Chemistry 106: General Chemistry
Syracuse University Project Advance
Final Exam, Fall 2004
Name
Date
The last page of each examination is a periodic table.
c = 3.00 x 108 m/sec
h = 6.63 x 10-34 Js
mp = 1.67 x 10-24 g (mass of proton)
Rydberg Constant (RH) = 2.18 x 10-18 J
(1)
What is the volume of a 12.2 g piece of metal with a density of 9.43 g/cm3?
(a)
(b)
(c)
(d)
(e)
(2)
Which of the following values contains 2 significant figures?
(a)
(b)
(c)
(d)
(e)
(3)
12.2 cm3
1.29 cm3
0.773 cm3
115 cm3
none of these
0.0004 kg
0.0040 L
0.0400 mm
0.4000 m
all of these
All atoms of a given element have the same
(a)
(b)
(c)
(d)
(e)
(4)
mass
number of neutrons
number of protons
same ratio of protons and neutrons
there is nothing constant about a given element
When a metal and a non metal react, the
the
tends to gain electrons
(a)
(b)
(c)
(d)
(e)
CHE 106
tends to lose electrons, and
metalloid, metal
nonmetal, nonmetal
metal, nonmetal
nonmetal, metal
none of these, these elements share electrons
1
Fall 2004 Final Exam
(5)
What is the chemical formula for iron(III) sulfide?
(a)
(b)
(c)
(d)
(e)
(6)
What is the percentage of Ca (by weight) in Ca3(PO4)2?
(a)
(b)
(c)
(d)
(e)
(7)
9.9%
20.0%
18.7%
38.8%
55.9%
What is the empirical formula of caffeine if it contains 5.19% H, 28.85% N,
16.48% O, and 49.48% C by weight?
(a)
(b)
(c)
(d)
(e)
(8)
Fe2(SO3)3
Fe2S3
Fe3(SO3)2
Fe2(SO4)3
Fe3(SO4)2
C10HN5O3
C4H5NO2
C3H5NO
C2H6NO2
C4H5N2O
What is the mass of copper produced if 10.0 g of Cu2S reacts with 16.0 g of O2 as
follows: (Atomic masses are Cu = 63.5; O = 16.0; S = 32.1)
Cu2S + O2  2 Cu + SO2
(a)
(b)
(c)
(d)
(e)
(9)
31.8 g
63.5 g
3.99 g
7.98 g
6.25 g
One gram of TNT, C7H5N3O6, has 7.95 x 1021 nitrogen atoms. How many
hydrogen atoms are there in 1.00 g of TNT?
(a)
(b)
(c)
(d)
(e)
CHE 106
7.95 x 1021
9.26 x 1021
1.33 x 1022
1.59 x 1022
1.86 x 1022
2
Fall 2004 Final Exam
(10)
How many grams of carbon dioxide (CO2, molar mass = 44.0 g/mol) are produced
in the combustion of 1.8 g glucose (C6H12O6, molar mass = 180.0 g/mol) according
to the following reaction:
C6H12O6(g) + 6 O2(g)  6 CO2(g) + 6 H2O (g)
(a)
(b)
(c)
(d)
(e)
(11)
140. amu
140.6 amu
141. amu
141.6 amu
142. amu

Balance the following equation: __Cl2O7 + __H2O  __HClO4 The ratio of the
coefficient of HClO4 to the coefficient of H2O is
(a)
(b)
(c)
(d)
(e)
(13)
1.08 g
0.440 g
4.40 g
0.264 g
2.64 g
A space explorer traveling to a distant planet in the universe found an element X
whose 2 isotopes had the approximate masses and percentage abundances 140.
amu (66.7%) and 143. amu (33.3%). What is the average relative atomic mass of
element X on that planet as compared with 126 C taken as 12 amu?
(a)
(b)
(c)
(d)
(e)
(12)
?
