Relevant bibliographies by topics / Chemical Thermodynamics

Contents

  1. Journal articles
  2. Dissertations / Theses
  3. Books
  4. Book chapters
  5. Conference papers
  6. Reports

Academic literature on the topic 'Chemical Thermodynamics'

Author: Grafiati
Published: 4 June 2021
Last updated: 6 September 2023

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Journal articles on the topic "Chemical Thermodynamics"

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Beda, László. "Chemical thermodynamics." Journal of Thermal Analysis and Calorimetry 44, no. 2 (February 1995): 513–16. http://dx.doi.org/10.1007/bf02636140.

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Vincze, Gy, and A. Szasz. "Critical analysis of the thermodynamics of reaction kinetics." JOURNAL OF ADVANCES IN PHYSICS 10, no. 1 (August 5, 2015): 2538–59. http://dx.doi.org/10.24297/jap.v10i1.1340.

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Our objective is to show the weakness of the recent thermodynamics of chemical reactions. We show that such a thermodynamic theory of chemical reactions, which could be similar to the generalized Onsager’s theory in thermodynamics, is not reality at the moment.Â
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Pekař, Miloslav. "Thermodynamics and foundations of mass-action kinetics." Progress in Reaction Kinetics and Mechanism 30, no. 1-2 (June 2005): 3–113. http://dx.doi.org/10.3184/007967405777874868.

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A critical overview is given of phenomenological thermodynamic approaches to reaction rate equations of the type based on the law of mass-action. The review covers treatments based on classical equilibrium and irreversible (linear) thermodynamics, extended irreversible, rational and continuum thermodynamics. Special attention is devoted to affinity, the applications of activities in chemical kinetics and the importance of chemical potential. The review shows that chemical kinetics survives as the touchstone of these various thermody-namic theories. The traditional mass-action law is neither demonstrated nor proved and very often is only introduced post hoc into the framework of a particular thermodynamic theory, except for the case of rational thermodynamics. Most published “thermodynamic'’ kinetic equations are too complicated to find application in practical kinetics and have merely theoretical value. Solely rational thermodynamics can provide, in the specific case of a fluid reacting mixture, tractable rate equations which directly propose a possible reaction mechanism consistent with mass conservation and thermodynamics. It further shows that affinity alone cannot determine the reaction rate and should be supplemented by a quantity provisionally called constitutive affinity. Future research should focus on reaction rates in non-isotropic or non-homogeneous mixtures, the applicability of traditional (equilibrium) expressions relating chemical potential to activity in non-equilibrium states, and on using activities and activity coefficients determined under equilibrium in non-equilibrium states.
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Penocchio, Emanuele, Francesco Avanzini, and Massimiliano Esposito. "Information thermodynamics for deterministic chemical reaction networks." Journal of Chemical Physics 157, no. 3 (July 21, 2022): 034110. http://dx.doi.org/10.1063/5.0094849.

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Information thermodynamics relates the rate of change of mutual information between two interacting subsystems to their thermodynamics when the joined system is described by a bipartite stochastic dynamics satisfying local detailed balance. Here, we expand the scope of information thermodynamics to deterministic bipartite chemical reaction networks, namely, composed of two coupled subnetworks sharing species but not reactions. We do so by introducing a meaningful notion of mutual information between different molecular features that we express in terms of deterministic concentrations. This allows us to formulate separate second laws for each subnetwork, which account for their energy and information exchanges, in complete analogy with stochastic systems. We then use our framework to investigate the working mechanisms of a model of chemically driven self-assembly and an experimental light-driven bimolecular motor. We show that both systems are constituted by two coupled subnetworks of chemical reactions. One subnetwork is maintained out of equilibrium by external reservoirs (chemostats or light sources) and powers the other via energy and information flows. In doing so, we clarify that the information flow is precisely the thermodynamic counterpart of an information ratchet mechanism only when no energy flow is involved.
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Tanabe, Katsuaki. "A time–energy uncertainty relation in chemical thermodynamics." AIP Advances 12, no. 3 (March 1, 2022): 035224. http://dx.doi.org/10.1063/5.0084251.

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An analogy between the thermodynamic inequalities presented by Nicholson et al. [Nat. Phys. 16, 1211 (2020)] and by Yoshimura and Ito [Phys. Rev. Res. 3, 013175 (2021)] is discussed. As a result, a time–energy uncertainty relation in chemical thermodynamics in terms of Gibbs free energy and chemical potential is derived. It is numerically demonstrated that the uncertainly relation holds in a model system of oscillatory Brusselator reactions. Our result bridges the thermodynamic time–information uncertainty relation and free energy evolution in chemical reactions.
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Sandler, S. I. "Unusual chemical thermodynamics." Pure and Applied Chemistry 71, no. 7 (July 30, 1999): 1167–81. http://dx.doi.org/10.1351/pac199971071167.

