1) What answer should be reported, with the correct number of significant figures, for the
following calculation? (965.43 × 3.911) + 9413.4136
A) 13189.2
B) 13189
C) 1.32 × 104
D) 1.3 × 104
E) 1.319 × 104
2) If the walls in a room are 955 square feet in area, and a gallon of paint covers 15
square yards, how many gallons of paint are needed for the room? (3 ft = 1 yd)
A)
B)
C)
D)
E)
2.3 gallons
24 gallons
7.1 gallons
47 gallons
21 gallons
3) The density of air under ordinary conditions at 25°C is 1.19 g/L. How many kilograms
of air are in a room that measures 11.0 ft X 11.0 ft and has an 8.00 ft ceiling? 1 ft. = 30. 4
cm; 1 L = 103 cm3
A)
B)
C)
D)
E)
2.93
32.6
40.4
0.0770
0.121
4) Choose the pure substance from the list below.
A)
B)
C)
D)
E)
air
milk
sugar
seawater
lemonade
5) Which of the following are examples of a chemical change?
A) copper building materials develop a green patina over time
B) a match burns
C) ethanol evaporates
D) Both A and B are examples of chemical change.
E) All of the above are examples of chemical change
6) A student performs an experiment to determine the density of a sugar solution. She
obtains the following results: 1.79 g/mL, 1.81 g/mL, 1.80 g/mL, 1.81 g/mL. If the actual
value for the density of the sugar solution is 1.80 g/mL, which statement below best
describes her results?
A) Her results are precise, but not accurate.
B) Her results are accurate, but not precise.
C) Her results are both precise and accurate
D) Her results are neither precise nor accurate.
E) It isn't possible to determine with the information given.
7) Identify the charges of the protons, neutrons, and electrons.
A) protons +1, neutrons 0, electrons -1
B) protons 0, neutrons -1, electrons +1
C) protons -1, neutrons 0, electrons +1
D) protons 0, neutrons +1, electrons -1
E) protons +1, neutrons -1, electrons 0
8) What does "X" represent in the following symbol? 79
35 X
A) mercury
B) chlorine
C) selenium
D) bromine
E) gold
9) Determine the number of protons, neutrons and electrons in X2- if we have:
65
29 X
A) p+ = 31
B) p+ = 29
C) p+ = 36
D) p+ = 29
E) p+ = 29
n° = 34
n° = 29
n° = 36
n° = 36
n° = 36
e- = 29
e- = 36
e- = 29
e- = 31
e- = 36
10) Which of the following elements is a metalloid?
A) Al
B) Ge
C) C
D) Sn
E) Ti
11) Silver has an atomic mass of 107.868 amu. The Ag-109 isotope (108.905 amu) is
48.16%. What is the amu of the other isotope?
A) 106.905 amu
B) 106.908 amu
C) 106.903 amu
D) 106.911 amu
12) How many atoms are in 2.50 moles of CO2?
24
A) 4.52 x 10 atoms
24
B) 1.52 x 10 atoms
23
C) 5.02 x 10 atoms
24
D) 3.01 x 10 atoms
23
E) 7.53 x 10 atoms
13) Which of the following contains BOTH ionic and covalent bonds?
A) CaI2
B) COS
C) CaSO4
D) SF6
E) None of the above contain both ionic and covalent bonds.
14) Write a possible molecular formula for C4H4O.
A) C8H8O2
B) C12H12O2
C) C2H2O
D) C8H8O
E) None of the above
15) Which of the following is a molecular element?
A) Magnesium
B) Argon
C) Xenon
D) Iodine
E) Lithium
16) Combustion analysis of 63.8 mg of a C, H and O containing compound produced
145.0 mg of CO2 and 59.38 mg of H2O. What is the empirical formula for the
compound?
A) C5H2O
B) CHO
C) C3H6O
D) C3H7O
E) C6HO3
17) 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)3 (aq) + (NH4)2PO4 (aq) → AlPO4 (s) + 2 NH4C2H3O2 (aq)
B) Al(C2H3O2)2 (aq) + (NH3)2PO4 (aq) → AlPO4 (s) + 2 NH3C2H3O2 (aq)
C) Al(CO3)2 (aq) + (NH3)2PO4 (aq) → AlPO4 (s) + 2 NH3CO3 (aq)
D) Al(C2H3O2)3 (aq) + (NH4)3PO4 (aq) → AlPO4 (s) + 3 NH4C2H3O2 (aq)
E) Al(CO2)3 (aq) + (NH4)3PO3 (aq) → AlPO3 (s) + 3 NH4CO2 (aq)
18) Identify a carboxylic acid and an ether from left to right.
