Solubility Of Propane Research Articles

Influence of high biomass concentrations on alkane solubilities

Alkane solubilities were measured experimentally for high-density biomass. The resulting Henry's law constants for propane were found to decrease significantly for both dense yeast suspensions and an actual propane-degrading biofilm consortium. At the biomass densities of a typical biofilm, propane solubility was about an order of magnitude greater than that in pure water. For example, a dense biofilm had a propane Henry's law constant of 0.09+/-0.04 atm m(3) mol(-1) compared to 0.6+/-0.1 atm m(3) mol(-1) measured in pure water. The results were modeled with mixing rules and compared with octanol-water mixtures. Hydrogels (agar) and salts decreased the alkane solubility. By considering a theoretical solubility of propane in dry biomass, estimates were made of intrinsic Henry's law constants for propane in pure yeast and biomass, which were 13+/-2 and 5+/-2 atm kg biomass mol(-1) for yeast and biofilm consortium, respectively.

Influence of high biomass concentrations on alkane solubilities

Alkane solubilities were measured experimentally for high-density biomass. The resulting Henry's law constants for propane were found to decrease significantly for both dense yeast suspensions and an actual propane-degrading biofilm consortium. At the biomass densities of a typical biofilm, propane solubility was about an order of magnitude greater than that in pure water. For example, a dense biofilm had a propane Henry's law constant of 0.09 ± 0.04 atm m3 mol−1 compared to 0.6 ± 0.1 atm m3 mol−1 measured in pure water. The results were modeled with mixing rules and compared with octanol-water mixtures. Hydrogels (agar) and salts decreased the alkane solubility. By considering a theoretical solubility of propane in dry biomass, estimates were made of intrinsic Henry's law constants for propane in pure yeast and biomass, which were 13 ± 2 and 5 ± 2 atm kg biomass mol−1 for yeast and biofilm consortium, respectively. © 2000 John Wiley & Sons, Inc. Biotechnol Bioeng 68: 279–284, 2000.

Vapor–liquid equilibrium ratios for hexane at infinite dilution in ethylene+impact polypropylene copolymer and propylene+impact polypropylene copolymer

Vapor–liquid equilibrium ratios ( K w1 ∞ values) for hexane at infinite dilution in propylene+impact polypropylene copolymer (ICP–PP) and ethylene+ICP–PP systems were measured at temperatures 323.2, 343.2 and 363.2 K and pressures up to 2.4 MPa using a chromatographic technique. The solubilities of propylene in polypropylene and those of propylene, ethylene, and hexane in ICP–PP were measured. The PVT properties of the polypropylene and ICP–PP were also studied. These data were used to determine the pure component and binary interaction parameters for the Sanchez–Lacombe equation of state (S–L EOS). The K w1 ∞ values were predicted by using the S–L EOS with binary parameters evaluated by correlation of phase-equilibrium data of binary systems. Good agreement between the experimental and calculated K w1 ∞ values was obtained by optimizing the equation parameters.

Relationships between the chemical structures and the solubility, diffusivity, and permselectivity of propylene and propane in 6FDA-based polyimides

The solubility, diffusivity, and permselectivity of propylene and propane in 40 different polyimides synthesized from 2,2-bis(3,4-decarboxyphenyl)hexafluoropropane dianhydride (6FDA) were determined at 298 K. The influence of the chemical structures on the physical and gas permeation properties of the 6FDA-based polyimides was studied. The solubility of propylene in an unrelaxed volume of a polymer matrix mainly contributes to the total solubility of propylene for various 6FDA-based polyimides. The diffusivity, the permeability of propylene, and the permselectivity in the propylene/propane mixed-gas system depend on the solubility of propylene. This is thought to be associated with the penetrant-induced plasticization effect. 6FDA-based polyimides, which have a high glass-transition temperature and a large fractional free volume, exhibit a high permeability with a relatively low permselectivity. Changing the number of-CH3 substituents in the phenylene linkage and changing the connectivity in the main chain are good ways of controlling the solubility of propylene and the corresponding permselectivity in the propylene/propane mixed-gas system. Some 6FDA-based polyimides restrict the solubility of propylene through the introduction of a -CONH- linkage between the phenylene linkage; the -Cl substituent in the phenylene linkage at the diamine moiety exhibits a high separation performance in the mixed-gas system. The polyimides are potentially useful membrane materials for the separation of propylene and propane in the petrochemical industry.

