Curriculum Map

Course: Thermodynamics

Authors
Don W. Green, Editor-in-Chief, Perry's Chemical Engineers' Handbook, 8th Edition, and Emeritus Distinguished Professor of Chemical and Petroleum Engineering, University of Kansas
Marylee Southard, Associate Professor, Chemical Engineering, University of Kansas
Ali Sadegh, Editor, Marks' Standard Handbook for Mechanical Engineers, 11th Edition

Course Topics

Variables, Definitions, Relationships

Relevant Material Type Description Source
Variables, Definitions, Relationships Text Five basic postulates, constant composition systems Perry's Chemical Engineers' Handbook
Nomenclature Table Nomenclature and units Perry's Chemical Engineers' Handbook
Thermodynamic property relations Table Table 4-1, basic mathematical relationships Perry's Chemical Engineers' Handbook

Property Calculation; Gases & Vapors

Relevant Material Type Description Source
Property Calculations for Gases and Vapors Text   Perry's Chemical Engineers' Handbook
Enthalpy, Entropy, Ideal Gas Text Mathematical relationships Perry's Chemical Engineers' Handbook
Residual Enthalpy, Entropy Text Use of PVT correlations Perry's Chemical Engineers' Handbook
Virial equation of state Text   Perry's Chemical Engineers' Handbook
Cubic equations of state Text   Perry's Chemical Engineers' Handbook
Parameters for cubic equations Table Table 4-2, parameter assignments Perry's Chemical Engineers' Handbook
Pitzer's generalized correlations Text   Perry's Chemical Engineers' Handbook
Thermal Properties Text Estimation of enthalpy and entropy of formation Perry's Chemical Engineers' Handbook
Ideal gas enthalpy of formation Example Example (Sect 2), enthalpy of formation of o-toluidine Perry's Chemical Engineers' Handbook
Ideal gas enthalpy of formation Example Example (Sect 2), enthalpy of formation of acetaldehyde Perry's Chemical Engineers' Handbook
Ideal gas entropy of formation Example Example (Sect 2), entropy of formation of o-toluidine Perry's Chemical Engineers' Handbook
Group contribution values Table Table 2-343, Group contributions-standard-state properties Perry's Chemical Engineers' Handbook
Latent Enthalpy Text Enthalpy of vaporization, sublimation & fusion Perry's Chemical Engineers' Handbook
Thermodynamic basis for evaporation Text Chemical potential difference between phases Perry's Chemical Engineers' Handbook
Enthalpy of vaporization Text Recommended methods of calculation Perry's Chemical Engineers' Handbook
Use of vapor-pressure correlation Example Example (Sect 2), enthalpy change for anisole Perry's Chemical Engineers' Handbook
Corresponding -states correlation Example Example (Sect 2), enthalpy change for anisole Perry's Chemical Engineers' Handbook
Vetere method Example Example (Sect 2), enthalpy change for anisole Perry's Chemical Engineers' Handbook
Enthalpy of fusion Text Recommended method of calculation Perry's Chemical Engineers' Handbook
Enthalpy of sublimation Text Recommended method of calculation Perry's Chemical Engineers' Handbook
Molar Properties of Water, H2O Table Table E-6 Schaum's Outline of Thermodynamics for Engineers, Second Edition
Saturated R134a - Pressure Table Table Table D-2 Schaum's Outline of Thermodynamics for Engineers, Second Edition
Saturated R134a - Temperature Table Table Table D-1 Schaum's Outline of Thermodynamics for Engineers, Second Edition
Molar Properties of Nitrogen, N2 Table Table E-2 Schaum's Outline of Thermodynamics for Engineers, Second Edition

Thermodynamics of Flow Processes

Relevant Material Type Description Source
Thermodynamics of Flow Processes Text   Perry's Chemical Engineers' Handbook
Mass, Energy & Entropy Balances Text Mathematical expressions of balances Perry's Chemical Engineers' Handbook
Applications to Flow processes Text
Perry's Chemical Engineers' Handbook
Duct Flow of Compressible Fluids Text Pressure changes, velocity & thermodynamic properties Perry's Chemical Engineers' Handbook
Pipe flow Text
Perry's Chemical Engineers' Handbook
Nozzles Text Friction loss reduction Perry's Chemical Engineers' Handbook
Nozzle characteristics Table Table 4-4, subsonic & supersonic Perry's Chemical Engineers' Handbook
Throttling process Text
Perry's Chemical Engineers' Handbook
Turbines (expanders) Text
Perry's Chemical Engineers' Handbook
Adiabatic expansion process Figure Figure 4-2, enthalpy-entropy behavior Perry's Chemical Engineers' Handbook
Compression processes Text
Perry's Chemical Engineers' Handbook
Adiabatic compression process Figure Figure 4-3,enthalpy-entropy behavior Perry's Chemical Engineers' Handbook
Adiabatic vaporization & compression Example Example 1, LNG vaporization & compression Perry's Chemical Engineers' Handbook

