Download SUPPLEMENTAL PROBLEMS FOR CHEM 110

Ordered according to coverage:
Chapter
1
2
6
7
8
Organic
3
9
10
18
11
4
13
Reactions
5
15
Answer key
page
21
21
24
26
28
30
22
32
35
44
37
23
40
45
23
42
53
SUPPLEMENTAL PROBLEMS
FOR CHEM 110
Ordered by chapter number:
Chapter
1
2
3
4
5
6
7
8
Organic
9
10
11
13
15
18
Reactions
Answer key
The problems are divided into chapters
matching the book’s chapter numbers, and
the chapters are arranged in order in which
they are covered in lectures (see the
syllabus).
19
page
21
21
22
23
23
24
26
28
30
32
34
37
40
42
44
45
53
20
Chapter 1
Chapter 2
1.
1.
13.2 nm is equal to
A.
B.
C.
D.
E.
2.
−
A. 23%
B. 91%
C. 77%
D. 45%
E. None of the above is within 10% of the correct
answer
−
−
2.
0.908 g/mL
1.10 g/mL
0.21 g/mL
Not determinable from the information given
None of the above answers is correct
A.
B.
C.
D.
E.
(1.025)(1.63)(94.0 + 18.13 ! 4.6) = 20.12949552
3.
8.925
to the correct number of significant figures is
4.
2
−
3
2
1.9 × 10
2
1.97 × 10
2
2.0 × 10
0.02
None of the above answers is correct
−
4.
−
?
p=8, n=9, e=10
p=8, n=9, e=8
p=8, n=9, e=6
p=9, n=8, e=11
p=9, n=8, e=9
X and Y are two species, each consisting of one
nucleus and a number of electrons. The two species
are found to contain the same number of protons, the
same number of neutrons, and different numbers of
electrons. Which of the following statements about X
and Y is correct?
Which of the following chemical formulas is NOT the
expected one for the compound named?
−
5
(107.36 – 99.2) (5.4033 × 10 ) = 4.4090928 × 10
A.
B.
C.
D.
E.
6
The above calculation, when expressed to the correct
number of significant figures and properly rounded,
should be written
A.
B.
C.
D.
E.
17 2−
8O
A. X and Y are both neutral atoms.
B. X and Y are isotopes of one another.
C. The two have different atomic numbers.
D. At least one of the species is an ion.
E. There is no correct answer above since A⎯D are
all incorrect.
The result of adding 1.17 × 10 and 8 × 10 is, to the
correct number of significant figures
A.
B.
C.
D.
E.
5.
20
1
2.01 × 10
1
2.0 × 10
20.13
1
2.012 × 10
−
How many protons, neutrons and electrons are
present in
The answer to the calculation
A.
B.
C.
D.
E.
35
−
A 112.6 g mass of unknown material is submersed in
102 mL of water to yield a final volume of 126 mL.
The apparent density of the unknown material is
A.
B.
C.
D.
E.
3.
6
1.32 × 10 cm
6
1.32 × 10 mm
8
1.32 × 10 cm
8
1.32 × 10 mm
None of the above answers is correct
37
Chlorine exists primarily as Cl and Cl and has an
average atomic weight of 35.453. The abundance of
Cl with atomic weight of 35 is
6
4.4 × 10
6
4.40 × 10
6
4.41 × 10
6
4.4090 × 10
6
4.4091 × 10
21
Ga2O3 – gallium oxide
AlCl3 – aluminum chloride
Li2O – lithium oxide
MgBr – magnesium bromide
SrI2 – strontium iodide
Chapter 2 continued
5. Which of the following formula–name combinations
is(are) correct?
1.
2.
3.
NH4Cl2
K2CO3
Ca3(PO4)2
5.
A.
B.
C.
D.
E.
ammonium chloride
potassium carbonate
calcium phosphate
The correct combination(s) is(are)
A. 1 only
B. 2 only
C. 1 and 3 only
D. 2 and 3 only
E. 1 and 2 only
6.
The molecular weight of ethylene glycol, C2H6O2, is
A.
B.
C.
D.
E.
2.
One gram of alum, KAl(SO4)2  12H2O, has 1.3 × 10
Al atoms. How many oxygen atoms are present in
1.0 g of alum?
A.
B.
C.
D.
E.
3.
7.
The percent mass of hydrogen in the following
compound is
A. 5.2%
B. 7.8%
C. 8.7%
D. 7.2%
E. 8.4%
21
H2
C
O
H2C
CH3
CH
N
O
H
CH3
H
H
22
1.3 × 10
22
2.6 × 10
22
1.6 × 10
22
1.0 × 10
22
2.1 × 10
8.
The carbon backbone for a molecule is given below.
What is the molecular weight of this compound?
A . 114 g/mol
B . 115 g/mol
C . 119 g/mol
D . 120 g/mol
E . 126 g/mol
63%
20%
43%
78%
None of the above is correct to within 5%.
9.
What is the empirical formula of a hydrocarbon
containing 84.2% C and 15.8% H by weight?
A.
B.
C.
D.
E.
N
Cl
P
Br
I
H
What is the weight percent of silver in silver nitrate,
AgNO3?
A.
B.
C.
D.
E.
4.
29 g/mole
34 g/mole
62 g/mole
94 g/mole
46 g/mole
0.1 moles of P4O10
0.2 moles of P4O6
0.3 moles of N2O5
0.4 moles of N2O4
0.5 moles of BiF3
“X” is an unknown element which forms an acid,
HXO3. The mass of 0.0133 mol of this acid is 1.123g.
Find the atomic mass of X and identify the element
represented by X. The element X is
A.
B.
C.
D.
E.
Chapter 3
1.
Which of the following samples contains the largest
total number of atoms?
C8H18
C16H3
C 3H 8
C5H12
C 4H 9
A Chem 110 TA synthesizes a compound composed
of carbon, hydrogen, and nitrogen and submits
0.1156 g of it to combustion analysis. The TA
recovers 0.3556 g of carbon dioxide and 0.0655 g of
water. What is the empirical formula of the
compound?
A.
B.
C.
D.
E.
22
C11H11
C20H18N2
C 5H 5N
C10H18
C10H9N
Chapter 4
Chapter 5
1.
1.
Which of the following aqueous solutions would you
expect to be the best conductor of electric current?
A.
B.
C.
D.
E.
2.
1.0 M sugar (C6H12O6)
1.0 M CaCl2
1.0 M ethanol (C2H5OH)
1.0 M acetic acid (HC2H3O2)
1.0 M NH4OH
A.
B.
C.
D.
E.
3.
A.
B.
C.
D.
E.
CH3COOH (HC2H3O2)
CH3COONa
C6H12O11 (table sugar)
NaClO4
2.
1 and 2 are weak electrolytes
1 and 3 are weak electrolytes
1, 2 and 3 are weak electrolytes
4 is the only weak electrolyte
1 is the only weak electrolyte
Given the following reactions and their enthalpy
changes
2 C2H2(g) + 5 O2(g) →
4 CO2(g) + 2 H2O(l)
C(s) + O2(g) → CO2(g)
ΔHRXN = –2599.2 kJ
2 H2(g) + O2(g) → 2 H2O(l)
ΔHRXN = –571.8 kJ
A.
B.
C.
D.
E.
1.1 L
910 mL
90 mL
540 mL
3.9 L
ΔHRXN = –393.5 kJ
620.2 kJ
−620.2 kJ
−453.4 kJ
226.7 kJ
None of the above is within 10% of the correct
answer
3.
Substance
SO2(g)
SO3(g)
SO2Cl2(g)
H2SO4((l)
H2O((l)
1.61 mL
7.73 mL
17.2 mL
41.5 mL
51.5 mL
ΔH° f (kJ/mol)
−297
−396
−364
−814
−286
The value of ΔH° for the following reaction is
–62.1 kJ. What is the value of ΔH°f (in kJ/mol) for
HCl(g)?
A 24.00 mL sample of a solution of Pb(ClO3)2 was
diluted with water to 52.00 mL. A 17.00 mL sample of
–
the dilute solution was found to contain 0.220 M ClO3
(aq). What was the concentration of Pb(ClO3)2 in the
original undiluted solution?
A.
B.
C.
D.
E.
ΔH = +189 kJ
ΔH = −4.97 kJ
ΔH = +388 kJ
ΔH = −194 kJ
None of the above is within 1% of the correct
answer
Calculate ΔH°f for acetylene, C2H2(g).
How many milliliters of a 132.00 mL solution of 1.98
M AlCl3 must be used to make 162.00 mL of a
–
solution that has a concentration of 0.630 M Cl (aq)?
A.
B.
C.
D.
E.
