College Chemistry II Practice Exam 2
Name___________________________________
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
1) A burning splint will burn more vigorously in pure oxygen than in air because ________.
A) oxygen is a reactant in combustion and concentration of oxygen is higher in pure oxygen than
is in air
B) oxygen is a catalyst for combustion
C) oxygen is a product of combustion
D) nitrogen is a product of combustion and the system reaches equilibrium at a lower
temperature
E) nitrogen is a reactant in combustion and its low concentration in pure oxygen catalyzes the
combustion
1)
2) Of the following, all are valid units for a reaction rate except ________.
A) mol/L
B) M/s
C) mol/hr
D) g/s
2)
E) mol/L-hr
3) Which one of the following is not a valid expression for the rate of the reaction below?
4NH3 + 7O2
A) -
1
7
4NO2 + 6H2 O
[O2 ]
t
B)
1
4
[NO2 ]
t
C)
1
6
[H2 O]
D) -
3)
t
1
4
[NH3 ]
t
E) All of the above are valid expressions of the reaction rate.
4) The rate law of a reaction is rate = k[D][X]. The units of the rate constant are ________.
A) mol L-1 s-1
B) L mol-1 s-1
C) mol2 L-2 s-1
D) mol L-1 s-2
E) L2 mol-2 s-1
1
4)
The data in the table below were obtained for the reaction:
A + B
P
Experiment
Initial Rate
Number
[A] (M) [B] (M)
(M/s)
1
0.273
0.763
2.83
2
0.273
1.526
2.83
3
0.819
0.763
25.47
5) The rate law for this reaction is rate = ________.
D) k[A]2 [B]2
E) k[A]2
D) 42.0
E) 2.21
D) 3
E) 4
8) What is the order of the reaction with respect to OH- ?
A) 0
B) 1
C) 2
D) 3
E) 4
9) What is the overall order of the reaction?
A) 4
B) 0
D) 2
E) 3
A) k[A][B]
B) k[P]
C) k[A]2 [B]
6) The magnitude of the rate constant is ________.
A) 38.0
B) 0.278
C) 13.2
5)
6)
The data in the table below were obtained for the reaction:
2 ClO2 (aq) + 2 OH- (aq)
ClO3 - (aq) + ClO2 - (aq) + H2 O (1)
Experiment
Initial Rate
Number
[ClO2 ] (M) [OH- ] (M)
(M/s)
1
0.060
0.030
0.0248
2
0.020
0.030
0.00276
3
0.020
0.090
0.00828
7) What is the order of the reaction with respect to ClO2 ?
A) 1
B) 0
C) 2
C) 1
10) What is the magnitude of the rate constant for the reaction?
A) 1.15 × 104
B) 4.6
C) 230
7)
9)
10)
D) 115
E) 713
11) Under constant conditions, the half-life of a first-order reaction ________.
A) is the time necessary for the reactant concentration to drop to half its original value
B) is constant
C) can be calculated from the reaction rate constant
D) does not depend on the initial reactant concentration
E) All of the above are correct.
2
8)
11)
12) The reaction
2NO2
12)
2NO + O2
follows second-order kinetics. At 300 °C, [NO2 ] drops from 0.0100 M to 0.00650 M in 100.0 s. The
rate constant for the reaction is ________ M-1 s-1 .
A) 0.096
B) 0.65
C) 0.81
D) 1.2
E) 0.54
13) The reaction
CH3 -N C
13)
CH3 -C N
is a first-order reaction. At 230.3 °C, k = 6.29 × 10-4 s-1 . If [CH3 N C] is 1.00 × 10-3 initially,
[CH3 N C] is ________ after 1.000 × 103 s.
A) 5.33 × 10-4
B) 2.34 × 10-4
C) 1.88 × 10-3
D) 4.27 × 10-3
E) 1.00 × 10-6
3
14) Which one of the following graphs shows the correct relationship between concentration and time
for a reaction that is second order in [A]?
A)
14)
B)
C)
D)
E)
15) The following reaction is second order in [A] and the rate constant is 0.025 M-1 s-1 :
A
15)
B
The concentration of A was 0.65 M at 33 s. The initial concentration of A was ________ M.
A) 2.4
The reaction A
Time (s)
[A] (M)
B) 0.27
C) 0.24
D) 1.4
E) 1.2 × 10-2
B is first order in [A]. Consider the following data.
