17. The rate constant k is dependent on
I. the concentration of the reactant
II. the nature of the reactants
III. the temperature
IV. the order of the reaction

(A) none of these
(B) one of these
(C) two of these
(D) three of these
(E) all of these

18. Consider the following equilibrium: 2NOCl(g) ⇌ 2NO(g) + Cl2(g) with K = 1.6 x 10-5. 1.00 mole of pure NOCl and 0.967 mole of pure Cl2 are placed in a 1.00-L container. Calculate the equilibrium concentration of Cl2(g). (A) 1.6 x 10-5 M (B) 0.969 M (C) 0.485 M (D) 2.03 x 10-3 M (E) 4.07 x 10-3 M

19. Substance X has a heat of vaporization of 52.1 kJ/mol at its normal boiling point (423°C). For the process X(l) → X(g) at 1 atm and 423°C calculate the value of ΔS. (A) 0 (B) 74.9 J/K mol (C) 123 J/K mol (D) -74.9 J/K mol (E) -123 J/K mol

20. The following reaction has a ΔG° value of 48.71 kJ/mol at 25°C. HB(aq) + H2O(l) ⇌ H3O+(aq) + B-(aq) Calculate the Ka for the acid HB. (A) 0.981 (B) -19.7 (C) 2.89 x 10-9 (D) 4.87 x 10-5 (E) -234

1. Boron consists of two naturally occurring isotopes, ¹⁰B and ¹¹B. Bromine also has two naturally occurring isotopes, ⁷⁹Br and ⁸¹Br. How many molecular-ion peaks would be expected in the mass spectrum of BBr₃? (A) 2 (B) 4 (C) 6 (D) 8 (E) 12

2. A balloon has a volume of 3.02 L at 27°C. The balloon is heated to 127°C at constant pressure. What is the new volume of the balloon? (A) 2.82 L (B) 3.27 L (C) 4.03 L (D) 4.88 L (E) 14.2 L

3. For the following hypothetical reactions,  I. A₂(g) + B₂(g) ⇌ 2AB(g) K_I = 10²  II. 2A₂(g) + C₂(g) ⇌ 2A₂C(g) K_II = 10⁻⁴ III. A₂C(g) + B₂(g) ⇌ 2AB(g) + 1/2 C₂(g) What is the equilibrium constant, K, for reaction III? (A) 10⁻² (B) 10² (C) 10⁴ (D) 10⁶ (E) 10⁸

4. Nitrogen gas reacts with hydrogen gas to form ammonia: N₂(g) + 3H₂(g) ⇌ 2NH₃(g) At 200°C in a rigid container, 1.2 atm of N₂ and 2.3 atm of H₂ are mixed. At equilibrium, the total pressure is 2.1 atm. What is the equilibrium partial pressure of H₂? (A) 0.92 atm (B) 0.20 atm (C) 1.2 atm (D) 1.8 atm (E) 0.35 atm

5. According to the Brønsted-Lowry definition, an acid is (A) a substance that increases the hydrogen ion concentration in solution. (B) a substance that increases the hydroxide ion concentration in solution. (C) a substance that can donate a proton to another species. (D) a substance that can accept a proton from another species. (E) an electron pair acceptor.

6. Which of the following 0.01 M aqueous solutions has the highest pH value? (A) HOAc (B) NaHCO₃ (C) H₂CO₃ (D) NaOAc (E) Na₂CO₃

7. Consider a solution of 2.0 M HCN (K_a = 6.2 × 10⁻¹⁰) and 1.0 M NaCN. Which statement is true? (A) The solution is not a buffer because [HCN] is not equal to [CN⁻]. (B) The buffer is more resistant to pH changes from added strong acid than from added strong base. (C) [OH⁻] > [H⁺] (D) The pH is below 7.00 because the concentration of the acid is greater than that of the base. (E) All of these statements are false.

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