e) l~· p~~ cruo. -~ 'bil'(a~ ( ~~fb'n~. 5
TRANSCRIPT
Chapter 11 and 13 Practice Test I1. Of the following substances. only has London dispersion forces as its onlyintermolecular force.
Notes: ~yd'(O~( 'a:n'S. ~ ...x1D'\-~O\o.x \X'Y\Dlg ~ ~
~D'"\dDr) c\.;..D?U"~\.. CY'\ ~ --\"Yu_ ~ \ ~ ~~ ~t) \..n_c..u...l..o.-r-{..\.
2. The solubility of oxygen gas in water at 25°C and 1.0 atrn pressure of oxygen is0.04] g/L, The solubility of oxygen in water at 3.0 atrn and 25°C is g/L,
A) 0.041 B)0.014 C)0,31 ®.12O'C4J.19/L :: Vt,_,: (1-.D ~~)
K('~ o. D~ "i. ~ l~·O-~Scj~ 0,D'-\ \ 'BIL' (A~ ( 5 .00...lrw<. )
55~0 I \ 'Z 5/ L3) Which one of the following should have the lowest boiling point?
E) 3.0 Notes:~\u bt.h-Rj a..ndp~~".-u..V\..-ncru...o. -~ rt..~1
~~fB'n~.
Notes: Nln---fD\o..X"' ~~f>~ ,.J)O ~ ~OJ') O'\.~ J.._~-~r--urSlCf'U -~ UJJt_~
~ ~1,
J ~\~\:'
4) "''''1"",,11,,\, I U A sample of potassium nitrate (49,0 g) is dissolved in 101 gof water at 100 "C, with precautions taken to avoid evaporation of any water. The solution iscooled to 30,0 "C and no precipitate is observed. This solution is _
A) hydrated B) placated C) saturated D) unsaturated ~lPcrsaturatedNotes: V
5) Of the following. has the highest boiling pOint.llfu ~\(~ cb~A) N~ @ Br~ C) H~ D) cr, E) O}. L-_ ------'c:5=l-~--!-------
6) A solution is prepared by dissolving 23.7 g of CaCl2 in 375 g of water. The density of theresulting solution is 1.05 g/ml.. The concentration of CaCI~ is % by mass.
&.94 B)6.32 C) 0.(l632 D)0.0594 E) 6.24 Notes:~ ~c.~.
'2 3 .1~ ( (DO) _ 5.C\ y %: fV'aS~ ~ $o\u.:\ion
31<;lJ-{-t.1':+j - >
7) In which of the following molecules is hydrogen bonding likely to be the most significantcomponent of the total intermolecular forces? f'D Notes: ~ +tu .
ie> '1<~ y~7 1-"- Juo6....roco..x 'oct\. ~A) CH4 B)C5H))OH ) C6H)3NH2 @H30H E)CO2 (.J) +Yu ~Mc..\l.v-*
8) The concentration of nitrate ion in a solution that contains 0.900 M aluminum nitrate is---- M. Notes: ~ ~ti'\..M... GO'Y'-~
A) 0.900 B)0.450 C)[email protected] E) 1.80 ~~k.l':} c~~
(A\ ({'.lD~)3-) ~\ ~-t + 3ND~ )f ) _ n rtO~~.qoa \.3 - -(..,w-r
9) Of the following, is an exothermic process.l
A) melting B) subliming(C)freezing D) boiling E) All of the above are exothermic.
Notes: t>(l),'~<lY\.U:-l.R"f0(.JJ::l:l..., ~.JU) cn~ ~+lJ4\.\b ~ ....o"OO-\t.X"A.
