CHEM 13 NEWS EXAM 2014
UNIVERSITY OF WATERLOO
DEPARTMENT OF CHEMISTRY
8 MAY 2014
TIME: 75 MINUTES
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Ontario, now studying Grade 12 Chemistry
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5. Carefully detach the last page. It is the datasheet.
6. Now answer the exam questions. Questions are not in
order of difficulty. Indicate your choice on the
STUDENT RESPONSE sheet by marking one letter
beside the question number.
• Mark only one answer for each question.
• Questions are all of the same value.
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answer, but no penalty if you do not answer.
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sheet white again.
Code 11 High school student outside Canada
Code 12 Teacher
Carefully detach the last page.
It is the Data Sheet.
1
Select the correct ending to make the following a true
o
statement. Compared to one litre of water at 25 C, two
o
litres of water at 25 C …
4
−6
is twice as dense
B
−2
B
is half as dense
C
0
C
has twice the heat capacity
D
+2
D
has half the heat capacity
E
+6
E
has a vapour pressure that is two times greater
For which of the following is the number of neutrons
equal to the number of electrons?
A
17
O
−
17
C
18
O
D
18
O
O
E
18
O
Which of the following processes consumes the
greatest quantity of energy per mole of sodium?
A
Na(g) → Na(s)
B
Na(l) → Na(s)
C
Na(g) → Na (g) + e
D
Na (g) → Na (g) + e
E
Na(g) + e → Na (g)
+
B
−
6
3
A
A
5
2
What is the oxidation state of Cr in K2CrO4?
+
Which statement is not correct for the reaction below?
2 NO(g)  N2(g) + O2(g)
−
+
+
−
2+
−
−
Which of the following statements about H2SO3, a
diprotic acid, is true?
A
There is just one lone pair on the sulfur atom.
B
It is a strong acid.
C
The hydrogen atoms are bonded directly to
the sulfur atom.
A
At equilibrium, the forward and reverse
reactions occur at equal rates.
D
The OSO bond angles are all approximately
120 degrees.
B
Reaction to the left or to the right occurs
spontaneously until the equilibrium state
is reached.
E
The oxidation state of sulfur is +6.
C
Reducing the volume of the system has no effect
on the equilibrium amounts of NO, N2 and O2.
D
The equilibrium amounts of NO, N2 and O2
depend on the initial amounts.
E
The equilibrium value of [N2 ] [O2 ] / [NO] is the
same at all temperatures.
7
2
2 /CHEM 13 NEWS EXAM © 2014 UNIVERSITY OF WATERLOO
What is the shape of the XeF4 molecule?
A
tetrahedral
B
trigonal pyramidal
C
square planar
D
see-saw
E
zig-zag
8
9
o
The density of an ideal gas at 90 C and 94.0 kPa is
2.80 g/L. What is the molar mass of the gas?
A
23 g/mol
B
45 g/mol
C
90 g/mol
D
180 g/mol
E
270 g/mol
Which of the following is an ionic compound?
A
HOCN
B
NH4NO2
C
D
E
12 Which of the following is a network covalent solid (an
extended network of atoms bonded to each other by
covalent bonds)?
A
I2(s)
B
H2O(s)
C
SiC(s)
D
C10H8(s)
E
CO2(s)
13 Which of the following Bronsted-Lowry acid-base
pairs is incorrect?
Base
Acid
−
H3O
A
OH
B
NH2
NH3
C
NH3
NH4
D
CO3
E
HSO3
CH3NH2
−
SiO2
+
PH3
o
o
+
2−
−
−
HCO3
H2SO3
10 What is the pH of pure water at 37 C? At 37 C,
−14
Kw = 2.4×10 .
A
6.90
B
7.10
C
14 What is the maximum mass of KBr that can be
obtained from a mixture containing 13.2 grams of
potassium (K) and 22.2 grams of bromine (Br2)?
A
13.2 g
B
22.2 g
C
33.1 g
D
35.4 g
E
40.2 g
7.19
D
7.00
E
6.81
11 What is the percentage by mass of Cr in Cr2O3?
o
A
34.2%
B
68.4%
C
76.5%
D
86.7%
E
93.2%
15 Diethyl ether, CH3CH2OCH2CH3, is a liquid at 25 C
and 101 kPa. Which of the following contribute to the
attraction amongst molecules in CH3CH2OCH2CH3(l)?
