Chemistry 12 - Weebly
Transcript of Chemistry 12 - Weebly
Contents: 19 pages Examination: 2 hours 50 multiple-choice questions Additional Time Permitted: 60 minutes © Province of British Columbia
Chemistry 12 Examination Booklet
2009/10 Released Exam January 2010 Form A
DO NOT OPEN ANY EXAMINATION MATERIALS UNTIL INSTRUCTED TO DO SO.
FOR FURTHER INSTRUCTIONS REFER TO THE RESPONSE BOOKLET.
Chemistry 12 – 1001 Form A Page 1
PART A: MULTIPLE CHOICE Value: 62.5% of the examination
Suggested Time: 80 minutes
INSTRUCTIONS: For each question, select the best answer and record your choice on the Answer Sheet provided. Using an HB pencil, completely fill in the bubble that has the letter corresponding to your answer.
You have Examination Booklet Form A. In the box above #1 on your Answer Sheet,
fill in the bubble as follows.
FA B C D E HGExam Booklet Form/Cahier d’examen
1. Which of the following reactions would you expect to proceed most rapidly
at room temperature? A. Ca s( ) +S s( ) → CaS s( )
B. H2 g( ) + Cl2 g( ) → 2HCl g( )
C. Pb2+ aq( ) + CO32− aq( ) → PbCO3 s( )
D. Br2 ( ) + H2O ( ) → 2Br− aq( ) + 1
2 O2 g( ) + 2H+ aq( )
2. Solid sodium metal reacts rapidly with water in an open beaker to produce aqueous
sodium hydroxide and hydrogen gas. A change in which of the following could be used to measure the rate of this reaction?
A. the volume of the solution B. the pressure of the hydrogen gas C. the concentration of the solid sodium D. the mass of the beaker and its contents
Page 2 Chemistry 12 – 1001 Form A
3. Consider the following PE diagram:
Progress of reaction
PE(kJ)
500
300
100
400
200
Which of the following is correct for the activated complex?
PE (kJ) Stability
A. 200 low
B. 200 high
C. 500 low
D. 500 high
4. When carbon disulphide reacts with chlorine gas, 238 kJ is released.
Which of the following correctly represent this reaction?
I CS2 g( ) + 3Cl2 g( ) → CCl4 g( ) + S2Cl2 g( ) + 238 kJ
II CS2 g( ) + 3Cl2 g( ) + 238 kJ → CCl4 g( ) + S2Cl2 g( )
III CS2 g( ) + 3Cl2 g( ) → CCl4 g( ) + S2Cl2 g( ) ΔH = +238 kJ
IV CS2 g( ) + 3Cl2 g( ) → CCl4 g( ) + S2Cl2 g( ) ΔH = −238 kJ
A. I and III only B. I and IV only C. II and III only D. II and IV only
Chemistry 12 – 1001 Form A Page 3
5. Consider the following reaction mechanism:
Step 1: 2NO → N2O2
Step 2: N2O2 + H2 → N2O + H2O
Step 3: N2O + H2 → N2 + H2O
Which of the following is correct?
Activated Complex Reaction Intermediate
A. N2O N2O2
B. N2O2 H2O
C. N2OH2 N2O
D. N2O2H2 N2
Page 4 Chemistry 12 – 1001 Form A
6. A student places some HI g( ) into a closed reaction container and the following equilibrium is established:
2HI g( ) →← I2 g( ) + H2 g( )
Which of the following describes the forward and reverse reaction rates? A.
reverse
forward
Time
ReactionRate
B.
forward
reverse
Time
ReactionRate
C.
reverse
forward
Time
ReactionRate
D.
forward
reverse
Time
ReactionRate
Chemistry 12 – 1001 Form A Page 5
7. Consider the equilibrium:
H2 g( ) + FeO s( ) →← H2O g( ) + Fe s( )
The following chemicals are placed in separate 1.0 L containers.
Container I H2, H2O
Container II Fe, FeO
Container III H2O, Fe
Container IV H2, H2O, FeO
In which container(s) will the equilibrium be established? A. Container III only B. Container IV only C. Containers I and II only D. Containers III and IV only 8. Consider the following:
energy + 6CO2 g( ) + 6H2O( )
?→← C6H12O6 s( ) + 6O2 g( )
Which of the following describes how enthalpy and entropy change in the forward direction?
Enthalpy Entropy
A. increases decreases
B. increases increases
C. decreases increases
D. decreases decreases
Page 6 Chemistry 12 – 1001 Form A
9. Consider the following system at equilibrium:
energy + N2H6CO2 s( ) →← 2NH3 g( ) + CO2 g( )
Which of the following is correct when the volume of the system is increased?
Equilibrium Shift Amount of N2H6CO2
A. left increases
B. left no change
C. right decreases
D. right no change
10. Consider the following system at equilibrium:
2NO g( ) + O2 g( ) →← 2NO2 g( )
Some O2 is added to the equilibrium. Which of the following describes how the
forward and reverse reaction rates change as a new equilibrium is being established?
Forward Rate Reverse Rate
A. increases decreases
B. increases increases
C. decreases increases
D. decreases decreases
Chemistry 12 – 1001 Form A Page 7
11. Consider the following equilibrium:
NH4NO2 s( ) →← N2 g( ) + 2H2O g( )
Which of the following correctly represents the H2O[ ] at equilibrium?
A. H2O[ ] =Keq
N2[ ]
B. H2O[ ] = 12
Keq
N2[ ]⎛⎝⎜
⎞⎠⎟
C. H2O[ ] =Keq NH4NO2[ ]
N2[ ]
D. H2O[ ] =Keq NH4NO2[ ]
N2[ ]
12. Consider the following:
I COCl2 g( ) →← CO g( ) + Cl2 g( ) Keq = 2.2 × 10−10
II 2NO g( ) →← N2 g( ) + O2 g( ) Keq = 2.4 × 103
III 2SO3 g( ) →← 2SO2 g( ) + O2 g( ) Keq = 4.1 × 10−3
Which of the following correctly lists the equilibria in order from most favouring
products to least favouring products? A. I, III, II B. II, I, III C. II, III, I D. III, II, I
Page 8 Chemistry 12 – 1001 Form A
13. Consider the equilibrium system:
N2 g( ) + 3Cl2 g( ) →← 2NCl3 g( ) ΔH = +460 kJ
Which of the following describes what happens when some NCl3 is added?
