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Questions 6-7 refer to the following solid compounds. (A) PbSO4 (B) CuO (C) KMnO4 (D) KCl (E) FeCl3 7. Is white and very soluble in water

... Cr2O7 2-(aq) + .. . H2S(g) + ... H+(aq) ... Cr3+(aq) + ... S(s) + ... H2O(l) 49. When the equation above is correctly balanced and all coefficients are reduced to lowest whole-number terms, the coefficient for H+(aq) is (A) 2 (B) 4 (C) 6 (D) 8 (E) 14

20. A flask contains 0.25 mole of SO2(g), 0.50 mole of CH4(g), and 0.50 mole of O2(g). The total pressure of the gases in the flask is 800 mm Hg. What is the partial pressure of the SO2(g) in the flask? (A) 800 mm Hg (B) 600 mm Hg (C) 250 mm Hg (D) 200 mm Hg (E) 160 mm Hg

21. In the laboratory, H2(g) can be produced by adding which of the following to 1 M HCl(aq)? I. 1 M NH3(aq) II. Zn(s) III. NaHCO3(s) (A) I only (B) II only (C) III only (D) I and II only (E) I, II, and Ill

3 C2H2(g) C6H6(g) 25. What is the standard enthalpy change, ΔH˚, for the reaction represented above? (ΔH˚f of C2H2(g) is 230 kJ mol-1; ΔH˚f of C6H6(g) is 83 kJ mol-1.) (A) -607 kJ (B) -147 kJ (C) -19 kJ (D) +19 kJ (E) +773 kJ

40. An excess of Mg(s) is added to 100. mL of 0.400 M HCl. At 0˚C and 1 atm pressure, what volume of H2 gas can be obtained? (A) 22.4 mL (B) 44.8 mL (C) 224 mL (D) 448 mL (E) 896 mL

59. All of the halogens in their elemental form at 25˚C and 1 atm are (A) conductors of electricity (B) diatomic molecules (C) odorless (D) colorless (E) gases

57. Molecules that have planar configurations include which of the following? I. BCl3 II. CHCl3 III. NCl3 (A) I only (B) III only (C) I and II only (D) II and III only (E) I, II, and III

57. rate = k[X] For the reaction whose rate law is given above, a plot of which of the following is a straight line? (A) [X] versus time (B) log [X] versus time (C) 1/[X] versus time (D) [X] versus 1/time (E) log [X] versus 1/time

69. What is the mole fraction of ethanol, C2H5OH, in an aqueous solution in which the ethanol concentration is 4.6 molal? (A) 0.0046 (B) 0.076 (C) 0.083 (D) 0.20 (E) 0.72

80. For which of the following molecules are resonance structures necessary to describe the bonding satisfactorily? (A) H2S (B) SO2 (C) CO2 (D) OF2 (E) PF3

(A) Activation energy (B) Free energy (C) Ionization energy (D) Kinetic energy (E) Lattice energy 3. The energy in a chemical or physical change that is available to do useful work

B (Free Energy)

32. A 2.00-liter sample of nitrogen gas at 27 °C and 600. millimeters of mercury is heated until it occupies a volume of 5.00 liters. If the pressure remains unchanged, the final temperature of the gas is (A) 68 °C (B) 120 °C (C) 477 °C (D) 677 °C (E) 950. °C

(A) Activation energy (B) Free energy (C) Ionization energy (D) Kinetic energy (E) Lattice energy 1. The energy required to convert a ground-state atom in the gas phase to a gaseous positive ion

C (Ionization Energy)

(A) O (B) La (C) Rb (D) Mg (E) N 3. Which of the elements above has the smallest ionic radius for its most commonly found ion?

(A) a solution with a pH less than 7 that is not a buffer solution (B) a buffer solution with a pH between 4 and 7 (C) a buffer solution with a pH between 7 and 10 (D) a solution with a pH greater than 7 that is not a buffer solution (E) a solution with a pH of 7 Ionization Constants CH3COOH = 1.8 x 10¯5 NH3 = 1.8 x 10¯5 H2CO3; K1 = 4 x 10¯7 H2CO3; K2 = 4 x 10¯11 9. A solution prepared to be initially 1 M in Na2CO3 and 1 M in CH3COONa

Questions 11-13 (A) Pb (B) Ca (C) Zn (D) As (E) Na 12. Is added to silicon to enhance its properties as a semiconductor

23. How many grams of calcium nitrate, Ca(NO3)2, contains 24 grams of oxygen atoms? (A) 164 grams (B) 96 grams (C) 62 grams (D) 50. grams (E) 41 grams

Questions 1-4 (A) Heisenberg uncertainty principle (B) Pauli exclusion principle (C) Hund's rule (principle of maximum multiplicity) (D) Shielding effect (E) Wave nature of matter 2. Explains the experimental phenomenon of electron diffraction

Look at Equation 23. Neutron bombardment of uranium can induce the reaction represented above. Nuclide X is which of the following? (A) 92 35 Br (B) 94 35 Br (C) 91 37 Rb (D) 92 37 Rb (E) 94 37 Rb

Questions 1-2 Consider atoms of the following elements. Assume that the atoms are in the ground state. (A) S (B) Ca (C) Ga (D) Sb (E) Br 1. The atom that contains exactly two unpaired electrons

Questions 1-2 Consider atoms of the following elements. Assume that the atoms are in the ground state. (A) S (B) Ca (C) Ga (D) Sb (E) Br 2. The atom that contains only one electron in the highest occupied energy sublevel

Questions 8-10 refer to the following gases at 0˚C and 1 atm. (A) Ne (B) Xe (C) O2 (D) CO (E) NO 8. Has an average atomic or molecular speed closest to that of N2 molecules at 0˚C and 1 atm

Questions 8-10 refer to the following gases at 0˚C and 1 atm. (A) Ne (B) Xe (C) O2 (D) CO (E) NO 10. Has the greatest rate of effusion through a pinhole

Questions 8-10 refer to the following gases at 0˚C and 1 atm. (A) Ne (B) Xe (C) O2 (D) CO (E) NO 9. Has the greatest density

Rate = k[M][N]2 57. The rate of a certain chemical reaction between substances M and N obeys the rate law above. The reaction is first studied with [M] and [N] each 1 x 10^-3 molar. If a new experiment is conducted with [M] and [N] each 2 x 10^-3 molar, the reaction rate will increase by a factor of (A) 2 (B) 4 (C) 6 (D) 8 (E) 16

26. Approximately what mass of CuSO4•5H2O (250 g mol-1) is required to prepare 250 mL of 0.10 M copper(II) sulfate solution? (A) 4.0 g (B) 6.2 g (C) 34 g (D) 85 g (E) 140 g

(A) hydrogen bonding (B) hybridization (C) ionic bonding (D) resonance (E) van der Waals forces (London dispersion forces) 12. Is used to explain why the boiling point of HF is greater than the boiling point of HBr

18. Reacts with water to form a strong base (A) Lithium (B) Nickel (C) Bromine (D) Uranium (E) Fluorine

24. The formula for potassium hexacyanoferrate(II) is (A) K4[Fe(CN)6] (B) K3[Fe(CN)6] (C) K2[Pt(CN)4] (D) K2[Pt(CN)6] (E) KCN

56. A yellow precipitate forms when 0.5 M NaI(aq) is added to a 0.5 M solution of which of the following ions? A) Pb2+(aq) B) Zn2+(aq) C) CrO42¯(aq) D) SO42¯(aq) E) OH¯(aq)

Look for Answers 43. Which of the following pairs of compounds are isomers? (A) (B) (C) (D) (E)

1. Forms monatomic ions with 2¯ charge in solutions (A) F (B) S (C) Mg (D) Ar (E) Mn

16. Commercial vinegar was titrated with NaOH solution to determine the content of acetic acid, HC2H3O2. For 20.0 milliliters of the vinegar 26.7 milliliters of 0.600-molar NaOH solution was required. What was the concentration of acetic acid in the vinegar if no other acid was present? (A) 1.60 M (B) 0.800 M (C) 0.600 M (D) 0.450 M (E) 0.200 M

18. For the types of radiation given, which of the following is the correct order of increasing ability to penetrate a piece of lead? (A) Alpha particles < gamma rays < beta particles (B) Alpha particles < beta particles < gamma rays (C) Beta particles < alpha particles < gamma rays (D) Beta particles < gamma rays < alpha particles (E) Gamma rays < alpha particles < beta particles

23. Step 1: Ce4+ + Mn2+ ---> Ce3+ + Mn3+ Step 2: Ce4+ + Mn3+ ---> Ce3+ + Mn4+ Step 3: Mn4+ + Tl+ ---> Tl3+ + Mn2+ The proposed steps for a catalyzed reaction between Ce4+ and Tl+ are represented above. The products of the overall catalyzed reaction are (A) Ce4+ and Tl+ (B) Ce3+ and Tl3+ (C) Ce3+ and Mn3+ (D) Ce3+ and Mn4+ (E) Tl3+ and Mn2+

23. The density of an unknown gas is 4.20 grams per liter at 3.00 atmospheres pressure and 127 °C. What is the molecular weight of this gas? (R = 0.0821 liter-atm / mole-K) (A) 14.6 (B) 46.0 (C) 88.0 (D) 94.1 (E) 138

38. 98-Cf-251 ---> 2n + 54-Xe-131 + __ What is the missing product in the nuclear reaction represented above? (A) 42-Mo-118 (B) 44-Ru-118 (C) 42-Mo-120 (D) 44-Ru-120 (E) 46-Pd-122

58. N2(g) + 3 H2(g) ---> 2 NH3(g) The reaction indicated above is thermodynamically spontaneous at 298 K, but becomes nonspontaneous at higher temperatures. Which of the following is true at 298 K? (A) DG, DH, and DS are all positive. (B) DG, DH, and DS are all negative. (C) DG and DH are negative, but DS is positive. (D) DG and DS are negative, but DH is positive. (E) DG and DH are positive, but DS is negative.

63. What is the maximum mass of copper that could be plated out by electrolyzing aqueous CuCl2 for 16.0 hours at a constant current of 3.00 amperes? (1 faraday = 96,500 coulombs) (A) 28 grams (B) 57 grams (C) 64 grams (D) 114 grams (E) 128 grams

63. Which of the following characteristics is common to elemental sulfur, chlorine, nitrogen, and carbon? (A) They are gaseous elements at room temperature. (B) They have oxides that are acid anhydrides. (C) They have perceptible color at room temperature. (D) They form ionic oxides. (E) They react readily with hydrogen at room temperature.

71. In a qualitative ananlysis for the presence of Pb2+, Fe2+, and Cu2+ ions in a aqueous solution, which of the following will allow the separation of Pb2+ from the other ions at room temperature? A) Adding dilute Na2S(aq) solution B) Adding dilute HCl(aq) solution C) Adding dilute NaOH(aq) solution D) Adding dilute NH3(aq) solution E) Adding dilute HNO3(aq) solution

72. After completing an experiment to determine gravimetrically the percentage of water in a hydrate, a student reported a value of 38 percent. The correct value for the percentage of water in the hydrate is 51 percent. Which of the following is the most likely explanation for this difference? A) Strong initial heating caused some of the hydrate sample to spatter out of the crucible. B) The dehydrated sample absorbed moisture after heating. C) The amount of the hydrate sample used was too small. D) The crucible was not heated to constant mass before use. E) Excess heating caused the dehydrated sample to decompose.

74. Equal volumes of 0.10-molar H3PO4 and 0.20-molar KOH are mixed. After equilibrium is established, the type of ion an solution in largest concentration, other than the K+ ion, is (A) H2PO4¯ (B) HPO42¯ (C) PO43¯ (D) OH¯ (E) H3O+

75. A direct-current power supply of low voltage (less than 10 volts) has lost the markings that indicate which output terminal is positive and which is negative. A chemist suggests that the power supply terminals be connected to a pair of platinum electrodes that dip into 0.1-molar KI solution. Which of the following correctly identifies the polarities of the power supply terminals? (A) A gas will be evolved only at the positive electrode. (B) A gas will be evolved only at the negative electrode. (C) A brown color will appear in the solution near the negative electrode. (D) A metal will be deposited on the positive electrode. (E) None of the methods above will identify the polarities of the power supply terminals.

76. HgO(s) + 4 I¯ + H2O <===> HgI42¯ + 2 OH¯; DH < 0 Consider the equilibrium above. Which of the following changes will increase the concentration of HgI42¯? (A) Increasing the concentration of OH¯ (B) Adding 6 M HNO3 (C) Increasing the mass of HgO present (D) Increasing the temperature (E) Adding a catalyst

Assume that you have an "unknown" consisting of an aqueous solution of a salt that contains one of the ions listed above. Which ions must be absent on the basis of each of the following observations of the "unknown"? 10. The solution is colorless (A) CO32¯ (B) Cr2O72¯ (C) NH4+ (D) Ba2+ (E) Al3+

Look at the Phase Diagram for 5-7 (A) Sublimation (B) Condensation (C) Solvation (D) Fusion (E) Freezing 6. If the temperature decreases from 110° C to 40° C at a constant pressure of 1.1 atmospheres, which of the processes occurs?

Look at the Phase Diagram for 5-7 (A) Sublimation (B) Condensation (C) Solvation (D) Fusion (E) Freezing 7. If the pressure increases from 0.5 to 1.5 atmospheres at a constant temperature of 50° C, which of the processes occurs?

7. Has amphoteric properties (A) Hydrofluoric acid (B) Carbon dioxide (C) Aluminum hydroxide (D) Ammonia (E) Hydrogen peroxide

Questions 1-4 (A) Heisenberg uncertainty principle (B) Pauli exclusion principle (C) Hund's rule (principle of maximum multiplicity) (D) Shielding effect (E) Wave nature of matter 1. Can be used to predict that a gaseous carbon atom in its ground state is paramagnetic

(A) hydrogen bonding (B) hybridization (C) ionic bonding (D) resonance (E) van der Waals forces (London dispersion forces) 14. Is used to explain the fact that the carbon-to-carbon bonds in benzene, C6H6, are identical

*SEE DIAGRAM ON TEST 77. Which of the following compounds exhibits optical isomerism? (A) (B) (C) (D) (E)

*SEE DIAGRAM ON TEST The spontaneous reaction that occurs when the cell above operates is: 2Ag+ + Cd(s) ---> 2 Ag(s) + Cd2+ (A) Voltage increases. (B) Voltage decreases but remains at zero. (C) Voltage becomes zero and remains at zero. (D) No change in voltage occures. (E) Direction of voltage change cannot be predicted without additional information. Which of the above occurs for each of the following circumstances? 15. The silver electrode is made larger.

*USE THE PHASE DIAGRAM FROM THE TEST 51. For the substance represented in the diagram, which of the phases is most dense and which is least dense at - 15 °C. Most Dense Least Dense (A) Solid Gas (B) Solid Liquid (C) Liquid Solid (D) Liquid Gas (E) The diagram gives no information about densities.

