oxidation and reduction working out

8/17/2019 Oxidation and Reduction working out

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Oxidation and Reduction Reactions Workbook

S.No Contents Work Sheet

1 Oxidation, Reduction, Agents, & Reactions WS 12 Oxidation Numbers Spontaneous Reactions WS23 Oxidation Numbers, Application to Reactions WS34 Balancing Redox Hal Reactions Acid!Base" WS#5 Balancing Redox Reactions in Acid!Base WS$6 Standard %otentials sing '(art WS)7 *lectroc(emical 'ells WS+8 *lectroltic 'ells" WS- Application o *lectroltic 'ells WS.

1! 'orrosion, Redox /itrations, Breat(al0er WS1

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Worksheet "1

Redox #a$% Reactions and Reactions

eine eac( 1" Oxidation2" Reduction3" Oxidi0ing agent#" Reducing agent Write (al reactions or eac( o t(e olloing atoms or ions" 4abel eac( as oxidation or reduction"

$" Al

)" S

+" O52

-" Ba26

." N35

1" Br 2

11" %

12" 'a

13 7a36

1#" S

1$" H2

1)" H6

1+" 85

1-" %35

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Balance eac( spontaneous redox e9uation" :denti t(e entities reduced and oxidi0ed" State t(ereducing agent and t(e oxidi0ing agent" 1." Al & ;n26

2" 82 & O25

21" O2 & 'a

22" Al36 & 4i

Write t(e oxidation and reduction reactions or eac( redox reaction" /(e irst one is done or ou"

23" 8e26 6 'o ⇄ 'o26 6 8e

Oxidation< 'o → 'o26 6 2e5

Reduction< 8e26 6 2e5 → 8e

2#" 3 Ag6 6 Ni ⇄ Ni36 6 3 Ag

Oxidation<

Reduction<

2$" 'u26 6 %b ⇄ %b26 6 'u

Oxidation<Reduction<

2)" O2 6 2 Sn ⇄ O25 6 2 Sn26

Oxidation<

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Reduction<

2+" 'o26 6 2 85 ⇄ 'o 6 82

Oxidation<

Reduction< 2-" /(ere are nine ormulas or oxidi0ing agents rom 9uestions 1. to 2-" 4ist t(em all" Onl

consider ormulas t(at are on t(e let side o an e9uation" /(e irst one is done or ou"

;n26

2." /(ere are nine ormulas or reducing agents rom 9uestions 1. to 2-" 4ist t(em all" Onl

consider ormulas t(at are on t(e let side o an e9uation" /(e irst one is done or ou"

Al

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Worksheet "2

Redox #a$% Reactions and Reactions

1" State t(e Oxidation Number o eac( o t(e elements t(at is underlined"

a= NH3 >>>>> b= H2SO# >>>>>

c= ;nSO3 >>>>> d= Al?OH=3 >>>>>

e= Na >>>>> = 'l2 >>>>>

g= AgNO3 >>>>> (= 'lO#5 >>>>>

i= SO2 >>>>> @= 2'r 2O# >>>>>

= 'a?'lO3=2 >>>>> l= 2'r 2O+ >>>>>

m= H%O325 >>>>> n= H'lO >>>>>

o= CnO2 >>>>> p= 'lO3 >>>>>

9= %bO2 >>>>> r= %bSO# >>>>>

s= 2SO# >>>>> t= NH#6 >>>>>

u= Na2O2 >>>>> D= 8eO >>>>>

= 8e2O3 >>>>> x= SiO##5 >>>>>

= Na:O3 >>>>> 0= 'lO35 >>>>>

aa= NO35 >>>>> bb= 'r?OH=# >>>>>

cc= 'aH2 >>>>> dd= %t?H2O=$?OH=26 >>>>>

ee= 8e?H2O=)36 >>>>> = 'H3'OOH>>>>>

2" W(at is t(e oxidation number o carbon in eac( o t(e olloing substancesE

a= 'O >>>>> b= ' >>>>>

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c= 'O2 >>>>> d= 'O325 >>>>>

e= '2H) >>>>> = 'H3OH >>>>> 3" 8or eac( o t(e olloing reactants, identi< t(e oxidi0ing agent, t(e reducing agent, t(e

substance oxidi0ed and t(e substance reduced"

a= 'u26 ?a9=6 ;n ?s= F 'u?s= 6 ;n26 ?a9=

Substance oxidi0ed >>>>> Substance reduced >>>>> Oxidi0ing agent >>>>> Reducing agent >>>>>

b= 'l2 ?g= 6 2 Na ?s= F 2 Na6 ?a9= 6 2 'l5 ?a9=

Substance oxidi0ed >>>>> Substance reduced >>>> Oxidi0ing agent >>>>> Reducing agent >>>>>

Worksheet " 3

S&ontaneous and Non's&ontaneous Redox Reactions

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escribe eac( reaction as spontaneous or non5spontaneous" 1" Au36 6 8e36 F 8e26 6 Au

2" %b 6 8e36 F 8e26 6 %b26

3" 'l2 6 85 F 82 6 2'l5

#" S2O-25 6 %b F 2SO#25 6 %b26

$" 'u26 6 2Br 5 F 'u 6 Br 2

)" Sn26 6 Br 2 F Sn#6 6 2Br 5

+" %b26 6 8e26 F 8e36 6 %b

-" 'an ou eep 1 C H'l in an iron containerE : t(e anser is no, rite a balanced e9uation or t(e reaction t(at ould occur"

." 'an ou eep 1 C H'l in an Ag containerE : t(e anser is no, rite a balanced e9uation ort(e reaction t(at ould occur"

1" 'an ou eep 1 C HNO3 in an Ag containerE : t(e anser is no, rite a balanced e9uation

or t(e reaction t(at ould occur" ?HNO3 consists o to ions H6 and NO35=

11" 'an ou eep 1 C HNO3 in an Au containerE : t(e anser is no, rite a balanced e9uationor t(e reaction t(at ould occur" ?Remember, HNO3 consists o to ions H6 and NO35=

12" 'ircle eac( ormula t(at is able to lose an electron

O2 'l5 8e Na6

13" etermine t(e oxidation number or t(e element underlined"

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%bSO# >>>>>>>>>> 'lO35 >>>>>>>>>> H%325 >>>>>>>>>> Na2O2 >>>>>>>>>> 'aH2 >>>>>>>>>> Al2?SO#=3 >>>>>>>>>> Na:O3 >>>>>>>>>> '#H12 >>>>>>>>>>

1#" Al36 6 ;n F Al 6 ;n26

Substance oxidi0ed >>>>>>> Oxidi0ing agent >>>>>>>>

1$" 'r 2O+25 6 'lO25 F 'r 36 6 'lO#5

Substance reduced >>>>>>>> Oxidi0ing agent >>>>>>>>

1)" State t(e Oxidation Number o eac( o t(e elements t(at is underlined"

a= NH3 >>>>>>>>>> b= H2SO# >>>>>>>>>> c= ;n'O3 >>>>>>>>>> d= Al?OH=3 >>>>>>>>>> e= Na >>>>>>>>>> = 'l2 >>>>>>>>>>

1+" Balance t(e redox e9uation using t(e (al reaction met(od"

Al & AgNO3

1-" 'ircle eac( ormula t(at is able to lose an electron

O2 'l5 8e Na6

etermine t(e oxidation number or t(e element underlined"1." %bSO# >>>>>>>>>> 2" 'lO35 >>>>>>>>>> 21" H%O325 >>>>>>>>>> 22" Na22 >>>>>>>>>> 23" 'aH2 >>>>>>>>>> 2#" Na:O3 >>>>>>>>>> 2$" '#H12 >>>>>>>>>> 2)" Al2?SO#=3 >>>>>>>>>>

2+" Al36 6 ;n F Al 6 ;n26

Substance oxidi0ed >>>>>>>>>> Oxidi0ing agent >>>>>>>>>>

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2-" 'r 2O+25 6 'lO25 F 'r 36 6 'lO#5

Substance reduced >>>>>>>>>> Oxidi0ing agent >>>>>>>>>>

2." O3 6 H2O 6 SO2 F SO#25 6 O2 6 2H6

Substance oxidi0ed>>>>>>>>>> Reducing agent >>>>>>>>>>

3" 3As2O3 6 #NO35 6 +H2O 6 # H6 F )H3AsO# 6 #NO

Substance reduced >>>>>>>>>> Reducing agent >>>>>>>>>>

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Worksheet " 4

(a$ancin) Redox Reactions

Balance eac( o t(e olloing (al5cell reactions" ?:n eac( case assume t(at t(e reaction taes placein an *C+,+C solution"= Also, state (et(er t(e reaction is oxidation or reduction"

1" S2O325 F SO#25

2" CnO#5 F Cn26

3" As F AsO#35

#" 'r 36 F 'r 2O+25

$" %b26 F %bO2

)" SO#25 F S

+" NO35 F NO

-" NO35 F NH#6

." BrO35 F Br 2

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(a$ancin) #a$% Ce$$ Reactions

Balance in basic solution" 1" NO35 F NO

11" CnO#5 F Cn26

12" As F AsO#35

13" 'r 36 F 'r 2O+25

1#" %b26 F %bO2

1$" SO#25 F S

1)" S2O325 F SO#25

1+" NO35 F NH#6

1-" BrO35 F Br 2

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1." etermine i eac( o t(e olloing c(anges is oxidation, reduction or neit(er"

SO325 F SO#25 >>>>>>>>>>>>>>>>

'aO F 'a >>>>>>>>>>>>>>>>

'rO#25 F 'r 2O+25 >>>>>>>>>>>>>>>>

'rO#25 F 'r 36 >>>>>>>>>>>>>>>>

2:5 F :2 >>>>>>>>>>>>>>>>

:O35 F :2 >>>>>>>>>>>>>>>>

CnO#5 F Cn26 >>>>>>>>>>>>>>>>

'lO25 F 'lO5 >>>>>>>>>>>>>>>>

2" 'r 2O+25

6 8e

26

F 'r

36

6 8e

36

Substance oxidi0ed >>>>> Substance reduced >>>>> Oxidi0ing agent >>>>> Reducing agent >>>>>

Worksheet " 5

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(a$ancin) Redox Reactions in *cid and (asic So$ution

Balance eac( redox e9uation" Assume all are spontaneous" se t(e (al reaction met(od"

1" O25

6 82

2" Al 6 O2

3" 6 ;n62

Balance eac( (al reaction in basic solution"

#" 'r 2O+2 5

F 'r 36

$" NO F NO35

)" SO#25 F SO2

+" CnO2 F Cn2O3

Balance eac( redox reaction in acid solution using t(e (al reaction met(od"

-" H2O2 6 'r 2O+25 F O2 6 'r 36

." /eO325 6 N2O# F /e 6 NO35

1" ReO#5 6 :O5 F :O35 6 Re

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11" %bO2 6 :2 F %b26 6 :O35

12" As F H2AsO#5

6 AsH3

Balance eac( redox reaction in basic solution using t(e (al reaction met(od"

