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Journal articles on the topic 'Partial molar volume'

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Published: 4 June 2021
Last updated: 11 June 2025

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1

Imai, Takashi, and Fumio Hirata. "Hydrophobic effects on partial molar volume." Journal of Chemical Physics 122, no. 9 (2005): 094509. http://dx.doi.org/10.1063/1.1854626.

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2

Hadded, M., M. Biquard, P. Letellier, and R. Schaal. "Propriétés volumiques du nitrate d'éthylammonium fondu à 298 K et de ses mélanges avec l'eau." Canadian Journal of Chemistry 63, no. 3 (1985): 565–70. http://dx.doi.org/10.1139/v85-092.

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Partial molar volumes of water and ethylammonium nitrate EAN are determined accurately in all water–EAN mixtures, between pure water and pure fused salt at 298 K. It has been found that the partial molar volume of water decreases linearly with molar fraction of salt, x, in concentrated solution of EAN (C > 2 mol L−1, x > 0.04). The main thermodynamic relations are established to describe the volumetric behaviour of salt, water, and solution. It has been shown that the intrinsic volume of salt can be identified roughly with the molar volume of the pure fused salt and the value of apparent molar volume of water with the actual volume of water in solution.
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3

Janik, Ireneusz, Alexandra Lisovskaya, and David M. Bartels. "Partial Molar Volume of the Hydrated Electron." Journal of Physical Chemistry Letters 10, no. 9 (2019): 2220–26. http://dx.doi.org/10.1021/acs.jpclett.9b00445.

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4

Hamidi, Nasrollah. "On the total, apparent partial molar, partial molar, apparent partial specific and partial specific volume of the binary systems." Physics and Chemistry of Liquids 51, no. 3 (2013): 317–37. http://dx.doi.org/10.1080/00319104.2012.713555.

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5

Radovic, Ivona, Mirjana Kijevcanin, Aleksandar Tasic, Bojan Djordjevic, and Slobodan Serbanovic. "Derived thermodynamic properties of alcohol + cyclohexylamine mixtures." Journal of the Serbian Chemical Society 75, no. 2 (2010): 283–93. http://dx.doi.org/10.2298/jsc1002283r.

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Thermal expansion coefficients, ?, excess thermal expansion coefficients, ?E, isothermal coefficients of pressure excess molar enthalpy, (?HE/?p)T,x, partial molar volumes, V?i, partial molar volumes at infinite dilution, V?i?, partial excess molar volumes, V?Ei, and partial excess molar volumes at infinite dilution, V?Ei?, were calculated using experimental densities and excess molar volumes, VE, data. All calculations are performed for the binary systems of cyclohexylamine with 1-propanol or 1-butanol or 2-butanol or 2-methyl-2-propanol. The Redlich-Kister polynomial and the reduced excess molar volume approach were used in the evaluation of these properties. In addition, the aim of this investigation was to provide a set of various volumetric data in order to asses the influence of temperature, chain length and position of hydroxyl group in the alcohol molecule on the molecular interactions in the examined binary mixtures.
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6

Xu, Yuming, Lili Li, and Loren G. Hepler. "Partial molar volumes of acidic gases in physical solvents and prediction of solubilities at high pressures." Canadian Journal of Chemistry 70, no. 1 (1992): 55–57. http://dx.doi.org/10.1139/v92-010.

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Partial molar volumes at infinite dilution for three acidic gases (carbon dioxide, hydrogen sulfide, and sulfur dioxide) in four physical solvents (propylene carbonate, methyl cyanoacetate, N-formyl morpholine, and Selexol) have been obtained using our new dilatometer. These partial molar volumes, in combination with the Henry's law constants obtained previously, have been used in the Krichevsky–Kasarnovsky equation for predicting the solubilities of acidic gases in physical solvents at high pressures. Keywords: partial molar volume, solubility, physical solvents.
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7

SAWAMURA, Seiji. "High-Pressure Solubility and Related Partial Molar Volume." Review of High Pressure Science and Technology 25, no. 3 (2015): 239–46. http://dx.doi.org/10.4131/jshpreview.25.239.

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8

Md Nayeem, Sk, M. Kondaiah, K. Sreekanth, and D. Krishna Rao. "Thermoacoustic, Volumetric, and Viscometric Investigations in Binary Liquid System of Cyclohexanone with Benzyl Benzoate at T = 308.15, 313.15, and 318.15 K." Journal of Thermodynamics 2014 (December 29, 2014): 1–13. http://dx.doi.org/10.1155/2014/487403.