10) The concentration ofa benzene solution prepared by mixing 12.0 g C6Hr, with 38.0 g CCI~ is
molal.----
~4.04
\'L.O~
Notes:~c \ 0 ~ SD \ u..~fY'- ..._ \~ C>~ SO\\Jt.n..tB) 0.240 C) 0.622 D) 0.316 E) 0.508
b, \S4f't\.D \0, D3>~ \(3 - 4-, DS""r'"\ ~D\o.J. J..O ~
~(LN. OJ:>
uY'O\o.U:~--------- - ---- --_--- -----_--------------- _ ..----- ----
11) The heat of fusion of water is 6.0 I kJ /rnol. The heat capacity of liquid water is75.3 J I mol ~K . The conversion of 50.0 g of ice at 0.00 °C to liquid water at 22.0 °C requires
kJ of heat.----
A) 3.8x IO~® 21.3 C) 17.2 D) 0.469 E) Insufficient·dat..-3 _ar_c........_iv_c_n. ---,-__,5D.0') _lm_o\ -:. '2.. Irt~mo \ Notes: ic -e, -> \"'bUAA. o..:r
~ <6 .() -zs. D • 00 0<:. = ~-t- v.-S.{ (R, 0\ -\~'.)/i'?6'\ )( 2.1-1- ~\ )-:: \ lJ. Lt K:r ~-\-1'~o, l,~~ MAST
(~C_1-:.:t~~(-ts.~~\.2 ('2'1. D) .,_"J~"l$ -':>4 ")(\ I<J -=- 21... 'H::'"J12) A solution is prepared by dissolving 15.0 g of Nil) in 250.0 g of water. The density of the
resulting solution is 0.974 g/rnl.. The mole fraction of NH., in the solution is
A) 0.0640rB)).0597 C) 0.940 D) 0.922 E)' 16.8lNotes:
IS,Do. ~ ~ c9_.__~~.) 11.D'-\5 D:'6<6D-t'\3$r=O.O'3iu__ -J
2$1)· C) ~~5 -_ \?" '1$1
"--'---:\--"E~q1id&.~fi8.'
Notes:
13) Ileal added (J) The heating curve shown was generated bymeasuring the heat flow and temperature for a solid as it was heated. The slope of the____ segment corresponds to the heat capacity of the liquid of the substance. '
A)AB B)BC @D D)DE E)EF
14) A solution is prepared by dissolving 15.0 g of NH)in 250.0 g of water. The density of the
resulting solution is 0.974 glmL. The molarity of N~I-I2.J~in~t=h.::..c.::..so=l.::..ut~io~n~i.::..s_=======:_____ ......,
E) 3 53 Notes:. tJ\ov\Ct ~ -\0
add ~\LL'c_ ex: 'SD\lJtj\j-
15) Of the following, __ . _ ..... should have the highest critical temperature.
@CB~1 B) CCI.: C) CF.: D) CH.I E) H~ I ;~\-\JY\O~c.u\O r
. ~fV"16) A solution is prepared by dissolving 23.7 g of CaCl2 in 375 g of water. The density of the
resulting solution is 1_05 g/rnl.. The concentration of Cl in this solution is M.
{
Notes:A) 0.214 B) 0.562 12 D) 1.20 E) 6.64 x 10-2
'2.~ I '+~ ~\ _- C\ '1. -=- O. ~ 'L'"\-(nO' _"!J l \ O·D~ \~\ CAC\2 ~ .l.W. D. 3iriU - 1-.t ~fJ\G(O-.r<\'5o~~C>,~~~ ~ 3q i ~ \M ~~",----,"",o....L.....,,,.£...3Io.O~-=---":""-"----==------'----
\.OS~17) Of the following, is the most volatile. I. \_~ _1.- ........_ ...... Notes: l-A~r\.;T\_.u\ ~~ .
A) CBI:; B) CCI.; C) CF4 @CH4 E) C(>HI4 '!Ohd..on -c\.J...,? ~;~ ~<)Y\.}L ~\U" "",~\.Ao.Jor I
(.J .
18) What is the molarity of sodium chloride in solution that is 13.0% by mass sodium chlorideand that has a density of 1.10 g/rnl.?
