CHEF111, Trimester 1 2010/2011
PROGRAMME
SUBJECT CODE
SUBJECT
DATE
TIME
: Foundation of Engineering
: CHEF111
: Chemistry Laboratory
: 12 October 2010
: 1½ hours
INSTRUCTIONS TO CANDIDATES:
1.
This paper contains TWENTY (20) multiple choice questions, ONE (1) structured question, and a Periodic Table in ELEVEN (11) pages, including the cover page.
2.
Answer all questions.
3.
For Section A, there is only ONE best response to each question. Read all responses, choose the BEST one and circle it on the page. Then, mark the letter corresponding to that response in the answer sheet (page 10) .
4.
For Section B, write down your answer in the loose paper provided.
5.
You will submit the answer sheets (page 10) and the papers that have been used up.
Please make sure that you write your name, student ID, Lab section, instructor’s name and seat number on the answer sheets. Do not forget to tie your answer sheets together.
THIS QUESTION PAPER CONSISTS OF 11 PRINTED PAGES INCLUDING THIS
COVER PAGE.
Page 1 of 11

CHEF111, Trimester 1 2010/2011
TABLE OF CONSTANTS
Avogadro's number = 6.022 x 10
23
mol
-1
Gas constant, R = 0.0821 L. atm / K. mol
1 atm = 760 mmHg = 760 torr = 101325 Pa
1 J = 1 kg. m 2 / s 2
Planck’s constant, h = 6.63 x 10
-34
J.s
Rydberg constant, R
H
= 2.18 x 10
-18
J.
Gas constant, R = 8.314 J / K. mol
Speed of light, c = 3.0 x 10 8 ms -1
SECTION A: Multiple Choice Questions (20 points).
There is ONE best response to each question. Read all responses, choose the best one and circle it on the page. Blacken the circle on the answer sheet on page 10 corresponding to this answer .
1.
Match the correct names of the following laboratory apparatus.
A.
B. Graduated cylinder
C.
Erlenmeyer flask
Volumetric flask
D. Volumetric flask
Beaker
Beaker
Crucible
Wash bottles
Watch glass
Filter funnel
Filter funnel
Erlenmeyer flask
E. Graduated cylinder Beaker Erlenmeyer flask
2.
The skull and crossbones (Figure 1) are a classic warning sign in laboratories. What is the type of danger?
Figure 1
A.
Fat-dissolving chemicals.
B.
Flammable materials.
C.
Toxic or poisonous materials.
D.
Someone died while using the chemicals.
E.
Radioactive materials.
Page 2 of 11

CHEF111, Trimester 1 2010/2011
3.
Figure 2 shows one of the separation techniques. What is the name of the technique?
A. Discharging.
B. Evaporation
C. Distillation.
D. Filtration.
E. Magnetization.
Figure 2
4.
Which of the following is the disadvantage of evaporation?
A.
All of the solute is recovered.
B.
The solvent cannot be recovered.
C.
It cannot be used for insoluble solid.
D.
It always requires heat.
E.
It can be done under the hot sun.
Questions 5 and 6 refer to the following statement:
A student mixes 10.0 mL of 0.10 M AgNO
3
with excess copper metal. Balanced equation for the reaction is: 2 AgNO
3
(aq) + Cu (s)

Cu(NO
3
)
2
(aq) + 2 Ag (s)
The reaction should produce 0.107 g of solid silver. However, the student obtains a mass of
1.50 g of silver.
5.
The percent yield is more than 100%. Plausible explanation might include
I.
The student did not substract the mass of filter paper before recording the result.
II.
The student did not thoroughly dry the sample before weighing.
III.
The copper metal did not react completely.
A.
I only.
B.
II only.
C.
I and II only.
D.
I and III only.
E.
I, II and III.
Page 3 of 11

CHEF111, Trimester 1 2010/2011
6.
From the statement, which of the following is CORRECT ?
Limiting reagent Actual yield Theoretical yield
A.
B.
AgNO
3
(aq)
Cu (s)
1.50 g
1.50 g
0.107 g
0.107 g
C.
D.
AgNO
3
(aq)
Cu (s)
0.107 g
0.107 g
1.50 g
1.50 g
E. Cu(NO
3
)
2
(aq) 1.50 g 0.107 g
7.
Stoichiometry of the precipitation reactions can be used to determine the empirical formula of compounds. However, the method is NOT SUITABLE to determine the empirical formula of
A.
calcium oxalate. D.
zinc carbonate.
B.
calcium phosphate. E.
sodium oxalate.
C.
barium chromate.
8.
In the stoichiometry precipitation experiment to determine the empirical formula of magnesium stearate, reaction between 3.0 mL of 0.10 M magnesium cation solution and 12.0 mL of 0.05 M stearate anion solution was found to yield the highest level of precipitation in the test tube. From this result, it can be concluded that the empirical formula for magnesium stearate is
A.
MgC
17
H
35
COO D.
Mg
3
C
17
H
35
COO
B.
Mg
2
C
17
H
35
COO E.
Mg(C
17
H
35
COO)
2
C.
Mg(C
17
H
35
COO)
3
9.
Which of the following statements is/are TRUE about ‘Graham’s Law of Diffusion’?
I.
II.
III.
Under equal condition of temperature and pressure, gases diffuse at rates inversely proportional to the square roots of their molecular masses or densities.
Graham’s law states that the rate at which gas molecules diffuse is also inversely proportional to the square root of its density.
The distance travelled by heavier gas (gas with greater molecular mass), will be less than that travelled by the lighter gas in the same period of time.
A.
I only.
B.
II only.
C.
I and II only.
D.
I and III only.
E.
I, II and III.
Page 4 of 11

