exam name...a) ch3ob)c2h6o c) cho d) c4h13o2 e) ch4o3 41) 42) determine the molecular formula of a...
TRANSCRIPT
Exam
Name___________________________________
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
1) Which of the following is an ionic compound?
A) NO2 B) CF4 C) PCl3 D) SeBr2 E) LiCl
1)
2) Which of the following is an ionic compound?
A) CH2O
B) Cl2O
C) PF5
D) Mg3(PO4)2
E) SCl2
2)
3) Which of the following contains BOTH ionic and covalent bonds?
A) CaI2
B) CaSO4
C) COS
D) SF6
E) None of the above contain both ionic and covalent bonds.
3)
4) Which of the following is a molecular compound?
A) RbBr B) N2O4 C) NaNO3 D) SrSO3 E) CuCl2
4)
5) Which of the following is a molecular compound?
A) P4O10 B) ZnS C) NaCN D) SrI2 E) LiOH
5)
6) A covalent bond is best described as:
A) a bond between a metal and a polyatomic ion.
B) a bond between a metal and a nonmetal.
C) a bond between two polyatomic ions.
D) the transfer of electrons.
E) the sharing of electrons between atoms.
6)
7) An ionic bond is best described as:
A) the attraction that holds the atoms together in a polyatomic ion.
B) the transfer of electrons from one atom to another.
C) the attraction between 2 nonmetal atoms.
D) the attraction between 2 metal atoms.
E) the sharing of electrons.
7)
8) Which of the following is a molecular element?
A) S B) Ag C) Kr D) Mg E) Ti
8)
9) Which of the following is a molecular element?
A) Xe B) I C) Li D) Mg E) Ar
9)
1
10) Which of the following is an atomic element?
A) Mg B) Br C) O D) H E) N
10)
11) What is the empirical formula for C4H10O2?
A) C2H4O B) CHO C) CHO2 D) CH2O E) C2H5O
11)
12) What is the empirical formula for Hg2(NO3)2?
A) Hg2NO3
B) Hg(NO3)2
C) Hg4(NO3)4
D) HgNO3
E) Hg2(NO3)2
12)
13) Write the formula for the compound formed between potassium and sulfur.
A) KS2 B) K2S C) KS D) K2SO3 E) K3S2
13)
14) Write the formula for barium nitrite.
A) Ba3N2 B) Ba(NO2)2 C) B(NO2)3 D) BaNO3 E) BN
14)
15) Write the formula for copper (II) sulfate pentahydrate.
A) CuS*5H2O
B) CuSO4·5H2O
C) (CuSO4)5
D) Cu2S*H2O
E) Cu2SO3·H5
15)
16) Write the formula for strontium nitride.
A) Sr3N2 B) Sr(NO3)2 C) Sr(NO2)2 D) Sr2N3 E) SrN
16)
17) Determine the name for TiCO3. Remember that titanium forms several ions.
A) titanium carbonite
B) titanium (II) carbonate
C) titanium (II) carbonite
D) titanium carbide
E) titanium (I) carbonate
17)
18) Write the name for Sn(SO4)2. Remember that Sn forms several ions.
A) tin (IV) sulfate
B) tin (II) sulfite
C) tin sulfide
D) tin (I) sulfate
E) tin (I) sulfite
18)
2
19) Write the name for Ca3(PO4)2.
A) calcium (III) phosphite
B) calcium phosphate
C) tricalcium phosphorustetraoxide
D) calcium phosphite
E) calcium (II) phosphite
19)
20) Determine the name for CoCl2·6H2O. Remember that Co forms several ions.
A) cobalt (I) chloride
B) cobalt (II) chloride heptahydrate
C) cobalt (I) chloride heptahydrate
D) cobalt chloride hydrate
E) cobalt (II) chloride hexahydrate
20)
21) Determine the name for P4O10.
A) phophorus oxide
B) diphosphorus pentaoxide
C) phosphorus (IV) oxide
D) phosphorus (II) oxide
E) tetraphophorus decaoxide
21)
22) Determine the name for N2O5.
A) nitrogen tetraoxide
B) dinitrogen pentaoxide
C) nitrogen (IV) oxide
D) nitrogen oxide
E) nitrogen (II) oxide
22)
23) Determine the name for Cl2O.
A) chlorine oxide
B) dichloro monoxide
C) chlorate
D) chlorine (II) oxide
E) chlorine (I) oxide
23)
24) Determine the name for H2CO3.
A) hydrocarbonic acid
B) hydrocarbide acid
C) carbonic acid
D) dihydrogen carbonate
E) carbonous acid
24)
25) Determine the name for HClO3.
A) chlorate acid
B) perchloric acid
C) hydrochlorus acid
D) chloric acid
E) hydrochloric acid
25)
3
26) Determine the name for aqueous HBr.
A) hydrobromic acid
B) bromous acid
C) hydrobromous acid
D) bromic acid
E) hydrogen bromate
26)
27) Which of the following is one possible form of pentane?
A) CH3CH2CH2CH2CH2CH3
B) CH3CH2CH2CH2CH2NH2
C) CH3CH2CH2CH2CH3
D) CH3CH=CHCH2CH3
E) CH3CH2-O-CH2CH2CH3
27)
28) Which of the following compounds is ethanol?
