Liquids and Solutions
|
|
- Amberlynn Daniel
- 6 years ago
- Views:
Transcription
1 Liquids and Solutions Introduction This course examines the properties of liquids and solutions at both the thermodynamic and the molecular level. The main topics are: Liquids, Ideal and Regular Solutions, Polymer Solutions, and Electrolyte Solutions. This question sheet covers each of these topics. Suggested Reading 1. Dr Bob Thomas has an excellent website with sample questions, quizzes, and tutorial pages including interactive Java applets at: 2. P. W. Atkins, Physical Chemistry, any edition, OUP. 3. Murrell, J. N. and Jenkins, A. D., Properties of Liquids and Solutions, 2nd ed., Wiley, D. J. Walton and J. P. Lorimer, Polymers, OUP Primer 85, K. A. Dill and S. Bromberg, Molecular Driving Forces, Garland, Notation and Common Pitfalls Units and accuracy As ever, give your answers to an appropriate number of significant figures, with their correct units, and label the axes of your graphs clearly. This can be particularly tricky when deducing polymer molecular masses and virial coefficients, so take extra care here. Diagrams Parts of the Liquids and Solutions course are quite descriptive - illustrate your answers to descriptive questions with clear labelled diagrams wherever possible. Notes Make your own notes for use in revision on the following topics. Don t hand them in. Ideal liquid solutions; Raoult s law; Henry s law. Non-ideal liquid solutions; excess enthalpy and Gibb s energy of mixing; regular solutions; immiscibility. The radial distribution function. Polymer solutions; the random-walk model; self-avoidance; the Flory- Huggins model of polymer solution thermodynamics; the van t Hoff equation and its derivation; the polymer virial coefficient.
2 Electrolyte solutions; Debye-Hückel theory and its application; implications for solubility: salting-in and the common-ion effect. Questions 1. [ls2-i] (a) What is an ideal solution? (b) Show that the Gibbs free energy of mixing and entropy of mixing of two liquids to form an ideal solution of mole fractions x A and x B is mix G = nrt (x A ln x A + x B ln x B ), mix S = nr(x A ln x A + x B ln x B ), where n = n A + n B is the total amount of solution resulting from n A of liquid A and n B moles of liquid B. (c) What mole fractions give the maximum entropy of mixing? Explain why an ideal solution is always miscible. (d) What are the main features of a regular solution? Give expressions for mix H, mix S, and mix G for a regular solution. (e) Define the parameter β that appears in the theory of regular solutions in terms of the pairwise interactions between its components, H AA, H BB and H AB. (f) For a regular solution, the first and second derivatives of mix G m with respect to mole fraction vanish at the upper critical solution temperature (UCST), T c, above which all compositions of the solution are miscible. Writing mix G m in terms of x A alone: mix G m = RT (x A ln x A + (1 x A ) ln(1 x A )) + βx A (1 x A ), evaluate the second derivative at x A = 1 2 to show that T c = β 2R. (g) The excess free energy of mixing of an equimolar mixture of acetonitrile and CCl 4 is 1190 J mol 1 at 45 C. Assuming that the mixture behaves as a regular solution, calculate the UCST. 2. [ls2-d] How is the activity of a solution defined? Show by writing a A = γ A x A, that mix G has the same form as that of a regular solution if the activity coefficients satisfy the Margules equations: RT ln γ A = βx 2 B RT ln γ B = βx 2 A. Hence show that the partial pressure of A is given by p A = x A e β(1 xa)2 /RT p A. Determine the limits of p A as x A 1 and x A 0 and sketch p A vs. x A for a solution with β > 0, commenting on the limiting behaviour in relation to Raoult s law and Henry s law.
3 3. [ls2-f] (a) What is the osmotic pressure, Π, of a solution? Derive the van t Hoff equation, stating your assumptions: Π = [B]RT, where [B] = n B /V is the molar concentration of the solute, B. (b) In practice, the known concentration is in terms of the mass of polymer dissolved in a known volume of solvent, c, e.g. in g dm 3. If M is the molar mass of the polymer, show that Π c = RT M. (c) For dilute polymer solutions, the deviation from ideality is such that the osmotic pressure has to be written as a virial expansion: Π c = RT (1 + Bc +...) M The table below shows values of the osmotic pressure for a solution of a given sample of poly(styrene) at two different temperatures: c /kg m T = 320 K Π/ N m T = 330 K Π/ N m By plotting a suitable graph, determine the molar mass of the polymer and values for the second virial coefficient, B, at the two temperatures. (d) Explain why B migh vary with temperature and, assuming that B varies linearly with temperature over the range 300 to 340 K, calculate the Flory θ-temperature for poly(styrene) in this solvent. 4. [ls2-a: Q2003.Adv.Q4.solutions] (a) The chemical potential of a monovalent electrolyte, M + X, in solution satisfies µ = µ + 2RT ln γ ± (m/m ) where ln γ ± is given by the Debye-Hückel limiting law as ln γ ± 2.303A I. (i) Define the term I, the ionic strength, in this equation. (ii) Given that A is proportional to (ɛt ) 3/2, where ɛ is the relative permittivity of the solvent and T is the temperature, show that I µ µ ideal C ɛ 3 T, where C is a positive constant.