13" O2 6 'r 36 F H2O2 6 'r 2O+25

1#" /e 6 NO35 F /eO325 6 N2O#

1$" :O35 6 Re F ReO#5 6 :O5

1)" %b26 6 :O35 F %bO2 6 :2

1+" 'r 2O+25 6 Hg F Hg26 6 'r 36

State o t(e c(ange represents oxidation, reduction or neit(er"se oxidation Gs"Remember t(at i t(e oxidation G increases it means oxidation and (en it decreases it meanreduction

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1-" CnO2 F Cn2O3 1." NH3 F NO2 2" H'lO# F H'l 6 H2O

21" O2 F O25

22" %2O$ F %#H1

etermine t(e oxidation number 23" H2S O# 22" HS O#5

2#" % # 23" NaH

2$" O3 2#" Na2O 2

2)" 2O$ 2$" % b SO#

Worksheet " 6

Re-ie

1" escribe eac( in our on ords%age 15 o 117


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a= Oxidation b= Reductionc= Oxidi0ing agentd= Reducing agent

2" Write (al reactions or eac(" escribe as oxidation or reduction" 'ircle all oxidi0ing agents"

a= Na b= 'ac= Al36

d= 815

e= N2= O25

3" Write t(e reaction beteen t(e olloing< se t(e (al reaction met(od"

a= 'a 6 Al?NO3=3

b= Sn 6 AgNO3

c= Sn 6 Au?NO3=3

#" 'ircle eac( reducing agent< 'u 'u6 Al Al36 $" 'ircle eac( oxidi0ing agent< 85 8 O25 O2 )" Ni62 reacts it( Cn, (oeDer, Al63 does not react it( Cn" Ran t(e oxidi0ing agents in order

o decreasing strengt(" Ran t(e reducing agents in order o decreasing strengt("

+" Ag6 reacts it( %b, (oeDer, 'a62 does not react it( %b" Ran t(e reducing agents in ordero decreasing strengt(" Ran t(e oxidi0ing agents in order o decreasing strengt("

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-" 'l2 reacts it( Ag, (oeDer, Ag does not react it( Cg62" Ran t(e oxidi0ing agents in ordero decreasing strengt(" Ran t(e reducing agents in order o decreasing strengt("

." Ni62 reacts it( Cn, (oeDer, Al63 does not react it( Cn" Ran t(e reducing agents in ordero decreasing strengt(" Ran t(e oxidi0ing agents in order o decreasing strengt("

1" 'l2 reacts it( Br 5, (oeDer, :2 does not react it( Br 5" Ran t(e oxidi0ing agents in order odecreasing strengt(" Ran t(e reducing agents in order o decreasing strengt("

'lassi as oxidation, reduction or neit(er" 11" SO#25 F S25

12" CnO2 F CnO#5

13" 'r 2O+25 F 'rO#25

1#" :O35 F :2 1$" 7iDen t(e olloing lab data

Sn'l2 & Ni Spontaneous Ni?NO3=2 & 8e Spontaneous'r?NO3=3 & 8e Non spontaneous"

i= Write t(ree balanced e9uations"

ii= Ran t(e oxidi0ing agents in decreasing order o strengt("

iii= Ran t(e reducing agents in decreasing order o strengt("%age 17 o 117


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iD= Will Sn'l2 react it( 'rE *xplainE

D= Will 8e26 react it( SnE 1)" etermine t(e oxidi0ing and reducing agent" Balance in acidic solution"

CnO#5 6 H2S F S 6 CnO

1+" etermine t(e oxidi0ing and reducing agent" Balance in acidic solution" SO#25 6 Br 2 F S2O325 6 BrO35

1-" Balance in basic solution CnO#5 6 H2S F S 6 CnO

1." escribe as spontaneous or non5spontaneous" se our reduction potential c(art"

a= ;n'l2 & 'u b= 'u'l2 & Na'lc= Br 2 & 8e26 d= H2S & Al36

2" 'an ou eep H'l in a ;n containerE *xplainE W(at about an Au containerE

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Balance in basic solution

21" SO#25 6 Br 2 F S2O325 6 BrO35

'lassi as an oxidi0ing agent, reducing agent or bot( based on its position on t(e table"State t(e *o or Doltage o its position" Some o t(ese are bot(, so state to Doltages and indicate t(at itcan be an oxidi0ing and reducing agent" e"g" CnO#5 ?in acid= oxidi0ing agent 1"$1 I

22" Br 2 >>>>>>>>>>>>>>>>> >>>>>>>>>>>>>>>>> 23" 8e26 >>>>>>>>>>>>>>>>> >>>>>>>>>>>>>>>>>

2#" CnO#5 ?ater=>>>>>>>>>>>>>>>>> >>>>>>>>>>>>>>>>> 2$" Ni >>>>>>>>>>>>>>>>> >>>>>>>>>>>>>>>>> 2)" 'r 36 >>>>>>>>>>>>>>>>> >>>>>>>>>>>>>>>>> 2+" H2O >>>>>>>>>>>>>>>>> >>>>>>>>>>>>>>>>>

:ndicate as spontaneous or non5spontaneous"

2-" CnO#5 ?Alaline= & 8e26

2." HNO3 & Ag

3" H'l & Cg

Write eac( oxidation and reduction (al reaction or eac( 9uestion aboDe" etermine t(e *o or eac("'alculate t(e *o or t(e oDerall reaction" 3#"

3$"

3)"

Worksheet " 7

/$ectroche0ica$ Ce$$s

1" Oxidation is (en electrons are "

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2" Reduction is (en electrons are " 3" /(e reducing agent undergoes " #" /(e oxidi0ing agent undergoes " $" A negatiDe Doltage means t(e reaction is "

)" :n an electroc(emical cell electrons exit t(e electrode (ic( is " +" :n an electroc(emical cell t(e reduction reaction is on t(e c(art, (ile t(e

oxidation reaction is " -" /(e cat(ode is t(e site o and t(e anode is t(e site o " ." Anions migrate to t(e and cations migrate to t(e " 1" Anions (aDe a c(arge and cations (aDe a c(arge"

ra and completel anal0e eac( electroc(emical cell" 11" ;n ! ;n?NO3=2 ll 'u ! 'u?NO3=2

12" Ag ! AgNO3 ll H2 ! H'l

Worksheet " 8

/$ectro$tic Ce$$s

1" :n an electroltic cell, reduction occurs at t(e electrode and oxidation occurs at

t(e electrode"

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2" : t(ere are to possible reduction reactions, t(e one on t(e c(art occurs"

3" 8or reduction, t(e c(art is read rom to " #" 8or oxidation, t(e c(art is read rom to and t(e sign o t(e

Doltage is "

$" : t(ere are to possible oxidation reactions, t(e one on t(e c(art occurs" )" 'orrosion o a metal is " +" *lectrolsis electrical energ" -" *lectroc(emical cells electrical energ" ." *lectroltic cells electrical energ" 1" W(at is t(e standard reerence cellE *o J D

,ra and co0&$ete$ ana$e each e$ectro$tic ce$$.

11" Colten Na'l

12" A9ueous Na2SO#

13" 4i9uid 2O

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1#" 1" C 4i:

1$" 2$" m4 o "2 C CnO#5 reacts it( excess SO352" Ho man grams oCnO2 are producedE /(is is '(emistr 11 stoic(iometr"

2CnO#5 6 3SO325 6 H2O F 2CnO2 6 3SO#25 6 2OH5

1)" etermine t(e oxidation number or eac( underlined atom" CnO2 'r 2O+25 :O35 '2O#25 Al?NO3=3

1+" escribe eac( term<

Salt bridge

*lectrolte

Anode

'at(ode

Spontaneous *lectron ainit

1-" W(at ould (appen i ou used an aluminum spoon to stir a solution o 8eSO#?a9=E Write a

reaction and calculate *o"

1." ra an electroc(emical cell using 'u and Ag electrodes"

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2" 2$" m4 o "$ C CnO#5 are re9uired to titrate a 1" ml sample o SO352" 'alculate t(eKSO352L 2CnO#5 6 3SO325 6 H2O F 2CnO2 6 3SO#25 6 2OH5

21" Ho is t(e breat(al0er reaction used to determine blood alco(ol content ?ou mig(t need toloo t(is up in our textbooE

22" 2H6 6 Cg F Cg26 6H2Oxidi0ing agent>>>>>>>>>> Reducing agent>>>>>>>>>

Worksheet "

/$ectro$tic /$ectroche0ica$ Ce$$s *&&$ication

etermine t(e (al reactions or eac( cell and t(e cell Doltage or minimum t(eoretical Doltage andoDerall e9uation"

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1" Ag ! %b electroc(emical cell"

Anode< 'at(ode<Anode reaction< 'at(ode reaction<ODerall reaction< Ioltage<

2" ;n'l2?l= electroltic cell ?electroinning=

Anode< 'at(ode<Anode reaction< 'at(ode reaction<ODerall reaction< C/I<

3" 'uSO#?a9= electroltic cell ?electroinning=


#" /(e electrolsis o 1C Na: ?electroinning=


$" /(e reaction needed to mae Al" /(e electrolte is and its p(ase is?molten or a9ueous="

/o loer t(e mp" rom 2 o' to - o' is used"Anode< 'at(ode<Anode reaction< 'at(ode reaction<ODerall reaction<

)" /(e reaction needed to electroplate a copper penn it( silDer"

Anode< 'at(ode<Anode reaction< 'at(ode reaction<

%ossible *lectrolte<

+" /(e reaction needed to nicke$ &$ate a copper penn"



-" /(e reaction used in t(e e$ectro re%inin) o lead"%age 24 o 117


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Worksheet " 1!

