TEST 3 - CHEM 1212 Test 2 Form B Student Make sure that...

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Unformatted text preview: CHEM 1212 Test 2 Form B Student: Make sure that your W are clearly printed on the Seantron form. Each multiple choice question has one correct answer. Buhhle in your choice on the Seantron form. You may write all over the test and the scratch paper, but only the Scantron form will be graded. l. ls the rate of a reaction determined by the fastest step in the mechanism? ‘03 filamursH' 54%.? 13. yes 2. Is a reaction intermediate a species which is generated in one elementary step and consumed in a subsequent elementary step? A. no 3. Suppose a first order reaction is carried out with water as the solvent. If some water evaporates from the reaction vessel, does the reaction rate increase? A. no “ta-mi:- {T “do. @ liven-wot. Cflficflhlc r 4. For the reaction A —Jr Products, the reaction is zero order in A. Is the reaction rate equal to the rate constant, k? c it no (on. 1 9K 1: A1 «as- a 5. Does the half-life of a second order reaction depend on the initial concentration of reactant? A. no ,J/ff ta 7' Mm" a. Is it true that the greater the activation energy, E“, the faster the reaction? 5.51am]? Fflné'. E. yes i Page I 'Jf ffifir}:*‘w Ell-take tch corresponds to a potential energy,»' maximum on a reaction energy 3". Is a transiriorr stars a species A. no . yes f1.“ prgfi 'l' 1"!“ 3. Do the units of the W depend on the order of the reaction? “5; Jpn sea-5975' @ Bar at asst-ri B. yes 9. Are terrnolecular steps possible but improbable? A. no it]. Which of the following is N01" a reason that reaction rate increases as temperature increases? A. the number of reactant-reactant collisions increases as temperature increases B. the fraction of reactant—reactant collisions having an energyr greater than or equal to the activation C. the orientation probabilityr factor increases as the temperature increases 11. A reaction has the following rate law: Rate = nnjrsf In experiment 1, the concentrations of fir and B are both [Lil] moi L4; in experiment 2, the concentrations are both GED mo1 L'l. if the temperature stays constant, what is the value of the ratio, Rate[2)iRate(l)? a. 3n 1” B so arr—5.1. QXLL“ ”(a 33 . . _______—-- _________._————-—"':I c. an {mi , iii-it fits i) n. 13 — E. 2? Q - 1‘} _.- Page 2 12. A start-ir of the decomposition reaction 3R5: —3r,3$+ 63 yields the following initial rate data initial [Rflgflmoi 1:1} ___ isiiiai m‘ rate [moi-i [L - 5]}: one ' fl.fl394 . one also (has-n i3 ”VAW‘ l3 me ”3 5 s. l H fl.35fl 0.214 rm W 3L E its {5... uses ones ._-—r— r. M was a. 32. ER“: :3 3 . a M 1|i'lii‘hat is the rate constant for the reaction? ELSE _J tit": \ 11nd,; E! 35! U a. -' -1 ‘3' i“ DfllflBLmols 1 n5 : (I-HEAJ 3. c.2453 Lmol'ls'l m T. 1.. C. 11511 Lntol'js'] G. Li? L mol'ls'] _ _ -— _ c.5'flal“\ @) ostri- W‘i’fi 13H“ l3. Consider the following reaction saig) + 5mg} -} soig} + 613(3) If [C] is increasing at the rate of 4.0 tool L"s'1, at what rate is [B] changing? to} i rib-[£1 Wont _. v2; err ~= a, 1'? in _ _ “H __ S c; .. i, “Mom , M C. —4.{lmoll_'ls" L ‘e NV D. 45.4 mol L'ls'l 15.1353 .. _. 1.5 5- ff— .- 2; '3: 14- The rate constant for the reaction A —3 Products is 4.65 L mol'ls']. What is the overall order of the t‘ 'i' H W" H _ i. ”3‘“ is” Ms. i at rm 1, a a a A. zero a”; 1' A “a B. first 1%" Mfg, _: lit M .