4 (iii) Use the formula in part (ii) to deduce the circumstances for which the Debye limiting law will be most accurate. (b) Use your understanding of the physical basis of Debye-Hückel theory to explain why µ µ ideal : (i) is negative, (ii) increases in magnitude with increasing ionic strength, (iii) decreases in magnitude with increasing solvent permittivity, and (iv) decreases in magnitude with increasing temperature. (c) EMF measurements in water and in methanol at 298 K lead to the values of the mean activity coefficient, γ ±, of HCl shown in the following table. 5. [ls2-b] water methanol m = 0.002m m = 0.005m m = 0.008m (i) Show that the Debye-Hückel limiting law is valid for both solvents at these molalities. (ii) Given that the relative permittivity of water is 78.6 at 298 K, calculate the relative permittivity of methanol. (iii) The Debye length λ, which is often taken as a measure of the radius of the ionic atmosphere surrounding an ion, is proportional to ɛ/i, where ɛ and I are as above. Given that λ is approximately 10 nm in an aqueous solution of monovalent electrolyte M + X of molality 0.001m, use your result from (c)(ii) to calculate the values of λ for HCl in water and in methanol at a molality of 0.008m. Comment on the results that you obtain. The Random Flight Model is the simplest model for describing the conformations of polymer chains in a solution. A polymer is treated as consisting of N segments, each of which is characterized by a vector l k of length l. In the Random Flight Model, the orientations of these segments are random, i.e. l j l k = 0 where j and k are two different segments. The vector R connecting the two ends of the polymer is R = N l k. k=1 (a) Show that the mean square distance between the two ends can be written R 2 = R R = Nl 2 (b) Calculate the predicted value, in the Random Flight Model, of the root-mean-square end-to-end distance, R 2 1/2 for polyethylene oxide of molecular weight 10 6 u, taking the segment to be (CH 2 CH 2 O) with a molecular weight of 44 u and a length of 0.36 nm.
5 (c) The value of R 2 1/2 inferred from light scattering is 110 nm. Comment on the Random Flight Model in the light of this value. In the previous question you assumed that each monomer unit was a random flight segment - how many monomer units actaully comprise a random flight segment? 6. [ls2-h] (a) What is meant by the radial distribution function for a liquid or a solid? Sketch and explain the form of the radial distribution functions you would expect for the following: (i) Solid Argon, (ii) Liquid Argon, (iii) An ideal gas. (b) The position of the first peak in the radial distribution funtion, r, the first ionization energy, I, and the polarizability, α, for the liquid states of Ne, Ar, and Xe are given in the table below. r /nm I /kj mol 1 α /10 3 nm 3 Ne Ar Xe The magnitude of the interaction between pairs of these atoms is given by the London formula as U = 3α 2 I 4r 6. Explain the origin of this formula and calculate U for pairs of Ne, Ar, and Xe atoms at their distance of closest approach. (c) Taking the entropy of vaporization of Xe to be vap S (Xe) = 80 J K 1 mol 1 and its boiling point to be T b (Xe) = 166 K, calculate the enthalpy of vaporization of Xe, vap H (Xe). Also calculate vap U (Xe). Estimate the co-ordination number in liquid xenon. (d) Assuming the same co-ordination numbers, estimate the boiling points of Ar and Ne. [Hint: Trouton s rule]. Answers to Selected Questions 1. (g) K 3. (d) K 4. (c) (ii) 32.4 (iii) λ H2O(0.008m ) = nm, λ MeOH (0.008m ) = nm 5. (b) 54.3 nm, (c) s = (c) vap H = 13.3 kj mol 1, vap U = 11.9 kj mol 1, z = 12; (d) 27 K, 89 K
Liquids and Solutions
Liquids and Solutions Physical Chemistry Tutorials Mark Wallace, Wadham College mark.wallace@chem.ox.ac.uk CRL Floor 1 Office 1 Phone (2)75467 Taken from Thomas Group Website, Problems 1. The answers are
More informationLiquids and Solutions Crib Sheet
Liquids and Solutions Crib Sheet Determining the melting point of a substance from its solubility Consider a saturated solution of B in a solvent, A. Since the solution is saturated, pure solid B is in
More informationLecture 6. NONELECTROLYTE SOLUTONS
Lecture 6. NONELECTROLYTE SOLUTONS NONELECTROLYTE SOLUTIONS SOLUTIONS single phase homogeneous mixture of two or more components NONELECTROLYTES do not contain ionic species. CONCENTRATION UNITS percent
More informationSimple Mixtures. Chapter 7 of Atkins: Section
Simple Mixtures Chapter 7 of Atkins: Section 7.5-7.8 Colligative Properties Boiling point elevation Freezing point depression Solubility Osmotic Pressure Activities Solvent Activity Solute Activity Regular
More information5.4 Liquid Mixtures. G i. + n B. = n A. )+ n B. + RT ln x A. + RT ln x B. G = nrt ( x A. ln x A. Δ mix. + x B S = nr( x A
5.4 Liquid Mixtures Key points 1. The Gibbs energy of mixing of two liquids to form an ideal solution is calculated in the same way as for two perfect gases 2. A regular solution is one in which the entropy
More informationm m 3 mol Pa = Pa or bar At this pressure the system must also be at approximately 1000 K.
