Scholarship Chemistry 2nd Semesrer Examination 2005/2006Scholarship Chemistry 2nd Semester Examination practiceMultiple ChoiceIdentify the letter of the choice that best completes the statement or answers the question.____1.What type of ions have names ending in -ide?a.only cationsc.only metal ionsb.only anionsd.only gaseous ions____2.What is the correct name for the N ion?a.nitrate ionc.nitride ionb.nitrogen iond.nitrite ion____3.When naming a transition metal ion that can have more than one common ionic charge, the numerical value of the charge is indicated by a ____.a.prefixc.Roman numeral following the nameb.suffixd.superscript after the name____4.In which of the following are the symbol and name for the ion given correctly?a.Fe: ferrous ion; Fe: ferric ionb.Sn: stannic ion; Sn: stannous ionc.Co: cobalt(II) ion; Co: cobaltous iond.Pb: lead ion; Pb: lead(IV) ion____5.Which of the following is NOT a cation?a.iron(III) ionc.Cab.sulfated.mercurous ion____6.In which of the following are the symbol and name for the ion given correctly?a.NH: ammonia; H: hydridec.OH: hydroxide; O: oxideb.CHO: acetate; CO : oxalited.PO: phosphate; PO: phosphite____7.An -ate or -ite at the end of a compound name usually indicates that the compound contains ____.a.fewer electrons than protonsc.only two elementsb.neutral moleculesd.a polyatomic anion____8.Which of the following compounds contains the Mn ion?a.MnSc.MnOb.MnBrd.MnO____9.How are chemical formulas of binary ionic compounds generally written?a.cation on left, anion on rightb.anion on left, cation on rightc.Roman numeral first, then anion, then cationd.subscripts first, then ions____10.Which of the following formulas represents an ionic compound?a.CSc.NOb.BaId.PCl____11.Which of the following compounds contains the lead(II) ion?a.PbOc.Pb2Ob.PbCl4d.Pb2S____12.Which set of chemical name and chemical formula for the same compound is correct?a.ammonium sulfite, (NH)Sc.lithium carbonate, LiCOb.iron(III) phosphate, FePOd.magnesium dichromate, MgCrO____13.Molecular compounds are usually ____.a.composed of two or more transition elementsb.composed of positive and negative ionsc.composed of two or more nonmetallic elementsd.exceptions to the law of definite proportions____14.When naming acids, the prefix hydro- is used when the name of the acid anion ends in ____.a.-idec.-ateb.-ited.-ic____15.When the name of an anion that is part of an acid ends in -ite, the acid name includes the suffix ____.a.-ousc.-ateb.-icd.-ite____16.In any chemical compound, the elements are always combined in the same proportion by ____.a.chargec.volumeb.massd.density____17.Which of the following pairs of substances best illustrates the law of multiple proportions?a.H and Oc.CaCl and CaBrb.PO and PHd.NO and NO____18.What SI unit is used to measure the number of representative particles in a substance?a.kilogramc.kelvinb.ampered.mole____19.Avogadro's number of representative particles is equal to one ____.a.kilogramc.kelvinb.gramd.mole____20.How many moles of silver atoms are in 1.8 10 atoms of silver?a.3.0 10c.3.0 10b.3.3 10d.1.1 10____21.How many molecules are in 2.10 mol CO?a.2.53 10 moleculesc.3.49 10 moleculesb.3.79 10 moleculesd.1.26 10 molecules____22.The atomic masses of any two elements contain the same number of ____.a.atomsc.ionsb.gramsd.milliliters____23.What is true about the molar mass of chlorine gas?a.The molar mass is 35.5 g.b.The molar mass is 71.0 g.c.The molar mass is equal to the mass of one mole of chlorine atoms.d.none of the above____24.The molar mass of CH and the molar mass of CaCO contain approximately the same number of ____.a.carbon atomsc.cationsb.anionsd.grams____25.How many moles of CaBr are in 5.0 grams of CaBr?a.2.5 10 molc.4.0 10 molb.4.2 