9. The following data were collected for the reaction between $H_2$ and NO at $700^{\circ}C$: The rate law of this reaction can be written as: $rate = (P{H2})^x(P{NO})^y$. Determine the coefficients x and y.
(A) x=1, y=0
(B) x=1, y=1
(C) x=1, y=2
(D) x=2, y=0
(E) x=2, y=1

10. Which compound is expected to have the highest melting point? (A) BaCl2 (B) HClO3 (C) C2H5OH (D) C6H12O6

11. Which of the following polymers is NOT synthesized by addition polymerization? (A) PP (B) PVC (C) PS (D) Teflon (E) PET

12. A gas has a mass of 30.8 grams and occupies \(9.24 \times 10^6\) mm3 at 0.873 atm and 21 °C. Assuming ideal gas behavior, determine the molar mass of this gas. (A) 16.0 g mol-1 (B) 44.1 g mol-1 (C) 70.9 g mol-1 (D) 92.1 g mol-1 (E) 106.2 g mol-1

13. Which graph below describes the vapor pressures (total and individual) of an ethanol (C2H5OH) and hexane (C6H14) mixture? Mixing ethanol and hexane is (A) I; endothermic (B) I; exothermic (C) II; endothermic (D) II; exothermic (E) III; endothermic

14. In the development of the hydrogen economy, one of the most crucial challenges is safely storing hydrogen gas. For example, magnesium metal has the hcp (hexagonal close-packed) lattice structure and can use the empty space between Mg atoms (interstitial sites) to store smaller hydrogen molecules. The overall reaction can be represented as: Mg(s) + H2(g) ⇌ MgH2(s) The equilibrium pressures of hydrogen gas at different temperatures are plotted in the figure to the right. Based on these data, what are the signs of ΔH and ΔS for this reaction? (A) ΔH > 0, ΔS > 0 (B) ΔH < 0, ΔS < 0 (C) ΔH < 0, ΔS > 0 (D) ΔH > 0, ΔS < 0 (E) There is no sufficient information to determine the signs of ΔH and ΔS

15. After adding 10 mL of 0.15 M KOH into 30 mL of 0.08 M HNO2 (Ka = 4.5 x 10-4), which of the following statements is NOT correct? (A) The neutralization reaction between KOH and HNO2 almost reaches completion. (B) The solution has a higher buffer capacity against strong bases than against strong acids. (C) The solution pH is still within the most effective buffer range. (D) The solution pH is approximately 3.57. (E) Compared to the original solution, the percent ionization of HNO2 is decreased. 

16. Which of the following compounds will be more soluble in an acidic solution than in pure water? (A) Ca3(PO4)2 (B) NH4Cl (C) FeBr3 (D) CuS (E) Sr(OH)2

17. Choose all correct descriptions of orbital hybridization. (A) A hybrid orbital is a special type of molecular orbital. (B) For the same atom, the energy of a sp hybrid orbital is lower than that of a sp2 hybrid orbital. (C) The sulfur atom in SF4 is sp3d-hybridized. (D) The central atoms of ClF4+ and PF5 have the same hybridization type. (E) The central atoms of CO2 and SO2 have the same hybridization type.

18. For a chemical reaction that has reached equilibrium, which statements are correct? (A) The concentrations of reactants and products do not change with time. (B) More products can be formed by increasing the temperature. (C) The reaction quotient equals the equilibrium constant K. (D) The Gibbs free energy change ΔG = 0. (E) The forward reaction rate and the reverse reaction rate are the same.

19. Using valence bond theory, which following statements correctly describe bonding in the nitrate ion (NO₃⁻)? (A) There exist multiple resonance structures. (B) Resonance structures transform rapidly between each other. (C) The nitrogen atom is sp² hybridized. (D) Among all three N-O bonds, one is shorter than the other two. (E) NO₃⁻ has no net dipole moment because the N-O bonds are non-polar.

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