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1. A student must prepare 6.00 L of 0.100 A4Na2C03 (106 g/mol). Which is the best`procedure-,+for -'+ -

preparing this solution?A) Measure 10.6 g Na2C03 and add 6.00 kg of H20.8) Measure 10.6 g Na2C03 and add H20 until the final homogeneous solution has a

;a?i volume of 6.00 L.Measure 63.6 g Na2C03 and add H20 until the final homogeneous solution has avolume of 6.00 L.

D) Measure 63.6 g Na2C03 and add 6.00 kg of H20.E) Measure 63.6 gNa2C03 and add 6.00 L ofH20.

2. What is the lnolariLfy~~6F an Nal solution that contains 4.9 g of Nal in 42.0 mL of solutio>,gp

FX1412Spgl7 ID:A

5. For the reaction of the ammonium ion with nitrous acid, the net reaction is

NH4+(og) + HN02(c!g) + N2(g) + 2H200 + H+(czg)

|ftheinitial;8r;;entrationofnitrousacidisl.00A4and,after45.4_s_ha.sil_ap`sed,theconcentrationof nitrous acid has

0.042 M/s-0.0024 A4/s

0.0024 A4/s-0.020 A4/s

0.020 A4/s

fallen tQftyo=§*£.€4£.what is the average rate of the reaction over this time interval?

i-4 ,rT= f 74E-

rc} , fr# ~ /, Oi) )

#rFFrf i:,,;rSAir;(t=;€§r`

iba

4'J' 6. The followingdatawere;`f v#4~f/PF`5..a

I- ; -,

hypothetical reaction 2A + 8 + products.

[A]o (A4) [B]o (A4) Initial Rate (M/s)-- ::i I

::;J7-.-1` `f\l:,i ---

0.6 0.1f` -45

What is the overall order of this reaction?

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= £`.`--:-if-i-i---:-i:i fd8f i -I 3 ,;ff,E^f:; i f_

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7.```NItrortyr€hlorideisproducedfromthereactionofnitrogenmonoxideandchlorine:

2NO(g) + C12(g) + 2NOcl(g)

The following initial rates at a given temperature were obtained for the concentrations listed below.

Experiment

FX1412Spgl7

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9. For the hypothetical first-order reaction A + products, 4 = 0.0161 s-1. If the initial concentrationof A is 0.516 A41, how long would it take for A toj)e 91.3% consumed?A) 5.65sa) 62.1sC) 43.1 s €- ,::,-=#;A-f8! :=f:a/`\c

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10.Afirst-orderchemicalreactionisobservedtohavearateconstantq±±~i±T¥xpla±isthecorresponding half-life for the reaction?A) 47.2s

f=,`,9===A-Ezi

:-/, - (:`Jif€_?-i=,

E) 48min

11. For the first-order reaction

1/2 N204(g) + N02(g); Aft = 28.6 kJ'

the activation energy is 53 .7 kJ7inol.A) 15.2kJ/mol8) 82.3 kJ/mol

Ca,^i'f#ife#CF2R

What is the activation energy for the reverse reaction?``/

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/

0,±rf `S-:¢^ ;; A :a = r~f--`3 . art /_I-~

L--9r- --L ---- ` ----.--.--, ^-.-

;^4ft =` =3S^,i -at:ri::ie/c-j~

::-=_-I_I_I_-__f€i::)

12. Which of the following statements is true in a reaction system at equilibrium?A) The equilibrium constant is zero.8) The number of collisions per unit time between reactants is equal to the number of

collisions per unit time between products.are reacting to form produ

form reactants. './. G* tf,`j Jl. }r..f,ft I '_±Ff ri,,?ts at the same rate as products are reacting to

I FI I,/a

D) Reactants and products are present in equimolar amounts.E) The product of the concentrations of the products divided by the product of the

concentrations of the reactants is always a constant.

FX1412Spgl7

13. The following reaction is investigated (assume an ideal gas mixture):

2N20(g) + N2H4(g) = 3N2(g) + 2H20(g)

- i? ,.,- / _ i `2. /;22 -a

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14. For the reaction Br2(g) + C12(g) = 2Brcl(g), at equilibrium, it is found that the concentrations

of Br2, C12, and Brcl are 0.3941141, 0.260 A41, and 1.76 x 10-3 A4, respectively. What is the value of

3.01 x 1

5.84 xl01

C) 1.20x|o4

D) 1.71x|o-2

E) 3.32x|o4

Fgr=7~ iAft7fe~ faf rfl`fJ`

a,-` -I I, ( .--.