Systems of Variable Composition

Relevant Material Type Description Source
Systems of Variable Composition Text Relationships for changing composition Perry's Chemical Engineers' Handbook
Partial Molar Properties Text
Perry's Chemical Engineers' Handbook
Partial molar Equation-of-State parameters Text Mixing rules Perry's Chemical Engineers' Handbook
Partial molar Gibbs Energy Text
Perry's Chemical Engineers' Handbook
Solution Thermodynamics Text
Perry's Chemical Engineers' Handbook
Ideal gas mixture model Text
Perry's Chemical Engineers' Handbook
Fugacity & fugacity coefficient Text
Perry's Chemical Engineers' Handbook
Ideal solution model Text
Perry's Chemical Engineers' Handbook
Excess properties Text
Perry's Chemical Engineers' Handbook
Property changes of mixing Table Table 4-5, connecting relations, excess properties Perry's Chemical Engineers' Handbook
Fundamental Property Relations Text Property relations based on Gibbs Energy Perry's Chemical Engineers' Handbook
Residual property relations Text
Perry's Chemical Engineers' Handbook
Property relation equations Table Table 4-6, Gibbs Energy & related properties Perry's Chemical Engineers' Handbook
Excess property relations Text
Perry's Chemical Engineers' Handbook
Models for Excess Gibbs Energy Text
Perry's Chemical Engineers' Handbook
Property changes of mixing Figure Figure 4-4, 50 0C, six binary liquid systems Perry's Chemical Engineers' Handbook
Excess properties Figure Figure 4-5, 50 0C, six binary liquid systems Perry's Chemical Engineers' Handbook
Activity coefficients Figure Figure 4-6, 50 0C, six binary liquid systems Perry's Chemical Engineers' Handbook
Solvent Screening Methods Text
Perry's Chemical Engineers' Handbook
Solute-solvent interactions Table Table 15-2, Robbins' Chart - qualitative Perry's Chemical Engineers' Handbook
Use of activity coefficients Text Intro, prediction methods Perry's Chemical Engineers' Handbook
Liquid-liquid miscibility methods Text Godfrey's methods Perry's Chemical Engineers' Handbook
Godfrey miscibility numbers Table Table 15-3 Perry's Chemical Engineers' Handbook
Godfrey standard solvents Table Table 15-4 Perry's Chemical Engineers' Handbook
Computer-aided molecular design Text
Perry's Chemical Engineers' Handbook
High-throughput experiments Text
Perry's Chemical Engineers' Handbook

