Transcript Final Review

Final Review
Chemistry 107
Park University
April Senger
Short Answer Topics
• Reduction and Oxidation
• Basics: atoms, elements, compounds,
molecules, pure substances, and mixtures
(homo & hetero)
• Naming rules for ionic and covalent bonds
• Intermolecular forces: dispersion, dipoledipole, hydrogen bonding and ion-dipole
1. Which of the following contains
the largest number of molecules?
a)
b)
c)
d)
10.0 g CH4
10.0 g C2H6
10.0 g SO2
10.0 g Xe
2. Which of the following contains
the largest mass percent
hydrogen?
a)
b)
c)
d)
10.0 g CH4
10.0 g C2H6
10.0 g H2O
10.0 g H2S
3. How many neutrons are in 1000
atoms of Cl-37?
A)
B)
C)
D)
E)
37
37,000
20
20,000
Can not be determined
4. Which sample represents the
greatest number of moles?
a)
b)
c)
d)
e)
44.01g CO2
1.0 mol C3H8
6.022 x 1023 molecules of C4H10
18.02 g H2O
All the samples have the same number
of moles
5. Calculate the number of carbon
atoms in 25.0 grams of isopropyl
alcohol (C3H8O)
a)
b)
c)
d)
e)
1.25 C atoms
15.0 C atoms
2.51 x 1023 atoms
7.52 x1023 atoms
2.07 x 10-24 atoms
6. An unknown compound contains
the following percents by mass: C:
60.86%, H: 5.83%, O: 23.16%, and
N: 10.14%. Find the empirical
formula.
A)
B)
C)
D)
E)
C6H8O2N2
C 7H 8O 2N
C 6H 8O 2N
C 8H 8O 2N
C8H8ON
7. What are the coefficients for the
decomposition of nitroglycerin?
___C3H5N3O9  ___ N2 + ___ CO2 + ___H2O + ___O2
A)
B)
C)
D)
E)
2,3,6,2,1
2,3,6,5,1
4,6,12,10,12
4,3,12,10,1
4,6,12,10,1
8. Ammonia is produced using the
Haber process:
3 H2 + N2  2 NH3
What percent yield of ammonia produced from 15.0
kg each of H2 and N2, if 13.7 kg of product are
recovered? Assume the reaction goes to
completion.
A)
B)
C)
D)
E)
7.53 x 10-2 %
1.50 x 10-1 %
75.3%
15.0 %
16.2 %
9. What mass, in grams, of sodium
bicarbonate, NaHCO3, is required to
neutralize 1000.0 L of 0.350 M H2SO4?
H2SO4 + 2NaHCO3  2 CO2 + Na2SO4 + 2H2O
a)
b)
c)
d)
e)
2.94 x 104 g
1.47 x 104 g
5.88 x 104 g
3.50 x 103 g
1.75 x 103 g
10. What is the maximum number
of grams of PbI2 precipitated upon
mixing 25.0 ml of 0.150 M KI with
15.0 ml of 0.175 M Pb(NO3)2?
a)
b)
c)
d)
e)
0.864 g
1.73 g
1.21 g
2.07 g
None of the above
2 KI + Pb(NO3)2  PbI2 + 2 KNO3
11. What is the molarity of an
aqueous solution containing 22.5 g
of sucrose (C12H22O11) in a 35.5 ml
solution?
a)
b)
c)
d)
e)
0.0657 M
1.85 x 10-3 M
1.85 M
3.52 M
0.104 M
12. How many moles of Helium are
found in a balloon that contains 5.5
L of Helium at a pressure of 1.15
atm and a temperature of 22.0
degrees C?
a)
b)
c)
d)
e)
3.5
0.26
2.6
0.35
3.8
13. A 3.50 g sample of diatomic gas
in a 1.5 L container has a pressure
of 2.42 atm at 355 K. Determine
the identity of the gas.
a)
b)
c)
d)
e)
H2
N2
Cl2
O2
F2
14. A gas phase mixture of H2 and
N2 has a total pressure of 784 torr
with a H2 partial pressure of 124
torr. What mass of N2 gas is
present in 2.00 L of the mixture at
298
K?
