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Journal articles on the topic 'Alkanol'

Author: Grafiati

Published: 4 June 2021

Last updated: 4 March 2023

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1

Koch, Daniel J., Mike M. Chen, Jan B. van Beilen, and Frances H. Arnold. "In Vivo Evolution of Butane Oxidation by Terminal Alkane Hydroxylases AlkB and CYP153A6." Applied and Environmental Microbiology 75, no. 2 (November 14, 2008): 337–44. http://dx.doi.org/10.1128/aem.01758-08.

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ABSTRACT Enzymes of the AlkB and CYP153 families catalyze the first step in the catabolism of medium-chain-length alkanes, selective oxidation of the alkane to the 1-alkanol, and enable their host organisms to utilize alkanes as carbon sources. Small, gaseous alkanes, however, are converted to alkanols by evolutionarily unrelated methane monooxygenases. Propane and butane can be oxidized by CYP enzymes engineered in the laboratory, but these produce predominantly the 2-alkanols. Here we report the in vivo-directed evolution of two medium-chain-length terminal alkane hydroxylases, the integral membrane di-iron enzyme AlkB from Pseudomonas putida GPo1 and the class II-type soluble CYP153A6 from Mycobacterium sp. strain HXN-1500, to enhance their activity on small alkanes. We established a P. putida evolution system that enables selection for terminal alkane hydroxylase activity and used it to select propane- and butane-oxidizing enzymes based on enhanced growth complementation of an adapted P. putida GPo12(pGEc47ΔB) strain. The resulting enzymes exhibited higher rates of 1-butanol production from butane and maintained their preference for terminal hydroxylation. This in vivo evolution system could be useful for directed evolution of enzymes that function efficiently to hydroxylate small alkanes in engineered hosts.

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2

Jetter, Reinhard, and Markus Riederer. "Cuticular waxes from the leaves and fruit capsules of eight Papaveraceae species." Canadian Journal of Botany 74, no. 3 (March 1, 1996): 419–30. http://dx.doi.org/10.1139/b96-052.

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Cuticular waxes from leaves and fruit capsules of Papaver alpinum sensu Markgr., P. bracteatum Lindl., P. dubium L., P. nudicaule L., P. orientale L., P. rhoeas L., P. somniferum L., and Eschscholtzia californica Cham. were investigated. They consisted of n-alkanes (< 19%), alk-1-ylesters (< 18%), alk-2-ylesters (< 6%), alkanals (< 19%), secondary alkanols (21–71%, mainly nonacosan-10-ol), triglycerides (< 6%), primary alkanols (2–33%), alkanediols (2–23%, mainly isomeric nonacosanediols), alkanoic acids (< 8%), and alkaloids (< 12%). In addition, minor amounts of iso- and anteiso-alkanes, alkanoic acid methyl esters, esters of alkan-10-ols, benzyl- and phenyl-ethylalcohol, triterpenols and phytosterols, ketols, and ketones were detectable. The isomer composition of the secondary alkanols and their alkanediol, ketol, and ketone derivatives is used to deduce the probable sequence of steps in the respective biosynthetic pathways. Keywords: Papaver, Eschscholtzia, Papaveraceae, cuticular wax, secondary alkanols, biosynthesis.

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3

Ives, H. E., and A. S. Verkman. "Effects of membrane fluidizing agents on renal brush border proton permeability." American Journal of Physiology-Renal Physiology 249, no. 6 (December 1, 1985): F933—F940. http://dx.doi.org/10.1152/ajprenal.1985.249.6.f933.

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H+ permeability (PH) of brush border membrane vesicles isolated from rabbit renal cortex was measured from the rate of collapse of preformed pH gradients using acridine orange fluorescence quenching. n-Alkanols increased PH from 0.005 to 0.1 cm/s in a dose-dependent manner. At 25 degrees C, PH increased to 0.01 cm/s at [n-alkanol] = 90 mM (butanol), 30 mM (pentanol), 7 mM (hexanol), and 1.8 mM (heptanol). Activation energy (Ea) of PH was 21.6 kcal/mol (5-50 degrees C), which decreased to 18.5 kcal/mol in the presence of either 200 mM butanol or 12 mM hexanol. Membrane fluidity was estimated from diphenylhexatriene anisotropy (r). n-Alkanols decreased r from 0.25 to 0.18 in a dose-dependent manner. At 25 degrees C, r = 0.22 at [n-alkanol] = 200 mM (butanol), 27 mM (pentanol), 9.5 mM (hexanol), and 2 mM (heptanol). The effects of n-alkanols on PH and r correlated well with known n-alkanol lipid-water partition coefficients. Similar increases in PH and decreases in r were observed for nonalkanol lipid anesthetics. The effects of n-alkanols on the Na+-H+ antiporter and on osmotically driven water transport were also studied. At concentrations of n-alkanol that resulted in a 10-fold increase in PH, there was no significant effect on either Na+-H+ exchange or water transport. These results suggest a lipid pathway for brush border H+ diffusion that is distinct from both the Na+-H+ antiporter and the water transport pathway.

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4

Abraham, Michael H., Joelle le, and William E. Acree. "The Solvation Properties of the Aliphatic Alcohols." Collection of Czechoslovak Chemical Communications 64, no. 11 (1999): 1748–60. http://dx.doi.org/10.1135/cccc19991748.

