SC112%2012-wk%202007%20exam%20w%20key

SC112%2012-wk%202007%20exam%20w%20key - SCI l2 12-week...

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Unformatted text preview: SCI l2 - 12-week Common Exam Name: Alpha: 1. 5. 6-. United States Naval Academy Chemistry Department SCI 12: Foundations of Chemistry 12-Week Examination Spring 2007 Instructions DO NOT open this exam until told to do so. {in the top of all pages, write your name, section number, and alpha number. On the scantron sheet, write your name, section number, instructor‘s name, and alpha number. Also, bubble in your alpha number. There are 4 pages to this exam (including this cover sheet). The exam contains 25 multiple choice questions. Select the best answer and record it on the exam and on the scantron sheet. There is no penalty for guessing, Periodic Table, constants, and equations are on the back of this cover sheet. Read the following statement: This exam will be given to all SCI 12 students over the period 4 April to 5 April. in order to ensure a fair exam and be consistent with the USNA policies concerning graded academic work, you are not allowed to discuss ang aspect of this exam tformat, length, content, eta! until 12 April. 5C1 l2 — 12-week Common Exam Marne: Alpha: Periodic Table of the Elements HI = 6.fl22l4 x10” ml" H ”3“ . R=e.eazeeLaImmuI-’K" R=E.314Jmol"K" 5:“. ifililfl I: I3 I! I6 I? it 15:»- IIIIII III'IIIfl-‘l 30313?“ mm 35.112? :II'JIII n-I'I 2| :4 16 2!. ‘15 36 ll 31 1! 35 M Sc Ti Fe NI Cu Zn Ga Ge As Br Kr HIE”! Ea“ .9591!) 41.!“ SUN” Hf!“ 54333:! 55.“! H.933“ 3:!“ £1.14! 55.311 “.123 T1.“ Mama: mm [3.” H 15 41' 4i 5!] 51 31 54 I? III Ma IIIIIIIIIIII I161 1m“ 9|!“ m“ 95-9"- [HJ “II-UT 1mm I342 "I? It III—III itlflfl LIIJH III-60 III—1i 55 55 51' 1'3 Ti 1-! T5 I5 1? 'II III III II E I! H I5 It I III—NH! 1.31.32? new: I“ 1M9“! In.“ 135.311? “0.23 Imn I953)?! "63655 no WEI IIJI‘J mam: {1119} me] I1 ll 39 104 IE5 IN 1111' I“ III? I11} ll: Fr Ra II If m, s M III-$- 1311} m6} [111'] nil} {“11 I W) I355} 0-H] W] (111'! III Ne IEIIII? I‘M-51'4- [SHIN 1m: 2M?” 5a :9 III III. e: a III 1 '- I- 5| ill 71 I411” mm“ mm II-Isj Isms mm um ”LII mm: mu “”341: [13.04 mm III: III In I: III 95 I» III In I» III III: Th Pa U NI} Pu Am Cm Bk Cf Es Md 1' mm mmm mum a: [2441 [143} r- T} v I} I?!” Rm r {am {293 - . E Kw = [HT-[DH] = II) I III” {at 25°C) new = '5'?" {at constant T} KI-KI = Kw me = - lug (KI) as” = ‘fif‘fl pH = —Iog[H*] pDH = —]eg[0H'] “Swim: = 35mm + fiSsum-ndznss PH + NH = 14 {at 25°C) M” = Z *1 *3°(Pmdum} - E m +S°Irwctants) pKa + pr = 14 {at 25°C) a0 = 5H -T-.II5 £6” = are -T-.£IS" _ [hm] = . ° _ . ° pH — pKa + 10g [acid] Zn IIIGf (pmducts) Em 11G f {reactants} + as = M3” + RiT-In ea ionization 1:1]: xlflfl Q EIG°— — FR-Tran'” E“: = E” cathede — E'" made a a: mil: } redI: } an=_%H (9“: Egg" = PM {cathode} + Puxianede} SCI 12 - 12-week Cflmfllfln Exam Name: Alpha: 1. Which oftheae aqueous solutions would function as a hufl'er‘? a. 1-0qu and HCiOl h. HE: and Br‘ c. HCN and CH“ d. NaCIH and HCl 2. What is the pH of a solution that contains 0.500 M NaHCU; and 0.300I M H1003 (K. = 4.3 x 10”}? a. 059 h. 2.22 c. 6.14 d. 10.4? 