1. On average, a sample of human blood whose dimensions are 0.1
mm × 0.1 mm × 0.1 mm contains 6.0 × 103 red blood cells. The
volume of blood in a typical adult is about 5 L. How many red blood
cells are there in an adult?
A. 3 x 1013 red blood cells
B. 5 x 107 red blood cells
C. 6 x 109 red blood cells
D. 3 x 1011 red blood cells
E. None of the above
2. A substance that can’t be chemically broken down into simpler
substances is considered
A. a homogeneous mixture
B. a pure substance
C. a heterogeneous mixture
D. a compound
E. an element
3. The mass unit most commonly used for precious stones is the
carat. 1 carat = 3.168 grains, and 1 gram = 15.4 grains. Find the total
mass in kilograms (kg) (with the correct number of significant figures)
of a 2.0 carat diamond.
A. 0.41 kg
B. 9.7 kg
C. 4×10–4 kg
D. 4.1×10–4 kg
E. 9.7×10–3 kg
4. If 0.467 moles of a substance has a mass of 63.9 g, what is the
molar mass of the substance in g/mol?
A. 0.00731 g/mol
B. 13.7 g/mol
C. 137 g/mol
D. 210 g/mol
E. none of the above
5. Which sample contains the largest number of moles of molecules?
A. 1.0 g ethanol (C2H6O)
B. 1.0 g diethyl ether (C2H6O)
C. 1.0 g methane (CH4)
D. 1.0 g hydrogen cyanide (HCN)
E. 1.0 g water (H2O)
1
6. An atom of thallium has about 10 times the mass of a neon atom. A
comparison of 1000g samples of each element reveals the following:
A. the number of thallium atoms and neon atoms is the same
B. there are 1000 times as many neon atoms as thallium atoms
C. there are ten times as many neon atoms as thallium atoms
D. there are ten times as many thallium atoms as neon atoms
E. none of the above
7. In the
52
24
Cr isotope of chromium there are:
A. 52 protons, 52 electrons, 52 neutrons
B. 24 protons, 24 electrons, 52 neutrons
C. 24 protons, 52 electrons, 24 neutrons
D. 24 protons, 24 electrons, 28 neutrons
E. 52 protons, 52 electrons, 28 neutrons
8. For 0.5 mol H2O, 23 g Na and 6.02 × 1023 N2 molecules, arrange in
order of increasing number of atoms in each sample (starting with a
sample containing the smallest number of atoms). For each sample
count all atoms, even if they belong to different elements.
A. H2O, Na, N2
B. H2O, N2, Na
C. Na, N2, H2O
D. Na, H2O, N2
E. N2, H2O, Na
9. Gallium is a Group 13 (3A) element and sulfur is a Group 16 (6A)
element. The expected formula for the ionic compound gallium sulfide
is
A) Ga2S3
B) GaS3
C) Ge3S2
D) GaS
E) None of the above
2
10. What is the approximate percentage by mass of sulfur in calcium
sulfite (CaSO3)?
A. 32.1 %
B. 26.7 %
C. 23.6 %
D. 20.0 %
E. None of the above
11. The correct name for the compound N2O4 is:
A. dinitrogen tetroxide
B. nitrogen oxide
C. nitric oxide
D. nitrous tetroxide
E. None of the above
12. The balanced equation for the reaction of gaseous ammonia with
oxygen gas to yield nitrogen oxide and water is:
A. 2 NH3(g) + 5O2(g) → 2NO(g) + 6 H2O(g)
B. 4 NH3(g) + 3O2(g) → 4NO(g) + 6 H2O(g)
C. 6 NH3(g) + 5O2(g) → 6NO(g) + 6 H2O(g)
D. 4 NH3(g) + 5O2(g) → 4NO(g) + 6 H2O(g)
E. None of the above
13. How many significant figures are contained in the number
0.002306 mg?
A. 3
B. 4
C. 5
D. 6
E. None of the above
14. Combustion of 63.8 mg of a C, H, and O containing compound
produces 145.0 mg of CO2 and 59.38 mg of H2O. What is the
empirical formula of the compound?
A.
B.
C.
D.
E.