A) C2H6
B) CH3CO2CH3
C) CH3CO2H
D) C2H5OH
E) CH3-O-CH3
28)
29) Calculate the molar mass for Mg(ClO4)2.
A) 247.52 g/mol
B) 119.52 g/mol
C) 123.76 g/mol
D) 223.21 g/mol
E) 75.76 g/mol
29)
30) Calculate the molar mass of Al(C2H3O2)3.
A) 139.99 g/mol
B) 258.09 g/mol
C) 86.03 g/mol
D) 204.13 g/mol
E) 56.00 g/mol
30)
31) Calculate the molar mass of Ca3(PO4)2.
A) 87.05 g/mol
B) 310.18 g/mol
C) 215.21 g/mol
D) 279.21 g/mol
E) 246.18 g/mol
31)
4
32) Write a balanced equation to show the reaction of sulfurous acid with lithium hydroxide to form
water and lithium sulfite.
A) HSO3 (aq) + LiOH (aq) → H2O (l) + LiSO3 (aq)
B) H2S (aq) + 2 LiOH (aq) → 2 H2O (l) + Li2S (aq)
C) HSO4 (aq) + LiOH (aq) → H2O (l) + LiSO4 (aq)
D) H2SO3 (aq) + 2 LiOH (aq) → 2 H2O (l) + Li2SO3 (aq)
E) H2SO4 (aq) + LiOH (aq) → H2O (l) + Li2SO4 (aq)
32)
33) Write a balanced equation to show the reaction of gaseous ethane with gaseous oxygen to form
carbon monoxide gas and water vapor.
A) 2 C2H6 (g) + 5 O2 (g) → 4 CO (g) + 6 H2O (g)
B) 2 C2H6 (g) + 7 O2 (g) → 4 CO2 (g) + 6 H2O (g)
C) C2H6 (g) + 5 O (g) → 2 CO (g) + 3 H2O (g)
D) 2 CH3 (g) + 5 O (g) → 2 CO (g) + 3 H2O (g)
E) C2H6 (g) + 7 O (g) → 2 CO2 (g) + 3 H2O (g)
33)
34) 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(CO3)2 (aq) + (NH3)2PO4 (aq) → AlPO4 (s) + 2 NH3CO3 (aq)
B) Al(C2H3O2)2 (aq) + (NH4)2PO4 (aq) → AlPO4 (s) + 2 NH4C2H3O3 (aq)
C) Al(CO2)3 (aq) + (NH4)3PO3 (aq) → AlPO3 (s) + 3 NH4CO2 (aq)
D) Al(C2H3O2)2 (aq) + (NH3)2PO4 (aq) → AlPO4 (s) + 2 NH3C2H3O3 (aq)
E) Al(C2H3O2)3 (aq) + (NH4)3PO4 (aq) → AlPO4 (s) + 3 NH4C2H3O3 (aq)
34)
35) How many N2O4 molecules are contained in 76.3 g N2O4? The molar mass of N2O4 is 92.02
g/mol.
A) 4.59 × 1025 N2O4 molecules
B) 7.26 × 1023 N2O4 molecules
C) 5.54 × 1025 N2O4 molecules
D) 1.38 × 1024 N2O4 molecules
E) 4.99 × 1023 N2O4 molecules
35)
36) How many C2H4 molecules are contained in 45.8 mg of C2H4? The molar mass of C2H4 is 28.05
g/mol.
A) 7.74 × 1026 C2H4 molecules
B) 4.69 × 1023 C2H4 molecules
C) 9.83 × 1020 C2H4 molecules
D) 3.69 × 1023 C2H4 molecules
E) 2.71× 1020 C2H4 molecules
36)
37) What is the mass (in kg) of 6.89 × 1025 molecules of CO2? The molar mass of CO2 is 44.01 g/mol.
A) 3.85 kg B) 2.60 kg C) 5.04 kg D) 6.39 kg E) 3.03 kg
37)
5
38) What is the mass of 9.44 × 1024 molecules of NO2? The molar mass of NO2 is 46.01 g/mol.
A) 341 g B) 685 g C) 294 g D) 205 g E) 721 g
38)
39) Determine the empirical formula for a compound that is 36.86% N and 63.14% O by mass.
A) N2O3 B) NO3 C) N2O D) NO E) NO2
39)
40) Determine the empirical formula for a compound that is found to contain 10.15 mg P and 34.85 mg
Cl.
A) PCl3 B) PCl C) P3Cl D) P2Cl3 E) PCl2
40)
41) Determine the empirical formula for a compound that contains C, H and O. It contains 52.14% C
and 34.73% O by mass.
A) CH3O B) C2H6O C) CHO D) C4H13O2 E) CH4O3
41)
42) Determine the molecular formula of a compound that has a molar mass of 183.2 g/mol and an
empirical formula of C2H5O2.
A) C6H15O6 B) C8H20O8 C) C3H7O3 D) C2H5O2 E) C4H10O4
42)
43) Determine the molecular formula of a compound that has a molar mass of 92.0 g/mol and an
empirical formula of NO2.