5. PHASES AND SOLUTIONS n Thermodynamics of Vapor Pressure 5.. At equilibrium, G(graphite) G(diamond); i.e., G 2 0. We are given G 2900 J mol. ( G/ P) T V V 2.0 g mol.95 0 6 m 3 mol Holding T constant
More informationBrief reminder of the previous lecture
Brief reminder of the previous lecture partial molar quantities: contribution of each component to the properties of mixtures V j V = G µ = j n j n j pt,, n pt,, n dg = Vdp SdT + µ dn + µ dn +... A A B
More informationChapter 11 Review Packet
Chapter 11 Review Packet Name Multiple Choice Portion: 1. Which of the following terms is not a quantitative description of a solution? a. molarity b. molality c. mole fraction d. supersaturation 2. Which
More informationChapter 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 informationLECTURE 6 NON ELECTROLYTE SOLUTION
LECTURE 6 NON ELECTROLYTE SOLUTION Ch 45.5 pplied Phy Chem First Sem 2014-15 Ch 45.5 Exam II September 1/3 (Multiple Choice/Problem Solving) Coverage: Second/Third Laws of Thermodynamics Nonelectrolyte
More informationGeneral Physical Chemistry I
General Physical Chemistry I Lecture 14 Aleksey Kocherzhenko April 9, 2015" Last time " Chemical potential " Partial molar property the contribution per mole that a substance makes to an overall property
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 informationFIRST PUBLIC EXAMINATION SUBJECT 3: PHYSICAL CHEMISTRY
CCHE 4273 FIRST PUBLIC EXAMINATION Trinity Term 2005 Preliminary Examination in Chemistry SUBJECT 3: PHYSICAL CHEMISTRY Wednesday June 8 th 2005, 9:30am Time allowed: 2 ½ hours Candidates should answer
More information7 Simple mixtures. Solutions to exercises. Discussion questions. Numerical exercises
7 Simple mixtures Solutions to exercises Discussion questions E7.1(b For a component in an ideal solution, Raoult s law is: p xp. For real solutions, the activity, a, replaces the mole fraction, x, and
More informationChemistry 452/ August 2012
Chemistry 45/456 7 August 0 End- of-term Examination Professor G. Drobny Enter your answers into a blue or green Composition Book. Perform only the number of problems required. Answers must be given in
More informationActivities and Activity Coefficients
CHEM 331 Physical Chemistry Fall 017 Activities and Activity Coefficients We now finish answering the question we asked during our last lecture, what is the form of the chemical potential i (T,P,x i )
More informationSubject : Chemistry Class : XII Chapter-2.Solutions Work Sheet ( WS 2. 1) Topic- 2.1 Henry s & Raoult s Laws
Work Sheet ( WS 2. 1) Topic- 2.1 Henry s & Raoult s Laws Name -. Class/ sec.. Roll No.. A. Fill in the blanks: 1. Solutions are mixtures of two or more than two components. 2. Generally, the component
More informationThermodynamics IV - Free Energy and Chemical Equilibria Chemical Potential (Partial Molar Gibbs Free Energy)
Thermodynamics IV - Free Energy and Chemical Equilibria Chemical Potential (Partial Molar Gibbs Free Energy) increase in the Gibbs free energy of the system when 1 mole of i is added to a large amount
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 information70 Example: If a solution is m citric acid, what is the molar concentration (M) of the solution? The density of the solution is 1.