Solubility of propane in aqueous solutions of sodium dodecyl sulfate–polyacrylamide with and without NaOH

The solubility of propane in aqueous solutions of sodium dodecyl sulfate (SDS)–0.1 wt.% polyacrylamide (PAM) and SDS–0.1 wt.% PAM–NaOH (0.1 mol L-1) has been determined at 298.15, 308.15 and 318.15 K. The concentration of SDS (mSDS) is up to 50 mmol kg-1. The solubility decreases with increasing temperature, and increases linearly with the concentration of SDS above its critical micelle concentration (CMC) or critical aggregation concentration (CAC), indicating that micelles in the solutions solubilize the gas molecules. It was found that the solubilization properties of the micelles bound to PAM and the free micelles are nearly the same. The solubilization property of SDS is changed by addition of PAM, although the solubilizing effect of the polymer alone is not considerable. Addition of NaOH decreases the ability of SDS to solubilize the hydrophobic gas. The standard Gibbs energies for the transfer of propane from bulk phase to the micelle phase are large negative values, indicating that the hydrophobic gas prefers to exist in the hydrophobic interior of the micelles.

Enriched Gas Pressure Cycling Process For Depleted Heavy Oil Reservoirs

Abstract The majority of Canadian heavy oil reservoirs cannot be exploited, after primary production, by thermal recovery as formations are thin or bottom water exists. Thermal process applications to these reservoirs are not promising due to excessive heat losses to the surrounding formations. Solvent vapour extraction process (VAPEX) and other similar processes are faced with major problems, mainly reservoir depletion, existence of channels "wormholes" following primary production and high costs of new horizontal wells, facilities and solvent. The proposed process is based on pressure cycling of depleted heavy oil reservoirs. It involves injection of natural gas with a specified concentration of vapourized propane into a number of wells for a period of time to pressurize the producing channels connected with injection wells and surrounding reservoir volume. After reaching a pressure target, injection is terminated and the blowdown phase is started. Production is continued until most of the effects of the injection phase are diminished, then the cycle is repeated a number of times. The composition of the injected enriched gas is selected based on the expected reservoir pressure range during the pressurizing phase to achieve high solubility of propane in oil. The process involves relatively low injection rates and to be operated at low pressures and has the potential for low injectant losses and effective oil recovery. This paper reviews the proposed enriched gas pressure cycling process and discusses the various mechanisms controlling it. The process appears to be a viable improved recovery method for depleted heavy oil reservoirs if appropriate reservoir conditions can be achieved. Incremental recovery is expected to be dependent on the target application, process design and number of cycles. The process appears to have many attractive features. It is designed to utilize reservoir conditions created by primary recovery. It requires no new wells, utilizes existing wells, requires reasonable volumes of solvent, requires no water treating or major facilities and the associated risk with its application is minimal. Introduction The observed primary production of many heavy oil reservoirs in Alberta and Saskatchewan such as Lindbergh, Frog Lake and many Lloydminister fields, has been significantly higher than predicted by Darcy flow models. Many of these reservoirs produced over 10% of the original-oil-in-place (OOIP) during primary and many of them are currently depleted or approaching depletion. However, at the termination of primary recovery production, 80 to 90% of the OOIP remains in the reservoirs. An economically viable post-primary improved oil recovery process would add substantially to heavy oil reserves. The most efficient method of increasing heavy oil mobility has been reservoir heating by thermal recovery methods, based mainly on steam or air injection. However, the majority of Canadian heavy oil reservoirs cannot be exploited economically after the primary production phase by thermal recovery as formations are thin or bottomwater exists. Over 80% of Canadian heavy oil reservoirs are less than 6.0 m thick(1). Applications of steam processes to these reservoirs, including the steam assisted gravity drainage process (SAGD), are not promising due to excessive heat losses to surrounding formations.

