Exam 3, Chemistry 481, 8 December 2017
|
|
- Oswin Wilkins
- 5 years ago
- Views:
Transcription
1 1 Exam 3, Chemistry 481, 8 December 2017 Show all work for full credit Useful constants: k B = J K 1 ; R (molar gas constant) = J K 1 mol 1 Helmholz free energy: A = U S, so that da Sd d Gibbs free energy: G = H S, so that dg Sd +d 1. One Maxwell relation is ( ) (1) a. Derive, in the case where and are the independent variables, the corresponding expression for ( S/). (12 pts) Since and are the independent variables, solution starts from the equation da Sd d. Comparing this with the general mathematical expression for the total differential da = ( A/ ) d + ( A/) d, we see S ( A/ ) and ( A/). Since the mixed 2nd derivatives of A with respect to and are identical, it follows that ( S/) = ( / ) Another, more circuitous, derivation is as follow: By the chain rule = ( ) (2) Now the cyclic rule is ( ) ( ) ( ) 1 which can be rearranged to give ( ) Substituting this into Eq. (2) gives ( ) ( ) ( ) ( ) We can now introduce the Maxwell relation given in the statement of this exam question
2 2 [( S/ ) (/ ) ] to show that ( ) ( ) ( ) = + he first and the second terms on the right hand side are reciprocals of each other, and hence cancel each other out, with the result that which is the desired answer. = ( ) b. We showed that ( ) U + ( ) Starting from the definition G = H S, obtain a similar expression for ( H/ ) in terms of the variables,, and. (13 pts) We know G = H S. Differentiation w/ respect to at constant gives ( G/ ) = ( H/ ) ( S/ ). Replace the 2nd term on the right hand side by the Maxwell relation given in problem 1, to get ( G/ ) = ( H/ ) (/ ) (1) Now wealso know thatdg Sd+d. Equatingthis with the mathematical relation dg = ( G/ ) d +( G/ ) d shows that ( G/ ) d =. Substitution of this result into Eq. (1) gives the desired answer ( H/ ) = +(/ ) c. In general, the energy U is a function of and. Show that the energy is a function of only the temperature for a gas that obeys the equation of state ( b) = R where b is a constant. (13 pts) o prove that the energy is a function of only the temperature, we need to show that ( U/) = 0. We know from part (b) that ( U/) + ( / ). For the given equation of state, = R/( b), so ( / ) = R/( b) and hence +( / ) R/( b)+r/( b) = 0. hus ( U/) =0.
3 3 d. In terms of the translational partition function, the definitions of the average energy and the pressure is E = k 2 ( lnq tr / ) and = k( lnq tr /), where ( ) 2πmk 3/2 q tr (,) = Starting from these expressions, derive an expression for ( E / ) in terms of the thermophysical variables,, and. (13 pts) Hint: should statistical mechanics, where the average energy is E, give the same result as thermodynamics? We have h 2 = k 2 ( ) lnqtr We can reverse the order of the differentiation in the mixed partial derivative to get Substituting in = k( lnq tr /) gives = k 2 = k 2 ( ) lnqtr ( ) ( ) + k his is the same result as given in part (b) but with U replaced by E 2. he Clapeyron equation states that the derivative of the coexistence curve of two phases α and β is ( ) = S β S α = S G=0 β α a. Derive the Clausius-Clapeyron equation, which relates ( / ) along a liquid-vapor coexistence curve, to the enthalpy of vaporization H vap. (13 pts) For a liquid vapor transition S = H/ vap. Also if we assume that the vapor is an ideal gas and that g l, then gas = R/ (for one mole). hus / = H/(Rvap 2 ). We can rearrange this equation to d/ = Hd/R 2. Integration gives ln/ o ( H/R)(1/ 1/ o ) 3. he phase diagram for water is: And a table of some thermodynamic and physical properties of water is a. What will be the melting point ( C) at the critical pressure? Assume the solid-liquid coexistence curve is linear, that fus and S fus are independent of temperature. (12