10 mold.1.0 10 mol____26.What is the number of moles in 500 L of He gas at STP?a.0.05 molc.22 molb.0.2 mold.90 mol____27.What is the percent composition of chromium in BaCrO?a.4.87%c.20.5%b.9.47%d.25.2%____28.The lowest whole-number ratio of the elements in a compound is called the ____.a.empirical formulac.binary formulab.molecular formulad.representative formula____29.Which of the following is NOT an empirical formula?a.CNHc.BeCrOb.CHOd.SbS____30.What is the empirical formula of a substance that is 53.5% C, 15.5% H, and 31.1% N by weight?a.CHNc.CHNb.CHNd.CHN____31.Which of the following sets of empirical formula, molar mass, and molecular formula is correct?a.CH, 78 g, CHc.CaO, 56 g, CaOb.CHN, 90 g, CHNd.CHO, 120 g, CHO____32.What does the symbol in a chemical equation mean?a.Heat is supplied to the reaction.c.yieldsb.A catalyst is needed.d.precipitate____33.A skeleton equation does NOT show which of the following?a.the correct formulas of the reactants and productsb.the reactants on the left, the products on the rightc.an arrow connecting the reactants to the productsd.the relative amounts of reactants and products____34.In the chemical equation HO(aq) HO(l) O(g), the is a ____.a.catalystc.productb.solidd.reactant____35.Which of the following is the correct skeleton equation for the reaction that takes place when solid phosphorus combines with oxygen gas to form diphosphorus pentoxide?a.P(s) O(g) PO(g)c.P(s) O2(g) PO(s)b.P(s) O(g) PO(g)d.PO(s) P(s) O(g)____36.What are the coefficients that will balance the skeleton equation below?AlCl + NaOH Al(OH) NaCla.1, 3, 1, 3c.1, 1, 1, 3b.3, 1, 3, 1d.1, 3, 3, 1____37.Which of the following statements is NOT true about what happens in all chemical reactions?a.The ways in which atoms are joined together are changed.b.New atoms are formed as products.c.The starting substances are called reactants.d.The bonds of the reactants are broken and new bonds of the products are formed.____38.What are the missing coefficients for the skeleton equation below?Cr(s) Fe(NO)(aq) Fe(s) Cr(NO)(aq)a.4, 6, 6, 2c.2, 3, 3, 2b.2, 3, 2, 3d.1, 3, 3, 1____39.In order to predict whether or not a single-replacement reaction takes place, you need to consult a chart that shows the ____.a.periodic tableb.activity series of metalsc.common polyatomic ionsd.ionic charges of representative elements____40.In order for the reaction 2Al 6HCl 2AlCl 3H to occur, which of the following must be true?a.Al must be above Cl on the activity series.b.Al must be above H on the activity series.c.Heat must be supplied for the reaction.d.A precipitate must be formed.____41.What are the correct formulas and coefficients for the products of the following double-replacement reaction? RbOH HPO a.Rb(PO) HOc.RbPO 3HOb.RbPO 2HOd.HRb POOH____42.A double-replacement reaction takes place when aqueous cobalt(III) chloride reacts with aqueous lithium hydroxide. One of the products of this reaction is ____.a.Co(OH)c.LiCob.Co(OH)d.LiCl____43.The first step in most stoichiometry problems is to ____.a.add the coefficients of the reagentsc.convert given quantities to volumesb.convert given quantities to molesd.convert given quantities to masses____44.Which of the following is true about the total number of reactants and the total number of products in the reaction shown below?CH(l) + 8O(g) 5CO(g) + 6HO(g)a.9 moles of reactants chemically change into 11 moles of product.b.9 grams of reactants chemically change into 11 grams of product.c.9 liters of reactants chemically change into 11 liters of product.d.9 atoms of reactants chemically change into 11 atoms of product.