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Ultrasonic velocities (u), densities (ρ), and viscosities (η) of binary liquid mixtures of cyclohexanone with benzyl benzoate, including pure liquids, over the entire composition range have been measured at 308.15 K, 313.15 K, and 318.15 K. Using the experimental results, parameters such as molar volume (Vm), isentropic compressibility (ks), intermolecular free length (Lf), acoustic impedance (Z), internal pressure (πi), enthalpy (H), Gibbs free energy of activation of viscous flow (G*E), and excess/deviation properties of these including partial molar volumes (V-m,1 and V-m,2), excess partial molar volumes (V-m,1E and V-m,2E), partial molar volume of the components at infinite dilution (V-m,1∞, V-m,2∞), and excess partial molar volume at infinite dilution (V-m,1E,∞and V-m,2E,∞) have been computed. The observed negative values of VmE, Δks, LfE, and πiE and positive values of zE, HE, ΔG*E, Δη, and Δu for all the liquid mixtures studied clearly indicate the presence of strong dipole-dipole-type interactions, fitting of smaller molecules into bigger molecules. Further theoretical values of sound velocity and viscosity in the mixtures have been evaluated using various theories and have been compared with experimental values to verify the applicability of such theories to the systems studied.
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9

Wang, Jianji, Yang Zhao, Kelei Zhuo, and Ruisen Lin. "A partial-molar volume study of electrolytes in propylene carbonate-based lithium battery electrolyte solutions at 298.15 K." Canadian Journal of Chemistry 80, no. 7 (2002): 753–60. http://dx.doi.org/10.1139/v02-092.

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Apparent molar volumes (V2, ϕ ) and standard partial-molar volumes (V20, ϕ ) of LiClO4 and LiBr at 298.15 K have been determined from precise density measurements in solvent mixtures of propylene carbonate (PC) with dimethylformamide (DMF), tetrahydrofuran (THF), acetonitrile (AN), and methyl formate (MF). The scaled particle theory is used to calculate the contributions of the cavity formation and the electrolyte-solvent interactions to the standard partial-molar volumes. It is shown that V20, ϕ is strongly dependent on the nature of the solvents, and the trends in V20, ϕ with composition of the solvent mixtures are determined by the interaction volumes of electrolytes with solvents. The results are discussed in terms of ionic preferential solvation, packing effect of solvents in the solvation shell, and electrostriction of solvents by ion.Key words: partial-molar volume, scaled particle theory, lithium salts, propylene carbonate, solvent mixtures, lithium battery electrolytes.
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10

Palepu, Ramamurthy, Joan Oliver, and Brian MacKinnon. "Viscosities and densities of binary liquid mixtures of m-cresol with substituted anilines. Part 3." Canadian Journal of Chemistry 63, no. 5 (1985): 1024–30. http://dx.doi.org/10.1139/v85-174.

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Densities and viscosities were determined for the binary systems of m-cresol with aniline, N-methylaniline, N, N-dimethylaniline, N-ethylaniline, and N, N-diethylaniline at five different temperatures. From the experimental results, the excess volume, excess viscosity, excess molar free energy of activation of flow, excess partial molar volume, and partial molar volumes were calculated. Also various thermodynamic parameters of activation of flow were calculated from the dependence of viscosity on temperature. The deviations from ideality of thermodynamic and transport functions are explained on the basis of molecular interactions between the components of the mixture.
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11

Vollárová, Oľga, and Ján Benko. "Transfer Thermodynamic Functions ∆Gt0, ∆Ht0 and T∆St0 of cis- and trans-[CoCl2(en)2]+ Isomers in Aqueous Mixtures of Methanol, tert-Butyl Alcohol and Acetonitrile." Collection of Czechoslovak Chemical Communications 65, no. 9 (2000): 1455–63. http://dx.doi.org/10.1135/cccc20001455.

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The solubility, partial molar volume and standard integral molar enthalpy of solution of cis- and trans-[CoCl2(en)2]Cl in water, aqueous methanol, aqueous tert-butyl alcohol and aqueous acetonitrile are reported. The transfer functions ∆Gt0, ∆Ht0 and T∆St0 as well as partial molar volumes are used to obtain information on the solute-solvent interactions. Results obtained are discussed in terms of differences in the surface charge distribution in isomeric coordination species.
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12

Lin, Guimei, Pingfeng Bian, and Ruisen Lin. "The limiting partial molar volume and transfer partial molar volume of glycylglycine in aqueous sodium halide solutions at 298.15K and 308.15K." Journal of Chemical Thermodynamics 38, no. 2 (2006): 144–51. http://dx.doi.org/10.1016/j.jct.2005.04.012.

