MSE 360 Exam 1 Spring Points Total

Size: px
Start display at page:

Download "MSE 360 Exam 1 Spring Points Total"

Transcription

1 MSE 360 Exam 1 Spring Points otal Name(print) ID number No notes, books, or information stored in calculator memories may be used. he NCSU academic integrity policies apply to this exam. As such, by taking this exam you are implicitly agreeing with the statement: I have neither given nor received unauthorized aid on this test. All work must be written on these pages and turned in. o receive full or partial credit on numerical problems, you must show your calculations in step-by-step fashion. Units must be shown when applicable and plots must have labeled axes. Be sure that you read and answer all parts of each question. Constants, equations, and data are given at the end of the exam ) (3 Points Each-39 Points otal) Multiple Choice 1. See the figure on the right, which represents the Gibbs free energy along a reaction path for a single phase to transform from state 1 to state. he reaction kinetics can be expressed by A) rate C exp(-δg 1 /R), B) rate C exp(-δg /R). With increasing temperature and constant pressure, the Gibbs free energy of a single phase A) increase, B) decrease 3. he internal energy of a system consists of and 4. A regular solution will likely form an ordered atomic structure if: d.) Ω 0 b.) Ω > 0 c.) Ω < 0 5. From the Gibbs phase rule for a -component system, at constant pressure, within a -phase region of the equilibrium phase diagram: a.) and composition can be independently varied b.) choosing a fixes the equilibrium compositions c.) neither nor composition can be varied d.) phases cannot be in equilibrium 6. Concerning the vacancy concentration, and the equilibrium concentration of a dilute solute atom B where ΔH mix is >>0: a.) for both cases, entropy favors mixing, while enthalpy discourages mixing b.) for both cases, the equilibrium concentration is dependent c.) for both cases, enthalpy favors mixing d.) both a) and b) e.) both b) and c) 7 With increasing melting point, the activation enthalpy for diffusion generally becomes A. higher B. lower C. same 8. he Gibbs phase rule is written as P+F C+. his is valid under the following conditions A) Constant pressure 1

2 B) Constant temperature C) Binary alloy system D) Single element system E) Varying temperature and pressure F) Constant temprature and pressure 9. Which of the following is not an example of a high-diffusivity pathway: a.) Diffusion along Grain Boundaries b.) Diffusion along Dislocation Defects c.) Diffusion along Vacancy Defects d.) Diffusion along Free-Surfaces e.) All are High Diffusivity Pathways 10. Comparing the substitutional diffusion relative to the vacancy diffusion in a single element system: a.) Both have the same magnitude of diffusion flux b.) Both have the same diffusion coefficient c.) Both a) and b) 11. he mechanism of diffusion for a dilute solute atom of small atomic radius compared to the host material would be best described by: a.) Substitutional diffusion b.) Interstitial diffusion c.) Vacancy diffusion d.) all of the above 1 During a non-steady state diffusion, A. the concentration behavior does not change with time B. the concentration behavior changes with time C. the diffusion process can be described by Fick s Second Law D. both B and C 13. he driving force of the diffusion process is A. the gradient in Gibbs free energy B. the gradient in chemical composition C. the gradient in stress field D. the gradient in electrical field 14 (10 points): Estimate the change in equilibrium melting temperature of Cu caused by a change of pressure of 50 MPa. he molar volume of Cu is 8.0x10-6 m 3 for the liquid and 7.6x10-6 m 3 for the solid phase. ΔH m kj/mol, m 1085 C.

3 15 (6 points): Assuming B atom has a solubility of 0.1% at 400 C, and 0.8% at 900 C. What is its solubility at 700 C? 16 (1 points): See the Ag-Cu phase diagram. Draw schematically the Gibbs free energy curves of all phases at 900 C, 779 C, and 700 C. 3

4 17. (15 Points) Regular Solution Problem. a.) Write here, and explain the general meaning of (one sentence), the equation for the ideal entropy of mixing for a solution comprised of N A atoms of type A, and N B atoms of type B. b.) Calculate the ΔS mix (with units) for an ideal solution at 800K with X B 0.5. c.) Assume the enthalpy of mixing term exactly offsets the entropy of mixing term (in the expression for ΔG mix ) at a composition of X B 0.5 and temperature of 800K. Calculate the for ΔG mix at 500K. 18 (10 points). A 3 mm long Cu rod is welded to a 7 mm long Zn rod and the rod is heated to 400 C to allow diffusion to proceed. Draw schematically the phase/composition along the rod during the diffusion. 4

5 19 (5 points) he diffusion coefficient can be written as DD 0 exp(-q/r). What is the meaning of Q in terms of thermodynamics? Hint: ΔG ΔH - ΔS. 0 (8 points). For the carbonization of steel at 800 C, it takes hours to reach a C concentration of 0.4% at a depth of 100 µm. Assuming that the diffusion coefficient does not change with composition. If the carbonization time is increased to 6 hours, Calculate the depth at which the C concentration reaches 0.4%. Answer Key for 1-13: 1A, B, 3 Potential energy & kinetics energy, 4C, 5B, 6D, 7A, 8E, 9C, 10A, 11B, 1D, 13A 5