70 Example: If a solution is 0.688 m citric acid, what is the molar concentration (M) of the solution? The density of the solution is 1.049 g/ml molality definition molarity definition To solve the problem,
More informationChapter 4 Polymer solutions
Chapter 4 Polymer solutions 4.1 Introduction Solution: any phase containing more than one component.(gas, liquid or solid) Polymer solution is important: Classical analyses of polymers are conducted on
More information(name) Place the letter of the correct answer in the place provided. Work must be shown for non-multiple choice problems
(name) Place the letter of the correct answer in the place provided. Work must be shown for non-multiple choice problems 1. According to Raoults Lab the change in the vapor pressure of a solution containing
More informationconcentration of solute (molality) Freezing point depression constant (for SOLVENT)
74 FREEZING POINT DEPRESSION concentration of solute (molality) Freezing point depression constant (for SOLVENT) Freezing point depression: The amount the freezing temperature is LOWERED by the solute.
More informationReview of differential and integral calculus and introduction to multivariate differential calculus.
Chemistry 2301 Introduction: Review of terminology used in thermodynamics Review of differential and integral calculus and introduction to multivariate differential calculus. The properties of real gases:
More informationChem 260 Quiz - Chapter 4 (11/19/99)
Chem 260 Quiz - Chapter 4 (11/19/99) Name (print) Signature Terms in bold: phase transitions transition temperature phase diagram phase boundaries vapor pressure thermal analysis dynamic equilibrium boiling
More information- Applications: In chemistry, this effect is often used to determine the molecular weight of an unknown molecule.
73 FREEZING POINT DEPRESSION concentration of solute (molality) Freezing point depression constant (for SOLVENT) Freezing point depression: The amount the freezing temperature is LOWERED by the solute.
More informationSOLUTIONS. Chapter Test B. A. Matching. Column A. Column B. Name Date Class. 418 Core Teaching Resources
16 SOLUTIONS Chapter Test B A. Matching Match each term in Column B to the correct description in Column A. Write the letter of the correct term on the line. Column A Column B 1. the number of moles of
More informationOverview. Types of Solutions. Intermolecular forces in solution. Concentration terms. Colligative properties. Osmotic Pressure 2 / 46
1 / 46 2 / 46 Overview Types of Solutions. Intermolecular forces in solution Concentration terms Colligative properties Osmotic Pressure 3 / 46 Solutions and Colloids A solution is a homogeneous mixture
More informationKEMS448 Physical Chemistry Advanced Laboratory Work. Freezing Point Depression
KEMS448 Physical Chemistry Advanced Laboratory Work Freezing Point Depression 1 Introduction Colligative properties are properties of liquids that depend only on the amount of dissolved matter (concentration),
More informationChapter 11 Properties of Solutions
Chapter 11 Properties of Solutions Solutions Homogeneous mixtures of two or more substances Composition is uniform throughout the sample No chemical reaction between the components of the mixture Solvents
More informationCHEMISTRY 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
More informationSOLUBILITY AS AN EQUILIBRIUM PHENOMENA
SOLUBILITY AS AN EQUILIBRIUM PHENOMENA Equilibrium in Solution solute (undissolved) solute (dissolved) Solubility A saturated solution contains the maximum amount of solute that will dissolve in a given
More informationPhysical Chemistry Chapter 4 The Properties of Mixtures
Physical Chemistry Chapter 4 The Properties of Mixtures by Izirwan Bin Izhab FKKSA izirwan@ump.edu.my Chapter Description Aims Determine the fugacity and fugacity coefficients for pure species using generic
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 informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Chapter 13 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) The process of solute particles being surrounded by solvent particles is known as. A)
More informationThe 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 informationFreezing point depression - The freezing temperature of a SOLUTION gets lower as the CONCENTRATION of a solution increases.
