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PX312-1718 ____ 1. What is the solubility product expression for Th(IO3)4? A) Ksp = [Th4+][4IO3–]4 B) Ksp = [Th4+][IO3–] C) Ksp = [Th][IO3]4 D) Ksp = [Th4+][IO3–]4 E) Ksp = [Th4+][IO3–] ____ 2. What is the solubility product expression for La2(CO3)3? A) Ksp = [2La3+]2[3CO32–]3 B) Ksp = [La2+]2[CO32–]3 C) Ksp = [2La3+]2[CO32–]3 D) Ksp = [2La3+][3CO32–] E) Ksp = [La3+]2[CO32–]3 ____ 3. After mixing an excess PbCl2 with a fixed amount of water, it is found that the equilibrium concentration of Pb2+ is 1.6 10–2 M. What is Ksp for PbCl2? A) 4.0 10–6 B) 1.6 10–5 C) 2.5 10–4 D) 4.8 10–2 E) 1.0 10–6 ____ 4. The solubility of lead(II) sulfate is 4.0 10–2 g/L. What is the solubility product constant for lead(II) sulfate? A) 1.7 10–8 B) 1.3 10–4 C) 1.6 10–3 D) 4.6 10–15 E) 8.9 10–12 ____ 5. The silver-ion concentration in a saturated solution of silver(I) chromate is 1.3 10–4 M. What is Ksp for silver(I) chromate? A) 2.9 10–16 B) 4.2 10–9 C) 8.8 10–12 D) 1.1 10 12 E) 1.7 10–8 ____ 6. Which of the following salts has the lowest molar solubility? A) SrCO3 (Ksp = 9.3 10–10) B) MnS (Ksp = 2.5 10–10) C) BaF2 (Ksp = 1.0 10–6) D) BaSO4 (Ksp = 1.1 10–10) E) AgCl (Ksp = 1.8 10–10) ____ 7. Rank the following metal sulfides in order of increasing molar solubility in water. Salt CoS CuS FeS HgS MnS A) B) C) D) E) Ksp 4 10–21 6 10–36 6 10–18 1.6 10–52 2.5 10–10 MnS < FeS < CoS < CuS < HgS FeS < HgS < CoS < CuS < MnS HgS < CuS < CoS < FeS < MnS CuS < CoS < FeS < MnS < HgS CoS < CuS < FeS < HgS < MnS ____ 8. What is the molar solubility of calcium sulfate at 25°C? The solubility product constant for calcium sulfate is 2.4 10–5 at 25°C. A) 2.4 10–5 M B) 3.5 10–2 M C) 1.2 10–5 M D) 1.8 10–2 M E) 4.9 10–3 M ____ 9. What is the molar solubility of barium fluoride at 25°C? The solubility product constant for barium fluoride is 1.0 10–6 at 25°C. A) 6.3 10–3 M B) 1.0 10–6 M C) 5.0 10–7 M D) 1.0 10–3 M E) 1.6 10–2 M ____ 10. What is the pH of a saturated solution of Ni(OH)2? For Ni(OH)2, Ksp = 2.0 10–15. A) 4.80 B) 8.90 C) 5.10 D) 9.20 E) 7.00 ____ 11. The insoluble salts AV, B2W, C2X3, DY2, and EZ3, which were formed from the metal ions A+, B+, C3+, D2+, and E3+ and the nonmetals V1–, W2–, X2–, Y1–, and Z1–, all have the same Ksp value. Which salt has the highest molar solubility? A) AV B) EZ3 C) DY2 D) B2W E) C2X3 ____ 12. In which of these solutions would silver(I) carbonate have the lowest molar solubility? For silver(I) carbonate, Ksp = 8.5 10–12. A) 0.03 M H2CO3 B) 0.1 M AgNO3 C) 0.01 M AgNO3 D) 0.1 M Na2CO3 E) pure water ____ 13. What is the concentration of silver(I) ion in a saturated solution of silver(I) carbonate containing 0.0030 M Na2CO3? For Ag2CO3, Ksp = 8.6 10–12. A) 6.0 10–4 M B) 2.0 10–9 M C) 8.0 10–9 M D) 5.4 10–5 M E) 8.0 10–4 M ____ 14. What is the molar solubility of MgF2 in a 0.40 M Mg(NO3)2 solution? For MgF2, Ksp = 8.4 10–8. A) 8.0 10–8 M B) 2.3 10–4 M C) 2.0 10–-8 M D) 4.6 10–4 M E) 3.2 10–3 M ____ 15. The solubility of La(IO3)3 in a 0.62 M KIO3 solution is 1.0 10–7 mol/L. Calculate Ksp for La(IO3)3. A) 6.2 10–8 B) 2.4 10–22 C) 2.4 10–1 D) 2.4 10–8 E) none of these ____ 16. How many moles of CaF2 will dissolve in 3.0 L of 0.051 M NaF solution? (Ksp for CaF2 = 4.0 10–11) A) 2.6 10–10 B) 1.5 10–8 C) 4.6 10–8 D) 5.1 10–9 E) none of these ____ 17. Which of Figures I–IV represent(s) the result of mixing aqueous solutions of Na2S and NiCl2 in which the ion product Qc > Ksp for the insoluble product? (C = cation, A = anion) A) B) C) D) E) both I and II