CHAPTER 17 Internal Pressure and Internal Energy of Saturated and Compressed Phases Ainstitute of Physics of the Dagestan Scient
Total Page:16
File Type:pdf, Size:1020Kb
Load more
Recommended publications
-
Chapter 3. Second and Third Law of Thermodynamics
Chapter 3. Second and third law of thermodynamics Important Concepts Review Entropy; Gibbs Free Energy • Entropy (S) – definitions Law of Corresponding States (ch 1 notes) • Entropy changes in reversible and Reduced pressure, temperatures, volumes irreversible processes • Entropy of mixing of ideal gases • 2nd law of thermodynamics • 3rd law of thermodynamics Math • Free energy Numerical integration by computer • Maxwell relations (Trapezoidal integration • Dependence of free energy on P, V, T https://en.wikipedia.org/wiki/Trapezoidal_rule) • Thermodynamic functions of mixtures Properties of partial differential equations • Partial molar quantities and chemical Rules for inequalities potential Major Concept Review • Adiabats vs. isotherms p1V1 p2V2 • Sign convention for work and heat w done on c=C /R vm system, q supplied to system : + p1V1 p2V2 =Cp/CV w done by system, q removed from system : c c V1T1 V2T2 - • Joule-Thomson expansion (DH=0); • State variables depend on final & initial state; not Joule-Thomson coefficient, inversion path. temperature • Reversible change occurs in series of equilibrium V states T TT V P p • Adiabatic q = 0; Isothermal DT = 0 H CP • Equations of state for enthalpy, H and internal • Formation reaction; enthalpies of energy, U reaction, Hess’s Law; other changes D rxn H iD f Hi i T D rxn H Drxn Href DrxnCpdT Tref • Calorimetry Spontaneous and Nonspontaneous Changes First Law: when one form of energy is converted to another, the total energy in universe is conserved. • Does not give any other restriction on a process • But many processes have a natural direction Examples • gas expands into a vacuum; not the reverse • can burn paper; can't unburn paper • heat never flows spontaneously from cold to hot These changes are called nonspontaneous changes. -
7 Apr 2021 Thermodynamic Response Functions . L03–1 Review Of
7 apr 2021 thermodynamic response functions . L03{1 Review of Thermodynamics. 3: Second-Order Quantities and Relationships Maxwell Relations • Idea: Each thermodynamic potential gives rise to several identities among its second derivatives, known as Maxwell relations, which express the integrability of the fundamental identity of thermodynamics for that potential, or equivalently the fact that the potential really is a thermodynamical state function. • Example: From the fundamental identity of thermodynamics written in terms of the Helmholtz free energy, dF = −S dT − p dV + :::, the fact that dF really is the differential of a state function implies that @ @F @ @F @S @p = ; or = : @V @T @T @V @V T;N @T V;N • Other Maxwell relations: From the same identity, if F = F (T; V; N) we get two more relations. Other potentials and/or pairs of variables can be used to obtain additional relations. For example, from the Gibbs free energy and the identity dG = −S dT + V dp + µ dN, we get three relations, including @ @G @ @G @S @V = ; or = − : @p @T @T @p @p T;N @T p;N • Applications: Some measurable quantities, response functions such as heat capacities and compressibilities, are second-order thermodynamical quantities (i.e., their definitions contain derivatives up to second order of thermodynamic potentials), and the Maxwell relations provide useful equations among them. Heat Capacities • Definitions: A heat capacity is a response function expressing how much a system's temperature changes when heat is transferred to it, or equivalently how much δQ is needed to obtain a given dT . The general definition is C = δQ=dT , where for any reversible transformation δQ = T dS, but the value of this quantity depends on the details of the transformation. -
Estimation of Internal Pressure of Liquids and Liquid Mixtures
