Download Fall Final 2009

Chemistry 106: General Chemistry
Syracuse University Project Advance
Final Exam, Fall 2009
Name
Date
The last page of each examination is a periodic table.
Rydberg Constant (RH) = 2.18 x 10-18 J
1. A sample that cannot be separated into two or more substances by physical means is:
a. A compound
b. An element
c. Either a compound or an element
d. A homogeneous mixture
e. A heterogenous mixture
2. Given the following enthalpies of formation, Hf°: CH4(g), -74.8 kJ/mol; H2O(g), -242
kJ/mol; CO2(g), -394 kJ/mol; O3, +143kJ/mol; what is H° in kJ for the following reaction?
3 CH4(g) + 4 O3(g) ------> 3 CO2(g) + 6 H2O
a.
b.
c.
d.
e.
3(394) + 6(242) – 4(143) + 3(74.8)
3(394) + 6(242) + 4(143) + 3(74.8)
-3(394) – 6(242) – 4(143) + 3(74.8)
-3(394) – 6(242) + 4(143) – 3(74.8)
-3(394) – 6(242) – 4(143) – 3(74.8)
3. The bromide ion, 80Br -, contains
a.
b.
c.
d.
e.
4.
35 protons and 35 electrons
45 neutrons and 34 electrons
45 neutrons and 45 electrons
35 protons and 80 neutrons
35 protons and 36 electrons
Which angular distribution plot represents an s orbital?
A
(a)
(b)
(c)
(d)
(e)
B
C
D
E
a
b
c
d
all can have a principal quantum number of 3
5. The formula for aluminum sulfate is:
a.
b.
c.
d.
e.
Al2(SO3)3
Al2(SO4)3
Al3(SO4)2
Al2S3
Al3S2
6. The __________ subshell contains only one orbital.
a.
b.
c.
d.
e.
5d
6f
4s
3d
1p
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7. What is the mass percentage of carbon in l-carvone, C10H14O (mw = 150.2 amu)?
a.
b.
c.
d.
e.
30%
40%
60%
70%
80%
8. In a beaker, we have 200 mL of a solution of acetic acid, a weak, monoprotic acid, and, in a
burette, we have a solution of 0.100M KOH. The KOH solution is dripped into the beaker
until the solution becomes basic. This requires 24.8 mL of the KOH solution. What was the
molarity of the acetic acid solution?
a.
b.
c.
d.
e.
0.00496M
0.0124M
0.0248M
0.0588M
0.158M
9. Ammonia burns in the presence of a copper catalyst to form nitrogen gas according to the
equation:
4 NH3(g) + 3 O2(g) ------> 2 N2(g) + 6 H2O(g)
H = -1267 kJ
What is the enthalpy change when 1.79 on NH3 is burned? [Note: Molar masses are:
NH3, 17.03 g/mol; O2, 32.00 g/mol; N2, 28.01 g/mol; H2O, 18.02 g/mol]
a. 633.5J
b. -633.5 J
c. -33.3 kJ
d. -133 J
e. -100 J
10. How many grams of oxygen are required to burn 8.8 g of C3H8?
C3H8 + O2 → CO2 + H2O
a.
b.
c.
d.
e.
6.4
12
16
32
64
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11. Balance the following equation and report the coefficient for hydrogen.
___NaBH4 + ___H2SO4 → ___B2H6 + ___H2 + ___Na2SO4
a. 1
b. 2
c. 3
d. 4
e. 5
12.
For the oxidation-reduction reaction below which of the following statements are true?
Zn(s) + 2Ag+(aq)  Zn2+(aq) + 2Ag(s)
1.
2.
3.
4.
5.
6.
a.
b.
c.
d.
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1,4,5
2,3,5
2,3,6
1,4,6
The density magnesium is 1.74 g/cm3. What is the mass of a block that measures 2.5 cm
by 3.5 cm by 1.5 cm?
(a)
(b)
(c)
(d)
(e)
14.
Zn is oxidized.
Zn is reduced.
Ag+ is oxidized.
Ag+ is reduced.
Zn is the reducing agent.
Zn2+ is the oxidizing agent.
48 g
23 g
12 g
7.5 g
2.2 g
A neutralization reaction between an acid and a metal hydroxide produces
a. Water and a salt
b. Hydrogen gas
c. Oxygen gas
d. Sodium hydroxide
e. ammonia
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15.
Given the following reactions:
2S (s) + 3O2 (g) → 2SO3 (g)
S (s) + O2 (g) → SO2 (g)
ΔH = -790 kJ
ΔH = -297 kJ
Find the enthalpy of the reaction in which sulfur dioxide is oxidized to sulfur trioxide:
2SO2 (g) + O2 (g) → 2SO3 (g)
a.
b.
c.
d.
e.
196 kJ
-196 kJ
1087 kJ
-1384 kJ
-543 kJ
16. The ______________ quantum number defines the shape of an orbital.
a. principle
b. angular momentum
c. magnetic
d. spin
e. psi
17. Fumaric acid, which occurs in many plants, contains by mass 42.4% carbon, 3.47%
hydrogen, and 55.1% oxygen. A 0.050 mole sample of this compound weighs 5.80 grams.
