Thermodynamic solution model for trona brines

Haynes, Henry W.

doi:10.1002/aic.690490724

Cited by 22 publications

(19 citation statements)

References 26 publications

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“…8, and method 3 from the experimental data and the activity coefficients of the components of the solutions. Method 2 is generally the first choice because the accuracy of K values is independent of the solubility data as well as the model used to describe the activity coefficients 18–21. Therefore, in this work, the values of K 1 and K 2 were determined by method 2.…”

Section: Resultsmentioning

confidence: 99%

Modeling solid–liquid equilibrium of NH₄Cl‐MgCl₂‐H₂O system and its application to recovery of NH₄Cl in MgO production

Wang

2011

AIChE Journal

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A new method to recover NH 4 Cl from NH 4 Cl-rich aqueous solutions generated in the magnesia (MgO) production is developed on the basis of modeling the solid-liquid equilibrium (SLE) for the NH 4 Cl-MgCl 2 -H 2 O system with the Pitzer model embedded in Aspen Plus TM platform. The SLE values for the ternary system were determined from 278.15 to 348.15 K. The new standard-state chemical potentials of NH 4 Cl and MgCl 2 Á6H 2 O were judicially obtained. The resulting equilibrium constants were used to determine new interaction parameters for the NH 4 Cl-H 2 O and MgCl 2 -H 2 O systems. These new parameters, together with the mixing parameters determined from correlating the experimental values, were used to correlate the equilibrium constant for NH 4 MgCl 3 Á6H 2 O, which plays a key role in NH 4 Cl recovery. The results could extend SLE calculation for the NH 4 Cl-MgCl 2 -H 2 O system from 278.15 to 388.15 K, satisfying the process identification and simulation requirement involved in the recovery process. The phase-equilibrium diagram generated by modeling was illustrated to identify the process alternatives for recovering NH 4 Cl. The resulting course to recover NH 4 Cl by three fractional crystallization operations was finally proved feasible.

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Section: Resultsmentioning

confidence: 99%

Modeling solid–liquid equilibrium of NH₄Cl‐MgCl₂‐H₂O system and its application to recovery of NH₄Cl in MgO production

Wang

2011

AIChE Journal

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“…• N aHCO at constant pressure, both thermodynamic potentials can be obtained by integrating C P (T ) with respect to temperature [44]. For a generic specific heat capacity polynomial of the form C P (T ) = n a n T n available for all components involved as given in [28,33], the ideal gas enthalpy and entropy are evaluated as 18Considering one single heterogeneous reaction, molar flow rates of component i in phase j n j i can be expressed as a function of reaction extent ξ. For a generic reaction, the change in number of moles relative to the stoichiometry of any component is preserved and equals the change of reaction coordinate dξ.…”

Section: Discussionmentioning

confidence: 99%

“…To find the optimal calciner operating temperature, the equilibrium constants of all possible reactions involved must be evaluated. According to thermochemical analysis of Trona brines by [28] utilising Pitzer's activity coefficient model, the equilibrium constants of above reactions as a function of temperature K i = f (T ) can be approximated by…”

Section: Methodsmentioning

confidence: 99%

“…In this section, calciner reactor outlet compositions as predicted by Aspen Plus V9 are validated against a simple thermodynamic model describing the dependence of Gibbs free energy with respect to changes in various operating parameters is outlined. Specific heat capacity data utilised throughout this section is taken from [28] for N aHCO 3(s) and from the NASA Glenn Coefficients for Calculating Thermodynamic Properties of Individual Species [33] for all remaining components. A detailed analysis and derivation of all formulae obtained is presented in Appendix A and Appendix B.…”

Section: Gibbs Free Energy Minimisationmentioning

confidence: 99%

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Sodium carbonate-based post combustion carbon capture utilising trona as main sorbent feed stock

Furcas

Pragot

Chacartegui

et al. 2020

Energy Conversion and Management

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In the pursuit of shifting technology towards sustainable, environmentally benign processes, post-combustion carbon capture technology is recognised to be a timely mitigation option. This paper presents the development of a novel sodium carbonate-based post combustion carbon capture process utilising the carbonate mineral trona (trisodium hydrogendicarbonate dihydrate) as main sorbent feedstock source. The energy penalty, the fraction of energy sacrificed to capture CO 2 relative to the net energy produced serves as main performance indicator. Investigations on the correlative relationship between energy penalty as a function of capture efficiency are carried out by retrofitting the process to a 600 M W reference coal-fired power plant. The energy penalty of the global system features a distinct local minimum of 3.99 %, corresponding to a CO 2 capture efficiency of 90.00 % and a CO 2 outlet purity of 99.90%. The Specific Primary Energy Consumption for CO 2 Avoided (SPECCA) index corresponding to this minimum is evaluated to be SPECCA = 0.514 M J kg CO −1 2 . Sensitivity analyses on the effect of increasingly high SO 2 flue gas volume fractions y SO 2 show that the capture efficiency is virtually unimpaired for calcination temperatures of 190 ≤ T ≤ 280 • C and y SO 2 ranging from 0.50 to 0.70 %. Whilst commercially available CO 2 capture technology is energy intense and prone to sorbent degradation, the process developed retains high capture efficiencies of calcium oxide-based looping cycles at low operating temperatures and eliminates the predisposition of amine-based sorbents utilised in scrubbing capture schemes to deplete due to the presence of SO 2 in the inlet flue gas stream. It can be concluded that sodium carbonate based post-combustion capture processes are a competitive alternative to existing CO 2 capture technologies.

