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CHM 2046 Study Union Review - Spring 2020 Andy Nguyen

Chapter 11: Liquids, Solids, and Intermolecular Forces

D 0 Rank the following in order of increasing boiling point: CH30H, CH3CI, CH4, CH3CH2CH3

a. CH3CH2CH3 < CH4 < CH3CI < CH30H / f\ k,nvio / e v~(()( +orr..e.,s b. CH3CH2CH3 < CH4 < CH30H < CH3CI c. CH4 < CH3CH2CH3 < CH30H < CH3CI @) CH4 < CH3CH2CH3 < CH3CI < CH30H e. CH30H < CH3CI < CH3CH2CH3 < CH4

(A.,t '-f (._ C,H 3 Ll-t l. U-1 J

0 (v G) (i)

L--Ofr [)pole. -J1f'°~

{ µ ~-~) J.-{- 6 on,h 'F /0 11 -J ;fo i{,

loi er r>l,O{ t.vlt :::- ore. J,,,.()h 2. Which substance isJ,+;ost soluble in water?

6

OG)

4.

A

a. Ethane, CH3CH3 @ Ethanol, CH3CH20H /-I -bond

c. N-butane, CH3CH2CH2CH3 d. 1-butanol, CH3CH2CH2CH20H

Which of the following will cause an increase in vapor pressure? a. Increasing strength of intermolecular forces b. Increasing surface area c. Increasing temperature

@) B and Conly e. A, 8, and C

Prcs111re.

t I Mf- s 1-rc-j f+-1'" J f' t-c,_ CL {). rt:.,.~

'f

Determine the amount of heat (in kJ) required to vaporize 1.55 kg of water at its boiling point. For water, ~Hvap = 40. 7 kJ/mol (at 100°().

@) 3.50 x 103

kJ Hz,O b. 1.14 x 106 kJ C. 2.89 X 10S kJ

Ii j/,,., i 9 1'1 liH ] 6 H -= L-1 o , 1 l.:;t yv, o I

d. 2.11 kJ e. 686 kJ

{ I 5? It,/ //f z O IC I C)OO cf r:' _ / f"l jO ( = b ' I I /j !<l>f

9 {9 le, I p,.,r, )( '1 o 7 t<d/,-11') 1 :-- 3 tj{j-{ < 7 kJ

or

3 · 5 )! IO 3 j_. )


@) Use the following phase diagram of a pure compound to find which statement is true:

D 1 A•

B

I

I •B ----- T, °C·---

/ A C represents sublimation .J.J,.' 1 , · s wJ I-,~ (!Jr,~,, ) ):I. Following the compound would first melt and then vaporize s,e l:rv-.<. , JJ.v- liJtdt .,

/ If the compound is in state A, continued reduction of pressure (at constant temperature) will cause it to melt 5v~;""'-- , r10'- ~A-

@) None of these statements are correct

Chapter 12: Solids and Modern Materials

@ Lithium crystallizes in a body-centered cubic unit cell. What is the mass of one unit cell in grams?

_ 1 o_ h-J ,v1 < r9u ,J1\, r c.t..l\

a. 1.15 X 10-23 g @> 2.30 X 10-23 g

C. 5. 75 X 10-23 g d. 1.04 X 10-22 g

- l = L--lr

- {,,; :c f_o. ~4 J/ r.-. ol

(.L.,{ I

CHM 2046 Study Union Review- Spring 2020 Andy Nguyen

~=~/ lJ) Copper crystallizes in a face-centered cubic lattice. If the edge of the unit cell is 361 pm,

A what is the radius ofthe copper atom?

