The Solubility of Propane in Non-polar Solvents.

Thomsen, E.; Gjaldbæk, J. Chr.; Holm, Anu; Nielsen, Per Halfdan; Munch‐Petersen, Jon

doi:10.3891/acta.chem.scand.17-0134

Cited by 13 publications

(5 citation statements)

References 0 publications

Supporting

Mentioning

Contrasting

Order By: Relevance

“…For this type of interaction where exist explicit normative models for maximal, ideal, interaction: transfer of alkanes from aqueous solution to liquid alkanes (see, e.g., Kauzmann, 1959) or, for convenience, to the interior of detergent micelles (Wishnia, 1963). The thermodynamic parameters to be expected for the progressively weaker interactions of alkanes with solvents of increasing polarity (e.g., hexane, benzene, and dioxane, Thomsen and Gjaldbaek, 1963;methanol, ethanol, and 2-propanol, Kretschmer and Wiebe, 1952; among others) are also known.…”

mentioning

confidence: 99%

Thermodynamic basis of induced fit. Specific alkane binding to proteins

Wishnia¹

1969

Biochemistry

View full text Add to dashboard Cite

mentioning

confidence: 99%

Thermodynamic basis of induced fit. Specific alkane binding to proteins

Wishnia¹

1969

Biochemistry

View full text Add to dashboard Cite

“…The notion (Schoenborn et al, 1965) that xenon binding is stabilized by strong London forces arising from the high polarizability of xenon, and is therefore not a hydrophobic interaction, misses the point. The molar polarizability of xenon is not exceptional when compared, say, with ethane: both substances have similar boiling points and similar energies of vaporization per unit volume (Hildebrand and Scott, 1964); both are most soluble in alkanes (it is noteworthy, however, that the solubility of xenon in alkanes is almost double the ideal solubility), and become less soluble as solvent polarity increases (Saylor and Battino, 1958; Thomsen and Gjaldbaek, 1963); it is the transfer to water which is unusual, and which provides the quintes- sential feature of a "hydrophobic interaction," with its characteristic AH, AS, and ACP. The hydrophobe seeks any port in a storm, to get out of the wet.…”

Section: Discussionmentioning

confidence: 99%

Section: Discussionmentioning

confidence: 99%

Substrate specificity at the alkane binding sites of hemoglobin and myoglobin

Wishnia¹

1969

Biochemistry

View full text Add to dashboard Cite

“…It is noted that this temperature is roughly equivalent to the critical temperature of octane (569'K). It appears that neither Equation ( 5 ) nor Equation ( 6 ) can be used without some modification to predict accurately the solubility of ethane in normal paraffin solvents. Although we have used a constant reference temperature in the calculations, yet in fact, a close scrutiny of the experimental data suggested that we could have simply chosen the critical temperature of the particular solvent as the reference temperature and obtained at least an approximate fit of the solubility data.…”

Section: Theoretical Rignificancementioning

confidence: 99%

“…These calculated values together with our experimental solubilities and those of Thomsen and Gjaldbaek are shown in Table 3 . It appears that neither Equation ( 5 ) nor Equation ( 6 ) can be used without some modification to predict accurately the solubility of ethane in normal paraffin solvents. The same general conclusion could be drawn for the solubilities of hydrogen, oxygen, nitrogen, and propane, by referring to the paper published by Thomsen and Gjaldback. Solubilities in normal paraffins predicted by either of the regular solution theory equations deviated generally by more than 10% and as much as 47% from cxperiniental values.…”

Section: Theoretical Rignificancementioning

confidence: 99%

Solubilities of ethane and other gases in normal paraffin solvents

Hayduk

Cheng

1970

Can J Chem Eng

View full text Add to dashboard Cite

The design of a gas solubility apparatus utilizing the basic principle of the Morrison and Billet apparatus is described. The solubilities at atmospheric pressure of ethane in the normal paraffin solvents, hexane, heptane, octane, dodecane and hexadecane, and alm of the same gar in the two-component solvent solutions consisting of hexane and hexadeeane are reported. The solubilities of twelve gases were empirically correlated utilizing one constant for each gas. The empirical equations permit a n estimate of the solubility in any normal paraffin solvent from hexane to hexadecane and for any temperature between 15°C and 40°C from a single solubility measurement. Extrapolation of gas solubilities in normal paraffinsknowledge of the equilibrium solubilities of gases is required for the design of gas-liquid mass transfer equip Because gas solubilities are diffcult to measure accurately, it would be very useful to be able to predict solubilities from a limited number of measurements, and further to extrapolate solubility data from a particular temperature to any other temperature. In their considerable conkibutions to the understanding of solubility, Hilderbrand and Scott(',*) have indicated the possibility of predicting the solubility of a gas in a range of liquids (based on the regular solution theory) and for a range of ternperaturcs, from a single solubility measurement. The application of the regular solution theory for quantitatively predicting gas solubilities in normal paraffins has been only partially succcssful, however, as discussed later. To provide an alternate method for quantitatively estimating gas solubilities in n-paraffins we have formulated a system of empirical equations based on available data and including our own solubility measurements for ethane. These equations appear to represent well all the consistent data available, and should be useful in predicting solubilities to an accuracy of within about 4% (usually better) for any gas for which at least one solubility is known, and for a temperature range at least from 15°C to 40°C. If the logarithm of the (mole fraction) solubility and the logarithm of the absolute temperature could be expected to remain linear, an extrapolation over a widcr temperature range would be possible. Because solubility data are scarce for temperature much below l5OC and much above 4O0C, the accuracy of predictions has not been tested beyond the indicated tenipcrature range.As part of our investigation using n-paraffins, we measured the solubilitics at 2S°C of cthane in hexane, heptane, octane, dodecane and hcxadecanc. To see whether there was some systematic arrangement of gas solubilities in these homologous liquids, we collected from the literature data for various other gases. \ifhen the logarithm of the mole fraction solubility was plotted as the ordinate and the number of carbon atoms in the solvent as tlic absissa, for all the data we obtained, a systematic

show abstract

The Solubility of Propane in Non-polar Solvents.

Cited by 13 publications

References 0 publications

Thermodynamic basis of induced fit. Specific alkane binding to proteins

Thermodynamic basis of induced fit. Specific alkane binding to proteins

Substrate specificity at the alkane binding sites of hemoglobin and myoglobin

Solubilities of ethane and other gases in normal paraffin solvents

Contact Info

Product

Resources

About