____45.How many moles of aluminum are needed to react completely with 1.2 mol of FeO? 2Al(s) + 3FeO(s) 3Fe(s) + AlO(s)a.1.2 molc.1.6 molb.0.8 mold.2.4 mol____46.How many moles of glucose, CHO, can be "burned" biologically when 10.0 mol of oxygen is available? CHO(s) + 6O(g) 6CO(g) + 6HO(l)a.0.938 molc.53.3 molb.1.67 mold.60.0 mol____47.At STP, how many liters of oxygen are required to react completely with 3.6 liters of hydrogen to form water? 2H(g) + O(g) 2HO(g)a.1.8 Lc.2.0 Lb.3.6 Ld.2.4 L____48.The equation below shows the decomposition of lead nitrate. How many grams of oxygen are produced when 11.5 g NO is formed?a.1.00 gc.2.88 gb.2.00 gd.32.0 g____49.Which of the following statements is true about the following reaction?3NaHCO(aq) + CHO(aq) 3CO(g) + 3HO(s) +NaCHO(aq)a.22.4 L of CO(g) are produced for every liter of CHO(aq) reacted.b.1 mole of water is produced for every mole of carbon dioxide produced.c.6.02 10 molecules of NaCHO(aq) are produced for every mole of NaHCO(aq) used.d.54 g of water are produced for every mole of NaHCO(aq) produced.____50.Which of the following is NOT true about limiting and excess reagents?a.The amount of product obtained is determined by the limiting reagent.b.A balanced equation is necessary to determine which reactant is the limiting reagent.c.Some of the excess reagent is left over after the reaction is complete.d.The reactant that has the smallest given mass is the limiting reagent.____51.Identify the limiting reagent and the volume of CO formed when 11 L CS reacts with 18 L O to produce CO gas and SO gas at STP.CS(g) + 3O(g) CO(g) + 2SO(g)a.CS; 5.5 L COc.CS; 11 L COb.O; 6.0 L COd.O; 27 L CO____52.Which statement is true if 12 mol CO and 12 mol FeO are allowed to react?3CO(g) + FeO(s) 2Fe(s) + 3CO(g)a.The limiting reagent is CO and 8.0 mol Fe will be formed.b.The limiting reagent is CO and 3.0 mol CO will be formed.c.The limiting reagent is FeO and 24 mol Fe will be formed.d.The limiting reagent is FeO and 36 mol CO will be formed.____53.Which of the following is NOT true about "yield"?a.The value of the actual yield must be given in order for the percent yield to be calculated.b.The percent yield is the ratio of the actual yield to the theoretical yield.c.The actual yield may be different from the theoretical yield because reactions do not always go to completion.d.The actual yield may be different from the theoretical yield because insufficient limiting reagent was used.____54.In a particular reaction between copper metal and silver nitrate, 12.7 g Cu produced 38.1 g Ag. What is the percent yield of silver in this reaction?Cu + 2AgNO Cu(NO) + 2Aga.56.7%c.88.2%b.77.3%d.176%____55.According to the kinetic theory, collisions between molecules in a gas ____.a.are perfectly elasticc.never occurb.are inelasticd.cause a loss of total kinetic energy____56.Which of the following statements is NOT true, according to the kinetic theory?a.There is no attraction between particles of a gas.b.Only particles of matter in the gaseous state are in constant motion.c.The particles of a gas collide with each other and with other objects.d.All of the statements are true.____57.What is the SI unit of pressure?a.candelac.pascalb.moled.newton____58.What is one standard atmosphere of pressure in kilopascals?a.0 kPac.101.3 kPab.760 kPad.1 kPa____59.How does the atmospheric pressure at altitudes below sea level compare with atmospheric pressure at sea level?a.The atmospheric pressure below sea level is higher.b.The atmospheric pressure below sea level is lower.c.The pressures are the same.d.Differences in pressures cannot be determined.____60.What happens to the average kinetic energy of the particles in a sample of matter as the temperature of the sample is increased?a.The average kinetic energy decreases.b.The average kinetic energy increases.c.The average kinetic energy does not change.d.The change in average kinetic energy cannot be determined.