only I only II only III only IV ____ 18. Which of the following will apply to a saturated solution of an ionic compound? A) Qc < Ksp B) Qc > Ksp C) Qc = Ksp D) Ksp = 1 E) Qc = 1 ____ 19. To 1.0 L of water, 3.0 10–6 mol of Pb(NO3)2, 4.0 10–6 mol of K2CrO4, and 1.0 mol of NaCl are added. What will happen? Salt PbCrO4 PbCl2 A) B) C) D) E) Ksp 1.8 10–14 1.6 10–5 A precipitate of KCl will form. A precipitate of PbCrO4 will form. A precipitate of PbCl2 will form. No precipitate will form. Both a precipitate of PbCl2 and a precipitate of PbCrO4 will form. ____ 20. What will happen if 0.1 mol of solid silver(I) nitrate is added to 1.0 L of a saturated solution of silver(I) chromate? For Ag2CrO4, Ksp = 2.4 10–12. A) The AgNO3 will settle to the bottom without dissolving. B) The concentration of CrO42– will increase. C) Some Ag2CrO4 will precipitate. D) Nothing will happen. E) The concentration of Ag+ in solution will not change. ____ 21. What is the minimum mass of Na2CO3 that must be added to 24.6 mL of a 9.5 10–4 M AgNO3 solution in order for precipitation to occur? For Ag2CO3, Ksp = 8.6 10–12 . A) 2.5 10–3 g B) 3.1 10–4 g C) 1.2 10–3 g D) 2.4 10–8 g E) 2.5 10–5 g ____ 22. What is the maximum concentration of carbonate ions that will precipitate BaCO3 but not MgCO3 from a solution that is 2.7 10 3 M each in Mg2+ and Ba2+? For MgCO3, Ksp = 1.0 10–5 and for BaCO3, Ksp = 2.6 10–9. A) 3.7 10 3 M B) 9.6 10 7 M C) 2.7 10 8 M D) 7.0 10 12 M E) 2.6 10–14 M ____ 23. Which of the following solutions should be added to a solution containing both copper(II) ions and silver(I) ions in order to precipitate only one of the ions? A) HCl(aq) B) H2S(aq) C) HNO3(aq) D) H2S(aq) + HCl(aq) E) H2S(aq) + HNO3(aq) ____ 24. For which pair of cations would the addition of dilute hydrobromic acid precipitate one but not the other? A) Ag+ and Ca2+ B) Hg22+ and Ag+ C) Ba2+ and Na+ D) Ca2+ and Ba2+ E) Pb2+ and Ag+ ____ 25. Sodium chloride is added slowly to a solution that is 0.010 M in Cu+, Ag+, and Au+. The Ksp values for the chloride salts are 1.9 10–7, 1.6 10–10, and 2.0 10–13, respectively. Which compound will precipitate first? A) AuCl(s) B) All will precipitate at the same time. C) It cannot be determined. D) AgCl(s) E) CuCl(s) ____ 26. Solid KCN is added to a solution composed of 0.10 M Ag+ and 0.10 M Zn2+ just until a precipitate forms. What is the composition of this initial precipitate? AgCN Ksp = 2.2 10-16 and Zn(CN)2 Ksp = 3 10-16. A) The precipitate is pure AgCN(s). B) The precipitateis pure Zn(CN)2(s). C) The precipitate is a mixture of AgCN(s) and Zn(CN)2(s). D) The precipitate is a mixture of KCN(s) and AgCN(s). E) The precipitate is a mixture of KCN(s) and Zn(CN)2(s). ____ 27. Suppose hydrogen sulfide is added to a solution that is 0.0010 M in Fe2+, Cd2+, Co2+, and Mn2+ such that the concentration of H2S is 0.10 M. When the pH of the solution is adjusted to 3, a precipitate forms. What is the composition of the precipitate? H2S(aq) + 2H2O(l) Salt FeS CdS CoS MnS A) B) C) D) E) ____ 2H3O+(aq) + S2–(aq); Kc = 1.1 10–20 Ksp 6.0 10–18 8.0 10–27 4.0 10–21 2.5 10–10 CdS only CdS, CoS, FeS, and MnS CdS, CoS, and FeS CdS and FeS CdS and CoS 28. Suppose sodium hydroxide is added to a 0.0016 M solution of zinc nitrate such that the pH of the solution is 13.42. What is the equilibrium concentration of Zn2+? Zn2+(aq) + 4OH–(aq) A) B) C) D) E) Zn(OH)42–(aq); Kf = 2.8 1015 2.2 10–18 M 1.6 10–3 M 6.6 10–2 M 1.2 10–16 M 2.2 10–18 M ____ 29. In the sulfide scheme for qualitative analysis, the cations of Analytical Group IV are