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13

Afrin, Sadaf, and Riyaz uddeen. "Interaction of methimazole/curcumin with human serum albumin: Partial molar volume and partial molar isentropic compressibility studies." Journal of Chemical Thermodynamics 91 (December 2015): 80–85. http://dx.doi.org/10.1016/j.jct.2015.07.001.

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14

Potuzak, M. "A partial molar volume for ZnO in silicate melts." American Mineralogist 91, no. 2-3 (2006): 366–74. http://dx.doi.org/10.2138/am.2006.1817.

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15

Ramsden, J. J. "Partial molar volume of solutes in bilayer lipid membranes." Journal of Physical Chemistry 97, no. 17 (1993): 4479–83. http://dx.doi.org/10.1021/j100119a036.

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16

Courtial, Philippe, and Donald B. Dingwell. "A partial molar volume for La2O3 in silicate melts." Journal of Non-Crystalline Solids 352, no. 4 (2006): 304–14. http://dx.doi.org/10.1016/j.jnoncrysol.2005.12.002.

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17

Scherer, J. R. "The partial molar volume of water in biological membranes." Proceedings of the National Academy of Sciences 84, no. 22 (1987): 7938–42. http://dx.doi.org/10.1073/pnas.84.22.7938.

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18

Kamiya, Yoshinori, Yasutoshi Naito, and Keishin Mizoguchi. "Sorption and partial molar volume of gases in polybutadiene." Journal of Polymer Science Part B: Polymer Physics 27, no. 11 (1989): 2243–50. http://dx.doi.org/10.1002/polb.1989.090271107.

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19

Kirchheim, R. "Partial molar volume of small molecules in glassy polymers." Journal of Polymer Science Part B: Polymer Physics 31, no. 10 (1993): 1373–82. http://dx.doi.org/10.1002/polb.1993.090311012.

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20

Salamanca, Constain, Martín Contreras, and Consuelo Gamboa. "Partial molar volume of anionic polyelectrolytes in aqueous solution." Journal of Colloid and Interface Science 309, no. 2 (2007): 435–39. http://dx.doi.org/10.1016/j.jcis.2006.11.029.

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21

Cui, Wanjing, Hongfang Hou, Jiaojiao Chen, Yafei Guo, Lingzong Meng, and Tianlong Deng. "Apparent molar volumes of sodium arsenate aqueous solution from 283.15 K to 363.15 K at ambient pressure: an experimental and thermodynamic modeling study." Pure and Applied Chemistry 92, no. 10 (2020): 1673–82. http://dx.doi.org/10.1515/pac-2019-1102.

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AbstractDensities of the sodium arsenate aqueous solution with the molality varied from (0.04165 to 0.37306) mol · kg−1 were determined experimentally at temperature intervals of 5 K from 283.15 K to 363.15 K and ambient pressure using a precise Anton Paar Digital vibrating-tube densimeter. The apparent molar volumes (Vϕ), thermal expansion coefficient (α) and partial molar volume $({\bar V_{\rm{B}}})$ were obtained based on the results of density measurement. The 3D diagram of apparent molar volume against temperature and molality as well as the diagram of thermal expansion coefficient and partial molar volume against molality were plotted, respectively. On the basis of the Pitzer ion-interaction equation of apparent molar volume model, the Pitzer single-salt parameters ($(\beta _{{\rm{M,X}}}^{(0)v},\beta _{{\rm{M,X}}}^{(1)v},{\rm{ }}\beta _{{\rm{M,X}}}^{(2)v}{\rm{ and }}C_{{\rm{M,X}}}^v,MX = N{a_3}As{O_4})$ and their temperature-dependent correlation F(i, p, T) = a1 + a2ln(T/298.15) + a3(T – 298.15) + a4/(620 – T) + a5/(T – 227) (where T is temperature in Kelvin, ai is the correlation coefficient) for Na3AsO4 were obtained on account of the least-squares method. Predictive apparent molar volumes agree well with the experimental values, and those results indicate that the single-salt parameters and their relational coefficients of temperature-dependence for Na3AsO4 obtained are reliable.
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22

Marcus, Yizhak. "On the solubility of non-ionic organic solutes in seawater." Pure and Applied Chemistry 87, no. 5 (2015): 503–8. http://dx.doi.org/10.1515/pac-2014-0908.

