chem 114 sample midterm exam
DESCRIPTION
Practice questions for first year university Chem course.TRANSCRIPT
7212019 Chem 114 Sample Midterm Exam
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7212019 Chem 114 Sample Midterm Exam
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2
6 A biker rides at an average speed of 25 km per hour How many minutes will it take for this biker to
ride a distance of 20 km
a) 25 min
b) 32 min
c) 38 mind) 42 min
e) 48 min
7 Which of the following statements is incorrect about the nuclear theory of the atom proposed by
Rutherford
a) Most of the mass of an atom is contained in the nucleus
b) The atom is mostly empty space
c) The number of neutrons and electrons in the atom are equal
d) The nucleus is surrounded by a cloud of electrons
e) The number of protons and electrons in the atom are equal
8 How many neutrons protons and electrons are found in 35Cl (NOTE 35Cl is an isotope of elementa
chlorine)
a) 17 neutrons 35 protons 36 electrons
b) 35 neutrons 17 protons 18 electrons
c) 18 neutrons 17 protons 17 electrons
d) 18 neutrons 17 protons 18 electrons
e) 17 neutrons 17 protons 17 electrons
9 Rubidium (Rb) possesses two stable isotopes and has an average atomic mass of 855 gmol If oneisotope of Rb has a mass of 849 gmol and a percent abundance of 722 than what is the mass of
the other Rb isotope
a) 861 gmol
b) 857 gmol
c) 883 gmol
d) 871 gmol
e) 894 gmol
10 What is the name of the column in the period table that contains Iodine
a) Metals
b) Metalloids
c) Noble gasses
d) Halogens
e) Actinides
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11 How many atoms of hydrogen are present in 68 x 102 g of hydrogen peroxide H2O2
a) 24 x 1025 atoms
b) 121 x 1025 atoms
c) 12 x 1025
atomsd) 241 x 1025 atoms
e) 12 x 1020 atoms
12 A lead (Pb) cube that is 300 cm on each side contains 891 x 1023 atoms What is the density of this
cube in gcm3
a) 341 gcm3
b) 114 gcm3
c) 00550 gcm3
d) 0990 gcm3
e) 267 gcm3
13 Which set of pure substances represent molecular elements
a) CO N2 H2 P4S10
b) I2 P4 N2 H2O
c) CO N2 H2 P4
d) O2 N2 H2 Ne
e) I2 N2 P4 H2
14 How many of the following chemical species are represented by their empirical formula
(NH4)2SO3 CO2 B2H6 C6H12O6 C6H6
a) 1
b) 2
c) 3
d) 4
e) 5
15 Which formula name combination listed below is incorrect
a) HClO4 (aq) perchloric acid
b) K2Cr2O7 potassium chromatec) NaC2H3O2 sodium acetate
d) Li3PO410H2O lithium phosphate decahydrate
e) N2O dinitrogen monoxide
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16 Calculate the total number of atoms present in 00346 g of morphine acetate (C19H23NO5)
a) 290 times 1019
b) 603 times 1021
c) 603 times 1019
d) 290 times 1021
e) 139 times 1021
17 The correct chemical formula for manganese (II) sulfate pentahydrate is
a) Mg(SO4)25H2O
b) MnSO45H2O
c) Mn(HSO4)27H2O
d) MnSO35H2O
e) Mn(SO4)210H2O
18 How many of the following compounds are ionic
N2O5 ICl4 PBr3 C12H22O11
a) None
b) 1
c) 2
d) 3
e) 4
19 A sugar crystal contains 18 times 1017 sucrose (C12H22O11) molecules What is the mass of the sugar
crystal in mg
a) 10 mg
b) 10 mg
c) 010 mg
d) 110 mg
e) Not enough information is provided to answer the question
20 A metal hydroxide with the formula M(OH)2 contains 5486 oxygen by mass Which of the
following metals is present in this compound
a) Mgb) Ca
c) Na
d) Zn
e) Be
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21 In the compound having the molecular formula C6H12O6 what is the percent mass composition of
each element listed in the order C H and O (Hint Assume that you have 1 mole of C6H12O6)
a) 6 12 6
b) 67 400 533
c) 400 533 67 d) 400 67 533
e) 234 359 600
22 What are the stoichiometric coefficients (a b c d ) for the following chemical reaction
a C2H4(g) + b O2(g) c H2O(l) + d CO2(g)
a) 1 3 2 2
b) 2 3 1 2
c) 3 2 2 2
d) 2 1 1 1
e) 1 2 3 1
23 Given the following balanced equation how many moles of F2 are needed to produce 200 moles of
PF3 if the reaction has a 78 yield (Assume that P4(s) is present in excess)
P4(s) + 6F2(g) 4PF3(g)
a) 100
b) 200
c) 385
d) 412
e) 600
24 The empirical formula of a compound is NPCl2 If the (molecular) molar mass of the compound is
34764 gmol what is the molecular formula of the compound
a) NPCl2
b) N2P2Cl4
c) N3P3Cl6
d) N4P4Cl8
e) N5P5Cl10
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25 What is the maximum number of moles of SO2 that can be obtained when a mixture of 30 g of CS 2(g
and 60 g of O2(g) is reacted according to the following balanced equation
CS2(g) + 3O2(g) CO2(g) + 2SO2(g)
a) 0039 moles
b) 0079 molesc) 0125 moles
d) 0175 moles
e) 0375 moles
26 What mass of CO2 is needed to produce 180 g of glucose during photosynthesis
Given 6CO2(g) + 6H2O(l) 6O2(g) + C6H12O6(aq) (Assume that H2O(l) is present in excess)
a) 440 g
b) 180 g
c) 264 gd) 372 g
e) 512 g
27 Table salt (sodium chloride) is 391 sodium by mass How many grams of table salt contain 720 g o
sodium
a) 282 g
b) 720 g
c) 102 g
d) 2820 g
e) 184 x 102 g
28 What is the maximum amount of solid lead (II) iodide (PbI2) that can be made from mixing a 100 mL
solution of 010 M lead (II) nitrate (Pb(NO3)2)and a 100 mL solution of 010 M potassium iodide (KI)
(Hint write a balanced equation)
a) 0010 moles
b) 0020 moles
c) 00050 moles
d) 0040 moles
e) 0 moles ndash no precipitate will form
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29 What mass of CoCl26H2O needs to be dissolved in water to make 255 mL of a 00100 M solution of
CoCl2(aq)
a) 0316 g
b) 0607 g
c) 0947 gd) 0101 g
e) 200 g
30 How much water would you need to add to 200 L of a 0250 M NaCl solution in order to make a NaC
solution having a final concentration of 0100 M
a) 100 L
b) 700 L
c) 300 L
d) 200 L
e) 500 L
31 Which of the following is true of a 010 M sodium sulfate solution
a) It is a non-electrolyte solution
b) The concentration of sodium cations and sulfate anions will be equal
c) The solution will not conduct electricity
d) The concentration of sodium ions will be 020 M
e) This would be an acidic solution
32 When a 010 M solution of Ba(ClO4)2 is mixed with a 010 M solution of ZnSO4 what will happen
a) Barium sulfate will precipitate
b) Zinc perchlorate will precipitate
c) There will be no precipitate
d) Zinc chlorate will precipitate
e) Not enough information to answer the question
33 Which are the spectator ions in a reaction between AgNO3(aq) and LiCl(aq)
a) Ag1+ (aq) and Cl- (aq)
b) Li+ (aq) and NO32- (aq)c) Li+ (aq) and NO3- (aq)
d) All of the ions are spectator ions no reaction occurs
e) None of the ions are spectator ions
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34 What is the net ionic equation for the reaction of NaOH(aq) and HCl(aq)
a) NaOH (aq) + HCl (aq) H2O (l) + NaCl (aq)
b) OH- (aq) + H+ (aq) H2O (l)
c) NaOH (aq) + HCl (aq) NaClH2O (s)d) Na+ (aq) + Cl- (aq) NaCl (aq)
e) OH- (aq) + Cl- (aq) HOCl (aq)
35 The balanced chemical equation presented below describes the acid-base neutralization reactio
between HCl(aq) and Ba(OH)2(aq) Determine the concentration of a 1500 mL HCl(aq) solution tha
would be needed to neutralize 2000 mL of Ba(OH)2(aq) which has a concentration of 0400 molL
2HCl(aq) + Ba(OH)2(aq) BaCl2(aq) + 2H2O(l)
a) 0533 molLb) 107 molL
c) 267 molL
d) 0600 molL
e) 267 molL
36 Identify the final products (in proper stoichiometric proportions) that would be formed when
Na2CO3(aq) reacts with HI(aq)
a) H2CO3(aq) + CO2(g) + HI(aq)b) H2CO3(aq) + NaI(aq)
c) H2O(l) + CO2(g) + 2NaI(aq)
d) H2O(l) + NaI(aq) + CO(g)
e) NaI2(aq) + H2CO3(aq) + H2O(l)
37 How many of the following compounds contain S having an oxidation state of 6+ H2S H2SO4 H2SO3
Fe2(SO4)3 CaSO3
a) 1
b) 2
c) 3d) 4
e) 5
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38 Identify the reducing agent in the following balanced REDOX reaction
4SrO(s) + 2Fe2O3(s) + O2(g) 4SrFeO3(s)
a) SrO
b) Fe2O3
c) O2 d) SrFeO3
e) None of the compounds are a reducing agent as this is not a REDOX reaction
39 How many of the following balanced equations describe REDOX reactions
i) 2CaO(s) + Fe2O3(s) Ca2Fe2O5(s)
ii) 2C6H14(l) + 19O2(g) 12CO2(g) + 14H2O(g)
iii) K2SO3(aq) + 2HCl(aq) 2KCl(aq) + H2O(l) + SO2(g)
iv) TiO2(s) + 2C(s) Ti(s) + 2CO(g)
a) 0
b) 1
c) 2
d) 3
e) 4
40 Which statement below correctly describes Avogadrorsquos Law
a) For a fixed amount of gas at a constant temperature the gas volume is inversely proportional to gas
pressure
b) For a fixed amount of gas at constant pressure the volume is directly proportional to the
temperature
c) For a fixed temperature and pressure the volume of a gas is directly proportional to the number of
gas molecules
d) All of the above statements correctly describe Avogadrorsquos Law
e) None of the above statement s correctly describe Avogadrorsquos Law
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41 The following reaction is used to generate hydrogen gas in the laboratory If a 243 mL sample of hydrogen
gas is collected over water at 298 K at a pressure of 745 mm Hg what mass of hydrogen has been produced
The vapor pressure of water at 298 K is 2378 mm Hg Assume ideality
Mg(s) + 2 HCl(aq) rarr MgCl2(aq) + H2(g)
a) 00196 g b) 00717 gc) 00190 g
d) 00144 g
e) None of the above
42 At STP a sample of gas occupies a volume of 678 mL Assuming ideality what would its volume be at
500 oC and 0808 atm
a) 854 mL
b) 783 mL
c) 587 mLd) 538 mL
e) none of the above
43 A gaseous mixture of helium and hydrogen is 600 helium by mass The total pressure of a sample of this
mixture is 100 atm What is the partial pressure of hydrogen in this sample
a) 0400
b) 0430c) 0570
d) 0600e) Need more information to answer
44 In the Van der Waals equation (below) the term +a(nV)2 accounts for the fact that in a real gas
a) the particles have a finite mass
b) the particles attract each otherc) the particles are non-linear
d) the particles have a finite size
e) none of the above is true
45 A gas sample has a pressure of
216 atm The temperature (in K) of the sample is increased by a factor of three and it is compressed to half its previous volume Assuming ideality the pressure is now
a) 0360 atm
b) 130 atm
c) 324 atmd) 114 atm
e) Cannot answer without more information
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11A
Periodic Table of the Elements8
1
H100794
22A
133A
144A
155A
166A
177A
H4
3
Li
6941
4
Be
901218
5
B
10811
6
C
12011
7
N
140067
8
O
159994
9
F
189984
N2
11
Na
229898
12
Mg
243050
33B
44B
55B
66B
77B
88B
98B
108B
111B
122B
13
Al
269815
14
Si
280855
15
P
309738
16
S
32066
17
Cl
354527
A3
19
K 390983
20
