2004 AP Chem_full

2004 AP Chem_full - MATERIAL IN THE FOLLOWING TABLE MAY...

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Unformatted text preview: MATERIAL IN THE FOLLOWING TABLE MAY BE'USEFUL 1N ANSWERING THE QUEST! SECTION OF THE EXAMINATION. Ill entr . PERIODIC TABLE OF THE ELEMENTS Id. 1112004 rAProln 1111.71 121.75 1 14.82 21 Sc 4436 47.90 39 Y . . 88.91 55 56 57 72 73 4 Cs Ba *La H! To 137.91 13733 138.91 178.49 180.95 1 20 Ca 40118 33 S1- 37 62 19 K 39.10 37 Rb as 47 eeEntrneE Intln ntA rllreered. nd . 0911!. team TbDy 158.93 Gd 59 P1- 1409] 104 Rf (2m 89 TAc 217 03 58 Ce 88 Ra mo: ‘Lanthnnide Series 87 Fr (27-?) rAPtdentndmu. Ho Er 164.93 167.16 99 Es 168. 162.50 97 Bk (:4 '33. 5 V1 .— 62 Sm 15114 60 61 Nd Pm 144.24 (145) 140.12 101 100 Fm 25 *5 95 Am 94 P11 (244) 93 N 237 92 U 91 Pa 90 Th P TActinide Series ONS lel'HlS (152) 3 243 .05 232.04 731.04 238.03 Section I ’ CHEMISTRY Section 1 Time—:1 hour and 30 minutes NO CALCULATOR MAY BE USED WITH SECI'ION 1. Note: For all questions. assume that the temperature is 298 K. the pressure is 1.00 atmosphere. and solutions are aqueous unless otherwise specified. 1 Throughout the test the following symbols have the definitions specified unless otherwise noted. 1‘ = temperature L. m1. = liter(s). milliliter(s) P = pressure 3 = gram(a) V = volume 11m = nanometer(s) S = entropy em = atmospherds) . H = enthalpy mm Hg = millimeters of mercury G = Gibbs free energy J. k] = joule(s),lcilojoule(s) R = molar gas constant V = volt(s) n = number of moles moi = mole(s) M = molar m = molal Part A blrectlona: Each set of lettered choices below refers to the numbered statements immediately following it. Select the one lettered choice that best fits each statement and then fill in the corresponding oval on the answer sheet. A- choice may be used once, more than once, or not at all in each set. Questions 3-5 refer to the Iollowlng molecules. Questions 1-2 Consider atoms of the following elements. Assume (A) C02 that the atoms are in the ground state. (B) H20 (C) CH4 (A) S (3) ca (D) (C) Ga (E) PH; (D) Sb - . (E) Br 3. The molecule with only one double bond 1. The atom that contains exactly two unpaired 4. The molecule with the largest dipole moment electrons 5. The molecule that has trigonal pyramidal geometry 2. The atom that contains only one electron in the highest occupied energy sublevel Unified lnme n rl tl allo. (30 ON TOTHE NEXT PAGE / nt 2004 eeEntrneE lntln vd.A unsaved .An._.- -a ._... Its-m a-» Section I Section I . Questions 6-7 refer to the following solid ' .Questlons 8-10 refer to the following gases at 0°C Part B compounds. and I aim. Directions: Each of the questions or incomplete statements below is followed by five suggested answers or (A) l’bSO. (A) Ne completions. Select the one that is best in each case and then fill in the corresponding oval on the answer sheet. (B) CuO (B) Xe (C) gin“ (C) 02 Questions 15-15 relate to the graph below. The 17. In which of the following groups are the three (D) (D) CO graph shows the temperature of a pure substance as it species isoelectronic; i.e., have the same number (5) m: (E) NO 5 is heated at a constant rate in an open vessel at 1.0 of electrons? ~ stm pressure. The substance changes from the solid to (A) s,_ K; 032+ 8. Has an average atomic or