1,2-dichloroethane, thermodynamic propertie

Li, J.C.M., Pitzer, K.S. (1956) The thermodynamic properties of 1,1-dichloroethane heat capacities from 14 to 294 K, heats of fusion and vaporization, vapor pressure and entropy of the ideal gas. The barrier to internal rotation. J. Am. Chem. Soc. 78, 1077-1080. 

Our present knowledge of the helix-coil transition in synthetic polypeptides, with particular reference to the poly-y-benzyl-h-glutamate-dichloroacetic acid-1,2-dichloroethane system, is briefly reviewed. Recent results concerning the effect of solvent composition and of polypeptide and solvent deuteration on the thermodynamic properties of the transition show that both the thermodynamics and presumably the molecular mechanism of the transition are generally more complicated than had been previously supposed. 

Table 9 Calculated and observed thermodynamic properties of 1,2-dichloroethane...

Chao, J.-P. Zhang, F.-Q. Dai, M. Studies of thermodynamic properties of binary mixtures containing an alcobol.XVIII. Excess molar enthalpies of each of (one of the four butanols -t trichloromethane or 1,2-dichloroethane) J. Chem. Thermodyn. 1992,24... 

Despite the favorable properties of acetonitrile as a solvent, its use for equilibrium acidity measurements has its definite limitations. The pK range that is tolerable is limited at the high end by onset of solvent deprotonation, and at the low end by substrate autodissociation, as has been implicated for HCo(CO)4 [14a] and TpCr(CO)3H [22b]. These limitations can be overcome by the choice of a less polar solvent, e.g. 1,2-dichloroethane (DCE), dichloromethane, or THE. To make reliable, quantitative comparisons of thermodynamic data obtained in different solvents, it is necessary to link the acidity scales and electrode potential references in the different solvents. This has all too often proven to be a far from trivial task. Although, in principle, 1 1 relationship between the acidity scales in different solvents never exists, pK differences between closely related compounds are often almost constant when compared in different solvents. This is because their solvation properties are similar, because of similarities in size and charge distribution. In less... 

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