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Physical chemistry for engineering and applied sciences /
THINGS YOU SHOULD KNOW BUT PROBABLY FORGOT Basic Definitions SI Units Dalton's Atomic Theory Stoichiometry Equivalent Weight Amount of Substance: the Mole Avogadro's HypothesisConservation of Mass Conservation of ChargeAtomic Mass Scales STATES OF MATTER AND THE PROPERTIES OF GASES The Thr...
| Clasificación: | Libro Electrónico |
|---|---|
| Autor principal: | |
| Formato: | Electrónico eBook |
| Idioma: | Inglés |
| Publicado: |
Hoboken :
CRC Press,
2012.
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| Temas: | |
| Acceso en línea: | Texto completo |
MARC
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| 001 | EBOOKCENTRAL_ocn908078035 | ||
| 003 | OCoLC | ||
| 005 | 20240329122006.0 | ||
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| 008 | 150509s2012 nju ob 001 0 eng d | ||
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| 100 | 1 | |a Foulkes, F. R., |e author. | |
| 245 | 1 | 0 | |a Physical chemistry for engineering and applied sciences / |c by Frank R. Foulkes. |
| 260 | |a Hoboken : |b CRC Press, |c 2012. | ||
| 300 | |a 1 online resource (682 pages) | ||
| 336 | |a text |b txt |2 rdacontent | ||
| 337 | |a computer |b c |2 rdamedia | ||
| 338 | |a online resource |b cr |2 rdacarrier | ||
| 588 | 0 | |a Print version record. | |
| 505 | 0 | |6 880-01 |a Front Cover; Dedication & Appreciation; Contents; Preface; About The Author; Nomenclature; Chapter 1 Things You Should Know But Probably Forgot; Chapter 2 States Of Matter And The Properties Of Gases; Chapter 3 The Ideal Gas; Chapter 4 The Kinetic Theory Of Gases; Chapter 5 Real Gases; Chapter 6 Thermodynamics (I); Chapter 7 Thermodynamics (Ii); Chapter 8 Thermodynamics (Iii); Chapter 9 Thermodynamics (Iv); Chapter 10 Thermodynamics (V); Chapter 11 Thermodynamics (Vi); Chapter 12 Thermodynamics (Vii); Chapter 13 Chemical Equilibrium (I); Chapter 14 Chemical Equilibrium (Ii). | |
| 505 | 8 | |a Chapter 15 Phase Equilibrium (I)Chapter 16 Phase Equilibrium (Ii); Chapter 17 Mixtures; Chapter 18 Colligative Properties; Chapter 19 Ionic Equilibrium; Chapter 20 Cid And Base Dissociation; Chapter 21 Bases And Their Salts; Chapter 22 Buffer Solutions; Chapter 23 Solubility Equilibria; Chapter 24 Oxidation- Reduction Reactions; Chapter 25 Electrochemistry; Chapter 26 Chemical Reaction Kinetics; Appendices; Appendix 1. Properties Of The Elements; Appendix 2. Thermodynamic Data For Selected Gasesand Vapors At P° = 1 Bar And 298.15 K. | |
| 505 | 8 | |a Appendix 3. Thermodynamic Data For Selected Liquidsat P° = 1 Bar And 298.15 KAppendix 4. Thermodynamic Data For Selected Solidsat P° = 1 Bar And 298.15 K; Appendix 5. Thermodynamic Data For Selectedaqueous Ions(1) At P° = 1 Bar And 298.15 K; Appendix 6. Analytical Solution Of A Cubic Equation; Appendix 7. The Newton-raphson Method; Appendix 8. Understanding Basic Integration; APPENDIX 9. UNDERSTANDING LOGARITHMS, EXPONENTIALS, AND dx x1; Appendix 10(a). Standard Reduction Potentials (v Vs. She) In Aqueoussystems At 25°c And One Atm Pressure: By Potential; Appendix 11. Answers To Exercises. | |
