110年 - 110 高雄醫學大學_學生轉系考：普通化學#113615

科目：轉學考-普通化學 | 年份：110年 | 選擇題數：25 | 申論題數：0

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所屬科目：轉學考-普通化學

選擇題 (25)

1. A 25.00-g sample of a solid is placed in a graduated cylinder, and then the cylinder is filled to the 50.0-mL mark with benzene. The mass of benzene and solid together is 58.80 g. Assuming that the solid is insoluble in benzene and that the density of benzene is 0.880 g/cm3, please calculate the density of the solid to be _____g/dm3.(A) 2160(B) 2200(C) 2.16(D) 2.2(E) 2
2. Which one of the following statements is incorrect? (A) Sodium arsenate has its formulas of Na3AsO4. (B) A halogen with 85 protons and 85 electrons is At. (C) A possible name for FeBr3 is ferrous bromide. (D) The systematic name for Pb(C2H3O2)2·3H2O is lead (II) acetate trihydrate (E) The systematic name for K2O2 is potassium peroxide

3. Ten tablets with a total mass of 0.5894 g contained saccharin (C7H5NO3S) and were dissolved in water. The saccharin was oxidized to convert all the sulfur to sulfate ion, which was precipitated by adding an excess of barium chloride solution. The mass of barium sulfate obtained was 0.5032 g. The average mass percent of saccharin in the tablets is thus_____. (A) 33.00% (B) 0.052% (C) 53.10% (D) 95.95% (E) 67.00%
4. Consider three identical flasks filled with different gases: Flask A, CO at 760 torr and 0°C； Flask B, N2 at 250 torr and 0°C； Flask C, H2 at 100 torr and 0°C. Which one of the following statements is consistent with the conditions described above? (A) Ranking the gases in order of increasing average kinetic energy: Flask A＞ Flask B ＞ Flask C (B) Ranking the gases in order of increasing average velocity: Flask A ＞ Flask B ＞ Flask C (C) Ranking the gases in order of increasing average velocity: Flask B ＞ Flask A ＞ Flask C (D) Ranking the gases in order of increasing average kinetic energy: Flask A = Flask B = Flask C (E) Ranking the gases in order of increasing average kinetic : Flask A ＜ Flask B ＜ Flask C

5. At elevated temperatures, sodium chlorate decomposes to produce sodium chloride and oxygen gas. A 0.8765-g sample of impure sodium chlorate was heated until the production of oxygen gas ceased. The oxygen gas collected over water occupied 57.2 mL at a temperature of 22°C and a pressure of 734 torr. At 22°C the vapor pressure of water is 19.8 torr. The mass percentage of sodium chlorate in the original sample is_____. (A) 46.5% (B) 18.0% (C) 23.3% (D) 76.7% (E) 53.5%

6. Consider the dissolution of CaCl2: CaCl2(s)→Ca2+(aq) +2Cl ̄(aq), △H = -81.5 kJ. An 11.0-g sample of CaCl2 is dissolved in 125 g water, with both substances at 25°C. Assuming no heat loss to the surroundings and assuming the solution has a specific heat capacity of 4.18 J/°C g, the final temperature of the solution is _____°C. (A) 39.2(B) 26.8(C) 14.2(D) 23.7(E) 30.0
7. Which one of the following statements is incorrect? (A) An unknown nonmetal element with a valence electron configuration of ns2np4 has a smaller radius than barium. (B) The set of quantum numbers, n = 4, l = 3, ml = 4 is not allowed in the hydrogen atom. (C) A certain oxygen atom with the electron configuration of 1s22s22px22py2 has no unpaired electrons. (D) The order of increasing first ionization energy among K, Br, Ni is: Br ＜ Ni ＜K (E) (Kr)5s24d105p5 is the expected ground-state electron configuration for the element with one unpaired 5p electron that forms a covalent compound with fluorine.

8. For the transition of n = 3 →n = 2 to occur in the hydrogen atom, the wavelength of the resulting emitted light is _____ nm.(A) 121.6(B) 656.7 (C) 1876(D) 486.4(E) 48.64
9. Which one of the following statements is correct? (A) SO4 is more energetically stable than XeO4. (B) The order of increasing ionization energy in CI+ ＞ CI ＞ Se ＞ Se- is valid. (C) SeO3 has a T shape structure. (D) N2O is a nonpolar molecule. (E) The AsF5 molecule has a square pyramidal structure.

10. Consider the following reaction: H2C=CH2(g) + F2(g)→H2FC-CFH2(g), △H = -549 kJ. Please estimate the carbon-fluorine bond energy to be _____ kJ/mol given that the C-C bond energy is 347 kJ/mol, the C=C bond energy is 614 kJ/mol, and the F-F bond energy is 154 kJ/mol. (A) 239 (B)-184(C) -92(D) -327(E) 485

11. Consider three molecules: A, B, and C. Molecule A has a hybridization of sp3. Molecule B has two more effective pairs (electron pairs around the central atom) than molecule A. Molecule C consists of two σ bonds and two π bonds. Thus, which one of the following statements relating to A, B and C is incorrect? (A) Molecule A has a tetrahedral arrangement of electron pairs. (B) Molecule B has a square planar structure. (C) Molecule B has a bond angle of 109.5°. (D) The structure of HCN is similar to C. (E) Molecule C is consistent with a linear arrangement of electron pairs exhibiting sp hybridization.