____61.With which temperature scale is temperature directly proportional to average kinetic energy?a.Celsiusc.Kelvinb.Fahrenheitd.centigrade____62.Consider an iron cube and an aluminum cube. If the two cubes were at the same temperature, how would the average kinetic energy of the particles in iron compare with the average kinetic energy of the particles in aluminum?a.The average kinetic energy of the iron particles would be greater.b.The average kinetic energy of the aluminum particles would be greater.c.There would be no difference in the average kinetic energies.d.No determination can be made based on the information given.____63.What is the key difference between a liquid and a gas?a.intermolecular attractionsc.average kinetic energyb.the ability to flowd.the motion of their particles____64.Why does a liquid's rate of evaporation increase when the liquid is heated?a.More molecules have enough energy to overcome the attractive forces holding them in the liquid.b.The average kinetic energy of the liquid decreases.c.The surface area of the liquid is reduced.d.The potential energy of the liquid increases.____65.If a liquid is sealed in a container and kept at constant temperature, how does its vapor pressure change over time?a.It continues to steadily increase.b.It increases at first, then remains constant.c.It increases at first, then decreases.d.It continues to steadily decrease.____66.When the vapor pressure of a liquid is equal to the atmospheric pressure, the liquid ____.a.has no observable changes.c.evaporates.b.boils vigorously.d.begins to boil.____67.What is the pressure when a liquid is boiling at its normal boiling point?a.0 kPac.202 kPab.101.3 kPad.505 kPa____68.When the external pressure is 505 kPa, what is the vapor pressure of water at its boiling point?a.0 kPac.505 kPab.101.3 kPad.1010 kPa____69.The normal boiling point of chloroform, which has a higher vapor pressure than water at 100C, is ____.a.higher than the normal boiling point of waterb.lower than the normal boiling point of waterc.the same as the normal boiling point of waterd.unable to be measured____70.The direct change of a substance from a solid to a gas is called ____.a.evaporationc.condensationb.sublimationd.solidification____71.How are conditions of pressure and temperature, at which two phases coexist in equilibrium, shown on a phase diagram?a.by a line separating the phasesb.by the endpoints of the line segment separating the phasesc.by the planar regions between lines in the diagramd.by a triple point on the diagram____72.Why is a gas easier to compress than a liquid or a solid?a.Its volume increases more under pressure than an equal volume of liquid does.b.Its volume increases more under pressure than an equal volume of solid does.c.The space between gas particles is much less than the space between liquid or solid particles.d.The volume of a gass particles is small compared to the overall volume of the gas.____73.Why does the pressure inside a container of gas increase if more gas is added to the container?a.There is an increase in the number of collisions between particles and the walls of the container.b.There is an increase in the temperature of the gas.c.There is a decrease in the volume of the gas.d.There is an increase in the force of the collisions between the particles and the walls of the container.____74.If the volume of a container of gas is reduced, what will happen to the pressure inside the container?a.The pressure will increase.b.The pressure will not change.c.The pressure will decrease.d.The pressure depends on the type of gas.