102年 - 102 台灣聯合大學系統_學士班轉學生考試試題_A6：普通化學#139282

1. Which of the following is *not* the correct chemical formula for the compound named? (A)\( Al(OH)_2 \) aluminum hydroxide (B) LiCN lithium cyanide (C) \( Fe_2O_3 \) Iron(III) oxide (D) ZnSe zinc selenide (E) \( Mg(C_2H_3O_2)_2 \) magnesium acetate

2. Which is the correct formula for gold(I) sulfide? (A) AuS (B) \( Au_2S \) (C) \( AuS_2 \) (D) \( Au_2S_3 \) (E) \( Au_2S_2 \)

3. When \( NH_3(aq) \) is added to \( Cu^{2+}(aq) \), a precipitate initially forms. What is its formula? (A) \( Cu(NH_3)_2 \) (B) \( Cu(NO_3)_2 \) (C) CuO (D) \( Cu(NH_3)_2^{2+} \) (E) \( Cu(OH)_2 \)

4. True or false? The equation \( 2C_2H_6 + 7O_2 \rightarrow 4CO_2 + 6H_2O \) is an oxidation-reduction reaction. (A) True; the oxygen is reduced and the hydrogen is oxidized. (B) True; the carbon is oxidized and the hydrogen is reduced. (C) True; the carbon is oxidized and the oxygen is reduced. (D) True; the carbon is reduced and the oxygen is oxidized. (E) False

5. Consider two samples of helium in separate containers of the same volume. Sample 1 has an absolute temperature four times that of Sample 2. Both samples are at the same pressure. Calculate the ratio \( n_1:n_2 \). (A) 1:1 (B) 1:2 (C) 2:1 (D) 1:4 (E) 4:1

6. Which of the following statements concerning equilibrium is *not* true? (A) A system that is disturbed from an equilibrium condition responds in such a way as to restore equilibrium. (B) A system moves spontaneously toward a state of equilibrium. (C) Equilibrium in molecular systems is dynamic, with two opposing processes balancing one another. (D) The value of the equilibrium constant for a given reaction mixture is the same regardless of the direction from which equilibrium is attained. (E) The equilibrium constant is independent of temperature.

7. For the reaction \( 2H_2(g) + O_2(g) \rightleftharpoons 2H_2O(g) \), what is the relationship between \( K \) and \( K_p \) at temperature \( T \)? (A) \( K = K_p \) (B) \( K = K_p(RT) \) (C) \( K_p = K(RT) \) (D) \( K = K_p(RT)^2 \) (E) \( K_p = K(RT)^2 \)

8. When the substances in the equation below are at equilibrium at pressure \( P \) and temperature \( T \), how can the equilibrium be shifted to favor the products? \( CuO(s) + H_2(g) \rightleftharpoons Cu(s) + H_2O(g) \) Change in enthalpy = −2.0 kJ. (A) Decrease the temperature. (B) Increase the temperature. (C) Add a catalyst. (D) Increase the pressure by adding an inert gas such as nitrogen. (E) Allow some gas to escape at constant pressure and temperature.

9. The acids \( HC_2H_3O_2 \) and HF are both weak, but HF is a stronger acid than \( HC_2H_3O_2 \). HCl is a strong acid. Order the following according to base strength. (A) \( C_2H_3O_2^- ＞ F^- ＞ Cl^- ＞ H_2O \) (B) \( Cl^- ＞ F^- ＞ C_2H_3O_2^- ＞ H_2O \) (C) \( C_2H_3O_2^- ＞ F^- ＞ H_2O ＞ Cl^- \) (D) \( F^- ＞ C_2H_3O_2^- ＞ H_2O ＞ Cl^- \) (E) none of these

10. HOAc \( K_a = 1.8 \times 10^{-5} \) \( H_2CO_3 \) \( K_{a1} = 4.3 \times 10^{-7} \), \( K_{a2} = 5.6 \times 10^{-11} \) Which of the following 0.01 M solutions has the highest pH? (A) HOAc (B) NaOAc (C) \( H_2CO_3 \) (D) \( Na_2CO_3 \) (E) \( NaHCO_3 \)

11. Determine the pH of the following aqueous solution. Choose your answer from the given pH ranges. 0.5 M \( NH_4F \) (\( pK_b \) for \( NH_3 = 4.74 \), \( pK_a \) for \( HF = 3.14 \)) (A) pH 0.00–2.99 (B) pH 3.00–5.99 (C) pH 6.00–8.99 (D) pH 9.00–10.99 (E) pH 11.00–14.00