Equilibrium Shift Value of Keq
A. right remains constant
B. right increases
C. left remains constant
D. left decreases
14. Consider the following equilibrium:
2BN s( ) + 3Cl2 g( ) →← 2BCl3 g( ) + N2 g( ) Keq = 1.6 × 10−3
At equilibrium, there were 0.30 mol BN , 0.20 mol BCl3 and 0.10 mol N2 in a 2.0 L container.
How many moles of Cl2 were present? A. 0.31mol
B. 1.4 mol
C. 2.7mol
D. 4.8mol
15. Which solute will result in a molecular solution? A. HCN B. Ba OH( )2
C. CH 3COOH
D. CH 3CH2OH
Chemistry 12 – 1001 Form A Page 9
16. Which best describes the equilibrium in a saturated solution? A. The rate of crystallization determines the solubility. B. The rate of crystallization equals the rate of dissolving. C. There is no solid solute on the bottom of the container. D. The solute is completely dissolved and the equilibrium favours the products. 17. Which compound will have a solubility greater than 0.1M at 25°C ? A. SrS
B. CoS
C. BaSO4
D. Ag2SO4 18. What is the net ionic equation for the reaction between 0.10 M Na2S and 0.10 M Zn NO3( )2 ? A. Zn2+ aq( ) + S2− aq( ) → ZnS s( )
B. Na+ aq( ) + NO3−
aq( ) → NaNO3 s( ) C. Na2S aq( ) + Zn NO3( )2 aq( ) → ZnS s( ) + 2NaNO3 aq( )
D. 2Na+ aq( ) + S2− aq( ) + Zn2+ aq( ) + 2NO3−
aq( ) → ZnS s( ) + 2Na+ aq( ) + 2NO3−
aq( ) 19. Which of the following correctly represents a K sp expression?
A. Ksp = Ag+⎡⎣ ⎤⎦2
S2−⎡⎣ ⎤⎦
B. Ksp =Ba2+⎡⎣ ⎤⎦ NO3
−⎡⎣ ⎤⎦2
Ba NO3( )2⎡⎣
⎤⎦
C. Ksp =CaCO3⎡⎣ ⎤⎦
CO2⎡⎣ ⎤⎦ CaO⎡⎣ ⎤⎦
D. Ksp = 1
Cu2+⎡⎣ ⎤⎦ Cl−⎡⎣ ⎤⎦2
Page 10 Chemistry 12 – 1001 Form A
20. What is the solubility of the salt PbSO4 ?
A. 3.2 ×10−16 M
B. 9.0 ×10−9 M
C. 1.8 ×10−8 M
D. 1.3 ×10− 4 M 21. What is the maximum I −[ ] that can exist in a solution with Pb2+[ ] = 8.5 × 10−3 M ? A. 2.0 × 10−6 M
B. 1.0 × 10−6 M
C. 5.0 × 10−4 M
D. 1.0 × 10−3 M
22. Which of the following occurs when a sample of 0.1M HNO3 is tested? A. phenolphthalein turns pink
B. bromthymol blue turns yellow
C. Ca s( ) reacts and produces CO2 g( ) D. Na s( ) reacts and produces NO2 g( ) 23. Given the equilibrium:
HCO3− + NH4
+ →← H2CO3 + NH3
Which species is the Brønsted-Lowry base for the forward reaction? A. NH3
B. NH4+
C. HCO3−
D. H2CO3
Chemistry 12 – 1001 Form A Page 11
24. What is the conjugate acid for NH2− in water?
A. H 3O+
B. NH4+
C. NH3
D. NH2− 25. What is a characteristic common to all strong acids? A. They ionize 100%. B. They are concentrated. C. They only react with strong bases. D. They have strong conjugate bases. 26. Which equation represents the behaviour of a strong Arrhenius base? A. CaO s( ) + H2O( ) → Ca OH( )2 s( )
B. RbOH aq( ) → Rb+ aq( ) + OH− aq( )
C. Co OH( )2
s( ) →← Co2+ aq( ) + 2OH − aq( ) D. Al H2O( )
6
3+aq( ) + H2O( ) →← Al H2O( )
5OH( )2+
aq( ) + H 3O+ aq( )
27. Which of the following equations represents the ionization of water?
A. H2O( ) →← H2 aq( ) + 1
2 O2 aq( )
B. H2O( ) →← H+ aq( ) + OH− aq( )
C. 2H2O( ) →← H3O
+ aq( ) + O2− aq( )
D. H2O( ) + H2O( ) →← H+ aq( ) + OH− aq( )
Page 12 Chemistry 12 – 1001 Form A
28. The ionization of water is endothermic. Which of the following is a reasonable value of Kw
if the temperature of water is greater than 25º C ? A. 1.2 × 10−15
B. 0.81 × 10−14
C. 1.0 × 10−14
D. 2.0 × 10−14
29. What is the pOH of 0.25M HNO3 ?
A. 4.0 × 10−14
B. − 0.60
C. 0.60
D. 13.40
30. What is the equilibrium constant expression for the predominant equilibrium in HPO42− aq( )?
A. H3O
+⎡⎣
⎤⎦ PO4
3−⎡⎣ ⎤⎦HPO4
2−⎡⎣ ⎤⎦
B. H2PO4
−⎡⎣ ⎤⎦ OH−⎡⎣ ⎤⎦HPO4
2−⎡⎣ ⎤⎦
C. HPO4
2− aq( ) + H2O( ) →← H2PO4− aq( ) + OH− aq( )
D. HPO4
2− aq( ) + H2O( ) →← H3O+ aq( ) + PO4
3− aq( )
