LEADER 01331nas 2200469 a 450 001 996210884703316 005 20240413021243.0 011 $a2057-763X 035 $a(OCoLC)47189955 035 $a(CKB)954928562479 035 $a(CONSER) 2010250621 035 $a(DE-599)ZDB1472964-7 035 $a(EXLCZ)99954928562479 100 $a20010626b19751988 sy 101 0 $aeng 135 $aurmnu||||| 181 $ctxt$2rdacontent 182 $cc$2rdamedia 183 $acr$2rdacarrier 200 10$aJournal of physics. G: Nuclear physics 210 $a[London] $cInstitute of Physics 300 $a"A Europhysics journal." 311 $a0305-4616 517 $aJournal of physics G. Nuclear physics 517 3 $aNuclear physics 517 $aFormerly 531 $aJ PHYS G 531 $aJ. PHYS. G: NUCL. PHYS 531 $aJOURNAL OF PHYSICS G 531 0 $aJ. phys. G 606 $aNuclear physics$vPeriodicals 606 $aParticles (Nuclear physics)$vPeriodicals 606 $aKernfysica$2gtt 615 0$aNuclear physics 615 0$aParticles (Nuclear physics) 615 17$aKernfysica. 676 $a539.7/05 712 02$aInstitute of Physics (Great Britain) 906 $aJOURNAL 912 $a996210884703316 996 $aJournal of physics. G: Nuclear physics$9794577 997 $aUNISA LEADER 05375nam 2200697Ia 450 001 9910956916603321 005 20251116192012.0 010 $a1-281-05800-9 010 $a9786611058005 010 $a0-08-050100-1 035 $a(CKB)1000000000384360 035 $a(EBL)316836 035 $a(OCoLC)476108322 035 $a(SSID)ssj0000120409 035 $a(PQKBManifestationID)11130308 035 $a(PQKBTitleCode)TC0000120409 035 $a(PQKBWorkID)10080129 035 $a(PQKB)10949865 035 $a(Au-PeEL)EBL316836 035 $a(CaPaEBR)ebr10206700 035 $a(CaONFJC)MIL105800 035 $a(OCoLC)162580304 035 $a(MiAaPQ)EBC316836 035 $a(EXLCZ)991000000000384360 100 $a20040525d2004 uy 0 101 0 $aeng 135 $aur|n|---||||| 181 $ctxt 182 $cc 183 $acr 200 10$aChemical energy and exergy $ean introduction to chemical thermodynamics for engineers /$fNorio Sato 205 $a1st ed. 210 $aSan Diego, CA ;$aAmsterdam $cElsevier$d2004 215 $a1 online resource (161 p.) 300 $aDescription based upon print version of record. 311 08$a0-444-51645-X 320 $aIncludes bibliographical references (p. [145]) and index. 327 $aFront Cover; Chemical Energy and Exergy: An Introduction to Chemical Thermodynamics for Engineers; Copyright Page; CONTENTS; PREFACE; CHAPTER 1. THERMODYNAMIC STATE VARIABLES; 1.1. Thermodynamic systems; 1.2. Variables of the state; 1.3. Extensive and intensive variables; 1.4. Partial molar quantities; 1.5. The extent of a chemical reaction; CHAPTER 2. CONSERVATION OF ENERGY; 2.1. Energy as a physical quantity of the state; 2.2. Conservation of energy; 2.3. Internal energy U with independent variables T, V, and ?; 2.4. Enthalpy H with independent variables T, p, and ? 327 $a2.5. Enthalpy and heat of reaction2.6. Enthalpy of pure substances; CHAPTER 3. ENTROPY AS A STATE PROPERTY; 3.1. Introduction to entropy; 3.2. Reversible and irreversible processes; 3.3. The creation of entropy and uncompensated heat; 3.4. The creation of entropy and thermodynamic potentials; 3.5. Affinity of irreversible processes; 3.6. Entropy of pure substances; 3.7. Entropy of heat transfer; 3.8. Entropy of gas expansion; 3.9. Entropy of mixing; CHAPTER 4. AFFINITY IN IRREVERSIBLE PROCESSES; 4.1. Affinity in chemical reactions; 4.2. Affinity and heat of reaction 327 $a4.3. The average heat of reaction4.4. The average affinity of reaction; CHAPTER 5. CHEMICAL POTENTIAL; 5.1. Thermodynamic potentials in open systems; 5.2. The partial molar quantity of energy and the chemical potential; 5.3. Chemical potentials and the affinity of reaction; 5.4. Chemical potentials and thermodynamic energy functions; 5.5. Chemical potentials in homogeneous mixtures: the Gibbs-Duhem equation; 5.6. Chemical potentials of substances in ideal mixtures; 5.7. Activity and activity coefficient; 5.8. Chemical potentials of pure substances 327 $a5.9. Thermodynamic potentials in ideal mixtures5.10. The unitary and mixing terms of thermodynamic potentials; CHAPTER 6. UNITARY AFFINITY AND EQUILIBRIUM; 6.1. Affinity and equilibrium in chemical reactions; 6.2. The unitary affinity; 6.3. Equilibrium constants and concentration units; 6.4. Equilibrium constants as a function of pressure and temperature; CHAPTER 7. GASES, LIQUIDS, AND SOLIDS; 7.1. Perfect and ideal gases; 7.2. Non-ideal gases; 7.3. Liquids and solids; 7.4. The state equation and thermodynamic functions of condensed substances; CHAPTER 8. SOLUTIONS 327 $a8.1. Ideal and non-ideal solutions8.2. Perfect solutions and ideal solutions; 8.3. Reference systems for thermodynamic unitary quantity; 8.4. Thermodynamic excess functions in non-ideal solutions; 8.5. Units of the concentration; 8.6. Osmotic pressure; 8.7. Electrolytic solutions; CHAPTER 9. ELECTROCHEMICAL ENERGY; 9.1. Electrochemical potential of charged particles; 9.2. Transfer of charged particles between two condensed phases; 9.3. Electrode and electrode potential; 9.4. Electrochemical cells; 9.5. Equilibrium electrode potential of electronic transfer reactions 327 $a9.6. Equilibrium electrode potential of ionic transfer reactions 330 $aThis book is a beginners introduction to chemical thermodynamics for engineers. In the textbook efforts have been made to visualize as clearly as possible the main concepts of thermodynamic quantities such as enthalpy and entropy, thus making them more perceivable. Furthermore, intricate formulae in thermodynamics have been discussed as functionally unified sets of formulae to understand their meaning rather than to mathematically derive them in detail.In this textbook, the affinity of irreversible processes, defined by the second law of thermodynamics, has been treated as the main 606 $aThermochemistry 606 $aIrreversible processes 606 $aExergy 615 0$aThermochemistry. 615 0$aIrreversible processes. 615 0$aExergy. 676 $a541.36902462 676 $a541/.36 22 676 $a541.36902462 700 $aSato?$b Norio$0725552 801 0$bMiAaPQ 801 1$bMiAaPQ 801 2$bMiAaPQ 906 $aBOOK 912 $a9910956916603321 996 $aChemical energy and exergy$91425586 997 $aUNINA