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Sandler, Stanley I. "Unusual chemical thermodynamics." Journal of Chemical Thermodynamics 31, no. 1 (January 1999): 3–25. http://dx.doi.org/10.1006/jcht.1998.0420.

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Dymond, J. H. "Basic chemical thermodynamics." Talanta 38, no. 9 (September 1991): 1067–68. http://dx.doi.org/10.1016/0039-9140(91)80329-x.

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Kocherginsky, Nikolai, and Martin Gruebele. "Mechanical approach to chemical transport." Proceedings of the National Academy of Sciences 113, no. 40 (September 19, 2016): 11116–21. http://dx.doi.org/10.1073/pnas.1600866113.

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Nonequilibrium thermodynamics describes the rates of transport phenomena with the aid of various thermodynamic forces, but often the phenomenological transport coefficients are not known, and the description is not easily connected with equilibrium relations. We present a simple and intuitive model to address these issues. Our model is based on Lagrangian dynamics for chemical systems with dissipation, so one may think of the model as physicochemical mechanics. Using one main equation, the model allows a systematic derivation of all transport and equilibrium equations, subject to the limitation that heat generated or absorbed in the system must be small for the model to be valid. A table with all major examples of transport and equilibrium processes described using physicochemical mechanics is given. In equilibrium, physicochemical mechanics reduces to standard thermodynamics and the Gibbs–Duhem relation, and we show that the First and Second Laws of thermodynamics are satisfied for our system plus bath model. Out of equilibrium, our model provides relationships between transport coefficients and describes system evolution in the presence of several simultaneous external fields. The model also leads to an extension of the Onsager–Casimir reciprocal relations for properties simultaneously transported by many components.
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Sevilla, Francisco J. "Thermodynamics of Low-Dimensional Trapped Fermi Gases." Journal of Thermodynamics 2017 (January 26, 2017): 1–12. http://dx.doi.org/10.1155/2017/3060348.

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The effects of low dimensionality on the thermodynamics of a Fermi gas trapped by isotropic power-law potentials are analyzed. Particular attention is given to different characteristic temperatures that emerge, at low dimensionality, in the thermodynamic functions of state and in the thermodynamic susceptibilities (isothermal compressibility and specific heat). An energy-entropy argument that physically favors the relevance of one of these characteristic temperatures, namely, the nonvanishing temperature at which the chemical potential reaches the Fermi energy value, is presented. Such an argument allows interpreting the nonmonotonic dependence of the chemical potential on temperature, as an indicator of the appearance of a thermodynamic regime, where the equilibrium states of a trapped Fermi gas are characterized by larger fluctuations in energy and particle density as is revealed in the corresponding thermodynamics susceptibilities.
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Dissertations / Theses on the topic "Chemical Thermodynamics"

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Haghtalab, Ali. "Thermodynamics of aqueous electrolyte solutions." Thesis, McGill University, 1990. http://digitool.Library.McGill.CA:80/R/?func=dbin-jump-full&object_id=74540.

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The focus of this work is the thermodynamics of aqueous solutions of strong electrolytes for both binary and multicomponent systems.
A new excess Gibbs energy function to represent the deviations from ideality of binary electrolyte solutions was derived. The function consists of two contributions, one due to long-range forces, represented by the Debye-Huckel theory, and the other due to short-range forces represented by the local composition concept. The model is valid for the whole range of electrolyte concentrations, from dilute solutions up to saturation. The model consistently produces better results particularly at the higher concentration regions in which the other models deteriorate.
An electrochemical cell apparatus using Ion-Selective Electrodes (ISE) was constructed to measure the electromotive force (emf) of ions in the aqueous electrolyte mixtures. For the NaCl-NaNO$ sb3$-H$ sb2$O system, the data for the mean ionic activity coefficient of NaCl was obtained in order to show the reproducibility of literature data and to test the validity of the experimental procedure. The data for mean ionic activity coefficient of the following systems were also collected: (1) NaBr-NaNO$ sb3$-H$ sb2$O (a system with common ion); (2) NaBr-Ca(NO$ sb3$)$ sb2$-H$ sb2$O (a system with no-common-ion).
A novel mixing rule was proposed for the mean activity coefficients of electrolytes in mixtures in terms of the mean ionic activity coefficients of electrolytes in the binary solutions. The rule is applicable to multicomponent systems which obey Harned's Rule. Predictions are in excellent agreement with experimental data for ternary systems which follow the Bronsted specific ionic theory.
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Avlonitis, Dimitrios Anastassios. "Thermodynamics of gas hydrate equilibria." Thesis, Heriot-Watt University, 1992. http://hdl.handle.net/10399/803.

