Decane, 38 Table

Though monomethyl isomers, as a whole, are primary products, the rates of formation of individual members may differ substantially from each other. Furthermore they depend on the degree of conversion. With, e. g., n-decane (Table III) at low degrees of conversion relative rates of formation for 2-methyl-nonane 3-methylnonane 4-methylnonane 5-methylnonane are 1 2 2 1 and shift to 2 2 2 1 at high degrees of conversion. 

Product distributions from the hydrocracking of typical normal paraffins with nickel sulfide on silica alumina catalyst (34, 59) are shown in Figure 1 (n-hexadecane) and Table I (n-decane). Table I also includes results with silica-alumina and with nickel on silica-alumina (discussed later). 

Pyrolysis of bicyclopentanes usually leads to the cleavage of the central C—C bond to give a vibrationally excited diradical, which suffers a consecutive 1,2-H shift (Table 8 entries Ic, 4b, 6b) or subsequent C—C bond cleavage (Table 8 entries 5b, 6b, 9, 10a, b, 12b, 13a, 14, 16). In other cases syn/anti isomerizations of the substrates are observed (Table 8 entries 2e, 4a, 10c). The higher annulated syn/anti-pentacyclo[5.3.0.0 . 0 . 0 ]-decanes (Table 8 entry 18) react preferably by pyrolytic cleavage of the cyclobutane unit, whereas the cyclopropane ring is not affected. 

An interesting example for the kinetic stability of strained alkanes is hexacyclo-[4.4.0.0 . 0 . 0 .0 ]decane (Table 8 entry 21). Despite its strain energy of ca... 

What is the minimum selectivity of decane which must be achieved for profitable operation The values of the materials involved together with their molecular weights are given in Table 4.1. 

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

This is a highly efficient barrier against evaporative losses of volatile compounds, which also improves the peak width of the early eluting compounds. This system has been successfully applied to a group of pesticides, using -decane as the co-solvent and has enabled a group of volatile phosphorus pesticides to be determined (95). The experimental conditions used in this work are shown in Table 13.2. 

Comparison of the IFT results for AOS 1618 samples in entries 2 and 9 indicate that the minor differences in di monosulfonate ratio of these AOS surfactants (entries 1 and 2 in Table 10) would have little effect on deionized water IFT values against decane. 

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

The results in Table 22 for a series of one atmosphere 75 °C foaming experiments indicate the effect of hydrophobe carbon number. The foam stability of C18 AS is greater than that of C16 AS in the absence of an oil phase, in the presence of decane, and in the presence of the decane-toluene mixture. The foam stability of C18 HAS is greater than that of C16 HAS in the absence of an oil phase. In the presence of decane and in the presence of the decane-toluene mixture, the foam stability of the C18 HAS is, if anything, slightly less than that of C16 HAS. This may have been the result of partitioning effects. 

Temperature Effects. The chemical ionization spectra of three paraffins (n-decane, 2,2,3,3-tetramethylhexane (compound 13), and 2,2,5,5-tetramethylhexane (compound 14) have been determined at several different temperatures of the mass spectrometer ionization chamber, and the relative intensities obtained for the MW — 1 ions are give in Table VII. The relative intensities decrease for all three compounds as the temperature increases, in accordance with the behavior found for the chemical ionization spectrum of ethyl-/3-chloropropionate... 

Table 5 shows HDS product distributions over several catalysts prepared by using the molybdenum-nickel cluster 2. Sulfur content in decane was adjusted to 5.0 wt% in these experiments. MoNi/NaY was found to be more active than MoNi/Al203. It is to be noted that during the high temperature pretreatment the original cluster structure would have been changed. However, the high activity of the MoNi/NaY catalyst for benzothiophene HDS is probably due to the formation of active sites derived from this particular mixed metal cluster. 

Reasonable NO conversion can be achieved using n-decane as reductant. In the absence of sulfur dioxide, the catalytic activity is roughly related to the r ucibility of the Cu phase of Cu ions in zeolites the reaction temperature needed to reach 20% NO conversion parallels that of the TPR peak (Table 7). This relation also practically holds for Cu on simple oxides, therefore a redox mechanism in which reduction of Cu + cations is the slow step could account for the results. 

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. 70. NSE spectra for 2% linear h-PI in deuterated n-decane at Q/A 1 values of 0.064 ( ), 0.089 ( ) and 0.115 ( ). The solid lines represent a common fit with the dynamic structure factor of the Zimm model (see Table 1) neglecting possible effects of translational diffusion. (Reprinted with permission from [174]. Copyright 1993 The American Physical Society, Maryland)...

