Carbon dioxide + decane

Kobe Murti determined by Macleod method values a, A, B C for several compds which have been used by Rush Gamson. These compds included ethane, propane, pentane, heptane, cyclohexane, hydrogen, oxygen, benzene, CCI2F2, carbon dioxide, decane and chlorine. The results were similar to those repotted by R G but better correlation was obtd... 

In binaiy mixtures of caibon dioxide and the normal hydrocarbons heavier than C7, coexisting liquid-vapour, liquid-liquid, and liquid-liquid-vapour phase splits have been observed above 273.15 K. Pressure-composition diagrams predicted by the PR equation of state for carbon dioxide/decane mixtures at two different temperatures are shown in Figures 5. At 260 K, binaiy mixtures of carbon dioxide and decane separate into a liquid and a vapour phase at low pressures. As the pressure is increasexl, a value is... 

Figure 3. The pressure composition sections of the binary system carbon dioxide/decane at (a) 260.0 K, with liquid-liquid phase split and (b) 319.3 K. Both figures have been obtained from the PR equation of state. Open ircles are experiments [22].

The interfacial tension behaviour of carbon dioxide/decane mixtures appears to be very interesting due to the formation of the second liquid phase at low temperatures. To see the similarities between the interfacial tension behaviour and the phase behaviour at constant temperature, the interfacial tensions are being presented in a similar way as p-x,y sections in Figure 3. In Figure 4 the relations between pressure, interfacial tension and composition are shown schematically for a system in which a three-phase equilibrium is present. 

To demonstrate how this works in practice, the calculated results are shown in Figures Sa and b for the system carbon dioxide/ decane at 260.0 and 319.3 K. The left branch in Figure Sb represents the interfacial tension as a function of the liquid mole-fraction. The right branch in Figure Sb represents the interfocial tension as a function of the mole-fi action in the vapour phase. It also shows that both branches decrease to zero as the critical point is approached. 

Figure 5. The interfacial tension of carbon dioxide/decane at 260 K (a), and at 319.3 K (b). The solid lines represent the PR equation, while the open circles represent the experimental results [22].

Bipyridylnickel(II) o-carborane-l,2-dicarboxylate eliminated two carbon dioxide molecules in refluxing decane and formed a complex with a QNi three-membered ring [Eq. (99), M = Ni] (107). Both carbon dioxide... 

Chemical/Physical. Complete combustion in air yields carbon dioxide and water vapor. Decane will not hydrolyze because it has no hydrolyzable functional group. 

Several researchers have measured the absorption rate at the presence of dispersed organic phase [1,17-18,37,39,49,51-53]. Bruining et al. [37] measured the oxygen absorption in stirred vessels with plane interface in the presence of small amounts of decane, hexadecane, c = 0.01 - 0.1 while van Ede et al. [49] applied octene as a dispersed phase. Littel et al.[39] used carbon dioxide for absorption in dispersion of toluene droplets with c = 0 - 0.4. The theoretical data in the literature were mostly verified by the experimental results of the above... 

Viscosity " Oxygen (02) b Carbon Dioxide (C02) Methane (CH4)c Helium (He)c Benzene (1 Decane d Acetone ... 

Exercise 4-3 The heat of combustion of 1 mole of liquid decane to give carbon dioxide and liquid water is 1620.1 kcal. The heat of vaporization of decane at 25° is 11.7 kcal mole-1. Calculate the heat of combustion that would be observed for all the participants in the vapor phase. 

The carbon di oxi de/lemon oil P-x behavior shown in Figures 4, 5, and 6 is typical of binary carbon dioxide hydrocarbon systems, such as those containing heptane (Im and Kurata, VO, decane (Kulkarni et al., 1 2), or benzene (Gupta et al., 1 3). Our lemon oil samples contained in excess of 64 mole % limonene so we modeled our data as a reduced binary of limonene and carbon dioxide. The Peng-Robinson (6) equation was used, with critical temperatures, critical pressures, and acentric factors obtained from Daubert and Danner (J 4), and Reid et al. (J 5). For carbon dioxide, u> - 0.225 for limonene, u - 0.327, Tc = 656.4 K, Pc = 2.75 MPa. It was necessary to vary the interaction parameter with temperature in order to correlate the data satisfactorily. The values of d 1 2 are 0.1135 at 303 K, 0.1129 at 308 K, and 0.1013 at 313 K. Comparisons of calculated and experimental results are given in Figures 4, 5, and 6. 

