Name_________________________________________
Block__________
1
Practice Final Exam
Each question is worth 1 point. You will get 1 point for every question answered correctly and 0
points for every question answered incorrectly or left blank. It is to your advantage to answer
every question.
_____6. Which can be used most accurately
_____1. Which is an example of a chemical
to measure the volume of a liquid?
change?
a. beaker
a. rusting iron
b. crucible
b. melting wax
c. Erlenmeyer flask
c. boiling ethanol
d. graduated cylinder
d. cutting aluminum foil
_____7. In addition to a balance, which
_____2. Express the measurement of 3750
piece of glassware is best used to determine
m in correct scientific notation.
the density of zinc by displacement?
1
a. 375 x 10 m
a. graduated cylinder
b. 37.5 x 102 m
b. Erlenmeyer flask
c. 3.75 x 103 m
c. beaker
4
d. 3.750 x 10 m
d. pipet
_____3. Convert 52,045 mm to km.
a. 0.000 052 045 km
b. 0.052 045 km
c. 52.045 km
d. 52,045,000 km
_____4. For an atom, which set is correct?
a. He, 4 protons, 4 electrons
b. Zn, 30 protons, 60 electrons
c. Ca, 20 protons, 20 electrons
d. Cs, 55 protons, 132.9 electrons
_____5. What is the average atomic mass of
this element with the given isotope
abundance?
Isotopes of an Element
Mass (amu) Abundance (%)
41.98
75.06
42.98
10.74
45.98
14.18
a.
b.
c.
d.
33.33 amu
41.98 amu
42.65 amu
43.65 amu
_____8. An unidentified element is tested
and has these properties:
 a colorless gas at room
temperature
 a nonconductor of electricity
 reacts with alkali metals
 “pops” when ignited
The element is most likely
a. helium, He
b. hydrogen, H2
c. chlorine, Cl2
d. nitrogen, N2
_____9. Which atom has the smallest
radius?
a. As
b. P
c. S
d. Se
_____10. In which set do all the elements
have the same number of valence electrons?
a. P, S, Cl
b. P, As, N
c. Cu, Zn Ga
d. Na, Ca, Ba
Name_________________________________________
_____11. If the oxides of some Period 6
elements are HgO, Tl2O, PbO2, and Bi2O3,
what formula could be expected fro the
oxide of element 114, ununquadium, Uuq?
a. UuqO
b. Uuq2O
c. UuqO2
d. Uuq2O3
_____12. How are metallic substances
distinguished from other classes of chemical
substances?
a. They are brittle.
b. They have high boiling points.
c. They have high electrical
conductivity in the solid state.
d. They have high electrical
conductivity in the liquid state.
_____13. Which molecule has two
unshared pairs of electrons on the central
atom?
a. NH3
b. CO2
c. H2S
d. SiH4
_____14. Which combination of elements
would be expected to produce the most polar
covalent bond?
a. O-O
b. O-N
c. O-Cl
d. O-H
_____15.
a.
b.
c.
d.
Which compound is polar?
CO2
CH4
CCl4
CH3Cl
_____16. What is the IUPAC name for
Cu2SO3?
a. copper (I) sulfite
b. copper (I) sulfate
c. copper (II) sulfite
d. copper (II) sulfate
Block__________
2
_____17. Which compound’s name has its
correct formula?
a. barium sulfate, Ba(SO4)2
b. aluminum bromide, Al2Br3
c. ammonium nitrate, (NH4)2NO3
d. copper (II) acetate, Cu(C2H3O2)2
_____18. A compound made of nitrogen
and oxygen has a 30.4% nitrogen content by
mass. What is its empirical formula?
a. NO2
b. N2O4
c. N2O9
d. N2O2
_____19. Lysine has a molecular formula of
NH2 (CH2)4CHNH2COOH. What is the
empirical formula for lysine?
a. C2H7ON
b. C3H7ON
c. C4H14O2N2
d. C6H14O2N2
_____20. How many atoms of carbon, C,
are in a 0.200 g diamond?
a. 7.22 x 1023
b. 1.20 x 1023
c. 2.01 x 1022
d. 1.00 x 1022
_____21. Which is the mass of one mole of
(NH4)2CO3?
a. 78 g
b. 82 g
c. 96 g
d. 120 g
_____22. The empirical formula of a
compound is HCO2 and its molecular mass
is 90 g/mol. What is its molecular formula?
a. HCO2
b. H2CO3
c. H2C2O4
d. H3C3O4
Name_________________________________________
_____23. Which sample of gas at STP has
the same number of molecules as 2.0 L of
neon, Ne, at STP?
a. 2.0 L of fluorine, F2
b. 2.0 g of argon, Ar
c. 4.0 g helium, He
d. 22.4 L of hydrogen, H2
_____24. Which is the volume of 7.50 mol
argon, Ar, at STP?
a. 0.334 L
b. 7.50 L
c. 168 L
d. 300. L
_____25. _____H3PO4 + _____Ca(OH)2 
_____Ca3(PO4)2 +
?