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Reservoir fluids are usually saturated with water at reservoir conditions and may form gas hydrates in transfer lines, which potentially may plug the system. For long subsea pipelines, methanol injection is the practical means for preventing hydrate formation and for decomposing blockages. For efficient and economical pipeline design and operation, phase boundaries, phase fractions and distribution of water and methanol among the equilibrium phases of the system must be accurately known. The system comprising reservoir fluids, water and methanol demonstrates a complex multiphase behaviour and currently no quantitatively adequate description for it has been detailed in the open literature. The problem is addressed in this thesis by a consistent application of classical equilibrium thermodynamics. At ordinary operating conditions any combination of as many as six phases can be potentially present. For the description of the vapour and all liquid phases, we use one cubic equation of state with nonconventional mixing rules developed as part of this work. Classical thermodynamics together with the cell theory of van der Waals and Platteeuw were employed for the development of a general model for the calculation of heat capacities of gas hydrates. A consistent methodology has also been developed for obtaining the potential parameters of the cell model. Thereafter, application of the model demonstrates that for nearly spherical guest molecules the classical cell theory is a strictly valid description of gas hydrates. However, complex guest molecules distort the hydrate lattice, resulting in variation of the numerical values of certain parameters of the model. This work presents an efficient algorithm for the solution of the problem of the identity of the equilibrium phases in multiphase systems where gas hydrates are potentially present. The algorithm is based on the alternative use of two equivalent forms of the Gibbs tangent plane criterion and it is believed to be more appropriate for systems involving gas hydrate equilibria than previous methods. Application of the proposed algorithm in several regions of the phase diagram of both binary and multicomponent systems shows that it can be used reliably to solve any phase equilibria problem, including the location of phase boundaries. In summary this work presents a consistent, efficient and reliable scheme for multiphase equilibrium calculations of systems containing reservoir fluids, water and methanol. Favourable results have been obtained by comparison with diverse experimental data reported in the open literature and it is believed that the proposed correlation can be used reliably for pipeline design and operation.
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Rickards, Andrew M. J. "Hygroscopic organic aerosol : thermodynamics, kinetics, and chemical synthesis." Thesis, University of Bristol, 2015. http://ethos.bl.uk/OrderDetails.do?uin=uk.bl.ethos.686238.

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Aerosols play a crucial role in many areas of scientific relevance including in new technologies to deliver medicine to the lungs, and in fuel injection and spray drying. Aerosols have a profound impact on the atmosphere, influencing radiative forcing both by scattering solar radiation and by influencing cloud properties. Organic aerosols are a major component, making up 20 - 90 % of the submicron mass by region, and are emitted from many natural and anthropogenic sources. This thesis presents new measurements of the hygroscopic behaviour of single organic droplets confined using two techniques: aerosol optical tweezers (AOT) and an electrodynamic balance (EDB). Values of the hygroscopicity parameter (K) are derived and added to a comprehensive literature survey to elucidate a relationship with droplet composition, in terms of the molecular ratio of oxygen to carbon atoms (OIC). These data are shown to be in broad qualitative agreement. However, variation in K for droplets of the same OIC is found to be significant, and discrepancies between subsaturated and supersaturated data are evident. The variabilities and uncertainties associated with characterising the kinetics of water transport in ultraviscous sucrose droplets are also presented. Droplets are exposed to a perturbation in relative humidity, and the resultant characteristic relaxation timescale (r) is determined from stimulated Raman spectra. Comparison of the experimental· evaporation data with simulated timescales shows excellent agreement, and r is shown to increase strongly with droplet radius. Qualitative agreement between experimental condensation data and simulated timescales is presented, and r is shown to increase with wait time (the time the perturbation is applied for). Finally, factors influencing the ability to perform controlled chemical synthesis in single droplets are investigated. The formation of Nylon-6,1 0 at the droplet-gas phase interface is used as a test case of the system, and the interplay between droplet volatility and reactivity is shown to be crucial for controlling the reaction. Further investigations demonstrate synthesis of picomolar concentrations (equivalent to a single dose) of a functionalised caprolactam anti-cancer drug. The challenges in reliably validating drug formation in aerosol are presented.
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Tamim, Jihane. "A continuous thermodynamics model for multicomponent droplet vaporization." Thesis, National Library of Canada = Bibliothèque nationale du Canada, 1997. http://www.collectionscanada.ca/obj/s4/f2/dsk3/ftp05/mq20955.pdf.

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Khoshkbarchi, Mohammad Khashayar. "Thermodynamics of amino acids in aqueous electrolyte solutions." Thesis, McGill University, 1996. http://digitool.Library.McGill.CA:80/R/?func=dbin-jump-full&object_id=42068.