molecular speed closest the liquid to the gas phase. to that of N, molecules at 0°C and 1 sun 6. Is le in ueous solution M aq (B) Sc. Ti, V“ (C) 01-.s=-.c1- (D) Mg2+‘ Ca2+, sr2+ (E) Cs.aa1+,l.s3+ 7. ls white and very soluble in water 9. Has the greatest density 10. Has the greatest me of effusion though a pinhole f" o . Pressure (am) 9 kl! Questions 11-14 refer to the reactions represented below. (A) HZSeO4(aq) + 2Cl’(aq) + 2H+(oq) —) H,Se0,(aq) + 02(5) 4. H200) (B) S,(.:) + 801(3) -> 8501(5) 0 15.Thesubstsnceisatitsnormnlfreezingpointat 0 20 40 60 80100 (C) 3 Br1(aq) + 6 OH-(aq) -+ 5 Br'(aq) + Br03'(aq) + 3 H20“) Lune Tmm (’0) 2 2— (D) C“ +0”) + $04 ("4) —) C‘so‘m (A) ‘1 ' 18. The phue diagram for the pure substance X is (B) PtCl‘(s) + 2 Cl'(aq) —9 Ptle'qu) (B) '2 shown above. The temperature of a sample of (C) ‘3 ' pure solid X is slowly raised from 10°C to It. A precipitation reaction (D) t4 - . 100°C at a constant pressure of 0.5 atrn. What 2 A . mm . l (E) :5 is the expected behavior of the substance? 1 ‘ Eamon that mm a 0 won comp ex (A) It first melts to a liquid and then boils at about l6. Which of the following best describes what 70°C. 13. A reaction in which the same reactant undergoes both oxidation andmducdm happens to the substance between :4 and :5 7 (B) It first melts to a liquid and then boils at about (A The molecules are leavin the li uid phase. 30°C . , 14. A combustion reaction (3; The solid Md liquid PM; bought in (C) It melts to a liquid at a temperature of shout equilibrium 10°C and remains a liquid until the (C) The vapor pressure of the substance is temperature is greater than 100°C. deeming. - (D) It sublimes to vapor at an equilibrium (D) The average intermolecular distance is temperature of about 20°C. decreasing. (E) It remains a solid until the temperature is (E) The temperature of the substance is greater than 100°C. . increasing. Un r n at! in r rs e U I. 9° °NT°THE NEXT PAGE 60 ON TO THE NEXT PAGE . nt 2004 eeEntrnsE lnlln rd.A rltraerod. “lemuaerd. rAPreln nd .oerri. Idenl rAPldenlndrem. til 2004 eeEntrnoE lnlln rutA dtraored. Ht am. so I‘d. rAPteln nd . ee rd. tdom yAPtdent nd rent. Section! 19. 21. In which of the following species docs sulfur have the same oxidetion number as it does in HZS‘O4 ? (A) 112303 (B) 8203* (C) S" (D) S. (E) sozc12 . A flask contains 0.25 mole of 802(3)..0.50 mole of CHAg),md0.50 mole of O,(g).Thetotel pressuteofthegnsesintheflukisSOOmmHg. Whatisthepartinlpreuureofthe 502(3) inthe flask? ’ ' (A) 800mmHg (B) 600mmHs (C) 250MB: (D) 200ch (B) 160mmHs In the laboratoly- 112(3) can be produced by adding which of the following to l M HCl(aq) ? I. 1 M Nfls(aq) II. Zn(.r) III. Narrows) (A) lonly (B) 11 only (C) 111 only (Dndeme (E) 1.1LnndIII 2NH,2NH;+NH1- In liquid ammonia, the reaction represented above occurs. In the reaction NH] acts as (A) a catalyst (B) bothanncidendabaee (C) the conjugate acid of NH,J (D) the reducing agent (E) the oxidizing agent Unlded hrne n It (I Illei 23. 