4 4 quantity ice water steam S (J/mol K) (m 3 ) R/ pts) Here we use the Clapeyron equation (roblem 2) ( / ) G=0 = S/. Here, for one mole, S (in the direction ice water) = =28.95 J/K. Similarly (also for one mole) = ( ) 10 5 m 3. So / = 28.95/ If we assume the solid-liquid coexistence curve is linear, then / ( crit norm )/( crit norm ) = ( ) /( crit ) a/k Solving this equation for crit gives or 1.22 C. b. he vapor pressures of solid and liquid water are given by ln( s /atm) = K ln( l /atm) = K Use this information to calculate the temperature ( C) and pressure (atm) at the triple point. (12 pts) hese two functions describe the solid-gas and solid-liquid interfaces in the figures. Where they intersect is the triple point. At that point s = l. So we can set these two equations equal at the triple point to get / = /. Solving gives = K = 0.01 C. Substituting this value into one of equations gives ln = /273.16=
5 5 Exponentiation gives = exp( )= atm. 4. In terms of thermodynamic properties, derive the value of the expressions: (Note, just stating the answer is not sufficient.) and ( ) (G/) [ ] (G/) (1/) (8pts) (4pts) By definition G = H S, so G/ = H/ S or ( ) G/ H ( ) H H 2 + C C H 2 Now let x = 1/ or = 1/x so by the chain rule, d/dx = (d/d)(d/x) (1/x 2 )d/d = 2 d/d. hus [ ] (G/) (1/) 2 ( H 2 ) = H
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 informationCHEM-UA 652: Thermodynamics and Kinetics
1 CHEM-UA 652: hermodynamics and Kinetics Notes for Lecture 14 I. HE CLAEYRON EQUAION he Clapeyron attempts to answer the question of what the shape of a two-phase coexistence line is. In the - plane,
More informationFinal Exam, Chemistry 481, 77 December 2016
1 Final Exam, Chemistry 481, 77 December 216 Show all work for full credit Useful constants: h = 6.626 1 34 J s; c (speed of light) = 2.998 1 8 m s 1 k B = 1.387 1 23 J K 1 ; R (molar gas constant) = 8.314
More informationChapter 12 Intermolecular Forces of Attraction
Chapter 12 Intermolecular Forces of Attraction Intermolecular Forces Attractive or Repulsive Forces between molecules. Molecule - - - - - - Molecule Intramolecular Forces bonding forces within the molecule.
More informationThermodynamic condition for equilibrium between two phases a and b is G a = G b, so that during an equilibrium phase change, G ab = G a G b = 0.
CHAPTER 5 LECTURE NOTES Phases and Solutions Phase diagrams for two one component systems, CO 2 and H 2 O, are shown below. The main items to note are the following: The lines represent equilibria between
More informationPhase Diagrams. NC State University
Chemistry 433 Lecture 18 Phase Diagrams NC State University Definition of a phase diagram A phase diagram is a representation of the states of matter, solid, liquid, or gas as a function of temperature
More informationProblem Set 10 Solutions
Chemistry 360 Dr Jean M Standard Problem Set 10 Solutions 1 Sketch (roughly to scale) a phase diagram for molecular oxygen given the following information: the triple point occurs at 543 K and 114 torr;
More informationThe 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 informationPractice 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 informationCHAPTER 4 Physical Transformations of Pure Substances.
I. Generalities. CHAPTER 4 Physical Transformations of Pure Substances. A. Definitions: 1. A phase of a substance is a form of matter that is uniform throughout in chemical composition and physical state.
