Kinetic solvent

The second-order rate constants for hydration and the kinetic solvent isotope effect for hydration of several 2-substituted 1,3-butadienes ate given below. Discuss the information these data provide about the hydration mechanism. 

In analyzing the behavior of these types of tetrahedral intermediates, it should be kept in mind that proton-transfer reactions are usually fast relative to other steps. This circumstance permits the possibility that a minor species in equilibrium with the major species may be the major intermediate. Detailed studies of kinetics, solvent isotope effects, and the nature of catalysis are the best tools for investigating the various possibilities. 

Tetrahydrofuran (THF) is usually the solvent of choice for poly (acrylates). It is an excellent thermodynamic as well as kinetic solvent, its only drawback being its volatility and flammability. 

FOTi M and RUBERTO G (2001) Kinetic solvent effects on phenolic antioxidants determined by spectrophosometric measiuements, JAgric Food Chem, 49, 342-8. 

The kinetic solvent effect of the liquid-liquid interface is very sensitive to the location where the adsorbed molecules react [6]. The interfacial solvent effect has to be studied more extensively. 

Kinetic solvent isotope effects 268 The TBr scale for bromination 270... 

Information on the mechanism is mainly obtained from kinetic solvent and substituent effects, i.e. from p- and m-values, as discussed below. These coefficients are therefore a composite of p- and m-values for CTC and ionization steps as shown in (9). Obviously, neither Pctc nor mCTC is available... 

Kinetic solvent isotope effect as a measure of electrophilic assistance to bromide ion departure limiting values rate data in ethanol, methanol and their aqueous mixtures using Bentley s TBr scale its decrease corresponds to the involvement of nucleophilic assistance. R = (/caqhtOII//cAcoH)r as a measure of nucleophilic solvent assistance. Model for a limiting bromination mechanism. Ruasse et al. (1991). /Ruasse and Zhang (1984). 9Argile and Ruasse (to be published). Modro et al. (1979). 

Fig. 5 Variation in kinetic solvent isotope effect, k(H20)/A (D20), for the normal proton-transfer reaction (28)...

The kinetic solvent-isotope effects on these reactions are made up of primary and secondary kinetic isotope effects as well as a medium effect, and for either scheme it is difficult to estimate the size of these individual contributions. This means that the value of the isotope effect does not provide evidence for a choice between the two schemes (Kresge, 1973). The effect of gradual changes in solvent from an aqueous medium to 80% (v/v) Me2SO—H20 on the rate coefficient for hydroxide ion catalysed proton removal from the monoanions of several dicarboxylic acids was interpreted in terms of Scheme 6 (Jensen et al., 1966) but an equally reasonable explanation is provided by Scheme 5. 

At low hydroxide-ion concentrations, the rate of approach to equilibrium after a temperature jump decreases as the hydroxide-ion concentration increases. At higher concentrations the reaction becomes first order in hydroxide ion. The value of the kinetic solvent deuterium isotope effect on the reaction shows little variation over the range of hydroxide-ion concentrations studied as shown in Fig. 19. The ratio t-1(H20)/t 1(D20) at a particular concentration of OL (L = H or D) remains within the range 2.0 to 3.0 for OL" concentrations of 0.001 to 0.100 mol dm - 3 and provides little mechanistic information. Similar results were obtained in the original work (Perlmutter-Hayman and Shinar, 1978). 

The quantitative treatment of micellar rate effects upon spontaneous reactions is simple in that the overall effect can be accounted for in terms of distribution of the substrate between water and the micelles and the first-order rate constants in each pseudophase (Scheme 2). The micelles behave as a submicroscopic solvent and to a large extent their effects can be related to known kinetic solvent effects upon spontaneous reactions. It will be convenient first to consider unimolecular reactions and to relate micellar effects to mechanism. 