/$ectro$tic /$ectroche0ica$ Ce$$s Corrosion Cathodic rotection

etermine t(e (al reactions or eac( cell and t(e cell Doltage or minimum t(eoretical Doltage" 1" ;n ! Cg electroc(emical cell

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Anode< 'at(ode<Anode reaction< 'at(ode reaction<ODerall reaction< Ioltage<

2" /(e electroltic cell used to produce Al"

*lectrolte< %(ase ?a9ueous or molten=Anode< 'at(ode<Anode reaction< 'at(ode reaction<ODerall reaction<

3" /(e electrolsis :?a9=

Anode< 'at(ode<Anode reaction< 'at(ode reaction<ODerall reaction< C/I

#" /(e electroreining o %b


$" Nicel plating a iron nail"

Anode< 'at(ode<Anode reaction< 'at(ode reaction<*lectrolte/(e 5De side o t(e poer suppl is connected to t(e

)" ra an Ag! ;n electroc(emical cell"

+" ra a 8?l= electroltic cell"

-" ra a 8?a9= electroltic cell"

." ra a 8e:2?a9= electroltic cell"%age 26 o 117


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1" ra a 'd!%b electroc(emical cell" 'd is not on t(e reduction c(art, (oeDer, t(e 'delectrode gains mass and t(e total cell potential is "$ D" etermine t(e (al5cell potential or

'd"

11" Write t(e oDerall reaction and describe t(e anode and cat(ode or a ;n!', uel, alaline andlead!acid cell"

12" 2H:O3 6 $H2SO3 F :2 6 $H2SO# 6 H2O

oxidi0ing agent substance oxidi0edsubstance reduced reducing agent

13" W(at is t(e electrolte in a uel cellE

1#" W(at is t(e uel in a uel cellE

1$" escribe t(e dierences and similarities beteen an electroltic and electroc(emical cell"

1)" escribe and giDe to examples o electroinning"

1+" escribe and giDe one example o electroreining"

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1-" 4ist t(ree metals t(at can be on rom a9ueous solution"

1." 4ist t(ree metals t(at cannot be on rom a9ueous solution"

2" 4ist t(e electrolte in eac( o t(e olloing"

8uel cell,Alaline batterr 'ell ?4eclanc(e=4ead acid batter

21" State to metals t(at can be used to cat(odicall protect 8e" escribe (o t(e protect iron

rom corrosion"

22" Write t(e (al reaction t(at describes t(e corrosion o iron"

23" Write t(e (al reaction t(at describes t(e reduction reaction t(at occurs (en iron corrodes inair and ater"

2#" W( does iron corrode aster in salt aterE

2$" Write t(e anode and cat(ode reaction in an electroltic cell it( a 'a'l2?l= electrolte"

2)" *xplain ( ou ould c(oose ;n or 'u to cat(odicall protect ironE2+" '(oose a suitable redox reactant to oxidi0e 'l5 to 'lO#5 in a redox titration"

2-" escribe as an electroc(emical or electroltic cell<

a= 8uel cell b= '(arging a car batter

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c= isc(arging a car batterd= Ni platinge= :ndustrial Al production= 'l2 production

2." Write t(e anode and cat(ode reactions or eac( o t(e aboDe processes"

3" Al and AgNO3?a9= are mixed and t(e surace o t(e Al darens" 4ist t(e to oxidi0ing agents indecreasing strengt(" 4ist t(e to reducing agents in decreasing strengt("

31" *na$e his 4abel eac( anode and cat(ode"Write eac( anode and cat(ode reaction":ndicate t(e ion migration in eac( cell"etermine t(e initial cell Doltage o t(e electroc(emical cell"etermine t(e C/I or t(e electroltic cell"Will electrolsis occurE:ndicate electron lo":ndicate all electrodes t(at gain mass":ndicate all electrodes t(at lose mass"W(at (appens to KNO35L in t(e Cg (al5cellEW(at (appens to t(e KAg6L in t(e Ag (al5cellEW(at (appens to KCg26L in t(e Cg (al5cellEW(at is t(e e9uilibrium electroc(emical cell potentialEW(at c(emical is made at t(e %t electrode on t(e rig(tEW(at c(emicals are made at t(e %t electrode on t(e letE

%age 2 o 117

1" C NO3

1 C Cg?NO3=2

AgCg

1 C AgNO3

%t

%t

1 C 'uSO#


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ui "1

*)ents S&ontaneous Reactions Oxidation "s and Stren)th

1" :n a redox reaction, t(e species t(at loses electrons

A" is oxidi0ed%age 3! o 117


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B" is called t(e cat(ode'" gains mass at t(e electrode" decreases in oxidation number

2" W(ic( o t(e olloing is t(e strongest oxidi0ing agentE

A" 'u26

B" %b26'" Ni26

" Sn26

3" Cetallic platinum reacts spontaneousl it( Au36?a9= but does not react it( Ag6?a9=" /(e metals,

in order o increasing strengt( as reducing agents, are

A" Ag, %t, AuB" %t, Au, Ag'" Au, Ag, %t" Au, %t, Ag

#" CnO#5 6 $8e26 6 -H6 F Cn26 6 $8e36 6 #H2O /(e oxidi0ing agent in t(e reaction is

A" 8e26

B" 8e36

'" Cn26

" CnO#5

$" CnO#5 6 $8e26 6 -H6 F Cn26 6 $8e36 6 #H2O

uring t(e reaction, electrons transer rom

A" 8e36 to 8e26B" 8e26 to CnO#5

'" CnO#5 to 8e26

" CnO#5 to Cn26

)" As an element is oxidi0ed, its oxidation number

A" increases as electrons are lostB" decreases as electrons are lost'" increases as electrons are gained" decreases as electrons are gained

+" A solution o 1" C %b?NO3=2 ill not react it( a container made o

A" 'uB" 8e'" Sn" ;n

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-" A spontaneous redox reaction occurs (en a piece o iron is placed in 1" C 'uSO#" /(ereducing agent is

A" 8eB" 'u26

'" H2O" SO#25

." A substance is oxidi0ed (en it

A" loses protonsB" gains protons'" loses electrons" gains electrons

1" A strip o titanium, /i, is placed in 1" C Sn?NO3=2" /(e s(in surace o t(e titanium darens,

indication t(at a reaction (as occurred" 8rom t(is obserDation it ma be concluded t(at

A" /i26 is a eaer reducing agent t(an Sn26B" /i26 is a eaer oxidi0ing agent t(an Sn26

'" /i26 is a stronger reducing agent t(an Sn26

" /i26 is a stronger oxidi0ing agent t(an Sn26

11" 'onsider t(e olloing redox reaction < Hg26 6 'u F Hg 6 'u26 " :n t(is reaction, Hg26

is a

A" eaer reducing agent t(an 'u26

B" eaer oxidi0ing agent t(an 'u26

'" stronger reducing agent t(an 'u26

" stronger oxidi0ing agent t(an 'u26 12" /(e species (ic( gains electrons in a redox reaction

A" loses massB" is oxidi0ed'" is t(e oxidi0ing agent" increases in oxidi0ation number

13" Samples o ranium, Ianadium and Mttrium ?, I, M= ere placed in solutions containing t(e

metallic ions 36

, I26

, and M36

" /(e olloing obserDations ere recorded" ria$ +on 9eta$ Obser-ation

1 36 M reaction2 I26 reaction3 I26 M reaction# M36 I no reaction

%age 32 o 117


33/117

/(e oxidi0ing agents rom t(e strongest to t(e eaest are

A" I26, 36, M36

B" 36, I26, M36

'" M36, 36, I26

" I26, M36, 36

ui "2

*)ents S&ontaneous Reactions Oxidation "s and Stren)th

1" W(ic( o t(e olloing pairs o ions ill react spontaneousl in a solutionE

A" 'u26 and 8e26

B" %b26 and Sn26

'" 'o26 and 'r 26

%age 33 o 117


34/117

" Cn26 and 'r 26

2" W(en NO2 reacts to orm N2O# t(e oxidation number o nitrogen

A" increases b 2B" increases b #'" increases b -

" does not c(ange 3" 'onsider t(e olloing redox e9uation<

12H6?a9= 6 2:O35?a9= 6 18e26?a9= F 18e36?a9= 6 :2?s= 6 )H2O?l=

/(e reducing agent is

A" :2B" H6

'" 8e26

" :O35

#" /(e oxidation number o nitrogen increases in

A" NO35 F NOB" N2O# F N:3'" NH3 F NH#6

" NO2 F N2O$ $" W(ic( o t(e olloing represents a balanced reduction (al5reactionE

A" IO2 6 2H6 6 2e5 F I26 6 H2OB" IO2 6 H2 F I26 6 H2O 6 le5

'" IO2 6 2H6 6 le5 F I26 6 H2O" IO2 6 #H6 6 2e5 F I26 6 2H2O

)" 'onsider t(e olloing (al reaction< Sb2O3 6 )H6 6 )e5 ⇄ 2Sb 6 3H2O

/(e oxidation number o antimon in Sb2O3 A" increases b 3B" increases b )'" decreases b 3" decreases b )

+" 'onsider t(e olloing unbalanced (al5reaction H'lO2 ⇄ H'lO /(e balanced (al5reaction ould (aDe

%age 34 o 117


35/117

A" 1 electron on t(e letB" 1 electron on t(e rig(t'" 2 electrons on t(e let" 2 electrons on t(e rig(t

-" /(e oxidation number o platinum in %t?H2O=#26 is

A" 62B" '" 6#" 61!2

." 'onsider t(e olloing (al5reaction< BrO5 F Br 5 ?basic=/(e balanced e9uation or t(e (al5reaction is

A" BrO5 6 2H6 6 2e5 F Br 5 6 H2OB" BrO5 6 2H6 F Br 5 + H2O 6 2e5

'" BrO5 6 H2O F Br 5 6 2OH5 6 2e5" BrO5 6 H2O 6 2e5 F Br 5 6 2OH5

1" 'onsider t(e olloing redox reaction<

2CnO#5 6 $'H3'HO 6 )H6 F $'H3'OOH 6 2Cn26 6 3H2O

/(e species t(at loses t(e electron is

A" H2OB" CnO#5

'" 'H3'HO" 'H3'OOH 11" Hdrogen (as an oxidation number o 1 in

A" H2B" NaH'" H2O" OH

12" 'onsider t(e olloing<

2NO35 6 #H6 6 2e5 F N2O# 6 2H2O

/(is e9uation represents

A" reductionB" oxidation'" neutrali0ation" decomposition

%age 35 o 117


36/117

13" W(ic( o t(e olloing (al5reactions is balancedE

A" :O35 6 )H6 6$e5 F :2 6 3H2OB" :O35 6 )H6 6 #e5 F1!2 :2 6 3H2O'" :O35 6 )H6 F :2 6 3H2O 6 $e5

" :O35 6 )H6 6 $e5 F :2 6 3H2O

1#" 'onsider t(e olloing redox reaction< Al 6 CnO#5 6 2H2O FAl?OH=#5 6 CnO2 /(e c(emical species being oxidi0ed is

A" AlB" CnO#5

'" Al?OH=#5

" CnO2

1$" 'onsider t(e olloing redox reaction<

)H6 6 ):5 6 'lO35 F 3:2 6 3H2O 6 'l5

/(e reducing agent is

A" :5

B" :2'" H6

" 'lO35

1)" Nitrogen (as an oxidi0ation number o 0ero in A" N2B" NO2'" NH3" HNO3

1+" W(en CnO#5 reacts to orm Cn26, t(e manganese in CnO#5 is

A" reduced as its oxidation number increasesB" reduced as its oxidation number decreases'" oxidi0ed as its oxidation number increases" oxidi0ed as its oxidation number decreases

1-" 'onsider t(e olloing reaction<

2HNO3 6 3H2S F 2NO 6 3S 6 #H2O

%age 36 o 117


37/117

/(e nitrogen in HNO3 undergoes

A" reductionB" oxidation'" electrolsis" neutrali0ation

1." /(e oxidation number in carbon in 'a'2O# is

A" 62B" 63'" 6#" 6)