Available online at www.ilcpa.pl International Letters of Chemistry, Physics and Astronomy 5 (2012) 1-7 ISSN 2299-3843 Estimation of internal pressure of liquids and liquid mixtures N. Santhi 1, P. Sabarathinam 2, G. Alamelumangai 1, J. Madhumitha 1, M. Emayavaramban 1 1Department of Chemistry, Government Arts College, C.Mutlur, Chidambaram-608102, India 2Retd. Registrar & Head of the Department of Technology, Annamalai University, Annamalainagar-608002, India E-mail address: [email protected] ABSTRACT By combining the van der Waals’ equation of state and the Free Length Theory of Jacobson, a new theoretical model is developed for the prediction of internal pressure of pure liquids and liquid mixtures. It requires only the molar volume data in addition to the ratio of heat capacities and critical temperature. The proposed model is simple, reliably accurate and capable of predicting internal pressure of pure liquids with an average absolute deviation of 4.24% in the predicted internal pressure values compared to those given in literature. The average absolute deviation in the predicted internal pressure values through the proposed model for the five binary liquid mixtures tested varies from 0.29% to 1.9% when compared to those of literature values. Keywords: van der Waals, pressure of liquids, theory of Jacobson, capacity of heat liquids, equation of Srivastava and Berkowitz 1. INTRODUTION The importance of internal pressure in understanding the properties of liquids and the full potential of internal pressure as a structural probe did become apparent with the pioneering work of Hildebrand 1, 2 and the first review of the subject by Richards 3 appeared in 1925. -
High Temperature and High Pressure Equation of State of Gold
Journal of Physics: Conference Series OPEN ACCESS Related content - The equation of state of B2-type NaCl High temperature and high pressure equation of S Ono - Thermodynamics in high-temperature state of gold pressure scales on example of MgO Peter I Dorogokupets To cite this article: Masanori Matsui 2010 J. Phys.: Conf. Ser. 215 012197 - Equation of State of Tantalum up to 133 GPa Tang Ling-Yun, Liu Lei, Liu Jing et al. View the article online for updates and enhancements. Recent citations - Equation of State for Natural Almandine, Spessartine, Pyrope Garnet: Implications for Quartz-In-Garnet Elastic Geobarometry Suzanne R. Mulligan et al - High-Pressure Equation of State of 1,3,5- triamino-2,4,6-trinitrobenzene: Insights into the Monoclinic Phase Transition, Hydrogen Bonding, and Anharmonicity Brad A. Steele et al - High-enthalpy crystalline phases of cadmium telluride Adebayo O. Adeniyi et al This content was downloaded from IP address 170.106.202.8 on 25/09/2021 at 03:55 Joint AIRAPT-22 & HPCJ-50 IOP Publishing Journal of Physics: Conference Series 215 (2010) 012197 doi:10.1088/1742-6596/215/1/012197 High temperature and high pressure equation of state of gold Masanori Matsui School of Science, University of Hyogo, Kouto, Kamigori, Hyogo 678–1297, Japan E-mail: [email protected] Abstract. High-temperature and high-pressure equation of state (EOS) of Au has been developed using measured data from shock compression up to 240 GPa, volume thermal expansion between 100 and 1300 K and 0 GPa, and temperature dependence of bulk modulus at 0 GPa from ultrasonic measurements. -
Calculation of Thermal Pressure Coefficient of Lithium Fluid by Data
International Scholarly Research Network ISRN Physical Chemistry Volume 2012, Article ID 724230, 11 pages doi:10.5402/2012/724230 Research Article Calculation of Thermal Pressure Coefficient of Lithium Fluid by pVT Data Vahid Moeini Department of Chemistry, Payame Noor University, P.O. Box 19395-3697, Tehran, Iran Correspondence should be addressed to Vahid Moeini, v [email protected] Received 20 September 2012; Accepted 9 October 2012 Academic Editors: F. M. Cabrerizo, H. Reis, and E. B. Starikov Copyright © 2012 Vahid Moeini. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited. For thermodynamic performance to be optimized, particular attention must be paid to the fluid’s thermal pressure coefficients and thermodynamics properties. A new analytical expression based on the statistical mechanics is derived for thermal pressure coefficients of dense fluids using the intermolecular forces theory to be valid for liquid lithium as well. The results are used to predict the parameters of some binary mixtures at different compositions and temperatures metal-nonmetal lithium fluid which agreement with experimental data. In this paper, we have used newly presented parameters of analytical expressions based on the statistical mechanics and predicted the metal-nonmetal transition for liquid lithium. The repulsion term of the effective pair potential for lithium shows well depth at 1600 K, and the position of well depth maximum is in agreement with X-ray diffraction and small-angle X-ray scattering. 1. Introduction would be observed if each pair was isolated. -
The Carnot Cycle, Reversibility and Entropy
entropy Article The Carnot Cycle, Reversibility and Entropy David Sands Department of Physics and Mathematics, University of Hull, Hull HU6 7RX, UK; [email protected] Abstract: The Carnot cycle and the attendant notions of reversibility and entropy are examined. It is shown how the modern view of these concepts still corresponds to the ideas Clausius laid down in the nineteenth century. As such, they reflect the outmoded idea, current at the time, that heat is motion. It is shown how this view of heat led Clausius to develop the entropy of a body based on the work that could be performed in a reversible process rather than the work that is actually performed in an irreversible process. In consequence, Clausius built into entropy a conflict with energy conservation, which is concerned with actual changes in energy. In this paper, reversibility and irreversibility are investigated by means of a macroscopic formulation of internal mechanisms of damping based on rate equations for the distribution of energy within a gas. It is shown that work processes involving a step change in external pressure, however small, are intrinsically irreversible. However, under idealised conditions of zero damping the gas inside a piston expands and traces out a trajectory through the space of equilibrium states. Therefore, the entropy change due to heat flow from the reservoir matches the entropy change of the equilibrium states. This trajectory can be traced out in reverse as the piston reverses direction, but if the external conditions are adjusted appropriately, the gas can be made to trace out a Carnot cycle in P-V space. -
Pressure—Volume—Temperature Equation of State
Pressure—Volume—Temperature Equation of State S.-H. Dan Shim (심상헌) Acknowledgement: NSF-CSEDI, NSF-FESD, NSF-EAR, NASA-NExSS, Keck Equations relating state variables (pressure, temperature, volume, or energy). • Backgrounds • Equations • Limitations • Applications Ideal Gas Law PV = nRT Ideal Gas Law • Volume increases with temperature • VolumePV decreases= nRTwith pressure • Pressure increases with temperature Stress (σ) and Strain (�) Bridgmanite in the Mantle Strain in the Mantle 20-30% P—V—T EOS Bridgmanite Energy A Few Terms to Remember • Isothermal • Isobaric • Isochoric • Isentropic • Adiabatic Energy Thermodynamic Parameters Isothermal bulk modulus Thermodynamic Parameters Isothermal bulk modulus Thermal expansion parameter Thermodynamic Parameters Isothermal bulk modulus Thermal expansion parameter Grüneisen parameter ∂P 1 ∂P γ = V = ∂U ρC ∂T ✓ ◆V V ✓ ◆V P—V—T of EOS Bridgmanite • KT • α • γ P—V—T EOS Shape of EOS Shape of EOS Ptotal Shape of EOS Pst Pth Thermal Pressure Ftot = Fst + Fb + Feec P(V, T)=Pst(V, T0)+ΔPth(V, T) Isothermal EOS dP dP K = = − d ln V d ln ρ P V = V0 exp − K 0 Assumes that K does not change with P, T Murnaghan EOS K = K0 + K00 P dP dP K = = − d ln V d ln ρ K00 ρ = ρ0 1 + P Ç K0 å However, K increases nonlinearly with pressure Birch-Murnaghan EOS 2 3 F = + bƒ + cƒ + dƒ + ... V 0 3/2 =(1 + 2ƒ ) V F : Energy (U or F) f : Eulerian finite strain Birch (1978) Second Order BM EOS 2 F = + bƒ + cƒ 3K V 7/3 V 5/3 5/2 0 0 0 P = 3K0ƒ (1 + 2ƒ ) = 2 V V ñ✓ ◆ − ✓ ◆ ô dP K V 7/3 V 5/3 0 0 0 5/2 K = V = 7 5 = K0(1 + 7ƒ )(1 + 2ƒ ) dV 2 V V − ñ ✓ ◆ − ✓ ◆ ô Birch (1978) Third Order BM EOS 2 3 F = + bƒ + cƒ + dƒ 7/3 5/3 2/3 3K0 V0 V0 V0 P = 1 ξ 1 2 V V V ñ✓ ◆ − ✓ ◆ ô® − ñ✓ ◆ − ô´ 3 ξ = (4 K00 ) 4 − Birch (1978) Truncation Problem 2 3 F = + bƒ + cƒ + dƒ + .. -
