LXXIII.—Determinations of vapour-pressures of alcohols and organic acids, and the relations existing between the vapour-pressures of the alcohols and organic acids

Richardson, Arthur P.

doi:10.1039/ct8864900761

Cited by 26 publications

(14 citation statements)

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“…It is important to stress that these parameters were obtained in this way because the Q-electrolattice EOS reduces to the MTC EOS in the absence of electrolytes. Figure 1 shows that the vapor pressures of pure methanol (Ramsay and Young, 1887;Young, 1909) and pure ethanol (Richardson, 1886;Kalafati et al, 1967;Mousa, 1987;Diogo et al 1995;Khoiroh and Lee, 2011) are in good agreement with the experimental data in the studied temperature range. Figure 2 shows that the methanol liquid density (Gmehling, 2012) tends to be underestimated at temperatures below 290 K, while for the ethanol (Gmehling, 2012) this occurs below 280 K. In addition, the ethanol liquid density is slightly overestimated above 300 K.…”

Section: Pure Solventssupporting

confidence: 74%

Thermodynamic Properties of Nonaqueous Single Salt Solutions Using the Q-Electrolattice Equation of State

Zuber

Checoni

Castier

2015

Braz. J. Chem. Eng.

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-The correlation of thermodynamic properties of nonaqueous electrolyte solutions is relevant to design and operation of many chemical processes, as in fertilizer production and the pharmaceutical industry. In this work, the Q-electrolattice equation of state (EOS) is used to model vapor pressure, mean ionic activity coefficient, osmotic coefficient, and liquid density of sixteen methanol and ten ethanol solutions containing single strong 1:1 and 2:1 salts. The Q-electrolattice comprises the lattice-based Mattedi-Tavares-Castier (MTC) EOS, the Born term and the explicit MSA term. The model requires two adjustable parameters per ion, namely the ionic diameter and the solvent-ion interaction energy. Predictions of osmotic coefficient at 298.15 K and liquid density at different temperatures are also presented.

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Section: Pure Solventssupporting

confidence: 74%

Thermodynamic Properties of Nonaqueous Single Salt Solutions Using the Q-Electrolattice Equation of State

Zuber

Checoni

Castier

2015

Braz. J. Chem. Eng.

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“…As can be seen on Fig. 1 all available vapor pressures for glycerol are remarkably consistent (except for [14]). Richardson [14], measure vapor pressures of glycerol in a broad temperature range with the Ramsay and Young method.…”

Section: Evaluation Of Vapor Pressures Of Glycerolsupporting

confidence: 65%

“…2. It has turned out, that practically all available vapor pressure data (except of few low temperature points from [14] as discussed above) fit very well in the arc-like representation, proving their high consistency.…”

Section: Evaluation Of Vapor Pressures Of Glycerolmentioning

confidence: 72%

“…1is not informative enough. More detailed insight in the quality of vapor pressures measured with different methods [14,[16][17][18][19][20][21][22][23][24][25] can be obtained from the "arc representation" developed by Oonk et al [26][27][28].The main idea of this approach is to collect all available data in a possibly broad temperature range and to approximate vapor pressures at the beginning and the end of the temperature range with the linear equation.…”

Section: Evaluation Of Vapor Pressures Of Glycerolmentioning

confidence: 99%

“…Much research has been done on the vaporization of glycerol since 1886 [14]. We have carefully collected and analyzed the available vapor pressure temperature dependencies (see Fig.…”

Section: Evaluation Of Vapor Pressures Of Glycerolmentioning

confidence: 99%

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Thermodynamic properties of glycerol: Experimental and theoretical study

Verevkin

Zaitsau

Emel′yanenko

et al. 2015

Fluid Phase Equilibria

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Viscosity of liquids

Albright

Lohrenz

1956

AIChE Journal

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Three viscosity correlations were tested for liquids at their boiling points. Compounds studied included normal paraffins, branched-chain hydrocarbons, aromatics, halogenated methanes and ethanes, water, and aliphatic alcohols. The correlations were tested for the most part with viscosity and thermodynamic data found in the literature. Some experimental viscosity measurements were made, however, for normal paraf3ns from pentane to octane at temperatures up to about 300"F., which is higher than has previously been reported.Two correlations are based on Eyring's theory of absolute reaction rates. The third is based on the compressibility factor of the saturated liquid, and this correlation is unique, as all available data for normal paraffins with eight or more carbon atoms are represented by a single curve. The three correlations presented here can be used to extrapolate viscosity data over large temperature ranges up to the critical temperature. Logical predictions of the viscosities of related compounds are possible.The theory of absolute reaction rates (17) was applied to the viscosity of liquids by Eyring and coworkers (16, 18, 22, 27, 39). It was postulated that before a molecule can flow (move) a "hole" must be available for it to move into. Energy is required to make this hole, and the following equation was developed to represent the relationship between the free energy of activation and the viscosity in centipoises:Since a flow process can be considered to be at constant volume, the energy required to make a hole the size of a molecule is the internal energy of vaporization. It was thought (22, 39) that the relationship between the internal energy of vaporization and the free energy of activation might be significant. The ratio of these two values has been designated the energy ratio n: Lylo F. .4lbright is at Purdue Universit W y t Lafayette, Indiana, and John Lohrens at t k University of Kansan, Lawrence, Kanaas.TEYERATLRZ. T Fig. 1. Vis-osity measurements of lightparaffin hydrocarbon liquids at their boiling points. Page 290This energy ratio was reported (22, 39)to be equal to approximately 2.45 for numerov liquids including water, alcohols, and hydrocarbons. The alcohols and hydrocarbons tested or the temperatures of any of the liquids however were not specified. Since at the critical temperature the internal energy of vaporization is zero and since the free energy of activation is still presumably finite, the energy ratio is also probably zero at this temperature. It appears, therefore, that the energy ratio is a function of temperature. Another equation (22) based on the theory of absolute reaction rates is as follows: temperature over a large pressure range within about 30% accuracy. As far as can be determined, however, the equation was tested for a given compound a t only one temperature. Viscosity data have been extrapolated frequently in the past by means of the following plots: (1) viscosity vs. temperature, (2) logarithm of viscosity vs. the reciprocal of absolute temperature, and (3) logarit...

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LXXIII.—Determinations of vapour-pressures of alcohols and organic acids, and the relations existing between the vapour-pressures of the alcohols and organic acids

Abstract: of Vapour-pressures of Alcohols and Organic Acids, and the Relations existing between the Tapour-pressuq-es of the Alcohob and Organic Acids.

Cited by 26 publications

References 0 publications

Thermodynamic Properties of Nonaqueous Single Salt Solutions Using the Q-Electrolattice Equation of State

Thermodynamic Properties of Nonaqueous Single Salt Solutions Using the Q-Electrolattice Equation of State

Thermodynamic properties of glycerol: Experimental and theoretical study

Viscosity of liquids

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