21. A 7.05-g sample of potassium chlorate was decomposed according to the following equation:

\[ 2\text{KClO}_3 \rightarrow 2\text{KCl} + 3\text{O}_2 \]

How many moles of oxygen are formed? (KClO₃ 122.55 g/mol)
(A) 0.0863 mol
(B) 0.0575 mol
(C) 0.0384 mol
(D) 0.0288 mol

22. The limiting reactant in a reaction (A) has the lowest coefficient in a balanced equation. (B) is the reactant for which you have the fewest number of moles. (C) has the lowest ratio of coefficient in the balanced equation/moles available. (D)has the lowest ratio of moles available/coefficient in the balanced equation. 

23. Consider the following reaction: 2A + B  3C + D. 3.0 mol A and 2.0 mol B react to form 3.8 mol C. What is the percent yield of this reaction? (A) 63% (B) 75% (C) 84% (D) 89%

24. Determine the mass of a nonvolatile, nonionizing compound that must be added to 3.90 kg of water to lower the freezing point to -1.30°C. The molar mass of the compound is 50.0 g/mol and the Kf for water is 1.86°C kg/mol. (A) 8.96 g (B) 18.3 g (C) 68.0 g (D) 136 g

25. Initial rate data have been determined at a certain temperature for the gaseous reaction 2NO + 2H2 <=> N2 + 2H2O What is the rate law? (A) Rate = k[NO][H2] (B) Rate = k[NO][H2]2 (C) Rate = k[NO]2[H2] (D) Rate = k[NO]2[H2]2

26. Chemists commonly use a rule of thumb that an increase of 10 K in temperature doubles the rate of a reaction. What must the activation energy be for this statement to be true for a temperature increase from 20°C to 30°C? (A) 51.2 (B) 49.5 (C) 46.1 (D) 56.7 kJ/mol

27. The value of the equilibrium constant, K, is dependent on: I. the nature of the reactants and products II., the concentration of the reactants and products, III. the temperature of the system, IV. the pressure of the system. (A) I, II (B) I, III (C) I, II, III (D) I, II, IV

28. The autoionization of water, \( \text{H}_2\text{O}(l) + \text{H}_2\text{O}(l) \rightleftharpoons \text{H}_3\text{O}^+(aq) + \text{OH}^-(aq) \), is known to be endothermic. Which of the following correctly states what occurs as the temperature of water is raised? (A) The pH of the water does not change, and the water remains neutral. (B) The pH of the water decreases, and the water becomes more acidic. (C) The pH of the water increases, and the water remains neutral. (D) The pH of the water decreases, and the water remains neutral.

29. Which of the following is the strongest reducing agent? \( \text{Zn}^{2+} + 2\text{e}^- \rightleftharpoons \text{Zn} \quad E^\circ = -0.76 \text{ V}; \text{MnO}_4^- + 4\text{H}^+ + 3\text{e}^- \rightleftharpoons \text{MnO}_2 + 2\text{H}_2\text{O} \quad E^\circ = 1.68 \text{ V}; 2\text{H}^+ + 2\text{e}^- \rightleftharpoons \text{H}_2 \quad E^\circ = \) 0.00 V; \( \text{Cl}_2 + 2\text{e}^- \rightleftharpoons 2\text{Cl}^- \quad E^\circ = 1.36 \text{ V}. \) (A) Zn (B) MnO2 (C) H2 (D) Cl2

30. What is the potential at 25°C for the cell: Cr|Cr3+(0.030 M)||Ag+(0.00030 M)|Ag? Cr3+ + 3e- <=> Cr Eo = -0.73 V; Ag+ + e- <=> Ag Eo = 0.80 V (A) 0.95 V (B) 1.35 V (C) 1.49 V (D) 1.71 V

31. Which of the following solutions will be the best buffer at a pH of 4.74? (Ka for acetic acid, HC2H3O2, is 1.8 × 10-5, Ka for benzoic acid, HC7H5O2, is 6.4×10-5) (A) 0.10 M HC2H3O2 + 0.10 M NaC2H3O2 (B) 5.0 M HC2H3O2 + 5.0 M Na C2H3O2 (C) 0.50 M HC7H5O2 + 0.14 M KC7H5O2 (D) 5.0 M HC7H5O2 + 1.4 M KC7H5O2

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