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Solubilities of solute gases and vapours, as log L, where L is the Ostwald solubility coefficient, in the alkan-1-ols from methanol to decan-1-ol have been correlated through the solvation equation of Abraham. It is shown that there is a regular progression of solvent properties from methanol to decan-1-ol, except for the solvent hydrogen-bond basicity that remains the same along the series, and, indeed, is the same as that of water. A slightly different solvation equation is used to correlate the partition of solutes from water to the dry alkanols. For the longer chain alkanols, the coefficients in the solvation equations approach those in equations for partition from water to the wet (water-saturated) alkanols, showing that the solvation properties of the wet and dry alkanols are quite close for the higher alkanol homologues.

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5

Bao, Xuefei, Xu Li, Chunfeng Jiang, Wei Xiao, and Guoliang Chen. "Recent advances in catalysts for the Henry reaction." Australian Journal of Chemistry 75, no. 10 (November 8, 2022): 806–19. http://dx.doi.org/10.1071/ch22136.

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The Henry reaction, the coupling of a nitro alkane and a carbonyl group, is an important C–C bond-forming reaction giving nitro alkanols, which are useful, versatile intermediates in synthetic organic chemistry and for the pharmaceutical industry. Among the catalysts employed in the Henry reaction, transition metal complex catalysts play an important role. Transition metal complexes, including small molecules and nanoparticles, catalyze the asymmetric Henry reaction efficiently and in most of the cases give chiral nitro alkanol products in good yield and enantiomeric excess. This review summarizes transition metal complex catalysts, metal-free organic catalysts and nanoparticle catalysts for the Henry reaction.

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6

González, Juan Antonio, I. García De La Fuente, and J. C. Cobos. "Thermodynamics of mixtures containing the CO and OH groups. II. DISQUAC predictions on VLE and HE for ternary mixtures containing 1-alkanols, n-alkanones, and one organic solvent." Canadian Journal of Chemistry 75, no. 10 (October 1, 1997): 1424–33. http://dx.doi.org/10.1139/v97-171.

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Thermodynamic properties: vapour–liquid equilibria, VLE, or excess enthalpies, HE, for a set of 21 ternary mixtures of the type 1-alkanol + n-alkanone + organic solvent are studied in the framework of the DISQUAC group contribution model. This treatment is extended to the binaries involved. The DISQUAC analysis is developed on the basis of binary interactions only, that is, ternary interactions are neglected. Most of the interchange coefficients needed are available in the literature. The average relative standard deviations are 0.026 for pressure in the VLE (12 systems) and 0.098 in the HE (9 systems). The discrepancies observed are briefly discussed. Keywords: 1-alkanols, n-alkanones, group contribution, liquids, ternary systems, thermodyamics.

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7

Bhagat, Payal, and Sanjeev Maken. "Study of Intermolecular Interactions of Binary Mixture of sec- and tert-Amines with Alkanols (C1-C3): Refractive Indices." Asian Journal of Chemistry 32, no. 10 (2020): 2443–49. http://dx.doi.org/10.14233/ajchem.2020.22719.

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In this work, the refractive indices (nD) of binary mixture of diisopropylamine (DIPA) and tributylamine (TBA) (as sec- and tert-amines) with alkanol (methanol, ethanol, 1-propanol, 2-propanol) were measured from 298.15 K to 318.15 K. The sec- and tert-amines were selected to study the effect of branching at N-atom of amine on intermolecular interactions with alkanols having different chain length. It was found that the TBA interacts strongly with alkanol in comparison to DIPA due to steric hindrance offered by isopropyl group at N-atom. Various mixing rules were applied to evaluate the refractive index compared well with the experimental refractive indices data for the present binary mixtures. The experimental refractive indices was also fitted to Redlich-Kister polynomial.

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8

González, J. A., U. Domanska, and J. Lachwa. "Thermodynamics of binary mixtures containing a very strongly polar compound — Part 3: DISQUAC characterization of NMP + organic solvent mixtures." Canadian Journal of Chemistry 81, no. 12 (December 1, 2003): 1451–61. http://dx.doi.org/10.1139/v03-159.

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Binary mixtures of 1-methyl pyrrolidin-2-one (NMP) with alkanes, benzene, toluene, 1-alkanol, or 1-alkyne have been investigated in the framework of the DISQUAC model. The reported interaction parameters change regularly with the molecular structure of the mixture components. The model consistently describes a set of thermodynamic properties, including liquid–liquid equilibria, vapor–liquid equilibria, solid–liquid equilibria, and molar excess enthalpies. A brief comparison of the DISQUAC results and those obtained from the UNIFAC and ERAS models is presented. The experimental excess enthalpies are better represented by DISQUAC than by UNIFAC because this quantity strongly depends on molecular structure. For NMP + alkane mixtures, the liquid–liquid equilibria data are also better represented by DISQUAC, while UNIFAC more accurately describes the vapor–liquid equilibria measurements at temperatures close to the critical point. This result suggests that a mean field theory is not able to represent simultaneously, with the same set of interaction parameters, liquid–liquid and vapor–liquid equilibria at the mentioned temperatures. ERAS fails when treating mixtures with 1-alkanols. This has been attributed to the strong dipole–dipole interactions between NMP molecules, characteristic of the investigated systems. Mixture structure is briefly studied in terms of the concentration–concentration structure factor.Key words: thermodynamics, NMP, organic solvent, self-association, dipole–dipole interactions.

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9

Bui, Huong Thi. "\(\textit{n}\)-alkanol stress-induced cell envelope injury of \(σ^{E}\) promoter in \(\textit{Escherichia coli}\)." Academia Journal of Biology 44, no. 2 (June 23, 2022): 91–104. http://dx.doi.org/10.15625/2615-9023/17136.