G) 128pm b. 171 pm C. 181 pm d. 255 pm

- l--f 0 1-c,~,s f-e.r w' - .£~ 'LrI'f _ C.,v ::: (o 3. 5£.l C:, j/'"'0 l

1-;_ 3 bl fM = 2-rfi in zn

('flrl

Chapter 13: Solutions r = 121. t:. r~•-

A

What is the molarity of a solution made by dissolving 8.56 g of sodium acetate in water and diluting to ~Molar mass of NaC2H30 2 = 82.03 g/mol)

a. 5.30 M j\A _ mol ~o/.;/.e., >Div k " ,oJ,'vv-,. at..tA-c,,k. £) 0.139 M - L- I ;.; s:.o lJt,,.-1-- "' Wuk-r

So " Or" c. 0.104 M d. 0.0783 M i.6 lo i sol"k.- \( I iM,o l

i2.- .o3 Jf

0. I 3 CC /\I\. Q,1 So L-- ,1, -, l11h -rn-

9. A potassium bromide (KBr) solution (f.ss% b;-~~~ and its density is 1.03 g/ml. What mass of potassium bromide is contaio-edm-3S:-8ml of the solution?

0 2.78g ./ b. 2.70 g 7 ,5, i. _!:'~k c. 4.88 g 1 D I f • d. 2.62g D j 5 0 1/J1,0Y 1..

J e,~tJ ,·i-y -:. I, o 3 j S'" IA,'11-/\ f'A- L- SDiiJ l-.'o,,-..

( , '5 ') ) Jo~vk. -{_ i.~"~ Y- 35 .i ~ A

loO ~Y' rt0---~Ji·~,,, :_1 ____ _J

o b f J'VlLtSS'


A (i§) Which 0.1 m aqueous solution will have the lowest freezing point?

@ Al(No,1, " t,. T , ,·,.,. J{.r Kr " . t. H, ,c, j"" b. CaCb 3 F b , ' rtol-- f'l,,,u,.;r"r'/

; I '("-(}(Ir' I • t-K,, ,~s . c. C2H50H Al [N01\ 3

i \ ..its~ fr<,t,v"' d. NaCl 1. 0 f~

f Al; r f. 3 N03 -:L-/ (:=4)

(1, 0,. ,·""-r(J r- ,-,. ,.., 1-

f\\Clvl

' 1

s

[,(LO i ,/,

1cp. i~112. cr • 3 C; ,3 )

ofllf ~,' fwe,/\""' ,r •~ ?-fof-.f /rx~r I

,J IA" r r: tp.l"-' iid-l.. i° hr ec,J....

11. 800 g of ethanol (C2H

5OH) was added to 8.0 x 103 g of water. How much would this

lower the freezing point? (Kt for water= 1.86 °C/m)

a. 3.2 °C 4.1 °C

c. 8.2 °C d. 16 °C

t:,. Tr ~ ;"" tr I : I

-. _ )/ .[!_}j ,-,,/ )[, jl:,of_) M ;; /2 { ( . (I l i /j J,/,,,o M

1\1\o I s-ollJ J.e ----/J'j so t-Jeft~

'r / Lf, oY O C ()-ke,,/lo I O L{ b J / 1"'1-D l

i 00 j eJ,w.,~o l x ~(-: 17 . 3 ...,, " r fl'" ' t+-h"" e- l

ODO j I-/ 2, D -; ?:, /t,,J 1--/z,,O

12. A technician has measured the osmotic pressure of a solution to determine the molar D mass of a covalent solute. Which other information would need to be measured in

order to determine the molar mass?

a. Only I b. Only Ill c. Only I and II @)1, II, and Ill

I I. II. Ill.

Temperature Volume of solution Mass of solute

fV\.Ol vr f\'1b 15

l<Jrr-O bvrv\ {'I\ ~ tyto ( .>Pl1,1Lt

Wt.. {i-~oW

- o> Mo 1-,· .... ffl~u{t, l -rr,

- f<. :s C,.Jfll.J/-r,.,,..~

{.,.... svlv h of\..

\,JC.. rJf=.f;..0 -Te,,w.p - I,. 5 ul v hd'\

- j f olvk,


Chapter 14: Chemical Kinetics

®Under certain conditions, the average rate of appearance of oxygen gas in the reaction

A

6

2 O3(g) 3 O2(g)

Is 1.2 x 10·3 atm/s. What is the average rate, expressed in atm/s, for the disappearance of 03?

