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111年 - 111 國立清華大學學士後西醫學系單獨招生考試_學士後醫學系自然科學組：化學#110532

科目：學士後◆化學 | 年份：111年 | 選擇題數：30 | 申論題數：0

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所屬科目：學士後◆化學

選擇題 (30)

1. One mole of an ideal gas undergoes an isothermal reversible expansion at 300 K. During this process, the system absorbs 450 J of heat from the surroundings. When this gas is compressed to the initial state in one step isothermally, twice as much work is done on the system as was performed on the surroundings during the expansion. Which of the following statements about these processes are correct?
I. for the one-step isothermal compression is 1.5 J/K.
II. for the one-step isothermal compression is 3.0 J/K. 
III. for the reversible isothermal expansion is zero.
IV. for the overall process (expansion and compression) is zero.
V. for the overall process (expansion and compression) is -1.5 J/K. (A)I,II (B)Ⅱ,Ⅲ(C)Ⅱ,Ⅲ,IV(D)Ⅱ，Ⅲ，V (E)I,IV,V

2. Which of the following statements about ligands, d-block metals, and coordination complexes is correct? (A) The cyanate ion (OCN' can have three different Lewis structures, in which all the N atoms have the same formal charge. (B) Zinc is a component of vitamin, which is essential for the metabolism of carbohydrates, fats, and proteins. (C) [Co(NH3)4Cl2]+ has cis-trans isomers, and the cis isomer is optically active. (D) [Cr(en)(NH3)2l2]+(en = ethylenediamine) has three geometrical isomers. (E) The octahedral complexes are more appropriate than the octahedral complexes to be used to determine the field strength of a ligand.

3. Consider 1.0 mole of an ideal gas contained in a 2.0 L bulb at 27℃. This bulb is connected to a 10.0 L sealed, initially evacuated bulb via a valve. When the valve is opened, the temperature is assumed to remain constant. Which of the following statements is incorrect? (gas constant R = ) (A) The final pressure at equilibrium will be 2.1 atm. (B) The enthalpy change (△H) for this process is zero. (C) This is a spontaneous process. (D) Work does not occur during the expansion of this gas. (E) The driving force for this process to occur is an increase in the internal energy.

4. Compound X, like most substances, exhibits only three phases: solid, liquid, and vapor. The triple point of X is at 90 torr and 115 ℃. Which of the following statements concerning the liquid and gaseous X is correct? (A) X(I) cannot exist at 1 atmosphere pressure.(B) X(I) cannot exist above 115℃. (C) X(g) cannot exist below 115 ℃. (D) X(I) cannot have a vapor pressure greater than 90 torr. (E) X(l) cannot exist at a pressure of 15 torr.

5. Given the following half-reactions and associated standard reduction potentials:
Calculate the standard reduction potential for the following half-reaction:
(A)-0.23V (B) -0.46 V (C) -0.85 (D) -1.23 V (E) -1.70 V
6. How many of the following statements are correct?
 I. All the group 13 elements are metals.
 II. Alkaline earth metals react less vigorously with water than do alkali metals. 
III. Salts can consist of hydrogen. 
IV. Because Li has a more negative standard reduction potential than Na and K, it reacts most quickly with water among these three alkali metals. 
V. BeO is amphoteric. (A) 1 (B) 2 (C) 3 (D) 4 (E) 5

7. Given the following eleven gascous molecules:Which of the following statements about these molecules is correct? (A) There are six molecules with all their atoms lying in the same plane. (B) Same hybridized orbitals are used by the N atoms in NF3 and NO3. (C) Both TeF4 and KrF4 are nonpolar molecules. (D) All the C-atoms in the four carbon-containing molecules use sp2 hybridized orbital. (E) Both H2O2 and NO2 exhibit resonance.

8. Ammonium benzoate is a salt formed from ammonia (NH3) and benzoic acid (C6H5COOH). Calculate the pH of a 0.10 M solution of ammonium benzoate at 25 ℃. (Ka = 6.4 x for C6H5COOH, Kb = 1.8 x for NH3； log2 = 0.301； 10g3 = 0.477； log7 = 0.845) (A) 4.74(B) 5.96 (C) 6.73 (D) 7.28 (E) 8.04
9. Yellow phosphorus (P4) undergoes disproportionation in NaOH(aq) to produce PH3 and NaH2PO2. If 16.0 g of P4 was used in the reaction, how many grams of P4 would behave as the oxidizing agent? (atomic weight of P = 31 u)(A) 12.0 g (B) 10.0 g (C) 8.0 g (D) 6.4 g (E) 4.0g 