The switching of a switchable solvent (a) Reversible protonation of 1,8-diazabicyclo-[5.4.0]-undec-7-ene (DBU) in the presence of an alcohol and carbon dioxide, (b) Polarity switching in reaction (a), (c) Miscibility of decane with the alcohol-DBU mixture (non-polar) under nitrogen and separation of decane from the ionic liquid (polar) under carbon dioxide. [Reprinted with permission from Nature 2005, 436, 1102. Copyright 2005 Nature Publishing Group.]... 

In Figure 3, heat transfer coefficients are shown for n-pentane--C02 at 8.9 MPa and bulk fluid CO2 mole fractions of 0.830 on the liquid side of the LOST, 0.865 precisely at the LOST, and 0.876 on the vapor side. For comparison, we also show results for pure carbon dioxide at the same bulk temperature and pressure. A similar set of results is shown for n-decane--C02 for each of two pressures in Figures 4 and 5. In Figure 4, at 10.4 MPa, the LOST of 325 K occurs at a CO2 mole fraction x of 0.93 0.02 according to our Peng-Robinson fit of the phase equilibrium data. Thus, only the results for x - 0.973 are clearly on the vapor side of the LOST and only those for x - 0.867 are on the liquid side. In Figure 5, for 12.2 MPa, the LOST has shifted slightly to x - 0.91 + 0.02 and T -335 K. Therefore, we expect the data for x - 0.940 to now be on the vapor side. 

Iodine Potassium Iodide Dodecylbenzene Tridecyibenzene Hydroquinone Propionaldehyde Methylform amide Diacetone Alcohol Isoamyl Alcohol Pentanedione (2,4-) Acetylacetone Paraldehyde Butylaldehyde Butyraldehyde Levulinic Acid Dioctyl Adipate Acetic Acid Butyl Ester Butyl Acetate Dioxane (1,4-) Dioxane Dioxane (p-) Isoamyl Acetate Thiodiacetic Acid Butyl Stearate Santoprene 201-73 Kamax T-260 Adipic Acid Ethylene Chloroformate Caprylic Acid Octanoic Acid Hexamethylenediamine Butyl Carbitol Acetate Decane Carbon Dioxide Dimethylamine Sodium Methylate Freon 114B2 Tetrachloropentane Santicizer 141 Santoprene 201-64 Ecolan Hetron 99P Calcium Hydride Triton Sulfolane Tributyl Phosphate Tributylphosphate Sodium Diacetate Methacrylonitrile... 

Huie, N. C., K. D. Luks, and J. P. Kohn. 1973. Phase-equilibria behavior of systems carbon dioxide-n-eicosane and carbon dioxide-n-decane-n-eicosane. J. Chem. Eng. Data 18 311. 

As we can see from these results, there is very little /i-decane in the vapor. This is because of the large volatility difference between carbon dioxide and n-decane. The three-phase experimental data for this system confirm this behavior. ... 

Various alternative precursor delivery processes have been designed specifically to circumvent the low volatility and low thermal stability problems associated with (Ba(dpm)2 (see Sect. 2.4.1.2). The first method involves the dissolution of Y(dpm)j, Ba(dpm)2 and Cu(dpm)2 precursors in solvents such as butylacetate [188], THF [153, 156], toluene [189], decane [190] and supercritical carbon dioxide [191]. According to this process, termed aerosol-assisted CVD (AACVD), the multicomponent precursor solution is atomized or vaporized into a carrier gas stream or directly into the reaction chamber, with deposition occurring on a heated substrate. Some attractive features of AACVD include deposition at atmospheric pressure, the ability to use thermally sensitive precursors, and a high precursor transport rate [189]. Figure 2-30 shows a sum-... 

Type II have systems have liquid-liquid immiscibility at lower temperatures while locus of liquid-liquid critical point (UCST) is distinct from gas liquid critical line. Examples include water -l- phenol, water -l- tetralin, water -l- decalin, carbon dioxide -l- n-oetane, and carbon dioxide -I- n-decane. 

To test the ability of the gradient method to predict interfacial tensions of binary mixtures, a mixture composed of carbon dioxide and decane will be examined. It must be noted that for the volatile caibon dioxide a temperature independent influence parameter is used, while for decane the linear temperature dependence is used as was suggested in section 2. For mixtures the c parameters of the non-like interactions are related to the pure component values as is shown in Equation 5. 

The main and most important component is the so-caUed 6-gingerol, (5S)-5-hydroxy-l-(4-hydroxy-3-methoxyphenyl)decan-3-one, which represents about 75% of hot substances in oleoresins obtained by extraction with supercritical carbon dioxide. The... 

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