Chem 1010 Name__________________________________Unit 4-5 Tes.docx

Chem 1010 Name__________________________________
Unit 4-5 Test
MULTIPLE CHOICE. Choose the one alternative that best
completes the statement or answers the question.
1) When the following equation is balanced, the coefficient of
Al is __________.
Al (s) + H2O (l) → Al(OH)3 (s) + H2 (g)
A) 4
B) 1
C) 3
D) 5
E) 2
NaOH is __________.
H3PO4 (aq) + NaOH (aq) → Na3PO4 (aq) + H2O (l)
A) 1
B) 4
C) 2
D) 0
E) 3
O2 is __________.
C2H4O (g) + O2 (g) → CO2 (g) + H2O (g)

A) 5
B) 3
C) 4
D) 2
E) 1
C3H8O3 is __________.
C3H8O3 (g) + O2 (g) → CO2 (g) + H2O (g)
A) 2
B) 5
C) 7
D) 1
E) 3
1
5) Write a balanced equation to show the reaction of aqueous
aluminum acetate with aqueous ammonium
phosphate to form solid aluminum phosphate and aqueous
ammonium acetate.
A) Al(C2H3O2)2(aq) + (NH4)2PO4(aq) → AlPO4(s) + 2
NH4C2H3O2(aq)
B) Al(CO2)3(aq) + (NH4)3PO3(aq) → AlPO3(s) + 3
NH4CO2(aq)
C) Al(C2H3O2)2(aq) + (NH3)2PO4(aq) → AlPO4(s) + 2
NH3C2H3O2(aq)
D) Al(C2H3O2)3(aq) + (NH4)3PO4(aq) → AlPO4(s) + 3
NH4C2H3O2(aq)
E) Al(CO3)2(aq) + (NH3)2PO4(aq) → AlPO4(s) + 2
NH3CO3(aq)

6) When the reaction shown is correctly balanced, the
coefficients are:
C6H6 (l) + O2 (g) → CO2 (g) + H2O (g)
A) 1, 3.5, 6, 7
B) 2, 16.5, 12, 7
C) 2, 15, 12, 6
D) 1, 9.5, 6, 7
E) 1, 6, 6, 7
7) The balanced reaction between aqueous nitric acid and
aqueous strontium hydroxide is ________.
A) 2HNO3 (aq) + Sr(OH)2 (aq) → 2H2O (l) + Sr(NO3)2
(aq)
B) 2HNO3 (aq) + Sr(OH)2 (aq) → Sr(NO3)2(aq) + 2H2 (g)
C) HNO3 (aq) + Sr(OH)2 (aq) → H2O (l) + Sr(NO3)2 (aq)
D) HNO3 (aq) + Sr(OH)2 (aq) → Sr(NO3)2 (aq) + H2 (g)
E) HNO3 (aq) + SrOH (aq) → H2O (l) + SrNO3 (aq)
8) What are the spectator ions in the reaction between Mg(OH)2
(aq) and HCl (aq)?
A) H+ and OH-
B) Mg2+ and H+
C) H+ and Cl-
D) OH- only
E) Mg2+ and Cl-
9) When aqueous solutions of AgNO3 and KI are mixed, AgI
precipitates. The balanced net ionic equation is
________.
A) Ag+ (aq) + NO3- (aq) → AgNO3 (aq)
B) Ag+ (aq) + I- (aq) → AgI (s)
C) AgNO3 (aq) + KI (aq) → AgI (s) + KNO3 (aq)

D) AgNO3 (aq) + KI (aq) → AgI (aq) + KNO3 (s)
E) Ag+ (aq) + NO3- (aq) → AgNO3 (s)
10) A neutralization reaction between an acid and a metal
hydroxide produces ________.
A) oxygen gas
B) sodium hydroxide
C) ammonia
D) water and a salt
E) hydrogen gas
2
11) When H2SO4 is neutralized by NaOH in aqueous solution,
the net ionic equation is ________.
A) SO42- (aq) + 2Na+ (aq) → Na2SO4 (s)
B) 2H+ (aq) + 2NaOH (aq) → 2H2O (l) + 2Na+ (aq)
C) SO42- (aq) + 2Na+ (aq) → Na2SO4 (aq)
D) H2SO4 (aq) + 2OH- (aq) → 2H2O (l) + SO42- (aq)
E) H+ (aq) + OH- (aq) → H2O (l)
12) Which of the following is an oxidation-reduction reaction?
A) Pb(C2H3O2)2(aq) + 2 NaCl(aq) → PbCl2(s) + 2
NaC2H3O2(aq)
B) HCl(aq) + LiOH(aq) → LiCl(aq) + H2O(l)
C) Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g)
D) NaI(aq) + AgNO3(aq) → AgI(s) + NaNO3(aq)
E) All of the above are oxidation-reduction reactions.
13) What reactant (if any) is gaining electrons in the following
reaction?