2'r 36?a9= 6 3'l2?a9= 6 +H2O?l= F 'r 2O+25?a9= 6 )'l5?a9= 6 1#H6?a9=

/(e species (ic( loses electrons is A" 'l2B" 'r 36

'" H2O" 'r 2O+25

ui "3

(a$ancin) Redox reactions' *cid (ase Ce$$ otentia$s

1" 'onsider t(e olloing oDerall reaction<2R(6 6 %b?s= F 2R(?s= 6 %b265 * J "+3 I

/(e * or t(e (al5reaction R(6 6 e5 ⇄ R( is

A" 5"-) IB" 5") I

%age 37 o 117


38/117

'" 6") I" 6"-) I

2" W(ic( o t(e olloing sstems ould be correct i t(e 0inc (al5cell ould (aDe been c(osen

as t(e standard instead o t(e (drogen (al5cellE

A" /(e reduction potentials o all t(e (al5cells ould remain unc(anged

B" /(e reduction potentials o all t(e (al5cells ould increase b "+) I'" /(e reduction potentials o all t(e (al5cells ould (aDe positiDe Dalues "

/(e reduction potentials o t(e (drogen (al5cell decrease b "+) I 3" /(ree beaers contain 1" C 'u'l2" A piece o metal is placed in eac( o t(e beaers

B*A*R SO4/:ON C*/A41 'u'l2 ;n2 'u'l2 Ag3 'u'l2 Ni

Reactions occur in

A" beaer 2 onlB" beaers 1, 2, and 3'" beaers 1 and 2 onl" beaers 1 and 3 onl

#" 'onsider t(e olloing redox reaction<

3SO2 6 3H2O 6 'lO35 F 3SO#25 6 )H6 6 'l5

/(e reduction (al5reaction is

A" 'lO35 6 )H6 F 'l5 6 3H2O 6 )e5

B" 'lO35 6 )H6 6 )e5 F 'l 5 6 3H2O'" SO2 6 2H2O F SO#25 6 #H6 6 2e5

" SO2 6 2H2O 6 2e5 F SO#25 6 #H6

$" W(at to substances are produced (en 'r and 1" C CnO#5 react in a basic solutionE

A" Cn26 and 'r 36

B" CnO2 and 'r 36

'" Cn26 and 'r 26

" CnO2 and 'rO#25

)" Bromine, Br 2, ill react spontaneousl it(

%age 38 o 117


39/117

A" :5

B" :2'" 'l5

" 'l2 +" /(e substances H2O2, H3%O# and H2SO3 in order o increasing strengt(s as oxidi0ing agents

are"

A H2O2, H3%O#, H2SO3B" H2SO3, H3%O#, H2O2 '" H3%O#, H2SO3 , H2O2" H2O2,H2SO3 , H3%O#

-" 'onsider t(e olloing oDerall e9uation or an electroc(emical cell<3Ag6 6 'r F 'r 36 6 3Ag

At standard conditions ,t(e initial cell Doltage is

A" 6") I

B" 6"3. I'" 61"21 I" 61"$# I

." A solution o 1" C 'o?NO3=2 s(ould be stored in a container made o

A" tinB" 0inc'" aluminum" magnesium

1" A strong oxidi0ing agent (as a

A" ea attraction or electronsB" strong attraction or electrons'" ea abilit to become reduced" strong abilit to become oxidi0ed

11" /(e to species (ic( react spontaneousl in acidic solutions are

A" :O35 and :2B" SO#25 and S

'" BrO35

and Br5

" Au'l#5 and Au 12" 'onsider t(e olloing redox reaction<

'o26?a9= 6 2Ag?s= F 2Ag6?a9= 6 'o?s= /(e reaction is

A" spontaneous and *o is positiDe"B" spontaneous and *o is negatiDe"

%age 3 o 117


40/117

'" non5spontaneous and *o is positiDe"" non5spontaneous and *o is negatiDe

13" Reerring to t(e data boolet, (ic( o t(e olloing can act as an oxidi0ing agent but not as a

reducing agentE

A" ;n

B" 'l5'" Sn26

" 8e36

1#" W(ic( e9uation represents a redox reactionE

A" %b26 6 2'l5 F %b'l2B" 'aO 6 'O2 F 'a'O3'" Cg 6 2H'l F Cg'l2 6 H2" H'l 6 NaOH F Na'l 6 H2O

1$" :n a redox reaction, 'lO5 as conDerted to 'l5 in a basic solution" /(e balanced (al5reactionor t(is process is

A" 'lO5 6 H2O 6 2e5 F 'l5 6 2OH5

B" 'lO5 6 2OH5 F 'l5 6 2e5 6 H2O'" 'lO5 6 H2O F 'l5 6 2e5 6 2OH5

" 'lO5 6 2OH5 6 2e5 F 'l5 6 H2O

ui "4

/$ectroche0ica$ Ce$$s:/$ectro$tic Ce$$s

%age 4! o 117

1" C NO3

1C ;n?NO3=

2

%b;n

1C %b?NO3=

2

Doltmeter


41/117

1" :n t(e electroc(emical call aboDe, t(e electrons lo rom

A" 0inc to lead and t(e mass o 0inc increasesB" 0inc to lead and t(e mass o lead increases'" lead to 0inc and t(e mass o 0inc increases" lead to 0inc and t(e mass o lead increases

2" /(e initial cell Doltage is

A" 5"-. I

B" 5")3 I'" 6")3 I" 6"-. I

3" :n an operating lead50inc electroc(emical cell s(on aboDe, t(e cat(ode

A" gains mass as anions are reducedB" loses mass as anions are reduced'" gains mass as cations are reduced" loses mass as cations are reduced

#" /(e e9uation or t(e (al5reaction at t(e anode is

A" ;n26 6 2e5 F ;nB" %b26 6 2e5 F %b'" ;n F ;n26 6 2e5

" %b F %b26 6 2e5

$" /(e e9uation or t(e (al5reaction at t(e cat(ode is

A" ;n26 6 2e5 F ;nB" %b26 6 2e5 F %b'" ;n F ;n26 6 2e5

" %b F %b26 6 2e5

)" /(e direction o electron lo in an electroc(emical cell is rom

A" anode to cat(ode t(roug( t(e external ire%age 41 o 117


42/117

B" cat(ode to anode t(roug( t(e external ire'" anode to cat(ode t(roug( t(e external ire and bac t(roug( t(e salt bridge" cat(ode to anode t(roug( t(e external ire and bac t(roug( t(e salt bridge

+" W(ic( o t(e olloing is ormed at t(e anode during t(e electrolsis o 1" C Na:E

A" :2

B" O2'" H2" Na

-" As t(is cell operates

A" 'l5 is oxidi0ed at t(e anodeB" Cg26 is oxidi0ed at t(e anode'" 'l5 is oxidi0ed at t(e cat(ode" Cg26 is oxidi0ed at t(e cat(ode

." :n an operating electroc(emical cell, t(e anions migrate

A" toards t(e anode t(roug( t(e ireB" toards t(e cat(ode t(roug( t(e ire'" toards t(e anode t(roug( t(e salt bridge" toards t(e cat(ode t(roug( t(e salt bridge

%age 42 o 117

1" C NO

3

1 C Cg?NO3=

2

'uCg

1 C 'uSO#

Doltmeter

%oer Source

5 6

%t

%t

Colten Cg'l2


43/117

1" As t(e aboDe electroc(emical cell operates

A" nitrate ions migrate into t(e copper (al5cellB" copper?::= ions migrate t(roug( t(e salt bridge'" magnesium ions migrate t(roug( t(e salt bridge" potassium ions migrate into t(e magnesium (al5cell

11" :n t(e aboDe electroc(emical cell, t(e reaction at t(e anode is

A" 'u F 'u26 6 2e5

B" 'u26 6 2e5 F 'u'" Cg F Cg26 6 2e5

" Cg26 6 2e5 F Cg

12" :n t(e aboDe electroc(emical cell, t(e initial Doltage is

A" 2"3 IB" 2"$2 I'" 2"+1 I" 2"-. I

13" W(ic( o t(e olloing a9ueous solutions produces H2?g= and O2?g= during electrolsis

A" 1" C :B" 1" C 'u:2

'" 1" C 2SO#" 1" C 'uSO#

1#" :n t(e electrolsis o molten 0inc c(loride, t(e (al5reaction at t(e anode is

A" 'l2 6 2e5 F 2'l5

B" 2'l5 F 'l2 6 2e5

'" ;n26 2e5 F ;n" ;n F ;n26 6 2e5

1$" /(e initial cell Doltage at 2$o' is

%age 43 o 117


44/117

A" 51") IB" 5"$# I'" 6"$# I" 61") I

1)" /(e balanced e9uation or t(e oDerall reaction is

A" Ni6?a9= 6 Ag?s= F Ag6?a9= 6 Ni?s=B" Ni?s= 6 Ag6?a9= F Ag?s= 6 Ni6?a9='" Ni26?a9= 6 2Ag?s= F 2Ag6?a9= 6 Ni?s=" Ni?s= 6 2Ag6?a9= F 2Ag?s= 6 Ni26?a9=

1+" /(is redox reaction occurs because

A" Ag?s= is a stronger oxidi0ing agent t(an Ni ?s=B" Ag?s= is a eaer reducing agent t(an Ni?s=

'" Ag6?a9= is a stronger reducing agent t(an Ni26?a9=" Ag6?a9= is a eaer oxidi0ing agent t(an Ni26?a9=

1-" /(e direction o t(e electron lo is A" rom Au to %b t(roug( t(e ireB" rom %b to Au rom t(e ire'" rom Au to %b t(roug( t(e salt bridge" rom %b to Au t(roug( t(e salt bridge

%age 44 o 117

1" C NO3

1 C Ni?NO3=

2

Ag Ni

1 C AgNO3

Doltmeter

1" C NO3

1 C Au?NO3=

3

%bAu

1 C %b?NO3=

2

Doltmeter


45/117

1." As t(e cell operates

A" NO35 and 6 ill migrate toard t(e %b (al5cellB" NO35 and 6 ill migrate toard t(e Au (al5cell'" NO35 migrates toard t(e %b (al5cell and 6 ill migrate toard t(e Au" NO35 migrates toard t(e Au (al5cell and 6 ill migrate toard t(e %b

2" /(e initial Doltage is A" 51"3+ IB" " I'" 1"3+ I" 1")3 I

21" W(ic( o t(e olloing is a balanced (al5reaction in baseE

A" 'l2 6 3H2O F 'lO35 6 )H6 6 $e5

B" 'l2 6 )OH5 F 'lO35 6 $e5 6 3H2O

'" 'l2 6 )H2O F 2'lO35 6 12H6 6 1e5" 'l2 6 12OH5 F 2'lO35 6 )H2O 6 1e5

22" :n (ic( o t(e olloing unbalanced e9uations does c(romium undergo oxidationE

A" 'r 36 F 'r B" 'r 36 F 'r 26

'" 'r 36 F 'r 2O+25

" 'rO#25 F 'r 2O+25

ui "5

*&&$ication o% Ce$$s

1" /(e corrosion o iron can be preDented b attac(ing a piece o 0inc to t(e iron because t(e