Ca
40078
21
Sc
449559
22
Ti
4788
23
V 509415
24
Cr
519961
25
Mn
549381
26
Fe
55847
27
Co
589332
28
Ni
58693
29
Cu
63546
30
Zn
6539
31
Ga
69723
32
Ge
7261
33
As
749216
34
Se
7896
35
Br
79904
K
37
Rb
854678
38
Sr
8762
39
Y 889059
40
Zr
91224
41
Nb
929064
42
Mo
9594
43
Tc
(98)
44
Ru
10107
45
Rh
102906
46
Pd
10642
47
Ag
107868
48
Cd
112411
49
In
114818
50
Sn
118710
51
Sb
121757
52
Te
12760
53
I
126904
X1
55
Cs
132905
56
Ba
137327
57
La
138906
72
Hf 17849
73
Ta
180948
74
W
18384
75
Re
186207
76
Os
19023
77
Ir
19222
78
Pt
19508
79
Au
196967
80
Hg
20059
81
Tl
204383
82
Pb
2072
83
Bi
208980
84
Po
(209)
85
At
(210)
R
87
Fr
(223)
88
Ra
226025
89
Ac
227028
104
Rf (261)
105
Db
(262)
106
Sg
(263)
107
Bh
(262)
108
Hs
(265)
109
Mt
(266)
110
(269)
111
(272)
112
(272)
114
(287)
116
(289)
58
Ce
140115
59
Pr
140908
60
Nd
14424
61
Pm
(145)
62
Sm
15036
63
Eu
151965
64
Gd
15725
65
Tb
158925
66
Dy
16250
67
Ho
164930
68
Er
16726
69
Tm
168934
70
Yb
17304
L1
90
Th
232038
91
Pa
231036
92
U
238029
93
Np
237048
94
Pu
(244)
95
Am
(243)
96
Cm
(247)
97
Bk (247)
98
Cf (251)
99
Es
(252)
100
Fm
(257)
101
Md
(258)
102
No
(259)
L
Physical Constants
Constant Symbol Value
Atomic mass unit u 16605 times 10-27 kg Avogadro number N A 60221 times 1023 mol-1
Gas Constant R 0082058 L atm mol-1K -1 83145 J K -1 mol-1 62364 L mmHg mol-1 K -1
Molar volume of an ideal gas at STP V m 22414 L mol-1
Electron mass m e 9109 times 10-31 Kg
Some SI Derived Units
Physical Quantity Unit Symbol Definition
Force Newton N kg m s-2
Energy Joule J kg m2 s-2 Pressure Pascal Pa N m-2 = kg m-1 s-2
STP Conditions P = 1 atm = 760 torr = 760 mmHg = 101325 kPa
Temperature = 0 ordmC = 27315 K
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2
6 A biker rides at an average speed of 25 km per hour How many minutes will it take for this biker to
ride a distance of 20 km
a) 25 min
b) 32 min
c) 38 mind) 42 min
e) 48 min
7 Which of the following statements is incorrect about the nuclear theory of the atom proposed by
Rutherford
a) Most of the mass of an atom is contained in the nucleus
b) The atom is mostly empty space
c) The number of neutrons and electrons in the atom are equal
d) The nucleus is surrounded by a cloud of electrons
e) The number of protons and electrons in the atom are equal
8 How many neutrons protons and electrons are found in 35Cl (NOTE 35Cl is an isotope of elementa
chlorine)
a) 17 neutrons 35 protons 36 electrons
b) 35 neutrons 17 protons 18 electrons
c) 18 neutrons 17 protons 17 electrons
d) 18 neutrons 17 protons 18 electrons
e) 17 neutrons 17 protons 17 electrons
9 Rubidium (Rb) possesses two stable isotopes and has an average atomic mass of 855 gmol If oneisotope of Rb has a mass of 849 gmol and a percent abundance of 722 than what is the mass of
the other Rb isotope
a) 861 gmol
b) 857 gmol
c) 883 gmol
d) 871 gmol
e) 894 gmol
10 What is the name of the column in the period table that contains Iodine
a) Metals
b) Metalloids
c) Noble gasses
d) Halogens
e) Actinides
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3
11 How many atoms of hydrogen are present in 68 x 102 g of hydrogen peroxide H2O2
a) 24 x 1025 atoms
b) 121 x 1025 atoms
c) 12 x 1025
atomsd) 241 x 1025 atoms
e) 12 x 1020 atoms
12 A lead (Pb) cube that is 300 cm on each side contains 891 x 1023 atoms What is the density of this
cube in gcm3
a) 341 gcm3
b) 114 gcm3
c) 00550 gcm3
d) 0990 gcm3
e) 267 gcm3
13 Which set of pure substances represent molecular elements
a) CO N2 H2 P4S10
b) I2 P4 N2 H2O
c) CO N2 H2 P4
d) O2 N2 H2 Ne
e) I2 N2 P4 H2
14 How many of the following chemical species are represented by their empirical formula
(NH4)2SO3 CO2 B2H6 C6H12O6 C6H6
a) 1
b) 2
c) 3
d) 4
e) 5
15 Which formula name combination listed below is incorrect
a) HClO4 (aq) perchloric acid
b) K2Cr2O7 potassium chromatec) NaC2H3O2 sodium acetate
d) Li3PO410H2O lithium phosphate decahydrate
e) N2O dinitrogen monoxide
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16 Calculate the total number of atoms present in 00346 g of morphine acetate (C19H23NO5)
a) 290 times 1019
b) 603 times 1021
c) 603 times 1019
d) 290 times 1021
e) 139 times 1021
17 The correct chemical formula for manganese (II) sulfate pentahydrate is
a) Mg(SO4)25H2O
b) MnSO45H2O
c) Mn(HSO4)27H2O
d) MnSO35H2O
e) Mn(SO4)210H2O
18 How many of the following compounds are ionic
N2O5 ICl4 PBr3 C12H22O11
a) None
b) 1
c) 2
d) 3
e) 4
19 A sugar crystal contains 18 times 1017 sucrose (C12H22O11) molecules What is the mass of the sugar
crystal in mg
a) 10 mg
b) 10 mg
c) 010 mg
d) 110 mg
e) Not enough information is provided to answer the question
20 A metal hydroxide with the formula M(OH)2 contains 5486 oxygen by mass Which of the
following metals is present in this compound
a) Mgb) Ca
c) Na
d) Zn
e) Be
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21 In the compound having the molecular formula C6H12O6 what is the percent mass composition of
each element listed in the order C H and O (Hint Assume that you have 1 mole of C6H12O6)
a) 6 12 6
b) 67 400 533
c) 400 533 67 d) 400 67 533
e) 234 359 600
22 What are the stoichiometric coefficients (a b c d ) for the following chemical reaction
a C2H4(g) + b O2(g) c H2O(l) + d CO2(g)
a) 1 3 2 2
b) 2 3 1 2
c) 3 2 2 2
d) 2 1 1 1
e) 1 2 3 1
23 Given the following balanced equation how many moles of F2 are needed to produce 200 moles of
PF3 if the reaction has a 78 yield (Assume that P4(s) is present in excess)
P4(s) + 6F2(g) 4PF3(g)
a) 100
b) 200
c) 385
d) 412
e) 600
24 The empirical formula of a compound is NPCl2 If the (molecular) molar mass of the compound is
34764 gmol what is the molecular formula of the compound
a) NPCl2
b) N2P2Cl4
c) N3P3Cl6
d) N4P4Cl8
e) N5P5Cl10
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25 What is the maximum number of moles of SO2 that can be obtained when a mixture of 30 g of CS 2(g
and 60 g of O2(g) is reacted according to the following balanced equation
CS2(g) + 3O2(g) CO2(g) + 2SO2(g)
a) 0039 moles
b) 0079 molesc) 0125 moles
d) 0175 moles
e) 0375 moles
26 What mass of CO2 is needed to produce 180 g of glucose during photosynthesis
Given 6CO2(g) + 6H2O(l) 6O2(g) + C6H12O6(aq) (Assume that H2O(l) is present in excess)
a) 440 g
b) 180 g
c) 264 gd) 372 g
e) 512 g
27 Table salt (sodium chloride) is 391 sodium by mass How many grams of table salt contain 720 g o
sodium
a) 282 g
b) 720 g
c) 102 g
d) 2820 g
e) 184 x 102 g
28 What is the maximum amount of solid lead (II) iodide (PbI2) that can be made from mixing a 100 mL
solution of 010 M lead (II) nitrate (Pb(NO3)2)and a 100 mL solution of 010 M potassium iodide (KI)
(Hint write a balanced equation)
a) 0010 moles
b) 0020 moles
c) 00050 moles
d) 0040 moles
e) 0 moles ndash no precipitate will form
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29 What mass of CoCl26H2O needs to be dissolved in water to make 255 mL of a 00100 M solution of
CoCl2(aq)
a) 0316 g
b) 0607 g
c) 0947 gd) 0101 g
e) 200 g
30 How much water would you need to add to 200 L of a 0250 M NaCl solution in order to make a NaC
solution having a final concentration of 0100 M
a) 100 L
b) 700 L
c) 300 L
d) 200 L
e) 500 L
31 Which of the following is true of a 010 M sodium sulfate solution
a) It is a non-electrolyte solution
b) The concentration of sodium cations and sulfate anions will be equal
c) The solution will not conduct electricity
d) The concentration of sodium ions will be 020 M
e) This would be an acidic solution
32 When a 010 M solution of Ba(ClO4)2 is mixed with a 010 M solution of ZnSO4 what will happen
a) Barium sulfate will precipitate
b) Zinc perchlorate will precipitate
c) There will be no precipitate
d) Zinc chlorate will precipitate
e) Not enough information to answer the question
33 Which are the spectator ions in a reaction between AgNO3(aq) and LiCl(aq)
a) Ag1+ (aq) and Cl- (aq)
b) Li+ (aq) and NO32- (aq)c) Li+ (aq) and NO3- (aq)
d) All of the ions are spectator ions no reaction occurs
e) None of the ions are spectator ions
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34 What is the net ionic equation for the reaction of NaOH(aq) and HCl(aq)
a) NaOH (aq) + HCl (aq) H2O (l) + NaCl (aq)
b) OH- (aq) + H+ (aq) H2O (l)
c) NaOH (aq) + HCl (aq) NaClH2O (s)d) Na+ (aq) + Cl- (aq) NaCl (aq)
e) OH- (aq) + Cl- (aq) HOCl (aq)
35 The balanced chemical equation presented below describes the acid-base neutralization reactio
between HCl(aq) and Ba(OH)2(aq) Determine the concentration of a 1500 mL HCl(aq) solution tha
would be needed to neutralize 2000 mL of Ba(OH)2(aq) which has a concentration of 0400 molL
2HCl(aq) + Ba(OH)2(aq) BaCl2(aq) + 2H2O(l)
a) 0533 molLb) 107 molL
c) 267 molL
d) 0600 molL
e) 267 molL
36 Identify the final products (in proper stoichiometric proportions) that would be formed when
Na2CO3(aq) reacts with HI(aq)
a) H2CO3(aq) + CO2(g) + HI(aq)b) H2CO3(aq) + NaI(aq)
c) H2O(l) + CO2(g) + 2NaI(aq)
d) H2O(l) + NaI(aq) + CO(g)
e) NaI2(aq) + H2CO3(aq) + H2O(l)
37 How many of the following compounds contain S having an oxidation state of 6+ H2S H2SO4 H2SO3
Fe2(SO4)3 CaSO3
a) 1
b) 2
c) 3d) 4
e) 5
7212019 Chem 114 Sample Midterm Exam
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9
38 Identify the reducing agent in the following balanced REDOX reaction
4SrO(s) + 2Fe2O3(s) + O2(g) 4SrFeO3(s)
a) SrO
b) Fe2O3
c) O2 d) SrFeO3
e) None of the compounds are a reducing agent as this is not a REDOX reaction
39 How many of the following balanced equations describe REDOX reactions
i) 2CaO(s) + Fe2O3(s) Ca2Fe2O5(s)
ii) 2C6H14(l) + 19O2(g) 12CO2(g) + 14H2O(g)
iii) K2SO3(aq) + 2HCl(aq) 2KCl(aq) + H2O(l) + SO2(g)
iv) TiO2(s) + 2C(s) Ti(s) + 2CO(g)
a) 0
b) 1
c) 2
d) 3
e) 4
40 Which statement below correctly describes Avogadrorsquos Law
a) For a fixed amount of gas at a constant temperature the gas volume is inversely proportional to gas
pressure
b) For a fixed amount of gas at constant pressure the volume is directly proportional to the
temperature
c) For a fixed temperature and pressure the volume of a gas is directly proportional to the number of
gas molecules
d) All of the above statements correctly describe Avogadrorsquos Law
e) None of the above statement s correctly describe Avogadrorsquos Law
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 1011
10
41 The following reaction is used to generate hydrogen gas in the laboratory If a 243 mL sample of hydrogen
gas is collected over water at 298 K at a pressure of 745 mm Hg what mass of hydrogen has been produced
The vapor pressure of water at 298 K is 2378 mm Hg Assume ideality