12. Which of the following solutions will be the best buffer at a pH of 9.26? (\( K_a \) for \( HC_2H_3O_2 \) is \( 1.8 \times 10^{-5} \); \( K_b \) for \( NH_3 \) is \( 1.8 \times 10^{-5} \).) (A) 0.20 M \( HC_2H_3O_2 \) and 0.20 M \( NaC_2H_3O_2 \) (B) 3.0 M \( HC_2H_3O_2 \) and 3.0 M \( NH_4Cl \) (C) 3.0 M \( HC_2H_3O_2 \) and 3.0 M \( NH_3 \) (D) 0.20 M \( NH_3 \) and 0.20 M \( NH_4Cl \) (E) 3.0 M \( NH_3 \) and 3.0 M \( NH_4Cl \)

13. A 100.0-mL sample of 0.2 M \( (CH_3)_3N \) (\( K_b = 5.3 \times 10^{-5} \)) is titrated with 0.2 M HCl. What is the pH at the equivalence point? (A) 7.0 (B) 3.1 (C) 10.4 (D) 5.4 (E) 9.5

14. Which of the following compounds has the lowest solubility, in moles per liter, in water? (A) CdS \( K_{sp} = 1.0 \times 10^{-28} \) (B) \( Al(OH)_3 \) \( K_{sp} = 2 \times 10^{-32} \) (C) \( PbSO_4 \) \( K_{sp} = 1.3 \times 10^{-8} \) (D) \( Sn(OH)_2 \) \( K_{sp} = 3 \times 10^{-27} \) (E) \( MgC_2O_4 \) \( K_{sp} = 8.6 \times 10^{-5} \)

15. Given the following values of equilibrium constants:

\( Cu(OH)_2(s) \rightleftharpoons Cu^{2+}(aq) + 2OH^-(aq) \) \( K_{sp} = 1.6 \times 10^{-19} \)

\( Cu(NH_3)_4^{2+}(aq) \rightleftharpoons Cu^{2+}(aq) + 4NH_3(aq) \) \( K = 1.0 \times 10^{-13} \)

What is the value of the equilibrium constant for the following reaction? \( Cu(OH)_2(s) + 4NH_3(aq) \rightleftharpoons Cu(NH_3)_4^{2+}(aq) + 2OH^-(aq) \) (A) \( 1.6 \times 10^{-19} \) (B) \( 1.6 \times 10^{-6} \) (C) \( 6.2 \times 10^{31} \) (D) \( 1.6 \times 10^{-32} \) (E) \( 1.0 \times 10^{13} \)

16. Consider the following reaction: \( 2SO_2(g) + O_2(g) \rightarrow 2SO_3(g) \) \( \Delta H = -198 \) kJ. Calculate the energy change associated with 0.334 mole of \( SO_2 \) reacting with excess \( O_2 \). (A) −33.1 kJ (B) −66.1 kJ (C) −132 kJ (D) −198 kJ (E) −424 kJ

17. For the reaction \( H_2O(l) \rightarrow H_2O(g) \) at 298 K, 1.0 atm, \( \Delta H \) is more positive than \( \Delta E \) by 2.5 kJ/mol. This quantity of energy can be considered to be (A) the heat flow required to maintain a constant temperature. (B) the value of \( \Delta H \) itself. (C) the work done in pushing back the atmosphere. (D) the difference in the H–O bond energy in \( H_2O(l) \) compared to \( H_2O(g) \). (E) none of these.

18. Given: \( Cu_2O(s) + \frac{1}{2}O_2(g) \rightarrow 2CuO(s) \) \( \Delta H^\circ = -144 \) kJ

\( Cu_2O(s) \rightarrow Cu(s) + CuO(s) \) \( \Delta H^\circ = +11 \) kJ

Calculate the standard enthalpy of formation of CuO(s). (A) −166 kJ (B) −299 kJ (C) +299 kJ (D) +155 kJ (E) −155 kJ

19. For which process is \( \Delta S \) negative? (A) evaporation of 1 mol of \( CCl_4(l) \) (B) mixing 5 mL of ethanol with 25 mL of water (C) raising the temperature of 100 g of Cu from 275 K to 295 K (D) compressing 1 mol of Ne at constant temperature from 1.5 atm to 0.5 atm (E) grinding a large crystal of KCl to powder

20. For the reaction \( A + B \rightarrow C + D \), \( \Delta H^\circ = +40 \) kJ and \( \Delta S^\circ = +50 \) J/K. Therefore, the reaction under standard conditions is (A) spontaneous at temperatures less than 10 K. (B) spontaneous at temperatures greater than 800 K. (C) spontaneous only at temperatures between 10 K and 800 K. (D) spontaneous at all temperatures. (E) nonspontaneous at all temperatures.