C:, 8.0x 10·4

b. 1.2 X 10·3

C. 1.8 X 10·3

d. 5.3 X 10·3

. "'°re:> ' I~ I~

,rv14c,.,hv<-, • c,.S lc,.s 'J , \-' ~·

<,'11\l? si:i f f~l--0 j-,,

r f r~ ~sv~ 'tO ' (I. ,1 , \~«r- ~Jv

V' {l.t,f' l!1)The following data were obtained from this reaction

CH3Cl(g) + H2O(g) CH3OH(g) + HCl(g)

2 3

[CH3CI] (M) 2.00 4.00 2.00

What are the reaction orders?

[H2O] (M) 1.00 1.00 2.00

a. CH3CI: first order; H2O: first order @ CH3CI: first order; H2O: second order c. CH3CI: second order; H2O: first order d. CH3CI: second order; H2O: second order

Mx- or-Ju )(

- r:c.-"- row~ I -1 'L

- L,JN,r\ [ L,H}vi l - Hv;S I S Id

JoJblu, rc,.1-e. ctl) o J.')vbU..J

orJc.r Cx <: I )

1-i, , or-t>U + - pi'v l'-- n, vS / +- 5 _ LJ ~ [1-/ 1- 0j JQvbU5 1 n. k 1"t,. Jrvpi.f

- J-1,..; j ,s i,,J orJu- L y -;. i )

Initial rate (M/s) 0.52 1.05 1.98

o• vSl..

~k 2.. - ( b,2.] ) . [ t]

v,1 1.vt-- f\ :: 'I- or y

(\. '


6 @rhe experimental data from a certain reaction gives these three graphs. What is the

most likely order for this reaction?

-tim~ a. Zero

@ First c. Second d. Not enough information

t 1/[AJ

5 e,.,ol"'-J

( -timo-+

~bd

_,,.--------- - ---t [A]

-time--

i,,- 11' ~'7,lkJ (G.k low

[A1 t -k.--1- f- [ A]o

_1,,{AJt - ll--J- ~(AJo

5c.c,o.ul =-

G) f""tA-1--u1,,. ,j-v"rtis w ,1---1,,-. Uf'r-t-<./" e...o/ il"'-1-i ~"

A (i) -hr,) t,Jh,i'v\,, j n,fj,_ ;J / ,'11,t.o..r

A \lS!The decomposition of hydrogen peroxide in the presence of iodide ion is believed to occur via this mechanism:

\) H20 2(aqJ H20(IJ s 1,.) H10i(aqJ § ffiO(I) + O,t1J t1-,~

In this mechanism~n~yre, respectively

(V Catalyst; intermediate b. Intermediate; catalyst c. Reactant; product d. Catalyst; catalyst e. Intermediate; intermediate

I/\, be._,'"";) I

bc,(.k t> r 1-k c,.,J

= (.n..,:. k.c) j I'\ 00. t 5 Hf a.t<J t,,o/1\S u~ ; "- Hx


@ consider the reaction

l 2NO:(g) + F2(g) 2NQiF(g)

0

A proposed mechanism for the reaction is NOl + F2~ N02F + F NO! + F~ N02F

What is the rate law for this mechanism?

[N02F] a. rate = k [ l2 1 N02 [F2

b. rate= k[N02]2[Fz] @) rate= k[N02 ][F2]

d. rate = k[N02][F]

Chapter 15: Chemical Equilibrium

@what is the correct equilibrium expression for this reaction? 2C(,} +Oz<,,# 2C0<1) [CO]

a. KC = [C][02]

[C0] 2

b. Kc= [c]2[02J

[2CO] c. KC = [2C][02]

f [C0] 2

\VKc= [021

)l_ l

llt

::: [ rroJ~ t.k.S J C r(MVW' h J

::: C c,,ol 1

C-01-l 1:1J;,.1 Ju

vi D [cJU)

I) f ,,. 1

f_,q ,1, I; b,~JV"'I

~ or the reaction 2 A(g) B(g), the equilibrium constant is Kp= 0.76. A reaction mixture initially contains 2.0 atm of each gas (PA= 2.0 atm and Pa= 2.0 atm). Which statement is true of the reaction mixture?

a. The reaction mixture is at equilibrium (§) The reaction mixture will proceed toward products

r-;" J & ~l'-J {,;;)V'rv-(_

f o /L c. The reaction mixture will proceed toward reactants d. Not enough information to determine the direction of the reaction mixture

Q-: (P] [e] l i ) 2- I o, S Jl () . 7 :: - ::: ::-

( rt 1 [A1 1 - - -:. -(i) ); "'{ 2 Q LI<

0.~ o ,7 c, /)(I'\ s J...: ?fs nj hl-

____,,


@ consider this reaction at equilibrium.

