Past Exam Questions_Exam 2_Fa2023
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11500 Past Exam Questions
Exam 2
Fall 2023
DISCLAIMER:
These questions are from past 11500 exams.
Your exam this year will be a
mixture
of multiple choice and open response questions.
We are providing these questions to give you an idea of what types of questions might be on
your exam this year.
This is NOT a practice exam.
Make sure to study ALL the concepts
and calculations covered by the Learning Objectives.
The answer key is on p. 12.
1.
One piece of gold jewelry at 120 °C has exactly one half of the mass of another piece, which
is at 40 °C. Both pieces are placed inside a calorimeter whose heat capacity is negligible.
What is the final temperature inside the calorimeter in °C?
2.
If you wished to warm your room by taking 10 kg of a heated substance at 99 °C into it,
which one of the following would be the best choice? The specific heat capacity for each
substance is given in parentheses.
(a)
iron (0.450 J/g·K)
(b) copper (0.387 J/g·K)
(c)
granite (0.79 J/g·K)
(d) gold (0.129 J/g·K)
(e)
water (4.184 J/g·K)
Page
1
of
12
3.
A student in lab combined 41.514 g
of 1.0 M HCl solution (
d
= 1.0 g/mL)
with 51.158 g of 1.0 M NaOH
solution (
d
= 1.0 g/mL) in a coffee
cup calorimeter and recorded the
temperature data below.
Calculate
the enthalpy change (
∆ H
rxn
°
) in kJ
per mole of HCl.
(Assume the
specific heat capacity of the solution
is the same as water, 4.184 J/g K.)
‧
HCl(
aq
) + NaOH(
aq
)
→
H
2
O(
l
) + NaCl(
aq
)
T
i
= 20.39
°
C
T
f
= 26.95
°
C
4.
A student in lab added 4.029 g of solid CaCl
2
·2 H
2
O to 49.03 g of deionized water at 20.77
°C in a coffee cup calorimeter.
The maximum temperature measured in the calorimeter after
the addition of the solid was 26.20 °C.
Calculate ΔH (in kJ/mol) for the dissolution of
CaCl
2
·2 H
2
O.
Assume that the solution has the same specific heat capacity as water.
Page
2
of
12
5.
Choose the
best
answers to complete the following sentences based on the information given
below.
When 50.0 mL of 1.0 M HCl and 50.0 mL of 1.0 M NaOH are combined at room
temperature in a coffee cup calorimeter, the temperature of the resulting solution is
higher
than room temperature.
The reaction of HCl and NaOH is an _____________ process.
The sign of q
solution
is _________________________.
(a)
endothermic; positive
(b) endothermic; negative
(c)
exothermic; positive
(d) exothermic; negative
6.
Deterioration of buildings, bridges, and other structures as a result of rusting of iron (Fe)
costs millions of dollars every day.
Although the actual process also requires water, a
simplified equation (with rust shown as Fe
2
O
3
) is:
4Fe(
s
) + 3O
2
(
g
)
→
2Fe
2
O
3
(
s
)
ΔH
rxn
= 1.65 x 10
‒
3
kJ
What is ΔH
rxn
(in kJ) when
0.250 kg
of iron (Fe) rusts?
7.
Using the following data,
N
2
(
g
) + 3O
2
(
g
) + H
2
(
g
)
→
2HNO
3
(
aq
)
ΔH = 414.8 kJ
‒
N
2
O
5
(
g
) + H
2
O(
g
)
→
2HNO
3
(
aq
)
ΔH = 218.4 kJ
2H
2
O(
g
)
→
2H
2
(
g
) + O
2
(
g
)
ΔH = 483.6 kJ
calculate ΔH (in kJ) for the following reaction,
2N
2
(
g
) + 5O
2
(
g
)
→
2N
2
O
5
(
g
)
Page
3
of
12
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8.
For which one of the following reactions is
∆ H
rxn
°
equal to the standard enthalpy (heat) of
formation,
∆ H
f
°
,
for gaseous ammonia, NH
3
(
g
)?
(a) 3H
2
(
g
) + N
2
(
g
)
→
2NH
3
(
g
)
(b)
3
2
H
2
(
g
) +
1
2
N
2
(
g
)
→
NH
3
(
g
)
(c) 2NH
3
(
g
)
→
3H
2
(
g
) + N
2
(
g
)
(d) NH
3
(
g
)
→
3
2
H
2
(
g
) +
1
2
N
2
(
g
)
9.