21. For which of the following processes would \( \Delta S^\circ \) be expected to be most positive? (A) \( O_2(g) + 2H_2(g) \rightarrow 2H_2O(g) \) (B) \( H_2O(l) \rightarrow H_2O(s) \) (C) \( N_2O_4(g) \rightarrow 2NO_2(g) \) (D) \( 2NH_4NO_3(s) \rightarrow 2N_2(g) + O_2(g) + 4H_2O(g) \) (E) \( NH_3(g) + HCl(g) \rightarrow NH_4Cl(g) \)

22. Which of the following is the best reducing agent?

\( Cl_2 + 2e^- \rightarrow 2Cl^- \) \( E^\circ = 1.36 \) V

 \( Mg^{2+} + 2e^- \rightarrow Mg \) \( E^\circ = -2.37 \) V

\( 2H^+ + 2e^- \rightarrow H_2 \) \( E^\circ = 0.00 \) V (A) \( Cl_2 \) (B) \( H_2 \) (C) Mg (D) \( Mg^{2+} \) (E) \( Cl^- \)

23. The standard potential for the reaction \( Zn + 2Ag^+ \rightarrow Zn^{2+} + 2Ag \) is 1.56 V. Given that the standard reduction potential for \( Ag^+ + e^- \rightarrow Ag \) is 0.80 V, determine the standard reduction potential for \( Zn^{2+} + 2e^- \rightarrow Zn \). (A) −0.76 V (B) 0.04 V (C) 0.76 V (D) 2.36 V (E) none of these

24. The standard reduction potentials are as follows:

 \( MnO_4^- + 8H^+ + 5e^- \rightarrow Mn^{2+} + 4H_2O \) \( E^\circ = 1.51 \) V

\( Cr_2O_7^{2-} + 14H^+ + 6e^- \rightarrow 2Cr^{3+} + 7H_2O \) \( E^\circ = 1.33 \) V

How many electrons are transferred in the balanced reaction (that is, what will be the value of n in the Nernst equation)? (A) 5 (B) 6 (C) 12 (D) 30 (E) 36

25. From the following list of observations, choose the one that most clearly supports the conclusion that atoms contain electrons. (A) the emission spectrum of hydrogen (B) the photoelectric effect (C) the scattering of alpha particles by metal foil (D) diffraction (E) cathode "rays"

26. What is the electron configuration of \( Cr^{3+} \)? (A) [Ar] \( 4s^23d^1 \) (B) [Ar] \( 4s^13d^2 \) (C) [Ar] \( 3d^3 \) (D) [Ar] \( 4s^23d^4 \) (E) none of these

27. An element has the electron configuration \( [Kr] 4d^{10}5s^25p^2 \). The element is a(n) (A) nonmetal (B) transition metal (C) lanthanide (D) metal (E) chalcogenide

28. Which element listed below has the highest electronegativity? (A) K (B) Rb (C) Te (D) I (E) Br

29. The molecule \( XCl_5^- \) has a square pyramidal shape. Which of the following atoms could be X? (A) S (B) Xe (C) O (D) P (E) At least two of these atoms could be X.

30. Which molecule or ion violates the octet rule? (A) \( H_2O \) (B) \( I_3^- \) (C) \( NO_3^- \) (D) \( PF_3 \) (E) none of these

31. What is the hybridization of the central atom in \( PCl_4^+ \)? (A) sp (B) \( sp^2 \) (C) \( sp^3 \) (D) \( dsp^3 \) (E) \( d^2sp^3 \)

32. Which of the following statements is correct? (A) A triple bond is composed of two \( \sigma \) bonds and one \( \pi \) bond. (B) \( \sigma \) bonds result from the head-to-head overlap of atomic orbitals. (C) Free rotation may occur about a double bond. (D) \( \pi \) bonds have electron density on the internuclear axis. (E) More than one of these statements are correct.

33. The configuration \( (\sigma_{2s})^2(\sigma_{2s}^*)^2(\pi_{2py})^2(\pi_{2pz})^1 \) is the molecular orbital description for the ground state of which of the following species? (A) \( B_2 \) (B) \( B_2^{2-} \) (C) \( Li_2^+ \) (D) \( C_2 \) (E) \( Be_2 \)

34. The following data were obtained for the reaction of NO with \( O_2 \). Concentrations are in molecules/cm³ and rates are in molecules/cm³·s.