10. Consider the titration of 50.0 mL of 0.100 M NaH2PO4(aq) with 0.100 M NaOH(aq). For H3 PO4, = 7.5 x . Three pH values during the titration are listed as follows.
(1) Before the addition of NaOH(aq), the pH is x.
(2) After the addition of 25.0 mL NaOH(aq), the pH is y.
 (3) After the addition of 50.0 mL NaOH(aq), the pH is z.
Which of the following statements about x, y, and z is correct? (log2 = 0.301,10g3 = 0.477,log5=0.699) (A)x＜4,y＞7(B)x>4，z>10 (C)y＞7,z＜10(D)y＞8,z＞9 

11. Element X has only two isotopes, 1 and 2, and its atomic weight is y.33 u. Of the following combinations of isotope abundance and corresponding neutron number, which is the most reasonable? (note: y, z, p, q and r are integers)(A)(B)(C)(D)(E)

12. Which of the following molecular formulae has the most structural isomers, all containing a hydroxyl group? (A)C3H6O (B) C3H8O (C) C4H8O (D)(E)

13. Which of the following statements about the dominant Lewis structures ofis correct? (A) ClO obeys the octet rule. (B) ClO- has 1π bond. (C) has 8 lone pair electrons. (D) has 2 π bonds. (E) has 10 lone pair electrons
14. Which of the following statements about the van der Waals equation is incorrect?
(P+■)(V-□)=nRT (A) The van der Waals equation describes the behavior of real gases. (B) ■ =n2a/V2 and is used to compensate for the attraction force bctwecn gas molecules. (C) □= nb and is used to correct the volume of real gases. (D) ■is negative for most gases. (E)□  is positive for most gases.

15. If the reaction starts with only 1 mole of A and 1 mole of B in a 1.0 L sealed reaction vessel, the equilibrium constant of this reaction is K. Which of the following statements is correct? (A) The expression for K of this reaction is ([C]2[D])([A][B)3). (B) If K = 1, [A] is 0.5 M at equilibrium. (C) If K= 1, [C] is 0.3 M at equilibrium. (D) If [C] = 0.5 M at equilibrium, K = 0.08. (E) If [D] 0.25 M at equilibrium, K = 0.17.

16. Which of the following comparisons for the acidity of the following species in an aprotic solvent is correct? (A) Acidity: (B) Acidity: NaNH2＞ NH3 (C) Acidity: (D) Acidity: CH3OH >NH4CI (E) Acidity: C6H5OH ＞ (CH3)3COH

17. Which of the following compounds (1-5) is optically active?
(A)1 (B) 2 (C) 3 (D) 4 (E) 5

18. Which of the following compounds (6-10) is chiral?
  (A)6 (B)7 (C) 8 (D) 9 (E) 10

19. Which of the following compounds (11-15) is not monosaccharide?
(A)11 (B) 12 (C) 13 (D) 14 (E) 15
20. Each of the longest wavelength of the spectral lines recorded for two electron transitions from n = 2 and n = 4 of hydrogen atoms is X and Y, respectively. What is the relationship between X and Y? (A) X:Y = 11:34 (B) X:Y = 5:4 (C) X:Y= 1:4 (D) X:Y = 5:144 (E) X:Y=7:108

21. As shown in Fig, 1, a container with a frictionless movable partitions fixed volume at constant temperature is divided into three compartments (A, B, Hz and C) by two partitions, which are movable without friction. Compartments A and C are filled with an equal amount of mass of gas X and Y. When two partitions stop sliding, the density of X is equal to that of Y. Which of the following statements is correct?
  (A) Volume of gas: V(X) ＞ V(H2) ＞ V(Y) (B) Number of moles of gas: n(X) ＜n(H2) ＜n(Y) (C) Number of moles of gas: n(X) = n(H2) = n(Y) (D) The molecular mass of X is equal to the molecular mass of Y. (E) The molecular mass of X is smaller than the molecular mass of Y.