precipitated as phosphates or carbonates. Analytical Group IV consists of A) alkaline earth elements. B) the halogens. C) alkali metals. D) transition metals having +2 ions. E) none of these ____ 30. Consider a solution containing the following cations: Na+, Hg2+, Mn2+, Al3+ and Ag+. Treatment of the solution with dilute, HCl followed by saturation with H2S, results in formation of precipitate(s). Which ions still remain in solution (did not precipitate)? A) Na+, Hg2+, Al3+ B) Na+ only C) Ag+ and Hg2+ D) Ag+ only E) Na+, Al3+, and Mn2+ ____ 31. The following reaction represents a step in the separation of which analytical group of cations? Cu2+(aq) + S2–(aq) CuS(s) A) B) C) D) E) ____ Analytical Group I Analytical Group III Analytical Group V Analytical Group IV Analytical Group II 32. Which of the following statements concerning entropy change is/are true? 1. 2. 3. A) B) C) D) E) For a spontaneous process, For a spontaneous process, . . For an equilibrium process (such as a phase change), . 1 only 2 only 3 only 2 and 3 1, 2, and 3 ____ 33. The total entropy of a system and its surroundings always increases for a spontaneous process. This is a statement of A) the third law of thermodynamics. B) the law of constant composition. C) the second law of thermodynamics. D) the law of conservation of matter. E) the first law of thermodynamics. ____ 34. At the normal boiling point of o-xylene, H°vap = 36.2 kJ/mol and S°vap = 86.7 J/(molK). What is the normal boiling point of o-xylene? A) 314 K B) 373 K C) 115 K D) 867 K E) 418 K ____ 35. Which of the following is not a spontaneous process at 25°C and 1 atm pressure? A) salt dissolving B) ice melting C) water boiling D) iron rusting E) steam condensing ____ 36. For the process Cl2(g) 2Cl(g), A) H is + and S is + for the reaction. B) H is + and S = 0 for the reaction. C) H is – and S is – for the reaction. D) H is – and S is + for the reaction. E) H is + and S is – for the reaction. ____ 37. What is the change in entropy when 0.646 g of water decomposes to form hydrogen gas and oxygen gas at 298 K? 2H2O(l) 2H2(g) + O2(g); S° = 326.3 J/K at 298 K A) B) C) D) E) ____ 38. Determine G° for the following reaction: CH4(g) + 2O2(g) CO2(g) + 2H2O(l) Substance Gf° (kJ/mol) CH4(g) –50.72 O2(g) 0 CO2(g) –394.4 H2O(l) –237.4 A) B) C) D) E) ____ 5.85 J/K 0.0785 J/K 23.4 J/K 11.7 J/K 211 J/K –581.1 kJ –818.5 kJ 131.1 kJ –682.5 kJ –919.9 kJ 39. Based on the following data, what is the standard Gibbs free energy of formation of the sulfate ion at 298 K? (R = 8.31 J/(Kmol)) CaSO4(s) Substance Ca2+(aq) CaSO4(s) A) B) C) D) E) ____ Ca2+(aq) + SO42–(aq); Ksp = 2.4 10–5 G°f (kJ/mol) at 298 K –553.5 –1322.0 –768.5 kJ/mol –1849.2 kJ/mol –1875.5 kJ/mol –742.2 kJ/mol 794.8 kJ/mol 40. A certain reaction is found to be product favored. Which of the following is a correct description of the reaction? A) G° < 0, K > 1 B) G° > 0, K < 1 C) G° > 0, K > 1 D) G° < 0, K < 1 E) G° = 0, K > 1 ____ 41. The standard free energy of formation of nitric oxide, NO, at 1000. K (roughly the temperature in an automobile engine during ignition) is 78.0 kJ/mol. Calculate the equilibrium constant for the reaction 2NO(g) at 1000. K. (R = 8.31 J/(Kmol)) A) 0.95 B) 7.0 10–9 C) 1.6 105 D) –15 E) 8.4 10–5 ____ 42. Consider the following hypothetical reaction (at 316.8 K). Standard free energies, in kJ/mol, are given in parentheses. A (–32.2) B (207.8) + C (–237.0) G° = ? What is the value of the equilibrium constant for the reaction at 316.8 K? A) 0.42 B) 1.0 C) 273 D) 6.5 104 E) 0.32 ____ 43. A 0.0997 M solution