Excess enthalpies of binary solvent mixtures of N,N-dimethylacetamide with aliphatic alcohols

Molar excess enthalpies of binary mixtures of [tributyl phosphate+{CH3(CH2)nOH (n=0 to 3)}] at 298.15K

“…As the carbon number of the alcohol increases, the excess molar enthalpy also increases. This order is similar to many references for the binary mixture between low molar mass aliphatic alcohols and other polar component [20,[24][25][26][27][28][29][30][31]. It should be pointed out that in general methanol and other aliphatic alcohols have the same thermodynamic behavior (i.e.…”

“…It should be pointed out that in general methanol and other aliphatic alcohols have the same thermodynamic behavior (i.e. the excess molar enthalpies are both negative or both positive) in the binary mixture of aliphatic alcohols with other component [20,[24][25][26][27][28][29][30][31]. Only a little literature reported the difference thermodynamic behavior between methanol and other aliphatic alcohols [31].…”

(Vapour+liquid) equilibrium in (N,N-dimethylacetamide+methanol+water) at the temperature 313.15 K

“…Note that the absolute values of Q ¼ G E =RT are small, especially for (amide + water) mixtures. This is in contrast with the heat of mixing data: for the aqueous mixtures, the mixing process is strongly exothermic [16][17][18][19][20][21], and for the amide mixtures with methanol, the thermal effects are comparatively large as well [21][22][23][24][25][26]. Thus we can draw two conclusions.…”

Preferential solvation in {amide + alcohol} binary mixtures. : Part 2. The N-methylpyrrolidinone + methanol mixture at T = 313.15 K: thermodynamic results and molecular dynamics calculations

“…This is in contrast with the experimental heat of mixing data for {amide + methanol} mixtures. The H E values at equimolar composition are: [28][29][30][31][32][33] +258 J mol À1 for NMF, À101 J mol À1 for DMF, À77 J mol À1 for NMA, À737 J mol À1 for DMA (all the data at 313.15 K), À650 J mol À1 for NMP (at 298.15 K), and +44 J mol À1 for 2PY (at 303.15 K), and these values indicate strong intermolecular interactions in the solution. Hence we conclude that intermolecular interactions between molecules lead mainly to the orientation effects within solvation shell, but its composition remains unchanged.…”