Notes:
A) 143 ~.45 C) 2.56 D) 2.23 E) 1.43 x 10-2
\3 DS \ O't> \ -=. 0- '(...:2.Z, 'f"O \s-y.445 fDD ~ , ......~D
<oj i,\OS ,CI)br'\.~ • 09 \ L
I' (111m)
,.o -10 0 10 20 )0 0 so 60 70
19) T ('C) The normal boiling point of the substance \vith thephase diagram shown above is "C.
Notes:
A) 10 8) 20 C) 30 ~o E) 50
20) The vapor pressure of pure water at 25°C is 23.8 torr. Determine the vapor pressure (torr) ofwater at 25 °C above a solution prepared by dissolving 35 g of urea(a nonvolatile, non-electrolyte, MW = 60.0 glmol)in 75 g of water.
A) 2.9 8) 3.3@21D)27E)0.88 r-I-N-ot-es-:-------------,
-L"j ~.~~(.D ;. Lt 1\ (, fiJk. _(-'" ."'vl. \ ~" t<) .<;""qpL{. \ \Q -t D. OS ~ ~ -~ ..-, ....... _.'" /" _ _ _ '\. _ n --J I
etA. (N05/221) What is the freezing point (OC) of a solution prepared hy dissolving 11.3 g of C~lci~l ni~~(formula weight = 164 g/rnol) in 115 g of water? The molal freezing point depression constant
for water is 1.86 °C/m. I INotes:@3.34 B) -1.11 C) 3.34 D) 1.11 E) 0.00 A \f ~Ksr'~: L .
6Tt:: CI·<619~)(O:·~(3)rY'
L\\f ~3.3'-l DOc., - :3!<t ~~. \\.3~ ~~-:. O. lJ (p~ l\:) .TI$'Iui-- . "\22) A solution containing 10.0 g of an unln'%~~iquid and 90.0 g water has a freezing poinf~f -3.33 "C. Given Kf'-'- 1.86 °C/m for water, the molar mass of the unknown liquid is _
g/mol. . I A'"Tj -?) 3.2Notes: Ll If -_-,;, z»
A)69.0 8)333 C)619 D) 161 C§J;2.1':3. ?:>5c.-:: C \ .~l!> Df:. ') ~ ) 10
N'l 0 LA 9 L__ ___
:),':?,3~G- {O,Oq ~') -:.1_,8lo~c;<,~ O.t~(~o' :::. (oIJ.... i S/fY\C\23) Which one of the fo(fowing substances is more likely to dissolve in CCI4 ?
r+'j~~ 'lr-----.c... ~-iA\'r +-> H Jr=' ;'\ I I ~otes:&-8r, 8) HBr C) 110 D) CH,CH,O "'E) NaC1'J.~t:lw:.r..-
.i» j_24) The osmotic pressure ora solution formed by dissolving 25.0 mg of aspirin (C9Hg04) in
atm. I Notes:
A) 13.6 8) 1.14x 10 ; @.0136 D) 2.45 E) 1.38
2S.D(Y\<j ~ 1OOQ\Cq \-\<zU'-1 -= L3C\ ~ \L_D---~--\-------t~3 \''60. \1- 6~1.SOL f'r\o:: 5.5~x lD-Y},--,\
(5,6\0 ~,t)4 V)(()l)~~Olo.kt-·Q~ )(_'2-~<2"K.)=. O. Di3(P~'('PO\.~
0.250 L of water at 25°C is
..... -_ ... --_.. _ .... __ . --- __ . --_
ANSWER THE FOLLOWING QUESTIONS USING THE HEATING CURVE
<r.---~-_;j'i.
\ilqlli,' anrl )las
A '
Iln.laddcdfn fA)A8 8)8C C)CD O)DE E)EF.""-.. ~/
___A_25. The heating curve shown was generated by measuring the heat flow and temperaturefor a solid as it was heated. The slope of the _... segment corresponds to the heatcapacity of the sol id.
t 26. The heating curve shown was generated by measuring the heat flow and temperaturefor a solid as it was heated. The slope of the segment corresponds to the heatcapacity of the gas.
p 27. The heating curve shown was generated by measuring the heat flow and temperatureof a solid as it was heated. The heat flow into the sample in the segment will yieldthe value of the .1 Hvap of this substance
l? 28. The heating curve shown was generated by measuring the heat flow and temperatureof a solid as it was heated. The heat flow into the sample in the segment.. . _. . __ will yieldthe value of the .1H[usion of this substance .