3. Which of the conjugate acidrhase pairs would he the best choice for preparing a buffer with a pH - 5.0? a. Hfifly’i‘iaHCD; 13K. = 6.3? b. HC1H301MaQHgfl; PK. = 4.74 e. Nanzsomasnro. pK. = 1.21 a. Nalnsomawo. pK.= 12.4 4. If 0. I 3] moles ofNaUI-i is added to a [.00 L aqueous solution of 0.332 M hypochloroos acid (H.001, K. = 3.5 3: I04] what is the resulting pH? Assume no change hi volume. a. Til-i h. 3.43 o. 5.50 d. 3.13 5. A student carries out a titration of a {{an solution with a Nam-IE...) solution. Which one of the following is true regarding the pH at the equivalence point of this titration? a. The pH will equal 1". h. The pH 1tirill be above T. c. The pH will he below T. d. The pH will equal thepKiofI-IF. 15. What volume of0.336 M nitric acid {W03} eolun'on is required to completely neutralize 32.3 mL of 0.135 M NaDH solution? a. 13.21113. 1:. Blfitni. e. 2.49mi. d. 25.0mL SCI 12 — 12~week Common Exam Name: Alpha: 1". For a buffer, when the concentration of the acidic component is equal to the concentration of the basic component, the pH will be a. equal to 'i' b equal to the pK. of the acidic component c. equal to the pK.J oftiie basic component d. equal 10 pm 3. In which of the following solutions is magnesium carbonate {MgCDfl less soluble in than it would he in pure water? 3.. 11“} M END} b. 111$ M NazCU; c. {1143 M CsHD; d. 1114:} M HNCIJ, 9. In a saturated solution ofCafiJHJ; at equilibiimn, the concentration of calcium ions is 131.015 M and the concentration of hydroxide ions is {1.330 M. What is the predicted value ofKi, for CHLOE-1h? a. to x it!" e. 1 .4 x In"5 c. 4.5 it 10“ o. 9.23510" ifl. Determine the value offiG at 25°C for the reaction. 2 Hmm r. Ngoirg} not is -s.4o H mm no2 Leo N104 one a. - lflflflki b. —4.soio c. +8.33kJ d. 46.44k] l 1. Which of these processes is expected to be accompanied by the largest increase in the entropy of the system? 3. H10 {L} —r H10 [3] b. H10 (3.} —r H30 [5] c. H10 {5] —+ H20 {E} :1. H10 {5] —+ H10 {g} SC] 12 — 12~weelt Common Exam Name: Alpha: 11. A reaction {system} is at equilibrium: at a given temperature when a. fiE’U b. fill-I‘D c. £510 at. $5313 [3. A reaction has a fill-I“ value of +4913 It] and a £53“ value of +13. 14 kitK. Under what temperature conditions 1will no" be negative? at?” will be negative at all temperatures. so” will be negative at temperantres above 35!] K. nos will he negative at temperatures below 354:} K. no“ will be positive at all tamperattnes. 51?er 14. The aos value for this reaction is +3633 it]. What is the value of the equilibrium constant for the reaction at 25 “C? Hamlin} ‘-'~ H‘tan + HCDa'tan a. seals—7 a. 2.4mm c. 1.1mmJ :1. Teams“ 15. Calculate the no“ for the combustion of propane at 25°C. | CaHeifil + s 01th —»3 Cflzifil + 41st: to tone-— '1311 a. r2108kl a. -fiSSkJ c. amass s. “asset ‘tfirhiatuldent mixes a solution of lean ions (Plath) with a solution of sulfate ions {5044] and. a leaiflI-l- " sulfaterPESBfl—pamifiitate forms. Which of the following statements is figmtfor-flte'reaction? -~—. —~—.._\____ _ _F__,_.