課程名稱︰普通化學丙
課程性質︰系定必修
課程教師︰鄭淑芬
開課學院：工學院
開課系所︰機械系
考試日期（年月日）︰2008/5/12
考試時限（分鐘）：110分鐘
是否需發放獎勵金：是
（如未明確表示，則不予發放）
試題 :
(一) Multiple-Choice Questions (15%, -0.5 points per mistake)
1.Which of the following species is non-polar?
(a)PF5 (b)NF3 (c)IF3 (d)SF4 (e)SiF4
2.Which of the following is a covalent compound?
(a)Na2O (b)CaCl2 (c)Cl2O (d)CsCl (e)S8
3.Which one of the following molecules and ions will have a planar geometry?
(a)PCl3 (b)BF4- (c)XeF4 (d)BrF5 (e)H3O+
4.Decide on the appropriate hybridization of phosphorus in the ion PCl4-
(Phosphorus is the central atom)
(a)sp3 (b)sp2 (c)sp (d)sp3d (e)sp3d2
5.Which of the following statements relating to molecular orbital (MO) theory
is correct?
(a)Combination of two atomic orbitals produces one bonding and one antibonding
MO.
(b)A bonding MO is lower in energy than the two atomic orbitals from which it
is formed.
(c)Combination of two 2p orbitals may result in either σ or π-MOs.
(d)A species with a bond order of zero will not be stable.
(e)In a stable molecule having an even number of electrons, all electrons must
be paired.
6.Which one, if any, of the follwing statements about the MO treatment of the
bonding in benzene is correct?
(a)MO theory uses resonance to describe the delocalized nature of the bonding
in benzene.
(b)Each pi-bonding orbital in benzene can hold up to 6 electrons.
(c)MO theory predicts that benzene should be paramagnetic.
(d)The lowest energy pi-bonding MO in benzene has two electrons forming
hexagonal lobes, above and below the plane of the carbon atoms
(e)Benzene has three pi-bonding orbitals.
7.Which of the following is true for pure oxygen gas, O2(g) at 25℃?
(a)ΔHf°=0
(b)ΔHf°<0
(c)ΔGf°=0
(d)ΔGf°<0
(e)S°>0
8.Which of the following is true for a system at equilibrium?
(a)ΔS°(sys)=ΔS°(surr)
(b)ΔS°(sys)=-ΔS°(surr)
(c)ΔH°(sys)>0
(d)ΔG°(sys)=0
(e)ΔG°(sys)<0
(二) Single Choice Questions (18%, 3 points per question)
9.Calculate ΔS°for the reaction: 2SO2(g) + O2(g) → 2SO3(g)
S° in J/mol‧K for: SO2(g)=248.1 SO3=256.6 O2(g)=205.0
(a)-537 J/mol‧K (b)+145 J/mol‧K (c)-188 J/mol‧K (d)+547 J/mol‧K
10.What is the molar solubility of CaF2? (Ksp = 3.9 * 10^-11)
(a)6.24*10^-6 M (b)4.41*10^-6 M (c)2.14*10^-4 M (d)9.27*10^-5 M
11.What is the pH of a 0.150M NaOH solution?
(a)0.82 (b)3.05 (c)11.66 (d)13.18
12.Diethyl ether, used as a solvent for extraction of organic compounds from
aqueous solutions, has a high vapor pressure which makes it a potential fire
hazard in laboratories in which it is used. How much energy is released
when 100.0g is cooled from 53.0℃ to 100.0℃?
Boiling point: 34.5℃ Heat of vaporization: 351J/g
Specific heat capacity, (CH3)2O(l): 3.74J/(g‧K)
Specific heat capacity, (CH3)2O(g): 2.35J/(g‧K)
(a)10.1kJ (b)13.1kJ (c)16.1kJ (d)45.2kJ (e)48.6kJ
13.The synthesis of the pesticide thionyl chloride (OSCl2) proceeds according
to: SO3(g) + SCl2(l) ← → OSCl2(l) + SO2(g)
If ΔG°=-106 kJ/mol for this reaction at 298K, what is the Keq at this
temperature? (R = 8.314 J/mol‧K)
(a)7.21*10^12 (b)3.50*10^14 (c)3.81*10^18 (d)1.19*10^20
14.From the values given for ΔH° and ΔS° at 298K, which of the following
reactions is spontaneous under standard conditions at 298K?
