Chemistry 106: General Chemistry
Syracuse University Project Advance
Final Exam, Fall 2011
Name
ID No.
The last page of each examination should be a periodic table.
Rydberg Constant (RH) = 2.18 x 10-18 J
(1) A combination of sand, salt, and water is an example of a
(a)
(b)
(c)
(d)
(e)
.
pure substance
heterogeneous mixture
solid
compound
homogeneous mixture
(2) Gold has a density of 0.01932 kg/cm3. What volume (in cm3) would be occupied by a
33.3 g sample of pure gold?
(a)
(b)
(c)
(d)
(e)
5.80 x 10-4
0.663
0.581
5.80
1.72
CHE 106, Fall 2011, Final Exam
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(3) In which of the following numbers are none of the zeros significant?
(a)
(b)
(c)
(d)
(e)
100.0
0.00001
0.0100
1065
1.003450
(4) All atoms of a given element have the same
(a)
(b)
(c)
(d)
(e)
number of electrons and neutrons.
density.
mass.
number of protons.
number of neutrons.
(5) There are
of 13254 Xe ?
(a)
(b)
(c)
(d)
(e)
electrons,
protons, and
neutrons in an atom
78, 78, 54
54, 54, 78
54, 54, 132
78, 78, 132
132, 132, 54
(6) The formula weight of (K3PO4) is
(a)
(b)
(c)
(d)
(e)
.
amu.
196.27
212.27
173.17
86.07
251.37
(7) When the following equation is balanced, the coefficients are
NH3 (g) + O2 (g) ------> NO2 (g) + H2O (g)
(a)
(b)
(c)
(d)
(e)
4, 7, 4, 6
2, 3, 2, 3
1, 1, 1, 1
4, 3, 4, 3
1, 3, 1, 2
CHE 106, Fall 2011, Final Exam
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.
(8) How many oxygen atoms are there in 52.06 g of carbon dioxide?
(a)
(b)
(c)
(d)
(e)
5.088 x 1023
1.424 x 1024
1.204 x 1024
1.018 x 1024
6.022 x 1023
(9) Element X has three naturally occurring isotopes. The masses (amu) and %
abundances of the isotopes are given in the table below. The average atomic mass
of the element is
amu.
Isotope
38
X
39
X
42
X
(a)
(b)
(c)
(d)
(e)
Abundance
5.07
15.35
79.85
Mass
37.919
39.017
42.111
33.33
41.54
39.68
39.07
38.64
(10) Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride:
S (s) + 3 F2 (g) ------> SF6 (g)
The maximum amount of SF6 that can be produced from the reaction of 3.5 g of
sulfur with 4.5 g of fluorine is
g.
(a)
(b)
(c)
(d)
(e)
3.2
5.8
12
16
8.0
(11) Which of the following is an oxidation-reduction reaction?
A. HCl (aq) + NaOH (aq) ------> H2O (l) + NaCl (aq)
B. AgNO3 (aq) + HCl (aq) ------> AgCl (s) + HNO3 (aq)
C. Cu (s) + 2 AgNO3 (aq) ------> 2 Ag (s) + Cu(NO3)2 (aq)
D. Ba(C2H3O2)2 (aq) + Na2SO4 (aq) ---- BaSO4 (s) + 2 NaC2H3O2 (aq)
E. H2CO3 (aq) + Ca(NO3)2 (aq) ------> 2 HNO3 (aq) + CaCO3 (s)
CHE 106, Fall 2011, Final Exam
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(12) The net ionic equation for the reaction between aqueous sulfuric acid and aqueous
sodium hydroxide is
.
A. H+(aq) + HSO4-(aq) + 2OH-(aq) ------> 2 H2O(l) + SO42-(aq)
B. H+(aq) + HSO4-(aq) + 2Na+(aq) + 2OH-(aq) ------> 2H2O(l) +2Na+(aq) + SO42-(aq)
C. SO42-(aq) + 2Na+(aq) ------> 2Na+(aq) + SO42-(aq)
D. 2H+(aq) + SO42-(aq) + 2Na+(aq) + 2OH-(aq) ------> 2H2O(l) + 2Na+(aq) + SO42-(aq)
E. H+(aq) + OH1-(aq) ------> H2O(l)
(13) What volume (mL) of 0.135 M NaOH is required to neutralize 13.7 mL of 0.129 M
HCl?
(a)
(b)
(c)
(d)
(e)
13.1
0.24
6.55
14.3
0.076
(14) Which one of the following statements is true?
(a)
(b)
(c)
(d)
H is the value of q measured under conditions of constant volume.
Enthalpy is an intensive property.
Enthalpy is a state function.