Prediction of Solubility of Nonpolar Gases in Micellar Solutions of Ionic Surfactants

The solubilities of methane, carbon dioxide, ethane, and propane have been determined experimentally at 1 atm partial pressure and 25°C in aqueous solutions of sodium dodecyl sulfate and cetyltrimethylammonium bromide. For this purpose a specially developed apparatus is used, which is relatively simple compared to those reported in the literature hitherto. Above the CMC, the solubility of each gas increases linearly with surfactant concentration indicating micellar solubilization. The degree of solubilization is greatest for propane and decreases in the order propane > ethane > carbon dioxide > methane. Both the length of the alkyl chain and the properties of the head-group region (i.e., the micelle–water interfacial tension) are observed to determine the intramicellar solubility. A method for estimating the solubilities is also proposed based on the rationale that the micellar phase may be represented by a droplet of a “model solvent” into which the solubilizate molecule dissolves as it would in a bulk solvent. The mixture of the solute species and the model solvent is assumed to behave as a regular solution. Accordingly, a characteristic solubility parameter is estimated for the model solvent from the interaction potential between two adjacent surfactant molecules in a micelle. The solubility computed using the regular solution approximation is further corrected for the Laplace pressure that acts across the curved micelle–water interface and generally reduces the intramicellar solubility. It is concluded that for small nonpolar solutes, micellar solubilities may be reasonably well predicted by assuming that the model solvent has a solubilizing capacity (i.e., solubility parameter) close to that of a bulk equivalent alkane.

A model for the solubility of light hydrocarbons in water and aqueous solutions of alkanolamines

A model is presented for correlating the solubility of methane, ethane, and propane in pure water and aqueous solutions of alkanolamines. The model, which can be applied to both liquid and gaseous hydrocarbons, uses a form of Henry's law for the aqueous phase and an equation of state for the non-aqueous phases. It is demonstrated that only a relatively simple modification of the pure water model is required to extend the model for the solubility of hydrocarbons in alkanolamine solutions.

Pure hydrocarbon sorption properties of poly(1-trimethylsilyl-1-propyne) (PTMSP), poly(1-phenyl-1-propyne) (PPP), and PTMSP/PPP blends

Propane and n-butane sorption in blends of poly(1-trimethylsilyl-1-propyne) (PTMSP) and poly(1-phenyl-1-propyne) (PPP) have been determined. Solubilities of propane and n-butane increased as the PTMSP content in the blends increased. This result is consistent with the higher free volume of PTMSP-rich blends and the better thermodynamic compatibility between PTMSP and these hydrocarbons. Propane and n-butane sorption isotherms were well described by the dual-mode model for sorption in glassy polymers. PTMSP/PPP blends are strongly phase-separated, heterogeneous materials. A noninteracting domain model developed for sorption in phase-separated glassy polymer blends suggests that sorption in the Henry's law regions (i.e., the equilibrium, dense phase of the blends) is consistent with the model. However, Langmuir capacity parameters in the blends are lower than predicted from the domain model, suggesting that the amount of nonequilibrium excess free volume associated with the Langmuir sites depends on blend composition. © 1996 John Wiley & Sons, Inc.

Enzyme recovery from reversed micellar solution through formation of gas hydrates

The phase behavior of gas hydrate in reversed micellar solution without as well as with an enzyme were measured using propane and HCFC22 as gas species ,and cytochrome c and α-chymotrypsin as enzymes. Equilibrium pressure without an enzyme decreased as the water to surfactant(AOT) ratio, W 0, decreased like the hydrate-formation from salt containing aqueous solution. After the hydrate was formed, the final value of W 0 were constant(W 0=3 ∼ 4) independent of the initial W 0. By adding HCFC22 and also cooling the reversed micellar solution containing an enzyme and AOT, most of the free water in the pool of the micelle was converted to gas hydrate and caused the desolubilized enzyme to precipitate as a solid phase. Propane could form gas hydrate for the enzyme-containing micellar solution but not result in so much precipitation as HCFC22 because of the small solubility of propane in water. Finally we have proposed a new method for the recovery of enzyme from reversed micellar solution involving precipitation of the enzyme through formation of gas hydrate.