Mg(s) + 2 HCl(aq) rarr MgCl2(aq) + H2(g)
a) 00196 g b) 00717 gc) 00190 g
d) 00144 g
e) None of the above
42 At STP a sample of gas occupies a volume of 678 mL Assuming ideality what would its volume be at
500 oC and 0808 atm
a) 854 mL
b) 783 mL
c) 587 mLd) 538 mL
e) none of the above
43 A gaseous mixture of helium and hydrogen is 600 helium by mass The total pressure of a sample of this
mixture is 100 atm What is the partial pressure of hydrogen in this sample
a) 0400
b) 0430c) 0570
d) 0600e) Need more information to answer
44 In the Van der Waals equation (below) the term +a(nV)2 accounts for the fact that in a real gas
a) the particles have a finite mass
b) the particles attract each otherc) the particles are non-linear
d) the particles have a finite size
e) none of the above is true
45 A gas sample has a pressure of
216 atm The temperature (in K) of the sample is increased by a factor of three and it is compressed to half its previous volume Assuming ideality the pressure is now
a) 0360 atm
b) 130 atm
c) 324 atmd) 114 atm
e) Cannot answer without more information
7212019 Chem 114 Sample Midterm Exam
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11
11A
Periodic Table of the Elements8
1
H100794
22A
133A
144A
155A
166A
177A
H4
3
Li
6941
4
Be
901218
5
B
10811
6
C
12011
7
N
140067
8
O
159994
9
F
189984
N2
11
Na
229898
12
Mg
243050
33B
44B
55B
66B
77B
88B
98B
108B
111B
122B
13
Al
269815
14
Si
280855
15
P
309738
16
S
32066
17
Cl
354527
A3
19
K 390983
20
Ca
40078
21
Sc
449559
22
Ti
4788
23
V 509415
24
Cr
519961
25
Mn
549381
26
Fe
55847
27
Co
589332
28
Ni
58693
29
Cu
63546
30
Zn
6539
31
Ga
69723
32
Ge
7261
33
As
749216
34
Se
7896
35
Br
79904
K
37
Rb
854678
38
Sr
8762
39
Y 889059
40
Zr
91224
41
Nb
929064
42
Mo
9594
43
Tc
(98)
44
Ru
10107
45
Rh
102906
46
Pd
10642
47
Ag
107868
48
Cd
112411
49
In
114818
50
Sn
118710
51
Sb
121757
52
Te
12760
53
I
126904
X1
55
Cs
132905
56
Ba
137327
57
La
138906
72
Hf 17849
73
Ta
180948
74
W
18384
75
Re
186207
76
Os
19023
77
Ir
19222
78
Pt
19508
79
Au
196967
80
Hg
20059
81
Tl
204383
82
Pb
2072
83
Bi
208980
84
Po
(209)
85
At
(210)
R
87
Fr
(223)
88
Ra
226025
89
Ac
227028
104
Rf (261)
105
Db
(262)
106
Sg
(263)
107
Bh
(262)
108
Hs
(265)
109
Mt
(266)
110
(269)
111
(272)
112
(272)
114
(287)
116
(289)
58
Ce
140115
59
Pr
140908
60
Nd
14424
61
Pm
(145)
62
Sm
15036
63
Eu
151965
64
Gd
15725
65
Tb
158925
66
Dy
16250
67
Ho
164930
68
Er
16726
69
Tm
168934
70
Yb
17304
L1
90
Th
232038
91
Pa
231036
92
U
238029
93
Np
237048
94
Pu
(244)
95
Am
(243)
96
Cm
(247)
97
Bk (247)
98
Cf (251)
99
Es
(252)
100
Fm
(257)
101
Md
(258)
102
No
(259)
L
Physical Constants
Constant Symbol Value
Atomic mass unit u 16605 times 10-27 kg Avogadro number N A 60221 times 1023 mol-1
Gas Constant R 0082058 L atm mol-1K -1 83145 J K -1 mol-1 62364 L mmHg mol-1 K -1
Molar volume of an ideal gas at STP V m 22414 L mol-1
Electron mass m e 9109 times 10-31 Kg
Some SI Derived Units
Physical Quantity Unit Symbol Definition
Force Newton N kg m s-2
Energy Joule J kg m2 s-2 Pressure Pascal Pa N m-2 = kg m-1 s-2
STP Conditions P = 1 atm = 760 torr = 760 mmHg = 101325 kPa
Temperature = 0 ordmC = 27315 K
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 311
3
11 How many atoms of hydrogen are present in 68 x 102 g of hydrogen peroxide H2O2
a) 24 x 1025 atoms
b) 121 x 1025 atoms
c) 12 x 1025
atomsd) 241 x 1025 atoms
e) 12 x 1020 atoms
12 A lead (Pb) cube that is 300 cm on each side contains 891 x 1023 atoms What is the density of this
cube in gcm3
a) 341 gcm3
b) 114 gcm3
c) 00550 gcm3
d) 0990 gcm3
e) 267 gcm3
13 Which set of pure substances represent molecular elements
a) CO N2 H2 P4S10
b) I2 P4 N2 H2O
c) CO N2 H2 P4
d) O2 N2 H2 Ne
e) I2 N2 P4 H2
14 How many of the following chemical species are represented by their empirical formula
(NH4)2SO3 CO2 B2H6 C6H12O6 C6H6
a) 1
b) 2
c) 3
d) 4
e) 5
15 Which formula name combination listed below is incorrect
a) HClO4 (aq) perchloric acid
b) K2Cr2O7 potassium chromatec) NaC2H3O2 sodium acetate
d) Li3PO410H2O lithium phosphate decahydrate
e) N2O dinitrogen monoxide
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 411
4
16 Calculate the total number of atoms present in 00346 g of morphine acetate (C19H23NO5)
a) 290 times 1019
b) 603 times 1021
c) 603 times 1019
d) 290 times 1021
e) 139 times 1021
17 The correct chemical formula for manganese (II) sulfate pentahydrate is
a) Mg(SO4)25H2O
b) MnSO45H2O
c) Mn(HSO4)27H2O
d) MnSO35H2O
e) Mn(SO4)210H2O
18 How many of the following compounds are ionic
N2O5 ICl4 PBr3 C12H22O11
a) None
b) 1
c) 2
d) 3
e) 4
19 A sugar crystal contains 18 times 1017 sucrose (C12H22O11) molecules What is the mass of the sugar
crystal in mg
a) 10 mg
b) 10 mg
c) 010 mg
d) 110 mg
e) Not enough information is provided to answer the question
20 A metal hydroxide with the formula M(OH)2 contains 5486 oxygen by mass Which of the
following metals is present in this compound
a) Mgb) Ca
c) Na
d) Zn
e) Be
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 511
5
21 In the compound having the molecular formula C6H12O6 what is the percent mass composition of
each element listed in the order C H and O (Hint Assume that you have 1 mole of C6H12O6)
a) 6 12 6
b) 67 400 533
c) 400 533 67 d) 400 67 533
e) 234 359 600
22 What are the stoichiometric coefficients (a b c d ) for the following chemical reaction
a C2H4(g) + b O2(g) c H2O(l) + d CO2(g)
a) 1 3 2 2
b) 2 3 1 2
c) 3 2 2 2
d) 2 1 1 1
e) 1 2 3 1
23 Given the following balanced equation how many moles of F2 are needed to produce 200 moles of
PF3 if the reaction has a 78 yield (Assume that P4(s) is present in excess)
P4(s) + 6F2(g) 4PF3(g)
a) 100
b) 200
c) 385
d) 412
e) 600
24 The empirical formula of a compound is NPCl2 If the (molecular) molar mass of the compound is
34764 gmol what is the molecular formula of the compound
a) NPCl2
b) N2P2Cl4
c) N3P3Cl6
d) N4P4Cl8
e) N5P5Cl10
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 611
6
25 What is the maximum number of moles of SO2 that can be obtained when a mixture of 30 g of CS 2(g
and 60 g of O2(g) is reacted according to the following balanced equation
CS2(g) + 3O2(g) CO2(g) + 2SO2(g)
a) 0039 moles
b) 0079 molesc) 0125 moles
d) 0175 moles
e) 0375 moles
26 What mass of CO2 is needed to produce 180 g of glucose during photosynthesis
Given 6CO2(g) + 6H2O(l) 6O2(g) + C6H12O6(aq) (Assume that H2O(l) is present in excess)
a) 440 g
b) 180 g
c) 264 gd) 372 g
e) 512 g
27 Table salt (sodium chloride) is 391 sodium by mass How many grams of table salt contain 720 g o
sodium
a) 282 g
b) 720 g
c) 102 g
d) 2820 g
e) 184 x 102 g
28 What is the maximum amount of solid lead (II) iodide (PbI2) that can be made from mixing a 100 mL
solution of 010 M lead (II) nitrate (Pb(NO3)2)and a 100 mL solution of 010 M potassium iodide (KI)
(Hint write a balanced equation)
a) 0010 moles
b) 0020 moles
c) 00050 moles
d) 0040 moles
e) 0 moles ndash no precipitate will form
7212019 Chem 114 Sample Midterm Exam
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7
29 What mass of CoCl26H2O needs to be dissolved in water to make 255 mL of a 00100 M solution of
CoCl2(aq)
a) 0316 g
b) 0607 g
c) 0947 gd) 0101 g
e) 200 g
30 How much water would you need to add to 200 L of a 0250 M NaCl solution in order to make a NaC
solution having a final concentration of 0100 M
a) 100 L
b) 700 L
c) 300 L
d) 200 L
e) 500 L
31 Which of the following is true of a 010 M sodium sulfate solution
a) It is a non-electrolyte solution
b) The concentration of sodium cations and sulfate anions will be equal
c) The solution will not conduct electricity
d) The concentration of sodium ions will be 020 M
e) This would be an acidic solution
32 When a 010 M solution of Ba(ClO4)2 is mixed with a 010 M solution of ZnSO4 what will happen
a) Barium sulfate will precipitate
b) Zinc perchlorate will precipitate
c) There will be no precipitate
d) Zinc chlorate will precipitate
e) Not enough information to answer the question
33 Which are the spectator ions in a reaction between AgNO3(aq) and LiCl(aq)
a) Ag1+ (aq) and Cl- (aq)
b) Li+ (aq) and NO32- (aq)c) Li+ (aq) and NO3- (aq)
d) All of the ions are spectator ions no reaction occurs
e) None of the ions are spectator ions
7212019 Chem 114 Sample Midterm Exam
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8
34 What is the net ionic equation for the reaction of NaOH(aq) and HCl(aq)
a) NaOH (aq) + HCl (aq) H2O (l) + NaCl (aq)
b) OH- (aq) + H+ (aq) H2O (l)
c) NaOH (aq) + HCl (aq) NaClH2O (s)d) Na+ (aq) + Cl- (aq) NaCl (aq)
e) OH- (aq) + Cl- (aq) HOCl (aq)
35 The balanced chemical equation presented below describes the acid-base neutralization reactio
between HCl(aq) and Ba(OH)2(aq) Determine the concentration of a 1500 mL HCl(aq) solution tha
would be needed to neutralize 2000 mL of Ba(OH)2(aq) which has a concentration of 0400 molL
2HCl(aq) + Ba(OH)2(aq) BaCl2(aq) + 2H2O(l)
a) 0533 molLb) 107 molL
c) 267 molL
d) 0600 molL
e) 267 molL
36 Identify the final products (in proper stoichiometric proportions) that would be formed when
Na2CO3(aq) reacts with HI(aq)
a) H2CO3(aq) + CO2(g) + HI(aq)b) H2CO3(aq) + NaI(aq)
c) H2O(l) + CO2(g) + 2NaI(aq)
d) H2O(l) + NaI(aq) + CO(g)
e) NaI2(aq) + H2CO3(aq) + H2O(l)
37 How many of the following compounds contain S having an oxidation state of 6+ H2S H2SO4 H2SO3
Fe2(SO4)3 CaSO3
a) 1
b) 2
c) 3d) 4
e) 5
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 911
9
38 Identify the reducing agent in the following balanced REDOX reaction
4SrO(s) + 2Fe2O3(s) + O2(g) 4SrFeO3(s)
a) SrO
b) Fe2O3
c) O2 d) SrFeO3
e) None of the compounds are a reducing agent as this is not a REDOX reaction
39 How many of the following balanced equations describe REDOX reactions
i) 2CaO(s) + Fe2O3(s) Ca2Fe2O5(s)
ii) 2C6H14(l) + 19O2(g) 12CO2(g) + 14H2O(g)
iii) K2SO3(aq) + 2HCl(aq) 2KCl(aq) + H2O(l) + SO2(g)
iv) TiO2(s) + 2C(s) Ti(s) + 2CO(g)
a) 0
b) 1
c) 2
d) 3
e) 4
40 Which statement below correctly describes Avogadrorsquos Law
a) For a fixed amount of gas at a constant temperature the gas volume is inversely proportional to gas
pressure
b) For a fixed amount of gas at constant pressure the volume is directly proportional to the
temperature
c) For a fixed temperature and pressure the volume of a gas is directly proportional to the number of
gas molecules
d) All of the above statements correctly describe Avogadrorsquos Law
e) None of the above statement s correctly describe Avogadrorsquos Law
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 1011
10