L 2S02(g) + 0 2(g) 2S03(g) Mi= - 198 kJ

Which change would cause an increase in the SOJS02 mole ratio? Afl;\ t [ SD1] or

,;t: Adding a catalyst ,10 c.(f'..<c,r-

)Y. Removing 0 2(g) sl-AI- Ldl- ( 't 0°1-] , l 0°J]) @) Decreasingthetemperature t"o~·L, P st.-.;f+. ,,.;jhr

£ Decreasing the pressure 3 """' Jn k f. 1-- 1 , 2- ""' 01

fl(" Adding S03(g) sh.; p It N

Consider the reaction of A to form B: 2 A(g) B(g) Kc= 1.8 x 10·5 (at 298 K)

( 1' C.Su:J , j [Jui,] l or- '°'jh,~ I S~ {-fl

A reaction mixture at 298 K initially contains [A] = 0.50 M. What is the concentration of

/eN

D B when the reaction reaches equilibrium? l A{~) r==- B CJ)

_5 /i <- 0 I , g,<. ( O

a. 9.0x 10·6 M I <) . 5o I'-" 0 ----=-----+----b. 0.060 M c. 0.030 M @) 4.5 x 10"6 M

l __ -_...!::..2-.:..x_ -1--_r_ X_ E o,5 -V

/{. t =-( o.5 -J.,<l.) 1.

X. -:: 1,i),{.10-t;

Chapter 16: Acids and Bases

@ which pair is a Bronsted-Lowry conjugate acid-base pair?

[u.'5 ) i

X 0,1?

L a. H30~;oH·_ tp"J' l) jt..k t-)(3 {J",'" n.~ CI04; CI03 J,' f w by un.l,i

NH3; NH/ ' d. HCI; HBr

-s / ,?> ><I D

L


A

6

@. Find the pH of a 0.350 M aqueous benzoic acid solution. For benzoic acid, Ka = 6.5 x 10-5

a. 4.64 HA· 1-1 +- +- A - tc. c,. :. G , 5 .,,_ Io - t; ,r-b. 4.19 I o,35o O 0

(y 2.32 C _ x +-- 'f- 1--- x. d. 11.68 C ,1

i::: Q. 3~0-)( X ,.

/cc,, -::: &,. '5 i<. LO_ t; 0 .35D~

J t- I _5 ,... :;: (;, , '5 "- 0

o, ,?D F <=r i - i 75 ... 10 X. :. 1,;,/ . 7 7 I<. I O - 3 = C J--1 f J

fµ - laj Cf-tr J pl-l' _\ ,i('-1.ll•I O-l )

pH i .~ 1 @) Which compound forms an acidic solution when dissolved in water?

&;; NH4CI NH--t vi No Ll I( ;f tP~ 1 fro,.,. ~ , b. NaCl I L - '- L srnn J ().C:.J I b c,!.f.... I u c. KN02 NH'i~ c) No'" U - f',Wrv--t-. I d. Ca(N03)i A N N N ~~------

[t,,.ho11 "- o C-:J 1 '- c>r ® i\It,..t1N'£L I fl.LA'fYi,.. I

\ ' boS;'- ~r llrJ o1 c~ (t-Jo3 h ll~•.)A "" f\V/, .... v-- t

J ' }( 1-- N Di Ca. z ' J\.\ u 3 -

N 6 i\.J N Ne,vht• I

25. Calculate [H30+] for a solution with a pOH of 9.5 a. 3.2 x 10-10 M

@. 3.2 X 10-5 M c. 1.6 X 10-10 M d. 1.6x 10-5 M


Chapter 17: Aqueous Ionic Equilibrium

B ~What is the pH of a buffer that is 0.120 M in formic acid (HCH02) and 0.080 Min potassium formate (KCH02)? For formic acid, Ka= 1.8 x 10-4. [ i., c, ,.e.]

