Vaporization enthalpy and the molar surface Gibbs free energy for ionic liquids [C n Dmim][NTF 2 ] ( n = 2, 4)

2016 ◽  
Vol 101 ◽  
pp. 278-284 ◽  
Author(s):  
Jie Wei ◽  
Ben-Han Fan ◽  
Yi Pan ◽  
Nan-Nan Xing ◽  
Shu-Qin Men ◽  
...  
Keyword(s):  
Free Energy ◽  
Ionic Liquids ◽  
Gibbs Free Energy ◽  
Vaporization Enthalpy

Physicochemical properties of hydrophobic hexafluoroantimonate ionic liquids and applications of the mole surface Gibbs free energy

Ionics ◽  
2020 ◽  
Vol 26 (11) ◽  
pp. 5585-5595
Author(s):  
Qiang Yan ◽  
Jie Wei ◽  
Jin Liu ◽  
Zhiheng Zhang ◽  
Dawei Fang
Keyword(s):  
Free Energy ◽  
Ionic Liquids ◽  
Physicochemical Properties ◽  
Gibbs Free Energy

Chemical equilibrium and chemical kinetics

2018 ◽  
Author(s):  
Dennis Sherwood ◽  
Paul Dalby
Keyword(s):  
Free Energy ◽  
Equilibrium Constant ◽  
Gibbs Free Energy ◽  
Chemical Kinetics ◽  
Chemical Equilibrium ◽  
First Principles ◽  
Effect Of Temperature ◽  
Total System ◽  
Free Energies

Building on the previous chapter, this chapter examines gas phase chemical equilibrium, and the equilibrium constant. This chapter takes a rigorous, yet very clear, ‘first principles’ approach, expressing the total Gibbs free energy of a reaction mixture at any time as the sum of the instantaneous Gibbs free energies of each component, as expressed in terms of the extent-of-reaction. The equilibrium reaction mixture is then defined as the point at which the total system Gibbs free energy is a minimum, from which concepts such as the equilibrium constant emerge. The chapter also explores the temperature dependence of equilibrium, this being one example of Le Chatelier’s principle. Finally, the chapter links thermodynamics to chemical kinetics by showing how the equilibrium constant is the ratio of the forward and backward rate constants. We also introduce the Arrhenius equation, closing with a discussion of the overall effect of temperature on chemical equilibrium.

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