Chemistry 12 – 1001 Form A Page 13
31. Which of the following 0.10 M solutions would have the highest pH? A. H2S
B. HIO3
C. HNO2
D. CH3COOH
32. Which of the following describes the predominant hydrolysis reaction that occurs in KHCO3 aq( ) ?
A. KHCO3 aq( ) →← K+ aq( ) + HCO3− aq( )
B. HCO3
− aq( ) + H2O ( ) →← H3O+ aq( ) + CO32− aq( )
C. CO3
2− aq( ) + H2O ( ) →← HCO3− aq( ) + OH− aq( )
D. HCO3
− aq( ) + H2O ( ) →← H2CO3 aq( ) + OH− aq( )
33. Which of the following represents an acidic salt solution? A. NH3 aq( )
B. NH4Cl aq( )
C. NaNO3 aq( )
D. K2CO3 aq( )
34. A chemical indicator changes colour at its A. titration point. B. transition point. C. equivalence point. D. stoichiometric point.
Page 14 Chemistry 12 – 1001 Form A
35. A solution was tested with two indicators and the following results were obtained.
Indicator Colour
chlorophenol red red
phenolphthalein pink
Which of the following could be the approximate pH of the solution? A. 6.0 B. 7.0 C. 9.2 D. 11.7 36. What is the complete ionic equation for the reaction of hydrochloric acid with NaOH aq( )?
A. H+ aq( ) + OH− aq( ) → H2O ( )
B. HCl aq( ) + NaOH aq( ) → NaCl aq( ) + H2O ( )
C. HCl aq( ) + NaOH aq( ) + H2O ( ) → NaCl aq( ) + H3O+ aq( ) + OH− aq( )
D. H+ aq( ) + Cl− aq( ) + Na+ aq( ) + OH− aq( ) → Na+ aq( ) + Cl− aq( ) + H2O ( )
37. Consider the following buffer equilibrium system:
HCN aq( ) + H2O ( ) →← H3O+ aq( ) + CN− aq( )
What is the net result of adding a small amount of HNO3 ? A. The pH increases slightly.
B. The pH decreases slightly.
C. The CN−⎡⎣ ⎤⎦ increases slightly.
D. The HCN⎡⎣ ⎤⎦ decreases slightly.
Chemistry 12 – 1001 Form A Page 15
38. An oxide of which of the following elements will form a solution that acts only as a base? A. P B. N C. Li D. Zn 39. The reduced substance in a chemical reaction can best be described as a substance that A. is the reducing agent and loses electrons. B. is the reducing agent and gains electrons. C. is the oxidizing agent and loses electrons. D. is the oxidizing agent and gains electrons. 40. Consider the following redox equation:
3C3H8O + K2Cr2O7 + 4H2SO4 → 3C3H6O + Cr2 SO4( )3 + K2SO4 + 7H2O
Which species is the oxidizing agent? A. C in C3H8O
B. H in C3H8O
C. O in C3H8O
D. Cr in K2Cr2O7
41. How does the oxidation number of arsenic As( ) change as As4 reacts to form H3AsO4 ? A. It decreases by 5.
B. It increases by 5 4 .
C. It increases by 5.
D. It increases by 20.
Page 16 Chemistry 12 – 1001 Form A
42. Tests between metals X, Y and Z and their ions produced the following results:
X + Y+ → no reaction
Y+ + Z → Y + Z+
Which of the following describes the relative strengths of the oxidizing agents? A. X > Y > Z
B. Z > Y > X
C. X+ > Y+ > Z+
D. Z+ > Y+ > X+ 43. The following skeletal equation can be balanced in acidic solution:
As2O3 → AsH3 Which of the following appear in the balanced equation?
Electrons Water
A. 3e− 32
H2O
B. 6e− 3H2O
C. 9e− 32
H2O
D. 12e− 3H2O
44. A solution of H2O2 is titrated with KMnO4 aq( ) according to the redox equation shown below:
5H2O2 + 2MnO4− + 6H+ → 5O2 + 2Mn2+ + 8H2O
A 10.00 mL sample of H2O2 is reacted with 13.5mL of 0.0241M KMnO4 .
What is the molarity of the H2O2 solution? A. 0.0130 M
B. 0.0325 M
C. 0.0346 M
D. 0.0813 M
Chemistry 12 – 1001 Form A Page 17
45. Consider the following diagram of a standard electrochemical cell:
1.
0 M KNO
3
Metal ZMetal X
1.0 M X(NO3)2 1.0 M Z(NO3)2
Voltse–e–
Which of the following is correct as the cell operates?
Metal Z Anion Migration
A. anode towards Metal X
B. anode towards Metal Z
C. cathode towards Metal X
D. cathode towards Metal Z
Page 18 Chemistry 12 – 1001 Form A
Use the following diagram to answer questions 46, 47 and 48.
1.0 M HCl 1.0 M AgNO3
Ag
H2(g)
Pt (inert)
Volts
PorousBarrier
46. What is the cathode half-cell reaction?
A. Ag → Ag+ + e−
B. Ag+ + e− → Ag
C. 2H+ + 2e− → H2
D. 2Cl− + 2e− → Cl2
47. Which of the following is correct as the cell operates?
Direction of Ag+ Migration
pH Near the Pt Electrode
A. towards Pt increases
B. towards Pt decreases
C. towards Ag increases
D. towards Ag decreases
Chemistry 12 – 1001 Form A Page 19
48. Which of the following is correct as the cell operates?
Direction of Electron Flow Mass of Pt Electrode
A. from Ag to Pt increases
B. from Ag to Pt decreases
C. from Pt to Ag decreases
D. from Pt to Ag does not change
49. An iron pipeline can be protected from rusting by connecting it to A. a zinc nitrate solution. B. a silver nitrate solution. C. the positive terminal of a direct current power supply. D. the negative terminal of a direct current power supply. 50. Which of the following is the anode half-cell reaction for molten KBr ?
