MULUNGUSHI UNIVERSITY
SCHOOL OF NATURAL AND APPLIED SCIENCES
DEPARTMENT OF CHEMISTRY AND BIOLOGY
CHE 111 TEST 1 SEMESTER I 2023/24
Instructions.
Duration: 1 hour 30 minutes
Attempt ALL questions in this test. Answer by crossing out the correct answer using a pencil preferably.
Answer all questions using the answer grid provided.
Write your name, student ID and TG number on the answer grid.
___________________________________________________________________________________________________________
Q1. Covert 2.3 atm in mm Hg.
A. 2300 mm Hg
B. 1750 mm Hg
C. 2.3 mm Hg
D. 0.0030 mm Hg
Q2. Which states that if temperature is constant,
pressure is inverse to the volume?
A. Charles’ law B. Boyles’ Law
C. Gay Lussac’s D. Ideal gas Law
Q3. Calculate the temperature at which 32g N2
occupies a volume of 8 liters at 4.48 atm.
A. 179K B. 382.1K C. 141.1K D. 714K
Q4. What is the molecular mass of a gaseous
compound at S.T.P if the gas in a 1.00 L bulb weighs
0.672 g at 25.0 °C and 733.4 mm Hg?
A. 0.672 g/mol
B. 2.46 g/mol
C. 29.34g/mol
D. 17.03g/mol
Q5. When the temperature of 500 ml of air rises
from 23°C to 43°C under constant pressure, what is
the increase in volume?
A. 533.8 mL
B. 500.0 mL
C. 33.8 mL
D. 1033.8 mL
Q6. Given a gas in a rigid container is heated from
100 OC to 500 OC. Which statement best describes
the pressure of the gas in a rigid container?
A. Pressure decrease by a factor of 5
B. Pressure increases by a factor of 5
C. Pressure increases by a factor of 2
D. Pressure decreases by a factor of 2
Q7. Avogadro’s law states that equal volumes of a
gas at the same temperature and pressure should
have equal…
A. Number of molecules
B. Number of grams
C. Molar masses
D. Speeds
Q8. A mixture of Neon and Krypton were placed in a
2.0 dm3 volume container. The partial pressure of
Neon is 0.40 atm and 1.20 atm. What is the mole
fraction of neon?
A. 0.20
B. 0.25
C. 0.33
D. 0.50
Q9. A gas of 3.4 moles occupies a volume of 40.6 mL
at 298K. What is the pressure of the gas?
A. 2.1 x 105KPa
B. 1.57 x 106KPa
5
C. 1.05 x 10 KPa
D. 3.14 x 106KPa
Q10. Which diagram does not represents the
Boyles’ Law of gases?
Q11. A breast implant bag has a volume of 5.0 mL
at a pressure of 0.90 atm. It rises to an altitude,
acquires a new volume of 25.0 mL. Which statement
is correct about the implant?
A. Pressure in the bag decreases
B. Pressure in the bag increases
C. Pressure in the bag remain the same
D. None of the statement is correct
Q12. What is the temperature that corresponds to
S.T.P conditions in degree Celsius?
A. 100 OC B. 0 OC
C. 25 OC
D. -273 OC
Page 1 of 6
Q13. The kinetic-molecular theory explains the
behavior of…
A. Gases only
B. Solids and Liquids
C. Liquids and Gases D. Solids, Liquids and Gases
Q14. According to the kinetic theory of matter, the
greater the mass or velocity of a particle, the
________ the kinetic energy.
A. lesser
B. same
C. greater
D. All the above
Q15. SO2 (5.00 g) and CO2 (5.00 g) are placed in a
750.0 mL container at 50.0°C. The partial pressure
of SO2 in the container was __________ atm.
A. 1.26
B. 2.76
C. 6.78
D. 4.02
Q16. Of the following gases, ___ will have the
greatest rate of effusion at a given temperature.
A. NH3
B. O2
C. CO
D. HBr
Q17. At 323 K, which of the pairs of gases below
would have the most nearly identical rates of
effusion?