0.0
0.20
5.0
0.14
10.0
0.10
15.0
0.071
20.0
0.050
16) The rate constant for this reaction is ________ s-1 .
A) 6.9 × 10-2
B) 3.0 × 10-2
C) 14
D) 0.46
17) The concentration of A is ________ M after 40.0 s.
A) 1.3 × 10-2
B) 1.2
C) 0.17
E) 4.0 × 102
16)
17)
D) 3.5 × 10-4
4
E) 0.025
18) The rate constant of a first-order process that has a half-life of 3.50 min is ________ s-1 .
A) 0.693
B) 1.65 × 10-2
18)
C) 1.98
D) 0.198
E) 3.30 ×10-3
B (aq) is first order in [A]. A solution is prepared with [A] = 1.22 M. The
19) The reaction A (aq)
following data are obtained as the reaction proceeds:
Time (s)
[A] (M)
0.0
1.22
6.0
0.61
12.0
0.31
19)
18.0
0.15
The rate constant for this reaction is ________ s-1 .
A) 0.23
B) 1.0
C) 0.17
D) 0.12
E) -0.12
20) One difference between first- and second-order reactions is that ________.
A) the half-life of a first-order reaction does not depend on [A]0 ; the half-life of a second-order
reaction does depend on [A]0
B) the rate of both first-order and second-order reactions do not depend on reactant
concentrations
C) the rate of a first-order reaction depends on reactant concentrations; the rate of a
second-order reaction does not depend on reactant concentrations
D) a first-order reaction can be catalyzed; a second-order reaction cannot be catalyzed
E) None of the above are true.
5
20)
21) At elevated temperatures, methylisonitrile (CH3 NC) isomerizes to acetonitrile (CH3 CN):
CH3NC (g)
21)
CH3 CN (g)
The reaction is first order in methylisonitrile. The attached graph shows data for the reaction
obtained at 198.9 °C.
The rate constant for the reaction is ________ s-1 .
A) -1.9 × 104
B) +1.9 × 104
C) -5.2 × 10-5
D) +5.2 × 10-5
E) +6.2
22) The decomposition of N2 O5 in solution in carbon tetrachloride proceeds via the reaction
2N2 O5 (soln)
4NO2 (soln) + O2 (soln)
The reaction is first order and has a rate constant of 4.82 × 10-3 s-1 at 64 °C. The rate law for the
reaction is rate = ________.
A) k[N2 O5 ]2
B) k
[NO2 ]4 [O2 ]
[N2 O5 ]2
C) k[N2 O5 ]
D) k
[N2 O5 ]2
[NO2 ]4 [O2 ]
E) 2k[N2 O5 ]
6
22)
23) As the temperature of a reaction is increased, the rate of the reaction increases because the
________.
A) reactant molecules collide less frequently
B) reactant molecules collide more frequently and with greater energy per collision
C) activation energy is lowered
D) reactant molecules collide less frequently and with greater energy per collision
E) reactant molecules collide more frequently with less energy per collision
23)
24) The rate of a reaction depends on ________.
A) collision frequency
B) collision energy
C) collision orientation
D) all of the above
E) none of the above
24)
25) Which energy difference in the energy profile below corresponds to the activation energy for the
forward reaction?
25)
A) x
B) y
C) x + y
D) x - y
E) y - x
26) In the energy profile of a reaction, the species that exists at the maximum on the curve is called the
________.
A) product
B) activated complex
C) activation energy
D) enthalpy of reaction
E) atomic state
26)
27) In the Arrhenius equation,
27)
k = Ae-Ea/RT
________ is the frequency factor.
A) k
B) A
C) e
D) Ea
28) In general, as temperature goes up, reaction rate ________.
A) goes up if the reaction is exothermic
B) goes up if the reaction is endothermic
C) goes up regardless of whether the reaction is exothermic or endothermic
D) stays the same regardless of whether the reaction is exothermic or endothermic
E) stays the same if the reaction is first order
7
E) R
28)
29) In general, as activation energy increases, reaction rate ________.
A) goes down if the reaction is exothermic
B) goes down if the reaction is endothermic
C) stays the same regardless of whether the reaction is exothermic or endothermic
D) goes down regardless of whether the reaction is exothermic or endothermic
E) none of the above
29)
30) At elevated temperatures, methylisonitrile (CH3 NC) isomerizes to acetonitrile (CH3 CN):
30)
CH3NC (g)
CH3 CN (g)
The dependence of the rate constant on temperature is studied and the graph below is prepared
from the results.