High Pressure and Temperature Dependence of Thermodynamic Properties of Model Food Solutions Obtained from in Situ Ultrasonic Measurements
HIGH PRESSURE AND TEMPERATURE DEPENDENCE OF THERMODYNAMIC PROPERTIES OF MODEL FOOD SOLUTIONS OBTAINED FROM IN SITU ULTRASONIC MEASUREMENTS By ROGER DARROS BARBOSA A DISSERTATION PRESENTED TO THE GRADUATE SCHOOL OF THE UNIVERSITY OF FLORIDA IN PARTIAL FULFILLMENT OF THE REQUIREMENTS FOR THE DEGREE OF DOCTOR OF PHILOSOPHY UNIVERSITY OF FLORIDA 2003 Copyright 2003 by Roger Darros Barbosa To Neila who made me feel reborn, and To my dearly loved children Marina, Carolina and especially Artur, the youngest, with whom enjoyable times were shared through this journey ACKNOWLEDGMENTS I would like to express my sincere gratitude to Dr. Murat Ö. Balaban and Dr. Arthur A. Teixeira for their valuable advice, help, encouragement, support and guidance throughout my graduate studies at the University of Florida. Special thanks go to Dr. Murat Ö. Balaban for giving me the opportunity to work in his lab and study the interesting subject of this research. I would also like to thank my committee members Dr. Gary Ihas, Dr. D. Julian McClements and Dr. Robert J. Braddock for their help, suggestions, and words of encouragement along this research. A special thank goes to Dr. D. Julian McClements for his valuable assistance and for receiving me in his lab at the University of Massachusetts. I am grateful to the Foundation for Support of Research of the State of São Paulo (FAPESP 97/07546-4) for financially supporting most part of this project. I also gratefully acknowledge the Institute of Food and Agricultural Sciences (IFAS) Research Dean, the chair of the Food Science and Human Nutrition Department, the chair of Department of Agricultural and Biological Engineering at the University of Florida, and the United States Department of Agriculture (through a research grant), for financially supporting parts of this research. -
Pressure Vessels
PRESSURE VESSELS David Roylance Department of Materials Science and Engineering Massachusetts Institute of Technology Cambridge, MA 02139 August 23, 2001 Introduction A good deal of the Mechanics of Materials can be introduced entirely within the confines of uniaxially stressed structural elements, and this was the goal of the previous modules. But of course the real world is three-dimensional, and we need to extend these concepts accordingly. We now take the next step, and consider those structures in which the loading is still simple, but where the stresses and strains now require a second dimension for their description. Both for their value in demonstrating two-dimensional effects and also for their practical use in mechanical design, we turn to a slightly more complicated structural type: the thin-walled pressure vessel. Structures such as pipes or bottles capable of holding internal pressure have been very important in the history of science and technology. Although the ancient Romans had developed municipal engineering to a high order in many ways, the very need for their impressive system of large aqueducts for carrying water was due to their not yet having pipes that could maintain internal pressure. Water can flow uphill when driven by the hydraulic pressure of the reservoir at a higher elevation, but without a pressure-containing pipe an aqueduct must be constructed so the water can run downhill all the way from the reservoir to the destination. Airplane cabins are another familiar example of pressure-containing structures. They illus- trate very dramatically the importance of proper design, since the atmosphere in the cabin has enough energy associated with its relative pressurization compared to the thin air outside that catastrophic crack growth is a real possibility. -
Ideal Gas Temperature.)
