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Queens University *
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Course
112
Subject
Chemistry
Date
Jan 9, 2024
Type
Pages
12
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1
Practice Exam
Student Number:_____________________
Name: _______________________________________
INSTRUCTIONS:
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–
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–
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PLEASE NOTE:
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This material is copyrighted and is for the sole use of students registered in CHEM112 and writing this exam. This
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Page 2 of 11
1.
Which of the following represents a base unit in the SI system of measurements?
A.
m
2
B.
kg
C.
g/cm
3
D.
m/s
E.
liter
2.
What is the mass of a 468 mL sample of ethanol? The density of ethanol is 0.789 g/mL.
A.
234 g
B.
739 g
C.
468 g
D.
593 g
E.
369 g
3.
Choose the INCORRECT name formula combination.
A.
Fe
2
O
3
iron(III) oxide
B.
H
2
SO
3
sulfurous acid
C.
NH
4
ClO
3
ammonium chlorate
D.
CaH
2
calcium hydride
E.
SiO
2
silicon oxide
4.
2.404 g of a compound were burned in oxygen and found to produce only 3.520 g CO
2
(g), 2.564 g
SO
2
(g) and 1.440 g H
2
O(l). Determine the empirical formula of the compound.
A.
CSH
B.
C
2
SH
4
C.
C
4
SH
2
D.
C
2
S2H
4
E.
C
2
SH
2
5.
What is the sum of the coefficients when the following is balanced with the smallest integer
coefficients?
CaC
2
(s) + H
2
O(l) → Ca(OH)
2
(s) + C
2
H
2
(g)
A.
8
B.
4
C.
5
D.
10
E.
9
Page 3 of 11
6.
Lithium and nitrogen react to produce lithium nitride:
6 Li(s) + N
2
(g) →
2Li
3
N(s)
How many moles of lithium nitride are produced when 0.450 mol of lithium react in this fashion?
A.
0.150
B.
0.900
C.
0.0750
D.
1.35
E.
0.225
7.
Assuming ideal gas behavior, which of the following gases would have the lowest density at standard
temperature and pressure?
A.
SF
6
B.
CF
2
Cl
2
C.
CO
2
D.
N
2
E.
Kr
8.
Which of the following is a characteristic of an ideal gas?
A.
The gas cannot be compressed infinitely.
B.
Inter-particle forces are prominent.
C.
Collisions between gas particles are perfectly elastic.
D.
Collisions between gas particles and container walls are not elastic.
E.
Individual gas particles occupy fixed volume.
9.
If someone were to light a cigar at one end of a closed room, persons at the other end of the room might
soon perceive an odor due to gaseous emissions from the cigar. Such a phenomenon is an example of:
A.
monometry
B.
ideality
C.
effusion
D.
diffusion
E.
barometry
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Page 4 of 11
10.
A balloon filled with helium gas at 20 °C occupies 4.91 L at 1.00 atm. The balloon is immersed in liquid
nitrogen at -196 °C, while the pressure is raised to 5.20 atm. What is the volume of the balloon in the
liquid nitrogen?
A.
0.25 L
B.
3.6 L
C.
6.7 L
D.
97 L
11.
Choose the INCORRECT statement.
A.
Temperatures of two bodies are equal when the average kinetic energies of the two bodies become the
same.
B.
The heat capacity is the quantity of heat required to change the temperature of the system by one degree.
C.
The specific heat is the heat capacity for one mole of substance.
D.
The law of conservation of energy can be written:
q
system
+
q
surroundings
= 0.
E.
Most metals have low specific heats, as metals can be heated quickly.
12.
The complete combustion of 1 mole of nitrobenzene, C
6
H
5
NO
2
, in a bomb calorimeter liberates 3088 kJ
of heat and increases the temperature of the calorimeter assembly by 140.0 °C. What is the heat
capacity of this bomb calorimeter?
A.
1.25 kJ/ °C
B.
4.53 kJ/ °C
C.
22.1 kJ/ °C
D.
432 kJ/ °C
E.
43.1 kJ/ °C
13.
