77. What are the signs (+, –, or 0) of ΔH, ΔS, and ΔG for the spontaneous vaporization of a liquid to a vapor?
(A) (ΔH, ΔS, ΔG) = (+, +, +)
(B) (ΔH, ΔS, ΔG) = (+, –, +)
(C) (ΔH, ΔS, ΔG) = (0, 0, 0)
(D) (ΔH, ΔS, ΔG) = (+, +, –)
(E) (ΔH, ΔS, ΔG) = (–, – , –)

73. At a certain temperature, placing one mole of ammonia gas into a sealed container results in 40% ammonia decomposition at equilibrium. What is the equilibrium constant KC for ammonia decomposition at that temperature? (ammonia decomposition: 2NH3(g) → N2(g) + 3H2(g)) (A) 0.043 (B) 0.12 (C) 0.80 (D) 8.33 (E) 17

74. Complete the Lewis structure for the molecular formula (C5H7ON) below. This molecule has _____ single bonds, _____ multiple bonds and ____ sp2 hybridized atoms. (A) 4, 2, 2 (B) 4, 2, 4 (C) 11, 2, 2 (D) 11, 2, 4 (E) 11, 5, 4

75. A product is electroplated by copper from CuSO4 solution. A constant current of 9.65 amp is applied by an external power supply. How long will it take to deposit 6.35 × 102 g of Cu onto the surface of product? (Cu = 63.5 g/mol) (1F = 96485 C/mol) (A) 14.22 s (B) 8.9 min (C) 2.54 h (D) 55.5 h (E) 1.37 days

76. An unknown compound is cooled at 1 atm, and it freezes at 50.0 K to form Solid I. At a lower temperature, Solid I rearranges to Solid II, which has a different crystal structure. Thermal measurements show that ΔH an ΔS for the I → II phase transition are –700.0 J/mol and –20.0 J/K mol, respectively. What is the temperature of Solids I and II in equilibrium? (A) 13.6 K (B) 19.8 K (C) 35.0 K (D) 59.8 K (E) 98.2 K

78. The reduction potentials for Au3+ and Cr3+ are as follows: (A) –7.37 × 102 kJ (B) –5.79 ×102 kJ (C) –1.6 × 102 kJ (D) 7.37 × 102 kJ (E) 10 × 102 kJ

79. How many different structures do SeCl4, CBr4, KrF4, CH4, and TeF4 have? (A) 1 (B) 2 (C) 3 (D) 4 (E) 5

80. A weak acid HA is dissolved in enough water to prepare an acidic solution. The pH value and osmotic pressure of resulting solution at 27o C are 6 and 0.246 atm, respectively. What is the Ka of HA? (R = 0.082 L· atm/K·mol； assuming Van’t Hoff factor = 1) (A) 1.00 × 10–10 (B) 2.30 × 10–10 (C) 1.10 × 10–9 (D) 6.10 × 10–9 (E) 5.80 × 10–8

81. The pH of a bottle of vinegar is 2.75 at 25℃. What is the mass percentage concentration (w/w) of acetic acid in this vinegar, assuming no other acid is presented? (Ka of acetic acid: 1.8x10-5； pKa of acetic acid: 4.74； 10-2.75 = 0.0018； 102.75 = 562.3； assuming the density of vinegar = 1 g/cm3 ； CH3COOH=60 g/mol) (A) 5.0% (B) 4.0% (C) 3.0% (D) 2.0% (E) 1.0%

82. Which of the following complexes can exhibit optical isomerism? (en = H2N–CH2–CH2–NH2) (A) cis–Co(NH3)4Cl2 (B) trans–Co(en)2Br2 (C) cis–Co(en)2Cl2 (D) Co(NH3)3Cl3 (E) none of these

83. A compound has a formula of [Pt(PPh3)2(NCS)2]. How many isomers does this compound have? (A) 2 (B) 3 (C) 4 (D) 5 (E) 6