Equilibrium

Relevant Material Type Description Source
Equilibrium Text   Perry's Chemical Engineers' Handbook
Criteria for Equilibrium Text Fundamental relationships for equilibrium Perry's Chemical Engineers' Handbook
Phase Rule Text
Perry's Chemical Engineers' Handbook
Application of the phase rule Example Example 2, two miscible, nonreacting species Perry's Chemical Engineers' Handbook
Duhem's theorem Text
Perry's Chemical Engineers' Handbook
Vapor-Liquid Equilibrium Text
Perry's Chemical Engineers' Handbook
Modified Raoult's Law Text
Perry's Chemical Engineers' Handbook
Dew & bubble-point calculation Example Example 3, application of Raoult's Law Perry's Chemical Engineers' Handbook
Solute-solvent systems Text Henry's Law discussed Perry's Chemical Engineers' Handbook
Henry's Law constants Text References to data Perry's Chemical Engineers' Handbook
Henry's Law constants Table Table 2-124, various compounds in water at 25 0C Perry's Chemical Engineers' Handbook
Henry's Law constants Table Table 2-125, from infinite dilution activity coefficients Perry's Chemical Engineers' Handbook
K values, VLE, flash calculations Text
Perry's Chemical Engineers' Handbook
Flash calculation Example Example 4, continuation of Example 3 Perry's Chemical Engineers' Handbook
Equation-of-state approach Text Application of fugacity coefficients Perry's Chemical Engineers' Handbook
Isothermal flash Text Rachford-Rice method Perry's Chemical Engineers' Handbook
Adiabatic flash Text
Perry's Chemical Engineers' Handbook
Complex phase flash Text
Perry's Chemical Engineers' Handbook
VLE as function of T Example Example 5, methanol/acetone system at different T's Perry's Chemical Engineers' Handbook
Constant pressure VLE data Table Table 13-1, data for four binary systems Perry's Chemical Engineers' Handbook
Graphical K value correlations Text
Perry's Chemical Engineers' Handbook
- Y-x curve for benzene-toluene Figure Figure 13-3 Perry's Chemical Engineers' Handbook
- T-x-y curves for benzene-toluene Figure Figure 13-4 Perry's Chemical Engineers' Handbook
- Azeotropic y-x curves for two systems Figure Figure 13-5 Perry's Chemical Engineers' Handbook
- Azeotropic T-x-y curve for ethyl acetate-ethanol Figure Figure 13-6 Perry's Chemical Engineers' Handbook
- Azeotropic T-x-y curve for chloroform-acetone Figure Figure 13-7 Perry's Chemical Engineers' Handbook
- Azeotropic T-x-y curve for n-butanol-water Figure Figure 13-8 Perry's Chemical Engineers' Handbook
- DePriester: K(T, P) of light hydrocarbons Figure Figures 13-9 Perry's Chemical Engineers' Handbook
- K(P) of light hydrocarbons in crude oil Figure Figure 13-10 Perry's Chemical Engineers' Handbook
- K(P) of light hydrocarbons Figure Figure 13-11 Perry's Chemical Engineers' Handbook
- K(P) of pentane Figure Figure 13-12 Perry's Chemical Engineers' Handbook
- K(P) of light hydrocarbons at 250F Figure Figure 13-13 Perry's Chemical Engineers' Handbook
Analytical K value correlations Text
Perry's Chemical Engineers' Handbook
- Binary interaction parameters for selected systems Table Table 13-2 Perry's Chemical Engineers' Handbook
- activity coefficient equations Table Table 13-3, 3 models Perry's Chemical Engineers' Handbook
- Liquid-phase activity coefficients for an n-heptane -toluene system at 101.3 kPa (1 atm) Figure Figure 13-14 Perry's Chemical Engineers' Handbook
- Liquid-phase activity coefficients for an ethanol - n-hexane system Figure Figure 13-15 Perry's Chemical Engineers' Handbook
- Antoine vapor pressure constants Table Table 13-4 Perry's Chemical Engineers' Handbook
Chemical Reaction Equilibria Text
Perry's Chemical Engineers' Handbook
Single reaction equilibrium Example Example 6, hydrogenation of benzene to produce cyclohexane Perry's Chemical Engineers' Handbook
Chemical equilibrium constant Text
Perry's Chemical Engineers' Handbook
Thermo model: reactive absorption Text Model for initial step: species generation in gas/liquid Perry's Chemical Engineers' Handbook
Liquid-Liquid Equilibrium Text Fundamental basis for extraction processes Perry's Chemical Engineers' Handbook
Activity coefficients, partition ratio Text
Perry's Chemical Engineers' Handbook
Extraction and separation factors Text
Perry's Chemical Engineers' Handbook
Solvent-to-feed ratio limits Text
Perry's Chemical Engineers' Handbook
Temperature effects Text
Perry's Chemical Engineers' Handbook
Salt effects on solute solubility Text
Perry's Chemical Engineers' Handbook
pH effects on solute partition Text Figure 15-14, pH effect on partition ratio of penicillin Perry's Chemical Engineers' Handbook
Phase diagrams showing data Text Phase compositions in Type I and II systems Perry's Chemical Engineers' Handbook
- Temp-composition diagram, water + 2-butoxyethanol Figure Figure 15-15 Perry's Chemical Engineers' Handbook
- Temp-composition diagram, ethylene glycol + triethylamine Figure Figure 15-16 Perry's Chemical Engineers' Handbook
- Composition diagram, water + acetic acid + MIBK, 25C Figure Figure 15-17 Perry's Chemical Engineers' Handbook
- Composition diagram, heptane + toluene + sulfolane, 25C Figure Figure 15-18 Perry's Chemical Engineers' Handbook
- Composition diagram, MIBK + water, 30C Figure Figure 15-19 Perry's Chemical Engineers' Handbook
Experimental methods Text
Perry's Chemical Engineers' Handbook
Data correlation equations Text Tie lines, Figure 15-20, water + acetic acid + MIBK, 25C Perry's Chemical Engineers' Handbook
Thermo. models of equilibria Text NRTL, UNIQUAC, SAFT Perry's Chemical Engineers' Handbook
Partition ratios Table Table 15-1, weight ratio of solute in binary solvent mixture Perry's Chemical Engineers' Handbook
Other data and model sources Text
Perry's Chemical Engineers' Handbook
Solid-Fluid Equilibrium Text Adsorption equilibrium Perry's Chemical Engineers' Handbook
Theory of adsorption Text Molecular forces, excess energy, isotherms, heat Perry's Chemical Engineers' Handbook
Single component exchange Text Flat surfaces or pores, ion exchange, separation factor Perry's Chemical Engineers' Handbook
Multiple component exchange Text
Perry's Chemical Engineers' Handbook
Supercritical Fluid Equilibria Text Classification of systems, thermodynamic models Perry's Chemical Engineers' Handbook
Psychrometric Chart, P = 1 atm Text Fig. F-1 Schaum's Outline of Thermodynamics for Engineers, Second Edition
Compressibility Chart Text Fig. G-1 Schaum's Outline of Thermodynamics for Engineers, Second Edition

