Use the following answers for questions 1 - 3

AP Multiple Choice Study and Review Packet18p 1 4. Hydrogen peroxide: Is a good oxidizing agent5. Hydrofluoric acid: Is used to etch glass chemically6. Ammonia: Is used extensively for the production of fertilizers7. Aluminum hydroxide: Has amphoteric properties63. Sulfur, chlorine, nitrogen, and carbon: have oxides that are acid anhydrides. (They make acids in water)64. Solutions of Zn satls are colorless. 11. Zn is utilized as a coating to protect Fe from corrosion (galvanizations)12. As is added to silicon to enhance its properties as a semiconductor13. Pb is Utilized as a shield from sources of radiation1. Ionization energy: The energy required to convert a ground-state atom in the gas phase to a gaseous positive ion 2. Lattice energy: The energy change that occurs in the conversion of an ionic solid to widely separated gaseous ions 3. Free energy: The energy in a chemical or physical change that is available to do useful work 4. Activation energy: The energy required to form the transition state in a chemical reaction 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 (D) 4.5 M 67. A student wishes to prepare 2.00 liters of 0.100-molar KIO3 (molecular weight 214). The proper procedure is to weigh out (B) 42.8 grams of KIO3 and add H2O until the final homogeneous solution has a volume of 2.00 liters68. 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 (B) 0.160 M69. (B) 0.076 is the mole fraction of ethanol, C2H5OH, in an aqueous solution in which the ethanol concentration is 4.6 molal?15. The weight of H2SO4 (molecular weight 98.1) in 50.0 milliliters of a 6.00-molar solution is(C) 29.4 grams26. (C) 260 mL of 11.6-molar HCl must be diluted to obtain 1.0 liter of 3.0-molar HCl?43. (A) CH3OH does NOT behave as an electrolyte when it is dissolved in water?72. (C) 0.24 mole 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? 28. Given that a solution is 5 percent sucrose by mass, what additional information is necessary to calculate the molarity of the solution? II. The density of the solution and III. The molar mass of sucrose

p 2 47. (D) 0.1 M HF has the lowest conductivity? (Weak acid)53. If 87 grams of K2SO4 (molar mass 174 grams) is dissolved in enough water to make 250 milliliters of solution? (E) [K+] 4.0 M, [SO42] 2.0 M 33. A 1.0 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) ? (C) 0.30 mol56. 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)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? C) 0.28 M69. 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)? C) 0.025 M70. 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+]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? B) Adding dilute HCl(aq) solution73. 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 D) 110. mL21. 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? (B) The pressure of the gas23. 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) (B) 46.039. 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? (C) It depends on the relative molecular masses of X, Y, and Z.50. Two flexible containers for gas 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? (E) The average speed of the hydrogen molecules is the same as the average speed of the oxygen molecules. 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

p 3 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? (C) Vapor pressure of the water78. 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) volume85. 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 (C) 7.46 liters16. 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? (C) 0.63 atm24. A sample of 0.010 mole of oxygen gas is confined at 127 C and 0.80 atmosphere. What would be the pressure of this sample at 27 C and the same volume? (C) 0.60 atm30. 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? (B) 733 mm Hg32. 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 (C) 477 C40. 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 (D) 4.48 liters62. As the temperature is raised from 20 C to 40 C, the average kinetic energy of neon atoms changes by a factor of (B) [square root of](313/293)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? (C) 0.201 atm33. 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 (C) C3H637 A sample of 3.0 grams of an ideal gas at 121 C and 1.0 atmosphere pressure has a volume of 1.0 Iiters. Which of the following expressions is correct for the molar mass of the gas? The ideal gas constant, R, is 0.08 (L-atm) / (mole K). (D) [(3.0)(0.08)(400)] / [(1.0)(1.5)]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? (C) XeF440. The system shown below 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 (C) 133 mm Hg