Calculate the standard enthalpy of formation of Cl
-
(aq), given the following thermochemical data at 1
atm, and knowing that the standard enthalpies of formation of H
2
(g) and H
+
(aq) are both zero.
HCl(g) → H
+
(aq) + Cl
-
(aq)
Δ
r
H°
= -75.15 kJ/mol
H
2
(g) + Cl
2
(g) →
2HCl(g)
Δ
r
H°
= -184.62 kJ/mol
A.
-167.46 kJ/mol
B.
+109.47 kJ/mol
C.
-17.16 kJ/mol
D.
+34.32 kJ/mol
E.
+ 167 kJ ?mol
Page 5 of 11
13.
From the following thermochemical equations, calculate Δ
r
H°
for the reaction:
SO
2
(g) + NO
2
(g)
→
SO
3
(g) + NO(g)
2 SO
2
(g) + O
2
(g)
→
2 SO
3
(g)
Δ
r
H°
= -197.8 kJ/mol
2 NO(g) + O
2
(g) → 2 NO
2
(g)
Δ
r
H°
= -114.14 kJ/mol
A.
-83.66 kJ /mol
B.
-311.9 kJ/mol
C.
+155.9 kJ/mol
D.
-155.9 kJ/mol
E.
-41.83 kJ/mol
Answer:
E
14.
The photoelectric effect:
A.
was discovered by Max Planck
B.
describes the phenomenon of producing light by shining a beam of electrons by on any metal surface
C.
contradicted the view that light energy was dependent upon intensity only
D.
is not the same principle used in modern electric eyes and solar calculators
E.
results in a beam of electrons which increases in number, but not velocity, as the wavelength of incident
light decreases
15.
When an electron in an atom goes from a high energy state to a low one, what occurs?
A.
Another electron goes from a low energy state to a high one.
B.
The atom moves faster.
C.
Light is given off.
D.
Light is absorbed.
E.
This process is not possible.
16.
Calculate the wavelength in meters of light absorbed by an electron in an atom of hydrogen as it moves
that makes a transition from
n
= 6 to
n
= 3.
A.
1.65 × 10
-11
m
B.
1.09 × 10
-6
m
C.
1.83 × 10
-7
m
D.
8.22 × 10
-7
m
E.
3.28 × 10
-6
m
Page 6 of 11
17.
What is the smallest acceptable value for the missing quantum number?
n
= ?, ℓ = 2,
m
ℓ
= 0,
m
s
= +1/2
A.
3
B.
2
C.
4
D.
5
E.
1
18.
Which of the following statements concerning quantum numbers is NOT correct?
A.
"
n
" relates the most probable distance from the nucleus.
B.
"
l
" denotes geometric shape.
C.
"
m
" denotes orientation of an orbital with respect to the others.
D.
The fourth quantum number refers to electron spin.
E.
The four quantum numbers are derived from wave mechanics.
19.
Exceptions to ________ are represented by chromium and copper in the 4th row of the periodic table.
A.
the Aufbau Principle
B.
Hund's Rule
C.
the Bohr Theory
D.
the Heisenberg Principle
E.
the Pauli Exclusion Principle
20.
The quantum numbers of the last electron of nickel could be:
A.
n
= 3, ℓ = 2,
m
ℓ
= 0,
m
s
= -1/2
B.
n
= 4, ℓ = 2,
m
ℓ
= 0,
m
s
= +1/2
C.
n
= 3, ℓ = 1,
m
ℓ
= 0,
m
s
= +1/2
D.
n
= 3, ℓ = 2,
m
ℓ
= 0,
m
s
= 0
E.
n
= 3, ℓ = 2,
m
ℓ
= 1/2,
m
s
= +1/2
21.
The ground state electron configuration of Sc is ________.
A.
1s
2
2s
2
2p
6
2d
10
3s
1
B.
1s
2
1p
6
2s
2
2p
6
3d
5
C.
1s
2
2s
2
2p
6
3s
2
3p
6
3d
3
D.
1s
2
2s
2
2p
6
3s
2
3p
6
4s
2
3d
1
E.
1s
2
2s
2
2p
6
3s
2
3p
6
4s
2
4p
1
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Page 7 of 11
22.