A
dipole-dipole forces only
B
London dispersion forces only
C
hydrogen bonding forces only
D
dipole-dipole and London dispersion forces
E
hydrogen bonding and London dispersion forces
© 2014 UNIVERSITY OF WATERLOO CHEM 13 NEWS EXAM / 3
16 According to the reaction profile below, what is the
activation energy for the reverse reaction P → R?
19 Which of the following illustrates how the potential
energy (PE) of a proton and an electron depends on
the distance, r, between them?
PE
Potential energy
20 kJ/mol
A
r
30 kJ/mol
25 kJ/mol
P
10 kJ/mol
R
Reaction progress
A
35 kJ/mol
B
45 kJ/mol
C
50 kJ/mol
D
−10 kJ/mol
E
B
PE
r
C
−45 kJ/mol
PE
r
17 What is the ground electronic state of Mn
2
2
6
2
6
5
2
2
2
6
2
6
3
2
2
2
6
2
6
5
2
2
6
2
6
2
A
1s 2s 2p 3s 3p 3d 4s
B
1s 2s 2p 3s 3p 3d 4s
C
1s 2s 2p 3s 3p 3d
D
1s 2s 2p 3s 3p 4s 4p
E
1s 2s 2p 3s 3p 4s 4d
2+
?
D
2
2
6
2
6
2
PE
3
r
3
−1
18 A solution of 0.060 mol L pyridine (a weak base) has
−
−6
−1
[OH ] = 9.1×10 mol L . What is Kb for pyridine?
A
1.5×10
−4
−4
B
3.0×10
C
8.3×10
D
9.1×10
E
1.4×10
−11
−6
−9
4 /CHEM 13 NEWS EXAM © 2014 UNIVERSITY OF WATERLOO
E
PE
r
20 The equilibrium constants for the following reactions
are denoted by K1, K2, and K3, respectively.
HNO2(aq) + H2O(l)  NO2−(aq) + H3O (aq)
K1
2 H2O(l)  H3O (aq) + OH−(aq)
K2
+
+
NH3(aq) + H2O(I)  NH4 (aq) + OH (aq)
+
−
K3
What is the equilibrium constant for the reaction below?
HNO2(aq) + NH3(aq)  NO2−(aq) + NH4 (aq)
+
23 A current of 4.27 amperes passes through an
electrolysis cell containing CuSO4 for exactly two
hours. How many grams of copper are deposited?
Assume the cell operates with 95.1% efficiency.
(Note: 1 ampere = 1 coulomb per second)
A
4.82 g
B
9.63 g
C
10.1 g
D
10.6 g
E
19.2 g
A
K1 – K2 + K3
B
K1 K3
C
K1 K3 / K2
D
K1 K2 K3
A
0.0946 mol
E
K2 / (K1 K3)
B
0.106 mol
C
0.0113 mol
D
0.112 mol
E
1.15 mol
24 A mixture of N2(g) and Ne(g) has a mass of 2.88 g and
occupies a volume of 2.50 L at 298 K and 105 kPa.
How many moles of N2 are there in this mixture?
21 Which of these molecules contains at least one
triple bond?
A
oxalic acid, H2C2O4 (HOOCCOOH)
B
cyanogen, C2N2 (NCCN)
C
allene, C3H4 (H2CCCH2)
D
ethanal, C2H4O (CH3CHO)
A
−35 kJ
E
diazene, N2H2 (HNNH)
B
+35 kJ
C
−50 kJ
D
+50 kJ
E
−529 kJ
25 What is ∆H for the reaction below?
CH4(g) + I2(g) → CH3I(g) + HI(g)
22 Select the correct ending to make the following a
true statement. A catalyst ...
A
always provides a surface on which
molecules react
Bond
energies
(in kJ/mol)
H−C, 413
C−I, 230
H−I, 299
I−I, 151
26 How many electrons are needed to fill the 4f subshell
of an atom?