41 The following reaction is used to generate hydrogen gas in the laboratory If a 243 mL sample of hydrogen
gas is collected over water at 298 K at a pressure of 745 mm Hg what mass of hydrogen has been produced
The vapor pressure of water at 298 K is 2378 mm Hg Assume ideality
Mg(s) + 2 HCl(aq) rarr MgCl2(aq) + H2(g)
a) 00196 g b) 00717 gc) 00190 g
d) 00144 g
e) None of the above
42 At STP a sample of gas occupies a volume of 678 mL Assuming ideality what would its volume be at
500 oC and 0808 atm
a) 854 mL
b) 783 mL
c) 587 mLd) 538 mL
e) none of the above
43 A gaseous mixture of helium and hydrogen is 600 helium by mass The total pressure of a sample of this
mixture is 100 atm What is the partial pressure of hydrogen in this sample
a) 0400
b) 0430c) 0570
d) 0600e) Need more information to answer
44 In the Van der Waals equation (below) the term +a(nV)2 accounts for the fact that in a real gas
a) the particles have a finite mass
b) the particles attract each otherc) the particles are non-linear
d) the particles have a finite size
e) none of the above is true
45 A gas sample has a pressure of
216 atm The temperature (in K) of the sample is increased by a factor of three and it is compressed to half its previous volume Assuming ideality the pressure is now
a) 0360 atm
b) 130 atm
c) 324 atmd) 114 atm
e) Cannot answer without more information
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 1111
11
11A
Periodic Table of the Elements8
1
H100794
22A
133A
144A
155A
166A
177A
H4
3
Li
6941
4
Be
901218
5
B
10811
6
C
12011
7
N
140067
8
O
159994
9
F
189984
N2
11
Na
229898
12
Mg
243050
33B
44B
55B
66B
77B
88B
98B
108B
111B
122B
13
Al
269815
14
Si
280855
15
P
309738
16
S
32066
17
Cl
354527
A3
19
K 390983
20
Ca
40078
21
Sc
449559
22
Ti
4788
23
V 509415
24
Cr
519961
25
Mn
549381
26
Fe
55847
27
Co
589332
28
Ni
58693
29
Cu
63546
30
Zn
6539
31
Ga
69723
32
Ge
7261
33
As
749216
34
Se
7896
35
Br
79904
K
37
Rb
854678
38
Sr
8762
39
Y 889059
40
Zr
91224
41
Nb
929064
42
Mo
9594
43
Tc
(98)
44
Ru
10107
45
Rh
102906
46
Pd
10642
47
Ag
107868
48
Cd
112411
49
In
114818
50
Sn
118710
51
Sb
121757
52
Te
12760
53
I
126904
X1
55
Cs
132905
56
Ba
137327
57
La
138906
72
Hf 17849
73
Ta
180948
74
W
18384
75
Re
186207
76
Os
19023
77
Ir
19222
78
Pt
19508
79
Au
196967
80
Hg
20059
81
Tl
204383
82
Pb
2072
83
Bi
208980
84
Po
(209)
85
At
(210)
R
87
Fr
(223)
88
Ra
226025
89
Ac
227028
104
Rf (261)
105
Db
(262)
106
Sg
(263)
107
Bh
(262)
108
Hs
(265)
109
Mt
(266)
110
(269)
111
(272)
112
(272)
114
(287)
116
(289)
58
Ce
140115
59
Pr
140908
60
Nd
14424
61
Pm
(145)
62
Sm
15036
63
Eu
151965
64
Gd
15725
65
Tb
158925
66
Dy
16250
67
Ho
164930
68
Er
16726
69
Tm
168934
70
Yb
17304
L1
90
Th
232038
91
Pa
231036
92
U
238029
93
Np
237048
94
Pu
(244)
95
Am
(243)
96
Cm
(247)
97
Bk (247)
98
Cf (251)
99
Es
(252)
100
Fm
(257)
101
Md
(258)
102
No
(259)
L
Physical Constants
Constant Symbol Value
Atomic mass unit u 16605 times 10-27 kg Avogadro number N A 60221 times 1023 mol-1
Gas Constant R 0082058 L atm mol-1K -1 83145 J K -1 mol-1 62364 L mmHg mol-1 K -1
Molar volume of an ideal gas at STP V m 22414 L mol-1
Electron mass m e 9109 times 10-31 Kg
Some SI Derived Units
Physical Quantity Unit Symbol Definition
Force Newton N kg m s-2
Energy Joule J kg m2 s-2 Pressure Pascal Pa N m-2 = kg m-1 s-2
STP Conditions P = 1 atm = 760 torr = 760 mmHg = 101325 kPa
Temperature = 0 ordmC = 27315 K
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 411
4
16 Calculate the total number of atoms present in 00346 g of morphine acetate (C19H23NO5)
a) 290 times 1019
b) 603 times 1021
c) 603 times 1019
d) 290 times 1021
e) 139 times 1021
17 The correct chemical formula for manganese (II) sulfate pentahydrate is
a) Mg(SO4)25H2O
b) MnSO45H2O
c) Mn(HSO4)27H2O
d) MnSO35H2O
e) Mn(SO4)210H2O
18 How many of the following compounds are ionic
N2O5 ICl4 PBr3 C12H22O11
a) None
b) 1
c) 2
d) 3
e) 4
19 A sugar crystal contains 18 times 1017 sucrose (C12H22O11) molecules What is the mass of the sugar
crystal in mg
a) 10 mg
b) 10 mg
c) 010 mg
d) 110 mg
e) Not enough information is provided to answer the question
20 A metal hydroxide with the formula M(OH)2 contains 5486 oxygen by mass Which of the
following metals is present in this compound
a) Mgb) Ca
c) Na
d) Zn
e) Be
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 511
5
21 In the compound having the molecular formula C6H12O6 what is the percent mass composition of
each element listed in the order C H and O (Hint Assume that you have 1 mole of C6H12O6)
a) 6 12 6
b) 67 400 533
c) 400 533 67 d) 400 67 533
e) 234 359 600
22 What are the stoichiometric coefficients (a b c d ) for the following chemical reaction
a C2H4(g) + b O2(g) c H2O(l) + d CO2(g)
a) 1 3 2 2
b) 2 3 1 2
c) 3 2 2 2
d) 2 1 1 1
e) 1 2 3 1
23 Given the following balanced equation how many moles of F2 are needed to produce 200 moles of
PF3 if the reaction has a 78 yield (Assume that P4(s) is present in excess)
P4(s) + 6F2(g) 4PF3(g)
a) 100
b) 200
c) 385
d) 412
e) 600
24 The empirical formula of a compound is NPCl2 If the (molecular) molar mass of the compound is
34764 gmol what is the molecular formula of the compound
a) NPCl2
b) N2P2Cl4
c) N3P3Cl6
d) N4P4Cl8
e) N5P5Cl10
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 611
6
25 What is the maximum number of moles of SO2 that can be obtained when a mixture of 30 g of CS 2(g
and 60 g of O2(g) is reacted according to the following balanced equation
CS2(g) + 3O2(g) CO2(g) + 2SO2(g)
a) 0039 moles
b) 0079 molesc) 0125 moles
d) 0175 moles
e) 0375 moles
26 What mass of CO2 is needed to produce 180 g of glucose during photosynthesis
Given 6CO2(g) + 6H2O(l) 6O2(g) + C6H12O6(aq) (Assume that H2O(l) is present in excess)
a) 440 g
b) 180 g
c) 264 gd) 372 g
e) 512 g
27 Table salt (sodium chloride) is 391 sodium by mass How many grams of table salt contain 720 g o
sodium
a) 282 g
b) 720 g
c) 102 g
d) 2820 g
e) 184 x 102 g
28 What is the maximum amount of solid lead (II) iodide (PbI2) that can be made from mixing a 100 mL
solution of 010 M lead (II) nitrate (Pb(NO3)2)and a 100 mL solution of 010 M potassium iodide (KI)
(Hint write a balanced equation)
a) 0010 moles
b) 0020 moles
c) 00050 moles
d) 0040 moles
e) 0 moles ndash no precipitate will form
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 711
7
29 What mass of CoCl26H2O needs to be dissolved in water to make 255 mL of a 00100 M solution of
CoCl2(aq)
a) 0316 g
b) 0607 g
c) 0947 gd) 0101 g
e) 200 g
30 How much water would you need to add to 200 L of a 0250 M NaCl solution in order to make a NaC
solution having a final concentration of 0100 M
a) 100 L
b) 700 L
c) 300 L
d) 200 L
e) 500 L
31 Which of the following is true of a 010 M sodium sulfate solution
a) It is a non-electrolyte solution
b) The concentration of sodium cations and sulfate anions will be equal
c) The solution will not conduct electricity
d) The concentration of sodium ions will be 020 M
e) This would be an acidic solution
32 When a 010 M solution of Ba(ClO4)2 is mixed with a 010 M solution of ZnSO4 what will happen
a) Barium sulfate will precipitate
b) Zinc perchlorate will precipitate
c) There will be no precipitate
d) Zinc chlorate will precipitate
e) Not enough information to answer the question
33 Which are the spectator ions in a reaction between AgNO3(aq) and LiCl(aq)
a) Ag1+ (aq) and Cl- (aq)
b) Li+ (aq) and NO32- (aq)c) Li+ (aq) and NO3- (aq)
d) All of the ions are spectator ions no reaction occurs
e) None of the ions are spectator ions
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 811
8
34 What is the net ionic equation for the reaction of NaOH(aq) and HCl(aq)
a) NaOH (aq) + HCl (aq) H2O (l) + NaCl (aq)
b) OH- (aq) + H+ (aq) H2O (l)
c) NaOH (aq) + HCl (aq) NaClH2O (s)d) Na+ (aq) + Cl- (aq) NaCl (aq)
e) OH- (aq) + Cl- (aq) HOCl (aq)
35 The balanced chemical equation presented below describes the acid-base neutralization reactio
between HCl(aq) and Ba(OH)2(aq) Determine the concentration of a 1500 mL HCl(aq) solution tha
would be needed to neutralize 2000 mL of Ba(OH)2(aq) which has a concentration of 0400 molL
2HCl(aq) + Ba(OH)2(aq) BaCl2(aq) + 2H2O(l)
a) 0533 molLb) 107 molL
c) 267 molL
d) 0600 molL
e) 267 molL
36 Identify the final products (in proper stoichiometric proportions) that would be formed when
Na2CO3(aq) reacts with HI(aq)
a) H2CO3(aq) + CO2(g) + HI(aq)b) H2CO3(aq) + NaI(aq)
c) H2O(l) + CO2(g) + 2NaI(aq)
d) H2O(l) + NaI(aq) + CO(g)
e) NaI2(aq) + H2CO3(aq) + H2O(l)
37 How many of the following compounds contain S having an oxidation state of 6+ H2S H2SO4 H2SO3
Fe2(SO4)3 CaSO3
a) 1
b) 2
c) 3d) 4
e) 5
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 911
9
38 Identify the reducing agent in the following balanced REDOX reaction
4SrO(s) + 2Fe2O3(s) + O2(g) 4SrFeO3(s)
a) SrO
b) Fe2O3
c) O2 d) SrFeO3
e) None of the compounds are a reducing agent as this is not a REDOX reaction
39 How many of the following balanced equations describe REDOX reactions
i) 2CaO(s) + Fe2O3(s) Ca2Fe2O5(s)
ii) 2C6H14(l) + 19O2(g) 12CO2(g) + 14H2O(g)
iii) K2SO3(aq) + 2HCl(aq) 2KCl(aq) + H2O(l) + SO2(g)
iv) TiO2(s) + 2C(s) Ti(s) + 2CO(g)
a) 0
b) 1
c) 2
d) 3
e) 4
40 Which statement below correctly describes Avogadrorsquos Law
a) For a fixed amount of gas at a constant temperature the gas volume is inversely proportional to gas
pressure
b) For a fixed amount of gas at constant pressure the volume is directly proportional to the
temperature
c) For a fixed temperature and pressure the volume of a gas is directly proportional to the number of
gas molecules
d) All of the above statements correctly describe Avogadrorsquos Law
e) None of the above statement s correctly describe Avogadrorsquos Law
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 1011
10
41 The following reaction is used to generate hydrogen gas in the laboratory If a 243 mL sample of hydrogen
gas is collected over water at 298 K at a pressure of 745 mm Hg what mass of hydrogen has been produced
The vapor pressure of water at 298 K is 2378 mm Hg Assume ideality
Mg(s) + 2 HCl(aq) rarr MgCl2(aq) + H2(g)
a) 00196 g b) 00717 gc) 00190 g
d) 00144 g
e) None of the above
42 At STP a sample of gas occupies a volume of 678 mL Assuming ideality what would its volume be at
500 oC and 0808 atm
a) 854 mL
b) 783 mL
c) 587 mLd) 538 mL
e) none of the above
43 A gaseous mixture of helium and hydrogen is 600 helium by mass The total pressure of a sample of this
mixture is 100 atm What is the partial pressure of hydrogen in this sample
a) 0400
