Reflection. Review of Energy Balances. Class 28. Concepts. Professional Program Application. After Action Report
|
|
|
- Hugh Harris
- 5 years ago
- Views:
Transcription
1 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 Bio class that satisfies GE can be used, not just Bio 00 Professors cannot do this all on the last day, so start early!! Application required before you can get an add code for ChEn 374 (Fluids) Review of Energy Balances Class 8 Enthalpies, eat Capacities eats of Formation, Oh My! Enthalpies needed to calculate heat or work terms Methods to calculate enthalpy (so far): Steam tables Graph (P- diagram) Interpolation from given values Needed: Method to get enthalpies for any species as a function of & P Concepts Concept. Enthalpy Is A State Function. Enthalpy is a state function. eat Capacities 3. Latent eats (phase change) 4. eat of Formation 5. Calculating as f(,p) P Rankine cycle (most common method to generate electricity!) is the same here regardless of path Enthalpy is independent of path Always talk about from some reference condition Steam tables: 0at triple point Other tables are different (e.g., in able B., for = 0 at 5C) Don t mix and match tables!!!
2 Concept. eat Capacities Concept. eat Capacities (cont.), d, d Now define heat capacities:, For ideal gases:, For solids and liquids: d Generally small C p not linear area = like slope of vs curve, prob 7.5 so 3 4 For ideal gases: C p = C v + R For solids and liquids, A Practical View Wouldn t it be nice to have a polynomial equation for! = a + b + c his would not work for different reference enthalpies! Solution: Polynomial for C p C P = a + b + c + d (= d/d) Fit to thermodynamic data 0.08 (kj/mol) vs. for Benzene gas Cp (kj/(mol*deg C) (deg C) Cp vs for Benzene gas (deg C) Caution! When getting a heat capacity coefficient from able B., use the multiplier at the top of the column Example: Acetone a = 3 multiplier = 0 3 (i.e., the actual number was multiplied by 0 3 to make it look nicer in the table) herefore, a = kj/(gmolk) C p Integrated form: DIPPR Format C A B sinh D C coshe E C C E E BC coth coth DE tanh C pd A tanh
3 Concepts. Enthalpy is a state function. eat Capacities 3. Latent eats (phase change) 4. eat of Formation 5. Calculating as f(,p) Concept 3. Phase Changes (pure substances) melt ice liquid vap gas Slope = (tabulated) (tabulated) Also we could find Remember that for a pure substance, is constant during a phase change Kopp s Rule: C p kc p, k kelement where k = moles of element k in molecule So for solid phenol, C 6 5 O, C = 6 = 6 O = C p = 6* * = 9.6 J/(mol C) (Dippr = 9 J/(mol C) at 5C) Only use this out of desperation! Other Estimation Formulas routon s rule (8.4-3) v = f( b ) Chen s equation (8.4-4) v = f( b, c, P c ) Clapeyron equation (8.4-7) v = f(p*) Watson s correlation (8.4-8) v vs. using c Only use these equations out of desperation! 3
4 Simplifications Concepts Sometimes we get lazy and assume an average heat capacity for some temperature range = We will use this on exams! I am not testing you on integration skills. Enthalpy is a state function. eat Capacities 3. Latent eats (phase change) 4. eat of Formation 5. Calculating as f(,p) Concept 4. eat of Formation Wanted: Common reference state for all species! Can use as a reference at 5C, atm Good for reaction chemistry = 0 for species whose natural state is 5C, atm N, O,, C(graphite),, abulated in able B. Balances wo Methods to Get. Path Method 4,, 3 98, 98 where a i, b i, and c i are the heat capacity coefficients for species i 98 3 Note that for a chemical reaction, the number of moles of each species (n i ) changes. f0 method,, So compute 4 and and subtract 4
5 Example Example: Find for acetone vapor at 65C forming a liquid at 0 C and 5 atm (Path method) Calculate the enthalpy change for acetone going from a vapor at 65C and atm to a liquid at 0 C and 5 atm A. Path method using vap at atm and boiling B. eat of formation method a Acetone (vapor) 65C, atm, Acetone (vapor) 56C, atm = =? c b 0C, 5 atm 0C, atm, 56C, atm,,, Example: Find for acetone vapor at 65C forming a liquid at 0 C and 5 atm ( fo method) Bottom Line Acetone (vapor) 65C, atm,, = =?,, 0C, 5 atm You Should Know Both Methods to Get. Path Method. fo method,,,, 5,,,, Remember that is just part of energy balance 5