More informationChapter 11 Spontaneous Change and Equilibrium
Chapter 11 Spontaneous Change and Equilibrium 11-1 Enthalpy and Spontaneous Change 11-2 Entropy 11-3 Absolute Entropies and Chemical Reactions 11-4 The Second Law of Thermodynamics 11-5 The Gibbs Function
More informationMS212 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 informationApplication of Thermodynamics in Phase Diagrams. Today s Topics
Lecture 23 Application of Thermodynamics in Phase Diagrams The Clausius Clapeyron Equation A. K. M. B. Rashid Professor, Department of MME BUET, Dhaka Today s Topics The Clapeyron equation Integration
More information= = 10.1 mol. Molar Enthalpies of Vaporization (at Boiling Point) Molar Enthalpy of Vaporization (kj/mol)
Ch 11 (Sections 11.1 11.5) Liquid Phase Volume and Density - Liquid and solid are condensed phases and their volumes are not simple to calculate. - This is different from gases, which have volumes that
More informationHomework Week 8 G = H T S. Given that G = H T S, using the first and second laws we can write,
Statistical Molecular hermodynamics University of Minnesota Homework Week 8 1. By comparing the formal derivative of G with the derivative obtained taking account of the first and second laws, use Maxwell
More informationpv m = RT + Bp The simplest equation for calculating fugacity, given an equation of state, is Z=1 + B RT p
Chem 42/523 Chemical hermodynamics Homework Assignment # 5 1. *Assume O 2 gas obeys the virial equation pv m = R + Bp with B = 12.5 cm 3 mol 1 at 298.15 K. Calculate the fugacity of oxygen at p = 1. MPa
More informationB. Correct! Good work. F = C P + 2 = = 2 degrees of freedom. Good try. Hint: Think about the meaning of components and phases.
Physical Chemistry - Problem Drill 06: Phase Equilibrium No. 1 of 10 1. The Gibbs Phase Rule is F = C P + 2, how many degrees of freedom does a system have that has two independent components and two phases?
More informationPhysical 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 informationCHEM-UA 652: Thermodynamics and Kinetics
1 CHEM-UA 652: Thermodynamics and Kinetics Notes for Lecture 13 I. PHASE DIAGRAMS The different phases of substances are characterized by different ranges of thermodynamic variables in which these phasesarethestablephases.
More informationGeneral Physical Chemistry I
General Physical Chemistry I Lecture 11 Aleksey Kocherzhenko March 12, 2015" Last time " W Entropy" Let be the number of microscopic configurations that correspond to the same macroscopic state" Ø Entropy
More informationPhase Change (State Change): A change in physical form but not the chemical identity of a substance.
CHM 123 Chapter 11 11.1-11.2 Phase change, evaporation, vapor pressure, and boiling point Phase Change (State Change): A change in physical form but not the chemical identity of a substance. Heat (Enthalpy)
More informationln( 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 informationFor an incompressible β and k = 0, Equations (6.28) and (6.29) become:
Internal Energy and Entropy as Functions of T and V These are general equations relating the internal energy and entropy of homogeneous fluids of constant composition to temperature and volume. Equation
More informationFrom what we know now (i.e, ΔH and ΔS) How do we determine whether a reaction is spontaneous?
pontaneous Rxns A&G-1 From what we know now (i.e, Δ and Δ) ow do we determine whether a reaction is spontaneous? But Δ and Δ are not enough... here is competition between lowering energy and raising entropy!
More informationExam 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 informationChemistry 425 September 29, 2010 Exam 1 Solutions
Chemistry 425 September 29, 2010 Exam 1 Solutions Name: Instructions: Please do not start working on the exam until you are told to begin. Check the exam to make sure that it contains exactly 6 different
More informationChemistry 360 Spring 2017 Dr. Jean M. Standard April 19, Exam points
Chemistry 360 pring 2017 Dr. Jean M. tandard April 19, 2017 Name Exam 3 100 points Note: You must show your work on problems in order to receive full credit for any answers. You must turn in your equation
More informationPractice 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 informationChapter 8 Phase Diagram, Relative Stability of Solid, Liquid, and Gas
Chapter 8 Phase Diagram, Relative Stability of Solid, Liquid, and Gas Three states of matter: solid, liquid, gas (plasma) At low T: Solid is most stable. At high T: liquid or gas is most stable. Ex: Most
More informationPhase Equilibrium: Preliminaries
Phase Equilibrium: Preliminaries Phase diagrams for two one component systems, CO 2 and H 2 O, are shown below. The main items to note are the following: The lines represent equilibria between two phases.