b) 0430c) 0570
d) 0600e) Need more information to answer
44 In the Van der Waals equation (below) the term +a(nV)2 accounts for the fact that in a real gas
a) the particles have a finite mass
b) the particles attract each otherc) the particles are non-linear
d) the particles have a finite size
e) none of the above is true
45 A gas sample has a pressure of
216 atm The temperature (in K) of the sample is increased by a factor of three and it is compressed to half its previous volume Assuming ideality the pressure is now
a) 0360 atm
b) 130 atm
c) 324 atmd) 114 atm
e) Cannot answer without more information
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 1111
11
11A
Periodic Table of the Elements8
1
H100794
22A
133A
144A
155A
166A
177A
H4
3
Li
6941
4
Be
901218
5
B
10811
6
C
12011
7
N
140067
8
O
159994
9
F
189984
N2
11
Na
229898
12
Mg
243050
33B
44B
55B
66B
77B
88B
98B
108B
111B
122B
13
Al
269815
14
Si
280855
15
P
309738
16
S
32066
17
Cl
354527
A3
19
K 390983
20
Ca
40078
21
Sc
449559
22
Ti
4788
23
V 509415
24
Cr
519961
25
Mn
549381
26
Fe
55847
27
Co
589332
28
Ni
58693
29
Cu
63546
30
Zn
6539
31
Ga
69723
32
Ge
7261
33
As
749216
34
Se
7896
35
Br
79904
K
37
Rb
854678
38
Sr
8762
39
Y 889059
40
Zr
91224
41
Nb
929064
42
Mo
9594
43
Tc
(98)
44
Ru
10107
45
Rh
102906
46
Pd
10642
47
Ag
107868
48
Cd
112411
49
In
114818
50
Sn
118710
51
Sb
121757
52
Te
12760
53
I
126904
X1
55
Cs
132905
56
Ba
137327
57
La
138906
72
Hf 17849
73
Ta
180948
74
W
18384
75
Re
186207
76
Os
19023
77
Ir
19222
78
Pt
19508
79
Au
196967
80
Hg
20059
81
Tl
204383
82
Pb
2072
83
Bi
208980
84
Po
(209)
85
At
(210)
R
87
Fr
(223)
88
Ra
226025
89
Ac
227028
104
Rf (261)
105
Db
(262)
106
Sg
(263)
107
Bh
(262)
108
Hs
(265)
109
Mt
(266)
110
(269)
111
(272)
112
(272)
114
(287)
116
(289)
58
Ce
140115
59
Pr
140908
60
Nd
14424
61
Pm
(145)
62
Sm
15036
63
Eu
151965
64
Gd
15725
65
Tb
158925
66
Dy
16250
67
Ho
164930
68
Er
16726
69
Tm
168934
70
Yb
17304
L1
90
Th
232038
91
Pa
231036
92
U
238029
93
Np
237048
94
Pu
(244)
95
Am
(243)
96
Cm
(247)
97
Bk (247)
98
Cf (251)
99
Es
(252)
100
Fm
(257)
101
Md
(258)
102
No
(259)
L
Physical Constants
Constant Symbol Value
Atomic mass unit u 16605 times 10-27 kg Avogadro number N A 60221 times 1023 mol-1
Gas Constant R 0082058 L atm mol-1K -1 83145 J K -1 mol-1 62364 L mmHg mol-1 K -1
Molar volume of an ideal gas at STP V m 22414 L mol-1
Electron mass m e 9109 times 10-31 Kg
Some SI Derived Units
Physical Quantity Unit Symbol Definition
Force Newton N kg m s-2
Energy Joule J kg m2 s-2 Pressure Pascal Pa N m-2 = kg m-1 s-2
STP Conditions P = 1 atm = 760 torr = 760 mmHg = 101325 kPa
Temperature = 0 ordmC = 27315 K
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 511
5
21 In the compound having the molecular formula C6H12O6 what is the percent mass composition of
each element listed in the order C H and O (Hint Assume that you have 1 mole of C6H12O6)
a) 6 12 6
b) 67 400 533
c) 400 533 67 d) 400 67 533
e) 234 359 600
22 What are the stoichiometric coefficients (a b c d ) for the following chemical reaction
a C2H4(g) + b O2(g) c H2O(l) + d CO2(g)
a) 1 3 2 2
b) 2 3 1 2
c) 3 2 2 2
d) 2 1 1 1
e) 1 2 3 1
23 Given the following balanced equation how many moles of F2 are needed to produce 200 moles of
PF3 if the reaction has a 78 yield (Assume that P4(s) is present in excess)
P4(s) + 6F2(g) 4PF3(g)
a) 100
b) 200
c) 385
d) 412
e) 600
24 The empirical formula of a compound is NPCl2 If the (molecular) molar mass of the compound is
34764 gmol what is the molecular formula of the compound
a) NPCl2
b) N2P2Cl4
c) N3P3Cl6
d) N4P4Cl8
e) N5P5Cl10
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 611
6
25 What is the maximum number of moles of SO2 that can be obtained when a mixture of 30 g of CS 2(g
and 60 g of O2(g) is reacted according to the following balanced equation
CS2(g) + 3O2(g) CO2(g) + 2SO2(g)
a) 0039 moles
b) 0079 molesc) 0125 moles
d) 0175 moles
e) 0375 moles
26 What mass of CO2 is needed to produce 180 g of glucose during photosynthesis
Given 6CO2(g) + 6H2O(l) 6O2(g) + C6H12O6(aq) (Assume that H2O(l) is present in excess)
a) 440 g
b) 180 g
c) 264 gd) 372 g
e) 512 g
27 Table salt (sodium chloride) is 391 sodium by mass How many grams of table salt contain 720 g o
sodium
a) 282 g
b) 720 g
c) 102 g
d) 2820 g
e) 184 x 102 g
28 What is the maximum amount of solid lead (II) iodide (PbI2) that can be made from mixing a 100 mL
solution of 010 M lead (II) nitrate (Pb(NO3)2)and a 100 mL solution of 010 M potassium iodide (KI)
(Hint write a balanced equation)
a) 0010 moles
b) 0020 moles
c) 00050 moles
d) 0040 moles
e) 0 moles ndash no precipitate will form
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 711
7
29 What mass of CoCl26H2O needs to be dissolved in water to make 255 mL of a 00100 M solution of
CoCl2(aq)
a) 0316 g
b) 0607 g
c) 0947 gd) 0101 g
e) 200 g
30 How much water would you need to add to 200 L of a 0250 M NaCl solution in order to make a NaC
solution having a final concentration of 0100 M
a) 100 L
b) 700 L
c) 300 L
d) 200 L
e) 500 L
31 Which of the following is true of a 010 M sodium sulfate solution
a) It is a non-electrolyte solution
b) The concentration of sodium cations and sulfate anions will be equal
c) The solution will not conduct electricity
d) The concentration of sodium ions will be 020 M
e) This would be an acidic solution
32 When a 010 M solution of Ba(ClO4)2 is mixed with a 010 M solution of ZnSO4 what will happen
a) Barium sulfate will precipitate
b) Zinc perchlorate will precipitate
c) There will be no precipitate
d) Zinc chlorate will precipitate
e) Not enough information to answer the question
33 Which are the spectator ions in a reaction between AgNO3(aq) and LiCl(aq)
a) Ag1+ (aq) and Cl- (aq)
b) Li+ (aq) and NO32- (aq)c) Li+ (aq) and NO3- (aq)
d) All of the ions are spectator ions no reaction occurs
e) None of the ions are spectator ions
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 811
8
34 What is the net ionic equation for the reaction of NaOH(aq) and HCl(aq)
a) NaOH (aq) + HCl (aq) H2O (l) + NaCl (aq)
b) OH- (aq) + H+ (aq) H2O (l)
c) NaOH (aq) + HCl (aq) NaClH2O (s)d) Na+ (aq) + Cl- (aq) NaCl (aq)
e) OH- (aq) + Cl- (aq) HOCl (aq)
35 The balanced chemical equation presented below describes the acid-base neutralization reactio
between HCl(aq) and Ba(OH)2(aq) Determine the concentration of a 1500 mL HCl(aq) solution tha
would be needed to neutralize 2000 mL of Ba(OH)2(aq) which has a concentration of 0400 molL
2HCl(aq) + Ba(OH)2(aq) BaCl2(aq) + 2H2O(l)
a) 0533 molLb) 107 molL
c) 267 molL
d) 0600 molL
e) 267 molL
36 Identify the final products (in proper stoichiometric proportions) that would be formed when
Na2CO3(aq) reacts with HI(aq)
a) H2CO3(aq) + CO2(g) + HI(aq)b) H2CO3(aq) + NaI(aq)
c) H2O(l) + CO2(g) + 2NaI(aq)
d) H2O(l) + NaI(aq) + CO(g)
e) NaI2(aq) + H2CO3(aq) + H2O(l)
37 How many of the following compounds contain S having an oxidation state of 6+ H2S H2SO4 H2SO3
Fe2(SO4)3 CaSO3
a) 1
b) 2
c) 3d) 4
e) 5
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 911
9
38 Identify the reducing agent in the following balanced REDOX reaction
4SrO(s) + 2Fe2O3(s) + O2(g) 4SrFeO3(s)
a) SrO
b) Fe2O3
c) O2 d) SrFeO3
e) None of the compounds are a reducing agent as this is not a REDOX reaction
39 How many of the following balanced equations describe REDOX reactions
i) 2CaO(s) + Fe2O3(s) Ca2Fe2O5(s)
ii) 2C6H14(l) + 19O2(g) 12CO2(g) + 14H2O(g)
iii) K2SO3(aq) + 2HCl(aq) 2KCl(aq) + H2O(l) + SO2(g)
iv) TiO2(s) + 2C(s) Ti(s) + 2CO(g)
a) 0
b) 1
c) 2
d) 3
e) 4
40 Which statement below correctly describes Avogadrorsquos Law
a) For a fixed amount of gas at a constant temperature the gas volume is inversely proportional to gas
pressure
b) For a fixed amount of gas at constant pressure the volume is directly proportional to the
temperature
c) For a fixed temperature and pressure the volume of a gas is directly proportional to the number of
gas molecules
d) All of the above statements correctly describe Avogadrorsquos Law
e) None of the above statement s correctly describe Avogadrorsquos Law
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 1011
10
41 The following reaction is used to generate hydrogen gas in the laboratory If a 243 mL sample of hydrogen
gas is collected over water at 298 K at a pressure of 745 mm Hg what mass of hydrogen has been produced
The vapor pressure of water at 298 K is 2378 mm Hg Assume ideality
Mg(s) + 2 HCl(aq) rarr MgCl2(aq) + H2(g)
a) 00196 g b) 00717 gc) 00190 g
d) 00144 g
e) None of the above
42 At STP a sample of gas occupies a volume of 678 mL Assuming ideality what would its volume be at
500 oC and 0808 atm
a) 854 mL
b) 783 mL
c) 587 mLd) 538 mL
e) none of the above
43 A gaseous mixture of helium and hydrogen is 600 helium by mass The total pressure of a sample of this
mixture is 100 atm What is the partial pressure of hydrogen in this sample
a) 0400
b) 0430c) 0570
d) 0600e) Need more information to answer
44 In the Van der Waals equation (below) the term +a(nV)2 accounts for the fact that in a real gas
a) the particles have a finite mass
b) the particles attract each otherc) the particles are non-linear
d) the particles have a finite size
e) none of the above is true
45 A gas sample has a pressure of
216 atm The temperature (in K) of the sample is increased by a factor of three and it is compressed to half its previous volume Assuming ideality the pressure is now
a) 0360 atm
b) 130 atm
c) 324 atmd) 114 atm
e) Cannot answer without more information
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 1111
11
11A
Periodic Table of the Elements8
1
H100794
22A
133A
144A
155A
166A
177A
H4
3
Li
6941
4
Be
901218
5
B
10811
6
C
12011
7
N
140067
8
O
159994
9
F
189984
N2
11
Na
229898
12
Mg
243050
33B
44B
55B
66B
77B
88B
98B
108B
111B
122B
13
Al
269815
14
Si
280855
15
P
309738
16
S
32066
17
Cl
354527
A3
19
K 390983
20
Ca
40078
21
Sc
449559
22
Ti
4788
23
V 509415
24
Cr
519961
25
Mn
549381
26
Fe
55847
27
Co
589332
28
Ni
58693
29
Cu
63546
30
Zn
6539
31
Ga
69723
32
Ge
7261
33
As
749216
34
Se
7896
35
Br
79904
K
37
Rb
854678
38
Sr
8762
39
Y 889059
40
Zr
91224
41
Nb
929064
42
Mo
9594
43
Tc
(98)
44
Ru
10107
45
Rh
102906
46
Pd
10642
47
Ag
107868
48
Cd
112411
49
In
114818
50
Sn
118710
51
Sb
121757
52
Te
12760
53
I
126904
X1
55
Cs
132905
56
Ba
137327
57
La
138906
72
Hf 17849
73
Ta
180948
74
W
18384
75
Re
186207
76
Os
19023
77
Ir
19222
78
Pt
19508
79
Au
196967
80
Hg
20059
81
Tl
204383
82
Pb
2072
83
Bi
208980
84
Po
(209)
85
At
(210)
R
87
Fr
(223)
88
Ra
226025
89
Ac
227028
104
