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59-240 Physical Chemistry - Question Set #8 - Lecture 8 - v. 2.1 - updated Oct. 14, 2018Assigned questions for Lecture 8 are listed below (there are two sets). The questions occur in thefollowing editions of “Physical Chemistry” by P.W. Atkins:11th edition10th edition9th edition8th editionNote: The letter “P” in front of a number indicates that the question is in the “Problem” categoryas opposed to the “Exercise” category in Atkins’ books. Updates are highlighted in yellow. Thisquestion set is a bit unusual in comparison to the previous sets in that the majority of theseproblems have disappeared from the 10th and 11th editions without explanation.Question 8.01n/an/a2.62.6Question is missing from the 10th edition.2.6(a) (8th, 9th) A sample of 1.00 mol H2O(g) is condensed isothermally and reversibly to liquidwater at 100 C. The standard enthalpy of vaporization of water at 100 C is40.656 kJ mol 1. Find w, q, ΔU, and ΔH for this process.2.6(b) (8th, 9th) A sample of 2.00 mol CH3OH(g) is condensed isothermally and reversibly toliquid at 64 C. The standard enthalpy of vaporization of methanol at 64 C is 35.3 kJ mol 1. Findw, q, ΔU, and ΔH for this process.Question 8.02n/an/a2.162.16Question is missing from the 10th edition.2.16(a) (8th, 9th) A certain liquid has ΔvapH 26.0 kJ mol-1. Calculate q, w, ΔH, and ΔU when0.50 mol is vaporized at 250 K and 750 Torr.2.16(b) (8th, 9th) A certain liquid has ΔvapH 32.0 kJ mol-1 . Calculate q, w, ΔH, and ΔUwhen 0.75 mol is vaporized at 260 K and 765 Torr.University of Windsor - Department of Chemistry and Biochemistry - R.W. Schurko1
59-240 Physical Chemistry - Question Set #8 - Lecture 8 - v. 2.1 - updated Oct. 14, 2018Question 8.03n/an/a2.1720.21(b only)Question is missing from the 10th and 11th editions, and only the b-list question is given in the8th edition for some reason.2.17(a) (9th) Calculate the lattice enthalpy of SrI2 from the following data:2.17(b) (8th, 9th) Calculate the lattice enthalpy of MgBr2 from the following data:Question 8.04n/an/an/an/aOld 7th edition question.(Ex. 2.31a, 7th Ed.) Calculate the standard enthalpy of hydrogenation of 1-hexene to hexanegiven that the standard enthalpy of combustion of 1-hexene is -4003 kJ mol-1.(Ex. 2.31b, 7th Ed.) Calculate the standard enthalpy of hydrogenation of 1-butene to butane giventhat the standard enthalpy of combustion of 1-butene is -2717 kJ mol-1.Question 8.052C.22C.22.182.172C.2(a) The standard enthalpy of formation of ethylbenzene is 12.5 kJ mol-1. Calculate itsstandard enthalpy of combustion.2C.2(b) The standard enthalpy of formation of phenol is 165.0 kJ mol-1. Calculate its standardenthalpy of combustion.University of Windsor - Department of Chemistry and Biochemistry - R.W. Schurko2
59-240 Physical Chemistry - Question Set #8 - Lecture 8 - v. 2.1 - updated Oct. 14, 2018Question 8.06P2C.3, P2C.42C.32.192.18P2C.3(a) The standard enthalpy of combustion of cyclopropane is 2091 kJ mol-1 at 25 C. Fromthis information and enthalpy of formation data for CO2(g) and H2O(g), calculate the enthalpy offormation of cyclopropane. The enthalpy of formation of propene is 20.42 kJ mol-1. Calculatethe enthalpy of isomerization of cyclopropane to propene.P2C.4(b) From the following data, determine for diborane, B2H6(g), at 298 K:Question 8.072C.42C.52.22.192C.4(a) When 120 mg of naphthalene, C10H8(s), was burned in a bomb calorimeter thetemperature rose by 3.05 K. Calculate the calorimeter constant. By how much will thetemperature