11. The mass percent of iron in an iron oxide is 77.7%. Find the empirical formula.
(A) Fe3O2
(B) Fe3O4
(C) Fe2O3
(D) FeO
(E) none of these

12. When the equation FeCr2O4 + K2CO3 + O2 → K2CrO4 + Fe2O3 + CO2 is balanced with the smallest set of integers, the sum of the coefficients is (A) 9 (B) 15 (C) 6 (D) 37 (E) 24

13. Which of below does not have the same units as energy or energy per mole? (A) PV (B) RT (C) TS (D) nFE (E) I2R

14. Consider the following numbered processes: 1. A → 2B 2. B → C + D 3. E → 2D ΔH for the process A → 2C + E is (A) ΔH1 + ΔH2 (B) ΔH1 + 2ΔH2 – ΔH3 (C) ΔH1 + ΔH2 + ΔH3 (D) ΔH1 + 2ΔH2 + ΔH3 (E) ΔH1 + ΔH2 – ΔH3

15. Which is wrong? (A) bomb calorimeter measures ΔH directly. (B) In an adiabatic process, q = 0 and ΔS = 0. (C) In a process of free expansion, w = 0. (D) In an isothermal process, ΔH = 0. (E) Breaking a chemical bonding is usually an endothermic reaction.

16. The following reaction is investigated (assume an ideal gas mixture). 2N2O(g) + N2H4(g) 3N2(g) + 2H2O(g) Initially there are 0.08 mol of N2O and 0.38 mol of N2H4, in a 30.0-L container. If there is 0.050 mol of N2O at equilibrium, how many moles of N2 are present at equilibrium? (A) 0.053 (B) 0.045 (C) 0.12 (D) 0.030 (E) 0.15

17. When doubling the volume of a buffer solution containing a weak acid and its conjugate base, which is correct? (A) pH will shift toward the pKa of the acid. (B) pH will significantly increase. (C) The buffer capacity will decrease. (D) Its titration curve remains the same. (E) pH will decrease when using a base and it conjugated acid as the buffer solution.

18. Calculate the concentration of chromate ion, CrO4 2–, in a saturated solution of CaCrO4 (Ksp = 7.1 × 10–4). (A) 2.7 × 10–2 M (B) 3.5 × 10–2 M (C) 7.1 × 10–4 M (D) 3.5 × 10–4 M (E) 5.0 × 10–7 M

19. How many moles of HCl(g) must be added to 1.0 L of 2.0 M NaOH to achieve a pH of 0.00? (Neglect any volume change.) (A) 3.0 mol (B) 10. mol (C) 1.0 mol (D) 2.0 mol (E) none of these

20. For a titration reaction of a weak acid, which is correct? (A) The pH of the equivalence point is dependent of the original concentrations or volumes. (B) At the equivalence point, the pH can be found by the pKa of the acid and pKb of the base. (C) The pH of the end point is depended on the pKa of the acid and pKb of the base. (D) The initial pH is not affected by the concentration. (E) The end point is always at the center of the steepest section of the titration curve no matter of the stoichiometry of reactions or the choice of indicator.

21. How many electrons are transferred in the following reaction? SO3 2–(aq) + MnO4 – (aq) → SO4 2–(aq) + Mn2+(aq) (A) 4 (B) 10 (C) 3 (D) 2 (E) 6

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