6 Constants and Equations N A 6.0 x 10 3 mole -1 k (or R) 8.6 x 10-5 ev/atom-k (or 8.31 J/mol K) K C nm 1 m 10 cm 1 m P + F C + P + F C + 1 G H S HU+PV du ds - PdV G X aga + X bgb ΔGmix H C p " C p d S d 0 dp d ΔH V 0 eq eqδ Δ ΔH m S m L m Δ G LΔ m ω conf ( N a N a + N b )!! N! b 1 "S mix #R(X a ln X a + X b ln X b ) Δ ε ε AB ( ε AA ε BB ) Ω zδε N a H mix ΩX a X b Δ "G mix "H mix # "S mix γvm γvm γvm Δ Gγ ΔPVm X r X exp X (1 + ) r Rr Rr ΔGv Qv nv exp N exp X e B Ae " Q R k k J number area time dc d C D dt dx dc J D dx x C(x,t) C s " #C erf (" Dt ) $ C C + " 0 sin #x ' % &! ( ) * exp +t, l [ ] where: τ π D Qd ΔS D D0 exp( ) D 1 d d 0 zν exp k 6 K 6

7 7

Introduction To Materials Science FOR ENGINEERS, Ch. 5. Diffusion. MSE 201 Callister Chapter 5

Introduction To Materials Science FOR ENGINEERS, Ch. 5. Diffusion. MSE 201 Callister Chapter 5 Diffusion MSE 201 Callister Chapter 5 1 Goals: Diffusion - how do atoms move through solids? Fundamental concepts and language Diffusion mechanisms Vacancy diffusion Interstitial diffusion Impurities Diffusion

More information

MATSCI 204 Thermodynamics and Phase Equilibria Winter Chapter #4 Practice problems

MATSCI 204 Thermodynamics and Phase Equilibria Winter Chapter #4 Practice problems MATSCI 204 Thermodynamics and Phase Equilibria Winter 2013 Chapter #4 Practice problems Problem: 1-Show that for any extensive property Ω of a binary system A-B: d ( "# ) "# B, = "# + 1$ x B 2- If "# has

More information

Extrinsic Point Defects: Impurities

Extrinsic Point Defects: Impurities Extrinsic Point Defects: Impurities Substitutional and interstitial impurities Sol solutions, solubility limit Entropy of ing, eal solution model Enthalpy of ing, quasi-chemical model Ideal and regular

More information

Exam 3 Solutions. ClO g. At 200 K and a total pressure of 1.0 bar, the partial pressure ratio for the chlorine-containing compounds is p ClO2

Exam 3 Solutions. ClO g. At 200 K and a total pressure of 1.0 bar, the partial pressure ratio for the chlorine-containing compounds is p ClO2 Chemistry 360 Dr. Jean M. Standard Fall 2016 Name KEY Exam 3 Solutions 1.) (14 points) Consider the gas phase decomposition of chlorine dioxide, ClO 2, ClO 2 ( g) ClO ( g) + O ( g). At 200 K and a total

More information

CHAPTER 4 IMPERFECTIONS IN SOLIDS PROBLEM SOLUTIONS

CHAPTER 4 IMPERFECTIONS IN SOLIDS PROBLEM SOLUTIONS 4-1 CHAPTER 4 IMPERFECTIONS IN SOLIDS PROBLEM SOLUTIONS Vacancies and Self-Interstitials 4.1 In order to compute the fraction of atom sites that are vacant in copper at 1357 K, we must employ Equation

More information

OCN 623: Thermodynamic Laws & Gibbs Free Energy. or how to predict chemical reactions without doing experiments

OCN 623: Thermodynamic Laws & Gibbs Free Energy. or how to predict chemical reactions without doing experiments OCN 623: Thermodynamic Laws & Gibbs Free Energy or how to predict chemical reactions without doing experiments Definitions Extensive properties Depend on the amount of material e.g. # of moles, mass or

More information

Lecture 20. Chemical Potential

Lecture 20. Chemical Potential Lecture 20 Chemical Potential Reading: Lecture 20, today: Chapter 10, sections A and B Lecture 21, Wednesday: Chapter 10: 10 17 end 3/21/16 1 Pop Question 7 Boltzmann Distribution Two systems with lowest

More information

Unit 5: Spontaneity of Reaction. You need to bring your textbooks everyday of this unit.

Unit 5: Spontaneity of Reaction. You need to bring your textbooks everyday of this unit. Unit 5: Spontaneity of Reaction You need to bring your textbooks everyday of this unit. THE LAWS OF THERMODYNAMICS 1 st Law of Thermodynamics Energy is conserved ΔE = q + w 2 nd Law of Thermodynamics A

More information

Disorder and Entropy. Disorder and Entropy

Disorder and Entropy. Disorder and Entropy Disorder and Entropy Suppose I have 10 particles that can be in one of two states either the blue state or the red state. How many different ways can we arrange those particles among the states? All particles

More information

Chapter 19 Chemical Thermodynamics Entropy and free energy

Chapter 19 Chemical Thermodynamics Entropy and free energy Chapter 19 Chemical Thermodynamics Entropy and free energy Learning goals and key skills: Explain and apply the terms spontaneous process, reversible process, irreversible process, and isothermal process.

More information

Practice Examinations Chem 393 Fall 2005 Time 1 hr 15 min for each set.

Practice Examinations Chem 393 Fall 2005 Time 1 hr 15 min for each set. Practice Examinations Chem 393 Fall 2005 Time 1 hr 15 min for each set. The symbols used here are as discussed in the class. Use scratch paper as needed. Do not give more than one answer for any question.