p 4 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? III. The average speed of the molecules (only)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 Gas effuses at approximately one-half that rate? (D) Cl2 (molar mass 71 grams)52. Under which of the following sets of conditions could the most O2(g) be dissolved in H2O(l)? B) PO2 5.0 Temp 20oC23. A hot-air balloon rises. Which of the following is the best explanation for this observation? (E) The air density inside the ballon is less than that of the surrounding air. 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? (C) The average speed of the gas molecules remains th same.53. W(g) + X(g) --> Y(g) + Z(g) Gas W and X react in a closed, rigid vessel to form Gas 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 atm60. NH4NO3(s) --> N2O(g) + 2 H2O(g) A 0.03 mol sample of 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 volume of the flask appears to be missing?]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 Gas remaining in the vessel after some of the gas mixture has effused? A) PHe < PNe < PAr74. Which of the following Gas deviates most from ideal behavior? A) SO247. CH4(g) + 2 O2(g) ---> CO2(g) + 2 H2O(l); H = - 889.1 kJ Hf H2O(l) = - 285.8 kJ / mole Hf CO2(g) = - 393.3 kJ / mole What is the standard heat of formation of methane, Hf CH4(g), as calculated from the data above? (E) 210.0 kJ/mole 48.Which of the following is a graph that describes the pathway of reaction that is endothermic and has high activation energy? [NONE of them!]25. H2(g) + O2(g) ---> H2O(l) H = x 2Na(s) + O2(g) ---> Na2O(s) H = y Na(s) + O2(g) + H2(g) ---> NaOH(s) H = z Based on the information, what is the standard enthalpy change for the following reaction? Na2O(s) + H2O(l) ---> 2 NaOH(s) (D) 2z - x - y58. Which of the following represents the ground state electron configuration for the Mn3+ ion? (A) 1s2 2s22p6 3s23p63d4

p 5 30. The energy diagram for the reaction X + Y ---> Z is shown below. The addition of a catalyst to this reaction would cause a change in which of the indicated energy differences? (D) I and II only (Ea forward and reverse)19. Which of the following best describes the role of the spark from the spark plug in an automobile engine? (C) The spark supplies some of the energy of activation for the combustion reaction.22. 1s2 2s22p6 3s23p3 Atoms of an element, X, have the electronic configuration shown above. The compound most likely formed with magnesium, Mg, is (E) Mg3X2 43. The elements in which of the following have most nearly the same atomic radius? (E) Cr, Mn, Fe, Co 66. Ca, V, Co, Zn, As Gaseous atoms of which of the elements above are paramagnetic? (D) V, Co, and As only70. 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? (E) 5, 0, 0, 1/2 1. Forms monatomic ions with 2 charge in solutions: (B) S2. Forms a compound having the formula KXO4: (E) Mn 3. Forms oxides that are common air pollutants and that yield acidic solution in water: (B) S1. What is the most electronegative element of the above? (A) O2. Which element exhibits the greatest number of different oxidation states? (E) N 3. Which of the elements above has the smallest ionic radius for its most commonly found ion? (A) O33. Which of the following conclusions can be drawn from J. J. Thomson's cathode ray experiments? (A) Atoms contain electrons.For questions 4 - 7.(A) 1s2 2s22p5 3s23p5(D) 1s2 2s22p6 3s23p63d54. An impossible electronic configuration (C) 1s2 2s22p62d10 3s23p65. The ground-state configuration for the atoms of a transition element (E) 1s2 2s22p6 3s23p63d3 4s2 6. The ground-state configuration of a negative ion of a halogen (B) 1s2 2s22p6 3s23p67. The ground-state configuration of a common ion of an alkaline earth element (B) 1s2 2s22p6 3s23p61. Can be used to predict that a gaseous carbon atom in its ground state is paramagnetic (C) Hund's rule (principle of maximum multiplicity)2. Explains the experimental phenomenon of electron diffraction (E) Wave nature of matter 3. Indicates that an atomic orbital can hold no more than two electrons (B) Pauli exclusion principle4. Predicts that it is impossible to determine simultaneously the exact position and the exact velocity of an electron (A) Heisenberg uncertainty principle27. 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) ? (C) 4, 1, 1, 1/254. All of the following statements concerning the characteristics of the halogens are true EXCEPT: (D) Iodine liberates free bromine from a solution of bromide ion.

