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Relevant bibliographies by topics / Equation de Van't Hoff

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Journal articles

Academic literature on the topic 'Equation de Van't Hoff'

Author: Grafiati

Published: 4 June 2021

Last updated: 1 February 2022

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Journal articles on the topic "Equation de Van't Hoff"

1

Holtzer, Alfred. "Persistent confusion on the van't Hoff equation." Biopolymers 42, no. 5 (1997): 499–503. http://dx.doi.org/10.1002/(sici)1097-0282(19971015)42:5<499::aid-bip1>3.0.co;2-l.

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2

FAN, Sen, and Yuanhai ZHU. "Application of Van't Hoff Equation to Phase Equilibrium." University Chemistry 33, no. 3 (2018): 70–73. http://dx.doi.org/10.3866/pku.dxhx201711022.

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3

Han, Shu-ying, Hui-min Yu, Yu-qiong Pei, and Yu-mei Chi. "Selectivity-column temperature relationship as a new strategy in predicting separation of structural analogues in HPLC by using different stationary phases." RSC Advances 5, no. 77 (2015): 62686–96. http://dx.doi.org/10.1039/c5ra09524g.

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The effect of changes in column temperature on van't Hoff equation, as well as relationship of separation and column temperature in high performance liquid chromatography (HPLC) by using different stationary phases, have been discussed and compared.

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4

Rao, Sudhakar M., and P. Shivananda. "Role of osmotic suction in swelling of salt-amended clays." Canadian Geotechnical Journal 42, no. 1 (2005): 307–15. http://dx.doi.org/10.1139/t04-086.

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The present study examines the influence of extraneous salt addition on pore-fluid osmotic suction of a clay soil. The dependence of swell potentials of the salt-amended clay specimens on initial pore-fluid osmotic suction is also examined. The osmotic suctions predicted by Van't Hoff's equation are in excess or smaller than the values calculated from the pore water electrical conductivity, depending on whether the Van't Hoff factor in the Van't Hoff equation is included or not. Experimental results suggest that the salt-amended specimens absorbed water and swelled in response to matric suction and chemical concentration gradients on inundation with water in oedometer cells. Salt also diffused from the soil pores of salt-amended specimens to the reservoir water in oedometer cells in response to chemical concentration gradients. Reduction in effective stress from osmotic flow into the soil specimen and increase in interparticle repulsion from reduction in pore-water salt concentration rendered the total swell potentials of salt-amended specimens independent of initial pore-fluid osmotic suction. The initial pre-fluid osmotic suction does, however, significantly affect the rate of swelling.Key words: clays, chemical properties, swell potential, suction.

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5

Stepanov, I. A. "The Heats of Chemical Reactions: the Van't-Hoff Equation and Calorimetry." Zeitschrift für Physikalische Chemie 219, no. 8 (2005): 1089–97. http://dx.doi.org/10.1524/zpch.2005.219.8.1089.

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6

Son, Changjin, and Sangwoo Lim. "Kinetic Study on the Si₃N₄ Etching in Superheated Water." Solid State Phenomena 314 (February 2021): 113–18. http://dx.doi.org/10.4028/www.scientific.net/ssp.314.113.

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Wet etching of Si3N4 was conducted in superheated water at 160 °C with different additives type and concentration. In general, etching rate of Si3N4 increased with the pH of solution. However, it is difficult to fully explain the Si3N4 etching behavior just with the pH of solution. The OH- concentration (or pH) in superheated water at 160 °C are different from the pH of solution at room temperature. Therefore, the OH- concentrations in superheated water at 160 °C were calculated using van't Hoff equation, equilibrium constant equations, mass and charge balance equations. The calculated OH- concentration at 160 °C showed better correlation with Si3N4 etching rate than that of initial pH of solution.

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7

Xu, Huan Yan, Xue Li, Yan Li, Ping Li, and Wei Chao Liu. "Photocatalytic Degradation of Methyl Orange by TiO₂/Schorl Photocatalyst: Kinetics and Thermodynamics." Applied Mechanics and Materials 713-715 (January 2015): 2789–92. http://dx.doi.org/10.4028/www.scientific.net/amm.713-715.2789.

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An active dye, Methyl Orange (MO) was employed as the target pollutant to evaluate the photocatalytic activity of TiO2/schorl composite and the kinetics and thermodynamics of this process was emphasized in this work. Langmuir–Hinshelwood kinetic model was employed for the kinetic studies and the results revealed that the process of MO photocatalytic discoloration by TiO2/schorl composite followed one order reaction kinetic equation under different conditions. The reaction rate constant (k) increased with initial MO concentration decreasing. When the catalyst dosage or solution pH increased,kvalues increased and then decreased. The possible reasons for these phenomena were discussed. Finally, the thermodynamic parameters ΔG, ΔH, ΔSwere obtained by the classical Van't Hoff equation.

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8

Oberoi, L. M., K. S. Alexander, and A. T. Riga. "Evaluation of an index based on van't Hoff equation to predict PEG-drug eutectic composition." Journal of Thermal Analysis and Calorimetry 78, no. 1 (2004): 83–89. http://dx.doi.org/10.1023/b:jtan.0000042156.21899.de.

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9

Wu, Yun, Hui Mao, Bo Zhao, and Jian Shen. "The interaction of clenbuterol hydrochloride with bovine hemoglobin using spectroscopic techniques and molecular modeling methods." Spectroscopy 23, no. 5-6 (2009): 271–79. http://dx.doi.org/10.1155/2009/696434.

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The interaction of clenbuterol hydrochloride (CL) to bovine hemoglobin (BHb) under physiological conditions was investigated by using UV-vis absorption, fluorescence, circular dichroism (CD) and molecular modeling. The fluorescence intensity of BHb decreased regularly with the gradual increasing concentration of CL. It is observed that there was a prominent interaction between CL and BHb. The fluorescence data revealed that the fluorescence quenching is a static process, and the thermodynamic parameters were calculated according to the Van't Hoff equation. The alternations of protein secondary structure in the presence of CL were determined by the evidence of CD. Molecular modeling study that corroborate our experimental results revealed that the binding mode of CL–BHb complex could be attributed to the hydrophobic interaction and hydrogen bonding, but electronic interaction cannot be excluded.

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10

Gaínza, Alberto Hernández. "Associations of ajmaline and homatropine with bromocresol green and bromophenol blue in dichloromethane: thermodynamic and kinetic parameters." Canadian Journal of Chemistry 65, no. 6 (1987): 1279–91. http://dx.doi.org/10.1139/v87-215.

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Ajmaline (AJ) and homatropine (HM) react with bromocresol green (BCG) and bromophenol blue (BPB) in dichloromethane forming 1:1 and 1:2 ion pairs clearly in a chemical equilibrium. Thermodynamic parameters ΔG0, ΔH0, and ΔS0 are calculated using the Van't Hoff equation. In a large excess of HM a product P is formed from the 1:2 ion pair in a pseudo-first order kinetic process which fits Arrhenius' equation. The P product has been identified as a type of charge transfer complex. The thermodynamic parameters corresponding to the formation of the ion pairs BPB—(AJ)2, BCG—(AJ)2, BPB—(HM)2, and BCG—(HM)2 are, respectively: ΔG0 at 294 K, −26, −21, −26, and −19 kJ/mol; ΔH0, −63, −39, −63, and −61 kJ/mol; ΔS0, −125, −62, −125, and −138 J/K mol (ΔH0 and ΔS0 determined in a 288 to 313 K range). The values of the activation energy, Ea, for the reaction of HM (in large excess) with BCG and BPB are 58 and 91 kJ/mol.

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