} Bk: {In 5 t C. second :3 D. third E. More information is needed to determine the overall order. 15. For the reaction sing) + 2mg] —) 2Cfg) + 213(3) the following data was cdllectéilateonstant temperature. Determine the correct rate law for this reaction mm meant] Initial [a] W Esta ”‘1 I‘ t {11mm [moHL] tmnltflzminll when 1" AH“ T 1 0.200 mm - 5.0th we as; swam? “5’ RA 2 tl.ltl[l also 1.5mm"? '. “a a’M' 3 13.260 case [2.3 x m1 + E -. -1 E s t- 4 cans [1.21m 2.Tfl><1[l KM g was Vie!- = rail-1n AM a. Rate Hana] . vs”!- arch-r 5n 9. 3- Rate = new? C. Rate = aafmf D- Rfltffieiiflj Jam = Hafm} ' 16- The reaction 2 C4Hfi —:. Cal-I]; has a rate as of rate = 0.014 Lambs) [am]? What will he the concentration of mm; after 31} hours if the initial concentration is (1.625 M? h. _ t i Q) flat - M 4* am y- ascent :fa.o-~t)[10‘6w} 4' o-fi'l-S (3.433.; , E.fl.flflflflM IT. Tetrafluoroethylene, Cqu, decomposes to give products. A plot of l![C2F4] vs. time gives a straight line with a slope of [112F443 L muffs-II What is the rate law for this reaction? r @ga-EL _ Jfi L5} 915‘”. ‘3 ‘“ is" ‘ a a. Rate = on44s (L mol"s"}[c2F4] mfg 2k _ _, " up)" B. Rate = 22.3 {mol L ls)[C2F4] * “m ‘3“: (a, C- Rate = {113443 (L mfi'fimgsif 3-?- 'J' D. Rate = 22.3 (mm L" s)[CgF4}2 E- Rate = 0.0443 s" ['2ng Page 4 13' The decomposition of hydrogen peroxide is aflorder process with a rate constant of LUIS 3'! lfl'3 min". How long will it take for the concentration of H102 to dncp from flflEUU M to {H.fllltl M? .k a. . En}.- __ _ .312. 5: A. 1mm 3"“ EPA; II E. 155 min a 1 D g, r; .- 3 i L -- F ' (C. 431 min ".- aa‘LL- ) - _--" Ill"hill n. 4550 min ELM; a" E. 31,4oo min " 19. The rate law for the reaction 3A —} C is Rate = 4.36 x lo'2 L Incl" hr"[A]2 What is the half-life for the reaction if the initial concentration ofA is 0.2511] M? A.fl.fllfl9hr pr, 1n}- crel-u 3 2%?“ = flacflla __ _H" a. mason F 1““) C. ljtghl : E-'_1.‘)LOI (_qfi’lia D._23.9hr EH.- aif'} if 2'1 The rate law for the reaction 3A —> RE is rate = HA] with a rate constant of Mil-44? hr". What is the half- life of the reaction? 1'53— H r” c: . E‘F 3.’ M A. o.o224hr Jr V =- f “I «‘61 a. comm * (E 15511;} n. 22.4w E. 44.7w 21. A reactant R is being consumed in a first—order reaction. What fraction of the initial R is consumed in 4.1:] half-lives? I: if}: ,4 ,r-——~. .JL, ____._—— : —1kx - w Elk-1s B. . 53W“ c. or: a. o. are k __, SWL/k.” E. aces )M L” L135 1 ‘ f" (Ur are“) case an, ”la—3k as“ c E? 1 a “a D.‘13?L?Pas=5 li: a DEE-L: .-' 22. 1What is the molectdarity of the following elementary my? NH1C1(nq)+ OH'[oq]I —; NHC1'(eq} + H20“) ..- Q Where‘s: A; unimolecular 5mm ____..I-r e. bimolecularfi‘ . tennolecuiar D. tetramolecular r E. Need to know the reaction order before molecularity can be determined. 23. Ammonia will react with oxygen in the presence of a copper catalyst to form nitrogen and water. From 43?.5 K to 4521} K, the rate constant increases by a factor of 4.27. What is the activation energy of this oxidation reaction? [R = 8.314 E - 3 kamol ] he a. .,. E a... I n '- j 9,... 