FUNDAMENTALS OF CLASSICAL AND STATISTICAL THERMODYNAMICS SPRING 2005 1 1. Basic Concepts of Thermodynamics The basic concepts of thermodynamics such as system, energy, property, state, process, cycle, pressure, and temperature are explained. Thermodynamics can be defined as the science of energy. Energy can be viewed as the ability to cause changes. Thermodynamics is concerned with the transfer of heat and the appearance or disappearance of work attending various chemical and physical processes. • The natural phenomena that occur about us; • Controlled chemical reactions; • The performance of engines • Hypothetical processes such as chemical reactions that do not occur but can be imagined. HISTORY: Thermodynamics emerged as a science with the construction of the first successful atmospheric steam engines in England by Thomas Savery in 1697 and Thomas Newcomen in 1712. These engines were very slow and inefficient, but they opened the way for the development of a new science. The first and second laws of thermodynamics emerged 2 simultaneously in the 1850s primarily out of the works of William Rankine, Rudolph Clausius, and Lord Kelvin (formerly William Thomson). The term thermodynamics was first used in a publication by Lord Kelvin in 1849. The first thermodynamic textbook was written in 1859 by William Rankine, a professor at the University of Glasgow. 3 Classical vs. Statistical Thermodynamics Substances consist of large number of particles called molecules. The properties of the substance naturally depend on the behavior of these particles. For example, the pressure of a gas in a container is the result of momentum transfer between the molecules and the walls of the container. -
Lecture452 2 12.Pdf
University of Washington Department of Chemistry Chemistry 452/456 Summer Quarter 2012 Lecture 2. 6/20/12 A. Differentials and State Functions • Thermodynamics allows us to calculate energy transformations occurring in systems composed of large numbers of particles, systems so complex as to make rigorous mechanical calculations impractical. • The limitation is that thermodynamics does not allow us to calculate trajectories. We can only calculate energy changes that occur when a system passes from one equilibrium state to another. • In thermodynamics, we do not calculate the internal energy U. We calculate the change in internal energy ∆U, taken as the difference between the internal energy of the initial equilibrium state and the internal energy of the final equilibrium state: ∆=UUfinal − U initial • The internal energy U belongs to a class of functions called state functions. State function changes ∆F are only dependent on the initial state of the system, described by Pinitial, Vinitial, Tinitial, ninitial, and the final state of the system, described by Pfinal, Vfinal, Tfinal, and nfinal. State function changes do not depend upon the details of the specific path followed (i.e. the trajectory). • Quantities that are path-dependent are not state functions. • Thermodynamic state functions are functions of several state variables including P, V, T, and n. changes in the state variable n is are not considered at present. We will concentrate at first on single component/single phase systems with no loss or gain of material. Of the three remaining state variables P, V, T only two are independent because of the constraint imposed by the equation of state. -
3. the First Law of Thermodynamics and Related Definitions
09/30/08 1 3. THE FIRST LAW OF THERMODYNAMICS AND RELATED DEFINITIONS 3.1 General statement of the law Simply stated, the First Law states that the energy of the universe is constant. This is an empirical conservation principle (conservation of energy) and defines the term "energy." We will also see that "internal energy" is defined by the First Law. [As is always the case in atmospheric science, we will ignore the Einstein mass-energy equivalence relation.] Thus, the First Law states the following: 1. Heat is a form of energy. 2. Energy is conserved. The ways in which energy is transformed is of interest to us. The First Law is the second fundamental principle in (atmospheric) thermodynamics, and is used extensively. (The first was the equation of state.) One form of the First Law defines the relationship among work, internal energy, and heat input. In this chapter (and in subsequent chapters), we will explore many applications derived from the First Law and Equation of State. 3.2 Work of expansion If a system (parcel) is not in mechanical (pressure) equilibrium with its surroundings, it will expand or contract. Consider the example of a piston/cylinder system, in which the cylinder is filled with a gas. The cylinder undergoes an expansion or compression as shown below. Also shown in Fig. 3.1 is a p-V thermodynamic diagram, in which the physical state of the gas is represented by two thermodynamic variables: p,V in this case. [We will consider this and other types of thermodynamic diagrams in more detail later.