A. K → K+ + e−
B. K+ + e− → K
C. 2Br− → Br2 + 2e−
D. H2O → 2e− + 2H+ + 12 O2
You have Examination Booklet Form A. In the box above #1 on your Answer Sheet,
ensure that you have filled in the bubble as follows.
FA B C D E HGExam Booklet Form/Cahier d’examen
This is the end of the multiple-choice section. Answer the remaining questions in the Response Booklet.
Chemistry 12 Data Page 1
Bas
ed o
n m
ass
of C
12 a
t 12.
00.
Valu
es in
par
enth
eses
ar
e th
e m
asse
s of
the
mos
t st
able
or
best
kno
wn
isot
opes
for
elem
ents
whi
ch d
o no
t occ
ur n
atur
ally
.
PER
IOD
IC T
AB
LE
OF
TH
E E
LE
ME
NT
S
12
34
56
78
910
1112
1314
1516
1718
4 Be
Bery
llium
9.0
11 Na
Sodi
um
23.0
12 Mg
Mag
nesi
um
24.3
19 KPo
tass
ium
39.1
20 Ca
Cal
cium
40.1
37 Rb
Rub
idiu
m
85.5
55 Cs
Ces
ium
132.
9
56 Ba
Bariu
m
137.
3
87 Fr
Fran
cium
(223
)
88 Ra
Rad
ium
(226
)
21 Sc
S can
dium
45.0
2 2 Ti
Tita
n ium
47.9
39 YYt
trium
88.9
40 Zr
Zirc
o niu
m
91.2
57 La
L ant
hanu
m
1 38.
9
7 2 Hf
Haf
n ium
178.
5
89 Ac
Actin
ium
(227
)
104
Rf
Rut
her fo
rdiu
m
(26 1
)
23 VVa
nadi
um
50.9
24 Cr
Chr
omiu
m
52.0
41 Nb
Nio
bium
92.9
42 Mo
Mol
ybde
num
95.9
73 TaTa
ntal
um
180.
9
74 WTu
ngst
en
183.
8
105
Db
Dub
nium
(262
)
106
Sg
Seab
orgi
um
(263
)
25 Mn
Man
gane
se
54.9
26 Fe
Iron
55.8
43 Tc
Tech
netiu
m
(98)
44 Ru
Rut
heni
um
101.
1
75 Re
Rhe
nium
186.
2
76 Os
Osm
ium
190.
2
107
Bh
Bohr
ium
(262
)
108
Hs
Has
sium
(265
)
27 Co
Cob
alt
5 8.9
45 Rh
Rh o
dium
1 02.
9
77 IrIr i
dium
1 92.
2
1 09
Mt
Me i
tner
ium
(266
)
28 Ni
Nick
e l
58. 7
78 Pt
Plat
inu m
195 .
1
29 Cu
Cop
per
63.5
47 Ag
Silve
r
107.
9
79 Au
Gol
d
197.
0
30 Zn
Zinc
65.4
48 Cd
Cad
miu
m
112.
4
80 Hg
Mer
cury
200.
6
5 B Boro
n
10.8
13 Al
Alum
inum
27.0
31 Ga
Gal
lium
69.7
49 In Indi
um
114.
8
81 Tl
Thal
lium
204.
4
6 CC
arbo
n
12.0
14 Si
Silic
on
28.1
32 Ge
Ger
man
ium
72.6
50 Sn
Tin
118.
7
82 Pb
Lead
207.
2
7 NN
itrog
en
14. 0
1 5 PPh
osp h
orus
31.0
3 3 As
Ars e
nic
74.9
5 1 Sb
Antim
ony
121.
8
8 3 Bi
Bism
uth
209.
0
8 OO
xyge
n
16.0
16 SSu
lphu
r
32.1
34 Se
Sele
nium
79.0
52 TeTe
lluri u
m
127.
6
84 Po
Polo
nium
(209
)
9 FFl
uorin
e
19.0
17 Cl
Chl
orin
e
35.5
35 Br
Brom
ine
79.9
53 IIo
dine
126.
9
85 At
Asta
tine
(210
)
10 Ne
Neo
n
20.2
18 Ar
Argo
n
39.9
36 Kr
Kryp
ton
83.8
54 Xe
Xeno
n
131.
3
86 Rn
Rad
on
(222
)
2 He
Hel
ium
4.0
58 Ce
Cer
i um
140.
1
90 Th
Thor
ium
232.
0
59 Pr
Pras
eody
miu
m
140.
9
91 Pa
Prot
actin
ium
231.
0
60 Nd
Neo
dym
ium
144.
2
92 UU
rani
um
238.
0
61 Pm
Prom
ethi
um
(145
)
93 Np
Nep
tuni
um
(237
)
62 Sm
Sam
ariu
m
1 50.
4
94 Pu
Plu t
oniu
m
(244
)
63 Eu
Euro
pium
152.
0
95 Am
Amer
iciu
m
(243
)
64 Gd
Gad
olin
ium
157.
3
96 Cm
Cur
ium
(247
)
65 Tb
Terb
ium
158.
9
97 Bk
Berk
eliu
m
(247
)
66 Dy
Dys
pros
ium
162.
5
98 Cf
Cal
iforn
ium
(251
)
67 Ho
Hol
miu
m
164.
9
99 Es
E ins
tein
ium
(252
)
6 8 Er
Erb i
u m
167.
3
100
Fm
Ferm
ium
(25 7
)
69 Tm
Thul
ium
168.
9
101
Md
Men
dele
vium
(258
)
70 Yb
Ytte
rbiu
m
173.
0
102
No
Nob
eliu
m
(259
)
71 Lu
Lute
tium
175.
0
103
Lr
Law
renc
ium
(262
)
1 HH
ydro
gen
1.0
46 Pd
Palla
dium
106 .