1/2
2/3
1/1
3/2
2/1
You want to prepare 250 mL of 0.10 M Na2SO4 (aq). The molar masses of H2O
and Na2SO4 are 18.02 g/mol and 142.04 g/mol respectively. The mass of Na2SO4
required is
(a)
(b)
(c)
(d)
(e)
CHE 106
0.451 g
3.55 g
3550 g
0.000176 g
0.176 g
3
Fall 2004 Final Exam
(14)
How many ml of 0.100 M H2SO4 are required to react with 0.840 g of NaHCO3
(molar mass = 84.01 g/mol) according to the following equation?
H2SO4(aq) + 2NaHCO3(aq)  Na2SO4(aq) + 2H2O(l) + 2CO2(g)
(a)
(b)
(c)
(d)
(e)
(15)
200 mL
150 mL
100 mL
50.0 mL
none of the above
Obtain the oxidation number for the element noted in each of the following:
I. N in NH2II. I in IO3III. Al in Al(OH)4Add together the results of I, II and III. The sum is
(a)
(b)
(c)
(d)
(e)
(16)
-3
-1
+1
+3
+5
Consider the oxidation-reduction reaction:
2FeI3(aq) + 3Mg(s)  2Fe(s) + 3MgI2(aq).
Which of the following statements is not true about this reaction?
(a)
(b)
(c)
(d)
(e)
(17)
Iron (Fe) acts as an oxidizing agent.
Magnesium (Mg) acts as a reducing agent.
The oxidation number of iron is lowered.
The oxidation number of Mg is lowered.
Iodide ion (I-) is a spectator ion.
How many moles of sulfate ions are there in a 0.20 L solution of 0.030 molar
Al2(SO4)3?
(a)
(b)
(c)
(d)
(e)
CHE 106
0.0030
0.0060
0.012
0.018
0.024
4
Fall 2004 Final Exam
(18)
Calculate the standard heat of formation of acetaldehyde, CH3CHO(g), given the
following information:
5
O2(g)  2H2O(l) + 2CO2(g)
H = -1194 kJ
2
Hf° H2O(l) = -286 kJ/mol Hint: Write out Hf equations for H2O and CO2
Hf° CO2(g) = -394 kJ/mol
CH3CHO(g) +
(a)
(b)
(c)
(d)
(e)
(19)
Hfus for sulfur is 17.7 kJ/mol. How many grams of sulfur can be melted by 29.0
kJ of energy?
(a)
(b)
(c)
(d)
(e)
(20)
 kJ
-452
-332 kJ
-166 kJ
166 kJ
332 kJ
9.8 g
19.5 g
26.2 g
40.7 g
52.5 g
Given the following data at 25°C and 1.00 atm pressure:
Pb(s) + PbO2(s) + 2H2SO4(l)  2PbSO4(s) + 2H2O(l)
SO3(g) + H2O(l)  H2SO4(l)
H°(kJ/mol)
-509.2
-130
Evaluate H° for the reaction below at 25°C.
Pb(s) + PbO2(s) + 2SO3(g)  2PbSO4(s)
(a)
(b)
(c)
(d)
(e)
CHE 106
-3.77 x 103 kJ
3.77 x 103 kJ
-639 kJ
-521 kJ
-769 kJ
5
Fall 2004 Final Exam
(21)
Calculate the standard enthalpy change of the reaction of the combustion of
propane:
C3H8(g) + 5O2(g)  3CO2(g) + 4H2O(l)
Use the following data: Hf° (kJ/mol)
C3H8(g)
CO2(g)
H2O(g)
(a)
(b)
(c)
(d)
(e)
(22)
+575.5 kJ
-575.5 kJ
-2428. kJ
+2200. kJ
-2200. kJ
The possible value(s) of the magnetic quantum number m1 for a 5d electron is(are)
(a)
(b)
(c)
(d)
(d)
(23)
[Ar] 3d64s2
[Ar] 3d34s2
[Ar] 3d44s1
[Ar] 3d5
[Ar] 3d6
In the Periodic Table, Mg is in Group IIA and Period 3, Ca is in Group IIA and
Period 4, and S is in Group VIA and Period 3. Arrange these elements in order of
increasing ionization energy.