The effect of micelles on these spontaneous hydrolyses is difficult to explain in terms of kinetic solvent effects on these reactions. Mukerjee and his coworkers have refined earlier methods for estimating apparent dielectric constants or effective polarities at micellar surfaces. For cationic and zwitterionic betaine sulfonate micelles Def is lower by ca 15 from the value in anionic dodecyl sulfate micelles (Ramachandran et al., 1982). We do not know whether there is a direct connection between these differences in effective dielectric constant and the relation between reaction rates and micellar charge, but the possibility is intriguing. 

It is easy to understand the lower reactivity of non-ionic nucleophiles in micelles as compared with water. Micelles have a lower polarity than water and reactions of non-ionic nucleophiles are typically inhibited by solvents of low polarity. Thus, micelles behave as a submicroscopic solvent which has less ability than water, or a polar organic solvent, to interact with a polar transition state. Micellar medium effects on reaction rate, like kinetic solvent effects, depend on differences in free energy between initial and transition states, and a favorable distribution of reactants from water into a micellar pseudophase means that reactants have a lower free energy in micelles than in water. This factor, of itself, will inhibit reaction, but it may be offset by favorable interactions with the transition state and, for bimolecular reactions, by the concentration of reactants into the small volume of the micellar pseudophase. 

Analysis of deacylation by histidinyl-functionalized micelles suggests that the histidinyl group can act both nucleophilically, generating an acylated histidine intermediate, and as a general base. These conclusions are consistent with the kinetic solvent hydrogen isotope effect (Murakami et al., 1981). 

Quite generally, kinetic solvent effects on the Diels-Alder reaction are small, and, in fact, the small solvent effects have been taken as evidence for minor charge separation during the activation process, consistent with a concerted mechanism. 

The 42-residue peptide KO-42 folds in solution into a hairpin helix-loop-helix motif that dimerizes to form a four-helix bundle. On the surface of the folded motif there are six histidines with assigned piC values in the range 5.2 to 7.2 (Fig. 1) and the second-order rate constant for the hydrolysis of mono-p-nitro-phenyl fumarate is 1140 times larger than that of the 4-methylimidazole-cataly-zed reaction at pH 4.1 and 290 K [13]. The reaction mechanism was found to be pH dependent as the kinetic solvent isotope effect was 2.0 at pH 4.7 and 1.0 at pH 6.1 and the pH dependence showed that the reaction rate depended on residues in their unprotonated form with piCj, values around 5. It was thus established that there are functional cooperative reactive sites that contain protonated and unprotonated His residues. 

Kinetic studies of the reaction of Z-phenyl cyclopropanecarboxylates (1) with X-benzylamines (2) in acetonitrile at 55 °C have been carried out. The reaction proceeds by a stepwise mechanism in which the rate-determining step is the breakdown of the zwitterionic tetrahedral intermediate, T, with a hydrogen-bonded four-centre type transition state (3). The results of studies of the aminolysis reactions of ethyl Z-phenyl carbonates (4) with benzylamines (2) in acetonitrile at 25 °C were consistent with a four- (5) and a six-centred transition state (6) for the uncatalysed and catalysed path, respectively. The neutral hydrolysis of p-nitrophenyl trifluoroacetate in acetonitrile solvent has been studied by varying the molarities of water from 1.0 to 5.0 at 25 °C. The reaction was found to be third order in water. The kinetic solvent isotope effect was (A h2o/ D2o) = 2.90 0.12. Proton inventories at each molarity of water studied were consistent with an eight-membered cyclic transition state (7) model. 

CHEMICAL KINETICS SOLVENT-TRAPPED INTERMEDIATES SOLVENT ISOTOPE EFFECT KINETIC ISOTOPE EFFECT Solvent parameter,... 

Kinetic Solvent Isotope Effect A Simple Multipurpose Physical Chemistry Experiment 247... 

Remarkable kinetic solvent effects reportedly occur in the reaction between 138 and acrylonitrile 2 the observed large differences in the activation parameters between chloroform (A// = 5.4 kcal moP AS = — 50.3 eu) and carbon tetrachloride (A// = 22.4 kcal mol AS = + 10.3 eu) have been criticized. ... 

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