73 COLLIGATIVE PROPERTIES - properties unique to solutions. - depend only on the CONCENTRATION of a solution and not the IDENTITY of the solute** **ionic solutes: Remember that they dissociate into MULTIPLE
More informationChemistry 201: General Chemistry II - Lecture
Chemistry 201: General Chemistry II - Lecture Dr. Namphol Sinkaset Chapter 14 Study Guide Concepts 1. Solutions are homogeneous mixtures of two or more substances. 2. solute: substance present in smaller
More informationDATA THAT YOU MAY USE UNITS Conventional Volume ml or cm 3 = cm 3 or 10-3 dm 3 Liter (L) = dm 3 Pressure atm = 760 torr = Pa CONSTANTS
DATA THAT YOU MAY USE UNITS Conventional S.I. Volume ml or cm 3 = cm 3 or 0-3 dm 3 Liter (L) = dm 3 Pressure atm = 760 torr =.03 0 5 Pa torr = 33.3 Pa Temperature C 0 C = 73.5 K PV L-atm =.03 0 5 dm 3
More informationCHEMICAL THERMODYNAMICS
CHEMICAL THERMODYNAMICS Basic Theory and Methods Sixth Edition IRVING M. KLOTZ Morrison Professor Emeritus Northwestern University ROBERT M. ROSENBERG MacMillen Professor Emeritus Lawrence University Visiting
More informationBushra Javed Valencia College CHM 1046 Chapter 12 - Solutions
Bushra Javed Valencia College CHM 1046 Chapter 12 - Solutions 1 Chapter 12 :Solutions Tentative Outline 1. Introduction to solutions. 2. Types of Solutions 3. Solubility and the Solution Process: Saturated,
More informationChapter 13. Ions in aqueous Solutions And Colligative Properties
Chapter 13 Ions in aqueous Solutions And Colligative Properties Compounds in Aqueous Solution Dissociation The separation of ions that occurs when an ionic compound dissolves H2O NaCl (s) Na+ (aq) + Cl-
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 informationChapter Solutions. MockTime.com. (a) M urea (b) 0.01 M KNO3 (c) 0.01 M Na2 SO4 (d) M glucose Ans: (c)
47 Chapter Solutions 1. Freezing point of an aqueous solution is ( 0.186) C. Elevation of boiling point of the same solution is K b = 0.512 C,Kf = 1.86 C, find the increase in boiling point. [2002] (a)
More informationGENERAL CHEMISTRY II CHM202 Unit 1 Practice Test Solutions
GENERAL CHEMISTRY II CHM202 Unit 1 Practice Test Solutions 1. Which one of the following substances is expected to have the highest boiling point? D) I2 Since these are all nonpolar ecules, the only interecular
More informationCHEM 1032 PRACTICE EXAM I CLASS SPRING 2017
1 CHEM 1032 PRACTICE EXAM I CLASS SPRING 2017 1. Select the characteristic(s) of the liquid phase: (You may need a periodic table. Useful information appears on page 5.) (i) adopts the shape of the container
More information(B) Which of the following in each pair will be more soluble in water?
CHM 112 Chapter 11 Solutions: Study Guide Purpose: This is a guide for your as you work through the chapter. The major topics are provided so that you can write notes on each topic and work the corresponding
More informationColligative Properties. Vapour pressure Boiling point Freezing point Osmotic pressure
Colligative Properties Vapour pressure Boiling point Freezing point Osmotic pressure Learning objectives Describe meaning of colligative property Use Raoult s law to determine vapor pressure of solutions
More informationUse your time wisely. Do not get stuck on one question. WORK MUST BE SHOWN CAREFULLY, WITH UNITS AT EVERY STEP OF SETUP.
Spring 2014 CCBC-Catonsville (Wed 3/12/14) Use your time wisely. Do not get stuck on one question. WORK MUST BE SHOWN CAREFULLY, WITH UNITS AT EVERY STEP OF SETUP. PAGE TOTAL SCORE POSSIBLE YOUR SCORE
More informationSolution. Types of Solutions. Concentration and Solution Stoichiometry
Concentration and Solution Stoichiometry Solution homogenous mixture of 2 or more pure substances only one perceptible phase species do not react chemically Types of Solutions solid liquid gas Solutions
More informationx =!b ± b2! 4ac 2a moles particles solution (expt) moles solute dissolved (calculated conc ) i =
Properties of Solution Practice Exam Solutions Name (last) (First) Read all questions before you start. Show all work and explain your answers. Report all numerical answers to the proper number of sig.
More information75 A solution of 2.500g of unknown dissolved in g of benzene has a freezing point of C. What is the molecular weight of the unknown?
75 A solution of 2.500g of unknown dissolved in 100.0 g of benzene has a freezing point of 4.880 C. What is the molecular weight of the unknown? Solving for Cm (molality) will allow us to calculate how
More informationUnit - 2 SOLUTIONS VSA QUESTIONS (1 - MARK QUESTIONS) 1. Give an example of liquid in solid type solution.
