Kinetics Of Reactions In Solution Research Articles

Analysis of solvent effects on the kinetics of reactions in solution using Kirkwood-Buff integral functions: alkaline hydrolysis of the diazabutadiene complex tris[glyoxal bis(methylimine)]iron(II) complex and spontaneous hydrolysis of 4-methoxyphenyl 2,2-dichloropropionate in water + 2-methyl-2-propanol mixtures at 298.2 K

ADVERTISEMENT RETURN TO ISSUEPREVArticleNEXTAnalysis of solvent effects on the kinetics of reactions in solution using Kirkwood-Buff integral functions: alkaline hydrolysis of the diazabutadiene complex tris[glyoxal bis(methylimine)]iron(II) complex and spontaneous hydrolysis of 4-methoxyphenyl 2,2-dichloropropionate in water + 2-methyl-2-propanol mixtures at 298.2 KMichael J. Blandamer, N. J. Blundell, J. Burgess, H. J. Cowles, J. B. F. N. Engberts, I. M. Horn, and P. Warrick Jr.Cite this: J. Am. Chem. Soc. 1990, 112, 19, 6854–6858Publication Date (Print):September 1, 1990Publication History Published online1 May 2002Published inissue 1 September 1990https://doi.org/10.1021/ja00175a018RIGHTS & PERMISSIONSArticle Views96Altmetric-Citations10LEARN ABOUT THESE METRICSArticle Views are the COUNTER-compliant sum of full text article downloads since November 2008 (both PDF and HTML) across all institutions and individuals. These metrics are regularly updated to reflect usage leading up to the last few days.Citations are the number of other articles citing this article, calculated by Crossref and updated daily. Find more information about Crossref citation counts.The Altmetric Attention Score is a quantitative measure of the attention that a research article has received online. Clicking on the donut icon will load a page at altmetric.com with additional details about the score and the social media presence for the given article. Find more information on the Altmetric Attention Score and how the score is calculated. Share Add toView InAdd Full Text with ReferenceAdd Description ExportRISCitationCitation and abstractCitation and referencesMore Options Share onFacebookTwitterWechatLinked InReddit PDF (599 KB) Get e-Alerts Get e-Alerts

Kinetics of reactions in solutions containing monochloramine and bromide

The reactions of monochloramine in saline solutions containing bromide have been investigated. Monochloramine oxidizes the bromide ion via NH 3Cl + formation. The rate constant for the second-order reaction was found to be 6 ± 1 × 10 4 mol −1 dm 3 s −1 at 25°C. Further rapid reactions follow, resulting predominantly in the formation of NHBr 2 NHBr 2 − and NClBr − at pH ∼ 7. The distribution of these species appears to be thermodynamically controlled and dependent upon the pH, the ionic strength and chloride/bromide ratio. The equilibrium constants at 25°C for NBr 2 − and NClBr − formation with respect to NHBr 2 were estimated to be H +NBr 2 −/[NHBr 2] = 1.3 ± 0.1 × 10 −7 mol dm −3 and H + NClBr − Br −/[NHBr 2] Cl − = 6.1 ± 0.2 × 10 −10moldm −3, respectively. These species decay through a series of reaction steps resulting in nitrogen formation. In unbuffered solutions, these reactions can lower the pH sufficiently for Br 3 − formation to occur.

Theoretical aspects of the application of head-space analysis to the investigation of reaction kinetics in solutions

Theoretical aspects of the application of head-space analysis to the investigation of reaction kinetics in solutions

STOPPED-FLOW X-RAY ABSORPTION SPECTROSCOPY IN DISPERSIVE MODE

new stopped-flow device particularly suitable for X-ray absorption spectroscopy in dispersive mode has been built. Time-resolved measurements of X-ray absorption spectra have been made for reactions in mixed solutions of (i) iron(II1) nitrate and catechol and (ii) iron(II1) nitrate and sodium thiosulfate with time resolutions of -5 ms to a few seconds. Two-step variation of the spectra was observed for the former reaction, while one-step variation for the latter. Introduction Using the energy dispersive X-ray absorption spectrometer/l-3/, a whole profile of an absorption spectrum of interest can be recorded simultaneously without any mechanical motion during the measurement. Thus, the method is suitable for time resolved X-ray absorption spectroscopy. Preliminary results of time resolved experiments using dispersive X-ray absorption spectrometers were reported by Matsushita et a1.141, Fontaine et a1.151 and Sayers et a1.161. In these proceedings Tourillon et a1.171 also give more detailed report on the time-resolved in-situ investigation of the inclusion of metallic aggregates within a conducting polymer using the dispersive EXAFS technique. In the present paper we report the present status of the stopped-flow experiment for kinetic studies of reactions in solutions using the dispersive X-ray absorption spectrometer at the Photon Factory. The stopped-flow method using optical absorption in visible region is an established technique in studying kinetics of reactions in solutions. In the X-ray region, stopped-flow scattering experiments were performed using synchrotron radiationJ8-101. In one/lO/ of these works, a new stopped-flow device having a slit type mixer was developed and used, which give uniform mixing over a large window area of the observation cell. In the previous report/4/, we used this type of device for the preliminary stopped-flow Article published online by EDP Sciences and available at http://dx.doi.org/10.1051/jphyscol:19868104