4
38 Sr
Stro
ntiu
m
87.6
3 Li
Lith
ium
6.9
14
Si
Si
li
co
n
28.1
Ato
mic
Num
ber
Sym
bol
Nam
eA
tom
ic M
ass
14 Si
Silic
on
28.1
Data Page 2 Chemistry 12
ATOMIC MASSES OF THE ELEMENTSBased on mass of C12 at 12.00.
Values in parentheses are the mass number of the most stable or bestknown isotopes for elements that do not occur naturally.
ActiniumAluminumAmericiumAntimonyArgonArsenicAstatineBariumBerkeliumBerylliumBismuthBoronBromineCadmiumCalciumCaliforniumCarbonCeriumCesiumChlorineChromiumCobaltCopperCuriumDubniumDysprosiumEinsteiniumErbiumEuropiumFermiumFluorineFranciumGadoliniumGalliumGermaniumGoldHafniumHeliumHolmiumHydrogenIndiumIodineIridiumIronKryptonLanthanumLawrenciumLeadLithiumLutetiumMagnesiumManganeseMendelevium
AcAlAmSbArAsAtBaBkBeBiBBrCdCaCfCCeCsClCrCoCuCmDbDyEsErEuFmFFrGdGaGeAuHfHeHoHInIIrFeKrLaLrPbLiLuMgMnMd
89 13 95 51 18 33 85 56 97 4 83 5 35 48 20 98 6 58 55 17 24 27 29 96 105 66 99 68 63 100 9 87 64 31 32 79 72 2 67 1 49 53 77 26 36 57 103 82 3 71 12 25 101
(227) 27.0 (243) 121.8 39.9 74.9 (210) 137.3 (247) 9.0 209.0 10.8 79.9 112.4 40.1 (251) 12.0 140.1 132.9 35.5 52.0 58.9 63.5 (247) (262) 162.5 (252) 167.3 152.0 (257) 19.0 (223) 157.3 69.7 72.6 197.0 178.5 4.0 164.9 1.0 114.8 126.9 192.2 55.8 83.8 138.9 (262) 207.2 6.9 175.0 24.3 54.9 (258)
MercuryMolybdenumNeodymiumNeonNeptuniumNickelNiobiumNitrogenNobeliumOsmiumOxygenPalladiumPhosphorusPlatinumPlutoniumPoloniumPotassiumPraseodymiumPromethiumProtactiniumRadiumRadonRheniumRhodiumRubidiumRutheniumRutherfordiumSamariumScandiumSeleniumSiliconSilverSodiumStrontiumSulphurTantalumTechnetiumTelluriumTerbiumThalliumThoriumThuliumTinTitaniumTungstenUraniumVanadiumXenonYtterbiumYttriumZincZirconium
HgMoNdNeNpNiNbNNoOsOPdPPtPuPoKPrPmPaRaRnReRhRbRuRfSmScSeSiAgNaSrSTaTcTeTbTlThTmSnTiWUVXeYbYZnZr
804260109328417
102768
461578948419596191888675453744
10462213414471138167343526581906950227492235470393040
200.6 95.9 144.2 20.2 (237) 58.7 92.9 14.0 (259) 190.2 16.0 106.4 31.0 195.1 (244) (209) 39.1 140.9 (145) 231.0 (226) (222) 186.2 102.9 85.5 101.1 (261) 150.4 45.0 79.0 28.1 107.9 23.0 87.6 32.1 180.9 (98) 127.6 158.9 204.4 232.0 168.9 118.7 47.9 183.8 238.0 50.9 131.3 173.0 88.9 65.4 91.2
Element Symbol Atomic Number
AtomicMass Element Symbol Atomic
NumberAtomicMass
Chemistry 12 Data Page �
NAMES, FORMULAE, AND CHARGES OF SOME COMMON IONS * Aqueous solutions are readily oxidized by air.** Not stable in aqueous solutions.
Negative Ions(Anions)
Po s i t i v e I o n s( C a t i o n s )
Aluminum
Ammonium
Barium
Calcium
Chromium(II), chromous
Chromium(III), chromic
Copper(I)*, cuprous
Copper(II), cupric
Hydrogen
Hydronium
Iron(II)*, ferrous
Iron(III), ferric
Lead(II), plumbous
Al3+
NH4+
Ba2+
Ca2+
Cr2+
Cr3+
Cu+
Cu2+
H+
H3O+
Fe2+
Fe3+
Pb2+
Hydroxide
Hypochlorite
Iodide
Monohydrogen phosphate
Nitrate
Nitrite
Oxalate
Oxide**
Perchlorate
Permanganate
Phosphate
Sulphate
Sulphide
Sulphite
Thiocyanate
OH–
ClO–
I–
HPO42–
NO3–
NO2–
C2O42–
O2–
ClO4–
MnO4–
PO4?–
SO42–
S2–
SO32–
SCN–
Bromide
Carbonate
Chlorate
Chloride
Chlorite
Chromate
Cyanide
Dichromate
Dihydrogen phosphate
Ethanoate, acetate
Fluoride
Hydrogen carbonate, bicarbonate
Hydrogen oxalate, binoxalate
Hydrogen sulphate, bisulphate
Hydrogen sulphide, bisulphide
Hydrogen sulphite, bisulphite
Br–
CO32–
ClO3–
Cl–
ClO2–
CrO42–
CN–
Cr2O72–
H2PO4–
CH3COO–
F–
HCO3–
HC2O4–
HSO4–
HS–
HSO3–
Lead(IV), plumbic
Lithium
Magnesium
Manganese(II), manganous
Manganese(IV)
Mercury(I)*, mercurous
Mercury(II), mercuric
Potassium
Silver
Sodium
Tin(II)*, stannous
Tin(IV), stannic
Zinc
Pb4+
Li+
Mg2+
Mn2+
Mn4+
Hg22+
Hg2+
K+
Ag+
Na+
Sn2+
Sn4+
Zn2+
Data Page � Chemistry 12
SOLUBILITY OF COMMON COMPOUNDS IN WATER
The term soluble here means > 0.1 mol/L at 25°C.