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AbstractGiven the solubilities of non-ionic organic solutes in water, their solubilities in seawater are obtained by correlation expressions involving two descriptors for the constituent ions (or salts) of seawater and two descriptors of the solutes. The former are the standard partial molar volumes and the intrinsic molar volumes and the latter are the molar volume (the Le Bas variant of it) and either the Hildebrand solubility parameter δH or the Kamlet–Taft solvatochromic π*.
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23

Zheng, Lan, Yu Qi Wang, Kai Xun Chen, and Lin Wang. "Solubilities Prediction and Partial Molar Volume Calculation for 2-Butanol and CO2 Binary Mixture at High Pressure." Applied Mechanics and Materials 138-139 (November 2011): 1032–39. http://dx.doi.org/10.4028/www.scientific.net/amm.138-139.1032.

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A constant-volume visual cell was used to measure vapor-liquid phase equilibrium data of 2-butanol in supercritical carbon dioxide from 323.2K to 353.2K. The phase equilibrium solubilities were predicted by Peng-Robinson equation of state together with Vander Waals-2 mixing regulation. Dependence of solubility of CO2 in liquid 2-butanol on pressure was discussed by Krichevsky-kasarnovsky equation. Meanwhile, Henry’s constants and partial molar volume at infinite dilution were determined. Also partial molar volumes of vapor phase and liquid phase at equation state were evaluated from proposed model. The correlation between calculated values and the experimental data showed good agreement.
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24

Pradhan, Rajendra, and Biswajit Sinha. "Thermophysical properties of binary blends of cyclohexane with some esters." Journal of the Serbian Chemical Society 82, no. 2 (2017): 189–202. http://dx.doi.org/10.2298/jsc160315075p.

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From the densities (?) and viscosities (?) measured for three binary blends consisting of methyl acetate (MA), ethyl acetate (EA) and methyl salicylate (MS) over the entire composition range with cyclohexane (CH) at 298.15?318.15 K under atmospheric pressure, the excess molar volumes (VEm ) and excess viscosities (?E) were derived. In addition, the excess isentropic compressibilities (KEs ) excess intermolecular free lengths (LEf) and excess molar refractions (R Em) were derived from measured ultrasonic speeds of sound (u) and refractive indices (nD) for the binary blends at 298.15 K. Various derived properties are discussed in terms of molecular interactions and structural effects. Partial molar volumes ( 0 Vm,1 and 0 Vm,2 ) and excess partial molar volumes ( 0,E Vm,1 and 0,E Vm,2 ) at infinite dilution are also discussed in terms of volume changes in the blends. Furthermore, the excess molar volumes (V Em ) and viscosities (?) of the blends were correlated with the Prigogine?Flory?Paterson (PFP) theory and the Peng?Robinson Equation of State (PR-EOS).
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25

Koga, Y. "Fluctuations in aqueous methanol, ethanol, and propan-1-ol: amplitude and wavelength of fluctuation." Canadian Journal of Chemistry 77, no. 12 (1999): 2039–45. http://dx.doi.org/10.1139/v99-213.

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Density, heat capacity, and isentropic compressibility data for aqueous methanol, ethanol, and propan-1-ol by Benson's group were used to evaluate two kinds of fluctuations; mean-square fluctuation densities; and (mean-square) normalized fluctuations, respectively, in volume, entropy, and cross (entropy/volume) effect. The mean-square fluctuation densitiesprovide measures for the amplitude (intensity) of the fluctuation, while the normalized fluctuations contain information regarding the wavelength (extensity) of the fluctuation. Furthermore, their composition derivatives, the partial molar fluctuationsof alcohols were calculated. These quantities signify the effect of additional solute on the respective fluctuations. These data were interpreted in terms of mixing schemes learned earlier in this laboratory by using the data of excess partial molar enthalpy, entropy, and volume, and the respective alcohol-alcohol interaction functions, i.e., the composition derivatives of partial molar quantities. Key words: aqueous methanol, ethanol, and propan-1-ol;fluctuation density; normalized fluctuation; partial molar fluctuations of alcohol.
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26

Iqbal, M., M. Asghar Jamal, Maqsood Ahmed, and Bashir Ahmed. "Partial molar volumes of some drugs in water and ethanol at 35 °C." Canadian Journal of Chemistry 72, no. 4 (1994): 1076–79. http://dx.doi.org/10.1139/v94-135.