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A novel method has been developed for the measurement of the activity coefficients of an amino acid and the mean ionic activity coefficients of an electrolyte in water-electrolyte-amino acid systems. The method uses an electrochemical cell with two ion selective electrodes and a reference electrode. Activity coefficient data, at 298.15 K, for eight water-electrolyte-amino acid systems were measured. The cell consisted of a cation and an anion ion selective electrode, and the potential of each was measured versus a double junction reference electrode. The amino acids studied were glycine, DL-alanine, DL-valine and DL-serine and the electrolytes studied were NaCl and KCl. For the same systems, the solubilities at 298.15 K of the amino acids were measured at various electrolyte concentrations. The results show that the activity coefficients and the solubility of the amino acid in aqueous electrolyte solutions are strongly affected by the concentrations of both the electrolyte and the amino acid, the chemical structure of the amino acid and the nature of the cation of the electrolyte.
The activity coefficients of amino acids in aqueous electrolyte solutions were modelled using a two-parameter excess Gibbs free energy model based on the contribution of a long range interaction term represented by the Bromley or the K-V model and a short range interaction term represented by the NRTL or the Wilson model.
A model based on the perturbation of a hard sphere reference system, coupled with a mean spherical approximation model, was also developed to correlate the activity coefficient of the amino acid and the mean ionic activity coefficient of the electrolyte in water-electrolyte-amino acid systems. The model can also predict the activity coefficients of amino acids in aqueous electrolyte solutions, without adjusting any parameter, at low electrolyte concentrations and slightly deviates from the experimental data at higher electrolyte concentrations.
A model was developed to correlate the solubilities of amino acids in aqueous and aqueous electrolyte solutions. The activity coefficients of amino acids in both aqueous and aqueous electrolyte solutions were represented by the perturbed mean spherical approximation model. It was shown that upon availability of independently evaluated experimental data for $ Delta h$ and $ Delta g$, the water-amino acid solubility model can accurately predict the solubility of amino acids in aqueous solutions without any adjustable parameter.
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Ferguson, Todd R. (Todd Richard). "Lithium-ion battery modeling using non-equilibrium thermodynamics." Thesis, Massachusetts Institute of Technology, 2014. http://hdl.handle.net/1721.1/87133.

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Thesis: Ph. D., Massachusetts Institute of Technology, Department of Chemical Engineering, 2014.
This electronic version was submitted by the student author. The certified thesis is available in the Institute Archives and Special Collections.
Cataloged from student-submitted PDF version of thesis.
Includes bibliographical references (pages 147-161).
The focus of this thesis work is the application of non-equilibrium thermodynamics in lithium-ion battery modeling. As the demand for higher power and longer lasting batteries increases, the search for materials suitable for this task continues. Traditional battery modeling uses dilute solution kinetics and a fit form of the open circuit potential to model the discharge. This work expands on this original set of equations to include concentrated solution kinetics as well as thermodynamics-based modeling of the open circuit potential. This modification is advantageous because it does not require the cell to be built in order to be modeled. Additionally, this modification also allows phase separating materials to be modeled directly using phase field models. This is especially useful for materials such as lithium iron phosphate and graphite, which are currently modeled using a fit open circuit potential and an artificial phase boundary (in the case of lithium iron phosphate). This thesis work begins with a derivation of concentrated solution theory, beginning with a general reaction rate framework and transition state theory. This derivation includes an overview of the thermodynamic definitions used in this thesis. After the derivation, transport and conduction in porous media are considered. Effective transport properties for porous media are presented using various applicable models. Combining concentrated solution theory, mass conservation, charge conservation, and effective porous media properties, the modified porous electrode theory equations are derived. This framework includes equations to model mass and charge conservation in the electrolyte, mass conservation in the solid intercalation particles, and electron conservation in the conducting matrix. These mass and charge conservation equations are coupled to self-consistent models of the charge transfer reaction and the Nernst potential. The Nernst potential is formulated using the same thermodynamic expressions used in the mass conservation equation for the intercalation particles. The charge transfer reaction is also formulated using the same thermodynamic expressions, and is presented in a form similar to the Butler-Volmer equation, which determines the reaction rate based on the local overpotential. This self-consistent set of equations allows both homogeneous and phase separating intercalation materials to be modeled. After the derivation of the set of equations, the numerical methods used to solve the equations in this work are presented, including the finite volume method and solution methods for differential algebraic equations. Then, example simulations at constant current are provided for homogeneous and phase separating materials to demonstrate the effect of changing the solid diffusivity and discharge rate on the cell voltage. Other effects, such as coherency strain, are also presented to demonstrate their effect on the behavior of particles inside the cell (e.g. suppression of phase separation). After the example simulations, specific simulations for two phase separating materials are presented and compared to experiment. These simulations include slow discharge of a lithium iron phosphate cell at constant current, and electrolyte-limited discharge of a graphite cell at constant potential. These two simulations are shown to agree very well with experimental data. In the last part of this thesis, the most recent work is presented, which is based on modeling lithium iron phosphate particles including coherency strain and surface wetting. These results are qualitatively compared with experimental data. Finally, future work in this area is considered, along with a summary of the thesis.
by Todd R. Ferguson.
Ph. D.
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Cowles, Heather Jane. "Kinetics and thermodynamics of chemical reactions in aqueous solutions." Thesis, University of Leicester, 1990. http://hdl.handle.net/2381/34067.