Rf (261)
105
Db
(262)
106
Sg
(263)
107
Bh
(262)
108
Hs
(265)
109
Mt
(266)
110
(269)
111
(272)
112
(272)
114
(287)
116
(289)
58
Ce
140115
59
Pr
140908
60
Nd
14424
61
Pm
(145)
62
Sm
15036
63
Eu
151965
64
Gd
15725
65
Tb
158925
66
Dy
16250
67
Ho
164930
68
Er
16726
69
Tm
168934
70
Yb
17304
L1
90
Th
232038
91
Pa
231036
92
U
238029
93
Np
237048
94
Pu
(244)
95
Am
(243)
96
Cm
(247)
97
Bk (247)
98
Cf (251)
99
Es
(252)
100
Fm
(257)
101
Md
(258)
102
No
(259)
L
Physical Constants
Constant Symbol Value
Atomic mass unit u 16605 times 10-27 kg Avogadro number N A 60221 times 1023 mol-1
Gas Constant R 0082058 L atm mol-1K -1 83145 J K -1 mol-1 62364 L mmHg mol-1 K -1
Molar volume of an ideal gas at STP V m 22414 L mol-1
Electron mass m e 9109 times 10-31 Kg
Some SI Derived Units
Physical Quantity Unit Symbol Definition
Force Newton N kg m s-2
Energy Joule J kg m2 s-2 Pressure Pascal Pa N m-2 = kg m-1 s-2
STP Conditions P = 1 atm = 760 torr = 760 mmHg = 101325 kPa
Temperature = 0 ordmC = 27315 K
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 611
6
25 What is the maximum number of moles of SO2 that can be obtained when a mixture of 30 g of CS 2(g
and 60 g of O2(g) is reacted according to the following balanced equation
CS2(g) + 3O2(g) CO2(g) + 2SO2(g)
a) 0039 moles
b) 0079 molesc) 0125 moles
d) 0175 moles
e) 0375 moles
26 What mass of CO2 is needed to produce 180 g of glucose during photosynthesis
Given 6CO2(g) + 6H2O(l) 6O2(g) + C6H12O6(aq) (Assume that H2O(l) is present in excess)
a) 440 g
b) 180 g
c) 264 gd) 372 g
e) 512 g
27 Table salt (sodium chloride) is 391 sodium by mass How many grams of table salt contain 720 g o
sodium
a) 282 g
b) 720 g
c) 102 g
d) 2820 g
e) 184 x 102 g
28 What is the maximum amount of solid lead (II) iodide (PbI2) that can be made from mixing a 100 mL
solution of 010 M lead (II) nitrate (Pb(NO3)2)and a 100 mL solution of 010 M potassium iodide (KI)
(Hint write a balanced equation)
a) 0010 moles
b) 0020 moles
c) 00050 moles
d) 0040 moles
e) 0 moles ndash no precipitate will form
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 711
7
29 What mass of CoCl26H2O needs to be dissolved in water to make 255 mL of a 00100 M solution of
CoCl2(aq)
a) 0316 g
b) 0607 g
c) 0947 gd) 0101 g
e) 200 g
30 How much water would you need to add to 200 L of a 0250 M NaCl solution in order to make a NaC
solution having a final concentration of 0100 M
a) 100 L
b) 700 L
c) 300 L
d) 200 L
e) 500 L
31 Which of the following is true of a 010 M sodium sulfate solution
a) It is a non-electrolyte solution
b) The concentration of sodium cations and sulfate anions will be equal
c) The solution will not conduct electricity
d) The concentration of sodium ions will be 020 M
e) This would be an acidic solution
32 When a 010 M solution of Ba(ClO4)2 is mixed with a 010 M solution of ZnSO4 what will happen
a) Barium sulfate will precipitate
b) Zinc perchlorate will precipitate
c) There will be no precipitate
d) Zinc chlorate will precipitate
e) Not enough information to answer the question
33 Which are the spectator ions in a reaction between AgNO3(aq) and LiCl(aq)
a) Ag1+ (aq) and Cl- (aq)
b) Li+ (aq) and NO32- (aq)c) Li+ (aq) and NO3- (aq)
d) All of the ions are spectator ions no reaction occurs
e) None of the ions are spectator ions
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 811
8
34 What is the net ionic equation for the reaction of NaOH(aq) and HCl(aq)
a) NaOH (aq) + HCl (aq) H2O (l) + NaCl (aq)
b) OH- (aq) + H+ (aq) H2O (l)
c) NaOH (aq) + HCl (aq) NaClH2O (s)d) Na+ (aq) + Cl- (aq) NaCl (aq)
e) OH- (aq) + Cl- (aq) HOCl (aq)
35 The balanced chemical equation presented below describes the acid-base neutralization reactio
between HCl(aq) and Ba(OH)2(aq) Determine the concentration of a 1500 mL HCl(aq) solution tha
would be needed to neutralize 2000 mL of Ba(OH)2(aq) which has a concentration of 0400 molL
2HCl(aq) + Ba(OH)2(aq) BaCl2(aq) + 2H2O(l)
a) 0533 molLb) 107 molL
c) 267 molL
d) 0600 molL
e) 267 molL
36 Identify the final products (in proper stoichiometric proportions) that would be formed when
Na2CO3(aq) reacts with HI(aq)
a) H2CO3(aq) + CO2(g) + HI(aq)b) H2CO3(aq) + NaI(aq)
c) H2O(l) + CO2(g) + 2NaI(aq)
d) H2O(l) + NaI(aq) + CO(g)
e) NaI2(aq) + H2CO3(aq) + H2O(l)
37 How many of the following compounds contain S having an oxidation state of 6+ H2S H2SO4 H2SO3
Fe2(SO4)3 CaSO3
a) 1
b) 2
c) 3d) 4
e) 5
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 911
9
38 Identify the reducing agent in the following balanced REDOX reaction
4SrO(s) + 2Fe2O3(s) + O2(g) 4SrFeO3(s)
a) SrO
b) Fe2O3
c) O2 d) SrFeO3
e) None of the compounds are a reducing agent as this is not a REDOX reaction
39 How many of the following balanced equations describe REDOX reactions
i) 2CaO(s) + Fe2O3(s) Ca2Fe2O5(s)
ii) 2C6H14(l) + 19O2(g) 12CO2(g) + 14H2O(g)
iii) K2SO3(aq) + 2HCl(aq) 2KCl(aq) + H2O(l) + SO2(g)
iv) TiO2(s) + 2C(s) Ti(s) + 2CO(g)
a) 0
b) 1
c) 2
d) 3
e) 4
40 Which statement below correctly describes Avogadrorsquos Law
a) For a fixed amount of gas at a constant temperature the gas volume is inversely proportional to gas
pressure
b) For a fixed amount of gas at constant pressure the volume is directly proportional to the
temperature
c) For a fixed temperature and pressure the volume of a gas is directly proportional to the number of
gas molecules
d) All of the above statements correctly describe Avogadrorsquos Law
e) None of the above statement s correctly describe Avogadrorsquos Law
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 1011
10
41 The following reaction is used to generate hydrogen gas in the laboratory If a 243 mL sample of hydrogen
gas is collected over water at 298 K at a pressure of 745 mm Hg what mass of hydrogen has been produced
The vapor pressure of water at 298 K is 2378 mm Hg Assume ideality
Mg(s) + 2 HCl(aq) rarr MgCl2(aq) + H2(g)
a) 00196 g b) 00717 gc) 00190 g
d) 00144 g
e) None of the above
42 At STP a sample of gas occupies a volume of 678 mL Assuming ideality what would its volume be at
500 oC and 0808 atm
a) 854 mL
b) 783 mL
c) 587 mLd) 538 mL
e) none of the above
43 A gaseous mixture of helium and hydrogen is 600 helium by mass The total pressure of a sample of this
mixture is 100 atm What is the partial pressure of hydrogen in this sample
a) 0400
b) 0430c) 0570
d) 0600e) Need more information to answer
44 In the Van der Waals equation (below) the term +a(nV)2 accounts for the fact that in a real gas
a) the particles have a finite mass
b) the particles attract each otherc) the particles are non-linear
d) the particles have a finite size
e) none of the above is true
45 A gas sample has a pressure of
216 atm The temperature (in K) of the sample is increased by a factor of three and it is compressed to half its previous volume Assuming ideality the pressure is now
a) 0360 atm
b) 130 atm
c) 324 atmd) 114 atm
e) Cannot answer without more information
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 1111
11
11A
Periodic Table of the Elements8
1
H100794
22A
133A
144A
155A
166A
177A
H4
3
Li
6941
4
Be
901218
5
B
10811
6
C
12011
7
N
140067
8
O
159994
9
F
189984
N2
11
Na
229898
12
Mg
243050
33B
44B
55B
66B
77B
88B
98B
108B
111B
122B
13
Al
269815
14
Si
280855
15
P
309738
16
S
32066
17
Cl
354527
A3
19
K 390983
20
Ca
40078
21
Sc
449559
22
Ti
4788
23
V 509415
24
Cr
519961
25
Mn
549381
26
Fe
55847
27
Co
589332
28
Ni
58693
29
Cu
63546
30
Zn
6539
31
Ga
69723
32
Ge
7261
33
As
749216
34
Se
7896
35
Br
79904
K
37
Rb
854678
38
Sr
8762
39
Y 889059
40
Zr
91224
41
Nb
929064
42
Mo
9594
43
Tc
(98)
44
Ru
10107
45
Rh
102906
46
Pd
10642
47
Ag
107868
48
Cd
112411
49
In
114818
50
Sn
118710
51
Sb
121757
52
Te
12760
53
I
126904
X1
55
Cs
132905
56
Ba
137327
57
La
138906
72
Hf 17849
73
Ta
180948
74
W
18384
75
Re
186207
76
Os
19023
77
Ir
19222
78
Pt
19508
79
Au
196967
80
Hg
20059
81
Tl
204383
82
Pb
2072
83
Bi
208980
84
Po
(209)
85
At
(210)
R
87
Fr
(223)
88
Ra
226025
89
Ac
227028
104
Rf (261)
105
Db
(262)
106
Sg
(263)
107
Bh
(262)
108
Hs
(265)
109
Mt
(266)
110
(269)
111
(272)
112
(272)
114
(287)
116
(289)
58
Ce
140115
59
Pr
140908
60
Nd
14424
61
Pm
(145)
62
Sm
15036
63
Eu
151965
64
Gd
15725
65
Tb
158925
66
Dy
16250
67
Ho
164930
68
Er
16726
69
Tm
168934
70
Yb
17304
L1
90
Th
232038
91
Pa
231036
92
U
238029
93
Np
237048
94
Pu
(244)
95
Am
(243)
96
Cm
(247)
97
Bk (247)
98
Cf (251)
99
Es
(252)
100
Fm
(257)
101
Md
(258)
102
No
(259)
L
Physical Constants
Constant Symbol Value
Atomic mass unit u 16605 times 10-27 kg Avogadro number N A 60221 times 1023 mol-1
Gas Constant R 0082058 L atm mol-1K -1 83145 J K -1 mol-1 62364 L mmHg mol-1 K -1
Molar volume of an ideal gas at STP V m 22414 L mol-1
Electron mass m e 9109 times 10-31 Kg
Some SI Derived Units
Physical Quantity Unit Symbol Definition
Force Newton N kg m s-2
Energy Joule J kg m2 s-2 Pressure Pascal Pa N m-2 = kg m-1 s-2
STP Conditions P = 1 atm = 760 torr = 760 mmHg = 101325 kPa
Temperature = 0 ordmC = 27315 K
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 711
7
29 What mass of CoCl26H2O needs to be dissolved in water to make 255 mL of a 00100 M solution of
CoCl2(aq)
a) 0316 g
b) 0607 g
c) 0947 gd) 0101 g
e) 200 g
30 How much water would you need to add to 200 L of a 0250 M NaCl solution in order to make a NaC
solution having a final concentration of 0100 M
a) 100 L
b) 700 L
c) 300 L
d) 200 L
e) 500 L
31 Which of the following is true of a 010 M sodium sulfate solution
a) It is a non-electrolyte solution
b) The concentration of sodium cations and sulfate anions will be equal
c) The solution will not conduct electricity
d) The concentration of sodium ions will be 020 M
e) This would be an acidic solution
32 When a 010 M solution of Ba(ClO4)2 is mixed with a 010 M solution of ZnSO4 what will happen
a) Barium sulfate will precipitate
b) Zinc perchlorate will precipitate
c) There will be no precipitate
d) Zinc chlorate will precipitate
e) Not enough information to answer the question
33 Which are the spectator ions in a reaction between AgNO3(aq) and LiCl(aq)
a) Ag1+ (aq) and Cl- (aq)
b) Li+ (aq) and NO32- (aq)c) Li+ (aq) and NO3- (aq)
d) All of the ions are spectator ions no reaction occurs
e) None of the ions are spectator ions
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 811
8
34 What is the net ionic equation for the reaction of NaOH(aq) and HCl(aq)
a) NaOH (aq) + HCl (aq) H2O (l) + NaCl (aq)
b) OH- (aq) + H+ (aq) H2O (l)
c) NaOH (aq) + HCl (aq) NaClH2O (s)d) Na+ (aq) + Cl- (aq) NaCl (aq)
e) OH- (aq) + Cl- (aq) HOCl (aq)