A) CH3CH2OCH2CH3, CH3CH2OH
B) CH3COOH, CH3CH2OH
C) CH3CH2CH2CH3, CH3CH2NH2
D) CH3CH2OCH2CH3, CH3CH2CH2CH3
E) CH3COOH, CH3CH2OCH2CH3
19) The solid compound, Mg(NO3)2, contains
2-
A) Mg2+, N5+, and O ions.
B) Mg2+ and (NO3)-1 ions.
C) Mg 2+ and (NO3)-2 ions.
D) Mg(NO3)2 molecules.
2E) Mg2+, N3+, and O ions
20) What is the chemical formula for magnesium hydride?
A) MgH2
B) MnH2
C) Mn(OH)2
D) Mg(OH)2
E) Mn(OH)3
21) The compound, Cu(IO3)2, is named
A) copper iodate(II).
B) copper(I) iodite.
C) copper(I) iodate(II).
D) copper(II) iodate
E) copper(II) iodite
22) The compound, ClO, is named
A) chlorite.
B) hypochlorite.
C) chlorous
D) chlorine monoxide.
E) chlorine ( II) oxide.
23) The chemical formula for phosphorous acid is
A) H3P(aq).
B) H2PO2(aq).
C) H3PO3 (aq).
D) H3P2O6 (aq
E) H3PO4 (aq).
24) Calcium phosphate reacts with sulfuric acid to form calcium sulfate and phosphoric
acid. What is the coefficient for sulfuric acid when the equation is balanced using the
lowest, whole-numbered coefficients?
A) 1
B) 2
C) 3
D) 4
E) none of these
25) How many moles of PCl3 contain 3.68 × 1025 chlorine atoms?
A) 61.1 moles PCl3
B) 20.4 moles PCl3
C) 16.4 moles PCl3
D) 54.5 moles PCl3
E) 49.1 moles PCl3
26) Which of the following has the greatest mass?
22
A) 3.88 × 10 molecules of O2
B) 1.00 g of O2
C) 0. 0312 mol of O2
D) 1.00 g of O.
E) All of the above have the same mass.
27) Give the complete ionic equation for the reaction (if any) that occurs when aqueous
solutions of MgSO3 and HI are mixed.
2-
A) 2 H+(aq) + SO3 (aq) → H2SO3(s)
2+
B) Mg (aq) + 2I (aq) → MgI2(s)
+
22+
C) 2 H (aq) + SO3 (aq) + Mg (aq) + 2 I (aq)→ H2SO3(s) + MgI2(aq)
+
2D) 2 H (aq) + SO3 (aq) → H2O(l) + SO2(g)
E) No reaction occurs.
28) If the percent yield for the following reaction is 75.0%, how many grams of KClO3
are needed to produce 32.0 g of O2?
2 KClO3(s) → 2 KCl(s) + 3 O2(g)
A) 53.1 g
B) 81.7 g
C) 126 g
D) 283 g
E) 109 g
29) How many grams of oxygen are formed when 6.21 moles of KOH are formed?
4 KO(s) + 2 H2O(l) → 4 KOH(s) + O2(g)
A) 19.9 g O2
B) 27.9 g O2
C) 49.7 g O2
D) 3.59 g O2
E) 11.7 g O2
30) A 18.01 g sample of N2 reacts with 3.02 g of H2 to form ammonia (NH3). What mass
of ammonia is formed?
A) 17.01 g
B) 1.10 g
C) 14.01 g
D) 3.02 g
E) 23.07 g
31) Consider the following balanced reaction. What mass (in g) of CO2 can be formed
from 288 mg of O2? Assume that there is excess C3H7SH present.
C3H7SH(l) + 6 O2(g) → 3 CO2(g) + SO2(g) + 4 H2O (g)
A) 0.396 g CO2
B) 0.209 g CO2
C) 0.792 g CO2
D) 0.126 g CO2
E) 0.198 g CO2
32) How many molecules of HCl are formed when 50.0 g of water reacts according to the
following balanced reaction? Assume excess ICl3.