a) 0.0133 g
b)
c)
d)
e)
0.0710 g
0.374 g
0.994 g
1.99 g
15. A 3.54 g piece of aluminum is heated to 96.2
degrees C and allowed to cool to room
temperature, 22.5 degrees C. Calculate the heat
(in kJ) associated with the cooling process. The
specific heat of aluminum is 0.9013 J/g·K.
a)
b)
c)
d)
e)
+0.236
-236
+236
-0.236
-0.638
16. Determine the wavelength (in
nm) of an X-ray with a frequency of
4.2 x 1018 Hz.
a)
b)
c)
d)
e)
7.1 x 10-11
7.1 x10-2
1.3 x1027
1.4 x1010
7.1 x10-18
17. A major league pitcher throws a
148.8 g baseball at a speed of 92.5
mph (41.4 m/s). What is the de
Broglie wavelength of the baseball
in meters?
a)
b)
c)
d)
e)
4.81 x10-38
4.81 x10-41
1.08 x10-34
1.08 x10-37
1.08 x10-40
18. What is the frequency (Hz) of
an infrared light that emits 24.5
kJ/mol of energy?
a)
b)
c)
d)
e)
3.70 x1034
6.14 x1013
4.92 x1019
8.17 x10-8
2.70 x10-35
19. Consider the following isoelectric
series:
ClAr
K+
Ca2+
Which particle is the largest?
a)
b)
c)
d)
ClAr
K+
Ca2+
20. What is the ground state
electron configuration for S?
a)
b)
c)
d)
[Ne]3s23p4
[Ne]2s23p5
[Ar]2s22d4
[Ne]2s22d4
21. How many valance electrons
does chlorine have?
a)
b)
c)
d)
e)
1
2
5
6
7
22. Rank the following in order of
increasing bond polarity:
H-F
H-Br
F-F
Na-Cl
a)
b)
c)
d)
e)
H-F < H-Br < F-F < Na-Cl
F-F < H-F < H-Br < Na-Cl
H-Br < H-F < F-F < Na-Cl
F-F < H-Br < H-F < Na-Cl
Na-Cl < H-F < H-Br < F-F
23. Use the average bond energies to
determine the ∆Hrxn for the burning of H2.
H2 (g) + ½ O2 (g)  H2O (g)
a)
b)
c)
d)
e)
6 kJ
470 kJ
-243 kJ
-350 kJ
-421 kJ
H-H 436
O=O 498
O-O 142
O-H 464
24. Draw the best Lewis structure
for Ca(OH)2. How many lone pairs
of electrons are on Ca?
a)
b)
c)
d)
e)
0
1
2
3
4
25. PCl3 is an industrial chemical used in
many herbicides and insecticides. What is
the molecular shape of PCl3?
a) Bent
b) Tetrahedral
c) Trigonal pyramidal
d) T-shaped
e) Trigonal planar
Copyright © 2011 Pearson Education, Inc.
26. What is the approximate angle
of the O─C─O bond in the citric
acid molecule below?
O
a) 120 º
b) 109.5 º
c) < 120 º
d) < 109.5 º
e) > 120 º
O
OH
OH
O
HO
Copyright © 2011 Pearson Education, Inc.
HO
27. What is the hybridization of the
central atom in XeF2?
a) sp
b) sp2
c) sp3
d) sp3d
e) sp3d2
Copyright © 2011 Pearson Education, Inc.
28. How many lone pairs are found
in a caffeine molecule?
a) 0
b) 4
c) 6
d) 8
e) 12
Copyright © 2011 Pearson Education, Inc.
29. How much energy is required to vaporize
32.9 g of ethanol at its boiling point, if its
Hvap is 40.5 kJ/ mol.
a) 28.9 kJ
b) 3.83 kJ
c) 6.30 kJ
d) 17.6 kJ
e) 7.60 kJ
Copyright © 2011 Pearson Education, Inc.
The Answers
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
A
A
D
E
D
B
E
C
C
A
C
B
13. B
14. E
15. D
16. B
17. C
18. B
19. A
20. A
21. E
22. D
23. C
24. A
25. C
26. E
27. D
28. D
29. A