6 aboo Equations 3 rd Edition Page 45: 9.5-a and 9.5-b st Eqn. on page 457 Page 463: last equation (under section 5) 4 th Edition Page 506: 9.5-a and 9.5-b st Eqn. on page 5 Page 59: last equation (under section 5) Problem Solving (pp ). Solve material balances (mass or moles). Write energy balance (drop appropriate terms) 3. Choose reference state(s) 4. able of n i & i in and out (or m i, U i, etc.) 5. Find sys or U sys 6. Find W, W s, E k, E p as needed 7. Solve energy balance omework Problems int on Prob 8. PV = nr QUIZ. What is meant by the statement that enthalpy is a state function?. What is a heat capacity? 3. For water, draw a graph with temperature on the y axis and enthalpy on the x axis, starting from ice and proceeding to steam, labeling the different portions of the line. 4. ow do you use the heat of formation to calculate enthalpy? (eqn. needed). What is meant by the statement that enthalpy is a state function? is not dependent on & P path. What is a heat capacity? Change in enthalpy with temperature 3. For water, draw a graph with temperature on the y axis and enthalpy on the x axis, starting from ice and proceeding to steam, labeling the different portions of the line. ice melting boiling water steam. ow do you use the heat of formation to calculate enthalpy? melt ice liquid vap gas Slope = 6
Energy Balances. F&R Chapter 8
Energy Balances. F&R Chapter 8 How do we calculate enthalpy (and internal energy) changes when we don t have tabulated data (e.g., steam tables) for the process species? Basic procedures to calculate enthalpy
Phase 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)
Heating and Cooling Curves
Heating and Cooling Curves $ Under normal circumstances, particles will undergo more than one type of change when heated or cooled $ During a phase change, the temperature will not change $ Parts of the
Lecture Notes 2: Physical Equilibria Phase Diagrams
Lecture Notes 2: Physical Equilibria Phase Diagrams There are number of graphical means to help to understand the relationships between the different phases of a particular substance. The first thing we
Vapor 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
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.
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:
Chapter 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.
Let's look at how different properties affect vapor pressure. P =0 P =vapor pressure P =vapor pressure. first all liquid
Let's look at how different properties affect vapor pressure P =0 P =vapor pressure P =vapor pressure Quick Quiz You have two containers. one has a total volume of 2 L and one has a total volume of 1 L
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.
Duncan. Q = m. C p. T. Q = heat (Joules) m = mass (g) C p = specific heat capacity (J/g.o C) T = change in temp. ( o C)
HEAT ENERGY NOTES SECTION (A): phase(s) of matter = SECTION (B): phase(s) of matter = energy difference at same temp = temp is called the SECTION (C): phase(s) of matter = SECTION (D): phase(s) of matter
LECTURE 4 Variation of enthalpy with temperature
LECTURE 4 Variation of enthalpy with temperature So far, we can only work at 25 C. Like c v we define a constant pressure heat capacity, c p, as the amount of heat energy needed to raise the temperature
There 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
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
Contents and Concepts
Contents and Concepts 1. First Law of Thermodynamics Spontaneous Processes and Entropy A spontaneous process is one that occurs by itself. As we will see, the entropy of the system increases in a spontaneous
Contents and Concepts
Contents and Concepts 1. First Law of Thermodynamics Spontaneous Processes and Entropy A spontaneous process is one that occurs by itself. As we will see, the entropy of the system increases in a spontaneous
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
Sample Exercise 11.1 Identifying Substances That Can Form Hydrogen Bonds