Negative Ions(Anions)
Positive Ions(Cations)
Solubility ofCompounds
All
All
All
Soluble
Soluble
Soluble
All Soluble
Soluble
Low Solubility
All others
Soluble
Low Solubility
Soluble
Low Solubility
Soluble
Low Solubility
Soluble
Low Solubility
All others
All others
All others
All others
or
or
or
or
14243
14253
123
123
123
Alkali ions: Li+, Na+, K+, Rb+, Cs+, Fr+
Ammonium ion: NH4+
Chloride, Cl–
Bromide, Br–
Iodide, I–
Nitrate, NO3–
Hydrogen ion: H+
Ag+, Pb2+, Cu+
Sulphide, S2–Alkali ions, H+, NH4
+, Be2+, Mg2+, Ca2+, Sr2+, Ba2+
Sulphate, SO42–
Hydroxide, OH–Alkali ions, H+, NH4
+, Sr2+ ?
Sulphite, SO32–
Phosphate, PO43–
Carbonate, CO32–
Alkali ions, H+, NH4+
Ag+, Ca2+, Sr2+, Ba2+, Pb2+
Chemistry 12 Data Page �
SOLUBILITY PRODUCT CONSTANTS AT 25°C
Name Formula
Barium carbonate
Barium chromate
Barium sulphate
Calcium carbonate
Calcium oxalate
Calcium sulphate
Copper(I) iodide
Copper(II) iodate
Copper(II) sulphide
Iron(II) hydroxide
Iron(II) sulphide
Iron(III) hydroxide
Lead(II) bromide
Lead(II) chloride
Lead(II) iodate
Lead(II) iodide
Lead(II) sulphate
Magnesium carbonate
Magnesium hydroxide
Silver bromate
Silver bromide
Silver carbonate
Silver chloride
Silver chromate
Silver iodate
Silver iodide
Strontium carbonate
Strontium fluoride
Strontium sulphate
Zinc sulphide
BaCO3
BaCrO4
BaSO4
CaCO3
CaC2O4
CaSO4
CuI
Cu(IO3)2
CuS
Fe(OH)2
FeS
Fe(OH)3
PbBr2
PbCl2
Pb(IO3)2
PbI2
PbSO4
MgCO3
Mg(OH)2
AgBrO3
AgBr
Ag2CO3
AgCl
Ag2CrO4
AgIO3
AgI
SrCO3
SrF2
SrSO4
ZnS
2.6 10–9
1.2 10–10
1.1 10–10
5.0 10–9
2.3 10–9
7.1 10–5
1.3 10–12
6.9 10–8
6.0 10–37
4.9 10–17
6.0 10–19
2.6 10–39
6.6 10–6
1.2 10–5
3.7 10–13
8.5 10–9
1.8 10–8
6.8 10–6
5.6 10–12
5.3 10–5
5.4 10–13
8.5 10–12
1.8 10–10
1.1 10–12
3.2 10–8
8.5 10–17
5.6 10–10
4.3 10–9
3.4 10–7
2.0 10–25
K sp
Data Page � Chemistry 12
Perchloric HClO H ClO
Hydriodic HI H I
Hydrobromic HBr H Br
Hydrochloric HCl H Cl
Nitric HNO H NO
Sulphuric H SO H HSO
4 4
3 3
2 4 4
→ +
→ +
→ +
→ +
→ +
→ +
+ −
+ −
+ −
+ −
+ −
+ −
very large
very large
very large
very large
very large
very large
Hydronium Ion H O H H O
Iodic HIO H IO
Oxalic H C O H HC O
Sulphurous SO H O H SO H HSO
Hydrogen sulphate ion HSO H SO
3 2
3 31
2 2 4 2 42
2 2 2 3 32
4 42 2
1 0
1 7 10
5 9 10
1 5 10
1 2 10
+ +
+ − −
+ − −
+ − −
− + − −
→← +→← + ×→← + ×
+( ) →← + ×→← + ×
.
.
.
.
.
Phosphoric H PO H H PO
Hexaaquoiron ion iron ion Fe H O H Fe H O OH
Citric H C H O H H C H O
Nitrous HNO H NO
Hydrofluoric HF
III
3 4 2 43
2 63
2 52 3
3 6 5 7 2 6 5 74
2 24
7 5 10
6 0 10
7 1 10
4 6 10
→← + ×
( ) →← + ( ) ( ) ×→← + ×→← + ×
+ − −
+ + + −
+ − −
+ − −
.
, .
.
.
( )
→→← + ×+ − −H F 3 5 10 4.
Methanoic formic HCOOH H HCOO
Hexaaquochromium ion chromium ion Cr H O H Cr H O OH
Benzoic C H COOH H C H COO
Hydrogen oxalate ion HC O H C O
Ethanoic acetic
III
, .
, .
.
.
,
( )
→← + ×
( ) →← + ( ) ( ) ×→← + ×→← + ×
+ − −
+ + + −
+ − −
− + − −
1 8 10
1 5 10
6 5 10
6 4 10
4
2 63
2 52 4
6 5 6 55
2 4 2 42 5
CHCH COOH H CH COO3 351 8 10→← + ×+ − −.
Dihydrogen citrate ion H C H O H HC H O
Al H O H Al H O OH
Carbonic CO H O H CO H HCO
Monohydrogen citrate ion HC H O H
2 6 5 7 6 5 72 5
2 63
2 52 5
2 2 2 3 37
6 5 72
1 7 10
1 4 10
4 3 10
− + − −
+ + + −
+ − −
− +
→← + ×
( ) →← + ( ) ( ) ×
+( ) →← + ×→←
.
.
.
Hexaaquoaluminum ion, aluminum ion
++ ×→← + ×
− −
− + − −
C H O
Hydrogen sulphite ion HSO H SO
6 5 73 7
3 32 7
4 1 10
1 0 10
.
.