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Partial molar volumes, V0, of six drugs, mostly anaesthetics, viz., cinchocaine HCl, lidocaine HCl, mepivacaine HCl, procaine HCl, propranolol HCl, tetracaine HCl, in water and ethanol, calculated from precision densities obtained at 35 °C from a vibrating tube densitometer, are reported in this work. The data represent the smaller volumes of drug molecules in ethanol than in water. Volume contribution of hydrochloride part were calculated and excluded from V0 to assess the volume of free base component of the solutes. Volumes of free bases were also found smaller in ethanol, although much closer to those in water. The differences in volumes are interpreted as due to hydrophobicity of solutes. Relative hydrophobicities were estimated from volumes of transfer from aqueous to organic media. Correlation of V0 with van der Waal volumes are also reported. The hydrophobicity of these compounds is proposed to play a key role in the resulting drug action. Possible mechanism of drug binding with the membrane structure is also discussed.
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27

Bolton, Barbara A., S. Kint, G. F. Bailey, and James R. Scherer. "Ethanol sorption and partial molar volume in cellulose acetate films." Journal of Physical Chemistry 90, no. 6 (1986): 1207–11. http://dx.doi.org/10.1021/j100278a049.

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28

Moučka, Filip, and Ivo Nezbeda. "Partial molar volume of methanol in water: Effect of polarizability." Collection of Czechoslovak Chemical Communications 74, no. 4 (2009): 559–63. http://dx.doi.org/10.1135/cccc2008202.

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The available pairwise additive intermolecular interaction models used so far in simulations in combination with common combining rules do not seem to be able to reproduce the most distinct feature of aqueous solutions of alcohols, the minimum of the partial molar volume at low alcohol concentrations. Nonetheless, this fundamental failure seems to have been paid little attention to, partly because of very high requirements for accuracy and, hence, CPU time of simulations. As an attempt to go beyond empirical combining rules and account in a more physical and yet simple way for the cross interactions, a feasibility study has been undertaken using a polarizable model of water in molecular simulations of the water–methanol mixture at ambient conditions. It turns out that the inclusion of polarizability may qualitatively change the behavior of the mixture bringing the result in agreement with experiment.
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29

Bouhifd, Ali M., Alan Whittington, and Pascal Richet. "Partial molar volume of water in phonolitic glasses and liquids." Contributions to Mineralogy and Petrology 142, no. 2 (2001): 235–43. http://dx.doi.org/10.1007/s004100100286.

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30

Mehrotra, K. N., A. Kumar, and R. P. Varma. "Partial molar volume and expansibility of alkaline earth metal soaps." Journal of Colloid and Interface Science 124, no. 1 (1988): 63–66. http://dx.doi.org/10.1016/0021-9797(88)90325-6.

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31

Ghazoyan, Heghine H., and Shiraz A. Markaryan. "VOLUMETRIC PROPERTIES OF SOLUTIONS OF DIMETHYLSULFONE IN ETHANOL-WATER MIXTURE AT TEMPERATURES RANGE OF 298.15-323.15 K." IZVESTIYA VYSSHIKH UCHEBNYKH ZAVEDENIY KHIMIYA KHIMICHESKAYA TEKHNOLOGIYA 60, no. 7 (2017): 27. http://dx.doi.org/10.6060/tcct.2017607.5564.

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This paper studies volumetric properties of ternary dimethylsulfone-ethanol-water systems. The biomedical and environmental significance for the fundamental investigations of aqueous solution of dimethylsulfone and influences of third component on volumetric behavior of this system arises from several reasons. In the global sulfur cycle dimethylsulfide is converted to dimethylsulfone leading to an annual atmospheric production of some million tones of dimethylsulfone, much of which would be deposited in rain and snow. In addition, dimethylsulfone has been extensively studied from a medical point of view. It was established that dimethylsulfone is contained in small amounts in human blood and urine. Also of interest is that methionine is transformed into dimethylsulfone in living organisms. In this work densities of solution of dimethylsulfone in ethanol-water mixtures with various compositions have been measured over available concentration range. As it is evident from experimental data, the increase in a temperature leads to the reduction of density. The apparent and partial molar volumes of solutions were determined over the 298.15–323.15K temperature range. As it follows from these data, the apparent molar volumes increase with increasing of temperature. The influence of ethanol on the volumetric behavior has been taken into account by changing the apparent molar volume compared with the apparent molar volume of the binary aqueous solutions of DMSO2. It is found also the effect of the amount of ethanol on the volumetric properties of these solutions. It is interesting that the effect of ethanol on the values of apparent molar volumes does not change monotone with increasing in quantity of ethanol in ethanol-water mixture. In dimethylsulfone+(ethanol-water) solutions the partial molar volume of dimethylsulfone increases when quantity of ethanol in ethanol-water mixture more than 0.5 molar fraction. The observed phenomena are explained by the presence of competition of intermolecular interactions. In the DMSO2-ethanol-water system the strongest interaction between ethanol and water molecules leads to the increase in partial molar volumes for DMSO2.For citation:Ghazoyan H.H., Markaryan S.A. Volumetric properties of solutions of dimethylsulfone in ethanol-water mixture at tempe-ratures range of 298.15-323.15 K. Izv. Vyssh. Uchebn. Zaved. Khim. Khim. Tekhnol. 2017. V. 60. N 7. P. 27-33.
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32

Nishimura, Norio, Tohru Tanaka, and Takushi Motoyama. "Additivity of the partial molar volumes of organic compounds." Canadian Journal of Chemistry 65, no. 9 (1987): 2248–53. http://dx.doi.org/10.1139/v87-375.