Zn(s) + 2 AgNO3(aq) → Zn(NO3)2(aq) + 2 Ag(s)
A) N
B) Ag
C) Zn
D) O
E) There is no transfer of electrons in this reaction.
14) What reactabt (if any) is losing electrons in the following
reaction?
Zn(s) + 2 AgNO3(aq) → Zn(NO3)2(aq) + 2 Ag(s)
A) O
B) N
C) Ag
D) Zn
E) There is no transfer of electrons in this reaction.
15) A compound that is composed of only carbon and hydrogen
contains 80.0% C and 20.0% H by mass. What is
the empirical formula of the compound?
A) C7H20
B) C20H60
C) CH4
D) C2H6
E) CH3
3
16) What is the empirical formula of a compound that contains
27.0% S, 13.4% O, and 59.6% Cl by mass?
A) SO2Cl

B) SOCl
C) S2OCl
D) ClSO4
E) SOCl2
17) An oxide of aluminum contains 0.545 g of Al and 0.485 g of
O. Find the empirical formula for the oxide.
A) Al2O3
B) Al3O2
C) AlO
D) Al6O2
18) A compound that is composed of carbon, hydrogen, and
oxygen contains 70.6% C, 5.9% H, and 23.5% O by
mass. The molecular weight of the compound is 136 amu. What
is the molecular formula?
A) C8H4O
B) C8H8O2
C) C9H12O
D) C5H6O2
E) C4H4O
19) A compound contains 40.0% C, 6.71% H, and 53.29% O by
mass. The molecular weight of the compound is
90.09 amu. The molecular formula of this compound is
________.
A) CHO2
B) C2H4O2
C) C3H6O3
D) C2H3O4
E) CH2O
20) A certain metal sulfide, MS2, is determined to be 40.064%
sulfur by mass. What is the identity of the metal
M?
A) Molybdenum

B) Tungsten
C) Chromium
D) Iron
E) Cobalt
21) Which of the following statements about gases is false?
A) Gas mixtures are homogeneous.
B) All gases are colorless and odorless at room temperature.
C) Distances between molecules of gas are very large compared
to bond distances within molecules.
D) Gases expand spontaneously to fill the container they are
placed in.
E) Gases are highly compressible.
4
22) Gaseous mixtures ________.
A) are all heterogeneous
B) are all homogeneous
C) can only contain molecules
D) can only contain isolated atoms
E) must contain both isolated atoms and molecules
23) When the pressure is 1.00 atm, he volume of an ideal gas is
22.4L at ________.
A) -273 K
B) -45 °F
C) -273 °C
D) 0 °C
E) -363 K
24) A sample 0.100 moles of a gas is collected at at STP. What
is the volume of the gas in liters?
A) 2.24 L

B) 0.205 L
C) 22.4 L
D) 2.44 L
E) 0.0205 L
25) A sample a gas is collected is maintained at a temperature
of 25°C and has a volume of 1.30 L at 0.987 atm of
pressure. How many moles of gas are present in the sample?
A) 0..981 moles
B) 0.205 L
C) 0.00209 moles
D) 0.0525 moles
E) 0..469 moles
26) A sample of a gas (5.0 mol) at 1.0 atm is expanded at
constant temperature from 10 L to 15 L. The final
pressure is ________ atm.
A) 0.67
B) 1.5
C) 3.3
D) 15
E) 7.5
27) A sample of a gas originally at 25 °C and 1.00 atm pressure
in a 2.5 L container is subject to a pressure of 0.85
atm and a temperature of 15 °C. The final volume of the gas is
________ L.
A) 0.38
B) 3.0
C) 2.8
D) 2.6
E) 2.1
5

28) A 0.250. L sample of gas at 1.00 atm and 20.0°C has the
temperature increased to 40.0°C and the volume
increased to 0.500 L. What is the new pressure?
A) 2.14 atm
B) 0.374 atm
C) 0.468 atm
D) 1.87 atm
E) 0.534 atm
29) What volume of carbon dioxide gas in liters is produced at
STP by the decomposition of 0.150 g CaCO3 via
the equation:
CaCO3 (s) → CaO (s) + CO2 (g)
A) 2.24 L
B) 6.31 L
C) 0.0196 L
D) 0.0336 L
E) 1.31 L
30) What quantity of sodium azide in grams is required to fill a
56.0 liters air bag with nitrogen gas at 1.00 atm
and exactly 0 °C :
2 NaN3 (s) → 2Na (s) + 3N2 (g)
A) 12.3 g
B) 6.31 g
C) 108 g
D) 162 g
E) 25.2 g
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Ryan Holcomb
R = 0.08206 L•atm/mol•K
Soluble Ionic Compounds (aq) Insoluble Ionic Compounds (s)
Contain these ions: Exceptions: Contain these ions Exceptions
Cations: Anions:
Group I Cations
and ammonia
Li+
Na+
K+
Rb+
Cs+
NH4+
Compounds with Group

I and ammonia cations
are always soluble
CO32-
CrO42-
PO43-
S2-
compounds with Group
1 cations and NH4+
Anions: OH- compounds with Group 1 cations, NH4+
C2H3O2-
HCO3-
NO3-
ClO3-
Compounds with these
anions are always
soluble
Cl-
Br-
I-
compounds with Ag+,
Hg22+, and Pb2+
F-
compounds with Group
II metal cations (Be2+,
Mg2+, Ca2+, Sr2+, Ba2+) as
well as Pb2+ and Fe3+

SO42-
compounds with Ag+,
Ba2+, Ca2+, Hg22+,
Pb2+ and Sr2+
Sheet1Question #ABCDENameClassCHEM 1010-301-
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Chem 1010 Name__________________________________Unit 4-5 Tes.docx