CHE 105
EXAMINATION II
University of Kentucky
July 5, 2013
Department of Chemistry
READ THESE DIRECTIONS CAREFULLY BEFORE STARTING THE EXAMINATION!
It is extremely important that you fill in the answer sheet EXACTLY as indicated, otherwise your
answer sheet may not be processed; ALL entries are to be made on SIDE 1 of the answer sheet. Use a #2 pencil
(or softer); fill in the circles completely and firmly. Erasures must be complete. Use only the following
categories:
NAME:
Print your name starting at the first space, LAST NAME first, then a space,
followed by your FIRST NAME, then another space, followed by your MIDDLE
INITIAL. Fill in the correct circles below your printed name corresponding to the
letters of your name; for the spaces, fill in the top blank circle.
STUDENT
NUMBER:
This is VERY IMPORTANT! Under IDENTIFICATION NUMBER, put in your
8 DIGIT STUDENT ID NUMBER (do not use the 9 at the beginning of your
number) beginning in column A and continuing through column H, column I will
be blank, (do NOT use column J at this time); be sure to fill in the correct circles (a
common error to be avoided is mistaking "0" for "1").
TEST FORM:
Fill in the "1" blank in the J column under IDENTIFICATION NUMBER (to
indicate Hour Examination I).
SPECIAL
CODES:
Use for course and section number; in positions K-P write in the following:
Dr. Owen
SIGNATURE:
105-020
You MUST sign the examination answer sheet (bubble sheet) on the line directly
above your printed name. Use your legal signature.
Answering Questions:
Starting with answer "1" on SIDE 1, fill in the circle indicating the one best answer for each of the 25
questions in this examination. Your score is the sum of the appropriate credit for each response. On the day
following the examination, an examination key will be posted on Blackboard.
Grading and Reporting:
The examination scores will be posted in Blackboard as soon as possible after the examination. If an
error has occurred in scoring your answers, inform your instructor within 48 hours of the posting of your score.
BE SURE THAT YOUR TEST HAS 25 QUESTIONS, A PERIODIC TABLE, AND ONE SHEET OF
SCRATCH PAPER. You may NOT use your own scratch paper during this examination. Cell phones,
computers, and pagers are to be turned off and out of sight during the exam.
1.
How many moles of water are produced when 8.00 moles of methane (CH4) are
completely combusted according to following chemical equation?
Commented [OU1]: Done!
Commented [LYB2]: I’d at least ask for moles of H2O to make
it a little tougher. Or, go for a more robust combustion reaction! 
CH4(g) + 2 O2(g) → 2 H2O(g) + CO2(g)
2.
A.
8.00 moles CO2
C.
4.00 moles CO2
B.
2.00 moles CO2
D.
16.00 moles CO2
For the following balanced reaction equation, how much carbon dioxide is produced
from a reaction of 39.6 grams of potassium carbonate (molar mass = 138.206 g/mol)
with an excess of hydrochloric acid?
2 HCl(aq) + K2CO3(aq) → H2O(l) + CO2(g) + 2 KCl(aq)
3.
A.
12.6 g CO2
C.
39.6 g CO2
B.
15.8 g CO2
D.
6.23 g CO2
What is the percent yield of sulfur when 28.0 grams of sulfur are formed from the
reaction of 44.0 grams of hydrogen sulfide (molar mass = 34.08 g/mol) with 57.6 grams
of sulfur dioxide (molar mass = 64.06 g/mol) according to the balanced equation below?
2 H2S(g) + SO2(g) → 3 S(s) + 2 H2O(l)
A.
30.0%
C.
80.0%
B.
15.4%
D.
45.1%
4.
5.
How many grams of strontium chloride are required to make 3.51 L of a 5.2 M strontium
chloride solution?
A.
1.5 × 103 g
C.
2.9 × 103 g
B.
4.5 × 103 g
D.
9.2 × 103 g
According to the following balanced chemical equation, how many grams of calcium
chloride (molar mass = 110.98 g/mol) form when 27.00 mL of 0.0496 M calcium
hydroxide (molar mass = 74.08 g/mol) reacts with excess chlorine gas?
2 Ca(OH)2(aq) + 2 Cl2(g) → Ca(OCl)2(aq) + CaCl2(s) + 2 H2O(l)
6.
A.
1.24 × 10‒1 g
C.
7.43 × 10‒2 g
B.
1.55 × 10‒2 g
D.
6.22 × 10‒2 g
What volume of 4.27 M sodium hydroxide solution is needed to prepare 75.0 mL of
0.289 M sodium hydroxide solution?
A.
7.62 mL
C.
35.0 mL
B.
5.08 mL
D.
10.2 mL
Commented [LYB3]: I get 5.08 mL
Commented [OU4]: Me too, thanks!
7.
Which compound is the most soluble in water?
A.
CaS
C.
CaSO4
B.
AgCl
D.
Ca3(PO4)2
8.
What is the complete, balanced, ionic equation for the reaction that occurs when an
aqueous solution of silver acetate reacts with magnesium chloride?
A.
Commented [LYB5]: Redundant, but may nudge students in the
right direction.
Commented [OU6]: Done!
Ag+(aq) + C2H3O2‒(aq) + Mg2+(aq) + Cl‒ (aq) →
Ag+(aq) + Cl‒(aq) + Mg2+(aq) + C2H3O2‒(aq)
B.
2 Ag+(aq) + 2 C2H3O2‒(aq) + Mg2+(aq) + 2 Cl‒(aq) →
2 Ag+ (aq) + 2 Cl‒ (aq) + Mg(C2H3O2)2(s)
9.
