2. Compound X₂Y is 60% X by mass. Calculate the percent Y by mass of the compound X₂Y₂.
(A) 30%
(B) 80%
(C) 40%
(D) 20%
(E) 60%

1. Which of the experiments listed below did not provide the information stated about the nature of the atom? (A) The Rutherford experiment proved that the Thomson "plum pudding" model of the atom was essentially correct. (B) The Rutherford experiment determined the charge on the nucleus. (C) The cathode-ray tube proved that electrons have a negative charge. (D) Millikan's oil-drop experiment showed that the charge on any particle was a simple multiple of the charge on the electron.

3. The following unbalanced reaction occurs in basic media:Fe2+ + Cr2O72- → Fe3+ + Cr3+The coefficient for water in the balanced equation is _______ and water appears on the _______ side of the equation. (A) 14, left (B) 14, right (C) 7, right (D) 7, left (E) none of these

4. How is the observed pressure of a gas related to the ideal pressure? (A) The relationship depends on the gas. (B) They are equal. (C) The observed pressure is greater than the ideal pressure. (D) The observed pressure is less than the ideal pressure. (E) none of these

5. For the reaction 2H2(g) + O2(g) ⇌ 2H2O(g), what is the relationship between K and Kp at temperature T? (A) Kp = K(RT)2 (B) K = Kp(RT) (C) K = Kp (D) Kp = K(RT) (E) K = Kp(RT)2

6. The acids HC2H3O2 and HF are both weak, but HF is a stronger acid than HC2H3O2. HCl is a strong acid. Order the following according to base strength. (A) Cl- ＞ F- ＞ C2H3O2- ＞ H2O (B) C2H3O2- ＞ F- ＞ H2O ＞ Cl- (C) C2H3O2- ＞ F- ＞ Cl- ＞ H2O (D) F- ＞ C2H3O2- ＞ H2O ＞ Cl- (E) none of these

7. Consider a solution consisting of the following two buffer systems:H2CO3 ⇌ HCO3- + H+  pKa = 6.4H2PO4- ⇌ HPO42- + H+  pKa = 7.2At pH 6.4, which one of the following is true of the relative amounts of acid and conjugate base present? (A) [H2CO3] ＞ [HCO3-] and [H2PO4-] ＞ [HPO42-] (B) [HCO3-] ＞ [H2CO3] and [HPO42-] ＞ [H2PO4-] (C) [H2CO3] ＞ [HCO3-] and [HPO42-] ＞ [H2PO4] (D) [H2CO3] = [HCO3-] and [HPO42-] ＞ [H2PO4] (E) [H2CO3] = [HCO3-] and [H2PO4-] ＞ [HPO42-]

8. Which statement is true of a process in which 1 mol of a gas is expanded from state A to state B? (A) The final volume of the gas will depend on the path taken. (B) The amount of work done in the process must be the same, regardless of the path. (C) When the gas expands from state A to state B, the surroundings are doing work on the system. (D) The amount of heat released in the process will depend on the path taken. (E) It is not possible to have more than one path for a change of state.

9. Consider the dissociation reaction of the acidHF.HF(aq) ⇌ H+(aq) + F-(aq)Why is ΔS negative? (A) The reaction is expected to be exothermic, and ΔS thus should be negative. (B) The reaction is expected to be endothermic, and thus ΔS should be negative. (C) Each HF molecule produces two ions when it dissociates. (D) The ions are hydrated. (E) none of these

10. In which of the following cases can Eº be equal to zero?I. In any cell at equilibrium II. In a concentration cellIII. Eº can never be equal to zero. (A) I only (B) III (C) I and II (D) II only (E) none of these

11. For a reaction in a voltaic cell, both ΔHº and ΔSº are positive. Which of the following statements is true? (A) Eºcell will increase with an increase in temperature. (B) Eºcell will decrease with an increase in temperature. (C) Eºcell will not change when the temperature increases. (D) ΔGº> 0 for all temperatures. (E) None of the above statements is true.

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