How many unpaired electrons are in the ground state electron configuration of chromium?
A.
5
B.
6
C.
4
D.
2
E.
0
23.
Calculate the deBroglie wavelength of a ball of mass 125 grams and velocity 90 m/s.
A.
0.59 m
B.
5.9 × 10
-31
m
C.
5.9 × 10
-35
m
D.
590 m
E.
1.7 × 10
34
m
24.
The transition elements refer to what group of elements?
A.
s
-block elements
B.
d
-block elements
C.
actinides
D.
lanthanides
E.
p
-block elements
25.
What is the general valence electronic configuration (where
n
= principal quantum number) that best
describes the halogens as a group?
A.
ns
1
np
6
B.
ns
2
np
4
C.
ns
2
np
5
D.
ns
2
np
6
E.
ns
2
np
3
26.
Which of the following has the largest radius?
A.
Se
2-
B.
Kr
C.
Rb
+
D.
Br
-
E.
Y
3+
Page 8 of 11
27.
What is the relationship between ionization energy and atomic radii?
A.
Energy increases as radii increase.
B.
Energy is negative for all large radii.
C.
Energy decreases as radii decrease.
D.
Energy decreases as radii increase
E.
Energy increases as radii decrease
28.
Which of the following species contains a triple bond?
A.
NH
3
B.
HCCl
3
C.
NO
3
-
D.
CO3
2-
E.
CN
-
29.
Which of the following exhibits covalent bonding?
A.
NaF
B.
SrO
C.
LiH
D.
OF
2
E.
K
2
S
30.
An expanded octet may occur:
A.
in the 1st and 2nd period only
B.
in families IA, IIA, and IIIA only
C.
anywhere except period 1 and 2
D.
in all families except IA
E.
in the 3rd and 4th period only
31.
Which of the following is diamagnetic?
A.
ClO
2
B.
NO
C.
CO
D.
NO
2
E.
CH
3
Page 9 of 11
32.
Which of the following molecules is polar?
A.
NBr
3
B.
CH
4
C.
CS
2
D.
NH
4
+
E.
PCl
5
33.
Which of the following molecules has both an electron group geometry and a molecular shape
described as trigonal planar?
A.
SiH
4
B.
PF
3
C.
OF
2
D.
CHF
3
E.
BF
3
34.
What is the formal charge on B in BF
4
-
?
A.
+1
B.
-1
C.
+2
D.
0
E.
-2
35.
Given the bond enthalpies I
—
Cl (209), H
—
H (435), H
—
I (297), and H
—
Cl (431) in kJ/mol, compute
Δ
H°
in kJ/mol for: ICl
3
(g) + 2 H
2
(g) → HI(g) + 3 HCl(g).
A.
+264 kJ/mol
B.
-84 kJ/mol
C.
-93 kJ/mol
D.
-523 kJ/mol
E.
+84 kJ/mol
36.
Which of the following sets of molecules and information regarding MO theory are INCORRECT?
A.
O2: Bond order = 2, paramagnetic
B.
N2: Bond order = 3, paramagnetic
C.
NO: Bond order = 2.5, paramagnetic
D.
F2: Bond order = 1, diamagnetic
E.
BC: Bond order = 1.5, paramagnetic
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Page 10 of 11
37.
When a liquid is in dynamic equilibrium with its vapor at a given temperature, the following
conditions could exist:
I) There is no transfer of molecules between liquid and vapor.
II) The vapor pressure has a unique value.
III)
The opposing processes, (liquid to vapor) and (vapor to liquid), proceed at equal rates.
IV)
The concentration of vapor is dependent on time.
Which of the above choices are applicable?
A.
I
B.
II and III
C.
I, II, and III
D.
II and IV
E.
II, III and IV
38.
Given the data below, determine the molar enthalpy of vaporization of COCl
2
.
, P
1
= 40 mmHg, t
1
= -50.3 °C, P
2
= 100 mmHg, t
2
= -35.6 °C
A.
0.518 kJ/mol
B.
27.4 kJ/mol
C.
