Elementary physical chemistry /:
This book is designed for a one-semester course, for undergraduates, not necessarily chemistry majors, who need to know something about physical chemistry. The emphasis is not on mathematical rigor, but subtleties and conceptual difficulties are not hidden. It covers the essential topics in physical...
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| Format: | Elektronisch E-Book |
| Sprache: | English |
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Singapore ; Hackensack, NJ :
World Scientific,
©2011.
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| Online-Zugang: | Volltext |
| Zusammenfassung: | This book is designed for a one-semester course, for undergraduates, not necessarily chemistry majors, who need to know something about physical chemistry. The emphasis is not on mathematical rigor, but subtleties and conceptual difficulties are not hidden. It covers the essential topics in physical chemistry, including the state of matter, thermodynamics, chemical kinetics, phase and chemical equilibria, introduction to quantum theory, and molecular spectroscopy. |
| Beschreibung: | 1 online resource (xiii, 143 pages) : illustrations |
| ISBN: | 9789814299688 9814299685 |
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| 505 | 0 | |a 1. State of matter. Properties of gases. 1.1. State of matter. 1.2. Description of some states of matter. 1.3. Units. 1.4. Ideal or perfect gas law. 1.5. Evaluation of the gas constant, R. 1.6. Mixtures of gases. 1.7. The kinetic theory of gases. 1.8. Molecular collisions. 1.9. Diffusion of gases. Graham's Law. 1.10. Molecular Basis of Graham's Law. 1.11. Real gases -- 2. The first law of thermodynamics. 2.1. Classification. 2.2. System and surrounding. 2.3. Work and heat. 2.4. Measurement of work. 2.5. Reversible process. 2.6. Measurement of heat. 2.7. Internal energy. 2.8. Exact and inexact differentials. 2.9. Relation of [symbol]U to qv (q at constant volume). 2.10. Heat capacity. 2.11. Enthalpy changes in chemical reactions. 2.12. Standard enthalpy. 2.13. Variation of enthalpy with temperature -- 3. The second law of thermodynamics. 3.1. Statements of the second law. 3.2. Carnot cycle. 3.3. Engine efficiency. 3.4. Determination of entropy -- 4. The third law of thermodynamics. 4.1. Standard entropy. 4.2. Molecular interpretation of entropy. 4.3. The surroundings. 4.4. The entropy of the surroundings -- 5. The free energy functions. 5.1. The Gibbs free energy. 5.2. Free energy changes in chemical reactions. 5.3. Variation of G with T and P. 5.4. Generalization of the free energy activity. 5.5. Partial molar, molal quantities. 5.6. The chemical potential. 5.7. Relation of [symbol] to the equilibrium constant, K. 5.8. Variation of K with T -- 6. Phase and chemical equilibria. 6.1. Phase equilibrium. 6.2. Chemical equilibrium. Mixtures -- 7. Chemical kinetics. 7.1. The rates of reactions. 7.2. Order of reaction. 7.3. Units of the reaction rate constant, k. 7.4. Determination of the rate law. 7.5. Integrated rate law. 7.6. Half-lives. 7.7. Other reaction orders. 7.8. Concentration of products. 7.9. Temperature-dependent reaction rates. The Arrhenius Equation. 7.10. Reaction rate theories. 7.11. Rate law mechanisms. 7.12. The steady state approximation. 7.13. The rate-determining step (or equilibrium) approximation. 7.14. Unimolecular reactions. 7.15. Chain reactions. | |
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| contents | 1. State of matter. Properties of gases. 1.1. State of matter. 1.2. Description of some states of matter. 1.3. Units. 1.4. Ideal or perfect gas law. 1.5. Evaluation of the gas constant, R. 1.6. Mixtures of gases. 1.7. The kinetic theory of gases. 1.8. Molecular collisions. 1.9. Diffusion of gases. Graham's Law. 1.10. Molecular Basis of Graham's Law. 1.11. Real gases -- 2. The first law of thermodynamics. 2.1. Classification. 2.2. System and surrounding. 2.3. Work and heat. 2.4. Measurement of work. 2.5. Reversible process. 2.6. Measurement of heat. 2.7. Internal energy. 2.8. Exact and inexact differentials. 2.9. Relation of [symbol]U to qv (q at constant volume). 2.10. Heat capacity. 2.11. Enthalpy changes in chemical reactions. 2.12. Standard enthalpy. 2.13. Variation of enthalpy with temperature -- 3. The second law of thermodynamics. 