A" iron acts as an anodeB" 0inc reduces more readil t(an iron

%age 45 o 117


46/117

'" electrons lo rom t(e 0inc to t(e iron" iron ions orm more readil t(an 0inc ions

2" An iron spoon is electroplated it( copper"/(e e9uation representing t(e reduction

reaction is

A" 'u26?a9= 6 2e5 F 'u?s=B" 'u?s= F 'u26?a9= 6 2e5

'" 8e26?a9= 6 2e5 F 8e?s=" 8e?s= F 8e26?a9= 6 2e5

3" :n an operating 0inc5copper electroc(emical cell, t(e oxidi0ing agent

A" loses electrons at t(e anodeB" loses electrons to t(e cations'" gains electrons at t(e cat(ode" gains electrons rom t(e anions

#" An example o electro reining is t(e

A" extraction o aluminum rom bauxiteB" puriication o lead rom an impure anode'" recoDer o 0inc rom a 0inc sulp(ide solution" production o c(lorine rom a sodium c(loride solution

$" *lectroplating alas inDolDes t(e

A" oxidation o anions

B" reduction o cations'" reduction at t(e anode" oxidation at t(e cat(ode

)" Hdrogen and oxgen react to proDide energ in a

A" dr cellB" uel cell'" alaline cell" lead5acid storage cell

+" *n electroltic process is used to puri impure lead" /(e electrodes are

%age 46 o 117

ANO* 'A/HO*A" carbon impure leadB" pure lead carbon

'" pure lead impure lead" impure lead pure lead


47/117

-" :n t(e cell belo t(e (al5reaction at t(e cat(ode is

A" 'u26 6 2e5 F 'u?s=B" 2SO#25 F S2O-25 6 2e5

'" H2O F O2?g= 6 2H6 6 2e5

" 2H2O 6 2e5 F H2?g= 6 2OH5

." :n t(e electrolsis o molten %bBr 2, t(e products at t(e anode and cat(ode are

ANO*?:N*R/=

'A/HO*?:N*R/=

Br 2 H2

O2 %b%b Br 2Br 2 %b

1" nder (ic( conditions could an electroc(emical cell proDide ".3IE

Anode 'at(ode'u CgCg 'uAg %b%b Ag

%age 47 o 117

A"

B"'""

%oer Source

5 6

%t

:ron e

1" C 'uSO#

A"B"'""


48/117

11" /(e reduction reaction in t(e aboDe electroc(emical cell is

A" %b26 6 2e5 F %bB" %b F %b26 6 2e5

'" Ag6 6 e5 F Ag" Ag F Ag6 6 e5

12" An industrial process inDolDing electrolsis is t(e reduction o

A" ater orming oxgen gasB" ater orming (drogen gas'" sea ater orming c(lorine gas" sea ater orming bromine li9uid

13" /o plate a nicel coin it( copper

A" t(e nicel coin must be t(e cat(odeB" t(e cat(ode must be made o copper

'" t(e electrons must lo to t(e anode" t(e solution must contain nicel ions 1#" W(ic( o t(e olloing ions can be reduced rom an a9ueous solution

A" Ba26

B" Al36

'" Sn26

" Na6

1$" /(e principal unction o a uel cell is to A" produce uelB" electrol0e uel'" produce (drogen" produce electricit

1)" : a piece o nicel is to be gold5plated using an electroltic process, (ic( (al5reactionoccurs at t(e cat(odeE

A" Ni F Ni26

6 2e5

B" Ni26 6 2e5 F Ni'" Au F Au36 6 3e5

" Au36 6 3e5 F Au 1+" 'onsider t(e olloing redox reaction

As2O3 6 2NO35 6 2H2O 6 2H6 F 2H3AsO# 6 N2O3 :n t(is reaction, nitrogen

%age 48 o 117


49/117

A" loses electrons and increases in oxidation number B" gains electrons and increases in oxidation number '" loses electrons and decreases in oxidation number " gains electrons and decreases in oxidation number

1-" :n an electroc(emical cell, t(e cat(ode

A" is reducedB" loses mass'" is t(e reducing agent" is t(e site o reduction

1." W(en 1" C Na: is electrol0ed, bubbles o gas orm on one electrode and a reddis(5bron

substance orms on t(e ot(er" /(e (al5reaction at t(e cat(ode is

A" 2:5 F :2 6 2e5

B" Na6 6 e5 F Na

'" H2O 6 O2 6 2H6 6 2e5" 2H2O 62e5 F H2 6 2OH5

ui "6

Corrosion Cathodic rotection itration

1" W(ic( o t(e olloing metals could be used to cat(odicall protect a sample o leadE

A" ironB" gold'" silDer " copper

%age 4 o 117


50/117

2" A piece o iron can be preDented rom corroding b

A" maing it a cat(odeB" placing it in an acidic solution'" attac(ing a small piece o lead to it" attac(ing a small piece o gold to it

3" /o determine t(e K8e26L in a solution o 8eSO# b a redox titration, a suitable reagent ould be an acidiied solution o

A" 'r 36

B" Cn26

'" SO#25

" 'r 2O+25

#" As a metal corrodes,

A" it gains electrons

B" it becomes reduced'" it acts as a reducing agent" its oxidation number decreases

$" W(ic( met(od ill cat(odicall protect a piece o ironE

A" %aint t(e ironB" 'oDer t(e iron it( grease'" Attac( a piece o lead tot (e iron" Attac( a piece o magnesium to t(e iron

)" 'orrosion o iron can be preDented b attac(ing a piece o

A" CnB" 'u'" %b" Sn

+" A student attempted to determine t(e *o ?Dolts= o t(e olloing (al5reaction<%d26 6 2e5 F %d %d26 reacts it( 'u?s= but not it( Hg?l="

Based on t(e aboDe, t(e *o

?Dolts= o a %d (al5cell is A" less t(an "3# IB" greater t(an 1"$ I'" greater t(an "-$ I but less t(an 1"$ I" greater t(an "3# I but less t(an "-$ I

-" 'onsider t(e olloing redox e9uation<

Br 2 6 SO2 6 Na2SO# 6 2H2O F 2H2SO# 6 2NaBr %age 5! o 117


51/117

W(ic( o t(e olloing is gaining electronsE

A" Br 2B" SO2'" H2O" Na2SO#

." /(e reaction t(at occurs (en pieces o lead, 0inc, copper and silDer are placed in a solutiono Ni?NO3=2 is

A" %b 6 Ni26 F %b26 6 NiB" ;n 6 Ni26 F ;n26 6 Ni'" 'u 6 Ni26 F 'u26 6 Ni" 2Ag 6 Ni26 F 2Ag6 6 Ni

1" :n t(e electroc(emical cell aboDe, t(e electrons lo rom

A" copper to lead t(roug( t(e ireB" lead to copper t(roug( t(e ire'" copper to lead t(roug( t(e salt bridge" lead to copper t(roug( t(e salt bridge

11" :n t(e electroc(emical cell aboDe, t(e initial *o Dalue is

A" "3 I

B" "21 I'" "2. I" "#+ I

12" A reaction t(at occurs during t(e corrosion o iron is

A" 8e 6 3e5 F 8e36

B" 8e F 8e26 6 2e5

'" 8e26 6 2e5 F 8e%age 51 o 117

1" C NO3

1C %b?NO3=

2

'u%b

1C 'u?NO3=

2

Doltmeter


52/117

" 8e36 6 e5 F 8e26

13" 'onsider t(e olloing reaction

;n?s= 6 2Ag6?a9= F ;n26?a9= 6 2Ag?s=W(at Dolume o "$ C AgNO3 is re9uired to react completel it( )"$# g o 0incE

A" "131 4

B" "2)2 4'" "2 4" "# 4

Redox Web Re-ie

1= W(ic( most readil gains electronsE

'u 'u26 8e262 ;n26 Au36

2= W(ic( most readil loses electronsE

Hg?l= 'u26 Sn#6 Ba Al

'alculate t(e cell potentials or Doltages ?*= :ndicate spontaneit"

3" 'l2 6 2Br 5 F 2'l5 6Br 2

#" 2CnO#5 6 $%b 61)H6 F 2Cn26 6 -H2O 6 $%b26

$" Will AgNO3 react it( ;nE Write a balanced redox reaction and calculate *o

)" W(at ould (appen i ou used an iron spoon to stir a solution o Al2?SO#=3?a9= E Write a balanced redox reaction and calculate *o"

%age 52 o 117


53/117

+" W(at are t(e dierences beteen an electroc(emical cell and an electroltic cellE

*lectroc(emical cell *lectroltic cell

-" W(at are t(e similarities beteen an electroc(emical cell and an electroltic cellE

*lectroc(emical cell or *lectroltic cell

." State (o ou ould determine eac( o t(e olloing in an electroc(emical or electrolticcell"

*lectroc(emical 'ell *lectroltic 'ell

%age 53 o 117


54/117

/(e site o reduction

/(e site o oxidation

/(e 6De electrode

/(e 5De electrode

/(e anions migrate to t(e

/(e cations migrate to t(e

/(e electrode t(at gains mass

/(e electrode t(at loses mass

/(e electrons lo rom

1" ra an operating electroc(emical cell using an Al (al5cell and a Cg (al5cell" 4abel t(e parts o t(e electroc(emical cell including t(e anode or cat(ode, and all reagents and materialsused" Write t(e reactions and determine t(e *"

11" Write t(e (al reaction t(at occurs at eac( electrode during t(e electrolsis o a9ueous

1" C Na:"

Anode <

'at(ode <

W(at is t(e minimum re9uired Doltage or t(is processE

12" Write t(e (al reaction t(at occurs at eac( electrode during t(e electrolsis o molten Na:"

Anode <

%age 54 o 117


55/117

'at(ode <

W(at is t(e minimum re9uired Doltage or t(is processE

13" Aluminum is produced industriall rom aluminum oxide, Al2O3" emonstrate ourunderstanding o t(is process b

?i= escribing (o t(e process is carried out,

?ii= Writing e9uations o t(e reactions inDolDed in t(e process, and

?iii= escribing (o t(e problem o t(e (ig( melting point oAl2O3 is oDercome"

1#" 'onsider t(e olloing redox data<

3I 6 27a36 F 3I26 6 27a *o J 6")# I

3I26 6 2Al F 3I 6 2Al36 *o J 6"#) I

Based on t(ese obserDations, a student concludes t(at 7a63 and Al ill react spontaneousl"4ist t(e oxidi0ing agents in order o decreasing strengt(" Write reduction reactions or eac("

etermine t(e strongest reducing agent" etermine i 7a63 and Al ill react spontaneousl"

1$" Balance t(e e9uation or t(e olloing (al reaction occurring in acid solution<

I?s= F HI2O+35

1)" Balance t(e olloing redox reaction occurring in basic solution<

CnO#5 6 '2O#25 F CnO2 6 'O2

%age 55 o 117


56/117

1+" 2$" ml "2C CnO#5 reacts it( excess SO325" Ho man grams o CnO2 are producedE

2CnO#5 6 3SO325 6H2O F 2CnO2 63SO#25 6 2OH5

1-" etermine t(e oxidation number or eac( bo$d atom"

