# CUNY College of Staten Island Equilibrium Chemistry Thermodynamics Solved Quiz

10:43 “‘t7
.111
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D
Question 1
Exit
4 pts
Above what temperature does the
following reaction become
nonspontaneous?
2 H2S(g) + 3 02(g) ➔ 2 S02(g) + 2
H20(g)
L.\H = -1036 kJ; L.\S =
-153.2 J/K
0
298K
0
6.762
0
158.7 K
O
This reaction is nonspontaneous at all
temperatures.
O
This reaction is spontaneous at all
X
103 K
temperatures.
D
Question 2
Ct.J•
4 pts
10:43 “‘t7
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Question 2
4 pts
Place the following in order of increasing
molar entropy at 298 K.
D
Question 3
Calculate ~S 0 rxn for the following
reaction. The 5° for each species is
shown below the reaction.
4 pts
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Question 3
4 pts
Calculate ~5°rxn for the following
reaction. The 5° for each species is
shown below the reaction.
C2H6(g)
S0 {J/mol·K)
200.9
130.7
229.2
0
-233.1 J/K
0
+560.8 J/K
0
+303.3 J/K
0
229.2 J/K
0
-102.4 J/K
D
Question4
4 pts
10:44 ~
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Question4
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4 pts
Estimate ~G 0 rxn for the following
reaction at 775 K.
2 Hg(g) + 02(g) ➔ 2 HgO(s)
~H 0 = -304.2 kJ; ~5°= -414.2 J/K
Q +17 kJ
0
+321 kJ
0
-110 kJ
0
-181 kJ
0
-625 kJ
D
Question 5
4 pts
Determine the equilibrium constant for
the following reaction at 655 K.
10:44 ~
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Question 5
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4 pts
Determine the equilibrium constant for
the following reaction at 655 K.
I
HCN(g) + 2 H2(g) ➔
CH3NH2(g)
~H 0 = -158 kJ; fi5°=
-219.9 J/K
0
3.07
X
1011
0
3.26
X
10- 12
0
3.99
X
1012
0
2.51
X
10- 13
013.0
D
Question 6
4 pts
Use Hess’s law to calculate ~G 0 rxn using
the following information.
10:44 ~
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Question 6
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4 pts
Use Hess’s law to calculate ~G 0 rxn using
the following information.
CIO(g) + 03(g) ➔ Cl(g) + 2
~G 0 rxn = ?
02(g)
~G 0 rxn =
02(g)
+489.6 kJ
Cl(g) + 03(g) ➔ CIO(g) +
~G 0 rxn = -34.5 kJ
02(g)
0
-210.3 kJ
0
+262.1 kJ
0
+524.1 kJ
0
+455.1 kJ
Q -472.4 kJ
.~..——
10:44~
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C>Question 7
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4 pts
Place the following in order of increasing
standard molar entropy.
I
D
Question 8
4 pts
Consider a reaction that has a positive
~H and a negative ~S. Which of the
following statements is TRUE?
10:44~
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C>Question 8
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4 pts
Consider a reaction that has a positive
8H and a negative 85. Which of the
following statements is TRUE?
O
This reaction will be nonspontaneous only
at high temperatures.
O
This reaction will be spontaneous at all
temperatures.
O
This reaction will be spontaneous only at
high temperatures.
O
It is not possible to determine without
more information.
O
This reaction will be nonspontaneous at all
temperatures.
D
Question 9
4 pts
Consider a reaction that has a positive
8H and a positive 85. Which of the
following
statements is TRUE?
10:44 ~
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Question 9
Exit
4 pts
Consider a reaction that has a positive
~Hand a positive ~S. Which of the
following statements is TRUE?
O
This reaction will be nonspontaneous only
at high temperatures.
O
It is not possible to determine without
more information.
O
This reaction will be nonspontaneous at all
temperatures.
O
This reaction will be spontaneous at all
temperatures.
O
This reaction will be spontaneous only at
high temperatures.
D
Question 10
4 pts
Which ion would you expect to have the
largest crystal field splitting?
10:44 ~
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Question 10
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4 pts
Which ion would you expect to have the
largest crystal field splitting?
0 [ Rh(CN)6] 4 –
0 [ Rh(CN)6] 3 –
D
Question 11
4 pts
What is the electron configuration for
Cr3 +?
—– —–
0
[Ar] 3d
0
[Ar] 45 1 3d 2
0
[Ar] 452 3d 7
0
[Ar] 45 2 3d 1