of a particular monoprotic weak acid, HA, has a pH of 6.00 at 298 K. What is G° for the following equilibrium? HA(aq) + H2O(l) A) B) C) D) E) H3O+(aq) + A–(aq) 28.5 kJ 34.2 kJ 620 kJ 5.71 kJ 62.7 kJ ____ 44. The reaction CaO(s) + SO3(g) CaSO4(s) is nonspontaneous at 2200 K, whereas it is spontaneous at room temperature. Which of the following statements is false? A) The change in enthalpy is the main driving force of the reaction. B) Both H and S are negative for the reaction. C) G is negative at room temperature. D) The change in entropy is the main driving force of the reaction. E) G becomes zero at a temperature between 300 and 2200 K. ____ 45. For the reaction CaCO3(s) CaO(s) + O2(g) at 1 atm pressure, the values of H and S are both positive, and the process is spontaneous at high temperatures. Which of the following statements about this reaction is true? A) The change in entropy is the driving force for the reaction. B) The process is exothermic at high temperatures and endothermic at room temperature. C) The reverse reaction is endothermic. D) The reverse reaction is nonspontaneous at room temperature. E) G at room temperature is negative. ____ 46. Which of the following statements is true concerning the reaction below? CH4(g) + N2(g) HCN(g) + NH3(g); H° = 164.1 kJ; G° = 159.1 kJ at 298 K A) B) C) D) E) ____ It is nonspontaneous at all temperatures. It is spontaneous at relatively low temperatures only. It is spontaneous at all temperatures. It is at equilibrium at 298 K. It is spontaneous at relatively high temperatures only. 47. Which of the following statements is true for the following reaction? NH4HS(s) NH3(g) + H2S(g); H° = 93 kJ A) B) C) D) E) The reaction is not spontaneous at any temperature. The reaction is spontaneous only at relatively high temperatures. The reaction is at equilibrium under standard-state conditions. The reaction is spontaneous at all temperatures. The reaction is spontaneous only at relatively low temperatures. ____ 48. Sublimation is an example of a process for which A) H is positive and S is negative at all temperatures. B) H is negative and S is positive at all temperatures. C) H, S, and G are negative at all temperatures. D) H and S are positive at all temperatures. E) H, S, and G are positive at all temperatures. ____ 49. For the reaction reaction at 700. K? A) 1.00 B) 1.54 C) 10.1 D) 2.31 E) none of these ____ 50. Consider the following reaction: G°700K = –13.457 kJ. What is Kp for this 2C(s) + 3H2(g) C2H6(g); H° = –84.68 kJ; S° = –173.8 J/K at 298 K What is the equilibrium constant at 400.0 K for this reaction? A) 1.0 10–2 B) 2.0 104 C) 1.0 D) 9.5 101 E) 8.6 10–10 PX312-1718 Answer Section 1. ANS: OBJ: TOP: MSC: 2. ANS: OBJ: TOP: MSC: 3. ANS: OBJ: TOP: MSC: 4. ANS: OBJ: TOP: MSC: 5. ANS: OBJ: TOP: MSC: 6. ANS: OBJ: TOP: KEY: 7. ANS: OBJ: TOP: KEY: 8. ANS: OBJ: TOP: MSC: 9. ANS: OBJ: TOP: MSC: 10. ANS: OBJ: TOP: MSC: 11. ANS: OBJ: D PTS: 1 DIF: easy REF: 17.1 Write solubility product expressions. (Example 17.1) solubility | solubility equilibria KEY: solubility product constant general chemistry E PTS: 1 DIF: easy REF: 17.1 Write solubility product expressions. (Example 17.1) solubility | solubility equilibria KEY: solubility product constant general chemistry B PTS: 1 DIF: moderate REF: 17.1 Calculate Ksp from the solubility (more complicated example).(Example 17.3) solubility | solubility equilibria KEY: solubility product constant general chemistry A PTS: 1 DIF: moderate REF: 17.1 Calculate Ksp from the solubility (more complicated example).