p 6 Question 5-8 refer to atoms with the occupied atomic orbitals shown. 5. Represents an atom that is chemically unreactive: D6. Represents an atom in an excited state: A7. Represents an atom that has four valence electrons: C8. Represents an atom of a transition metal: E50. In the periodic table, as the atomic number increases from 11 to 17, what happens to the atomic radius? (D) It decreases only.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? (E) The positive charge of an atom is concentrated in a small region. 37. First, 580; Second, 1815; Third, 2740; Fourth, 11600; Five, 14800 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 (C) AI41. Which of the following molecules has the shortest bond length? (A) N251. Pi bonding occurs in each of the following species EXCEPT (E) CH4 60. Which of the following has a zero dipole moment? (E) PF5 8. Solid ethyl alcohol, C2H5OH: (C) A molecular solid with hydrogen bonding9. Silicon dioxide, SiO2: (A) A network solid with covalent bonding80. For which of the following molecules are resonance structures necessary to describe the bonding satisfactorily? (B) SO2 18. HF: +19C; HCl: - 85C; HBr: - 67C; HI: - 35C The liquefied hydrogen halides have the normal boiling points given below. The relatively high boiling point of HF can be correctly explained by which of the followng? (E) HF molecules tend to form hydrogen bonds. 11. Is used to explain why iodine molecules are held together in the solid state (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 (A) hydrogen bonding13. Is used to explain the fact that the four bonds in methane are equivalent (B) hybridization14. Is used to explain the fact that the carbon-to-carbon bonds in benzene, C6H6, are identical (D) resonance17. The Lewis dot structure of which of the following molecules shows only one unshared pair of valence electron? (C) NH331. The structural isomers C2H5OH and CH3OCH3 would be expected to have the same values for which of the following? (A) Gaseous densities at the same temperature and pressure42. The SbCl5 molecule has trigonal bipyramid structure. Therefore, the hybridization of Sb orbitals should be (D) dsp347. CCl4, CO2, PCl3, PCl5, SF6 Which of the following does not describe any of the molecules above? (C) Square planar

p7 59. Which of the following compounds is ionic and contains both sigma and pi covalent bonds? (E) NaCN 15. In a molecule in which the central atom exhibits sp3d2 hybrid orbitals, the electron pairs are directed toward the corners of (C) a trigonal bipyramid32. 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 (D) hydrogen bonding34.X = CH3-CH2-CH2-CH2-CH3Y = CH3-CH2-CH2-CH2-OHZ = HO-CH2-CH2-CH2-OHBased 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? (E) X < Y < Z 57. Molecules that have planar configurations include which of the following? I. BCl3 only62. The electron-dot structure (Lewis structure) for which of the following molecules would have two unshared pairs of electrons on the central atom? (A) H2S68. Which of the following molecules has a dipole moment of zero? (A) C6H6 (benzene)8. Has the largest bond-dissociation energy (C) N29. Has a bond order of 2 (D) O210. Contains 1 sigma (s) and 2 pi (p) bonds (C) N260. I---I 150, Cl---Cl 240, I---Cl 210I2(g) + 3 Cl2(g) ---> 2 ICl3(g)According to the data in the table, what is the value of H for the reaction represented above? (B) - 390 kJ28. The melting point of MgO is higher than that of NaF. Explanations for this observation include: I. Mg2+ is more positively charged than Na+ & II. O2 is more negatively charged than F32. Types of hybridization exhibited by the C atoms in propene, CH3CHCH2, include which of the following? II. sp2 & III. sp3 40. Of the following molecules, which has the largest dipole moment? (D) HF58. On a mountaintop, it is observed that water boils at 90C, not at 100C as at sea level. This phenomenon occurs because on the mountaintop the C) equilibrium water vapor pressure equals the atmospheric pressure at a lower temperature68. In which of the following processes are covalent bonds broken? D) C(diamond) --> C(g)19. Which of the following represents a pair of isotopes? (D) 1: Z = 7, A = 13 & 2: Z = 7, A = 14