More information

Gibbs Free Energy. Evaluating spontaneity

Gibbs Free Energy. Evaluating spontaneity Gibbs Free Energy Evaluating spontaneity Predicting Spontaneity An increase in entropy; Changing from a more structured to less structured physical state: Solid to liquid Liquid to gas Increase in temperature

More information

Chemistry and the material world Unit 4, Lecture 4 Matthias Lein

Chemistry and the material world Unit 4, Lecture 4 Matthias Lein Chemistry and the material world 123.102 Unit 4, Lecture 4 Matthias Lein Gibbs ree energy Gibbs ree energy to predict the direction o a chemical process. Exergonic and endergonic reactions. Temperature

More information

2) C 2 H 2 (g) + 2 H 2 (g) ---> C 2 H 6 (g) Information about the substances

2) C 2 H 2 (g) + 2 H 2 (g) ---> C 2 H 6 (g) Information about the substances Thermochemistry 1) 2 C 4 H 10 (g) + 13 O 2 (g) ------> 8 CO 2 (g) + 10 H 2 O(l) The reaction represented above is spontaneous at 25 C. Assume that all reactants and products are in their standard states.

More information

Last Name or Student ID

Last Name or Student ID 10/06/08, Chem433 Exam # 1 Last Name or Student ID 1. (3 pts) 2. (3 pts) 3. (3 pts) 4. (2 pts) 5. (2 pts) 6. (2 pts) 7. (2 pts) 8. (2 pts) 9. (6 pts) 10. (5 pts) 11. (6 pts) 12. (12 pts) 13. (22 pts) 14.

More information

Appendix 4. Appendix 4A Heat Capacity of Ideal Gases

Appendix 4. Appendix 4A Heat Capacity of Ideal Gases Appendix 4 W-143 Appendix 4A Heat Capacity of Ideal Gases We can determine the heat capacity from the energy content of materials as a function of temperature. The simplest material to model is an ideal

More information

MSE 3050: Thermodynamics and Kinetics of Materials

MSE 3050: Thermodynamics and Kinetics of Materials University of Virginia, Department of Materials Science and Engineering Spring 2019, Tuesday and Thursday, 9:30 10:45 am Mechanical Engineering Building 339 MSE 3050: Thermodynamics and Kinetics of Materials

More information

1 What is energy?

1 What is energy? http://www.intothecool.com/ 1 What is energy? the capacity to do work? (Greek: en-, in; + ergon, work) the capacity to cause change to produce an effect? a certain quantity that does not change in the

More information

The Laws of Thermodynamics

The Laws of Thermodynamics Entropy I. This, like enthalpy, Thus, II. A reaction is ( more on this later) if: (H, enthalpy) (S, entropy) III. IV. Why does entropy happen? Probability It s harder to keep things in order (look at my

More information

Chemical Thermodynamics. Chapter 18

Chemical Thermodynamics. Chapter 18 Chemical Thermodynamics Chapter 18 Thermodynamics Spontaneous Processes Entropy and Second Law of Thermodynamics Entropy Changes Gibbs Free Energy Free Energy and Temperature Free Energy and Equilibrium

More information

Concept of the chemical potential and the activity of elements

Concept of the chemical potential and the activity of elements Concept of the chemical potential and the activity of elements Gibb s free energy, G is function of temperature, T, pressure, P and amount of elements, n, n dg G G (T, P, n, n ) t particular temperature

More information

The underlying prerequisite to the application of thermodynamic principles to natural systems is that the system under consideration should be at equilibrium. http://eps.mcgill.ca/~courses/c220/ Reversible

More information

THERMODYNAMICS I. TERMS AND DEFINITIONS A. Review of Definitions 1. Thermodynamics = Study of the exchange of heat, energy and work between a system

THERMODYNAMICS I. TERMS AND DEFINITIONS A. Review of Definitions 1. Thermodynamics = Study of the exchange of heat, energy and work between a system THERMODYNAMICS I. TERMS AND DEFINITIONS A. Review of Definitions 1. Thermodynamics = Study of the exchange of heat, energy and work between a system and its surroundings. a. System = That part of universe

More information

Saturday Study Session 1 3 rd Class Student Handout Thermochemistry

Saturday Study Session 1 3 rd Class Student Handout Thermochemistry Saturday Study Session 1 3 rd Class Student Handout Thermochemistry Multiple Choice Identify the choice that best completes the statement or answers the question. 1. C 2 H 4 (g) + 3 O 2 (g) 2 CO 2 (g)

More information

UNIVERSITY OF SOUTHAMPTON

UNIVERSITY OF SOUTHAMPTON UNIVERSITY OF SOUTHAMPTON PHYS1013W1 SEMESTER 2 EXAMINATION 2014-2015 ENERGY AND MATTER Duration: 120 MINS (2 hours) This paper contains 8 questions. Answers to Section A and Section B must be in separate

More information

Chapter 6 Thermodynamic Properties of Fluids

Chapter 6 Thermodynamic Properties of Fluids Chapter 6 Thermodynamic Properties of Fluids Initial purpose in this chapter is to develop from the first and second laws the fundamental property relations which underlie the mathematical structure of

More information

Physical Chemistry I Exam points

Physical Chemistry I Exam points Chemistry 360 Fall 2018 Dr. Jean M. tandard October 17, 2018 Name Physical Chemistry I Exam 2 100 points Note: You must show your work on problems in order to receive full credit for any answers. You must

More information

The Second Law of Thermodynamics (Chapter 4)

The Second Law of Thermodynamics (Chapter 4) The Second Law of Thermodynamics (Chapter 4) First Law: Energy of universe is constant: ΔE system = - ΔE surroundings Second Law: New variable, S, entropy. Changes in S, ΔS, tell us which processes made

More information

For more info visit

For more info visit Basic Terminology: Terms System Open System Closed System Isolated system Surroundings Boundary State variables State Functions Intensive properties Extensive properties Process Isothermal process Isobaric

More information

Equations: q trans = 2 mkt h 2. , Q = q N, Q = qn N! , < P > = kt P = , C v = < E > V 2. e 1 e h /kt vib = h k = h k, rot = h2.