1; t- T C 4: 4r. A. 24.5 lrJa’mol ”En. (if _ ’1’, a _ C. B. 165 Mil-hole} 1N ”“11 ' R ll“ 437.: c. 242 lrmeol n. isso th'moi g... :- re s E. a lfl4kamol 24. The decomposition of dinitrogen pentaoxide has an activation energy of it}? Irifmoi and mm = + 55 k]? mol. What is the activation energy for the reverse reaction? — . E"- T whence i. as J, W a C. 1755 kamoI D. +102 kamoi ye 1' 5 S- E. e 4? th'moi -’r v» "i 25. Can the rate law be predicted from the stoichiomenyr of an overall chemical reaction? E. yes - 26. Suppose a reversible reaction has K: = Li] E - 45?. arbitrary amounts of all species in the reaction [i.e., all products and all reactants} are placed into a vessel. Can we state with certainty that the reaction reaches dynamic equilibrium very slowly? hi9 3%" aw .35 -'* *5 frame 1:“ *Hl- WXNJ so)". .Jse 9’” PagetS are" 27. The reaction quotient, Qt, for a reaction has a smile of T5 while the equilibrium constant, Kc, has a value of 195. TIWhich of the following statements is accurate? A. The reaction must proceed to the left to establish equilibrium. _,_.—-—-—~—._._\_\_|___|_n_-_ LE C Mt, E f s. K a. Wmfifomfim: G. a C. The concentrations of the magnets wiil be nmeh smaller than the concentrations of the reactants when the system is at equilibrium. D. The rate of the reverse reaction exceeds that of the forward reaction. E. None of these statements is accurate. 23. The equilibrium constant for the reaction of bromine with chlorine to form bromine monochloride is 53.!) at a certain temperature. Brats] + Chis} 7"” EBICHE) What is the equilibrium constant for the following reaction? .r t 1r" BrCng} == confiscate _ F\ a. 2.97 x 1o" 13- LIFE x lli':i 0- 3.45 x in2 E. 33- lflfl 29. 1|Write Hie concentration reaction quotient expression, Q“ , for the following heterogeneous chemical reaction. Fefiaqnsoutaq) == mouse) A. [sateen] cornea-1* 3‘ tFI=“.lt0H'l’ ' [Fauna] C. 1 [Fea * “0H" 3 13- [Hahn-3H"? E. 1 [176+ ]3[GH‘ j Page i‘ 31}. The two equilibrium constants for the same reaction. Kc and KP, will always equal one another Whfll‘t A. all of the reactants and products are gases. in the reaction equation, the number of moles of gaseous products equals the number of moles of gaseous reactants. C. in the reaction equation, the number of moles of gaseous products is greater than the number of moles of gaseous reactants. _ D. in the reaction equation, tliicnumber of moles of gaseous products is smaller than the number of moles of gaseous reactants. '- E. in the reaction equation, the total number of moles of reactants equals that of the products. 31. Consider the reactions of cadmium with the thiosulf'ate anion. All”! e (L “i “"- ’t‘ . 54L ~31“ Cd2+{aq} + 32032 {fig} "1 Cd{3203)[fl9}; K] = 3.3 3‘ ll]:I e «*5 E“ “if“ _ E- Cdtszcatao + some = Cdtszcnf {as}; at = 2.5 X It]2 the watt K“ What is the value for the equilibrium constant for the following reaction? :2. it t : 9- ‘ E 1. ‘l-' Cdttae + 2320321an *1 catszcnftaq} A. UJJE-fl B. 33 C. at a to” D. as x to3 E. 11):“? In" 32. A mixture of llfiflfl mol of bromine and 1.600 mol of iodine is placed into a rigid LEIGH-L container at 353M], Bet. + I L :1 1 "J: Eur fl {1 -- [filfifl I. L «- l_".._:|-'—El LICID Er;[g}+13{g} =-= EIBI[g} ' "'1'.“ ' 1 When the mixture has come to equilibrium, the concentration of iodine monobromide is 1.19s M. What is the equilibrium constant for this reaction at 350°C? 1-.