Vapor-Liquid Equilibria of Hydrocarbon Mixtures

Bromiley, E. C.; Quiggle, D.

doi:10.1021/ie50286a019

Cited by 76 publications

(37 citation statements)

References 2 publications

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“…For this determinination two binary mixtures were used for which the boilingpoint-composition data for the liquid and vapor phases seem to be well known. These were benzene-ethylene chloride [12,13] and heptane-toluene [1], the data for the latter system being apparently more .0020 (1. 40) __ __ • ___ _ • __ consistent and reliable than those for the former.…”

Section: Experimental Results and Conclusionmentioning

confidence: 99%

“…The boiling point increases linearly with increase in D20, the largest deviation of any point from the straight line labeled "liquid" being only a few tenthousandths of 1 0 . This line is represented by the equation (1) in which !1T is the increase in normal boilin~ point accompanying the increase in D 20 . The ease and rapidity WIth which comparisons of boiling points can be made with precision, by means of the ebulliometric technique of ~wi~toslawski, suggests this method as a convenient analytical procedure for following the early stages in the production of heavy water.…”

Section: Experimental Results and Conclusionmentioning

confidence: 99%

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Boiling-point-composition diagram for dilute aqueous solutions of deuterium oxide

Smith¹,

Wojciechowski²

1936

J. RES. NATL. BUR. STAN.

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The differences between the boiling points of dilute aqueous solutions of heavy water and the boiling point of ordinary water were measured in the range from 0.3 to 7 percent of D 20. The boiling p oints were found to increase linearly with increa se in D 20, according to the equation mole % of D20 = 70.9 (tJ.T), where tJ.T is the boiling point in degrees centigrade minus 100. The measmements, made with ebulliometers of the type devised by W. Swi~toslawski, were found to offer a. rapid method for the analysis of solutions of heavy water.The differences between the boiling points and condensation temperatures of the same solutions were measured in a differential ebulliometer which gave a fractionation equivalent to about one theoretical plate. The small separation between the vapor and liquid lines on the boiling-point-composition diagram shows that the separation of heavy water by fractional distillation would require columns of extremely high efficiency.

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Section: Experimental Results and Conclusionmentioning

confidence: 99%

Section: Experimental Results and Conclusionmentioning

confidence: 99%

Boiling-point-composition diagram for dilute aqueous solutions of deuterium oxide

Smith¹,

Wojciechowski²

1936

J. RES. NATL. BUR. STAN.

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“…J., 20, 497 (1926). (3) Coward, Dyer, Morton, and Gaddum, Ibid., 25, 1102 (1931 HE efficient separation of small quantities of close-boiling T liquids is a widely recognized problem of increasing importance. I n order to separate mixtures of hydrocarbons whose boiling points differ by 2' or 3' C. a fractionating column of 80 to 100 theoretical plates is necessary.…”

Section: Discussionmentioning

confidence: 99%

An Efficient Low-Holdup Laboratory Column

Selker¹,

Burk²,

Lankelma³

1940

Ind. Eng. Chem. Anal. Ed.

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DiscussionFrom the graphs presented it is obvious that it is possible to measure the blue color developed with antimony trichloride with accuracy, even though the rate of change in the intensity of color is rapid.An attempt was made to slow down the rate of fading of the blue color through addition of acids, dehydrating agents, or phenols ( 7 ) . Of the materials tried phosphoric acid seemed the most efficient, but its effect was only apparent, since a slight cloudiness developed in the solution that tended to compensate for the fading of the blue color.Fading continued progressively beyond the readings given, although a t a slower rate, but on the more dilute solution was complete in from 5 to 10 minutes.

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“…The data obtained by Bromiley and Quiggle [12] for the analysis of this mixture by refractive index were used. The number of theoretical plates was computed with the aid of the equation derived by Fenske [13], using for the relative volatility, a, the value 1.07 given by Beatty and Calingaert [14].…”

Section: Methodsmentioning

confidence: 99%