rise when 150 mg of phenol, C6H5OH(s), is burned in the calorimeter under the sameconditions?2C.4(b) When 225 mg of anthracene, C14H10(s), was burned in a bomb calorimeter thetemperature rose by 1.75 K. Calculate the calorimeter constant. By how much will thetemperature rise when 125 mg of phenol, C6H5OH(s), is burned in the calorimeter under the sameconditions? Note: In the 8th/9th editions, the mass of anthracene is 2.25 mg.Question 8.08n/an/a2.212.2Question is missing from the 10th and 11th editions.2.21(a) (9th), 2.22(a) (8th) Calculate the standard enthalpy of solution of AgCl(s) in water fromthe enthalpies of formation of the solid and the aqueous ions.2.21(b) (9th), 2.22(b) (8th) Calculate the standard enthalpy of solution of AgBr(s) in water fromthe enthalpies of formation of the solid and the aqueous ions.Question 8.09n/an/an/an/aOld 7th edition question.(Ex. 2.39a, 7th Ed.) Use the standard enthalpies of formation to calculate the standard enthalpiesof the following reactions:(a) 2NO2 (g) N2O4 (g)(b) NH3 (g) HCl (g) NH4Cl (g)University of Windsor - Department of Chemistry and Biochemistry - R.W. Schurko3
59-240 Physical Chemistry - Question Set #8 - Lecture 8 - v. 2.1 - updated Oct. 14, 2018(Ex. 2.39b, 7th Ed.) Use the standard enthalpies of formation to calculate the standard enthalpiesof the following reactions:(a) cyclopropane (g) propene (g)(b) HCl (aq) NaOH (aq) NaCl(aq) H2O (aq)Question 8.10n/an/a2.222.21Question is missing from the 10th edition.2.22(a) (9th), 2.23 (8th) The standard enthalpy of decomposition of the yellow complex H3NSO2into NH3 and SO2 is 40 kJ mol-1. Calculate the standard enthalpy of formation of H3NSO2.2.22(a) (9th), 2.23 (8th) Given that the standard enthalpy of combustion of graphite is 393.51 kJ mol-1 and that of diamond is 395.41 kJ mol-1, calculate the enthalpy of the graphiteto-diamond transition.Question 8.11n/an/a2.262.25Question is missing from the 10th edition.2.26(a) (9th), 2.25(a) (8th). Use the information in Table 2.2 (Appendix, 8th & 9th)/Table 2B.1(Appendix 10th, 11th) to predict the standard reaction enthalpy of 2 NO2(g) N2O4(g) at 100 Cfrom its value at 25 C. Assume that the heat capacities are constant over this temperature range.2.26(b) (9th), 2.25(b) (8th). Use the information in Table 2.2 (Appendix, 8th & 9th)/Table 2B.1(Appendix 10th, 11th) to predict the standard reaction enthalpy of 2 H2(g) O2(g) 2 H2O(l) at100 C from its value at 25 C. Assume that the heat capacities are not constant over thistemperature range, and are parameterized as Cp,m a bT c /T 2.Question 8.122C.72C.82.272.262C.7(a). From the data in the appendix tables, calculate ΔrH and ΔrU at (a) 298 K, (b) 478 Kfor the reaction C(graphite) H2O(g) CO(g) H2(g). Assume all heat capacities to beconstant over the temperature range of interest.Note: the temperature for (b) in the 10th edition is 378 K - not sure why they changed it.2C.7(b). Calculate ΔrH and ΔrU at 298 K and ΔrH at 427 K for the hydrogenation of ethyne(acetylene) to ethene (ethylene) from the enthalpy of combustion and heat capacity data in theappendix tables. Assume the heat capacities to be constant over the temperature range involved.Note: In the 8th/9th editions the temperature is 348 K.University of Windsor - Department of Chemistry and Biochemistry - R.W. Schurko4