15. Carbon dioxide, CO2(s) (A) Lattice of positive and negative ions held together by electrostatic forces. (B) Closely packed lattice with delocalized electrons throughout (C) Strong single covalent bonds with weak intermolecular forces. (D) Strong multiple covalent bonds (including bonds.) with weak intermolecular forces (E) Macromolecules held tgether with strong polar bonds.

17. Relatively slow rates of chemical reaction are associated with which of the following? (A) The presence of a catalyst (B) High temperature (C) High concentration of reactants (D) Strong bonds in reactant molecules (E) Low activation energy

19. Which of the following represents a pair of isotopes? Atomic Number Mass Number (A) I. 6 14 II. 7 14 (B) I. 6 7 II. 14 14 (C) I. 6 14 II. 14 28 (D) I. 7 13 II. 7 14 (E) I. 8 16 II. 16 20

24. The safest and most effective emergency procedure to treat an acid splash on skin is to do which of the following immediately? (A) Dry the affected area with paper towels (B) Sprinkle the affected area with powdered Na2SO4(s) (C) Flush the affected area with water and then with a dilute NaOH solution (D) Flush the affected area with water and then with a dilute NaHCO3 solution (E) Flush the affected area with water and then with a dilute vinegar solution

25. H2(g) + (1/2) O2(g) ---> H2O(l) DH° = - 286 kJ 2 Na(s) + (1/2) O2(g) ---> Na2O(s) DH° = - 414 kJ Na(s) + (1/2) O2(g) + (1/2) H2(g) ---> NaOH(s) DH° = - 425 kJ Based on the information above, what is the standard enthalpy change for the following reaction? Na2O(s) + H2O(l) ---> 2 NaOH(s) (A) -1,125 kJ (B) -978 kJ (C) -722 kJ (D) -150 kJ (E) +275 kJ

75. If a copper sample containing some zinc impurity is to be purified by electrolysis, the anode and the cathode must be which of the following? Anode Cathode (A) Pure copper Pure zinc (B) Pure zinc Pure copper (C) Pure copper Impure copper sample (D) Impure copper sample Pure copper (E) Impure copper sample Pure zinc

75. Which of the following pairs of liquids forms the solution that is most ideal (most closely follows Raoult's law)? A) C8H18(l) and H2O(l) B) CH3CH2CH2OH(l) and H2O(l) C) CH3CH2CH2OH(l) and C8H18(l) D) C6H14(l) and C8H18(l) E) H2SO4(l) and H2O(l)

8-10 Refer to the following diatomic species (A) Li2 (B) B2 (C) N2 (D) O2 (E) F2 9. Has a bond order of 2

81. What is the net ionic equation for the reaction that occurs when aqueous copper(II) sulfate is added to excess 6-molar ammonia? (A) Cu2+ + SO42¯ + 2 NH4+ + 2 OH¯ ---> (NH4)2SO4 + Cu(OH)2 (B) Cu2+ + 4 NH3 + 4 H2O --> Cu(OH)42¯ + 4 NH4+ (C) Cu2+ + 2 NH3 + 2 H2O --> Cu(OH)2 + 2 NH4+ (D) Cu2+ + 4 NH3 --> Cu(NH3)42+ (E) Cu2+ + 2 NH3 + H2O --> CuO + 2 NH4+

Look at Diagram for 30 30. The energy diagram for the reaction X + Y ---> Z is shown above. The addition of a catalyst to this reaction would cause a change in which of the indicated energy differences? (A) I only (B) II only (C) III only (D) I and II only (E) I, II, and III

50. Which of the following acids can be oxidized to form a stronger acid? (A) H3PO4 (B) HNO3 (C) H2CO3 (D) H3BO3 (E) H2SO3

51. Pi bonding occurs in each of the following species EXCEPT (A) CO2 (B) C2H4 (C) CN¯ (D) C6H6 (E) CH4

51. Which of the following is a correct interpretation of the results of Rutherford's experiments in which gold atoms were bombarded with alpha particles? (A) Atoms have equal numbers of positive and negative charges. (B) Electrons in atoms are agganged in shells. (C) Neutrons are at the center of an atom. (D) Neutrons and protrons in atoms have nearly equal mass. (E) The positive charge of an atom is concentrated in a small region.

52. The test for the presence of Ag+ in an unknown solution involves the treatment of the solver-ammonia complex with dilute hydrochloric acid. The appearance of a white precipitate at this point indicates the presence of silver ion in the original sample. The net ionic equation that represents this test is (A) Ag(NH4)4+ + 4 H+ <===> Ag(s) + 4 NH4+ (B) Ag(NH4)4+ + Cl¯ <===> AgCl(s) + 4 NH4+ (C) Ag(NH3)4+ + 4 HCl <===> AgCl(s) + 4 NH4+ + 3 Cl#175; (D) Ag(NH3)4+ + Cl¯ <===> Ag(NH3)2Cl(s) (E) Ag(NH3)4+ + 2 H+ + Cl#175; <===> AgCl(s) + 2 NH4+

60. Which of the following has a zero dipole moment? (A) HCN (B) NH3 (C) SO2 (D) NO2 (E) PF5

8. Represents an atom of a transition metal. - Answer Choices on Picture

(A) Activation energy (B) Free energy (C) Ionization energy (D) Kinetic energy (E) Lattice energy 2. The energy change that occurs in the conversion of an ionic solid to widely separated gaseous ions

E (Lattice Energy)

H2(g) + Br2(g) <=> 2 HBr(g) 42. At a certain temperature, the value of the equilibrium constant, K, for the reaction represented above is 2.0105. What is the value of K for the reverse reaction at the same temperature? (A) -2.0 x 10-5 (B) 5.0 x 10-6 (C) 2.0 x 10-5 (D) 5.0 x 10-5 (E) 5.0 x 10-4

HCO3-(aq) + OH-(aq) <=> H2O(l) + CO32-(aq) ΔH = -41.4 kJ 37. When the reaction represented by the equation above is at equilibrium at 1 atm and 25˚C, the ratio [(CO3)2-] [HCO3-] can be increased by doing which of the following? (A) Decreasing the temperature (B) Adding acid (C) Adding a catalyst (D) diluting the solution with distilled water (E) Bubbling neon gas through the solution

Look at Graph 18. The phase diagram for the pure substance X is shown above. The temperature of a sample of pure solid X is slowly raised from 10˚C to 100˚C at a constant pressure of 0.5 atm. What is the expected behavior of the substance? (A) It first melts to a liquid and then boils at about 70˚C. (B) It first melts to a liquid and then boils at about 30˚C. (C) It melts to a liquid at a temperature of about 20˚C and remains a liquid until the temperature is greater than 100˚C. (D) It sublimes to vapor at an equilibrium temperature of about 20˚ C. (E) It remains a solid until the temperature is greater than 100˚C.

Look at Graph 68. Liquid naphthalene at 95˚C was cooled to 30˚C as represented in the cooling curve above. From which section of the curve can the melting point of naphthalene be determined? (A) A (B) B (C) C (D) D (E) E

Look at Graph Questions 15-16 relate to the graph below. The graph shows the temperature of a pure substance as it is heated at a constant rate in an open vessel at 1.0 atm pressure. The substance changes from the solid to the liquid to the gas phase. 15. The substance is at its normal freezing point at time (A) t1 (B) t2 (C) t3 (D) t4 (E) t5

Look at Graph Questions 15-16 relate to the graph below. The graph shows the temperature of a pure substance as it is heated at a constant rate in an open vessel at 1.0 atm pressure. The substance changes from the solid to the liquid to the gas phase. 16. Which of the following best describes what happens to the substance between t4 and t5? (A) The molecules are leaving the liquid phase. (B) The solid and liquid phases coexist in equilibrium. (C) The vapor pressure of the substance is decreasing. (D) The average intermolecular distance is decreasing. (E) The temperature of the substance is increasing.

Look at Question (B)

Look at Question 62

Look at Table 55. A reaction was observed for 20 days and the percentage of the reactant remaining after each day was recorded in the table above. Which of the following best describes the order and the half-life of the reaction? Rxn Order Half-life (days) (A) First 3 (B) First 10 (C) Second 3 (D) Second 6 (E) Second 10

Look at graph 39. On the basis of the solubility curves shown above, the greatest percentage of which compound can be recovered by cooling a saturated solution of that compound from 90˚C to 30˚C? (A) NaCl (B) KNO3 (C) K2CrO4 (D) K2SO4 (E) Ce2(SO4)3

17. In which of the following groups are the three species isoelectronic; i.e., have the same number of electrons? (A) S2-, K+, Ca2+ (B) Sc, Ti, V2+ (C) O2-, S2-, Cl- (D) Mg2+, Ca2+, Sr2+ (E) Cs, Ba2+, La3+

19. In which of the following species does sulfur have the same oxidation number as it does in H2SO4? (A) H2SO3 (B) (S2O3)2- (C) (S)2- (D) S8 (E) SO2Cl2

2 H2O(l) + 4 MnO4-(aq) + 3 (ClO2)-(aq) => 4MnO2(s) + 3 (ClO4)-(aq) + 4 OH-(aq) 60. According to the balanced equation above, how many moles of (ClO)2-(aq) are needed to react completely with 20. mL of 0.20 M KMnO4 solution? (A) 0.0030 mol (B) 0.0053 mol (C) 0.0075 mol (D) 0.013 mol (E) 0.030 mol

2 N2H4(g) + N2O4(g) => 3 N2(g) + 4 H2O(g) 58. When 8.0 g of N2H4 (32 g mol-1) and 92 g of N2O4 (92 g mol-1) are mixed together and react according to the equation above, what is the maximum mass of H2O that can be produced? (A) 9.0 g (B) 18 g (C) 36 g (D) 72 g (E) 144 g

2 NH3 <=> (NH4)+ + NH2- 22. In liquid ammonia, the reaction represented above occurs. In the reaction NH4 + acts as (A) a catalyst (B) both an acid and a base (C) the conjugate acid of NH3 (D) the reducing agent (E) the oxidizing agent

24. A compound contains 1.10 mol of K, 0.55 mol of Te, and 1.65 mol of 0. What is the simplest formula of this compound? (A) KTeO (B) KTe2O (C) K2TeO3 (D) K2TeO6 (E) K4TeO6

27. A possible mechanism for the overall reaction represented above is the following. (1) NO(g) + NO(g) => N2O2(g) slow (2) N2O2(g) + O2(g) => 2 NO2(g) fast Which of the following rate expressions agrees best with this possible mechanism? (A) Rate = k[NO]2 (B) Rate = k[NO] [O2] (C) Rate = k[NO]2 [O2] (D) Rate = k[NO]2[O2] (E) Rate = k[N2O2][O2]

28. Of the following compounds, which is the most ionic? (A) SiCl4 (B) BrCl (C) PCl3 (D) Cl2O (E) CaCl2

29. The best explanation for the fact that diamond is extremely hard is that diamond crystals (A) are made up of atoms that are intrinsically hard because of their electronic structures (B) consist of positive and negative ions that are strongly attracted to each other (C) are giant molecules in which each atom forms strong covalent bonds with all of its neighboring atoms (D) are formed under extreme conditions of temperature and pressure (E) contain orbitals or bands of delocalized electrons that belong not to single atoms but to each crystal as a whole

3 Cu(s) + 8 H+(aq) + 2 NO3-(aq) =>3 Cu2+(aq) + 2 NO(g) + 4 H2O(l) 51. True statements about the reaction represented above include which of the following? I. Cu(s) acts as an oxidizing agent. II. The oxidation state of nitrogen changes from +5 to +2. III. Hydrogen ions are oxidized to form H2O(l). (A) I only (B) II only (C) III only (D) I and II (E) II and III

30. At 25˚C aqueous solutions with a pH of 8 have a hydroxide ion concentration, [OH-], of (A) 1 x 10-14 M (B) 1 x 10-8 M (C) 1 x 10-6 M (D) 1 M (E) 8 M

32. Which of the following oxides is a gas at 25˚C and 1 atm? (A) Rb2O (B) N2O (C) Na2O2 (D) SiO2 (E) La2O3

35. A solution is made by dissolving a nonvolatile solute in a pure solvent. Compared to the pure solvent, the solution (A) has a higher normal boiling point ' (B) has a higher vapor pressure (C) has the same vapor pressure (D) has a higher freezing point (E) is more nearly ideal

36. A sample of a solution of an unknown was treated with dilute hydrochloric acid. The white precipitate formed was filtered and washed with hot water. A few drops of potassium iodide solution were added to the hot water filtrate and a bright yellow precipitate was produced. The white precipitate remaining on the filter paper was readily soluble in ammonia solution. What two ions could have been present in the unknown? (A) Ag+(aq) and (Hg2)2+(aq) (B) Ag+(aq) and (Pb)2+(aq) (C) (Ba)2+(aq) and Ag+(aq) (D) (Ba)2+(aq) and (Hg2)2+(aq) (E) (Ba)2+(aq) and (Pb)2+(aq)

38. A 0.10 M aqueous solution of sodium sulfate, Na2SO4, is a better conductor of electricity than 0.10 M aqueous solution of sodium chloride, NaCl. Which of the following best explains this observation? (A) Na2SO4 is more soluble water than NaCl is. (B) Na2SO4 has a higher molar mass than NaCl has. (C) To prepare a given volume of 0.10 M solution, the mass of Na2SO4 needed is more than twice the mass of NaCl needed. (D) More moles of ions are present in a given volume of 0.10 M Na2SO4 than in the same volume of 0.10 M NaCl. (E) The degree of dissociation of Na2SO4 in solution is significantly greater than that of NaCl.

4. The molecule with the largest dipole moment (A) CO2 (B) H20 (C) CH4 (D) C2H4 (E) PH3

41. When solid NH4SCN is mixed with solid Ba(OH)2 in a closed container, the temperature drops and a gas is produced. Which of the following indicates the correct signs for ΔG, ΔH, and ΔS for the process? ΔG ΔH ΔS (A) — — (B) — + — (C) — + + (D) + — + (E) + — —

43. The atomic mass of copper is 63.55. Given that there are only two naturally occurring isotopes of copper, 63Cu and 65Cu, the natural abundance of the 65Cu isotope must be approximately (A) 90% (B) 70% (C) 50% (D) 25% (E) 10%

44. Which of the following properties generally decreases across the periodic table from sodium to chlorine? (A) First ionization energy (B) Atomic mass (C) Electronegativity (D) Maximum value of oxidation number (E) Atomic radius

45. What is the mole fraction of ethanol, C2H5OH, in an aqueous solution that is 46 percent ethanol by mass? (The molar mass of C2H5OH is 46 g; the molar mass of H2O is 18 g.) (A) 0.25 (B) 0.46 (C) 0.54 (D) 0.67 (E) 0.75

46. The effective nuclear charge experienced by the outermost electron of Na is different than the effective nuclear charge experienced by the outermost electron of Ne. This difference best accounts for which of the following? (A) Na has a greater density at standard conditions than Ne. (B) Na has a lower first ionization energy than Ne. (C) Na has a higher melting point than Ne. (D) Na has a higher neutron-to-proton ratio than Ne. (E) Na has fewer naturally occurring isotopes than Ne.