24. I'll2004 Ill anti. ee rd. rAPreln no eeEntrneE |ntln niA Ill . ee n1. ‘fiU +§n —) 'ng +3,’,n +X Neutron bombardment of uranium can induce the reaction represented above. Nuclide X is which of the following? (A) gm (3) am (C) :le (D) #Rb (B) 3R1: A compound contains 1.10 mol of K. 0.55 mol of Te. and 1.65 Incl of 0. What is the simplest formula of this compound? (A) KTeO (B) KTe20 (C) KQTeO, (D) KzTeoe (E) K4Te06 3 (3232(3) -> 0636(3) .Whetisdresmrderdenthalpychnnge, AH',for the reaction ebove? (AH; of QHZCg) is 230 It! mol"; AH} of col-16(3) is 83 k1 incl") (A) ~607 U (B) -l47 k] (C) -19 k] (D) +19 ld (E) +773 kl . Approny whet mass of CuSO4 ‘ 51420 (250 g mol") is required to prepare 250 mL of 0.10 M copperflI) sulfate solution? (A) 4.0g (B) 628 (C) 34s (D) 853 (E) 140: GO ON TOTHE NEXT PAGE veered. Idem rAPtdent M rem. .4 Section I 2N0(g) + 01(3) —» 2No,(g) 27. A possible mechanism for the overall reaction represented above is the following. (1) Noe) + N005) -) N202(8) (2) N202“) + 02(5) —-) 2N02(s) ffl-‘ft Which of the following rate expressions agrees best With this possible mechanism? (A) Rate = k[NO]’ a» Rm = kmoflod (E) m kINzozHoz] vlt2004 [E] eeEntIneE lntln rd.A rltreered. slaw GO ON TOTHE NEXT PAGE Section I 28. 0f the following compounds. which is the most Seclionl ionic? C52“) + 3 02(3) 4 C02“) + 2 802(8) . . Questions 33-34 35. A lsolution is made1 by dissolving a nonglatile . . . > r aouteinapuresovenLComparedtc pure (A) Sick 31' w: Volume: ?2@)p::q““°d t° mm The graph below shows the titration curve that solvent, the solution (B) BIC] ' V5 “9635 2( ) to “C9 4-0 L 0f (302(8) 7 results when 100. mL of 0.0250 M acetic acid is (A) has . hi . . . . . gbel- normal balling paint (C) PCl3 (Assume all gases are measured at 0°C and 1 atm.) “med “'"h 0100 M N‘OH‘ (B) has a higher vapor pressure (D) C120 (A) 12 L (C) has the'same vapor pastime (E) Can 14.0 (D) has nhlsherfigezingpomt .(B) 22.4 L 12.0 (B) ls more nearly deal 29. The best explanation for the fact that diamond is extremely hard ill that diamond crystals (C) % X 22-4 L 10.0 36' {33.11:an ‘ mluhfllmco? ofmn'iu’ll'llsgxipmm (A) are made up of atoms that are intrinsically PH 8‘0 Ema Wh’fild'm“ m, mm W, “Pm, hard because of their electronic mch (D) 2 x 22-4 L 6'0 A few drops of potassium iodide solution were . (B) 6033!? positive ltnd negative ions that m 3 x 22 4 L 4.0 “med to me but water mmmmi: high? yeutgw s gyattracted ceac other ' 2.0 W10" W88 “ced- W “WWII. (C) are giant molecules in which each atom fonns _ . . . a o o . termini“: on they?!“ paper W My mum]: strong covalent bonds with all of it: 32- mfg? Mm“! 0nd“ 18 I 8“ It 25 C ' o s 10 15 20 2.5 30 35 40 45 in m. i. solution. What two ions could have neighboring atoms been present in the unknown? (D) are formed under extreme conditions of (A) R520 “‘L °f (“00 M N'OH Added + and “ tempt-attire and pressure _ (3) N20 (A) A: (“(1) H82 (‘4) (E) flmfltflsflm “of 3:31,,” mm W (C) N120: 33. Which ofthe following indicatmais thebest choice 03) A8244) Ind P3709) ,0 ml, crystal .8 I who], - (D) Sioz . for the titration? (C) Bazfaq) and Ag in) ' (E) ngog pH Range of (D) B! (M) Ind HS: (04) 30. At 25°C. aqueous solutions with a pH of 8 have a Mime: W (E) Ba’flaq) and Pb”(aq) hydroxide ion concentration, [0H ‘]. of (A) Methyl me 32 _ 44 (A) l X lO‘MM (B) Methyl red 4.8 - 6.0 (B) 1 x lo-IM (C) Bromothymol blue 6.1 - 7.6 6 (D) Phenolphthalein 8.2 - 10.0 (g; lenr M (E) AW 11.0-12.4 (’3) 8“ 34.Whaipmeimemvempondmmeopdmm buffer action for the acetic acid/acetate ion pair? (A) Point V (B) Point X (C) Point Z (D) Along all of section WY (B) Along all of section