____75.As the temperature of the gas in a balloon decreases, which of the following occurs?a.The volume of the balloon increases.b.The average kinetic energy of the gas decreases.c.The gas pressure inside the balloon increases.d.all of the above____76.Why does air escape from a tire when the tire valve is opened?a.The pressure outside the tire is lower than the pressure inside the tire.b.The pressure outside the tire is greater than the pressure inside the tire.c.The temperature is higher outside the tire than inside the tire.d.There are more particles of air outside the tire than inside the tire.____77.The volume of a gas is doubled while the temperature is held constant. How does the gas pressure change?a.It is reduced by one half.b.It does not change.c.It is doubled.d.It varies depending on the type of gas.____78.When the pressure and number of particles of a gas are constant, which of the following is also constant?a.the sum of the volume and temperature in kelvinsb.the difference of the volume and temperature in kelvinsc.the product of the volume and temperature in kelvinsd.the ratio of the volume and temperature in kelvins____79.A gas occupies a volume of 2.4 L at 14.1 kPa. What volume will the gas occupy at 84.6 kPa?a.497 Lc.14 Lb.2.5 Ld.0.40 L____80.If a balloon containing 3000 L of gas at 39C and 99 kPa rises to an altitude where the pressure is 45.5 kPa and the temperature is 16C, the volume of the balloon under these new conditions would be calculated using the following conversion factor ratios: ____.a.3000 L c.3000 L b.3000 L d.3000 L ____81.How is the ideal gas law usually written?a. = Rc.PV = nRTb. = nRd.P = ____82.If the atmospheric pressure on Mt. Everest is one-third the atmospheric pressure at sea level, the partial pressure of oxygen on Everest is ____.a.one-sixth its pressure at sea levelc.one-half its pressure at sea levelb.one-third its pressure at sea leveld.equal to its pressure at sea level____83.If oxygen is removed from a sample of air as iron rusts, what happens to the partial pressure of oxygen in the air?a.It increases.c.It decreases.b.It stays the same.d.The change cannot be determined.____84.When a container is filled with 3.00 moles of H, 2.00 moles of O, and 1.00 mole of N, the pressure in the container is 768 kPa. What is the partial pressure of O?a.256 kPac.128 kPab.128 kPad.192 kPa____85.The tendency of molecules to move toward areas of lower concentration is called ____.a.suffusionc.effusionb.suspensiond.diffusion____86.Which of the following gases will effuse the most rapidly?a.brominec.ammoniab.chlorined.hydrogen____87.What causes water's low vapor pressure?a.dispersion forcesc.hydrogen bondingb.covalent bondingd.ionic attractions____88.Which atom in a water molecule has the greatest electronegativity?a.one of the hydrogen atomsb.both hydrogen atomsc.the oxygen atomd.There is no difference in the electronegativities of the atoms in a water molecule.____89.The fact that ice is less dense than water is related to the fact that ____.a.the molecular structure of ice is much less orderly than that of waterb.the molecules of ice are held to each other by covalent bondingc.ice has a molecular structure in which water molecules are arranged randomlyd.ice has a molecular structure that is an open framework held together by hydrogen bonds____90.Which of the following substances is the most soluble in water?a.sodium chloridec.bromineb.methaned.carbon____91.Which of the following substances dissolves most readily in gasoline?a.CHc.NHb.HCld.NaBr____92.An electric current can be conducted by ____.a.methane gasc.a salt solutionb.a sugar solutiond.rubbing alcohol____93.Which of the following materials is NOT a colloid?a.gluec.smokeb.alloyd.muddy water____94.Which of the following usually makes a substance dissolve faster in a