More informationCh. 6 Enthalpy Changes
Ch. 6 Enthalpy Changes Energy: The capacity to do work. In Physics, there are 2 main types of energy Kinetic (energy of motion) = ½ mv 2 Potential (energy of position due to gravity)= mgh In Chemistry,
More informationExam 2 Solutions. for a gas obeying the equation of state. Z = PV m RT = 1 + BP + CP 2,
Chemistry 360 Dr. Jean M. Standard Fall 016 Name KEY 1.) (14 points) Determine # H & % ( $ ' Exam Solutions for a gas obeying the equation of state Z = V m R = 1 + B + C, where B and C are constants. Since
More informationChapter 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 informationChapter 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 informationThere are five problems on the exam. Do all of the problems. Show your work
CHM 3400 Fundamentals of Physical Chemistry Second Hour Exam March 8, 2017 There are five problems on the exam. Do all of the problems. Show your work R = 0.08206 L atm/mole K N A = 6.022 x 10 23 R = 0.08314
More informationFree energy dependence along the coexistence curve
Free energy dependence along the coexistence curve In a system where two phases (e.g. liquid and gas) are in equilibrium the Gibbs energy is G = GG l + GG gg, where GG l and GG gg are the Gibbs energies
More informationEquations: 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 informationChapter 11. Intermolecular Forces and Liquids and Solids. Chemistry, Raymond Chang 10th edition, 2010 McGraw-Hill
Chemistry, Raymond Chang 10th edition, 2010 McGraw-Hill Chapter 11 Intermolecular Forces and Liquids and Solids Ahmad Aqel Ifseisi Assistant Professor of Analytical Chemistry College of Science, Department
More informationLecture 14. Phases of Pure Substances (Ch.5)
ecture 4. hases of ure Substances (Ch.5) Up to now we have dealt almost exclusively with systems consisting of a single phase. In this lecture, we will learn how more complicated, multiphase systems can
More informationSolutions to Problem Set 9
Solutions to Problem Set 9 1. When possible, we want to write an equation with the quantity on the ordinate in terms of the quantity on the abscissa for each pf the labeled curves. A B C p CHCl3 = K H
More informationCHAPTER 3 LECTURE NOTES 3.1. The Carnot Cycle Consider the following reversible cyclic process involving one mole of an ideal gas:
CHATER 3 LECTURE NOTES 3.1. The Carnot Cycle Consider the following reversible cyclic process involving one mole of an ideal gas: Fig. 3. (a) Isothermal expansion from ( 1, 1,T h ) to (,,T h ), (b) Adiabatic
More informationLast 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 informationName: 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 informationIntroduction to Chemical Thermodynamics. (10 Lectures) Michaelmas Term
Introduction to Chemical Thermodynamics Dr. D. E. Manolopoulos First Year (0 Lectures) Michaelmas Term Lecture Synopsis. Introduction & Background. Le Chatelier s Principle. Equations of state. Systems
More informationPhysical Chemistry Physical chemistry is the branch of chemistry that establishes and develops the principles of Chemistry in terms of the underlying concepts of Physics Physical Chemistry Main book: Atkins
More informationTemperature C. Heat Added (Joules)
Now let s apply the heat stuff to real-world stuff like phase changes and the energy or cost it takes to carry it out. A heating curve...a plot of temperature of a substance vs heat added to a substance.
More informationChapter 16. Thermodynamics. Thermochemistry Review. Calculating H o rxn. Predicting sign for H o rxn. Creative Commons License
Chapter 16 Thermodynamics GCC CHM152 Creative Commons License Images and tables in this file have been used from the following sources: OpenStax: Creative Commons Attribution License 4.0. ChemWiki (CC
More informationIntroduction to Chemical Thermodynamics. D. E. Manolopoulos First Year (13 Lectures) Michaelmas Term
Introduction to Chemical Thermodynamics D. E. Manolopoulos First Year (13 Lectures) Michaelmas Term Lecture Synopsis 1. Introduction & Background. Le Chatelier s Principle. Equations of state. Systems
More information3.012 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 informationChapter 6. Phase transitions. 6.1 Concept of phase
Chapter 6 hase transitions 6.1 Concept of phase hases are states of matter characterized by distinct macroscopic properties. ypical phases we will discuss in this chapter are liquid, solid and gas. Other
More informationUniversity of Washington Department of Chemistry Chemistry 452/456 Summer Quarter 2011
Homework Assignment #: Due at 500 pm Wednesday July 6. University of Washington Department of Chemistry Chemistry 45/456 Summer Quarter 0 ) he respiratory system uses oxygen to degrade glucose to carbon
More informationDisorder 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 informationPhysical transformations of pure substances Boiling, freezing, and the conversion of graphite to diamond examples of phase transitions changes of
Physical transformations of pure substances Boiling, freezing, and the conversion of graphite to diamond examples of phase transitions changes of phase without change of chemical composition. In this chapter
More information* The actual temperature dependence for the enthalpy and entropy of reaction is given by the following two equations:
CHM 3400 Problem Set 5 Due date: Tuesday, October 7 th Do all of the following problems. Show your work. "The first essential in chemistry is that you should perform practical work and conduct experiments,
More informationChem 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 informationWEEK 6. Multiphase systems
WEEK 6 Multiphase systems Multiphase systems P 237. Processes usually deal with material being transferred from one phase (gas, liquid, or solid) to another. 6.1a Phase diagrams F = force on piston Water
More informationExam 1. Name: Recitation Section Lenny.: 6:30 7:30 (circle one): Greg.: 6:30 7:30 Student Number: Nic.: 6:30 7:30
Exam 1 Name: Recitation Section Lenny.: 6:30 7:30 (circle one): Greg.: 6:30 7:30 Student Number: Nic.: 6:30 7:30 Please show your work and either circle your answers or put your answers in the boxes provided.
