Travaux du bureau international d'étalons physico-chimiques

Timmermans, Jean; Delcourt, Y.

doi:10.1051/jcp/1928250411

Cited by 77 publications

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“…7 in the temperature range from 190 K to the critical point (466.7 K). [18]; - [89]; - [34]; - [17]; ×- [31] (run-1); ∇- [31] (run-2); - [18]; ♦- [31] (run-3); +- [31] (run-4); - [125,126]; - [20]; - [124]; - [127]; ⊗- [25]; * - [23]; ⊗-this work All reported saturated-density and vapor-pressure data in the immediate vicinity of the critical point display significant scatter that is larger than the author's claimed uncertainties. This is probably due to the sample purity and thermal instability of the DEE molecules.…”

Section: Resultsmentioning

confidence: 99%

Experimental Study of the Thermodynamic Properties of Diethyl Ether (DEE) at Saturation

et al. 2011

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The isochoric heat capacities C V 1 , C V 1 , C V 2 , C V 2 , saturation densities (ρ S and ρ S ), vapor pressures (P S ), thermal-pressure coefficients γ V = (∂ P/∂ T ) V , and first temperature derivatives of the vapor pressure γ S = (dP S /dT ) of diethyl ether (DEE) on the liquid-gas coexistence curve near the critical point have been measured with a high-temperature and high-pressure nearly constant-volume adiabatic piezocalorimeter. The measurements of (C V 1 , C V 1 , C V 2 , C V 2 ) were made in the liquid and vapor one-and two-phase regions along the coexistence curve. The calorimeter was additionally supplied with a calibrated extensometer to accurately and simultaneously measure the PVT , C V VT , and thermal-pressure coefficient, γ V , along the saturation curve. The measurements were carried out in the temperature range from 416 K to 466.845 K (the critical temperature) for 17 liquid and vapor densities from 212.6 kg · m −3 to 534.6 kg · m −3 . The quasi-static thermo-(reading of PRT, T − τ 123 560 Int J Thermophys (2011) 32:559-595 plot) and baro-gram (readings of the tensotransducer, P − τ plot) techniques were used to accurately measure the phase-transition parameters (P S , ρ S , T S ) and γ V . The total experimental uncertainty of density (ρ S ), pressure (P S ), temperature (T S ), isochoric heat capacities (C V 1 , C V 1 , C V 2 , C V 2 ), and thermal-pressure coefficient, γ V , were estimated to be 0.02 % to 0.05 %, 0.05 %, 15 mK, 2 % to 3 %, and 0.12 % to 1.5 %, respectively. The measured values of saturated caloric C V 1 , C V 1 , C V 2 , C V 2 and saturated thermal (P S , ρ S , T S ) properties were used to calculate other derived thermodynamic properties C P , C S , W, K T , P int , H vap , and (∂ V /∂ T ) P of DEE near the critical point. The second temperature derivatives of the vapor pressure, d 2 P S /dT 2 , and chemical potential, d 2 μ/dT 2 , were also calculated directly from the measured one-and two-phase liquid and vapor isochoric heat capacities (C V 1 , C V 1 , C V 2 , C V 2 ) near the critical point. The derived values of d 2 P S /dT 2 from calorimetric measurements were compared with values calculated from vapor-pressure equations. The measured and derived thermodynamic properties of DEE near the critical point were interpreted in terms of the "complete scaling" theory of critical phenomena. In particular, the effect of a Yang-Yang anomaly of strength R μ on the coexistence-curve diameter behavior near the critical point was studied. Extended scaling-type equations for the measured properties P S (T ), ρ S (T ), and (C V 1 , C V 1 , C V 2 , C V 2 ) as a function of temperature were developed.

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Section: Resultsmentioning

confidence: 99%

Experimental Study of the Thermodynamic Properties of Diethyl Ether (DEE) at Saturation

et al. 2011

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“…Such an interpretation is indeed scarcely possible in the case of the system carbon tetrachloride-acetone as described by Wyatt, since his data are presented in graphical form only. But for the systems carbon tetrachloride-chloroform (figure 1) as reported by Kanolt (9) and by Sameshima and Hiramatsu (15), carbon tetrachloride-carbon disulfide as reported by Timmermans (20), and carbon tetrachloride-2,6 lutidine (figure 2) as studied in this laboratory (22), application of solution theory brings out an interesting concordance between the experimental data and the temperature-concentration curve as calculated from the Schróder-LeChatelier equation, as will be shown below.…”

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confidence: 69%

“…transition between the two crystalline modifications of carbon tetrachloride. Since, however, up to the present scarcely more than qualitative explanations (20) have been offered for these facts, it appeared worth while to attempt a quantitative interpretation of the freezing-point data in terms of the theory of the ideal solution. Such an interpretation is indeed scarcely possible in the case of the system carbon tetrachloride-acetone as described by Wyatt, since his data are presented in graphical form only.…”

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confidence: 99%

The Cryoscopic Behavior of Carbon Tetrachloride

Aw¹,

Wj²,

Ci³

1948

J. Phys. Chem.

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“…in vucuo was 0.7904 with a possible error of two or three units in the last figure. In particular this value was indicated by the work of Young (1933) and by that of Timmermans (1928). Timmermans, in his recently published compilation of authoritative values, quotes the value of 0.7904 and a few that are slightly higher.…”

Section: On the Dryness And Density Of Acetone By P Thirion And E Cmentioning

confidence: 94%

On the dryness and density of acetone

Thirion¹,

Craven²

1952

J. Appl. Chem.

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The paper gives the combined experience of a French and a British firm on the relation between the density and water content of good commercial acetone samples. It is confirmed that, in a relative way, density is a good guide to water content but there remains some doubt concerning the density of dry acetone. A figure has been found 0.0005 lower than was previously accepted but still 0.0005 higher than those given recently by American workers. The lower values quoted by American authors may be due to the presence of isopropyl ether. The direct chemical determination of water in acetone by the Smith & Bryant acetyl chloride–pyridine method appears to be reliable and this is recommended. The Karl Fischer method has not yet been made applicable to acetone–water mixtures.

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Travaux du bureau international d'étalons physico-chimiques

Cited by 77 publications

References 0 publications

Experimental Study of the Thermodynamic Properties of Diethyl Ether (DEE) at Saturation

Experimental Study of the Thermodynamic Properties of Diethyl Ether (DEE) at Saturation

The Cryoscopic Behavior of Carbon Tetrachloride

On the dryness and density of acetone

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