47. Which of the following is a correct statement about reaction order? (A) Reaction order can only be a whole number. (B) Reaction order can be determined only from the coefficients of the balanced equation for the reaction. (C) Reaction order can be determined only by experiment. (D) Reaction order increases with increasing temperature. (E) A second-order reaction must involve at least two different compounds as reactants.

48. Sodium chloride is LEAST soluble in which of the following liquids? (A) H2O (B) CCl4 (C) HF (D) CH3OH (E) CH3COOH

5. The molecule that has trigonal pyramidal geometry (A) CO2 (B) H20 (C) CH4 (D) C2H4 (E) PH3

50. Which of the following represents acceptable laboratory practice? (A) Placing a hot object on a balance pan (B) Using distilled water for the final rinse of a buret before filling it with standardized solution (C) Adding a weighed quantity of solid acid to a titration flask wet with distilled water (D) Using 10 mL of standard strength phenolphthalein indicator solution for titration of 25 mL of acid solution (E) Diluting a solution in a volumetric flask to its final concentration with hot water

52. Propane gas, C3H8, burns in excess oxygen gas. When the equation for this reaction is correctly balanced and all coefficients are reduced to their lowest whole-number terms, the coefficient for O2 is (A) 4 (B) 5 (C) 7 (D) 10 (E) 22

53. According to the VSEPR model, the progressive decrease in the bond angles in the series of molecules CH4, NH3, and H2O is best accounted for by the (A) increasing strength of the bonds (B) decreasing size of the central atom (C) increasing electronegativity of the central atom (D) increasing number of unshared pairs of electrons (E) decreasing repulsion between hydrogen atoms

54. Which of the following must be true for a reaction for which the activation energy is the same for both the forward and the reverse reactions? (A) A catalyst is present. (B) The reaction order can be obtained directly from the balanced equation. (C) The reaction order is zero. (D) ΔH for the reaction is zero. (E) ΔS for the reaction is zero.

56. The boiling points of the elements helium, neon, argon, krypton, and xenon increase in that order. Which of the following statements accounts for this increase? (A) The London (dispersion) forces increase. (B) The hydrogen bonding increases. (C) The dipole-dipole forces increase. (D) The chemical reactivity increases. (E) The number of nearest neighbors increases.

61. How can 100. mL of sodium hydroxide solution with a pH of 13.00 be converted to a sodium hydroxide solution with a pH of 12.00? (A) By diluting the solution with distilled water to a total volume of 108 mL (B) By diluting the solution with distilled water to a total volume of 200 mL (C) By diluting the solution with distilled water to a total volume of 1.00 L (D) By adding 100. mL of 0.10 M HCl (E) By adding 100. mL of 0.10 M NaOH

63. Mixtures that would be considered buffers include which of the following? I. 0.10 M HCl + 0.10 M NaCl II. 0.10 M HF + 0.10 M NaF III. 0.10 M HBr + 0.10 M NaBr (A) I only (B) II only (C) III only (D) I and II (E) II and III

64. Ascorbic acid, H2C6H6O6(s), is a diprotic acid with K1 = 7.9x10^-5 and K2 = 1.6x10^-12. In a 0.005 M aqueous solution of ascorbic acid, which of the following species is present in the lowest concentration? (A) H2O(l) (B) H3O+(aq) (C) H2C6H6O6(aq) (D) HC6H6O6-(aq) (E) (C6H6O6)2-(aq)

65. Which of the following substances is LEAST soluble in water? (A) (NH4)2SO4 (B) KMnO4 (C) BaCO3 (D) Zn(NO3)2 (E) Na3PO4

66. A 2 L container will hold about 4 g of which of the following gases at 0˚C and 1 atm? (A) SO2 (B) N2 (C) CO2 (D) C4H8 (E) NH3

67. Which of the following describes the changes in forces of attraction that occur as H2O changes phase from a liquid to a vapor? (A) H—O bonds break as H—H and O—O bonds form. (B) Hydrogen bonds between H2O molecules are broken. (C) Covalent bonds between H2O molecules are broken. (D) Ionic bonds between H+ ions and OH- ions are broken. (E) Covalent bonds between H+ ions and H2O molecules become more effective.

69. If 200. mL of 0.60 M MgCl2(aq) is added to 400. mL of distilled water, what is the concentration of Mg2+(aq) in the resulting solution? (Assume volumes are additive.) (A) 0.20 M (B) 0.30 M (C) 0.40 M (D) 0.60 M (E) 1.2 M

70. Of the following pure substances, which has the highest melting point? (A) S8 (B) I2 (C) SiO2 (D) SO2 (E) C6H6

71. In the electroplating of nickel, 0.200 faraday of electrical charge is passed through a solution of NiSO4. What mass of nickel is deposited? (A) 2.94 g (B) 5.87 g (C) 11.7 g (D) 58.7 g (E) 294 g

72. A colorless solution is divided into three samples. The following tests were performed on samples of the solution. Sample Test Observation 1 Add H+(aq) No change 2 Add NH3(aq) No change 3 Add (SO4)2-(aq) No change Which of the following ions could be present in the solution at a concentration of 0.10 M? (A) Ni2+(aq) (B) Al3+(aq) (C) Ba2+(aq) (D) Na+(aq) (E) CO3 2-(aq)

73. Which of the following is true for any substance undergoing the process represented above at its normal melting point? (A) ΔS < 0 (B) ΔH = 0 (C) ΔH = TΔG (D) TΔS = 0 (E) ΔH = TΔS

74. A pure, white crystalline solid dissolves in water to yield a basic solution that liberates a gas when excess acid is added to it. On the basis of this information, the solid could be (A) KNO3 (B) K2CO3 (C) KOH (D) KHSO4 (E) KCl

75. In a saturated solution of Zn(OH)2 at 25˚C the value of [OH-] is 2.0x10^-6 M. What is the value of thesolubility-product constant, Ksp, for Zn(OH)2 at 25˚C? (A) 4.0x10^-18 (B) 8.0x10^-18 (C) 1.6x10^-17 (D) 4.0x10^-12 (E) 2.0x10^-6

(A) NH3 and NH4Cl (B) H3PO4 and NaH2PO4 (C) HCl and NaCl (D) NaOH and NH3 (E) NH3 and HC2H3O2 (acetic acid) 11. A buffer at a pH > 8

(A) O (B) La (C) Rb (D) Mg (E) N 1. What is the most electronegative element of the above?

(A) a solution with a pH less than 7 that is not a buffer solution (B) a buffer solution with a pH between 4 and 7 (C) a buffer solution with a pH between 7 and 10 (D) a solution with a pH greater than 7 that is not a buffer solution (E) a solution with a pH of 7 Ionization Constants CH3COOH = 1.8 x 10¯5 NH3 = 1.8 x 10¯5 H2CO3; K1 = 4 x 10¯7 H2CO3; K2 = 4 x 10¯11 8. A solution prepared to be initially 1 M in NaCl and 1 M in HCl.

*USE GRAPHS FROM TEST FOR Q48 48.Which of the following is a graph that describes the pathway of reaction that is endothermic and has high activation energy? (A) (B) (C) (D) (E)

13. Cesium chloride, CsCl (s) (A) Lattice of positive and negative ions held together by electrostatic forces. (B) Closely packed lattice with delocalized electrons throughout (C) Strong single covalent bonds with weak intermolecular forces. (D) Strong multiple covalent bonds (including bonds.) with weak intermolecular forces (E) Macromolecules held tgether with strong polar bonds.

21. Which of the following is true at the triple point of a pure substance? (A) The vapor pressure of the solid phase always equal the vapor pressure of the liquid phase. (B) The temperature is always 0.01 K lower that the normal melting point. (C) The liquid and gas phases of the substance always have the same density and are therefore indistinguishable. (D) the solid phase always melts if the pressure increases at constant temperature. (E) The liquid phase always vaporizes if the pressure increases at constant temperature.

27. Appropriate uses of a visible-light spectrophtometer include which of the following? I. Determining the concentration of a solution of Cu(NO3)2 II. Measuring the conductivity of a solution of KMnO4 III. Determining which ions are present in a solution that may contain Na+, Mg2+, Al3+ (A) I only (B) II only (C) III only (D) I and II only (E) I and III only

29. Cu(s) + 2 Ag+ ---> Cu2+ + 2 Ag(s) If the equilibrium constant for the reaction above is 3.7 x 1015, which of the following correctly describes the standard voltage, E°, and the standard free energy change, DG°, for this reaction? (A) E° is positive and DG° is negative. (B) E° is negative and DG° is positive. (C) E° and DG° are both positive. (D) E° and DG° are both negative. (E) E° and DG° are both zero

29. When an aqueous solution of NaOH is added to an aqueous solution of potassium dichromate, K2Cr2O7 the dichromate ion is converted to (A) CrO42¯ (B) CrO2 (C) Cr3+ (D) Cr2O3(s) (E) Cr(OH)3(s)

31. The structural isomers C2H5OH and CH3OCH3 would be expected to have the same values for which of the following? (Assume ideal behavior.) (A) Gaseous densities at the same temperature and pressure (B) Vapor pressures at the same temperature (C) Boiling points (D) Melting points (E) Heats of vaporization

32. The net ionic equation for the reaction between silver carbonate and hydrochloric acid is (A) Ag2CO3(s) + 2 H+ + 2 Cl¯ ---> 2 AgCl(s) + H2O + CO(g) (B) 2 Ag+ + CO32¯ + 2 H+ + 2 Cl¯ ---> 2 AgCl(s) + H2O + CO2(g) (C) CO32¯ + 2 H+ ---> H2O + CO2(g) (D) Ag+ + Cl¯ ---> AgCl(s) (E) Ag2CO3(s) + 2 H+ ---> 2Ag+ + H2CO3

33. Which of the following conclusions can be drawn from J. J. Thomson's cathode ray experiments? (A) Atoms contain electrons. (B) Practically all the mass of an atom is contained in its nucleus. (C) Atoms contain protons, neutrons, and electrons. (D) Atoms have a positively charged nucleus surrounded by an electron cloud. (E) No two electrons in one atom can have the same four quantum numbers.

38. The radioactive decay of 6-C-14 to 7-N-14 occurs by the process of (A) beta particle emission (B) alpha particle emission (C) positron emission (D) electron capture (E) neutron capture

40. The geometry of the SO3 molecule is best described as (A) trigonal planar (B) trigonal pyramidal (C) square pyramidal (D) bent (E) tetrahedral

41. Which of the following molecules has the shortest bond length? (A) N2 (B) O2 (C) Cl2 (D) Br2 (E) I2

43. Which of the following does NOT behave as an electrolyte when it is dissolved in water? (A) CH3OH (B) K2CO3 (C) NH4Br (D) HI (E) Sodium acetate, CH3COONa

45. The alkenes are compounds of carbon and hydrogen with the general formula CnH2n. If 0.561 gram of any alkene is burned in excess oxygen, what number of moles of H2O is formed? (A) 0.0400 mole (B) 0.0600 mole (C) 0.0800 mole (D) 0.400 mole (E) 0.800 mole

48. PCl3(g) + Cl2(g) <===> PCl5(g) + energy Some PCl3 and Cl2 are mixed in a container at 200 °C and the system reaches equilibrium according to the equation above. Which of the following causes an increase in the number of moles of PCl5 present at equilibrium? I. Decreasing the volume of the container II. Raising the temperature III. Adding a mole of He gas at constant volume (A) I only (B) II only (C) I and III only (D) II and III only (E) I, II, and III

5. Is used to etch glass chemically (A) Hydrofluoric acid (B) Carbon dioxide (C) Aluminum hydroxide (D) Ammonia (E) Hydrogen peroxide

52. 3 Ag(s) + 4 HNO3 <===> 3 AgNO3 + NO(g) + 2 H2O The reaction of silver metal and dilute nitric acid proceeds according to the equation above. If 0.10 mole of powdered silver is added to 10. milliliters of 6.0-molar nitric acid, the number of moles of NO gas that can be formed is (A) 0.015 mole (B) 0.020 mole (C) 0.030 mole (D) 0.045 mole (E) 0.090 mole

54. Which of the following statements is always true about the phase diagram of any one-component system? (A) The slope of the curve representing equilibrium between the vapor and liquid phases is positive. (B) The slope of the curve representing equilibrium between the liquid and solid phases is negative. (C) The slope of the curve representing equilibrium between the liquid and solid phases is positive. (D) the temperature at the triple point is greater than the normal freezing point. (E) The pressure at the triple point is greater than 1 atmosphere.

