A control oriented low order dynamic model for planar SOFC using minimum Gibbs free energy method

2007 ◽  
Vol 165 (1) ◽  
pp. 253-266 ◽  
Author(s):  
Handa Xi ◽  
Jing Sun ◽  
Vasilios Tsourapas
Keyword(s):  
Free Energy ◽  
Dynamic Model ◽  
Gibbs Free Energy ◽  
Energy Method ◽  
Minimum Gibbs Free Energy ◽  
Low Order

Chemical Tension in VLS Nanostructure Growth Process: From Nanohillocks to Nanowires

2007 ◽  
Vol 1017 ◽  
Author(s):  
Na Li ◽  
Teh Y. Tan ◽  
Ulrich Gösele
Keyword(s):  
Free Energy ◽  
Energy Release ◽  
Gibbs Free Energy ◽  
Thermodynamic Limit ◽  
Equilibrium Model ◽  
Growth Process ◽  
Energy State ◽  
Crystal Layer ◽  
Global Equilibrium ◽  
Minimum Gibbs Free Energy

AbstractABSTRACTWe formulate a global equilibrium model to describe the growth of 1-d nanostructures in the VLS process by including also the chemical tension in addition to the physical tensions. The chemical tension derives from the Gibbs free energy release due to the growth of a crystal layer. The system global equilibrium is attained via the balance of the static physical tensions and the dynamic chemical tension, which allows the system to reach the minimum Gibbs free energy state. The model predicts, and provides conditions for the growth of nanowires of all sizes exceeding a lower thermodynamic limit. The model also predicts the conditions distinguishing the growth of nanaohillocks from nanowires.

Ionization equilibrium and thermodynamic and transport properties of a non-ideal hydrogen plasma

2002 ◽  
Vol 68 (4) ◽  
pp. 241-247 ◽  
Author(s):  
T. S. RAMAZANOV ◽  
K. N. DZHUMAGULOVA
Keyword(s):  
Free Energy ◽  
Thermodynamic Functions ◽  
Energy Method ◽  
Hydrogen Plasma ◽  
Charged Particles ◽  
Correlation Effects ◽  
Collective Phenomena ◽  
Ionization Equilibrium ◽  
Minimum Gibbs Free Energy ◽  
Ideal Plasma

The composition of a non-ideal plasma and the thermodynamic functions and conductivity of the system are calculated using the minimum Gibbs free energy method. Interactions of charged particles are described by a pseudopotential model that takes into account collective phenomena (high-order correlation effects) in the plasma.

Gasification of Waste Tyres: Thermodynamic Attainable Region Approach

2021 ◽  
Vol 1045 ◽  
pp. 179-185
Author(s):  
Athi Enkosi Mavukwana ◽  
Celestin Sempuga
Keyword(s):  
Carbon Dioxide ◽  
Free Energy ◽  
Gibbs Free Energy ◽  
Effect Of Temperature ◽  
Syngas Production ◽  
Attainable Region ◽  
Waste Tyres ◽  
Graphical Technique ◽  
Region Approach ◽  
Minimum Gibbs Free Energy

The innovative G-H graphical technique, a plot of Enthalpy vs Gibbs free energy was utilized to obtain a thermodynamically attainable region (AR) for the gasification of waste tyres. The AR is used to examine the interaction between the competing reactions in a gasifier and used to identify optimal targets for the conversion of waste tyres. The objective is to investigate the effect of temperature on the product selectivity. a temperature range of 25-1500°C at 1 bar was used for the analysis. The results show that at temperatures from 200°C to 600°C methane and carbon dioxide are dominant products at minimum Gibbs free energy. However, as the temperature increases, methane production decreases and hydrogen production become more favourable. Between 600°C and 700°C, carbon dioxide and hydrogen are dominant products. The AR results show that the products of gasification (CO and H2) are preferred products at minimum Gibbs free energy only at temperatures from 800°C to 1500°C, when both water and oxygen are used as oxidants. Therefore, syngas production from tyres is only feasible at high temperatures. Temperatures above 1000°C are recommended to prevent the formation of intermediate radicals.

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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