Equations: q trans = 2 mkt h 2. , Q = q N, Q = qn N! , < P > = kt P = , C v = < E > V 2. e 1 e h /kt vib = h k = h k, rot = h2. Constants: R = 8.314 J mol -1 K -1 = 0.08206 L atm mol -1 K -1 k B = 0.697 cm -1 /K = 1.38 x 10-23 J/K 1 a.m.u. = 1.672 x 10-27 kg 1 atm = 1.0133 x 10 5 Nm -2 = 760 Torr h = 6.626 x 10-34 Js For H 2 O

More information

Final Exam for Physics 176. Professor Greenside Wednesday, April 29, 2009

Final Exam for Physics 176. Professor Greenside Wednesday, April 29, 2009 Print your name clearly: Signature: I agree to neither give nor receive aid during this exam Final Exam for Physics 76 Professor Greenside Wednesday, April 29, 2009 This exam is closed book and will last

More information

Practice Midterm Exam 1 March, 2011

Practice Midterm Exam 1 March, 2011 NAME: MSE 508: Solid State Thermodynamics Department of Materials Science & Engineering Boise State University Spring 2011 Practice Midterm Exam 1 March, 2011 Problem Total Points Points Obtained 1. 2.

More information

CHEM 341 PHYSICAL CHEMISTRY FINAL EXAM. Name

CHEM 341 PHYSICAL CHEMISTRY FINAL EXAM. Name CHEM 341 PHYSICAL CHEMISTRY FINAL EXAM Name Do not open this exam until told to do so. The exam consists of 6 pages, including this one. Count them to insure that they are all there. Constants: R = 8.31

More information

3.012 PS 7 Thermo solutions Issued: Fall 2003 Graded problems due:

3.012 PS 7 Thermo solutions Issued: Fall 2003 Graded problems due: 3.012 PS 7 Thermo solutions 3.012 Issued: 11.17.03 Fall 2003 Graded problems due: 11.26.03 Graded problems: 1. Analysis of equilibrium phases with a binary phase diagram. Shown below is the phase diagram

More information

CHEMISTRY 102 FALL 2009 EXAM 2 FORM B SECTION 501 DR. KEENEY-KENNICUTT PART 1

CHEMISTRY 102 FALL 2009 EXAM 2 FORM B SECTION 501 DR. KEENEY-KENNICUTT PART 1 NAME CHEMISTRY 102 FALL 2009 EXAM 2 FORM B SECTION 501 DR. KEENEY-KENNICUTT Directions: (1) Put your name on PART 1 and your name and signature on PART 2 of the exam where indicated. (2) Sign the Aggie

More information

Collision Theory. Unit 12: Chapter 18. Reaction Rates. Activation Energy. Reversible Reactions. Reversible Reactions. Reaction Rates and Equilibrium

Collision Theory. Unit 12: Chapter 18. Reaction Rates. Activation Energy. Reversible Reactions. Reversible Reactions. Reaction Rates and Equilibrium Collision Theory For reactions to occur collisions between particles must have Unit 12: Chapter 18 Reaction Rates and Equilibrium the proper orientation enough kinetic energy See Both In Action 1 2 Activation

More information

Thermodynamics II. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.

Thermodynamics II. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Thermodynamics II Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Spontaneous Physical and Chemical Processes A waterfall runs downhill A lump of sugar dissolves

More information

Chapter 3: Energy and Work. Energy and Work, con t. BCH 4053 Spring 2003 Chapter 3 Lecture Notes. Slide 1. Slide 2

Chapter 3: Energy and Work. Energy and Work, con t. BCH 4053 Spring 2003 Chapter 3 Lecture Notes. Slide 1. Slide 2 BCH 4053 Spring 2003 Chapter 3 Lecture Notes 1 Chapter 3: Thermodynamics of Biological Systems 2 Energy and Work Work = force x distance Energy = ability to do work Mechanical Energy Kinetic Energy = mv

More information

Minority Carrier Diffusion Equation (MCDE)

Minority Carrier Diffusion Equation (MCDE) ECE-305: Spring 2015 Minority Carrier Diffusion Equation (MCDE) Professor Mark undstrom Electrical and Computer Engineering Purdue University, West afayette, IN USA lundstro@purdue.edu Pierret, Semiconductor

More information

Thermodynamics: A Brief Introduction. Thermodynamics: A Brief Introduction

Thermodynamics: A Brief Introduction. Thermodynamics: A Brief Introduction Brief review or introduction to Classical Thermodynamics Hopefully you remember this equation from chemistry. The Gibbs Free Energy (G) as related to enthalpy (H) and entropy (S) and temperature (T). Δ

More information

Ch 17 Free Energy and Thermodynamics - Spontaneity of Reaction

Ch 17 Free Energy and Thermodynamics - Spontaneity of Reaction Ch 17 Free Energy and Thermodynamics - Spontaneity of Reaction Modified by Dr. Cheng-Yu Lai spontaneous nonspontaneous Spontaneous Processes Processes that are spontaneous in one direction are nonspontaneous

