Enthalpies of dilution of aqueous solutions of formamide, acetamide, propionamide, andN,N-dimethylformamide

Wood, Robert H.; Hiltzik, L. H.

doi:10.1007/bf00650136

Cited by 69 publications

(13 citation statements)

References 12 publications

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“…Also given in Table 3 are the values of hi, evaluated according to the group contribution method, following the same procedure used by Savage and Wood (6) and considering biuret as the sum of an "amide" and of a "urea group". Table 3 also contains the value for the "urea group" recalculated more recently by Wood and Hiltzik (27). Even considering biuret as the sum of two "urea groups" the disagreement was beyond the limits of uncertainty (f 220 J mol-I (mol kg-')-') found by those authors for other substances.…”

Section: Resultsmentioning

confidence: 89%

Excess enthalpies of aqueous solutions of biuret at 25 °C. Interaction with urea

Barone¹,

Cacace²,

Castronuovo³

et al. 1981

Can. J. Chem.

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The heats of dilution in water of biuret and the heats of mixing of biuret with urea have been determined by flow microcalorimetry at 25 °C. The excess enthalpies obtained from the experimental data can be expressed as virial expansions of the molalities.The value of the cross interaction coefficient hUB is compared to that calculated through the empirical relation hUB2 = (hUUhBB). The agreement between the two values outlines the strict analogy in the behaviour of these two solutes. The cited combining rule, verified up to now for pairs of solutes having both hii, hjj > 0, is here applied for the first time to a pair having hii, hjj < 0.

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Section: Resultsmentioning

confidence: 89%

Excess enthalpies of aqueous solutions of biuret at 25 °C. Interaction with urea

Barone¹,

Cacace²,

Castronuovo³

et al. 1981

Can. J. Chem.

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“…As for alcohols [18,20], alkylamides [21,22] and alkylureas [23][24][25][26], the excess thermodynamic properties of aqueous solutions of peptides seem to be determined by the existence of weak, non-bonding, water-mediated interactions [7][8][9][10][11][12][13]. The hydrophobic interactions, like the polar ones, make favourable contributions to the free energy coefficients, which are overall negative.…”

Section: Resultsmentioning

confidence: 95%

“…However, especially in determining the positive values of hxr for such "mixed" solutes bearing both alkyl groups and polar functions, an important role is also played by the "mixed interactions" polar-apolar, as outlined by Wood and coworkers [21,22].…”

Section: Resultsmentioning

confidence: 97%

Chiral recognition of enantiomeric peptides in water at 25° by calorimetry

Barone

Castronuovo

Elia

et al. 1985

Journal of Thermal Analysis

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The heats of dilution in water of binary and ternary solutions of the two enantiomeric forms of N-acetylalanineamide have been measured at 25°. The excess enthalpies, expressed as virial expansion series, permit evaluation of the pairwise self and cross enthalpic coefficients. As for the chiral forms of some monosaccharides, the cross coefficient for the interaction between the D and L forms of N-acetylalanineamide is slightly but significantly different from the corresponding self coefficient. A weak, water-mediated chiral recognition can be assumed to exist between pairs of amide molecules. © 1985 Wiley Heyden Ltd., Chichester and Akadémiai Kiadó, Budapest

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“…It was calculated by the Savage-Wood method, according to which the hydrophobic effect of CH 2 -group is taken to be unity. The effect of CH 3group corresponds to 1.5CH 2 , and the effect of CHgroup is equal to 0.5CH 2 [31,32]. Movement from AlaAla to an AlaβAla molecule and then to βAlaβAla is accompanied by a drop in h xy , indicating enhancement of the intermolecular interactions between AC (DMSO) molecules and AlaβAla and βAlaβAla molecules.…”

Section: Resultsmentioning

confidence: 99%

Dependence of the enthalpies of alanyl-alanine dissolution on the composition of mixed water + acetone and water + DMSO solvents at 298.15 K

Smirnov

Badelin

2015

Russ. J. Phys. Chem.

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The enthalpies of dissolution of two dipeptides, DL-α-alanyl-β-alanine and β-alanyl-β-alanine, in mixed solvents H 2 O + acetone (AC) and H 2 O + dimethyl sulfoxide (DMSO) are measured via calorimetry at an organic component concentration of x 2 = 0-0.25 mole fraction at 298.15 K. The standard enthalpies of dissolution ( ) and the transfer ( ) of dipeptides from water to the mixed solvent and the enthalpic coefficients of pairwise interactions (h xy ) with AC and DMSO molecules are calculated from these data. The effect the composition of aqueous organic mixtures has on the enthalpy characteristics of the dissolution of DL-α-alanyl-β-alanine and β-alanyl-β-alanine is considered. A comparative analysis of h xy values is performed for alanine dipeptides in the investigated mixed solvents.

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Enthalpies of dilution of aqueous solutions of formamide, acetamide, propionamide, andN,N-dimethylformamide

Cited by 69 publications

References 12 publications

Excess enthalpies of aqueous solutions of biuret at 25 °C. Interaction with urea

Excess enthalpies of aqueous solutions of biuret at 25 °C. Interaction with urea

Chiral recognition of enantiomeric peptides in water at 25° by calorimetry

Dependence of the enthalpies of alanyl-alanine dissolution on the composition of mixed water + acetone and water + DMSO solvents at 298.15 K

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