CHEM 3739 - Physical Chemistry 1 Exam II (Leskiw)

CHEM 3739 - Physical Chemistry 1 Exam II (Leskiw) - Week #...

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Unformatted text preview: Week # 1 10 11 12 13 14 15 Date AUG 25 27 29 SEPT 1 3 5 8 10 12 15 17 19 22 24 26 29 OCT 1 3 6 8 10 13 15 17 20 22 24 27 29 30 31 NOV 3 5 7 10 12 14 17 19 21 24 26 28 DEC 1 3 5 DEC 10 “$3 “$3 "‘23 "1123 “$3 "122 E “‘23 “SE 123 “$3 “‘23 “15123 “$3 "123 “‘23 TENTATIVE LECTURE SCHEDULE Chapter 1 l 1 * * * «boom WMN MN intuit LII-b4:- A1:- -J-J-J O\O\O\ *** 19 19 19 *** 20 20 20 20 1:31:31: 20 20 20 8:00 —- 10:00 am. Suggested Problems 1.12,16,17,22,37 Topics Introduction, Temperature Equations of State, Gas Laws Virial/ van der Waals Equation of state No Class Reversible / Irreversible work State Functions 2.6,8,14,15,16,17,23,24,39,40 CF, CV, Isothermal Expansion Adiabatic Expansion Enthalpy 3.4,6, 12,14,15,16,19,31,32 Spontaneity, Entropy Carnot Cycle ASE“, Entropy of mixing EXAM I: Chapters 1, 2, 3 Review! Spontaneity Spontaneity, Gibbs Energy 4.8,9,10,14,29,33,37,45,47 Maxwell Relations Chemical Potential van’t Hoff Equation 5.5,10,11,14,21,27,28 Equilibria in Single-Component Systems 6.6,10,14,15,19,30,38,39 Clapeyron Equation Clausius—Clapeyron, Phase Diagrams Gibbs Phase Rule, Binary Solutions 7.5,6,8,12,14,21,22,28,33,34 Pressure, Temperature, Composition Phase Diagrams Raoult’s Law, Azeotropes EXAM H: Chapters 4, 5, 6, 7 Review/ Electrochemical Potentials Solid/ Solid Solutions, Eutectics 8.1,5,6,9,11,12,14,18,25,33,35 Electrolytes, Redox Reactions Cell Potentials, Half-Rxns LAST DAY TO WITHDRAW WITH A "W" Nemst Equation, K5,, Mean Ionic Activity, Ionic Strength Debye-Huckel Theory Kinetic Theory of Gases 19.2,4,6,7,13,15,20,22,23,24,28,39 Maxwell Distribution, Speed Mean Free Path Diffiision, Gas Viscosity EXAM III: Chapters 7, 8, 19 Review I Introduction to Kinetics Integrated Rate Laws, Reaction Order 20.3,4,7,8,12,13,14,24,28,44,46,58 Elementary Steps, Consecutive Reactions Parallel Reactions No Class Arrhenius Equation Collision and Transition State Theory Collision and Transition State Theory FINAL EXAM (Comprehensive) Youngstown B STATE UNIVERSITY Chemistry 3739 Second Exam Fall, 2008 Dr. B.D. Leskiw 1) I} /25 6) If /15 2) 3 /20 7) I- no 3) ’2 /10 4) Q 110 5) i /10 R = 0.082058 L atm/K mol R = 8.314 J/K mol 1atm=1.01325bar 101.3J=1Latm PERIODIC CHART OF THE ELEMENTS INERT IA HA 1113 IVB VB VIB VIIB VIII 13 113 "IA IVA 17A VIA VIIA GASES 1 2 1.00797 4.0026 5 B 7 B 9 19 10.1111 12.0112 14.0067 15.9994 10.9904 20.103 1 14_ 15 1B 17 10 I I 2 9 90 20.9015 20.006 30.9730 32.0114 35.453 9.949 21 22 23 24 25 25 27 29 29 30 3 3 35 30 0.00 44.956 47.90 50.942 51.996 54.9300 55.847 50.9332 50.71 63.54 65.37 69.72 . 9 70.96 7.909 03.00 39 40 1 4 43 44 45 40 47 4B 49 5 53 . 54 2 00.905 91.22 92.906 95.94 99] 101.07 102. 05 00.4 107. 112.40 114.02 110.69 121.75 127.60 126.904 131.30 1 1.00 97 L .9 1 2. 1 3 I 535. a .7 w ... 2:}3 M 350 A In GESG) “‘0' ~11 « M 3 m IE 55 56 *57 72 73 74 75 70 77 70 79 00 B1 02 93_ : - 05 00 mfifllhflfiflwflflflflfififlflfi 132.905 137.34 130.91 170.49 100.940 103.05 106.2 190.2 192.2 195.09 195.967 200. 