55. H2PO4¯ + HBO32¯ <===> HPO42¯ + H2BO3¯ The equilibrium constant for the reaction represented by the equation above is greater than 1.0. Which of the following gives the correct relative strengths of the acids and bases in the reaction? Acids Bases (A) H2PO4¯ > H2BO3¯ and HBO32¯ > HPO42¯ (B) H2BO3¯ > H2PO4¯ and HBO32¯ > HPO42¯ (C) H2PO4¯ > H2BO3¯ and HPO42¯ > HBO32¯ (D) H2BO3¯ > H2PO4¯ and HPO42¯ > HBO32¯ (E) H2PO4¯ = H2BO3¯ and HPO42¯ = HBO32¯

58. Which of the following represents the ground state electron configuration for the Mn3+ ion? (Atomic number Mn = 25) (A) 1s2 2s22p6 3s23p63d4 (B) 1s2 2s22p6 3s23p63d5 4s2 (C) 1s2 2s22p6 3s23p63d2 4s2 (D) 1s2 2s22p6 3s23p63d8 4s2 (E) 1s2 2s22p6 3s23p63d3 4s1

6. Represents an atom in an excited state - Answers Choices on Picture

62. The electron-dot structure (Lewis structure) for which of the following molecules would have two unshared pairs of electrons on the central atom? (A) H2S (B) NH3 (C) CH4 (D) HCN (E) CO2

64. Equal numbers of moles of He(g), Ar(g), and Ne(g) are placed in a glass vessel at room temperature. If the vessel has a pinhole-sized leak, which of the following will be true regarding the relative values of the partial pressures of the gases remaining in the vessel after some of the gas mixture has effused? A) PHe < PNe < PAr B) PHe < PAr < PNe C) PNe < PAr < PHe D) PAr < PHe < PNe E) PHe = PAr = PNe

65. Barium sulfate is LEAST soluble in a 0.01-molar solution of which of the following? (A) Al2(SO4)3 (B) (NH4)2SO4 (C) Na2SO4 (D) NH3 (E) BaCl2

65. Which of the following compounds is NOT appreciably soluble in water but is soluble in dilute hydrochloric acid? A) Mg(OH)2(s) B) (NH4)2CO3(s) C) CuSO4(s) D) (NH4)2SO4(s) E) Sr(NO3)2(s)

66. When solid ammonium chloride, NH4Cl(s) is added to water at 25 °C, it dissolves and the temperature of the solution decreases. Which of the following is true for the values of H and DS for the dissolving process? DH DS A) Postive Positive B) Positive Negative C) Positive Equal to zero D) Negative Positive E) Negative Negative (the dH means change in H (the triangle sign))

68. Which of the following molecules has a dipole moment of zero? (A) C6H6 (benzene) (B) NO (C) SO2 (D) NH3 (E) H2S

69. A white solid is observed to be insoluble in water, insoluble in excess ammonia solution, and soluble in dilute HCl. Which of the following compounds could the solid be? (A) CaCO3 (B) BaSO4 (C) Pb(NO3)2 (D) AgCl (E) Zn(OH)2

70. To determine the molar mass of a solid mono protic acid, a student titrated a weighed sample of the acid with standardized aqueous NaOH. Which of the following could explain why the student obtained a molar mass that was too large? I. Failure to rinse all acid from the weighing paper into the titration vessel II. Addition of more water than was needed to dissolve the acid III. Addition of some base beyond the equivalence point (A) I only (B) III only (C) I and II only (D) II and III only (E) I, II, and III

70. When 100 mL of 1.0 M Na3PO4 is mixed with 100 mL of 1.0 M AgNO3, a yellow precipitate forms and [Ag+] becomes negligibly small. Which of the following is a correct listing of the ions remaining in solution in order of increasing concentration? A) [PO43¯] < [NO3¯] < [Na+] B) [PO43¯] < [Na+] < [NO3¯] C) [NO3¯] < [PO43¯] < [Na+] D) [Na+] < [NO3¯] < [PO43¯] E) [Na+] < [PO43¯] < [NO3¯]

72. How many moles of solid Ba(NO3)2 should be added to 300. milliliters of 0.20-molar Fe(NO3)3 to increase the concentration of the NO3¯ ion to 1.0-molar? (Assume that the volume of the solution remains constant.) (A) 0.060 mole (B) 0.12 mole (C) 0.24 mole (D) 0.30 mole (E) 0.40 mole

73. 2 SO2(g) + O2(g) <===> 2 SO3(g) When 0.40 mole of SO2 and 0.60 mole of O2 are placed in an evacuated 1.00-liter flask, the reaction represented above occurs. After the reactants and the product reach equilibrium and the initial temperature is restored, the flask is found to contain 0.30 mole of SO3. Based on these results, the equilibrium constant, Kc for the reaction is (A) 20. (B) 10. (C) 6.7 (D) 2.0 (E) 1.2

73. Adding water to some chemicals can be dangerous because large amounts of heat are liberated. Which of the following does NOT liberate heat when water is added to it? (A) KNO3 (B) NaOH (C) CaO (D) H2SO4 (E) Na

74. A solution of calcium hypochlorite, a common additive to swimming-pool water, is (A) basic because of the hydrolysis of the OCl¯ ion (B) basic because Ca(OH)2 is a weak and insoluble base (C) neutral if the concentration is kept below 0.1 molar (D) acidic because of the hydrolysis of the Ca2+ ions (E) acidic because the acid HOCl is formed

74. Which of the following gases deviates most from ideal behavior? A) SO2 B) Ne C) CH4 D) N2 E) H2

78. When the actual gas volume is greater then the volume predicted by the ideal gas law, the explanation lies in the fact that the ideal gas law does NOT include a factor for molecular. (A) volume (B) mass (C) velocity (D) attractions (E) shape

83. NH3(g) + 2 CH4(g) + 5/2 O2(g) <===> H2NCH2COOH(s) + 3 H2O(l) At constant temperature, DeltaH, the change in enthalpy for the reaction above is approximately equal to (A) DeltaE - (11/2)RT (B) DeltaE - (7/2)RT (C) DeltaE + RT (D) DeltaE + (7/2)RT (E) DeltaE (11/2)RT

84. Which of the following aqueous solutions has the highest boiling point? (A) 0.10 M potassium sulfate, K2SO4 (B) 0.10 M hydrochloric acid, HCl (C) 0.10 M ammonium nitrate, NH4NO3 (D) 0.10 M magnesium sulfalte, MgSO4 (E) 0.20 M sucrose, C12H22O11

9. Silicon dioxide, SiO2 (A) A network solid with covalent bonding (B) A molecular solid with zero dipole moment (C) A molecular solid with hydrogen bonding (D) An ionic solid (E) A metallic solid

Assume that you have an "unknown" consisting of an aqueous solution of a salt that contains one of the ions listed above. Which ions must be absent on the basis of each of the following observations of the "unknown"? 11. The solution gives no apparent reaction with dilute hydrochloric acid. (A) CO32¯ (B) Cr2O72¯ (C) NH4+ (D) Ba2+ (E) Al3+

H3AsO4 + 3I¯ + 2 H3O+ ---> H3AsO3 + I3¯ + H2O The oxidation of iodide ions by arsenic acid in acidic aqueous solution occurs according to the stoichiometry shown above. The experimental rate law of the reaction is: Rate = k [H3AsO4] [I¯] [H3O+] 26. According to the rate law for the reaction, an increase in the concentration of hydronium ion has what effect on this reaction? (A) The rate of reaction increases. (B) The rate of reaction decreases. (C) The value of the equilibrium constant increases. (D) The value of the equilibrium constant decreases. (E) Neither the rate nor the value of the equilibrium constant is changed.

HC2H3O2(aq) + CN¯(aq) <===> HCN(aq) + C2H3O2¯(aq) 62. The reaction represented above has an equilibrium constant equal to 3.7 x 104. Which of the following can be concluded from this information? A) CN¯(aq) is a stronger base than C2H3O2¯(aq) B) HCN(aq) is a stronger acid than HC2H3O2(aq) C) The conjugate base of CN¯(aq) is C2H3O2¯(aq) D) The equilibrium constant will increase with an increase in temperature. E) The pH of a solution containing equimolar amounts of CN¯(aq) and HC2H3O2(aq) is 7.0.

Look at the Phase Diagram for 5-7 (A) Sublimation (B) Condensation (C) Solvation (D) Fusion (E) Freezing 5. If the temperature increases from 10° C to 60° C at a constant pressure of 0.4 atmosphere, which of the processes occurs?

M(s) + 3 Ag+(aq) --> 3 Ag(s) + M3+(aq) E = +2.46 V Ag+(aq) + e¯ --> Ag(s) E = +0.80 V 57. According to the information above, what is the standard reduction potential for the half-reaction M3+(aq) + 3 e¯ --> M(s)? A) -1.66 V B) -0.06 V C) 0.06 V D) 1.66 V E) 3.26 V

NH4NO3(s) --> N2O(g) + 2 H2O(g) 60. A 0.03 mol sample of NH4NO3(s) is placed in a 1 L evacuated flask, which is then sealed and heated. The NH4NO3(s) decomposes completely according to the balanced equation above. The total pressure in the flask measured at 400 K is closest to which of the following? ( The value of the gas constant, R, is 0.082 L atm mol¯1 K¯1) (A) 3 atm (B) 1 atm (C) 0.5 atm (D) 0.1 atm (E) 0.03 atm

Questions 1-4 (A) Heisenberg uncertainty principle (B) Pauli exclusion principle (C) Hund's rule (principle of maximum multiplicity) (D) Shielding effect (E) Wave nature of matter 4. Predicts that it is impossible to determine simultaneously the exact position and the exact velocity of an electron

Questions 11-13 (A) Pb (B) Ca (C) Zn (D) As (E) Na 13. Utilized as a shield from sources of radiation

Questions 34-35 refer to an electrolytic cell that involves the following half-reaction. AlF63¯ + 3 e¯ ---> Al + 6F¯ 34. Which of the following occurs in the reaction? (A) AlF 63¯ is reduced at the cathode. (B) Al is oxidized at the anode. (C) Aluminum is converted from the -3 oxidation state to the 0 oxidation state. (D) F¯ acts as a reducing agent. (E) F¯ is reduced at the cathode.

W(g) + X(g) --> Y(g) + Z(g) 53. Gases W and X react in a closed, rigid vessel to form gases Y and Z according to the equation above. The initial pressure of W(g) is 1.20 atm and that of X(g) is 1.60 atm. No Y(g) or Z(g) is initially present. The experiment is carried out at constant temperature. What is the partial pressure of Z(g) when the partial pressure of W(g) has decreased to 1.0 atm? A) 0.20 atm B) 0.40 atm C) 1.0 atm D) 1.2 atm E) 1.4 atm

(A) Activation energy (B) Free energy (C) Ionization energy (D) Kinetic energy (E) Lattice energy 4. The energy required to form the transition state in a chemical reaction

A (Activation Energy)

(A) 1s2 2s22p5 3s23p5 (B) 1s2 2s22p6 3s23p6 (C) 1s2 2s22p62d10 3s23p6 (D) 1s2 2s22p6 3s23p63d5 (E) 1s2 2s22p6 3s23p63d3 4s2 6. The ground-state configuration of a negative ion of a halogen

(A) 1s2 2s22p5 3s23p5 (B) 1s2 2s22p6 3s23p6 (C) 1s2 2s22p62d10 3s23p6 (D) 1s2 2s22p6 3s23p63d5 (E) 1s2 2s22p6 3s23p63d3 4s2 7. The ground-state configuration of a common ion of an alkaline earth element

(A) NH3 and NH4Cl (B) H3PO4 and NaH2PO4 (C) HCl and NaCl (D) NaOH and NH3 (E) NH3 and HC2H3O2 (acetic acid) 12. A buffer at a pH < 6

(A) a solution with a pH less than 7 that is not a buffer solution (B) a buffer solution with a pH between 4 and 7 (C) a buffer solution with a pH between 7 and 10 (D) a solution with a pH greater than 7 that is not a buffer solution (E) a solution with a pH of 7 Ionization Constants CH3COOH = 1.8 x 10¯5 NH3 = 1.8 x 10¯5 H2CO3; K1 = 4 x 10¯7 H2CO3; K2 = 4 x 10¯11 10. A solution prepared to be initially 0.5 M in CH3COOH and 1 M in CH3COONa

(A) hydrogen bonding (B) hybridization (C) ionic bonding (D) resonance (E) van der Waals forces (London dispersion forces) 13. Is used to explain the fact that the four bonds in methane are equivalent

*USE THE PHASE DIAGRAM FROM THE TEST 50. The phase diagram above provides sufficient information for determining the (A) entropy change on vaporization (B) conditions necessary for sublimation (C) deviations from ideal gas behavior of the gas phase (D) latent heat of vaporization (E) latent heat of fusion

14. Gold, Au(s) (A) Lattice of positive and negative ions held together by electrostatic forces. (B) Closely packed lattice with delocalized electrons throughout (C) Strong single covalent bonds with weak intermolecular forces. (D) Strong multiple covalent bonds (including bonds.) with weak intermolecular forces (E) Macromolecules held tgether with strong polar bonds.

19. In which of the following compounds is the mass ratio of chromium to oxygen closest to 1.62 to 1.00 ? (A) CrO3 (B) CrO2 (C) CrO (D) Cr2O (E) Cr2O3

20. What mass of Au is produced when 0.0500 mol of Au2S3 is reduced completely with excess H2? (A) 9.85 g (B) 19.7 g (C) 24.5 g (D) 39.4 g (E) 48.9 g

21. When a sample of oxygen gas in a closed container of constant volume is heated until its absolute temperature is doubled, which of the following is also doubled? (A) The density of the gas (B) The pressure of the gas (C) The average velocity of the gas molecules (D) The number of molecules per cm3 (E) The potential energy of the molecules

21. When a solution of sodium chloride is vaporized in a flame, the color of the flame is (A) blue (B) yellow (C) green (D) violet (E) White

24. The mass of element Q found in 1.00 mole of each of four different compounds is 38.0 grams, 57.0 grams, 76.0 grams, and 114 grams, respectively. A possible atomic weight of Q is (A) 12.7 (B) 19.0 (C) 27.5 (D) 38.0 (E) 57.0

28. The melting point of MgO is higher than that of NaF. Explanations for this observation include which of the following? I. Mg2+ is more positively charged than Na+ II. O2¯ is more negatively charged than F¯ III. The O2¯ ion is smaller than the F¯ ion (A) II only (B) I and II only (C) I and III only (D) II and III only (E) I, II, and III

2NO(g) + O2(g) <===> 2 NO2(g) H < 0 54. Which of the following changes alone would cause a decrease in the value of Keq for the reaction represented above? A) Decreasing the temperature B) Increasing the temperature C) Decreasing the volume of the reaction vessel D) Increasing the volume of the reaction vessel E) Adding a catalyst

3. Forms oxides that are common air pollutants and that yield acidic solution in water (A) F (B) S (C) Mg (D) Ar (E) Mn

30. Hydrogen gas is collected over water at 24 °C. The total pressure of the sample is 755 millimeters of mercury. At 24 °C, the vapor pressure of water is 22 millimeters of mercury. What is the partial pressure of the hydrogen gas? (A) 22 mm Hg (B) 733 mm Hg (C) 755 mm Hg (D) 760 mm Hg (E) 777 mm Hg

35. When phenolphthalein is used as the indicator in a titration of an HCl solution with a solution of NaOH, the indicator undergoes a color change from clear to red at the end point of the titration. This color change occurs abruptly because (A) phenolphthalein is a very strong acid that is capable of rapid dissociation (B) the solution being titrated undergoes a large pH change near the end point of the titration (C) phenolphthalein undergoes an irreversible reaction in basic solution (D) OH¯ acts as a catalyst for the decomposition of phenolphthalein (E) phenolphehalein is involved in the rate-determining step of the reaction between H3O+ and OH¯

38. A molecule or an ion is classified as a Lewis acid if it (A) accepts a proton from water (B) accepts a pair of electrons to form a bond (C) donates a pair of electrons to form a bond (D) donates a proton to water (E) has resonance Lewis electron-dot structures

39. When a hydrate of Na2CO3 is heated until all the water is removed, it loses 54.3 percent of its mass. The formula of the hydrate is (A) Na2CO3 . 10 H2O (B) Na2CO3 . 7 H2O (C) Na2CO3 . 5 H2O (D) Na2CO3 . 3 H2O (E) Na2CO3 . H2O

42. Metallic copper is heated strongly with concentrated sulfuric acid. The products of this reaction are (A) CuSO4(s) and H2(g) only (B) Cu2+, SO2(g), and H2O (C) Cu2+, H2(g), and H2O (D) CuSO4(s), H2(g), and SO2(g) (E) Cu2+, SO3(g), and H2O

46. If 0.060 faraday is passed through an electrolytic cell containing a solution of In3+ ions, the maximum number of moles of In that could be deposited at the cathode is (A) 0.010 mole (B) 0.020 mole (C) 0.030 mole (D) 0.060 mole (E) 0.18 mole

48. If 87.5 percent of a sample of pure 131I decays in 24 days, what is the half-life of 131I? (A) 6 days (B) 8 days (C) 12 days (D) 14 days (E) 21 days

49. The isomerization of cyclopropane to propylene is a first-order process with a half-life of 19 minutes at 500 °C. The time it takes for the partial pressure of cyclopropane to decrease from 1.0 atmosphere to 0.125 atmosphere at 500 °C is closest to (A) 38 minutes (B) 57 minutes (C) 76 minutes (D) 152 minutes (E) 190 minutes

52. Under which of the following sets of conditions could the most O2(g) be dissolved in H2O(l)? Pressure of O2(g) Temperature of H2O Above H2O(l) (atm) °(C) A) 5.0 80 B) 5.0 20 C) 1.0 80 D) 1.0 20 E) 0.5 20

52. When dilute nitric acid was added to a solution of one of the following chemicals, a gas was evolved, This gas turned a drop of limewater, Ca(OH)2, cloudy, due to the formation of a white precipitate. The chemical was (A) household ammonia, NH3 (B) baking soda, NaHCO3 (C) table salt, NaCl (D) epsom salts, MgSO4 . 7H2O (E) bleach, 5% NaOCl

53. Which, if any, of the following species is in the greatest concentration in a 0.100-molar solution of H2SO4 in water? (A) H2SO4 molecules (B) H3O+ ions (C) HSO4¯ ions (D) SO42¯ ions (E) All species are in equilibrium and therefore have the same concentrations.