solvent?a.agitating the solutionb.increasing the particle size of the solutec.lowering the temperatured.decreasing the number of particles____95.Which of the following expressions is generally used for solubility?a.grams of solute per 100 grams of solventb.grams of solute per 100 milliliters of solventc.grams of solute per 100 grams of solutiond.grams of solute per 100 milliliters of solution____96.The solubility of a gas in a liquid is ____.a.proportional to the square root of the pressure of the gas above the liquidb.directly proportional to the pressure of the gas above the liquidc.inversely proportional to the pressure of the gas above the liquidd.unrelated to the pressure of the gas above the liquid____97.To increase the solubility of a gas at constant temperature from 1.20 g/L, at 1.4 atm, to 2.3 g/L, the pressure would have to be increased to ____.a.0.37 atmc.1.37 atmb.0.7 atmd.2.7 atm____98.In which of the following is the solution concentration expressed in terms of molarity?a.c.b.d.____99.What is the molarity of a solution containing 56 grams of solute in 959 mL of solution? (molar mass of solute = 26 g/mol)a.1.5Mc.2.1Mb.2.2Md.0.0022M____100.The volume of alcohol present in 620 mL of a 40.0% (v/v) solution of alcohol is ____.a.372 mLc.248 mLb.40.0 mLd.580 mL____101.Colligative properties depend upon the ____.a.nature of the solutec.number of solute particles in a solutionb.nature of the solventd.freezing point of a solute____102.The molality of a solution containing 8.1 moles of solute in 4847 g of solvent is ____.a.39mc.0.17mb.1.7md.598m____103.What is the mole fraction of ethanol in a solution of 3.00 moles of ethanol and 5.00 moles of water?a.0.375c.1.67b.0.6d.15____104.To which of the following variables is change in boiling point directly proportional?a.molarity of solutionc.percent by volume of solutionb.molality of solutiond.percent (mass/mass) of solution____105.The freezing point of a solution that contains 0.550 moles of NaI in 615 g of water is ____. (K = 1.86C/m; molar mass of water = 18 g)a.1.66Cc.3.33Cb.1.66Cd.3.33C____106.What is the boiling point of a solution of 0.1 mole of glucose in 200 mL of water? (K = 0.512C/m)a.100.06Cc.100.26Cb.100.13Cd.100.5C____107.How does a calorie compare to a joule?a.A calorie is smaller than a joule.c.A calorie is equal to a joule.b.A calorie is larger than a joule.d.The relationship cannot be determined.____108.If heat is released by a chemical system, an equal amount of heat will be ____.a.absorbed by the surroundingsc.released by the surroundingsb.absorbed by the universed.released by the universe____109.What is the amount of heat required to raise the temperature of 200.0 g of aluminum by 10C? (specific heat of aluminum = 0.21 )a.420 calc.42,000 calb.4200 cald.420,000 cal____110.What does the symbol H stand for?a.the specific heat of a substanceb.the heat capacity of a substancec.the heat of reaction for a chemical reactiond.one Calorie given off by a reaction____111.The heat content of a system is equal to the enthalpy only for a system that is at constant ____.a.temperaturec.pressureb.volumed.mass____112.Calculate the energy required to produce 7.00 mol ClO on the basis of the following balanced equation. 