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15. IfKc = 0.137 for A2 + 28 = 2AB, what is the value ofKc for the reaction1Q'

4AB = 2A2 + 48?A) 0.2748) -0.137C) 3.65

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16.

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ill-iiiE=RE_iEiiiEEEl!Hifr /c;\,jj± ;I: r!,,p,7d3: ~ y\``_i

CS2(g) + 3C12(g) I CC14(g) + S2C12(g)At a given temperature, the reaction above is at equilibrium when [CS2] = 0.050 A4, [C12] = 0.25 A4l,

[CC14] = 0.15 A4, and [S2C12] = 0.351141. What will be the direction of the reaction when thereactants and products have the following concentrations: CS2 = 0.14 A4, C12 = 0.21 A4, CC14 = 0.31A4, and S2C12 = 0.29 AV

A) totheright8) cannot predict unless we know whether the reaction is endothermic or exothermicC) cannot predict unless we know the temperature

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17. Which of the following equilibria would flQf be affected by pressure changes at constant

C02(g) + H2(g) = CO(g) + H20(g)

a) CO(g)+ I02(g) = C02(g)C) 2Hgo + 02(g) = 2Hgo(5')D) 2H2(g) + 02(g) = 2H20(J)E) Cac03(s) = Cao(s) + C02(g)

\)-F2#r-#`;I

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18. What is the net ionic equation for the acid-base reaction that occurs when acetic acid andjg4j±±]aLf rg A= f fl ¢rJ '#-^xp5:*Ff2so of -g,-i- /-}

I.,QH-(CJg) i C2H302-(czg) + H20(08) H-(c,g) + H2C) H30+(czg) + OH-(c}g) i 2H200

-,` --,,J',dr= =->,

•'*2#at._ck;f3,'fy!-->p.fl crf;rf+te

Oifd3'#+i._{st

D) C2H302-(czg) + H+(czg) + Na+(czg) + OH-(czg) + Na+(czg) + C2H302~(czg) + H20(D

E) HC2H302(czg) + NaoH-(c!g) i Nac2H302-(c7g) + H20(J)

19. The reaction of Hcl with NaoH is represented by the equation

Hcl(czg) + NaoH(czg) + Nacl(cJg) + H200

What volume of 0.3 07 A4 Hcl

D) 4.08mLE) 3.26mL

Consider the Ka

is required to titrate 16.3 mL of 0.816 A4NaoH?\

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varhosfyoituhe"ffoflffS=::ar:;;ffi>Cyanic acid, HOCN, 3.5 x 104Fomic acid, HCH02,1.7 x 104

-:::f,:;i;g::-a:cd:£T;#-;#

C) lactic acidD) formic acidE) cyanic

.,.

-`j r;,,,:--ed# f yse

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/.- =`-

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21. Rank acetic acid (HC2H302), hydrocyanic acid (HOCN), and hydrofluoric acid (HF) in order ofincreasing strength.

Acid ftHC2H302 1.8 x 10-5

HOCN 3.5 x 104HF 6.8 x 104

A) HC2H302

FX1412Spgl7

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iEIE

i\jpr/ `

NaoH(c7g) + Hcl(c!g) + Nacl(czg) + H20(/) L3 £€+f=

A) 0.10„ 4ial.prpl9?f`=`3. h, i¢Lt of.A+:a{'.9,/£,J G-A C//--fGL /#``, #L`£-#-7gr€-,j`p` rtif-

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26.Whatisthehydronium-ionconcentrationinasolutionfo/::i:gpedbycombining4L±g±=±±of

:::-£r9;o+HH::tt:9],5L:qivL-a-::{oa.:,o+"H::t]; cchf¢~f24 -j2¥NAR;\o:ti;Oqy'M;:\:Lhtrfaq=F¥::qn±::::t,:'^£;;;p;;::=dffa:i;±£44%g3ap

-Z r`3'f `-r ) i F,st{ /¢r/AI Grfr{fr-` -' -

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C) 0.045A4

`,+,-_iiJ REH1.0 x 10-727. What is the pH of a 0.14 A4 solution of methylamine (CH3NH2, Kb =

D) 0.85E) 2.12

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I Qifif e, ¥# ,,ifty f6,{if 7fi#if ±-A o, oc;77ma© f f i -1-i = €`,£sif e&£ ,SB i:att3Bft?

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28. Which of the following salts is inost likely to form an aqueous solution having the pH shown in thefigure below?