54. Which of the following is the correct equilibrium expression for the hydrolysis of CO32¯ ? (A) K = [HCO3¯ ] / ( [CO32¯ ] [H3O+] ) (B) K = ( [HCO3¯] [OH¯] ) / [CO32¯] (C) K = ( [CO32¯ ] [OH¯] ) / [HCO3¯] (D) K = [CO32¯ ] / ( [CO2] [OH¯]2 ) (E) K = ( [CO32¯ ] [H3O+] ) / [HCO3¯]

56. It is suggested that SO2 (molar mass 64 grams), which contributes to acid rain, could be removed from a stream of waste gases by bubbling the gases through 0.25-molar KOH, thereby producing K2SO3. What is the maximum mass of SO2 that could be removed by 1,000. liters of the KOH solution? (A) 4.0 kg (B) 8.0 kg (C) 16 kg (D) 20. kg (E) 40. kg

57. For the reaction A(g) <===> B(g) + C(g), the equilibrium constant, Kp, is 2 x 10¯4 at 25 °C. A mixture of the three gases at 25 °C is placed in a reaction flask and the initial pressures are PA = 2 atmosphere, PB = 0.5 atmosphere, and PC = 1 atmosphere, At the instant of mixing, which of the following is true for the reaction as written? (A) DG < 0 (B) DG > 0 (C) DS = 0 (D) DG° = 0 (E) DG° < 0

60. I2(g) + 3 Cl2(g) ---> 2 ICl3(g) According to the data in the table below, what is the value of DH° for the reaction represented above? Bond Average Bond Energy (kilojoules / mole) I---I 149 Cl---Cl 239 I---Cl 208 (A) - 860 kJ (B) - 382 kJ (C) + 180 kJ (D) + 450 kJ (E) + 1,248 kJ

61. A 1-molar solution of which of the following salts has the highest pH ? (A) NaNO3 (B) Na2CO3 (C) NH4Cl (D) NaHSO4 (E) Na2SO4

61. When acidified K2Cr2O7 solution is added to Na2S solution, green Cr3+ ions and free S are formed. When acidified K2Cr2O7 solution is added to NaCl, no change occurs. Of the substances involved in these reactions, which is the best reducing agent? (A) K2Cr2O7 (B) Na2S (C) Cr3+ (D) S (E) NaCl

67. A student wishes to prepare 2.00 liters of 0.100-molar KIO3 (molecular weight 214). The proper procedure is to weigh out (A) 42.8 grams of KIO3 and add 2.00 kilograms of H2O (B) 42.8 grams of KIO3 and add H2O until the final homogeneous solution has a volume of 2.00 liters (C) 21.4 grams of KIO3 and add H2O until the final homogeneous solution has a volume of 2.00 liters (D) 42.8 grams of KIO3 and add 2.00 liters of H2O (E) 21.4 grams fo KIO3 and add 2.00 liters of H2O

67. BrO3¯ + 5 Br¯ + 6 H+ <===> 3 Br2 + 3 H2O If 25.0 milliliters of 0.200-molar BrO3¯ is mixed with 30.0 milliliters of 0.450-molar Br¯ solution that contains a large excess of H+, the amount of Br2 formed, according to the equation above, is (A) 5.00 x 10¯3 mole (B) 8.10 x 10¯3 mole (C) 1.35 x 10¯2 mole (D) 1.50 x 10¯2 mole (E) 1.62 x 10¯2 mole

68. A 20.0-milliliter sample of 0.200-molar K2CO3 solution is added to 30.0 milliliters of 0.400-molar Ba(NO3)2 solution. Barium carbonate precipitates. The concentration of barium ion, Ba2+, in solution after reaction is (A) 0.150 M (B) 0.160 M (C) 0.200 M (D) 0.240 M (E) 0.267 M

85. A sample of 9.00 grams of aluminum metal is added to an excess of hydrochloric acid. The volume of hydrogen gas produced at standard temperature and pressure is (A) 22.4 liters (B) 11.2 liters (C) 7.46 liters (D) 5.60 liters (E) 3.74 liters

Look at 63, Need Graph 63. The graph above shows the results of a study of the reaction of X with a large excess of Y to yield Z. The concentrations of X and Y were measured over a period of time. According to the results, which of the following can be concluded about the rate of law for the reaction under the conditions studied? A) It is zero order in [X]. B) It is first order in [X]. C) It is second order in [X]. D) It is the first order in [Y]. E) The overall order of the reaction is 2.

Look at Table 36. The initial-rate data in the table above were obtained for the reaction represented below. What is the experimental rate la for the reaction? (A) rate = k[NO] [O2] (B) rate = k[NO] [O2]2 (C) rate = k[NO]2 [O2] (D) rate = k[NO]2 [O2]2 (E) rate = k[NO] / [O2]

Questions 1-4 (A) Heisenberg uncertainty principle (B) Pauli exclusion principle (C) Hund's rule (principle of maximum multiplicity) (D) Shielding effect (E) Wave nature of matter 3. Indicates that an atomic orbital can hold no more than two electrons

(A) 1s2 2s22p5 3s23p5 (B) 1s2 2s22p6 3s23p6 (C) 1s2 2s22p62d10 3s23p6 (D) 1s2 2s22p6 3s23p63d5 (E) 1s2 2s22p6 3s23p63d3 4s2 4. An impossible electronic configuration

(A) NH3 and NH4Cl (B) H3PO4 and NaH2PO4 (C) HCl and NaCl (D) NaOH and NH3 (E) NH3 and HC2H3O2 (acetic acid) 9. The solution with the lowest pH

*USE THE PHASE DIAGRAM FROM THE TEST 49. The normal boiling point of the substance represented by the phase diagram above is (A) -15 °C (B) -10 °C (C) 140 °C (D) greater than 140 °C (E) not determinable from the diagram

. . . Li3N(s) + . . . H2O(l) ---> . . . Li+ (aq) + . . . OH¯(aq) + . . . NH3(g) 42. When the equation above is balanced and all coefficients reduced to lowest whole number terms, the coefficient for OH¯(aq) is (A) 1 (B) 2 (C) 3 (D) 4 (E) 6

. . .C10H12O4S(s) + . . O2(g) ---> . . . CO2(g) + . . . SO2(g) + . . . H2O(g) 26. When the equation above is balanced and all coefficients are reduced to their lowest whole-number terms, the coefficient for O2(g) is? (A) 6 (B) 7 (C) 12 (D) 14 (E) 28

14. Which of the following is lower for a 1.0-molar aqueous solution of any solute than it is for pure water? (A) pH (B) Vapor pressure (C) Freezing point (D) Electrical conductivity (E) Absorption of visible light

15. The weight of H2SO4 (molecular weight 98.1) in 50.0 milliliters of a 6.00-molar solution is (A) 3.10 grams (B) 12.0 grams (C) 29.4 grams (D) 294 grams (E) 300. grams

16. A gaseous mixture containing 7.0 moles of nitrogen, 2.5 moles of oxygen, and 0.50 mole of helium exerts a total pressure of 0.90 atmosphere. What is the partial pressure of the nitrogen? (A) 0.13 atm (B) 0.27 atm (C) 0.63 atm (D) 0.90 atm (E) 6.3 atm

16. Methane, CH4(s) (A) Lattice of positive and negative ions held together by electrostatic forces. (B) Closely packed lattice with delocalized electrons throughout (C) Strong single covalent bonds with weak intermolecular forces. (D) Strong multiple covalent bonds (including bonds.) with weak intermolecular forces (E) Macromolecules held tgether with strong polar bonds.

17. The Lewis dot structure of which of the following molecules shows only one unshared pair of valence electron? (A) Cl2 (B) N2 (C) NH3 (D) CCl4 (E) H2O2

19. In the titration of a weak acid of unknown concentration with a standard solution of a strong base, a pH meter was used to follow the progress of the titration. Which of the following is true for this experiment? (A) The pH is 7 at the equivalence point. (B) The pH at the equivalence point depends on the indicator used. (C) The graph of pH versus volume of base added rises gradually at first and then much more rapidly. (D) The graph of pH versus volume of base added shows no sharp rise. (E) The [H+] at the equivalence point equals the ionization constant of the acid.

19. Which of the following best describes the role of the spark from the spark plug in an automobile engine? (A) The spark decreases the energy of activation for the slow step. (B) The spark increases the concentration of the volatile reactant. (C) The spark supplies some of the energy of activation for the combustion reaction. (D) The spark provides a more favorable activated complex for the combustion reaction. (E) The spark provides the heat of vaporization for the volatile hydrocarbon.

24. A sample of 0.0100 mole of oxygen gas is confined at 37° C and 0.216 atmosphere. What would be the pressure of this sample at 15° C and the same volume? (A) 0.0876 atm (B) 0.175 atm (C) 0.201 atm (D) 0.233 atm (E) 0.533 atm

26. How many milliliters of 11.6-molar HCl must be diluted to obtain 1.0 liter of 3.0-molar HCl? (A) 3.9 mL (B) 35 mL (C) 260 mL (D) 1,000 mL (E) 3,900 mL

26. Which of the following actions would be likely to change the boiling point of a sample of a pure liquid in an open container? I. Placing it in a smaller container II. Increasing the number of moles of the liquid in the container III. Moving the container and liquid to a higher altitude (A) I only (B) II only (C) III only (D) II and III only (E) I, II, and III

27. I. Difference in temperature between freezing point of solvent and freezing point of solvent and freezing point of solution II. Molal freezing point depression constant, Kf, for solvent In addition to the information above, which of the following gives the minimum data required to determine the molecular mass of a nonionic substance by the freezing point depression technique? (A) No further information is necessary. (B) Mass of solute (C) Mass of solute and mass of solvent (D) Mass of solute and volume of solvent (E) Mass of solute, mass of solvent, and vapor pressure of solvent

27. Which of the following sets of quantum numbers (n, l, ml, ms) best describes the valence electron of highest energy in a ground-state gallium atom (atomic number 31) ? (A) 4, 0, 0, 1/2 (B) 4, 0, 1, 1/2 (C) 4, 1, 1, 1/2 (D) 4, 1, 2, 1/2 (E) 4, 2, 0, 1/2

28. 2 A(g) + B(g) <===> 2 C(g) When the concentration of substance B in the reaction above is doubled, all other factors being held constant, it is found that the rate of the reaction remains unchanged. The most probable explanation for this observation is that (A) the order of the reaction with respect to substance B is 1 (B) substance B is not involved in any of the steps in the mechanism of the reaction (C) substance B is not involved in the rate-determining step of the mechanism, but is involved in subsequent steps (D) substance B is probably a catalyst, and as such, its effect on the rate of the reaction does not depend on its concentration (E) the reactant with the smallest coefficient in the balanced equation generally has little or no effecton the rate of the reaction

30. When 84-Po-214 decays, the emission consists consecutively of an alpha particle, then two beta particles, and finally another alpha particle. The resulting stable nucleus is (A) 83-Bi-206 (B) 83-Bi-210 (C) 82-Pb-206 (D) 82-Pb-208 (E) 81-Tl-210

31. H2C2O4 + 2 H2O ---> 2 H3O+ + C2O42¯ Oxalic acid, H2C2O4, is a diprotic acid with K1 = 5.36 x 10¯2 and K2 = 5.3 x 10¯5. For reaction above, what is the equilibrium constant? (A) 5.36 x 10¯2 (B) 5.3 x 10¯5 (C) 2.8 x 10¯6 (D) 1.9 x 10¯10 (E) 1.9 x 10¯13

31. If the temperature of an aqueous solution of NaCl is increased from 20 °C to 90 °C, which of the following statements is true? (A) The density of the solution remains unchanged. (B) The molarity of the solution remains unchanged. (C) The molality of the solution remains unchanged. (D) The mole fraction of solute decreases. (E) The mole fraction of solute increases.

