Exam I d

Exam I d - {fllliiltiistrlii 1302-2, 5 Spring Exam 1...

Info iconThis preview shows pages 1–7. Sign up to view the full content.

View Full Document Right Arrow Icon
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Background image of page 2
Background image of page 3

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Background image of page 4
Background image of page 5

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Background image of page 6
Background image of page 7
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: {fllliiltiistrlii 1302-2, 5 Spring Exam 1 February 20, 2002 1 Name - . i' ' - _- 11.? Jr Section #2 #5 Mulu'ple choice {3439i I] l; gaghi. Mark your answer on the scantmil Be careful to erase completely if you change an answer. Only the scanner: will be graded. Check goufianswem; don‘t be careless: I. An aqueous solution containing 1.00 g of bovine insulin ( a non—ionized protein) per liter has an osmotic pressure of 3.1 min I-Ig-atl 25°C. What is the molar mass of the protein? _ _ A. 500 gshei '. i t .. s. as - - - “’- " f . 6.0 it lflsgi‘mol 3 i : ___._ x C. 7.8 x 1'5)3 gfmol i -_-, D. 340gi'rnol -- __~_ . .' none of the above. " 2. Given K. for /oii/gi + 03th K is + £13 and Kiifor [Cloigi 1306 S [Clio + 03g], what is Kfor CiOtg} + Q: {g} C].th + Oats} ‘? A. UK. 3. mm.- C. Ki-KH KiKKji {E} KiJ'Kii 3. Which of the following is the conjugateflcid org}? 1%. o:- _' 'E__ .‘i _- -‘ B‘ffiifiv .- -- f" '_ flake. OH" ' . :r i .n. (DD 02 E. none of the above 4. Consider the following gaseous system at equilibrium at 2300K: Nets) 1 i0: is) C 2 NOigi K: = 1.7 x 10-3 Calculate KP for this reaction at 2300K. R = 0.082116 L-atmi'moI-K 1.7 x 10'3 I. I. I U a - . C. 9.0 x Iii"5 '— o. 6.0 x m5 E none of the above is 0.0l94 g sample ofan unknown substance is dissolved in 2.135 g of benzene. The molalit'v of this solution, determined by freezing point depression. is What is the molecular mass of the unknown substance? '5: _ -— r- | I' A. 327 gtmol -_ _ _ i if a _ _ ' |796 gtmol ' i ' 533 'J F ' C. 1630 glmol JET-'52: - n. :22 gene] I r - - ' r E. Not enough information is given to solve the problem. .: , L ' ' ' 6. Equilibrium constants (Kc) have been determined for the following reactions at 823°K. in o: {g} + NE N; {g} no is} K“ = 56.4 x 10-1“ { _.._..J_—~n 'i 02 {g} + 2 N: (a) 2 N20 {g} [id 5.3 s [ti-315 ,J Calculate the Kc at the same temperature for the reaction N20 is} + “2 02 {s} 2 NO {g} KG 2 :i . A. 4.2x101? ,_ - f _ I I -: ,I t. “Egg 1.? Kill-13 .. . z._ I._ -._ C. 5.9 X 1012 HT: t- r“ Q 4. rt? : ' _ I'll-j D. I. ‘0.“ I, . -_. 1 E. none of the above 1 -:' .- Ila-1:3?" ’1' r I _' . ..- 7. Consider the gaseous equilibrium system below in a 2,0 L flask; 2 NE}th + (13th -..—-— 2 NOCltg] /. _. __,. _. if the volume is expanded to 3.0 L. A. there will be no change in component concentrations. 1" _ the equilibrium will be shifted to the right producing more NOC‘l. the equilibrium will be shifted to the left producing more ND and (31;. D. the pressure of each component in the system increases. E none of the above 3. Consider the following reaction where we start with pure NOCI: If, initially, [NGCI] = 2.!30 M, and. at equilibrium, {NOI = 9.66: M, what is Kc? A {116 W- 2. U‘DM - if? a B. 0.21 ' '1 V :2 a a 0”“ I'i- Bil .iois .33 0.030 E w: a E I MEN 3 E. — — i": —“—'_'_ ___.___.._— A Z _. __ _ ._. PI rd none of the above I f: r: 2 El. 2 II. I H 3 L9 I_._ x _.