The enthalpy change for a reaction is independent of the state of the reactants and
products.
(e) The enthalpy change of a reaction is the reciprocal of the H of the reverse
reaction.
(15) The E of a system that releases 12.4 J of heat and does 4.2 J of work on the
surrounding is
J?
(a)
(b)
(c)
(d)
(e)
-16.5
-8.2
4.2
12.4
16.6
(16) A sample of iron absorbs 67.5 J of heat, upon which the temperature of the sample
increases from 21.5°C to 28.5°C. If the specific heat of iron is 0.450 J/g-C, what is
the mass (in grams) of the sample?
(a)
(b)
(c)
(d)
(e)
11
1100
4.3
1.1 x 103
21
CHE 106, Fall 2011, Final Exam
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(17) Consider the following two reactions:
A ----> 2B
A ----> C
H°rxn
H°rxn
= 456.7 kJ/mol
= -22.1 kJ/mol
Determine the enthalpy change for the process:
2B ----> C
(a)
(b)
(c)
(d)
(e)
434.6 kJ/mol
478.8 kJ/mol
-478.8 kJ/mol
More information is needed to solve the problem.
-434.6 kJ/mol
(18) Given the data in the table below, H°rxn for the reaction is
J?
Ca(OH)2 + 2H3AsO4 ------> Ca(H2AsO4)2 + 2 H2O
Substance
Ca(OH)2
H3AsO4
Ca(H2AsO4)2
H2O
(a)
(b)
(c)
(d)
(e)
Hf°
(kJ/mol)
-986.6
-900.4
-2346.0
285.9
-4219
-4519
-76.4
-744.9
-130.4
(19) Given the data in the table below, H°rxn for the reaction is
C2H5OH(l) + O2(g) ------> CH3CO2H(l) + H2O(l)
Substance
C2H4(g)
C2H5OH (l)
CH3CO2H (l)
H2O (l)
(a)
(b)
(c)
(d)
(e)
Hf°
(kJ/mol)
52.3
-277.7
-484.5
-285.8
-1048.0
-476.4
-79.0
-492.6
the value of H°f for O2 is required for the calculation.
CHE 106, Fall 2011, Final Exam
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kJ.
(20) The value of H° for the reaction below is -186 kJ.
H2(g) + Cl2(g) ------> 2 HCl(g)
The value of Hf° for HCl is
(a)
(b)
(c)
(d)
(e)
kJ/mol.
-3.72 x 102
-186
+186
-1.27 x 102
-93.0
(21) The energy (J) required for an electronic transition in a Bohr hydrogen atom from n
= 2 to n = 3 is
J?
(a)
(b)
(c)
(d)
(e)
3.00 x 10-19
-7.90 x 10-19
4.60 x 1014
4.00 x 10-19
-3.00 x 10-19
(22) An electron cannot have the quantum numbers n =
(a)
(b)
(c)
(d)
(e)
,l=
, ml =
.
3, 1, -1
2, 1, -1
3, 2, 1
1, 1, 1
2, 0, 0
(23) Which one of the following is the correct electron configuration for a ground state
nitrogen atom?
CHE 106, Fall 2011, Final Exam
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(24) Which of the following correctly represents the second ionization of aluminum?
A.
B.
C.
D.
E.
Al+ (g) ------> Al2+ (g) + eAl+ (g) + e- ------> Al (g)
Al (g) ------> Al+ (g) + eAl+ (g) + e- ------> Al2+ (g)
Al- (g) + e- ------> Al2- (g)
(25) Which of the following elements has the most negative electron affinity?
(a)
(b)
(c)
(d)
(e)
S
Se
Cl
Br
I
(26) Which of the following is soluble in water at 25° C?
(a)
(b)
(c)
(d)
(e)
FeS
Fe(NO3)2
FeCO3
Fe3(PO4)2
Fe(OH)2
(27) The atomic radius of main-group elements generally increases down a group because
?
(a)
(b)
(c)
(d)
(e)
the effective nuclear charge increases down a group.
the effective nuclear charge decreases down a group.
the effective nuclear charge zigzags down the group.
the principal number of the valence orbitals increases.
both effective nuclear charge increases down a group and the principal quantum
number of the valence orbitals increases.
(28) Choose the statement that is TRUE:
(a)
(b)
(c)
(d)
(e)
Outer electrons efficiently shield one another from nuclear charge.
Core electrons are the easiest of all electrons to remove.
Valence electrons are the most difficult of all electrons to remove.
Core electrons efficiently shield outer electrons.
All of the above are true.
CHE 106, Fall 2011, Final Exam
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(29) The Lewis structure of N2H2 shows
(a)
(b)
(c)
(d)
(e)
.