33. A 1.0 L sample of an aqueous solution contains 0.10 mol of NaCl and 0.10 mol of CaCl2. What is the minimum number of moles of AgNO3 that must be added to the solution in order to precipitate all of the Cl¯ as AgCl(s) ? (Assume that AgCl is insoluble.) (A) 0.10 mol (B) 0.20 mol (C) 0.30 mol (D) 0.40 mol (E) 0.60 mol

33. A hydrocarbon gas with an empirical formula CH2 has a density of 1.88 grams per liter at 0 °C and 1.00 atmosphere. A possible formula for the hydrocarbon is (A) CH2 (B) C2H4 (C) C3H6 (D) C4H8 (E) C5H10

35. As steady current of 10 amperes in passed though an aluminum-production cell for 15 minutes. Which of the following is the correct expressions for calculating the number of grams of aluminum produced? (1 faraday = 96,500 coulombs) (A) (10 x 15 x 96500)/ (27 x 60) (B) (10 x 15 x 27)/ (96500 x 60) (C) (10 x 15 x 60 x 27)/ (3 x 96500) (D) (27 x 96500)/ (10 x 15 x 60 x 3) (E) (27 x 3)/ (96500 x 10 x 15 x 60)

36. CuO(s) + H2(g) <===> Cu(s) + H2O(g); DH = - 2.0 kilojoules When the substances in the equation above are at equilibrium at pressure P and temperature T, the equilibrium can be shifted to favor the products by (A) increasing the pressure by means of a moving piston at constant T (B) increasing the pressure by adding an inert gas such as nitrogen (C) decreasing the temperature (D) allowing some gases to escape at constant P and T (E) adding a catalyst

36. Zn(s) + Cu2+ ---> Zn2+ + Cu(s) An electrolytic cell based on the reaction represented above was constructed from zinc and copper half-cells. The observed voltage was found to be 1.00 volt instead of the standard cell potential, E°, of 1.10 volts. Which of the following could correctly account for this observation? (A) The copper electrode was larger than the zinc electrode. (B) The Zn2+ electrolyte was Zn(NO3)2, while the Cu2+ electrolyte was CuSO4. (C) The Zn2+ solution was more concentrated than the Cu2+ solution. (D) The solutions in the half-cells had different volumes. (E) The salt bridge contained KCl as the electrolyte.

38. Concentrations of colored substances are commonly measured by means of a spectrophotometer. Which of the following would ensure that correct values are obtained for the measured absorbance? I. There must be enough sample in the tube to cover the entire light path. II. The instrument must be periodically reset using a standard. III. The solution must be saturated. (A) I only (B) II only (C) I and II only (D) II and III only (E) I, II, and III

39. Equal masses of three different ideal gases, X, Y, and Z, are mixed in a sealed rigid container. If the temperature of the system remains constant, which of the following statements about the partial pressure of gas X is correct? (A) It is equal to 1/3 the total pressure (B) It depends on the intermolecular forces of attraction between molecules of X, Y, and Z. (C) It depends on the relative molecular masses of X, Y, and Z. (D) It depends on the average distance traveled between molecular collisions. (E) It can be calculated with knowledge only of the volume of the container.

39. Samples of F2 gas and Xe gas are mixed in a container of fixed volume. The initial partial pressure of the F2 gas is 8.0 atmospheres and that of the Xe gas is 1.7 atmospheres. When all of the Xe gas reacted, forming a solid compound, the pressure of the unreacted F2 gas was 4.6 atmospheres. The temperature remained constant. What is the formula of the compound? (A) XeF (B) XeF3 (C) XeF4 (D) XeF6 (E) XeF8

44. A rigid metal tank contains oxygen gas. Which of the following applies to the gas in the tank when additional oxygen is added at constant temperature? (A) The volume of the gas increase. (B) The pressure of the gas decreases. (C) The average speed of the gas molecules remains th same. (D) The total number of gas molecules remains the same. (E) The average distance between the gas molecules increases.

45. A sample of an ideal gas is cooled from 50.0 °C to 25.0 °C in a sealed container of constant volume. Which of the following values for the gas will decrease? I. The average molecular mass of the gas II. The average distance between the molecules III. The average speed of the molecules (A) I only (B) II only (C) III only (D) I and III (E) II and III

46. Which of the following occurs when excess concentrated NH3(aq) is mixed throughly with 0.1 M Cu(NO3)2(aq) ? (A) A dark red precipitate forms and settles out. (B) Separate layers of immiscible liquids form with a blue layer on top. (C) The color of the solution turns from light blue to dark blue. (D) Bubbles of ammonia gas form. (E) The pH of the solution decreases.

47. CCl4, CO2, PCl3, PCl5, SF6 Which of the following does not describe any of the molecules above? (A) Linear (B) Octahedral (C) Square planar (D) Tetrahedral (E) Trigonal pyramidal

47. CH4(g) + 2 O2(g) ---> CO2(g) + 2 H2O(l); D = - 889.1 kJ DHf° H2O(l) = - 285.8 kJ / mole DHf° CO2(g) = - 393.3 kJ / mole What is the standard heat of formation of methane, DHf° CH4(g), as calculated from the data above? (A) -210.0 kJ/mole (B) -107.5 kJ/mole (C) -75.8 kJ/mole (D) 75.8 kJ/mole (E) 210.0 kJ/mole

47. When hafnium metal is heated in an atmosphere of chlorine gas, the product of the reaction is found to contain 62.2 percent Hf by mass and 37.4 percent Cl by mass. What is the empirical formula for this compound? (A) HfCl (B) HfCl2 (C) HfCl3 (D) HfCl4 (E) Hf2Cl3

49. Each of the following can act as both a Brönsted acid and a Brönsted base EXCEPT (A) HCO3¯ (B) H2PO4¯ (C) NH4+ (D) H2O (E) HS¯

53. Which of the following must be true for a reaction that proceeds spontaneously from initial standard state conditions? (A) G° > 0 and Keq > 1 (B) G° > 0 and Keq < 1 (C) G° < 0 and Keq > 1 (D) G° < 0 and Keq > 1 (E) G° = 0 and Keq = 1

55. What volume of 0.150-molar HCl is required to neutralize 25.0 millilters of 0.120-molar Ba(OH)2? (A) 20.0 mL (B) 30 0 mL (C) 40.0 mL (D) 60.0 mL (E) 80.0 mL

56. A 0.20-molar solution of a weak monoprotic acid, HA, has a pH of 3.00. The ionization constant of this acid is (A) 5.0 x 10¯7 (B) 2.0 x 10¯7 (C) 5.0 x 10¯6 (D) 5.0 x 10¯3 (E) 2.0 x 10¯3

56. A cube of ice is added to some hot water in a rigid, insulated container, which is then sealed. There is no heat exchange with the surroundings. What has happened to the total energy and the total entropy when the system reaches equilibrium? Energy Entropy (A) Remains constant Remains constant (B) Remains constant Decreases (C) Remains constant Increases (D) Decreases Increases (E) Increases Decreases

58. (CH3)3CCl(aq) + OH¯ ---> (CH3)3COH(aq) + Cl¯ For the reaction represented above, the experimental rate law is given as follows. Rate = k [(CH3)3CCl] If some solid sodium solid hydroxide is added to a solution that is 0.010-molar in (CH3)3CCl and 0.10-molar in NaOH, which of the following is true? (Assume the temperature and volume remain constant.) (A) Both the reaction rate and k increase. (B) Both the reaction rate and k decrease. (C) Both the reaction rate and k remain the same. (D) The reaction rate increases but k remains the same. (E) The reaction rate decreases but k remains the same.

58. On a mountaintop, it is observed that water boils at 90°C, not at 100°C as at sea level. This phenomenon occurs because on the mountaintop the A) equilibrium water vapor pressure is higher due to the higher atmospheric pressure B) equilibrium water vapor pressure is lower due to the higher atmospheric pressure C) equilibrium water vapor pressure equals the atmospheric pressure at a lower temperature D) water molecules have a higher average kinetic energy due to the lower atmospheric pressure E) water contains a greater concentration of dissolved gases

59. A 40.0 mL sample of 0.25 M KOH is added to 60.0 mL of 0.15 M Ba(OH)2. What is the molar concentration of OH¯(aq) in the resulting solution? (Assume that the volumes are additive) A) 0.10 M B) 0.19 M C) 0.28 M D) 0.40 M E) 0.55 M

62. As the temperature is raised from 20 ° C to 40 ° C, the average kinetic energy of neon atoms changes by a factor of (A) 1/2 (B) [square root of](313/293) (C) 313/293 (D) 2 (E) 4

65. The solubility of CuI is 2 x 10¯6 molar. What is the solubility product constant, Ksp, for CuI? (A) 1.4 x 10¯3 (B) 2 x 10¯6 (C) 4 x 10¯12 (D) 2 x 10¯12 (E) 8 x 10¯18

69. Correct procedures for a titration include which of the following? I. Draining a pipet by touching the tip to the side of the container used for the titration II. Rinsing the buret with distilled water just before filling it with the liquid to be titrated III. Swirling the solution frequently during the titration (A) I only (B) II only (C) I and III only (D) II and III only (E) I, II, and III

69. What is the final concentration of barium ions, [Ba2+], in solution when 100. mL of 0.10 M BaCl2(aq) is mixed with 100. mL of 0.050 M H2SO4(aq)? A) 0.00 M B) 0.012 M C) 0.025 M D) 0.075 M E) 0.10 M

7. Represents an atom that has four valence electrons. - Answer Choices on Picture

71 ... Fe(OH)2 + ... O2 + ... H2O ---> ... Fe(OH)3 If 1 mole of O2 oxidizes Fe(OH)2 according to the reaction represented above, how many moles of Fe(OH)3 can be formed? (A) 2 (B) 3 (C) 4 (D) 5 (E) 6

72. A compound is heated to produce a gas whose molecular weight is to be determined. The gas is collected by displacing water in a water-filled flask inverted in a trough of water. Which of the following is necessary to calculate the molecular weight of the gas, but does NOT need to be measured during the experiment? (A) Mass of the compound used in the experiment (B) Temperature of the water in the trough (C) Vapor pressure of the water (D) Barometric pressure (E) Volume of water displaced from the flask

8-10 Refer to the following diatomic species (A) Li2 (B) B2 (C) N2 (D) O2 (E) F2 10. Contains 1 sigma (s) and 2 pi (p) bonds

8-10 Refer to the following diatomic species (A) Li2 (B) B2 (C) N2 (D) O2 (E) F2 8. Has the largest bond-dissociation energy

8. Solid ethyl alcohol, C2H5OH (A) A network solid with covalent bonding (B) A molecular solid with zero dipole moment (C) A molecular solid with hydrogen bonding (D) An ionic solid (E) A metallic solid

82. Step 1) N2H2O2 <===> N2HO2¯ + H+ (fast equilibrium) Step 2) N2HO2¯ ---> N2O + OH¯ (slow) Step 3) H+ + OH¯ ---> H2O (fast) Nitramide, N2H2O2, decomposes slowly in aqueous solution. This decomposition is believed to occur according to the reaction mechanism above. The rate law for the decomposition of nitramide that is consistent with this mechanism is given by which of the following? (A) Rate = k [N2H2O2] (B) Rate = k [N2H2O2] [H+] (C) Rate = (k [N2H2O2]) / [H+] (D) Rate = (k [N2H2O2]) / [N2HO2¯] (E) Rate = k [N2H2O2] [OH¯]

Assume that you have an "unknown" consisting of an aqueous solution of a salt that contains one of the ions listed above. Which ions must be absent on the basis of each of the following observations of the "unknown"? 12. No odor can be detected when a sample of the solution is added drop by drop to a warm solution of sodium hydroxide. (A) CO32¯ (B) Cr2O72¯ (C) NH4+ (D) Ba2+ (E) Al3+

Look at 25 for Graph 25. The cooling curve for a pure substance as it changes from a liquid to a solid is shown right. The solid and the liquid coexist at (A) point Q only (B) point R only (C) all points on the curve between Q and S (D) all points on the curve between R and T (E) no point on the curve

Look at diagram 40. The system shown above is at equilibrium at 28 °C. At this temperature, the vapor pressure of water is 28 millimeters of mercury. The partial pressure of O2(g) in the system is (A) 28 mm Hg (B) 56 mm Hg (C) 133 mm Hg (D) 161 mm Hg (E) 189 mm Hg

Look at graph picture 39. The phase diagram for a pure substance is shown above. Which point on the diagram corresponds to the equilibrium between the solid and liquid phases at the normal melting point? (A) A (B) B (C) C (D) D (E) E

Look at table 37. The ionization energies for element X are listed in the table above. On the basis of the data, element X is most likely to be (A) Na (B) Mg (C) Al (D) Si (E) P

Questions 11-13 (A) Pb (B) Ca (C) Zn (D) As (E) Na 11. Utilized as a coating to protect Fe from corrosion

CS2(l) + 3 O2(g) => CO2(g) + 2 SO2(g) 31. What volume of O2(g) is required to react with excess CS2(l) to produce 4.0 L of CO2(g)? (Assume all gases are measured at 0˚C and 1 atm.) (A) 12 L (B) 22.4 L (C) 1/3 x 22.4 L (D) 2 x 22.4 L (E) 3 x 22.4 L

10 HI + 2 KMnO4 + 3 H2SO4 --> 5 I2 + 2 MnSO4 + K2SO4 + 8 H2O 55. According to the balanced equation above, how many moles of HI would be necessary to produce 2.5 mol of I2, starting with 4.0 mol of KMnO4 and 3.0 mol of H2SO4? A) 20 B) 10 C) 8.0 D) 5.0 E) 2.5

20. . . . Ag+ + . . . AsH3(g) + . . . OH¯ ---> . . . Ag(s) + . . . H3AsO3(aq) + . . . H2O When the equation above is balanced with lowest whole-number coefficients, the coefficient for OH¯ is (A) 2 (B) 4 (C) 5 (D) 6 (E) 7

21. Correct statements about alpha particles include which of the following? I. They have a mass number of 4 and a charge of +2. II. They are more penetrating than beta particles. III. They are helium nuclei. (A) I only (B) III only (C) I and II (D) I and III (E) II and III

22. __ Cr2O72¯ + __ e¯ + __ H+ ---> __ Cr3+ + __ H2O(l) When the equation for the half reaction above is balanced with the lowest whole-number coefficients, the coefficient for H2O is (A) 2 (B) 4 (C) 6 (D) 7 (E) 14

25. The simplest formula for an oxide of nitrogen that is 36.8 percent nitrogen by weight is (A) N2O (B) NO (C) NO2 (D) N2O3 (E) N2O5

28. Which of the following is probably true for a solid solute with a highly endothermic heat of solution when dissolved in water? (A) The solid has a low lattice energy. (B) As the solute dissolves, the temperature of the solution increases. (C) The resulting solution is ideal. (D) The solid is more soluble at higher temperatures. (E) the solid has a high energy of hydration.

