Liquid-liquid-vapor immiscibility limits in carbon dioxide + n-paraffin mixtures

1985 ◽  
Vol 30 (1) ◽  
pp. 82-88 ◽  
Author(s):  
David J. Fall ◽  
Jaimie L. Fall ◽  
Kraemer D. Luks
Keyword(s):  
Carbon Dioxide ◽  
Liquid Vapor

Liquid-vapor equilibria of the hydrogen-carbon dioxide system

1968 ◽  
Vol 13 (2) ◽  
pp. 168-171 ◽  
Author(s):  
J. O. Spano ◽  
C. K. Heck ◽  
P. L. Barrick
Keyword(s):  
Carbon Dioxide ◽  
Liquid Vapor

Molecular dynamics investigations of liquid–vapor interaction and adsorption of formaldehyde, oxocarbons, and water in graphitic slit pores

2014 ◽  
Vol 16 (29) ◽  
pp. 15289-15298 ◽  
Author(s):  
Pei-Hsing Huang ◽  
Shang-Chao Hung ◽  
Ming-Yueh Huang
Keyword(s):  
Carbon Dioxide ◽  
Molecular Dynamics ◽  
Carbon Monoxide ◽  
Fundamental Interaction ◽  
Adsorption Study ◽  
Vapor Adsorption ◽  
Adsorption Behaviors ◽  
Slit Pores ◽  
The Ideal ◽  
Liquid Vapor

We report a multi-component liquid–vapor adsorption study that allowed us to predict the ideal adsorption conditions and to explore the fundamental interaction and adsorption behaviors for formaldehyde, carbon dioxide, carbon monoxide, and water mixtures in GR slit pores.

Carbon and Oxygen Isotope Fractionation of Pressurized CO2 as a Function of Temperature

2020 ◽  
Author(s):  
Tracey Jacksier ◽  
Rick Socki
Keyword(s):  
Phase Transition ◽  
Carbon Dioxide ◽  
Elevated Temperatures ◽  
Isotopic Fractionation ◽  
Oxygen Isotope Fractionation ◽  
Cold Temperatures ◽  
Carbon And Oxygen Isotope ◽  
To Come ◽  
Gas Expansion ◽  
Liquid Vapor

<p>During liquid-vapor phase transition, CO<sub>2</sub> can undergo isotopic fractionation in both C and O.  This phase transition can occur during routine cylinder handling, such as gas expansion or while subjecting the cylinder to cold temperatures without allowing the cylinders to come to thermal equilibrium prior to use. </p><p>This work examines the isotope changes for both C and O in a series of controlled experiments on dual phase (liquid-vapor) and single-phase (vapor only) carbon dioxide contained in pressurized gas cylinders at sub-freezing, ambient and elevated temperatures.  The isotopic values were measured during the temperature equilibration from either cold or elevated temperatures to room temperature.  Isotopic values were observed to vary when the gas was at sub-freezing temperatures but not from elevated temperatures.  Stable isotope practitioners, who rely on pressurized carbon dioxide as a working IRMS laboratory reference gas, will find this work useful.</p>

Phase Behavior and Its Effects on Reactions in Liquid and Supercritical Carbon Dioxide

2004 ◽  
Author(s):  
Lynnette A. Blanchard ◽  
Gang Xu
Keyword(s):  
Carbon Dioxide ◽  
Melting Point ◽  
Vapor Pressure ◽  
Phase Behavior ◽  
Critical Point ◽  
Pressure Curve ◽  
Light Component ◽  
Vapor Pressure Curve ◽  
Solid Liquid ◽  
Liquid Vapor

Carbon dioxide, either as an expanded liquid or as a supercritical fluid, may be a viable replacement for a variety of conventional organic solvents in reaction systems. Numerous studies have shown that many reactions can be conducted in liquid or supercritical CO2 (sc CO2) and, in some cases, rates and selectivities can be achieved that are greater than those possible in normal liquid- or gas-phase reactions (other chapters in this book; Noyori, 1999; Savage et al., 1995). Nonetheless, commercial exploitation of this technology has been limited. One factor that contributes to this reluctance is the extremely complex phase behavior that can be encountered with high-pressure multicomponent systems. Even for simple binary systems, one can observe multiple fluid phases, as shown in Figure 1.1. The figure shows the pressure–temperature (PT) projection of the phase diagram of a binary system, where the vapor pressure curve of the light component (e.g., CO2) is the solid line shown at temperatures below TB. It is terminated by its critical point, which is shown as a solid circle. The sublimation curve, melting curve, and vapor pressure curve of the pure component 2 (say, a reactant that is a solid at ambient conditions) are the solid lines shown at higher temperatures on the right side of the diagram; that is, the triple point of this compound is above TE. The solid might experience a significant melting point depression when exposed to CO2 pressure [the dashed–dotted solid/liquid/vapor (SLV) line, which terminates in an upper critical end point (UCEP)]. For instance, naphthalene melts at 60.1 °C under CO2 pressure (i.e., one might observe a three-phase solid/liquid/vapor system), even though the normal melting point is 80.5 °C (McHugh and Yogan, 1984). To complicate things even further, there will be a region close to the critical point of pure CO2 where one will observe three phases as well, as indicated by the dashed–dotted SLV line that terminates at the lower critical end point (LCEP). The dotted line connecting the critical point of the light component and the LCEP is a vapor/liquid critical point locus.

Solid-liquid-vapor phase behavior of the methane-carbon dioxide system

AIChE Journal ◽  
1962 ◽  
Vol 8 (4) ◽  
pp. 537-539 ◽  
Author(s):  
J. A. Davis ◽  
Newell Rodewald ◽  
Fred Kurata
Keyword(s):  
Carbon Dioxide ◽  
Phase Behavior ◽  
Vapor Phase ◽  
Solid Liquid ◽  
Methane Carbon ◽  
Liquid Vapor

Study of Liquid–Liquid and Liquid–Liquid–Vapor Equilibria for Crude Oil Mixtures with Carbon Dioxide and Methane Using Short-Wave Infrared Imaging: Experimental and Thermodynamic Modeling

2020 ◽  
Vol 34 (11) ◽  
pp. 14109-14123
Author(s):  
Jose F. Romero Yanes ◽  
Hosiberto B. de Sant’Ana ◽  
Filipe X. Feitosa ◽  
Magali Pujol ◽  
Julien Collell ◽  
...  
Keyword(s):  
Carbon Dioxide ◽  
Crude Oil ◽  
Thermodynamic Modeling ◽  
Infrared Imaging ◽  
Short Wave ◽  
Oil Mixtures ◽  
Short Wave Infrared ◽  
Liquid Vapor
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