4.32 kJ/mol
D.
0.928 kJ/mol
E.
0.112 kJ/mol
39.
The unit cell parameter for iron (bcc) is measured to be 286 pm.
What is the diameter of an iron atom.
A.
124 pm
B.
101 pm
C.
248 pm
D.
202 pm
40.
Surface tension is thought to be due to:
A.
surface area trying to increase
B.
air absorbed on the surface
C.
solute concentrated on the surface
D.
surface molecules having lower energy than bulk molecules
E.
surface molecules having higher energy than molecules in the bulk
Page 11 of 11
41.
According to the phase diagram given, which of the following statements is INCORRECT?
A.
At the temperature and pressure of point 1, W exists as a three-phase equilibrium system.
B.
At the temperature of point 2, a pressure of 500 Torr will cause W to liquefy.
C.
If the system is maintained at the temperature of point 3 while pressure is decreased, more W will
vaporize.
D.
If W is maintained at the pressure of point 4 while the temperature is increased to 80 °C, the liquid will
vaporize.
E.
The existence of liquid W at -40 °C and 500 Torr represents the metastable condition of "supercooling."
Table of Electronegativies
Data/Formula Sheet
Symbol
Value
R
8.31451 J K
–
1
mol
–
1
0.08206 L-atm mol
–
1
K
–
1
k
b
1.3807 × 10
–
23
J K
–
1
N
A
6.0221 × 10
23
mol
–
1
F
96485. C mol
–
1
e
1.6022 × 10
–
19
C
Page 12 of 11
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
1A
2A
3B
4B
5B
6B
7B
8B
8B
8B
1B
2B
3A
4A
5A
6A
7A
8A
1
2
1
H
He
1.008
4.003
3
4
5
6
7
8
9
10
2
Li
Be
B
C
N
O
F
Ne
6.941
9.012
10.81
12.01
14.01
16.00
18.99 20.18
11
12
13
14
15
16
17
18
3
Na
Mg
Al
Si
P
S
Cl
Ar
22.99
24.30
26.98
28.09
30.97
32.07
35.45 39.95
19
20
21
22
23
24
25
26
27
28
29
30
31
32
33
34
35
36
4
K
Ca
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
Ga
Ge
As
Se
Br
Kr
39.1
40.08
44.96
47.87
50.94
52.00
54.94
55.84
58.99
58.34
63.55
65.39
69.72
73.61
74.92
78.96
79.90
83.8
37
38
39
40
41
42
43
44
45
46
47
48
49
50
51
52
53
54
5
Rb
Sr
Y
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Ag
Cd
In
Sn
Sb
Te
I
Xe
85.47
87.62
88.91
91.22
92.91
95.94
99
101.1
102.9
106.4
107.9
112.4
114.8
118.7
121.8
127.6
126.9 131.3
55
56
57
72
73
74
75
76
77
78
79
80
81
82
83
84
85
86
6
Cs
Ba
La
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Tl
Pb
Bi
Po
At
Rn
132.9
137.3
138.9
138.9
181.0
183.8
186.2
190.2
192.2
195.1
197.0
200.6
204.4
207.2
209.0
209
210
222
87
88
89
7
Fr
Ra
Ac
223
226
227
58
59
60
61
62
63
64
65
66
67
68
69
70
71
6
Ce
Pr
Nd
Pm
Sm
Eu
Gd
Tb
Dy
Ho
Er
Tm
Yb
Lu
140
141
144
145
150
152.0
157
159
163
165
167
169
173.0
175.0
90
91
92
93
94
95
96
97
98
99
100
101
102
103
7
Th
Pa
U
Np
Pu
Am
Cu
Bk
Cf
Es
Fm
Md
No
Lr
232
231.0
238.0
237
244
243
247
247
251
252
257
258
259
262
1atm = 101.325 kPa = 760 mm Hg = 760 torr | 750 mm Hg = 100 kPa = 1 bar
1L = 1 dm
3
|
0ºC = 273.15 K
|
E = h
|
c =
|
𝜆 =
ℎ
𝑝
=
ℎ
?𝑢
|
𝑉 = 𝑖?𝑅𝑇
d = m/V
𝐸 = ℎ𝜈 = 𝑅
𝐻
|
1
?