9nO2 +O35 Cr2O+25 C2O#25 *$?NO3=3 NH#'l Na#

HOOH NO35 H3O# Na2C2O# +2 N2O3 t?H2O=#26

1." 2$" m4 o "$C CnO#5 are re9uired to titrate a 1" ml sample o SO352" 'alculate t(eKSO352L

2CnO#5 6 3SO325 6H2O F 2CnO2 6 3SO#256 2OH5

2" Ho is t(e breat(al0er reaction used to determine BA'E Write t(e reaction and describe (oit ors"

21" 2H6 6 Cg F Cg26 6 H2

etermine t(e Oxidi0ing agent>>>>>>>>>> and t(e Reducing agent>>>>>>>>>

%age 56 o 117


57/117

22" '(oose a suitable redox reactant to oxidi0e 'l5 to'lO#5 in a redox titration"

23" escribe as an electroc(emical or electroltic cell<

a= 8uel cell

b= '(arging a car batter

c= isc(arging a car batter

d= Ni plating

e= :ndustrial Al production

= 'l2 production

g= *lectroinning

2#= W(ic( o t(e reactants is gaining electronsE W(ic( o t(e reactants is t(e oxidi0ing agentE

Br 2 6 SO2 6 Na2SO# 6 H2O F 2H2SO# 6 2NaBr

2$= A student studied t(e olloing reactions and s(e recorded<

%d26

6 'u F %d 6 'u26

spontaneous%d26 6 Au F no reaction

%d26 6 Hg F no reaction

Au36 6 Hg F Au 6 Hg26 spontaneous

%age 57 o 117


58/117

4ist t(e oxidi0ing agents rom strongest to eaest" 4ist t(e reducing agents rom strongest toeaest" %redict i t(e reaction ill occur"

Au36 6 'u F

2)= Catc( eac( tpe o electroltic cell it( t(e example cell"

*lectroinning A silDer anode oxidi0es & Ag reduces on a 'u cat(ode

*lectroplating %ure %b is reduced at t(e cat(ode (ile impure %b oxidi0es at t(e anode

*lectroreining %ure Al is reduced at t(e cat(ode rom molten bauxite ?Al2O3="

2+" 4ist t(e anode, cat(ode, anode reaction , cat(ode reaction, and electrolte or eac(commercial electroc(emical cell"

'ell anode anode reaction cat(ode cat(ode reaction electrolte

4eclanc(e or'ommon r'ell

Alaline 'ell

4ead Storage or'ar Batter

8uel 'ell

2-" W(ic( o t(e aboDe cells re9uires continuous input o O2 and H2 and is produced b Ballard:ndustriesE

2." 4ist t(e anode, cat(ode, anode reaction, cat(ode reaction, and electrolte or eac( commercialelectroltic cell"

'ell anode anode reaction cat(ode cat(ode reaction electrolte

%age 58 o 117


59/117

*lectrolsis oColten Al2O3

*lectrolsis oA9ueous Na'l

SilDer5plating a'u plating

*lectroreining pure %b romimpure %b

3" escribe eac( term<

salt bridge

electrolte

anode

cat(ode

spontaneous

electron ainit

cation

anion

electroc(emicalcell

electroltic cell

oxidation number

electrolsis

oxidation

%age 5 o 117


60/117

reduction

oxidi0ing agent

reducing agent

electrode

corrosion

electroinning

electroreining

oDer potentialeect

uel cell

31" eine corrosion o a metal, and illustrate our deinition it( reerence to an example, usingappropriate e9uations" 7iDe /WO met(ods b (ic( corrosion can be preDented and describe(o eac( met(od ors" /(e to met(ods must inDolDe dierent c(emical principles"

32" W(ic( ou ould c(oose ;n or 'u to cat(odicall protect ironE

33" A26 does not react it( B, (ile '26 reacts it( B" Ran t(e oxidi0ing agents in decreasingorder o strengt(" Ran t(e reducing agents in decreasing order o strengt(" Will A26 react it('E

3#" Write (al reactions or eac( using t(e reduction table and list t(e (al5cell potential"

Hal Reaction *o

oxidation o ater

%age 6! o 117


61/117

oxidation o ater in acid

reduction o ater

reduction o ater in alaline

oxidation o H2 in ater

oxidation o H2 in acid

oxidation o H2 in base

reduction o 'r 2

O+25

in acid

reduction o HBr

%age 61 o 117


62/117

3$" 'ompletel anal0e t(e olloing electroc(emical cell"

/(e anode reaction is<

/(e cat(ode reaction is<

/(e electrons lo rom >>> to >>>

/(e ions t(at migrate to t(e ;n electrode are<

/(e ions t(at migrate to t(e 'u electrode are<

/(e initial Doltage o t(is cell is<

/(e Doltage o t(is cell once e9uilibrium is reac(ed is<

escribe t(e c(ange in K'u62L in t(e 'u (al cell

escribe t(e c(ange in KNO351L in t(e ;n (al cell

%age 62 o 117

1" C NO3

1 C ;n?NO3=

2

'u;n

1 C 'u?NO3=

2

Doltmeter


63/117

3)" 'ompletel anal0e t(e olloing electroc(emical cell"

/(e anode reaction is<

/(e cat(ode reaction is<

/(e electrons lo rom >>> to >>>

/(e ions t(at migrate to t(e %t electrode are<

/(e ions t(at migrate to t(e 'u electrode are<

/(e intial Doltage o t(is cell is<

/(e Doltage o t(is cell once e9uilibrium is reac(ed is<

escribe t(e c(ange in K'u62L in t(e 'u (al cell

escribe t(e c(ange in KNO351L in t(e H6!H2 (al cell

%age 63 o 117

1 C H'l

'u

1 C 'u?NO3=

2

Doltmeter

H2?g=

1" C NO3


64/117

3+" 'ompletel anal0e t(e olloing electroltic cell"

Anode Reaction

'at(ode Reaction

'(emicals produced at t(e anode

'(emicals produced at t(e cat(ode

/(e electrons lo rom >>to >>

/(e c(emical used to loer t(e mp is<

W(ic( electrode is t(e anode E

3-" 'ompletel anal0e t(e olloing electroltic cell" Note t(at t(e electrodes are not inert and because o t(at, t(e anode mig(t oxidi0e"

%age 64 o 117

%oer Source

5 6

'

'

Colten Al2O

3

%oer Source

5 6

'u

'u

1 C Na8


65/117

Anode Reaction

'at(ode Reaction

'(emicals produced at t(e anode

'(emicals produced at t(e cat(ode

/(e electrons lo rom

/(e C/I

W(ic( electrode is t(e anode E

/$ectroche0istr ractice est " 1

1" /(e olloing represents t(e process used to produce iron rom iron ::: oxide<

8e2O3 6 3'O F 28e 6 3'O2 W(at is t(e reducing agent in t(is processE

A" 8eB" 'O'" 'O2" 8e2O3

2" 'onsider t(e olloing reaction< 2HNO2 6 2:5

6 2H6

F 2NO 6 :2 62H2O/(e oxidation number or eac( nitrogen atom

A" increases b 1B" increases b 2'" decreases b 1" decreases b 2

3" W(ic( o t(e olloing reactions is spontaneousE

A" 2:5 6 Ag F Ag6 6 :2

B" 'o

26

6 'u F 'o 6 'u

26

'" 'u26 6 %b F %b26 6 'u" Ni26 6 2Ag F 2Ag6 6 Ni

%age 65 o 117


66/117

#" 'onsider t(e olloing redox reaction or a lead5acid storage cell<%b 6 %bO2 6 #H6 6 2SO#25 → 2%bSO# 6 2H2O/(e balanced, reduction (al reaction is

A" %b 6 SO#25 F 2%bSO# 6 2e5

B" %b 6 2H6 6 SO#25 F %bSO# 6 2H2O 6 2e5

'" %bO2 6 #H6 6 SO#25 6 2e5 F %bSO# 6 2H2O

" %bO2 6 2SO#2 6 2H2O 6 2e5 F %bSO# 6 2OH5 $" 'onsider t(e olloing reaction< 'd26?a9= 6 ;n?s= F 'd?s= ;n26?a9=

/(e potential or t(e reaction is 6"3) I" W(at is t(e reduction potential or t(e cadmium ionE

A" 51"12 IB" 5"# I'" 6"# I" 61"12 I

)" W(ic( o t(e olloing inDolDes a nonspontaneous redox reactionE

A" uel cellB" electroplating'" redox titration" carbon dr cell

+" 'onsider t(e olloing redox reaction<

2CnO#5 6 1)H6 6 $Sn26 F 2Cn26 6 -H2O 6 $Sn#6

:n a redox titration, ") mole o CnO# reacts completel it( a solution o Sn?NO3=2" Homan moles o Sn?NO3=2 ere present in t(e solutionE

A" "2# molesB" ") moles'" 1"$ moles" "3 moles

-" W(ic( o t(e olloing is not a redox reactionE

A" 'u 6 Br 2 F 'uBr 2B" 'O 6 H2O F 'O2 6 H2'" 'H# 6 H2O F 'O2 6 2H2O" NaOH 6 H'l F Na'l 6 H2O

." W(at is t(e minimum Doltage re9uired to orm nicel rom an a9ueous solution o Ni:2 usinginert electrodesE

A" "2) IB" "2- I'" "$# I" "- I

%age 66 o 117


67/117

1" W(at substances are ormed at t(e anode and cat(ode during electrolsis o molten sodiumc(lorideE

Anode 'at(ode

A" O2 H2B" Na 'l2

'" 'l2 H2" 'l2 Na

11" A solution containing an unnon cation reacts spontaneousl it( bot( 0inc and copper" /(eunnon cation is

A" 1" C H6

B" 1" C Ag6

'" 1" C Sr 26

" 1" C Cn26

12" W(ic( o t(e olloing (al5reactions are balancedE A" 'lO5 6 H2O 6 e5 F 'l2 6 2OH5

B" 2'lO5 6 H2O 6 2e5 F 'l2 6 3OH5

'" 2'lO5 6 2H2O 6 2e5 F 'l2 6 #OH5

" 2'lO5 6 2H2O F 'l2 6 #OH5 6 2e5

13" W(ic( o t(e olloing is a spontaneous redox reactionE

A" Ag6 6 :5 F Ag:B" Ag6 6 8e26 F Ag 6 8e36

'" 3Ag6 6 Au F 3Ag 6 Au36" 2Ag6 6 Ni26 F 2Ag 6 Ni 1#" Salting t(e roads during t(e inter increases t(e amount o corrosion o cars" /(e is because

t(e salt

A" reacts it( t(e ironB" proDides an electrolte'" acts as a reducing agent" acts as an oxidi0ing agent

