106年 - 106 臺灣綜合大學系統_學士班轉學生聯合招生試題：普通化學B#122179

選擇題 (25)

1. Which of the experiments listed below did not provide the information stated about the nature of the atom? (A)The Rutherford experiment proved that the Thomson "plum pudding" model of the atom was essentially correct. (B) The Rutherford experiment determined the charge on the nucleus. (C) The cathode-ray tube proved that electrons have a negative charge. (D)Millikan's oil-drop experiment showed that the charge on any particle was a simple multiple of the charge on the electron. (E) none of these

2. The limiting reactant in a reaction (A)is the reactant for which you have the least number of moles. (B) has the lowest coefficient in a balanced equation. (C) has the lowest ratio of coefficient in the balanced equation to moles available. (D)has the lowest ratio of moles available to coefficient in the balanced equation. (E) none of these

3. A solution contains the ions Ag⁺, Pb²⁺, and Ni²⁺. Dilute solutions of NaCl, Na₂SO₄, and Na₂S are available to separate the positive ions from each other. In order to effect separation, the solutions should be added in which order? (A)Na₂S, NaCl, Na₂SO₄ (B) Na₂SO₄, NaCl, Na₂S (C) Na₂SO₄, Na₂S, NaCl (D)NaCl, Na₂S, Na₂SO₄ (E) NaCl, Na₂SO₄, Na₂S

4. 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.

In which flask do the molecules have the greatest momentum per impact? (A)The molecules in all the flasks have the same momentum per impact. (B) The molecules in two of the flasks have the same momentum per impact. (C) flask C (D)flask A (E) flask B

5. Consider the following equilibrium:
N₂(g) + 3H₂(g) ⇄ 2NH₃(g)
with K = 2.3 × 10^-6. 1.00 mol each of all reactants and products is placed in a 1.00-L container. Which way will the reaction initially proceed? (A)To the right. (B) We need to know the temperature. (C) The system is at equilibrium. (D)To the left. (E) none of these

6. As water is heated, its pH decreases. This means that (A)[OH^-] > [H⁺]. (B) [H⁺] >[OH^-]. (C) the water is no longer neutral. (D)Two of these are correct. (E) None of these is correct.

7. The reaction Cr(s) + NO₃¯(aq) → Cr³⁺(aq) + NO(g) takes place in acidic solution.
What is the coefficient of H₂O(l) in the balanced equation? (A)3 (B) 5 (C) 4 (D)2 (E) 1

8. For a particular process q = -10 kJ and w = 25 kJ. Which of the following statements is true? (A)The system does work on the surroundings. (B) Heat flows from the surroundings to the system (C) ΔE = −35 kJ (D)All of these are true. (E) None of these is true.

9. For the reaction H₂O(l) → H₂O(g) at 298 K, 1.0 atm, ΔH is more positive than ΔE 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 work done in pushing back the atmosphere. (C) the difference in the H—O bond energy in H₂O(l) compared to H₂O(g) (D)the value of ΔH itself. (E) none of these

10. Choose the correct statement. (A)A reaction that exhibits a negative value of ΔS cannot be spontaneous. (B) Exothermic reactions are always spontaneous. (C) Free energy is independent of temperature. (D)At constant pressure and temperature, a decrease in free energy ensures an increase in the entropy of the system (E) none of these

11. Consider a solution consisting of the following two buffer systems:
H₂CO₃ ⇌ HCO₃^- + H⁺ pK_a= 6.4 ； H₂PO₄^-⇌ HPO₄^2- + H⁺ pK_a = 7.2

At pH 6.4, which one of the following is true of the relative amounts of acid and conjugate base present? (A)[H₂CO₃] ＞ [HCO₃¯] and [H₂PO₄^-] ＞ [HPO₄^2-] (B) [HCO₃^-] ＞ [H₂CO₃] and [HPO₄^2-] ＞ [H₂PO₄^-] (C) [H₂CO₃] ＞ [HCO₃^-] and [HPO₄^2-] ＞ [H₂PO₄^-] (D)[H₂CO₃] = [HCO₃^-] and [HPO₄^2-] ＞ [H₂PO₄^-] (E) [H₂CO₃] = [HCO₃^-] and [H₂PO₄^-] ＞ [HPO₄^2-]

