Homework 1, due Friday 10 January.
H1 Solve the following equations on your calculator. Some of these equations have multiple solutions:
find all of them. First solve each case graphically e.g. by plotting the relevant equation on your calculator
and find
Phase Equilibrium: Fugacity and Equilibrium Calculations (FEC)
Phase Equilibrium: Fugacity and Equilibrium Calculations
Relate the fugacity and the chemical potential (or the partial molar Gibbs free energy)
Use the fugacity coefficient to calculate the v
Phase Equilibrium: Conditions for Equilibrium (CfE)
Phase Diagrams: Conditions for Equilibrium (CfE)
Write down the conditions for equilibrium for: a pure single phase system, a pure
multi-phase system, and a multi-phase mixture
Explain how energetic an
Equations of State (EoS)
Equations of State
From molecular considerations, identify which intermolecular interactions are
significant (including estimating relative strengths of dipole moments, polarizability,
etc.)
Apply simple rules for calculating P,
The Second Law of Thermodynamics (SL)
Entropy and The Second Law of Thermodynamics
Explain and manipulate the second law
State and illustrate by example the second law of thermodynamics
Write both the integral and differential forms of the second law
Iden
The First Law of Thermodynamics (FL)
The First Law of Thermodynamics
Explain and manipulate the first law
Write the integral and differential forms of the first law
Describe the physical meaning of each of the terms within both the integral and
differe
Thermodynamic Properties (TP)
Thermodynamic Properties
Define and articulate some of the critical language and concepts of Thermodynamics
Distinguish between the universe, system, surroundings, and boundary
Define open system, closed system, and isolated
Laura Fulton
PeopleSoft #: 3836294
Lab Instructor: Dong Wang
Time of Class: Grabowski MWF 4-4:50pm
Lab time: Thursday 8-11:50am
Pre-lab Assignment
1.) Lab Notes were read, goals of the lab were identified, and important
procedural parts in the instruction
Laura Fulton
PeopleSoft #: 3836294
Lab Instructor: Mr. Walters
Time of Class: Mough MWF 3-3:50pm
Lab time: Tuesday 6-9:50 pm
Pre-lab #6 Assignment
1. One important goal of Part B is to determine which liquid - I2 in water or I2 in
kerosene is more soluble
Laura Fulton
PeopleSoft #: 3836294
Lab Instructor: Dong Wang
Time of Class: Grabowski MWF 4-4:50pm
Lab time: Thursday 8-11:50am
Pre-lab Experiment #7
1.) The principal goals of this experiment are: determining the limiting reactant
of the magnesium metal
CHE 0200 - CHEMICAL ENGINEERING TI-IERMODYNAMICS
Spring 2016
Assiggment N0. 2 Due: Wednesday, January 203 2016
1. Read Chapters 1 and 2 of Engjgeering and Chemical Thermodynamics by
Milo Koretsky.
2. Work problems: 1.23, 1.28, 1.30, 1.36, 2.7, 2.19 and 2.
CHE 0200 - CHEMICAL ENGINEERING THERMODYNAMICS
Spring 2016
Assiggment No. 3 Due: Monday, Januatjy 25 a 2016
1. Re-read Chapter 2 of EggLneering and Chemical Thermodynamics by
Milo Koretsky.
2. Work problems: 2.20, 2.25, 2.37, 2.42 and 2.44. 2.28 The n
CHE 0200 — CHEMICAL ENGINEERING THERMODYNAMICS
Spring 2016
Assignment N0. 4 Due: Monday, February 1, 2016
1. Re—read Chapter 2 and Read Chapter 3 of Engineering and Chemical
Thermodmamics by Milo Koretsky.
2. - Work problems: 2.46, 2.53, 2.59, 2.63, 2.66,
Chemical Reaction Equilibrium (CRE)
Chemical Reaction Equilibrium
Explain the relationship between energy and entropy in reacting systems (i.e., show
why the Gibss Free Energy is still the proper state function for equilibirium)
Write balance chemical r
Course Outline and Outcomes
Thermodynamic Properties
Define and articulate some of the critical language and concepts of Thermodynamics
Distinguish between the universe, system, surroundings, and boundary [Ch 1.1-1.2]
Define open system, closed system, an
What if it is something other than water?