YZ 9° ONTO THE NEXT PAGE co ONTOTHE NEXT PAGE EZI HI 2004 soEnlrneE lnun "1A rumored. Ill entr. co rd. rAPreln nd ‘ . ae rd. Men! rAPldent nd IBM. [E llt 2004 eoEntrnoE Inun MA ntnerod. Ht amused. rAPreIn nd .eevd. (dent rAPldentndram. Section I HC03"(aq) + 0H ‘(aq) «'1 H200) + C031”) AH s —4l.4kJ 37. When the reaction represented by the equation above is at equilibrium at 1 atm and 25°C, the ratio _ [C0311 1400;] can be increased by doing which of the following? (A) Decreasing the temperature (B) Adding acid (C) Adding acatalyst (D) Diluting the solution with distilled water (E) Bubbling neon gas through the solution 38. A 0.10 M aqueous solution of sodium sulfate, Naiso‘. is a better conductor of electricity than a 0.10 M aqueons solution of sodium chloride. NaCl. Which of the following best explains this obsemu'on? (A) NazSO4 is more soluble in water than NaCl is. (B) Naaso‘ has a higher molar mass than NaCl has. (C) To prepare a given volume of 0.10 M solution, the mass of 1132804 needed is more than twice the mass of NaCl needed. (D) More moles ofions are present in a given volume of 0.10 M NaZSQ. than in the same volume of 0.10 M NaCI. (E) The degree of dissociation of Na2804 in solution is significantly greater than that Unttled hnee n 11 ll ollo. Ilt antr. GO ONTOTHE NEXT PAGE of NaCl. Ill 20M uEntrnoE lnltn 1d.A "treated. “rd. IAProln nd .urd. Idem rAPtdont nd rent. Ht entr. on rd. Solubility (g solute pa 100 3 water) Section I 1020304050607080901100 TemperatureC’C) 39. On the basis of the solubility curves shown above, the greetest percentage of which compound can be recovered by cooling a satunwd solution of that compound from 90°C to 30°C ? (A) NaCl (3) 19103 (C) K1010. (D) K1304 (B) Como», “2004 rAPreln DE! GO ON TO THE NEXT PAGE IeEntrneE htln MA rltneud. nd .00 rd. idem vAPldlnl rid rent. Section I ~ 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 Hz gas can be obtained? (A) 22.4 mL (B) 44.8 mL (C) 224 mL (D) 448 mL (B) 896 ml. 41. When solid NH4$CN is mixed with solid Ba(OH)2 in a closed container, the temperature dropaandagasispmduced.Whichofthefol- lowing indicates the correct signs for AG, AH. and AS for the process? AQMAS (A)— ~ — (B)- + — (c)- + + (D)+ — + (E)+ — - I{2(8) + 312(8) 7—) 2151(8) 42. At a certain temperature, the value of the equilibrium constant, K, for the reaction represented above is 2.0 x 105. What is the value of K for the m reaction at the same temperature? (A) -2.0 x 10-5 (B) 5.0x10" (C) 2.0x10-5 (D) 5.0x10'5 . (13) 5.0x10" untried in me an tl alle. 43. 44. 45. 46. rll2004 Ht entr. ee yd. rAPraIn M The atomic mass of copper is 63.55. Given that there are only two naturally occurring isotopes of copper. “Cu and 6’Cn. the natural abundance of the “Cu isotope mustbe approximately (A) 90% (B) 70% (C) 50% (D) 25% (E) 10% 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 (B) Atomic radius What is the mole fraction of ethanol, C2HSOH. in an aqueous solution that is 46 percent ethanol by mass? (The molar mass of Gil-I50}! is 46 g; the molar mass of H20 is 18 g.) (A) 0.25 (B) 0.46 (C) 0.54 (D) 0.67 (E) 0.75 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 greaterdensity atstandard conditions than Ne. (B) Na has a lower first ionization energy than Ne. (C) Na has a higher melting point than Ne. (1)) Na has a higher neutron-to-proton ratio than Ne. (E) Na has fewer naturally occurring isotopes than Ne. 80 ON TOTHE NEXT PAGE eeEntrnaE lntln «LA rumored. . 