More information

Entropy, Free Energy, and Equilibrium

Entropy, Free Energy, and Equilibrium Entropy, Free Energy, and Equilibrium Chapter 17 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Spontaneous Physical and Chemical Processes A waterfall runs

More information

Diffusion in Dilute Alloys

Diffusion in Dilute Alloys Chapter 3 Diffusion in Dilute Alloys Our discussion of the atomistic mechanisms for diffusion has been confined to the situations where the diffusing species is chemically identical to the host atom. We

More information

Chapter Eighteen. Thermodynamics

Chapter Eighteen. Thermodynamics Chapter Eighteen Thermodynamics 1 Thermodynamics Study of energy changes during observed processes Purpose: To predict spontaneity of a process Spontaneity: Will process go without assistance? Depends

More information

Chemical reaction equilibria

Chemical reaction equilibria Chemical reaction equilibria Chemical reaction equilibria in metallurgical processes and the conditions that maintain equilibrium are important to obtain maximum efficiency from production processes For

More information

Chemical Equilibrium. Chapter 8

Chemical Equilibrium. Chapter 8 Chemical Equilibrium Chapter 8 Equilibrium is a state in which there are no observable changes as time goes by. Chemical equilibrium is achieved when: the rates of the forward and reverse reactions are

More information

MS212 Thermodynamics of Materials ( 소재열역학의이해 ) Lecture Note: Chapter 7

MS212 Thermodynamics of Materials ( 소재열역학의이해 ) Lecture Note: Chapter 7 2017 Spring Semester MS212 Thermodynamics of Materials ( 소재열역학의이해 ) Lecture Note: Chapter 7 Byungha Shin ( 신병하 ) Dept. of MSE, KAIST Largely based on lecture notes of Prof. Hyuck-Mo Lee and Prof. WooChul

More information

( 7) ( 9) ( 8) Applying Thermo: an Example of Kinetics - Diffusion. Applying Thermo: an Example of Kinetics - Diffusion. dw = F dr = dr (6) r

( 7) ( 9) ( 8) Applying Thermo: an Example of Kinetics - Diffusion. Applying Thermo: an Example of Kinetics - Diffusion. dw = F dr = dr (6) r Fundamental Phyic of Force and Energy/Work: Energy and Work: o In general: o The work i given by: dw = F dr (5) (One can argue that Eqn. 4 and 5 are really one in the ame.) o Work or Energy are calar potential

More information

Phase Transformation of Materials

Phase Transformation of Materials 2009 fall Phase Transformation of Materials 09.08.2009 Eun Soo Park Office: 33-316 Telephone: 880-7221 Email: espark@snu.ac.kr Office hours: by an appointment 1 Contents for previous class Chapter 1 -

More information

3.012 PS 7 3.012 Issued: 11.05.04 Fall 2004 Due: 11.12.04 THERMODYNAMICS 1. single-component phase diagrams. Shown below is a hypothetical phase diagram for a single-component closed system. Answer the

More information

Chapter 19 Chemical Thermodynamics

Chapter 19 Chemical Thermodynamics Chapter 19 Chemical Thermodynamics Spontaneous Processes Entropy and the Second Law of Thermodynamics The Molecular Interpretation of Entropy Entropy Changes in Chemical Reactions Gibbs Free Energy Free

More information

ASSIGNMENT SHEET #11 APQ ANSWERS

ASSIGNMENT SHEET #11 APQ ANSWERS ASSIGNMENT SHEET #11 APQ ANSWERS #1 a. The unit for q must be an energy unit, typically Joules or calories. The unit for mass is the gram. The unit for specific heat is J per gram-degree or calorie per

More information

School of Chemical & Biological Engineering, Konkuk University

School of Chemical & Biological Engineering, Konkuk University School of Chemical & iological Engineering, Konkuk University Lecture 7 Ch. 5 Simple Mixtures Colligative properties Prof. Yo-Sep Min Physical Chemistry I, Spring 2009 Ch. 5-2 he presence of a solute in

More information

THERMODYNAMICS. Dr. Sapna Gupta

THERMODYNAMICS. Dr. Sapna Gupta THERMODYNAMICS Dr. Sapna Gupta FIRST LAW OF THERMODYNAMICS Thermodynamics is the study of heat and other forms of energy involved in chemical or physical processes. First Law of Thermodynamics Energy cannot

More information

BAE 820 Physical Principles of Environmental Systems

BAE 820 Physical Principles of Environmental Systems BAE 820 Physical Principles of Environmental Systems Estimation of diffusion Coefficient Dr. Zifei Liu Diffusion mass transfer Diffusion mass transfer refers to mass in transit due to a species concentration

More information

UNIVERSITY OF SOUTHAMPTON VERY IMPORTANT NOTE. Section A answers MUST BE in a separate blue answer book. If any blue

UNIVERSITY OF SOUTHAMPTON VERY IMPORTANT NOTE. Section A answers MUST BE in a separate blue answer book. If any blue UNIVERSITY OF SOUTHAMPTON PHYS1013W1 SEMESTER 2 EXAMINATION 2011/12 ENERGY AND MATTER SOLUTIONS Duration: 120 MINS VERY IMPORTANT NOTE Section A answers MUST BE in a separate blue answer book. If any blue