10.
C.
2 Ag+(aq) + 2 C2H3O2‒(aq) + Mg2+(aq) + 2 Cl‒(aq) →
2 AgCl(s) + Mg2+(aq) + 2 (C2H3O2)‒ (aq)
D.
Ag+(aq) + Cl‒(aq) → AgCl(s)
What is the net ionic equation for the reaction that occurs when aqueous solutions of
strontium hydroxide and lithium sulfate are mixed?
A.
Sr2+(aq) + SO42‒ (aq) → SrSO4(s)
B.
Li+(aq) + OH‒(aq) → LiOH(s)
C.
Sr2+(aq) + SO42‒(aq) → SrSO4(aq)
D.
H+(aq) + OH‒(aq) → H2O(l)
How much 2.00 M Ca(OH)2 solution is required to neutralize 1.24 liters of a 2.00 M HCl
solution?
A.
6.20×102 mL
C.
3.20×102 mL
B.
4.44×102 mL
D.
1.28×102 mL
Commented [LYB7]: Not sure if you left these charges out on
purpose to make it “wronger” or not.
11.
12.
13.
The titration of 25.0 mL of a sulfuric acid (H2SO4) solution of unknown concentration
requires 83.6 mL of 0.12 M LiOH solution to neutralize the acid. What is the
concentration of the H2SO4 solution?
A.
0.45 M
C.
0.64 M
B.
0.30 M
D.
0.20 M
What is the oxidation state for each element in CaCr2O7?
A.
Ca = +2, Cr = +12, O = ‒2
C.
Ca = +2, Cr = +6, O = ‒1
B.
Ca = +2, Cr = +6, O = ‒2
D.
Ca = +2, Cr = +10, O = ‒2
Identify the redox reaction(s).
I.
II.
III.
IV.
14.
4 Li(s) + O2(g) → 2 Li2O(s)
Mg(s) + Fe2+(aq) → Mg2+(aq) + Fe(s)
Pb(NO3)2(aq) + Na2SO4(aq) → PbSO4(s) +2 NaNO3(aq)
HBr(aq) + KOH(aq) → H2O(l) + KBr(aq)
A.
I
C.
I and II
B.
I, II, and III
D.
All the above.
What is 3.80 atm in units of torr?
A.
1.14 × 103 torr
C.
4.01 × 103 torr
B.
5.34 × 103 torr
D.
2.89 × 103 torr
15.
16.
17.
18.
What volume will an ideal gas occupy at 386°C if it occupies 3.8 L at 286°C? Assume
the pressure remains constant.
A.
4.5 L
C.
6.0 L
B.
3.5 L
D.
7.8 L
An ideal gas occupies 6.8 L. What volume does the gas occupy when the amount of gas
is tripled at constant pressure and temperature?
A.
1.0 × 101 L
C.
2.8 × 101 L
B.
2.0 × 101 L
D.
3.2 L
Which of the following are standard temperature and pressure (STP) measurements?
A.
0 K, 1.00 atm
C.
273 K, 1.00 atm
B.
100°C, 760 torr
D.
32°F, 1 Pa
How many molecules of CO2 are contained in a 10.0 L tank at 7.53 atm and 485 K?
A.
1.14 × 1024 molecules
B.
5.52 × 1024 molecules
C.
3.65 × 1024 molecules
D.
2.39 × 1024 molecules
19.
20.
21.
22.
Which of the following gases occupy the largest volume at STP?
A.
22 g Cl2
C.
22 g O2
B.
22 g CO2
D.
22 g SO2
What is the density of krypton gas at 25°C and 0.996 atm?
A.
3.41 g/L
C.
4.48 g/L
B.
1.23 g/L
D.
7.51 g/L
A 0.133 gram sample of an ideal gas occupies 164 mL at 747 torr and 298 K. What is the
molar mass of the gas?
A.
4.00 g/mol
C.
83.8 g/mol
B.
20.2 g/mol
D.
39.9 g/mol
A gas cylinder contains argon, xenon, and krypton and the total pressure is 900 torr. If
argon and xenon have a combined pressure of 600 torr, what mass of krypton is present
in the gas cylinder? The volume of the gas cylinder is 3.0 L and temperature is
298 K.
A.
0.50 g
C.
8.0 g
B.
1.1 g
D.
4.0 g
23.
How many liters of oxygen (at STP) are required to completely oxidize 50.0 grams of
sodium metal to sodium oxide according to the balanced chemical equation below?
4 Na(s) + O2(g) → 2 Na2O(s)
24.
25.
A.
12.2 L
C.
6.02 L
B.
8.34 L
D.
3.01 L
Which of the following statements is FALSE concerning the kinetic molecular theory of
gases?
A.
The average kinetic energy of gas molecules is the same at a given
temperature.
B.
The kinetic molecular theory of gases is an explanation of why gases behave
according to gas laws.
C.
Lighter gases have slower velocities than heavier gases if all gas molecules
have the same average kinetic energy.
D.
Lighter gases have faster velocities than heavier gases if all gas molecules
have the same average kinetic energy.
Which of the following equations is used to correct for non-ideal gas behavior?
A.
PV = nRT
C.
B.
P1V1 = P2V2
D.
E = mc2
Answer Key:
1. D
2. A
3. D
4. C
5. C
6. B
7. A
8. C
9. A
10. A
11. D
12. B
13. C
14. D
15. A
16. B
17. C
18. A
19. C
20. A
21. B
22. D
23. A
24. C
25. C