(Example 17.3) solubility | solubility equilibria KEY: solubility product constant general chemistry D PTS: 1 DIF: difficult REF: 17.1 Calculate Ksp from the solubility (more complicated example).(Example 17.3) solubility | solubility equilibria KEY: solubility product constant general chemistry D PTS: 1 DIF: easy REF: 17.1 Calculate the solubility from Ksp. (Example 17.4) solubility | solubility equilibria solubility product constant | relative solubilities MSC: general chemistry C PTS: 1 DIF: easy REF: 17.1 Calculate the solubility from Ksp. (Example 17.4) solubility | solubility equilibria solubility product constant | relative solubilities MSC: general chemistry E PTS: 1 DIF: easy REF: 17.1 Calculate the solubility from Ksp. (Example 17.4) solubility | solubility equilibria KEY: solubility product constant general chemistry A PTS: 1 DIF: easy REF: 17.1 Calculate the solubility from Ksp. (Example 17.4) solubility | solubility equilibria KEY: solubility product constant general chemistry D PTS: 1 DIF: moderate REF: 17.1 Calculate the solubility from Ksp. (Example 17.4) solubility | solubility equilibria KEY: solubility product constant general chemistry E PTS: 1 DIF: difficult REF: 17.1 Calculate the solubility from Ksp. (Example 17.4) 12. 13. 14. 15. 16. 17. 18. 19. 20. 21. TOP: solubility | solubility equilibria KEY: solubility product constant | relative solubilities MSC: general chemistry ANS: B PTS: 1 DIF: easy REF: 17.2 OBJ: Explain how the solubility of a salt is affected by another salt that has the same cation or anion (common ion). TOP: solubility | solubility equilibria KEY: solubility and the common-ion effect MSC: general chemistry ANS: D PTS: 1 DIF: moderate REF: 17.2 OBJ: Calculate the solubility of a slightly soluble salt in a solution of a common ion. (Example 17.5) TOP: solubility | solubility equilibria KEY: solubility and the common-ion effect MSC: general chemistry ANS: B PTS: 1 DIF: moderate REF: 17.2 OBJ: Calculate the solubility of a slightly soluble salt in a solution of a common ion. (Example 17.5) TOP: solubility | solubility equilibria KEY: solubility and the common-ion effect MSC: general chemistry ANS: D PTS: 1 DIF: moderate REF: 17.2 OBJ: Calculate the solubility of a slightly soluble salt in a solution of a common ion. (Example 17.5) TOP: solubility | solubility equilibria KEY: solubility and the common-ion effect MSC: general chemistry ANS: C PTS: 1 DIF: moderate REF: 17.2 OBJ: Calculate the solubility of a slightly soluble salt in a solution of a common ion. (Example 17.5) TOP: solubility | solubility equilibria KEY: solubility and the common-ion effect MSC: general chemistry ANS: D PTS: 1 DIF: moderate REF: 17.3 OBJ: State the criterion for precipitation. TOP: solubility | solubility equilibria KEY: precipitation calculations MSC: general chemistry ANS: C PTS: 1 DIF: easy REF: 17.3 OBJ: State the criterion for precipitation. TOP: solubility | solubility equilibria KEY: precipitation calculations | criterion for precipitation MSC: general chemistry ANS: B PTS: 1 DIF: easy REF: 17.3 OBJ: Predict whether precipitation will occur (given ion concentrations). (Example 17.6) TOP: solubility | solubility equilibria KEY: precipitation calculations | criterion for precipitation MSC: general chemistry ANS: C PTS: 1 DIF: easy REF: 17.3 OBJ: Predict whether precipitation will occur (given ion concentrations). (Example 17.6) TOP: solubility | solubility equilibria KEY: precipitation calculations | criterion for precipitation MSC: general chemistry ANS: E PTS: 1 DIF: moderate REF: 17.3 OBJ: Predict whether precipitation will occur (given solution volumes and concentrations). (Example 17.7) TOP: solubility | solubility equilibria 22. 