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A critical test of additivity for partial molar volume has been made at 25 °C in CCl4 with polyethylene glycol dimethyl ethers, crown ethers, cycloalkanes, n-alkanes, and others. Plots of partial molar volume at infinite dilution [Formula: see text] against the properly chosen number of repeating unit (n) are linear except for small cyclic molecules, and the slopes of homologous straight chain and ring compounds are the same. The values of [Formula: see text] extrapolated to n = 0 for cycloalkanes and crown ethers support the validity of the contribution due to the translational kinetic energy that has been predicted recently on a theoretical basis. The importance of packing efficiencies around the solute molecules has been examined by means of simple models.
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33

Lin, Guimei, Ruisen Lin, and Lin Ma. "The limiting partial molar volume and apparent molar volume of glycylglycine in aqueous KCl solution at 298.15 and 308.15K." Thermochimica Acta 430, no. 1-2 (2005): 31–34. http://dx.doi.org/10.1016/j.tca.2004.12.008.

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34

Ji, Xiaoyan, and Hertanto Adidharma. "Prediction of molar volume and partial molar volume for CO2/ionic liquid systems with heterosegmented statistical associating fluid theory." Fluid Phase Equilibria 315 (February 2012): 53–63. http://dx.doi.org/10.1016/j.fluid.2011.11.014.

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35

Bartaria, Divya, Harish Chandra, M. M. Pandey, and V. Krishna. "Partial Molar Volume, Partial Molar Adiabatic Compressibility and Viscosity Coefficient of Aqueous Solution of Metal(II) Chelates of Ethylenediaminetetraacetic Acid." Proceedings of the National Academy of Sciences, India Section A: Physical Sciences 84, no. 1 (2014): 43–48. http://dx.doi.org/10.1007/s40010-013-0113-5.

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36

Duncan, Megan S., and Carl B. Agee. "The partial molar volume of carbon dioxide in peridotite partial melt at high pressure." Earth and Planetary Science Letters 312, no. 3-4 (2011): 429–36. http://dx.doi.org/10.1016/j.epsl.2011.10.021.

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37

Elangovan, Sampandam. "Density, Ultrasonic Velocity, Isentropic Compressibility, Molar Volumes and Related Excess Parameters Studies on Ethyl Acetate with 1-Ethanol at 303K, 308K, and 313K." Material Science Research India 18, no. 2 (2021): 171–78. http://dx.doi.org/10.13005/msri/180205.

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A binary liquid mixture that consists of ethyl acetate and 1-ethanol has been prepared at various concentrations by the mole fraction method. The ultrasonic velocity and density have been determined at 303K, 308K and 313K. From the experimental data, the excess isentropic compressibility, excess molar volumes, excess internal pressures, and excess molar enthalpy have been computed. The variations were observed as polynomial and fitted to the Redlich-Kister polynomial functions. By using this function, adjustable parameters and the standard deviations have been calculated. The experimental and theoretical data reveal that the existence of the intermolecular interactions between the selected liquid system. The partial molar compressibility’s and partial molar volume also calculated at infinite dilution of the system. In general, the intermolecular forces have tended to the variations in the magnitude and sign of the excess parameters. The excess molar volume (Vme), excess isentropic compressibility (), excess internal pressure ( ) and the enthalpy ( ) show the negative magnitude at the entire range of concentrations and temperatures. The significant variations of these parameters with the mole fraction of ethyl acetate have been analysed. Furthermore, the strength of the intermolecular interactions decreased with increasing the experimental temperatures as 303K > 308K >313K.
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38

Zhao, Yang, Jianji Wang, Xiaopeng Xuan, and Ruisen Lin. "Volumetric studies of ion solvation in propylene carbonate + N,N-dimethylformamide electrolyte solutions." Canadian Journal of Chemistry 81, no. 4 (2003): 307–14. http://dx.doi.org/10.1139/v03-061.