32. CH3CH2OH boils at 78 °C and CH3OCH3 boils at - 24 °C, although both compounds have the same composition. This difference in boiling points may be attributed to a difference in (A) molecular mass (B) density (C) specific heat (D) hydrogen bonding (E) heat of combustion

32. Types of hybridization exhibited by the C atoms in propene, CH3CHCH2, include which of the following? I. sp II. sp2 III. sp3 (A) I only (B) III only (C) I and II only (D) II and III only (E) I, II, and III

33. The pH of 0.1-molar ammonia is approximately (A) 1 (B) 4 (C) 7 (D) 11 (E) 14

34. ...CrO2¯ + ...OH¯ ---> ... CrO42¯ + ... H2O + ... e¯ When the equation for the half-reaction above is balanced, what is the ratio of the coefficients OH¯ / CrO2¯ ? (A) 1:1 (B) 2:1 (C) 3:1 (D) 4:1 (E) 5:1

34. All of the following species can function as Brönsted-Lowry bases in solution EXCEPT (A) H2O (B) NH3 (C) S2¯ (D) NH4+ (E) HCO3¯

35. For which of the following processes would DS have a negative value? I. 2 Fe2O3(s) ---> 4 Fe(s) + 3 O2(g) II. Mg2+ + 2 OH¯ ---> Mg(OH)2(s) III. H2(g) + C2H4(g) ---> 3 C2H6(g) (A) I only (B) I and II only (C) I and III only (D) II and III only (E) I, II, and III

35. The addition of an oxidizing agent such as chlorine water to a clear solution of an unknown compound results in the appearance of a brown color. When this solution is shaken with the organic solvent, methylene dichloride, the organic solvent layer turns purple. The unknown compound probably contains (A) K+ (B) Br¯ (C) NO3¯ (D) I¯ (E) Co2+

36. Appropriate laboratory procedures include which of the following? I. Rinsing a buret with distilled water just before filling it with the titrant for the first titration II. Lubricating glass tubing before inserting it into a stopper III. For accurate results, waiting until warm or hot objects have reached room temperature before weighing them (A) II only (B) I and II only (C) I and III only (D) II and III only (E) I, II, and III

37. A sample of 3.30 grams of an ideal gas at 150.0 °C and 1.25 atmospheres pressure has a volume of 2.00 liters. What is the molar mass of the gas? The gas constant, R, is 0.0821 L atm mol¯1 K¯1). (A) 0.0218 gram/mole (B) 16.2 grams/mole (C) 37.0 grams/mole (D) 45.8 grams/mole (E) 71.6 grams/mole

37. __ CH3CH2COOH(l) + __ O2(g) ---> __ CO2(g) + __ H2O(l) How many moles of O2 are required to oxidize 1 mole of CH3CH2COOH according to the reaction represented above? (A) 2 moles (B) 5/2 moles (C) 3 moles (D) 7/2 moles (E) 9/2 moles

40. 2 K + 2 H2O ---> 2 K+ + 2 OH¯ + H2 When 0.400 mole of potassium reacts with excess water at standard temperature and pressure as shown in the equation above, the volume of hydrogen gas produced is (A) 1.12 liters (B) 2.24 liters (C) 3.36 liters (D) 4.48 liters (E) 6.72 liters

40. Of the following molecules, which has the largest dipole moment? (A) CO (B) CO2 (C) O2 (D) HF (E) F2

41. A strip of metallic scandium, Sc, is placed in a beaker containing concentrated nitric acid. A brown gas rapidly forms, the scandium disappears, and the resulting liquid is brown-yellow but becomes colorless when warmed. These observations best support which of the following statements? (A) Nitric acid is a strong acid. (B) In solution scandium nitrate is yellow and scandium chloride is color less. (C) Nitric acid reacts with metals to form hydrogen. (D) Scandium reacts with nitric acid to form a brown gas. (E) Scandium and nitric acid react in mole propor tions of 1 to 3.

41. Which of the following reactions has the largest positive value of S per mole of Cl2 (A) H2(g) + Cl2(g) ---> 2 HCl(g) (B) Cl2(g) + 1/2 O2(g) ---> Cl2O(g) (C) Mg(s) + Cl2(g) ---> MgCl2(s) (D) 2 NH4Cl(s) ---> N2(g) + 4 H2(g) + Cl2(g) (E) Cl2(g) ---> 2 Cl(g)

42. Mass of an empty container = 3.0 grams Mass of the container plus the solid sample = 25.0 grams Volume of the solid sample = 11.0 cubic centimeters The data above were gathered in order to determine the density of an unknown solid. The density of the sample should be reported as (A) 0.5 g/cm3 (B) 0.50 g/cm3 (C) 2.0 g/cm3 (D) 2.00 g/cm3 (E) 2.27 g/cm3

42. The SbCl5 molecule has trigonal bipyramid structure. Therefore, the hybridization of Sb orbitals should be (A) sp2 (B) sp3 (C) dsp2 (D) dsp3 (E) d2sp3

43. A sample of 61.8 g of H3BO3, a weak acid is dissolved in 1,000 g of water to make a 1.0-molal solution. Which of the following would be the best procedure to determine to molarity of the solution? (Assume no additional information is available.) (A) Titration of the solution with standard acid (B) Measurement of the pH with a pH meter (C) Determination of the boiling point of the solution (D) Measurement of the total volume of the solution (E) Measurement of the specific heat of the solution

44. What number of moles of O2 is needed to produce 14.2 grams of P4O10 from P? (Molecular weight P4O10 = 284) (A) 0.0500 mole (B) 0.0625 mole (C) 0.125 mole (D) 0.250 mole (E) 0.500 mole

45. A measured mass of an unreactive metal was dropped into a small graduated cylinder half filled with water. The following measurements were made. Mass of metal = 19.611 grams Volume of water before addition of metal = 12.4 milliliters Volume of water after addition of metal = 14.9 milliliters The density of the metal should be reported as (A) 7.8444 grams per mL (B) 7.844 grams per mL (C) 7.84 grams per mL (D) 7.8 grams per mL (E) 8 grams per mL

45. What is the H+(aq) concentration in 0.05 M HCN (aq) ? (The Ka for HCN is 5.0 x 10¯10) (A) 2.5 x 10¯11 (B) 2.5 x 10¯10 (C) 5.0 x 10¯10 (D) 5.0 x 10¯6 (E) 5.0 x 10¯4

47. Which of the following has the lowest conductivity? (A) 0.1 M CuS04 (B) 0.1 M KOH (C) 0.1 M BaCl2 (D) 0.1 M HF (E) 0.1 M HNO3

5. Represents an atom that is chemically unreactive

50. In the periodic table, as the atomic number increases from 11 to 17, what happens to the atomic radius? (A) It remains constant. (B) It increases only. (C) It increases, then decreases. (D) It decreases only. (E) It decreases, then increases.

51. 4 HCl(g) + O2(g) <===> 2 Cl2(g) + 2 H2O(g) Equal numbers of moles of HCl and O2 in a closed system are allowed to reach equilibrium as represented by the equation above. Which of the following must be true at equilibrium? I. [HCl] must be less than [Cl2]. II. [O2] must be greater than [HCl]. III. [Cl2] must equal [H2O]. (A) I only (B) II only (C) I and III only (D) II and III only (E) I, II, and III

54. All of the following statements concerning the characteristics of the halogens are true EXCEPT: (A) The first ionization energies (potentials) decrease as the atomic numbers of the halogens increase. (B) Fluorine is the best oxidizing agent. (C) Fluorine atoms have the smallest radii. (D) Iodine liberates free bromine from a solution of bromide ion. (E) Fluorine is the most electronegative of the halogens.

55. At 20. °C, the vapor pressure of toluene is 22 millimeters of mercury and that of benzene is 75 millimeters of mercury. An ideal solution, equimolar in toluene and benzene, is prepared. At 20. °C, what is the mole fraction of benzene in the vapor in equilibrium with this solution? (A) 0.23 (B) 0.29 (C) 0.50 (D) 0.77 (E) 0.83

59. When 70. milliliter of 3.0-molar Na2CO3 is added to 30. milliliters of 1.0-molar NaHCO3 the resulting concentration of Na+ is (A) 2.0 M (B) 2.4 M (C) 4.0 M (D) 4.5 M (E) 7.0 M

59. When a 1.00-gram sample of limestone was dissolved in acid, 0.38 gram of CO2 was generated. If the rock contained no carbonate other than CaCO3, what was the percent of CaCO3 by mass in the limestone? (A) 17% (B) 51% (C) 64% (D) 86% (E) 100%

6. Is used extensively for the production of fertilizers (A) Hydrofluoric acid (B) Carbon dioxide (C) Aluminum hydroxide (D) Ammonia (E) Hydrogen peroxide

60. Fe2+ + 2e¯ ---> Fe(s) E° = - 0.44 volt Ni2+ + 2e¯ ---> Ni(s) E° = - 0.23 volt The standard reduction potentials for two half reactions are given above. The Nernst equation for a galvanic cell at 25° C in which Fe(s) reduces Ni2+ is the following. E = E° - 0.059/2 log [Fe2+] / [Ni2+] What is the equilibrium constant for the reaction below? Fe(s) + Ni2+ ---> Fe2+ + Ni(s) (A) 1.9 x 10¯23 (B) 7.6 x 10¯8 (C) 3.6 x 10+3 (D) 1.3 x 10+7 (E) 5.2 x 10+22

61. When a solution of potassium dichromate is added to an acidified solution of iron(II) sulfate, the products of the reaction are (A) FeCr2O7(s) and H2O (B) FeCrO4(s) and H2O (C) Fe3+, CrO42¯, and H2O (D) Fe3+, Cr3+, and H2O (E) Fe2(SO4)3(s), Cr3+ and H2O

62. A student pipetted five 25.00-milliliter samples of hydrochloric acid and transferred each sample to an Erlenmeyer flask, diluted it with distilled water, and added a few drops of phenolphthalein to each. Each sample was then titrated with a sodium hydroxide solution to the appearance of the first permanent faint pink color. The following results were obtained. Volumes of NaOH Solution First Sample..................35.22 mL Second Sample..............36.14 mL Third Sample.................36.13 mL Fourth Sample..............36.15 mL Fifth Sample..................36.12 mL Which of the following is the most probable explanation for the variation in the student's results? (A) The burette was not rinsed with NaOH solution. (B) The student misread a 5 for a 6 on the burette when the first sample was titrated. (C) A different amount of water was added to the first sample. (D) The pipette was not rinsed with the HCI solution. (E) The student added too little indicator to the first sample.

63. Acid Acid Dissociation Constant, Ka H3PO4 7 x 10¯3 H2PO4¯ 8 x 10¯8 HPO42¯ 5 x 10¯13 On the basis of the information above, a buffer with a pH = 9 can best be made by using (A) pure NaH2PO4 (B) H3PO4 + H2PO4¯ (C) H2PO4¯ + PO43¯ (D) H2PO4¯ + HPO42¯ (E) HPO42¯ + PO43¯

64. At 25 °C, a sample of NH3 (molar mass 17 grams) effuses at the rate of 0.050 mole per minute. Under the same conditions, which of the following gases effuses at approximately one-half that rate? (A) O2 (molar mass 32 grams) (B) He2 (molar mass 4.0 grams) (C) CO2 (molar mass 44 grams) (D) Cl2 (molar mass 71 grams) (E) CH4 (molar mass 16 grams)

66. Ca, V, Co, Zn, As Gaseous atoms of which of the elements above are paramagnetic? (A) Ca and As only (B) Zn and As only (C) Ca, V, and Co only (D) V, Co, and As only (E) V, Co, and Zn only

66. MnS(s) + 2 H+ <===> Mn2+ + H2S(g) At 25 °C the solubility product constant, Ksp, for MnS in 5 x 10¯15 and the acid dissociation constants K1 and K2 for H2S are 1 x 10¯7 and 1 x 10¯13, respectively. What is the equilibrium constant for the reaction represented by the equation above at 25 °C? (A) 1 x 10¯13 / 5 x 10¯15 (B) 5 x 10¯15 / 1 x 10¯7 (C) 1 x 10¯7 / 5 x 10¯20 (D) 5 x 10¯15 / 1 x 10¯20 (E) 1 x 10¯20 / 5 x 10¯15

66. What is the pH of a 1.0 x 10¯2-molar solution of HCN? (For HCN, Ka = 4.0 x 10¯10.) (A) 10 (B) Between 7 and 10 (C) 7 (D) Between 4 and 7 (E) 4

68. In which of the following processes are covalent bonds broken? A) I2(s) --> I2(g) B) CO2(s) --> CO2(g) C) NaCl(s) --> NaCl(l) D) C(diamond) --> C(g) E) Fe(s) --> Fe(l)

73. A 27.0-gram sample of an unknown hydrocarbon was burned in excess oxygen to form 88.0 grams of carbon dioxide and 27.0 grams of water. What is a possible molecular formula of the hydrocarbon? (A) CH4 (B) C2H2 (C) C4H3 (D) C4H6 (E) C4H10

73. The volume of distilled water that should be added to 10.0 mL of 6.00 M HCl(aq) in order to prepare a 0.500 M HCl(aq) solution is approximately A) 50.0 mL B) 60.0 mL C) 100. mL D) 110. mL E) 120. mL

74. How many moles of NaF must be dissolved in 1.00 liter of a saturated solution of PbF2 at 25 °C to reduce the [Pb2+] to 1 x 10¯6 molar? (Ksp of PbF2 at 25 °C = 4.0 x 10¯8) (A) 0.020 mole (B) 0.040 mole (C) 0.10 mole (D) 0.20 mole (E) 0.40 mole

Assume that you have an "unknown" consisting of an aqueous solution of a salt that contains one of the ions listed above. Which ions must be absent on the basis of each of the following observations of the "unknown"? 13. No precipitate is formed when a dilute solution of H2SO4 is added to a sample of the solution. (A) CO32¯ (B) Cr2O72¯ (C) NH4+ (D) Ba2+ (E) Al3+

H2Se(g) + 4 O2F2(g) ---> SeF6(g) + 2 HF(g) + 4 O2(g) 30. Which of the following is true regarding the reaction represented above? (A) The oxidation number of O does not change. (B) The oxidation number of H changes from -1 to +1. (C) The oxidation number of F changes from +1 to -1. (D) The oxidation number of Se changes from -2 to +6. (E) It is a disproportionation reaction for F.

(A) 1s2 2s22p5 3s23p5 (B) 1s2 2s22p6 3s23p6 (C) 1s2 2s22p62d10 3s23p6 (D) 1s2 2s22p6 3s23p63d5 (E) 1s2 2s22p6 3s23p63d3 4s2 5. The ground-state configuration for the atoms of a transition element

(A) NH3 and NH4Cl (B) H3PO4 and NaH2PO4 (C) HCl and NaCl (D) NaOH and NH3 (E) NH3 and HC2H3O2 (acetic acid) 10. The most nearly neutral solution

(A) O (B) La (C) Rb (D) Mg (E) N 2. Which element exhibits the greatest number of different oxidation states?