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The kinetics of reaction and solvation properties of binary aqueous mixtures are discussed from different theoretical standpoints. Kinetic data are reported for reactions involving several Iron (II) complex cations in binary aqueous mixtures. The Savage-Wood Additivity Group Scheme (SWAG) is applied to kinetic data for the aquation of [Fe (5-nitro-1, 10-phenanthroline) 3]2+ in binary aqueous mixtures. Limitations of the theory are examined. The theory works well for reactions in alcohol-water and some carboxylic acid-water mixtures but not for reactions in urea-water and cyclic ether-water mixtures. The conclusion is reached that this theory can only be applied to relatively simple solutions. Otherwise, the assumptions made in the theory are not valid. Attention is then turned to the Kirkwood-Buff theory which can be applied to reactions in mixtures containing significant amounts of the cosolvent. Few assumptions are made in its derivation. This theory is used to probe the properties of a wide range of binary aqueous mixtures. Kinetic data describing reactions in these binary mixtures are then examined, leading to a consideration of preferential solvation. Finally, the possibility of monitoring chemical reactions under isochoric conditions is considered. A meaningful isochoric volume is defined. Kinetic and equilibrium reaction data are then analysed under these isochoric conditions.
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TORNATORE, LUCA. "HYDRODYNAMICAL SIMULATIONS OF GALAXY CLUSTERS: THERMODYNAMICS AND CHEMICAL ENRICHMENT." Doctoral thesis, Università degli studi di Trieste, 2005. http://thesis2.sba.units.it/store/handle/item/13085.

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Angevine, Christopher. "Nanopore thermodynamics via infrared laser heating." VCU Scholars Compass, 2017. https://scholarscompass.vcu.edu/etd/5200.

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Single molecule nanopore spectroscopy is a label-free method for characterizing a wide variety of water-soluble molecules. Recently there have been efforts to expand nanopore sensing to new areas of study. Forensic investigators require an easy to deploy method to identify an unknown number of contributors in a solution. Currently there is no easily available method to distinguish between a single or multiple contributor solution of DNA before being processed by more advanced analytical techniques which has led to wasted time and resources increasing the backlog of samples waiting to be processed. In this work we present a new nanopore technique capable of distinguishing between single and multiple contributors with an easy to deploy infrared heating laser. Previous cluster-nanopore enhancement interaction studies, produced by this group, have found that polymers in the presence of a gold-nanopore complex spend longer periods of time inside the pore. This is of great interest to the nanopore sensing community because longer residence times enable more accurate statistics on single polymers. In order to understand why x some polymers see large enhancements in the residence times (i.e. 20x) while other polymers see much less enhancement (i.e. 3x) a more complete picture of the free energy components is required. By using a IR heating laser, we construct an Eyring transition graph to extract the enthalpic and entropic energy components to find entropy plays a more important role than previously thought when a polymer interacts with a the nanopore. For nanoconfined polymers, entropy plays an important role on how a polymer will interact with the cluster-nanopore structure which in turn may lead to an increase or decrease of the residence time enhancement factor. This work shows with the addition of an infrared laser heater to a nanopore system a new tool has been added to the field. The IR laser coupled to a nanopore system allows for precise adjustments to residence times of events and extracts the free energy components without the need to physically modify the nanopore.
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Cheong, Ae-Gyeong. "Interfacial thermodynamics of liquid crystals : applications to capillary instabilities." Thesis, McGill University, 2004. http://digitool.Library.McGill.CA:80/R/?func=dbin-jump-full&object_id=84493.