A) N3O6 B) N2O5 C) N2O4 D) NO2 E) N2O3
43)
44) How many atoms of oxygen are contained in 47.6 g of Al2(CO3)3? The molar mass of Al2(CO3)3
is 233.99 g/mol.
A) 1.10 × 1024 O atoms
B) 2.87 × 1025 O atoms
C) 2.96 × 1024 O atoms
D) 1.23 × 1023 O atoms
E) 3.19 × 1024 O atoms
44)
45) How many sodium ions are contained in 99.6 mg of Na2SO3? The molar mass of Na2SO3 is
126.05 g/mol.
A) 4.76 × 1020 sodium ions
B) 1.52 × 1027 sodium ions
C) 9.52 × 1020 sodium ions
D) 2.10 × 1021 sodium ions
E) 1.05 × 1021 sodium ions
45)
46) How many moles of N2O3 contain 2.55 × 1024 oxygen atoms?
A) 7.87 moles N2O3
B) 4.23 moles N2O3
C) 1.41 moles N2O3
D) 2.82 moles N2O3
E) 12.7 moles N2O3
46)
6
47) How many moles of PCl3 contain 3.68 × 1025 chlorine atoms?
A) 20.4 moles PCl3
B) 16.4 moles PCl3
C) 54.5 moles PCl3
D) 61.1 moles PCl3
E) 49.1 moles PCl3
47)
48) How many moles of C3H8 contain 4.95 × 1024 hydrogen atoms?
A) 9.73 moles C3H8
B) 6.58 moles C3H8
C) 1.03 moles C3H8
D) 3.09 moles C3H8
E) 8.22 moles C3H8
48)
49) How many millimoles of Ca(NO3)2 contain 4.78 × 1022 formula units of Ca(NO3)2? The molar
mass of Ca(NO3)2 is 164.10 g/mol.
A) 57.0 mmol Ca(NO3)2
B) 12.6 mmol Ca(NO3)2
C) 20.7 mmol Ca(NO3)2
D) 13.0 mmol Ca(NO3)2
E) 79.4 mmol Ca(NO3)2
49)
50) How many moles of C3H8 contain 9.25 × 1024 molecules of C3H8?
A) 15.4 moles C3H8
B) 65.1 moles C3H8
C) 46.2 moles C3H8
D) 34.9 moles C3H8
E) 28.6 moles C3H8
50)
51) Calculate the mass percent composition of sulfur in Al2(SO4)3.
A) 28.12 % B) 42.73 % C) 35.97 % D) 9.372 % E) 21.38 %
51)
52) Calculate the mass percent composition of lithium in Li3PO4.
A) 26.75 % B) 30.72 % C) 17.98 % D) 55.27 % E) 20.82 %
52)
53) Combustion analysis of 63.8 mg of a C, H and O containing compound produced 145.0 mg of CO 2
and 59.38 mg of H2O. What is the empirical formula for the compound?
A) C5H2O B) C6HO3 C) CHO D) C3H7O E) C3H6O
53)
7
54) How many molecules of ethane are contained in 25.0 mL of butane? The density of butane is
0.6011 g/mL and the molar mass is 58.12 g/mol.
A) 7.14 × 1025 molecules butane
B) 2.59 × 1023 molecules butane
C) 1.56 × 1023 molecules butane
D) 6.87 × 1023 molecules butane
E) 1.46 × 1027 molecules butane
54)
55) Determine the volume of hexane that contains 5.33 × 1022 molecules of hexane. The density of
hexane is 0.6548 g/mL and its molar mass is 86.17 g/mol.
A) 12.4 mL B) 7.40 mL C) 8.59 mL D) 13.5 mL E) 11.7 mL
55)
MATCHING. Choose the item in column 2 that best matches each item in column 1.
Match the following.
56) oxygen
57) chlorine
58) neon
59) calcium
60) iodine
A) O2 (g)
B) Ca2 (g)
C) Ca (s)
D) I2(s)
E) Cl2(g)
F) Ne2 (g)
G) Cl(g)
H) O (g)
I) I (g)
J) Ne (g)
56)
57)
58)
59)
60)
SHORT ANSWER. Write the word or phrase that best completes each statement or answers the question.
61) Describe the difference between ionic and molecular compounds. Give an example of
each.
61)
62) How can one compound contain both ionic and covalent bonds? Give an example. 62)
63) Why arenʹt prefixes used in naming ionic compounds? 63)
64) Describe the difference between a molecular formula and an empirical formula. Give an
example.
64)
8
65) Can you predict the chemical formula for a covalent compound between nitrogen and
oxygen? Explain your answer.
65)
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
66) According to the following balanced reaction, how many moles of NO are formed from 8.44 moles
of NO2 if there is plenty of water present?
3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)
A) 25.3 moles NO
B) 1.83 moles NO
C) 2.81 moles NO
D) 5.50 moles NO
E) 8.44 moles NO
66)
67) Consider the following reaction. How many moles of oxygen are required to produce 2.33 moles
of water? Assume that there is excess C3H7SH present.