Thermodynamic Analysis of Processes

Relevant Material Type Description Source
Thermodynamic Analysis of Processes Text Ideal work, steady-state, steady-flow processes Perry's Chemical Engineers' Handbook
Calculation of Ideal Work Text   Perry's Chemical Engineers' Handbook
Steady-State, Steady-Flow Processes Text Thermodynamic analysis of processes Perry's Chemical Engineers' Handbook
Lost-work analysis Example Example 7, Linde system for separation of air into O2 & N2 Perry's Chemical Engineers' Handbook

Ideal Cycles

Relevant Material Type Description Source
Ideal Gas Mixtures Text   Marks' Standard Handbook for Mechanical Engineers
Compressibility factors for gases and vapors Figure Fig. 4.1.3 Marks' Standard Handbook for Mechanical Engineers
Ideal Cycles with Perfect Gases Text   Marks' Standard Handbook for Mechanical Engineers
Ratio of actual power to maximum power as a function of ratio of actual thermal efficiency to Carnot efficiency Figure Fig. 4.1.8 Marks' Standard Handbook for Mechanical Engineers
Two main types of Stirling engine Figure Fig. 4.1.14 Marks' Standard Handbook for Mechanical Engineers
Gas Power Cycles Text   Schaum's Outline of Thermodynamics for Engineers, Second Edition
The Air-standard cycle Text   Schaum's Outline of Thermodynamics for Engineers, Second Edition
The Otto cycle Text   Schaum's Outline of Thermodynamics for Engineers, Second Edition
The Diesel cycle Text   Schaum's Outline of Thermodynamics for Engineers, Second Edition
The Stirling and Ericsson cycles Text   Schaum's Outline of Thermodynamics for Engineers, Second Edition
The Regenerative gas-turbine cycle Text   Schaum's Outline of Thermodynamics for Engineers, Second Edition
Solved problems Example   Schaum's Outline of Thermodynamics for Engineers, Second Edition

Psychrometric Charts

Relevant Material Type Description Source
Psychrometric Charts Text   Marks' Standard Handbook for Mechanical Engineers
Skeleton humidity chart Table Fig. 4.1.18 Marks' Standard Handbook for Mechanical Engineers

Combustion

Relevant Material Type Description Source
Combustion Text   Marks' Standard Handbook for Mechanical Engineers
Heats of combustion Table Table 4.1.6 Marks' Standard Handbook for Mechanical Engineers
Products of combustion Table Table 4.1.7 Marks' Standard Handbook for Mechanical Engineers
Temperature Attained by Combustion Text
Marks' Standard Handbook for Mechanical Engineers
Internal energy of gases Table Table 4.1.8 Marks' Standard Handbook for Mechanical Engineers
Flame temperatures, Deg R, at 14.7 psia, allowing for dissociation Table Table 4.1.9 Marks' Standard Handbook for Mechanical Engineers
Combustion of Solid Fuels Text
Marks' Standard Handbook for Mechanical Engineers
Ratio of air supplied per pound of combustible to that theoretically required Figure Fig. 4.1.37 Marks' Standard Handbook for Mechanical Engineers
Relation of CO2 to excess air for fuels Figure Fig. 4.1.38 Marks' Standard Handbook for Mechanical Engineers
Solved problems and examples of combustion Example Solved problems Schaum's Outline of Thermodynamics for Engineers, Second Edition