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Most current applications and uses of liquid crystalline materials involve surfaces and interfaces. Prominent examples are high performance carbonaceous mesophase fibers, liquid crystal polymer fibers, and thermoplastic/liquid crystal polymer in-situ composites. Fundamental surface science and engineering principles are needed to optimize and design fibers and composites derived from liquid crystalline precursors. Currently non-equilibrium liquid crystal surface phenomena are not well understood. Force balance equations describing static and dynamical interfacial phenomena are available but have not been adequately used to describe the mechanics of fiber and film microstructures.
This thesis explores the mechanics and stability of nematic liquid crystalline fibers embedded in inviscid and viscous matrices. A new theoretical framework for liquid crystal surface mechanics is formulated and used to model pattern formation and instability driven processes in fibers and fibrillar composites and blends. The liquid crystal Herring's formula and Laplace equation are derived and the role of liquid crystallinity is elucidated. In order to systematically analyze the role of the fundamental processes, linear stability analyses of capillary instabilities in nematic liquid crystalline fibers are performed by formulating and solving the governing nemato-capillary equations. An essential characteristic of liquid crystals, in contrast to isotropic liquids, is their mechanical anisotropy. Thus, the main parameters affecting the capillary instabilities are the isotropic and anisotropic surface tensions, the anisotropic viscosities, the bulk orientational elasticity, the isotropic viscosity of the matrix, and the surface bending modulus. Two asymptotic regimes are investigated: (a) the thin-fiber regime characterized by homogeneous bulk orientation and storage of surface elasticity, and (b) the thick-fiber regime characterized by bulk orientation distortions without surface elastic storage. Novel capillary instability mechanisms and symmetries of the instability modes for a nematic fiber embedded in a matrix are characterized. The predicted ability of capillary instabilities in nematic fibers to produce surface structures of well-defined symmetry and length scales, as well as chiral microstructures, is an important result that augments the pathways for targeted pattern formation. Deviations from classical Rayleigh capillary instabilities are identified and quantified in terms of liquid crystalline order.
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Books on the topic "Chemical Thermodynamics"

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Rankin, W. John. Chemical Thermodynamics. First edition. | Boca Raton, FL : CRC Press/Taylor & Francis Group, 2019.: CRC Press, 2019. http://dx.doi.org/10.1201/9780429277252.

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Keszei, Ernö. Chemical Thermodynamics. Berlin, Heidelberg: Springer Berlin Heidelberg, 2012. http://dx.doi.org/10.1007/978-3-642-19864-9.

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Chemical thermodynamics. New York: McGraw-Hill, 1990.

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M, Letcher T., ed. Chemical thermodynamics. Malden, Ma: Blackwell Science, 1999.

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Awode, Mahendra R. Chemical thermodynamics. Nagpur: Dattsons, 2002.

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Reid, Charles E. Chemical thermodynamics. Maidenhead: McGraw-Hill, 1990.

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Daubert, T. E. Chemical engineering thermodynamics. New York: McGraw-Hill, 1985.

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Chemical and process thermodynamics. 2nd ed. Englewood Cliffs, N.J: Prentice Hall, 1992.

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Kyle, B. G. Chemical and process thermodynamics. 3rd ed. Upper Saddle River, N.J: Prentice Hall PTR, 1999.

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Warn, J. R. W. (John Richard William), 1935-, ed. Concise chemical thermodynamics. 3rd ed. Boca Raton: Taylor & Francis, 2010.

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Book chapters on the topic "Chemical Thermodynamics"

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Astarita, Gianni. "Chemical Equilibria." In Thermodynamics, 269–89. Boston, MA: Springer US, 1989. http://dx.doi.org/10.1007/978-1-4899-0771-4_11.

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Yates, Paul C. "Thermodynamics." In Chemical Calculations, 57–121. 3rd ed. New York: CRC Press, 2023. http://dx.doi.org/10.1201/9781003043218-3.

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Norman, Richard, and James M. Coxon. "Chemical thermodynamics." In Principles of Organic Synthesis, 5–19. Dordrecht: Springer Netherlands, 1993. http://dx.doi.org/10.1007/978-94-011-2166-8_1.

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Evans, James W., and Lutgard C. De Jonghe. "Chemical Thermodynamics." In The Production and Processing of Inorganic Materials, 29–73. Cham: Springer International Publishing, 2016. http://dx.doi.org/10.1007/978-3-319-48163-0_2.

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Shaw, D. J., and H. E. Avery. "Chemical Thermodynamics." In Work Out Physical Chemistry, 13–66. London: Macmillan Education UK, 1989. http://dx.doi.org/10.1007/978-1-349-10006-4_2.

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Dehli, Martin, Ernst Doering, and Herbert Schedwill. "Chemical Thermodynamics." In Fundamentals of Technical Thermodynamics, 497–554. Wiesbaden: Springer Fachmedien Wiesbaden, 2022. http://dx.doi.org/10.1007/978-3-658-38910-9_12.

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Liberman, Michael A. "Chemical Thermodynamics." In Introduction to Physics and Chemistry of Combustion, 27–51. Berlin, Heidelberg: Springer Berlin Heidelberg, 2008. http://dx.doi.org/10.1007/978-3-540-78759-4_2.