3
10:44 ~
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What is the electron configuration for
Cr3+?
0
[Ar] 3d 3
0
[Ar] 45 1 3d 2
0
[Ar] 45 2 3d 7
0
[Ar] 45 2 3d 1
D
Question 12
4 pts
How many unpaired electrons would you
expect for the complex ion:
[Mn(NH3)6] 2 +?
02
oo
03
os
01
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Question 13
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4 pts
The complex ion, [Ni(NH 3) 6] 2+, has a
maximum absorption near 580 nm.
Calculate the crystal field splitting energy
(in kJ/mol) for this ion.
0
206 kJ/mol
0
292 kJ/mol
0
114 kJ/mol
0
485 kJ/mol
0
343 kJ/mol
D
Question 14
Name the following: Fe[AIF6]
0
ironaluminumhexafluoride
0
iron(II) hexafluoroaluminum
O
aluminumhexafluoroferrate
4 pts
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Question 14
Exit
4 pts
Name the following: Fe[AIF6]
0
ironaluminumhexafluoride
0
iron(II) hexafluoroaluminum
O
aluminumhexafluoroferrate
0
iron (111) hexafluoroaluminate
O
iron(I) aluminumhexafluoride
D
Question 15
4 pts
Determine the chemical formula for the
compound, tetracarbonylplatinum{IV)
chloride.
() PtCl,1l(Cd ),1
I
10:44 ~
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Question 15
Exit
4 pts
Determine the chemical formula for the
compound, tetracarbonylplatinum(IV)
chloride.
D
Question 16
4 pts
Which of the following pairs of
coordination compounds or complex ions
are examples of coordination isomers?
Q
[Fe(CO)sN02] 2+ and [Fe(CO)sON0] 2 +
I
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Question 16
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4 pts
Which of the following pairs of
coordination compounds or complex ions
are examples of coordination isomers?
Q
[Fe(C0)5N02] 2+ and [Fe(CO)sON0] 2+
Q
[Cu(CO)sBr]CI and [Cu(CO)sCl]Br
Q
[Fe(NH3)i(H20)4]Cl2 and
[Fe( N H3)i(H20)4] Br2
Q
[Fe(NH3)i(H20)4]Cl2 and
[Fe(NH3)4(H20)i]Cl2
Q
D
[MnCl3Br] 2- and [MnCIBr3] 2-
Question 17
4 pts
Which of the following pairs of
coordination compounds or complex ions
are examples of linkage isomers?
10:45 ~
.111
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Question 17
4 pts
Which of the following pairs of
coordination compounds or complex ions
are examples of linkage isomers?
Q
[Fe(NH3}i(H20)4]Cl2 and
[Fe(NH3)4(H20)2]Cl2
Q
[Fe(CO)sN02] 2+ and [Fe(CO)s0N0] 2+
Q
[Fe(NH3)i(H20)4]Cl2 and
[Fe( N H3)i(H20)4] Br2
Q
D
c+.J·
[Cu(NH3)5Br]CI and [Cu(NH3)5Cl]Br
Question 18
4 pts
You wish to prepare an HC2H 30 2 buffer
with a pH of 5.44. If the pKa of the acid
is 4.74, what ratio of C2H 3 2/HC2H302 must you use?
o
10:45 ~
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Question 18
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4 pts
You wish to prepare an HC2H 3 0 2 buffer
with a pH of 5.44. If the pKa of the acid
is 4.74, what ratio of C2H30 2/HC2H302 must you use?
01.1
0
5.0
0
0.20
0
1.4
0
0.70
D
Question 19
4 pts
Calculate the pH of a buffer that is 0.058
M HF and 0.058 M LiF. The Ka for HF is
3.5
X
10-4 .
0
3.46
n
10 4
10:45 ~
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Question 19
Exit
4 pts
Calculate the pH of a buffer that is 0.058
M HF and 0.058 M LiF. The Ka for HF is
3.5
X
10-4 .
0
3.46
0
10.54
0
4.69
0
9.31
0
2.86
D
Question 20
4 pts
Which pair of substances could form a
buffered aqueous solution?
Q
HCI, NaCl
Q
NH3, Na,..
0111H——-
10:45 ~
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Question 20
Exit
4 pts
Which pair of substances could form a
buffered aqueous solution?
0
HCI, NaCl
0
NH3, NaOH
0
HN03, NaN03
D
Question 21
4 pts
A 1.00 L buffer solution is 0.150 M in
HC1Hs02 and 0.250 M in LiC1Hs02.
Calculate the pH of the solution after the
addition of 100.0 ml of 1.00 M HCI. The
Ka for HC7H 50 2 is 6.5 x 10-5 .
0 5.03
0
4.41
10:45 ~
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Question 21
4 pts
A 1.00 L buffer solution is 0.150 M in
HC7Hs02 and 0.250 M in LiC7Hs02.
Calculate the pH of the solution after the
addition of 100.0 ml of 1.00 M HCI. The
Ka for HC7H 50 2 is 6.5 x 10-5.
0
5.03
0
4.41
0
3.34
0
4.19
0
3.97
D
Question 22
4 pts
When titrating a weak monoprotic acid
with NaOH, the
O
titration will require more moles of base
than acid to reach the equivalence point.
~
I