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“…Thus, in addiction to sodium bicarbonate (NaHCO3) other salts can be formed from the reactions involving CO2, water and soda ash: sodium carbonate decahydrate (Na2CO3•10H2O), sodium carbonate heptahydrate (Na2CO3•8H2O), sodium carbonate monohydrate (Na2CO3•H2O), Wegscheider's salt (Na2CO3•3NaHCO3) and trona (Na2CO3•NaHCO3•2H2O) [90]. Figure 4 shows the evolution of reaction equilibrium constants with temperature for the production of NaHCO3 and other salts used in this work (adapted from [9]).…”

Section: Chemistry Of the Processmentioning

confidence: 99%

Dry carbonate process for CO2 capture and storage: Integration with solar thermal power

Bonaventura

Chacartegui

Valverde

et al. 2018

Renewable and Sustainable Energy Reviews

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Capture and sequestration of CO2 released by conventional fossil fuel combustion is an urgent need to mitigate global warming. In this work, main CO2 capture and sequestration (CCS) systems are reviewed, with the focus on their integration with renewables in order to achieve power plants with nearly zero CO2 emissions. As a case study, the manuscript analyses the integration of a CO2 sorptiondesorption cycle based on Na2CO3/NaHCO3 into a coal fired power plant (CFPP) for CO2 capture with solar support for sorbent regeneration. The Dry Carbonate Process relies on the use of a dry regenerable sorbent such as sodium carbonate (Na2CO3) to remove CO2 from flue gases. Na2CO3 is converted to sodium bicarbonate (NaHCO3) through reaction with CO2 and water steam. Na2CO3 is regenerated when NaHCO3 is heated, which yields a gas stream mostly containing CO2 and H2O. Condensation of H2O produces a pure CO2 stream suitable for its subsequent use or compression and sequestration. In this paper, the application of the Dry Carbonate CO2 capture process in a coal-based power plant is studied with the goal of optimizing CO2 capture efficiency, heat and power requirements. Integration of this CO2 capture process requires an additional heat supply which would reduce the global power plant efficiency by around 9-10%. Dry Carbonate Process has the advantage compared with other CCS technologies that requires a relatively low temperature for sorbent regeneration (<200ºC). It allows an effective integration of medium temperature solar thermal power to assist NaHCO3 decarbonation. This integration reduces efficiency losses to the associated with mechanical parasitic consumption, resulting in a fossil fuel energy penalty of 3-4% (including CO2 compression). The paper shows the viability of the concept through economic analyses under different scenarios. The results suggest the interest of advancing in this Solar-CCS integrated concept, which shows favourable outputs compared to other CCS technologies.

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Thermodynamic solution model for trona brines

Cited by 22 publications

References 26 publications

Modeling solid–liquid equilibrium of NH₄Cl‐MgCl₂‐H₂O system and its application to recovery of NH₄Cl in MgO production

Modeling solid–liquid equilibrium of NH₄Cl‐MgCl₂‐H₂O system and its application to recovery of NH₄Cl in MgO production

Sodium carbonate-based post combustion carbon capture utilising trona as main sorbent feed stock

Dry carbonate process for CO2 capture and storage: Integration with solar thermal power

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Thermodynamic solution model for trona brines

Cited by 22 publications

References 26 publications

Modeling solid–liquid equilibrium of NH4Cl‐MgCl2‐H2O system and its application to recovery of NH4Cl in MgO production

Modeling solid–liquid equilibrium of NH4Cl‐MgCl2‐H2O system and its application to recovery of NH4Cl in MgO production

Sodium carbonate-based post combustion carbon capture utilising trona as main sorbent feed stock

Dry carbonate process for CO2 capture and storage: Integration with solar thermal power

Contact Info

Product

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Modeling solid–liquid equilibrium of NH₄Cl‐MgCl₂‐H₂O system and its application to recovery of NH₄Cl in MgO production

Modeling solid–liquid equilibrium of NH₄Cl‐MgCl₂‐H₂O system and its application to recovery of NH₄Cl in MgO production