Indirect Determination of Vapor Pressures by Capillary Gas–Liquid Chromatography: Analysis of the Reference Vapor-Pressure Data and Their Treatment

2012 ◽  
Vol 57 (5) ◽  
pp. 1349-1368 ◽  
Author(s):  
Květoslav Růžička ◽  
Bohumír Koutek ◽  
Michal Fulem ◽  
Michal Hoskovec
Keyword(s):  
Liquid Chromatography ◽  
Vapor Pressure ◽  
Gas Liquid Chromatography ◽  
Vapor Pressures ◽  
Pressure Data ◽  
Vapor Pressure Data ◽  
Indirect Determination ◽  
Chromatography Analysis

Indirect Determination of Water in Nitroglycerin-Nitrocellulose Pastes by gas-liquid chromatography

1979 ◽  
Vol 4 (2) ◽  
pp. 27-29 ◽  
Author(s):  
J. A. Blanco ◽  
A. O. Rucci ◽  
S. C. Revuelto ◽  
A. A. Dubini ◽  
R. A. Gonzalez
Keyword(s):  
Liquid Chromatography ◽  
Gas Liquid Chromatography ◽  
Indirect Determination

Vaporization Kinetics and Vapor Pressures for Petroleum Fractions Using Thermogravimetry Analysis

2011 ◽  
Vol 236-238 ◽  
pp. 534-537
Author(s):  
Dan Li
Keyword(s):  
Experimental Data ◽  
Vapor Pressure ◽  
Reasonable Agreement ◽  
Pressure Range ◽  
Vapor Pressures ◽  
Pressure Data ◽  
Vapor Pressure Data ◽  
Petroleum Fractions ◽  
Vaporization Process ◽  
Linear Trends

Thermogravimetric analysis (TGA) was extended to the measurements of vaporization kinetics and vapor pressures for three oil samples. The energies of activation for the vaporization process and the enthalpies of vaporization were obtained through the vaporization rates and the vapor pressure data. The experimental data from TGA and comparative ebulliometry are distributed in the same linear trends and are in reasonable agreement. The TGA method is a rapid and practical one for constructing vapor pressure curves, especially at low pressure range, for petroleum fractions. Combination of the TGA and the embulliometry, the vapor pressures in a wide temperature range can be obtained.

A developed equation for predicting the vapor pressure of C-H-O hydrocarbons

2015 ◽  
Vol 40 (3) ◽  
Author(s):  
Mehdi Reiszadeh ◽  
Ehsan Sanjari ◽  
Zahra Jali ◽  
Mohammad Saviz Baktash
Keyword(s):  
Experimental Data ◽  
Vapor Pressure ◽  
Critical Pressure ◽  
Vapor Pressures ◽  
Pressure Data ◽  
Acentric Factor ◽  
Vapor Pressure Data ◽  
Data Points ◽  
Reduced Temperature

AbstractPrediction of the available vapor pressure data in the case of C-H-O hydrocarbons led to derivation and recommendation of standard equations for this property. The accuracy of vapor pressure estimations is essential because it is used as a basis to calculate the acentric factor and the thermal and equilibrium properties. In this study, an accurately developed equation for calculation of vapor pressure is presented for 213 pure C-H-O hydrocarbons as a function of reduced temperature and critical pressure. With this equation, vapor pressures have been calculated and compared with the experimental data reported in the literatures for 213 pure hydrocarbons for more than 3800 data points, and the overall average absolute percentage deviation is only 0.286%. The accuracy of the developed equation has been compared to Antoine, Wagner, and other most used equations, and the comparison indicates that the developed method provides more accurate results than other methods used in this work.

Vapor Pressure Isotope Effects in Liquidand Solid Ammonia

1989 ◽  
Vol 44 (5) ◽  
pp. 359-370 ◽  
Author(s):  
Tseng-Ven King ◽  
Takao Oi ◽  
Anthony Popowicz ◽  
Karl Heinzinger ◽  
Takanobu Ishida
Keyword(s):  
Vapor Pressure ◽  
Cell Model ◽  
Isotope Effects ◽  
Experimental Uncertainty ◽  
Vapor Pressures ◽  
Pressure Data ◽  
Vapor Pressure Data ◽  
Molecular Forces ◽  
External Forces ◽  
Solid Ammonia