H2O
Which is the coefficient of water, H2O, in
this equation when it is balanced using
whole number coefficients?
a. 2
b. 4 c. 6
d. 8
_____26. What is produced when zinc,
Zn(s), reacts with dilute sulfuric acid, H2SO4
(aq)?
a. H2 + ZnSO4
b. H2O + ZnSO3
c. H2O + ZnSO4
d. H2 + ZnO4 + SO2
_____27. _____NH3 (g) +
?
O2 (g) 
____ NO (g) + _____H2O(g)
Which is the coefficient of oxygen, O2, in
this equation when it is correctly balanced?
a. 3
b. 4
c. 5
d. 6
Block__________
3
_____28. This is a representation of the
reaction of hydrogen H2, with bromine, Br2,
to form hydrogen bromide, HBr.
_____29. Which is the net ionic equation
for the reaction between potassium iodide,
KI (aq) , and silver nitrate, AgNO3 (aq)?
a. K+(aq) + I-(aq)  KI (s)
b. Ag+(aq) + I-(aq)  AgI (s)
c. K+(aq) + NO3-(aq)  KNO3 (s)
d. Ag+(aq) + NO3-(aq)  AgNO3 (s)
_____30. K2CO3(s) + 2 HCl (aq) 
2 KCl (aq) + H2O (l) + CO2 (g)
What mass of potassium chloride should be
theoretically produced when 41.46 g of
potassium carbonate is reacted with excess
hydrochloric acid?
Compound
Molar Mass, g/mol
potassium chloride, KCl
74.55
potassium carbonate, K2CO3 138.2
a. 11.18 g
b. 22.37 g
c. 41.43 g
d. 44.73 g
Name_________________________________________
_____31. Al2(CO3)3(s) + 6 HCl (aq) 
2 AlCl3 (aq) + 3 H2O (l) + 3 CO2 (g)
What volume of carbon dioxide gas, CO2,
would be produced at STP if 23.40 g of
aluminum carbonate reacts with excess
hydrochloric acid?
Compound
Molar Mass, g/mol
aluminum carbonate, Al2(CO3)3
234
a. 2.24 L
b. 6.72 L
c. 22.4 L
d. 672 L
_____32.
2 Al(s) + 3 S(s)  Al2S3(s)
How many grams of aluminum sulfide can
be produced when 2.00 mol of aluminum
react with 2.00 mol of sulfur?
Compound
Molar Mass, g/mol
aluminum sulide, Al2S3
150.
a.
b.
c.
d.
2.00 g
100. g
150. g
300. g
Block__________
_____35. If the atmospheric pressure is 99
kPa and the water vapor pressure is 3.0 kPa,
then what is the pressure of the gas collected
over water?
a.
b.
c.
d.
33 kPa
96 kPa
102 kPa
297 kPa
_____36. How many moles of gas would be
found in a rigid 5.0 L cylinder at 12.0 atm of
pressure at 15°C?
a. 0.0033 mol
b. 0.064 mol
c. 2.5 mol
d. 49 mol
_____33.
2 C2H6 (g) + 7 O2 (g) 4 CO2 (g) + 6 H2O (g)
If 18.0 liters at STP of ethane gas, C2H6,
reacts with an excess of oxygen gas, O2,
how many liters of carbon dioxide, CO2, are
produced at STP?
a. 1.24 L
b. 9.00 L
c. 18.0 L
d. 36.0 L
_____34. NH3, H2S, NO2, and Cl2 each has
a distinct odor. If you were standing one
meter away when bottles of each of these
gases were opened simultaneously which
gas would you smell first?
a. NH3
b. H2S
c. NO2
d. Cl2
4
_____37. These two gas samples, at the
conditions shown, have the same
a.
b.
c.
d.
mass.
density.
average velocity.
number of molecules.
Name_________________________________________
_____38. The gas pressure in a container
will always decrease when
a. the number of molecules is
decreased and the temperature is decreased
b. the number of molecules is
decreased and the temperature is increased
c. the number of molecules is
increased and the temperature is decreased.
d. the number of molecules is
increased and the temperature is increased.
_____39. When the atmospheric pressure is
750.0 mmHg, what pressure is exerted by
the enclosed gas?
Block__________
5
_____41. Which mass of solute is required
to prepare 500. mL of 0.200 M calcium
chloride, CaCl2?
