Professor H.D.B. Jenkins is based in the Department of Chemistry, University of Warwick, Coventry, UK

"Presenting thermodynamics in an appealing and instructive way is an ongoing problem and this text addresses this issue in its clarity and useful organisation". (The Higher Education Academy Physical Sciences Centre, June 2008) "This is a well-organised presentation of the standard material in a thermodynamics undergraduate course for chemists or chemical engineers." (Reviews)

• 0 Symbols and Notation. 1 Thermodynamic Changes, Properties and Types of Function.2 Integration in Thermodynamics.3 Graphical Gradients and Intercepts.4 The Ideal Gas.5 Partial Derivatives (∂ Z/∂Y )x Simplified.6 Logarithms and Exponentials.7 Thermodynamics Conventions.8 Heat and Work. First Law of Thermodynamics.9 Work of Expansion.10 Internal Energy, U and Enthalpy, H.11 Reference States.12 Bond Enthalpy (Energy).13 Spontaneity, Entropy and Gibbs Energy.14 Entropy and Second Law.15 Calculation of Entropy.16 The Third Law of Thermodynamics.17 The Statistical Definition of Entropy.18 Variation of G with T (dP = 0).19 Variation of H and S with T (dP = 0).20 Variation of G and S with P (dP = 0).21 Variation of G with T for Solid, Liquid and Gaseous Phase.22 Variation of H with T for Solid, Liquid and Gaseous Phase.23 Effect of Pressure on Melting Point and Boiling Point: Normal Substances.24 Effect of Pressure on Melting Point and Boiling Point: Water.25 Phase Equilibria. Clapeyron Equation.26 Clausius–Clapeyron Equation.27 Open Systems. Chemical Potential. Chemical Reactions.28 Coupled Reactions.29 Chemical Potentials Applied to Physical Processes.30 The Phase Rule.31 Ideal and Real Gases. Dalton’s Law of Partial Pressures.32 Ideal Liquid Mixtures. Vapour Pressure and Raoult’s Law.33 Ideal Liquid Mixtures. Real Liquid Mixtures.34 Binary Liquid Mixtures.35 Chemical Potentials and Equilibrium Relationships.36 Interpretation of Logarithmic Term. Molality.37 Thermodynamics of Ideal Mixing.38 Chemical Potentials of Real Gases. Fugacity.39 Chemical Potentials of Real Solutions. Activity.40 Measurements of Equilibrium Constant, K.41 Reaction Quotient, Q and Equilibrium Constant, K. Relationship Between _Go and Kp/po.42 Chemical Equilibrium.43 K for a Multiphase Reaction.44 Reactions Not at Equilibrium.45 Equilibrium Calculations for Reactions Not Initially at Equilibrium.46 Gibbs–Helmholtz Equation.47 Qualitative Interpretation of Van’t Hoff Equation. Coupled Reaction.48 Variation of Equilibrium Constant, K, with Overall Total Pressure, P.49 Le Chatelier’s Principle.50 Gibbs–Duhem Equation.51 Colligative Properties: Freezing Point.52 Colligative Properties: Boiling Point.53 Colligative Properties: Osmotic Pressure, _.54 Core Thermodynamic Relationships.Appendix A: The Logarithmic Function in Thermodynamics

Professor H.D.B. Jenkins is based in the Department of Chemistry, University of Warwick, Coventry, UK

"Presenting thermodynamics in an appealing and instructive way is an ongoing problem and this text addresses this issue in its clarity and useful organisation". (The Higher Education Academy Physical Sciences Centre, June 2008) "This is a well-organised presentation of the standard material in a thermodynamics undergraduate course for chemists or chemical engineers." (Reviews)

