課程名稱︰普通化學甲上 課程性質︰化工系必修 課程教師︰蔡蘊明 開課學院：理學院 開課系所︰化學系 考試日期（年月日）︰2020/1/8 考試時限（分鐘）：110 試題 : 1. Describe in brief the second law of thermodynamics related to chemical reactions. (5%) 2. Ammonium nitrate (NH4NO3) dissolves spontaneously and endothermically in water at room temperature. What can you deduce about the sign of ΔS for this solution process? Explain your answer. (5%) 3. The following diagram shows the structure of fully protonated glutamic acid and the corresponding pKa values. O O ∥ H2 H2 H ∥ HO─C─C─C─C─C─OH ←─pKa=2.19 ↑ │ │ NH3 ←─pKa=9.67 │ + pKa=4.25 (a) What is the PI value of glutamic acid? (3%) (b) Running an electrophoresis experiment in a buffered solution with pH=7.4, will glutamic acid move toward the positive or negative electrode? Explain your answer. (2%) 4. Consider the titration of 40.0 mL of 0.200M HOCl (Ka=3.50e-8) with 0.100M KOH. Calculate [H+] after the following volumes of KOH have been added. (a) 40.0 mL (2%) (b) 80.0 mL (3%) 5. Kf for the complex ion Ag(NH3)2 + is 1.7e7, Ksp for AgCl is 1.6e-10. Calculate the molar solubility of AgCl in 1.0M NH3. (10%) 6. Calculate Ksp for iron(II) sulfide given the following data: FeS(s) + 2e- → Fe(s) + S 2-(aq) ξ°=-1.01V Fe 2+(aq) + 2e- → Fe(s) ξ°=-0.440V (10%) 7. Consider the galvanic cell based on the following half-reactions: Au 3+(aq) + 3e- → Au(s) ξ°=1.50V Tl+(aq) + e- → Tl(s) ξ°=-0.34V (a) Calculate ΔG° and K for the cell reaction at 25℃. (6%) (b) Calculate ξcell at 25℃ when [Au 3+]=1.0e-2M and [Tl+]=1.0e-4M (4%) 8. Consider the process A(l) at 75℃ → A(g) at 155℃ which is carried out at constant pressure. The total ΔS for this process is known to be 75.0 J．K^(-1)．mol^(-1). For A(l) and A(g), Cp values are 75.0 J．K^(-1)．mol^(-1) and 29.0 J．K^(-1)．mol^(-1), respectively, and are not dependent on temperature. (a) Calculate ΔH_vaporization for A(l) at 125℃ (its boiling point). (7%) (b) Calculate ΔG_vaporization for A(l) at 125℃. (3%) 9. The equilibrium constant for a certain reaction decreases from 8.84 to 3.25e-2 when the temperature increases from 25℃ to 75℃. Calculate ΔH° and ΔS° for this reaction. (10%) 10. A sample of 2.00 moles of H2 (Cv=20.5 J．K^(-1)．mol^(-1)) at 25℃ and 1.50 atm undergoes a reversible adiabatic compression until the final pressure is 4.50 atm. Assume that the gas behaves ideally, calculate the final volume, w, ΔE, ΔH, and ΔS. (15%) 11. Knowing S° of H2 to be 131 J．K^(-1)．mol^(-1). (a) Calculate the entropy of 2.00 moles of H2 at 25℃ and 1.50 atm. (5%) (b) Calculate ΔG for question 10. (5%) 12. The following table listed the molar enthalpy of combustion for several alkanes. Predict the molar enthalpy of combustion for cyclohexane. Show your rational. (5%) Name Formula Structure ΔH°comb(kJ/mol) ────────────────────────────────── Pentane C5H12 CH3(CH2)3CH3 -3.509 Hexane C6H14 CH3(CH2)4CH3 -4.163 Heptane C7H16 CH3(CH2)5CH3 -4.817 Octane C8H18 CH3(CH2)6CH3 -5.471 H2C─CH2 ／ ＼ Cyclohexane C6H12 H2C CH2 ? ＼ ／ H2C─CH2 --

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