※ [本文轉錄自 NTU-Exam 看板] 作者: cg9313 (missing U) 看板: NTU-Exam 標題: [試題] 93上 曾文碧 普通化學甲 時間: Sun Jan 16 00:19:37 2005 課程名稱︰普通化學甲 課程性質︰ 課程教師︰曾文碧 開課系所︰大氣系 地質系 農化系 考試時間︰2005/01/14 試題 : R=0.08206 L*atm*K^-1*mol^-1 =8.3145 J*K^-1*mol^-1, 0度C=273K, Ka(HF)=7.2*10^-4, Kb(NH3)=1.8*10^-5 Van't Hoff equation: ln(K2/K1)=-(ΔH^0/R)[1/T1-1/T2] (1) For the following reaction:2 NO2 <=> N2O4 (g)+58J, in which direction will the position of the equillibrium be shifted for each of the following changes (10%) a.He(g) is added b.N2O4(g) is added c.NO2(g) is added d.The temperrature is decreased e.The volum of container is increased (2) Calculate the pH of a 1.00M solution of HF (5%) (3) A buffered solution contains 0.20M NH3 and 0.60M solution of HN4Cl.(10%) (a) Calculate the pH of this solution, (b) Calculate the pH of the solution that results when 0.10mol of gaseous HCl is added to the buffered solution from part (a). (4) Calculate the pH of a 1.0M NaH2PO4 (For H3PO4, Ka1=7.5*10^-3, Ka2=6.2*10^-8, Ka3=4.8*10^-13) (5%) (5) Briefly state the three laws of thermodynamics. (9%) (6) Why is ΔH odtained directly from the heat flow using a coffee cup calorimeter and ΔE odtained directly from the heat flow using a bomb calorimeter? (6%) (7) Consider 2.00 mol oh a monatomic ideal gas that is taken from state A (Pa=2.00 atm, Va=10.0 L) to state B (Pb=1.00 atm, Vb=30.0 L) by two different patways: Pathway one: step 1:(Pa=2.00 atm, Va=10.0 L)→(Pc=2.00 atm, Vc=30.0 L) step 2:(Pc=2.00 atm, Vc=30.0 L)→(Pb=1.00 atm, Vb=30.0 L) Pathway two: step 3:(Pa=2.00 atm, Va=10.0 L)→(Pd=1.00 atm, Vd=10.0 L) step 4:(Pd=1.00 atm, Vd=10.0 L)→(Pb=1.00 atm, Vb=30.0 L) (a) Calculate q, w, ΔE, and ΔH for each of the 4 steps. (16%) (b) Calculate q, w, ΔE, and ΔH for both patways. (8%) (c) Among q, w, ΔE, and ΔH, which two are state functions? Why? (4%) (8) For the following process:H20(l) → H2O(s), one expects that ΔS<0. In the real world, water spontaneously freezes at -10度C. Why? [Give a reasonnable interpretation on the basis of the second law of thermodynamics.] (6%) (9) Consider the reaction: 2SO2(g) + O2(g) → 2SO3(g) carried out at 25度C and 1 atm. calculate ΔH^0 , ΔS^0 , and ΔG^0 ,using the following data. (6%) ________________________________________________________ Substance ΔHf^0(kJ*mol^-1) ΔS^0 (j*k^-1*mol^-1) --------------------------------------------------------- SO2(g) -297 248 SO3(g) -396 257 O2(g) 0 205 _________________________________________________________ (10) The value of Kp=3.7*10^-6 at 900K for the ammonia synthesis reaction. Assuming the value of ΔH^0 for this reaction is -92kJ, calculate the value of Kp at 600K. (6%) (11) A 1.50mol sample of an ideal gas is allowed to expand adiabatcally and reversibly to twice its original volime. In the expansion the temperature dropped from 296K to 239K. Calculate ΔE^0 and ΔH^0 for the gas expansion. (8%) (12) When most biological enzymes are heated, they lose their catalytic activity, the change: Original enzymes → new form that occurs upon heating is endothermic and spontaneous. Is the structure of the original enzymes or its new formmore ordered? Explain your answer. (5%) --

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