12. What is the probability of finding a particle in a one-dimensional box in energy level n = 4 between x = L/4 and x = L/2? (L is the length of the box.) (A)50% (B) 12.5% (C) 33% (D)25% (E) 37.5%

13. According to the VSEPR model, the electron pairs around NH₃ and those around CH₄ are arranged (A)differently, because in each case there are a different number of atoms around the central atom. (B) the same, because both nitrogen and carbon are in the second period. (C) differently, because in each case there are a different number of electron pairs around the central atom. (D)differently or the same, depending on the conditions leading to maximum repulsion. (E) the same, because in each case there are the same number of electron pairs around the central atom.

14. Which statement about the thiocyanate ion, SCN^-, is true? (A)Only one correct resonance structure can be drawn. (B) Its Lewis structure contains an unpaired electron. (C) Its shape is bent like that of H₂O. (D)There are more than two σ bonds in the ion. (E) none of these

15. Initial rate data have been determined at a certain temperature for the gaseous reaction
2NO + 2H₂ → N₂+ 2H₂O
What is the numerical value of the rate constant? (A)1.5 (B) 9.9 (C) 3.0 (D)0.13 (E) 0.44

16. The reaction A → B + C is known to be zero order in A with a rate constant of 5.0 × 10^-2 mol/L • s at 25° C. An experiment was run at 25°C where [A]₀ = 1.0 × 10^-3M. What is the integrated rate law? (A)[A] = kt (B) [A]₀ - [A]= kt (C) [A] – [A]₀ = kt (D)(E)

17. A p-type semiconductor (A)is made by doping host atoms with atoms having more valence electrons than the host. (B) has electrons that lie close in energy to the conduction bands. (C) is made by doping host atoms with atoms having fewer valence electrons than the host (D)two of these (E) none of these

18. 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)II, IV (B) II, III (C) I, II (D)I, II, III (E) I, II, IV

19. What reason is given for the stability of C□O, N□N, and O□O bonds, compared to the instability of Si□Si, P□P, and S□S bonds? (A)Their metallic character varies greatly. (B) There are large differences in their abilities to form strong pi bonds. (C) There are large differences in their ionization energies. (D)There are large differences in their electronegativities. (E) none of these

20. Which of the following is diamagnetic? (A)F₂⁺ (B) C₂⁺ (C) H₂⁺ (D)N₂⁺ (E) N₂⁺

21. The U-238 nucleus decays to form Pb-206 by α and β decays. Calculate the number of α decays. (A)2 (B)4 (C) 6 (D)8 (E) none of these

22. In lecture, the professor named a molecule 2-ethyl-4-tertiary-butylpentane. An alert student pointed out that although the correct structure could be drawn from this name, the name did not follow systematic rules. What is the correct systematic name for the molecule? (A)3,5,6,6-tetramethylheptane (B) 2-ethyl-4,5,5-trimethylhexane (C) undecane (D)2,2,3,5-tetramethylheptane (E) 2-t-butyl-5-methylhexane

23. Which of the following is optically active (that is, chiral)? (A)3-chloropentane (B) 1-bromopentane (C) 2-chloropentane (D)dichloromethane (E) dimethylamine

24. For a reaction in a voltaic cell, both ΔH° and ΔS° are positive. Which of the following statements is true? (A)E°cell will increase with an increase in temperature. (B) E°cell will decrease with an increase in temperature. (C) E°cell will not change when the temperature increases. (D)ΔG°> 0 for all temperatures. (E) None of the above statements is true.

複選題
25. Which of the following coordination compounds will form a precipitate when treated with an aqueous solution of AgNO₃? (A)Na₃[CrCl₆] (B) [Cr(NH₃)₃Cl₃] (C) Na₃[Cr(CN)₆] (D)[Cr(NH₃)₆]Cl₃ (E) all of these

申論題 (20)

1. Consider the following diagram:

A porous container (A), filled with air at STP, is contained in a large enclosed container (B), which is flushed with H₂(g). What will happen to the pressure inside container A? Explain your answer. (4%)