B
lowers the energy of the products
C
induces an alternate reaction pathway
with a higher activation energy
D
increases the frequency of collisions
between molecules
E
is not consumed by the overall reaction although
it may be temporarily changed
A
two
B
six
C
ten
D
fourteen
E
eighteen
© 2014 UNIVERSITY OF WATERLOO CHEM 13 NEWS EXAM / 5
27 Which of the following bonds is the most polar?
A
H−O
B
C−N
C
H−C
D
E
31 Excess AgCl(s) is added to a dilute aqueous solution
of CaCl2(aq). Some but not all of the added AgCl
dissolves. Which of the following conditions must be
satisfied at equilibrium?
+
2+
+
2+
+
2+
1
3
−
A
[Ag ] = [Ca ] =
O−N
B
[Ag ] + [Ca ] = 3 [Cl ]
O−F
C
[Ag ] + [Ca ] = [Cl ]
D
[Ag ] + 2 [Ca ] = [Cl ]
E
[Ca ] =
28 Element 119 has yet to be discovered or synthesized.
However, because of its position in the periodic table,
only one of the following statements about this element
is likely to be incorrect. Which statement is incorrect?
+
−
−
−
2+
2+
1
2
[Cl ]
−
[Cl ]
32 The following standard reduction potentials are given.
A
The element would be a metal.
3+
B
The element (call it X) would combine with
fluorine to form a compound with formula XF2.
C
The element would be in the s block.
D
The element would react with water to form a
basic solution.
−
Fe + e  Fe
−
+
−
IO3 + 6 H + 5e
29 Which of the following have three unpaired electrons
in their ground electronic states?
the third period atoms (Na to Ar)
B
the group 3 atoms (B to Tl)
C
the group 15 atoms (N to Bi)
D
N
E
B
3−
3+
+
2+
IO3 + 6 H + 5 Fe
The element would combine with hydrogen to
form an ionic compound.
A
 ½ I2 + 3 H2O
E ° = 0.77 V
E ° = 1.19 V
What is E ° for the reaction below?
−
E
2+
A
+0.42 V
B
−0.53 V
C
−2.66 V
D
+5.04 V
E
+1.96 V
→ 5 Fe
3+
+ ½ I2 + 3 H2O
33 Propanoic acid, CH3CH2COOH, is a weak acid with
pKa = 4.87 at 298 K. What is the pH at the equivalence
−1
point in the titration of 30.0 mL of 0.200 mol L
−1
propanoic acid with 0.200 mol L NaOH(aq)?
(Note: pKa = −log10 Ka)
3−
and P
3+
and Al
30 Which of the following statements concerning the
−
nitrate ion, NO3 , is incorrect?
A
4.87
B
5.07
C
7.00
o
A
The ONO bond angles are all 120 .
D
8.94
B
One of the nitrogen-oxygen bonds is shorter than
the other two nitrogen-oxygen bonds.
E
9.13
C
The nitrogen atom has a formal charge of +1.
D
It is the conjugate base of a strong acid.
E
It is nonpolar.
6 /CHEM 13 NEWS EXAM © 2014 UNIVERSITY OF WATERLOO
38 Electronegativity is a measure of
34 Consider the reaction below.
2 NOCl(g)
 2 NO(g) + Cl2(g), ∆H > 0
Which of the following conditions maximize the
amount of Cl2(g) present at equilibrium?
A
low temperature, high pressure
B
high temperature, low pressure
C
low temperature, low pressure
D
high temperature, high pressure
E
high temperature, pressure has no effect
35 The solubility of MnS in water is 2.3×10
litre. What is Ksp for MnS?
A
B
−6
grams per
A
the magnitude of the charge of an electron
B
the energy released when an electron is
added to an atom
C
the energy required to remove an electron
from an atom
D
the ability of an atom to draw electron density
towards itself
E
the average repulsive force experienced by a
given electron
39 In which of the following solutions does the solute
have the highest degree of ionization? The Ka values
−5
−10
for CH3COOH and HCN are 1.8×10 and 4.8×10 ,
respectively.
