104年 - 104 台灣聯合大學系統_學士班轉學生考試試題_A1A5：普通化學#139172

1. Iron oxide can be reduced to iron by a reaction with carbon to form carbon monoxide

Fe₂O₃(s) + 3C(s) -＞ 2Fe(s) + 3CO(g)

If 95.0 grams of iron oxide is reacted with excess carbon yields 63.0 g of iron, what is the percent yield of this reaction? (A)12% (B)59% (C)66% (D)95% (E)100%

2. Choose the best statement regarding why diagram I is the better choice between these two Lewis diagrams for N₂O

(A)because II does not satisfy the octet rule for all atoms. (B)because structure I has fewer formal charges than II. (C)because structure I has the negative formal charge on the most electronegative atom. (D)because structure I has the positive formal charge on the most electronegative atom. (E)the best structure is actually structure II.

3. What is the probability of finding a particle in a box of length L between zero and L/2? (A)1 (B)0.5 (C)0.25 (D)L/2 (E)it depends on the quantum number n

4. A material is made from Al, Ga, and As. The mole fractions of these elements are 0.25, 0.26, and 0.49, respectively. This material would be (A)a metallic conductor because Al is present. (B)an insulator. (C)a p-type semiconductor. (D)an n-type semiconductor. (E)none of these

5. The uncertainty in the velocity of an electron is 1x10^5 m s^-1. What is the minimum uncertainty in its position? (A)5.79x10^-5 m (B)2.31x10^-9 m (C)5.79x10^-10 m (D)2.31x10^-10 m (E)1.08x10^-10 m

6. Rank from smallest to largest in terms of atom/ionic radii. (A)S^2-, Cl^-, Ar, K⁺, Ca²⁺ (B)Ca²⁺, K+, Ar, Cl^-, S^2- (C)Ca²⁺, S^2-, K⁺, Cl^-, Ar (D)Ar, K⁺, Cl^-, Ca²⁺, S^2- (E)Ar, Cl^-, K⁺, S^2-, Ca²⁺

7. Which of the following sets of quantum numbers is allowed for an electron in a one electron atom? (A)n=4, l=3, m=3, ms=0 (B)n=3, l=1, m=2, ms=-1/2 (C)n=2, l=0, m=1, m_s=1/2 (D)n=2, l=3, m=3, m_s=1/2 (E)n=6, l=5, m=-3, m_s=-1/2

8. A Lewis dot structure for benzene, C6H6 would give two equivalent resonance structures for this cyclic molecule with alternating single and double bonds. 

A combined LCAO and MO picture for the bonding of the carbon atoms in benzene would be

(A)1σ(Csp²-Csp²) bonds between each C atom, and 3π MO delocalized over the C's (B)2σ(Csp³-Csp³) bonds between each C atom, and 1π MO delocalized over the C's (C)1σ(Csp³-Csp³) bonds between each C atom, and 1π MO delocalized over the C's (D)1σ(Csp²-Csp²) bonds between each C atom, and 2π MO delocalized over the C's (E)3σ(C2p-C2p) bonds between each C atom

9. Which of the following has the highest bond order O₂, NO, N₂, NO⁺? ________are the same and the highest(A)O₂ (B)NO (C)N₂ (D)NO⁺ (E)N₂ and NO⁺ 

10. How many different isomers exist for Dichloro-ethene, C₂H₂Cl₂? (A)0 (B)1 (C)2 (D)3 (E)4

11. Which of the following best describes the lanthanide contraction? (A)f-orbitals are more directional than d-orbitals and therefore less effective at screening nuclear charge (B)f-orbitals are more diffuse than d-orbitals and therefore less effective at screening nuclear charge (C)the increase in atomic and ionic radii as one goes from left to right across the lanthanides (D)a and c (E)b and c

12. The octahedral compound [FeCl₃(NH₃)₃] is found to be paramagnetic. This means (A)it must be a high spin complex. (B)it must be a low spin complex. (C)it could be either a high spin or low spin complex. (D)it has a crystal field stabilization that is zero. (E)a & d

13. Which of the following statements is true for crystal field theory of an octahedral complex?

(A)The d_xy, d_yz, d_xz orbitals are lower in energy than the dz2, and the dx2-y2 because they are unaffected by the ligand field. 