(a)2POCl3(g) → 2PCl3(g) + O2(g) ΔH°=572kJ ΔS°=179J/K
(b)N2(g) + 3F2(g) → 2NF3(g) ΔH°=-249J ΔS°=-278J/K
(c)N2(g) + 3Cl2(g) → 2NCl3(g) ΔH°=460kJ ΔS°=-275J/K
(d)N2F4(g) → 2NF2(g) ΔH°=85kJ ΔS°=198J/K
(三) Problems:
15.The equilibrium constant for NH4HS(s) ← → NH3(g) + H2S(g)
at 25℃ is Kc = 1.6*10^-4
(a)What is the Kp value at this temperature? (4%)
(b)When solid NH4HS and 0.450 mol of gaseous NH3 were placed into a 2.0L vessel
at 25℃, what are the partial pressure of NH3 and H2S at equilibrium? (4%)
(c)The van't Hoff equation shows the relationship between the equilibrium
constant and the absolute temperature: ln(K1/K2) = -(ΔH(vap)/R)(1/T1-1/T2)
Knowing that Kc is 2.96*10^-4 at 40℃, estimate the enthalpy of this
reaction. (3%)
16.CdS can form a quantum dot solution. Determine the amount of Cd2+ and S2-
left in solution if 450mL of 0.06M Cd(NO3)2 and 450mL of 0.08M Na2S are
combined. Also, determine the pH of the solution. (Ksp of CdS = 3.6*10^-29
Ka1 of H2s = 9.1*10^-8, Ka2 of H2S = 1.1*10^-12) (10%)
17.What would happen if solid AgCl were added to a saturated solution of AgI?
What are the concentrations of Ag+, Cl- and I- ions in the solution?
(Ksp of AgCl = 1.8*10^-10, Ksp of AgI = 1.5*10^-16) (10%)
18.(a)Show the molecular orbital energy-level diagram of O2, indicating the
bonding and anti-bonding orbitals. (5%)
(b)Write the valence-shell electron configurations and bond orders of O2,
O2- and O2(2-). (6%)
(c)Put the above three species in the order of increasing bond length. (2%)
(d)Which of the above three species are "paramagnetic"? (3%)
19.ZnS is a semiconductor with a band gap of 3.54eV.
(a)Draw an energy-level diagram for this material, labeling the atomic
orbitals, electron filling, valence band, conduction band and band gap.
(b)If some of the sulfur is replaced with phosphorus, the conductivity of this
material changes. Draw an energy-level diagram for the doped material
indicating the filling of electrons. Is this material an n- or p-type
semiconductor? (10%)
20.A reference book lists the following values for gallium at 298K.
────────────────────────────────────
Substance ΔHf°(kJ/mol) ΔGf°(kJ/mol) S°(J/mol K)
────────────────────────────────────
Ga(s) 0 0 x
Ga(l) 5.578 0.0888 59.25
Ga(g) 271.96 233.76 169.03
────────────────────────────────────
(a)Estimate the noraml boiling point of gallium. (4%)
(b)Gallium metal has a melting point of 29.8℃. Estimate the S° value of
Ga(s). (6%)
21.Calculate the ΔE,ΔH,ΔS,ΔG, q and w values of isothermal expansion of the
ideal gas at 298K by three different pathways. (18%)
(三個Path,圖略)
Path 1 是兩個裝有活塞的燒杯(上端有開口)，活塞上放砝碼當做下壓力。
左罐放兩個砝碼，P1=6.0atm V1=0.40L 右罐一個砝碼 P2=3.0atm V2沒給
Path 2 是兩個玻璃球，中間以附有開關的細管連接，有兩組，第一組的左球裡面是
充滿氣體，右球空，左球P1=6.0atm V1=0.40L，右球V=0.40L
第二組是開關打開，左右兩球皆有氣體，V2=V1+V
Path 3 是兩個附有活塞，可抽為真空的罐子(有蓋)，活塞上放沙子當作下壓力，將活
塞上端抽為真空，下端為氣體。
左罐沙較多，P1=6.0atm V1=0.40L 右罐沙較少，P2=3.0atm V2沒給
Useful informations:
gas constant, R = 0.08206 atm‧L/mol‧K = 8.314 J/mol‧K
Avogadro constant Na = 6.022*10^23 /mol
Planck's constant, h = 6.626*10^-34 J‧s = 6.626*10^-27 erg‧s
1 atm = 760 mmHg = 760 Torr
1 eV = 96.487 kJ/mol
Speed of light, c = 2.9979*10^8 m/s
Mass of electron = 9.109*10^-31 kg
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