__
I ___
11_
__
~
_
11 _ _

_ I _
10:45 ~
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D
Question 22
Exit
4 pts
When titrating a weak monoprotic acid
with NaOH, the
O
titration will require more moles of base
than acid to reach the equivalence point.
O
pH will be less than 7 at the equivalence
point.
O
pH will be equal to 7 at the equivalence
point.
O
titration will require more moles of acid
than base to reach the equivalence point.
0

pH will be greater than 7 at the
equivalence point.
Question 23
4 pts
Give the expression for the solubility
product constant for PbCl 2 •
I
10:45 ~
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Question 23
Exit
4 pts
Give the expression for the solubility
product constant for PbCl 2 •
0
[Pb2+][ci-]2
0
[Pb 2+][Ci-] 2 / [PbCl2]
D
Question 24
4 pts
The molar solubility of Cul is 2.26 x 10-6
Min pure water. Calculate the Ksp for
Cul.
Q 4.52 X 10- 6
Q 1.02 X 10-H
() 5.11 X 1u ~-
Ct.J·
10:45 ~
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Question 24
Exit
4 pts
The molar solubility of Cul is 2.26 x 10-6
M in pure water. Calculate the Ksp for
Cul.
Q 4.52 X 10-6
Q 1.02 X 10-11
Q 5.11 X 10-12
Q 1.50 X 10-3
Q 4.62 X 10-17
D
Question 25
4 pts
A ligand is a molecule or ion that acts as a
0
Bronsted-Lowry base
0
none of the above
O
Bronsted-Lowry acid
BronstE:d-EOCO, 9 SJ§@
10:45 ~
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Exit
M in pure water. Calculate the Ksp for
Cul.
Q 4.52 X 10- 6
Q 1.02 X 10-11
Q 5.11 X 10-12
Q 1.50 X 10- 3
Q 4.62 X 10-17
D
Question 25
4 pts
A ligand is a molecule or ion that acts as a
O
Bronsted-Lowry base
0
none of the above
0
Bronsted-Lowry acid
0
Bronsted-Lowry base
0
Lewis acid
I

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