-"Calculate the concentration of an aqueous KOH solution that has {30H 2 3.50. w a. 3.2110'“ 3.2 X 10—4 - I C 1.0x 10']4 n. 3.2 x 10—10 E. none of the abo'Je 10. Which of the following salts will cause a basicsolution when dissolved in water".l 10103 M33 J - " Fifi: -- r-.J.-:'.i§+ B. NEBI" _.’_ r. -.. -: In; I :If .- .3 Hr} span-er” RhF - _ - ' a _1 1. WhiCh of the following interactions is the weakest? "53%. induced—oipolefinclucedndipole ionfdipole dipoleldi pole D. iom’ion E. ionfinduced-dipole 1 2. fimsystern has reached equilibrium when the forward and reverse reaction rates are equal . E. the concentrations of products and reactants are equal. C. the forward and reverse reactions cease. D. Keq for the forward reaction equals Keq forthe reverse reaction. E. Both A and D describe systems that have reached-equilibrium. . - ~._fi____h_|-_I‘_II {ha a“ "‘- Fzgl'i. Ill“? Twig-- 53 fix I ,_1 If the tnole fraction of neon mixed With oxygen is 0.3-3, how many gray of.ne.on.are {fl 1 in. present in 42 g of the gas solution? _ I . _ “ ._ ' E) An 20 Eli-"If Eli I9 3 xii-fax? fl :2- ; 3 3 “i tifl—Yl'i"';;?—"—'_' . iii- " W‘ 'i-i‘i' ' (5‘? '-"_!-'I.I.1'..-_I_;.ri If? r"! _ ‘I 5 “I: - 3'";- \U C. 5.0 " ' _- X t“ ,5. 3 D. 16 . _ _, 3‘ ~ '. ' E E. none of the above l I :37 :3 F" a _ *7 5;; .5. I rag: I "' i f? -" g_ __'I ._J ..-_'_:,-3- r. r: j _ 1.9- l- I :. : l- ' The complex cation [Ill‘o(H2Cl}._tj2+ is pink in solution. The complex anion {CoCm} is blue. For the endothermic reaction (forward direction) below, which of the following 1'? might cause the color of the solution to change from bin to pink? h - 3 . [CO{H20)IS]2+ {an} 4 Chtaq) [C0§1j_ (aqj +' 6 H20 [ll " «it A. Heat the solution. B. Add a catalyst. C. Add some Cl". 9.» Coo! the solution. E. none of the above. l 5. How many of the following are classified as stron acids? 1:15.», "I: .1. HNQ2 Hth3 BC] I I 't A. B. t} 1 2 3 4 1 6. What is the molarity of an aqueous o-chlorophenol, HOCfiHttCl, solution that is found to have a pH 24.36 't" HOCGPLCKaq} + H300) H30+(aq] + 'OcsttChaq) pKa = 3.49 A. 3.2 t Ill-QM 4-5“? ,2? .t 2 2 tar-fl 5.9 x 1mm 2. i- -- v" tr ‘“ ‘ C. v.6 .t Ill-13M : o. 1.4 t to-sttt um . - .- ‘* {Tia '1_-._ E. none of the above ' ' ' M —.. ' {a -. '- ‘ll III": II ___H 4,345 I. 17.‘ A 0.10 M solution of hydroeyanic sets has a pflgfi.fi._10. What is the an, of CN' '2 1.6 x 10‘5 _ - 3195;“?- germ-“l”? --= a 5.0 x 10-12 . at: 6.3 X 10'“) l ’3qule"‘” D. 1.4 a 10‘9 . . w "‘9 _ |I _t-._.._.l:} I ’2‘ x1fi-” E. none of the above --~-~--*'“""** .fi L"' ‘ “ ’. tnr‘lfilfif “30' l”; . rflqq‘l 1,6. .. 't' at r. -. . .ut-E . ,. i. til '1’“?!- if: -‘.‘\};.'- j gist :;‘.~' .1: .Whfll. is the __[:_iI_-I_ of a solution made from 50.0 mi. of 0.20 M HCI with 100.0 trtL of0.10 M NH3? K1, for ammonia = 1.3 x 10'5. A. 8.4 - ' ' _ 5- __J =__'-__ if, I.‘. I at 6-2 . . - -. . .: 3.3 I -- _ b ' ' __ _ i _h E. none of the above ' _ I. - I 19. KC was found to be {3.0 a 1034 for the smog-forming reaction (:13 tgi + No {g} o2 {gt + no: ta}. 1110ng 1.0 I»; are M, [not] : 1.0 x 10-3 M. 10310 = 8.2 x 10-3 M. and mo: 1.. = 2.5 a 10-4 M. then I A. Q; a: K. the equilibrium will more to the left. ' QC a: K, the equilibrium will more to the right. C. QC :- K. the equilibrium will more to the right. -- f - '- D. 0.; :2» K. the equilibrium will more to the left. '3 .’