Unit - 2 SOLUTIONS VSA QUESTIONS (1 - MARK QUESTIONS) 1. Give an example of liquid in solid type solution. 2. Which type of solid solution will result by mixing two solid components with large difference
More informationANSWERS CIRCLE CORRECT SECTION
CHEMISTRY 162 - EXAM I June 08, 2009 Name: SIGN: RU ID Number Choose the one best answer for each question and write the letter preceding it in the appropriate space on this answer sheet. Only the answer
More informationChapter 13 Properties of Solutions
Chapter 13 Properties of Solutions Learning goals and key skills: Describe how enthalpy and entropy changes affect solution formation. Describe the relationship between intermolecular forces and solubility,
More informationBig Idea Three Topics
Big Idea Three Topics 1. Molecular, Ionic, Net Ionic Equations 2. Stoichiometry 3. Synthesis, Decomposition Reactions 6. Chemical Change Evidence 7. Endothermic & Exothermic Reactions 8. Electrochemistry
More informationChem 1100 Pre-Test 3. Multiple Choice Identify the choice that best completes the statement or answers the question.
Chem 1100 Pre-Test 3 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. An open-tube manometer is used to measure the pressure in a flask. The atmospheric
More information(for tutoring, homework help, or help with online classes)
www.tutor-homework.com (for tutoring, homework help, or help with online classes) 1. Elemental iodine (I 2 ) is a solid at room temperature. What is the major attractive force that exists among different
More informationOFB Chapter 6 Condensed Phases and Phase Transitions
OFB Chapter 6 Condensed Phases and Phase Transitions 6-1 Intermolecular Forces: Why Condensed Phases Exist 6- The Kinetic Theory of Liquids and Solids 6-3 Phase Equilibrium 6-4 Phase Transitions 6-5 Phase
More informationCHEMISTRY 102 FALL 2010 EXAM 1 FORM D SECTION 502 DR. KEENEY-KENNICUTT PART 1
NAME CHEMISTRY 102 FALL 2010 EXAM 1 FORM D SECTION 502 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 informationModern Chemistry Chapter 12- Solutions
Modern Chemistry Chapter 12- Solutions Section 1- Types of Mixtures Solutions are homogeneous mixtures of two or more substances in a single phase. Soluble describes a substance as capable of being dissolved.
More informationPAPER No.6: PHYSICAL CHEMISTRY-II (Statistical
Subject PHYSICAL Paper No and Title Module No and Title Module Tag 6, PHYSICAL -II (Statistical 34, Method for determining molar mass - I CHE_P6_M34 Table of Contents 1. Learning Outcomes 2. Introduction
More informationChapter 10: CHM 2045 (Dr. Capps)
Phase Diagram Phase diagrams for CO 2 and H 2 O Chapter 13. Solutions and Their Physical Properties Shows pressures and temperatures at which gaseous, liquid, and solid phases can exist. Allows us to predict
More informationSoluble: A solute that dissolves in a specific solvent. Insoluble: A solute that will not dissolve in a specific solvent. "Like Dissolves Like"
Solutions Homogeneous Mixtures Solutions: Mixtures that contain two or more substances called the solute and the solvent where the solute dissolves in the solvent so the solute and solvent are not distinguishable
More informationChapter 11 Problems: 11, 15, 18, 20-23, 30, 32-35, 39, 41, 43, 45, 47, 49-51, 53, 55-57, 59-61, 63, 65, 67, 70, 71, 74, 75, 78, 81, 85, 86, 93
Chapter 11 Problems: 11, 15, 18, 20-23, 30, 32-35, 39, 41, 43, 45, 47, 49-51, 53, 55-57, 59-61, 63, 65, 67, 70, 71, 74, 75, 78, 81, 85, 86, 93 Chapter 11 Properties of Solutions Types of mixtures: homogenous
More informationPLEASE DO NOT MARK ON THE EXAM. ALL ANSWERS SHOULD BE INDICATED ON THE ANSWER SHEET. c) SeF 4
Chem 130 EXAM 4 Fall 99 PLEASE DO NOT MARK ON THE EXAM. ALL ANSWERS SHOULD BE INDICATED ON THE ANSWER SHEET QUESTIONS 1-5 MAY HAVE MORE THAN ONE POSSIBLE ANSWER CIRCLE ALL CORRECT RESPONSES TO EACH QUESTION
More informationCHEMISTRY 102 FALL 2010 EXAM 1 FORM C SECTION 502 DR. KEENEY-KENNICUTT PART 1
NAME CHEMISTRY 102 FALL 2010 EXAM 1 FORM C SECTION 502 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 informationOutline of the Course
Outline of the Course 1) Review and Definitions 2) Molecules and their Energies 3) 1 st Law of Thermodynamics Conservation of Energy. 4) 2 nd Law of Thermodynamics Ever-Increasing Entropy. 5) Gibbs Free
More informationTrinity Term Preliminary Examination in Physical Sciences SUBJECT 3: CHEMISTRY 3: PHYSICAL CHEMISTRY. also
FIRST PUBLIC EXAMINATION Trinity Term 2000 Preliminary Examination in Physical Sciences SUBJECT 3: CHEMISTRY 3: PHYSICAL CHEMISTRY also Preliminary Examination in Molecular and Cellular Biochemistry Wednesday,
More information1 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
More informationStudyHub: AP Chemistry
StudyHub+ 1 StudyHub: AP Chemistry Solution Composition and Energies, Boiling Point, Freezing Point, and Vapor Pressure StudyHub+ 2 Solution Composition: Mole Fraction: Formula: Mole Fraction of Component
More informationColligative Properties
Slide 1 Colligative Properties Practical uses of solutions Slide 2 Solution homogeneous mixtures composition may vary from one sample to another appears to be one substance, though really contains multiple
More informationUniversity of Washington Department of Chemistry Chemistry 452/456 Summer Quarter 2014
Lecture 9 8//4 University of Washington Department of Chemistry Chemistry 45/456 Summer Quarter 04. Solutions that re Very, Very on-ideal In the prior lectures on non-ideal solution behavior, we have considered
More informationChem 1100 Pre-Test 3. Multiple Choice Identify the choice that best completes the statement or answers the question.