(A) hydrogen bonding (B) hybridization (C) ionic bonding (D) resonance (E) van der Waals forces (London dispersion forces) 11. Is used to explain why iodine molecules are held together in the solid state

15. In a molecule in which the central atom exhibits sp3d2 hybrid orbitals, the electron pairs are directed toward the corners of (A) a tetrahedron (B) a square-based pyramid (C) a trigonal bipyramid (D) a square (E) an octahedron

17. Is a gas in its standard state at 298 K (A) Lithium (B) Nickel (C) Bromine (D) Uranium (E) Fluorine

18. 2 H2O + 4 MnO4¯ + 3 ClO2¯ ---> 4 MnO2 + 3 ClO4¯ + 4 OH¯ Which species acts as an oxidizing agent in the reaction represented above? (A) H2O (B) ClO4¯ (C) ClO2¯ (D) MnO2 (E) MnO4¯

2 SO3 (g) <===> 2 SO2 (g) + O2 (g) 41. After the equilibrium represented above is established, some pure O2 (g) is injected into the reaction vessel at constant temperature. After equilibrium is reestablished, which of the following has a lower value cmpared to its value at the original equilibrium? (A) Keq for the reaction (B) The total pressure in the reaction vessel. (C) The amount of SO3 (g) in the reaction vessel. (D) The amount of O2 (g) in the reaction vessel. (E) The amount of SO2 (g) in the reaction vessel.

2. Forms a compound having the formula KXO4 (A) F (B) S (C) Mg (D) Ar (E) Mn

20. .....Mg(s) + .....NO3¯(aq) +.....H+(aq) --->......Mg2+(aq) + ....NH4+(aq) + ....H2O(l) When the skeleton equation above is balanced and all coefficients reduced to their lowest whole-number terms. what is the coeficient for H+ ? (A) 4 (B) 6 (C) 8 (D) 9 (E) 10

20. 6 I¯ + 2 MnO4¯ + 4 H2O(l) ---> 3 I2(s) + 2 MnO2(s) + OH¯ Which of the following statements regarding the reaction represented by the equation above is correct? (A) Iodide ion is oxidized by hydroxide ion. (B) MnO4¯ is oxidized by iodide ion. (C) The oxidation number of manganese changes from +7 to +2. (D) The oxidation number of manganese remains the same. (E) The oxidation number of iodine changes from -1 to 0. 21. Which of the following is true at the triple point of a pure substance?

22. 1s2 2s22p6 3s23p3 Atoms of an element, X, have the electronic configuration shown above. The compound most likely formed with magnesium, Mg, is (A) MgX (B) Mg2X (C) MgX2 (D) MgX3 (E) Mg3X2

22. HSO4¯ + H2O <===> H3O+ + SO42¯ In the equilibrium represented above, the species that act as bases include which of the following? I. HSO4¯ II. H2O III. SO42¯ (A) II only (B) III only (C) I and II (D) I and III (E) II and III

22. Of the following reaction, which involves the largest decrease in entropy? (A) CaCO3(s) ---> CaO(s) + CO2(g) (B) 2 CO(g) + O2(g) ---> 2 CO2 (C) Pb(NO3)3 + 2 KI ---> PbI2 + 2 KNO3 (D) C3H8 + O2 ---> 3 CO2 + 4 H2O (E) 4 La + 3 O2 ---> 2 La2O3

23. A hot-air balloon, shown right, rises. Which of the following is the best explanation for this observation? (A) The pressure on the walls of the balloon increases with increasing tempearature. (B) The difference in temperature between the air inside and outside the ballon produces convection currents. (C) The cooler air outside the balloon pushes in on the walls of the ballon. (D) The rate of diffusion of cooler air is less than that of warmer air. (E) The air density inside the ballon is less than that of the surrounding air.

27. The critical temperature of a substance is the (A) temperature at which the vapor pressure of the liquid is equal to the external pressure (B) temperature at which the vapor pressure of the liquid is equal to 760 mm Hg (C) temperature at which the solid, liquid, and vapor phases are all in equilibrium (D) Temperature at which liquid and vapor phases are in equilibrium at I atmosphere (E) lowest temperature above which a substance cnnot be liquified at any applied pressure

28. Given that a solution is 5 percent sucrose by mass, what additional information is necessary to calculate the molarity of the solution? I. The density of water II. The density of the solution III. The molar mass of sucrose (A) I only (B) II only (C) III only (D) I and III (E) II and III

29. In which of the following systems would the number of moles of the substances present at equilibrium NOT be shifted by a change in the volume of the system at constant temperature? (A) CO(g) + NO(g) <===> CO2(g) + 1/2 N2(g) (B) N2(g) + 3 H2(g) <===> 2 NH3(g) (C) N2(g) + 2 O2(g) <===> 2 NO2(g) (D) N2O4(g) <===> 2 NO2(g) (E) NO(g) + O3(g) <===> NO2(g) + O2(g)

31. A 0.1-molar solution of which of the following ions is orange? (A) Fe(H2O)42+ (B) Cu(NH3)42+ (C) Zn(OH)42¯ (D) Zn(NH3)42+ (E) Cr2O72¯

34. X = CH3-CH2-CH2-CH2-CH3 Y = CH3-CH2-CH2-CH2-OH Z = HO-CH2-CH2-CH2-OH Based on concepts of polarity and hydrogen bonding, which of the following sequences correctly lists the compounds above in the order of their increasing solubility in water? (A) Z < Y < X (B) Y < Z < X (C) Y < X < Z (D) X < Z < Y (E) X < Y < Z

37. The molality of the glucose in a 1.0-molar glucose solution can be obtained by using which of the following? (A) Volume of the solution (B) Temperature of the solution (C) Solubility of glucose in water (D) Degree of dissociation of glucose (E) Density of the solution

4. Is a good oxidizing agent (A) Hydrofluoric acid (B) Carbon dioxide (C) Aluminum hydroxide (D) Ammonia (E) Hydrogen peroxide

43. The elements in which of the following have most nearly the same atomic radius? (A) Be, B, C, N (B) Ne, Ar, Kr, Xe (C) Mg, Ca, Sr, Ba (D) C, P, Se, I (E) Cr, Mn, Fe, Co

44. The metal calcium reacts with molecular hydrogen to form a compound. All of the following statements concerning this compound are true EXCEPT: (A) Its formula is CaH2. (B) It is ionic. (C) It is solid at room temperatur(E) (D) When added to water, it reacts to produce H2 gas. (E) When added to water, it forms an acidic solution.

44. Which of the following solutions has the lowest freezing point? (A) 0.20 m C6H12O6, glucose (B) 0.20 m NH4Br (C) 0.20 m ZnSO4 (D) 0.20 m KMnO4 (E) 0.20 m MgCl2

46. As the number of oxygen atoms increases in any series of oxygen acids, such as HXO, HXO2, HXO3, ...., which of the following is generally true? (A) The acid strength varies unpredictably. (B) The acid strength decreases only if X is a nonmetal. (C) The acid strength decreases only if X is a metal. (D) The acid strength decreases whether X is a nonmetal or a metal. (E) The acid strength increases.

46. Which of the following solids dissolves in water to form a colorless solution? (A) CrCl3 (B) FeCl3 (C) CoCl2 (D) CuCl2 (E) ZnCl2

48. Which of the following ions is the strongest Lewis acid? (A) Na+ (B) Cl¯ (C) CH3COO¯ (D) Mg2+ (E) Al3+

49. Which of the following techniques is most appropriate for the recovery of solid KNO3 from an aqueous solution of KNO3? (A) Paper chromatography (B) Filtration (C) Titration (D) Electrolysis (E) Evaporation to dryness

50. Two flexible containers for gases are at the same temperature and pressure. One holds 0.50 gram of hydrogen and the other holds 8.0 grams of oxygen. Which of the following statements regarding these gas samples is FALSE? (A) The volume of the hydrogen container is the same as the volume of the oxygen container. (B) The number of molecules in the hydrogen container is the same as the number of molecules in the oxygen container. (C) The density of the hydrogen sample is less than that of the oxygen sample. (D) The average kinetic energy of the hydrogen molecules is the same as the average kinetic energy of the oxygen molecules. (E) The average speed of the hydrogen molecules is the same as the average speed of the oxygen molecules.

53. If 87 grams of K2 SO4 (molar mass 174 grams) is dissolved in enough water to make 250 milliliters of solution, what are the concentrations of the potassium and the sulfate ions? [K+] [SO42¯] (A) 0.020 M 0.020 M (B) 1.0 M 2.0 M (C) 2.0 M 1.0 M (D) 2.0 M 2.0 M (E) 4.0 M 2.0 M

59. Which of the following compounds is ionic and contains both sigma and pi covalent bonds? (A) Fe(OH)3 (B) HClO (C) H2S (D) NO2 (E) NaCN

64. A solution is known to contain an inorganic salt of one of the following elements. The solution is colorless. The solution contains a salt of (A) Cu (B) Mn (C) Fe (D) Ni (E) Zn

64. The net ionic equation for the reaction that occurs during the titration of nitrous aicd with sodium hydroxide is (A) HNO2 + Na+ + OH¯ ---> NaNO2 + H2O (B) HNO2 + NaOH ---> Na+ + NO2¯ + H2O (C) H+ + OH¯ --->H2O (D) HNO2 + H2O ---> NO2¯ + H3O+ (E) HNO2 + OH¯ ---> NO2¯ + H2O

65. Which of the following species CANNOT function as an oxidizing agent? (A) Cr2O72¯ (B) MnO4¯ (C) NO3¯ (D) S (E) I¯

67. Substances X and Y that were in a solution were separated in the laboratory using the technique of fractional crystallization. This fractional crystallization is possible because substances X and Y have different (A) boiling points (B) melting points (C) densities (D) crystal colors (E) solubilities

67. What is the molar solubility in water of Ag2CrO4? (The Ksp for Ag2CrO4 is 8 x 10¯12.) A) 8 x 10¯12 M B) 2 x 10¯12 M C) (4 x 10¯12 M)1/2 D) (4 x 10¯12 M)1/3 E) (2 x 10¯12 M)1/3

68. The specific rate constant k for radioactive element X is 0.023 min -1. What weight of X wsa originally present in a sample if 40. grams is left after 60. minutes? (A) 10. grams (B) 20. grams (C) 80. grams (D) 120 grams (E) 160 grams

70. H2O(s) ---> H2O(l) When ice melts at its normal melting point, 273.16 K and 1 atmosphere, which of the following is true for the process shown above? (A) H < 0, S > 0, V > 0 (B) H < 0, S < 0, V > 0 (C) H > 0, S < 0, V < 0 (D) H > 0, S > 0, V > 0 (E) H > 0, S > 0, V < 0

70. One of the outermost electrons in a strontium atom in the ground state can be described by which of the following sets of four quantum numbers? (A) 5, 2, 0, 1/2 (B) 5, 1, 1, 1/2 (C) 5, 1, 0, 1/2 (D) 5, 0, 1, 1/2 (E) 5, 0, 0, 1/2

71. A solution of toluene (molecular weight 92.1) in benzene (molecular weight 78.1) is prepared. The mole fraction of toluene in the solution is 0.100. What is the molality of the solution? (A) 0.100 m (B) 0.703 m (C) 0.921 m (D) 1.28 m (E) 1.42 m

71. Which of the following reactions does NOT proceed significantly to the right in aqueous solutions? (A) H3O+ + OH¯ ---> 2 H2O (B) HCN + OH¯ ---> H2O + CN¯ (C) Cu(H2O)42+ + 4 NH3 ---> Cu(NH3)42+ + 4H2O (D) H2SO4 + H2O ---> H3O+ + HSO4¯ (E) H2O + HSO4¯ ---> H2SO4 + OH¯

72. The nuclide 245Cm is radioactive and decays by the loss of one beta ([beta]¯) particle. The product nuclide is (A) 245Pu (B) 95Am (C) 248Cm (D) 250Cm (E) 97Bk

75. If the acid dissociation constant, Ka, for an acid HA is 8 x 10¯4 at 25 °C, what percent of the acid is dissociated in a 0.50-molar solution of HA at 25 °C? (A) 0.08% (B) 0.2% (C) 1% (D) 2% (E) 4%

79. 5 Fe2+ + MnO4¯ + 8 H+ <===> 5 Fe3+ + Mn2+ + 4 H2O In a titration experiment based on the equation above, 25.0 milliliters of an acidified Fe2+ solution requires 14.0 milliliters of standard 0.050-molar MnO4¯ solution to reach the equivalence point. The concentration of Fe2+ in the original soluiton is (A) 0.0010 M (B) 0.0056 M (C) 0.028 M (D) 0.090 M (E) 0.14 M

C2H4(g) + 3 O2(g) --> 2 CO2(g) + 2 H2O(g) 61. For the reaction of ethylene represented above, DH is - 1,323 kJ. What is the value of DH if the combustion produced liquid water H2O(l), rather than water vapor H2O(g)? (DH for the phase change H2O(g) --> H2O(l) is -44 kJ mol¯1.) A) -1,235 kJ B) -1,279 kJ C) -1,323 kJ D) -1,367 kJ E) -1,411 kJ

Hydrogen Halide Normal Boiling Point, °C HF +19 HCl - 85 HBr - 67 HI - 35 The liquefied hydrogen halides have the normal boiling points given above. The relatively high boiling point of HF can be correctly explained by which of the followng? (A) HF gas is more ideal. (B) HF is the strongest acid. (C) HF molecules have a smaller dipole moment. (D) HF is much less soluble in water. (E) HF molecules tend to form hydrogen bonds.

Look at 29 for Picture 29. The organic compound represented above is an example of (A) an organic acid (B) an alcohol (C) an ether (D) an aldehyde (E) a ketone

Questions 11-14 refer to the reactions represented below. (A) H2SeO4(aq) + 2 Cl-(aq) + 2 H+(aq) H2SeO3(aq) + Cl2(g) + H2O(1) (B) S8(s) + 8 O2(g) 8 SO2(g) (C) 3 Br2(aq) + 6 OH-(aq) 5 Br-(aq) + BrO3 -(aq) + 3 H2O(l) (D) Ca2+(aq) + SO4 2-(aq) CaSO4(s) (E) PtCl4(s) + 2 Cl-(aq) PtCl6 2-(aq) 11. A precipitation reaction

Questions 3-5 refer to the following molecules. (A) CO2 (B) H20 (C) CH4 (D) C2H4 (E) PH3 3. The molecule with only one double bond

Questions 33-34 Look at Graph for 33 The graph below shows the titration curve that results when 100. mL of 0.0250 M acetic acid is titrated with0.100 M NaOH. 33. Which of the following indicators is the best choice for this titration? Indicator pH Range of Color Change (A) Methyl orange 3.2 - 4.4 (B) Methyl red 4.8 - 6.0 (C) Bromothymol blue 6.1 - 7.6 (D) Phenolphthalein 8.2 - 10.0 (E) Alizarin 11.0 - 12.4

Questions 33-34 Look at Graph for 33 The graph below shows the titration curve that results when 100. mL of 0.0250 M acetic acid is titrated with0.100 M NaOH. 34. What part of the curve corresponds to the optimum buffer action for the acetic acid/acetate ion pair? (A) Point V (B) Point X (C) Point Z (D) Along all of section WY (E) Along all of section YZ

Questions 6-7 refer to the following solid compounds. (A) PbSO4 (B) CuO (C) KMnO4 (D) KCl (E) FeCl3 6. Is purple in aqueous solution

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