22. Which of the following groups of species can coexist in significant amounts in a given solution at room temperature? (A) A solution that turns methyI orange red contains . (B) A solution that turns phenolphthalein red contains , and. (C) 0.1 M AgNO3 solution contains , and I-. (D) 0.1 M Na[Al(OH)4] solution contains H+, Na+, CI-, and. (E) An acidic potassium permanganate solution contains , and glucose.
23. Under the same conditions, Na, Mg, and Al of equal molar amounts are respectively added to three test tubes X, Y, and Z containing the same concentration and volume of dilute hydrochloric acid to fully react at room temperature. Which of the following three test tubes X, Y and Z must be incorrect in relation to the volume of gas produced? (A) X(Na) ＞ Y(Mg)＞ Z(Al) (B) X(Na) ＞ Y(Mg) = Z(Al) (C) X(Na) ＜Y(Mg)＜Z(Al) (D) X(Na) =Y(Mg)=Z(Al) (E) X(Na) ＜Y(Mg) = Z(Al)

24. A certain amount of Cl2is introduced into a n/mole certain concentration of potassium hydroxide 0.06 solution, where both reagents are completely consumed and heat is released. Three ionic species0.03 containing chlorine arc produced from this reaction, among which the amount (n/mole) of ClO- and ions and the reaction time (t/s) are shown in Which of the following statements is incorrect? (A) Different reactions of Cl2 and potassium hydroxide solutions may occur at different temperatures. (B) The number of electrons transferred in the reaction is (C) The amount of KOH in the original potassium hydroxide solution cannot be determined. (D) The amount of Cl- in the product is 0.21 mol. (E) The amount of K+in the solution is 0.30 mol. 
25. Based on the following experiments, which substance can prove to be bleaching? (A) When chlorine is introduced into a NaOH solution with phenolphthalein, the solution immediately discolors. (B) When a small amount of Na2O2 powder is added to the water with phenolphthalein, the solution first turns red and then discolors. (C) The red color of phenolphthalein solution fades after the addition of SO2. (D) When SO2 is added to an acidic solution of KMnO4, the purple color of the solution fades. (E) Addition of nitric acidified AgNO3 solution to chlorine water results in white precipitate.
26. Two bottles of gas are NO2(g) and Br2(g) with the same appearance. A chemist designed a variety of identification methods: 
I. wet test paper with starch/KI, 
II. addition of a small amount of NaCl solution,
III. addition of a small amount of AgNO3solution,
IV. addition of a small amount of water and then an appropriate amount of benzene, 
V. change the temperature 
Which methods can be used to distinguish NO2(g) from Br2(g)? (A) I, III, IV (B) II, III, IV (C) I, II, III, IV (D) I, II, III,V (E) II, III, IV, V

27. At 298 K and 101 kPa, 2 . At the same temperature and pressure, 2 moles of SO2 and 1 mole of O2 are introduced into a closed container, and when equilibrium is reached, the amount of heat given off is Q1. If I mole of SO2, 0.5 mole of O2 and 1 mole of SO3 are introduced into a container of the same volume, and the amount of heat given off at equilibrium is Q2, which of the following relationships is correct? (A) Q2 ＜Q1＜197kJ (B) Q2＞Q1＞ 197 kJ (C) Q2= Q1= 197 kJ (D) Q1＜Q2＜197 kJ (E) Q2= Q1 ＜197 kJ
28. After electrolyzing a certain concentration of copper sulfate solution with an inert electrode at a certain temperature for a certain period of time, 0.1 mole of basic copper carbonate [Cu2(OH)2CO3] is added to the resulting solution, and the concentration and pH are restored to exactly the same level as before electrolysis (without considering the dissolution of carbon dioxide). What is the total number of electrons transferred during the electrolysis? (A) 0.4 mole (B) 0.5 mole (C) 0.6 mole (D) 0.7 mole (E) 0.8 mole

29. Acetic acid is an electrolyte. Which of the following facts indicate that acetic acid is a weak electrolyte? ①Acetic acid and water are miscible in any ratio.
②Acetic acid solution conducts electricity.
③Acetic acid molecules are present in acetic acid solution.
④The pH of 0.1 M acetic acid solution is greater than that of 0.1 M hydrochloric acid.
⑤Acetic acid reacts with calcium carbonate to give off CO2.
⑥The pH of 0.1 M sodium acetate solution = 8.9.
⑦When zinc grains of the same size react with the same concentration of hydrochloric acid and acetic acid solution, the acetic acid starts to produce H, at a slower rate. (A)②⑥⑦(B)③④⑤⑥ (C)③④⑥⑦ (D)②④⑥⑦(E)①②

30. Five different types of chemical bonds in the molecular structure of ethanol are shown in Fig. 3. Which of the following statements about reactions in which ethanol breaks bonds is incorrect?
   (A) Bond ① breaks upon reaction with sodium metal. (B) Bond ② and bond ⑤ break, when heating with concentrated sulfuric acid to170℃. (C) Only bond ② breaks, when heating with concentrated sulfuric acid to140℃ (D) Bond① and bond ③ break upon reaction with O2 catalyzed by copper. (E) Only bond ① breaks, when reacting with carboxylic acids in the presence of concentrated sulfuric acid. 

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