Pentaborane B
5
H
9
(
s
) burns vigorously in oxygen to give B
2
O
3
(
s
) and liquid H
2
O.
2B
5
H
9
(
s
) + 12O
2
(
g
)
→
5B
2
O
3
(
s
) + 9H
2
O(
l
)
substance
ΔH°
f
(kJ/mol)
B
5
H
9
(
s
)
73.2
B
2
O
3
(
s
)
1273.5
‒
H
2
O(
l
)
285.8
‒
Calculate
Δ
H°
rxn
(in kJ/mol) for the reaction.
10. Calculate the wavelength (in nm) of light that has a frequency of 4.62 x 10
14
s
−1
.
11. Which one of the following arrangements of electromagnetic radiation begins with the lowest
energy (left) and increases to the highest energy (right)?
(a)
radio; visible; infrared; ultraviolet
(b) infrared; visible; ultraviolet; microwave
Page
4
of
12
(c)
visible; ultraviolet; infrared; gamma rays
(d) X-rays; visible; infrared; microwave
(e)
microwave; infrared; visible; ultraviolet
12. The number of distinct emission spectral lines that originate from electron transitions
between the first four energy levels in a hydrogen atom is ______.
Enter a whole number
(integer).
13. A hydrogen atom in the
n
= 6 energy level emits a photon of wavelength 410.2 nm.
What is
the final energy level,
n
, of the atom after it emits the photon?
Report n as a whole
number/integer.
14. The total number(s) of s atomic orbitals, and p atomic orbitals, respectively, for principle
quantum number
n
= 2 are __________ and __________.
Enter whole numbers/integers.
15. The radio station WAZY 96.5 of Lafayette broadcasts pop music at 96.5 MHz.
The
wavelength (in
m
) of WAZY broadcasting is
16. What is the energy of light (in kJ/mol) with wavelength of 558 nm?
Page
5
of
12
17. Light emitted from an excited state hydrogen atom with an electron transitioning from level 5
→
4 will have ______ (more/less) energy and ______ (longer/shorter) wavelength than light
emitted from emission between levels 6
→
5.
18. What frequency of light (in Hz) will bring the electron in ground state hydrogen to level 3 (n
= 3)?
19. What are the proper
n, l
values and the number of orbitals for sublevel 2
p
?
20. Which one of the following orbitals is represented by the radial probability distribution plot
pictured below?
(a) 2s
(b) 2p
(c) 3s
(d) 3d
(e) 3p
Page
6
of
12
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21. There are ______ valence and ______ core (inner) electrons in a neutral silicon (Si) atom.
22. Write the condensed shorthand, ground-state electron configuration for a neutral titanium (Ti)
atom.
23. Which one of the following elements has the
largest
first ionization energy (IE
1
)?
(a) B
(b) N
(c) P
(d) Si
(e) C
24. The successive ionization energies for a certain element are:
IE
1
=
578 kJ/mol
IE
4
=
11,600 kJ/mol
IE
2
=
1820 kJ/mol
IE
5
=
13,400 kJ/mol
IE
3
=
2750 kJ/mol
The element is
(a) Ne.
(b) Na.
(c) Mg.
(d) Al.
(e) Si.
25. Which one of the following equations represents the
second
ionization energy (IE
2
) for
aluminum (Al)?
(a) Al
+
(
g
) + e
‒
→
Al(
g
)
(b) Al(
g
)
→
Al
+
(
g
) +e
‒
(c) Al
+
(
g
)
→
Al
2+
(
g
) + e
‒
(d) Al
2+
(
g
)
→
Al
3+
(
g
) + e
‒
(e) Al(
g
)
→
Al
2+
(
g
) + 2e
‒
Page
7
of
12
26. Which one of the following elements is
most
metallic?
(a) P
(b) As
(c) Sb
(d) Te
(e) I
27. Write the full electron configuration of Zn
2+
.
28. Which one of the following is an
isoelectronic
series?