C3H7SH(l) + 6 O2(g) → 3 CO2(g) + SO2(g) + 4 H2O (g)
A) 2.33 moles O2
B) 3.50 moles O2
C) 4.14 moles O2
D) 1.55 moles O2
E) 6.21 moles O2
67)
68) According to the following balanced reaction, how many moles of KO are required to exactly react
with 5.44 moles of H2O?
4 KO(s) + 2 H2O(l) → 4 KOH(s) + O2(g)
A) 10.9 moles H2O
B) 16.7 moles H2O
C) 4.87 moles H2O
D) 8.33 moles H2O
E) 2.72 moles H2O
68)
9
69) Consider the following balanced reaction. How many grams of water are required to form 75.9 g
of HNO3? Assume that there is excess NO2 present. The molar masses are as follows: H2O =
18.02 g/mol, HNO3 = 63.02 g/mol.
3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)
A) 38.0 g H2O
B) 43.4 g H2O
C) 10.9 g H2O
D) 21.7 g H2O
E) 26.5 g H2O
69)
70) 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) 0.126 g CO2
B) 0.209 g CO2
C) 0.198 g CO2
D) 0.396 g CO2
E) 0.792 g CO2
70)
71) According to the following reaction, how many grams of sulfur are formed when 37.4 g of water
are formed?
2 H2S(g) + SO2(g) → 3 S(s) + 2H2O(l)
A) 66.6 g S B) 14.0 g S C) 44.4 g S D) 56.1 g S E) 99.8 g S
71)
72) How many grams of Li3N can be formed from 1.75 moles of Li? Assume an excess of nitrogen.
6 Li(s) + N2(g) → 2 Li3N(s)
A) 61.0 g Li3N
B) 20.3 g Li3N
C) 58.3 g Li3N
D) 18.3 g Li3N
E) 15.1 g Li3N
72)
73) 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) 4.97 g O2 B) 3.59 g O2 C) 11.7 g O2 D) 19.9 g O2 E) 27.9 g O2
73)
10
74) How many moles of oxygen are formed when 58.6 g of KNO3 decomposes according to the
following reaction? The molar mass of KNO3 is 101.11 g/mol.
4 KNO3(s) → 2 K2O(s) + 2 N2(g) + 5 O2(g)
A) 0.580 mol O2
B) 23.2 mol O2
C) 18.5 mol O2
D) 1.73 mol O2
E) 0.724 mol O2
74)
75) 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
A) 3.65 × 1024 molecules HCl
B) 2.78 × 1024 molecules HCl
C) 6.09 × 1025 molecules HCl
D) 1.67 × 1024 molecules HCl
E) 5.02 × 1025 molecules HCl
75)
76) How many molecules of H2S are required to form 79.0 g of sulfur according to the following
reaction? Assume excess SO2.
2 H2S(g) + SO2(g) → 3 S(s) + 2H2O(l)
A) 5.06 × 1025 molecules H2S
B) 2.44 × 1023 molecules H2S
C) 3.17 × 1025 molecules H2S
D) 1.48 × 1024 molecules H2S
E) 9.89 × 1023 molecules H2S
76)
77) Determine the limiting reactant (LR) and the mass (in g) of nitrogen that can be formed from 50.0 g
N2O4 and 45.0 g N2H4. Some possibly useful molar masses are as follows: N2O4 = 92.02 g/mol,
N2H4 = 32.05 g/mol.
N2O4(l) + 2 N2H4(l) → 3 N2(g) + 4 H2O(g)
A) LR = N2H4, 59.0 g N2 formed
B) LR = N2H4, 13.3 g N2 formed
C) No LR, 45.0 g N2 formed
D) LR = N2O4, 105 g N2 formed
E) LR = N2O4, 45.7 g N2 formed
77)
11
78) Determine the theoretical yield of HCl if 60.0 g of BCl3 and 37.5 g of H2O are reacted according to
the following balanced reaction. A possibly useful molar mass is BCl3 = 117.16 g/mol.
BCl3(g) + 3 H2O(l) → H3BO3(s) + 3 HCl(g)
A) 75.9 g HCl B) 132 g HCl C) 187 g HCl D) 25.3 g HCl E) 56.0 g HCl
78)
79) Determine the theoretical yield of H2S (in moles) if 4.0 mol Al2S3 and 4.0 mol H2O are reacted
according to the following balanced reaction. A possibly useful molar mass is Al2S3 = 150.17
g/mol.
Al2S3 (s) + 6 H2O(l) → 2 Al(OH)3 (s) + 3 H2S(g)
A) 6.0 mol H2S
B) 18 mol H2S
C) 12 mol H2S
D) 2.0 mol H2S
E) 4.0 mol H2S
79)
80) 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.
Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s)
A) 61.03 % B) 20.02 % C) 57.30 % D) 28.65 % E) 81.93 %
80)
81) Determine the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield
750.0 mL of solution.
A) 2.30 M B) 1.50 M C) 1.18 M D) 0.768 M E) 0.130 M
81)
82) Determine the molarity of a solution formed by dissolving 468 mg of MgI2 in enough water to
yield 50.0 mL of solution.