•• The phase changes B -- C and D -- E are not associated with temperature increases becausethe heat energy is used up to _
tA'Uncrease distances between molecules't()break intramolecular bondsC) rearrange atoms within moleculesD) increase the velocity of moleculesE) increase the density of the sample
--------- ------------ _.,
pB
T
29. On the phase diagram shown above, segment A~ corresponds to the conditions oftemperature and pressure under which the solid and the gas of the substance arc in equilibrium.
30. On the phase diagram shown above, the coordinates of point 1) correspond to the_.......__-critical temperature and pressure
i6Q
I'
T
31. The phase diagram of a substance is given above. The region that corresponds to the solidphase is \0 .32. The phase diagram of a substance is shown above. The area labeled ----o..U-t--the gas phase for the substance :J
indicates
33. Which one of the following exhibits dipole-dipole attraction between molecules?
~ ~,A) XeF~ &AsH, C) CO~ D) BCI) E) ci, rl- / I ~
H34. When NaCI dissolves in water, aqueous Na ' and Cl ions result. The force of attraction thatexists between Na ' and H20 is called a(n) interaction.
A) dipole-dipole B) ion-ion C) hydrogen bonding @ ion-dipole E) London dispersionforce
35. Which one of the following derivatives of ethane has the highest boiling point?
A) C,Br, B) C,F, ~,I, D) C,Ci, E) C,H,
t!'-jV-~~~~
,-...£-- 1 _>
36) What is the predominant intermolecular force in CBr4 ? \6 '( - C - ~
fA)tondon-dispersion forces B) ion-dipole attraction C) ionic bonding i(~dipolc-dipolc attraction E) hydrogen-bonding
37) Hydrogen bonding is a special case of .-_. -.------r::-~
A) London-dispersion forces B) ion-dipole attraction/-C)yiPole-dipole attractionsD) ion-ion interactions E) none of the above <--_, -
38) What types of intermolecular forces exist between HI and H~S?di I di I· d ' . 1 - D~ (S L unA) IpO e- IpO e an ion-dipo C t U",," &J'i_u:n-.,p
B) ~ispcr~i()n forces. dipole-dipole, ~nd i~n-dipo~e '. Uhc...a..r.v o..JJ..8.dispersion forces, hydrogen bondmg, dipole-dipole, and ion-dipole ~~c:...u.hJ:v~dispersion forces and dipole-dipole (i...r\Ij. ..4. l.Oo\.D _dJ..p~t..) dispersion forces, dipole-dipole, and ion-dipole ~ ~otD
j)t, '3<i rT\C> \ ,--LD ~,o...kd '39) Calculate the enthalpy change associated with the conversion of25.0 grams of Ice at -4.00 "C
25 fr"'lrl. to water vapor at I 10.0 "C. The specific heats of ice, water, and steam arc 2.09 J/g-K, 4. 18 J:g-K.~\~_ and 1.84 J/g-K, respectively. For H20. 6Hfus = 6,01 kl/rnol and 6Hvap = 40.67 kJ/mol.l<l.D'15\rrO\ C-L{ DOOC")(l).D) -~ ~~",. (~-S.,D ~)CZ.oq ') X ~ \::.)=. 0, '2,QC\ ~3
~ 64.8kJ (O.{)J°c...)-)~)-\.fu.s-=. (11).0\ ¥- T/Inp\)(l,'3C\~\) -=:- ~.?S \<.j
({_,~!)s.9 kJ 4 &D.OO°C._J.CQ'::>c:.)-')tT\~AT ( ~. \~ JIs.¥.) (!DD 1<..) t2~I~ '-lD\ ~~ \<. '3C) 1.11 x 10 4 k I(Y)0c -_ (-4CAto'uJrno' )(L3C\ Y"f\()\) ~ ~ iP.$ "- 'JD) 1.12 x 10 kJ \::E) 1.00xlO~ kJ IOO-Hc>°c -_ ('lSI D~)(l.tl"tNClD~) s: 9·'-\~ \(..J'
5' "15,'140. Large intermolecular forces in a substance are manifested by .