For water we have steam tables. How to get volume of other substances?
First find the critical point
If you are above criitcal temp, there is no
If you are below critical point, need to know if
Need
Use Antoine
Homework 4 due January 31
H26
(6)
Problem 2.48 (blue) / 2.73 (red). Argon is a monoatomic ideal gas so u =
3
RT . Hint:
2
It may prove more useful to express heat capacity values in units of R e.g. cv = 3.1R.
H27
(6)
Problem 2.12 (blue book) / 2.26 (red b
H18
(6+2) Problem 4.36 (blue book) / 4.48 (red book). First do this manually (calculate a and b for
acetylene and butane, use the mixing rules, find a and b for the mixture, then solve for v). Then repeat
using Aspen.
H19
(8)
Problem 4.37(blue book)/4.49
H53
(6)
For an irreversible adiabatic compression, prove that S univ > 0 . We have done such
logical reasoning exercises in class three times (isothermal irreversible expansion, isothermal irreversible
compression, adiabatic irreversible expansion). Here
H46 (10)
Problem 2.58 (bluebook)/2.83 (red book). Take k=1.4 for air. A schematic of the Pv or
PT diagram of a Carnot cycle will help you get started.
H47 (8)
One mole of air undergoes a Carnot refrigeration cycle. The hot reservoir is at room
temperature
H61 (3+6)
Problem 3.16 (blue book) / 3.32 (red book). Assume that nitrogen and oxygen have the
same cp and cv values (you will need this in part b). Hint: For part b, follow the procedure we used to find
the entropy of mixing.
H62
(6)
Problem 3.19 a-c. (b
H1
a.
b.
Calculate the reaction constant at 25C for the gas phase reactions
(4)
(2)
H2
The following gas phase reaction reaches equilibrium at 350 C and 3 bar
Assume ideal gas behavior.
a.
(6)
Find the equilibrium constant at 350 C and 3 bar.
b.
(6)
The s
H90
A mixture of three components A, B and C has the following properties
A
B
C
xi
0.3
0.01
0.69
gi/RT
2.1
2.3
0.5
G i /RT
a.
(2)
b.
(2)
0.95
-2.31
-0.13
Is this mixture non-ideal? Justify your answer.
Calculate the total free energy of the mixture g/RT.
H69 (5)
A supermarket has an unusual pricing scheme if you buy two kinds of fruits. The price of
a given fruit depends on what else you purchase. The table below shows what price you would pay if you
purchase the given number of fruits. Clearly, from the
CHE 0200 Chemical Engineering Thermodynamics
Sachin Velankar, Spring 2014, University of Pittsburgh
1. Review and PVT behavior of gases
1.1. Define types of properties and processes (e.g. extensive, state, reversible, isothermal,
adiabatic)
1.2. Perform m
ChE 200 Chemical Engineering Thermodynamics
Department of Chemical Engineering, University of Pittsburgh.
Spring 2014
Instructor
Sachin Velankar (Such-in Vey-lun-ker)
Room 1230 ; velankar@pitt.edu
Teaching assistants
Diana Lievano ; dml64@pitt.edu
Timings
Simple heat problems
Find out how much heat is released when
Block of metal is heated
Reaction occurs
Something melts or evaporates
Combination of the above
Inverted versions: how much mass ? What is final temperature?
Complex heat problems: equilib
Ok, preliminaries are done
We have learned basic definitions of state, equilibrium, process, etc.
We have learned basic how to use steam tables
Many other tables work in the same way
Lets now start with a topic that involves neither thermo nor dynamics
P
140106: Wake up quiz
A solution has 10% by weight of ethanol and 90% by weight of water. Find the mole % ethanol of the
solution. Find the volume % of ethanol of the solution. Densities: ethanol: 0.79 g/ml ; water 1.00 g/ml
basis :1 g mixture of ethanol a