- A-sssmo'i QJWX i 231; [5.1.24 fl .00 c.1.4? Gaff)“ o. 232" .325 Page 3 33. Ammonium iodide dissociates rain-termini)F to alumni-a and hydrogen iodide. NH—slt-t] ‘1 WEI-1(3) + HI[s1 At 4DIJDC, Kn = [1.215. Calculate the partial pressure of ammonia at equilibrituu when a sufficient quantity f i ‘ d‘de' h tedt 40TH o ammoniumio 1 is an o 1f 1 0-1,”; -.. Q?I-W§\evc Q? “In“: ‘I. A. o.1o3 atm . = is B. [1.215 atrn ' o. [1.232amt _ K 7' Edie: atm E. 2.flfl atm milk-1t dim 34~ The equilibrium constant, KP , has a value of 6.5 K [[14 at 3(13 K for the reaction of nitrogen monoxide with chlorine. 2ND[g}+Clg[g] == 2NOCl{g) What is the value of KD?[R=fl.fl32l}5Latmi (moi IQ] _ An'fi. a. 15 x11}? lit. ' if“? LET“) j". E. 6.55:1{14 : {p.gEr‘i{“°% 1H; 4K Ear-Q: C. Lsxto'i _ mm; D. 1.? E. none of these choices is correct 35. Nitric oxide and bromine were allowed to react in a sealed container. 1|When equilibrium was reached the following partial pressures of three gases were measured: NO: [1.526 ahu; Br}: 1.55|I atm; NOE-r: 1153 atm. Calculate K], for the reaction. 2ND[g}+Br2{g] =—* anonnzg) '- I 31.! am -' .5 A. “1.45 x 111-3 ('3',- fr’“ "r E.t1.lfl9 #7” £10 :3. ass (Lo ‘1 i n. 91.3 _ E. 134 3 Page 9 315. When a chemical system is at equilibrium, A. the concentrations of the reactants are c u .: ncentrations of the products. E. the concentrations of the reactants and products have reached constant values. (3. the forward and reverse reactions have stopped. D. the reaction quotient, Q, has reached a maximmu. E. the reaction quotient. Q, has reached a minimum. II. PRUE LEMS In this section, you must flow ALL your work NEATLY, fig correct units and correct number of significant figures. If you Willow ALL your work, or if I cannot mil your work, you will [one II pahtx. {15 PH) [1) In a LSD-L vessel, 0.13945 niol ofBrz was heated, causing 1116: following reaction to take plans: Br; {3) = 2 Br [3] 3n. -. n .a no N- g. ‘5‘!" a.fl£3¢ ‘Y— '11 The reaction Kc is 1.10 E — 3. Calculate [Era] and [Br] at equilibrium. [ Note 1: Ii-Pay careful attention to significant figures. Note 2: No slingfim ‘ assumntions will work hora. Solving a Quadratic guafion is nocessag to solving the Emblem] L 2. {2.1.} 5% .— ________..——-—'-_-_-— q... IWE“3 - , l a ot3¢-r- 96510 '* *1“ ..-_l __ LIDE" u -tfizE-f *0 ufir+1WE'gi b* nirfim° .. ;_"__n____—-aa-“‘ "L '- f DID YDU SHOW ALL YUUR WORK? {1"} Dis) (2] The oompound RX; decomposes according to the equatlon AB in 1:3 .1 sexae R+ n2x3+ 3x2 “tween- ’3, Ar in an experiment the following data were collected for the decomposition at 1DU°C. What is the average rate of reaction between 2 s end B 5? its} Iflzglimol L41 In use 2 (IE? - - c p.41 ' s 0.33 1J3:- o.£73m 9/) 1: £2.qu M/f: 12 oeo M, 3 14 ms (.55 .. LE '5- Show all work, use correct units, and correct number of significant figures. g- 3} "For the met-ell ehenfieal reeefi afi‘ A + 23 filefnllnwing mechanism hue?” _ .. -._='-.J. WA: A + -' ' = ._._._. k4 ' ' _._. - k; W: Q + “a -* 13.? 2C Derive an expression fer-fie rate law. [Recall that the . general form - ' rate- m- [31” Your "1:” _. line rate _= II_|.__.-'t h; “reused as I funeflun '-' ' for E e lnflvi-duel am You will need to include values fur Eli: your rate law expresslnn. Clearly shew ALL your work.) (533., 7- &1 Eta-3t Bhl\ eerie} me: x... Emanuele pm... an“ “laugh 5L1: Jag—516:5 3 &-1 fa“). ...
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