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Apparent molar volumes V2,ϕ and standard partial molar volumes V°2,ϕ for tetraethylammonium bromide (Et4NBr), tetrapropylammonium bromide (Pr4NBr), tetrabutylammonium bromide (Bu4NBr), and tetrahexylammonium bromide (Hex4NBr) have been determined at 298.15 K from precise density measurements in solvent mixtures of propylene carbonate (PC) with N,N-dimethylformamide (DMF). Combined with our previous data for LiClO4 and LiBr in the same solvents, ionic molar volumes of Li+, Et4N+, Pr4N+, Bu4N+, Hex4N+, and related anions have been deduced from the extrapolation method suggested by Conway and co-workers. It is shown that the molar volumes of these cations are quite independent of the nature of the solvent and the composition of the solvent mixtures, in contrast to those of ClO4– and Br– anions. This suggests that the Lewis-base-type solvents with similar molecular volumes have similar interactions with Li+. The constancy in partial molar volume for tetraalkylammonium ions provides helpful evidence for the lack of solvation of large tetraalkylammonium cations in organic solvents. These findings have been interpreted using scaled-particle theory. The results are discussed in terms of ion solvation, packing effects of solvent molecules in the solvation shell, and the electrostriction of solvents.Key words: ionic volumes, propylene carbonate, N,N-dimethylformamide, solvent mixtures, solvation, lithium batteries.
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39

Nikolova, Penka V., Sheldon JB Duff, Peter Westh, et al. "A thermodynamic study of aqueous acetonitrile: excess chemical potentials, partial molar enthalpies, entropies and volumes, and fluctuations." Canadian Journal of Chemistry 78, no. 12 (2000): 1553–60. http://dx.doi.org/10.1139/v00-140.

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We measured vapour pressures of aqueous acetonitrile (abbreviated as ACN) at 6, 20, and 37°C, from which excess chemical potentials of ACN (µ EACN) were calculated. We also determined excess partial molar enthalpies of ACN (H EACN) at 6, 20, 30, 37, and 45°C. From these data, excess partial molar entropies of ACN (S EACN) were calculated at 6, 20, and 37°C. Using density data by Benson's group, excess partial molar volumes of ACN (V EACN) were evaluated. The response function data by the same group were also used to evaluate amplitude and wavelength of mean-square fluctuations in terms of volume, entropy, and cross between volume and entropy. All the above quantities and their dependence on the mol fraction of solute, i.e., the effect of additional solute on the above quantities were used to study the effect of acetonitrile on the molecular organization of H2O. It was found that acetonitrile works as a stronger structure-making solute than methanol. Rather its effect on H2O is about the same as that of propan-1-ol.Key words: aqueous acetonitrile, interaction functions, fluctuations.
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40

Rajagopal, K., та S. Edwin Gladson. "Partial molar volume and partial molar compressibility of four homologous α-amino acids in aqueous sodium fluoride solutions at different temperatures". Journal of Chemical Thermodynamics 43, № 6 (2011): 852–67. http://dx.doi.org/10.1016/j.jct.2011.01.004.

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41

Kirchheim, R. "Sorption and partial molar volume of small molecules in glassy polymers." Macromolecules 25, no. 25 (1992): 6952–60. http://dx.doi.org/10.1021/ma00051a036.

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42

Kumar, Anil. "A Study on Partial Molar Volume and Expansion Of oagnesium Butyrate." Physics and Chemistry of Liquids 21, no. 1 (1990): 29–34. http://dx.doi.org/10.1080/00319109008028461.

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43

Hirata, F., T. Imai, and M. Irisa. "Organic Reactions and High Pressure. Molecular Theories of Partial Molar Volume." REVIEW OF HIGH PRESSURE SCIENCE AND TECHNOLOGY 8, no. 2 (1998): 96–103. http://dx.doi.org/10.4131/jshpreview.8.96.

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44

Kamiya, Yoshinori, Yasutoshi Naito, Takuji Hirose, and Keishin Mizoguchi. "Sorption and partial molar volume of gases in poly (dimethyl siloxane)." Journal of Polymer Science Part B: Polymer Physics 28, no. 8 (1990): 1297–308. http://dx.doi.org/10.1002/polb.1990.090280808.

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45

Sawamura, Seiji. "Partial molar volume of L-Valine in water under high pressure." High Pressure Research 33, no. 2 (2013): 245–49. http://dx.doi.org/10.1080/08957959.2013.767899.

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46

Bai, Yujia, Manale Maalouf, Alexander Papandrew, and Thomas A. Zawodzinski. "Proton Conductivity and Partial Molar Volume of Different Polymer Electrolyte Membranes." ECS Transactions 41, no. 1 (2019): 1545–53. http://dx.doi.org/10.1149/1.3635686.