5.
the enthalpy of reaction (per mole of H2 produced) is
How much 0.154 M NaCl, “physiological saline,” can
be prepared by dilution of 100 mL of a 6.0 M NaCl
solution?
A.
B.
C.
D.
E.
4.
2 K(s) + 2 H2O(l) → 2 KOH(aq) + H2(g)
Which of the following are weak electrolytes?
1.
2.
3.
4.
It is found that 6.00 g of potassium metal reacts with
excess water to release 29.8 kJ of heat. This means
that, for the reaction
SO2Cl2(g) + 2 H2O(l) → H2SO4(l) + 2 HCl(g)
A.
B.
C.
D.
E.
–2
3.60 × 10 M
–2
7.19 × 10 M
0.238 M
0.156 M
0.477 M
23
−184
−372
−1079
30
−92
Chapter 5 continued
Chapter 6
4.
1.
For which one of the following equations is ΔH°rxn
equal to ΔH°f for the product?
A.
B.
C.
D.
E.
5.
Xe(g) + 2F2(g) → XeF4(g)
CH4(g) + 2Cl2(g) → CH2Cl2(ℓ) + 2 HCl(g)
N2(g) + O3(g) → N2O3(g)
2 CO(g) + O2(g) → 2 CO2(g)
None of the above have ΔH°rxn equal to ΔH°f
2.
−367.6 kJ
−183.8 kJ
−667.4 kJ
not determinable from the data given
None of the above answers is correct
The reaction is exothermic with ΔH = −46.2 kJ.
The reaction is endothermic with ΔH = −92.4 kJ.
The reaction is exothermic with ΔH = 92.4 kJ.
The reaction is endothermic with ΔH = 92.4 kJ.
The reaction is endothermic with ΔH = 46.2 kJ.
−
−
−
14
5.81 × 10 J
19
3.85 × 10 J
27
1.28 × 10 J
36
4.29 × 10 J
44
1.43 × 10 J
−
−
−
−
4. Which photon has an energy that is greater than the
energy of a blue photon?
A.
B.
C.
D.
E.
0.0100 mole of dry, solid KClO3 is added to 50.0 g of
water at 20.10°C in a coffee–cup calorimeter. The
temperature is observed to drop to 18.10°C. ΔH of
hydration for one mole of KClO3 is (within 2%) [Heat
capacity of water = 4.18 J/°C g]
A.
B.
C.
D.
E.
27
1.29 × 10 J
16
1.99 × 10 J
10
1.21 × 10 J
8
1.21 × 10 J
10
3.34 × 10 J
Green light of wavelength 516 nm is absorbed by an
atomic gas. What is the energy difference between
the two quantum states involved in the transition?
A.
B.
C.
D.
E.
2 NH3(g) → 3 H2(g) + N2(g)
7.
What is the energy possessed by one mole of
x–ray photons if the wavelength of the x–ray is 1.00 ×
9
10 m?
A.
B.
C.
D.
E.
The standard heat of formation of ammonia, NH3(g),
is –46.2 kJ/mole. Which of the following is true about
the reaction:
A.
B.
C.
D.
E.
7.25 × 10 km
7
2.99 × 10 km
4
2.99 × 10 km
3.02 km
none of these
−
3.
6.
3
A.
B.
C.
D.
E.
The standard heat of formation for H2O(g) is
–241.8 kJ/mol, and for NaOH(s) it is –425.6 kJ/mol.
The enthalpy change for the reaction between Na(s)
and H2O(g) to produce NaOH(s) and H2(g) is, per
mole of H2(g) produced,
A.
B.
C.
D.
E.
A radio station broadcasts on a frequency of 99.5
kilocycles/s. What is the wavelength of this radiation
in km?
–0.836 kJ
0.836 kJ
–42.8 kJ
42.8 kJ
None of the above answers is correct.
5.
A He-Ne laser (λ = 633nm) is used to heat up a
sample. How many photons are needed to transfer 12
J of heat to the sample?
A.
B.
C.
D.
E.
24
microwave photon
radio photon
green photon
infrared photon
ultraviolet photon
19
3.8 × 10
12,000
11
6.3 × 10
19
3.2 × 10
6
1.6 × 10
−
Chapter 6 continued
6.
If the Bohr model is used, what frequency of light
would be required for ionization of hydrogen?
14
A.
B.
C.
D.
E.
7.
6.17 × 10 Hz
3
1.31 × 10 Hz
15
3.29 × 10 Hz
10
4.31 × 10 Hz
None of the above is within 5% of the correct
answer
2.
3.
A.
B.
C.
D.
E.
The radius of the orbit increases as the
principal quantum number increases.
The energy required to ionize the atom
increases as the principal quantum number
decreases.
Light emitted by the excited hydrogen atom
corresponds to transitions from orbits of
higher principal quantum number to lower
principal quantum number.
A.
B.
C.
D.
E.
1s
2s
A.
(⇅)
(⇅)
(⇅) (↑)
B.
(⇅)
(⇅)
(⇅) (⇅) (⇅)
(↑)
C.
(⇅)
(⇅)
D.
(⇅)
(⇅)
(⇅) (⇅) ( )
(⇅) (⇅) (⇅)
(⇅)
E.
(⇅)
(⇅)
(↑)
For electron distributions, which of the following
statements are true?
A.
B.
C.
D.
E.
3
9
15
5
None of the above
2p
3s
(↑)
(↑)
(↑)
13. Which of the following ground state electron
configurations can be ruled out by the Pauli Exclusion
Principle?
n = 3 to n = 4
n = 1 to n = 3
n = 6 to n = 4
n = 7 to n = 5
n = 2 to n = 5
3.
mℓ
0
1
0
0
12. Which of the following could not be an orbital diagram
for an atom in its ground state?
1 only
1and 2 only
2 and 3 only
1 and 3 only
1, 2, and 3
1.
2.
n
ℓ
4
3
3
0
4
1
4
0
None of these
11. An atom of phosphorus 15P has how many electrons
with quantum number ℓ = 1?
Which of the following electron transitions in a
hydrogen atom results in the greatest release of
energy from the atom?
A.
B.
C.
D.
E.
9.
A.
B.
C.
D.
E.
Which of the following statements are true for the
Bohr model of the hydrogen atom?
1.
8.
10. Which series of quantum numbers describes the
orbital in which the highest energy electron in
potassium resides in the ground state?
d orbitals have a spherical shape.
p orbitals have a high electron density at the
nucleus.
s orbitals have no electron density at the
nucleus.
A.
B.
C.
D.
E.
1 and 2
2 only
2 and 3
3 only
None of the statements is true
25
1.
1s
3
2s
2
2p
5
2.
1s
2
2s
2
2p
7
3s
2
3.
1s
2
2s
2
2p
6
3s
2
3p
6
4.
1s
2
2s
2
2p
6
3s
2
3p
6
1 only
1 and 3 only
1, 2, and 3 only
1, 2, 3, and 4 only
1 and 4 only
4s
2
3d
12
Chapter 6 continued
Chapter 7
14. In the ground state electronic configuration of Cr, how
many total shells, subshells and orbitals contain at
least one electron, and how many unpaired electrons
are present?
1.
Shells Subshells Orbitals
A. Elements D and G should form a compound which
is a gas at room temperature and which has
formula GD.
B. Elements D and G should form a compound which
is a solid at room temperature with formula GD.
C. Elements D and G should not react with each
other.
D. Elements D and G should react to form a covalent
compound with formula DG7.
E. None of the above is a true statement.
Unpaired
Electrons
A.
4
3
8
4
B.
4
7
15
6
C.
4
7
15
4
D.
4
7
14
4
E.
4
7
14
6
Elements D, E, and G have atomic numbers Z, Z+1,
and Z+2 respectively. E is a noble gas (not helium).
Which statement is true?
2.
15. Which orbital diagram(s) represents an excited state
electron configuration of C?
Atom X is in Group IIA and atom Y is in Group VIIA.
A compound formed between these two elements
would have the formula
A.
B.
C.
D.
E.
i.
X 2Y
XY2
X 2Y 7
X 7Y 2
None of the above
ii.
3.
Which of the following has the configuration of a
noble gas?
A.
B.
C.
D.
E.
i only
iii only
ii and iii
i and iii
i, ii and iii
A.
B.
C.
D.
E.
16. When light of wavelength 420 nm is focused on a
metal surface, electrons are ejected with a speed of
5
7.00 × 10 m/sec. The binding energy of a mole of
electrons to the metal is
A.
B.
C.
D.
E.
2+
1.
2.
3.
iii.
4.
4
26
−
1 only
2 only
1 and 2
2 and 3
1 and 3
The species which may not have the electron
2
2
6
2
6
1
1
configuration 1s 2s 2p 3s 3p 4s 4d is
A.
