The entropy method for reaction-diffusion systems without detailed balance: First order chemical reaction networks." Kinetic & Related Models 10, no. 4 (2017): 1055–87. http://dx.doi.org/10.3934/krm.2017042.

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38

Favorite, Jeffrey A. "SENSMG: First-Order Sensitivities of Neutron Reaction Rates, Reaction-Rate Ratios, Leakage,keff, andαUsing PARTISN." Nuclear Science and Engineering 192, no. 1 (July 23, 2018): 80–114. http://dx.doi.org/10.1080/00295639.2018.1471296.

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39

Tsao, Heng-Kwong. "Diffusion into a pair of reactive spheres with first-order reaction." Journal of Chemical Physics 114, no. 23 (June 15, 2001): 10247–51. http://dx.doi.org/10.1063/1.1375138.

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40

STRAJA, SORIN. "PARAMETERS ESTIMATION FOR A FIRST ORDER IRREVERSIBLE REACTION. A STOCHASTIC APPROACH." Chemical Engineering Communications 124, no. 1 (June 1993): 165–75. http://dx.doi.org/10.1080/00986449308936184.

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41

OLIVER, D. L. R., and K. J. DE WITT. "MASS TRANSFER TO A DROPLET WITH A FIRST-ORDER CHEMICAL REACTION." Chemical Engineering Communications 135, no. 1 (May 15, 1995): 63–69. http://dx.doi.org/10.1080/00986449508936338.

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42

Mitrovic, Bojan M., and Dimitrios V. Papavassiliou. "Effects of a first-order chemical reaction on turbulent mass transfer." International Journal of Heat and Mass Transfer 47, no. 1 (January 2004): 43–61. http://dx.doi.org/10.1016/s0017-9310(03)00380-6.

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43

Retsloff, David G., Paul C.-H. Chan, and B. Youssef Bisbis. "Sequential bifurcations, maximum multiplicity, and chaos for a first order reaction." Mathematical and Computer Modelling 11 (1988): 370–74. http://dx.doi.org/10.1016/0895-7177(88)90517-1.

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44

Frisch, H. L. "Diffusion with first-order reaction with a time-dependent rate coefficient." Journal of Colloid and Interface Science 153, no. 1 (October 1992): 292–93. http://dx.doi.org/10.1016/0021-9797(92)90320-l.

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45

Li, Genyuan, and Herschel Rabitz. "Determination of constrained lumping schemes for nonisothermal first-order reaction systems." Chemical Engineering Science 46, no. 2 (1991): 583–96. http://dx.doi.org/10.1016/0009-2509(91)80018-t.

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46

Caballero, N. B., A. E. Croce, E. Pensa, and C. Vicente Irrazábal. "The analytical resolution of parallel first- and second-order reaction mechanisms." International Journal of Chemical Kinetics 42, no. 9 (June 22, 2010): 562–66. http://dx.doi.org/10.1002/kin.20502.

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47

Sun, Yunwei, Thomas A. Buscheck, and Yue Hao. "Modeling reactive transport using exact solutions for first-order reaction networks." Transport in Porous Media 71, no. 2 (April 13, 2007): 217–31. http://dx.doi.org/10.1007/s11242-007-9121-8.

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48

Antić, V. V., M. P. Antić, M. N. Govedarica, and P. R. Dvornić. "Kinetics of the Formation of Poly(Methyldecylsiloxane) by Hydrosilylation of Poly(Methylhydrosiloxane) and 1-Decene." Materials Science Forum 555 (September 2007): 485–90. http://dx.doi.org/10.4028/www.scientific.net/msf.555.485.

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Poly(methylhydrosiloxane) [PMHS], prepared by siloxane equilibration reaction, was used for the hydrosilylation with 1-decene to obtain poly(methyldecylsiloxane) [PMDS]. Pt(0)-1,3- divinyltetramethyldisiloxane complex was used as a catalyst for hydrosilylation reaction. In order to investigate the kinetics of the formation of PMDS, a series of experiments was performed at different reaction temperatures (from 48 to 64 °C) with catalyst concentrations of 7.0 · 10-7 mol of Pt per mol of CH=CH2. All reactions were carried out in bulk, with equimolar amounts of the reacting Si-H and CH=CH2 groups. The course of the reactions was monitored by following the disappearance of the Si-H bands by quantitative infrared spectroscopy. The obtained results show that an induction period occurs at lower reaction temperatures and that the rate of Si-H conversion follows the first-order kinetics.

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49

Fan, Xiaoming. "Exponential Attractor for a First-Order Dissipative Lattice Dynamical System." Journal of Applied Mathematics 2008 (2008): 1–8. http://dx.doi.org/10.1155/2008/354652.

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We construct an exponential attractor for a first-order dissipative lattice dynamical system arising from spatial discretization of reaction-diffusion equations in . And we obtain fractal dimension of the exponential attractor.

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50

Yusnimar. "KINETIC MODELING STUDY FOR ACYLATION REACTION OF O-XYLENE TO 3,4-DIMETHYLBENZOPHENONE OVER H-BETA." Jurnal Riset Kimia 1, no. 1 (February 11, 2015): 89. http://dx.doi.org/10.25077/jrk.v1i1.100.

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ABSTRACTThe reaction of o-xylene with benzoic anhydride has been studied by the changing molar ratio of the reactants (20:1, 10:1, and 5:1) in a batch reactor under reaction temperature 120oC. The reaction carried out without catalyst and also with catalyst Zeolite beta which was activated at 300oC overnight. HPLC analysis results showed that the yield of the product increase with the changing molar ratio of the reactants. An attempt was made in determining the kinetics of the reaction. The results show that the reaction is neither first nor second order in the acylating agent. Obtaining the reaction order even initially is unsuitable for even simple reactions that do not go to completion. It is even less applicable where more than a single process which affects the rate is taking place right from the start. These might be any one or combination of diffusion, adsorption, desorption, inhibition of the reaction by the product and multi step reactions on the surface. Postulated reaction mechanisms may be required in combination with experimental data to determine even initial reaction orders. Key words: o-xylene, catalyst, kinetics, reaction order.

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