35 The balanced chemical equation presented below describes the acid-base neutralization reactio
between HCl(aq) and Ba(OH)2(aq) Determine the concentration of a 1500 mL HCl(aq) solution tha
would be needed to neutralize 2000 mL of Ba(OH)2(aq) which has a concentration of 0400 molL
2HCl(aq) + Ba(OH)2(aq) BaCl2(aq) + 2H2O(l)
a) 0533 molLb) 107 molL
c) 267 molL
d) 0600 molL
e) 267 molL
36 Identify the final products (in proper stoichiometric proportions) that would be formed when
Na2CO3(aq) reacts with HI(aq)
a) H2CO3(aq) + CO2(g) + HI(aq)b) H2CO3(aq) + NaI(aq)
c) H2O(l) + CO2(g) + 2NaI(aq)
d) H2O(l) + NaI(aq) + CO(g)
e) NaI2(aq) + H2CO3(aq) + H2O(l)
37 How many of the following compounds contain S having an oxidation state of 6+ H2S H2SO4 H2SO3
Fe2(SO4)3 CaSO3
a) 1
b) 2
c) 3d) 4
e) 5
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 911
9
38 Identify the reducing agent in the following balanced REDOX reaction
4SrO(s) + 2Fe2O3(s) + O2(g) 4SrFeO3(s)
a) SrO
b) Fe2O3
c) O2 d) SrFeO3
e) None of the compounds are a reducing agent as this is not a REDOX reaction
39 How many of the following balanced equations describe REDOX reactions
i) 2CaO(s) + Fe2O3(s) Ca2Fe2O5(s)
ii) 2C6H14(l) + 19O2(g) 12CO2(g) + 14H2O(g)
iii) K2SO3(aq) + 2HCl(aq) 2KCl(aq) + H2O(l) + SO2(g)
iv) TiO2(s) + 2C(s) Ti(s) + 2CO(g)
a) 0
b) 1
c) 2
d) 3
e) 4
40 Which statement below correctly describes Avogadrorsquos Law
a) For a fixed amount of gas at a constant temperature the gas volume is inversely proportional to gas
pressure
b) For a fixed amount of gas at constant pressure the volume is directly proportional to the
temperature
c) For a fixed temperature and pressure the volume of a gas is directly proportional to the number of
gas molecules
d) All of the above statements correctly describe Avogadrorsquos Law
e) None of the above statement s correctly describe Avogadrorsquos Law
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 1011
10
41 The following reaction is used to generate hydrogen gas in the laboratory If a 243 mL sample of hydrogen
gas is collected over water at 298 K at a pressure of 745 mm Hg what mass of hydrogen has been produced
The vapor pressure of water at 298 K is 2378 mm Hg Assume ideality
Mg(s) + 2 HCl(aq) rarr MgCl2(aq) + H2(g)
a) 00196 g b) 00717 gc) 00190 g
d) 00144 g
e) None of the above
42 At STP a sample of gas occupies a volume of 678 mL Assuming ideality what would its volume be at
500 oC and 0808 atm
a) 854 mL
b) 783 mL
c) 587 mLd) 538 mL
e) none of the above
43 A gaseous mixture of helium and hydrogen is 600 helium by mass The total pressure of a sample of this
mixture is 100 atm What is the partial pressure of hydrogen in this sample
a) 0400
b) 0430c) 0570
d) 0600e) Need more information to answer
44 In the Van der Waals equation (below) the term +a(nV)2 accounts for the fact that in a real gas
a) the particles have a finite mass
b) the particles attract each otherc) the particles are non-linear
d) the particles have a finite size
e) none of the above is true
45 A gas sample has a pressure of
216 atm The temperature (in K) of the sample is increased by a factor of three and it is compressed to half its previous volume Assuming ideality the pressure is now
a) 0360 atm
b) 130 atm
c) 324 atmd) 114 atm
e) Cannot answer without more information
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 1111
11
11A
Periodic Table of the Elements8
1
H100794
22A
133A
144A
155A
166A
177A
H4
3
Li
6941
4
Be
901218
5
B
10811
6
C
12011
7
N
140067
8
O
159994
9
F
189984
N2
11
Na
229898
12
Mg
243050
33B
44B
55B
66B
77B
88B
98B
108B
111B
122B
13
Al
269815
14
Si
280855
15
P
309738
16
S
32066
17
Cl
354527
A3
19
K 390983
20
Ca
40078
21
Sc
449559
22
Ti
4788
23
V 509415
24
Cr
519961
25
Mn
549381
26
Fe
55847
27
Co
589332
28
Ni
58693
29
Cu
63546
30
Zn
6539
31
Ga
69723
32
Ge
7261
33
As
749216
34
Se
7896
35
Br
79904
K
37
Rb
854678
38
Sr
8762
39
Y 889059
40
Zr
91224
41
Nb
929064
42
Mo
9594
43
Tc
(98)
44
Ru
10107
45
Rh
102906
46
Pd
10642
47
Ag
107868
48
Cd
112411
49
In
114818
50
Sn
118710
51
Sb
121757
52
Te
12760
53
I
126904
X1
55
Cs
132905
56
Ba
137327
57
La
138906
72
Hf 17849
73
Ta
180948
74
W
18384
75
Re
186207
76
Os
19023
77
Ir
19222
78
Pt
19508
79
Au
196967
80
Hg
20059
81
Tl
204383
82
Pb
2072
83
Bi
208980
84
Po
(209)
85
At
(210)
R
87
Fr
(223)
88
Ra
226025
89
Ac
227028
104
Rf (261)
105
Db
(262)
106
Sg
(263)
107
Bh
(262)
108
Hs
(265)
109
Mt
(266)
110
(269)
111
(272)
112
(272)
114
(287)
116
(289)
58
Ce
140115
59
Pr
140908
60
Nd
14424
61
Pm
(145)
62
Sm
15036
63
Eu
151965
64
Gd
15725
65
Tb
158925
66
Dy
16250
67
Ho
164930
68
Er
16726
69
Tm
168934
70
Yb
17304
L1
90
Th
232038
91
Pa
231036
92
U
238029
93
Np
237048
94
Pu
(244)
95
Am
(243)
96
Cm
(247)
97
Bk (247)
98
Cf (251)
99
Es
(252)
100
Fm
(257)
101
Md
(258)
102
No
(259)
L
Physical Constants
Constant Symbol Value
Atomic mass unit u 16605 times 10-27 kg Avogadro number N A 60221 times 1023 mol-1
Gas Constant R 0082058 L atm mol-1K -1 83145 J K -1 mol-1 62364 L mmHg mol-1 K -1
Molar volume of an ideal gas at STP V m 22414 L mol-1
Electron mass m e 9109 times 10-31 Kg
Some SI Derived Units
Physical Quantity Unit Symbol Definition
Force Newton N kg m s-2
Energy Joule J kg m2 s-2 Pressure Pascal Pa N m-2 = kg m-1 s-2
STP Conditions P = 1 atm = 760 torr = 760 mmHg = 101325 kPa
Temperature = 0 ordmC = 27315 K
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 811
8
34 What is the net ionic equation for the reaction of NaOH(aq) and HCl(aq)
a) NaOH (aq) + HCl (aq) H2O (l) + NaCl (aq)
b) OH- (aq) + H+ (aq) H2O (l)
c) NaOH (aq) + HCl (aq) NaClH2O (s)d) Na+ (aq) + Cl- (aq) NaCl (aq)
e) OH- (aq) + Cl- (aq) HOCl (aq)
35 The balanced chemical equation presented below describes the acid-base neutralization reactio
between HCl(aq) and Ba(OH)2(aq) Determine the concentration of a 1500 mL HCl(aq) solution tha
would be needed to neutralize 2000 mL of Ba(OH)2(aq) which has a concentration of 0400 molL
2HCl(aq) + Ba(OH)2(aq) BaCl2(aq) + 2H2O(l)
a) 0533 molLb) 107 molL
c) 267 molL
d) 0600 molL
e) 267 molL
36 Identify the final products (in proper stoichiometric proportions) that would be formed when
Na2CO3(aq) reacts with HI(aq)
a) H2CO3(aq) + CO2(g) + HI(aq)b) H2CO3(aq) + NaI(aq)
c) H2O(l) + CO2(g) + 2NaI(aq)
d) H2O(l) + NaI(aq) + CO(g)
e) NaI2(aq) + H2CO3(aq) + H2O(l)
37 How many of the following compounds contain S having an oxidation state of 6+ H2S H2SO4 H2SO3
Fe2(SO4)3 CaSO3
a) 1
b) 2
c) 3d) 4
e) 5
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 911
9
38 Identify the reducing agent in the following balanced REDOX reaction
4SrO(s) + 2Fe2O3(s) + O2(g) 4SrFeO3(s)
a) SrO
b) Fe2O3
c) O2 d) SrFeO3
e) None of the compounds are a reducing agent as this is not a REDOX reaction
39 How many of the following balanced equations describe REDOX reactions
i) 2CaO(s) + Fe2O3(s) Ca2Fe2O5(s)
ii) 2C6H14(l) + 19O2(g) 12CO2(g) + 14H2O(g)
iii) K2SO3(aq) + 2HCl(aq) 2KCl(aq) + H2O(l) + SO2(g)
iv) TiO2(s) + 2C(s) Ti(s) + 2CO(g)
a) 0
b) 1
c) 2
d) 3
e) 4
40 Which statement below correctly describes Avogadrorsquos Law
a) For a fixed amount of gas at a constant temperature the gas volume is inversely proportional to gas
pressure
b) For a fixed amount of gas at constant pressure the volume is directly proportional to the
temperature
c) For a fixed temperature and pressure the volume of a gas is directly proportional to the number of
gas molecules
d) All of the above statements correctly describe Avogadrorsquos Law
e) None of the above statement s correctly describe Avogadrorsquos Law
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 1011
10
41 The following reaction is used to generate hydrogen gas in the laboratory If a 243 mL sample of hydrogen
gas is collected over water at 298 K at a pressure of 745 mm Hg what mass of hydrogen has been produced
The vapor pressure of water at 298 K is 2378 mm Hg Assume ideality
Mg(s) + 2 HCl(aq) rarr MgCl2(aq) + H2(g)
a) 00196 g b) 00717 gc) 00190 g
d) 00144 g
e) None of the above
42 At STP a sample of gas occupies a volume of 678 mL Assuming ideality what would its volume be at
500 oC and 0808 atm
a) 854 mL
b) 783 mL
c) 587 mLd) 538 mL
e) none of the above
43 A gaseous mixture of helium and hydrogen is 600 helium by mass The total pressure of a sample of this
mixture is 100 atm What is the partial pressure of hydrogen in this sample
a) 0400
b) 0430c) 0570
d) 0600e) Need more information to answer
44 In the Van der Waals equation (below) the term +a(nV)2 accounts for the fact that in a real gas
a) the particles have a finite mass
b) the particles attract each otherc) the particles are non-linear
d) the particles have a finite size
e) none of the above is true
45 A gas sample has a pressure of
216 atm The temperature (in K) of the sample is increased by a factor of three and it is compressed to half its previous volume Assuming ideality the pressure is now
a) 0360 atm
b) 130 atm
c) 324 atmd) 114 atm
e) Cannot answer without more information
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 1111
11
11A
Periodic Table of the Elements8
1
H100794
22A
133A
144A
155A
166A
177A
H4
3
Li
6941
4
Be
901218
5
B
10811
6
C
12011
7
N
140067
8
O
159994
9
F
189984
N2
11
Na
229898
12
Mg
243050
33B
44B
55B
66B
77B
88B
98B
108B
111B
122B
13
Al
269815
14
Si
280855
15
P
309738
16
S
32066
17
Cl
354527
A3
19
K 390983
20
Ca
40078
21
Sc
449559
22
Ti
4788
23
V 509415
24
Cr
519961
25
Mn
549381
26
Fe
55847
27
Co
589332
28
Ni
58693
29
Cu
63546
30
Zn
6539
31
Ga
69723
32
Ge
7261
33
As
749216
34
Se
7896
35
Br
79904
K
37
Rb
854678
38
Sr
8762
39
Y 889059
40
Zr
91224
41
Nb
929064
42
Mo
9594
43
Tc
(98)
44
Ru
10107
45
Rh
102906
46
Pd
10642
47
Ag
107868
48
Cd
112411
49
In
114818
50
Sn
118710
51
Sb
121757
52
Te
12760
53
I
126904
X1
55
Cs
132905
56
Ba
137327
57
La
138906
72
Hf 17849
73
Ta
180948
74
W
18384
75
Re
186207
76
Os
19023
77
Ir
19222
78
Pt
19508
79
Au
196967
80
Hg
20059
81
Tl
204383
82
Pb
2072
83
Bi
208980
84
Po
(209)
85
At
(210)
R
87
Fr
(223)
88
Ra
226025
89
Ac
227028
104
Rf (261)
105
Db
(262)
106
Sg
(263)
107
Bh
(262)
108
Hs
(265)
109
Mt
(266)
110
(269)
111
(272)
112
(272)
114
(287)
116
(289)
58
Ce
140115
59
Pr
140908
60
Nd
14424
61
Pm
(145)
62
Sm
15036
63
Eu
151965
64
Gd
15725
65
Tb
158925
66
Dy
16250
67
Ho
164930
68
Er
16726
69
Tm
168934
70
Yb
17304
L1
90
Th
232038
91
Pa
231036
92
U
238029
93
Np
237048
94
Pu
(244)
95
Am
(243)
96
Cm
(247)
97
Bk (247)
98
Cf (251)
99
Es
(252)
100
Fm
(257)
101
Md
(258)
102
No
(259)
L
Physical Constants
Constant Symbol Value
Atomic mass unit u 16605 times 10-27 kg Avogadro number N A 60221 times 1023 mol-1