7.00pHMEt.ff

LJLJA) Na2C03 /C)8) RbF /„-G'C) NH4C| /L/'J

/`//`Phi#fl'E) Kcl-I.t-:--;,.,;-;-=-1: -#;? ,J; zz± i ;",„J,.€-I :..``'`...: .

at is the POH of a solution prepared by adding 1.82Water? Kb ofNH3 is 1.8 x |0-5A) 5.14a) 2.89C) 8.86

0E) 11.11

;=,..,z-/.f3

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= 0 { ®c? +r=2±ife = fc/%`4ELF/-_Z,_`-:--i

A,if A a #© fir ac,Ir2-nA -f ruo -.-/1'_

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30. A weak acid,ELF, is in solution with dissolved sodi±±±j±±±g!£4§[3\TaF.tlf H_C1_is 'added, which ionwill react with the extra hydrogen ions from the Hcl to keep the pH from changing?A) Na+8) OH-C) Na-

i+

E) none of these

- #,a¥ f t F -k ._eelf/giv-F#+_-ftF:J

31. Suppose a buffer solution is made from formic acid (HCH02) and sodium formate (NacH02).WhatisthenetionicequationforthereaT6H6fiiHF665HrswhnasmallamounTr6facid is added to the buffer?

D) Hcl(czg) + OH-(czg) + H200 + Cl-(czg)E) H30+(czg) + OH-(czg) i 2H200

:JJ3~f p,ii;3al .,.-. =f , - / '?(j`fr*,,Ua,:-ftyg

--=iJiT-jf I 6,grx ,0is required to create a bu[fer ;oluti8i 'having-a p

•r;-.-; ± A=/ ,7ff~ ¢J¥2_`>/. # fop , /,h-, -i,-7 => #dr# #97-#7f= O ,ipr

V _-''r"g;9)~_/oali/i-i/,r3

sample of anmonia (Kb = 1.8 x 10-5) is titrated with 0.1 A4 H.Cl. At the equivalence point, what

pH of the solution?

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ap`, + 4d~Or/aprfeffjifL-rf~fft3,ffalftifrf;,€:.ffi~>~

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k=!,i-4-+:) --#pir*:£i-, 8'` #f a =-=#f?::.§firf;;J!¥ fj/T2_ ££r(ffFSd3_,

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35. According to the following thermochemical equation, if 978.4 g ofN02 is produced, how muchheat is released at constant pressure?

2NO(g) + 02(g) +_ 2N02(g); AH° = -114.4 kJq7P.2jff -- F;P..a

A) 2.433x l03kT

D)` 1.119xl05kT

E) 5.379kJ

f uckse r|Jtiif ,ir` #\} I 2/, 2;7hArf2 # 02=

cj.ke&-402z--,i tfiif A-? ,).,, =a,,3} en-J#,©£---I? tr= r€-

81.3 mL of 0.6£fj._44p_9tassium chloride?>- --y--,,----.- _ ..---

2.' TL,?i_~fi^ifeJpap_ _ _ __ -

7Bse- . -y -€,

==j a / (# /C

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Howmuchheatisreleasedatconstantpressureif26.5mLofO.2£§Q44±i£:;erpitrateismixedwith__-ni . T r A /-A I / I . 1 1 . 1 f` `tl;,I E9.©p8pf wifef lp I ieT'!/iou¢Mife¢S-4fr±ts±gm+ Agc1(a) + KN03(c7g); AH° = -65.5 kJ

-0.465

kJkJkJ

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F===,-'=;:,_,',;:i::`~ --,-.-----.-.. _._ ,,,., __ -, _i:_

6.|°C to 66.8°C? The`*\.;::2,#$8fe-16,fft:

38. When 0.0400 mol of HC1(czg) is reacted with 0.0400 mol ofNaoH(czg) in 50.0 mL of water, thetemperature of the solution increases by4:Z3ic. What is the enthalpy of react\ion for the followingthermochemical equation?

Hcl(czg) + NaoH(czg) i Nac1(og) + H200

Assulne that the heat capacity of the solution and calorimetA) -0.0893 kJ8) -2.23kJC) 55.8kJ ## = ::f f iif .&1

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rs 47z.3 ,,0

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9

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=fTfflAT-''deAut

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FX1412Spgl7

39. What is AI7° for the following reaction?.\

2C2H2(g) + 502(g) i 4C02(g) +2H200 j

Substance AI7o/(k|/moi) ;49#;C2H2(g) +226. 7C02(g)H20(D

A) +1692.2kJ8) 452.6kJC) -1692.2kJ

-393.5

-.