Sample Exercise 11.1 Identifying Substances That Can Form Hydrogen Bonds In which of these substances is hydrogen bonding likely to play an important role in determining physical properties: methane (CH
Sensible Heat and Enthalpy Calculations
* Sensible Heat and Enthalpy Calculations Sensible Heat - The amount of heat that must be added when a substance undergoes a change in temperature from 298 K to an elevated temperature without a change
Remember Chapter 12.1 Introduction to Kinetic Molecular Theory and Intermolecular forces
Remember Chapter 12.1 Introduction to Kinetic Molecular Theory and Intermolecular forces 1 To understand properties, we want to connect what we see to what is happening on a molecular level. Start with
q = m. C p. T q = heat (Joules) m = mass (g) C p = specific heat (J/g.o C) T = change in temp. ( o C) UNIT 11 - SOLIDS, LIQUIDS, & PHASE CHANGES
HEAT ENERGY NOTES UNIT 11 - SOLIDS, LIQUIDS, & PHASE CHANGES SECTION (A): same temp or change? SECTION (B): same temp or change? temp is called the energy difference at same temp = SECTION (C): same temp
Phase Diagrams. Department of Mechanical Engineering Indian Institute of Technology Kanpur Kanpur India
Phase Diagrams 1 Increasing the temperature isobarically T-v diagram of constant-pressure phase-change processes of a pure substance at various pressures numerical values are for water. 2 Temperature -
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
Lecture 20. Phase Transitions. Phase diagrams. Latent heats. Phase-transition fun. Reading for this Lecture: Elements Ch 13.
Lecture 20 Phase ransitions Phase diagrams Latent heats Phase-transition fun Reading for this Lecture: Elements Ch 13 Lecture 20, p 1 Solid-gas equilibrium: vapor pressure Consider solid-gas equilibrium
HEMISTRY 110 EXAM 3 April 6, 2011 FORM A When the path is blocked, back up and see more of the way. 1. A 250 L vessel is evacuated and then connected to a 50.0 L bulb with compressed nitrogen. The pressure
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
Chapter 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
CHEMISTRY Topic #2: Thermochemistry and Electrochemistry What Makes Reactions Go? Fall 2018 Dr. Susan Findlay See Exercises in Topic 8
CHEMISTRY 2000 Topic #2: Thermochemistry and Electrochemistry What Makes Reactions Go? Fall 208 Dr. Susan Findlay See Exercises in Topic 8 Vapour Pressure of Pure Substances When you leave wet dishes on
Chapter 11 part 2. Properties of Liquids Viscosity Surface Tension Capillary Action. Phase Changes (energy of phase changes)
Chapter 11 part 2 Properties of Liquids Viscosity Surface Tension Capillary Action Phase Changes (energy of phase changes) Dynamic Equilibrium Vapor pressure Phase diagram 1 Structure Affects Function
Topic 5: Energetics. Heat & Calorimetry. Thursday, March 22, 2012
Topic 5: Energetics Heat & Calorimetry 1 Heat is energy that is transferred from one object to another due to a difference in temperature Temperature is a measure of the average kinetic energy of a body
Thinking Like a Chemist About Phase Changes UNIT 5 DAY 3
Thinking Like a Chemist About Phase Changes UNIT 5 DAY 3 What are we going to learn today? First day? Get a handout from a TA after class. Thinking Like a Chemist in the context of Phase Changes Vapor
Contents and Concepts
Contents and Concepts 1. First Law of Thermodynamics Spontaneous Processes and Entropy A spontaneous process is one that occurs by itself. As we will see, the entropy of the system increases in a spontaneous
Exam 3, Chemistry 481, 8 December 2017
1 Exam 3, Chemistry 481, 8 December 2017 Show all work for full credit Useful constants: k B = 1.3807 10 23 J K 1 ; R (molar gas constant) = 8.314 J K 1 mol 1 Helmholz free energy: A = U S, so that da
Practice 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.
Homework 01. Phase Changes and Solutions
HW01 - Phase Changes and Solu!ons! This is a preview of the published version of the quiz Started: Jan 16 at 1:pm Quiz Instruc!ons Homework 01 Phase Changes and Solutions Question 1 Given that you have
CHEM-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,
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.