Solvent additives to the melt (Table 3) fall into two categories extractive and reactive. The extractive solvents (decane, perchloroethane, o-dichlorobenzene, and pyrrolidine) had negligible effect on solubility, possibly due to the preferential wetting of the coal by the solvent and exclusion of the ZnCl2 melt. Reactive solvents (anthracene oil, indoline, cyclohexanol, and tetralin) all incorporated strongly. Donor solvents, tetralin and indoline, increase the "corrected solubility, whereas anthracene oil and cyclohexanol have negligible effect. 

The naming of these three heterocyclic fused (5 5 5) ring systems has been carried out according to the IUPAC system of nomenclature. Some examples are given as follows compound la (Table 1) is named (3-hydroxy-4-methoxyphenylthieno[2,3-3]pyrrolizin-8-one. Compound 15a (Table 2) is dithieno[3,2-3 2, 3 - 1thiophene. Compound 23a (Table 2) is dithieno[3,2-3 2, 3 - 1pyrrole. Compound 20a (Table 2) is dithicno[3,2-3 2, 3 -r/]thiophene-4,4-dio ide. Compound 13b (Table 2) is 3,4-dimethyldithieno[3,2-3 2, 3 -i/]thiophene-7,7-dioxide. Compound 38 (Table 4) is fM, r, r-10-azatricyclo[5.2.1.01 10]deca-2,5,8-triene. Compound 39 (Table 4) is cis,cis, m-10-azatricyclo[5.2.1.01 10]deca-2,8-diene. The nomenclature of compound 40 (Table 4) is 1,4,7 triaza tricy-clo[5.2.1.01,10]decane. 

Water retards the sulfoxidation of alkanes [25]. The results of experiments on decane sulfoxidation with addition of water (T=333K, pO2 = 980kPa, [S02]o = 6.2mol L 1, vio=5.0x 10-7 mol L-1 s 1) are given in the following table. The rate of sulfoxidation was observed to increase in time due to the accumulation of alkylsulfonic peracid and, hence, v0 -c vmax. 

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. 

Calculate the temperature at which the vapor pressure of n-decane corresponds to a stoichiometric vapor-air mixture. Compare your result with the value quoted for the firepoint of n-decane in Table 6.1. 

The work of adhesion is influenced by the orientation of the molecules at the interface. For example, with the help of Table A.4.1 and Eq. (A.4.8), the work of adhesion of n-decane-water (corresponding to a paraffinic oil-water system) and of glycerol-water can be computed to be 40 10 3 J nr2 and 56x 10 3 J nr2, respectively. It requires more work to separate the polar glycerol molecules (oriented with the OH groups toward the water) from the water phase than the nonpolar hydrocarbon molecules. For paraffinic oils Woo is about 44 mj nr2, for water Www is 144 mj nr2, and for glycerol Woo is 127 mJ nr2. 

The reaction was originally used by Starks ( ) in his early studies of ptc mechanism. The reaction was monitored by gas-liquid chromatography and decane served both as solvent and internal standard. The reaction was run using a quaternary onium salt, Aliquat 336, and 18-crown-6 for calibration. The rates are shown in Table II. Please note that the relative rate of 1.00 corresponds to an absolute rate at 105 of 1.34 X 10 M-lsec . ... 

Table V. Aryl Displacement using 140-bis-(4-Dihexylaminopyridinium) Decane Dibromide as PTC ...

Table Influence of the addition of methylated /3-cyclodextrin in the two-phase system propylene carbonate/dodecane. Reaction conditions 0.1 mmol [Rh(acac)(CO)2], 0.5 mmol BIPHEPHOS, 19.4 mmol trans-4-octene, 20 ml propylene carbonate, 20 ml do-decane, p(CO/H2 = 1/1) = 10bar, T = 125 °C, t = 4h, stirring velocity 500 rpm...

From the solubility data of n-decane in water, the enthalpy for the process n-decane (H2O) - n-decane (pure) at 25°C has been estimated by Boddard et al. ( ) to be -5.85 kJ moT. Substracting this value from the calculated AH°(25°c) values for CioBMG and C12BMT, in Tables III and IV, the AH (-W) values for micellization and for adsorption at the aqueous solution/air interface at 25 C can be estimated. Values are shown in Table V. 

We have found that emission spectra of the cooperatively excited ADF from upper electronic states and of the one quantum excited PF are different. ADF spectrum is shifted in the longwave direction with respect to PF spectrum (see Table II). The shift effect depends on solvent type. ADF spectral shift is most considerable and comprises 500 cm"l (see Fig. 1) for the case of ZnTPP in decane. 

The comparison of the genuine theoretical results with those predicted by this approximation shows a root-mean-square (rms) deviation of 0.2kcal/mol with those obtained in the HF/6-31G(if) calculations reported in Table 9.1. This result is all the more remarkable as it includes polycychc molecules (15-21), boat-cyclohexane stmctures (15, 21), as well as a twist-boat structure (19, twistane = tricyclo [4.4.00 ]decane). The use of this approximation for ZPE + — Hq in problems... 

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