Hydrogen sulphide H S H HS
Dihydrogen phosphate ion H PO H HPO
Boric H BO H H BO
Ammonium ion NH H NH
Hydrocyanic HCN H CN
28
2 4 42 8
3 3 2 310
4 310
10
9 1 10
6 2 10
7 3 10
5 6 10
4 9 10
→← + ×→← + ×→← + ×→← + ×→← + ×
+ − −
− + − −
+ − −
+ + −
+ − −
.
.
.
.
.
Phenol C H OH H C H O
Hydrogen carbonate ion HCO H CO
Hydrogen peroxide H O H HO
Monohydrogen phosphate ion HPO H PO
Water H O H OH
Hydroxide ion OH
6 5 6 510
3 32 11
2 2 212
42
43 13
214
1 3 10
5 6 10
2 4 10
2 2 10
1 0 10
→← + ×→← + ×→← + ×→← + ×→← + ×
+ − −
− + − −
+ − −
− + − −
+ − −
−
.
.
.
.
.
←← +
← +
+ −
+ −
H O very small
Ammonia NH H NH very small
2
3 2
RELATIVE STRENGTHS OF BRØNSTED-LOWRY ACIDS AND BASESin aqueous solution at room temperature.
Name of Acid Base Acid Ka
ST
RO
NG
WE
AK
ST
RO
NG
WE
AK
ST
RE
NG
TH
OF
AC
IDS
TR
EN
GT
H O
F B
AS
E
Chemistry 12 Data Page �
ACID-BASE INDICATORS
Indicator
yellow to blue
red to yellow
red to yellow
red to yellow
yellow to blue
red to yellow
yellow to red
yellow to blue
yellow to red
red to amber
yellow to blue
colourless to pink
colourless to blue
yellow to red
blue to yellow
Methyl violet
Thymol blue
Orange IV
Methyl orange
Bromcresol green
Methyl red
Chlorophenol red
Bromthymol blue
Phenol red
Neutral red
Thymol blue
Phenolphthalein
Thymolphthalein
Alizarin yellow
Indigo carmine
pH Range in WhichColour Change Occurs
Colour Changeas pH Increases
0.0 – 1.6
1.2 – 2.8
1.4 – 2.8
3.2 – 4.4
3.8 – 5.4
4.8 – 6.0
5.2 – 6.8
6.0 – 7.6
6.6 – 8.0
6.8 – 8.0
8.0 – 9.6
8.2 – 10.0
9.4 – 10.6
10.1 – 12.0
11.4 – 13.0
Data Page � Chemistry 12
F g e F
S O e SO
H O H e H O
MnO H e Mn H O
Au e Au s
2
2 82
42
2 2 2
42
23
2 2 2 87
2 2 2 01
2 2 2 1 78
8 5 4 1 51
3 1 50
( ) + →← +
+ →← +
+ + →← +
+ + →← + +
+ →← ( ) +
− −
− − −
+ −
− + − +
+ −
.
.
.
.
.
BrO H e Br H O
ClO H e Cl H O
Cl g e Cl
Cr O H e Cr H O
O g H e
312 2 2
4 2
2
2 72 3
2
12 2
6 5 3 1 48
8 8 4 1 39
2 2 1 36
14 6 2 7 1 23
2 2
− + −
− + − −
− −
− + − +
+ −
+ + →← ( ) + +
+ + →← + +
( ) + →← +
+ + →← + +
( ) + + →
l .
.
.
.
←← +H O2 1 23.
MnO s H e Mn H O
IO H e I s H O
Br e Br
AuCl e Au s Cl
NO H e NO g H
22
2
312 2 2
2
4
3 2
4 2 2 1 22
6 5 3 1 20
2 2 1 09
3 4 1 00
4 3 2
( ) + + →← + +
+ + →← ( ) + +
( ) + →← +
+ →← ( ) + +
+ + →← ( ) +
+ − +
− + −
− −
− − −
− + −
.
.
.
.
l
OO +0 96.
Fe e Fe
O g H e H O
MnO H O e MnO s OH
I s e I
Cu e Cu s
3 2
2 2 2
4 2 2
2
0 77
2 2 0 70
2 3 4 0 60
2 2 0 54
0 52
+ − +
+ −
− − −
− −
+ −
+ →← +
( ) + + →← +
+ + →← ( ) + +
( ) + →← +
+ →← ( ) +
.
.
.
.
.
H SO H e S s H O
Cu e Cu s
SO H e H SO H O
Cu e Cu
Sn e Sn
2 3 22
42
2 3 22
4 2
4 4 3 0 45
2 0 34
4 2 0 17
0 15
2 0 15
+ + →← ( ) + +
+ →← ( ) +
+ + →← + +
+ →← +
+ →← +
+ −
+ −
− + −
+ − +
+ − +
.
.
.
.
.
S s H e H S g
H e H g
Pb e Pb s
Sn e Sn s
Ni e Ni s
( ) + + →← ( ) +
+ →← ( ) +
+ →← ( ) −
+ →← ( ) −
+ →← ( ) −
+ −
+ −
+ −
+ −
+ −
2 2 0 14
2 2 0 00
2 0 13
2 0 14
2 0 26
2
22
2
2
.
.
.
.
.
H PO H e H PO H O
Co e Co s
Se s H e H Se
Cr e Cr
H O e H OH M
3 4 3 3 22
23 2
2 27
2 2 0 28
2 0 28
2 2 0 40
0 41
2 2 2 10 0 41
+ + →← + −
+ →← ( ) −
( ) + + →← −
+ →← −
+ →← + ( ) −
+ −
+ −
+ −
+ − +
− − −
.
.
.
.
.
Fe e Fe s
Ag S s e Ag s S
Cr e Cr s
Zn e Zn s
Te s H e H Te
2
22
3
2
2
2 0 45
2 2 0 69
3 0 74
2 0 76
2 2 0 79
+ −
− −
+ −
+ −
+ −
+ →← ( ) −
( ) + →← ( ) + −
+ →← ( ) −
+ →← ( ) −
( ) + + →← −
.
.
.
.
.