%age 67 o 117


68/117


69/117

1." /(e electrons lo

A" t(roug( t(e salt bridge rom 'u to NiB" t(roug( t(e salt bridge rom 'u to Ni'" t(roug( t(e ire rom 'u to Ni" t(roug( t(e ire rom Ni to 'u

2" W(ic( o t(e olloing ill not react spontaneousl it( 1" C H'lE

A" tinB" lit(ium'" mercur" magnesium

21" W(ic( o t(e olloing can be produced b electrolsis rom a 1" C a9ueous solution

containing its ionE

A" nicel

B" sodium'" aluminum" magnesium

22" :n order or an electroltic cell to operate, it must (aDe

A" a Doltmeter"B" a salt bridge"'" a poer suppl"" an a9ueous solution"

23" :n t(e electrolsis o molten ;n'l2 using carbon electrodes, t(e reaction t(at occurs at t(eanode is

A" ;n F ;n26 6 2e5

B" ;n26 6 2e5 F ;n'" 2'l5 F 'l2 6 2e5

" 'l2 6 2e5 F 2'l5

2#" :n t(e electrolsis o molten 0inc c(loride, t(e (al5reaction at t(e anode is

A" 'l2 6 2e5 F 2'l5

B" 2'l5

F 'l2 6 2e5

'" ;n26 6 2e5 F ;n" ;n F ;n26 6 2e5

%age 6 o 117


70/117

2$" /(e corrosion o iron can be preDented b attac(ing a piece o

A" CnB" 'u'" %b" Sn

2)" /(e oxidation number o carbon in 'a'2O# is

A" 62B" 63'" 6#" 6)

2+" /o plate a nicel coin it( copper,

A" t(e nicel coin must be t(e cat(ode"B" t(e cat(ode must be made out o copper

'" t(e electrons must lo to t(e anode" t(e solution must contain nicel ions

'onsider t(e olloing electroc(emical cell or t(e next iDe 9uestions"

2-" W(ic( o t(e olloing statements appl to t(is electroc(emical cellE

: *lectrons lo t(roug( t(e ire toard t(e copper electrode"

:: /(e copper electrode increases in mass"::: Anions moDe toard t(e ;n (al5cell"

A" : and :: onlB" : and ::: onl'" :: and ::: onl" :, ::, and :::

%age 7! o 117

;n'uuu

1" C NO3

1C 'u?NO3=

21C ;n?NO

3=

2

Doltmeter


71/117

2." /(e balanced e9uation or t(e oDerall reaction is

A" ;n 6 'u26 F 'u 6 ;n26

B" 'u 6 ;n26 F ;n 6 'u26

'" ;n26 6 'u F 'u26 6 ;n" 'u 6 ;n F ;n 6 'u

3" At e9uilibrium t(e Doltage o t(e aboDe cell is

A" 51"1 IB" " I'" 6"#2 I" 61"1 I

31" /(is redox reaction occurs because

A" ;n is a stronger oxidi0ing agent t(an 'uB" ;n is a stronger reducing agent t(an 'u,

'" 'u is a stronger oxidi0ing agent t(an ;n" ;n26 is a eaer reducing agent t(an 'u26

32" /(e initial cell Doltage at 2$ o' is

A" 51"1 IB" 61"1 I'" 6".1 I" 6"-) I

33" 'onsider t(e olloing redox reaction< 'o26?a9= 6 2Ag?s= ⇋ 2Ag6?a9= 6 'o?s=

/(e reaction is A" spontaneous and *o is positiDeB" spontaneous and *o is negatiDe'" non5spontaneous and *o is positiDe" non5spontaneous and *o is negatiDe

3#" W(en CnO#5 reacts to orm Cn26, t(e manganese in CnO#5 is

A" reduced as its oxidation number increasesB" reduced as its oxidation number decreases

'" oxidi0ed as its oxidation number increases" oxidi0ed as its oxidation number decreases

3$" /(e electrolte used in t(e alaline batter is%age 71 o 117


72/117

A" 'lB" NaOH'" H2SO#" OH

3)" /(e electrolte used in an automobile batter is

A" 'lB" NaOH'" H2SO#" OH

3+" /(e anode used in t(e commercial production o Aluminum is

A" 'B" %t'" Al

" Al2O3 3-" /(e anode and cat(ode used in t(e electroreining o impure lead to pure lead are

Anode 'at(ode

A" %ure %b :mpure %bB" :mpure %b %ure %b'" %b26 %b" %b %b26

3." /(e anode in t(e 4e'lanc(e or common dr cell is A" 'B" ;n'" Cg" OH

#" W(ic( o t(e olloing are electroltic cells

: *lectro inning:: *lectroplating

::: '(arging a car batter:I 8uel cell

A" : and :: onlB" :, ::, and ::: onl'" :: and :: onl" :, ::, :::, and :I

Sub;ecti-e

%age 72 o 117


73/117

1" Balance t(e olloing in basic solution"

CnO#5 6 '2O#25 F CnO2 6 'O2 ?basic=

2" 'onsider t(e electrolsis o 1" C H2SO# using platinum electrodes"

a= Write t(e oxidation (al5reaction

b= Write t(e reduction (al5reaction

c= Write t(e oDerall reaction and determine t(e minimum t(eoretical Doltage re9uired"

3" 'onsider t(e olloing diagram or t(e electro reining o lead"

%age 73 o 117

%oer Source

:mpure %b%ure %b


74/117

a= On t(e diagram, label t(e anode and cat(ode"

b= Write t(e ormula or a suitable electrolte

c= Write t(e e9uation or t(e reduction (al5reaction"

#" escribe to che0ica$$ di%%erent met(ods t(at can be used to preDent corrosion o iron andexplain ( eac( met(od ors"

Cet(od 1<

*xplanation<

Cet(od 2<

*xplanation<

$" /(e data belo ere obtained in a redox titration o a 2$" m4 sample containing Sn26 ionsusing "12$ C CnO# according to t(e olloing reaction<2CnO#5 6 1)H6 6 $Sn26 F 2Cn26 6 -H2O 6 $Sn#6

'alculate t(e KSn26L

Iolume o CnO# used ?m4=

/rial 1 /rial 2 /rial 3

:nitial burette reading 2" 13"- 2#"$$8inal burette reading 13"- 2#"$$ 3$"32

%age 74 o 117


75/117

)" A student anted to electroplate a coin it( copper"

a= :denti a suitable anode

b= :denti an appropriate electrolte

c= /o it( batter terminal ?positiDe or negatiDe= s(ould t(e coin be connectedE

+" 'onsider t(e electrolsis o molten magnesium c(loride it( 'u electrodes ?'u electrodesare not inert and can oxidi0e< 'l5, or 'u ill oxidi0e=

a= :denti t(e product at t(e anode"

b= Write t(e e9uation or t(e reduction (al5reaction"

c= Write t(e e9uation or t(e oDerall reaction"

-" 'ompletel anal0e t(e olloing electroc(emical cell"

%age 75 o 117

CnSn

nnn

1" C NO3

1C Sn?NO3=

21C CnNO

3=

2

Doltmeter


76/117

Che0istr 12

/$ectroche0istr ractice est 2

1" As t(e cell operates, t(e electrons lo rom t(e nicel electrode to t(e palladium electrode"/(e reaction occurring at t(e anode is

A %d → %d26 6 2e5

B Ni F Ni26 6 2e5

' %d26 6 2e5 F %b Ni26 6 2e5 F Ni

2" As t(e cell operates,

A bot( t(e 6 and t(e NO35 migrate into t(e nicel (al5cellB bot( t(e 6 and t(e NO35 migrate into t(e palladium (al5cell' t(e 6 migrates into t(e nicel (al5cell and t(e NO35 migrates into t(e palladium (al5

cell t(e 6 migrates into t(e palladium (al5cell and t(e NO35 migrates into t(e nicel (al5

cell

3" /(e initial cell Doltage is 1"21 I" /(e reduction potential o %d26 is

A 51"21 IB 5".$ I' 6".$ 61"21 I

%age 76 o 117

Ni%d

1" C 'l

1C %d?NO3=

21C Ni?NO

3=

2

Doltmeter


77/117

#" W(at substances are ormed at t(e anode and cat(ode during electrolsis o moltensodium c(loride, Na'l?l=E

Anode 'at(ode

A O2 H2B Na 'l2

' 'l2 H2 'l2 Na

$" 'onsider t(e olloing electroltic cell<

:n t(e cell aboDe A :5 migrates to t(e anode and gains electrons

B :5 migrates to t(e cat(ode and loses electrons' Na6 migrates to t(e anode and loses electrons

Na6 migrates to t(e cat(ode and gains electrons )" W(ic( o t(e olloing are necessar or electroplating to occur using an electroltic

cellE: /o electrodes:: A metal being reduced::: A direct current poer suppl

A : and :: onlB : and ::: onl' :: and ::: onl

:, ::, and ::: +" A uel cell consumes H2 and O2 gas, uses a OH electrolte, and produces electricit" /(ereaction at t(e anode is

A 2H6 6 2e5 F H2B 1!2O2 6 2H6 6 2e5 F H2O' #OH5 F O2 6 2H2O 6 #e5

H2 6 2OH5 F 2H2O 6 2e5

%age 77 o 117

%oer Source6 5

:nert*lectrode

:nert*lectrode

Colten Na:?l=


78/117

-" A student inDestigating redox reactions recorded t(e olloing results<

I26 6 /e25 F no reaction#6 6 /e25 F 36 6 /e

Based on t(ese results, t(e strengt(s o t(e oxidi0ing agents, arranged rom strongest to

eaest, are

A I26 /e #6

B #6 /e I26

' 36 /e25 I26

I26 /e25 36

." W(at is t(e minimum Doltage re9uired to orm nicel rom an a9ueous solution o Ni:2using inert electrodesE

A "2) I

B "2- I' "$# I "- I

1"

W(ic( o t(e olloing occurs as t(e cell operatesE

A t(e ;n electrode is reduced and increases in massB t(e ;n electrode is reduced and decreases in mass

' t(e ;n electrode is oxidi0ed and increases in mass t(e ;n electrode is oxidi0ed and decreases in mass 11" W(ic( o t(e olloing reactants ould produce an * o 6")3 IE

A Ag6 6 :2B %b26 6 ;n' Cg26 6 'a ;n26 6 Cn

%age 78 o 117

Ni;n

1" C NO3

1C ;n?NO3=

21C Ni?NO

3=

2

Doltmeter


79/117

12" /(e concentration o 8e26?a9= can be determined b a redox titration using

A Br B Sn'l2' CnO# ?basic= BrO3 ?acidic=

13" W(ic( o t(e olloing ill oxidi0e 8e26E

A :2?s=B Ni?s=' ;n?s= Br 2?l=

1#" /(e oxidation number o carbon in '2O#25 is

A 63

B 6#' 6$ 6)

1$" 'onsider t(e olloing reaction< 3As2O3 6 #NO35 6 +H2O F )H3AsO# 6 #NO

/(e oxidi0ing agent is

A H6

B H2O' NO35

AsO3 1)" W(en W2O$ is conDerted to WO2 in a redox reaction, t(e W (as been

A reduced since its oxidation number (as increasedB reduced since its oxidation number (as decreased' oxidi0ed since its oxidation number (as increased oxidi0ed since its oxidation number (as decreased