2Cl(g) + 7O(g) + 130 kcal 2ClO(g)a.7.00 kcalc.130 kcalb.65 kcald.455 kcalScholarship Chemistry 2nd Semesrer Examination 2005/2006Answer SectionMULTIPLE CHOICE1.ANS:BDIF:L1REF:p. 254OBJ:9.1.12.ANS:CDIF:L1REF:p. 254OBJ:9.1.13.ANS:CDIF:L1REF:p. 254, p. 255OBJ:9.1.14.ANS:ADIF:L2REF:p. 254, p. 255OBJ:9.1.15.ANS:BDIF:L1REF:p. 254, p. 255, p. 257OBJ:9.1.1, 9.1.26.ANS:CDIF:L2REF:p. 254, p. 257OBJ:9.1.1, 9.1.27.ANS:DDIF:L2REF:p. 257OBJ:9.1.28.ANS:CDIF:L1REF:p. 262, p. 263OBJ:9.2.19.ANS:ADIF:L1REF:p. 261OBJ:9.2.110.ANS:BDIF:L2REF:p. 262OBJ:9.2.111.ANS:ADIF:L2REF:p. 262, p. 263OBJ:9.2.112.ANS:BDIF:L2REF:p. 264, p. 265, p. 266OBJ:9.1.3, 9.2.213.ANS:CDIF:L1REF:p. 268OBJ:9.3.1, 9.3.214.ANS:ADIF:L2REF:p. 272OBJ:9.4.115.ANS:ADIF:L2REF:p. 272OBJ:9.4.116.ANS:BDIF:L1REF:p. 274OBJ:9.5.117.ANS:DDIF:L2REF:p. 274OBJ:9.5.118.ANS:DDIF:L1REF:p. 290OBJ:10.1.219.ANS:DDIF:L1REF:p. 290OBJ:10.1.220.ANS:ADIF:L2REF:p. 290, p. 291OBJ:10.1.221.ANS:DDIF:L2REF:p. 291, p. 292OBJ:10.1.222.ANS:ADIF:L1REF:p. 294OBJ:10.1.323.ANS:BDIF:L2REF:p. 294OBJ:10.1.324.ANS:DDIF:L2REF:p. 295, p. 296OBJ:10.1.425.ANS:ADIF:L2REF:p. 299OBJ:10.2.126.ANS:CDIF:L2REF:p. 301OBJ:10.2.227.ANS:CDIF:L2REF:p. 307OBJ:10.3.128.ANS:ADIF:L1REF:p. 309OBJ:10.3.229.ANS:ADIF:L1REF:p. 309OBJ:10.3.230.ANS:CDIF:L2REF:p. 310OBJ:10.3.231.ANS:BDIF:L2REF:p. 312OBJ:10.3.332.ANS:ADIF:L1REF:p. 323OBJ:11.1.233.ANS:DDIF:L1REF:p. 323OBJ:11.1.234.ANS:CDIF:L1REF:p. 323OBJ:11.1.235.ANS:CDIF:L2REF:p. 323OBJ:11.1.236.ANS:ADIF:L1REF:p. 324, p. 325OBJ:11.1.337.ANS:BDIF:L1REF:p. 325OBJ:11.1.338.ANS:CDIF:L2REF:p. 324, p. 325OBJ:11.1.339.ANS:BDIF:L1REF:p. 333OBJ:11.2.140.ANS:BDIF:L1REF:p. 333OBJ:11.2.141.ANS:CDIF:L2REF:p. 334, p. 335OBJ:11.2.142.ANS:ADIF:L1REF:p. 334, p. 335OBJ:11.2.243.ANS:BDIF:L1REF:p. 356OBJ:12.1.244.ANS:ADIF:L2REF:p. 356OBJ:12.1.245.ANS:BDIF:L1REF:p. 359, p. 360OBJ:12.2.146.ANS:BDIF:L2REF:p. 359, p. 360OBJ:12.2.147.ANS:ADIF:L1REF:p. 363, p. 364, p. 365, p. 366OBJ:12.2.248.ANS:BDIF:L2REF:p. 360, p. 361, p. 362OBJ:12.2.249.ANS:BDIF:L2REF:p. 363, p. 364, p. 365, p. 366OBJ:12.2.250.ANS:DDIF:L1REF:p. 369OBJ:12.3.151.ANS:BDIF:L2REF:p. 371OBJ:12.3.152.ANS:ADIF:L2REF:p. 369OBJ:12.3.153.ANS:DDIF:L1REF:p. 372OBJ:12.3.254.ANS:CDIF:L2REF:p. 375OBJ:12.3.255.ANS:ADIF:L1REF:p. 385OBJ:13.1.156.ANS:BDIF:L2REF:p. 385OBJ:13.1.157.ANS:CDIF:L1REF:p. 387OBJ:13.1.258.ANS:CDIF:L1REF:p. 387OBJ:13.1.259.ANS:ADIF:L2REF:p. 386OBJ:13.1.260.ANS:BDIF:L1REF:p. 388OBJ:13.1.361.ANS:CDIF:L1REF:p. 389OBJ:13.1.362.ANS:CDIF:L3REF:p. 388OBJ:13.1.363.ANS:ADIF:L1REF:p. 390OBJ:13.2.164.ANS:ADIF:L2REF:p. 391OBJ:13.2.265.ANS:BDIF:L2REF:p. 392OBJ:13.2.366.ANS:DDIF:L1REF:p. 393OBJ:13.2.467.ANS:BDIF:L2REF:p. 395OBJ:13.2.468.ANS:CDIF:L2REF:p. 394OBJ:13.2.469.ANS:BDIF:L3REF:p. 394, p. 395OBJ:13.2.470.ANS:BDIF:L1REF:p. 401OBJ:13.4.171.ANS:ADIF:L2REF:p. 402OBJ:13.4.272.ANS:DDIF:L2REF:p. 413, p. 414OBJ:14.1.173.ANS:ADIF:L1REF:p. 415OBJ:14.1.274.ANS:ADIF:L1REF:p. 416OBJ:14.1.275.ANS:BDIF:L1REF:p. 417OBJ:14.1.276.ANS:ADIF:L2REF:p. 416OBJ:14.1.277.ANS:ADIF:L1REF:p. 418OBJ:14.2.178.ANS:DDIF:L1REF:p. 421OBJ:14.2.179.ANS:DDIF:L2REF:p. 419OBJ:14.2.180.ANS:CDIF:L2REF:p. 419OBJ:14.2.281.ANS:CDIF:L1REF:p. 426OBJ:14.3.182.ANS:BDIF:L1REF:p. 433OBJ:14.4.183.ANS:CDIF:L2REF:p. 433OBJ:14.4.184.ANS:ADIF:L2REF:p. 434OBJ:14.4.185.ANS:DDIF:L1REF:p. 435OBJ:14.4.286.ANS:DDIF:L2REF:p. 436OBJ:14.4.287.ANS:CDIF:L1REF:p. 447OBJ:15.1.188.ANS:CDIF:L2REF:p. 446OBJ:15.1.189.ANS:DDIF:L2REF:p. 448, p. 449OBJ:15.1.290.ANS:ADIF:L2REF:p. 451OBJ:15.2.291.ANS:ADIF:L2REF:p. 451OBJ:15.2.292.ANS:CDIF:L1REF:p. 452, p. 453OBJ:15.2.393.ANS:BDIF:L1REF:p. 460OBJ:15.3.294.ANS:ADIF:L2REF:p. 471, p. 472OBJ:16.1.195.ANS:ADIF:L2REF:p. 473OBJ:16.1.296.ANS:BDIF:L2REF:p. 476OBJ:16.1.397.ANS:DDIF:L2REF:p. 476, p. 477OBJ:16.1.498.ANS:DDIF:L1REF:p. 480, p. 481OBJ:16.2.199.ANS:BDIF:L3REF:p. 481OBJ:16.2.1100.ANS:CDIF:L2REF:p. 485OBJ:16.2.3101.ANS:CDIF:L2REF:p. 487, p. 488OBJ:16.3.1102.ANS:BDIF:L1REF:p. 491OBJ:16.4.1103.ANS:ADIF:L1REF:p. 492OBJ:16.4.1104.ANS:BDIF:L1REF:p. 494OBJ:16.4.2105.ANS:DDIF:L2REF:p. 495OBJ:16.4.2106.ANS:CDIF:L3REF:p. 495, p. 496OBJ:16.4.2107.ANS:BDIF:L1REF:p. 506OBJ:17.1.1108.ANS:ADIF:L1REF:p. 506OBJ:17.1.1109.ANS:ADIF:L1REF:p. 508OBJ:17.1.3110.ANS:CDIF:L1REF:p. 514OBJ:17.2.1111.ANS:CDIF:L1REF:p. 511OBJ:17.2.1112.ANS:DDIF:L2REF:p. 515OBJ:17.2.2