38. In the unit cell of sphalerite, \( Zn^{2+} \) ions occupy half the tetrahedral holes in a face-centered cubic lattice of \( S^{2-} \) ions. What is the number of formula units of ZnS in the unit cell?
(A) 2
(B) 3
(C) 4
(D) 6
(E) 8

1. Which of the following is *not* the correct chemical formula for the compound named? (A)\( Al(OH)_2 \) aluminum hydroxide (B) LiCN lithium cyanide (C) \( Fe_2O_3 \) Iron(III) oxide (D) ZnSe zinc selenide (E) \( Mg(C_2H_3O_2)_2 \) magnesium acetate

2. Which is the correct formula for gold(I) sulfide? (A) AuS (B) \( Au_2S \) (C) \( AuS_2 \) (D) \( Au_2S_3 \) (E) \( Au_2S_2 \)

3. When \( NH_3(aq) \) is added to \( Cu^{2+}(aq) \), a precipitate initially forms. What is its formula? (A) \( Cu(NH_3)_2 \) (B) \( Cu(NO_3)_2 \) (C) CuO (D) \( Cu(NH_3)_2^{2+} \) (E) \( Cu(OH)_2 \)

4. True or false? The equation \( 2C_2H_6 + 7O_2 \rightarrow 4CO_2 + 6H_2O \) is an oxidation-reduction reaction. (A) True; the oxygen is reduced and the hydrogen is oxidized. (B) True; the carbon is oxidized and the hydrogen is reduced. (C) True; the carbon is oxidized and the oxygen is reduced. (D) True; the carbon is reduced and the oxygen is oxidized. (E) False

5. Consider two samples of helium in separate containers of the same volume. Sample 1 has an absolute temperature four times that of Sample 2. Both samples are at the same pressure. Calculate the ratio \( n_1:n_2 \). (A) 1:1 (B) 1:2 (C) 2:1 (D) 1:4 (E) 4:1

6. Which of the following statements concerning equilibrium is *not* true? (A) A system that is disturbed from an equilibrium condition responds in such a way as to restore equilibrium. (B) A system moves spontaneously toward a state of equilibrium. (C) Equilibrium in molecular systems is dynamic, with two opposing processes balancing one another. (D) The value of the equilibrium constant for a given reaction mixture is the same regardless of the direction from which equilibrium is attained. (E) The equilibrium constant is independent of temperature.

7. For the reaction \( 2H_2(g) + O_2(g) \rightleftharpoons 2H_2O(g) \), what is the relationship between \( K \) and \( K_p \) at temperature \( T \)? (A) \( K = K_p \) (B) \( K = K_p(RT) \) (C) \( K_p = K(RT) \) (D) \( K = K_p(RT)^2 \) (E) \( K_p = K(RT)^2 \)

8. When the substances in the equation below are at equilibrium at pressure \( P \) and temperature \( T \), how can the equilibrium be shifted to favor the products? \( CuO(s) + H_2(g) \rightleftharpoons Cu(s) + H_2O(g) \) Change in enthalpy = −2.0 kJ. (A) Decrease the temperature. (B) Increase the temperature. (C) Add a catalyst. (D) Increase the pressure by adding an inert gas such as nitrogen. (E) Allow some gas to escape at constant pressure and temperature.

9. The acids \( HC_2H_3O_2 \) and HF are both weak, but HF is a stronger acid than \( HC_2H_3O_2 \). HCl is a strong acid. Order the following according to base strength. (A) \( C_2H_3O_2^- ＞ F^- ＞ Cl^- ＞ H_2O \) (B) \( Cl^- ＞ F^- ＞ C_2H_3O_2^- ＞ H_2O \) (C) \( C_2H_3O_2^- ＞ F^- ＞ H_2O ＞ Cl^- \) (D) \( F^- ＞ C_2H_3O_2^- ＞ H_2O ＞ Cl^- \) (E) none of these

10. HOAc \( K_a = 1.8 \times 10^{-5} \) \( H_2CO_3 \) \( K_{a1} = 4.3 \times 10^{-7} \), \( K_{a2} = 5.6 \times 10^{-11} \) Which of the following 0.01 M solutions has the highest pH? (A) HOAc (B) NaOAc (C) \( H_2CO_3 \) (D) \( Na_2CO_3 \) (E) \( NaHCO_3 \)

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