00 rd. Idem rAPldem nd Mil. 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) Reactionordercanbedeterminedonlyby 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 thefollowing liquids? ~ (A) 320 (B) 0014 (C) HP (D) arson (E) CHGCOOH Section I ...c:20,2-(aq) + ...H,S(g) + naming) -» ...C13*(aq) + ...S(s) +V...H,O(l) 49. When the equation above is correctly balanced and all coefficients are minced to lowest whole-number terms, ' the coefficient for H’(aq) is (A) 2 (B) 4 (C) 6 (D) 8 (E) 14 In em. Unified ln no. n it tl ellc. Id. eeEntrneE Intin rd.A ntroored. . se rd. tdent llt2004 rAPraln nd 60 ONTOTHE NEXT PAGE rAPtdentndrent. 1‘“?! Section | Section I . - 50. Which of the following represents acceptable 53. According to the VSEPR model, the progressive 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 is weighed quantity of solid acid to a titration flask wet with distilled water decrease in the bond angles in the series of molecules CH‘. N143. and HZO is best accounted for by the (A) increasing strength of the bands (13) decreasing size of the central atom (C) increasing electronegativity of the central (D) Using lOmLof standard stren m“ phenolphthalein indicator solfi‘ti‘on for (D) incrensing number of unshared pairs of titration of25 mLofacid solution steam . (B) Diluting a solution in a volumetric flask to (E) decreasmg repulsion between by it! find communism with hot water atoms _» 54. Whichofthefollowingmustbetmeforareaction for whichtheactivationenergy is the samet'or boditheforwardsnddiereversereactions'l (A) A catalyst is present. (B) 'I'hereactionordercanbeobtnmed' directly from the balanced equation. (C) The reaction order is zero. (D) AH for the reaction is zero. - (E) Asforthereactioniszero. 3 Cu(s) + 8.1-?(041) + 2 NO3‘(aq) —> 3 Cuz“(aq) + 2 N0(g) + 4 1110(1) 51. True statements about the reaction represented above include which of the following? I. Cn(.r) acts as an oxidizing agent. I]. The oxidation state of nitrogen changes from +5 to +2. [I]. Hydrogen ions are oxidized to form 820(1). (A) Ionly (B) 11 only (C) 111 only (D) [and II (E) II and Ill 52. Propane gas. (3H3, burns in excess oxygen gas. 55. A reaction was observed for 20 days and the percentage of the reactant remaining after each day When the equation for this reaction is correctly was recorded in the table above. Which of the following best describes the order and the half-life balanced and all coefficients are reduced to their Of’hc MW? lowest whole-number terms, the coefficient for W W 02 is . (A) First 3 (A) 4 (B) first 10 (B) 5 (C) Second ' 3 (c) 7 ‘ (D) Second 6 (D) 10 (E) Second 10 (B) 22 U tried In run GO ON TOTHE NEXT PAGE “,3 “If” “.f 1‘; no on TO THE NEXT PAGE rlt 2004 asErnrnaE lntln rd.A ntreared. "12004 ooEntrneE Inttn ntA ntnersd. “tenthurd, rAPvaIn nd .aard. Idem rAPtdentndmm. Ilt sntr.oard. rAPraIn no .eent. Idem rAPtdentndrentr Section I . Section | 56. Theboiling points of the elements helium, neon, ZNZH‘Q) + Nzo‘m) —) 3 Nz(g) + 4H20(g) 211200) + 4Mn0"(aq) + 3 C1021”) —) 4 Mnozm + 3 ClO"(aq) 4- 401-1144) 57. argon. krypton, and xenon increase in thatorder. Which of the following statements accounts for this increase?) 