Decane data

Ci2Es-waterKlecane. L + O is microemulsion with excess oil and L + W is the microemulsion and excess water and L is the microemulsion L is the lamellar phase and L3 is the bicontinuous bilayer phase. Figures are adapted from ref [113] and the data taken for 2a from ref [113], 2b from ref [131] and 2c from ref [113] with the decane data in 2c coming from ref [123]. 

It is interesting to note that by replacing octane for pentane both and n° produced minimum at 308 K when aUcanols were butanol, pentanol, and hexanol (data not shown). The value on the other hand exhibited minimum at 308 K for both butanol and hexanol in the case of pentanol, there was a regular increase in K. Digout et al. [42] also studied microemulsion forming systems with nonane and decane (data not shown) as oil, and observed almost similar types of behavior as found for systems with pentane and octane. This simply indicated that chain length of alkanols and hydrocarbon oils have a large say on the overall microemulsion formation and their structures. 

Estimate the surface tension of n-decane at 20°C using Eq. 11-39 and data in Table II-4. 

Using Eqs. VI-30-VI-32 and data from the General References or handbooks, plot the retarded Hamaker constant for quartz interacting through water and through n-decane. Comment on the relative importance of the zero frequency contribution and that from the vuv peak. 

Figure Bl.14.13. Derivation of the droplet size distribution in a cream layer of a decane/water emulsion from PGSE data. The inset shows the signal attenuation as a fiinction of the gradient strength for diflfiision weighting recorded at each position (top trace = bottom of cream). A Stokes-based velocity model (solid lines) was fitted to the experimental data (solid circles). The curious horizontal trace in the centre of the plot is due to partial volume filling at the water/cream interface. The droplet size distribution of the emulsion was calculated as a fiinction of height from these NMR data. The most intense narrowest distribution occurs at the base of the cream and the curves proceed logically up tlirough the cream in steps of 0.041 cm. It is concluded from these data that the biggest droplets are found at the top and the smallest at the bottom of tlie cream.

Solvent polarity also affects the rate of peroxide decomposition. Most peroxides decompose faster in more polar or polari2able solvents. This is tme even if the peroxide is not generally susceptible to higher order decomposition reactions. This phenomenon is illustrated by various half-life data for tert-huty peroxypivalate [927-07-1]. The 10-h half-life temperature for tert-huty peroxypivalate varies from 62°C in decane (nonpolar) to 55°C in ben2ene (polari2able) and 53°C in methanol (polar). 

For R = r-butoxy, the rate data are given for several temperatures in decane. 

The reaction is about 50% faster in ethoxyethanol than in decane. Calculate the activation parameters at 150°C. Although precisely comparable data are not available, for the gas-phase isomerization of norbomadiene is 50kcal/mol. Draw a sketch... 

C. In their first series of experiments, six data sets were obtained for (H) and (u), employing six solvent mixtures, each exhibiting different diffusivities for the two solutes. This served two purposes as not only were there six different data sets with which the dispersion equations could be tested, but the coefficients in those equations supported by the data sets could be subsequently correlated with solute diffusivity. The solvents employed were approximately 5%v/v ethyl acetate in n-pentane, n-hexane, n-heptane, -octane, -nonane and n-decane. The solutes used were benzyl acetate and hexamethylbenzene. The diffusivity of each solute in each solvent mixture was determined in the manner of Katz et al. [3] and the values obtained are included... 

The data in Tables 10, 12-14 indicate that olefinsulfonates customarily exhibit lower IFT values against California heavy stock tank oils than against decane. 

Self-diffusion data [37] derived from NMR PGSE measurements for decane, water, and AOT are illustrated in Fig. 3. The self-diffusion of decane decreases gradually as a decreases from 1.0 to 0.3. The magnitude of decane self-diffusion suggests that the microstructure remains substantially continuous in decane over this composition range. Both water and AOT diffusion initially decrease as a decreases. One can readily see that in this... 

FIG. 3 Self-diffusion coefficients of decane (A), water (B), and AOT ( ) in brine, decane, and AOT microemulsions at 45°C as a function of decane weight fraction, a (relative to decane and brine). Breakpoints in the self-diffusion data for both water and AOT are observed at a = 0.85 and at 0.7. (Reproduced by permission of the American Institute of Physics from Ref. 37.)... 

FIG. 4 Apparent mole fraction (x) water in continuous phase of brine, decane, and AOT microemulsion system derived from the water self-diffusion data of Fig. 3 using the two-state model of Eq. (1). 

FIG. 5 Order parameter for disperse pseudophase water (percolating clusters versus isolated swollen micelles and nonpercolating clusters) derived from self-diffusion data for brine, decane, and AOT microemulsion system of single-phase region illustrated in Fig. 1. The a and arrow denote the onset of percolation in low-frequency conductivity and a breakpoint in water self-diffusion increase. The other arrow (b) indicates where AOT self-diffusion begins to increase. 