A) 0.0107 M B) 0.0936 M C) 0.0337 M D) 0.0651 M E) 0.0297 M
82)
83) How many milliliters of a 0.184 M NaNO3 solution contain 0.113 moles of NaNO3?
A) 326 mL B) 543 mL C) 614 mL D) 163 mL E) 885 mL
83)
84) How many liters of a 0.0550 M KCl solution contain 0.163 moles of KCl?
A) 2.96 L B) 8.97 L C) 3.37 L D) 1.48 L E) 1.12 L
84)
85) How many moles of LiI are contained in 258.6 mL of 0.0296 M LiI solution?
A) 7.65 × 10-3 mol
B) 1.31 × 10-3 mol
C) 8.74 × 10-3 mol
D) 1.14 × 10-3 mol
E) 3.67 × 10-3 mol
85)
12
86) How many moles of CH3CH2OH are contained in 548 mL of 0.0788 M CH3CH2OH solution?
A) 4.32 × 10-2 mol
B) 1.44 × 10-2 mol
C) 2.32 × 10-2 mol
D) 5.26 × 10-2 mol
E) 6.95 × 10-2 mol
86)
87) How many molecules of sucrose (C12H22O11, molar mass = 342.30 g/mol) are contained in 14.3
mL of 0.140 M sucrose solution?
A) 1.21 × 1021 molecules C12H22O11
B) 1.63 × 1023 molecules C12H22O11
C) 5.90 × 1024 molecules C12H22O11
D) 8.29 × 1022 molecules C12H22O11
E) 6.15 × 1022 molecules C12H22O11
87)
88) How many chloride ions are present in 65.5 mL of 0.210 M AlCl3 solution?
A) 5.79 × 1024 chloride ions
B) 4.02 × 1023 chloride ions
C) 1.21 × 1022 chloride ions
D) 2.49 × 1022 chloride ions
E) 8.28 × 1021 chloride ions
88)
89) What is the concentration of nitrate ions in a 0.125 M Mg(NO3)2 solution?
A) 0.125 M B) 0.250 M C) 0.375 M D) 0.0625 M E) 0.160 M
89)
90) Which of the following solutions will have the highest concentration of chloride ions?
A) 0.10 M NaCl
B) 0.10 MAlCl3
C) 0.05 M CaCl2
D) 0.10 M MgCl2
E) All of these solutions have the same concentration of chloride ions.
90)
91) Which of the following solutions will have the highest electrical conductivity?
A) 0.045 M Al2(SO4)3
B) 0.10 M KF
C) 0.10 M NaI
D) 0.10 M LiBr
E) 0.050 M (NH4)2CO3
91)
92) How many milliliters of a 0.266 M LiNO3 solution are required to make 150.0 mL of 0.075 M
LiNO3 solution?
A) 18.8 mL B) 42.3 mL C) 35.1 mL D) 23.6 mL E) 53.2 mL
92)
13
93) What volume (in L) of 0.0887 M MgF2 solution is needed to make 275.0 mL of 0.0224 M MgF2
solution?
A) 14.4 mL B) 72.3 mL C) 10.9 mL D) 69.4 mL E) 91.8 mL
93)
94) Determine the concentration of a solution prepared by diluting 25.0 mL of a stock 0.188 M
Ca(NO3)2 solution to 150.0 mL.
A) 0.0199 M B) 1.13 M C) 0.0501 M D) 0.0887 M E) 0.0313 M
94)
95) Which of the following is NOT a strong electrolyte?
A) MgCO3
B) LiOH
C) Li2SO4
D) NaC2H3O2
E) CaCl2
95)
96) Which of the following is considered a STRONG electrolyte?
A) PbCl2
B) HC2H3O2
C) C12H22O11
D) NH4NO3
E) CH3OH
96)
97) According to the following reaction, what volume of 0.244 M KCl solution is required to react
exactly with 50.0 mL of 0.210 M Pb(NO3)2 solution?
2 KCl(aq) + Pb(NO3)2 (aq) → PbCl2(s) + 2 KNO3(aq)
A) 97.4 mL B) 43.0 mL C) 116 mL D) 58.1 mL E) 86.1 mL
97)
98) 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) 345 mL B) 139 mL C) 581 mL D) 278 mL E) 173 mL
98)
99) What mass (in g) of AgCl is formed from the reaction of 75.0 mL of a 0.078 M AgC2H3O2 solution
with 55.0 mL of 0.109 M MgCl2 solution?
2 AgC2H3O2(aq) + MgCl2(aq) → 2 AgCl(s) + Mg(C2H3O2)2(aq)
A) 1.70 g B) 2.56 g C) 0.839 g D) 0.859 g E) 1.72 g
99)
100) According to the following reaction, what mass of PbCl2 can form from 235 mL of 0.110 M KCl
solution? Assume that there is excess Pb(NO3)2.
2 KCl(aq) + Pb(NO3)2 (aq) → PbCl2(s) + 2 KNO3(aq)
A) 5.94 g B) 3.59 g C) 1.80 g D) 1.30 g E) 7.19 g
100)
14
101) According to the following reaction, how many moles of Fe(OH)2 can form from 175.0 mL of 0.227
M LiOH solution? Assume that there is excess FeCl2.