B.
C.
D.
E.
8.22 × 10 J/mole
5
1.50 × 10 J/mole
2
2.72 × 10 J/mole
1
5.63 × 10 J/mole
None of the above is correct to within 5%
S
Br
4+
Si
2+
Sc
+
Sc
Ca
1
K
2+
Ti
−
Chapter 7 continued
5.
9.
Which of the following is a true statement?
2
2
−
7.
C. A valence electron in O
Cl(g)
Cl (g)
Cl(g) + e
Cl(g) + e
Cl(g)
−
−
−
→
→
→
→
→
+
Cl (g) + e
Cl(g) + e
+
Cl (g)
Cl (g)
Cl (g) + e
A.
B.
C.
D.
E.
−
−
−
A.
B.
C.
D.
E.
3+
1
2
3
4
5
A.
1s ⇅
2s ⇅
2p ⇅ ↑ ↑
B.
1s ⇅
2s ⇅
2p ⇅ ⇅ ↑
C.
1s ⇅
2s ⇅
2p ⇅ ↑ _
D.
1s ⇅
2s ⇅
2p ↑ ↑ ↑
E.
1s ⇅
2s ⇅
3s ⇅ 4s ⇅
12. Which of the following gives the correct relationships
among the first ionization energies of the elements?
Pick the pair that has the lowest (easiest to ionize)
ionization energy and the most endothermic (most
difficult to attach an electron) electron affinity.
Lowest I.E.
Cs
O
Na
Na
Cs
experiences the least
11. A correct orbital diagram for the ground state of the
+
O ion is
2+
The ionization energy for Li is expected to be
greater than that for H because:
A. Lithium is a metal whereas hydrogen is not.
B. The nuclear charge in lithium is greater than the
nuclear charge in hydrogen.
2+
C. The size of the Li ion is greater than the size of
the H atom.
D. The principal quantum number of the electron is
2+
greater in Li than in H.
E. The nucleus of the hydrogen atom has no
neutrons.
8.
2–
10. How many unpaired electrons are there in the Fe
ion when it is in its ground state?
−
−
–
effective nuclear charge.
D. All three species have a filled quantum level
n = 2.
–
E. F has the smallest radius.
The electron affinity of the chlorine atom is the energy
change which occurs in the reaction
A.
B.
C.
D.
E.
2−
A. The series is isoelectronic.
+
B. Na has the greatest ionization energy (for forming
2+
Na ).
4
A. The configuration 1s 2s 2p is the electronic
2
configuration of O .
2
2
3
B. The ground state for the configuration 1s 2s 2p
has one unpaired electron spin.
C. Sulfur is the only element in the third period with 2
unpaired electrons in the 3p subshell.
2
D. The configuration [Ar]3d is the configuration for
2+
Ti .
E. None of the above is a true statement.
6.
+
For the series of Na , O , F , which statement is
FALSE?
1.
2.
3.
4.
Most endothermic E.A.
O
Na
F
O
Mg
A.
B.
C.
D.
E.
27
Na
Rb
Se
He
>
>
>
>
Al > P
K > Li
S > O
Ne > Ar
1 only
2 only
3 only
4 only
Both 3 and 4 are correct.
Chapter 8
1.
Which of the following compounds would have the
largest lattice energy?
A.
B.
C.
D.
E.
2.
KF
KBr
CaO
PbS
ScN
A.
C
N
C
N
B.
C
N
N
C
C.
N
C
C
N
D.
E.
6.
Which of the following compounds would you expect
to possess a multiple bond?
A.
B.
C.
D.
E.
4.
CaO
CsI
BaS
NaF
NaCl
What is a reasonable Lewis structure for cyanogen,
C 2N 2?
Which of the following ionic crystals would you expect
to have the lowest melting point?
A.
B.
C.
D.
E.
3.
5.
SbH3
AlCl3
CBr4
C 2H 4
SiF4
H
C
O
H
7.
C
H
C
O
C
H
C
C
N
A.
B.
C.
D.
E.
O
8.
C
1.25 Å
N 2F 4
N 2F 2
N2
N2
N 2F 2
1.45 Å
N 2F 2
N 2F 4
N 2F 2
N 2F 4
N2
M: 2.1
Q: 2.4
R: 3.5
In which of the following diatomic molecules would
the least polar bond be expected?
H
H
E.
1.10 Å
N2
N2
N 2F 4
N 2F 2
N 2F 4
L: 1.1
H
D.
C
The electronegativities of four elements (L, M, Q, and
R) are as follows:
O
H
C.
N
Nitrogen–nitrogen bond lengths of 1.10, 1.25 and
1.45 Å have been measured for different molecules.
A.
B
C.
D.
E.
H
B.
N
Match the molecules N2F2, N2, N2F4 with appropriate
N−N bond length.
A reasonable Lewis structure for the molecule CH2O
is
A.
N
C
Which of the following species violates the octet rule?
A.
B.
C.
D.
E.
O
H
28
LM
MQ
QR
LR
MR
GeF4
TeF4
BH4
2
SO4
SiH4
−
−
Chapter 8 continued
9.
12. Given the following bond energies C−C (348
kJ/mole), C=C (614 kJ/mole), H−H (436 kJ/mole) and
the heat of reaction for the following process,
estimate the C−H bond energy.
Read the following statements:
1.
A.
B.
C.
D.
E.
BF3 and PF5 are examples of violations of the
octet rule.
2.
BF4 and BF3−NH3 are examples of violations
of the octet rule.
3.
Expanded valance shells occur most often
when the central atom is bonded to a small,
electronegative element.
4.
The central atoms most capable of having
expanded valence shells come from rows 3,
4, and 5 of the periodic table.
C 2H 4 + H 2 → C 2H 6
−
A.
B.
C.
D.
E.
ΔH = −137 kJ
420 kJ
283 kJ
525 kJ
350 kJ
645 kJ
13. Using the bond energy data tabulated below, estimate
the enthalpy of formation (per mole) of NH3(g).
Bond
Only statements 1, 3,and 4 are correct.
Only statements 1 and 4 are correct.
Only statements 2, 3, and 4 are correct.
Only statements 3 and 4 are correct.
Only statements 2 and 4 are correct.
N≡N(N2)
H−H
N−H
Average bond energy (kJ/mol)
941
436
391
The correct answer (in kJ/mol) is closest to
2−
10. From Lewis structures for SO2 and SO3 , we can
predict that
A.
B.
C.
D.
E.
A. SO2 has two different S−O bond lengths, one of
2
which is the same as in SO3 .
2
B. All S−O bonds in SO3 should be weaker than
S−O bonds in SO2.
2
C. All S−O bonds in SO3 are the same because
there are two Lewis resonance structures for this
ion.
2
D. S−O bonds in SO3 should be shorter than those
in SO2.
E. None of the above predictions follow from the
Lewis structures.
−
−
−422
−49
49
204
422
14. Following are some average bond energies (kJ/mol):
−
−
11. Which of the following is a TRUE statement?
A.
B.
C.
D.
SeO2 has two equivalent resonance structures.
XeF4 obeys the octet rule.
The structure NOBr is more stable than ONBr.
Because of fluorine’s high electronegativity, the
F−F bond is very polar.
E. None of the above statements is true.
C–H 413
O–H 463
C=C 614
C–C 348
O–O 146
C=O 799
C–O 358
O2 495
Estimate the heat released in the complete
combustion of ethylene, H2C=CH2.
A.
B.
C.
D.
E.
29
683 kJ/mol
802 kJ/mol
1297 kJ/mol
1403 kJ/mol
1792 kJ/mol
Organic
3. Which of the following Lewis structures are incorrect?
1.
Which of the following are not acceptable structures
for C4H10?
1)
2)
CH3
H
I
CH3 CH2 CH2 CH3
H
C C N
H
CH3 CH
H H H
CH3
H
C
C
H C C C H
4)
C H
H CH3
II
H H
H C H
C
2.
C
H
: :
H
III
CH3 CH CH2 CH3
H O C C N:
H
CH3
A.
B.
C.
D.
E.
H
C
H
H
5)
H
H
CH3
3)
H
1 and 2
2 and 3
3 and 4
3 and 5
1, 3 and 5
A.
B.
C.
D.
E.
I only
II only
III only
I and II
I, II and III
Which of the following is(are) not correct structure(s)
of octane C8H18?
1)
4. Of the structures shown below, which is a structural
isomer of n-pentane?
H
H
C H H H H
H
H
C C
C
C H
H C
C
C
H
H
H
H H H H
H
2)
H
H C
C
H
H
H H
H H
H
C C
C C
C H
C
H H
H
H
H
H
H
C
C
H C H
3)
H
H
H
C
H
A.