58. When 8.0 g of mm (32 g mol") and 92 g of N20‘ (92 g mol") ue mixed together and react 60. According to the balanced equation above. how many moles of ClOflaq) are needed to react completely with 20. mL of 0.20 M KMnO‘ solution? 23)) x gainegdgnpfifigmwse’ according to the equation above. what is the (A) 00030 mo] (C) The dipole-dipole forces increase. maximmn mass of H20 that can be Produced? (B) 0.0053 rnol (D) The chemical reactivity (A) 9.0 g (C) 0.0075 mol (E) The number of nearest neighbors increases. (B). 18 g (D) 0.013 mol (C) 36 g (B) 0.030 mol Rm=kiM1iN12 3,3,) 113: The rate of a certain chemical reaction between substances M and N obeysthernte law above. 'l'hereactionisfn'ststudiedwith [M] and [N] each 1 x 10’" molar. If s new experiment is 59. All of the halogens in their elemenul form at 25°C and I mm are (A) conductors of electricity (B) diatomic molecules 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 7 conductedwith [M] and [‘N]eac112><10‘3 ‘(Q “was . .. . . . . molar, the reaction rate will increase by a factor of (D) cola-m. (A) B£fifigv$mgzlagfimmued Wm” (A) 2 (B) 8‘s“ (B) By diluting the solution with distilled water (B) 4 mammlvolumeonOOmL. (C) 6 - (C) By diluting the solution with distilled water (D) 8 to a total volume of 1.00 L (E) 16 (D) By adding 100.1111. of 0.10 MHCl (B) By adding 100. mL of 0.10 MNaOl-I u (1 0n 6° °NT°THENEXTPAGE so onromeuexmee eeEmrnoE lnun MA nlreered. .ae yd. tdont rAPtdeM on rent. rll2004 rAPreln nd vi! 2004 esEmrneE lmin «LA directed. Ht minced. rAPveln nd .eevd. Idem rAPtdentndrent. Ht enir. ee rd. Section | I 63. Mixtures that would be considered buffers include H'— _ _ _Bt whichofthefollowing? 1.0.10MHCl+O.IOMNaCl I H H 1-1 1]. 0.10MHF+0.10MN:F . In. 0.10MHBr+0.lOMNaBr 62. Whichofthefollowingstructunlformulas A I immumlromerofthecompomdtlnthat Horny,- . structtmlformul I arepreaentedabove’l (C) manly > (D) Iandn iii (B) Band!!! (A) Br— -<f -H 64. Ascorbicecid. l-t,c,H,oG(i).indipmocnia H H H with x. - 7.9x10" and x, - 1.6x10‘“. ‘ lna0.005Meqneousolutionofascorbicscid, B If whichoffliefollowingspecieslspreeentinthe (3) n_+._ -3 . Monmouth? ' H ‘3! H ' (A) 1-120“) . H (B) 530109) (C) 32963606”) «2) n— — — I—a . .(menuq) ' H H B]. W621“) I. ‘ '65. Which of thefollowing substances isLBAST . If solubleth (D) 3P?" — "‘3‘ (A) W04 H H H (3) W4 (C) 3100, (D) 7110103); ®H______Br @tht H g H 66.A2Lcontainerwillholdabout4gofwhichof thefoliowinggleesatO'Cand ion-n? (A) 502 (5) N: (C) CO: (D) C4“: (E) NH; Un t tied In "I e 00 ON TOTHE NEXT PAGE tit 2004 eeEntrneE lntln td.A directed. in entr.eaid. rAPteln nd .eoid um rAPtdentndnm. 67. Which of the following describes the chsnges in forces of atnectim that occur as H20 changes phase from a liquid to a vapor? (A) H—O bonds break as H—l-l and 0-0 bonds form. ‘ (B) Hydrogen bonds between H20 molecules are broken. (C) Covalent bonds between [-120 molecules are broken. (D) Ionic bondsbetween 3+ ions Ind OH‘ ions are broken. (E). Covalent bonds between H" ions and H20 molecules become more effective. 100 . Temperanme 88888388 012 3 4 5 6 7 Time(minutes) . 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 detetmined? (A) A (B) B (C) C (D) D (E) E nlded in tree n It ti elle. 69.‘ 70. 