a. 2.33 HGH01. / jl(_,,~()~ pi,-1 :.- pllet 1- lo.J - 0,..; JJ ® 3.57 l,Jl,CA/c.. l;" ''l~o -Y~ r / (u ,u2oj £L,,; J 0 ,,s~ pH :: _j 04 [1 .o"' IO j 0, ,1 0

C. 3.74 J

d. 3.91 pH = '3 , 5 7

o_ @consider a buffer composed of the weak acid HA and its conjugate base A. Which pair 'U of concentrations results in the most effective buffer?

a. 0.10 M HA; 0.10 MA @ 0.50 M HA; 0.50 MA-

c. 0.90 M HA; 0.10 M A-d. 0.10 M HA; 0.90 MA-

'{"\ 0 S /-

~hat is the solubility product constant, Ksp, of Mg(OHh if its molar solubility in water is 6 l.6x10-4 M?

a. 2.6 X 10-8

1.6 X 10-ll c. l.0x 10-12

d. 4.1 X 10-12

/(_ff -= /.fo'-1 "/ o -" )lsp -=- l,<:.)(2,-,c', i D /{.sf = x.(41/ -) = L/x ? ,.. -4)~

29. Which compound is more soluble in acidic solution than in n~utral solution? f.. rf "L/{1· (, Iv a. PbBr2 0 /c... -h>r w t--:vk fc, /I , s be,;, c. b_ CuCI c. Agl ® BaF2

pi, Bri J

f// 1 z f3 r -A rJ rJ (3

B


Chapter 18: Free Energy and Thermodynamics

L @when a material in the liquid state is vaporized and then condensed into a liquid, the steps in the process are, respectively, /j, p i)et,, k-u- J,,0~ 1 -:-

a. Exothermic and exothermic CJ ,A.., J b. Exothermic and endothermic L baJJ -:

(!) Endothermic and exothermic (V J 5/nit1jtr d. Endothermic and endothermic

31. The combustion of ammonia is represented by this equation. 4 NH3(g) + 5 O2(g) 4 NO(g) + 6 H2O(g) 6H° nm= -904.8 kJ

~o/"1'] ll'Jo

~,,,,,..,., e1-o

Enthalpy of Formation Data H r,c,... -: i '61-l pl""'JJv/ I - ~bu ~Je.,. J- ;

NO<,> +90.4 kJ·mo1·1 7 [ { )j H,0/f/ -241,8 i<J,moJ•I L\H~ a 8 (NO\ f /, { i/iO) J - L4 / SH) ) 4 5 (),

* What is the enthalpy of formation of NH3(g)? G { t-f ) l{ -2L/f .9, )] Jy{N~)) 1- q { O )]

- qot.,/.i ~J -=- L4 qo. 1- [ ""

a. -449 kJ/mol - I o9/f. i J -[Y l N~ 1\J @)-46.1 kJ/mol _c/0~ ,'b -

c. -184 kJ/mol +-( v?, '( , 1 t- I i>CJ '{ · 2

I~~ -"' ~J = - '-l {tJrl,) - '1 ,,;, '1 H,.,H

,IL/]c- J - /../ 0, ( Id ::: N r -d. 227 kJ/mol

rv11, I

D @A particular chemical reaction has a negative 6H and negative 6S. Which statement is

correct? -C> H a. The reaction is spontaneous at all temperatures b. The reaction is nonspontaneous at all temperatures c. The reaction becomes spontaneous as temperature increases

The reaction becomes spontaneous as temperature decreases

- I,:\ f c,. J


A Which reaction is most likely to have a positive flS?

SiO2(s) + 3 C(s) SiC(s) + 2 CO(g) S - j b. 6 CO2(g) + 6 HzO(g) C5H12O5(s) + 6 O2(g) j Ji~

c. CO(g) + Cl2(g) COC!i(g) 1. - I d. 3 NO2(g) + H2O (I) 2 HNO3(1) + NO(g) 3 __, I

Chapter 19: Electrochemistry

D @Which of these ions is the best reducing agent?