More informationCHEM Exam 2 - October 11, INFORMATION PAGE (Use for reference and for scratch paper)
CHEM 5200 - Exam 2 - October 11, 2018 INFORMATION PAGE (Use for reference and for scratch paper) Constants and Conversion Factors: R = 0.082 L-atm/mol-K = 8.31 J/mol-K = 8.31 kpa-l/mol-k 1 L-atm = 101
More informationEntropy, 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 informationChapter 17.3 Entropy and Spontaneity Objectives Define entropy and examine its statistical nature Predict the sign of entropy changes for phase
Chapter 17.3 Entropy and Spontaneity Objectives Define entropy and examine its statistical nature Predict the sign of entropy changes for phase changes Apply the second law of thermodynamics to chemical
More information6 Physical transformations of pure substances
6 Physical transformations of pure substances E6.b E6.2b E6.3b E6.4b Solutions to exercises Discussion questions Refer to Fig. 6.8. The white lines represent the regions of superheating and supercooling.
More informationChemistry 2000 Fall 2017 Test 2 Version A Solutions
Chemistry 2000 Fall 207 Test 2 Version A Solutions. Start with a balanced reaction: (a) liquid water: C 2 H 4(g) + 3 O 2(g) 2 CO 2(g) + 2 H 2 O r S = 2S (CO 2 ) + 2S (H 2 O, l) [S (C 2 H 4 ) + 3S (O 2
More information1. Heterogeneous Systems and Chemical Equilibrium
1. Heterogeneous Systems and Chemical Equilibrium The preceding section involved only single phase systems. For it to be in thermodynamic equilibrium, a homogeneous system must be in thermal equilibrium
More informationExam Thermodynamics 12 April 2018
1 Exam Thermodynamics 12 April 2018 Please, hand in your answers to problems 1, 2, 3 and 4 on separate sheets. Put your name and student number on each sheet. The examination time is 12:30 until 15:30.
More informationThermodynamics. Thermodynamically favored reactions ( spontaneous ) Enthalpy Entropy Free energy
Thermodynamics Thermodynamically favored reactions ( spontaneous ) Enthalpy Entropy Free energy 1 Thermodynamically Favored Processes Water flows downhill. Sugar dissolves in coffee. Heat flows from hot
More informationChapter 7 PHASE EQUILIBRIUM IN A ONE-COMPONENT SYSTEM
Chapter 7 PHASE EQUILIBRIUM IN A ONE-COMPONENT SYSTEM 7.1 INTRODUCTION The intensive thermodynamic properties of a system are temperature, pressure, and the chemical potentials of the various species occurring
More informationCh 18 Free Energy and Thermodynamics:
P a g e 1 Ch 18 Free Energy and Thermodynamics: Homework: Read Ch 18, Work out sample/practice exercises in the sections as you read, Ch 18: 27, 31, 33, 41, 43, 47, 51, 55, 61, 63, 67, 71, 77, 87 Check
More informationName: Discussion Section:
CBE 141: Chemical Engineering Thermodynamics, Spring 2018, UC Berkeley Midterm 2 March 22, 2018 Time: 80 minutes, closed-book and closed-notes, one-sided 8 ½ x 11 equation sheet allowed Please show all
More informationReflection. Review of Energy Balances. Class 28. Concepts. Professional Program Application. After Action Report
Reflection After Action Report What did I learn from this W assignment? Professional Program Application Meet with you advisor an form Pink Form Excel course planning worksheet Due November 7! Note: Any
More informationChpt 19: Chemical. Thermodynamics. Thermodynamics
CEM 152 1 Reaction Spontaneity Can we learn anything about the probability of a reaction occurring based on reaction enthaplies? in general, a large, negative reaction enthalpy is indicative of a spontaneous
More informationChemical Thermodynamics
Chemical Thermodynamics David A. Katz Department of Chemistry Pima Community College Tucson, AZ 85709, USA First Law of Thermodynamics The First Law of Thermodynamics was expressed in the study of thermochemistry.