The energy of activation of this reaction is ________ kJ/mol.
A) 160
B) 1.6 × 105
C) 4.4 × 10-7
D) 4.4 × 10-4
E) 1.9 × 104
31) The mechanism for formation of the product X is:
A + B
B + D
C + D
X
31)
(slow)
(fast)
The intermediate reactant in the reaction is ________.
A) A
B) B
C) C
D) D
32) For the elementary reaction
NO3 + CO
E) X
32)
NO2 + CO2
the molecularity of the reaction is ________, and the rate law is rate = ________.
A) 2, k[NO3 ][CO]
B) 4, k[NO3 ][CO][NO2 ][CO2 ]
C) 2, k[NO2 ][CO2]
D) 2, k[NO3 ][CO]/[NO2 ][CO2 ]
E) 4, k[NO2 ][CO2]/[NO3 ][CO]
8
33) A possible mechanism for the overall reaction
is
Br2 (g) + 2NO (g)
NO (g) + Br2 (g)
33)
2NOBr (g)
k1
k-1
NOBr2 (g) + NO (g)
NOBr2 (g)
k2
2NOBr
(fast)
(slow)
The rate law for formation of NOBr based on this mechanism is rate = ________.
A) k1 [NO]1/2
B) k1 [Br2 ]1/2
C) (k2 k1 /k-1 )[NO]2[Br2]
D) (k1 /k-1 )2 [NO]2
E) (k2 k1 /k-1 )[NO][Br2 ]2
34) Which of the following is true?
A) If we know that a reaction is an elementary reaction, then we know its rate law.
B) The rate-determining step of a reaction is the rate of the fastest elementary step of its
mechanism.
C) Since intermediate compounds can be formed, the chemical equations for the elementary
reactions in a multistep mechanism do not always have to add to give the chemical equation
of the overall process.
D) In a reaction mechanism, an intermediate is identical to an activated complex.
E) All of the above statements are true.
34)
35) Of the following, ________ will lower the activation energy for a reaction.
A) increasing the concentrations of reactants
B) raising the temperature of the reaction
C) adding a catalyst for the reaction
D) removing products as the reaction proceeds
E) increasing the pressure
35)
36) The rate law of the overall reaction
36)
A + B
C
is rate = k[A]2 . Which of the following will not increase the rate of the reaction?
A) increasing the concentration of reactant A
B) increasing the concentration of reactant B
C) increasing the temperature of the reaction
D) adding a catalyst for the reaction
E) All of these will increase the rate.
9
37) A catalyst can increase the rate of a reaction ________.
A) by changing the value of the frequency factor (A)
B) by increasing the overall activation energy (Ea ) of the reaction
37)
38) The primary source of the specificity of enzymes is ________.
A) their polarity, which matches that of their specific substrate
B) their delocalized electron cloud
C) their bonded transition metal, which is specific to the target substrate
D) their locations within the cell
E) their shape, which relates to the lock-and-key model
38)
39) ________ are used in automotive catalytic converters.
A) Heterogeneous catalysts
B) Homogeneous catalysts
C) Enzymes
D) Noble gases
E) Nonmetal oxides
39)
40) The enzyme nitrogenase converts ________ into ________.
A) ammonia, urea
B) CO and unburned hydrocarbons, H2O and CO2
40)
C) by lowering the activation energy of the reverse reaction
D) by providing an alternative pathway with a lower activation energy
E) All of these are ways that a catalyst might act to increase the rate of reaction.
C) nitrogen, ammonia
D) nitrogen oxides, N2 and O2
E) nitroglycerine, nitric acid, and glycerine
41) The active site of nitrogenase is a cofactor that contains two transition metals. These transition
metals are ________.
A) Cr and Mg
B) Mn and V
C) Os and Ir
D) Fe and Zn
E) Fe and Mo
41)
42) Nitrogen fixation is a difficult process because ________.
A) there is so little nitrogen in the atmosphere
B) nitrogen exists in the atmosphere primarily as its oxides which are very unreactive
C) nitrogen is very unreactive, largely due to its triple bond
D) of the extreme toxicity of nitrogen
E) of the high polarity of nitrogen molecules preventing them from dissolving in biological
fluids, such as those inside cells
42)
43) Of the following, only ________ is a valid unit for reaction rate.