_'.': ' i E. QC 2 K. the system is at equilibrium. , '- 20. hieh of the following has the ionisation? W A. one M nitrous aeitl: tea : 4e ii iii-4 : ' a E. 0.1M aeetieaeid:1(a: 1.8 a 10'5 - " _ ._ 0.02 M ehlorous aeirl; KH 2 1.2 it 10'2 /'-' - D. 0.] M ehlorous aeid: K3 = 1.2 s 10'2 r E. 0.02 M hypoehiorous acid; K:l = 3.5 it 10's . ‘ ' " " ""3 t 2 1. An aqueous solution of_s_odium§};anjele is found to be basic. Which of the _ following reactions explains this faet? “rear-4W ram 3 (reg—“i a..__"“" House" +-----onrraqi B. -HCN-taql----+ Hagar—sew; 110* £an + ---E}N?~-{aq} G.’—Na*"{aqi ~+— -- --H29{1-} —--.——-——-- -----Nal-l {sq} + "Gilliam ® NaCNts} + more ' NaOHtaq} + HCNtaq} E. none of the above 2.2. What is theR_I-I_of a solution made from 100.0 mL of 0.100 M pyridine (a nitrogen base with KLh = 1.4 X 10'9), and an equimolar amount of 0.02.50 M HCl'? {13;} 3.1 3.4 C. 8.7 D. 5.3 E. Not enough information is given to solve the problem. f E Fluoroacetic acid occurs in one of the most poisonous of all plants. A 0.500 M solution of the acid is found to have a pH of 1.46. What if the Ka of the acid? {Are your alarm bells ringing?) #— A. 5.9:: 13'2 "J 3' . .- 2.3 x 10-3 F". ‘1. C. 2.2x10'3 V”;- F’ ' D. 7.2 x 10'4 E. none of the above 24. Reserpine is a natural product which acts as a tranquiliaer and sedative. When i .00 !_ tesoi‘fiine is dissolved in 25 .0 g catnphor. the freezing point depression is The melting point of camphor is 179.5°C. The reserpine__i_s dissolved rnelted camphor, and then the meltinggoint of the solution is’deterrnined to obtainétf. 1What is the molar “glass of reserpine? {Kr for camphor is 40.0 °hnolal.) A. 1.6x102gfmol _ . g _.»__ - a. 0.033 gltnol “3 w . _ - .J-f - w 6.1 x 102 glmol "Id " ‘ D. 114 gimo] "F to”? '- r} J K _ E. none of the above I"? '" if L g ;-_ .I A < l mo; - --{, H . ' ' (1161.5 .Jte gotta : ’1' 25. In which of the following for 0.100 M solutions of each case would the pH be the 9 lowest? w: ‘a 5" if “ a. hasaKfiz 1.3x10"5- -~ -I"' a 13.. 0.100 M solution has a pOH : 8.5 H 55 ;_' ' 0.100 M solution of its conjugate base has pH =_ 3.3 .- a . hasapr=L9 Kbcmtfi E Not enough information is given to answer the question. "f. ; '-. - Ti ' . ::;._.. fan) to. H v- .3 . ..._..1—--«-r 26. The equilibrium constant for the aqueous reaction below is 2.9 x 101:3 Hi1} (310“ + H30" HClO 4- H30 what is the Kb ::._I,_.:-__| .'_'_, —' t—-! .i C} -__ -- if“ -' . ' .: -, :1 I'N. _fl.wm H” __ _ K a. 3.4 x 10-3 ##4##? " «w 219x101f - Show“ =Vw L . J. ' C. 1.93m-5 : _ 0s: 1' .‘; D. 5.3 x 104 F " E. 10 ' ti] o as x 107 . I. . .. At 50°C, the dissociation constant for water, Kw, is 5.43 X 10714. What is the pH of pure water at 10°C? A. 6.6 B. 6.8 @ 7.0 5‘4?” o. 7.3 J. E. 6.4 28. The equilibrium constant for the reaction of HBrO4[aq] with CsOHfaq) is Q 1.0x10'14 4...; .-_I __ I .I_':+ B. 1.0x1023 = " ' * C. 1.0 x 107' ' 1.0 it 1014 E. 1.0 29. Using equations for (a) the-'autoion-ization of water. {13) ammonia acting as a base in water, and (c) HCN acting as an acid in water, show that the equilibrium constant for the reaction below is a I k I! (aq‘; + NH!“ [acfl 1——' HCN{aq} + N133 (aq) A- Kw KaKb I I - Kw+KflKb ~- - E. none of the above i {a '1 3 ...
View Full Document

This note was uploaded on 04/14/2008 for the course CHE 1302 taught by Professor Young during the Spring '08 term at Baylor.

Page1 / 7

Exam I d - {fllliiltiistrlii 1302-2, 5 Spring Exam 1...

This preview shows document pages 1 - 7. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online