Thermodynamic driving force, formation

Our analysis of literature data will focus on two closely related questions about the influence of changes in the relative thermodynamic driving force and Marcus intrinsic barrier for the reaction of simple carbocations with Bronsted bases (alkene formation) and Lewis bases (nucleophile addition) on the values of ks/kp determined by experiment. 

To what extent is the partitioning of simple aliphatic and benzylic a-CH-substituted carbocations in nucleophilic solvents controlled by the relative thermodynamic driving force for proton transfer and nucleophile addition reactions It is known that the partitioning of simple aliphatic carbocations favors the formation of nucleophile adducts (ksjkp > 1, Scheme 2) and there is good evidence that this reflects, at least in part, the larger thermodynamic driving force for the nucleophilic addition compared with the proton transfer reaction of solvent (A dd U Scheme 6).12 21,22,24... 

The more favorable partitioning of [1+ ] to form [l]-OH than to form [2] must be due, at least in part, to the 4.0 kcal mol-1 larger thermodynamic driving force for the former reaction (Kadd = 900 for conversion of [2] to [l]-OH, Table 1). However, thermodynamics alone cannot account for the relative values of ks and kp for reactions of [1+] that are limited by the rate of chemical bond formation, which may be as large as 600. A ratio of kjkp = 600 would correspond to a 3.8 kcal mol-1 difference in the activation barriers for ks and kp, which is almost as large as the 4.0 kcal mol 1 difference in the stability of [1]-OH and [2]. However, only a small fraction of this difference should be expressed at the relatively early transition states for the reactions of [1+], because these reactions are strongly favored thermodynamically. These results are consistent with the conclusion that nucleophile addition to [1+] is an inherently easier reaction than deprotonation of this carbocation, and therefore that nucleophile addition has a smaller Marcus intrinsic barrier. However, they do not allow for a rigorous estimate of the relative intrinsic barriers As — Ap for these reactions. 

From the recent advances the heteroatom-carbon bond formation should be mentioned. As for the other reactions in Chapter 13 the amount of literature produced in less than a decade is overwhelming. Widespread attention has been paid to the formation of carbon-to-nitrogen bonds, carbon-to-oxygen bonds, and carbon-to-sulfur bonds [29], The thermodynamic driving force is smaller in this instance, but excellent conversions have been achieved. Classically, the introduction of amines in aromatics involves nitration, reduction, and alkylation. Nitration can be dangerous and is not environmentally friendly. Phenols are produced via sulfonation and reaction of the sulfonates with alkali hydroxide, or via oxidation of cumene, with acetone as the byproduct. 

An important exception to this regularity is the cyclization of aromatic alkoxides containing aromatic radical moieties. In these cases, C-0 bond formation is not observed, but C-C bond formation is achieved instead. As Galli and Gentili (1998) pointed out, this is primarily due to the unfavorable thermodynamic driving force for C-0 bond formation compared to C-C bond formation. Thus, the photostimulated reaction depicted in Scheme 7.39 results in the formation of a six-membered carbocycle rather than an octa-membered oxa-heterocycle. The carbocycle is formed in 75% yield (Barolo et al. 2006). This product is a precursor to the thalicmidine biomolecule of the alkaloid group. 

Compound 9, which Is not detectably rehydrated by water or attacked by simple alcohols, Is also converted In high yield to cyclic acetals H at 70 C, pointing again to the significant thermodynamic driving force of cyclic acetal formation. This strongly favored acetal reaction Is one explanation for the excellent adhesion performance of this system on cellulosics and glass. 

The same catalytic system as described for the CDC of amines and ni-troalkanes, complemented with C0CI2 as a co-catalyst, also proved efficient for the allylic alkylation via cross-dehydrogenative coupling between various cycloalkenes and diketones (Eq. 9). Again, the exact mechanism or role of the organic peroxide are not known to date, but the formation of water probably provides the thermodynamic driving force for these reactions [121,122]. 

It can be seen that the thermodynamic driving force for carbon formation decreases as temperature increases. Carbon formation from the Boudouard reaction is thermodynamically favored at lower temperatures because this reaction is exothermic. This kind of carbon formation usually dominates at the reactor inlet (or feed lines) where the temperature is lower. However, higher temperatures favor the cracking reaction (7). Therefore it is often desirable to conduct the hydrocarbon reforming at an intermediate temperature where the thermodynamic driving force for carbon formation is minimal. 

There is also a thermodynamic driving force for the formation of elemental carbon for the ATR reaction, when both steam and oxygen are present in the feed. Consider the formation of elemental carbon as follows (this stoichiometry is based on thermal neutrality, AHgoo c = 0 kJ/mol, of the ATR of n-Cig) ... 

For this calculation, a synthetic gasoline is used, consisting of 35% n-Ce, 25% hexene, and 40% xylene. As expected, the results show that as the oxygen concentration ( air ratio ) increases, the thermodynamic driving force for coke formation decreases. Increasing the S/R ratio from zero i.e., POX) to 0.7 also decreases coke formation. Coke is not thermodynamically favored at air ratios above 0.3, which corresponds to temperatures above 850°C. 

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