(B)The d_xy, d_yz, d_xz orbitals are lower in energy than the dz2, and the dx2-y2 because their energy is increased less than the d_z2, and the d_x2-y2.

(C)in low spin complexes the dz2, and the d_x2-y2 are lower in energy than the d_xy, d_yz, d_xz orbitals.

(D)a & c (E)b & c

14. Helium effuses through a small opening at a rate of 1x10^-9 mol s^-1. An unknown gas at the same temperature and pressure is found to effuse through the same opening at a rate of 3.78x10^-10 mol s^-1. What is the molecular mass of the unknown gas? (A)4 g mol^-1 (B)14 g mol^-1 (C)18 g mol^-1 (D)28 g mol^-1 (E)40 g mol^-1

15. The triple point of a compound is at 38.2°C and a pressure of 0.75 atm. A gaseous sample of the substance is held at a constant pressure of 0.79 atm. Initially the sample is at 50°C and is slowly cooled until it is -25°C. What if any phase transitions occur? (A)condensation (B)deposition (C)condensation followed by freezing (D)simultaneous condensation and freezing (E)none of the above

16. At the same temperature and pressure, comparing one mole of a gas that is described the following equation of state, P(V - nb) = nRT where b ＞ 0 to one mole of an ideal gas (A)the volume will be larger or smaller depending on the pressure (B)the volume will be smaller than that of the ideal gas (C)the volume will be the same as that of the ideal gas (D)the volume will be larger or smaller depending on the temperature (E)the volume will be larger than that of the ideal gas

17. A mixture of solid NaCl and CaCl₂ contains 10.0 g of NaCl, and an unknown amount of CaCl₂. When the entire mixture is dissolved in 1.00 kg of water, the boiling point changes by 0.25°C. What mass of CaCl₂ was in the original mixture? Kb for water is 0.512 K kg mol^-1. (A)5.4 g (B)8.1 g (C)35.2 g (D)Not enough data to answer the question (E)None of the above

18. Acetone (mw = 58.08, P°_25°C = 232 mmHg) and butanone (mw = 72.11, P°_25°C = 100 mmHg) have the indicated molar masses and vapor pressures. A container holds 1.00 kg of butanone. How much acetone must be added to the butanone to elevate the total vapor pressure over the mixture to 125 mmHg at 25°C? (A)5.313 kg (B)290 g (C)188 g (D)More information needed (E)None of the above

19. The constant pressure heat capacity (c_p) generally increases with (A)the mass of the molecule (B)the internal degrees of freedom in the molecule (C)the number of atoms in the molecule (D)a and c (E)b and c

20. Which of the following has a standard state Gibbs free energy equal to zero? (A)Br₂(l) (B)I₂(g) (C)C(s, diamond) (D)a and c (E)all of the above

21. Name the following compound, Pt(H₂NCH₂CH₂NH₂)Cl₄Cl₂ (A)hexachloro(ethylenediamine)platinum (IV) (B)hexachloride(ethylenediamine)platinum (VI) (C)tetrachloro(ethylenediamine)platinum (IV) chloride (D)tetrachloro(ethylenediamine)platinum (VI) chloride (E)Platinum(ethylenediamine)hexachloride

22. A first-order reaction is 54% complete at the end of 12 min. What is the value of the rate constant? (A)6.5 × 10^-2 min^-1 (B)0.33 min^-1 (C)0.065 min^-1 (D)5.1 × 10^-2 min^-1

23. [Cu(CF₃)₄]^- is found to be diamagnetic. What is its structure? (A)tetrahedral (B)square planar (C)either square planar or tetrahedral (D)octahedral (with two other water ligands) (E)it will be an unusual shape with a steric number of 8

24. Calculate the total number of unpaired electrons in the following complex ions: [Zn(H₂O)₆]²⁺, [Ni(CN)₄]^2- (square planar), [Co(NH₃)₆]³⁺ (strong field). (A)0 (B)1 (C)2 (D)3 (E)4

