Chemistry 106: General Chemistry
Syracuse University Project Advance
Final Exam, Fall 2002
Name
(1)
Date
Which of the following columns (A, B, C, or D) is correct?
Symbol
Protons
Neutrons
Electrons
Mass No.
(a)
(b)
(c)
(d)
(e)
(2)
B
C
D
60Co2+
100Ru3+
210At1-
90
142
91
232
27
33
29
60
44
56
41
100
85
125
86
210
A
B
C
D
None of these is correct.
A piece of indium weighing 15.442 g is placed in 49.7 cm3 of ethyl alcohol (d =
0.798 g/cm3) in a graduated cylinder. The alcohol level increases to 51.8 cm3. The
best value for density of indium from these data is
(a)
(b)
(c)
(d)
(e)
(3)
A
232Th
7.353 g/cm3
7.35324 g/cm3
7.4 g/cm3
9.21 g/cm3
9.2 g/cm3
The correct formula of nickel(III) fluoride is
(a)
(b)
(c)
(d)
(e)
CHE 106
NiF2
NiF3
NiF
Ni3F3
Ni3F
1
Fall 2002 Exam Questions
(4)
One gram of washing soda, Na2CO3.10H2O, has 2.1 x 1021 carbon atoms. How
many oxygen atoms are present in 1.0 g of washing soda?
(a)
(b)
(c)
(d)
(e)
(5)
The formulas of the carbonate ion, ammonium ion, and the chlorate ion are
represented, respectively, as
(a)
(b)
(c)
(d)
(e)
(6)
2.1 x 1021
6.3 x 1021
8.4 x 1021
2.7 x 1022
3.2 x 1022
CO32-, NH21-, ClO31CO32-, NH3+1, ClO1CO21-, NH4+1, ClO1CO32-, NH4+1, ClO31P3-, NH3+1, ClO31-
Elemental phosphorus is often converted to phosphoric acid in the location where
it will be used. The conversion involves oxidation of molten phosphorus, followed
by the hydration of the P4O10 to phosphoric acid. The reactions are represented by
the overall equation:
P4 + 5 O2 + 6 H2O ------> 4 H3PO4
What minimum mass of phosphorus is needed to prepare 125 g of H3PO4?
(a)
(b)
(c)
(d)
(e)
(7)
A sample having a mass of 0.01532 g was burned in pure oxygen and 0.00565 g of
CO2 and 0.00116 g of H2O were obtained. What is the percent C and the percent H
in the compound?
(a)
(b)
(c)
(d)
(e)
(8)
9.88 g
24.3 g
39.5 g
97.2 g
123.9 g
11.0% C and 0.424% H
11.0% C and 0.847% H
11.0% C and 89.0% H
15.8% C and 0.424% H
15.8% C and 0.847% H
In 0.358 g of KAu(CN)2, there are 7.48 x 1020 atoms of gold. What is the total
number of atoms in this sample
(a) 1.50 x 1021
(b) 2.24 x 1021
(c) 2.99 x 1021
(d) 3.74 x 1021
(e) 4.49 x 1021
CHE 106
2
Fall 2002 Exam Questions
(9)
If 50.0 g of O2 are mixed with 50.0 g of H2 and the mixture is ignited, what mass
of water is produced?
(a)
(b)
(c)
(d)
(e)
(10)
Which of the following statements is incorrect?
I.
II.
III.
IV.
Potassium carbonate, K2CO3, is soluble in water.
The net ionic equation when AgNO3 is added to NaI in aqueous solution is
Ag+1(aq) + I1-(aq) ------> AgI(s)
MgSO4(aq) + NaOH(aq) ------> NR is a correct representation of the
molecular equation when these substances are placed in aqueous solution.
When Cu(NO3)2(aq) is added to (NH4)2S(aq) a precipitate is formed.
(a)
(b)
(c)
(d)
(e)
(11)
50.0 g
56.3 g
65.7 g
71.4 g
100.0 g
I
II
III
IV
All are correct
Aqueous HCl was added to neutralize 400.0 mL of 0.05250 M Ba(OH)2. After the
neutralization was complete the volume of the resulting solution was 450.0 mL.
What concentrations of the ions are present in the solution?