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Kondepudi, Dilip. "Chemical Thermodynamics." In Encyclopedia of Sciences and Religions, 344–52. Dordrecht: Springer Netherlands, 2013. http://dx.doi.org/10.1007/978-1-4020-8265-8_1126.

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Guénault, Tony. "Chemical thermodynamics." In Statistical Physics, 137–52. Dordrecht: Springer Netherlands, 1995. http://dx.doi.org/10.1007/978-1-4020-5975-9_13.

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Nandagopal, Nuggenhalli S. "Chemical Thermodynamics." In Chemical Engineering Principles and Applications, 81–174. Cham: Springer International Publishing, 2023. http://dx.doi.org/10.1007/978-3-031-27879-2_2.

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Conference papers on the topic "Chemical Thermodynamics"

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Sabadash, Vira, and Jaroslaw Gumnitsky. "Thermodynamics of ortophosphoric acid adsorption under static conditions." In Chemical technology and engineering. Lviv Polytechnic National University, 2019. http://dx.doi.org/10.23939/cte2019.01.167.

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Sahu, Jyoti, and Vinay A. Juvekar. "Thermodynamics of Concentrated Electrolytes: Need for Modification of Debye-Hückel Theory." In Annual International Conference on Chemistry, Chemical Engineering and Chemical Process. Global Science & Technology Forum (GSTF), 2015. http://dx.doi.org/10.5176/2301-3761_ccecp15.22.

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Rebhan, Anton, Andreas Gerhold, and Andreas Ipp. "Thermodynamics of QCD at large quark chemical potential." In 29th Johns Hopkins Workshop on current problems in particle theory: strong matter in the heavens. Trieste, Italy: Sissa Medialab, 2006. http://dx.doi.org/10.22323/1.022.0013.

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Pourmovahed, A., C. M. Jeruzal, and S. M. A. Nekooei. "Teaching Applied Thermodynamics With EES." In ASME 2002 International Mechanical Engineering Congress and Exposition. ASMEDC, 2002. http://dx.doi.org/10.1115/imece2002-33161.

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Applied Thermodynamics is a graduate course at Kettering University. Undergraduate Thermodynamics serves as the only prerequisite. This course covers the concepts introduced in undergraduate thermodynamics and continues with the coverage of thermodynamic relations, mixtures and solutions, psychrometry, phase and chemical equilibrium, and chemical reactions. These concepts are then applied in detail to various power and refrigeration cycles. Topics such as mole fraction, mass fraction, enthalpy of formation, adiabatic flame temperature and the application of the Second Law to reacting mixtures are covered. Team projects are incorporated into this graduate course. Recent projects included a turbojet engine and a non-ideal regenerative steam power plant. The objective of the first project was to compute component efficiencies and the thrust force for a jet engine. The second project aimed to optimize the thermal efficiency of a non-ideal regenerative steam power plant by varying the feed-water heater pressure. Both projects utilized the Engineering Equation Solver (EES), a general equation solver with built-in functions for thermodynamic and transport properties. This article describes the projects and presents the solution techniques and the computed results. For the jet engine, computed results are based on actual test data obtained in Energy Systems Laboratory at Kettering University.
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Diawati, Chansyanah. "Students’ conceptions and problem-solving ability on topic chemical thermodynamics." In PROCEEDINGS OF INTERNATIONAL SEMINAR ON MATHEMATICS, SCIENCE, AND COMPUTER SCIENCE EDUCATION (MSCEIS 2015). AIP Publishing LLC, 2016. http://dx.doi.org/10.1063/1.4941152.

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IPP, ANDREAS. "THERMODYNAMICS OF DECONFINED QCD AT SMALL AND LARGE CHEMICAL POTENTIAL." In Proceedings of the SEWM2004 Meeting. WORLD SCIENTIFIC, 2005. http://dx.doi.org/10.1142/9789812702159_0034.

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HAQUE, Najmul. "NNLO HTL QCD thermodynamics at finite temperature and chemical potential." In 7th International Conference on Physics and Astrophysics of Quark Gluon Plasma. Trieste, Italy: Sissa Medialab, 2017. http://dx.doi.org/10.22323/1.242.0057.

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Blekhman, David. "A Fuel Cell Project for Advanced Thermodynamics Courses." In ASME 2006 International Mechanical Engineering Congress and Exposition. ASMEDC, 2006. http://dx.doi.org/10.1115/imece2006-14666.