1
2
−
1
?
2
2
|
x(A) +x(B) +
…=1
?
1
?
1
=
?
2
?
2
PV = nRT
P
1
V
1
= P
2
V
2
|
PV = nRT
|
w =
–
P
e
V =
–
n
gas
RT
|
E = q + w
|
E = q
v
|
H = q
p
p
B
= x
B
K
H
p
A
+ p
B
+ … = P
𝐶 =
q
Δ?
𝐶
?
=
Δ?
Δ?
𝐶
𝑃
=
Δ𝐻
Δ?
C
P
–
C
V
= R
p
A
= x
A
P
A
*
∆𝑇
𝑏
= 𝑖𝑘
𝑏
?
∆𝑇
𝑓
= 𝑖𝑘
𝑓
?
C = K
H
P
M
RT
u
rms
3
=
H =
U + P
V
|
|
P
1
V
1
= P
2
V
2
|
KE = ½ mv
2
|
h
= KE +
|
M = m/n
|
−
=
formed
broken
BE
BE
H
(
)
*
*
*
1
B
A
A
A
A
A
B
A
A
A
P
x
P
x
P
x
p
p
p
y
−
+
=
+
=
(
)
(
)
*
*
*
1
1
B
A
A
A
B
A
B
A
B
B
P
x
P
x
P
x
p
p
p
y
−
+
−
=
+
=
(
)
RT
b
V
V
a
P
m
m
=
−
+
2
C
C
P
T
R
a
64
27
2
2
=
C
P
RT
b
8
=
−
−
=
1
2
*
1
*
2
1
1
ln
T
T
R
H
P
P
vap
(
)
298
298
−
+
=
T
C
H
H
P
o
o
T
(R)
(P)
−
=
o
f
o
f
o
H
H
H
h
6.6261 × 10
–
34
J s
m
p
1.6726 × 10
–
27
kg
m
e
9.1094 × 10
–
31
kg
R
H
2.179 × 10
–
18
J
c
2.9979 × 10
8
m s
–
1
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C-14 --> ____________ + N-14
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adds-up to 100. You may use the periodic table previously provided, a calulator and clean scrap paper.
Timed Test This test has a time limit of 2 hours.This test will save and submit automatically when the time expires.
Warnings appear when half the time, 5 minutes, 1 minute, and 30 seconds remain.
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Remaining Time: 1 hour, 58 minutes, 38 seconds.
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A Moving to another question will save this response.
Question 4
A sodium chloride solution is 38% NaCl by mass and has a density of 1.12 g.ml, determine:
The Molarity of the solution
The molality of the solution
The mole fraction of water
A Moving to another question will save this response.
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Could someone Please Help with these!
No plagiarism Please!
A tire inflated with air is an example of a ___________________________.
Evidence -
Explanation -
A pellet of sodium (Na) sliced in two pieces is an example of a _____________________________.
Evidence -
Explanation -
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human answers only!
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iii)
iv)
v)
vi)
HBr
1) 03
2) H₂O, Zn
CH3
i
CH₂CH₂CCH3 + (C6H3)3P+____C(CH3)2
1) 03
2) H₂O, Zn
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a. What instrument was used to discover the structure of DNA?
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c. Who were the four main scientists involved in discovering the structure
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d. What did you notice about the process of science represented in the
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Edit View Insert
Format
Tools Table
12pt v
Paragraph v
BI
Address
DELL
F4
F5
F6
F7
F8
F9
F10
F11
II
88888:
$
&
4.
6.
7
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a. transmitting
b. absorbing
c. refelecting
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TRUE OR FALSE
__________ 6. The bowl of the funnel for gravity filtration may be filled to the brim.
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stirring rod.
__________ 8. Never touch, taste, or smell a chemical unless specifically told to do so.
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H2, Ni
+zog'20
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Draw the products of the reactions.
products
Select Draw Rings More
Erase
H
+ H,0
H+
products
Select DrawRings More
Erase
H
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c. manually stirring the solution
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