CHEF111, Trimester 1 2010/2011
10.
If a gas diffuses 1.65 times more rapidly than CO
2
, what is the molecular mass of the gas?
A.
16 g/mol.
B.
27 g/mol.
C.
118 g/mol.
D.
E.
82 g/mol.
11.
Which of the following statements is/are TRUE about a calorimeter?
I.
A calorimeter is a device used to measure heat changes that accompany physical or chemical processes.
II.
Exothermic process carried out inside a calorimeter resulted with a decrease of the calorimeter temperature.
III.
A.
I only.
B.
II only.
Endothermic process carried out inside a calorimeter resulted with a decrease of the calorimeter temperature.
D.
E.
I and III only.
I, II and III.
C.
I and II only.
12.
A calorimeter and its content have a heat capacity of 19.7 kJ/ o
C. When the temperature of the calorimeter changes from 25 o C to 98 o C, the energy change in the calorimeter and its content is
A.
1438 kJ gained.
B.
2423 kJ gained.
C.
1438 kJ lost.
D.
2423 kJ lost.
E.
1423 kJ lost.
13.
A group of elements from the Periodic Table have the following properties: they float on water; they readily react with oxygen; they burn in a bunsen flame with characteristic colours. The name of the group is
A.
the halogens.
B.
the alkaline earth metals.
C.
the noble gases.
D.
the alkali metals.
E.
the lanthanoids.
Page 5 of 11

CHEF111, Trimester 1 2010/2011
14.
Many fireworks colours come from burning metal salts and each metal salt has its own distinctive flame colour. How does flame colour being produced?
A.
Flame colour is produced from the reaction of the electrons in the metal ion with the electron in the anion of the salt.
B.
Flame colour is produced from the movement of protons and neutrons in the metal ion.
C.
Flame colour is produced when electrons in the metal ion collided with the electrons in the flame.
D.
Flame colour is produced from the reaction of the metal salts with oxygen in the burning process.
E.
Flame colour is produced from the movement of the electrons in the metal ions present in the salt.
15.
A student carries out an experiment to determine the reactivity of three metals with water. The metals belong to the same Group in the Periodic Table. The table below shows the observations recorded from the experiment.
Metal Observation
X The metal reacted vigorously with water at room temperature.
Y The metal reacted slightly with water at room temperature but the rate of reaction increased when the test tube is heated.
Z The metal has no reaction with water (at room temperature) or steam.
Based on the observation above, the arrangement of the metals in increasing order of reactivity is
A.
Z , X , Y .
B.
X , Y , Z .
D.
E.
X , Z , Y
Y , Z , X
.
.
C.
Z , Y , X .
Questions 16 and 17 refer to the data extracted from a student’s report sheet on Redox
Reaction as shown below:
(ii) Reactivity of Sn, Cu and Zn with Hydrogen ion.
Experiment Observation
Sn + H
+
Bubbles were formed and the test tube was warm.
Cu + H
+
No reaction.
Zn + H
+
Bubbles were formed but the amount was more than reaction between Sn & H
+
, and the test tube was warm.
Page 6 of 11

CHEF111, Trimester 1 2010/2011
16.
Which of the following is the CORRECT equation for the reaction between Zn and
H
+
?
A.
Zn + 2 H + 
Zn 2+ + H
2
B.
Zn + H
+ 
Zn
+
+ H
C.
Zn + 2 H
+ 
Zn
2+
+ 2 H
D.
2 Zn + H 2+  2 Zn + + H
2
E.
Zn
2+
+ 2 H
+ 
Zn + H
2
17.
Which of the following is the most plausible source of hydrogen ion in the experiment?
A.
6 M ZnH
2
.
B.
6 M HCl.
C.
6 M H
2
(gaseous).
D.
6 M H
2
Zn.
E.
6 M H
2
O.
Questions 18, 19 and 20 refer to the diagrams below:
Cell A Cell B
18.
What is the difference between Cell A and Cell B ?
A.
Cell A is a galvanic cell while Cell B is a voltaic cell.
B.
Cell A is a galvanic cell while Cell B is an electrolytic cell.
C.
Cell A is a voltaic cell while Cell B is a galvanic cell.
D.
Cell A is an electrolytic cell while Cell B is a galvanic cell.
E.
Both Cell A and Cell B are the same.
Page 7 of 11

