The heat capacities and volumes of some low molecular weight amides, ketones, esters, and ethers in water over the whole solubility range

Abstract

The densities and heat capacities per unit volunle of aqueous solutions of propionan~ide, methylacetate, ethylacetate, methylethylketone and diethylketone, and bis(2-ethoxyethy1)ether were measured over the whole solubility range with a flow densirneter and a flow microcalorimeter. Most systems were studied at 10, 25, a n d 40-C. Properties of the pure liquids were also measured whenever possible. The derived apparent molal volumes 6, all decrease with concentration in the water-rich region, except with ethyl acetate which increases at high temperature. !n general the more hydrophobic the solute the niore negative the initial slope.

Apparent molar volumes and apparent molar heat capacities of aqueous tetrahydrofuran, dimethyl sulfoxide, 1,4-dioxane, and 1,2-dimethoxyethane at temperatures from 278.15K to 393.15K and at the pressure 0.35MPa

“…Differences DV / (m, T) and DC p,/ (m, T) in our V / (m, T) and C p,/ (m, T) surfaces for these similar aqueous solutes can be represented by equations (6) and (7): THF arises from the addition of an oxygen atom to the ring. Our DV 2 ðDIOX-THFÞ $ 5:3 cm 3 Á mol À1 is less by 1.7 cm 3 AE mol À1 than the additive contribution of -O-to V 2 reported by Kiyohara et al [21], and is greater than that reported by Roux et al [34] by 1.2 cm 3 AE mol À1 .…”

Enthalpies and Heat Capacities of Ethyl Acetate Solutions in Water and in Several Organic Solvents at 298–318 K

“…2. OurC • p value in water at 298.15 K is found to be in a fair agreement with that reported by Desnoyers et al [10]. However, the temperature dependence of the partial molal heat capacities in our case appears to be greater.…”

“…Black symbols-this work; open symbols-[10]; the lines are the linear description arises both from the large positive enthalpy of alcohol reorganization in the solute solvation shell and from the relatively weak solute-solvent interaction.Thesol H • -f (T ) curves for EtOAc in the solvents studied are fit very well with the following linear dependences: sol H • (Water) = −9.49(0.05) + 0.226(0.04) × 298.15 1 − 298.15 T s f = 0.05 kJ·mol −1 (1) sol H • (DMF) = 0.832(0.01) − 0.0005(0.0003) × (T − 298.15) s f = 0.01 kJ·mol −1 (2) sol H • (Octane) = 6.24(0.01) − 0.0155(0.003) × (T − 298.15) s f = 0.01 kJ·mol −1 (3) sol H • (OctOH) = 7.54(0.01) + 0.0105(0.0003) × (T − 298.15) s f = 0.01 kJ·mol −1…”

Speeds of Sound and Isentropic Compressibilities of n-Alkoxyethanols and Polyethers with Propylamine at 298.15 K

“…All samples were kept in tightly sealed bottles to minimize the absorption of atmospheric moisture and CO 2 , and dried over 0.4 nm molecular sieve to reduce water content. The purity of the liquids were checked by measuring and comparing the densities at 298.15 K with their corresponding literature values [7,[9][10][11][12][13][14][15][16][17][18][19][20] in Table I. Also given in Table I are our measured or literature values of those quantities which were required in the estimation of K s,m , K E S,m , and u D .…”