12. A certain metal fluoride crystalizes in such a way that the fluoride ions occupy simple cubic lattice sites, while the metal ions occupy the body centers of half the cubes. The formula of the metal fluoride is thus_____. (A) MF (B) MF3 (C) MF5 (D) MF4 (E) MF2

13. The solubility of CaCl2 in cold water is 74.5 g per 100.0 g water. Assuming i = 2.6 for CaCl2, the freezing point for a saturated solution of CaCl2 will be _____°C. (A)0 (B) -0.32 (C) -13 (D) -32 (E) -37.4

14.For the reaction A →products, successive half-lives are observed to be 10.0, 20.0 and 40.0 min for an experiment in which [A]0 = 0.10 M. Based on the information, the concentration of A after 30 min of the reaction is ＿ M (A) 0.008 (B) 0.30 (C) 0.025 (D) 0.011 (E) 0.0021

15. Suppose the reaction system 2HI(g)⇌H2(g) + I2(g) has already reached equilibrium. Which of the following statements correctly predict the effect of each change on the equilibrium position? (A) Additional H2(g) added to the system will shift to the right to obtain the equilibrium. (B) As an exothermic reaction, the system will shift to the right to attain the equilibrium when increasing the system temperature. (C) When iodine gas is removed, the system will shift to the left to achieve the equilibrium. (D) Addition of argon gas into the reaction system will shift to the right to achieve the equilibrium. (E) When volume of the reaction container is doubled, the change will have no effects on its equilibrium.

16. In a 0.10-M aqueous solution of pyridine (Kь = 1.7 × 10-9), the percentage of pyridine (C5H5N) that forms pyridinium ion, C5H5NH+, is _____%. (A) 0.013 (B) 6.4 (C) 4.2 (D) 1.3 (E) 5.5

17. Consider the titration of 40.0 mL of 0.200 M HCIO4 by 0.100 M KOH. After adding 10.0 mL of the KOH solution, the pH of the resulting solution is _____. (A) 1.15 (B) 7.00 (C) 2.72 (D) 0.85 (E) 4.26
18. Which of the following mixtures would result in buffered solutions when 1.0 L of each of the two solutions are mixed? (A) 0.1 M KOH and 0.1 M CH3NH3Cl (B) 0.1 M KOH and 0.2 M CH3NH3Cl (C) 0.1 M KOH and 0.2 M CH3NH2 (D) 0.2 M KOH and 0.1 M CH3NH2 (E) 0.2 M KOH and 0.1 M CH3NH3CI
19. Which of the following substances does not show increased solubility as the pH of the solution becomes more acidic? (A) Hg2Cl2, Ksp = 1.1 × 10-18 (Hg22+ is the cation in solution.) (B) Ag3PO4, Ksp = 1.8 × 10-18 (C) CaCO3, Ksp = 8.7 × 10-9 (D) CdCO3, Ksp = 5.2 × 10-12 (E) Sr3(PO4)2, Ksp = 1.0 × 10-31

20. For the reaction at 800 K: N2(g) + 3F2(g)→2NF3(g), an equilibrium mixture contains the partial pressures of P(nitrogen) = 0.021 atm, P(fluorine) = 0.063 atm, and P(nitrogen trifluoride) = 0.48 atm. The △G° for the reaction at 527°C is thus _____kJ/mol. (A) 17 (B)-50 (C) 50 (D)-17 (E)-71

21. Which one of the following statements is correct? (A) The value of S° for N2O at 0 K is greater than that for He at 10 K. (B) At 1 atm and 25°C, the value of S° for He(g) is greater than that for N2O(g). (C) The sign of S° for the reaction of 2H2S(g) + SO2(g) → 3Srhombic(s) + 2H2O(g) is negative. (D) The sign of S° for the reaction of 2SO3(g) → 2SO2(g) + O2(g) is negative. (E) The sign of S° for the reaction of Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(g) is only positive.

22. When electrolyzing a sodium chloride solution at 50°C and 2.50 atm, the volume of _____ L H2(g) is acquired in addition of the production of 257 L Cl2(g) with both volumes measured in the same time. (A) 257(B) 128.5(C) 85.7(D) 514(E) 771
23. A rock contains 0.688 mg of 206 Pb for every 1.000 mg of 238U present. Assuming that no lead was originally present, which all the 206Pb formed over the years has remained in the rock, and that the number of nuclides in intermediate stages of decay between 238U and 206Pb is negligible, the age of the rock is calculated to be _____ years. (For 238U, t1/2 = 4.5 ×109 years.) (A) 3.8 × 106(B) 3.8 × 107(C) 3.8 × 108(D) 3.8 × 109(E) 3.8 × 1010
24. Which of the following statements is correct? (A) The diamagnetic Ni(CN)42- ion has a tetrahedral d8 structure. (B) The V(en)33+ ion has 0 unpaired electrons. (C) The systematic name for K2(PtCl4) is potassium tetrachloroplatinate(II). (D) The formulas for sodium dicyanobis(oxalate)ferrate(III) is Na4(Fe(CN)2(C2O4)2). (E) The transition metal ion in (Co(NH3)2(NH2CH2CH2NH2)2)l2 has an electron configuration of [Ar]3d6.
25. The average molar mass of one base pair of nucleotides in DNA is approximately 600 g/mol. The spacing between successive base pairs is about 0.34 nm, and a complete turn in the helical structure of DNA occurs about every 3.4 nm. If a DNA molecule has a molar mass of 4.5 × 109 g/mol, there are approximately _____ complete turns existing in the DNA a-helix structure. (A) 5.2 × 1012 (B) 4.6 × 109 (C) 8.0 × 105 (D) 2.6 × 106 (E) 9.4 × 103

申論題 (0)