B.
C.
D.
E.
C
H
b)
C
CH2
CH CH3
CH3
CH3
CH CH CH2
CH3
CH3
H
H
H
C
CH3
H
c)
H
C
a)
CH3
CH CH2
CH2
d)
CH2
CH2
CH2
CH2
H
CH2
H
CH2
CH3
H
e)
CH3 CH2
C CH3
CH3
1 only
3 only
1 and 2
2 and 3
all of these are possible structures for octane
30
CH3
Organic continued
7.
5. Which of the compounds shown below can have a
geometrical isomer?
CH3 CH2
1.
CH3
C C
Which one of these molecules is an alcohol?
A.
B.
CH3CCH2CH3
H
OH
O
H
O
C.
CH2CH2CH3
D.
CH3
HCCH2CH3
2.
CH3
CH2
CH3
CH2
C C
CH3
E.
H
none of these are alcohols
8. Identify the functional groups present in the following
structure.
CH3
3.
H
C C
H
1. ester
2. ether
3. amine
4. ketone
5. amide
CH3
a) 1 only
b) 2 only
c) 3 only
d) 1 and 2
e) 2 and 3
H
N
O
A. 1 and 5
B. 2 and 5
C. 2 and 3
D. 4 and 5
E. 3 and 4
6. Which of the following is/are geometric isomers of the
structure below?
Br
9. Threonine is a naturally occuring amino acid found in
many proteins. What functional groups are present in
threonine?
C2H5
H3C
H OH H O
Cl
H C C C C OH
H H NH2
Br
Br
Cl
1
CH 3
Cl
H3C
C2H5
2
H3C
Cl
a) alcohol, amine, ketone
Br
C2H5
b) alcohol, amine, ester
c) carboxylic acid, alcohol, amide
3
d) alcohol, carboxylic acid, amine
e) amide, amine, alcohol
A. 1
B. 2
C. 3
D. 1 and 2
E. 1 and 3
31
Chapter 9
1.
4.
Which of the following are correct statements about
the valence–shell electron–pair repulsion (VSEPR)
model of bonding?
1.
2.
3.
BeF2
2.
3.
CF4
NF3
OF2
What is the correct trend in FMF bond angle?
A.
BeF2 > BF3
> CF4
> NF3
> OF2
Electron–pair geometry in all cases
B.
BeF2 = OF2
> CF4
> BF3
= NF3
C.
BeF2 = OF2
> BF3
= NF3
> CF4
D.
BeF2 > BF3
> OF2
> NF3
> CF4
E.
CF4
= NF3
> BeF2
= OF2
LARGEST
1 only
2 only
3 only
1, 2, and 3
None of the above
5.
SO2
SO3
2
SO4
NO3
BF3
A.
B.
C.
D.
E.
−
The number of bonding pairs of electrons, non–
bonding pairs of electrons and molecular shape of the
+
H3O ion are
Bonding
Pairs
Non–bonding
A.
4
Pairs
0
tetrahedral
B.
3
1
tetrahedral
C.
2
2
bent
D.
3
1
trigonal
pyramidal
E.
3
0
trigonal
planar
2−
1.
2.
3.
4.
−
6.
Molecular
Shape
−
1 only
1, 2 and 3
1 and 3
1, 3 and 4
3 and 4
TeI4
SeBr4
XeCl4
NH3
AlF4
−
The bond angles in H2O2 are approximately:
A.
B.
C.
D.
E.
32
CO3
SOCl2
+
H 3O
2
SO3
Which of the following molecules and ions possesses
a tetrahedral molecular structure?
A.
B.
C.
D.
E.
7.
> BF3
SMALLEST
Which of the following molecules has a trigonal planar
structure?
Which of the following is non–planar?
A.
B.
C.
D.
E.
BF3
Electron pairs orient themselves to give the
smallest angles possible.
Only bonding electron pairs are important in
the VSEPR model.
describes the spatial geometry of the atoms
in the molecule.
A.
B.
C.
D.
E.
Among the following gaseous molecules
90°
105°
109.5°
120°
180°
Chapter 9 continued
8.
11. Which of the following benzene–like molecules do
you expect to have the largest dipole moment?
Identify which of the following bonds is(are) polar and
which element in each is the more electronegative.
HCl
NO
F
Cl
Si2
A.
Now consider these five statements about your
conclusions.
1.
2.
3.
4.
5.
F
Cl
F
HCl is polar, with H the more electronegative.
HCl is polar, with the Cl the more
electronegative.
NO is polar, with the N the more
electronegative.
NO is polar, with O the more electronegative.
Si2 is polar.
F
H
H
F
F
B.
H
Cl
The correct statement(s) above is(are)
A.
B.
C.
D.
E.
F
H
H
C.
2 only
2 and 3 only
2 and 4 only
2, 3 and 5 only
1 and 4 only
H
H
Cl
H
H
9.
D.
Consider the following molecules.
1. BF3
2. NH3
3. SOCl2
H
4. SiF4
F
H
H
Which of these should have a dipole moment?
A.
B.
C.
D.
E.
F
H
F
E.
2 only
2, 3 and 4 only
1, 2 and 3 ony
1 and 4 only
2 and 3 only
H
H
F
12. Which of the following statements is true?
10. Which of the following molecules has the largest
dipole moment?
A.
B.
C.
D.
E.
A. There are two π bonds in
H
H
XeF2
XeF4
PF5
SF4
SF6
C
C
H
H
B. The H–N–H angle in NH3 is slightly larger than
the H–C–H angle in CH4.
2
C. In CO2, the carbon is sp hybridized.
D. The molecule below possesses a dipole moment.
Cl
H
C
C
H
Cl
E. None of the above statements is true.
33
Chapter 9 continued
16. The following molecule should be used
13. Which of the following is a correct set of electron–pair
geometry, hybridization, and bond angle(s)?
Geometry
Hybridization
A.
linear
sp
2
B.
trigonal
planar
sp
2
C.
octahedral
d sp
D.
tetrahedral
dsp
E.
trigonal
bipyramidal
d sp
2
2
3
3
H
C1 C2
Bond
Angle(s)
180°
120°
H
H
The hybridizations of C1, C2 and C3 respectively are
60°
A.
B.
C.
D.
E.
120°, 90°
14. Of the following statements about delocalized bonds,
which are true?
1.
2.
3.
4.
5.
A.
B.
C.
D.
E.
C
C3
109.5°
3
H
They occur in molecules with alternating
single and double bonds.
2
They can be made from sp hybrid σ bonds.
They are most often found in bonds involving
heavy atoms.
They can be made from π bonds.
They rarely, if ever, involve bonds with
fluorine.
C1
3
sp
3
sp
3
sp
3
dsp
C2
3
sp
sp
3
sp
sp
C3
2
sp
2
sp
3
sp
2
sp
None of the above.
17. Borazine B3N3H6 has been called inorganic benzene.
What is the hybridization of the boron atoms?
H
H
H
N
B
B
N
H
1, 4, and 5 only
4 and 5 only
1, 3, and 4 only
1, 2, and 3 only
All of the above
A.
B.
C.
D.
E.
15. Which of the following statements is incorrect?
A. Hybridization accounts for the experimental
observation that all F−C−F bond angles in CF4 are
the same.
B. All C−C bond distances in benzene, C6H6, are the
same.
C. The energy required to break a carbon–carbon
triple bond is greater than that needed to break a
carbon–carbon double bond.
D. The bonding in benzene, C6H6, includes 12 sigma
(σ) bonds and 3 localized pi (π) bonds.
E. The π electrons in NO3 are delocalized.
−
34
sp
2
sp
3
sp
4
sp
3
dsp
N
B
H
H
Chapter 10
1.
4.
The volume of a large, irregularly shaped, closed tank
is determined as follows. The tank is first evacuated,
and then it is connected to a 50.0 L cylinder of
compressed nitrogen gas. The gas pressure in the
cylinder, originally at 21.5 atm, falls to 1.55 atm
without a change in temperature. What is the volume
of the tank?
mass of A reacted:
5.00g
mass of B reacted:
20.00g
mass of C produced:
15.00g
moles of D produced: 0.208 moles
A. 100 L
B. 644 L
C. 25 L
D. 744 L
E. There is not sufficient information to determine the
volume of the tank.
2.
Solid substances A and B react to form a solid
product C and a gaseous product D. Solids A, B, and
C are weighed, and the volume, temperature and
pressure of gas D are measured. From this and the
ideal gas law, the number of moles of D are
calculated. The data are:
The molecular weight of D is
A.
B.
C.
D.
E.