• 0 Symbols and Notation. 1 Thermodynamic Changes, Properties and Types of Function.2 Integration in Thermodynamics.3 Graphical Gradients and Intercepts.4 The Ideal Gas.5 Partial Derivatives (∂ Z/∂Y )x Simplified.6 Logarithms and Exponentials.7 Thermodynamics Conventions.8 Heat and Work. First Law of Thermodynamics.9 Work of Expansion.10 Internal Energy, U and Enthalpy, H.11 Reference States.12 Bond Enthalpy (Energy).13 Spontaneity, Entropy and Gibbs Energy.14 Entropy and Second Law.15 Calculation of Entropy.16 The Third Law of Thermodynamics.17 The Statistical Definition of Entropy.18 Variation of G with T (dP = 0).19 Variation of H and S with T (dP = 0).20 Variation of G and S with P (dP = 0).21 Variation of G with T for Solid, Liquid and Gaseous Phase.22 Variation of H with T for Solid, Liquid and Gaseous Phase.23 Effect of Pressure on Melting Point and Boiling Point: Normal Substances.24 Effect of Pressure on Melting Point and Boiling Point: Water.25 Phase Equilibria. Clapeyron Equation.26 Clausius–Clapeyron Equation.27 Open Systems. Chemical Potential. Chemical Reactions.28 Coupled Reactions.29 Chemical Potentials Applied to Physical Processes.30 The Phase Rule.31 Ideal and Real Gases. Dalton’s Law of Partial Pressures.32 Ideal Liquid Mixtures. Vapour Pressure and Raoult’s Law.33 Ideal Liquid Mixtures. Real Liquid Mixtures.34 Binary Liquid Mixtures.35 Chemical Potentials and Equilibrium Relationships.36 Interpretation of Logarithmic Term. Molality.37 Thermodynamics of Ideal Mixing.38 Chemical Potentials of Real Gases. Fugacity.39 Chemical Potentials of Real Solutions. Activity.40 Measurements of Equilibrium Constant, K.41 Reaction Quotient, Q and Equilibrium Constant, K. Relationship Between _Go and Kp/po.42 Chemical Equilibrium.43 K for a Multiphase Reaction.44 Reactions Not at Equilibrium.45 Equilibrium Calculations for Reactions Not Initially at Equilibrium.46 Gibbs–Helmholtz Equation.47 Qualitative Interpretation of Van’t Hoff Equation. Coupled Reaction.48 Variation of Equilibrium Constant, K, with Overall Total Pressure, P.49 Le Chatelier’s Principle.50 Gibbs–Duhem Equation.51 Colligative Properties: Freezing Point.52 Colligative Properties: Boiling Point.53 Colligative Properties: Osmotic Pressure, _.54 Core Thermodynamic Relationships.Appendix A: The Logarithmic Function in Thermodynamics

Professor H.D.B. Jenkins is based in the Department of Chemistry, University of Warwick, Coventry, UK

"Presenting thermodynamics in an appealing and instructive way is an ongoing problem and this text addresses this issue in its clarity and useful organisation". (The Higher Education Academy Physical Sciences Centre, June 2008) "This is a well-organised presentation of the standard material in a thermodynamics undergraduate course for chemists or chemical engineers." (Reviews)

• 0 Symbols and Notation. 1 Thermodynamic Changes, Properties and Types of Function.2 Integration in Thermodynamics.3 Graphical Gradients and Intercepts.4 The Ideal Gas.5 Partial Derivatives (∂ Z/∂Y )x Simplified.6 Logarithms and Exponentials.7 Thermodynamics Conventions.8 Heat and Work. First Law of Thermodynamics.9 Work of Expansion.10 Internal Energy, U and Enthalpy, H.11 Reference States.12 Bond Enthalpy (Energy).13 Spontaneity, Entropy and Gibbs Energy.14 Entropy and Second Law.15 Calculation of Entropy.16 The Third Law of Thermodynamics.17 The Statistical Definition of Entropy.18 Variation of G with T (dP = 0).19 Variation of H and S with T (dP = 0).20 Variation of G and S with P (dP = 0).21 Variation of G with T for Solid, Liquid and Gaseous Phase.22 Variation of H with T for Solid, Liquid and Gaseous Phase.23 Effect of Pressure on Melting Point and Boiling Point: Normal Substances.24 Effect of Pressure on Melting Point and Boiling Point: Water.25 Phase Equilibria. Clapeyron Equation.26 Clausius–Clapeyron Equation.27 Open Systems. Chemical Potential. Chemical Reactions.28 Coupled Reactions.29 Chemical Potentials Applied to Physical Processes.30 The Phase Rule.31 Ideal and Real Gases. Dalton’s Law of Partial Pressures.32 Ideal Liquid Mixtures. Vapour Pressure and Raoult’s Law.33 Ideal Liquid Mixtures. Real Liquid Mixtures.34 Binary Liquid Mixtures.35 Chemical Potentials and Equilibrium Relationships.36 Interpretation of Logarithmic Term. Molality.37 Thermodynamics of Ideal Mixing.38 Chemical Potentials of Real Gases. Fugacity.39 Chemical Potentials of Real Solutions. Activity.40 Measurements of Equilibrium Constant, K.41 Reaction Quotient, Q and Equilibrium Constant, K. Relationship Between _Go and Kp/po.42 Chemical Equilibrium.43 K for a Multiphase Reaction.44 Reactions Not at Equilibrium.45 Equilibrium Calculations for Reactions Not Initially at Equilibrium.46 Gibbs–Helmholtz Equation.47 Qualitative Interpretation of Van’t Hoff Equation. Coupled Reaction.48 Variation of Equilibrium Constant, K, with Overall Total Pressure, P.49 Le Chatelier’s Principle.50 Gibbs–Duhem Equation.51 Colligative Properties: Freezing Point.52 Colligative Properties: Boiling Point.53 Colligative Properties: Osmotic Pressure, _.54 Core Thermodynamic Relationships.Appendix A: The Logarithmic Function in Thermodynamics