(a)
(b)
(c)
(d)
(e)
0.05250 M Ba2+ and 0.1050 M Cl0.04667 M Ba2+ and 0.09333 M Cl0.05250 M Ba2+, 0.1050 M Cl-, 0.1050 M H3O+, and 0.1050 M Cl0.4667 M Ba2+, 0.09333 M Cl-, 0.0933 M H3O+, and 0.09333 M Cl0.04667 M Ba2+ and 0.09333 M OH-
(12)
What is the oxidation number for phosphorous in H2PO4-1 is
(a) +1 (b) +3 (c) +5 (d) –3 (e) -5
(13)
Suppose you want to prepare 250 mL of 0.100 M Na2SO4. The molar masses of
H2O and Na2SO4 are 18.02 g/mol and 142.05 g/mol, respectively. The mass of
Na2SO4 required to prepare this solution is
(a)
(b)
(c)
(d)
(e)
CHE 106
3.55 g
3.55 x 101 g
0.451 g
1.76 x 10-4 g
0.176 g
3
Fall 2002 Exam Questions
(14)
Calculate the enthalpy of reaction for the formation of anhydrous aluminum
chloride
2 Al(s) + 3 Cl2(g) ------> 2 AlCl3(s)
from the following data:
2 Al (s) + 6 HCl(aq) ------> 2 AlCl3(aq) + 3 H2
HCl(g) ------> HCl(aq)
H2(g) + Cl2(g) ------> 2 HCl(g)
AlCl3(s) ------> AlCl3(aq)
(a)
(b)
(c)
(d)
(e)
(15)
H1° = -1049 kJ
H2° = -73.5 kJ
H3° = -185 kJ
H4° = -323 kJ
-1399 kJ
593.0 kJ
-1581 kJ
1809.0 kJ
none of these
50.0 mL of 1.0 M HCl were mixed with 50.0 mL of 1.0 M NaOH in a coffee cup
calorimeter. The resulting solution changed temperature from 23.0°C to 29.8° C.
Which one of the following is not true concerning this experiment. Assume the
resulting solution had the density and specific heat of pure water.
(a)
(b)
(c)
(d)
The reaction was exothermic
2.8 kJ of heat were transferred during the process
For this reaction, H(reaction) = + 2.84 kJ
The heat flow monitored during this process was monitored under
constant pressure
(e) None of these
CHE 106
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Fall 2002 Exam Questions
(16)
An important reaction of alkenes is the addition of bromine to the double bond.
Given the following information, calculate the H for the bromination of ethylene.
H
H
C
C
H
(a)
(b)
(c)
(d)
(e)
Br
C
C
H
H
H
Bond Dissociation Energies (kJ mol-1)
348
614
146
358
463
413
193
276
-276 kJ mol-1
54 kJ mol-1
-93 kJ mol-1
183 kJ mol-1
None of the answers are within 10% of the correct value.
Which of the following statements is/are correct?
I.
II.
III.
When heat energy flows from a system to the surroundings, we know that
the temperature of the system is greater than that of the surroundings.
Given the thermochemical equation 4NH3(g) + 5O2(g) ---> 4NO(g) +
6H2O(g) H = -906 kJ, the enthalpy change for the following reaction is
+227 kJ: NO(g) + 3/2 H2O(g) ------> NH3(g) + 5/4 O2(g)
If a reaction has a very large positive value of H, then the reaction
proceeds to completion as written.
(a)
(b)
(c)
(d)
(e)
(18)
H
H
Bond Type
C-C
C=C
O-O
C-O
O-H
C- H
Br - Br
C - Br
(17)
+ Br2
Br
I
II
III
I and II
I and III
What is the wavelength of light emitted when the hydrogen atom undergoes a
transition from level n = 5 to level n = 2? [RH = 2.180 x 10-18 J]
(a)
(b)
(c)
(d)
(e)
CHE 106
663 nm
833 nm
546 nm
521 nm
434 nm
5
Fall 2002 Exam Questions
(19)
Which sketch represents an orbital that can have an azimuthal quantum number of
1? ( p orbital )
(1)
(a)
(b)
(c)
(d)
(e)
(20)
(4)
(5)
1
2 and 4
4 and 5
2 and 3
all of the above
1
3
5
7
9
Which of the following combination of quantum numbers are permissible?
I.
II.
III.
(a)
(b)
(c)
(d)
(e)
(22)
(3)
How many values are there for the magnetic quantum number ( m ) when the value
of the angular momentum quantum number ( l ) is 2?
