CHEM 102 Winter 12 Exam 2 (A) Questions and Answers
Potentially useful information: First order half-life: t1/2 = ln2 / k
[A]t = - kt + [A]o ln[A]t = - kt + ln[A]o 1/[A]t = kt +1/[A]o
1. Please choose the letter “a” as your answer for this question.
2. Which choice is an example of an...
CHEM 102 Winter 12 Exam 2 (A) Questions and Answers
Potentially useful information: First order half-life: t1/2 =
ln2 / k
[A]t = - kt +
[A]o ln[A]t = -
kt + ln[A]o
1/[A]t = kt
+1/[A]o
1. Please choose the letter “a” as your answer for this question.
2. Which choice is an example of an amorphous solid?
a. NaCl
b. graphite
c. iron
d. diamond
e. glass
3. Which choice is an example of an ionic solid?
a. NaCl
b. diamond
c. iron
d. quartz
e. glass
4. In body-centered cubic unit cells, of the atom in the center of the unit cell is
counted as part of that unit cell.
a. all
b. none
c. 1/2
d. 1/4
e. 1/8
5. Elements most likely to be used for doping silicon in making semiconductors are
a. Ba, La, and Y.
b. Ne, Ar, and Kr.
c. Ga, As, and B.
d. Au, Ag, and Cu.
e. Li, Na, and K.
6. In an n-type doped semiconductor the charge carriers are the because
.
a. holes; electrons move to fill a hole, thus leaving a hole elsewhere
b. holes; there are extra electrons that can move freely
c. nuclei; they are not locked into one location
d. electrons; there are extra electrons that move freely
e. electrons; the doping atoms have fewer electrons
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, 7. Which unit-1 is appropriate for describing reaction rates?
a. kJ mol
b. C min
-1
c. M min
-1
d. kJ g-1
e. g L-1
8. The rate of the chemical reaction involving two substances, A and B, is
measured. It is found that if the initial concentration of A used is doubled,
keeping the B concentration the same, the rate doubles. If the concentrations of
both A and B are doubled, the rate is eight times that measured in the first
experiment. The rate law for this reaction is rate =
a. k[A][B].
b. k[A]2[B].
c. k[A][B] 2.
d. 2k[A][B].
e. k[A][B]/2.
9. Consider the
reaction NO2 + O3 NO3 + O2
Use the data shown to determine the rate law for the reaction.
a. rate = k[NO2] [O3]
b. rate = k[NO2]2 [O3]2
c. rate = k[NO2] [O3]
d. rate = k[NO2]
e. rate = k[NO3] [O3]/ [NO2] [O2]
10. The rate law for a given reaction is rate = k [reactant]2, with k = 2.64 10-4
M-1 min-1. If the initial concentration is 0.0250 M, what is the initial rate,
with the correct units?
a. 4.36 10-11 M min-1
b. 1.65 10-7 min-1
c. 6.60 10-6 M min-1
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