課程名稱︰普通化學(丙)
課程性質︰森林系/心理系必修
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）︰2016/04/13
考試時限（分鐘）：120分鐘
試題 :
※註: 文中 ' = 。, 即標準狀態
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R = 0.08206 liter．atm．K^-1．mol^-1 = 8.3145 J．K^-1．mol^-1
Molar volume of ideal gas at 298.0 K = 24.60 L;
1. Name the following compounds according to IUPAC rules:
(a) HBrO (b) Na2SO3 (c) CuI2 (d) LiH (e) KH2PO4 (10%)
2. Write the formula for each of the following compounds:
(a) Nitrous acid (b) Potassium bicarbonate (c) Nitric oxide
(d) Perchloric acid (e) Tetraphosphorus decaoxide (10%)
3. How do you explain Charles's law using the postulates of
the kinetic molecular theory? (5%)
4. The mass spectrum of bromine(Br2) consists of three peaks
with the following characteristics:
┌────────┬─────────┐
│ Mass(u) │ Relative size │
├────────┼─────────┤
│ 157.84 │ 0.2534 │
├────────┼─────────┤
│ 159.84 │ 0.5000 │
├────────┼─────────┤
│ 161.84 │ 0.2466 │
└────────┴─────────┘
(a) How do you interpret these data? (5%)
(b) Calculate the average atomic mass of bromine. (5%)
5. Based on entropy, what is the second law of thermodynamics? (5%)
　　　　　　　　　　　
6. Calculate ω and △E when 1.00 mole of a liquid is vaporized at
its boiling point (80 ℃) and 1.00 atm pressure.
△Hvap for the liquid is 30.7 KJ/mol at 80℃. (10%)
7. The standard enthalpy of formation of H2O(l) at 298.0 K is
-285.8 KJ/mol. Calculate the change in internal energy for
the following process at 298.0 K and 1.000 atm:
H2O(l) → H2(g) + ½O2(g) △E'= ? (10%)
8. For ammonia (NH3), the enthalpy of fusion is 5.65 kJ/mol and
the entropy of fusion is 28.9 J/K‧mol. What is the melting
point of ammonia? (5%)
9. Consider the reaction
O2(g) → 2O(g)
Would the reaction be more spontaneous at high or low temperature?
Explain. (5%)
10.The equilibrium constant K for the reaction
2Cl(g) → Cl2(g)
Was measured as a function of temperature.
A graph of ln(K) versus 1/T for this reaction gives a straight line
with a slope of 1.352 ×10^4 K and a y-intercept of -14.51.
Determine the values of △H' and △S' for this reaction. (10%)
11.The standard free energies of formation and the standard enthalpies of
formation @ 298 K for difluoroacetylene(C2F2) & hexafluorobenzene(C6F6) are
┌─────┬────────┬─────────┐
│ 　│ △G'f(KJ/mol) │ △H'f(KJ/mol) │
├─────┼────────┼─────────┤
│ C2F2(g) │ 191.2 │ 241.3 │
├─────┼────────┼─────────┤
│ C6F6(g) │ 78.2 │ 132.8 │
└─────┴────────┴─────────┘
For the following reaction:
C6F6(g) <-> 3C2F2(g)
Calculate the equilibrium constant at 3000. K. (10%)
12.Do you expect the van der Walls constant "a" of water (H2O) to be smaller
or larger than that of methane(CH4)? Explain your answer. (5%)
13.1-Butene(C4H8) and trans-2-butene(C4H8) are isomers(異構物). They undergo
hydrogenation to give butane(C4H10) as shown below:
1-Butene + H2 → Butane △H' = -120 KJ
trans 2-Butene + H2 → Butane △H' = -115 KJ
Which will release more heat when completely burned to give CO2 and H2O,
1-butene or trans-2-butene? Explain. (5%)
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