p8 24. The formula for potassium hexacyanoferrate(II) is (A) K4[Fe(CN)6]44. What number of moles of O2 is needed to produce 14.2 grams of P4O10 from P? (Molecular weight P4O10 = 284) (D) 0.250 mole73. 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? (D) C4H623. How many grams of calcium nitrate, Ca(NO3)2, contains 24 grams of oxygen atoms? (E) 41 grams 25. The simplest formula for an oxide of nitrogen that is 36.8 percent nitrogen by weight is (D) N2O339. 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 (B) Na2CO3 . 7 H2O45. 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 (D) 7.8 grams per mL19. In which of the following compounds is the mass ratio of chromium to oxygen closest to 1.6 to 1.0? (B) CrO242.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 (D) 2.00 g/cm347. 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? (C) HfCl349. Which of the following techniques is most appropriate for the recovery of solid KNO3 from an aqueous solution of KNO3? (E) Evaporation to dryness 27. The critical temperature of a substance is the (C) temperature at which the solid, liquid, and vapor phases are all in equilibrium54. 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.

p9 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.49. The normal boiling point of the substanced represented by the phase diagram above is (C) 140 C 50. The phase diagram above provides sufficient information for determining the (B) conditions necessary for sublimation51. For the substance represented in the diagram, which of the phases is most dense and which is least dense at - 15 C. (A) Solid Gas 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? III. Moving the container and liquid to a higher altitude5. If the temperature increases from 10 C to 60 C at a constant pressure of 0.4 atmosphcre, which of the processes occurs? (A) Sublimation6. If the temperature decreases from 110 C to 40 C at a constant pressure of 1.1 atmospheres, which of the processes occurs? (B) Condensation7. If the pressure increases from 0.5 to 1.5 atmospheres at a constant temperature of 50 C, which of the processes occurs? (B) Condensation13. Cesium chloride, CsCl(s) (A) Lattice of positive and negative ions held together by electrostatic forces.15. Carbon dioxide, CO2(s) (D) Strong multiple covalent bonds (including bonds.) with weak intermolecular forces16. Methane, CH4(s) (C) Strong single covalent bonds with weak intermolecular forces.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 (C) all points on the curve between Q and S39. 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? (C) CAssume 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. (B) Cr2O7211. The solution gives no apparent reaction with dilute hydrochloric acid. (A) CO3212. No odor can be detected when a sample of the solution is added drop by drop to a warm solution of sodium hydroxide. (C) NH4+13. No precipitate is formed when a dilute solution of H2SO4 is added to a sample of the solution. (D) Ba2+

p10 37. The molality of the glucose in a 1.0-molar glucose solution can be obtained by using which of the following? (E) Density of the solution 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) 0.2384. Which of the following aqueous solutions has the highest boiling point? (A) 0.10 M potassium sulfate, K2SO4 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? (C) Mass of solute and mass of solvent28. Which of the following is probably true for a solid solute with a highly endothermic heat of solution when dissolved in water? (D) The solid is more soluble at higher temperatures.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? (E) 1.42 m 14. Which of the following is lower for a 1.0-molar aqueous solution of any solute than it is for pure water? (C) Freezing point44. Which of the following solutions has the lowest freezing point? (E) 0.20 m MgCl2 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? (C) The molality of the solution remains unchanged.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? (D) Measurement of the total volume of the solution75. Which of the following pairs of liquids forms the solution that is most ideal (most closely follows Raoult's law)? D) C6H14(l) and C8H18(l)For questions 25-26 H3AsO4 + 3I + 2 H3O+ ---> H3AsO3 + I3 + H2OThe 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+]25. What is the order of the reaction with respect to I? (A) 1 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.57. rate = k[X] For the reaction whose rate law is given above, a plot of which of the following is a straight line? (B) log [X] versus time