C5H2O
CHO
C2HO
C3H6O
None of the above
3
15. The name of the compound CoCl2⋅ 6H2O is:
A. cobalt (II) chloride hexahydrate
B. cobalt (I) chloride heptahydrate
C. cobalt chloride heptahydrate
D. cobalt (II) chlorohydrate
E. None of the above
16. Which of the following does not represent a redox reaction?
A. 2H2(g) + O2(g) → H2O(g)
B. H2SO4(aq) + Cu(s) → CuSO4(aq) + H2(g)
C. H2SO4(aq) + CO32– (aq) → H2CO3(aq) + SO42– (aq)
D. Fe(s) + O2(g) → FeO2(s)
E. All of the above are redox reactions
17. Calculate the atomic mass of element "X", if it has 2 naturally
occurring isotopes with the following masses and natural abundances:
X-45 44.8776 amu
32.88%
X-47 46.9443 amu
67.12%
A.
B.
C.
D.
E.
46.34 amu
46.27 amu
46.84 amu
45.91 amu
44.99 amu
18. How many moles of Ag are produced in the decomposition of 100
g of silver (I) oxide:
2 Ag2O (s)
A.
B.
C.
D.
E.
→
4 Ag (s) + O2 (g)
(balanced)
1.73 moles
3.46 moles
0.432 moles
17.3 moles
none of the above
4
19. What is the volume of an aluminum block (density = 2.85 g/cm3)
that yields 1.5 moles of H2 (g) when reacted with excess hydrochloric
acid.
2 Al (s) + 6 HCl (aq)
(balanced)
A.
B.
C.
D.
E.
→
2 AlCl3 (aq) + 3 H2(g)
9.47 cm3
94.7 cm3
14.2 cm3
142 cm3
18.8 cm3
20. Calculate the percent yield for the following reaction given that
15.0 g C4H9OH reacts with excess NaBr and H2SO4 to yield 17.1 g
C4H9Br, as follows:
C4H9OH + NaBr + H2SO4 → C4H9Br + H2O + NaHSO4
(balanced)
A. 61.7 %
B. 30.8 %
C. 15.4 %
D. 62.7 %
E. 60.7 %
21. Given the reaction given below, calculate the mass required of
sodium sulfide (Na2S(s)) required to react completely with 27.8 mL of
0.163 M AgNO3.
AgNO3(aq) + Na2S(s) → Ag2S(s) + NaNO3(aq)
(unbalanced)
A. 0.708 g
B. 0.0884 g
C. 0.354 g
D. 0.177 g
E. none of the above are correct
5
22. Which of the following chemical reactions will yield a precipitate?
i) NaOH (aq) + MgCl2 (aq) → ?
ii) BaS (aq) + CuSO4 (aq) → ?
iii) (NH4)2SO4(aq) + ZnCl2(aq) → ?
A. i) and iii)
B. ii) and iii)
C. i) and ii)
D. iii)
E. none of the above
23. Which compounds in the following two redox reactions serve as
the oxidizing agent:
N2H4 + H2 → 2 NH3
Fe2O3 + 3 CO → 2 Fe + 3CO2
A. N2H4 only
B. N2H4 and CO
C. N2H4 and Fe2O3
D. H2 and Fe2O3
E. H2 and N2H4
24. Arrange the following nitrogen containing molecules in terms of
increasing oxidation state (lowest to highest): i) NO, ii) N2, iii) NO3–,
and iv) N2O4?
A.
B.
C.
D.
E.
ii), i), iii), iv)
ii), i), iv), iii)
i), ii), iii), iv)
iv), iii), i), ii)
none of the above are correct
25. A 0.5043-g sample of potassium hydrogen phthalate (KHC8H4O4)
is dissolved in water and titrated with KOH(aq). What is the molarity
of the KOH solution, if 20.54 mL of this solution are needed to reach
the equivalence (end) point?
Molar mass of KHC8H4O4 equals to 204.22 g/mol. The titration
reaction is:
KHC8H4O4(aq) + KOH(aq) → K2C8H4O4(aq) + H2O(l)
A. 0.2404 M
B. 0.1202 M
C. 0.0601 M
D. 1.202×10–4 M
E. none of the above
6
26. How many of the following compounds are soluble in water?
Cu(OH)2, LiNO3, NH4Br and K2S
A. 0
B. 1
C. 2
D. 3
E. 4
27. Give the complete ionic equation for the reaction (if any) that
occurs when aqueous solutions of lithium sulphide, and copper (II)
nitrate are mixed.