| 500 | |a Appendix 12. Answers To ProblemsBack Cover. | ||
| 520 | |a THINGS YOU SHOULD KNOW BUT PROBABLY FORGOT Basic Definitions SI Units Dalton's Atomic Theory Stoichiometry Equivalent Weight Amount of Substance: the Mole Avogadro's HypothesisConservation of Mass Conservation of ChargeAtomic Mass Scales STATES OF MATTER AND THE PROPERTIES OF GASES The Three States of Matter Pressure Archimedes' Principle Temperature THE IDEAL GAS The Ideal Gas Equation of State Molar Volumes Combined Gas Equation Dalton's Law of Partial Pressures Mole Fractions Partial Volumes THE KINETIC THEORY OF GASES Postulates Simplified Derivation of the Ideal Gas Law The Meaning of Pre. | ||
| 504 | |a Includes bibliographical references and index. | ||
| 590 | |a ProQuest Ebook Central |b Ebook Central Academic Complete | ||
| 650 | 0 | |a Chemistry, Physical and theoretical |v Textbooks. | |
| 650 | 7 | |a SCIENCE |x Chemistry |x Physical & Theoretical. |2 bisacsh | |
| 650 | 7 | |a Chemistry, Physical and theoretical |2 fast | |
| 655 | 7 | |a Textbooks |2 fast | |
| 758 | |i has work: |a Physical chemistry for engineering and applied sciences (Text) |1 https://id.oclc.org/worldcat/entity/E39PCFGVWFF8bdJmQH4RkhJdQq |4 https://id.oclc.org/worldcat/ontology/hasWork | ||
| 776 | 0 | 8 | |i Print version: |a Foulkes, Frank R. |t Physical Chemistry for Engineering and Applied Sciences. |d Hoboken : CRC Press, ©2012 |z 9781466518469 |
| 856 | 4 | 0 | |u https://ebookcentral.uam.elogim.com/lib/uam-ebooks/detail.action?docID=1449711 |z Texto completo |
| 880 | 0 | |6 505-01/(S |a <P><STRONG>THINGS YOU SHOULD KNOW BUT PROBABLY FORGOT <BR></STRONG>Basic Definitions <BR>SI Units <BR>Dalton's Atomic Theory <BR>Stoichiometry <BR>Equivalent Weight <BR>Amount of Substance: the Mole <BR>Avogadro's Hypothesis<BR>Conservation of Mass <BR>Conservation of Charge<BR>Atomic Mass Scales <BR><B>STATES OF MATTER AND THE PROPERTIES OF GASES <BR></B>The Three States of Matter <BR>Pressure <BR>Archimedes' Principle <BR>Temperature <BR><B>THE IDEAL GAS <BR></B>The Ideal Gas Equation of State <BR>Molar Volumes <BR>Combined Gas Equation <BR>Dalton's Law of Partial Pressures <BR>Mole Fractions <BR>Partial Volumes <BR><B>THE KINETIC THEORY OF GASES <BR></B>Postulates <BR>Simplified Derivation of the Ideal Gas Law <BR>The Meaning of Pressure <BR>The Meaning of Temperature <BR>Diffusion and Effusion <BR>The Speeds of Gas Molecules <BR>Effect of Pressure on Speed <BR>Distribution of Molecular Speeds <BR>The Maxwell-Boltzmann Distribution as an Energy Distribution <BR>Fraction of Molecules Having <I>E</I>> <EM>E'<BR></EM>Concluding Remarks <BR><B>REAL GASES <BR></B>Real Gases <BR>Isotherms for Real Gases <BR>Equations of State for Real Gases <BR>The Virial Equation <BR>The Van der Waals Equation <BR>Liquefaction of Gases <BR><B>THERMODYNAMICS (I) <BR></B>Thermodynamics <BR>Definitions Used In Thermodynamics <BR>Work <BR><I>PV</I>-Work<BR>Maximum Work Obtainable from the Isothermal Expansion of an Ideal Gas<BR>Reversible Processes <BR><B>THERMODYNAMICS (II) <BR></B>Internal Energy (<I>U</I>) and the First Law of Thermodynamics <BR>State Functions <BR>Work and Heat Are Not State Functions <BR><I>Q</I> and <I>W</I> Have Algebraic Signs <BR>Another Look At <I>PV</I>-Work <BR>Chemical Reaction in a Constant Volume System <BR>The Heat Capacity of a Single Phase System <BR><I>ΔU</I> for the Isothermal Expansion of an Ideal Gas <BR>The Internal Energy of a Monatomic Ideal Gas <BR><B>THERMODYNAMICS (III) <BR></B>Enthalpy (<I>H</I>) <BR>Constant Pressure Processes <BR>Thermochemistry <BR><I>ΔH</I> for Fusion (Melting) and Freezing <BR><I>ΔH</I> for Vaporization and Condensation <BR><I>ΔH</I> for Sublimation <BR>Ionization Enthalpies <BR>Electron Affinities <BR>Bond Enthalpies <BR><B>THERMODYNAMICS (IV) <BR></B>The Standard State for Chemical Reactions <BR>Hess's Law of Constant Heat Summation <BR>Standard Enthalpies of Formation <BR>Variation of <I>ΔH</I> with Temperature at Constant Pressure <BR><B>THERMODYNAMICS (V) <BR></B>Spontaneous Processes <BR>Entropy (<I>S</I>) <BR><I>ΔS</I> for the Isothermal Expansion of an Ideal Gas <BR><I>ΔS</I> for a Constant Pressure Heating or Cooling Process <BR><I>ΔS</I> for a Constant Volume Heating or Cooling Process <BR><I>ΔS</I> for a Reversible Phase Change <BR>Whenever a Real Process Takes Place <I>ΔS<SUB>univ</I></SUB> Increases <BR>Trouton's Rule <BR><B>THERMODYNAMICS (VI) <BR></B>Absolute Entropies and the Third Law of Thermodynamics <BR>Dealing With Phase Transitions <BR>Entropy Changes for Chemical Reactions <BR><B>THERMODYNAMICS (VII) </B><BR>Gibbs Free Energy (<I>G</I>) <BR>Gibbs Free Energy Changes, "Other" Work, and Spontaneity <BR>Evaluation of <I>ΔG<SUB>T, P</I></SUB> <BR><I>ΔG°</I> for a Chemical Reaction <BR>Thermodynamic Stability <BR><B>CHEMICAL EQUILIBRIUM (I) </B><BR>Equilibrium Constants <BR>The Reaction Quotient (<I>Q</I>) and Relative Activities (<I>a<SUB>i</I></SUB>)<BR>Formulation of Equilibrium Constants <BR>Molar Free Energies <BR><I>ΔG<SUB>R</I></SUB> for Chemical Reactions <BR><B>CHEMICAL EQUILIBRIUM (II) </B><BR>Calculations Using Thermodynamic Equilibrium Constants <BR>Effect of Catalyst on <I>K</I> <BR>Effect of Temperature on <I>K</I> <BR>Effect of Pressure on K <BR><B>PHASE EQUILIBRIUM (I) </B><BR>Phase Change and Gibbs Free Energy <BR>Phase Diagram for a Single Pure Substance<BR>The Phase Rule <BR><B>PHASE EQUILIBRIUM (II) </B><BR>Phase Diagram for CO<SUB>2</SUB> <BR>Phase Diagram for Water <BR>The Clapeyron Equation <BR>Phase Diagram for Carbon <BR>Phase Diagram for Helium <BR>The Clausius-Clapeyron Equation <BR><B>MIXTURES </B><BR>Expressions for Concentration <BR>Partial Molar Volumes <BR>The Chemical Potential (<I>μ</I>) <BR>The Chemical Potential of a Component in an Ideal Gas Mixture <BR>More About Activities <BR>Ideal Liquid Solutions of Volatile Solutes: Raoult's Law <BR>Ideal Liquid Solutions of Non-Volatile Solutes <BR>Ideal Liquid Solutions of Two Volatile Liquids <BR>Real (Non-Ideal) Solutions <BR>Chemical Potential and Solvent Activity <BR>Ideal Dilute Solutions of Volatile Solutes: Henry's Law <BR>The Solubility of Gases <BR>Distillation <BR>The Lever Rule <BR>Liquid-Liquid