Application of reaction equilibrium thermodynamic model for correlation of H2S solubility in ionic liquids [emim][Ace] and [hmim][Ace] using CPA equation of state

2019 ◽  
Vol 37 (14) ◽  
pp. 1648-1654 ◽  
Author(s):  
Alireza Afsharpour
Keyword(s):  
Ionic Liquids ◽  
Equation Of State ◽  
Thermodynamic Model ◽  
Equilibrium Thermodynamic ◽  
Reaction Equilibrium

Surface thermodynamic properties of ionic liquids from new molecular thermodynamic model and ion-contribution equation of state

2015 ◽  
Vol 122 ◽  
pp. 622-629 ◽  
Author(s):  
Mohammad Mehdi Alavianmehr ◽  
Sayed Mostafa Hosseini ◽  
Behzad Haghighi ◽  
Jalil Moghadasi
Keyword(s):  
Ionic Liquids ◽  
Equation Of State ◽  
Thermodynamic Properties ◽  
Thermodynamic Model

scholarly journals Measuring and Modeling the Solubility of Hydrogen Sulfide in rFeCl3/[bmim]Cl

Processes ◽  
2021 ◽  
Vol 9 (4) ◽  
pp. 652
Author(s):  
Huanong Cheng ◽  
Na Li ◽  
Rui Zhang ◽  
Ning Wang ◽  
Yuanyuan Yang ◽  
...  
Keyword(s):  
Ionic Liquid ◽  
Hydrogen Sulfide ◽  
Equilibrium Constant ◽  
Chemical Reaction ◽  
Chemical Equilibrium ◽  
Thermodynamic Model ◽  
Equilibrium Thermodynamic ◽  
Mean Relative Error ◽  
The Mean ◽  
Reaction Equilibrium

The solubility of hydrogen sulfide in different mole ratios of ferric chloride and 1-butyl-3-methylimidazolium chloride ionic liquid (rFeCl3/[bmim]Cl, r = 0.6, 0.8, 1.0, 1.2, 1.4) at temperatures of 303.15 to 348.15 K and pressures of 100 to 1000 kPa was determined. The total solubility increased with the increase of pressure and the decrease of temperature. The solubility data were fitted using the reaction equilibrium thermodynamic model (RETM). The mean relative error between the predicted value and the measured value was less than 4%. Henry’s coefficient and the equilibrium constant of chemical reaction at each temperature were calculated. Henry’s coefficient first decreased and then increased with the increase of mole ratio, and increased with the increase of temperature. The equilibrium constant of the chemical reaction followed the same law as Henry’s coefficient. The chemical solubility was related to both Henry’s coefficient and the chemical equilibrium constant. H2S had the highest chemical solubility in FeCl3/[bmim]Cl at a mole ratio of 0.6 and a temperature of 333.15 K. The chemical solubility increased with the increase of pressure.

Modeling the Water Solubility in Imidazolium-Based Ionic Liquids Using the Peng–Robinson Equation of State

2019 ◽  
Vol 58 (10) ◽  
pp. 4341-4353
Author(s):  
Jeremías Martínez ◽  
María A. Zúñiga-Hinojosa ◽  
Ricardo Macías-Salinas
Keyword(s):  
Ionic Liquids ◽  
Equation Of State ◽  
Water Solubility ◽  
Robinson Equation

Molecular dynamics studies of CaAl2Si2O8 liquid. Part II: Equation of state and a thermodynamic model

2009 ◽  
Vol 73 (22) ◽  
pp. 6937-6951 ◽  
Author(s):  
Mark S. Ghiorso ◽  
Dean Nevins ◽  
Ian Cutler ◽  
Frank J. Spera
Keyword(s):  
Molecular Dynamics ◽  
Equation Of State ◽  
Thermodynamic Model ◽  
Liquid Part

A perturbed hard-sphere equation of state extended to imidazolium-based ionic liquids

Ionics ◽  
2010 ◽  
Vol 16 (8) ◽  
pp. 757-761 ◽  
Author(s):  
Sayed Mostafa Hosseini ◽  
Jalil Moghadasi ◽  
Mohammad Mehdi Papari
Keyword(s):  
Ionic Liquids ◽  
Equation Of State ◽  
Hard Sphere ◽  
Sphere Equation

A new perspective on the electron transfer: recovering the Butler–Volmer equation in non-equilibrium thermodynamics

2016 ◽  
Vol 18 (36) ◽  
pp. 24966-24983 ◽  
Author(s):  
Wolfgang Dreyer ◽  
Clemens Guhlke ◽  
Rüdiger Müller
Keyword(s):  
Electron Transfer ◽  
Asymptotic Analysis ◽  
Thermodynamic Model ◽  
Equilibrium Thermodynamic ◽  
Equilibrium Thermodynamics ◽  
Electrochemical Systems ◽  
New Perspective ◽  
Physical Phenomena ◽  
Insight Into ◽  
Non Equilibrium

Butler–Volmer equations can be recovered from a complete non-equilibrium thermodynamic model by application of asymptotic analysis. Thereby we gain insight into the coupling of different physical phenomena and can derive Butler–Volmer equations for very different materials and electrochemical systems.

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