Sensible Heat and Enthalpy Calculations
Sensible Heat and Enthalpy Calculations Sensible Heat - The amount of heat that must be added when a substance undergoes a change in temperature from 298 K to an elevated temperature without a change in
Thermodynamics. Chem 36 Spring The study of energy changes which accompany physical and chemical processes
Thermodynamics Chem 36 Spring 2002 Thermodynamics The study of energy changes which accompany physical and chemical processes Why do we care? -will a reaction proceed spontaneously? -if so, to what extent?
Liquids. properties & structure
Liquids properties & structure Energetics of Vaporization when the high energy molecules are lost from the liquid, it lowers the average kinetic energy if energy is not drawn back into the liquid, its
Q= mhvap. H= E+pV Q= mc T H= Hproducts Hreactants
Student Worksheet for Attempt to work the following practice problems after working through the sample problems in the videos. Answers are given on the last page(s). Relevant Equations C= Q T Q = E + p
CH 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:
Chapter 11. Intermolecular Forces, Liquids, and Solids
Sample Exercise 11.1 (p. 450) In which of the following substances is hydrogen bonding likely to play an important role in determining physical properties: methane (CH 4 ), hydrazine (H 2 NNH 2 ), methyl
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
Ch. 9 Liquids and Solids
Intermolecular Forces I. A note about gases, liquids and gases. A. Gases: very disordered, particles move fast and are far apart. B. Liquid: disordered, particles are close together but can still move.
Exam 4, Enthalpy and Gases
CHEM 1100 Dr. Stone November 8, 2017 Name_ G Exam 4, Enthalpy and Gases Equations and constants you may need: ΔE system = q + w PV = nrt R = 0.0821 (L*atm)/(mole*K) w = -PΔV K.E. = 1 2 m *µ 2 rms µ rms=
Distinguish between an isothermal process and an adiabatic process as applied to an ideal gas (2)
1. This question is about thermodynamic processes. (a) Distinguish between an isothermal process and an adiabatic process as applied to an ideal gas.......... An ideal gas is held in a container by a moveable
solid IMF>liquid IMF>gas IMF Draw a diagram to represent the 3 common states of matter of a given substance: solid liquid gas
Thermochemistry Part 1 Notes States of Matter and Intermolecular Forces (IMF) Chemistry HP At the end of this unit, students should be able to: Describe the various states of matter in terms of kinetic
Chpt 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
Chem Hughbanks Exam 3A, Solutions
Chem 107 - Hughbanks Exam 3A, Solutions 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
Lecture 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
For 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
l g vaporization, H+, S+ g l condensation, H-, S-
8.4 8.7 Phase Diagrams It is particularly instructive to assemble graphs and diagrams that contrast the properties of a compound's phases. For example, the phase diagram that is most famous is a plot of
Intermolecular Forces and States of Matter AP Chemistry Lecture Outline
Intermolecular Forces and States of Matter AP Chemistry Lecture Outline Name: Chemical properties are related only to chemical composition; physical properties are related to chemical composition AND the
Exothermic process is any process that gives off heat transfers thermal energy from the system to the surroundings. H 2 O (l) + energy
Exothermic process is any process that gives off heat transfers thermal energy from the system to the surroundings. H 2 O (g) H 2 O (l) + energy Endothermic process is any process in which heat has to
CHEM 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
Name: 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
General Chemistry 1 CHM201 Unit 3 Practice Test
General Chemistry 1 CHM201 Unit 3 Practice Test 1. Heat is best defined as a. a substance that increases the temperature and causes water to boil. b. a form of potential energy. c. a form of work. d. the
Name TA Name Lab Section # ALL work must be shown to receive full credit. Due at the beginning of lecture on Wednesday, August 29, 2001.