71. Section I if 200. mL or 0.60 M MgCl¢(aq) is added to400. mL of distilled water, whet is the concentntion of Mg’flaq) in the resulting solution? (Assume volumes are additive.) (A) 0.20 M (B) 0.30 M (C) 0.40M (D) 0.60 M (E) 1.2M 0f the following pure substnnces. which has the highest melting point? (A) S: (B) II (C) Sio2 (D) 50; (E) CoHc In the elecn'oplnting of nickel, 0.200 fareday of electrical charge is passed through a solution of NiSO4 . What mass of nickel is deposited? (A) 2.94; (B) 5.37; (C) 11.7g (D) 58.7g (E) 294: 72. [El til2004 lit entr. 9. rd. rAPveln no A colorleés solution is divided into three samples. The following tests were performed on samples of the solution. SEEK M W 1 Add H+(aq) No change 2 Add NI-i3(aq) No chmge 3 Add SO42”(aq) No change. Which of the following ions could be present-in the solution at a concentration ofOJO M ? (A) Ni“(aq) (B) M31414) (C) Bflaq) (D) Na”(aq) (E) Cogz'taq) GO ON TO THE NEXT PAGE eeErmneE Inttn rdA vitreered. . 9. Id. idem rAPtdentnoreni. E ,,. g. 21.... m;~.—i:u-=-,,.- .v ‘55-,- Section I X“) 4'3 X“) 75. In I “turned solution of Zn(OH)2 It 25°C. the al ' 2.0 IO‘SM. Whlti '73.Whichoftlsefollowingisuuefonnysubstmce V “mom? ‘9, x "1” mm me pm M We a its value of the Mummy-product constant. K”. for nomnl mailing point? Zn(OH)1 It 25°C 7 8) 2;“; (A) 4.0x10'“ (C; AH = TAG 8.0 x10‘“ (D) TAS I 0 ' 1.6 X 10‘" (B) A” 3 T“ ‘ (D) 4.0 x m-12 74. A pure. white crystalline solid dissolves in water (B) 2-0. x 10" toyieldsbasicsolntiontlntllbemessgaswhen emacidlsnddedtolLOnmebuisofthis information, the solid could be (A) mo, (3) K2003 (C) KOH . (D) mso‘ (E) KCI END OF SECTION I UnlflCd In"... n H ll olle. #12004 In sntr. as rd.‘ rAProln nd osEntrnoE Min MA II I nor“. . as rd. Idem IAP'IM "d um . i l. E Section II WY SECTION ll Time—90 minutes; Percent of anal wade—55 ThnefothA—40minutes.AnleerQuesfion l fldflmthflanGQnesdml CALCULANRSAREAUDWE),EKCE’TFORHIOSBWHH1YPEWRM(QWEITY)KEYBOARDS. WendyfihguluflsbIsmyhemcdwhuxmmhwmbemofmm dun. momma—56mmAmwaQuuuomm.andsnndeithaQuesum7uQmma. NOCALCULATOK9AREAL10WED.. General Instructions - 'l‘lsetinsesmesnAsnill’srlBwfllbennnmncedsepnntely.¥wmnypmceedfieelyfiommqwfionmmenext wiflfinemhmeonotspendwomuchfimemnnyoneqmflon. Page: containing a periodic table, reduction potenfisls. Ind lists confining equations Ind constants are princedin flsepinkbooklet. ‘ Youmayuseeltlmupenorlpencll.Mskemdmyonrwrifinglsclemlegible,snddukenoughtobeesslly read.Il‘youmhesnetmr.youmynvefimebycrouingitoutmhaflnnu’ylngmmltwmmmmm lntlxespeoeptovlded folldwinguchquesfion. WhenyosilremldmbegimopenywrfiooklanndmwmkoanA.Whenfimeiscllled.ymmustsu)pwmk mdputawuyyomcnlculnurudlsected.DoNOTsmwotkoanBInuilyonsretoldtobegln.Whenmldtodo so,openyouxbooklaloPmBmdwefullyteuounhegxeeninm INIPORTANT Anermmpkflng'memdrcleBELOW'thenmberoflhequuflonywchosetomwerlnPu-IA udhfllflwaullmdomfieqnuflomymlntmdedhdsoosenynotbeflnonuMare seEmrnsE lntln rd.A directed. rAPraln nd .ecrd. Idem rAPldomndvonl. “[2004 In em. as rd. ...
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This note was uploaded on 08/27/2010 for the course CHEM 1070 taught by Professor Sticker during the Spring '08 term at Northwestern IA.

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2004 AP Chem_full - MATERIAL IN THE FOLLOWING TABLE MAY...

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