A) M/s
B) mmol/mL
C) mol/g
D) g/L
43)
10
E) atm/g
44) The reaction shown below is ________, and it is a ________ elementary reaction.
A + B + C ABC
A) termolecular, rare
B) termolecular, common
C) unimolecular, common
D) bimolecular, rare
E) unimolecular, rare
44)
45) Of the units below, ________ are appropriate for a third-order reaction rate constant.
A) M-2 s-1
B) M s-1
C) s-1
D) M-1 s-1
E) mol/L
45)
46) The rate law for a reaction is
46)
rate = k[A][B]
Which one of the following statements is false?
A) The reaction is first order overall.
B) The reaction is first order in A.
C) The reaction is first order in [B].
D) k is the reaction rate constant
E) If [A] is doubled, the reaction rate will increase by a factor of 2.
47) Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction:
2NO2
47)
2NO + O2
In a particular experiment at 300 °C, [NO2 ] drops from 0.0143 to 0.00701 M in 261 s. The rate of
disappearance of NO2 for this period is ________ M/s.
A) 2.79 × 10-5
B) -8.16 × 10-5
C) 5.59 × 10-5
D) 1.40 × 10-5
E) 35,800
48) At elevated temperatures, dinitrogen pentoxide decomposes to nitrogen dioxide and oxygen:
2N2 O5 (g)
48)
4NO2 (g) + O2 (g)
When the rate of formation of O2 is 2.2 × 10-4 M/s, the rate of decomposition of N 2 O5 is
________ M/s.
A) 7.2 × 10-3
B) 3.6 × 10-3
C) 1.8 × 10-3
D) 1.4 × 10-2
E) 0.00090
49) The rate of disappearance of HBr in the gas phase reaction
2HBr (g)
49)
H2 (g) + Br2 (g)
is 0.190 M s-1 at 150 °C. The rate of appearance of Br2 is ________ M s-1 .
A) 2.63
B) 0.095
C) 0.0361
11
D) 0.380
E) 0.436
50) The rate of disappearance of HBr in the gas phase reaction
2HBr (g)
50)
H2 (g) + Br2 (g)
is 0.140 M s-1 at 150 °C. The rate of reaction is ________ M s-1 .
A) 3.57
B) 0.0700
C) 0.0196
D) 0.280
E) 0.0860
51) The combustion of ethylene proceeds by the reaction
C2 H4 (g) + 3O2 (g)
51)
2CO2 (g) + 2H2 O (g)
When the rate of disappearance of O2 is 0.13 M s-1 , the rate of appearance of CO2 is ________
M s-1 .
A) 0.087
B) 0.043
C) 0.39
D) 0.20
E) 0.26
52) The combustion of ethylene proceeds by the reaction
C2 H4 (g) + 3O2 (g)
52)
2CO2 (g) + 2H2 O (g)
When the rate of disappearance of O2 is 0.13 M s-1 , the rate of disappearance of C2 H4 is ________
M s-1 .
A) 0.087
B) 0.043
C) 0.39
D) 0.20
E) 0.26
53) Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction:
2NO2 (g)
53)
2NO (g) + O2 (g)
In a particular experiment at 300 °C, [NO2 ] drops from 0.0100 to 0.00800 M in 100 s. The rate of
appearance of O2 for this period is ________ M/s.
A) 1.0 × 10-5
B) 2.0 × 10-5
C) 4.0 × 10-5
D) 2.0 × 10-3
E) 4.0 × 10-3
54) At elevated temperatures, methylisonitrile (CH3 NC) isomerizes to acetonitrile (CH3 CN):
CH3NC (g)
54)
CH3 CN (g)
At the start of an experiment, there are 0.200 mol of reactant and 0 mol of product in the reaction
vessel. After 25 min, 0.121 mol of reactant (CH3 NC) remain. There are ________ mol of product
(CH3 CN) in the reaction vessel.
A) 0.022
B) 0.121
C) 0.200
D) 0.321
E) 0.079
55) A compound decomposes by a first-order process. If 13% of the compound decomposes in 60
minutes, the half-life of the compound is ________.
A) 299
B) 20
C) 12
D) -18
E) -5
55)
56) In a linear graphical representation of a zero-order reaction, what value is represented by the
y-intercept of the line drawn from plotting [A] vs. time?