(a)
(b)
(c)
(d)
(e)
(25)
0, 1, 2, 3
1, 2, 3, 4
2, 1, 0, -1, -2
3, 2, 1, 0, -1, -2, -3
4
What is the electron configuration of Fe+3?
(a)
(b)
(c)
(d)
(e)
(24)
-103.8
-393.5
-285.8
Mg Ca S
Mg S Ca
Ca Mg S
S Ca Mg
S Mg Ca
London-dispersion force is the attractive force between
(a)
(b)
(c)
(d)
(e)
CHE 106
an ion and a permanent dipole
an instantaneous dipole and an induced dipole
two permanent dipoles
two molecules with hydrogen bonds to an oxygen atom
two ions
6
Fall 2004 Final Exam
(26)
Write the Lewis Electron Dot Formula of [ClO]-. Which of the following
statements is/are incorrect?
I.
The total number of valence electrons is 14.
II. The skeleton structure is Cl-O.
III. The best Lewis formula is
(a) III
(b) II
(c) I
(d) I and II
(e) II and III
(27)
The octet rule is violated by at least one atom in each of the following species
except
(a)
(b)
(c)
(d)
(e)
(28)
ICl2-.
CH3-.
BF4-.
SF4.
ClF3.
A  (pi) bond is the result of the
(a)
(b)
(c)
(d)
(e)
(29)
Cl = O
overlap of an s orbital and a p orbital.
overlap of two p orbitals along their axes.
overlap of two s orbitals.
sidewise overlap of two s orbitals.
sidewise overlap of two parallel p orbitals.
The hybridization of the central atom in a molecule is described as sp. The
arrangement in space of the hybrid orbitals about that atom is
(a)
(b)
(c)
(d)
(e)
CHE 106
linear.
trigonal planar.
tetrahedral.
trigonal bipyramidal.
octahedral.
7
Fall 2004 Final Exam
(30)
During lecture a chemistry student inflates five identical balloons with the gases
below to a volume of 1 liter at 298 K and a pressure of 1 atm. The student
continues to observe the balloons for a long period of time, and notices that one
decrease in size. According to Graham’s law, which balloon would shrink over
time? (Air = 79% N2, 21% O2)
(a)
(b)
(c)
(d)
(e)
(31)
The volume of a sample of gas measured at 25.0°C and 1.00 atm pressure is 10.0
L. What must the final temperature be in order for the gas to have a final volume
of 7.5 L at 1.00 atm pressure?
(a)
(b)
(c)
(d)
(e)
(32)
The balloon filled with CO2.
The balloon filled with H2.
The balloon filled with NO2.
The balloon filled with Ar.
The balloon filled with SF6.
-55°C
-50°C
-45°C
-35°C
19°C
Magnesium metal reacts with hydrochloric acid to produce hydrogen gas, H2
according to the following reaction: Mg(s) + 2HCl(aq)  MgCl2(aq) + H2(g).
Calculate the volume (in liters) of hydrogen produced at 28°C and 665 mm Hg
from 0.0840 mol Mg and excess HCl.
(a)
(b)
(c)
(d)
(e)
CHE 106
1.82 L
2.37 L
0.220 L
0.169 L
None of the above
8
Fall 2004 Final Exam
(33)
Based on molecular mass and dipole moment of five compounds in the table
below, which should have the highest boiling point?
Compound
Molecular Mass (amu)
CH3CH2CH3
CH3OCH3
CH3Cl
CH3CHO
CH3CN
(a)
(b)
(c)
(d)
(e)
CHE 106
44
46
50
44
41
Dipole Moment (debye)
0.0
1.3
2.0
2.7
3.9
CH3CH2CH3
CH3OCH3
CH3Cl
CH3CHO
CH3CN
9
Fall 2004 Final Exam