3.1. Statements of the second law. 3.2. Carnot cycle. 3.3. Engine efficiency. 3.4. Determination of entropy -- 4. The third law of thermodynamics. 4.1. Standard entropy. 4.2. Molecular interpretation of entropy. 4.3. The surroundings. 4.4. The entropy of the surroundings -- 5. The free energy functions. 5.1. The Gibbs free energy. 5.2. Free energy changes in chemical reactions. 5.3. Variation of G with T and P. 5.4. Generalization of the free energy activity. 5.5. Partial molar, molal quantities. 5.6. The chemical potential. 5.7. Relation of [symbol] to the equilibrium constant, K. 5.8. Variation of K with T -- 6. Phase and chemical equilibria. 6.1. Phase equilibrium. 6.2. Chemical equilibrium. Mixtures -- 7. Chemical kinetics. 7.1. The rates of reactions. 7.2. Order of reaction. 7.3. Units of the reaction rate constant, k. 7.4. Determination of the rate law. 7.5. Integrated rate law. 7.6. Half-lives. 7.7. Other reaction orders. 7.8. Concentration of products. 7.9. Temperature-dependent reaction rates. The Arrhenius Equation. 7.10. Reaction rate theories. 7.11. Rate law mechanisms. 7.12. The steady state approximation. 7.13. The rate-determining step (or equilibrium) approximation. 7.14. Unimolecular reactions. 7.15. Chain reactions. |
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| discipline | Chemie / Pharmazie |
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| id | ZDB-4-EBA-ocn742233554 |
| illustrated | Illustrated |
| indexdate | 2024-11-27T13:17:55Z |
| institution | BVB |
| isbn | 9789814299688 9814299685 |
| language | English |
| oclc_num | 742233554 |
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| spelling | Linder, Bruno. http://id.loc.gov/authorities/names/n2004002568 Elementary physical chemistry / Bruno Linder. Singapore ; Hackensack, NJ : World Scientific, ©2011. 1 online resource (xiii, 143 pages) : illustrations text txt rdacontent computer c rdamedia online resource cr rdacarrier 1. State of matter. Properties of gases. 1.1. State of matter. 1.2. Description of some states of matter. 1.3. Units. 1.4. Ideal or perfect gas law. 1.5. Evaluation of the gas constant, R. 1.6. Mixtures of gases. 1.7. The kinetic theory of gases. 1.8. Molecular collisions. 1.9. Diffusion of gases. Graham's Law. 1.10. Molecular Basis of Graham's Law. 1.11. Real gases -- 2. The first law of thermodynamics. 2.1. Classification. 2.2. System and surrounding. 2.3. Work and heat. 2.4. Measurement of work. 2.5. Reversible process. 2.6. Measurement of heat. 2.7. Internal energy. 2.8. Exact and inexact differentials. 2.9. Relation of [symbol]U to qv (q at constant volume). 2.10. Heat capacity. 2.11. Enthalpy changes in chemical reactions. 2.12. Standard enthalpy. 2.13. Variation of enthalpy with temperature -- 3. The second law of thermodynamics. 3.1. Statements of the second law. 3.2. Carnot cycle. 3.3. Engine efficiency. 3.4. Determination of entropy -- 4. The third law of thermodynamics. 4.1. Standard entropy. 4.2. Molecular interpretation of entropy. 4.3. The surroundings. 4.4. The entropy of the surroundings -- 5. The free energy functions. 5.1. The Gibbs free energy. 5.2. Free energy changes in chemical reactions. 5.3. Variation of G with T and P. 5.4. Generalization of the free energy activity. 5.5. Partial molar, molal quantities. 5.6. The chemical potential. 5.7. Relation of [symbol] to the equilibrium constant, K. 5.8. Variation of K with T -- 6. Phase and chemical equilibria. 6.1. Phase equilibrium. 6.2. Chemical equilibrium. Mixtures -- 7. Chemical kinetics. 7.1. The rates of reactions. 7.2. Order of reaction. 7.3. Units of the reaction rate constant, k. 7.4. Determination of the rate law. 7.5. Integrated rate law. 7.6. Half-lives. 7.7. Other reaction orders. 7.8. Concentration of products. 7.9. Temperature-dependent reaction rates. The Arrhenius Equation. 7.10. Reaction rate theories. 7.11. Rate law mechanisms. 7.12. The steady state approximation. 7.13. The rate-determining step (or equilibrium) approximation. 7.14. Unimolecular reactions. 