Compound
Molar Mass, g/mol
calcium chloride, CaCl2
111
a. 10.0g
b. 11.1 g
c. 22.2 g
d. 100 g
_____42. Which type of compound is
always an electrolyte?
a. soluble ionic
b. network solid
c. polar covalent
d. nonpolar covalent
_____43. A saturated solution of potassium
nitrate can be made unsaturated by
a. stirring vigorously.
b. adding more solute.
c. raising the pressure.
d. raising the temperature.
a.
b.
c.
d.
18.0 mmHg
732.0 mmHg
750.0 mmHg
768.0 mmHg
_____40. What is the solubility of KNO3 in
100 g of water at 50°C?
_____44. Which is a property common to
acids such as HCl (aq) or H2SO4 (aq)?
a. They feel slippery to the touch.
b. They have pH values above 7.0.
c. They turn litmus blue and leave
phenolphthalein colorless.
d. They react with zinc to produce
hydrogen gas.
_____45. What is the [H3O+] of a solution
whose pH is 3.32?
a. 3.32 M
b. 0.521 M
c. 4.79 x 10-4 M
d. 2.09 x 103 M
a.
b.
c.
d.
35 g
70 g
80 g
90 g
Name_________________________________________
_____46. An aqueous solution contains
hydronium ion, H3O+, at a concentration
of 2.4 x 10-6 M. What is the hydroxide ion,
OH-, concentration in this solution?
Kw = 1.0 x 10-14.
a.
b.
c.
d.
_____48. What is the pH of a solution of
0.034 M HCl(aq)?
a. -1.47
b. 0.47
c. 1.47
d. 2.54
_____49. From the given data, what is the
molarity of the HNO3 solution if the KOH
solution was 0.120 M?
Acid, HNO3
Initial volume,mL
18.3
Final volume,mL
34.7
_____50.
a.
b.
c.
d.
Base, KOH
15.4
29.2
0.101 M
0.143 M
7.01 M
9.90 M
Which compound is baking soda?
NaHCO3
H2SO4
C12H22O11
NaCl
6
_____51. Which orbital notation best
represents the ground state valence electrons
of a nitrogen family element?
2.4 x 108 M
2.4 x 10-6 M
1.0 x 10-7 M
4.2 x 10-9 M
_____47. A student tests a liquid with red
litmus paper and no color change is
observed. The student interprets the results
to mean that the solution may be water.
Which is another possible interpretation of
the results?
a. The solution may be acidic
b. The solution may be basic.
c. The solution may contain NaOH.
d. The solution may contain
ammonia.
a.
b.
c.
d.
Block__________
_____52. The melting point of gallium is
29.8°C. What is the physical state of
gallium at 250 K?
a. gas
b. solid
c. liquid
d. not enough information
_____53. A crystalline solid, which is a
nonconductor in its solid state, has a high
melting point, and is water soluble, is
classified as
a. ionic.
b. metallic.
c. molecular.
d. network covalent
_____54. In which substance are the
intermolecular attractions the greatest?
a. H2O (g)
b. Br2 (g)
c. CO2 (g)
d. I2 (g)
_____55. Which statement best describes
the change of phase from a gas to a liquid?
a.
b.
c.
d.
It is exothermic because energy is released.
It is exothermic because energy is absorbed.
It is endothermic because energy is released.
It is endothermic because energy is absorbed.
Name_________________________________________
_____56. Consider this reaction.
N2(g) + O2(g)  2 NO(g) ∆H = +180.50 kJ
What will the enthalpy change be if 15.00 g
of NO forms?
Compound
Molar Mass, g/mol
nitrogen monoxide, NO
30.0
a.
b.
c.
d.
_____60. What is the equilibrium constant
expression for this reaction?
C(s) + O2(g)  2 CO2(g)
a. Keq = [C] [O2]
[CO2]
b. Keq = [CO2] 2
[O2]
-181 kJ
-90.3 kJ
+90.3 kJ
+45.1 kJ
_____57. What is the specific heat of lead,
Pb, if the addition of 3350 J changes the
temperature of 516 g from 20.8 °C to
70.8 °C?
a. 0.130 J/g°C
b. 6.49 J/g°C
a. 67.0 J/g°C
a. 77.2 J/g°C
_____58. Which of the labeled intervals
represent an increase in kinetic energy?
a.
b.
c.
d.
Block__________
L only
M only
L and M only
M and N only
_____59.
This represents the production of HCl (g).
H2(g) + Cl2(g)  2 HCl(g)
∆H = -184 kJ
The -184 kJ is
a. absorbed during the reaction
b. the net energy change of the reaction
c. stored as potential energy of the products
d. the energy required to break H-H and ClCl bonds.
c. Keq = [CO2] 2
[C][O2]
d. Keq = [O2]
[CO2]2
_____61. A catalyst effectively increases
the rate of a reaction by decreasing the
a. activation energy.
b. heat of reaction.
c. heat of the products.
d. heat of the reactants.