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Secondary thermodynamics courses study advanced energy cycles. They have also started to include some introduction to fuel cell operation. Seemingly difficult, the fuel cell concepts can naturally be drawn from the topics of chemical equilibrium, which are also introduced in these courses for chemical reactions and combustion. The Nernst equation, a cornerstone of fuel cell operation, is based on a change of the Gibbs energy in a non-equilibrium fuel cell reaction. The resulting terms in the Nernst equation include the concentrations of the reactants, which dynamically change as the fuel and oxidizer deplete in the reaction while flowing through the cell. This becomes particularly interesting in high temperature fuel cells that incorporate fuel reforming and fuel utilization into a single system. The introduced fuel cell project proposes to combine the chemical equilibrium and non-equilibrium concepts simultaneously coexisting in a high temperature fuel cell. Relatively low operational temperatures allow for a simplified chemical equilibrium analysis of the fuel flowing in the fuel cell while superimposing it on the fuel cell reaction and fuel/oxidizer utilization. The variety of fuel and oxidizer mixtures, operating temperatures and pressures allows for creating a large number of individualized assignments. Students will benefit from a project that reinforces their understanding of fuel cell performance while increasing their comfort with chemical equilibrium concepts.
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Burabayeva, N. M., V. N. Volodin, S. A. Trebukhov, A. V. Nitsenko, and K. A. Linnik. "Thermodynamics of Formation and Evaporation of Aluminum and Aluminum Telluride Melts." In The 8th World Congress on Mechanical, Chemical, and Material Engineering. Avestia Publishing, 2022. http://dx.doi.org/10.11159/mmme22.129.

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Levy, Yeshayahou, Arvind Rao, and Valery Sherbaum. "Chemical Kinetic and Thermodynamics of Flameless Combustion Methodology for Gas Turbine Combustors." In 43rd AIAA/ASME/SAE/ASEE Joint Propulsion Conference & Exhibit. Reston, Virigina: American Institute of Aeronautics and Astronautics, 2007. http://dx.doi.org/10.2514/6.2007-5629.

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Reports on the topic "Chemical Thermodynamics"

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Jonas, Otakar, and Howard J. White. Chemical thermodynamics in steam power cycles data requirements :. Gaithersburg, MD: National Bureau of Standards, 1985. http://dx.doi.org/10.6028/nbs.ir.85-3205.

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Dubrovin, Viktor Vasilievich. Chemical processes within the framework of non-equilibrium thermodynamics Dubrovin Viktor Vasilievich. DOI СODE, 2023. http://dx.doi.org/10.18411/doicode-2023.163.

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Terah, E. I. Practical classes in general chemistry for students of specialties «General Medicine», «Pediatrics», «Dentistry». SIB-Expertise, April 2022. http://dx.doi.org/10.12731/er0556.13042022.

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Videos of 11 practical lessons on general chemistry are presented. The following topics are considered – chemical thermodynamics and kinetics, chemical equilibrium, methods of expressing the concentration of solutions, electrolyte solutions, pH, buffer solutions, hydrolysis, redox pro-cesses. For each topic, the main theoretical provisions are given, as well as a detailed solution of typical calculation problems is given. The total dura-tion of the video lessons is 8 hours 21 minutes.
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C.F. Jovecolon. Technical Work Plan for: Thermodynamic Database for Chemical Modeling. US: Yucca Mountain Project, Las Vegas, Nevada, September 2006. http://dx.doi.org/10.2172/895366.

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Bruno, Thomas J., Marcia Huber, Arno Laesecke, Eric Lemmon, Mark McLinden, Stephanie L. Outcalt, Richard Perkins, Beverly L. Smith, and Jason A. Widegren. Thermodynamic, transport, and chemical properties of reference JP-8. Gaithersburg, MD: National Institute of Standards and Technology, 2010. http://dx.doi.org/10.6028/nist.ir.6659.

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Spencer, A. L. Modeling of thermodynamic and chemical changes in low-temperature geothermal systems. Office of Scientific and Technical Information (OSTI), December 1986. http://dx.doi.org/10.2172/6755538.

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Satterwhite, Elizabeth. Ribozyme/Duplex Binding Interactions as a Thermodynamic Basis for Chemical Game Theory. Portland State University Library, January 2016. http://dx.doi.org/10.15760/honors.311.

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Bruffey, Stephanie, and Randy Ngelale. CHEMICAL THERMODYNAMIC MODELING OF MOLTEN SALTS TO SUPPORT OFF-GAS ABATEMENT SYSTEMS. Office of Scientific and Technical Information (OSTI), July 2022. http://dx.doi.org/10.2172/1877494.

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Besmann, T. M., and R. H. Jr Cooper. Chemical thermodynamic assessment of the Li-U-O system for possible space nuclear applications. Office of Scientific and Technical Information (OSTI), June 1985. http://dx.doi.org/10.2172/5698847.

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Ahmadi, G., and J. Cao. A thermodynamical formulation for chemically active multi-phase turbulent flows. Office of Scientific and Technical Information (OSTI), March 1995. http://dx.doi.org/10.2172/78803.

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