−31
4.9×10
−1
0.10 mol L
B
0.010 mol L
C
0.10 mol L
D
0.010 mol L
E
0.0010 mol L
−23
2.8×10
−12
C
5.3×10
D
7.0×10
E
2.3×10
−16
−6
36 Which of the following is the weakest acid in water?
A
H2S
B
H2Se
C
H2Te
D
HBr
E
HI
HCN
A
−1
−1
HCN
CH3COOH
−1
CH3COOH
−1
CH3COOH
40 Which property is represented in the graph below?
37 What is the lightest element that has two 4s electrons
and eight 3d electrons in its lowest energy state?
A
Fe
B
Ar
C
Kr
D
Ni
E
Cu
A
atomic radius
B
electron affinity
C
density
D
first ionization energy
E
atomic volume
© 2014 UNIVERSITY OF WATERLOO CHEM 13 NEWS EXAM / 7
DATA SHEET
CHEM 13 NEWS EXAM
DETACH CAREFULLY
1
1A
1
H
1.008
3
Li
6.941
11
Na
22.99
19
K
39.10
37
Rb
85.47
55
Cs
132.9
87
Fr
(223)
2
2A
4
Be
9.012
12
Mg
24.31
20
Ca
40.08
38
Sr
87.62
56
Ba
137.3
88
Ra
226
3
4
3B
4B
21
22
Sc
Ti
44.96 47.88
39
40
Y
Zr
88.91 91.22
57-71
72
La-Lu
Hf
178.5
89-103 104
Ac-Lr
Rf
57
La
138.9
89
Ac
227.
58
Ce
140.1
90
Th
232.0
5
5B
23
V
50.94
41
Nb
92.91
73
Ta
180.9
105
Db
59
Pr
140.9
91
Pa
231.0
6
6B
24
Cr
52.00
42
Mo
95.94
74
W
183.9
106
Sg
60
Nd
144.2
92
U
238.0
7
7B
25
Mn
54.94
43
Tc
(98)
75
Re
186.2
107
Bh
61
Pm
(145)
93
Np
237.0
Constants:
NA =
R
6.022×10 mol−1
23
10
→
28
Ni
58.69
46
Pd
106.4
78
Pt
195.1
110
Ds
62
63
64
Sm
Eu
Gd
150.4 152.00 157.3
94
95
96
Pu
Am
Cm
(244) (243) (247)
11
1B
29
Cu
63.55
47
Ag
107.9
79
Au
197.0
111
Sg
65
Tb
158.9
97
Bk
(247)
12
2B
30
Zn
65.38
48
Cd
112.4
80
Hg
200.6
112
Cn
66
Dy
162.5
98
Cf
(251)
67
Ho
164.9
99
Es
(252)
68
Er
167.3
100
Fm
(257)
15
5A
7
N
14.01
15
P
30.97
33
As
74.92
51
Sb
121.8
83
Bi
209.0
69
Tm
168.9
101
Md
(258)
16
6A
8
O
16.00
16
S
32.07
34
Se
78.96
52
Te
127.6
84
Po
(209)
70
Yb
173.0
102
No
(259)
17
7A
9
F
19.00
17
Cl
35.45
35
Br
79.90
53
I
126.9
85
At
(210)
71
Lu
175.0
103
Lr
(260)
1 atm = 101.325 kPa = 760 torr = 760 mm Hg
−1
0.082058 atm L K
=
8.3145 kPa L K−1 mol−1
=
8.3145 J K−1 mol−1
−14
Kw =
1.0×10
F
96 485 C mol
Equations:
26
Fe
55.85
44
Ru
101.1
76
Os
190.2
108
Hs
9
8B
27
Co
58.93
45
Rh
102.9
77
Ir
192.2
109
Mt
14
4A
6
C
12.01
14
Si
28.09
32
Ge
72.59
50
Sn
118.7
82
Pb
207.2
Conversion factors:
=
=
8
←
13
3A
5
B
10.81
13
Al
26.98
31
Ga
69.72
49
In
114.8
81
Tl
204.4
−1
o
mol
0 C = 273.15 K
(at 298 K)
−1
PV = nRT
k t1/2 = 0.693
pH = pKa + log ( [base] / [acid] )
8 /CHEM 13 NEWS EXAM © 2014 UNIVERSITY OF WATERLOO
18
8A
2
He
4.003
10
Ne
20.18
18
Ar
39.95
36
Kr
83.80
54
Xe
131.3
86
Rn
(222)