A) low vapor pressure B) high boiling PO~C) high heats of fusion and vaporizationD) high critical temperatures and pressuresryll of the above
41. A solution is prepared by adding 30.00 g of lactose (milk sugar) to 110.0 g of water at 55°CThe partial pressure of water above the solution is torr. The vapor pressure of purewater at 55 °C is 118.0 torr. The MW of lactose is 342.3 glmol.
A) 1.670 B) 94.1 C) 169.4 @116.3 E) 92.7 _ /(\ aqI I \ l'n''''\ 1_ D ~ \) -;.. U) \ 0 - eJ. -\ (p\\0.09 nzu ~ z: l,l', l Lfr> M',_0 0 D'a':HDlq,D~ w,\ T ,
"'O.Ou.. ~se..~' =-0, C£+\.j '{) 3~'2,~
\)A ~ (O\q~\o)(,\\~-\1)'((')
~A- ~ \ \ It> ,3 \Ux-r
-----------_.. - _. - ,-
42. A. solution is prepared by dissolving 7.00
A) -121.3B) 0.752C) -107.9~ -113.8(9'-115.4
(C}-lsOH). The freezing point of the solution is "C. The freezing point of pure
ethanol is -114.6 "C at I atm. The molal-freezing-point-depression constant (K ) for ethanol isf
1.99 "Cim, The molar masses of plycerin and of ethanol arc 92.1 g/mol and 46.1 g/mol,respectively. ~Tf~ \<.t, m· \.. 1.0~ J.m.Q..\ --O,Oq..\o{'l'\O\
~t~--(l.~"()C./\'f{)C.D,"3q.~~)(1) rn:: 't'l·1.-3 0 ,'20\ ~
bT~-=-Q/1S'l. ~c, c. ~q~M~\tv.)wee-",Y\5 \,ut.rd'"' -l\ '1 ,l,t)C -0,'1-5"2, '- - H5\Y Vc.,
43. At 20 "C, a 0.376 M aqueous solution of ammonium chloride has a density of 1.0045 g/ml..What is the mass % of ammonium chloride in the solution? The formula weight of NH4CI is53.50g/mol. O.3'1-lomO\ en D,3~.«+lot:'r\O\of N.ti4~~· :LLo~ .- -\ - ,
A) 0.381 .r"~h~. , -, .. .~\.' I,. r '
B) O.705 O~3ctll> tl)Q \ .53 5£)3 -:. '2.D.1 \ \ ~ ~ 20,\\ t, (100)-:. 2,ooCt~C) 0.374 . ., . \v:nt>\ , , _. ,-3 .'- -) \004 ,$'cW'gg j_Ls!)\.:'I{~XAilL.::,*'5'~:IOMS
44. At 20 "C, an aqueous solution that is 24.0% by mass in ammonium chloride has a density of1.0674 g/ml.. What is the molarity of ammonium chloride in the solution? The formula weight ofNH"Cl is 53.50 glmol. 2.4 g'(oJ'l\S \'l \.-'t\t,\ Ln '005~ S~\~
2.4 .()D/C -)A) 5.90~0.479 Q..4,O~ ~\:. O. 44QmO\ / -=- L1 ~C\ M.(94.79 S35~ / ~3'l-L \\D)0.0445 {hi." ~ \mL ~ -e, (0, U 'E) 22.5 LJU~ o ~ l. D\o14 0l)(Dt'L.45. A solution is prepared by dissolving 16.2 g of benzene (C6H h) in 282 g of carbon
tetrachloride (CCI4). The concentration of henzene in this solution is molal. The
molar masses of C)-If> and eC14 are 78.1 g/mol and 154 g/mol, respectively.