The H/D and 14N/15N vapor pressure isotope effects in liquid and solid ammonia have been measured at temperatures between 163 K and 243 K. The isotopic vapor pressure data have been fitted to T ln (P′P) = A/T- B for the liquid/liquid, liquid/solid and solid/solid ranges of temperature. The triple points are; 195.41 K (45.49 torr) for 14NH3, 198.96 K (48.35 torr) for 14ND3, and 195.58 K (48.83 torr) for 15NH3. The isotopic difference in the vapor pressures of NH3 and ND3 at temperatures between 195.41 K and 198.96 K is nearly independent of temperature within the present experimental uncertainty. The phase ratios of the reduced partition function ratios, fliq/fgas and fsol/fgas, deduced from these results are well represented by Tin (fc/fg) = A/T-B. Molecular forces in the liquid and solid ammonias are discussed using a simple cell and a 4-molecular unit cell model, respectively. The librational motions in the liquid are almost as highly hindered as they are in the solid, but the directionality of the external forces on nitrogen atoms in liquid ammonia is not as well defined as in the solid.

The Interaction between Rubber and Liquids. 1. A Thermodynamical Study of the System Rubber-Benzene

1943 ◽  
Vol 16 (1) ◽  
pp. 89-110
Author(s):  
G. Gee ◽  
L. R. G. Treloar
Keyword(s):  
Vapor Pressure ◽  
Solution Temperature ◽  
Free Energies ◽  
Pressure Data ◽  
Heat Of Solution ◽  
Dilute Solutions ◽  
Heat Of Dilution ◽  
Vapor Pressure Data ◽  
Heats Of Dilution

Abstract Equations are developed relating the thermodynamic properties of a mixture of rubber + liquid with the vapor pressure of the liquid above the mixture. Experimental methods are described for the determination of vapor pressure over the whole range of composition of the mixture. By the use of four different methods, it was possible to measure relative vapor pressure lowerings Apo/po° from 2×10−6 to 0.997. Complete vapor pressure data are given for rubber-benzene mixtures at 25° C, together with the calculated Gibbs' free energies of dilution and solution. Temperature coefficient measurements at a number of concentrations are employed to calculate heats of dilution, and these are interpplated by a modified form of an equation due to Langmuir. In this way the heats of dilution and solution are also obtained over the whole range of composition. Combining the heat and free energy data gives the entropies of dilution and solution. The entropy of dilution is approximately twice the heat of dilution over a wide concentration range and, except in dilute solutions (< 5% rubber), both are independent of the molecular weight of the rubber. The entropy of dilution is very much larger than its ideal value, and can be approximately represented by an equation of Flory, though there are significant discrepancies in the region of dilute solutions. The molar heat of solution of rubber is so large that the miscibility of rubber and benzene can be explained only by the anomalously large entropy of solution.

scholarly journals Vapor pressures of phenolic compounds found in pyrolysis oil

2020 ◽  
Author(s):  
Parsa Mozaffari ◽  
Zachariah Baird ◽  
oliver järvik
Keyword(s):  
Phenolic Compounds ◽  
Vapor Pressure ◽  
Test Method ◽  
Measured Temperature ◽  
Pyrolysis Oil ◽  
Vapor Pressures ◽  
Pressure Data ◽  
Scanning Calorimetry ◽  
Vapor Pressure Data ◽  
Density Data

Oil produced from pyrolysis of Kukersi te oil shale and lignocellulosic biomass both contain significant amounts of phenolic compounds. Here we present new experimental vapor pressure data for two such compounds (4-ethyl-2-methoxyphenol and 5-methylresorcinol) and also for a mixture of phenolic compounds extracted from pyrolysis oil (HoneyolTM). Vapor pressure data was measured by high pressure differential scanning calorimetry (DSC), in accordance with the ASTM E 1782 standard test method. The measurements were conducted in the pressure range from 0.89 kPa to atmospheric pressure. The measured temperature ranges for the vapor pressure were 374.5 to 509.1 K for 4-ethyl-2-methoxyphenol, 428.0 to 565.0 K for HoneyolTM and 429.4 to 565.8 K for 5-methylresorcinol. Density data for 4-ethyl-2-methoxyphenol were also measured at 293.15 to 363.15 K. The experimental vapor pressure and density data for 4-ethyl-2-methoxyphenol were fitted using the PC-SAFT equation of state, and the vapor pressure data for the other compounds was fit using the Antoine equation. Enthalpies of vaporization were also calculated. The properties of these compounds were then compared to literature data for other pure phenolic compounds and mixtures of the phenolic compounds from Kukersite shale oil. This comparison indicates that some pure compounds, such as 4-ethyl-2-methoxyphenol, could be used as model compounds for estimating the properties of the phenolic portion of pyrolysis oil.

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