Apparent molal heat capacities of aqueous solutions of alkali halides and alkylammonium salts

Rueterjans, H.; Schreiner, F.; Sage, U.; Ackermann, Th.

doi:10.1021/j100724a038

Cited by 97 publications

(43 citation statements)

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“…The literature data were obtained from adiabatic calorimetry measurements, and are based on only three, relatively high concentration (0.498, 1.084, and 1.606mol kg-') of aqueous CsCl (12). The agreement is reasonable, but our e P ( T , m) values are about 5 J K-' mol-' less negative than the +c,(T, m)…”

Section: Experimental (A) General Approachmentioning

confidence: 56%

“…values of Riiterjans et al (12). We believe the reason for the discrepancy at higher temperatures is that the adiabatic calorimetric measurements (12) require vaporization corrections, because both liquid and vapour phases of the sample coexist during the course of C , measurement (12,21).…”

Section: Experimental (A) General Approachmentioning

confidence: 88%

“…High-temperature values Figure 2 shows a comparison of our data for (12). The literature data were obtained from adiabatic calorimetry measurements, and are based on only three, relatively high concentration (0.498, 1.084, and 1.606mol kg-') of aqueous CsCl (12).…”

Section: Experimental (A) General Approachmentioning

confidence: 99%

“…We believe the reason for the discrepancy at higher temperatures is that the adiabatic calorimetric measurements (12) require vaporization corrections, because both liquid and vapour phases of the sample coexist during the course of C , measurement (12,21). The large vaporization corrections at higher temperatures decrease the precision of the measured heat capacities and, consequently, of the +c,(T, m) values (12). The present flow calorimetric method does not require such vaporization corrections (1,13 (12).…”

Section: Experimental (A) General Approachmentioning

confidence: 99%

“…'Co-op student at the University of Victoria, Victoria, B.C., Canada. aqueous 1: 1 species are available at room temperature (7-lo), very few values (4,11,12) are available at higher temperatures. This is because both heat capacity and density measurements at elevated temperatures have been difficult.…”

Section: Introductionmentioning

confidence: 99%

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Apparent molar heat capacities and volumes of aqueous solutions of several 1:1 electrolytes at elevated temperatures

Saluja¹,

Leblanc²,

Hume³

1986

Can. J. Chem.

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. Can. J. Chem. 64,926 (1986). The results of heat capacity (C,) and density (d) measurements at 0.6 MPa and in the temperature range 298.15-373.15 K are presented for several 1:l electrolytes in water. The flow microcalorimeter and densimeter used for these measurements were modificatons of the room-temperature designs. Data were obtained over concentrations ranging from 0.02 to 1 . O mol kg-' (or to the solubility limit, whichever was lower). The heat capacity of a solution relative to that of water was measured with a precision of kO.l mJ K-' g-' at all temperatures. The density of a solution relative to that of water was measured with a precision of ?5 pg ~m -~. These C, and dresults were used to calculate the apparent molar heat capacities, +c,, and volumes, +v, at 298.15, 323.15,348.15, and 373.15 K, at a constant pressure of 0.6 MPa. These results are in good agreement with available literature data.

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Section: Experimental (A) General Approachmentioning

confidence: 56%