CHEF111, Trimester 1 2010/2011
19.
In Cell A , is it possible to have both compartment (left and right) filled with aqueous solution of copper(II) sulphate?
A.
No, the set-up of the cell must not be changed. The cell will not work properly if both compartments contain the same solution.
B.
Yes, but the CuSO
4
solutions must be of high concentrations and inert electrode must be used to replace both zinc and copper electrodes.
C.
No, because there will no electron movement in the solutions if both compartments contain aqueous solution of copper(II) sulphate.
D.
Yes, but the CuSO
4
solutions must be of different concentrations and both electrodes must be copper metals.
E.
Yes, but both electrodes must be zinc metals.
20.
If the electrolyte in Cell B is 0.5 M aqueous solution of CuSO
4
, what would be the observations at both electrodes?
Observation at Cathode Observation at Anode
A. Gas bubbles are produced.
B. Gas bubbles are produced.
Gas bubbles are produced.
Reddish-brown deposit is formed.
Gas bubbles are produced. C. Grey deposit is formed.
D.
Reddish-brown deposit is formed.
E. Gas bubbles are produced.
Gas bubbles are produced.
Grey deposit is formed.
Page 8 of 11

CHEF111, Trimester 1 2010/2011
SECTION B: Structured Question (10 points).
Write down your answer in the loose paper provided.
In chemistry, the density of many substances is usually compared to the density of water.
Does an object float on water or sink in the water? If an object such as a piece of wood floats on water it is less dense than water but if a rock sinks, it is more dense than water. a) State the formula (with appropriate units) used to calculate density. (2 points) b) You are given an irregular shaped metal object in an experiment. In order to calculate density, the volume of the object is needed. The volume can be determined using the water displacement technique. Write down the procedures involve in determining the mass and volume of the object. (2 points) c) List the appropriate laboratory glassware and/or equipment for question (b). (2 points) d) State two (2) precaution steps when using the water displacement technique. (2 points) e) If the irregular shaped metal object is broken in half, will the density change? Explain why. (2 points)
END OF QUESTION PAPER -
Page 9 of 11

CHEF111, Trimester 1 2010/2011
SEAT NUMBER:
PROGRAMME
SUBJECT CODE
SUBJECT
: Foundation of Engineering
: CHEF111
: Chemistry Laboratory
NAME: __________________________________ STUDENT ID.: _____________
INSTRUCTOR : __________________________ LAB SECTION : ____________
SECTION A: Please use 2B pencil to fill the circle completely.
Example:
1. 11.
2.
3.
4.
5.
6.
7.
8.
9.
10.
16.
17.
18.
19.
20.
12.
13.
14.
15.
Page 10 of 11

CHEF111, Trimester 1 2010/2011
PERIODIC TABLE
1
1A
1
H
1.008
2
2A
3
Li
6.941
11
Na
22.99
19
K
39.10
37
Rb
85.47
55
Cs
132.9
87
Fr
(223)
4
Be
9.012
12
Mg
24.31
20
Ca
40.08
38
Sr
87.62
56
Ba
137.3.
88
Ra
(226)
3
3B
21
Sc
44.96
39
Y
88.91
57
La
138.9
89
Ac
(227)
13
3A
4
4B
5
5B
6
6B
7
7B
22
Ti
47.90
40
Zr
91.22
72.
Hf
178.5
104
Rf
(261)
23
V
50.94
41
Nb
92.91
73
Ta
180.9
105
Db
(262)
24
Cr
52.00
42
Mo
95.94
74
W
183.9
106
Sg
(266)
25
Mn
54.94
43
Tc
98
75
Re
186.2
107
Bh
(264)
26
Fe
55.85
44
Ru
101.1
76
Os
190.2
108
Hs
(269)
27
Ir
Mt
Co
58.93
45
Rh
102.9
77
192.2
109
(268)
8 9 10
8B 9B 10B
11
1B
12
2B
28
Ni
58.70
46
Pd
106.4
78
Pt
195.1
110
Ds
(269)
29
Cu
63.55
47
Ag
107.9
79
Au
197.0
30
Zn
65.39
48
Cd
112.4
80
Hg
200.6
5
B
10.81
13
Al
26.98
31
Ga
69.72
49
In
114.8
81
Tl
204.4
58
90
Th
Ce
140.1
232.0
59
Pr
91
Pa
140.9
(231)
60
92
U
Nd
144.2
238.0
61
93
Np
Pm
(145)
(237)
62
Pu
Sm
150.4
94
(244)
63
Eu
152.0
95
Am
(243)
64
Gd
157.3
96
Cm
(247)
65
Tb
158.9
97
Bk
(247)
66
Dy
162.5
98
Cf
(251)
67
Ho
164.9
99
Es
(252)
14
4A
6
C
12.01
14
Si
28.09
32
Ge
72.61
50
Sn
118.7
82
Pb
207.2
68
Er
167.3
100
Fm
(257)
15
5A
16
6A
8
O
16.00
16
S
32.06
34
Se
78.96
52
Te
127.6
84
Po
(209)
7
N
14.01
15
P
30.97
33
As
74.92
51
Sb
121.8
83
Bi
209.0
17
7A
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)
9
F
19.00
17
Cl
35.45
35
Br
79.90
53
I
126.9
85
At
(210)
69
Tm
168.9
101
Md
(258)
70
Yb
173.0
102
No
(259)
71
Lu
175.0
103
Lr
(260)
Page 11 of 11