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To characterize the cellular stress by n-alkanols with different alkyl chain lengths in Escherichia coli, we investigated how n-alkanols damage cell envelope permeability and whether they enhance the promoter activity of the envelope stress response regulator, σE, by using variants of green fluorescent protein (GFP). By using E. coli cells having GFPuv expressing and localizing in the cytoplasm, the inner membrane, and the periplasm, after exposure to n-alkanols, the fluorescent intensity of GFPuv released from cells was examined. Our data showed that at the similar levels of cell death of about 90–97%, ethanol, a short-chain alkanol, at a concentration of 20% damaged the outer membrane more greatly than the inner membrane, whereas a longer-chain alkanol of pentanol at a concentration of 1.125% damaged both of the outer and inner membranes. Then we investigated the envelope stress response to n-alkanols by σE factor by ratiometric analysis of rpoE promoter activity for the downstream GFPuv expression referenced to that of housekeeping sigma 70 (σ70 ) recognizing lacUV5 promoter for red fluorescent protein (RFP) expression. The results indicated that the relative activity of rpoE promoter by pentanol was much greater than that of ethanol. The degree of its sensitization by rpoE deficiency was much more remarkable for cells treated with pentanol than for those with ethanol. The results suggest that the response of the σE plays a significant role in the membrane integrity and survival of E. coli cells treated with n-alkanols depending on the alkyl chain length of the molecule.

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10

Ortega, J., JA Pena, and MI Pazandrade. "Excess Molar Volumes of Binary Mixtures of Ethyl Acetate and Propyl Acetate With Normal Alkanols." Australian Journal of Chemistry 39, no. 10 (1986): 1685. http://dx.doi.org/10.1071/ch9861685.

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This article reports measurements of VE/m at 298.15 K for binary mixtures of n- alkanols CnH2n+1OH (from n = 2 to n = 10) with ethyl and propyl acetates. All the excess volumes are positive over the entire concentration range, with VE/m increasing with the length of the alkanol chain. Suitable equations have been fitted to the data for each mixture. The results are compared with data previously published.

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11

Wolf, Jeremy R. "Main Chain Noncentrosymmetric Hydrogen Bonded Macromolecules Incorporating Aniline, Alkanol, and Alkanoic Acid Hydrogen Bond Donors." Journal of Polymers 2014 (April 27, 2014): 1–7. http://dx.doi.org/10.1155/2014/472901.

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The syntheses and characterization of three noncentrosymmetric main chain hydrogen bonded macromolecules which incorporate aniline, alkanoic acid, and alkanol hydrogen bond donor units are reported. These macromolecules participate in weak intermolecular hydrogen bonding as demonstrated using attenuated total reflectance (ATR) FTIR. The phase transitions of these macromolecules depend on the identity of the hydrogen bond donor.

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12

Piekarski, Henryk, and Gus Somsen. "Enthalpies of solution of urea in water–alkanol mixtures and the enthalpic pair interaction coefficients of urea and several nonelectrolytes in water." Canadian Journal of Chemistry 64, no. 9 (September 1, 1986): 1721–24. http://dx.doi.org/10.1139/v86-284.

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Enthalpies of solution of urea in binary mixtures of isopropanol, s-butanol, and ethoxyethanol with water have been measured at high water content. Those in the binaries isopropanol + water and ethoxyethanol + water show endothermic maxima at 8 and 4 mol% alkanol, respectively. Enthalpic pair interaction coefficients are calculated for the interactions between urea and the alkanols and discussed in connection with these coefficients for interactions between urea and other nonelectrolytes and between N,N-dimethylformamide and several nonelectrolytes. The enthalpic pair interaction coefficients correlate linearly with the heat capacity change on hydration of the nonelectrolytes and with the enthalpy of hydrophobic hydration of the alkanols.

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13

Munk, Petr, Anwei Qin, and Dolly E. Hoffman. "Excess Volumes of Mixtures of Alkanols with Aromatic Hydrocarbons." Collection of Czechoslovak Chemical Communications 58, no. 11 (1993): 2612–24. http://dx.doi.org/10.1135/cccc19932612.

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The excess volumes of twenty binary mixtures of four aromatic hydrocarbons (benzene, toluene, ethylbenzene, and p-xylene) and five linear alkanols (methanol, ethanol, 1-propanol, 1-butanol, and 1-pentanol) at 20 °C are reported. The excess volume of systems with the same alkanol increases with increasing size and number of substituents on the benzene ring. For systems with the same aromatic hydrocarbon it increases with the length of the alkanols. The dependence of ∆V/φ1ϑ2 values on composition is noticeably asymmetric. Systems with benzene as one of the component show larger ∆V/φ1ϑ2 values than other systems and systems with methanol show different compositional dependence patterns.

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14

García, Begoña, Francisco J. Hoyuelos, Rafael Alcalde, and José M. Leal. "Molar excess volumes of binary liquid mixtures: 2-pyrrolidinone with C6–C10n-alkanols." Canadian Journal of Chemistry 74, no. 1 (January 1, 1996): 121–27. http://dx.doi.org/10.1139/v96-016.

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The excess volumes VE of the binary mixtures 2-pyrrolidinone–(C6–C10) n-alkanols have been calculated from density measurements over the whole composition range and the 298.15–318.15 K temperature range. The excess volumes were independent of temperature, but changed noticeably with the chain length of the alkanol. The VE values were only positive starting from heptanol, with the maximum value, 0.239 cm3 mol−1, for equimolar decanol. The observed changeover VE < 0 to VE > 0 suggests that the steric effect is primarily responsible for the positive contributions to VE. The thermal expansion coefficients α were evaluated from the variation of densities with temperature. Key words: excess volumes, 2-pyrrolidinone, n-alkanols, liquid mixtures, hydrogen bonding.