Phase Diagrams <BR>Liquid-Solid Phase Diagrams <BR>Compound Formation <BR><B>COLLIGATIVE PROPERTIES </B><BR>Colligative Properties <BR>Vapor Pressure Depression <BR>Boiling Point Elevation and Freezing Point Depression <BR>Osmotic Pressure <BR><B>IONIC EQUILIBRIUM </B><BR>Ionic Equilibrium <BR>Activities of Dissolved Species in Solution <BR>Activities and Activity Coefficients of Electrolytes in Solution <BR>Acids and Bases: The Brønsted-Lowry Concept <BR>The Self-Dissociation of Water <BR>Neutral Solutions <BR><B>ACID AND BASE DISSOCIATION </B><BR>Acid Dissociation Constants, <I>K<SUB>a</SUB> </I><BR>Dissociation of a Weak Acid <BR>Polyprotic Acid Calculation: Charge and Mass Balances <BR>Simplified Approach <BR><B>BASES AND THEIR SALTS </B><BR>Weak Bases: <I>B</I> or <I>BOH</I> <BR>The Salt of a Weak Acid: Hydrolysis <BR>The Rigorous Method <BR>The Salt of a Weak Base <BR>Acid-Base Titrations <BR><B>BUFFER SOLUTIONS </B><BR>Buffer Solutions <BR>Buffer of a Weak Acid and its Salt: <I>HA + NaA</I> <BR>Rigorous Derivation: <I>HA/NaA</I> Buffer <BR>Buffer of a Weak Base and Its Salt: <I>BOH + BCl</I> <BR>Rigorous Expression for <I>BOH/BCl</I> Buffer <BR>Acid-Base Indicators: <I>HIn</I> <BR><B>SOLUBILITY EQUILIBRIA </B><BR>Solubility Equilibria <BR>Relationship Between <I>K<SUB>SP</I></SUB> and Solubility for Different Salt Types <BR>Activity Effects and Solubility <BR>The Common Ion Effect <BR>Salting In <BR>Selective Precipitation <BR><B>OXIDATION-REDUCTION REACTIONS </B><BR>Oxidation-Reduction (Redox) Reactions <BR>Rules for Assignment of Oxidation Numbers <BR>Steps for Balancing Redox Reactions <BR><B>ELECTROCHEMISTRY </B><BR>Half-Reactions, Electrodes, and Electrochemical Cells <BR>Electrical Work <BR>Types of Cells <BR>Liquid Junctions and Salt Bridges <BR>Equilibrium Voltages <BR>The Nernst Equation <BR>Single Electrode Potentials <BR>Calculation of Equilibrium Cell Voltages from Half-Cell Potentials <BR>Equilibrium Constants from Cell Voltages <BR>Thermodynamic Functions from Cell Voltages <BR>Concentration Cells <BR><B>CHEMICAL REACTION KINETICS </B><BR>Rates of Reactions: Chemical Kinetics <BR>Concentration Profiles <BR>Expression of Reaction Rates <BR>Differential Rate Laws <BR>First Order Reactions <BR>Half-Lives <BR>Second Order Reactions <BR>Zeroth Order Reactions <BR>Experimental Determination of <I>k</I>, <I>m</I>, and <I>n</I> <BR>Reaction Mechanisms <BR>The Rate-Determining Step <BR>Reaction Rates and Equilibrium <BR>Reaction Intermediates <BR>Effect of Temperature <BR>Rates of Ionic Reactions <BR><B>APPENDICES </B><BR>Properties of the Elements <BR>Thermodynamic Data for Selected Gases and Vapors <BR>Thermodynamic Data for Selected Liquids <BR>Thermodynamic Data for Selected Solids <BR>Thermodynamic Data for Selected Aqueous Ions <BR>Analytical Solution of a Cubic Equation <BR>The Newton-Raphson Method <BR>Understanding Basic Integration <BR>Understanding Logarithms, Exponentials, and the Integral of <I>1/x</I> <BR>Standard Reduction Potentials <BR>Answers to Exercises <BR>Answers to Problems</P> | |
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