CHEM 340--Physical Chemistry I

(designed for Biochemistry Majors,

fulfills BS Biochem and BA Chem degree)

Department of Chemistry

University of Illinois at Chicago

 

Fall 2013, LC C3, 2-3 PM M-W-F + 3-4 F (Problem solving, quiz, exams)

 

Lecturer: Tim Keiderling

Office: 5407 B SES, Tele: 996-3156

Best to contact by e-mail: tak@uic.edu

Keiderling group web site link – find out what we do outside of class! (out of date, tells research interests): http://www.chem.uic.edu/takgroup/

Office Hours: after Class, 3à??? (5407 SES, time variable, depends on demand), M & W (not Friday) or any other time by appointment

(Co-instructor lecturer: Dr. Frank Vasquez, 4346 SES, fxv@uic.edu)

                  Office hours: M-W , 1-2 PM

Graders – Teaching Assistants:­­­­­­­­­­­­­­­­­­­­­­­­­­­­­­­­­­­­­­­­ Yue Wei, ywei20@uic.edu and Weiying Zhu, wzhu3@uic.edu, 4340 SES, Anjan Roy, aroy6@uic.edu, 4344 SES, and Xiaohan Liu, xliu98@uic.edu -- they will grade problem sets, tests and quizzes and aid Dr. Vasquez with problem solving

         Office Hours: Wed 11-12 am, Thurs 10 am to 1 pm, Fri 11-12 am – normally meet in 4342 SES to work problems

(Note --these hours are chosen to fit normal homework due date and aid in preparation for quizzes which will be given on Fridays. Times and names may change depending on student and TA availability, graders will share the office hours and change emphases during the semester). If you have a conflict, they will see you by appointment (e-mail), but please do not “drop-in” at outside times.

 

FINAL EXAM: in finals week – according to university schedule (1^st list) – 1-3PM, Wed, Dec. 11, 2013

Hour exams: 2 in class period, 2PM, dates set: Fri. Oct 4 and Fri. Nov. 8, 2013,

         each will allow you to stay until 3:50PM 

         --Note these hour exams will be held in BSB 250 !!

 

Prerequisites: Chem 114 or 118, Phys 107 or 142. Math 181, with Grade C or better, students not meeting these will be dropped

 

Warning—this course site is for information transfer for the course. It changes and is updated regularly

Mostly it is useful for lecture notes, problem sets and solutions and handouts, and is always under construction, all will be new, since I have not taught Chem 340 for a long time, there is no old material to post!!

--returning to it for periodic review, rather than printing any page, is suggested

---

Syllabus

List of Topics with textbook correlation

 

Homework : Set#1, Set#2, Set#3, Set#4, Set#5, Set #6, Set#7, Set #8, Set#9, Set #10, Set#11, Set#12,

         Note; problems will come from text and other sources, not necessary to buy, but you must have access to text- colors will change when updated for Fall 2013

Solutions: Set#1, Set#2, Set#3, Set#4, Set#5, Set#6, Set#7, Set#8, Set#9, Set#10, Set#11, Set#12,

 

Quizzes: Quiz1, Quiz2, Quiz3, Quiz4, Quiz5, Quiz6

 

Old Exams (I will try to find some examples, but they will be very old) –

HourExam #1, 2 from 80’s

HourExam # 2, 2 from 80’s

Hour Exam #3 – from Chem 342 – old optional, hopefully not happen!!

FinalExam, 1 from 80’s (recall, just 1 quarter, not semester!)

Fall 2013 Exams: 1^st Hour, 2^nd Hour 3^rd Hour (?) plus: Exam supplemental equations-2013 - 2^nd Exam supplement Equations – Final exam equation sheet

Solutions: Exam1, Exam2 Exam3

Review Summary-old - Exam 1

Review Summary-old - Exam 2

Review Summary-old - Exam 3

Links to other Physical Chem Sites (note may be upgraded as course moves on__________________)

 Math and Mechanics review chapter (coming_________________)

Thermochem tables from a text

 

Lecture Notes

Periodically I will make pdf versions of my lecture notes available. These will be often updated after the class period due to constraints of constructing readable versions. Consequently sometimes they will not be available before class, so show up and take notes..