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15

Oswal, S. L., K. D. Prajapati, P. Oswal, N. Y. Ghael, and S. P. Ijardar. "Viscosity of binary mixtures of 1-alkanol+cyclohexane, 2-alkanol+cyclohexane and 1-alkanol+methylcyclohexane at 303.15 K." Journal of Molecular Liquids 116, no. 2 (January 2005): 73–82. http://dx.doi.org/10.1016/j.molliq.2004.05.004.

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16

Kochergin, P. M., I. S. Mikhailova, and E. V. Aleksandrova. "The synthesis of (aminophenyl)alkanols by hydrogenation of (nitrophenyl)alkanol nitroesters." Pharmaceutical Chemistry Journal 32, no. 11 (November 1998): 598–99. http://dx.doi.org/10.1007/bf02465833.

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17

Pardo, J., V. Rodríguez, M. C. López, F. M. Royo, and J. S. Urieta. "Excess molar volumes VEm of (an alkanol + another alkanol) or (hexane + an alkanol) or (an alkanediol + an alkanol or another alkanediol) at the temperature 303.15 K." Journal of Chemical Thermodynamics 24, no. 2 (February 1992): 113–17. http://dx.doi.org/10.1016/s0021-9614(05)80039-4.

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18

González, Juan Antonio, Ángela Mediavilla, Isaías García de la Fuente, José Carlos Cobos, Cristina Alonso Tristán, and Nicolás Riesco. "Orientational Effects and Random Mixing in 1-Alkanol + Alkanone Mixtures." Industrial & Engineering Chemistry Research 52, no. 30 (July 19, 2013): 10317–28. http://dx.doi.org/10.1021/ie4019269.

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19

Casal, Margarida, Helena Cardoso, and Cecília Leão. "Effects of Ethanol and Other Alkanols on Transport of Acetic Acid in Saccharomyces cerevisiae." Applied and Environmental Microbiology 64, no. 2 (February 1, 1998): 665–68. http://dx.doi.org/10.1128/aem.64.2.665-668.1998.

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ABSTRACT In glucose-grown cells of Saccharomyces cerevisiae IGC 4072, acetic acid enters only by simple diffusion of the undissociated acid. In these cells, ethanol and other alkanols enhanced the passive influx of labelled acetic acid. The influx of the acid followed first-order kinetics with a rate constant that increased exponentially with the alcohol concentration, and an exponential enhancement constant for each alkanol was estimated. The intracellular concentration of labelled acetic acid was also enhanced by alkanols, and the effect increased exponentially with alcohol concentration. Acetic acid is transported across the plasma membrane of acetic acid-, lactic acid-, and ethanol-grown cells by acetate-proton symports. We found that in these cells ethanol and butanol inhibited the transport of labelled acetic acid in a noncompetitive way; the maximum transport velocity decreased with alcohol concentration, while the affinity of the system for acetate was not significantly affected by the alcohol. Semilog plots of V max versus alcohol concentration yielded straight lines with negative slopes from which estimates of the inhibition constant for each alkanol could be obtained. The intracellular concentration of labelled acid was significantly reduced in the presence of ethanol or butanol, and the effect increased with the alcohol concentration. We postulate that the absence of an operational carrier for acetate in glucose-grown cells of S. cerevisiae, combined with the relatively high permeability of the plasma membrane for the undissociated acid and the inability of the organism to metabolize acetic acid, could be one of the reasons why this species exhibits low tolerance to acidic environments containing ethanol.

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20

de Ruiz Holgado, M. EF, J. Fernandez, M. I. Paz Andrade, and E. L. Arancibia. "Excess molar enthalpies of mixtures of methyl derivatives of polyethylene glycol with 1-alkanol at 298.15 K and 101.3 kPa." Canadian Journal of Chemistry 80, no. 5 (May 1, 2002): 462–66. http://dx.doi.org/10.1139/v02-044.

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Excess molar enthalpies (H E) of the binary mixtures containing tetraethylene glycol dimethyl ether (TEGDME) or polyethylene glycol 350 monomethyl ether with a 1-alkanol (1-propanol, 1-butanol, or 1-pentanol) at 298.15 K and atmospheric pressure were measured using a Calvet microcalorimeter. All the H E experimental values were positive and increase as the 1-alkanol length increases. The results are discussed qualitatively in terms of molecular interactions. The UNIFAC and DISQUAC group contribution models have been used to compare the predicted and the experimental values.Key words: excess enthalpy, 1-alkanol, polyether, binary system.

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21

Marcus, Y. "Extraction of alkanol isomers." Journal of Organic Chemistry 55, no. 7 (March 1990): 2224–26. http://dx.doi.org/10.1021/jo00294a044.

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22

Lissi, E. A., and E. B. Abuin. "HYDROPHOBIC EFFECTS IN WATER AND WATER/UREA SOLUTIONS A COMPARISON." SOUTHERN BRAZILIAN JOURNAL OF CHEMISTRY 2, no. 2 (December 20, 1994): 71–82. http://dx.doi.org/10.48141/sbjchem.v2.n2.1994.72_1994.pdf.

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The partition of several n-alkanols, from methanol to n-nonanol, between n-hexane and water and between n-hexane and water containing 20 % (w/v) urea has been measured at temperatures ranging from 0 °C to 60 °C. The standard free energy of transfer from water to the urea-containing solution decreases with the length of the alkyl chain, being positive for the small alcohols and negative for the higher alkanols. The same tendency is observed upon all the temperature range considered. On the other hand, the standard entropy of transfer from water to the urea-containing solution increases with the length of the alkyl chain of the alkanol. These results are compatible with a simple description of the urea effect in terms of increasing the entropy of dissolution of the hydrophobic alkyl chain in the aqueous solution.