204.37 207.19 200.900 [210] [222] B7 88 +09 104 105 106 107 100 109 110 111 112 Hmmnmfl%wwflflfl [223] [220] [227] [261] [262] [26 [262] [255] [205] [271] [272] [277] Numbers in parenthesis “MISS *- Lanthanide Series ""“““’”‘°““"""'"‘°“ so 59 an 61 52 63 64 65 66 a? as 69 10 11 Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu 140.12 140.907 144.24 [1‘17] 150.35 151.96 157.25 150.924 162. 0 164.930 107.20 160.934 173.04 174.97 common isotope. Commission on Atomic Weights. + Actinide Series Atomic weights corrected to conform to the 1963 values of the - - 90 92 94 95 95 97 99 100 103 The group dESIUHIIIIIHS used hemm'immm‘w Th U Pu Am Cm Bk Cf Fm Lr *b‘m's‘mammbm' 23203023003 @ [242] [243) 1247) [247) {249) [253) [257] To receive full credit, Show all work for each problem. 1) Naphthalene, Clng, melts at 802°C. If the vapor pressure is 10 torr at 853°C and 40 torr at 119.30C, calculate the enthalpy of vaporization and the normal boiling point. -mp:%0;rc,;3532t1 prthRrr T|: 88,%GC I. (39%: 'l—OYF Tlexm?;c:3¢;3K w Ll OW) Qafi mg 3%.}:{15 38.8k ‘awafi Yfiffifififia tram 2) Develop an appropriate Maxwell relation to find how entropy changes as a function of volume at constant temperature for a gas that follows a van der Waals equation of state? What is the advantage dU = TdS — PdV of using Maxwell relations? dH = TdS + VdP dA = -SdT — PdV ol/l 3'5Jlepcl \/ JG?- ’5JT+VJP 4%) "(ii/>7. .u...‘ 9 \/ 3V ,3; M l. \ A n P ,f—flL Ta 0% 21—70" 0/ 1.. ortl 2 m o (-3-3- #16 (film/o ’- p h R. G; b m dG=—SdT+VdP P: nRT _an2 V—nb V2 1 r (7*) ®CD§nSitY 0f Hg (5) : 14.193 g cm'3 (9(1) p) 2 my CD 23*) (+3 P lEfl'lf) i. 3) Determine whether the solid-liquid curve on a P vs T phase diagram for pure Hg, has a positive or a negative slope? Explain briefly. AMI-1° = 2.292 kJ mol'] Normal melting point: 234.3 K @ Density 0ng a) = 13.690 g cm'3 933 m fimam laws 02. m Ix! AéusSUhObCQA/um, 4) Describe how a system at equilibrium would shift upon eh * - (K) a} 57 - re, b) temperature. A complete answer will describe appropriate equations and provide examples. n ’I J41 5) Predict the signs of AH, AS, AG of the system for the following processes at 1 atm if the normal melting point of ammonia is -77.7°C; a) ammonia solidifying at -60°C b) ammonia melting at -77.7°C c) ammonia melting at -100°C 6) Identify which of the following has a higher chemical potential. Provide reasoning for full credit. a) H20 (liq) or H20 (yap) at water’s normal boiling point. (00°C; v , a, , 1‘0] TRT [n 7“ Haodfialw [/&O(V9P)A/LQ@) #*({):/ui / 06.71.1350350 b) Benzene at 25°C, 1 bar or benzene in a 0.1 M toluene/ benzene solution at 25°C, 1 bar. 9 61 (swam/0 _ ’: . V“ {in Kb 0 ' J r ' 3\ MI + R T I - l I, . 0) Oxygeanr ozone at STP. ‘0 / ' ' M l 2.. 0. 3 on... w“ W Mn... $63 a t .u 9 a} M» i M) aw?" +RT lVlOC' < %_J . . . . . L . . 1' . 7) Non-Ideal solutions often show posmve or negatlve dev1atlons om Raoult’s law. Explam what may cause these deviations (both positive and negative) to occur. W .4; MMWW. ...
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This note was uploaded on 11/28/2011 for the course CHEM 3011 taught by Professor - during the Spring '11 term at University of Texas.

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CHEM 3739 - Physical Chemistry 1 Exam II (Leskiw) - Week #...

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