More information

MME 2010 METALLURGICAL THERMODYNAMICS II. Partial Properties of Solutions

MME 2010 METALLURGICAL THERMODYNAMICS II. Partial Properties of Solutions MME 2010 METALLURGICAL THERMODYNAMICS II Partial Properties of Solutions A total property of a system consisting of multiple substances is represented as nm = n i M i If the system consists of a liquid

More information

Lecture 1: Atomic Diffusion

Lecture 1: Atomic Diffusion Part IB Materials Science & Metallurgy H. K. D. H. Bhadeshia Course A, Metals and Alloys Lecture 1: Atomic Diffusion Mass transport in a gas or liquid generally involves the flow of fluid (e.g. convection

More information

du = δq + δw = δq rev + δw rev = δq rev + 0

du = δq + δw = δq rev + δw rev = δq rev + 0 Chem 4501 Introduction to hermodynamics, 3 Credits Kinetics, and Statistical Mechanics Module Number 6 Active Learning Answers and Optional Problems/Solutions 1. McQuarrie and Simon, 6-6. Paraphrase: Compute

More information

General Chemistry revisited

General Chemistry revisited General Chemistry revisited A(g) + B(g) C(g) + D(g) We said that G = H TS where, eg, H = f H(C) + f H(D) - f H(A) - f H(B) G < 0 implied spontaneous to right G > 0 implied spontaneous to left In a very

More information

Chem 112 Dr. Kevin Moore

Chem 112 Dr. Kevin Moore Chem 112 Dr. Kevin Moore Gas Liquid Solid Polar Covalent Bond Partial Separation of Charge Electronegativity: H 2.1 Cl 3.0 H Cl δ + δ - Dipole Moment measure of the net polarity in a molecule Q Q magnitude

More information

Chapter 8 Thermochemistry: Chemical Energy

Chapter 8 Thermochemistry: Chemical Energy Chapter 8 Thermochemistry: Chemical Energy 國防醫學院生化學科王明芳老師 2011-11-8 & 2011-11-15 Chapter 8/1 Energy and Its Conservation Conservation of Energy Law: Energy cannot be created or destroyed; it can only be

More information

3.20 Exam 1 Fall 2003 SOLUTIONS

3.20 Exam 1 Fall 2003 SOLUTIONS 3.0 Exam 1 Fall 003 SOLUIONS Question 1 You need to decide whether to work at constant volume or constant pressure. Since F is given, a natural choice is constant volume. Option 1: At constant and V :

More information

Chemistry 1A, Spring 2007 Midterm Exam 3 April 9, 2007 (90 min, closed book)

Chemistry 1A, Spring 2007 Midterm Exam 3 April 9, 2007 (90 min, closed book) Chemistry 1A, Spring 2007 Midterm Exam 3 April 9, 2007 (90 min, closed book) Name: KEY SID: TA Name: 1.) Write your name on every page of this exam. 2.) This exam has 34 multiple choice questions. Fill

More information

Chapter 17: Energy and Kinetics

Chapter 17: Energy and Kinetics Pages 510-547 S K K Chapter 17: Energy and Kinetics Thermochemistry: Causes of change in systems Kinetics: Rate of reaction progress (speed) Heat, Energy, and Temperature changes S J J Heat vs Temperature

More information

ln( P vap(s) / torr) = T / K ln( P vap(l) / torr) = T / K

ln( P vap(s) / torr) = T / K ln( P vap(l) / torr) = T / K Chem 4501 Introduction to Thermodynamics, 3 Credits Kinetics, and Statistical Mechanics Fall Semester 2017 Homework Problem Set Number 9 Solutions 1. McQuarrie and Simon, 9-4. Paraphrase: Given expressions

More information

Chapter 5. Simple Mixtures Fall Semester Physical Chemistry 1 (CHM2201)

Chapter 5. Simple Mixtures Fall Semester Physical Chemistry 1 (CHM2201) Chapter 5. Simple Mixtures 2011 Fall Semester Physical Chemistry 1 (CHM2201) Contents The thermodynamic description of mixtures 5.1 Partial molar quantities 5.2 The thermodynamic of Mixing 5.3 The chemical

More information

A proposed mechanism for the decomposition of hydrogen peroxide by iodide ion is: slow fast (D) H 2 O

A proposed mechanism for the decomposition of hydrogen peroxide by iodide ion is: slow fast (D) H 2 O Chemistry 112, Spring 2007 Prof. Metz Exam 2 Practice Use the following information to answer questions 1 through 3 A proposed mechanism for the decomposition of hydrogen peroxide by iodide ion is: H 2

More information

Homework Problem Set 8 Solutions

Homework Problem Set 8 Solutions Chemistry 360 Dr. Jean M. Standard Homework roblem Set 8 Solutions. Starting from G = H S, derive the fundamental equation for G. o begin, we take the differential of G, dg = dh d( S) = dh ds Sd. Next,

More information

Chapter 19 Chemical Thermodynamics

Chapter 19 Chemical Thermodynamics Chapter 19 Chemical Thermodynamics Kinetics How fast a rxn. proceeds Equilibrium How far a rxn proceeds towards completion Thermodynamics Study of energy relationships & changes which occur during chemical

More information

Chapter 19 Chemical Thermodynamics Entropy and free energy

Chapter 19 Chemical Thermodynamics Entropy and free energy Chapter 19 Chemical Thermodynamics Entropy and free energy Learning goals and key skills: Understand the meaning of spontaneous process, reversible process, irreversible process, and isothermal process.