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23

Lyu, Ruihe, Mohammed S. Alam, Christopher Stark, Ruixin Xu, Zongbo Shi, Yinchang Feng, and Roy M. Harrison. "Aliphatic carbonyl compounds (C<sub>8</sub>–C<sub>26</sub>) in wintertime atmospheric aerosol in London, UK." Atmospheric Chemistry and Physics 19, no. 4 (February 20, 2019): 2233–46. http://dx.doi.org/10.5194/acp-19-2233-2019.

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Abstract. Three groups of aliphatic carbonyl compounds, the n-alkanals (C8–C20), n-alkan-2-ones (C8–C26), and n-alkan-3-ones (C8–C19), were measured in both particulate and vapour phases in air samples collected in London from January to April 2017. Four sites were sampled including two rooftop background sites, one ground-level urban background site, and a street canyon location on Marylebone Road in central London. The n-alkanals showed the highest concentrations, followed by the n-alkan-2-ones and the n-alkan-3-ones, the latter having appreciably lower concentrations. It seems likely that all compound groups have both primary and secondary sources and these are considered in light of published laboratory work on the oxidation products of high-molecular-weight n-alkanes. All compound groups show a relatively low correlation with black carbon and NOx in the background air of London, but in street canyon air heavily impacted by vehicle emissions, stronger correlations emerge, especially for the n-alkanals. It appears that vehicle exhaust is likely to be a major contributor for concentrations of the n-alkanals, whereas it is a much smaller contributor to the n-alkan-2-ones and n-alkan-3-ones. Other primary sources such as cooking or wood burning may be contributors for the ketones but were not directly evaluated. It seems likely that there is also a significant contribution from the photo-oxidation of n-alkanes and this would be consistent with the much higher abundance of n-alkan-2-ones relative to n-alkan-3-ones if the formation mechanism were through the oxidation of condensed-phase alkanes. Vapour–particle partitioning fitted the Pankow model well for the n-alkan-2-ones but less well for the other compound groups, although somewhat stronger relationships were seen at the Marylebone Road site than at the background sites. The former observation gives support to the n-alkane-2-ones being a predominantly secondary product, whereas primary sources of the other groups are more prominent.

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24

Aspée, Alexis, and Eduardo Lissi. "Solubilization of Alkanols in DPPC LUVs: Dependence on the Alkanol Concentration and Topology." Journal of Colloid and Interface Science 175, no. 1 (October 1995): 225–29. http://dx.doi.org/10.1006/jcis.1995.1450.

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25

Bommel, Andrew van, Andrew Glennie, Danielle Chisholm, and Rama M. Palepu. "Dynamics of percolation and energetics in the clustering of water/AOT/oil microemulsions in the presence of ethanol amines." Canadian Journal of Chemistry 84, no. 3 (March 1, 2006): 412–20. http://dx.doi.org/10.1139/v06-011.

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Temperature-induced percolation in water/AOT/oil microemulsions in the presence of mono-, di-, and tri-ethanol amines have been studied using conductometric measurements. The percolation temperature of water/AOT/oil microemulsions depends on the nature of the alkanol amine added. Mono- and di-ethanol amines hinder the percolation process, while triethanol amine promotes the process. Percolation studies were also conducted with varying ω = [H2O]/[AOT] values and varying chain lengths of continuous oil phase (C6C10). The results indicate that increases in both ω and the chain length of the oil decrease the percolation temperature. The microemulsion systems have been analyzed in terms of percolation temperature, scaling equation parameters, and activation energies. The energetic parameters of the clustering process have also been determined employing the phaseseparation model. The influence of alkanol amines on the percolation phenomenon has been rationalized in terms of the changes in fluidity of the interfacial layer, the viscosity of the water micropool, and the attractive interactions of the microemulsion droplets. The influence of the alkanol amine additives on the stated parameters was discussed in view of the individual effects of the alcohol and amine moieties on the properties of water/AOT/oil microemulsions.Key words: microemulsion, percolation, conductometry, alkanol amine, surfactant.

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26

Panayiotou, Constantinos G. "Thermodynamics of alkanol-alkane mixtures." Journal of Physical Chemistry 92, no. 10 (May 1988): 2960–69. http://dx.doi.org/10.1021/j100321a048.

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27

Qin, Anwei, Dolly E. Hoffman, and Petr Munk. "Excess Volumes of Mixtures of Some Alkyl Esters and Ketones with Alkanols." Collection of Czechoslovak Chemical Communications 58, no. 11 (1993): 2625–41. http://dx.doi.org/10.1135/cccc19932625.

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Excess volumes were calculated from measured densities of binary mixtures of five linear alkanols (methanol, ethanol, 1-propanol, 1-butanol, and 1-pentanol) with five n-alkyl acetates (methyl, ethyl, propyl, butyl, and pentyl acetates) and with two ketones (acetone and 2-butanone) at 20 °C. The whole composition range was studied for all thirty-five binary systems. For a given alcohol, the ∆V/φ1ϑ2 value decreases with increasing size of the carbonyl compound. For a given carbonyl compound, it increases with the length of the alkanol. Systems with methyl acetate as one component have relatively large ∆V/φ1ϑ2 values, while systems with methanol display different compositional dependency in respect to systems with other alcohols.