Chem 1515 Problem Set #1 Fall 2001 Name TA Name Lab Section # ALL work must be shown to receive full credit. Due at the beginning of lecture on Wednesday, August 29, 2001. PS1.1. Using the Pre-Lecture
Chem 1310 A/B 2005, Professor Williams Practice Exam 3 (chapters 10, 11 and 12) Chapter 10 Thermochemistry
Chem 1310 A/B 2005, Professor Williams Practice Exam 3 (chapters 10, 11 and 12) Chapter 10 Thermochemistry 1. The heat capacity (C P ) is related to the heat absorbed at constant pressure (q P ) and the
Chemical Thermodynamics
Quiz A 42.8 ml solution of ammonia (NH 3 ) is titrated with a solution of 0.9713 M hydrochloric acid. The initial reading on the buret containing the HCl was 47.13 ml and the final reading when the endpoint
Name: Date: Grade. Work Session # 12: Intermolecular Forces
Name: Date: Grade Work Session # 12: Intermolecular Forces All questions below must be answered during the lab. Show all work and express your answers with appropriate units and the correct number of significant
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.
Temperature 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.
CHEM Thermodynamics. Entropy, S
hermodynamics Change in Change in Entropy, S Entropy, S Entropy is the measure of dispersal. he natural spontaneous direction of any process is toward greater dispersal of matter and of energy. Dispersal
1. Fill in the blanks with the following: kinetic, potential, chemical, thermal. One word will be used twice.
Thermo Worksheets Name Class Period Types of Energy and the Law of Conservation of Energy 1. Fill in the blanks with the following: kinetic, potential, chemical, thermal. One word will be used twice. Solar
Ch. 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,
Advanced Chemistry Practice Problems
Thermodynamics: Review of Thermochemistry 1. Question: What is the sign of DH for an exothermic reaction? An endothermic reaction? Answer: ΔH is negative for an exothermic reaction and positive for an
CHEM 10113, Exam 4. All equations must be balanced and show phases for full credit. Significant figures count, and box your answers!
CHEM 10113, Exam 4 November 30, 2011 Name (please print) All equations must be balanced and show phases for full credit. Significant figures count, and box your answers! 1. (10 points) Consider the phase
Entropy and Free Energy
Page 1 Entropy and Free Energy How to predict if a reaction can occur at a reasonable rate? KINEICS Chapter 17 How to predict if a reaction can occur, given enough time? HERMODYNAMICS 1 Objectives Spontaneity
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
Chapter 3 PROPERTIES OF PURE SUBSTANCES. Thermodynamics: An Engineering Approach, 6 th Edition Yunus A. Cengel, Michael A. Boles McGraw-Hill, 2008
Chapter 3 PROPERTIES OF PURE SUBSTANCES Thermodynamics: An Engineering Approach, 6 th Edition Yunus A. Cengel, Michael A. Boles McGraw-Hill, 2008 Objectives Introduce the concept of a pure substance. Discuss
Unit 7 Thermochemistry Chemistry 020, R. R. Martin
Unit 7 Thermochemistry Chemistry 020, R. R. Martin 1. Thermochemistry Heat is a form of energy - which may take many forms: - Kinetic energy due to motion, ½ mv 2 - Potential energy due to position - Electrical
Problem 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;
CHEM-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.
THE ENERGY OF THE UNIVERSE IS CONSTANT.
Chapter 6 Thermochemistry.notebook Chapter 6: Thermochemistry Jan 29 1:37 PM 6.1 The Nature of Energy Thermodynamics: The study of energy and its interconversions Energy: the capacity to do work or to
Chapter 3 PROPERTIES OF PURE SUBSTANCES
Thermodynamics: An Engineering Approach Seventh Edition Yunus A. Cengel, Michael A. Boles McGraw-Hill, 2011 Chapter 3 PROPERTIES OF PURE SUBSTANCES Copyright The McGraw-Hill Companies, Inc. Permission
Chemistry 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
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
Chapter 11. Thermochemistry. 1. Let s begin by previewing the chapter (Page 292). 2. We will partner read Pages
Chapter 11 Thermochemistry 1. Let s begin by previewing the chapter (Page 292). 2. We will partner read Pages 293-94 The Flow of energy - heat Thermochemistry concerned with the heat changes that occur
Chapter 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
Phase 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
ENTHALPY CHANGE CHAPTER 4
ENTHALPY CHANGE CHAPTER 4 ENTHALPY Is the total energy of a system. E k = Kinetic energy. Vibrational Rotational Translational E due to motion H = E k + E p E P = Potential energy Attractive force b/w
Chapter 3 PROPERTIES OF PURE SUBSTANCES
Thermodynamics: An Engineering Approach Seventh Edition in SI Units Yunus A. Cengel, Michael A. Boles McGraw-Hill, 2011 Chapter 3 PROPERTIES OF PURE SUBSTANCES Copyright The McGraw-Hill Companies, Inc.