A. Li+(aq) + S–(aq) + Cu+(aq) + NO3–(aq) → CuS(s) + LiNO3(aq)
B. 2Li+(aq) + S2– (aq) + Cu2+(aq) + 2NO3–(aq) → Cu2+(aq) + S2–(aq) +
2LiNO3(s)
C. 2Li+(aq) + S2–(aq) + Cu2+(aq) + 2 NO3–(aq) → CuS(s) + 2Li+(aq) +
2NO3– (aq)
D. LiS(s) + Cu+(aq) + NO3–(aq) → CuS(s) + Li+(aq) + NO3–(aq)
E. No reaction occurs.
28. Identify the spectator ions in the following molecular equation.
KBr(aq) + AgNO3(aq) → AgBr(s) + KNO3(aq)
A. K+ & NO3–
B. Ag+ & NO3–
C. Ag+ & Br–
D. K+ & Br–
E. There are no spectator ions in this reaction.
29. Which of the following is an acid base reaction?
A. 2 HClO4(aq) + Ca(OH)2(aq) → 2 H2O(l) + Ca(ClO4)2(aq)
B. C(s) + O2(g) → CO2(g)
C. Fe(s) + 2 AgNO3(aq) → 2 Ag(s) + Fe(NO3)2(aq)
D. MgSO4(aq) + Ba(NO3)2(aq) → Mg(NO3)2(aq) + BaSO4(s)
E. None of the above is an acid base reaction.
7
30. Which of the following reactants will produce CO2 gas when mixed
together at room temperature?
A. C(s) and KOH(aq)
B. K2CO3(aq) and KMnO4(aq)
C. CH3OH(l) and H2O(l)
D. K2CO3(aq) and KOH(aq)
E. NaHCO3(aq) and HCl(aq)
31. Which of the following solutions will have the highest
concentration of chloride ions?
A.
B.
C.
D.
E.
0.10 M AlCl3
0.10 M NaCl
0.10 M MgCl2
0.05 M CaCl2
All of these solutions have the same concentration of chloride ions.
32. What is the concentration of hydroxide ions in pure water at
30.0°C, if Kw at this temperature is 1.47 × 10–14?
A.
B.
C.
D.
E.
1.30 × 10–7 M
1.21 × 10–7 M
1.00 × 10–7 M
1.47 × 10–7 M
8.93 × 10–8 M
33. Which of the following is a STRONG acid?
A. H2O
B. C6H5CO2H
C. HClO4
D. NH4+
E. HCN
34. Which of the following is TRUE?
A. An acidic solution has [H3O+] > [OH–]
B. A basic solution does not contain H3O+
C. A neutral solution does not contain any H3O+ or OH–
D. A neutral solution contains [H2O] = [H3O+]
E. None of the above is true.
8
35. Calculate the pH of a solution that contains 7.8 ×10–6 M OH– at
25°C.
A. 1.28
B. 8.89
C. 5.11
D. 9.64
E. 12.72
36. Determine the pH of a 0.00598 M HCl solution.
A. 3.558
B. 1.777
C. 6.434
D. 7.566
E. 2.223
37. What is the density of oxygen, O2, at 100oC and 1.15 atm?
A. 0.601 g/L
B. 22.4 g/L
C. 0.0772 g/L
D. 3.1 g/L
E. none of the above
38. If the pressure of a sample of a gas with a constant number of
moles is tripled and the absolute temperature is halved, by what
factor does the volume change?
A. 8
B. 2
C. 1/2
D. 1/6
E. 1/8
39. What is the molar mass of Freon-11 gas if its density is 6.13 g/L at
STP?
A. 0.274 g/mol
B. 3.64 g/mol
C. 78.2 g/mol
D. 137 g/mol
E. 365 g/mol
9
40. The number of H2 molecules in 2.5 L of hydrogen gas at 37oC and
735 torr pressure is:
A. 4.3 × 1025
B. 5.7 × 1022
C. 3.6 × 1026
D. 4.7 × 1023
E. 7.2 × 1024
10