Which curve represents the relationship between the
volume of an ideal gas and its temperature in K at
constant pressure?
5.
A gaseous compound having the empirical formula
CH2 has a density of 1.88 g/L at STP. The molecular
formula for this compound is (assuming ideal
behavior)
A.
B.
C.
D.
E.
6.
(E) None of the above.
3.
A. Equal numbers of moles of two ideal gases of
different molecular weight will fill the same volume
at the same temperature and pressure.
B. If the temperature of a given amount of an ideal
gas is held constant, its pressure is directly
proportional to the volume it occupies.
C. The density of an ideal gas is independent of the
volume it occupies at a given temperature and
pressure.
D. The mass of an ideal gas is proportional to its
pressure at a fixed volume and temperature.
E. The pressure of an ideal gas is proportional to its
absolute temperature if its density is held constant.
35
CH2
C 2H 4
C 3H 6
C 4H 8
Not determinable from the data given.
A gas which has a density of 2.77 g/L at STP is found
to contain the following weight percents: 51.6%
oxygen, 9.7% hydrogen, and 38.7% carbon. [Atomic
weights are: C = 12.00 amu; H = 1.00 amu; O = 16.00
amu] The molecular formula for this gas is
A.
B.
C.
D.
E.
Which statement about ideal gases is incorrect?
48.1
2.08
72.1
208
Impossible to determine from the data given.
CH3O
C3H10O
C 3H 9O 3
C 2H 6O 2
C 2H 4O
Chapter 10 continued
7.
10. 3.0 L of He gas at 5.6 atm pressure and 25°C and 4.5
L of Ne gas at 3.6 atm and 25°C are combined at
constant temperature into a 9.0 L flask. What is the
total pressure (in atm) in the 9.0 L flask?
Consider the following gases: H2S, H2, and SO2.
Which of the following statements is accurate at any
given temperature?
A.
B.
C.
D.
E.
A. The average kinetic energy of H2S is the same as
that for H2.
B. The rms speed of SO2 will be the same as that of
H2S.
C. The rms speed of SO2 will be greater than that of
H2S.
D. The average kinetic energy of SO2 will be greater
than that of either H2S or H2.
E. All molecules of H2S will have the same kinetic
energy.
8.
11. A student collects the following data in the process of
collecting nitrogen gas by water displacement:
Volume of gas collected: 73.2 mL
Temperature of room air and of water: 22.5°C
Barometric pressure: 752 mm Hg
Vapor pressure of water at 22.5°C (interpolated):
20.45 mm Hg
An ideal gas at 200.0 K and 1.50 atm pressure is
heated to 1000.0 K and kept at 1.50 atm pressure.
Which of the statements 1–4 below are true?
1.
2.
Assuming ideal gas behavior, which of the following is
the number of moles of N2 the student collected?
The root mean square speed of the
molecules increases by a factor of five.
The average molecular kinetic energy
A.
B.
C.
D.
E.
increases by a factor of twenty–five.
3.
4.
A.
B.
C.
D.
E.
9.
2.6
9.2
1.0
3.7
4.6
The collision frequency with a unit area of
container wall increases.
The average molecular kinetic energy
increases by a factor of five.
0.00290 moles N2
0.00299 moles N2
2.21 moles N2
2.27 moles N2
None of these is within 1% of the correct answer.
12. Which of the following statements is false?
A. Dalton’s law of partial pressures indicates that in
gaseous mixtures at low pressure each kind of
molecule behaves independently of the others.
B. At high pressures different gases give different
values for the ratio PV/nRT.
C. The mean free path of a molecule depends on its
size.
D. Collisions of molecules with the container walls
give rise to the gas pressure.
E. At a given temperature, for a given gas, every
molecule has the same speed.
1 and 2
2 and 3
3 and 4
3 only
4 only
Ideal gases A and B are kept in a 5.0–liter container
at 20°C. The pressure of the gas mixture is 2.0 atm
and it is known that 0.10 mole of gas A is present in
the mixture. How many moles of B are present in the
mixture? (MW of A = 25 amu; MW of B = 100 amu)
13. If the temperature of an ideal gas is held constant
while its volume doubles, which one of the following
happens?
A. Insufficient information given to calculate moles of
B present.
B. 0.32 moles
C. 0.25 moles
D. 0.42 moles
E. 0.48 moles
A. The average velocity of the molecule increases.
B. The frequency of collisions of gas molecules with
a given area of wall decreases.
C. The mean free path of the molecules remains
unchanged.
D. The density of the gas remains unchanged.
E. None of the above is a true statement.
36
Chapter 10 continued
2.
14. The properties of a real gas are most likely to deviate
from those properties predicted for an ideal gas when
A.
B.
C.
D.
E.
A. The large London dispersion forces between
helium atoms make helium difficult to liquefy.
B. Intermolecular forces in a liquid are weaker than
intramolecular forces.
C. Ion⎯ion forces in an ionic solution are
independent of the distances between ions.
D. Dipole⎯dipole forces dominate in interactions
between carbon dioxide molecules.
E. Van der Waals forces account for the cohesive
energy of an ionic liquid.
the pressure is low.
the temperature is high.
the pressure is high and the temperature is low.
the pressure is low and the temperature is high.
the density of the gas is low.
15. The fact that the ideal gas law only approximately
describes the behavior of a gas might be partly
explained by one or more of the following:
1.
2.
3.
4.
Which of the following statements about
intermolecular forces is true?
3.
R is not really a constant.
Gas molecules really do not have zero
volume.
The kinetic energy of gas molecules is not
really directly proportional to the absolute
temperature.
Gas molecules really do interact with each
other.
Elementary phosphorus is a solid consisting of P4
molecules and melts at 44°C. The principal forces
between the molecules in the solid must be
A.
B.
C.
D.
E.
London dispersion.
ionic.
covalent.
dipolar.
metallic.
Which are correct?
A.
B.
C.
D.
E.
4.
2 only
3 only
4 only
1 and 2
2 and 4
The boiling points of the substances MgO, Ne, and
H2O should increase in the order
A.
B.
C.
D.
E.
H2O < MgO < Ne
Ne < MgO < H2O
MgO < Ne < H2O
MgO < H2O < Ne
Ne < H2O < MgO
Chapter 11
1.
5.
The boiling point of ammonia, NH3, is significantly
higher than that of analogous compounds from the
same group, e.g., PH3, AsH3, and SbH3. The
principal reason for the abnormally high boiling point
is
A.
B.
C.
D.
E.
The viscosity of a liquid is an important factor in
A.
B.
C.
D.
E.
London dispersion forces
ion⎯dipole forces
dipole⎯dipole interactions
hydrogen bonding
ion⎯induced dipole forces
6.
Which of the following properties is not increased
when the strength of intermolecular forces in a liquid
is increased?
A.
B.
C.
D.
E.
37
its rate of evaporation.
capillary rise.
bubble formation.
rate of flow through a tube.
its vapor pressure.
vapor pressure
heat of vaporization
viscosity
surface tension
normal boiling point
Chapter 11 continued
7.
10.
Consider the three compounds sketched below:
H H H H
H C C C C O H
H H H
H O C C C O H
H H H
F C C C
H H H H
H H H
H H H
1
2
3
F
The viscosities of these three compounds should
increase in the order
A.
B.
C.
D.
E.
8.
1<2<3
2<3<1
3<2<1
3<1<2
1<3<2
The vapor pressure curves for two substances are
shown in the figure. Identify which of X or Y has the
higher normal boiling point and the larger
intermolecular forces.
A pure substance has a triple point in its phase
diagram at 216 K and 5.1 atm. This means that:
Higher Boiling
Point
A. at a pressure of one atmosphere the substance
can coexist as a solid and vapor.
B. at room temperature and one atmosphere
pressure the substance is a liquid.
C. above the triple point pressure and temperature
the substance can exist only as a vapor.
D. at a constant temperature of 216 K the substance
is a solid at any pressure.
E. at a constant pressure of 5.1 atm the substance is
a liquid at any temperature.
9.
A.
B.
C.
D.
E.
Solid CO2 sinks in liquid CO2, and the triple point of
CO2 is at –56.4°C and 5.11 atm pressure. What state
of CO2 exists at –56.4°C and 6.00 atm pressure?
A.
B.
C.
D.
E.
Gas
Liquid
Solid
Supercritical fluid
Mixture of solid and liquid
.
38
Larger
Intermolecular
Forces
Y
Y
X
X
Y
X
X
Y
Insufficient data given to determine the
answer.
Chapter 11 continued
12.
11.
Which of the following compounds has the lowest
vapor pressure at 0 °C?
A.
Which of the following would you expect to have
the highest boiling point?
CH3 CH CH2 CH3
CH3
A
H
B.