23. 24. 25. 26. 27. 28. 29. 30. 31. 32. 33. KEY: ANS: OBJ: TOP: KEY: ANS: OBJ: TOP: KEY: ANS: OBJ: TOP: KEY: ANS: OBJ: TOP: KEY: ANS: OBJ: TOP: ANS: OBJ: TOP: MSC: ANS: OBJ: 17.9) KEY: ANS: OBJ: TOP: KEY: ANS: OBJ: TOP: KEY: ANS: OBJ: TOP: KEY: ANS: OBJ: ANS: OBJ: TOP: precipitation calculations | criterion for precipitation MSC: general chemistry A PTS: 1 DIF: moderate REF: 17.3 Explain how two ions can be separated using fractional precipitation. solubility | solubility equilibria precipitation calculations | fractional precipitation MSC: general chemistry A PTS: 1 DIF: easy REF: 17.3 Explain how two ions can be separated using fractional precipitation. solubility | solubility equilibria precipitation calculations | fractional precipitation MSC: general chemistry A PTS: 1 DIF: easy REF: 17.3 Explain how two ions can be separated using fractional precipitation. solubility | solubility equilibria precipitation calculations | fractional precipitation MSC: general chemistry A PTS: 1 DIF: moderate REF: 17.3 Explain how two ions can be separated using fractional precipitation. solubility | solubility equilibria precipitation calculations | fractional precipitation MSC: general chemistry A PTS: 1 DIF: moderate REF: 17.3 Explain how two ions can be separated using fractional precipitation. solubility | solubility equilibria E PTS: 1 DIF: difficult REF: 17.4 Explain the basis for the sulfide scheme to separate a mixture of metal ions. solubility | solubility equilibria KEY: effect of pH on solubility general chemistry D PTS: 1 DIF: moderate REF: 17.5 Calculate the concentration of a metal ion in equilibrium with a complex ion. (Example TOP: solubility | complex ion equilibria complex ion formation | equilibrium calculations with Kf MSC: general chemistry A PTS: 1 DIF: moderate REF: 17.7 Describe the main outline of the sulfide scheme for qualitative analysis. solubility | applications of solubility equilibria qualitative analysis of metal ions MSC: general chemistry E PTS: 1 DIF: moderate REF: 17.7 Describe the main outline of the sulfide scheme for qualitative analysis. solubility | applications of solubility equilibria qualitative analysis of metal ions MSC: general chemistry E PTS: 1 DIF: easy REF: 17.7 Describe the main outline of the sulfide scheme for qualitative analysis. solubility | applications of solubility equilibria qualitative analysis of metal ions MSC: general chemistry E PTS: 1 DIF: easy REF: 18.2 Entropy. TOP: thermochemistry | thermodynamics C PTS: 1 DIF: easy REF: 18.2 State the second law of thermodynamics in terms of system plus surroundings.. thermochemistry | thermodynamics 34. 35. 36. 37. 38. 39. 40. 41. 42. 43. 44. KEY: second law of thermodynamics | entropy MSC: general chemistry ANS: E PTS: 1 DIF: easy REF: 18.2 OBJ: Calculate the entropy change for a phase transition. (Example 18.1) TOP: thermochemistry | thermodynamics KEY: second law of thermodynamics | entropy change for a phase transition MSC: general chemistry ANS: C PTS: 1 DIF: easy REF: 18.2 OBJ: Describe how deltaH – TdeltaS functions as a criterion of a spontaneous reaction. TOP: thermochemistry | thermodynamics KEY: second law of thermodynamics | entropy and molecular disorder MSC: general chemistry ANS: A PTS: 1 DIF: moderate REF: 18.3 OBJ: Predict the sign of the entropy change of a reaction. (Example 18.2) TOP: thermochemistry | thermodynamics ANS: A PTS: 1 DIF: easy REF: 18.3 OBJ: Calculate deltaS for a reaction. (Example 18.3) TOP: thermochemistry | thermodynamics KEY: third law of thermodynamics | entropy change for a reaction MSC: general chemistry ANS: B PTS: 1 DIF: easy REF: 18.4 OBJ: Calculate deltaG from standard free energies of formation. (Example 18.5) TOP: thermochemistry | thermodynamics KEY: free energy | standard free-energies of formation MSC: general chemistry ANS: D PTS: 1 DIF: difficult REF: 18.6 OBJ: Give the relation between free energy change of a reaction and the reaction quotient. TOP: thermochemistry | thermodynamics KEY: free energy MSC: general chemistry ANS: A PTS: 1 DIF: easy REF: 18.6 OBJ: Relate the standard free-energy change to the thermodynamic equilibrium constant. TOP: thermochemistry | thermodynamics ANS: B PTS: 1 DIF: easy REF: 18.6 OBJ: Calculate K from the standard free-energy change (molecular equation). (Example 18.8) TOP: thermochemistry | thermodynamics KEY: thermodynamic equilibrium constant (K) MSC: general chemistry ANS: E PTS: 1 DIF: moderate REF: 18.6 OBJ: Calculate K from the standard free-energy change (molecular equation). (Example 18.8) TOP: thermochemistry | thermodynamics KEY: thermodynamic equilibrium constant (K) MSC: general chemistry ANS: E PTS: 1 DIF: difficult REF: 18.6 OBJ: Calculate K from the standard free-energy change (molecular equation). (Example 18.8) TOP: thermochemistry | thermodynamics KEY: thermodynamic equilibrium constant (K) MSC: general chemistry ANS: D PTS: 1 DIF: easy REF: 18.7 OBJ: Describe the how spontaneity or nonspontaneity of a reaction is related to each of the four possible choices of signs of deltaH and deltaS. TOP: thermochemistry | thermodynamics 45. 46. 47. 48. 49. 50. KEY: temperature dependence of free energy | spontaneity and temperature change MSC: general chemistry ANS: A PTS: 1 DIF: easy REF: 18.7 OBJ: Describe the how spontaneity or nonspontaneity of a reaction is related to each of the four possible choices of signs of deltaH and deltaS. TOP: thermochemistry | thermodynamics KEY: temperature dependence of free energy | spontaneity and temperature change MSC: general chemistry ANS: E PTS: 1 DIF: moderate REF: 18.7 OBJ: Describe the how spontaneity or nonspontaneity of a reaction is related to each of the four possible choices of signs of deltaH and deltaS. TOP: thermochemistry | thermodynamics KEY: temperature dependence of free energy | spontaneity and temperature change MSC: general chemistry ANS: B PTS: 1 DIF: moderate REF: 18.7 OBJ: Describe the how spontaneity or nonspontaneity of a reaction is related to each of the four possible choices of signs of deltaH and deltaS. TOP: thermochemistry | thermodynamics KEY: temperature dependence of free energy | spontaneity and temperature change MSC: general chemistry ANS: D PTS: 1 DIF: moderate REF: 18.7 OBJ: Describe the how spontaneity or nonspontaneity of a reaction is related to each of the four possible choices of signs of deltaH and deltaS. TOP: thermochemistry | thermodynamics KEY: temperature dependence of free energy | spontaneity and temperature change MSC: general chemistry ANS: C PTS: 1 DIF: easy REF: 18.7 OBJ: Calculate deltaG and K at various temperatures. (Example 18.10) TOP: thermochemistry | thermodynamics KEY: temperature dependence of free energy MSC: general chemistry ANS: D PTS: 1 DIF: difficult REF: 18.7 OBJ: Calculate deltaG and K at various temperatures. (Example 18.10) TOP: thermochemistry | thermodynamics KEY: temperature dependence of free energy MSC: general chemistry