25. What reason is given for the stability of C—C, 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 ionization energies. (C)There are large differences in their electronegativities. (D)There are large differences in their abilities to form strong pi bonds. (E)none of these

26. Consider the equation A(aq) + 2B(aq) ⇌ 3C(aq) + 2D(aq). 42.0 mL of 0.046 M A is mixed with 24.0 mL 0.105 M B. At equilibrium, the concentration of C is 0.0416 M. Calculate K. (A)2.9 × 10^-4 (B)0.074 (C)0.033 (D)4.8 (E)0.0029

27. Calculate [H⁺] in a 0.40 M solution of NaH₂PO₄. (For H₃PO₄, K_a1 = 7.5 × 10^-3, K_a2 = 6.2 × 10^-8, K_a3 = 4.8 × 10^-13) (A)2.2 × 10^-5 M (B)1.6 × 10^-4 M (C)0.40 M (D)2.5 × 10^-4 M (E)3.9 × 10^-11 M

28. Based on the plot below, estimate the value of Ka for the weak acid.

(A)4.7 (B)2.0 × 10^-5 (C)2.6 (D)2.5 × 10^-3 (E)None of the above

29. The reduction potentials for Au3+ and Ni2+ are as follows:

Au³⁺ + 3e^- -＞ Au E° = +1.50 V

Ni²⁺ + 2e^- -＞ Ni E° = -0.23 V

Calculate ΔG° (at 25°C) for the reaction: 2Au³⁺ + 3Ni → 3Ni²⁺ + 2Au (A)-5.00 × 10² kJ (B)+5.00 × 10² kJ (C)-2140 kJ (D)+1.00 × 10³ kJ (E)-1.00 × 10³ kJ

30. Which statement is true of a process in which 1 mol of a gas is expanded from state A to state B? (A)When the gas expands from state A to state B, the surroundings are doing work on the system. (B)The amount of work done in the process must be the same, regardless of the path. (C)It is not possible to have more than one path for a change of state. (D)The final volume of the gas will depend on the path taken. (E)The amount of heat released in the process will depend on the path taken.

31. An ethyl group (CH₃CH₂^-) that is attached to a substituent that does not contain a hydrogen atom appears as what in a NMR spectrum? (A)a doublet and a triplet with relative intensities of 2 and 3, respectively (B)a doublet and a triplet with relative intensities of 3 and 2, respectively (C)a triplet and a quartet with relative intensities of 2 and 3, respectively (D)a triplet and a quartet with relative intensities of 3 and 2, respectively (E)none of these

32. Which base-pair is most stable in Watson-Crick DNA Structure? (A)(B)(C)(D) (E)

1.  The reaction: CH₃CHCH₂(g) + HCl(g) →CH₃CHClCH₃(g) and the possible mechanism is 

Complex + (HCl)₂ CH₃CHClCH₃ + 2HCl                               Slow equilibrium

Derive the rate law for this reaction using this mechanism.

2.Consider the following galvanic cell:

 Calculate the K_sp value for Ag₂SO₄(s). Note that to obtain silver ions in the right compartment (the cathode compartment), excess solid Ag₂SO₄ was added and some of the salt dissolved. (10^3.38~2400, 10^2.38~240, √7.5~2.7, √75~8.6)

 a.  Assuming that = 8996 J/mol and = 11,718 J/mol, calculate the value of the equilibrium constant for this reaction. 

b.  Calculate the equilibrium pressure that result if 1.00 mole of A_(g) at 1.00 atm and 1.00 mole of B_(g) at 1.00 atm are mixed at 25°C. (e_1.1 = 3.0, e_2.1 = 8.2)

a.  Calculate the frequency u (cm-¹) for ¹H³⁵Cl from v-0 to v=1 (that means equal to v₀), with its force constant is 4.80x10² J m². (¹H=1.0078amu,³⁵C1-34.9689amu, 1amu=1.627x10^-27kg)

b. What is the zero-point energy of ¹H³5Cl?