Phase equilibria in binary mixtures of ethane and propane with sunflower oil

The solubility of ethane and propane in sunflower oil has been measured at temperatures between 298 K and 373 K, and pressures up to 8.88 MPa. Partial liquid miscibility was observed, for mixtures of high hydrocarbon concentrations, in the near-critial region of the solvent; the compositions of the coexisting liquid phases were calculated from a mass balance in the equilibrimn cell.

Propane Solubility in Aqueous Mineral Acids (0–100%): a Significant Difference in the Solvating Properties of H 2SO 4, HNO 3 and H 3PO 4

Unexpectedly high differences in propane solubility in the systems HNO 3 –H 2 O (salting-in), H 3 PO 4 –H 2 O (salting-out) and H 2 SO 4 –H 2 O (salting-out at low H 2 SO 4 concentrations and salting-in at high concentrations) have been revealed, and the data quantitatively interpreted within the framework of the previously suggested equation relating the excess amounts of solubility with the molar volume of a system; the general nature of these equations for systems of this type has been demonstrated.

The influence of chain configuration and, in turn, chain packing on the sorption and transport properties of poly(tert‐butyl acetylene)

AbstractA series of poly(tert‐butyl acetylene) (PTBA) polymers was prepared with cis contents, as characterized by 13C NMR spectroscopy, ranging from 44% to 100%. The sorption and transport properties of propane in this systematically varied series were determined by a sensitive gravimetric sorption technique. As the cis content of the polymer increased, propane solubility and diffusivity decreased markedly and the d‐spacing, determined by wide angle x‐ray diffraction spectroscopy, decreased monotonically with increasing cis content, suggesting that higher order molecular structure, related explicitly to configurational variations, may strongly influence chain packing in these rigid, glassy materials and, in turn, sorption and transport properties of small molecules in this polymer series. © 1993 John Wiley & Sons, Inc.

Solubility of carbon dioxide, methane, and propane in silicone polymers. Effect of polymer backbone chains

AbstractThe solubility of carbon dioxide, methane, and propane in poly(dimethyl silmethylene) [(CH3)2SiCH2]x and poly(tetramethyl silhexylene siloxane) [(CH3)2Si (CH2)6Si (CH3)2O]x was measured in the temperature range from 10.0 to 55.0°C and at elevated pressures. The present results are compared with similar measurements made with other silicone polymers. At a given temperature and pressure, the solubility of the above three gases is highest in poly(dimethyl siloxane) (Me2SiO)x. The gas solubility is decreased by either backbone‐chain or side‐chain substitutions of functional groups in (Me2SiO)x which increase the stiffness of the polymer chains and decrease the specific or fractional free volume of the polymers. It is conjectured that a decrease in the free volume of silicone polymers has a greater effect in decreasing the gas solubility than differences in gas/polymer interactions [with the exception of specific interactions (e.g., between CO2 and polar groups in the polymer)]. © 1993 John Wiley & Sons, Inc.

The solubility of propane in 1,2-ethanediol at elevated pressures

The solubility of propane in 1,2-ethanediol has been measured at five temperatures in the range 298.15 K to 398.15 K. Pressures up to 20.3 MPa were used and both (vapor + liquid) and (liquid + liquid) equilibria were observed. At lower temperatures the three-phase pressures were determined. The experimental results have been correlated with the Peng and Robinson equation of state.