More information

Kinetics. Rate of change in response to thermodynamic forces

Kinetics. Rate of change in response to thermodynamic forces Kinetics Rate of change in response to thermodynamic forces Deviation from local equilibrium continuous change T heat flow temperature changes µ atom flow composition changes Deviation from global equilibrium

More information

Chem 401 Unit 1 (Kinetics & Thermo) Review

Chem 401 Unit 1 (Kinetics & Thermo) Review KINETICS 1. For the equation 2 H 2(g) + O 2(g) 2 H 2 O (g) How is the rate of formation of H 2 O mathematically related to the rate of disappearance of O 2? 2. Determine the relative reaction rates of

More information

Thermal and Statistical Physics Department Exam Last updated November 4, L π

Thermal and Statistical Physics Department Exam Last updated November 4, L π Thermal and Statistical Physics Department Exam Last updated November 4, 013 1. a. Define the chemical potential µ. Show that two systems are in diffusive equilibrium if µ 1 =µ. You may start with F =

More information

10, Physical Chemistry- III (Classical Thermodynamics, Non-Equilibrium Thermodynamics, Surface chemistry, Fast kinetics)

10, Physical Chemistry- III (Classical Thermodynamics, Non-Equilibrium Thermodynamics, Surface chemistry, Fast kinetics) Subect Chemistry Paper No and Title Module No and Title Module Tag 0, Physical Chemistry- III (Classical Thermodynamics, Non-Equilibrium Thermodynamics, Surface chemistry, Fast kinetics) 0, Free energy

More information

Physics 360 Review 3

Physics 360 Review 3 Physics 360 Review 3 The test will be similar to the second test in that calculators will not be allowed and that the Unit #2 material will be divided into three different parts. There will be one problem

More information

Thermochemistry: the study of energy (in the from of heat) changes that accompany physical & chemical changes

Thermochemistry: the study of energy (in the from of heat) changes that accompany physical & chemical changes Thermochemistry Thermochemistry: the study of energy (in the from of heat) changes that accompany physical & chemical changes heat flows from high to low (hot cool) endothermic reactions: absorb energy

More information

EMA4303/5305 Electrochemical Engineering Lecture 02 Equilibrium Electrochemistry

EMA4303/5305 Electrochemical Engineering Lecture 02 Equilibrium Electrochemistry EMA4303/5305 Electrochemical Engineering Lecture 02 Equilibrium Electrochemistry Dr. Junheng Xing, Prof. Zhe Cheng Mechanical & Materials Engineering Florida International University 2 Equilibrium Electrochemistry

More information

MECH6661 lectures 6/1 Dr. M. Medraj Mech. Eng. Dept. - Concordia University. Fe3C (cementite)

MECH6661 lectures 6/1 Dr. M. Medraj Mech. Eng. Dept. - Concordia University. Fe3C (cementite) Outline Solid solution Gibbs free energy of binary solutions Ideal solution Chemical potential of an ideal solution Regular solutions Activity of a component Real solutions Equilibrium in heterogeneous

More information

MCB100A/Chem130 MidTerm Exam 2 April 4, 2013

MCB100A/Chem130 MidTerm Exam 2 April 4, 2013 MCB1A/Chem13 MidTerm Exam 2 April 4, 213 Name Student ID True/False (2 points each). 1. The Boltzmann constant, k b T sets the energy scale for observing energy microstates 2. Atoms with favorable electronic

More information

The Equilibrium State

The Equilibrium State Materials Science & Metallurgy Part III Course M16 Computation of Phase Diagrams (Revision) H. K. D. H. Bhadeshia The Equilibrium State Equilibrium is a state in which no further change is perceptible,

More information

Name: Math 1120, Final. December 12, Net id: PLACE AN X IN THE BOX TO INDICATE YOUR SECTION

Name: Math 1120, Final. December 12, Net id: PLACE AN X IN THE BOX TO INDICATE YOUR SECTION Math 1120, Final December 12, 2017 Name: Net id: PLACE AN X IN THE BOX TO INDICATE YOUR SECTION Ian Lizarraga MWF 8:00 8:50 Ian Lizarraga MWF 9:05 9:55 Swee Hong Chan MWF 12:20 1:10 Teddy Einstein MWF

More information

CH 223 Sample Exam Exam II Name: Lab Section:

CH 223 Sample Exam Exam II Name: Lab Section: Exam II Name: Lab Section: Part I: Multiple Choice Questions (100 Points) Use a scantron sheet for Part I. There is only one best answer for each question. 1. Which of the following equations is the solubility

More information

CHEMISTRY 107 Section 501 Exam #3 Version A November 16, 2016 Dr. Larry Brown

CHEMISTRY 107 Section 501 Exam #3 Version A November 16, 2016 Dr. Larry Brown NAME: (print) UIN #: CHEMISTRY 107 Section 501 Exam #3 Version A November 16, 2016 Dr. Larry Brown This is a 50-minute exam, and contains 7 problems. There should be 10 numbered pages, including this one.