Gas Constant R 0082058 L atm mol-1K -1 83145 J K -1 mol-1 62364 L mmHg mol-1 K -1
Molar volume of an ideal gas at STP V m 22414 L mol-1
Electron mass m e 9109 times 10-31 Kg
Some SI Derived Units
Physical Quantity Unit Symbol Definition
Force Newton N kg m s-2
Energy Joule J kg m2 s-2 Pressure Pascal Pa N m-2 = kg m-1 s-2
STP Conditions P = 1 atm = 760 torr = 760 mmHg = 101325 kPa
Temperature = 0 ordmC = 27315 K
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 911
9
38 Identify the reducing agent in the following balanced REDOX reaction
4SrO(s) + 2Fe2O3(s) + O2(g) 4SrFeO3(s)
a) SrO
b) Fe2O3
c) O2 d) SrFeO3
e) None of the compounds are a reducing agent as this is not a REDOX reaction
39 How many of the following balanced equations describe REDOX reactions
i) 2CaO(s) + Fe2O3(s) Ca2Fe2O5(s)
ii) 2C6H14(l) + 19O2(g) 12CO2(g) + 14H2O(g)
iii) K2SO3(aq) + 2HCl(aq) 2KCl(aq) + H2O(l) + SO2(g)
iv) TiO2(s) + 2C(s) Ti(s) + 2CO(g)
a) 0
b) 1
c) 2
d) 3
e) 4
40 Which statement below correctly describes Avogadrorsquos Law
a) For a fixed amount of gas at a constant temperature the gas volume is inversely proportional to gas
pressure
b) For a fixed amount of gas at constant pressure the volume is directly proportional to the
temperature
c) For a fixed temperature and pressure the volume of a gas is directly proportional to the number of
gas molecules
d) All of the above statements correctly describe Avogadrorsquos Law
e) None of the above statement s correctly describe Avogadrorsquos Law
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 1011
10
41 The following reaction is used to generate hydrogen gas in the laboratory If a 243 mL sample of hydrogen
gas is collected over water at 298 K at a pressure of 745 mm Hg what mass of hydrogen has been produced
The vapor pressure of water at 298 K is 2378 mm Hg Assume ideality
Mg(s) + 2 HCl(aq) rarr MgCl2(aq) + H2(g)
a) 00196 g b) 00717 gc) 00190 g
d) 00144 g
e) None of the above
42 At STP a sample of gas occupies a volume of 678 mL Assuming ideality what would its volume be at
500 oC and 0808 atm
a) 854 mL
b) 783 mL
c) 587 mLd) 538 mL
e) none of the above
43 A gaseous mixture of helium and hydrogen is 600 helium by mass The total pressure of a sample of this
mixture is 100 atm What is the partial pressure of hydrogen in this sample
a) 0400
b) 0430c) 0570
d) 0600e) Need more information to answer
44 In the Van der Waals equation (below) the term +a(nV)2 accounts for the fact that in a real gas
a) the particles have a finite mass
b) the particles attract each otherc) the particles are non-linear
d) the particles have a finite size
e) none of the above is true
45 A gas sample has a pressure of
216 atm The temperature (in K) of the sample is increased by a factor of three and it is compressed to half its previous volume Assuming ideality the pressure is now
a) 0360 atm
b) 130 atm
c) 324 atmd) 114 atm
e) Cannot answer without more information
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 1111
11
11A
Periodic Table of the Elements8
1
H100794
22A
133A
144A
155A
166A
177A
H4
3
Li
6941
4
Be
901218
5
B
10811
6
C
12011
7
N
140067
8
O
159994
9
F
189984
N2
11
Na
229898
12
Mg
243050
33B
44B
55B
66B
77B
88B
98B
108B
111B
122B
13
Al
269815
14
Si
280855
15
P
309738
16
S
32066
17
Cl
354527
A3
19
K 390983
20
Ca
40078
21
Sc
449559
22
Ti
4788
23
V 509415
24
Cr
519961
25
Mn
549381
26
Fe
55847
27
Co
589332
28
Ni
58693
29
Cu
63546
30
Zn
6539
31
Ga
69723
32
Ge
7261
33
As
749216
34
Se
7896
35
Br
79904
K
37
Rb
854678
38
Sr
8762
39
Y 889059
40
Zr
91224
41
Nb
929064
42
Mo
9594
43
Tc
(98)
44
Ru
10107
45
Rh
102906
46
Pd
10642
47
Ag
107868
48
Cd
112411
49
In
114818
50
Sn
118710
51
Sb
121757
52
Te
12760
53
I
126904
X1
55
Cs
132905
56
Ba
137327
57
La
138906
72
Hf 17849
73
Ta
180948
74
W
18384
75
Re
186207
76
Os
19023
77
Ir
19222
78
Pt
19508
79
Au
196967
80
Hg
20059
81
Tl
204383
82
Pb
2072
83
Bi
208980
84
Po
(209)
85
At
(210)
R
87
Fr
(223)
88
Ra
226025
89
Ac
227028
104
Rf (261)
105
Db
(262)
106
Sg
(263)
107
Bh
(262)
108
Hs
(265)
109
Mt
(266)
110
(269)
111
(272)
112
(272)
114
(287)
116
(289)
58
Ce
140115
59
Pr
140908
60
Nd
14424
61
Pm
(145)
62
Sm
15036
63
Eu
151965
64
Gd
15725
65
Tb
158925
66
Dy
16250
67
Ho
164930
68
Er
16726
69
Tm
168934
70
Yb
17304
L1
90
Th
232038
91
Pa
231036
92
U
238029
93
Np
237048
94
Pu
(244)
95
Am
(243)
96
Cm
(247)
97
Bk (247)
98
Cf (251)
99
Es
(252)
100
Fm
(257)
101
Md
(258)
102
No
(259)
L
Physical Constants
Constant Symbol Value
Atomic mass unit u 16605 times 10-27 kg Avogadro number N A 60221 times 1023 mol-1
Gas Constant R 0082058 L atm mol-1K -1 83145 J K -1 mol-1 62364 L mmHg mol-1 K -1
Molar volume of an ideal gas at STP V m 22414 L mol-1
Electron mass m e 9109 times 10-31 Kg
Some SI Derived Units
Physical Quantity Unit Symbol Definition
Force Newton N kg m s-2
Energy Joule J kg m2 s-2 Pressure Pascal Pa N m-2 = kg m-1 s-2
STP Conditions P = 1 atm = 760 torr = 760 mmHg = 101325 kPa
Temperature = 0 ordmC = 27315 K
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 1011
10
41 The following reaction is used to generate hydrogen gas in the laboratory If a 243 mL sample of hydrogen
gas is collected over water at 298 K at a pressure of 745 mm Hg what mass of hydrogen has been produced
The vapor pressure of water at 298 K is 2378 mm Hg Assume ideality
Mg(s) + 2 HCl(aq) rarr MgCl2(aq) + H2(g)
a) 00196 g b) 00717 gc) 00190 g
d) 00144 g
e) None of the above
42 At STP a sample of gas occupies a volume of 678 mL Assuming ideality what would its volume be at
500 oC and 0808 atm
a) 854 mL
b) 783 mL
c) 587 mLd) 538 mL
e) none of the above
43 A gaseous mixture of helium and hydrogen is 600 helium by mass The total pressure of a sample of this
mixture is 100 atm What is the partial pressure of hydrogen in this sample
a) 0400
b) 0430c) 0570
d) 0600e) Need more information to answer
44 In the Van der Waals equation (below) the term +a(nV)2 accounts for the fact that in a real gas
a) the particles have a finite mass
b) the particles attract each otherc) the particles are non-linear
d) the particles have a finite size
e) none of the above is true
45 A gas sample has a pressure of
216 atm The temperature (in K) of the sample is increased by a factor of three and it is compressed to half its previous volume Assuming ideality the pressure is now
a) 0360 atm
b) 130 atm
c) 324 atmd) 114 atm
e) Cannot answer without more information
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 1111
11
11A
Periodic Table of the Elements8
1
H100794
22A
133A
144A
155A
166A
177A
H4
3
Li
6941
4
Be
901218
5
B
10811
6
C
12011
7
N
140067
8
O
159994
9
F
189984
N2
11
Na
229898
12
Mg
243050
33B
44B
55B
66B
77B
88B
98B
108B
111B
122B
13
Al
269815
14
Si
280855
15
P
309738
16
S
32066
17
Cl
354527
A3
19
K 390983
20
Ca
40078
21
Sc
449559
22
Ti
4788
23
V 509415
24
Cr
519961
25
Mn
549381
26
Fe
55847
27
Co
589332
28
Ni
58693
29
Cu
63546
30
Zn
6539
31
Ga
69723
32
Ge
7261
33
As
749216
34
Se
7896
35
Br
79904
K
37
Rb
854678
38
Sr
8762
39
Y 889059
40
Zr
91224
41
Nb
929064
42
Mo
9594
43
Tc
(98)
44
Ru
10107
45
Rh
102906
46
Pd
10642
47
Ag
107868
48
Cd
112411
49
In
114818
50
Sn
118710
51
Sb
121757
52
Te
12760
53
I
126904
X1
55
Cs
132905
56
Ba
137327
57
La
138906
72
Hf 17849
73
Ta
180948
74
W
18384
75
Re
186207
76
Os
19023
77
Ir
19222
78
Pt
19508
79
Au
196967
80
Hg
20059
81
Tl
204383
82
Pb
2072
83
Bi
208980
84
Po
(209)
85
At
(210)
R
87
Fr
(223)
88
Ra
226025
89
Ac
227028
104
Rf (261)
105
Db
(262)
106
Sg
(263)
107
Bh
(262)
108
Hs
(265)
109
Mt
(266)
110
(269)
111
(272)
112
(272)
114
(287)
116
(289)
58
Ce
140115
59
Pr
140908
60
Nd
14424
61
Pm
(145)
62
Sm
15036
63
Eu
151965
64
Gd
15725
65
Tb
158925
66
Dy
16250
67
Ho
164930
68
Er
16726
69
Tm
168934
70
Yb
17304
L1
90
Th
232038
91
Pa
231036
92
U
238029
93
Np
237048
94
Pu
(244)
95
Am
(243)
96
Cm
(247)
97
Bk (247)
98
Cf (251)
99
Es
(252)
100
Fm
(257)
101
Md
(258)
102
No
(259)
L
Physical Constants
Constant Symbol Value
Atomic mass unit u 16605 times 10-27 kg Avogadro number N A 60221 times 1023 mol-1
Gas Constant R 0082058 L atm mol-1K -1 83145 J K -1 mol-1 62364 L mmHg mol-1 K -1
Molar volume of an ideal gas at STP V m 22414 L mol-1
Electron mass m e 9109 times 10-31 Kg
Some SI Derived Units
Physical Quantity Unit Symbol Definition
Force Newton N kg m s-2
Energy Joule J kg m2 s-2 Pressure Pascal Pa N m-2 = kg m-1 s-2
STP Conditions P = 1 atm = 760 torr = 760 mmHg = 101325 kPa
Temperature = 0 ordmC = 27315 K
7212019 Chem 114 Sample Midterm Exam
httpslidepdfcomreaderfullchem-114-sample-midterm-exam 1111
11
11A
Periodic Table of the Elements8
1
H100794
22A
133A
144A
155A
166A
177A
H4
3
Li
6941
4
Be
901218
5
B
10811
6
C
12011
7
N
140067
8
O
159994
9
F
189984
N2
11
Na
229898
12
Mg
243050
33B
44B
55B
66B
77B
88B
98B
108B
111B
122B
13
Al
269815
14
Si
280855
15
P
309738
16
S
32066
17
Cl
354527
A3
19
K 390983
20
Ca
40078
21
Sc
449559
22
Ti
4788
23
V 509415
24
Cr
519961
25
Mn
549381
26
Fe
55847
27
Co
589332
28
Ni
58693
29
Cu
63546
30
Zn
6539
31
Ga
69723
32
Ge
7261
33
As
749216
34
Se
7896
35
Br
79904
K
37
Rb
854678
38
Sr
8762
39
Y 889059
40
Zr
91224
41
Nb
929064
42
Mo
9594
43
Tc
(98)
44
Ru
10107
45
Rh
102906
46
Pd
10642
47
Ag
107868
48
Cd
112411
49
In
114818
50
Sn
118710
51
Sb
121757
52
Te
12760
53
I
126904
X1
55
Cs
132905
56
Ba
137327
57
La
138906
72
Hf 17849
73
Ta
180948
74
W
18384
75
Re
186207
76
Os
19023
77
Ir
19222
78
Pt
19508
79
Au
196967
80
Hg
20059
81
Tl
204383
82
Pb
2072
83
Bi
208980
84
Po
(209)
85
At
(210)
R
87
Fr
(223)
88
Ra
226025
89
Ac
227028
104
Rf (261)
105
Db
(262)
106
Sg
(263)
107
Bh
(262)
108
Hs
(265)
109
Mt
(266)
110
(269)
111
(272)
112
(272)
114
(287)
116
(289)
58
Ce
140115
59
Pr
140908
60
Nd
14424
61
Pm
(145)
62
Sm
15036
63
Eu
151965
64
Gd
15725
65
Tb
158925
66
Dy
16250
67
Ho
164930
68
Er
16726
69
Tm
168934
70
Yb
17304
L1
90
Th
232038
91
Pa
231036
92
U
238029
93
Np
237048
94
Pu
(244)
95
Am
(243)
96
Cm
(247)
97
Bk (247)
98
Cf (251)
99
Es
(252)
100
Fm
(257)
101
Md
(258)
102
No
(259)
L
Physical Constants
Constant Symbol Value
Atomic mass unit u 16605 times 10-27 kg Avogadro number N A 60221 times 1023 mol-1
Gas Constant R 0082058 L atm mol-1K -1 83145 J K -1 mol-1 62364 L mmHg mol-1 K -1
Molar volume of an ideal gas at STP V m 22414 L mol-1
Electron mass m e 9109 times 10-31 Kg
Some SI Derived Units
Physical Quantity Unit Symbol Definition
Force Newton N kg m s-2
Energy Joule J kg m2 s-2 Pressure Pascal Pa N m-2 = kg m-1 s-2
STP Conditions P = 1 atm = 760 torr = 760 mmHg = 101325 kPa
Temperature = 0 ordmC = 27315 K