Hydroxytelechelic polybutadiene, 9. Kinetics of reactions in solution and in bulk between radically obtained hydroxytelechelic polybutadiene and propyl and phenyl isocyanate studied by 1H NMR

AbstractThe kinetics of the reactions of radically obtained hydroxytelechelic polybutadiene (Arco R45M) with propyl isocyanate and phenyl isocyanate were studied by 1H NMR at high field. The reactivities of the three alcohol functions of Arco R45M were found to be different. The three individual reactions follow a 3rd order law and are accelerated by autocatalysis. There is competition between (OH, OH) auto‐association and (free OH + isocyanate) reactions. As a consequence, rate constants are strongly affected by (OH, OH) association phenomena.

Chapter 8. Kinetics of reactions in solution. Part 2: Fast reactions

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Chapter 8. Kinetics of reactions in solution. Part 1: Carbon acid reactivity

Chapter 8. Kinetics of reactions in solution. Part 1: Carbon acid reactivity

Synthesis and properties of poly (iminohydantoins) and poly (parabanic acids)

A number of poly(iminohydantoins) and poly(parabanic acids) have been prepared by polyaddition of diisocyanates and bis(cyanoformamides) in amidic solvents in the presence of tertiary amines, on using the method of “polymerization casting”. Investigation of reaction kinetics in solution shows that the reaction obeys the rules typical for the interaction of isocyanates with compounds containing active hydrogen. The properties of the resulting polyheteroarylenes have been studied.

Kinetics of reactions in solution: Method for the treatment of data from non-isothermal chemical kinetic experiments

A new method is proposed for the treatment of kinetic data derived from non-isothermal kinetic experiments for the determination of the parameters of the Arrhenius equation. The results obtained from its application show the excellent precision of this method.

Chapter 3. Kinetics of reactions in solution. Part II. Fast reactions

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Chapter 6. Kinetics of reactions in solution. Part I: Carbon acid reactivity

Chapter 6. Kinetics of reactions in solution. Part I: Carbon acid reactivity

Kinetics of reactions in solutions under pressure. 49. Chlorine kinetic isotope effects in the methylation of pyridine and 2,6-lutidine

Pyridine and 2,6-lutidine were methylated with methyl chloride in bromobenzene solution in sealed glass ampoules at 100.0/sup 0/C. The ionic chloride was isolated, purified, and completely reconverted to methyl chloride. Isotope ratios were determined with an isotope ratio mass spectrometer. It appears that the increase in the transition state is a manifestation of the Hammond postulate--the most hindered and slowest reaction possessing the most product-like transition state. 1 table.

Chapter 5. Kinetics of reactions in solution

Chapter 5. Kinetics of reactions in solution

Kinetics of reactions in solutions under pressure. 51. Shape and inversion of an allenic anion

Kinetics of reactions in solutions under pressure. 51. Shape and inversion of an allenic anion

Kinetics of reactions in solutions under pressure. 52. Effect of pressure on concerted and stepwise sigmatropic shifts

Kinetics of reactions in solutions under pressure. 52. Effect of pressure on concerted and stepwise sigmatropic shifts

The influence of an intermediate on reaction kinetics in organometallic systems: Formation of products apparently faster than the disappearance of reactants

In a spectrophotometric study of the kinetics of reactions in solution it is possible to find that products are apparently formed faster than the reactants are used up. This can arise when reaction proceeds via an intermediate in a two-step mechanism as found in many organometallic systems.

Kinetics of reactions in solutions under pressure. XXXVII. Pressure effects in solvolysis and solvolytic fragmentation. A correlation of activation volume with concertedness

Kinetics of reactions in solutions under pressure. XXXVII. Pressure effects in solvolysis and solvolytic fragmentation. A correlation of activation volume with concertedness

An infrared cell with inert windows; the application of a germanium cell to the study of chemical reactions in solution

The use of germanium plates as inert cell windows for i.r. solution spectroscopy is reported. This technique has been used to study reaction kinetics in solution.

Kinetics of reactions in solution under pressure. XXXV. Nature of the intermediates involved in the [2 + 2] cycloaddition to tetracyanoethylene and enol ethers

Kinetics of reactions in solution under pressure. XXXV. Nature of the intermediates involved in the [2 + 2] cycloaddition to tetracyanoethylene and enol ethers

Kinetics of reactions in solution under pressure. XXXVI. Effect of pressure on the [4 + 6] cycloaddition of tropone to cyclopentadiene

Kinetics of reactions in solution under pressure. XXXVI. Effect of pressure on the [4 + 6] cycloaddition of tropone to cyclopentadiene