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28

Heldebrant, David J., Phillip K. Koech, M. Trisha C. Ang, Chen Liang, James E. Rainbolt, Clement R. Yonker, and Philip G. Jessop. "Reversible zwitterionic liquids, the reaction of alkanol guanidines, alkanol amidines, and diamines with CO2." Green Chemistry 12, no. 4 (2010): 713. http://dx.doi.org/10.1039/b924790d.

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29

Romagnoli, Carlo, Bora Sieng, and Mohamed Amedjkouh. "Kinetic relationship in parallel autocatalytic amplifications of pyridyl alkanol and chiral trigger pyrimidyl alkanol." Chirality 32, no. 9 (June 30, 2020): 1143–51. http://dx.doi.org/10.1002/chir.23256.

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30

Carmona, F. J., F. J. Arroyo, I. García de la Fuente, J. A. González, and J. C. Cobos. "Excess molar volumes of methanol or ethanol + n-polyethers at 298.15 K." Canadian Journal of Chemistry 77, no. 10 (October 1, 1999): 1608–16. http://dx.doi.org/10.1139/v99-189.

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Excess molar volumes VmE at 298.15 K and atmospheric pressure for methanol and ethanol + 2,5-dioxahexane, + 3,6-dioxaoctane, + 2,5,8-trioxanonane, + 3,6,9-trioxaundecane, + 5,8,11-trioxapentadecane, + 2,5,8,11-tetraoxadodecane, and + 2,5,8,11,14-pentaoxapentadecane have been obtained from densities measured with an Anton-Paar DMA 602 vibrating-tube densimeter. All the excess volumes are negative over the whole mole fraction range.The VmE curves are shifted to the region rich in the alkanol, increasing their asymmetry with the number of oxygen groups in the polyethers. Results seem to remark the predominant contribution of free volume effects on interactional effects, particularly when the ethers are of the type CH3-(O-CH2CH2)m-CH3. In the case of polyethers with longer n-alkyl chain ends, self-association of methanol and ethanol is more relevant. A short comparative study with results for mixtures with higher 1-alkanols and polyethers is also presented.Key words: experimental, excess volumes, 1-alkanols, polyethers, self-association, free volume effects.

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31

Gürbüz, Elif I., David D. Hibbitts, and Enrique Iglesia. "Kinetic and Mechanistic Assessment of Alkanol/Alkanal Decarbonylation and Deoxygenation Pathways on Metal Catalysts." Journal of the American Chemical Society 137, no. 37 (September 10, 2015): 11984–95. http://dx.doi.org/10.1021/jacs.5b05361.

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32

Doğruer Akan, Bürge, and Ümide Demir Özkay. "Bazı piperazin alkanol türevlerinin antinosiseptif etkinlikleri." Cukurova Medical Journal 44, no. 3 (September 30, 2019): 729–44. http://dx.doi.org/10.17826/cumj.490690.

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33

Alcalde, Rafael, Mert Atilhan, José Luis Trenzado, and Santiago Aparicio. "Physicochemical Insights on Alkylcarbonate–Alkanol Solutions." Journal of Physical Chemistry B 120, no. 22 (May 26, 2016): 5015–28. http://dx.doi.org/10.1021/acs.jpcb.6b02961.

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34

Dewan, R. K., and S. K. Mehta. "Excess volumes of (ethylbenzene + an alkanol)." Journal of Chemical Thermodynamics 19, no. 8 (August 1987): 819–22. http://dx.doi.org/10.1016/0021-9614(87)90028-0.

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35

Vale, V., B. Rathke, S. Will, and W. Schröer. "Eigenschaften von CnmimNTf2/n-Alkanol Mischungen." Chemie Ingenieur Technik 81, no. 8 (August 2009): 1051. http://dx.doi.org/10.1002/cite.200950455.

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36

Endler, Ingolf, Gerd Hradetzky, and Hans-Joachim Bittrich. "Grenzaktivitätskoeffizienten in binären Systemen Benzen-Alkanol." Journal für Praktische Chemie 327, no. 4 (1985): 693–97. http://dx.doi.org/10.1002/prac.19853270422.

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37

González, Juan Antonio, Ismael Mozo, Isaías García de la Fuente, and José Carlos Cobos. "Thermodynamics of organic mixtures containing amines. IV. Systems with aniline." Canadian Journal of Chemistry 83, no. 10 (October 1, 2005): 1812–25. http://dx.doi.org/10.1139/v05-190.

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Binary mixtures of aniline with benzene, toluene, alkane, alkanol, or N,N-dialkylamide have been investigated in the framework of the DISQUAC model. The reported interaction parameters change regularly with the molecular structure of the mixture components. The model consistently describes a set of thermodynamic properties including liquidliquid equilibria, vaporliquid equilibria, and molar excess enthalpies. The two latter properties for ternary systems are well-represented by DISQUAC using binary parameters only (i.e., neglecting ternary interactions). A comparison of DISQUAC results and those obtained from the UNIFAC (Dortmund version) and ERAS models is also shown. The experimental molar excess enthalpies for binary and ternary mixtures are better described by DISQUAC than by UNIFAC. ERAS fails when representing molar excess enthalpies of those binary systems including methanol or ethanol. This may be due to the existence of strong dipolar interactions among aniline molecules as well as to effects related to the equation of state term, evaluated comparing molar excess enthalpies, and molar excess internal energies at constant volume. The study of the aniline systems in terms of the concentrationconcentration structure factor also underlines the importance of dipolar interactions in solutions with alkanes or alcohols, which may be due to the high polarizability of the aniline molecule.Key words: thermodynamics, mixtures, aniline, dipolar interactions, structural effects.