2 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
CHEMISTRY & YOU Chapter 17 Thermochemistry 17.1 The Flow of Energy 17. Measuring and Expressing Enthalpy Changes 17.3 Heat in Changes of State 17.4 Calculating Heats of Reaction Why does sweating help
= 1906J/0.872deg = 2186J/deg
Physical Chemistry 2 2006 Homework assignment 2 Problem 1: he heat of combustion of caffeine was determined by first burning benzoic acid and then caffeine. In both cases the calorimeter was filled with
12. 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
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
Chapter 17. Free Energy and Thermodynamics. Chapter 17 Lecture Lecture Presentation. Sherril Soman Grand Valley State University
Chapter 17 Lecture Lecture Presentation Chapter 17 Free Energy and Thermodynamics Sherril Soman Grand Valley State University First Law of Thermodynamics You can t win! The first law of thermodynamics
Chem 75 Winter, 2017 Practice Exam 1
This was Exam 1 last year. It is presented here with, first, just the problems and then with the problems and their solutions. YOU WILL BENEFIT MOST if you attempt first just the problems as if you were
1. III only 2. II, III. 3. II only. 4. I only 5. I, III. 6. I, II, III correct
Version 001 EXAM 8 PRACTICE PROBLEMS chemistry (78712) 1 This print-out should have 20 questions. Multiple-choice questions may continue on the next column or page find all choices before answering. 001
1 Which of the following compounds has the lowest solubility in water? (4 pts)
version: 516 Exam 1 - Sparks This MC portion of the exam should have 19 questions. The point values are given with each question. Bubble in your answer choices on the bubblehseet provided. Your score is
Exam 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.
Thermochemistry-Part 1
Brad Collins Thermochemistry-Part 1 Chapter 7 Thermochemistry Thermodynamics: The study of energy Thermochemistry: The study of energy in chemical reactions Energy: The capacity to do work Work = force
Entropy. Spontaneity. Entropy. Entropy mol of N 2 at 1 atm or 1 mol of N 2 at atm. process a process that occurs without intervention
Entropy Spontaneity process a process that occurs without intervention can be fast or slow Entropy (s) the measure of molecular randomness or disorder Think of entropy as the amount of chaos Entropy Predict
FORMULA SHEET (tear off)
FORMULA SHEET (tear off) N A = 6.022 x 10 23 C = ( 5 / 9 ) ( F - 32) F = ( 9 / 5 )( C) + 32 1 amu = 1.661 x 10-27 kg C = K - 273.15 K = C + 273.15 1 atm = 760 torr = 760 mm Hg 1 atm = 1.013 bar pv = nrt
Chemistry Heat Review. Heat: Temperature: Enthalpy: Calorimetry: Activation energy:
Chemistry Heat Review Name Date Vocabulary Heat: Temperature: Enthalpy: Calorimetry: Activation energy: Formulas Heat of phase change Heat for temperature increase Heat of reaction Endothermic/Exothermic
= = 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
Vapor Pressure of Liquids Equilibria and Thermodynamics
Chemistry 1B-Foothill College Vapor Pressure of Liquids Equilibria and Thermodynamics In this exercise, you will investigate the relationship between the vapor pressure of a liquid and the thermodynamic
Chapter 8 Thermochemistry
William L Masterton Cecile N. Hurley http://academic.cengage.com/chemistry/masterton Chapter 8 Thermochemistry Edward J. Neth University of Connecticut Outline 1. Principles of heat flow 2. Measurement