Solubility of carbon dioxide, methane, and propane in silicone polymers: Effect of polymer side chains

Journal of Polymer Science Part B: Polymer PhysicsVolume 30, Issue 10 p. 1185-1185 ErrataFree Access Solubility of carbon dioxide, methane, and propane in silicone polymers: Effect of polymer side chains V. M. Shah, V. M. Shah Dept. of Chemical Engineering and Materials Science, Syracuse University, Syracuse, NY 13244Search for more papers by this authorB. J. Hardy, B. J. Hardy Dept. of Chemical Engineering and Materials Science, Syracuse University, Syracuse, NY 13244Search for more papers by this authorS. A. Stern, S. A. Stern Dept. of Chemical Engineering and Materials Science, Syracuse University, Syracuse, NY 13244Search for more papers by this author V. M. Shah, V. M. Shah Dept. of Chemical Engineering and Materials Science, Syracuse University, Syracuse, NY 13244Search for more papers by this authorB. J. Hardy, B. J. Hardy Dept. of Chemical Engineering and Materials Science, Syracuse University, Syracuse, NY 13244Search for more papers by this authorS. A. Stern, S. A. Stern Dept. of Chemical Engineering and Materials Science, Syracuse University, Syracuse, NY 13244Search for more papers by this author First published: September 1992 https://doi.org/10.1002/polb.1992.090301016AboutPDF ToolsRequest permissionExport citationAdd to favoritesTrack citation ShareShare Give accessShare full text accessShare full-text accessPlease review our Terms and Conditions of Use and check box below to share full-text version of article.I have read and accept the Wiley Online Library Terms and Conditions of UseShareable LinkUse the link below to share a full-text version of this article with your friends and colleagues. Learn more.Copy URL Share a linkShare onFacebookTwitterLinked InRedditWechat No abstract is available for this article. Volume30, Issue10September 1992Pages 1185-1185 RelatedInformation

Analysis of gas solubilities in alkanes using a hard sphere equation of state

The one fluid model together with the hard sphere equation of state due to Guggenheim was used to calculate the solubility of argon, xenon, krypton, nitrogen, carbon monoxide, carbon tetrafluoride, sulphur hexafluoride, methane, ethane and propane in various alkanes (C 5–C 30) at a partial pressure of 1 atm and typically between 280 and 350 K. The agreement between theory and experiment is generally quite good. The ξ values obtained from the analysis reflect the strength of intermolecular interaction between unlike molecules.

A phase separation caused by the solubility of butane in 2-methylpropan-2-ol–water mixtures

The solubility of butane and propane at a partial pressure of 101.3 kPa has been measured at 278–335 K in a solvent consisting of water and t-butyl alcohol (2-methylpropan-2-ol), of composition up to 0.08 mole fraction t-butyl alcohol. In the solvent, a phase separation occurs when butane gas dissolves into it at low temperatures, and over a wide composition range. Conditions for this separation have been identified and related to the high solubility of butane in the solvents at atmospheric pressure. The phenomenon is compared to conventional salting-out of non-electrolytes from water.

Solubilities of methane, propane and carbon dioxide in solvent mixtures consisting of water, N,N-dimethylformamide, and N-methyl-2-pyrrolidone

Gas solubility measurements were carried out in a glass apparatus by a synthetic method. The amount of gas absorbed in aqueous solutions of technical solvents was determined at several temperatures and solvent compositions. The experimental results were reduced to Henry, Ostwald, and infinite dilution activity coefficients as a function of temperature and composition of the solute free solvent. Then the enthalpy and entropy of solution were calculated. In addition the molar volumes of the solvent mixtures were measured.

Solubility of hydrogen sulfide, sulfur dioxide, carbon dioxide, propane, and n-butane in poly(glycol ethers)

Data on the solubility of acid and hydrocarbon gases for poly(glycol ethers) are necessary for the development of the University of California, Berkeley, Sulfur Removal Process. An automated gas solubility measurement system was used to collect data on the solubility of hydrogen sulfide, carbon dioxide, propane, and n-butane in a variety of these solvents. The partial pressure of solute gas in these experiments was between 3 and 100 kPa. Correlations for Henry's law coefficients are given as a function of temperature. Gas solubility in the organic solvents decreases when small amounts of water (<6 wt %) are also present. Gas solubility in solvent-water mixtures at the conditions tested is shown to follow a simple mixing rule. An improved correlation is presented for previously published solubility data for sulfur dioxide, which includes the effect of composition as well as temperature on the Henry's law coefficient.