A. N2O and NO2
B. N2 and CO
C. CO2 and CO
D. None of the above
Q18. In deal gases law it is assumed that …
A. Volume of individual gases is negligible
A. C9H18O9
C. C6H12O6
B. C2H4O2
D. CH2O
Q22. A 100.0-g sample of a compound is made up
of 35.9 g of aluminum and 64.1 g of sulfur. The
empirical formula of the compound is:
A. Al2S3
B. Al4S6
C. AlS
D. Al3S2
Q23. Copper (II) sulphate has the formula
CuSO4.5H2O. What mass of water is contained in
50g of the salt?
A. 0.06g B. 5.60g
C. 18.0g
D. 28.1g
Q24. A compound with a molar mass of 78.0 g/mol
is found to contain 92.29% carbon and 7.71%
hydrogen, by mass. The molecular formula of the
compound is:
A. CH B. C2H3
C. C3H3.
D. C6H6.
Q25. What is the unit for relative molecular mass?
A. g
B. a.m.u
C. g/mol
D. no units
Q26. The ______ (Ar) of copper is the average mass
of the different isotopes (taking into account their
relative Abundances)
A. Isotopes
B. Isotopic abundance
C. Relative isotopic mass D. Relative atomic mass
Q27. What do isotopes of an element have in
common?
A. an equal number of neutrons
B. Volume of individual gases is counted to volume
C. Mass of gas is negligible
D. Mass of gas is accounted for.
B. a different number of protons
C. the same mass number
D. the same number of electrons
Q19. Arrange the following gases in order of
increasing average molecular speed at 25°C: He, O2,
CO2, and N2.
He < N2 < O2 < CO2
B. He < O2 < N2 < CO2
C. CO2 < O2 < N2 < He
D. CO2 < N2 < O2 < He
A.
Q28. Find the number of neutrons in a Zn2+ ion.
The mass number is 70.
A. 40
B. 36
C. 38
D. 34
Q29. What is the percentage composition of
phosphorus in calcium phosphate?
A. 35%
B. 30%
C. 25%
D. 20%
Q20. At what temperature in kelvins, will 0.444 mol
of CO gas occupies 11.8 L at 889 torr?
A. 379 K
B. 32 K
C. 73 K
D. 16 K
Q21. The empirical and molecular formula mass of
a compound are CH20 and 180g. What is the
molecular of the compound?
Q30. 0.1 mole of hydrate Y.nH2O contains 12.6g of
water. What is the value of n in Y.nH2O?
A. 4
B. 5
C. 6
D. 7
Q31. How many significant figures are in the
measurement 2.1032 x 104 g?
A. 2
B. 3
C. 4
D. 5
Page 2 of 6
Q32. Which of these equalities is NOT correct?
A. 100cg = 1g
B. 1000mm = 1m
3
C. 1.0 cm = 1.0 mL
D. 10Kg = 1 cg.
Q42. Calculate the mass of oxygen required
to react completely with 5.3960 grams of
aluminum according to the reaction:
4Al(s) + 3O2(g)→2Al2O3(S)
Q33. How many of the zeros in the measurement
0.000040200 m are significant?
A. 2
B. 3
C. 5
D. 7
Q34. How many milligrams are in 2.5 kg?
A. 2.5 x 106 mg
B. 25 mg
-4
C. 2.5 x 10 mg
D. 2.5 x 102 mg
Q35. Express the answer in scientific form for
145.75  (2.3 101 )
A. 1.4598 x 102
C. 1.4 x 10-2
B. 1.46 x 102
D. 1.5 x 102
Q36. Three students determined the volume of a
sample of ethanol. The results are: X (87.1, 88.2,
87.6); Y (86.9, 87.1, 87.2); Z (87.6, 87.8, 87.9). If the
true volume is 87.0 mL, which student was both
accurate and precise?
A. X
B. Y
C. Z
D. All of them
Q37. Concentrated hydrochloric acid has a density
of 1.19 g/ml. What is the mass, in milligrams, of 2.0
liters of this acid?
A. 2.4 x 106 mg
B. 24 mg
C. 2.4 x 10-4 mg
D. 2.4 x 102 mg
Q38. . Convert 7.58 cm to nm
A. 7.58 x 107 nm
B. 0.758 nm
C. 75.8 nm
D. 7.58 x 10-7 nm
Q39. A sample of water is heated from room
temperature to just below the boiling point. The
overall change in temperature is 72°C. Express this
temperature change in kelvins.