2 2 2 0 83
2 1 19
3 1 66
2 2 37
2 71
2 22
3
2
H O e H g OH
Mn e Mn s
Al e Al s
Mg e Mg s
Na e Na s
+ →← ( ) + −
+ →← ( ) −
+ →← ( ) −
+ →← ( ) −
+ →← ( ) −
− −
+ −
+ −
+ −
+ −
.
.
.
.
.
Ca e Ca s
Sr e Sr s
Ba e Ba s
K e K s
Rb e Rb s
2
2
2
2 2 87
2 2 89
2 2 91
2 93
2 98
+ −
+ −
+ −
+ −
+ −
+ →← ( ) −
+ →← ( ) −
+ →← ( ) −
+ →← ( ) −
+ →← ( ) −
.
.
.
.
.
Cs e Cs s
Li e Li s
+ −
+ −
+ →← ( ) −
+ →← ( ) −
3 03
3 04
.
.
Hg e Hg
O g H M e H O
NO H e N O H O
Ag e Ag s
Hg e Hg
2
12 2
72
3 2 4 2
12 2
2
2 0 85
2 10 2 0 82
2 4 2 2 0 80
0 80
0 80
+ −
+ − −
− + −
+ −
+ −
+ →← ( ) +
( ) + ( ) + →← +
+ + →← + +
+ →← ( ) +
+ →← ( ) +
l
l
.
.
.
.
.
STANDARD REDUCTION POTENTIALS OF HALF-CELLSIonic concentrations are at 1M in water at 25°C.
Reducing AgentsOxidizing AgentsS
TR
ON
GW
EA
KS
TR
ON
GW
EA
K
Overpotential Effect
Overpotential Effect
ST
RE
NG
TH
OF
OX
IDIZ
ING
AG
EN
TS
TR
EN
GT
H O
F R
ED
UC
ING
AG
EN
TE° Volts( )
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AnswerthefollowingquestionsinthespaceprovidedinthisResponse Booklet.Youareexpectedtocommunicateyourknowledgeandunderstandingofchemicalprinciplesinaclearandlogicalmanner.YourstepsandassumptionsleadingtoasolutionmustbewritteninthisResponse Booklet.Answersmustincludeunitswhereappropriateandbegiventothecorrectnumberofsignificantfigures.For questions involving calculations, full marks will NOT be given for providing only an answer.
Chemistry 12 – 1001 Response Booklet Page 1
PART B: WRITTEN RESPONSE Value: 37.5% of the examination
Suggested Time: 40 minutes
1. (4 marks)
Consider the following reaction mechanism:
Step 1 HBr + O2 → HOOBr slow
Step 2 HOOBr + HBr → 2HOBr fast
Step 3 2 HOBr + HBr → H2O + Br2( ) fast
Overall Reaction
Write the equation for the overall reaction. Given that the overall reaction is exothermic,
sketch a PE diagram for the mechanism on the axis provided.
Reaction time
PE(kJ)
Page 2 Chemistry 12 – 1001 Response Booklet
2. (4 marks)
Consider the following equilibrium:
2H2 g( ) + S2 g( ) →← 2H2S g( )
Initially, 9.0 × 10−4 mol S2 and 1.1 × 10−2mol H2S are placed in a 1.0 L container.
At equilibrium, there is 8.6 × 10−3mol H2S present. Calculate Keq .
Chemistry 12 – 1001 Response Booklet Page 3
3. (4 marks)
Will a precipitate form when 10.0 mL of 1.0 M Pb NO3( )2 is mixed with 40.0 mL of
2.0 × 10−2M NaCl ? Justify your answer.
Page 4 Chemistry 12 – 1001 Response Booklet
4. (3 marks)
For the reactant pair KHC 2O4 and Na2HPO4 , write the net ionic equation for the predominant
equilibrium that will be established. Predict whether the equilibrium will favour reactants or
products and explain why.
Chemistry 12 – 1001 Response Booklet Page 5
5. (5 marks)
Calculate the initial concentration of an NH4NO3 salt solution that has a pH = 4.70 .
Begin by writing the equation for the predominant equilibrium reaction.
Page 6 Chemistry 12 – 1001 Response Booklet
6. (3 marks)
A 10.00 mL sample of H 2SO4 is titrated with 0.50 M KOH in three separate trials
and the results are tabulated below.
Trial Volume of 0.50 M KOH
1 20.30 mL
2 19.10 mL
3 18.90 mL
Calculate the concentration of the H 2SO4 .
Chemistry 12 – 1001 Response Booklet Page 7
7. (4 marks)
Balance the following redox equation in acidic solution:
ClO4− + I2 + H2PO4
− → Cl2 + IPO4 (acidic)
Page 8 Chemistry 12 – 1001 Response Booklet
8. (3 marks)
Consider the electrolysis of an ionic solution as shown in the diagram.
Pt(inert)
Ionic Solution
DC Power Source
Cu
e–e–
Bubbles appear around the inert electrode and a shiny metal coating appears on the copper electrode. Give an example of one of the possible ionic solutions that could be used. Provide a set of corresponding half reactions which would explain these results.
Ionic Solution: Half-reaction at the Pt electrode: Half-reaction at the Cu electrode:
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Question 1
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Course Code = CH 12
Chemistry 122009/10 Released Exam
JANUARY 2010
Response Booklet
Course Code = CH 2009/10 Released ExamJanuary 2010
MINISTRY USE ONLYMINISTRY USE ONLY
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PlacePersonalEducationNumber(PEN)here. PlacePersonalEducationNumber(PEN)here.
Instructions:
AnswerthefollowingquestionsinthespaceprovidedinthisResponse Booklet.Youareexpectedtocommunicateyourknowledgeandunderstandingofchemicalprinciplesinaclearandlogicalmanner.YourstepsandassumptionsleadingtoasolutionmustbewritteninthisResponse Booklet.Answersmustincludeunitswhereappropriateandbegiventothecorrectnumberofsignificantfigures.For questions involving calculations, full marks will NOT be given for providing only an answer.