2 ICl3 + 3 H2O → ICl + HIO3 + 5 HCl
24
A) 2.78 × 10 molecules HCl
24
B) 1.67 × 10 molecules HCl
25
C) 5.02 × 10 molecules HCl
25
D) 6.09 × 10 molecules HCl
24
E) 3.65 × 10 molecules HCl
33) According to the following reaction, what amount of Al2S3 remains when 20.00 g of
Al2S3 and 2.00 g of H2O are reacted? A few of the molar masses are as follows: Al2S3 =
150.17 g/mol, H2O = 18.02 g/mol.
Al2S3(s) + 6 H2O(l) → 2 Al(OH)3(s) + 3 H2S(g)
A) 28.33 g
B) 14.00 g
C) 8.33 g
D) 19.78 g
E) 17.22 g
34) Determine the percent yield of a reaction that produces 28.65 g of Fe when 50.00 g of
Fe2O3 react with excess Al according to the following reaction.
A) 61.03 %
B) 28.65 %
C) 57.30 %
D) 20.02 %
E) 81.93 %
Fe2O3 (s) + 2 Al(s) → Al2O3 (s) + 2 Fe(s)
35) What is the concentration of nitrate ions in a 0.125 M Mg(NO3)2 solution?
A) 0.125 M
B) 0.0625 M
C) 0.375 M
D) 0.250 M
E) 0.160 M
36) How many grams of NaCl are required to make 250.0 mL of a 3.000 M solution?
A) 58.40 g
B) 175.3 g
C) 14.60 g
D) 43.83 g
E) 87.66 g
37) What volume of 0.305 M AgNO3 is required to react exactly with 155.0 mL of 0.274
M Na2SO4 solution? Hint: You will want to write a balanced reaction.
A) 581 mL
B) 173 mL
C) 278 mL
D) 139 mL
E) 345 mL
38) Which of the following solutions will have the highest electrical conductivity?
A) 0.065 M Na3PO4
B) 0.075 M (NH4)2CO3
C) 0.10 M LiBr
D) 0.10 M NaI
E) 0.10 M KF
39) Which of the following pairs of aqueous solutions will form a precipitate when
mixed?
A) LiOH + Na2S
B) (NH4)2SO4 + LiCl
C) Sr(C2H3O2)2 + Na2SO4
D) KNO3 + NaOH
E) None of the above solution pairs will produce a precipitate.
40) Give the net ionic equation for the reaction (if any) that occurs when aqueous
solutions of Al(C2H3O2)3 and LiNO3 are mixed.
3+
A) Al (aq) + 3 NO3 (aq) → Al(NO3)3(s)
+
B) Li (aq) + C2H3O2 (aq) → LiC2H3O2(s)
3+
+
C) Al (aq) + 3 NO3 (aq) + Li (aq) + C2H3O2 (aq) → Al(NO3)3(aq) + LiC2H3O2(s)
+
3D) 3 Li (aq) + (C2H3O2)3 (aq) → Li3(C2H3O2)3 (s)
E) No reaction occurs.
41) The titration of 25.0 mL of an unknown concentration H2SO4 solution requires 83.6
mL of 0.12 M LiOH solution. What is the concentration of the H2SO4 solution (in M)?
A) 0.20 M
B) 0.40 M
C) 0.10 M
D) 0.36 M
E) 0.25 M
42) Determine the oxidation state of P in PO33-.
A) +3
B) +6
C) +2
D) 0
E) -3
43) Which of the following is an oxidation-reduction reaction?
A) HCl(aq) + LiOH(aq) → LiCl(aq) + H2O(l)
B) NaI(aq) + AgNO3(aq) → AgI(s) + NaNO3(aq)
C) Pb(C2H3O2)2(aq) + 2 NaCl(aq) → PbCl2(s) + 2 NaC2H3O2(aq)
D) Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g)
E) All of the above are oxidation-reduction reactions.
44) What element is undergoing oxidation (if any) in the following reaction?
CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g)
A) O
B) H
C) C
D) both C and H
E) None of the elements is undergoing oxidation.
45) Determine the oxidizing agent in the following reaction.
Ni(s) + 2 AgClO4(aq) → Ni(ClO4)2(aq) + 2 Ag(s)
A) Ag
B) Ni
C) Cl
D) O
E) This is not an oxidation-reduction reaction.
46) List the spectator ions in the following reaction.
+2
-
+
-2
+
-
Ba (aq) + 2 OH (aq) + 2 Na (aq) + CO3 (aq) → 2 Na (aq) + 2OH (aq) + BaCO3 (s)
+2
-2
A) Ba , CO3
+2
B) Ba , OH
+
-2
C) Na , CO3
+
D) Na , OH
E) There are not any spectator ions.