C
CH3 CH
H
CH3
B
OH
C.
C HO
OH
CH3
D.
D
CH3
H3C
C
CH3
H
H
H
H
H H
H
C
C
C
C C
C
H
H
H
H C H
H
H
H
H
H H H H
H
H
C
C
C H
H C
C
C
H
H
H
H
H
H
CH3
H H H H H H
OH
E HOH C
2
E.
C
CH2OH
H C C C C C C H
H H H H
H
H C H
H C H
H
H
39
Chapter 11 continued
Chapter 13
13. Rank these in order of decreasing boiling point
1.
The mole fraction of CO2 in a certain solution with
4
H2O as the solvent is 3.6 × 10 . The molality of CO2
in this solution is about
−
A.
B.
C.
D.
E.
H H H
i)
H—C—C—C—H
H H H
2.
H Cl
ii)
iii)
H
Cl
H H
A.
B.
C.
D.
E.
A solution contains 4.00 g NaOH, 5.61 g KOH, and
1.03 g RbOH in 90.0 g of water. The solution has a
density of 1.08 g/mL. What is the molality of OH ?
A.
B.
C.
D.
E.
H—C—C—C—Br
H
−
−
H—C—C—Br
H
0.00036 m
0.0065 m
0.020 m
5
2.0 × 10 m
6.5 m
3.
2.33 m
2.09 m
2.52 m
2.16 m
None of the above is within 2% of the correct
answer.
The mole fraction of HCl in a 36% by weight aqueous
solution of HCl is
H H
A.
B.
C.
D.
E.
iii > ii > i
i > ii > iii
ii> i > iii
iii > i > ii
i > iii > ii
4.
A solution whose density is 0.935 g/mL contains
30.0% by weight H2CO, 10.0% C2H5OH and 60.0%
H2O. The molarity of the H2CO is
A.
B.
C.
D.
E.
5.
9.34 M
2.32 M
0.0107 M
4.51 M
0.0214 M
27.0 L of HCl gas at STP is dissolved in water, giving
785 mL of solution. The molarity of the HCl solution
is:
A.
B.
C.
D.
E.
40
0.11
0.22
0.36
0.64
0.99
9.46 M
1.53 M
0.946 M
15.3 M
None of the above is within 1% of the correct
answer.
Chapter 13 continued
6.
10.
Which one of the following statements is true?
A.
B.
C.
D.
A. The heat of solution in H2O for KOH is the same
as that for KOH H2O.
B. For a compound to spontaneously dissolve in H2O
at 25°C, the solution process must be exothermic.
C. Ne is less soluble in H2O at 2 atm pressure than at
1 atm pressure.
D. C2H4 is very soluble in liquid NH3.
E. None of the above.
Given the solutes NaCl and I2 and the solvents NH3(l)
and C7H16 (heptane), which is true?
CH2OH
Which one of the following would you expect to be
LEAST soluble in water
A.
B.
C.
D.
A. NaCl and I2 are both more soluble in NH3 than in
C7H16.
B. NaCl and I2 are both more soluble in C7H16 than in
NH3.
C. NaCl is more soluble in NH3; I2 is more soluble in
C7H16.
D. NaCl is more soluble in C7H16; I2 is more soluble in
C7H16.
E. In order to determine relative solubilities in these
cases one must know whether the solution
reactions are exothermic or endothermic.
8.
CH3OH
CH3CH2CH2OH
CH3CH2 CH2 CH2CH2OH
CH3CH2 CH2 CH2CH2CH3
E.
11.
7.
Which one of the following would you expect to me
MOST soluble in water?
CH3OH
CH3CH2CH2OH
CH3CH2 CH2 CH2CH2OH
CH3CH2 CH2 CH2CH2CH3
E.
CH2OH
12.
Rank these in order of decreasing solubility in water.
i)
The Henry’s law constant for He gas in H2O at 30°C
4
is 3.7 × 10 M/atm; that for N2 at 30°C is
4
6.0 × 10 M/atm. If a gaseous He-N2 mixture that has
a He mole fraction of 0.30 is placed over the water
CH3
−
−
ii) HO
A. the concentration of dissolved He will be greater
than that of dissolved N2.
B. the concentration ratio of dissolved He to
dissolved N2 would be 0.62.
C. the concentration ratio of dissolved He to
dissolved N2 will be 0.26.
D. the concentration ratio of dissolved He to
dissolved N2 will be 0.18.
E. the concentration ratio of dissolved He to
dissolved N2 will be 0.49.
9.
CH3
iii) CH3CH2OH
A.
B.
C.
D.
E.
A saturated solution of silver chloride, AgCl is weakly
conducting for electricity because
i > ii> iii
iii > i = ii
ii > iii > i
iii > ii > i
i = ii > iii
13. Arrange the following aqueous solutions in order of
increasing boiling points:
A. AgCl is essentially 100% ionized in solution, but is
not very soluble.
B. AgCl is quite soluble, but only dissociates into ions
slightly, in solution.
C. AgCl does not produce ions itself, but rather
induces hydrolysis to give AgOH and HCl, in
water.
D. AgCl is only slightly ionized in solution, and also is
only slightly soluble.
E. None of the above is a true statement.
1.
2.
3.
4.
5.
A.
B.
C.
D.
E.
41
0.1 M Fe2(SO4)3
0.2 M BaCl2
0.3 M glucose (blood sugar)
0.2 M LiCl
0.2 M AlCl3
3, 4, 2, 1, 5
2, 4, 5, 1, 3
5, 3, 1, 4, 2
3, 4, 1, 2, 5
3, 5, 2, 1, 4
Chapter 13 continued
18. Arrange the following aqueous solutions in order of
increasing vapor pressure:
14. Consider a solvent whose molecular weight is 100.0
amu and whose vapor pressure at 25°C is 25.00 mm
Hg. 100.0 g of a nonvolatile solute whose molecular
weight is 50.00 amu is dissolved in 1.000 kg of that
solvent. The solute is not an electrolyte. What is the
vapor pressure of the solution at 25°C?
A.
B.
C.
D.
E.
1.
2.
3.
4.
5.
A.
B.
C.
D.
E.
0.01 mm Hg
20.8 mm Hg
22.7 mm Hg
24.9 mm Hg
25.0 mm Hg
15. The compound ethylene glycol, C2H6O2, is widely
used as an automotive antifreeze. What is the
minimum weight, in grams, of this compound that
must be added to 8 kg of water to produce a solution
that will protect an automobile cooling system from
freezing at −20°F (−28.9°C)? Ethylene glycol is a
non–electrolyte.
A.
B.
C.
D.
E.
1, 2, 3, 4, 5
5, 4, 3, 2, 1
2, 1, 4, 3, 5
4, 2, 3, 1, 5
5, 3, 4, 1, 2
Chapter 15
1.
32.0
121
7720
965
5342
Kc for the reaction HCl(g) + NH3(g) → NH4Cl(s) is
A.
[NH 4 Cl]
[HCl][NH 3 ]
B.
[HCl][NH 3 ]
[NH 4 Cl]
C.
1
[HCl][NH 3 ]
D. [HCl] [NH3]
16. 7.50 g of a compound having the empirical formula
CH2O is dissolved in water to form 100.0 mL of
solution. This solution does not conduct electric
current and is found to have an osmotic pressure of
12.2 atm. at 25°C. The molecular formula for the
compound is
A.
B.
C.
D.
E.
0.5 M NaCl
0.4 M Na2SO4
0.1 M KCl
0.1 M Al2(SO4)3
0.1 M C6H12O6 (sugar)
E. [NH4Cl]
2.
CH2O
C 3H 6O 6
C5H10O5
C6H12O6
None of the above is the correct answer
Consider the following three reactions:
1.
H2(g) + Cl2(g) ⇄ 2 HCl(g)
2.
C(s) + H2O(g) ⇄ CO(g) + H2(g)
3.
Fe3O4(s) + 4H2(g) ⇄ 3 Fe(s) + 4H2O(g)
For which of these would Kp = Kc?
A.
B.
C.
D.
E.
17. The addition of nonvolatile solute to a solvent
A. increases the boiling point, decreases the freezing
point and increases the vapor pressure of the
solvent.
B. decreases the boiling point, decreases the
freezing point and decreases the vapor pressure
of the solvent.
C. decreases the boiling point, increases the freezing
point and increases the vapor pressure of the
solvent.
D. increases the boiling point, decreases the freezing
point and decreases the vapor pressure of the
solvent.
E. increases the boiling point, decreases the freezing
point but leaves the vapor pressure of the solvent
unaffected.
3.