p11 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 (C) substance B is not involved in the rate-determining step of the mechanism, but is involved in subsequent steps82. 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? Step 1) N2H2O2 N2HO2 + H+ fast equilibrium; Step 2) N2HO2 ---> N2O + OH (slow); Step 3) H+ + OH ---> H2O (fast). (D) Rate = (k [N2H2O2]) / [N2HO2]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 (B) 57 minutes58. (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.) (C) Both the reaction rate and k remain the same.17. Relatively slow rates of chemical reaction are associated with which of the following? (D) Strong bonds in reactant molecules23. The proposed steps for a catalyzed reaction between Ce4+ and Tl+ are represented above. The products of the overall catalyzed reaction are Step 1: Ce4+ + Mn2+ ---> Ce3+ + Mn3+; Step 2: Ce4+ + Mn3+ ---> Ce3+ + Mn4+; Step 3: Mn4+ + Tl+ ---> Tl3+ + Mn2+. (B) Ce3+ and Tl3+36. CuO(s) + H2(g) Cu(s) + H2O(g); H = - 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 (C) decreasing the temperature63. 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? B) It is first order in [X].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? (B) rate = k[NO] [O2]257. For the reaction A(g) B(g) + C(g), the equilibrium constant, Kp, is 2 x 104 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 atm, PB = 0.5 atm, and PC = 1 atm, At the instant of mixing, which of the following is true for the reaction as written? (A) G < 0

p12 76. HgO(s) + 4 I + H2O HgI42 + 2 OH; H < 0 Consider the equilibrium above. Which of the following changes will increase the concentration of HgI42?(B) Adding 6 M HNO329. 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? (E) NO(g) + O3(g) NO2(g) + O2(g) 48. PCl3(g) + Cl2(g) PCl5(g) + energySome 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 & III. Adding a mole of He gas at constant volume51. 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? II. [O2] must be greater than [HCl] & III. [Cl2] must equal [H2O].73. 2 SO2(g) + O2(g) 2 SO3(g) When 0.40 mole of SO3 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 S03. Based on these results, the expression for the equilibrium constant, Kc, of the reaction is (A) (0.30)2 / [(0.45)(0.10)2] 54. 2NO(g) + O2(g) 2 NO2(g) H < 0 Which of the following changes alone would cause a decrease in the value of Keq for the reaction represented above? B) Increasing the temperature33. The pH of 0.1-molar ammonia is approximately (D) 11 48. Which of the following ions is the strongest Lewis acid? (E) Al3+ 49. Each of the following can act as both a Brnsted acid and a Brnsted base EXCEPT (C) NH4+53. Which, if any, of the following species is in the greatest concentration in a 0.100-molar solution of H2SO4 in water? (B) H3O+ ions71. Which of the following reactions does NOT proceed significantly to the right in aqueous solutions? (E) H2O + HSO4 ---> H2SO4 + OH 75. If the acid dissociation constant, Ka, for an acid HA is 8 x 104 at 25 C, what percent of the acid is dissociated in a 0.50-molar solution of HA at 25 C? (A) 0.08%34. All of the following species can function as Brnsted-Lowry bases in solution EXCEPT (D) NH4+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? (E) The acid strength increases.