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38

González, Juan Antonio. "Thermodynamics of mixtures containing the CO and OH groups. I. Estimation of the DISQUAC interchange coefficients for 1-alkanol + n-alkanone systems." Canadian Journal of Chemistry 75, no. 10 (October 1, 1997): 1412–23. http://dx.doi.org/10.1139/v97-170.

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1-Alkanol + n-alkanone mixtures are treated in terms of the DISQUAC group contribution model, reporting the interaction parameters for hydroxyl–carbonyl contacts. The quasichemical interchange coefficients are independent of the compounds in the mixture; the dispersive interchange coefficients depend on the intramolecular environment of the hydroxyl and (or) carbonyl groups. Mixtures of a given 1-alkanol with isomeric ketones are characterized by the same first dispersive interaction parameter, which is constant from 2-pentanone. This type of system, when including an alcohol up to 1-pentanol, needs different dispersive enthalpic parameters depending on the symmetry of the ketone. In this case, such parameters are constant from 2-pentanone or 3-pentanone. A detailed comparison is presented between DISQUAC results and data available in the literature on vapour–liquid equilibria, VLE (including azeotropic data), molar Gibbs energies, GE, molar excess enthalpies, HE, solid–liquid equilibria, SLE, natural logarithms of activity coefficients, In [Formula: see text] and partial molar excess enthalpies at infinite dilution,[Formula: see text]. For 54 systems, the mean relative standard deviation in pressure is 0.018; for 61 systems, this magnitude in the case of the HE is 0.059. It is noteworthy that the model yields good predictions over a very wide range of temperature for VLE and SLE. HE is also reasonably well represented at different temperatures. Larger discrepancies are encountered, as usual, for partial molar quantities at infinite dilution. Keywords: liquids, mixtures, thermodynamic properties, group contributions.

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39

Dewan, Raj K., Surinder K. Mehta, Ravi Parashar, and Kiran Bala. "Topological investigations on the association of alkanols: excess volume of pyridine–alkanol (C1–C10) mixtures." J. Chem. Soc., Faraday Trans. 87, no. 10 (1991): 1561–68. http://dx.doi.org/10.1039/ft9918701561.

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40

Akhter, M. Salim, and Sadeq M. Alawi. "Micellar behaviour of cetyltrimethylammonium bromide in N-methyl acetamide—alkanol and N,N-dimethyl acetamide—alkanol mixtures." Colloids and Surfaces A: Physicochemical and Engineering Aspects 196, no. 2-3 (January 2002): 163–74. http://dx.doi.org/10.1016/s0927-7757(01)00864-0.

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41

Cen, Peipei, Weize Yuan, Shuchang Luo, Xiangyu Liu, Gang Xie, and Sanping Chen. "Solvent coligands fine-tuned the structures and magnetic properties of triple-bridged 1D azido-copper(ii) coordination polymers." New Journal of Chemistry 43, no. 2 (2019): 601–8. http://dx.doi.org/10.1039/c8nj04731f.

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42

Okada, Shuji, Hiro Matsuda, Masaaki Otsuka, Naoto Kikuchi, Kikuko Hayamizu, Hachiro Nakanishi, and Masao Kato. "Synthesis and Solid-State Polymerization ofω-(1,3-Butadiynyl) Substituted 1-Alkanol and Alkanoic Acid." Bulletin of the Chemical Society of Japan 67, no. 2 (February 1994): 455–61. http://dx.doi.org/10.1246/bcsj.67.455.

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43

Matsumoto, Arimasa, Ayame Tanaka, Yoshiyasu Kaimori, Natsuki Hara, Yuji Mikata, and Kenso Soai. "Circular dichroism spectroscopy of catalyst preequilibrium in asymmetric autocatalysis of pyrimidyl alkanol." Chemical Communications 57, no. 85 (2021): 11209–12. http://dx.doi.org/10.1039/d1cc04206h.

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44

Holland, A. R., S. T. Petsch, I. S. Castañeda, K. M. Wilkie, S. J. Burns, and J. Brigham-Grette. "A biomarker record of Lake El'gygytgyn, Far East Russian Arctic: investigating sources of organic matter and carbon cycling during marine isotope stages 1–3." Climate of the Past 9, no. 1 (January 30, 2013): 243–60. http://dx.doi.org/10.5194/cp-9-243-2013.

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Abstract. Arctic paleoenvironmental archives serve as sensitive recorders of past climate change. Lake El'gygytgyn (Far East Russian Arctic) is a high-latitude crater impact lake that contains a continuous sediment record influenced by neither glaciation nor glacial erosion since the time of impact 3.58 Ma ago. Prior research on sediments collected from Lake El'gygytgyn suggest times of permanent ice cover and anoxia corresponding to global glacial intervals, during which the sediments are laminated and are characterized by the co-occurrence of high total organic carbon, microscopic magnetite grains that show etching and dissolution, and negative excursions in bulk sediment organic matter carbon isotope (δ13C) values. Here we investigate the abundance and carbon isotopic composition of lipid biomarkers recovered from Lake El'gygytgyn sediments spanning marine isotope stages 1–3 to identify key sources of organic matter (OM) to lake sediments, to establish which OM sources drive the negative δ13C excursion exhibited by bulk sediment OM, and to explore if there are molecular and isotopic signatures of anoxia in the lake during glaciation. We find that during marine isotope stages 1–3, direct evidence for water column anoxia is lacking. A ~4‰ negative excursion in bulk sediment δ13C values during the Local Last Glacial Maximum (LLGM) is accompanied by more protracted, higher magnitude negative excursions in n-alkanoic acid and n-alkanol δ13C values that begin 20 kyr in advance of the LLGM. In contrast, n-alkanes and the C30 n-alkanoic acid do not exhibit a negative δ13C excursion at this time. Our results indicate that the C24, C26 and C28 n-alkanoic acids do not derive entirely from terrestrial OM sources, while the C30 n-alkanoic acid at Lake El'gygytgyn is a robust indicator of terrestrial OM contributions. Overall, our results strongly support the presence of a nutrient-poor water column, which is mostly isolated from atmospheric carbon dioxide during glaciation at Lake El'gygytgyn.