More informationCHEMISTRY. CHM202 Class #2 CHEMISTRY. Chapter 10. Chapter Outline for Class #2
CHEMISTRY Fifth Edition Gilbert Kirss Foster Bretz Davies CHM202 Class #2 1 Chemistry, 5 th Edition Copyright 2017, W. W. Norton & Company CHEMISTRY Fifth Edition Gilbert Kirss Foster Bretz Davies Chapter
More informationMATSCI 204 Thermodynamics and Phase Equilibria Winter Chapter #5 Practice problems
MATSCI 204 Thermodynamics and Phase Equilibria Winter 2013 Chapter #5 Practice problems Problem 4 a-assuming that you are cooling an equimolar liquid Au-Bi solution reversibly from 1200 C, describe the
More informationVapor Pressure is determined primarily from!vaph!vaph depends on the intermolecular forces
What do you remember from last time? What do you remember from last time? You have two containers. one has a total volume of 2 L and one has a total volume of 1 L Into each you place 500 ml of liquid ether
More informationSchool 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 informationLiquids and Solids. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Liquids and Solids Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Gases, Liquids and Solids Gases are compressible fluids. They have no proper volume and proper
More informationCHAPTER 11: Spontaneous Change and Equilibrium
CHAPTER 11: Spontaneous Change and Equilibrium Goal of chapter: Be able to predict which direction a reaction will go (cases where there is not necessarily an equilibrium) At high temperatures, ice always
More informationCHEMISTRY 443, Fall, 2014 (14F) Section Number: 10 Examination 2, November 5, 2014
NAME: CHEMISTRY 443, Fall, 2014 (14F) Section Number: 10 Examination 2, November 5, 2014 Answer each question in the space provided; use back of page if extra space is needed. Answer questions so the grader
More informationChapter 5. On-line resource
Chapter 5 The water-air heterogeneous system On-line resource on-line analytical system that portrays the thermodynamic properties of water vapor and many other gases http://webbook.nist.gov/chemistry/fluid/
More informationPhase Equilibria I. Introduction. Heat and Phase Changes
Phase Equilibria I 2 Introduction In the previous chapter, it was discussed the thermodynamics principles that are the basis of thermochemistry. It was shown how to calculate the energy involved in any
More informationThermodynamics of solids 5. Unary systems. Kwangheon Park Kyung Hee University Department of Nuclear Engineering
Thermodynamics of solids 5. Unary systems Kwangheon ark Kyung Hee University Department of Nuclear Engineering 5.1. Unary heterogeneous system definition Unary system: one component system. Unary heterogeneous
More informationCH 302 Spring 2008 Worksheet 4 Answer Key Practice Exam 1
CH 302 Spring 2008 Worksheet 4 Answer Key Practice Exam 1 1. Predict the signs of ΔH and ΔS for the sublimation of CO 2. a. ΔH > 0, ΔS > 0 b. ΔH > 0, ΔS < 0 c. ΔH < 0, ΔS > 0 d. ΔH < 0, ΔS < 0 Answer:
More informationANSWER KEY. Chemistry 25 (Spring term 2016) Midterm Examination
Name ANSWER KEY Chemistry 25 (Spring term 2016) Midterm Examination 1 Some like it hot 1a (5 pts) The Large Hadron Collider is designed to reach energies of 7 TeV (= 7 x 10 12 ev, with 1 ev = 1.602 x 10-19
More informationName: First three letters of last name
Name: First three letters of last name Chemistry 342 Third Exam April 22, 2005 2:00 PM in C6 Lecture Center Write all work you want graded in the spaces provided. Both the logical solution to the problem
More informationThere are five problems on the exam. Do all of the problems. Show your work.