p13 54. Which of the following is the correct equilibrium expression for the hydrolysis of CO32? (B) K = ( [HCO3] [OH] ) / [CO32]55. H2PO4 + HBO32 HPO42 + H2BO3The 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? (A) Acids: H2PO4- > H2BO3- & Bases: HBO32- > HPO42-56. A 0.20-molar solution of a weak monoprotic acid, HA, has a pH of 3.00. The ionization constant of this acid is (C) 5.0 x 10622. HSO4 + H2O H3O+ + SO42 In the equilibrium represented above, the species that act as bases include which of the following? II. H2O & III. SO4231. R. H2C2O4 + 2 H2O 2 H3O+ + C2O42 Oxalic acid, H2C2O4, is a diprotic acid with K1 = 5 x 102 and K2 = 5 x 105. Which of the following is equal to the equilibrium constant for the reaction represented above? (C) 2.5 x 10650. Which of the following acids can be oxidized to form a stronger acid? (E) H2SO3 61. A 1-molar solution of which of the following salts has the highest pH ? (B) Na2CO366. What is the pH of a 1.0 x 102-molar solution of HCN? (Ka = 4.0 x 1010.) (E) 4 38. A molecule or an ion is classified as a Lewis acid if it (B) accepts a pair of electrons to form a bond45. What is the H+(aq) concentration in 0.05 M HCN (aq) ? (The Ka for HCN is 5.0 x 1010) (E) 5.0 x 104 64. The net ionic equation for the reaction that occurs during the titration of nitrous aicd with sodium hydroxide is (C) H+ + OH ---> H2O74. 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 106 molar? (Ksp of PbF2 at 25 C = 4.0 x 108) (D) 0.20 mole(E) 0.40 mole 81. What is the net ionic equation for the reaction that occurs when aqueous copper(II) sulfate is added to excess 6-molar ammonia? (D) Cu2+ + 4 NH3 --> Cu(NH3)42+63. On the basis of the information below, a buffer with a pH = 9 can best be made by using (D) H2PO4 + HPO4219. 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? (C) The graph of pH versus volume of base added rises gradually at first and then much more rapidly.

p14 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 (B) the solution being titrated undergoes a large pH change near the end point of the titration52. 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 (B) Ag(NH4)4+ + Cl AgCl(s) + 4NH4+65. The solubility of CuI is 2 x 106 molar. What is the solubility product constant, Ksp, for CuI? (C) 4 x 101266. MnS(s) + 2 H+ Mn2+ + H2S(g) At 25 C the solubility product constant, Ksp, for MnS in 5 x 1015 and the acid dissociation constants K1 and K2 for H2S are 1 x 107 and 1 x 1013, respectively. What is the equilibrium constant for the reaction represented by the equation above at 25 C? (D) 5 x 1015 / 1 x 102069. 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) CaCO374. 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) H2PO48. A solution prepared to be initially 1 M in NaCl and 1 M in HCl. (A) a solution with a pH less than 7 that is not a buffer solution9. A solution prepared to be initially 1 M in Na2CO3 and 1 M in CH3COONa (D) a solution with a pH greater than 7 that is not a buffer solution10. A solution prepared to be initially 0.5 M in CH3COOH and 1 M in CH3COONa (B) a buffer solution with a pH between 4 and 716. Commercial vinegar was titrated with NaOH solution to determine the content of acetic acid, HC2H3O2. For 20.0 milliliters of the vinegar, 32.0 milliliters of 0.500-molar NaOH solution was required. What was the concentration of acetic acid in the vinegar if no other acid was present? (B) 0.800 M65. Barium sulfate is LEAST soluble in a 0.01-molar solution of which of the following? (A) Al2(SO4)374. A solution of calcium hypochlorite, a common additive to swimming-pool water, is (A) basic because of the hydrolysis of the OCl ion62. HC2H3O2(aq) + CN(aq) HCN(aq) + C2H3O2(aq) 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)65. Which of the following compounds is NOT appreciably soluble in water but is soluble in dilute hydrochloric acid? A) Mg(OH)2(s)67. What is the molar solubility in water of Ag2CrO4? (The Ksp for Ag2CrO4 is 8 x 1012.) D) (4 x 1012 M)1/3