Which of the following is the correct rate law? (A) Rate = \( k[NO][O_2] \) (B) Rate = \( k[NO]^2 \) (C) Rate = \( k[NO][O_2]^2 \) (D) Rate = \( k[NO]^2[O_2] \) (E) Rate = \( k[NO]^2[O_2]^2 \)

35. If the reaction \( 2HI \rightarrow H_2 + I_2 \) is second order, which of the following will yield a linear plot? (A) log [HI] vs. time (B) [HI] vs. time (C) ln [HI] vs. time (D) \( [HI]^{\frac{1}{2}} \) vs. time (E) 1/[HI] vs. time

36. What is the overall order of a reaction with the following rate law? Rate = \( [A]^2[B]^1[C]^0 \) (A) 0 (B) 1 (C) 2 (D) 3 (E) 4

37. Which intermolecular force is the strongest? (A) dipole-dipole interactions (B) hydrogen bonding (C) polar covalent bonds (D) London dispersion forces (E) ionic bonding

38. In the unit cell of sphalerite, \( Zn^{2+} \) ions occupy half the tetrahedral holes in a face-centered cubic lattice of \( S^{2-} \) ions. What is the number of formula units of ZnS in the unit cell? (A) 2 (B) 3 (C) 4 (D) 6 (E) 8

39. In which of the following processes is energy evolved as heat? (A) sublimation (B) crystallization (C) melting (D) vaporization (E) none of these

40. A liquid-liquid solution is called an ideal solution if

 I. it obeys \( PV = nRT \).

II. it obeys Raoult's law.

III. solute-solute, solvent-solvent, and solute-solvent interactions are very similar.

IV. solute-solute, solvent-solvent, and solute-solvent interactions are quite different. (A) I, II, III (B) II, III (C) I, II, IV (D) II, IV (E) I, II

41. Which of the following statements is(are) true? (A) The rate of dissolution of a solid in a liquid always increases with increasing temperature. (B) The solubility of a solid in a liquid always increases with increasing temperature. (C) According to Henry's law, the amount of gas dissolved in a solution is directly proportional to the pressure of the gas above the liquid. (D) Two of these statements are true. (E) All of these statements are true.

42. A solute added to a solvent raises the boiling point of the solution because (A) the solute particles lower the solvent's vapor pressure, thus requiring a higher temperature to cause boiling. (B) the temperature to cause boiling must be great enough to boil not only the solvent but also the solute. (C) the solute particles raise the solvent's vapor pressure, thus requiring a higher temperature to cause boiling. (D) the solute increases the volume of the solution, and an increase in volume requires an increase in the temperature to reach the boiling point (derived from \( PV = nRT \)). (E) Two of the above are correct.

43. In which group are the elements listed in correct order of increasing first ionization energy? (A) Na > P > Cl (B) Cs > Na > K (C) K > Ca > Ge (D) Al > Si > P (E) Cs < Rb < Na

44. Which metal ion has a \( d^6 \) electron configuration? (A) \( Mn^{2+} \) (B) \( Co^{3+} \) (C) \( Ni^{2+} \) (D) \( Ti^{2+} \) (E) \( Fe^{3+} \)

45. Which of the following coordination compounds will form a precipitate when treated with an aqueous solution of \( AgNO_3 \)? (A) \( [Cr(NH_3)_3Cl_3] \) (B) \( Na_3[CrCl_6] \) (C) \( [Cr(NH_3)_6]Cl_3 \) (D) \( Na_3[Cr(CN)_6] \) (E) two of these

46. The spectrochemical series is \( I^- ＜ Br^- ＜ Cl^- ＜ F^- ＜ OH^- ＜ H_2O ＜ NH_3 ＜ en ＜ NO_2^- ＜ CN^- \) Which of the following complexes will absorb visible radiation of the highest energy (shortest wavelength)? (A) \( [Co(H_2O)_6]^{3+} \) (B) \( [Co(I)_6]^{3-} \) (C) \( [Co(OH)_6]^{3-} \) (D) \( [Co(en)_3]^{3+} \) (E) \( [Co(NH_3)_6]^{3+} \)

47. Which of the following processes increases the atomic number by 1? (A) gamma-ray production (B) alpha production (C) neutron-particle production (D) proton production (E) beta-particle production

48. Vibrational transitions in molecules typically require energies that correspond to the ________ region of the electromagnetic spectrum. (A) UV (B) visible (C) IR (D) X-ray (E) microwave

49. Which of the following is *not* a structural isomer of 1-pentene? (A) 2-pentene (B) 1-methyl-cyclobutene (C) cyclopentane (D) 2-methyl-2-butene (E) 3-methyl-1-butene

50. Identify the type of organic compound shown:

(A) ester (B) aldehyde (C) amine (D) carboxylic acid (E) ketone