A. 345K
B. 72K
C. 0 K
D. 201K
Q40. _____ is a reagent in the reaction that is
responsible for final product formed.
A. Excess reagent
B. limiting reagent
C. Non wasting reagent
D. Wasting reagent
Q41. What are the missing coefficients for the
skeleton equation below?
Al2(SO4)3(aq) + KOH(aq)
Al(OH)3(aq) + K2SO4(aq)
A. 6.40g B. 4.80g C. 2.40g D. 3.20g
Q43. Which of the given chemical equations is
balanced?
A. H2O2 → H2O + O2
B. NaNO3 → NaNO2 + O2
C. CaCO3 → CaO + CO2 D. Al2CO3 → Al2O3 + CO2
Q44. How many moles are in 1.25 g of CH 4?
A. 0.0785
B. 0.0779
C. 0.156
D. 0.10
Q45. If a table spoon of maltose contains 3.423g of
sugar C12H22O11. How many molecules of maltose
are these?
A. 6.0 x 1023.
B. 6.0 x 1022.
21
C. 6.0 x 10 .
D. 6.0 x 1024.
Q46. If the reaction of 6.5 grams of C6H12O6
produces 2.5 grams of CO2, what is the percent
yield of CO2?
C6H12O6 → 2C2H5OH + 2CO2
A. 92.0%
B. 78.7%
C. 100%
D. 21.3%
Q47. Percentage yield is calculated by:
A.
B.
C.
D.
Ratio of theoretical over actual
Ratio of actual over theoretical
Ratio of molar masses
Ratio of mass over molar mass
Q48. Potassium chlorate decomposes upon slight
heating in the presence of a catalyst, according to
the reaction below. 2KClO3 → 2KCl + 3O2. What is
the molar ratio of products?
A. 2:2
B. 2:3
C. 1:3
D. 1:1
Q49. Urea (NH2)2CO is used as nitrogen enriching
fertilizer. What is the percentage of nitrogen in
urea?
A. 23%
B. 50%
C. 46%
D. 25%
Q50. 12.044 x 1023 contains ______ atoms of
oxygen.
A. 1.0 moles
B. 2.0 moles
C. 3.0 moles
D. 4.0 moles
A. 1,3,2,3 B. 2,12, 4,6 C. 4,6,2,3 D. 1,6,2,3
Page 3 of 6
VITAL DATA AND EQUATIONS
PV = nRT
Gas Constant Values (R)
Units
8.314
m3.Pa.K-1.mol-1
62.36
L.Torr.K-1.mol-1
1.987×10−3
kcal.K-1.mol-1
62.36
L⋅mmHg/K⋅mol
8.206×10−2
L.atm.K-1.mol-1
N0 = 6.0 x 1023 entities
PERIODIC TABLE
Page 4 of 6
Name………………………………….……….… Student ID ……………………….. TG ………….
1
A
B
C
D
26
A
B
C
D
2
A
B
C
D
27
A
B
C
D
3
A
B
C
D
28
A
B
C
D
4
A
B
C
D
29
A
B
C
D
5
A
B
C
D
30
A
B
C
D
6
A
B
C
D
31
A
B
C
D
7
A
B
C
D
32
A
B
C
D
8
A
B
C
D
33
A
B
C
D
9
A
B
C
D
34
A
B
C
D
10
A
B
C
D
35
A
B
C
D
11
A
B
C
D
36
A
B
C
D
12
A
B
C
D
37
A
B
C
D
13
A
B
C
D
38
A
B
C
D
14
A
B
C
D
39
A
B
C
D
15
A
B
C
D
40
A
B
C
D
16
A
B
C
D
41
A
B
C
D
17
A
B
C
D
42
A
B
C
D
18
A
B
C
D
43
A
B
C
D
19
A
B
C
D
44
A
B
C
D
20
A
B
C
D
45
A
B
C
D
21
A
B
C
D
46
A
B
C
D
22
A
B
C
D
47
A
B
C
D
23
A
B
C
D
48
A
B
C
D
24
A
B
C
D
49
50
A
A
B
B
C
C
D
D
25
A
B
C
D
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