# CHME 303. Chemical Engineering Thermodynamics

#### 1. Course number and name

CHME 303. Chemical Engineering Thermodynamics

#### 2. Credits and contact hours

4 credit hours = 60 contact hours per semester

#### 3. Instructor’s or course coordinator’s name

Dr. Daniel Gulino

#### 4. Text book, title, author, and year

Fundamentals of Chemical Engineering Thermodynamics, Dahm, K.D. & Visco, D.P., 1st edition, Cengage Learning, 2015, ISBN 1-111-58070-7.

none

#### 5. Specific course information

a. catalog description:  Applications of the First Law and Second Law to chemical process systems, especially phase and chemical equilibria and the behavior of real fluids. Development of fundamental thermodynamic property relations and complete energy and entropy balances. Modeling of physical properties for use in energy and entropy balances, heat and mass transfer, separations, reactor design, and process control.

b. prerequisites: CHME 201, MATH 291 co-requisite (or prerequisite): MATH 392

c. required, elective, or selected elective (as per Table 5-1): required

#### 6. Specific goals for the course

a. The student will be able…

• Use an engineering problem-solving strategy:
1. Identify the scope of the challenge or problem.
2. Draw a representation of the physical system.
3. Compile and evaluate known information about the problem.
4. Concisely describe what needs to be calculated or what criteria met.
5. List appropriate assumptions to simplify the problem.
6. Compile relevant property values and sources of information.
7. Apply conservation laws and rate equations.
8. Calculate solutions to equations in general terms and with numerical values.
9. Use estimation to check reasonableness of assumptions and solutions.
• Define system boundaries.
• Calculate the heat energy requirement for a chemical or physical process.
• Solve problems using an appropriate energy balance.
• Calculate the work requirement for a chemical or physical process.
• Solve problems using the appropriate entropy balance.
• Formulate and use ordinary and partial differential equations to solve thermodynamics problems.
• Determine equilibrium conditions for chemical species transfer between phases (i.e. boiling, melting, freezing, etc.).
• Estimate property values for a chemical species at a given state (i.e. temperature, pressure, molar volume, etc.).
• Communicate thermodynamic concepts in the context of phase change and energy conversion processes, such as refrigeration, engines, and electricity production.
• Describe what changes about thermochemical properties when more than one chemical species is present (i.e. in mixtures).
• State the conditions of equilibrium for multiphase systems;
• Understand and apply fugacity to phase equilibria problems;
• Compute the vapor pressure for single-component multiphase systems;
• Apply partial molar quantities to compute mixture properties;
• Know and apply models for excess Gibbs free energy in nonideal mixtures;
• Construct binary phase diagrams for multiple phase systems correcting for nonideal behavior using fugacity coefficients and activity coefficients;
• Perform calculations for vapor-liquid equilibrium; and
• Determine the equilibrium composition for a reacting system given the reaction stoichiometry, temperature and pressure.

b. Criterion 3 Student Outcomes specifically addressed by this course are found in a mapping of outcomes against all CHME courses in the curriculum.

#### 7. Brief list of topics to be covered

• mass balances
• energy balances
• energy conversions
• entropy balances
• 0th, 1st, 2nd, 3rd Laws of Thermodynamics
• thermodynamic cycles
• refrigeration/liquefaction
• engines
• turbines
• partial differential equations
• thermodynamic models
• equations of state
• phase equilibria for pure compounds
• properties of mixing
• Thermodynamics of multicomponent mixtures
• Estimation of Gibbs free energy and fugacity of components in mixtures including activity coefficient models
• Multiphase equilibrium in mixtures (vapor-liquid, liquid-liquid, vapor-liquid-liquid, solid-liquid equilibrium)
• Phase equilibrium in systems including solids
• Chemical reaction equilibrium