59-240 Physical Chemistry - Question Set #8 - Lecture 8 - v. 2.1 - updated Oct. 14, 2018Question 8.13n/an/a2.282.272.28(a) (9th), 2.29(a) (8th). Calculate ΔrH for the reaction Zn(s) CuSO4(aq) ZnSO4(aq) Cu(s) from the information in the appendix tables.2.28(a) (9th), 2.29(a) (8th). Calculate ΔrH for the reaction NaCl(aq) AgNO3(aq) AgCl(s) NaNO3(aq) from the information in the appendix tables.Question 8.14n/a2C.102.292.282C.10(a) Set up a thermodynamic cycle for determining the enthalpy of hydration of Mg2 ionsusing the following data: enthalpy of sublimation of Mg(s), 167.2 kJ mol-1; first and secondionization enthalpies of Mg(g), 7.646 eV and 15.035 eV; dissociation enthalpy of Cl2(g), 241.6kJ mol-1; electron gain enthalpy of Cl(g), 3.78 eV; enthalpy of solution of MgCl2(s), 150.5 kJmol-1; enthalpy of hydration of Cl (g), 383.7 kJ mol-1.2C.10(b) Set up a thermodynamic cycle for determining the enthalpy of hydration of Ca2 ionsusing the following data: enthalpy of sublimation of Ca(s), 178.2 kJ mol-1; first and secondionization enthalpies of Ca(g), 589.7 kJ mol-1 and 1145 kJ mol-1; enthalpy of vaporization ofbromine, 30.91 kJ mol-1; dissociation enthalpy of Br2(g), 192.9 kJ mol-1; electron gainenthalpy of Br(g), 331.0 kJ mol-1; enthalpy of solution of CaBr2(s), 103.1 kJ mol-1; enthalpy ofhydration of Br (g), 289 kJ mol-1.Note: This question is missing from only the 11th edition. Not sure why!University of Windsor - Department of Chemistry and Biochemistry - R.W. Schurko5
59-240 Physical Chemistry - Question Set #8 - Lecture 8 - v. 2.1 - updated Oct. 14, 2018Solution 8.01n/an/a2.62.6University of Windsor - Department of Chemistry and Biochemistry - R.W. Schurko6
59-240 Physical Chemistry - Question Set #8 - Lecture 8 - v. 2.1 - updated Oct. 14, 2018Solution 8.02n/an/a2.162.16University of Windsor - Department of Chemistry and Biochemistry - R.W. Schurko7
59-240 Physical Chemistry - Question Set #8 - Lecture 8 - v. 2.1 - updated Oct. 14, 2018Solution 8.03n/an/a2.1720.21(b only)University of Windsor - Department of Chemistry and Biochemistry - R.W. Schurko8
59-240 Physical Chemistry - Question Set #8 - Lecture 8 - v. 2.1 - updated Oct. 14, 2018Solution 8.04n/an/an/an/a(Ex. 2.31b, 7th Ed.)University of Windsor - Department of Chemistry and Biochemistry - R.W. Schurko9
59-240 Physical Chemistry - Question Set #8 - Lecture 8 - v. 2.1 - updated Oct. 14, 2018Solution 8.08n/an/a2.212.2n/an/an/aSolution 8.09n/a(Ex. 2.39b, 7th Ed.)!University of Windsor - Department of Chemistry and Biochemistry - R.W. Schurko10
59-240 Physical Chemistry - Question Set #8 - Lecture 8 - v. 2.1 - updated Oct. 14, 2018Solution 8.10n/an/a2.222.21University of Windsor - Department of Chemistry and Biochemistry - R.W. Schurko11
59-240 Physical Chemistry - Question Set #8 - Lecture 8 - v. 2.1 - updated Oct. 14, 2018Solution 8.11n/an/a2.262.25University of Windsor - Department of Chemistry and Biochemistry - R.W. Schurko12
59-240 Physical Chemistry - Question Set #8 - Lecture 8 - v. 2.1 - updated Oct. 14, 2018Solution 8.13n/an/a2.282.27University of Windsor - Department of Chemistry and Biochemistry - R.W. Schurko13
59-240 Physical Chemistry - Question Set #8 - Lecture 8 - v. 2.1 - updated Oct. 14, 2018Solution 8.14n/a2C.102.292.28University of Windsor - Department of Chemistry and Biochemistry - R.W. Schurko14
59-240 Physical Chemistry - Question Set #8 - Lecture 8 - v. 2.1 - updated Oct. 14, 2018University of Windsor - Department of Chemistry and Biochemistry - R.W. Schurko15
59-240 Physical Chemistry - Question Set #8 - Lecture 8 - v. 2.1 - updated Oct. 14, 2018 Question 8.06 P2C.3(a) The standard enthalpy of combustion of cyclopropane is 2091 kJ mol-1 at 25 C. From this information and enthalpy of formation data for CO
