課程名稱︰普通化學乙下 Gerneral Chemistry (b)(2) 課程性質︰必修 課程教師︰陳逸聰 開課學院：理學院 開課系所︰森林系、心理系 考試日期（年月日）︰2012年6月20日 考試時限（分鐘）：130分鐘 是否需發放獎勵金：是 試題 : 1. Consider the heterogeneous equilibrium process: C + CO ←→ 2CO (s) 2(g) (g) At 700℃, the total pressure of the system is found to be 4.50 atm. If the Equilibrium constant K is 1.52, calculate the equilibrium partial pressure of p CO and CO. (5%) 2 2. Consider the potential energy diagrams for two types of reactions A←→B. In each case, answer the following questions for the system at equilibrium. │ │ │ │ │ │ │ A ╱╲ │ │╴╴╱ ╲ │ Potential energy │ ╲ │ ╱╲ B │ ╲ B │ ╱ ╲╴╴ │ ╲╴╴ │ ╱ │ │ A ╱ │ │╴╴╱ │ │ │ │ │ │ └─────────── └─────────── Reaction progress Reaction progress (a) How would a catalyst affect the forward and reverse rates of the reaction? (2%) (b) How would a catalyst affect the energies of the reactant and product? (2%) (c) How would an increase in temperature affect the equilibrium constant? (3%) (d) If the only effect of a catalyst is to lower the activation energies for the forward and reverse reactions, show that the equilibrium constant remains unchanged if a catalyst is added to the reacting mixture. (3%) 3. A 0.0560-g quantity of acetic acid is dissolved in enough water to make + _ 50.0 mL of solution. Calculate the concentrations of H , CH COO , and CH COOH 3 3 -5 at equilibrium. (K for acetic acid = 1.8 x 10 .)(6%) a 4. Which of the following is the stronger acid: CH ClCOOH or CHCl COOH? 2 2 Explain your choice.(4%) 5. The equilibruim constant (K ) for the reaction is 4.40 at 2000K. p H + CO ←→ H O +CO 2(g) 2(g) 2 (g) (g) (a) Calculate ΔG°for the reaction.(3%) (b) Calculate ΔG for the reaction when the partial pressures are P = 0.25 H2 atm, P = 0.78 atm, P = 0.66 atm, and P = 1.20 atm. (5%) CO2 H2O CO 6. For reactions carried out under standard-state conditions, equation takes the form: ΔG°= ΔH°- TΔS°. (a) Assuming ΔH°and ΔS°are independent of temperature, derive the equation K2 ΔH° T2-T1 ㏑── = ─── (────) K1 R T1xT2 where K1 and K2 are the equilibrium constants at T1 and T2, respectively. (4%) -3 (b) Given that at 25℃ K is 4.63x10 for the reaction c N O ←→ 2NO ΔH°= 58.0 kJ/mol 2 4(g) 2(g) calculate the equilibrium constant at 65℃. (4%) 7. In the metabolism of glucose, the first step is the conversion of glucose to glucose 6-phosphate: glucose + H PO → glucose 6-phosphate + H O ΔG°=13.4 kJ/mol 3 4 2 Because ΔG°is positive, this reaction does not favor the formation of products. Show how the reaction can be made to proceed by coupling it with the hydrolysis of ATP. (a) Write an equation for the coupled reaction (2%) and (b) Estimate the equilibrium constant for the coupled process (4%). [hint: ADP + H PO → ATP + H O ΔG°= 31.0 kJ/mol] 3 4 2 8. Calculate E°, E, and ΔG for the following cell reactions. (9%) 2+ 2+ Mg + Sn → Mg + Sn (s) (aq) (aq) (s) 2+ 2+ [Mg ] = 0.045M, [Sn ] = 0.035M 2+ _ 2+ _ Sn + 2e → Sn E°= -0.14V Mg + 2e → Mg E°= -2.37V (s) (s) 9. Given that 2+ _ 2+ 2Hg + 2e → Hg E°= 0.92V (aq) 2 (aq) 2+ _ Hg + 2e → 2Hg E°= 0.85V 2 (aq) (l) Calculate ΔG°(2%) and K (4%) for the following process at 25℃: 2+ 2+ Hg → Hg + Hg 2 (aq) (aq) (l) (The preceging reaction in an example of a disproportionation reaction in which an element in one oxigation state is both oxidized and reduced.) 10. Draw structures of all geometric and optical isomers of each of these cobalt complexes: + (a) [Co(NH ) Cl ] (2%) 3 4 2 3+ (b) [Co(en) ] (2%) 3- 3 (c) [Co(C O ) ] (2%) 2 4 3 3+ 11. The absorption maximum for the complex ion [Co(NH ) ] occurs at 470 nm. 3 6 (a) Predict the color of the complex. (2%) (b) Calculate the crystal field splitting in kilojoules per mole. (3%) 3+ (c) Is [Co(NH ) ] paramagnetic or diamagnetic? Why? (4%) 3 6 12. Terminology, description, and illustration (if neccessary) (a) The three laws of thermodynamics. (6%) (b) The entropy defined by L. Boltzmann and the free energy defined by J. W. Gibbs. (4%) (c) How many vibrational degree of freedom are there in a water molecule? (2%) (d) Faraday constant and Nernst equation. (4%) (e) The reduction and oxidation half-cell reactions of a commonly recognized/used battery. (3%) (f) The systematic name of [Cr(en) ]Cl . (2%) 3 3 (g) High-spin and low-spin in transition-metal complexes. (2%) Have a nice summer break! --

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