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|15.04 - VLE calculations by an equation of state||Click here.||80||1||
PRMix.xlsx - Tutorial on use for bubble pressure (msu.edu) (10:06)
An overview of the organization of PRMix.xlsx, and a tutorial on the strategy to solve bubble pressure problems. Example 15.6 is worked in the screencast. After watching this screencast, you should be able to also solve dew or flash problems if you think about the strategy used to solve the problem. You may also be interested in a similar presentation from U.Colorado (learncheme, 6min).
|01.2 Molecular Nature of Temperature, Pressure, and Energy||Click here.||78||20||
Molecular Nature of Internal Energy: Thermal Energy
|01.2 Molecular Nature of Temperature, Pressure, and Energy||Click here.||77.2308||65||
Molecular Nature of Energy and Temperature (msu.edu) (3:34)
1. A 1m3 vessel contains 0.5m3 of saturated liquid in equilibrium with 0.5 m3 of saturated vapor. Which molecules are moving slower? (a) the vapor (b) the liquid (c) they are all the same.
2. A glass of ice water is sitting in your freezer, set to 0C and fully equilibrated. Which molecules are moving slower? (a) the gas (b) the liquid (c) the solid (d) they are all the same.
3. You walk into the kitchen in the morning to get some breakfast. The ceiling fan is on. You forgot your slippers. Which one is "hotter?" (a) the floor (b) the ceiling (c) the granite counter top (d) the air in the room (e) they are all the same.
|10.03 - Binary VLE using Raoult's Law||Click here.||73.3333||3||
Raoult's Law Calculation Procedures (11:45) (msu.edu)
Comprehension Questions: Assume the ideal solution SCVP model (Eqns. 2.47 and 10.8).
1. Estimate the bubble pressure (bars) of 30% acetone + 70% benzene at 333K.
|07.05 Cubic Equations of State||Click here.||73.3333||3||
Virial and Cubic EOS (11:18) (msu.edu)
1. To what region of pressure is the virial EOS limited at a given temperature? Why?
|13.04 - UNIQUAC||Click here.||73.3333||3||
UNIQUAC concepts (6:44) (msu.edu)
Concepts and assumptions used in developing the UNIQUAC activity coefficient method. This method introduced the use of surface area as an important quantity in calculation of activity coefficients.
|08.02 - The Internal Energy Departure Function||Click here.||73.3333||3||
The Internal Energy Departure Function (11min, uakron.edu) Deriving departure functions for a variety of equations of state is simplified by transforming to dimensionless units and using density instead of volume. This also leads to an extra simplification for the internal energy departure function.
1. What is the value of T(∂P/∂T)V - P for an ideal gas?
|04.02 The Microscopic View of Entropy||Click here.||72||5||
Principles of Probability III, Distributions, Normalizing, Distribution Functions, Moments, Variance. This screencast extends beyond material covered in the textbook, but may be helpful if you study statistical mechanics in another course. (msu.edu, 15min) (Flash)
|12.01 - The van der Waals Perspective for Mixtures||Click here.||70||4||
Mixing Rules (7:23) (msu.edu)
How should energy depend on composition? Should it be linear or non-linear? What does the van der Waals approach tell us about composition dependence? This screencasts shows that the mixing rule for 'a' in a random mixture should be quadratic. A linear mixing rule is usually used for the van der Waals size parameter.
|12.02 - The van Laar Model||Click here.||70||6||
The van Laar Equation (5:54) (msu.edu)
The van Laar equation uses the random mixing rules discussed in Section 12.1 with the internal energy to approximate the excess Gibbs Energy. What we learn is that it is possible to develop models using fundamental principles. Though this model is not used widely in process simulators, it provides a stepping stone to more advanced models.