p159. The solution with the lowest pH (C) HCl and NaCl10. The most nearly neutral solution (E) NH3 and HC2H3O2 (acetic acid) 11. A buffer at a pH > 8 (A) NH3 and NH4Cl56. 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 Entrop. when the system reaches equilibrium? (C) Energy Remains constant Entrop. Increases 41. Which of the following reactions has the largest positive value of S per mole of Cl2 (D) 2 NH4Cl(s) ---> N2(g) + 4 H2(g) + Cl2(g)53. Which of the following must be true for a reaction that proceeds spontaneously from initial standard state conditions? (C) G < 0 and Keq > 170. 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? (E) H > 0, S > 0, V < 0 35. For which of the following processes would S have a negative value? II. Mg2+ + 2 OH ---> Mg(OH)2(s) & III. H2(g) + C2H4(g) ---> 3 C2H6(g)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? (B) G, H, and S are all negative.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 S for the dissolving process? A) H Postive, S Positive 22. Of the following reaction, which involves the largest decrease in Entrop.? (E) 4 La + 3 O2 ---> 2 La2O3 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 (B) 0.020 mole14. A 50-milliliter sample of a 2-molar Cd(NO3)2 solution is added to the left beaker. (B) Voltage decreases15. The silver electrode is made larger. (D) No change in voltage occures.16. The salt bridge is replaced by a platinum wire (C) Voltage becomes zero and remains at zero.17. Current is allowed to flow for 5 minutes (B) Voltage decreases29. 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, G, for this reaction? (A) E is positive and G is negative.

p16 83. NH3(g) + 2 CH4(g) + 5/2 O2(g) H2NCH2COOH(s) + 3 H2O(l) At constant temperature, H, the change in enthalpy for the reaction above is approximately equal to (E) E + (11/2)RT [Dont need to know]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? (D) Anode: Impure Cu sample; Cathode: Pure Cu 60. 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) (D) 1.3 x 10+736. 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? (C) The Zn2+ solution was more concentrated than the Cu2+ solution.63. Which of the following expressions is correct for the maxirnum mass of copper, in grams, that cou1d be plated out by electrolyzing aqueous CuCl2 for 16 hours at a constant current of 3.0 amperes? (B) [(16)(3,600)(3.0)(63.55)] / [(96,500)(2)]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? (C) A brown color will appear in the solution near the negative electrode.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 V30. 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 (C) 82-Pb-20634. AlF63 + 3 e ---> Al + 6F Which of the following occurs in the reaction? (A) AlF 63 is reduced at the cathode.35. AlF63 + 3 e ---> Al + 6F 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? 38. The radioactive decay of 6-C-14 to 7-N-14 occurs by the process of (A) beta particle emission 18. For the types of radiation given, which of the following is the correct order of increasing ability to penetrate a piece of lead? (B) Alpha particles < beta particles < gamma rays

p 17 38. 98-Cf-251 -> 2n + 54-Xe-131 + __What is the missing product in the nuclear reaction represented above? (B) 44-Ru-11868. 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? (E) 160 grams 21. Correct statements about alpha particles include which of the following? I. They have a mass number of 4 and a charge of +2. & III. They are helium nuclei.72. The nuclide 245Cm is radioactive and decays by the loss of one beta ([beta]) particle. The product nuclide is (A) 245Pu48. If 87.5 percent of a sample of pure 131I decays in 24 days, what is the half-life of 131I? (B) 8 days77. Which of the following compounds exhibits optical isomerism? 43. Which of the following pairs of compounds are isomers? (A) 29. The organic compound represented below is an example of (E) a ketone 40. The geometry of the SO3 molecule is best described as (A) trigonal planar31. A 0.1-molar solution of which of the following ions is orange? (A) Fe(H2O)42+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 (D) I62. 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. (D) The pipette was not rinsed with the HCI solution.36. Appropriate laboratory procedures include which of the following? 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 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