The molecular formula of this compound is
a. CHO
b. C3H3O
c. C3H3O3
d. C4H4O4
e. C6H6O6
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18. Which of the following follow Pauli’s exclusion principle?
a. 1 and 2
b. 1 and 3
c. 1 and 4
d. 2 and 3
e. 2 and 4
19. The reaction shown below is ___________________, and therefore heat is
______________by the reaction.
a.
b.
c.
d.
e.
4Al (s) + 3O2 (g) → 2Al2O3 (s)
Endothermic, released
Endothermic, absorbed
Exothermic, released
Exothermic, absorbed
Thermoneutral, neither released or absorbed
ΔHo = -3351 kJ
20. Write the ground-state electron configuration of a Ni2+ ion. The Ni2+ ion is:
a. diamagnetic
b. paramagnetic with 1 unpaired electron
c. paramagnetic with 2 unpaired electrons
d. paramagnetic with 3 unpaired electrons
e. paramagnetic with 4 unpaired electrons
21. Which of the following properties, in general, increase as we move from left to right across
the periodic table?
1. Atomic radius
2. Ionization Energy
3. Metallic character
a. 1 only
b. 2 only
c. 3 only
d. 1 and 2 only
e. 2 and 3 only
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22. A sample of oxygen gas occupies a volume of 900 mL at a presume of 100 mmHg,. What is
the pressure of the gas if the volume is reduced to 300mL and the temperature is doubled?
a. 66.7 mm
b. 33.3 mm
c. 300 mm
d. 150 mm
e. 600 mm
23. Which ion in the isoelectronic series below has the largest ionic radius?
a. Al3+
b. Na+
c. O2d. Fe. N324. In which of the following compounds is the octet rule violated by the central atom?
a. PF3
b. SiF4
c. OF2
d. ClF3
e. ClF
25. If 4 mol of Neon gas and 6 mol of Krypton gas are contained in a flask whose total pressure
is 1000 mmHg, the partial pressure of Neon gas is:
a. greater than the partial pressure of the Krypton gas
b. less than the partial pressure of the Krypton gas
c. the same as the partial pressure of the Krypton gas
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26. Write the Lewis structure of the thiocyanate ion, SCN-, in which carbon has a double bond
with both the sulfur and nitrogen atoms. The formal charges on the sulfur, carbon, and
nitrogen atoms are, respectively
a.
b.
c.
d.
e.
-1, 0, 0
0, 0, -1
-1, +1, -1
-2, +1, 0
-2, 0, +1
27. In phosgene, Cl2CO, the electron pairs are located around the central carbon atom in a
__________ arrangement.
a. pyramidal
b. tetrahedral
c. trigonal planar
d. trigonal bipyramidal
e. square planar
28. Of the following, the central atom is sp3d2 hybridized only in
a. PCl5
b. XeF4
c. PH3
d. Br3e. BeF2
29. In molecular orbital theory, the σ1s orbital is _________ and the σ*1s orbital is__________ in
the H2 molecule.
a. filled, filled
b. filled, empty
c. filled, half-filled
d. half-filled, filled
e. empty, filled
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30.
Calculate the density of ammonia gas in a 4.32 L container at 837 torr and 45oC.
a.
b.
c.
d.
e.
3.85 g/L
0.719 g/L
0.432 g/L
0.194 g/L
none of the above
31. The properties of a real gas are most likely to deviate from those properties predicted for an
ideal gas when
a. the pressure is low.
b. the temperature is high
c. the pressure is high and the temperature is low
d. the pressure is low and the temperature is high
e. None of the above are true.
32. Which of the following is included as a postulate in the kinetic molecular theory of an ideal
gas?
a. The distance between gas molecules is small compared with the size of the molecule.
b. Collisions between molecules are all elastic.
c. In an average collision between molecules, both molecules have the same kinetic
energy.
d. All molecules move randomly in zigzag directions.
e. All the molecules have the same velocity.
33
Millikan’s oil drop experiment showed that;
(a)
(b)
(c)
(d)
(e)
matter is mostly composed of empty space.
the energy levels within an atom are quantized.
nature has a duality of wave-like and particle-lake behavior in atoms.
there is a fundamental charge on the electron.
an electron is much smaller that either the proton or the neutron.
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Which pair of elements below should be the most similar in chemical properties?
(a)
(b)
(c)
(d)
(e)
35
C and O
B and As
I and Br
K and Kr
Cs and He
The balanced net ionic equation for precipitation of PbSO4 when aqueous solutions of
Pb(NO3)2 and Na2SO4 are mixed is;
(a) Pb+2(aq) + 2 NO3–(aq) + 2Na+(aq) + SO4-2(aq) ------> PbSO4(s) + 2 NO3-1(aq) + 2Na+(aq)
(b) Pb+2(aq) + SO4-2(aq) ------> PbSO4(s)
(c) Pb+2(aq) + 2 NO3–(aq) ------> Pb(NO3)2 (aq)
(d) Pb(NO3)2 (aq) + Na2SO4 (aq) ------> PbSO4(s) + 2 NaNO3(aq)
(e) Pb(NO3)2 (aq) + Na2SO4 (aq) ------> PbSO4(aq) + 2 NaNO3(aq)
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Final Exam Fall 2009