7.15. Chain reactions. This book is designed for a one-semester course, for undergraduates, not necessarily chemistry majors, who need to know something about physical chemistry. The emphasis is not on mathematical rigor, but subtleties and conceptual difficulties are not hidden. It covers the essential topics in physical chemistry, including the state of matter, thermodynamics, chemical kinetics, phase and chemical equilibria, introduction to quantum theory, and molecular spectroscopy. Print version record. Chemistry, Physical and theoretical. http://id.loc.gov/authorities/subjects/sh85023027 Chimie physique et théorique. physical chemistry. aat SCIENCE Chemistry Physical & Theoretical. bisacsh Chemistry, Physical and theoretical fast has work: Elementary physical chemistry (Text) https://id.oclc.org/worldcat/entity/E39PCH7MbhhVpbkB9pdXDPprjd https://id.oclc.org/worldcat/ontology/hasWork Print version: Linder, Bruno. Elementary physical chemistry. Singapore ; London : World Scientific, ©2011 9789814299664 (OCoLC)495780597 FWS01 ZDB-4-EBA FWS_PDA_EBA https://search.ebscohost.com/login.aspx?direct=true&scope=site&db=nlebk&AN=374788 Volltext |
| spellingShingle | Linder, Bruno Elementary physical chemistry / 1. State of matter. Properties of gases. 1.1. State of matter. 1.2. Description of some states of matter. 1.3. Units. 1.4. Ideal or perfect gas law. 1.5. Evaluation of the gas constant, R. 1.6. Mixtures of gases. 1.7. The kinetic theory of gases. 1.8. Molecular collisions. 1.9. Diffusion of gases. Graham's Law. 1.10. Molecular Basis of Graham's Law. 1.11. Real gases -- 2. The first law of thermodynamics. 2.1. Classification. 2.2. System and surrounding. 2.3. Work and heat. 2.4. Measurement of work. 2.5. Reversible process. 2.6. Measurement of heat. 2.7. Internal energy. 2.8. Exact and inexact differentials. 2.9. Relation of [symbol]U to qv (q at constant volume). 2.10. Heat capacity. 2.11. Enthalpy changes in chemical reactions. 2.12. Standard enthalpy. 2.13. Variation of enthalpy with temperature -- 3. The second law of thermodynamics. 3.1. Statements of the second law. 3.2. Carnot cycle. 3.3. Engine efficiency. 3.4. Determination of entropy -- 4. The third law of thermodynamics. 4.1. Standard entropy. 4.2. Molecular interpretation of entropy. 4.3. The surroundings. 4.4. The entropy of the surroundings -- 5. The free energy functions. 5.1. The Gibbs free energy. 5.2. Free energy changes in chemical reactions. 5.3. Variation of G with T and P. 5.4. Generalization of the free energy activity. 5.5. Partial molar, molal quantities. 5.6. The chemical potential. 5.7. Relation of [symbol] to the equilibrium constant, K. 5.8. Variation of K with T -- 6. Phase and chemical equilibria. 6.1. Phase equilibrium. 6.2. Chemical equilibrium. Mixtures -- 7. Chemical kinetics. 7.1. The rates of reactions. 7.2. Order of reaction. 7.3. Units of the reaction rate constant, k. 7.4. Determination of the rate law. 7.5. Integrated rate law. 7.6. Half-lives. 7.7. Other reaction orders. 7.8. Concentration of products. 7.9. Temperature-dependent reaction rates. The Arrhenius Equation. 7.10. Reaction rate theories. 7.11. Rate law mechanisms. 7.12. The steady state approximation. 7.13. The rate-determining step (or equilibrium) approximation. 7.14. Unimolecular reactions. 7.15. Chain reactions. Chemistry, Physical and theoretical. http://id.loc.gov/authorities/subjects/sh85023027 Chimie physique et théorique. physical chemistry. aat SCIENCE Chemistry Physical & Theoretical. bisacsh Chemistry, Physical and theoretical fast |
| subject_GND | http://id.loc.gov/authorities/subjects/sh85023027 |
| title | Elementary physical chemistry / |
| title_auth | Elementary physical chemistry / |
| title_exact_search | Elementary physical chemistry / |
| title_full | Elementary physical chemistry / Bruno Linder. |
| title_fullStr | Elementary physical chemistry / Bruno Linder. |
| title_full_unstemmed | Elementary physical chemistry / Bruno Linder. |
| title_short | Elementary physical chemistry / |
| title_sort | elementary physical chemistry |
| topic | Chemistry, Physical and theoretical. http://id.loc.gov/authorities/subjects/sh85023027 Chimie physique et théorique. physical chemistry. aat SCIENCE Chemistry Physical & Theoretical. bisacsh Chemistry, Physical and theoretical fast |
| topic_facet | Chemistry, Physical and theoretical. Chimie physique et théorique. physical chemistry. SCIENCE Chemistry Physical & Theoretical. Chemistry, Physical and theoretical |
| url | https://search.ebscohost.com/login.aspx?direct=true&scope=site&db=nlebk&AN=374788 |
| work_keys_str_mv | AT linderbruno elementaryphysicalchemistry |