(a) B
5
‒
, Sr
4
‒
, As
3
‒
, Te
2
‒
(b) F
‒
, Cl
‒
, Br
‒
, I
‒
(c)
S, Cl, Ar, K
(d) Si
2
‒
, P
2
‒
, S
2
‒
, Cl
2
‒
(e) O
2
‒
, F
‒
, Ne, Na
+
29. Electron affinity (EA) values for phosphorus (P), sulfur (S) and chlorine (Cl) are listed
below.
Which one of the following statements best explains the
trend
in EA values?
element
EA (kJ/mol)
P
72.0
‒
S
200
‒
Cl
349
‒
(a)
The effective nuclear charge (Z
eff
) increases across a period.
(b) The effective nuclear charge (Z
eff
) decreases across a period.
(c)
The principle quantum number (n) of the outer electron(s) increases across a period.
(d) The principle quantum number (n) of the outer electron(s) decreases across a period.
30. Which one of the following sublevels is filled last?
(a) 3
d
(b) 4
s
(c) 4
p
(d) 4
d
(e) 5
s
Page
8
of
12
31. Put the following elements is order of
decreasing
atomic size (largest to smallest radius): B
(boron), Cs (cesium), F (fluorine), Li (lithium) and Na (sodium)?
32. Which one of the following elements has the
largest
first ionization energy?
(a) Na
(b) Cl
(c) Ca
(d) Te
(e) Br
33. The first four ionization energies of a certain element are listed below.
This element is most
likely in which column (group) of the periodic table?
34. The first, second and third ionization energies of boron are 0.80 MJ/mol, 2.43 MJ/mol and
3.66 MJ/mol, respectively.
How much energy (in MJ) would it take to remove the valence
electrons from 1.5 moles of boron?
35. For which one of the following properties does Mg have a larger value than Ba?
(a)
atomic radius
(b) ionic radius
(c)
first ionization energy
(d) number of protons
(e)
atomic weight
Page
9
of
12
Ionization Energy
kJ/mol
IE
1
899.5
IE
2
1757
IE
3
14,850
IE
4
21,000
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36. Which one of the following has the
largest
radius?
(a) F
(b) F
‒
(c) F
+
(d) Ne
37. Which of the following has the ground state electron configuration 1s
2
2s
2
2p
6
?
(a)
Mg
2+
(b)
Ne
(c)
Na
+
(d)
O
2
‒
(e)
all of the above
38. A chemist made a Beer’s law plot with standards of aqueous cobalt chloride at a particular
wavelength, as shown here:
If she tests a sample of CoCl
2
(
aq
) and measures an absorbance of 0.810 at the same
wavelength, what is the concentration (in M) of the sample?
Page
10
of
12
39. A spinach solution was prepared to determine the concentration of iron in the spinach.
A
10.00-mL sample of the
original
spinach solution was diluted to a total volume of 30.00 mL
with deionized water.
The absorbance of the
diluted
spinach solution was 0.285.
Use the
calibration plot below to determine the concentration (in M) of iron in the
original
spinach
solution.
0.00E+00
1.00E-05
2.00E-05
3.00E-05
4.00E-05
5.00E-05
0
0.05
0.1
0.15
0.2
0.25
0.3
0.35
0.4
f(x) = 8868.22 x + 0.02
Concentration (M)
Absorbance
Page
11
of
12
Key
1.
67
C
2.
e
3.
–61.3 kJ/mol
4.
–44.0 kJ/mol
5.
c
6.
1.85 x 10
‒
3
kJ
7.
782.8 kJ
‒
8.
b
9.
9086 kJ
‒
10. 6.49 x 10
2
nm
11. e
12. 6
13.
n
= 2
14. 1
s
orbital, 3
p
orbitals
15.
3.11 m
16.
2.14 x 10
2
kJ/mol
17.
more, shorter
18.
2.92 x 10
15
Hz
19.
2, 1, 3
20. c
21.
4, 10
22.
[Ar] 4s
2
3d
2
23. b
24. d
25. c
26. c
27. 1s
2
2s
2
2p
6
3s
2
3p
6
3d
10
28. e
29. a
30. d
31.
Cs > Na > Li > B > F
32. b
33.
Group 2
34.
10.3 MJ
35. c
36. b
37. e
38.
0.0047 M
39.
8.87 x 10
5
‒
M
Page
12
of
12
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Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY
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