Exam 2 Sample
1.
Which is the correct formula for copper(II) phosphate?
A.
B.
C.
D.
E.
2.
Cu2PO4
Cu3(PO4 )2
Cu2PO3
Cu(PO4 )2
Cu(PO3 )2
How many grams of sulfur are there in 6.0 g of Fe2(SO4)3?
A. 2.40 g
3.
D. 0.92 g
E. 1.44 g
B. -4
C. +2
D. -2
E. 0
The oxidation number of N in NaNO3 is
A.
B.
C.
D.
E.
5.
C. 6.00 g
The oxidation number of N in N2H4 is
A. +4
4.
B. 0.48 g
+6
+5
+3
-3
None of the above.
What is the theoretical yield of vanadium that can be produced by the reaction of 40.0 g of
V2O5 with 40.0 g of calcium based on the following chemical reaction?
V2O5(s) + 5Ca(l) 2V(l) + 5CaO(s)
A. 11.2 g
6.
B. 20.3 g
C. 22.4 g
D. 40.0 g
E. 5.6 g
Calculate the mass of excess reagent remaining at the end of the reaction in which 90.0 g of
SO2 are mixed with 100.0 g of O2.
2SO2 + O2 2SO3
A. 11.5 g
7.
B. 22.5 g
C. 67.5 g
D. 77.5 g
E. 400 g
Identify the reducing agent in the following chemical reaction.
5Fe2+(aq) + MnO4– + 8H+(aq) 5Fe3+(aq) + Mn2+(aq) + 4H2O(l)
A. Fe2+
B. MnO4–
C. H+
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D. Mn2+
E. Fe3+
8.
Calculate the mass of FeS formed when 9.42 g of Fe reacts with 8.50 g of S.
Fe(s) + S(s) FeS(s)
A.
B.
C.
D.
E.
9.
Which of the following samples contains the greatest number of atoms?
A.
B.
C.
D.
E.
10.
17.9 g
87.9 g
26.0 g
14.8 g
1.91 × 10-3 g
100 g of Pb
2.0 mole of Ar
0.1 mole of Fe
5 g of He
20 million O2 molecules
Hydrochloric acid can be prepared by the following reaction:
2NaCl(s) + H2SO4(aq) 2HCl(g) + Na2SO4(s)
How many grams of HCl can be prepared from 2.00 mol H2SO4 and 150 g NaCl?
A. 7.30 g
11.
D. 150 g
E. 196 g
P and Br
Cu and K
C and O
O and Zn
Al and Rb
What is the average mass, in grams, of one atom of iron?
A.
B.
C.
D.
E.
13.
C. 146 g
Which of the following pairs of elements would be most likely to form an ionic compound?
A.
B.
C.
D.
E.
12.
B. 93.5 g
6.02 × 1023 g
1.66 × 10–24 g
9.28 × 10–23 g
55.85 g
55.85 × 10-23 g
Which of the following is the correct net ionic equation for the reaction that occurs when
solutions of Pb(NO3)2 and NH4Cl are mixed?
A. Pb(NO3)2(aq) + 2NH4Cl(aq) NH4NO3(aq) + PbCl2(s)
B. Pb2+ + 2Cl– PbCl2(s)
C.
Pb 2+ (aq)  2NO3  (aq)  2NH 4 (aq)  2Cl - (aq)  2NH +4 (aq)  2NO3  (aq)  PbCl 2 (s)
D. NH4+(aq) + NO3– (aq) 2NH4NO3 2NH4NO3(s)
E. No reaction occurs when the solutions are mixed.
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14.
What element is oxidized in the following chemical reaction?
3Cu + 8HNO3 Cu(NO3)2 + 2NO + 4H2O
A. Cu
15.
B. H
C. N
D. O
E. H2O
Complete and balance the following redox equation. When properly balanced with whole
number coefficients, the coefficient of S is
H2S + HNO3 S + NO (acidic solution)
A. 1
16.
B. 2
C. 3
D. 5
E. 6
Identify the oxidizing agent in the following chemical reaction.