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47

Rybicki, E. "The Partial Molar Volume in Micellar Solutions of Sodium Dodecylbenzene Sulphonate." Tenside Surfactants Detergents 30, no. 1 (1993): 39–41. http://dx.doi.org/10.1515/tsd-1993-300113.

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48

Sharma, Shashi Kant, Nisha Sharma та Poonam Thakur. "A Comparative Study of Molecular Interactions of Three Tetracycline Derivatives with Aqueous β-Cyclodextrin Solution at Different Temperatures". Asian Journal of Chemistry 31, № 9 (2019): 2047–56. http://dx.doi.org/10.14233/ajchem.2019.22091.

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A comparative study of complexation behaviour of three tetracycline derivatives viz. doxycycline hydrochloride, oxytetracycline hydrochloride and minocycline hydrochloride with β-cyclodextrin (β-CD) has been done with the help of various thermodynamic and spectroscopic methods. Density (ρ) and conductivity measurements have been carried out for binary drug/water and ternary drug/water/(β-CD) systems at three different temperature viz. 305.15, 310.15 and 315.15 K. The interactions of these tetracycline derivatives with β-cyclodextrin in aqueous solutions are further studied by means of fluorescence spectroscopy and UV-visible spectroscopy. From the measured density (ρ) data, partial molar volume (Φ°ν), partial molar volume expansibility (ϕ°e), Hepler′s constant (∂2ϕ°ν / ∂T2)P and partial molar volume of transfer (Δϕ°ν) have been obtained. From the conductance studies, the energetically favourable interactions are interpreted in the form of free energy change (ΔG) and the apparent association constant (Ka) was estimated from the fluorescence data.
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49

Shekaari, Hemayat, Mohammed Taghi Zafarani-Moattar, Seyyedeh Narjes Mirheydari, and Elnaz Mazaher Haji Agha. "Effect of 1-Octyl-3-Methylimidazolium Salicylate as an Active Pharmaceutical Ingredient (API-IL) on the Thermodynamic Behavior of Aqueous Glycine Solutions at T= 298.15 K." Pharmaceutical Sciences 25, no. 2 (2019): 154–64. http://dx.doi.org/10.15171/ps.2019.23.

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Background: The thermophysical properties of 1-octyl-3-methylimidazolium salicylate as an active pharmaceutical ingredient based on ionic liquid have been investigated in the presence of aqueous solutions of glycine. Therefore, the scope of this article was to determine these properties by measuring the densities, speeds of sound, viscosities, electrical conductances and refractive indices for ternary (glycine + 1-octyl-3-methylimidazolium salicylate + water) soloutions at T = 298.15 K. Methods: A commercial density and speed of sound measurement apparatus was used to measure the density and speed of sound data. Viscosities, electrical conductivities and refractive indices of the studied solutions were measured using digital viscometer, conductivity meter and refractometer, respectively. Results: Variety of properties such as partial molar volume of transfer ∆traV0ϕ, partial molar isentropic compressibility of transfer ∆traK0ϕ, viscosity B-coefficients of transfer ∆traB, ion association constants (KA) and molar refraction RD were determined to investigate the solute-solute and solute-solvent interactions in these systems. Conclusion: The positive values of transfer properties including partial molar volume of transfer (∆traV0ϕ), partial molar isentropic compressibility of transfer (∆traK0ϕ), and viscosity B-coefficients of transfer (∆traB) indicated that in these systems, the ion-polar and polar-polar interactions are dominant. The calculated hydration number showed that dehydration of glycine occurs in presence of this ionic liquid.
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50

Kumar, Dinesh, and Shashi Kant Sharma. "Molecular Interactions Investigation of L-Histidine in Water and in Aqueous Citric Acid at Different Temperatures Using Volumetric and Acoustic Methods." Zeitschrift für Physikalische Chemie 232, no. 3 (2018): 393–408. http://dx.doi.org/10.1515/zpch-2017-0977.

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AbstractDensities,ρand ultrasonic speeds, u of L-histidine (0.02–0.12 mol·kg−1) in water and 0.1 mol·kg−1aqueous citric acid solutions were measured over the temperature range (298.15–313.15) K with interval of 5 K at atmospheric pressure. From these experimental data apparent molar volume ΦV, limiting apparent molar volume ΦVOand the slopeSV, partial molar expansibilities ΦEO, Hepler’s constant, adiabatic compressibilityβ, transfer volume ΦV, trO, intermolecular free length (Lf), specific acoustic impedance (Z) and molar compressibility (W) were calculated. The results are interpreted in terms of solute–solute and solute–solvent interactions in these systems. It has also been observed that L-histidine act as structure maker in water and aqueous citric acid.
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