Chemistry
Raymond Chang
10th edition
Chapter 3
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Question 1
A mole of carbon (molar mass about 12)
contains fewer atoms than a mole of oxygen
(molar mass about 16).
A) True
B) False
50%
50%
1
2
Question 2
One atom of oxygen weighs about 16 g.
A) True
B) False
50%
50%
1
2
Question 3
One atom of carbon weighs about 12 amu.
A) True
B) False
50%
50%
1
2
Question 4
One mole of carbon weighs about 12 g.
A) True
B) False
50%
50%
1
2
Question 5
If the ratio of moles of carbon to hydrogen
in a hydrocarbon compound is found by
experiment to be 1.5002:3.0005 then the
most likely empirical formula is
25%
25%
25%
2
3
25%
A) C2H3.
B) C15H30.
C) C2H6.
D) CH2.
1
4
Question 6
If 1.00 g of a compound composed of
hydrogen and oxygen is found to contain
0.94 g oxygen, then which of the following
molecular formulas is likely? 25% 25% 25%
A) H2O
B) H2O2
C) HO2
D) None of the above
1
2
3
25%
4
Question 7
Which of the following chemical equations
represents the decomposition of solid
calcium carbonate to yield oxygen gas and
25%
25%
25%
solid calcium oxide?
25%
A) CaCO2(s) → CaO(s) + O2(g)
B) CaCO3(s) → CaO(s) + O2(l)
C) CaCO3(s) → CaO(s) + O(g)
D) CaCO3(s) → CaO(s) + O2(g)
1
2
3
4
Question 8
How many moles of Zn would be
required to produce 4 moles of hydrogen
gas using the following reaction?
Zn(s) + 2HCl(aq) → ZnCl2(aq) +H2(g)
25%
25%
25%
2
3
25%
A) 8 mol
B) 4 mol
C) 2 mol
D) 1 mol
1
4
Question 9
How many moles of Zn would be required
to completely react with 1 mole of HCl
using the following reaction?
Zn(s) + 2HCl(aq) → ZnCl2(aq) +2H2(g)
25%
A)
B)
C)
D)
25%
25%
2
3
25%
0.5 mol
1 mol
2 mol
4 mol
1
4
Question 10
How much zinc chloride could be made
from one mole of Zn and 1 mole of HCl if
the reaction is?
Zn(s) + 2HCl(aq) → ZnCl2(aq) +H2(g)
25%
25%
25%
2
3
25%
A) 1 mol
B) 2 mol
C) 0.5 mol
D) 0 mol since the
molar ratio is
incorrect
1
4
Question 11
Avogadro's number represents
20%
A) the number of particles in a mole.
B) the ratio between 1 g and 1 amu.
C) the ratio between the molar mass of
NaCl and the molecular mass of NaCl.
D) the ratio between the molar mass of Cu
and the average atomic mass of Cu.
E) all of the above.
1
20%
20%
2
3
20%
4
20%
5
Question 12
Which of the following statements is/are
true?
20%
20%
20%
20%
A) 1.000 mol sodium weighs
22.99 g
B) 1.000 mol sodium chloride
contains 1.2044x1024 ions
C) 1.0 mol of aluminum
chloride contains twice as
many ions as 1.0 mol of
sodium chloride
D) All of the above
E) None of the above
1
2
3
4
20%
5
Question 13
What is the mass of 1.0 kmol of water?
20%
20%
20%
2
3
20%
20%
A) 18 g
B) 18 amu
C) 18 kg
D) 1000 amu
E) None of the above
1
4
5
Question 14
The mass % of manganese in potassium
20%
20%
20%
20%
permanganate is
20%
A) 24.75 %.
B) 34.77 %.
C) 40.51 %.
D) 27.87 %.
E) None of the above.
1
2
3
4
5
Question 15
The empirical formula of mercurous chloride is
20%
20%
20%
2
3
20%
20%
A) Hg2Cl2.
B) HgCl.
C) HgCl2.
D) Hg2Cl.
E) (HgCl)n.
1
4
5
Question 16
The mass percent composition of an
oxoacid of sulfur is : 1.75 % H, 56.14 % S,
42.11 % O. Determine the empirical formula
20%
20%
20%
20%
20%
of the acid.
A) H2SO4
B) H2SO3
C) H2S2O3
D) H2SO5
E) HSO1.5
1
2
3
4
5
Question 17
The chemical equation (NH4)2Cr2O7 →
Cr2O3 + N2 + 4H2O tells us the following:
20%
20%
20%
2
3
20%
20%
A) From 1 mol of (NH4)2Cr2O7 we
get 1 mol of Cr2O3
B) From 1 mol of (NH4)2Cr2O7 we
get 1 mol of N2
C) From 1 mol of (NH4)2Cr2O7 we
get 4 mol of H2O
D) All of the above
E) None of the above
1
4
5
Question 18
A balanced chemical equation tells us:
20%
20%
20%
2
3
20%
20%
A) The ratios of moles of reactants that
participate in the reaction.
B) The ratios of moles of products that are
formed in the reaction.
C) That we can calculate the amount of a
reactant needed based on how much of a
specific product we need.
D) That we can calculate the amount of
product formed based on the amount of one
reactant and excess of other reactants.
E) All of the above.
1
4
5
Question 19
Given the reaction: SO3(g) + H2O(g) →
H2SO4(l), calculate the amount of sulfur
trioxide necessary to produce 196 kg
sulfuric acid assuming 100% yield.
20%
20%
20%
2
3
20%
20%
A) 80 kg
B) 80 g
C) 160 g
D) 160 kg
E) None of the above
1
4
5
Question 20
Given the reaction: SO3(g) + H2O(g) →
H2SO4(l), which proceeds with a yield of
85.0%, calculate the amount of sulfuric acid
that is formed when 120. kg sulfur trioxide is
20%
20%
20%
20%
20%
mixed with 32.4 kg water.
A) 147 kg
B) 125 kg
C) 176 kg
D) 150 kg
E) None of the above
1
2
3
4
5
Answer Key – Chapter 3
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
B
B
A
A
D
B
D
C
A
C
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
E
D
C
B
B
C
D
E
D
B