Standard Redudlon Potentials Fc3+(aq) + e- Fci+(aq)

Cu2+(aq) + e- eu•(aq)

-~ .f--~1 e.1. 51,._,,.,1) a. Fe ~dwv.JJ b. Fe2

+

c. Cu 2+ ® Cu+

B° +0.77V +0.1S V

rtdv~~~ fA J{I\,~ :. 3ih o~J,zd . \ . ' 1-- :. qc)-r re-J.,l,f..-J

C, )(.I CI I lA", ;JU\ J _ IJ u.d ( ljr~ oJe._ )

i,._;f,,...s '- f o -= ':) t,,-1-.s ,-o, .

f-rv c.J;,re Fe 3"" JV5 re)J,._J D,._J , 1 c)X p.Je,. 1

TT-ui I L11~ 1,k 'D.,;J,'u,) , .. J , ·j rr-d Jt,/\ I-

C/'lD1- ev2.-1-- i )

@what is the coefficient for water (H2O) when the reaction below is balanced in acidic A solution?

@)1 b. 2 C. 3 d. 4 e. 5

Cr20?-(aq) + Mn2 .. (aq) Cr3· (aq) + Mn02(s)

wt N 1-1 1-- + Lr 1.. 0-, 2 - --...3) 2Cf 3'- t 7 H 2- o [ 'l HiD r jV\fl u - -~ ;ti\ n (\_ <--- l j f-1 rt l e, -1 )( 3

b H;o .,_ 3 f-1',r 1- J. --~ 3 /ArJ) z " j'L Ht t k-

7 -6 : I l-lz,. D

Cr i O l i - i- 3 )All z " +- H + ---4 L G- 3~ t :> f\ (\ D i f H '2. o

r

L


L

C

G. What is the standard cell potential, E0, for this reaction?

3 Mn(s) + 2 AuCl4-(aq) 3 Mn2+(aq) + 2 Au(s) + 8 cr(aq) Standard Reduction Potentials E°

Mn2+(aqJ + 2; Mll(.rJ -1.18V - ,:v,. +I.OOV-u1--AuCl;taqJ + 3e- Auf.rJ + 4Cl-(04)

a. -0.18 V b. -2.18 V

(s> +2.18 V d. +5.54 V

£ M / . oo v - { - t . J<J v ) E~, -=- 1-l . t~ I/

0-,c.. f<.t,J

f.-{j ~J [ /.- f oC) ptfeAhal -= <>J-h.oJe.

37. Copper is plated onto the cathode of an electrolytic cell containing CuCl2(aq). How long does it take to plate 111 mg of copper with a current of 3.8 A? / I L J ::: " 3 . s Lf" J ~"

a. 1.3 x 103 s [v O ) ---4 C.u 2..-1- t- 2,e,_ -44 s 111 (,,,; )( I !f )( I >l t -)t f/6'1'65 .£--,( I s

l.;:1 89 s 1000-,., 1,,3.5'-lh I~ /~e- 5-?:ik:-d. 22s /J ,____, ) ~"' . F 3-~ ,A

/ It; / 5,CZ fl-:: 3,'i~ c,'1 .J"'1-,or S 5

3i.7 5 I F =- q b'-13 5 .f-

,.,.;,1 e -@which statement is true for voltaic cells? ,trv<- P. r D a. Electrons flow from the anode to the cathode / b •

0"

b. Electrons flow from the more negatively charged electrode to the more positively charged electrode - off , {;,r t,lc.<.frol yi-J ·<.

c. Electrons flow from higher potential energy to lower potential energy

@) All of the above are true -~

CHM 2046 Study Union Review-Spring 2020 Andy Nguyen

Chapter 20: Nuclear Chemistry

\) Cobalt-60 undergoes beta decay. What is the balanced nuclear reaction for this process?

\ (A) ~Co~ ~p +:Fe

60Co 4 S6Mn (C) 27 ----+ 2« +25

40. What is the missing product of this reaction? ns+

U 16 -

(B) .w (C) ~'Y "a (D) 2

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