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:: 5-7/.i4= RE--£fi'± i ;-.i,-I Ffr/ Fip--`2#xp

40. The concentration of calcium carbonate in a saturated aqueous solution of the salt at 25°C is6.71 x 10-5 A41. What is the K;xp of this spalaringly soluble salt?

A) 4.06 x 10-28) 5.47x|o-16

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41. Which of the following salts has the±±gLheLSLmQ±ubility in water?A) Bacr04(Ksp= 1.2x |o-10) f~``

8) Pb?-(ife\-,-Cr

= 2.5 x |o-27

rc03 (Kxp = 9.3 x 10-10)

E) Agcl(Ksp=1.8x 10-[°)

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-^>..-;,-2?42. A saturated solution of which of the following salts will

chromate ion?

A82Cr04 (Kxp = 1.2 x 10-12) Z ,` /

acr04(K5p=2.1 x 10-t°) /

T12Cr04 (K5p = 9.8 x 10-13)2~,'#FT,F=/_

EiHEDEhave the lowest molar

--;FT= 4.H *. /,a

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`._:I_:fr=7

lf rf t#-per

E) Cucr04 (Kxp = 3.6 x 10-6) /.' / 6;u¢giv:

-:/,i-x„-r;#`_#rae--* !iQf'Af#Of ; = 6.`-Sr/3

D) Hg2Cr04 (ksp=2.0 x 10-9) „ ,,,,{LrT=t=-=€ora+|=n?jt -*j a __ #, 5T*rfg-J"

EI lourd "1-,inn"_-- /'9 X ,o-i

10

FX1412Spgl7 ID:A

43. What is the concentration of silver(I) ion in a saturated solution of silver(I) carbonate containing0.0068 A4Na2C03? ForAg2C03, KSp= 8.6 x l0=[-a. ,_ _ /3fr7faLr, p.For Ag2C03, Kfp_=_§:§._.¥ 1.0-I-a.

v„ zj;i_„f+ =2 =£g±st=,:f=;¥;,`#; , ,C,, __ 65frj7AZ77pj72__,7\`~`-a-`---===:= c'` ,}=_ ~giv=_:..,3>_ `,_~.~-pan"< _ ...+_..r `-`-_`3.6 x 10-5 „MM ~-#j `-i:;:-F2:-';,== if:; ,;: ;Ofaa;9 I.3, pb2 D7£ -;i,_:#:-\,

E) 8 o x |o4 M ;~=='4 ;'±,;=f=T+=:':=fafa=;\_;i =6/:;;;;grg=_;D) 2.Ox l0~9A4

+3-=z,FdF\

44. Suppose 50.00 mL of2.0 x lord A4FeQV03)3 is added to 50.00 mL of2.0 xl0nd MK103the following statements is true? For Fe(103)3, Asp = 1.0 x 10-14.

ri±A}-=~ndTH?e-Cifftai©ecause``j~#~ 8) No precipitate forms because oc Esp.E) No precipitate forms because oc = Asp.

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45. In which of the following solutions would Cac204 haveJt_he highest molar solubiliA) 0.01 MNa2C2043; :::i %#:2ci2u4 ce, ,~,?2 ,r-3j,` ==9 r#~-J' ¥~£_,.f_ A fgxp2

i \ i.-4 -.------ *

- ~--jf i

i fry i3 {7 p'/#/rS?,r3{o{ pf%,L2_klfuQ±japd Ago;ap = 86.7 I/(ri6

4,,/±

-:-.I-i;-,f-;-;,-0.01 A4NaHC204

At the normal boiling point of o-xylene,LA±£ri=36is the normal boiling point of o-xylene?

/4# =T4f tF T=? T=- 3 ,.grp>=J,i:--

t. f -?/ - ®in---=if```\

47. Consider the following reaction:

2C(S) + 2H2(g) i C2H4(g); Afro = 52.47 kJ; Ago = -53.5 J/K at 298 K

=:i_I..4Sf:_bntfe£=3f.€ff:.i;Z%:_.What is the equilibrium constant at 298 K for this reaction?A)J*Q--

J#_ 1.o x 1o-12

D) 1.6x|o-3

E) 9.8xl0ll

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i 48. A strip of iron is placed in a 1 A4solution of iron(II) sulfate, and a strip of copper is placed in a 1 "

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solution of copper(II) chloride. The two solutions are connected with a salt bridge, and the twometals are connected by a wire.

Reduction Half-ReactionFe2+(czg) + 2e~ = Fe(s)Cu2+(c}g) + 2e- = Cu(s) I:..34: ;) a--a ,i:I.I.y" _a 4?tf y^ 'T`=

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