NOTE: these topics may move about as we try to find the best presentation for you.

1.   Introduction: Math, gases, physics, energy

a.   Notes 1 – Introduction

b.   Notes 2 – Thermodynamic Concepts, 0^th Law, gas laws, Temperature equilibrium

                                              i.     Partial pressure example

                                           ii.     van der Waals example

2.   Heat, work and First Law:

a.   Notes 3 – heat and work – 1^st law, Energy and Enthalpy, Heat Capacity

                                              i.     Heat example

                                           ii.     Work-heat example

                                         iii.     Heat capacity vs. T

                                          iv.     Inexact differential

                                            v.     Reverse vs. Irreverse process

                                          vi.     Reversible isothermal and adiabatic

b.   Notes 4 – State Functions – properties, mathematics

c.    Notes 5 – Thermo chemistry

                                              i.       Thermochemistry problem examples

                                           ii.       

3.   Second and Third Law

a.   Notes 6 – Second law

                                              i.     Carnot example

                                           ii.     Irreversible process

                                         iii.     Entropy Lecture ex. #1 - reversible

                                          iv.     Entropy Lecture ex. #2 – state change

                                            v.     Entropy Lecture ex.#3 – gas expand

                                          vi.     Entropy Lecture ex.#4 – Liquid pressure

                                       vii.     Entropy Lecture ex.#5 – Rev-Irrev cycles

                                     viii.     Entropy Lecture ex.#6 – Phase changes

                                          ix.     Entropy Lecture ex.#7 -  mixing

                                            x.     Entropy disorder, third law example

                                          xi.     Entropy interpretation review

b.   Notes 7 – Free Energy

                                              i.     Engel example – collagen stretch DA

                                           ii.     Engel example – collagen stretch DG

                                         iii.     Free energy problems

                                          iv.     Review-old Free energy-entropy

                                            v.     Comments – Gibbs-Helmholtz

                                          vi.     Sources –fundamental equations

                                       vii.     Sources - Maxwell relations

                                     viii.     Summary Fundamental equ., Maxwell, Chemical potential

c.    Notes 8 – gas mixtures, equilibria (skip ahead in text)

                                              i.      Examples from Engel Ch. 6

                                           ii.     Gibbs equations review

                                         iii.     Gas phase reaction equilibria examples

4.   Systems and change (return to order)

a.   Notes 9 - Phase equilibria

                                              i.     Phase diagram properties

                                           ii.     Phase rule

                                         iii.     Clausius Clapeyron examples

                                          iv.     Engel Clausius Clapeyron example (2^nd sheet)

b.   Notes 10 – ideal and real solutions

                                              i.     Engel tie-line lever-rule example

                                           ii.     Engel Osmosis extrapolation

                                         iii.     Colligative properties review equations

                                          iv.     Colligative properties examples

5.   Equilibria

a.   Notes 11 – solution reaction equilibria

                                              i.     Solution reaction activity examples

                                           ii.     Ion activity table and examples

                                         iii.     Ion solution concentrations – Tinoco 4.7.1

                                          iv.     Ion solution concentrations – Tinoco 4.8.2

                                            v.     Ion solution concentrations – Tinoco 4.9.3

                                          vi.     Ion solution concentrations – Tinoco 4.10.4

                                       vii.     Ion solution concentrations – Tinoco 4.11.5

b.     Notes 12

                                               i.     Electrochemical cell examples

                                           ii.     Engel examples: Donnan, Biochem std, Biochem tables

6.     Biochemical applications

a.     Notes 13 – Biochemical energetics (Engel Ch.10)

                                               i.     Tinoco Glucose-pyruvate metabolism

                                             ii.      

b.     Notes 14 - Review