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Exam 3 Key - CHEM 1212 EXAM III Fall 2010 110 Points NAME 9...

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Unformatted text preview: CHEM 1212 EXAM III Fall 2010 110 Points NAME 9/ 810 Score SHOW ALL WORK TO RECEIVE FULL CREDIT. Periodic Table 2 He 4.003 5 6 8 9 10 B C O F Ne 10.81 12. 01 I? 01 16 19.00 0.18 13 15 18 Ar 21‘16. 98 288. 019 30F. 97 32S. 07 35. 4'5 39. 95 2 21 T21 23 24 25 26 27 28 29 30 35 36 CaSc6 VCrMnFeCoNiuC GaGe BrKr 40 08 449 47. 813 50.94 52.00 54.94 55.85 58.93 58.69 63.55 65. 39 69.72 72.61 if} .9s.2 78. 96 79. 90 83 80 38 39 41 42 43 44 45 46 49 50 53 54 Sr Y Zr Nb Mo Tc R11 Rh Pd Ag Cd In Sn Sb Te I 1Xe 87. 62 88 91 9122 92.91 95.94 (98) 101.1 102.9 106.4 107.9 112.4 114.3 118.7 121. 8 127 6 126913 56 5 lBa At .3 10 88 Ra 6. N N 73 74 75 76 77 78 79 80 81 82 83 8 Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi 11:3} 1735 1310 133.3 186.2 190.2 192.2 195.1 197.0 200.6 204.4 207.2 209.0 (P209) 2 222) 104 105 106 107 108 109 110 111 Rf Db Sg Bh Hs Mt Ds Rg 22A” (261) (262) (263) 262 265 (266 271 73 1. The rate law for the decomposition of hydrogen peroxide to water and oxygen is: rate = 1411202]. If it takes 8.0 hours for the concentration of H202 to decrease from 0.80 M to 0.40 M, how many hours are re- quired for the concentration to decrease fiom 0.60 M to 0.15 M? (Hint: Do you need the coefi‘icient of H202 in the balanced equation?) (8 pts) 241202 :5 2112.0 +07, (“Lt/1:1}: REPS" (5-1“? ‘ffls Mo 803'- [3 W7 =— 20.7031 1M“: z 2. Consider the following reaction profile. (12 pts) Potential Energy (kl/Incl) Progress of Reaction a) Write a possible mechanism for the reaction profile above. Identify the fast and the slow steps in tk mechanism. Write the overall reaction for the profile. b) Identify the reaction intermediates. mt @ c) Identify the reaction catalyst. No Qg‘l‘mlrjf'l‘ d) Is the reaction endothermic or exothermic? Using a dashed line, sketch the change in energy on th graph- Q/yxclo fixer m M The data listed in table below were obtained for the decomposition reaction, A —> products. mean mo- larity of A. (8 pts) ln[A] vs time —II'I-I'I-1EI 0-00 t} 10 20 30 4? E —l 00 y = -0.0539x - 0.1363 4.00 R2 -—- c.9578 _ time, mm 1/[A] vs Time S/aaejL [A] vs Time R [“03", IIHeLr 6.0 _ =—0 0273;; + 0 8462 ég'g/ % «T 3323:! R2=08369 H . . 0.00 i———r——% time, min time, min 30' a) What is the reaction order of A? Explain. (*5 2nd arcflef Pfla't a-F I 3 VS- énne [5 ”403+ 11"! ear 3) What is the rate constant for the reaction? 5 I 0 {9‘8 5 G.— K as 3Q K: on M’m‘m‘ :) What is the half-life of A? When 0.0200 moles of sulfur trioxide is introduced into an evacuated 1.52-L flask at 900 K, 0.0142 mol ( sulfur trioxide is found to be present at equilibrium. (10 pts) a) What is the value of Kc for the dissociation of sulfur trioxide at 900. K? W— : 0.0131 04 s03. 