This is a junior level course required for all chemical engineering students.  The Spring 2001 offering of the class uses Introductory Chemical Engineering Thermodynamics by Elliott and Lira and is divided into four modules.

Module 1: Thermodynamics of Processes- This module will cover the first four chapters of your book, and will be approximately three weeks long.  Topics include energy balances, forms of work, reversibility, entropy, thermodynamics of process equipment, and cycles.

Module 2: Analysis of Fluid Properties- This module will cover chapters 5-8 of your book, and will be approximately four weeks long.  Topics include thermodynamics of pure fluids, equations of state, reference states, departure functions, and phase equilibrium.

Module 3: Fluid Phase Equilibria- This module will cover chapters 9-12 of your book and will be approximately four weeks long.  Topics include multi-component fluids, phase equilibria of mixtures, and activity models.

Module 4: Reacting Systems- This module will cover chapter 14 of your book and will be approximately two weeks long.  Topics include reaction equilibria, energy balances in reacting systems, multi-reaction equilibria, and simultaneous reaction and phase equilibria.
   
Educational Objectives:

Module 1: At the end of this module, students should be able to:

• Define the terms internal energy, potential energy, kinetic energy, work, heat, entropy, and reversibility in their own words.
• Describe in words the physical behavior of an ideal gas and identify practical situations in which the ideal gas law would be a reasonable approximation.
• Use the steam tables to quantify the inter-relationships between P, V, T, U, H and S for liquid water and steam.
• Apply energy and entropy balances to calculate work, heat, and changes in energy and entropy for closed systems and open, steady-state systems.
• Describe the functions of process equipment such as pumps, turbines, throttling valves, compressors and heat exchangers, and apply energy and entropy balances to any of these systems.
• List and explain the steps in the following cycles: Carnot, Rankine, Refridgeration, Linde liquefaction, and Internal combustion.
• Quantify the overall efficiency or performance of any of the above cycles, as well as the individual steps within the cycle.

• Explain in words what an equation of state is and why they are useful.
• Use the Peng-Robinson, Compressibility Equation, or any other given equation of state to calculate and unknown P, V or T when the other two are known.
• Qualitatively describe the relationships between P, V and T for liquids and gases, and recognize conditions at which ideal gas behavior should be followed.
• Calculate changes in U, H, G and S, given the initial and final state of the system and an equation of state for the fluid.
• Use the expansion rule, triple product rule, and Maxwell's relations to reduce partial derivatives of U, H, G and A to measureable quantities.
• Explain in words what a departure function is, and why they are useful.
• Compute the departure function for U, H, G or S at any set of conditions, given an equation of state.
• Use departure functions in calculating changes in U, H, G or S.
• Explain in words the physical significance of the fugacity.
• Calculate the fugacity of a liquid or vapor, given an equation of state and a set of conditions (e.g. temp and press)
• Use the Poynting correction factor in estimating liquid fugacities.
• Estimate the boiling point of a compound using the Clausius-Clapeyron, Antoine or Generalized equations.

• Calculate the fugacities of pure liquids and vapors, given an Equation of State.
• Distinguish between pure component fugacity and fugacity of a component within a mixture, and which is applicable in a given situation.
• Compute fugacity for a component within an ideal gas mixture or ideal solution, given a composition and sufficient information to compute the pure component fugacities.
• Recognize that component fugacities are identical in phases at equilibrium, and use this fact to assess equilibrium conditions and compositions.
• Calculate values of K using the shortcut method.
• Describe in words the distinctions between ideal gases, ideal solutions and real solutions, and identify physical situations in which each is likely to apply.
• Use mixing rules to find EOS a and b values for mixtures, given compositions and the pure-component values.
• Fit the one and two parameter Margules equations to VLE data.
• Use the Margules equation, or activity coefficient values given in some other form, to assess equilibrium conditions and compositions for real mixtures.
• Use the UNIQUAC method to compute molecular volume and surface area fractions for mixtures.

Spring 2001 Instructor
Dr. Kevin D. Dahm
330 Rowan Hall
256-5318
dahm@rowan.edu