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|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.
|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?
|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.
|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.
|06.1 The Fundamental Property Relation||Click here.||70||2||
From the physical world to the realm of mathematics (uakron.edu, 15min) In Unit I, students develop the skills to infer simplified energy and entropy balances for various physical situations. In order to facilitate that approach for applications involving chemicals other than steam and ideal gases, we need to transform that approach into a realm of pure mathematics. In this context it suffices to apply the energy and entropy balance of a very simple system (piston/cylinder) then focus on the state functions that are involved (U,H,S,...). The mathematical realm is relatively abstract, but it is ideally suited for the generalizations required to extend our principles from steam and ideal gases to any chemical.
1. In example 4.16, we noted that the estimated work to compress steam was less when treated with the steam tables than when treated as an ideal gas. Explain why while referring to the molecular perspective.
2. In Chapter 5, we noted that the temperature drops when dropping the pressure across a valve when treating steam or a refrigerant with thermodynamic tables, but the energy balance suggests that the temperature drop for an ideal gas should be zero. Explain how these two apparently contradictory observations can both be true while referring to the molecular perspective.
3. What is the relation of the state variable dU to the state variables S and V according to the fundamental property relation?
4. What is the relation of the state variable dH to the state variables S and P according to the fundamental property relation?
5. What is the significance of writing changes of state variables in terms of changes in other state variables?
6. Why is the compressibility factor (Z=PV/RT) less than one sometimes?
7. Is it possible for Z to be greater than one? Explain.
8. What is the significance of having a relation for P = P(V,T)? How will that help us to solve problems involving chemicals other than steam and ideal gases?
|11.13 - Osmotic Pressure||Click here.||70||2||
MW of protein by osmotic pressure - (8:23) (learncheme.com)
An application of osmotic pressure measurement to determine MW of a protein.