18. Which one of the following decreases as the strength of the attractive intermolecular forces increases?
(A) the heat of vaporization
(B) the normal boiling temperature
(C) the extent of deviations from the ideal gas law
(D) the sublimation temperature of a solid
(E) the vapor pressure of a liquid

37. Which one of following decreases as the strength of the attractive intermolecular forces increases? (A)The heat of vaporization. (B)The normal boiling temperature. (C)The extent of deviations from the ideal gas law. (D)The sublimation temperature of a solid. (E)The vapor pressure of a liquid.

19. Determine the osmotic pressure of a solution that contains 0.048 g of a hydrocarbon solute (molar mass = 340 g/mol) dissolved in benzene to make a 350-mL solution. The temperature is 20.0°C. (A) 0.50 torr (B) 2.5 torr (C) 3.3 torr (D) 7.4 torr (E) 6.9 torr

20. For a reaction: aA → Products, $[\text{A}]_0 = 6.0 \text{ M}$, and the first two half-lives are 56 and 28 minutes, respectively. Calculate $[\text{A}]$ at $t = 105.9$ minutes. (A) 5.7 M (B) 12 M (C) 0.68 M (D) 0.33 M (E) none of these

21. Consider the following reaction: $\text{CS}2(g) + 4\text{H}2(g) \rightleftharpoons \text{CH}4(g) + 2\text{H}2\text{S}(g)$. The equilibrium constant $K$ is about 0.31 at 900°C. What is the $K_p$ at this temperature? (A) $2.9 \times 10^3$ (B) $3.2 \times 10^{-3}$ (C) $3.3 \times 10^{-5}$ (D) $3.0 \times 10^1$ (E) $1.1 \times 10^{-3}$

22. The questions below refer to the following system: $$\text{Co}(\text{H}2\text{O}){6}^{2+} + 4 \text{Cl}^- \rightleftharpoons \text{CoCl}4^{2-} + 6\text{H}2\text{O}$$ When cobalt(II) chloride is added to pure water, the $\text{Co}^{2+}$ ions hydrate. The hydrated form then reacts with the $\text{Cl}^-$ ions to set up the equilibrium shown here. Which statement below describes the change that the system will undergo if silver nitrate is added? (A) It should become more blue. (B) It should become more pink. (C) Water will be produced. (D) The silver ion will react with the $\text{CoCl}_4^{2-}$. (E) Nothing will change.

23. Using the following $K_a$ values, indicate the correct order of base strength. $$\text{HNO}_2 \text{ Ka} = 4.0 \times 10^{-4} \quad \text{HF Ka} = 7.2 \times 10^{-4} \quad \text{HCN Ka} = 6.2 \times 10^{-10}$$ (A) $\text{CN}^- > \text{NO}2^- > \text{F}^- > \text{H}2\text{O} > \text{Cl}^-$ (B) $\text{Cl}^- > \text{H}2\text{O} > \text{F}^- > \text{NO}2^- > \text{CN}^-$ (C) $\text{CN}^- > \text{F}^- > \text{NO}2^- > \text{Cl}^- > \text{H}2\text{O}$ (D) $\text{H}2\text{O} > \text{CN}^- > \text{NO}2^- > \text{F}^- > \text{Cl}^-$ (E) none of these

24. The standard molar free energies of formation of $\text{NO}2(g)$ and $\text{N}2\text{O}_4(g)$ at 25°C are 51.840 and 98.035 kJ/mol, respectively. What is the value of $Kp$ (in atm) for the reaction written as follows at 25°C? $2\text{NO}2 \rightleftharpoons \text{N}2\text{O}4$ (A) $6.24 \times 10^{11}$ (B) 1.00 (C) 9.76 (D) $4.38 \times 10^{-36}$ (E) $7.99 \times 10^{-9}$

25. The titration curve for 50.00 mL 1.000M disodium ascorbate, $\text{Na}_2\text{As}$, with standard 1.000M HCl is shown below: The pH at point I and III are 11.79 and 4.10, respectively, which of the following would be the pKa1 of the diprotic acid, $\text{H}_2\text{As}$ (A) 4.10 (B) 7.95 (C) 11.79 (D) 12.39 (E) none of these

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