Independent self-diffusion measurements [38] of molecularly dispersed water in decane over the 8-50°C interval were used, in conjunction with the self-diffusion data of Fig. 6, to calculate the apparent mole fraction of water in the pseudocontinuous phase from the two-state model of Eq. (1). In these calculations, the micellar diffusion coefficient, D ic, was approximated by the measured self-dilfusion coefficient for AOT below 28°C, and by the linear extrapolation of these AOT data above 28°C. This apparent mole fraction x was then used to graphically derive the anomalous mole fraction x of water in the pseudocontinuous phase. These mole fractions were then used to calculate values for... 

One characteristic of shear banded flow is the presence of fluctuations in the flow field. Such fluctuations also occur in some glassy colloidal materials at colloid volume fractions close to the glass transition. One such system is the soft gel formed by crowded monodisperse multiarm (122) star 1,4-polybutadienes in decane. Using NMR velocimetry Holmes et al. [23] found evidence for fluctuations in the flow behavior across the gap of a wide gap concentric cylindrical Couette device, in association with a degree of apparent slip at the inner wall. The timescale of these fluctuations appeared to be rapid (with respect to the measurement time per shear rate in the flow curve), in the order of tens to hundreds of milliseconds. As a result, the velocity distributions, measured at different points across the cell, exhibited bimodal behavior, as apparent in Figure 2.8.13. These workers interpreted their data... 

Experiments with monkeys given intramuscular injections of a mineral oil emulsion with [l-14C] -hexa-decane tracer provide data illustrating that absorbed C-16 hydrocarbon (a major component of liquid petrolatum) is slowly metabolized to various classes of lipids (Bollinger 1970). Two days after injection, substantial portions of the radioactivity recovered in liver (30%), fat (42%), kidney (74%), spleen (81%), and ovary (90%) were unmetabolized -hexadecane. The remainder of the radioactivity was found as phospholipids, free fatty acids, triglycerides, and sterol esters. Essentially no radioactivity was found in the water-soluble or residue fractions. One or three months after injection, radioactivity still was detected only in the fat-soluble fractions of the various organs, but 80-98% of the detected radioactivity was found in non-hydrocarbon lipids. 

Again at this stage, it cannot be determined exactly how large an excess of decane would be required in order to make Figure 13.7d feasible. This would have to be established from experimental data, but the size of the excess does not change the basic flowsheet structure. 

Ehase Inversion Temperatures It was possible to determine the Phase Inversion Temperature (PIT) for the system under study by reference to the conductivity/temperature profile obtained (Figure 2). Rapid declines were indicative of phase preference changes and mid-points were conveniently identified as the inversion point. The alkane series tended to yield PIT values within several degrees of each other but the estimation of the PIT for toluene occasionally proved difficult. Mole fraction mixing rules were employed to assist in the prediction of such PIT values. Toluene/decane blends were evaluated routinely for convenience, as shown in Figure 3. The construction of PIT/EACN profiles has yielded linear relationships, as did the mole fraction oil blends (Figures 4 and 5). The compilation and assessment of all experimental data enabled the significant parameters, attributable to such surfactant formulations, to be tabulated as in Table II. 

Fig. 69.oNSE spectra of 2% diblock copolymer (d-PS and h-PI blocks) in deuterated n-decane. The Q/A-1 values are 0.026, V 0.032, 0.038, x 0.051, O 0.064, A 0.089, O 0.115. Experimental data and theoretical dynamic structure for breathing modes are compared (solid lines). (Reprinted with permission from [174]. Copyright 1993 The American Physical Society, Maryland)... 

Chirico, R.D, Nguyen, A., Steele, W.V., Strube, M.M. (1989) Vapor pressure of n-alkanes revisited. New high-precision vapor pressure data on ra-decane, ra-eicosane, and n-octacosane. J. Chem. Eng. Data 34, 149-156. 

Dejoz, A., Gonzales-Alfaro, V., Miguel, P.J., Vazquez, M.I. (1996) Isobaric vapor-liquid equilibria for binary systems composed of octane, decane, and dodecane at 20 kPa. J. Chem. Eng. Data 41, 93-96. 

This relationship proves that the influence of solvents (decane, benzene, acetic acid, p-dichlorobenzene) on the rate constant is due to the nonspecific solvation of the reactants and the transition state. The values of the dipole moments of the TS calculated from experimenntal data within the scope of Equation (18.2) have the following values [87] ... 

Calculate the range of temperatures within which the vapor-air mixture above the liquid surface in a can of n-hexane at atmospheric pressure will be flammable. Data are found in Table 4.5. Calculate the range of ambient pressures within which the vapor/air mixture above the liquid surface in a can of n-decane (n-C10H22) will be flammable at 25 °C. 

The coefficients through a7 are generally provided for both high-and low-temperature ranges. Thermodynamic data in CHEMKIN format for liquid decane is given below. 

The non-aqueous system of spherical micelles of poly(styrene)(PS)-poly-(isoprene)(PI) in decane has been investigated by Farago et al. and Kanaya et al. [298,299]. The data were interpreted in terms of corona brush fluctuations that are described by a differential equation formulated by de Gennes for the breathing mode of tethered polymer chains on a surface [300]. A fair description of S(Q,t) with a minimum number of parameters could be achieved. Kanaya et al. [299] extended the investigation to a concentrated (30%, PI volume fraction) PS-PI micelle system and found a significant slowing down of the relaxation. The latter is explained by a reduction of osmotic compressibihty in the corona due to chain overlap. 

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