0.01:4 2M0; £093! [-er L [.324 50 r ' 503 :2; $01 47 OZ a+ebL ® I 02;){32 m . o O C @0038?!» M + 0.00335M + Ocaal93m f/rf/‘f—jom m E 0.0mm m 0'0”“ m KC=W=— 50.0mm”) b) What is the value of Kp for the dissociation of sulfur trioxide at 900. K? Consider the following reaction. Predict how the equilibrium concentration of the complex ion FeClZ will change (increase, decrease, or no change) when the following stresses are applied to the equilibrim system. '(8 pts) 3»me \ \\ 7r @965 - ,- Fefiaq) + Cl‘(aq) é FeC12+(aq) a) Fe(N03)3 is added. inc -e “ b) Pb(N03)3 is added. e g Q_ 0) F68 is added. no chem Wk d) A catalyst is added. 11 0 C L a a fig lne renewing plctures represent equilibrium mixtures at 500 K and 300 K for the following reaction. (8 DtS) A2(g) -T—"'" 2A(g) 00 d) 00 0% 0%8 o 8 00 o 00 c9 , 500K 300K a) Is the reaction endothermic or exothermic? Justify your answer. emote 45mm“? c @ More preclucl’f "Form b? raisfhg Wfl' Marci Kit is Jamie, (is. H MD. b) Draw a picture that represents the equilibrium mixture after the volume of the container at 500 K is in- creased. 500 K increased volume less A 2- 31assify each of the following as a strong acid, weak acid, strong base, weak base, insoluble base, soluble :alt, insoluble salt, or an amphoteric species. (16 pts) 1) H010 Wegk and b) NIL;+ weak goid :) PbBrz ’mgglu big sell d) CN we. '0 e. 3) Mg(OH)2 infiglublfi base t)HBr Siron QC‘ 6 ;) K1 Sbll‘blfi g H“ 11) mm” gszLOWI-ar‘t.c 3.250 g of barium hydroxide is dissolved in 865 mL of solution. Calculate the [H30] and the pOH of ti solution. (10 pts) Balm”; 9 80‘“ + ZOH’ .25— BotCOl-H'L ImolBa all) 7C ,_L__ —_—_ O 03 X ”Lag-MW)» 0.8451— .- -3 2mm“ , 3.37m was" quxzo"3m :3th " 2P3“ a [and] [340150; Q0 _ ‘ -3 100142-203 [3.37ny ] =E] LHQ = ['00 >0qu- q7xzo'p'f‘” Wm Zp-l-W was SF Consider the following reaction at 25 °C for which AH° is -26.9 k] and AS" is 11.4 5/K. (10 pts) u—h‘. a) Is the reaction spontaneous? Why or why not. (*ka AG -.- 4%.? 1c: — (29%) (0.0 [M k?) 14 @ £6: #30. 3 KIT @M {s span—InneOUS b) Determine KP .for the reaction at 25 °C. AC7 2 —?\T ln kf @ ““9: £36- : 40.316: “RT eoemofiwxw _{<_______1‘ (26'3“) wol-I’C 10. A 50.0-L reaction vessel contains 1.00 mol N2, 3.00 mol H2, and 0.500 mol NHg. Will more ammonia be formed or will it dissociate when the mixture goes to equilibrium at 400 °C. Kc is 0.500 at 400 °C. Justi- fy your answer Via calculation. (8 pts) 3H +N -'-2NH @ @ - @ Loan-0M2. 2 0-02.90 M 4/1 Zpfldauol HL: 0_b500 m . - H 33% W. T“ 5‘0 0L. ‘ O‘OIUUM A Q 1 [0.010011 @p‘txflg [0.22963 ' <9 : 2.3.1 63> R Q @[R‘fi 90-94 +0 IGAH‘I NH; :5 clissncm—l-ed 11. Gaseous hydrogen iodide is placed in a closed 1.00-L container at 425 “C, where it partially decomposes to hydrogen4and iodine. At equilibrium it is found that [HI] = 3.53 X 10'3 M, [[2] = 4.79 X 10'4 M, and, [H2] = 4.79 X 10 M 21%) “-— 12(g) + H2(g) If 1.00 x 10'3 me] of H1 is removed from the container, what are the new equilibrium concentrations of [H1], [12], and [Hz]? (12 pts) '2 Him 3 H 2C5" 4 T 45‘ @ facet/7?] /\ . 51A C' .. 3 W I 0.00353m 0'0“"? 7‘" 0,00,, W q [awass'fl‘dam ,— __ 0 00100 '7‘ If O'Isto -__—_ OtUOUijqFX fix. 0:0002JB +L>L Oar} %: [.07XIob‘f/Vl fj/ 3.7;thch~ m 7 ~‘f _ @ EILU‘ [01:] = 0-000#7qm -— LQ'MID WM. Q E? e; a) i I o O O 3 fl \p E ~1— IN) 25 3'. >5 6‘ f? V ll ...
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