(a)
(b)
(c)
(d)
(e)
(21)
(2)
11
4
3
10
3
2
-7
0
1
+1/2
-1/2
+1/2
I only
II only
III only
I and II only
I, II, and III
The ground state electron configuration of a Fe2+ ion is 1s22s22p63s23p63d6.
Therefore, Fe2+ is
(a)
(b)
(c)
(d)
(e)
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diamagnetic
paramagnetic with one unpaired electron
paramagnetic with two unpaired electrons
paramagnetic with three unpaired electrons
paramagnetic with four unpaired electrons
6
Fall 2002 Exam Questions
(23)
What is the valence shell electron configuration for the fourth period element in
Group IVA (Group 14)?
(a)
(b)
(c)
(d)
(e)
(24)
Which of the following properties, in general, increase as we move left to right
across a period in the periodic table?
I.
II.
III.
atomic radius
ionization energy
nonmetallic character
(a)
(b)
(c)
(d)
(e)
(25)
Ne and Ar
Na+ and K+
K+ and ClB3+ and Ne
Be2+ and Na+
In the ICl41- ion, how many valence electrons are there about the central iodine
atom?
(a)
(b)
(c)
(d)
(e)
(30)
I only
II only
III only
I and II only
II and III only
Which pair of species is isoelectronic?
(a)
(b)
(c)
(d)
(e)
(26)
5s25p2
4s25p3
4s24p2
5s24p3
4s23d3
4
6
8
10
12
What hybrid orbitals of silicon are involved in the bonding in silicon tetrafluoride?
(a)
(b)
(c)
(d)
(e)
CHE 106
sp
sp2
sp3
dsp3
d2sp3
7
Fall 2002 Exam Questions
(31)
How many moles are in a gas sample occupying 0.500 L at 170 mmHg and 25° C?
(a)
(b)
(c)
(d)
(e)
(32)
Which of the following is/are correct?
I.
II.
III.
If liquid “kryptonite” (from Superman’s home planet), with a density twice
that of mercury, is used in a barometer on Earth, one standard atmosphere
of pressure would support a column of mercury 380 mm in height.
At constant volume and number of moles of gas, the pressure exhibited by
an ideal gas is directly proportional to its absolute temperature
At standard temperature and pressure (STP), the volume of a mixture of
gases containing 0.400 mol H2, 0.600 mol N2, and 1.00 mol of O2 is 44.8
liters and the mole fraction of N2 is 0.300.
(a)
(b)
(c)
(d)
(e)
(33)
0.00457
0.00500
2.18
3.48
3.85
II
III
II and III
I and II
All are correct
Magnesium metal reacts with hydrochloric acid to produce hydrogen gas, H2,
according to the following reaction:
Mg(s) + 2 HCl(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)
(34)
1.82 L
2.37 L
0.220 L
0.169 L
None of the above
Using the phase diagram shown below, what phase transition takes place at point
F?
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Fall 2002 Exam Questions
Point E
Point F
Phase Z
1.0 atm
Curve C
curve D
Pressure
Phase X
Point B
Phase Y
Curve A
25° C
Temperature
(a)
(b)
(c)
(d)
(e)
(35)
phase z to/from phase x
phase z to/from phase y
phase y to/from phase x
phase x to/from phase z
not enough information provided
Which of the following is not a colligative property?
(a)
(b)
(c)
(d)
(e)
CHE 106
freezing point depression
boiling point elevation
osmotic pressure
solubility
None of these
9
Fall 2002 Exam Questions
Metal Activity Table
(easiest to oxidize at top)
Lithium
Potassium
Barium
Calcium
Sodium
Magnesium
Aluminum
Manganese
Zinc
Chromium
Iron
Cobalt
Nickel
Tin
Lead
HYDROGEN
Copper
Silver
Mercury
Platinum
Gold
Include Periodic Table
CHE 106
10
Fall 2002 Exam Questions
Final Exam
SUPA CHEM Fall 2002
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
19
20
21
22
23
24
25
26
27
28
29
30
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D
C
B
D
D
C
B
E
B
C
B
B
A
A
C
C
D
E
E
C
E
E
C
E
C
E
A
D
D
C
31
32
33
34
35
A
E
B
B
D
11
Fall 2002 Exam Questions