Thermodynamic Properties of Substances

Relevant Material Type Description Source
Thermophysical properties of selected solid elements Text Text Marks' Standard Handbook for Mechanical Engineers
Enthalpy and Psi functions for ideal-gas air Table Table 4.2.1 Marks' Standard Handbook for Mechanical Engineers
Temperature-entropy diagram for air Figure Fig. 4.2.1  Marks' Standard Handbook for Mechanical Engineers
International r, standard atmosphere Table Table 4.2.2  Marks' Standard Handbook for Mechanical Engineers
Saturated ammonia (R 717) Table Table 4.2.3  Marks' Standard Handbook for Mechanical Engineers
Enthalpy - log pressure diagram for air Figure Fig. 4.2.2  Marks' Standard Handbook for Mechanical Engineers
Enthalpy - log pressure diagram for ammonia (R717) Figure Fig. 4.2.3  Marks' Standard Handbook for Mechanical Engineers
Saturated carbon dioxide Table Table 4.2.4  Marks' Standard Handbook for Mechanical Engineers
Superheated carbon dioxide Table Table 4.2.5 Marks' Standard Handbook for Mechanical Engineers
Saturated normal hydrogen Table Table 4.2.7  Marks' Standard Handbook for Mechanical Engineers
Saturated Refrigerant 11 Table Table 4.2.9  Marks' Standard Handbook for Mechanical Engineers
Enthalpy - log pressure diagram for refrigerant 11.1 MPa 10 bar Figure Fig. 4.2.4  Marks' Standard Handbook for Mechanical Engineers
Saturated Refrigerant 12 Table Table 4.2.10  Marks' Standard Handbook for Mechanical Engineers
Enthalpy - log pressure diagram for refrigerant 12 Table Fig. 4.2.5  Marks' Standard Handbook for Mechanical Engineers
Saturated Refrigerant 22 Table Table 4.2.11  Marks' Standard Handbook for Mechanical Engineers
Enthalpy - log pressure diagram for refrigerant 22. 1 MPa 10 bar   Fig. 4.2.6  Marks' Standard Handbook for Mechanical Engineers
Saturated water substance Table Table 4.2.17  Marks' Standard Handbook for Mechanical Engineers
Temperature-entropy diagram for water substance, SI units Figure Fig. 4.2.10  Marks' Standard Handbook for Mechanical Engineers
Compressed steam Table Table 4.2.18 Marks' Standard Handbook for Mechanical Engineers
Saturated water substance, fps units Table Table 4.2.19  Marks' Standard Handbook for Mechanical Engineers
Compressed water substance, fps units Table Table 4.2.20 Marks' Standard Handbook for Mechanical Engineers
Temperature-entropy diagram for water substance, fps units Table Fig. 4.2.11  Marks' Standard Handbook for Mechanical Engineers
Phase transition and other data for 100 fluids Table Table 4.2.21 Marks' Standard Handbook for Mechanical Engineers
Saturation temperature, in Kelvins, of selected substances Table Table 4.2.24  Marks' Standard Handbook for Mechanical Engineers
Color scale of temperature for iron or steel Table Table 4.2.25  Marks' Standard Handbook for Mechanical Engineers
Mean specific heats of various solids (32 - 2128F, 273 -373 K) Table Table 4.2.27  Marks' Standard Handbook for Mechanical Engineers
Melting points of refractory materials Table Table 4.2.26 Marks' Standard Handbook for Mechanical Engineers
Thermophysical properties of selected solid elements Table Table 4.2.29  Marks' Standard Handbook for Mechanical Engineers
Solved problems and examples of properties of pure substances Example Solved problems Schaum's Outline of Thermodynamics for Engineers, Second Edition

First and Second Laws of Thermodynamics

Relevant Material Type Description Source
The First Law of Thermodynamics Text   Schaum's Outline of Thermodynamics for Engineers, Second Edition
Examples of The First Law of Thermodynamics Example Solved problems Schaum's Outline of Thermodynamics for Engineers, Second Edition
The Second Law of Thermodynamics Text   Schaum's Outline of Thermodynamics for Engineers, Second Edition
Examples of The Second Law of Thermodynamics Example Solved problems Schaum's Outline of Thermodynamics for Engineers, Second Edition