FeCl2(aq) + 2 LiOH(aq) → Fe(OH)2(s) + 2 LiCl(aq)
A) 3.97 × 10-2 moles
B) 6.49 × 10-2 moles
C) 2.52 × 10-2 moles
D) 1.99 × 10-2 moles
E) 5.03 × 10-2 moles
101)
102) How many of the following compounds are soluble in water?
Cu(OH)2 LiNO3 NH4Br K2S
A) 0 B) 3 C) 1 D) 4 E) 2
102)
103) Which of the following compounds is soluble in water?
A) MgCO3
B) CaS
C) PbCl2
D) BaSO4
E) None of these compounds is soluble in water.
103)
104) How many of the following compounds are insoluble in water?
KC2H3O2 CaSO4 SrS AlPO4
A) 3 B) 0 C) 1 D) 2 E) 4
104)
105) Which of the following compounds is insoluble in water?
A) Hg2I2
B) MgSO4
C) BaS
D) (NH4)2CO3
E) All of these compounds are soluble in water.
105)
106) Which of the following pairs of aqueous solutions will react when mixed?
A) NaCl + Li3PO4
B) AgC2H3O2 + Cu(NO3)2
C) Hg2(NO3)2 + LiI
D) NH4NO3 + Li2CO3
E) None of the above solution pairs will produce a reaction.
106)
15
107) Which of the following pairs of aqueous solutions will react when mixed?
A) Sr(C2H3O2)2 + Na2SO4
B) KNO3 + NaOH
C) LiOH + Na2S
D) (NH4)2SO4 + LiCl
E) None of the above solution pairs will produce a reaction.
107)
108) Which of the following pairs of aqueous solutions will react when mixed?
A) K2CO3 + HNO3
B) Li2S + HCl
C) HCl + LiOH
D) MgCl2 + KOH
E) All of these solution pairs will produce reactions.
108)
109) Give the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of
lithium sulfide and copper (II) nitrate are mixed. (the superscripts below arenʹt really acceptable
on most of the ions, I donʹt know how to make it any better)
A) Li+ (aq) + SO42-(aq) + Cu+(aq) + NO3-(aq) → CuS(s) + Li+(aq) + NO3-(aq)
B) 2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → Cu2+(aq) + S2-(aq) + 2 LiNO3(s)
C) Li+ (aq) + S-(aq) + Cu+(aq) + NO3-(aq) → CuS(s) + LiNO3(aq)
D) 2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → CuS(s) + 2 Li+(aq) + 2 NO3-(aq)
E) No reaction occurs.
109)
110) Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of K2S and
Fe(NO3)2 are mixed.
A) Fe2+(aq) + S2-(aq) → FeS(s)
B) Fe2+(aq) + S2-(aq) + 2 K+(aq) + 2 NO3-(aq) → FeS(s) + 2 K+(aq) + 2 NO3-(aq)
C) Fe2+(aq) + S2-(aq) + 2 K+(aq) + 2 NO3-(aq) → Fe2+(aq) + S2-(aq) + 2 KNO3(s)
D) K+(aq) + NO3-(aq) → KNO3(s)
E) No reaction occurs.
110)
111) Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of H2SO4
and KOH are mixed.
A) H+(aq) + OH-(aq) → H2O(l)
B) H+(aq) + OH-(aq) + 2 K+(aq) + SO42-(aq) → H2O(l) + K2SO4(s)
C) 2 K+(aq) + SO42-(aq) → K2SO4(s)
D) H22+(aq) + OH-(aq) → H2(OH)2(l)
E) No reaction occurs.
111)
16
112) Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of
Al(C2H3O2)3 and LiNO3 are mixed.
A) Al3+(aq) + 3 NO3-(aq) → Al(NO3)3(s)
B) Al3+(aq) + 3 NO3-(aq) + Li+(aq) + C2H3O2-(aq) → Al(NO3)3(aq) + LiC2H3O2(s)
C) 3 Li+(aq) + (C2H3O2)33-(aq) → Li3(C2H3O2)3 (s)
D) Li+(aq) + C2H3O2-(aq) → LiC2H3O2(s)
E) No reaction occurs.
112)
113) Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of
Na2CO3 and HCl are mixed.
A) 2 H+(aq) + CO32-(aq) → H2O(l) + CO2(g)
B) 2 H+(aq) + CO32-(aq) → H2CO3(s)
C) 2 Na+(aq) + CO32-(aq) + 2 H+(aq) + 2 Cl-(aq) → H2CO3(s) + 2 Na+(aq) + 2 Cl-(aq)
D) 2 Na+(aq) + CO32-(aq) + 2 H+(aq) + 2 Cl-(aq) → H2CO3(s) + 2 NaCl(aq)
E) No reaction occurs.
113)
114) Give the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of
MgSO3 and HI are mixed.
A) 2 H+(aq) + SO32-(aq) → H2O(l) + SO2(g)
B) 2 H+(aq) + SO32-(aq) + Mg2+(aq) + 2 I-(aq)→ H2SO3(s) + MgI2(aq)
C) Mg2+(aq) + 2 I-(aq) → MgI2(s)
D) 2 H+(aq) + SO32-(aq) → H2SO3(s)
E) No reaction occurs.