1 only
1 and 2 only
1 and 3 only
3 only
2 and 3 only
3
At 50°C, Kc = 2.2 × 10 for the reaction
3 Fe(s) + 4 H2O(g) ⇄ Fe3O4(s) + 4 H2(g)
What is the value of Kp at 200°C for this reaction?
A.
B.
C.
D.
E.
42
3
8.8 × 10
3
2.2 × 10
2
5.5 × 10
4
3.5 × 10
This question cannot be answered with the
information provided
Chapter 15 continued
4.
7.
For the following reaction, Kp = 1.96 at 700 K.
NOCl(g) ⇄ NO(g) + ½ Cl2(g)
At this same temperature, Kp for the reaction
Cl2(g) + 2 NO(g) ⇄ 2 NOCl (g)
A.
B.
C.
D.
E.
is
A.
B.
C.
D.
E.
5.
6.
1.96
3.85
0.260
0.509
None of the above is within 5% of the correct
answer.
8.
Kc for the reaction F2(g) + Cl2(g) ⇄ 2 FCl(g) equals
125 at a particular temperature. Suppose a system
involving this reaction is already at equilibrium and
the concentrations of F2 and Cl2 are found to be [F2] =
0.115 M and [Cl2] = 0.221 M. What is the
concentration of FCl in the system?
A.
B.
C.
D.
E.
2
[NO] = 0.25 M
[NO] = 0.50 M
[NO] = 1.0 M
[NO] = 0.67 M
None of the above is within 5% of the correct
answer
−
9.
At 750°C, Kp = 0.770 for the reaction
H2(g) + CO2(g) ⇄ H2O(g) + CO(g)
At a certain temperature, 0.300 moles of NO, 0.200
moles of Cl2, and 0.500 moles of ClNO were placed in
a 25.0 L vessel and allowed to reach equilibrium:
If 0.200 atm of H2 and 0.200 atm of CO2 are admitted
into a rigid container and allowed to reach equilibrium,
what should the equilibrium partial pressure of CO
be?
2 NO(g) + Cl2(g) ⇄ 2 ClNO(g).
At equilibrium, 0.600 moles of ClNO were present.
The number of moles of Cl2 present at equilibrium is
A.
B.
C.
D.
E.
6 – (X/2)
6–X
6 – 2X
3 – 2X
None of the above is correct
For the reaction N2(g) + O2(g) ⇄ 2 NO(g) Kc = 4.0 at a
particular temperature. Suppose we begin an
experiment by mixing 1.0 mol of N2 and 1.0 mol of O2
in a 1.0–liter container. What will be the
concentration of NO once equilibrium is reached at
the given temperature?
A.
B.
C.
D.
E.
[FCl] = 2.54 × 10 M
[FCl] = 3.17 M
[FCl] = 1.78 M
2
[FCl] = 1.43 × 10 M
None of the above is within 5% of the correct
answer
−
Consider the reaction 2 NH3(g) ⇄ N2(g) + 3 H2(g).
Suppose 6 moles of pure NH3 are placed in a 1.0–liter
flask and allowed to reach equilibrium. If X
represents the concentration in moles per liter of N2
present in the system once equilibrium is reached,
which one of the following will represent the
concentration of NH3 at equilibrium in moles per liter?
A.
B.
C.
D.
E.
0.100
0.150
0.200
0.250
0.300
43
0.0935 atm
0.109 atm
1.43 atm
0.100 atm
0.770 atm
13. For the reaction FeO(s) + CO(g) ⇄ Fe(s) + CO2(g),
Chapter 15 continued
10. At high temperatures one mole of hydrogen gas
reacts with one mole of bromine gas to form hydrogen
bromide. At a given temperature the equilibrium
constant is 57.6. If at the same temperature, a
3
3
mixture of 4.67 × 10 M bromine gas, 2.14 × 10
2
hydrogen gas, and 2.40 × 10 M hydrogen bromide
gas is made, then
−
A. the usual expression for the equilibrium constant is
Kc = [Fe] [CO2 ]
[FeO] [CO]
B. addition of CO2(g) will increase Kc.
C. increasing the volume of an equilibrium mixture at
constant temperature will cause the number of
−
−
moles of CO2 to increase as the mixture re–
A. the system is at equilibrium.
B. the system is far from equilibrium and will shift to
form more hydrogen gas.
C. the system is far from equilibrium and will shift to
form more hydrogen bromide gas.
D. nothing can be deduced since we do not know
whether the reaction is endothermic or exothermic.
E. nothing can be deduced since we do not know
whether the equilibrium constant is Kc or Kp.
equilibrates.
D. adding more FeO to an equilibrium mixture will
cause the number of moles of CO2 to increase as
the system re–equilibrates.
E. None of the above statements is true
Chapter 18
11. Which one of the following equilibriums is least
affected by a change in the volume of the system?
1.
A. 2 C(s) + O2(g) ⇄ 2 CO(g)
B. 2 NO2(g) ⇄ N2O4(g)
A.
B.
C.
D.
E.
C. H2(g) + S(ℓ) ⇄ H2S(g)
D. H2O(ℓ) ⇄ H2O(g)
E. 2 NO(g) + Cl2(g) ⇄ 2 NOCl(g)
12. Nickel (II) oxide can be reduced to nickel metal by
treatment with carbon monoxide as indicated in the
reaction
2.
If the reaction chamber contains some solid Ni and
NiO, 400 mm Hg of CO2 and 20 mm Hg of CO, all at
equilibrium, which one of the following changes will
lead to the reduction of more nickel oxide at 500°C?
3.
Doubling the amount of NiO(s) present.
Adding CO2 to raise its pressure to 700 mm Hg.
Adding CO to raise its pressure to 40 mm Hg.
Removal of half of the NiO(s) present.
Doubling the volume of the reaction chamber at
500°C.
275 nm
45.0 nm
742 nm
353 nm
137 nm
Which species is primarily responsible for absorbing
ultraviolet radiation in the stratosphere?
A.
B.
C.
D.
E.
44
CFCl3
CO2
O2
N2
NO2
The C−Cl bond dissociation energy in CF3Cl is 339
kJ/mol. What is the maximum wavelength of photons
that can rupture this bond?
A.
B.
C.
D.
E.
CO(g) + NiO(s) ⇄ CO2(g) + Ni(s) Kp=20 at 500°C
A.
B.
C.
D.
E.
Select the substance that is thought to be partially
responsible for depleting the concentration of ozone
in the upper atmosphere.
N2
O3
CO
CH2Cl2
CO2
REACTIONS
1.
5.
When the following equation
A. the compound contains C, H, and some other
element of unknown identity, so we can’t calculate
the empirical formula.
B. the compound contains only C and H and has the
empirical formula of C6H.
C. the compound contains C, H, and O and has the
empirical formula of CH3O.
D. the compound contains only C and H and has the
empirical formula of CH2.
E. None of the above is a true statement
C9H15S + O2 → CO2 + H2O + SO2
is balanced with the smallest possible set of integer
coefficients (no fractions), the coefficient preceding
CO2 is
A.
B.
C.
D.
E.
9
27
36
18
None of the above is correct
6.
2.
When the equation for the complete combustion of
ethanol, C2H5OH, to form CO2 and H2O is balanced
with lowest–integer coefficients, the coefficient for O2
is
A.
B.
C.
D.
E.
3.
Mixing solutions of K2SO4(aq) and BaCl2(aq)
produces an insoluble salt. Which of the following is
the correct list of spectator ions for this reaction?
A.
B.
C.
D.
E.
7
6
5
3
None of the above answers is correct
7.
A 100.0 g sample of a metal M is burned in air to
produce 103.7 g of its oxide with the formula M2O.
What is the atomic mass of the metal?
A.
B.
C.
D.
E.
1.00 g of a compound is combusted in oxygen and
found to give 3.14 g of CO2 and 1.29 g of H2O. From
these data we can tell that
+
2–
K , SO4 , Ba
+
2–
K , SO4
+
–
K , Cl
2+
–
Ba , Cl
2+
2–
Ba , SO4
2+
+3
2−
2+
A. 2Fe (aq)+ 3SO4 (aq) + 3Pb (aq)+ 6NO3 (aq) →
73 amu
150 amu
216 amu
290 amu
370 amu
2+
−
2−
2Fe(NO3)3(s) + 3Pb (aq) + 3SO4 (aq)
+3
2−
2+
B. Fe (aq)+ SO4 (aq) + Pb (aq) + 3NO3 (aq) →
−
Fe(NO3)3(s) + PbSO4(s)
C. Fe (aq) + 3NO3 (aq) → Fe(NO3)3(s)
4.31 g of a hydrocarbon is completely combusted in
oxygen and found to yield 6.36 g of water. The
empirical formula for the hydrocarbon is
A.