More information

b. The Arrhenius equation relates the rate constant k of a reaction to its activation energy Ea and the surrounding temperature T:

b. The Arrhenius equation relates the rate constant k of a reaction to its activation energy Ea and the surrounding temperature T: Question 1 Kinetic and thermodynamic reaction control can decide what the major product of a reaction would be for a given set of conditions. The following scenario illustrates this topic. Molecule A can

More information

concentrations (molarity) rate constant, (k), depends on size, speed, kind of molecule, temperature, etc.

concentrations (molarity) rate constant, (k), depends on size, speed, kind of molecule, temperature, etc. #80 Notes Ch. 12, 13, 16, 17 Rates, Equilibriums, Energies Ch. 12 I. Reaction Rates NO 2(g) + CO (g) NO (g) + CO 2(g) Rate is defined in terms of the rate of disappearance of one of the reactants, but

More information

Chapter 17: Spontaneity, Entropy, and Free Energy

Chapter 17: Spontaneity, Entropy, and Free Energy Chapter 17: Spontaneity, Entropy, and Free Energy Review of Chemical Thermodynamics System: the matter of interest Surroundings: everything in the universe which is not part of the system Closed System:

More information

plane in a cubic unit cell. Clearly label the axes. (b) Draw two directions in the ( 112)

plane in a cubic unit cell. Clearly label the axes. (b) Draw two directions in the ( 112) Midterm Examination - Thursday, February 5, 8:00 9:5 AM Place all answers in a 8.5" x " Bluebook Allowed:, double-sided 8.5" x " page of notes must return with exam. Required: Picture ID when returning

More information

Dr. White Chem 1B Saddleback College 1. Experiment 15 Thermodynamics of the Solution Process

Dr. White Chem 1B Saddleback College 1. Experiment 15 Thermodynamics of the Solution Process Dr. White Chem 1B Saddleback College 1 Experiment 15 Thermodynamics of the Solution Process Objectives To learn about the relationship between K and ΔG. To learn how the van't Hoff equation can be used

More information

Physics is time symmetric Nature is not

Physics is time symmetric Nature is not Fundamental theories of physics don t depend on the direction of time Newtonian Physics Electromagnetism Relativity Quantum Mechanics Physics is time symmetric Nature is not II law of thermodynamics -

More information

CHEMISTRY 202 Practice Hour Exam III. Dr. D. DeCoste T.A (60 pts.) 21 (15 pts.) 22 (20 pts.) 23 (25 pts.) Total (120 pts)

CHEMISTRY 202 Practice Hour Exam III. Dr. D. DeCoste T.A (60 pts.) 21 (15 pts.) 22 (20 pts.) 23 (25 pts.) Total (120 pts) CHEMISTRY 202 Practice Hour Exam III Fall 2016 Dr. D. DeCoste Name Signature T.A. This exam contains 23 questions on 10 numbered pages. Check now to make sure you have a complete exam. You have two hours

More information

Free-energy change ( G) and entropy change ( S)

Free-energy change ( G) and entropy change ( S) Free-energy change ( G) and entropy change ( S) A SPONTANEOUS PROCESS (e.g. diffusion) will proceed on its own without any external influence. A problem with H A reaction that is exothermic will result

More information

Steady-state diffusion is diffusion in which the concentration of the diffusing atoms at

Steady-state diffusion is diffusion in which the concentration of the diffusing atoms at Chapter 7 What is steady state diffusion? Steady-state diffusion is diffusion in which the concentration of the diffusing atoms at any point, x, and hence the concentration gradient at x, in the solid,

More information

CHM 112 Chapter 16 Thermodynamics Study Guide

CHM 112 Chapter 16 Thermodynamics Study Guide CHM 112 Chapter 16 Thermodynamics Study Guide Remember from Chapter 5: Thermodynamics deals with energy relationships in chemical reactions Know the definitions of system, surroundings, exothermic process,

More information

MCB100A/Chem130 MidTerm Exam 2 April 4, 2013

MCB100A/Chem130 MidTerm Exam 2 April 4, 2013 MCBA/Chem Miderm Exam 2 April 4, 2 Name Student ID rue/false (2 points each).. he Boltzmann constant, k b sets the energy scale for observing energy microstates 2. Atoms with favorable electronic configurations

More information

Chapter 2: Equilibrium Thermodynamics and Kinetics

Chapter 2: Equilibrium Thermodynamics and Kinetics Chapter 2: Equilibrium Thermodynamics and Kinetics Equilibrium Thermodynamics: predicts the concentrations (or more precisely, activities) of various species and phases if a reaction reaches equilibrium.

More information

Second Law of Thermodynamics

Second Law of Thermodynamics Second Law of Thermodynamics First Law: the total energy of the universe is a constant Second Law: The entropy of the universe increases in a spontaneous process, and remains unchanged in a process at

More information

Transport of Chemicals, Kinetics, and Equilibrium

Transport of Chemicals, Kinetics, and Equilibrium Transport of Chemicals, Kinetics, and Equilibrium Module 1: Basic Concepts, Lecture Chemical Fate and Transport in the Environment, nd edition. H.F. Hemond and E.J. Fechner-Levy. Academic Press. London.

More information

Chem Hughbanks Exam 3, April 19, 2012

Chem Hughbanks Exam 3, April 19, 2012 Chem 107 - Hughbanks Exam 3, April 19, 2012 Name (Print) UIN # Section 503 Exam 3, Version # A On the last page of this exam, you ve been given a periodic table and some physical constants. You ll probably

More information

Name: Discussion Section:

Name: Discussion Section: CBE 141: Chemical Engineering Thermodynamics, Spring 2017, UC Berkeley Midterm 2 FORM B March 23, 2017 Time: 80 minutes, closed-book and closed-notes, one-sided 8 ½ x 11 equation sheet allowed lease show

More information