112年 - 112 臺灣綜合大學系統_學士班轉學生聯合招生考試試題：普通化學A#120232

選擇題 (32)

1. When 3.0 L of oxygen gas (O₂) reacts with 1.5 L of nitrogen gas (N₂), 3.0 L of gaseous product is formed. All volumes of gases are measured at the same temperature and pressure. What is the formula of the product? (A) NO₄ (B) NO₂ (C) N₂O₃ (D) N₂O (E) NO

2. What is the correct formula for manganese (IV) oxide? (A) MnO₄ (B) MnO₃ (C) Mg₂O₃ (D) MnO₂ (E) MgO

3. The empirical formula of styrene is CH； its molar mass is 78.1. What is the molecular formula of styrene? (A) C₆H₆ (B) C₈H₈ (C) (D) (E)

4. When the equation NH₃ + O₂ → NO + H₂O is balanced with the smallest set of integers, the sum of the coefficients is: (A) 4 (B) 12 (C) 14 (D) 19 (E) 24

5. In the following reaction, which species is the reducing agent?
(A) H+ (B) N in NO (C) Cu (D) (E) N in HNO₃

6. How much water must be added to 20.0 mL of a 9.60 M sulfuric acid solution to make a 0.480 M solution? (Assume volumes are additive.) (A) 400 mL (B) 200 mL (C) 180 mL (D) 380 mL (E) none of these

7. Consider three 1-L flasks at the same temperature and pressure. Flask A contains CO gas, flask B contains N2 gas, and flask C contains O₂ gas. Which contains the lowest density? (A) flask A (B) flask B (C) flask C (D) Two of the flasks contain gases at the same density. (E) All are the same

8. Calculate the following ratio of effusion rate at T₁ / Effusion rate at T₂ for a gas at Kelvin temperatures T₁ and T₂ where T₂= 2T₁. (A) 0.5 (B) 2.0 (C) 1.0 (D) 1/√2 (E) √2

9. Calculate the temperature at which the average kinetic energy of O₂ gas is twice that of He gas at 10.0°C. (A) 293°C (B) 20°C (C) 2.5°C (D) 40°C (E) 859°C

10. The reduction potentials for Au³+ and Ni2+ are as follows: (Hint: 96500 x 1.73 = 167,000)
Calculate △G° (at 25°C) for the reaction:
(A) -5.0 x 10² kJ (B) 5.0 x 10² kJ (C) –2140 kJ (D) 1.0 x 10³ kJ (E) −1.0 x 10³ kJ

11. To decrease the value of K for the following exothermic reaction, we should
2A(g)+B(g) ⇌ 2C(g) (A) decrease the temperature. (B) increase the temperature. (C) decrease the pressure. (D) increase the C pressure. (E) Two of these are necessary

12. Calculate the pH of the M NaOH aqueous solutions at 25°C. (A) pH ≈ 2.0 (B) pH ≈ 12 (C) pH ≈ 4.0 (D) pH ≈ 6.0 (E) pH ≈7.0

13. At 25°C, given that the Ka for HA is 3.5 x 10⁻⁸, calculate the K value for the reaction of HA with . (A) 3.5 x 10⁶ (B) 3.5 x 10⁻⁸ (C) 3.5 x 10⁻²² (D) 2.9 x 10⁻⁷ (E) none of these

14. Which of the following species is present in the greatest concentration in a 0.100 M H₂SO₄ solution in H₂O? (A) H3O⁺ (B) HSO4¯ (C) H₂SO₄ (D) SO4²¯ (E) All species have the same concentration

15. A 10-mL sample of tartaric acid () is titrated to a phenolphthalein endpoint with 20. mL of 1.0 M NaOH. What is the molarity of the acid? (A) 0.5 (B) 1.0 (C) 2.0 (D) 4.0 (E) impossible to determine

16. How many different possible triethylbenzenes exist? (A) 6 (B) 5 (C) 4 (D) 3 (E) 2

17. When heat is added to proteins, the hydrogen bonding in the secondary structure breaks apart. What are the algebraic signs of AH and AS for the denaturation process? (A) ΔΗ ＜ 0 and △S ＜ 0 (B) ΔΗ = 0 and △S ＞ 0 (C) ∆H ＞ 0 and △S ＞ 0 (D) ΔΗ ＜ 0 and △S ＞ 0 (E) ΔΗ ＞ 0 and △S ＜ 0