— a. oisgreaiermau Ka- ' "__‘.'.-.-.=-»-:':'.T.'._' b. Q isless than Km. " i"“'--‘ ---.._ e. Qisequalto__K,Fr—---""H__ _ -. __ -. ___ thug- is tqfl'eii to zero. flaw {Sluté ”Thai '3' SC] 12 - 12-week Common Exam Name: Alpha: [7. Under standard conditions, at 29% K1 o5“ = 482.3 k] and EH" = 449.6 M. The reaction below is: MENU: {iii} —* N10 [3] “l' 1 H10 {E} exothermic and [amount-favored {spontaneous} endothermic and modulo-favored {spontaneous} exothermic and reactant-flavored (non-spontaneous} endothermic and reeetaot-fivored [non-spontaneous} 9519's“ [3. The following reaction at standard state and at 298 K has all“ - —3'?.E 1d and K“ =- {1315: CH3'UH {U + Com} —* CH3C01H {E} What is the value for $5“? a. 436 Himol-K] b. 2.85 Mmol-K] o. IE? JJ'IImol-K} d. -5I5.| itimol-K} 1: reaction shown below. is the oxidizing agent and is the redueiog agent. Znts] + 2 H‘ tan e HiiB} + 21121an 19. // 2i}. When this oxidation-reduction tion below is balaneed in eeidtéolution with each substance beefing the smallest whole number ooet'f t, the ouefiieient forfliefiaq} is: Mum-{am + Fe {5 —: Mnfiafi+ Fa” {no} a. 2 it": b. 3 -‘ N.“ o. 4 walk ti. 5 . a 21. Calculate E“ for the reaction‘fiemw. given the standard reduction po ials E’t'NiHMi] = 43.23 V and 94:26an = 41% is?! W ‘_.,*';Ni!‘taq}+2o{s] -+ Nitsl-t 2:111an \} L‘a. a. -l.{ldlK 1.. b. -o 3*»! Hm o. .. .48 V “N f/dlf +1.04 V .x’ 5C1 I 2 - 12-week Common Exam Name: Alpha: . Idontify tho strongest utilizing agent. / Table of Standard Reduction Pomotlals Wm {21 + Zo' -+ 2 CI‘ mi WEE—HM its] ; Cuts} Nifs} ; mo} SC112 - 12-week Common Exam Name: Alpha: 24. In conducting Experiment 32: Buffers, a midsiu'pman prepares the following two solutions: Ifl mL offllflfl M CHyflflflHtjaq] lit ml. offlflflzuu M CHfiDDHta-qj + + l'EI' mL offllfli} M CH CDDN a JD mLofilflilEDfl H CH CODNa =- Upon the addition ofE drops urea M HCI to time solutions, one should expect to exhibit a smaller change in pH hoeause . Solution A; it has a higher buffer capacity Solution A; it has a lower buffer capacity Solution B; it has a higher buffer capacity Solution B; it has a lower buffer capacity PF?!” 25. For the reaction Fe+1 taqj + SCH‘ {an} -? FeSCITZ {no} the foilewing graph was obtained from the measurement ofequiiibrium constants at neveral temperatures. What is the equilibrium constant at 215T? In K V3. 111' plot 5.15 5.10 -- I one 5 son 4.95 y: 905.39: + 139i}! 4.90 1 9.013335 0.003443 nooata 0.003513 0.130355 0.1313355 1rr {K41 a. 45.33 b. 38.15 c. Hit? d. 4.932 SC] 12 Spring 2W? 12-week Common Exam Answer Key C A B A E ‘PWH? $mmm} m&% ma ISJK 19.1} 213.12) ...
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