p 1838. 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.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? (D) Scandium reacts with nitric acid to form a brown gas.46. Which of the following solids dissolves in water to form a colorless solution? (E) ZnCl2 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 (B) baking soda, NaHCO367. 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 (E) solubilities 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 & III. Swirling the solution frequently during the titration70. To determine the molar mass of a solid monoprotic 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 (only)21. When a solution of sodium chloride is vaporized in a flame, the color of the flame is (B) yellow24. The safest and most effective emergency procedure to treat an acid splash on skin is to do which of the following immediately? (D) Flush the affected area with water and then with a dilute NaHCO3 solution27. Appropriate uses of a visible-light spectrophtometer include which of the following? I. Determining the concentration of a solution of Cu(NO3)2 (only)46. Which of the following occurs when excess concentrated NH3(aq) is mixed thoroughly with 0.1 M Cu(NO3)2(aq)? (E) The pH of the solution decreases. 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+? (E) 10

p19 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? B) The dehydrated sample absorbed moisture after heating.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 + CO2(g)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 ? (E) 5:1 42. Metallic copper is heated strongly with concentrated sulfuric acid. The products of this reaction are (B) Cu2+, SO2(g), and H2O45. The alkenes are compounds of carbon and hydrogen with the Genl 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 mole61. When a solution of potassium dichromate is added to an acidified solution of iron(II) sulfate, the products of the reaction are (D) Fe3+, Cr3+, and H2O65. Which of the following species CANNOT function as an oxidizing agent? (E) I 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 (E) 0.14 M 20. 6 I + 2 MnO4 + 4 H2O(l) ---> 3 I2(s) + 2 MnO2(s) + OHWhich of the following statements regarding the reaction represented by the equation above is correct? (E) The oxidation number of iodine changes from -1 to 0. 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 (D) 737. __ 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? (E) 9/2 moles 44. The metal calcium reacts with molecular hydrogen to form a compound. All of the following statements concerning this compound are true EXCEPT: (E) When added to water, it forms an acidic solution.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? (B) Na2S67. 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 (B) 8.10 x 103 mole18. 2 H2O + 4 MnO4 + 3 ClO2 ---> 4 MnO2 + 3 ClO4 + 4 OH Which species acts as an oxidizing agent in the reaction represented above? (E) MnO4

p20 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 (D) 629. When an aqueous solution of NaOH is added to an aqueous solution of potassium dichromate, K2Cr2O7 the dichromate ion is converted to (A) CrO4255. What volume of 0.150-molar HCl is required to neutralize 25.0 milliliters of 0.120-molar Ba(OH)2? (C) 40.0 mL56. It is suggested that SO2 (molar mass 64 grams), which contributes to acid rain, could be removed from a stream of waste Gas by bubbling the Gas 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? (C) 16 kg59. R. When a 1.25-gram sample of limestone was dissolved in acid, 0.44 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? (D) 80%71 ... Fe(OH)2 + ... O2 + ... H2O ---> ... Fe(OH)3If 1 mole of O2 oxidizes Fe(OH)2 according to the reaction represented above, how many moles of Fe(OH)3 can be formed? (C) 417. Is a gas in its standard state at 298 K: (E) Fluorine 18. Reacts with water to form a strong base: (A) Lithium20. What mass of Au is produced when 0.0500 mol of Au2S3 is reduced completely with excess H2? (B) 19.7 g26. . . .C10H12O4S(s) + . . O2(g) ---> . . . CO2(g) + . . . SO2(g) + . . . H2O(g) When the equation above is balanced and all coefficients are reduced to their lowest whole-number terms, the coefficient for O2(g) is? (C) 1242. . . . Li3N(s) + . . . H2O(l) ---> . . . Li+ (aq) + . . . OH(aq) + . . . NH3(g) When the equation above is balanced and all coefficients reduced to lowest whole number terms, the coefficient for OH(aq) is (E) 6 55. 10 HI + 2 KMnO4 + 3 H2SO4 --> 5 I2 + 2 MnSO4 + K2SO4 + 8 H2O 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? D) 5.0