_____62. Given:
N2(g) + 3 H2(g)  2 NH3(g)
Keq = 1.3 x 10-2
At equilibrium, the concentrations of
nitrogen and hydrogen are both 0.10 M.
What is the ammonia concentration?
a. 1.3 x 10-2 M
b. 0.0011 M
c. 0.050 M
d. 0.20 M
_____63. Which of these acids is the
strongest?
Acid
Formula
Ka
acetic
CH3COOH 1.8 x 10-5
formic
HCOOH
1.8 x 10-4
hydrosulfuric H2S
1.0 x 10-7
phosphoric
H3PO4
3.7 x 10-2
a.
b.
c.
d.
acetic
formic
hydrosulfuric
phosphoric
7
Name_________________________________________
_____64. In the diagram, which letter
represents the activation energy for the
reverse reaction?
Block__________
8
_____68. Given:
CO2(g) + H2(g)  CO(g) + H2O (g)
A mixture at equilibrium contains
0.552 mol CO2, 0.552 mol H2, 0.448 mol
CO, 0.448 mol H2O in a 1.00 L container.
What is the value of Keq for this reaction?
a. 0.659
b. 0.812
c. 1.23
d. 1.52
_____69. What is the oxidation number of
sulfur in sodium thiosulfate, Na2S2O3?
a. +6
b. +4
c. +2
d. -2
a. A
b. B
c. C
d. D
_____65.
Mg(s) + 2 HCl(aq  H2(g) + MgCl(aq)
How can the rate of H2(g) production be
increased in an open test tube?
a. Increase the size of the Mg(s) pieces.
b. Decrease the concentration of HCl(aq).
c. Increase the concentration of HCl(aq).
d. Decrease the test tube size.
_____66.C(s) + CO2(g)  2 CO(g) ∆H = +119.8 kJ
What is the effect of adding CO2(g) to this
system at equilibrium?
a. There will be no change.
b. The temperature will increase.
c. The amount of C(s) will increase.
d. The amount of CO(g) will
increase.
_____67. A change in which condition will
affect the value of the equilibrium constant?
a. concentration of the products
b. temperature of the reaction
c. concentration of the reactants
d. partial pressures of the reactants
_____70. In an oxidation-reduction reaction
MnO4- becomes Mn2+. How many electrons
must be transferred by manganese, Mn?
a. two electrons lost
b. five electrons lost
c. two electrons gained
d. five electrons gained
_____71. Which description of HNO3(aq) is
correct in this chemical equation?
3 S(s) + 4 HNO3(aq)  3 SO2(g) + 4 NO(g) + 2 H2O (l)
a.
b.
c.
d.
It is oxidized and is the oxidizing agent.
It is reduced and is the reducing agent.
It is oxidized and is the reducing agent.
It is reduced and is the oxidizing agent.
_____72.
_____MnO4-(aq) + _____Cl-(aq) + _____H+(aq)
? Cl2(g) + _____ Mn2+(aq) + ____ H2O (l)

What is the coefficient of Cl2 when this
oxidation-reduction equation is balanced?
a. 10
b. 8
c. 5 d. 2
Name_________________________________________
_____73. Given:
Ag+(aq) + e-  Ag (s)
Zn2+(aq) + 2 e-  Zn (s)
°
E = +0.80 V
E°= -0.76 V
Block__________
9
_____77. Which symbol is needed to
balance this nuclear equation?
Which equation describes the reaction at the
anode of this cell?
A.
C.
4
2
2
4
He
He
B. -1 e
D. 4 e0
_
____78. Which best represents a pair of
isotopes?
a. 2 Ag+(aq) + 2 e-  2 Ag (s)
b. 2 Ag (s)  2 Ag+(aq) + 2 ec. Zn2+(aq) + 2 e-  Zn (s)
d. Zn (s)  Zn2+(aq) + 2 e_____74.
alkene?
a.
b.
c.
d.
Which formula represents an
C2H2
C2H6
C3H6
C4H6
_____75. Which structural group identifies
an alcohol?
a. alkyl
b. phenyl
c. hydroxyl
d. carboxyl
_____76. Ten grams of a certain isotope has
a half-life of 12 hours. What mass of this
isotope remains after 48 hours?
a. 0.31 g
b. 0.63 g
c. 1.3 g
d. 2.5 g
Xand168X
A.
16
7
B.
35
17
37
Xand17
X
C.
16
8
Xand147 X
D.
34
17
36
Xand18
X
_____79. Which nitrogen-containing
compound is one cause of acid rain?
a. N2
b. NO2
c. AsN3
d. CH3COONH2
_____80. Which procedure should be
followed when mixing a concentrated acid
and water?
a. Add the acid to the water.
b. Add the water to the acid.
c. Never mix an acid and water.
d. Combine the water and acid
simultaneously.