\ LP\'L<j ~roO\ ~ L") I rz.0' yY\ 0\ ri. '3 ~'1~ , \ ~ 0 I 'Z.5~-i.\(,9 -: 0, T r(\7.36 X 10-\
.736
.102D) 0.0543E) 5.43
46. The ideal value of i (van't Hoff factor) for(NHJ»04'
A) J 8) 2 C) 38 E) 5 L~-l-1.0 31,1-1-14t ~ 1>043=&47. The most likely van't Hoff factor for an 0.01 m Cal solution is .'
@l9" ~~~~~~~A) 1.00 B) 3.00 C) 1.27 U) L·W'" E) 3.29 4+u-.k~oJ. \fc;...\W:T'r\A ~.ob\JCt\w. ~ bit. &..I., ~ ~ 1.+1' 'L1:. - -::. .:3 ..CD ~ ~ ~ ~d.-bt "l.(9C1
48. 'Of the following, a 0.2 M aqueous solution of will have the highest freezingpoint.~ Ju_~hno-\-.frtt~ ~ ~+'ru -llano\-(.,VCl\w.. ~
A) (NHJ,P04 B) Pb(~O)2 C) Na,P04 D) Mg(NO)7' ~
L.\ 3 '-1 3 2-49. A solution contains 15 ppm of benzene. The density of the solution is 1.00 g/mL. This meansthat ----0~re are 15 mg of benzene in 1.0 L of this solution8) 100 g of the solution contains 15 g of benzeneC) 100 g of the solution contains 15 mg of benzeneD) the solution is 15% by mass of benzeneE) the molarity of the solution is 15
~8x 10-1 M~.2xlO-I M
C) 4.9x]04 M
D) 3.8 X 10-4 ME) 1.1 x 1O-~M
50. The solubility of nitrogen gas at 25°C and 1 atm is 6.8 x 10 4 moll L . If the partial pressureof nitrogen gas in air is 0.76 atm, what is the concentration (molarity) of dissolved nitrogen?
LP ,~'X \.D~l\-MtL ~Q_~.)C':L.~ ')K:::. lJ,~ i.\O..(_\ t4?t\.. ,lG.~
~ =-- (~.~)(.\D-4~ )(0 1~(,c._J,m)L- ,o.\;tf\
~ -=- S ,2'J_ \D-\.\ t-\51. George is making spaghetti for dinner. He places 4.01 kg of water in a pan and brings it to aboil. Before adding the pasta. he adds 58 go ab e sa aCl) to the water and again hrings it toa hail. The temperature of the salty, boiling water is "C.
L~Q...Assume a pressure of 1.00 atm and negligihle evaporation of water. Kh for water iSu.,k0.52 °Clm tDlliS <rl\.,\ ..e, ~ (J ro\?~, u:)\..g. ..c.k..... ~ t.ODl
61~--Kb 11'(\\ L. .v , q...~c.
() "I~ ....(9 ::y~,OC./~(On.'ti- ,...:X:2)~O. 2..~ ;) _\())0c.,. ~ D, 'lJ~c.-
1cD. '2.l.o DC
· ....,52, Seawater consists of 3 s~l~~.f'orevery liter of solution. Assuming that thesolute is entirely' ium chlori (this is a reasonable approximation) the osmoticpressure of seawater at 20 \)Cis: J.... $0\ lJ.-.-k L =- '2..A) 1.4 atm •
~~tv\~1L,~tm
D) 3.5 atrn 3 tl- _unD\ ~ 0 D?~ '2 \E) 2.4 atm • <3 15%AtlS · \ L 1\"00::
f 0,05& '2l-J'\h\ ) (0,m 'lJ)~ ~,a:\'M )('2.'t~) ('2,)l I~ ~.~
~ 2\Z CL*m
--_ ....._ ...._---- --------------