Chem 1100 Pre-Test 3 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Determine the oxidation number of the underlined element in K 2CO 3. a. 1 b. 2 c.
More informationVAPOR PRESSURE LOWERING - Described by RAOULT'S LAW
73 VAPOR PRESSURE LOWERING - Described by RAOULT'S LAW partial pressure of the VAPOR of solvent molecules. mole fraction of component A vapor pressure of pure component A (depends on temperature) partial
More informationLet's look at the following "reaction" Mixtures. water + salt > "salt water"
Mixtures What happens to the properties (phase changes) when we make a solution? Let's look at the following "reaction" water + salt ------> "salt water" Which has the higher entropy? A. The water + the
More informationColligative properties CH102 General Chemistry, Spring 2011, Boston University
Colligative properties CH12 General Chemistry, Spring 211, Boston University here are four colligative properties. vapor-pressure lowering boiling-point elevation freezing-point depression osmotic pressure
More informationThinking Like a Chemist About Solution Properties UNIT 5 DAY 4
UNIT5-DAY4-LaB1230 Page 1 UNIT5-DAY4-LaB1230 Wednesday, January 23, 2013 5:43 PM Thinking Like a Chemist About Solution Properties UNIT 5 DAY 4 What are we going to learn today? Thinking Like a Chemist
More informationChem GENERAL CHEMISTRY II MIDTERM EXAMINATION
Concordia University CHEM 206 Winter 2009, Dr. C. Rogers, Section 01 LAST NAME: FIRST NAME: STUDENT ID: Chem 206 - GENERAL CHEMISTRY II MIDTERM EXAMINATION INSTRUCTIONS: PLEASE READ THIS PAGE WHILE WAITING
More informationMixtures. What happens to the properties (phase changes) when we make a solution? Principles of Chemistry II. Vanden Bout
Mixtures What happens to the properties (phase changes) when we make a solution? Let's look at the following "reaction" water + salt ------> "salt water" Which has the higher entropy? A. The water + the
More information2011, Robert Ayton. All rights reserved.
Solutions Outline 1. Solubility 2. Concentration Calculations 3. Colligative Properties 4. Freezing Point Depression or Boiling Point Elevation Problems 5. Graphs of Colligative Properties Review 1. Solubility
More informationPX-III Chem 1411 Chaps 11 & 12 Ebbing
PX-III Chem 1411 Chaps 11 & 12 Ebbing 1. What is the name for the following phase change? I 2 (s) I 2 (g) A) melting B) condensation C) sublimation D) freezing E) vaporization 2. Which of the following
More informationPSI AP Chemistry: Solutions Practice Problems
PSI AP Chemistry: Solutions Practice Problems Name Solutions: Mixtures, Solubility and Concentration Classwork 1. A student determined that there were 0.032 grams of oxygen gas dissolved in a 200.0 ml
More informationName CHM 1051 Spring 2018 February 4 EXAMINATION ONE TENTATIVE SOLUTIONS I II III IV V
Name CHM 1051 Spring 2018 February 4 EXAMINATION ONE TENTATIVE SOLUTIONS I II III IV V Total Glance over the entire exam, and then attempt the problems in the order of your choice. Rough point values are
More informationChapter 11 section 6 and Chapter 8 Sections 1-4 from Atkins
Lecture Announce: Chapter 11 section 6 and Chapter 8 Sections 1-4 from Atkins Outline: osmotic pressure electrolyte solutions phase diagrams of mixtures Gibbs phase rule liquid-vapor distillation azeotropes
More informationSolutions and Their Properties
Chapter 11 Solutions and Their Properties Solutions: Definitions A solution is a homogeneous mixture. A solution is composed of a solute dissolved in a solvent. When two compounds make a solution, the
More informationClass XII Chapter 2 Solutions Chemistry
Class XII Chapter 2 Solutions Chemistry Question 2.1: Calculate the mass percentage of benzene (C 6 H 6 ) and carbon tetrachloride (CCl 4 ) if 22 g of benzene is dissolved in 122 g of carbon tetrachloride.