CHM 3410 - Physical Chemistry 1 Second Hour Exam October 22, 2010 There are five problems on the exam. Do all of the problems. Show your work. R = 0.08206 L. atm/mole. K N A = 6.022 x 10 23 R = 0.08314
More informationLecture 26: Liquids 1: phase changes & heat capacity
Lecture 26: Liquids 1: phase changes & heat capacity Read: BLB 5.5; 11.4 HW: BLB 5:48,49,51; 11:33,37,39 Know: viscosity, surface tension cohesive & adhesive forces phase changes heat capacity calorimetry
More information12. Heat of melting and evaporation of water
VS 12. Heat of melting and evaporation of water 12.1 Introduction The change of the physical state of a substance in general requires the absorption or release of heat. In this case, one speaks of a first
More informationChemical 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 informationChapter 19. Chemical Thermodynamics
Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 19 John D. Bookstaver St. Charles Community College Cottleville, MO First Law of You will
More informationThe Gibbs Phase Rule F = 2 + C - P
The Gibbs Phase Rule The phase rule allows one to determine the number of degrees of freedom (F) or variance of a chemical system. This is useful for interpreting phase diagrams. F = 2 + C - P Where F
More informationProblem Set #10 Assigned November 8, 2013 Due Friday, November 15, 2013 Please show all work for credit To Hand in
Problem Set #10 Assigned November 8, 2013 Due Friday, November 15, 2013 Please show all work for credit To Hand in 1. 2. 1 3. 4. The vapor pressure of an unknown solid is approximately given by ln(p/torr)
More informationN h (6.02x10 )(6.63x10 )
CHEM 5200 - Final Exam - December 13, 2018 INFORMATION PAGES (Use for reference and for scratch paper) Constants and Conversion Factors: R = 8.31 J/mol-K = 8.31 kpa-l/mol-k = 0.00831 kj/mol-k 1 L-atm =
More informationChemistry 123: Physical and Organic Chemistry Topic 2: Thermochemistry
Recall the equation. w = -PΔV = -(1.20 atm)(1.02 L)( = -1.24 10 2 J -101 J 1 L atm Where did the conversion factor come from? Compare two versions of the gas constant and calculate. 8.3145 J/mol K 0.082057
More informationChapter 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 informationPractice Midterm Exam 1 March, 2005
NAME: MSE 308: Thermodynamics of Materials Department of Materials Science & Engineering Boise State University Spring 2005 Practice Midterm Exam 1 March, 2005 Problem Total Points Points Obtained 1. 2.
More informationClass XI Chapter 6 Thermodynamics Question 6.1: Choose the correct answer. A thermodynamic state function is a quantity (i) used to determine heat changes (ii) whose value is independent of path (iii)
More informationName: Discussion Section:
CBE 141: Chemical Engineering Thermodynamics, Spring 2017, UC Berkeley Midterm 2 FORM A March 23, 2017 Time: 80 minutes, closed-book and closed-notes, one-sided 8 ½ x 11 equation sheet allowed Please show
More informationPhysics 408 Final Exam
Physics 408 Final Exam Name You are graded on your work, with partial credit where it is deserved. Please give clear, well-organized solutions. 1. Consider the coexistence curve separating two different
More informationaa + bb ---> cc + dd
17 Chemical Equilibria Consider the following reaction: aa + bb ---> cc + dd As written is suggests that reactants A + B will be used up in forming products C + D. However, what we learned in the section
More informationIntermolecular Forces and Liquids and Solids Chapter 11
Intermolecular Forces and Liquids and Solids Chapter 11 A phase is a homogeneous part of the system in contact with other parts of the system but separated from them by a well defined boundary. Phases
More information