A) [A]0
B) ln[A]0
C) 1/[A]0
D) [A]0 2
E) [A]/k
56)
12
57) The rate constant for a particular zero-order reaction is 0.075 M s-1 . If the initial concentration of
reactant is 0.537 M it takes ________ s for the concentration to decrease to 0.100 M.
A) 5.8
B) -5.8
C) -0.047
D) 7.2
E) 0.040
57)
58) The reaction A
58)
Time (s)
0.0
10.0
20.0
B is first order in [A]. Consider the following data.
[A] (M)
2.7
0.68
0.17
The rate constant for this reaction is ________ s-1 .
A) 0.014
B) 0.030
59) The reaction A
Time (s)
0.0
10.0
20.0
C) 0.013
D) 3.0
E) 3.1 × 10-3
59)
B is first order in [A]. Consider the following data.
[A] (M)
3.0
0.75
0.19
The half-life of this reaction is ________ s.
A) 5.0
B) 0.97
C) 7.1
D) 3.0
E) 0.14
60) The rate constant of a first-order process that has a half-life of 462 s is ________ s-1 .
A) 1.50 × 10-3
60)
B) 3.20 × 102
C) 6.67 × 102
D) -1.08 × 10-3
E) 2.16 × 10-3
61) The following reaction is second order in [A] and the rate constant is 0.039 M-1 s-1 :
A
61)
B
The concentration of A was 0.26 M at 28 s. The initial concentration of A was ________ M.
A) 0.36
B) 2.8
C) -1.2
D) -1.5
E) -0.83
62) A compound decomposes by a first-order process. If 17.0% of the compound decomposes in 30
minutes, the half-life of the compound is ________.
A) 112 minutes
B) 12 minutes
C) 8 minutes
D) 223 minutes
E) 56 minutes
13
62)
63) The isomerization of methylisonitrile to acetonitrile
CH3NC (g)
63)
CH3 CN (g)
is first order in CH3 NC. The rate constant for the reaction is 9.45 × 10-5 s-1 at 478 K. The half-life
of the reaction when the initial [CH3 NC] is 0.030 M is ________ s.
A) 1.06 × 104
B) 5.29 × 103
C) 3.53 × 105
D) 7.33 × 103
E) 1.36 × 10-4
64) The elementary reaction
2NO2 (g)
64)
2NO (g) + O2 (g)
is second order in NO2 and the rate constant at 660 K is 5.23 M-1 s-1 . The reaction half-life at this
temperature when [NO2 ]0 = 0.45 M is ________ s.
A) 2.4
B) 7.6
C) 0.19
D) 0.13
E) 0.42
65) The isomerization of methylisonitrile to acetonitrile
CH3 NC (g)
65)
CH3 CN (g)
is first order in CH3 NC. The half-life of the reaction is 2.70 × 104 s at 463 K. The rate constant when
the initial [CH3 NC] is 0.030 M is ________ s-1 .
A) 3.90 × 104
B) 1.23 × 10-3
C) 2.57 × 10-5
D) 8.10 × 102
E) 1.25 × 107
66) The decomposition of N2 O5 in solution in carbon tetrachloride proceeds via the reaction
2N2 O5 (soln)
4NO2 (soln) + O2 (soln)
The reaction is first order and has a rate constant of 4.82 × 10-3 s-1 at 64 °C. If the reaction is
initiated with 0.072 mol in a 1.00-L vessel, how many moles remain after 151 s?
A) 0.067
B) 0.074
C) 0.035
14
D) 9.6
E) 1.6 × 103
66)
67) SO2 Cl2 decomposes in the gas phase by the reaction
SO2 Cl2 (g)
67)
SO2 (g) + Cl2 (g)
The reaction is first order in SO2 Cl2 and the rate constant is 3.0 × 10-6 s-1 at 600 K. A vessel is
charged with 3.6 atm of SO2 Cl2 at 600 K. The partial pressure of SO2 Cl2 at 3.0 × 105 s is ________
atm.
A) 0.85
B) 3.2
C) 1.5
D) 0.19
E) 9.3 × 104
68) The rate constant for a particular second-order reaction is 0.47 M-1s-1 . If the initial concentration
of reactant is 0.25 mol/L, it takes ________ s for the concentration to decrease to 0.20 mol/L.
