19. For which of the following species are the intermolecular interactions entirely due to dispersion forces?
(A) C₂H₆
(B) CH₃OCH₃
(C) NO₂
(D) H₂S

20. Which of the following liquids would have the highest viscosity at 25°C? (A) CH3OCH3 (B) C2H5OH (C) CH3Br (D) HOCH2CH2OH

21. A 15.00 % by mass solution of lactose (C12H22O11, 342.30 g/mol) in water has a density of 1.0602 g/mL at 20°C. What is the molarity of this solution? (A) 0.03097 M (B) 0.4133 M (C) 0.4646 M (D) 1.590 M (E) 1.379 M

22. Which of the following systems possesses the lowest freezing point? (A) 0.1 M FeCl3(aq) (B) 0.1 M K2SO4(aq) (C) 0.1 M CaCl2(aq) (D) 0.3 M C6H12O6, glucose (E) 0.1 M NaCl

23. For a particular process q = 20 kJ and w = 15 kJ. Which of the following statements is true? (A) Heat flows from the system to the surroundings. (B) The system does work on the surroundings. (C) E = 35 kJ (D) All of the above are true. (E) None of these choices is correct.

24. Which of the following results in a decrease in the entropy of the system? (A) O2(g), 300 K→O2(g), 400 K (B) H2O(s), 0°C→ H2O(l), 0°C (C) N2(g), 25°C→N2(aq), 25°C (D) NH3(l), -34.5°C→ NH3(g), -34.5°C (E) 2H2O2(g)→ 2H2O(g) + O2(g)

25. Given the following acids and Ka values:What is the order of increasing base strength? (A) CN–, F–, OAc–, ClO4– (B) CN–, OAc–, F–, ClO4– (C) CN–, ClO4–, F–, OAc– (D) ClO4–, OAc–, CN–, F– (E) ClO4–, F–, OAc–, CN–

26. According to the first law of thermodynamics, the energy of the universe is constant. Does this mean that ΔE is always equal to zero? (A) Yes, ΔE = 0 at all times, which is why q = -w. (B) No, ΔE does not always equal zero, but this is only due to factors like friction and heat. (C) No, ΔE does not always equal zero because it refers to the system's internal energy, which is affected by heat and work. (D) No, ΔE never equals zero because work is always being done on the system or by the system. (E) None of these

27. Calculate the pH of the following aqueous solution: 0.66 M NaF (pKa for HF = 3.14) (A) 5.52 (B) 2.96 (C) 8.48 (D) 11.04 (E) none of these

28. Colligative properties depend on (A) the chemical properties of the solute. (B) the chemical properties of the solvent. (C) the masses of the individual ions. (D) the molar mass of the solute. (E) the number of particles dissolved.

29. A 0.100 m K2SO4 solution has a freezing point of -0.43°C. What is the van't Hoff factor for this solution? Kf = 1.86°C/m (A) 0.77 (B) 1.0 (C) 2.3 (D) 3.0 (E) >3.0

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