More informationFinal Exam Review-Honors Name Period
Final Exam Review-Honors Name Period This is not a fully comprehensive review packet. This packet is especially lacking practice of explanation type questions!!! You should study all previous review sheets
More informationa) 1.3 x 10 3 atm b) 2.44 atm c) 8.35 atm d) 4.21 x 10-3 atm e) 86.5 atm
1. (6 pts) A sample of gas with a volume of 750 ml exerts a pressure of 756 mm Hg at 30.0 0 C. What pressure (atm) will the sample exert when it is compressed to 250 ml and cooled to -25.0 0 C? a) 1.3
More informationChemistry Grade : 11 Term-3/Final Exam Revision Sheet
Chemistry Grade : 11 Term-3/Final Exam Revision Sheet Exam Date: Tuesday 12/6/2018 CCS:Chem.6a,6b,6c,6d,6e,6f,7a,7b,7d,7c,7e,7f,1g Chapter(12):Solutions Sections:1,2,3 Textbook pages 378 to 408 Chapter(16):Reaction
More informationSalinity Gradients for Sustainable Energy: Primer, Progress, and Prospects
Supporting Information Salinity Gradients for Sustainable Energy: Primer, Progress, and Prospects Ngai Yin Yip *,, Doriano Brogioli, Hubertus V. M. Hamelers, and Kitty Nijmeijer Department of Earth and
More informationChapter 12. Properties of Solutions
Chapter 12. Properties of Solutions What we will learn: Types of solutions Solution process Interactions in solution Types of concentration Concentration units Solubility and temperature Solubility and
More informationWarm up. 1. What is a solution? 2. What is a solute? 3. What is a solvent?
Warm up 1. What is a solution? 2. What is a solute? 3. What is a solvent? Solutions Chapter 12.2 Solubility The amount of substance that can dissolve at a given temperature to produce a saturated solution
More informationAqueous Solutions (When water is the solvent)
Aqueous Solutions (When water is the solvent) Solvent= the dissolving medium (what the particles are put in ) Solute= dissolved portion (what we put in the solvent to make a solution) Because water is
More informationChapter 13. Properties of Solutions
Chapter 13 Properties of Solutions Warm - Up Why doesn t salt dissolve in nonpolar solvents such as hexane? How does the orientation of water around Na + differ from the orientation of water around Cl
More informationCOLLIGATIVE PROPERTIES. Engr. Yvonne Ligaya F. Musico 1
COLLIGATIVE PROPERTIES Engr. Yvonne Ligaya F. Musico 1 Colligative Properties Properties that depend on the collective effect of the number of solute particles. Engr. Yvonne Ligaya F. Musico 2 COLLEGATIVE
More informationChem. 112 spring 2012 Exam 1 7:30am/Odago Wednesday March 7, 2012
Chem. 112 spring 2012 Exam 1 7:0am/Odago Wednesday March 7, 2012 Attempt all the questions and fill in your answers correctly on the scantron provided 1. A particular gas exerts a pressure of 4.6 atm.
More information1) Define the following terms: a) solution, b) miscible, c) hydration, d) percent by mass (solute), e) colligative property, f) hypotonic.
Problems - Chapter 13 (with solutions) 1) Define the following terms: a) solution, b) miscible, c) hydration, d) percent by mass (solute), e) colligative property, f) hypotonic. a) solution - A homogeneous
More informationColligative Properties
Slide 1 Colligative Properties Practical uses of solutions Slide 2 Units of Concentration Whatever units you use, the goal is the same: specify the quantity of 1 component (the solute s ) relative to the
More informationSolutions: Formation and Properties
New Jersey Center for Teaching and Learning Slide 1 / 48 Progressive Science Initiative This material is made freely available at www.njctl.org and is intended for the non-commercial use of students and
More information