A) 2.1
B) 1.4
C) 1.0
D) 0.47
E) 0.20
68)
69) The reaction
69)
2NOBr (g)
2 NO (g) + Br2 (g)
is a second-order reaction with a rate constant of 0.80 M-1 s-1 at 11 °C. If the initial concentration of
NOBr is 0.0440 M, the concentration of NOBr after 6.0 seconds is ________.
A) 0.0276 M
B) 0.0324 M
C) 0.0363 M
D) 0.0348 M
E) 0.0402 M
70) A first-order reaction has a rate constant of 0.33 min-1 . It takes ________ min for the reactant
concentration to decrease from 0.13 M to 0.066 M.
A) 0.085
B) 0.13
C) 0.89
D) 2.4
E) 2.1
70)
71) The initial concentration of reactant in a first-order reaction is 0.27 M. The rate constant for the
reaction is 0.75 s-1 . What is the concentration (mol/L) of reactant after 1.8 s?
71)
72) The rate constant for a second-order reaction is 0.13 M-1 s-1 . If the initial concentration of reactant
is 0.26 mol/L, it takes ________ s for the concentration to decrease to 0.07 mol/L.
A) 0.017
B) 1.4
C) 14
D) 80.
E) 10.
72)
73) At elevated temperatures, nitrogen dioxide decomposes to nitrogen oxide and oxygen:
73)
A) 6.0
NO2 (g)
B) 1.7
NO (g) +
C) 0.070
D) 0.012
E) 1.0
1
O (g)
2 2
The reaction is second order in NO2 with a rate constant of 0.543 M-1 s-1 at 300 °C. If the initial
[NO2 ] is 0.260 M, it will take ________ s for the concentration to drop to 0.075 M.
A) 3.34
B) 0.0880
C) 2.29
D) 0.299
15
E) 17.5
74) A particular first-order reaction has a rate constant of 1.35 × 102 s-1 at 25.0 °C. What is the
magnitude of k at 65.0°C if Ea = 55.5 kJ/mol?
74)
A) 1.92 × 103
B) 1.95 × 104
C) 358
D) 3.48 × 1073
E) 1.35 × 102
75) A particular first-order reaction has a rate constant of 1.35 × 102 s-1 at 25.0 °C. What is the
magnitude of k at 75.0 °C if Ea = 55.3 kJ/mol?
A) 2.24 × 104
B) 3.34 × 103
D) 2.49 × 106
C) 433
E) 1.35 × 102
76) Consider the following reaction:
3A
75)
76)
2B
The average rate of appearance of B is given by [B]/ t. Comparing the rate of appearance of B and
the rate of disappearance of A, we get [B]/ t = ________ × (- [A]/ t).
A) -2/3
B) +2/3
C) -3/2
D) +1
E) +3/2
77) Which substance in the reaction below either appears or disappears the fastest?
4NH3 + 7O2
77)
4NO2 + 6H2 O
A) NH3
B) O2
C) NO2
D) H2 O
E) The rates of appearance/disappearance are the same for all of these.
78) Consider the following reaction:
A
78)
2C
The average rate of appearance of C is given by [C]/ t. Comparing the rate of appearance of C
and the rate of disappearance of A, we get [C]/ t = ________ × (- [A]/ t).
A) +2
B) -1
C) +1
D) +1/2
E) -1/2
16
A flask is charged with 0.124 mol of A and allowed to react to form B according to the reaction A(g) B(g). The following data are
obtained for [A] as the reaction proceeds:
Time (s)
Moles of A
0.00
0.124
10.0
0.110
20.0
0.088
30.0
0.073
40.0
0.054
79) The average rate of disappearance of A between 10 s and 20 s is ________ mol/s.
A) 2.2 × 10-3
79)
B) 1.1 × 10-3
C) 4.4 × 10-3
D) 454
E) 9.90 × 10-3
80) The average rate of disappearance of A between 20 s and 40 s is ________ mol/s.
A) 8.5 × 10-4
B) 1.7 × 10-3
C) 590
D) 7.1 × 10-3
80)
E) 1.4 × 10-3
81) The average rate of appearance of B between 20 s and 30 s is ________ mol/s.
A) +1.5 × 10-3
81)
B) +5.0 × 10-4
C) -1.5 × 10-3
D) +7.3 × 10-3
E) -7.3 × 10-3
82) The average rate disappearance of A between 20 s and 30 s is ________ mol/s.