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45

Holland, A. R., S. T. Petsch, I. S. Castañeda, K. M. Wilkie, S. J. Burns, and J. Brigham-Grette. "A biomarker record of Lake El'gygytgyn, far east Russian Arctic: investigating sources of organic matter and carbon cycling during marine isotope stages 1–3." Climate of the Past Discussions 8, no. 5 (September 20, 2012): 4625–61. http://dx.doi.org/10.5194/cpd-8-4625-2012.

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Abstract. Paleoenvironmental archives in Arctic regions serve as sensitive recorders of past climate change where summer temperatures hover near freezing and small climate variations may exhibit strong threshold-crossing environment responses. Lake El'gygytgyn (Far East Russian Arctic) is a high-latitude crater impact lake that contains a continuous sediment record influenced by neither glaciation nor glacial erosion since the time of impact at 3.58 Ma. Prior research on sediments collected from Lake El'gygytygyn suggest times of permanent ice cover and anoxia corresponding to global glacial intervals, during which the sediments are laminated and are characterized by the co-occurrence of high total organic carbon, microscopic magnetite grains that show etching and dissolution, and negative excursions in bulk sediment organic matter carbon isotope (δ13C) values. Here, we investigate the abundance and carbon isotopic characteristics of lipid biomarkers recovered from Lake El'gygytygn sediments spanning marine isotope stages 1–3, to identify key sources of organic matter (OM) to lake sediments, to establish which compounds and thus OM sources drive the negative δ13C excursion exhibited by bulk sediment OM, and to explore if there are molecular and isotopic signatures of anoxia in the lake during glaciation. We find that during marine isotope stages 1–3, direct evidence for water column anoxia is lacking. A ∼4‰ negative excursion in bulk sediment δ13C values during the local Last Glacial Maximum (LLGM) is accompanied by more protracted, higher magnitude negative excursions in n-alkanoic acid and n-alkanol δ13C values that begin 20 kyr in advance of the LLGM. In contrast, n-alkanes and the C30 n-alkanoic acid do not exhibit a negative δ13C excursion at this time. Our results indicate that the C24, C26 and C28 n-alkanoic acids do not derive entirely from terrestrial OM sources, while the C30 n-alkanoic acid at Lake El'gygytgyn is a robust indicator of terrestrial OM contributions. Overall, our results strongly support the presence of a nutrient-poor water column, which is mostly isolated from atmospheric carbon dioxide during glaciation at Lake El'gygytgyn.

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46

Schäfer, Imke K., Verena Lanny, Jörg Franke, Timothy I. Eglinton, Michael Zech, Barbora Vysloužilová, and Roland Zech. "Leaf waxes in litter and topsoils along a European transect." SOIL 2, no. 4 (October 25, 2016): 551–64. http://dx.doi.org/10.5194/soil-2-551-2016.

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Abstract. Lipid biomarkers are increasingly used to reconstruct past environmental and climate conditions. Leaf-wax-derived long-chain n-alkanes and n-alkanoic acids may have great potential for reconstructing past changes in vegetation, but the factors that affect the leaf wax distribution in fresh plant material, as well as in soils and sediments, are not yet fully understood and need further research. We systematically investigated the influence of vegetation and soil depth on leaf waxes in litter and topsoils along a European transect. The deciduous forest sites are often dominated by the n-C27 alkane and n-C28 alkanoic acid. Conifers produce few n-alkanes but show high abundances of the C24 n-alkanoic acid. Grasslands are characterized by relatively high amounts of C31 and C33 n-alkanes and C32 and C34 n-alkanoic acids. Chain length ratios thus may allow for distinguishing between different vegetation types, but caution must be exercised given the large species-specific variability in chain length patterns. An updated endmember model with the new n-alkane ratio (n-C31 + n-C33) / (n-C27 + n-C31 + n-C33) is provided to illustrate, and tentatively account for, degradation effects on n-alkanes.

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Ghazipour, H., A. Gutiérrez, D. Mohammad-Aghaie, M. M. Alavianmher, S. M. Hosseini, and S. Aparicio. "Insights on biodiesel blends with alkanol solvents." Journal of Molecular Liquids 332 (June 2021): 115864. http://dx.doi.org/10.1016/j.molliq.2021.115864.

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González, J. A., I. Mozo, I. García de la Fuente, and J. C. Cobos. "Thermodynamics of 1-alkanol+linear alkanoate mixtures." Physics and Chemistry of Liquids 43, no. 2 (April 2005): 175–94. http://dx.doi.org/10.1080/00319100500038652.

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49

Wanasundara, Janitha P. D., and Fereidoon Shahidi. "Alkanol-ammonia-water/hexane extraction of flaxseed." Food Chemistry 49, no. 1 (January 1994): 39–44. http://dx.doi.org/10.1016/0308-8146(94)90230-5.

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50

Sánchez, Jaime, Héctor Artigas, Ignacio Gascón, and Carlos Lafuente. "Thermodynamic behaviour of alkyl lactate–alkanol systems." Journal of Chemical Thermodynamics 127 (December 2018): 33–38. http://dx.doi.org/10.1016/j.jct.2018.07.013.

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