2MnO4– + 5H2SO3 2Mn2+ + 5SO42– + 4H+ + 3H2O
A. MnO4–
17.
D. SO42–
E. H+
ZnCl2 will precipitate; Mg2 and SO42– will be spectator ions.
ZnSO4 will precipitate; Mg2+ and Cl– will be spectator ions.
MgSO4 will precipitate; Zn2+ and Cl– will be spectator ions.
MgCl2 will precipitate; Zn2+ and SO42– will be spectator ions.
No precipitate will form.
The chemical name for ClO3– is chlorate ion. Therefore, the name of HClO3 is
A.
B.
C.
D.
E.
19.
C. Mn2+
Based on the solubility rules, which of the following will occur when solutions of
ZnSO4(aq) and MgCl2(aq) are mixed?
A.
B.
C.
D.
E.
18.
B. H2SO3
hydrochloric acid
chloroform
hydrogen trioxychloride
chlorous acid
chloric acid
How many sodium atoms are there in 6.0 g of Na3N?
A.
B.
C.
D.
E.
3.6 × 1024 atoms
4.6 × 1022 atoms
1.3 × 1023 atoms
0.217 atoms
0.072 atoms
Page 3
20.
Vanadium (V) oxide reacts with calcium according to the chemical equation below. When
10.0 mole of V2O5 are mixed with 10.0 mole of Ca, which is the limiting reagent?
V2O5(s) + 5Ca(l)  2V(l) + 5CaO(s)
A.
B.
C.
D.
E.
21.
V2O5
Ca
V
CaO
Neither reagent is limiting.
Balance the following equation, then add together the coefficients. Don't forget to count
coefficients of one. The sum of the coefficients is
___ Al + ___ H2SO4 ___ Al2(SO4)3 + ___ H2
A.
B.
C.
D.
E.
22.
3.
5.
6.
9.
12.
The percent composition by mass of a compound is 76.0% C, 12.8% H, and 11.2% O. The
molar mass of this compound is 284.5 g/mol. What is the molecular formula of the
compound?
A. C10H6O
23.
C. C16H28O4
D. C20H12O2
E. C18H36O2
D. +2
E. -4
The highest possible oxidation number of carbon is
A. +8
24.
B. C9H18O
B. +6
C. +4
Complete and balance the following redox equation. What is the coefficient of H2S when
the equation is balanced with the set of smallest whole numbers?
H2S + MnO4– Mn2+ + SO42– (acidic solution)
A.
B.
C.
D.
E.
25.
1
2
4
5
None of the above.
Which choice gives the correct oxidation numbers for all three elements in Rb2SO3 in the
order that the elements are shown in the formula?
A. -2, +6, -2
B. -1, +4, -3
C. +2, +4, -2
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D. +1, +4, -2
E. +1, +6, -6
26.
When a chemical equation is balanced, it will have a set of whole number coefficients that
cannot be reduced to smaller whole numbers. What is the coefficient for O2 when the
following combustion reaction of a hydrocarbon is balanced?
___ C7H14 + ___ O2 ___ CO2 + ___ H2O
A.
B.
C.
D.
E.
27.
42
21
11
10
none of these
If 0.274 moles of a substance weighs 62.5 g, what is the molar mass of the substance, in
units of g/mol?
A.
B.
C.
D.
E.
2.28 × 102 g/mol
1.71 × 101 g/mol
4.38 × 10-3 g/mol
2.17 × 102 g/mol
none of these
Page 5
Answer Key for Test "Exam2_Sample.tst", 10/20/2003
No. in
Q-Bank
2-25
3-37
4-39
4-29
3-78
3-69
4-46
3-67
3-16
3-66
2-19
3-3
4-20
4-48
4-54
4-45
4-19
2-26
3-27
3-72
3-61
3-49
4-37
4-57
4-40
3-54
3-9
No. on
Test
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
19
20
21
22
23
24
25
26
27
Correct
Answer
B
E
D
B
B
D
A
D
B
B
D
C
B
A
C
A
E
E
C
B
D
E
C
D
D
B
A
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