1+" 'onsider t(e olloing<

: Water :: Oxgen gas::: Nitrogen

At 2$o', a piece o iron rusts in t(e presence oA : onlB ::: onl' : and :: onl :: and ::: onl

%age 7 o 117


80/117

1-" W(ic( o t(e olloing represents a redox reactionE

A H2'O3 F H2O 6 'O2B 'uS 6 H2 F H2S 6 'u' AgNO3 6 Na'l F Ag'l 6 NaNO3 2H'l 6 Na2SO3 F 2Na'l 6 H2SO3

1." /(e olloing reaction occurs in an electroc(emical cell<3'u26 6 'r F 2'r 36 6 3'u/(e *o or t(e cell is

A "# IB "+$ I' 1"- I 2"$ I

2" uring t(e corrosion o magnesium, t(e anode reaction is

A Cg F Cg26 6 2e5B Cg26 6 2e5 F Cg' #OH5 F O2 6 2H2O 6 #e5

O2 6 2H2O 6 #e5 F #OH5

21" A molten binar salt, ;n'l2, undergoes electrolsis" /(e cat(ode reaction is

A ;n F ;n26 6 2e5

B 2'l5 F 'l2 6 2e5

' 'l2 6 2e5 F 2'l5

;n26 6 2e5 F ;n

22" W(ic( o t(e olloing represents a redox reactionE

A 'a'O3 F 'aO 6 'O2B Si'l# 6 2Cg F Si 6 2Cg'l2' 2NaOH 6 H2SO# F 2H2O 6 Na2SO# AgBr 6 2S2O325 F Ag?S2O3=235 6 Br 5

23" /(e process o appling an electric current t(roug( a cell to produce a c(emical c(ange

is called

A corrosionB ioni0ation' (drolsis electrolsis

%age 8! o 117


81/117

2#" A student inDestigating redox reactions recorded t(e olloing results<

I26 6 /e25 F no reaction

#6 6 /e25 F 36 6 /e

Based on t(ese results, t(e strengt(s o t(e oxidi0ing agents, arranged rom strongest to

eaest, are

A I26 /e #6

B #6 /e I26

' 36 /e25 I26

I26 /e25 36

2$" A spontaneous redox reaction occurs (en Sn26 is mixed it(

A :2B 'u

' H2S Ag2S 2)" 'onsider t(e redox reaction< 2BrO35 6 1'l5 6 12H6 F Br 2 6 $'l2 6 )H2O

t(e oxidation (al5reaction iDolDed in t(is reaction is

A 2'l5 F 'l2 6 2e5

B 2H6 F H2 6 2e5

' BrO35 6 )H6 6 $e5 F Br 2 6 3H2O BrO35 6 )H6 F Br 2 6 3H2O + 5e-

2+" W(ic( o t(e olloing is not a redox reactionE A 'u 6 Br 2 F 'uBr 2B 'O 6 H2O F 'O2 6 H2' 'H# 6 O2 F 'O2 6 2H2O NaOH 6 H'l F Na'l 6 H2O

2-" uring t(e electrolsis o 1" C Na2SO#, t(e reaction at t(e cat(ode is

A Na6 6 1e5 F NaB 2SO#25 F S2O-25 6 2e5

' 2H2O F O2 6 H6 6 #e5 2H2O 6 2e5 F H2 6 2OH5

2." An oxidi0ing agent ill cause (ic( o t(e olloing c(angesE

A %tO2 F %tOB %tO3 F %tO2' %t?OH=2 F %t %t?OH=226 F %tO3

%age 81 o 117


82/117

3" 'onsider t(e oDerall reaction o t(e nicel5cadmium batter<

NiO2?s= 6 'd?s= 6 2H2O?l= F Ni?OH=2?s= 6 'd?OH=2?s= W(ic( o t(e olloing occurs at t(e anode as t(e reaction proceedsE

A 'd loses 2e5 and orms 'd?OH=2?s=

B 'd gains 2e5 and orms 'd?OH=2?s=' NiO2 loses 2e5 and orms Ni?OH=2?s= NiO2 gains 2e5 and orms Ni?OH=2?s=

31" W(ic( o t(e olloing can be produced b t(e electrolsis rom a 1" C a9ueous solutioncontaining its ionsE

A nicelB sodium' aluminum magnesium

32" :n t(e electrolsis o molten ;n'l2 using carbon electrodes, t(e reaction t(at occurs at t(eanode is A ;n F ;n26 6 2e5

B ;n26 6 2e5 F ;n' 2'l5 F 'l2 6 2e5

'l2 6 2e5 F 2'l5

33" :n order or t(e electroltic cell to operate, it must (aDe

A a Doltmeter B a salt bridge' a poer suppl an a9ueous solution

%age 82 o 117


83/117

Sub@ectiDe 1" a= :ndicate in t(e blan spaces on t(e olloing c(art (et(er or not a reaction ill

occur (en t(e metals are added to t(e a9ueous ions"

%d R( %t

%d26

R(26 no reaction no reaction

%t26 reaction reaction

b= 4ist t(e oxidi0ing agents in order o strongest to eaest

2" 'onsider t(e olloing reaction or t(e ormation o rust<

8e?s= 6 O2?g= 6 H2O?l= F 8e?OH=2

escribe and explain to met(ods, using dierent c(emical principles, to preDent t(eormation o rust"

a=

b=


H2Se 6 SO#25

6 2H6

F Se 6 H2SO3 6 H2O 'alculate t(e *o or t(e reaction"

%age 83 o 117


84/117


85/117

+" 'onsider t(e olloing diagram in t(e electro reining o lead<

a= On t(e diagram aboDe, label t(e anode and cat(ode"

b= Write t(e ormula or a suitable electrolte"

c= Write t(e e9uation or t(e reduction (al5reaction"

d= Write t(e anode reaction

%age 85 o 117

%oer Source

:mpure %b %ure %b


86/117

Oxidation and Reduction Reactions Workbook

Notes' doub$e c$ick on the $esson nu0ber and don$oad %oer %oint Iieer i ou do not(aDe it"

Wors(eets Pui0

1" Oxidation, Reduction, Agents, & Reactions" WS 1

2" 4ab< /(e Strengt( o Oxidi0ing Agents"

3" Oxidation Numbers Spontaneous Reactions WS 2 1

#" Oxidation Numbers, Application to Reactions" WS 3

$" Balancing Redox Hal Reactions Acid!Base" WS # 2

)" Balancing Redox Reactions in Acid!Base" WS $

+" Standard %otentials sing '(art" WS ) 3

-" *lectroc(emical 'ells" WS +

." *lectroc(emical 'ells 4ab"

1" *lectroltic 'ells" WS - #

11" *lectroltic 'ells 4ab"

12" Application o *lectroltic 'ells" WS . $ 13" Application o *lectroc(emical 'ells< Bat & 'or" WS 1 )

1#" Breat(al0er and reDie" :nternet ReDie Pui0mebc

1$" ReDie %ractice /est G 1

1)" ReDie %ractice /est G 2

1+" /est"

ext book #ebden Read >

%age 86 o 117

http://www.microsoft.com/downloads/details.aspx?FamilyID=7C404E8E-5513-46C4-AA4F-058A84A37DF1&displaylang=ENhttp://www.microsoft.com/downloads/details.aspx?FamilyID=7C404E8E-5513-46C4-AA4F-058A84A37DF1&displaylang=ENhttp://www.microsoft.com/downloads/details.aspx?FamilyID=7C404E8E-5513-46C4-AA4F-058A84A37DF1&displaylang=ENhttp://www.microsoft.com/downloads/details.aspx?FamilyID=7C404E8E-5513-46C4-AA4F-058A84A37DF1&displaylang=ENhttp://www.microsoft.com/downloads/details.aspx?FamilyID=7C404E8E-5513-46C4-AA4F-058A84A37DF1&displaylang=ENhttp://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Redox/Powerpoint/1.IntroductionRedox.ppthttp://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Redox/Workbookredoxanswers.htm#ws1%23ws1http://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Redox/Powerpoint/2.Oxidizingagentslab.ppthttp://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Redox/Powerpoint/3.Oxidationnumbers.ppthttp://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Redox/Workbookredoxanswers.htm#ws2%23ws2http://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Quizzes/redox/redoxquiz1ans.htmhttp://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Quizzes/redox/redoxquiz1ans.htmhttp://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Redox/Powerpoint/4.Usingoxidationnumbers.ppthttp://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Redox/Workbookredoxanswers.htm#ws3%23ws3http://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Redox/Powerpoint/5.Balancingredoxhalfreactions.ppthttp://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Redox/Workbookredoxanswers.htm#ws4%23ws4http://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Quizzes/redox/redoxquiz2ans.htmhttp://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Quizzes/redox/redoxquiz2ans.htmhttp://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Redox/Powerpoint/6.Balancingredoxfullreactions.ppthttp://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Redox/Workbookredoxanswers.htm#ws5%23ws5http://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Redox/Powerpoint/7.Standardhalfcellsusingchart.ppthttp://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Redox/Workbookredoxanswers.htm#ws6%23ws6http://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Quizzes/redox/redoxquiz3ans.htmhttp://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Redox/Powerpoint/8.Electrochemicalcells.ppthttp://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Redox/Workbookredoxanswers.htm#ws7%23ws7http://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Redox/Powerpoint/9.%20Electrochemicalcelllab.ppthttp://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Redox/Powerpoint/10.Electrolyticcells.ppthttp://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Redox/Workbookredoxanswers.htm#ws8%23ws8http://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Quizzes/redox/redoxquiz4ans.htmhttp://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Redox/Powerpoint/11.%20Electrolyticcelllab.ppthttp://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Redox/Powerpoint/12.Applicationelectrolyticells.ppthttp://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Redox/Workbookredoxanswers.htm#ws9%23ws9http://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Quizzes/redox/redoxquiz5ans.htmhttp://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Redox/Powerpoint/13.Applicationelectrochemicalcells.ppthttp://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Redox/Workbookredoxanswers.htm#ws10%23ws10http://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Quizzes/redox/redoxquiz6ans.htmhttp://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Quizzes/redox/redoxquiz6ans.htmhttp://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Redox/Powerpoint/14.Breathalyzer.ppthttp://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Chemistry12Answers/Redoxa.htmlhttp://www.quizmebc.ca/http://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Redox/Powerpoint/15.Review.ppthttp://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Quizzes/redox/electrochempracticetestanswers.htmhttp://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Redox/Powerpoint/15.Review.ppthttp://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Quizzes/redox/Redox%20%20Practice%20Test%202%20Answers.htmhttp://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Redox/Powerpoint/1.IntroductionRedox.ppthttp://www.mouatonline.com/Teachers/MIannone/Science/Chemistry/Iannone/Redox/Workbookredoxanswers.htm#ws1%23ws1http:/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