114)
115) Identify the spectator ions in the following molecular equation.
KBr(aq) + AgNO3(aq) → AgBr(s) + KNO3(aq)
A) Ag+ & Br-
B) Ag+ & NO3-
C) K+ & Br-
D) K+ & NO3-
E) There are no spectator ions in this reaction.
115)
116) Choose the statement below that is TRUE.
A) The term ʺweak electrolyteʺ means that the substance is inert.
B) A strong acid solution consists of only partially ionized acid molecules.
C) The term ʺstrong electrolyteʺ means that the substance is extremely reactive.
D) A weak acid solution consists of mostly nonionized acid molecules.
E) A molecular compound that does not ionize in solution is considered a strong electrolyte.
116)
17
117) Which of the following is an acid base reaction?
A) MgSO4(aq) + Ba(NO3)2(aq) → Mg(NO3)2(aq) + BaSO4(s)
B) 2 HClO4(aq) + Ca(OH)2(aq) → 2 H2O(l) + Ca(ClO4)2(aq)
C) C(s) + O2(g) → CO2(g)
D) Fe(s) + 2 AgNO3(aq) → 2 Ag(s) + Fe(NO3)2(aq)
E) None of the above are acid base reactions.
117)
118) Which of the following is a precipitation reaction?
A) 2 LiI(aq) + Hg2(NO3)2(aq) → Hg2I2(s) + 2 LiNO3(aq)
B) NaCl(aq) + LiI(aq) → NaI(aq) + LiCl(aq)
C) HCl(aq) + KOH(aq) → KCl(aq) + H2O(l)
D) Zn(s) + 2 AgNO3(aq) → 2 Ag(s) + Zn(NO3)2(aq)
E) None of the above are precipitation reactions.
118)
119) Which of the following is a gas-evolution reaction?
A) 2 C2H6(l) + 7 O2(g) → 4 CO2(g) + 6 H2O(g)
B) LiCl(aq) + NaNO3(aq) → LiNO3(aq) + NaCl(g)
C) NH4Cl(aq) + KOH(aq) → KCl(aq) + NH3(g) + H2O(l)
D) 2 H2(g) + O2(g) → 2 H2O(g)
E) None of the above are gas-evolution reactions.
119)
120) Which of the following is an oxidation-reduction reaction?
A) NaI(aq) + AgNO3(aq) → AgI(s) + NaNO3(aq)
B) Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g)
C) HCl(aq) + LiOH(aq) → LiCl(aq) + H2O(l)
D) Pb(C2H3O2)2(aq) + 2 NaCl(aq) → PbCl2(s) + 2 NaC2H3O2(aq)
E) All of the above are oxidation-reduction reactions.
120)
121) Determine the oxidation state of P in PO33-.
A) 0 B) +6 C) +2 D) +3 E) -3
121)
122) Determine the oxidation state of Sn in Sn(SO4)2.
A) +4 B) +2 C) -2 D) +6 E) 0
122)
123) What element is undergoing oxidation (if any) in the following reaction?
CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g)
A) H
B) C
C) O
D) both C and H
E) None of the elements is undergoing oxidation.
123)
18
124) What element is undergoing reduction (if any) in the following reaction?
Zn(s) + 2 AgNO3(aq) → Zn(NO3)2(aq) + 2 Ag(s)
A) Ag
B) Zn
C) O
D) N
E) This is not an oxidation-reduction reaction.
124)
125) Determine the reducing agent in the following reaction.
2 Li(s) + Fe(C2H3O2)2(aq) → 2 LiC2H3O2(aq) + Fe(s)
A) Fe B) Li C) C D) O E) H
125)
126) Determine the oxidizing agent in the following reaction.
Ni(s) + 2 AgClO4(aq) → Ni(ClO4)2(aq) + 2 Ag(s)
A) Cl
B) O
C) Ni
D) Ag
E) This is not an oxidation-reduction reaction.
126)
127) 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) 0.10 M B) 0.25 M C) 0.20 M D) 0.36 M E) 0.40 M
127)
128) The titration of 80.0 mL of an unknown concentration H3PO4 solution requires 126 mL of 0.218 M
KOH solution. What is the concentration of the H3PO4 solution (in M)?
A) 0.138 M B) 1.03 M C) 0.343 M D) 0.0461 M E) 0.114 M
128)
129) Chose the reaction that represents the combustion of C6H12O2.
A) C6H12O2(l) + 9 O2(g) → 6 CO2(g) + 6 H2O(g)
B) C6H12O2(l) → 6 C(s) + 6 H2(g) + O2(g)
C) Mg(s) + C6H12O2(l) → MgC6H12O2(aq)
D) 6 C(s) + 6 H2(g) + O2(g) → C6H12O2(l)
E) None of the above represent the combustion of C6H12O2.
129)
130) Determine the number of grams H2 formed when 250.0 mL of 0.743 M HCl solution reacts with
3.41 x 1023 atoms of Fe according to the following reaction.