B.
C.
D.
E.
–
When aqueous solutions of Fe2(SO4)3 (aq) and
Pb(NO3)2(aq) are mixed, an insoluble salt forms.
Which of the following reactions is the correct net
ionic equation that describes this reaction?
+3
4.
, Cl
−
2+
D. Pb (aq)+ 2NO3 (aq) → Pb(NO3)2(s)
2+
−
2−
E. Pb (aq)+ SO4 (aq)→ PbSO4(s)
C 3H 7
CH4
C 7H 4
C21H4
CH
8.
Which of these reactions will form a precipitate in
water?
A. Mg(OH )2 + 2 HCl → Mg(Cl)2 + 2H2O
B. Mg(OH)2 + (NH4)2SO4 → MgSO4 + 2 NH3 + 2 H2O
C. CaCO3 + 2 HCl → CaCl2 + CO2 + H2O
D. HCl + CH3COOK → CH3COOH + KCl
E. Ba(NO3)2 + K2SO4 → BaSO4 + 2 KNO3
45
REACTIONS continued
12. The oxidation number of Mo (molybdenum) in
6
Mo7O24 is:
−
9.
Which one of the following (unbalanced) equations
describes a spontaneous reaction?
A.
B.
C.
D.
E.
A. Ag(s) + HCl(aq) → AgCl(s) + H2(g)
3+
2+
B. Hg(l) + Al (aq) → Hg (aq) + Al(s)
2+
+6
+5
+4
+3
+2
2+
C. Cu (aq) + Zn(s) → Cu(s) + Zn (aq)
D. Ni(s) + H2O(l) → Ni(OH)2(s) + H2(g)
13. 100.0 mL of Ca(OH)2 solution is titrated with
2
5.00 × 10 M HBr. It requires 36.5 mL of the acid
solution for neutralization. The concentration of the
Ca(OH)2 solution is
E. None of the above describes a spontaneous
reaction.
10.
−
A.
B.
C.
D.
E.
Given that the three standard reactions shown below
proceed as written, which of the subsequent 3
reactions do not occur.
Standard reactions
Mg(s) + ZnCl2(aq) → Zn(s) + MgCl2(aq)
3
9.12 × 10 M
4
1.82 × 10 M
4
9.12 × 10 M
3
1.82 × 10 M
None of the above is within 1% of the correct
answer
−
−
−
−
Zn(s) + FeCl2(aq) → Fe(s) + ZnCl2(aq)
14. Given the balanced equation for the oxidation of
ethanol, C2H5OH, by potassium dichromate:
Fe(s) + CuCl2(aq) → Cu(s) + FeCl2(aq)
I.
Mg(s) + FeCl2(aq) → Fe(s) + MgCl2(aq)
3C2H5OH + 2K2Cr2O7 + 16HCl →
II. Zn(s) + CuCl2(aq) → Cu(s) + ZnCl2(aq)
3C2H4O2 + 4CrCl3 + 4KCl + 11H2O
III. Fe(s) + ZnCl2(aq) → Zn(s) + FeCl2(aq)
A.
I only
B.
II only
C.
III only
D.
I and II
E.
I and III
Calculate the volume of a 0.600 M K2Cr2O7 solution
needed to generate 0.1665 moles of C2H4O2 from a
solution containing excess ethanol and HCl.
A.
B.
C.
D.
E.
11. Which of the following reactions are redox reactions?
15. How many grams of solid NaOH will be needed to
neutralize 85.0 mL of a 0.275 M solution of H2SO4?
1. Ni(OH)2(s) + H2SO4(aq) → NiSO4(aq) + 2 H2O()
A.
B.
C.
D.
E.
2. 8 NH3(g) + 6 NO2(g) → 7 N2(g) + 12 H2O()
3. 3 PbO(s) + 2 NH3(aq) → N2(g) + 3 H2O() + 3 Pb(s)
A.
B.
C.
D.
E.
278 mL
185 mL
111 mL
6.60 mL
None of the above answers is correct
1 only
2 only
3 only
1 and 3
2 and 3
0.94 g
19.1 g
1.87 g
0.47 g
6.41 g
16. When 47.3 mL of 0.107 M HCl is added to 54.7 mL of
0.213 M NaOH, the resulting OH concentration is:
−
A.
B.
C.
D.
E.
46
0.028 M
0.065 M
0.114 M
0.120 M
0.213 M
REACTIONS continued
17. A method of removing CO2(g) from a spacecraft is to
allow it to react with solid NaOH:
20. Which of the following compounds would react most
rapidly with bromine (Br2) at room temperature?
a) pentane
2 NaOH(s) + CO2(g) → Na2CO3(s) + H2O(ℓ)
How many liters of CO2(g) at 26.0°C and 755 mm Hg
can be removed per kg NaOH?
b) toluene
A.
B.
C.
D.
E.
c) ethanol
24.7
16.3
12400
618
309
e) 2-hexene
CH3 - CH2 - OH
CH3 - CH2 - CH2 - CH = CH - CH3
21. Choose the appropriate words to fill in the blanks. A
condensation reaction between a _______ and a
_______ will form an _________.
10.0 L
20.0 L
30.0 L
40.0 L
None of the above is correct.
A. amide, ester, alcohol
B. amine, carboxylic acid, amide
C. alcohol, amine, amide
D. alcohol, alcohol, ester
E. alcohol, carboxylic acid, amide
19. The following reactions involve only gases. Which of
them, if carried out in a closed container at constant
temperature, would proceed with a decrease in
pressure?
A.
B.
C.
D.
E.
CH3
d) cyclopentane
18. A gaseous sample of pure methane, CH4, is found to
occupy a volume of 20.0 L at 25°C and 1 atm
pressure. What volume of O2, at the same
temperature and pressure, should be just sufficient to
permit complete combustion of the methane?
A.
B.
C.
D.
E.
CH3 - CH2 - CH2 - CH2 - CH3
2 CO + O2 → 2 CO2
2 NH3 → N2 + 3 H2
N2 + O2 → 2 NO
2 O3 → 3 O2
2 HI → H2 + I2
47
Chem 110
Supplemental Problems
Answer Key
Chapter 1
1.
A
2.
E
3.
B
4.
C
5.
A
Chapter 2
1.
C
2.
A
3.
D
4.
D
5.
D
Chapter 3
1.
C
2.
B
3.
A
4.
E
5.
D
6.
B
7.
B
8.
D
9.
E
Chapter 4
1.
B
2.
E
3.
E
4.
C
5.
C
Chapter 5
1.
E
2.
D
3.
E
4.
A
5.
A
6.
D
7.
D
Chapter 6
1.
D
2.
D
3.
B
4.
E
5.
A
6.
C
7.
E
8.
C
9.
E
10.
D
11.
B
12.
C
13.
C
14.
B
15.
A
16.
B
Chapter 7
1.
B
2.
B
3.
D
4.
A
5.
D
6.
D
7.
B
8.
E
9.
E
10.
E
11.
D
12.
D
Chapter 8
1.
A
2.
B
3.
D
4.
B
5.
E
6.
B
7.
B
8.
B
9.
A
10.
B
11.
A
12.
A
13.
B
14.
C
Organic
1.
D
2.
D
3.
D
4.
A
5.
C
6.
B
7.
B
8.
E
9.
D
Chapter 9
1.
E
2.
C
3.
D
4.
A
5.
A
6.
E
7.
B
8.
C
9.
E
10.
D
11.
D
12.
E
13.
B
14.
A
15.
D
16.
E
17.
B
Chapter 10
1.
B
2.
B
3.
B
4.
A
5.
C
6.
D
7.
A
8.
E
9.
B
10.
D
11.
A
12.
E
13.
B
14.
C
15.
E
48
Chapter 11
1.
D
2.
B
3.
A
4.
E
5.
D
6.
A
7.
D
8.
A
9.
C
10.
A
11.
E
12.
E
13.
A
Chapter 13
1.
C
2.
A
3.
B
4.
A
5.
B
6.
E
7.
C
8.
C
9.
A
10.
A
11.
D
12.
D
13.
D
14.
B
15.
C
16.
C
17.
D
18.
C
Chapter 15
1.
C
2.
C
3.
E
4.
C
5.
C
6.
B
7.
C
8.
C
9.
A
10.
A
11.
C
12.
C
13.
E
Chapter 18
1.
A
2.
D
3.
B
Chemical
Reactions
1.
C
2.
D
3.
C
4.
A
5.
D
6.
C
7.
E
8.
E
9.
C
10.
C
11.
E
12.
A
13.
A
14.
B
15.
C
16.
B
17.
E
18.
D
19.
A
20.
E
21.
B
49