18. A solution containing 10. mmol of and 5.0 mmol of is titrated with 1.0 M HCl. What volume of HCl must be added to reach the first equivalence point? (A) 5.0 mL (B) 10.0 mL (C) 15.0 mL (D) 20.0 mL (E) 25.0 mL

19. A radioactive isotope of vanadium, , decays by producing β particles and gamma rays. The nuclide formed has the atomic number. (A) 52 (B) 54 (C) 23 (D) 22 (E) 24

20. The number of a certain radioactive nuclide present in a sample decays from 2.41 x 10² to 6.02 x 10¹ in 30 minutes. What is the half-life of this radioactive species? (A) 2.0 x 10¹ minutes (B) 2.4 x 10² minutes (C) 1.5 x 10¹ minutes (D) 6.0 x 10² minutes (E) 1.0 x 10¹ minutes

21. Which of the following complexes shows geometric isomerism? (A) [Co(H₂O)₅Cl]SO₄ (B) [Co(H₂O)₆]Cl₃ (C) [Co(H₂O)₅Cl]Cl₂ (D) K[Co(H₂O)₂Cl₄] (E) Na₃ [CoCl₆]

22. How many unpaired electrons are there in the complex ion ? For this ion, the nitrate ligands produce a very strong crystal field. (Co: [Ar]4s²3d⁷) (A) 1 (B) 2 (C) 3 (D) 4 (E) 5

23. What ions are very important for the proper functioning of biologic systems, such as nerves and muscles? (A) alkali metal ions (B) nitrogen ions (C) oxygen ions (D) sulfur ions (E) alkaline earth metal ions

24. What is the expected osmotic pressure, in torr, of a 0.0100 M solution of NaCl in water at 25°C? (1.0 atm = 760 torr) (A) 0.245 torr (B) 0.495 torr (C) 374 torr (D) 187 torr (E) 561 torr

25. How many of the following molecules and ions contain double or triple bonds?
N₂；H₂CO；C₂H₄ ；C₂H₆；SCN^- (A) 1 (B) 2 (C) 3 (D) 4 (E) 5

26. How many acceptable and equivalent resonance structures can be drawn for NO₃¯? (A) 0 (B) 1 (C) 2 (D) 3 (E) 4

27. Which of the following molecules has a dipole moment? (A) SiCl₄ (B) BCl₃ (C) PCl₃ (D) Cl₂ (E) none of these

28. A certain substance, X, has a triple-point temperature of 20°C at a pressure of 2.0 atm. Which one of the following statements cannot possibly be true? (A) X can exist as a liquid above 20°C. (B) X can exist as a solid above 20°C. (C) Liquid X can exist as a stable phase at 25°C, 1 atm. (D) Both liquid and solid X have the same vapor pressure at 20°C (E) All of these statements could be true

29. Calculate △E for a system that releases 32 J of heat while 56 J of work is done on it. (A) 24 J (B) 88 J (C) -88 J (D) –24 J (E) 56 J

30. Which of the following statements is true for a monatomic ideal gas? (A) (B)= 2.5 R (C) Cv = Cp + R (D) Cv is temperature dependent (E) Cv = Cp

31. Specify the hybridization of the nitrogen atom in each of the following, in order.
(A) sp³, sp², sp² (B) sp², sp, sp² (C) sp², sp², sp² (D) sp², sp, sp (E) sp², sp, sp³

32. Identify the type of organic compound shown on right-hand side:
(A) alcohol (B) ketone (C) ether (D) aldehyde (E) ester

申論題 (5)

二、非選擇題
1. (a) Justify: at constant pressure, qp = △H. (3%)

(b) Justify: at constant temperature and pressure, △G = maximum of Wuseful (4%)

2. (a) Please derive the integrated rate law of the first-order reaction. (4%)

(b) Briefly describe how to get the activation energy of a chemical reaction. (3%)

3. Use the molecular orbital model to draw MO energy-level diagrams for predicting the magnetism and bond order of B₂ molecule. (6%)

112年 - 112 臺灣綜合大學系統_學士班轉學生聯合招生考試試題：普通化學A#120232

試卷資訊

選擇題 (32)

申論題 (5)