2 HCl(aq) + Fe(s) → H2(g) + FeCl2(aq)
A) 1.51 g B) 1.33 g C) 0.187 g D) 0.374 g E) 1.14 g
130)
19
131) According to the following reaction, what amount of Al2O3 remains when 20.00 g of Al2O3 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) 14.00 g B) 19.78 g C) 28.33 g D) 11.67 g E) 8.33 g
131)
SHORT ANSWER. Write the word or phrase that best completes each statement or answers the question.
132) Describe the difference between complete ionic and net ionic equations. 132)
133) Explain the difference between a strong and weak electrolyte. Give an example of each. 133)
134) What causes a precipitation reaction to occur between two soluble compounds? 134)
135) How can you tell if a reaction is an oxidation-reduction reaction? 135)
136) How would the concentration change if a1.0 L flask of 1.0 M NaCl were left uncapped on a
laboratory bench for several days. Why?
136)
MATCHING. Choose the item in column 2 that best matches each item in column 1.
Match the following.
137) CH4(g) + 2 O2(g) → CO2(g) + 2
H2O(g)
138) H2SO4(aq) + 2 LiOH(aq) → 2 H2O(l) +
Li2SO4(aq)
139) Mg(s) + Cu(NO3)2(aq) →
Mg(NO3)2(aq) + Cu(s)
140) HCl(aq) + (NH4)2S(aq) → H2S(g) +
2NH4Cl(aq)
141) NaCl(aq) + AgNO3(aq) → AgCl(s) +
NaNO3(aq)
A) Oxidation Reduction
B) Combustion
C) Acid Base
D) Gas Evolution
E) Precipitation
137)
138)
139)
140)
141)
20
Answer KeyTestname: UNTITLED3
1) E
2) D
3) B
4) D
5) A
6) E
7) B
8) A
9) B
10) A
11) E
12) D
13) B
14) B
15) B
16) A
17) B
18) A
19) B
20) E
21) E
22) B
23) B
24) C
25) D
26) A
27) C
28) D
29) D
30) D
31) B
32) D
33) A
34) E
35) E
36) C
37) C
38) E
39) A
40) A
41) B
42) A
43) C
44) A
45) C
46) C
47) A
48) C
49) E
50) A
21
Answer KeyTestname: UNTITLED3
51) A
52) C
53) E
54) C
55) E
56) A
57) E
58) J
59) C
60) D
61) An ionic compound is formed between a metal and a nonmetal (or polyatomic ions) and is held together through the
attraction of opposite charges. An example is NaCl. A molecular compound is usually formed between 2 or more
nonmetals and is held together through the sharing of electrons between atoms. An example is CO2.
62) An ionic compound that contains a polyatomic ion, such as NaNO3, has both ionic bonds (that hold the sodium and
nitrate ions together) as well as covalent bonds (that hold the atoms within the nitrate ion together).
63) The charges on the ions dictate how many must be present to form a neutral unit. Molecular compounds do not have
such constraints and therefore must use prefixes to denote the number of atoms present.
64) A molecular formula is the exact number of each type of atom necessary to build a specific molecule. An empirical
formula is simply the smallest whole number ratio between atoms in a compound. For example, C2H4 is the
molecular formula for ethene. The empirical formula for ethene is CH2, the smallest whole number ratio between the
elements.
65) No, since nitrogen and oxygen are both nonmetals, they combine by sharing electrons. This can be done in multiple
different ways. Some possible compounds are N2O, N2O3, NO2.
66) C
67) B
68) A
69) C
70) C
71) E
72) B
73) A
74) E
75) B
76) E
77) E
78) E
79) D
80) E
81) B
82) C
83) C
84) A
85) A
86) A
87) A
88) D
89) B
90) B
22
Answer KeyTestname: UNTITLED3
91) A
92) B
93) D
94) E
95) A
96) D
97) E
98) D
99) C
100) B
101) D
102) B
103) B
104) D
105) A
106) C
107) A
108) E
109) D
110) A
111) A
112) E
113) A
114) A
115) D
116) D
117) B
118) A
119) C
120) B
121) D
122) A
123) B
124) A
125) B
126) D
127) C
128) E
129) A
130) C
131) D
132) A complete ionic equation shows all of the substances present in the reaction mixture. A net ionic equation only
shows the substances that are participating in the reaction. The spectator ions are absent in the net ionic equation.
133) A strong electrolyte is either an ionic compound that is soluble in water or a molecular compound that ionizes
completely in water. Possible examples are NaCl or HCl. A weak electrolyte is only slightly soluble or does not
ionize to any great extent in water. Possible examples are AgCl or HC2H3O2.
134) A precipitate, or insoluble compound, forms from a pair of the ions present. This ʺtrapsʺ some of the ions into a newly
formed compound causing reaction.
135) At least one species is losing electrons while at least one other species is gaining electrons. This can be evaluated by
assigning oxidation numbers to each element present and looking to see if these change from reactant to product.
23
Answer KeyTestname: UNTITLED3
136) The concentration would slowly increase as water from the solution evaporated. This is because the amount of NaCl
in the flask would remain constant while the amount of water decreases.
137) B
138) C
139) A
140) D
141) E
24