A nitrogen-nitrogen triple bond.
Each hydrogen has one nonbonding electron pair.
A nitrogen-nitrogen single bond.
Each nitrogen has two nonbonding electron pairs.
Each nitrogen has one nonbonding electron pair.
(30) According to Molecular Orbital Theory, overlap of two s atomic orbitals produces?
(a)
(b)
(c)
(d)
(e)
(31)
One bonding molecular orbital and one hybrid orbital.
Two bonding molecular orbital and one antibonding molecular orbital.
Two bonding molecular orbitals.
Two bonding molecular orbital and two antibonding molecular orbitals.
One bonding molecular orbital and one antibonding molecular orbital.
Which of the following species has a bond order of 2.0?
(a)
(b)
(c)
(d)
(e)
(32) There are
O2
O2O22O2+
NO bonds and
 bonds in:
CH3-CH2-CH=CH-CH2-CH=CH2
(a)
(b)
(c)
(d)
(e)
13, 2
12, 2
18, 2
14, 2
10, 3
(33) The molecular geometry of the BeCl2 molecule is
(a)
(b)
(c)
(d)
(e)
Trigonal planar, polar.
Bent, polar
Linear polar.
Bent, nonpolar.
Linear, nonpolar
CHE 106, Fall 2011, Final Exam
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and the molecule is
.
(34) The molecular geometry of the SF2 molecule is
(a)
(b)
(c)
(d)
(e)
.
trigonal planar
linear
bent
tetrahedral
octahedral
(35) According to valence bond theory, which orbitals on bromine atoms overlap in the
formation of the bond in Br2?
(a)
(b)
(c)
(d)
(e)
3s
3p
4s
4p
3d
(36) Which of the following diatomic species would you expect to have the longest bond
length?
(a)
(b)
(c)
(d)
(e)
F2
NOO2
O2+2
C22-
(37) Of the following, only
(a)
(b)
(c)
(d)
(e)
(38)
has sp2 hybridization of the central atom.
ICl3
PF5
CO32I3PH3
Calculate the total pressure in atmospheres (atm) of a mixture of 0.03000 mol of
helium (He) and 0.0200 mol of oxygen (O2) in a 4.00 liter flask at 20° C. Assume
ideal gas behavior.
(a)
(b)
(c)
(d)
(e)
0.900 atm
0.120 atm
0.180 atm
0.602 atm
0.301 atm
CHE 106, Fall 2011, Final Exam
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(39) 2.50 g of XeF4 gas is placed into an evacuated 3.00 liter container at 80°C. What is
the pressure in the container?
(a)
(b)
(c)
(d)
(e)
(40)
3.01 torr
0.117 torr
0.288 atm
0.117 atm
none of the above
What mass of nitrogen dioxide would be contained in a 4.32 L vessel at 48° C and
1062 torr?
(a)
(b)
(c)
(d)
(e)
(41)
5.35 x 104 g
53.5 g
10.5 g
105.0 g
none of the above
A mixture of 0.924 g of N2O and 0.825 g of NO exerts a pressure on a container
of 1.32 atm. The partial pressure of each gas is
.
(a)
(b)
(c)
(d)
(e)
N2O = 1.32 atm and NO = 1.32 atm
N2O = 0.70 atm and NO = 0.62 atm
N2O = 0.57 atm and NO = 0.75 atm
N2O = 0.66 atm and NO = 0.66 atm
N2O = 0.78 atm and NO = 0.54 atm
(42) A sample of a pure gas occupied a volume of 500 mL at a temperature of 27°C and
a pressure of 0.4 atm. The number of moles present in this sample is
.
(a)
(b)
(c)
(d)
(e)
(43)
(a)
(b)
(c)
(d)
(e)
0.45
0.008
0.91
8.13
0.182
Suppose 3.15 L of neon at 21°C and P = 0.951 atm is compressed to 1.292 atm,
with the temperature held constant. The new volume is
.
2.32 L
3.00 L
3.15 L
4.10 L
4.44 L
CHE 106, Fall 2011, Final Exam
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(44)
Using the phase diagram shown below, in which phase does this substance exist at
tempertures above 25°C and at pressures less than 0.1 atm?
(a)
(b)
(c)
(d)
(e)
w
x
y
z
not enough information provided
CHE 106, Fall 2011, Final Exam
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KEY
CHE 106, Fall 2011 Final Exam
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27
28
29
30
31
32
33
34
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38
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40
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B
E
B
D
B
B
A
B
B
B
C
E
A
C
A
E
C
E
D
E
A
D
A
A
C
B
D
A
E
E
A
C
E
C
D
A
C
E
D
C
C
B
A
C
CHE 106, Fall 2011, Final Exam
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