A) 5.0 × 10-4
82)
B) 1.6 × 10-2
C) 1.5 × 10-3
D) 670
E) 0.15
83) How many moles of B are present at 10 s?
A) 0.011
B) 0.220
84) How many moles of B are present at 30 s?
A) 2.4 × 10-3
B) 0.15
83)
C) 0.110
D) 0.014
C) 0.073
D) 1.7 × 10-3
E) 1.4 × 10-3
84)
17
E) 0.051
The peroxydisulfate ion (S2 O8 2- ) reacts with the iodide ion in aqueous solution via the reaction:
S2 O8 2- (aq) + 3I-
2SO4 (aq) + I3 - (aq)
An aqueous solution containing 0.050 M of S2 O8 2- ion and 0.072 M of I- is prepared, and the progress of the reaction followed by
measuring [I-]. The data obtained is given in the table below.
Time (s)
[I- ] (M)
0.000
400.0
800.0
1200.0
1600.0
0.072
0.057
0.046
0.037
0.029
85) The average rate of disappearance of I- between 400.0 s and 800.0 s is ________ M/s.
A) 2.8 × 10-5
B) 1.4 × 10-5
C) 5.8 × 10-5
D) 3.6 × 104
E) 2.6 × 10-4
85)
86) The average rate of disappearance of I- in the initial 400.0 s is ________ M/s.
A) 6.00
B) 3.8 × 10-5
C) 1.4 × 10-4
D) 2.7 × 104
86)
E) 3.2 × 10-4
87) The average rate of disappearance of I- between 1200.0 s and 1600.0 s is ________ M/s.
A) 1.8 × 10-5
B) 1.2 × 10-5
C) 2.0 × 10-5
D) 5.0 × 104
E) 1.6 × 10-4
87)
88) The concentration of S2 O8 2- remaining at 400 s is ________ M.
88)
A) +0.015
B) +0.035
C) -0.007
D) +0.045
E) +0.057
89) The concentration of S2 O8 2- remaining at 800 s is ________ M.
89)
A) 0.046
B) 0.076
C) 4.00 × 10-3
D) 0.015
E) 0.041
90) The concentration of S2 O8 2- remaining at 1600 s is ________ M.
A) 0.036
B) 0.014
C) 0.043
90)
D) 0.064
E) 0.029
91) At elevated temperatures, dinitrogen pentoxide decomposes to nitrogen dioxide and oxygen:
2N2 O5 (g)
4NO2 (g) + O2 (g)
When the rate of formation of NO2 is 5.5 × 10-4 M/s, the rate of decomposition of N2 O5 is ________
M/s.
A) 2.2 × 10-3
B) 1.4 × 10-4
C) 10.1 × 10-4
D) 2.8 × 10-4
E) 5.5 × 10-4
18
91)
92) At elevated temperatures, methylisonitrile (CH3 NC) isomerizes to acetonitrile (CH3 CN):
CH3 NC (g)
92)
CH3 CN (g)
At the start of the experiment, there are 0.200 mol of reactant (CH3 NC) and 0 mol of product
(CH3 CN) in the reaction vessel. After 25 min of reaction, 0.108 mol of reactant (CH3 NC) remain.
The average rate of decomposition of methyl isonitrile, CH3 NC, in this 25 min period is ________
mol/min.
A) 3.7 × 10-3
B) 0.092
D) 4.3 × 10-3
C) 2.3
E) 0.54
93) A reaction was found to be second order in carbon monoxide concentration. The rate of the reaction
________ if the [CO] is doubled, with everything else kept the same.
A) doubles
B) remains unchanged
C) triples
D) increases by a factor of 4
E) is reduced by a factor of 2
93)
94) If the rate law for the reaction
94)
2A + 3B
products
is first order in A and second order in B, then the rate law is rate = ________.
A) k[A][B]
B) k[A]2 [B]3
C) k[A][B]2
D) k[A]2 [B]
E) k[A]2 [B]2
95) If the rate law for the reaction
2A + 3B
95)
products
is second order in A and first order in B, then the rate law is rate = ________.
A) k[A][B]
B) k[A]2 [B]3
C) k[A][B]2
D) k[A]2 [B]
E) k[A]2 [B]2
96) The overall order of a reaction is 1. The units of the rate constant for the reaction are ________.
A) M/s
B) M-1 s-1
C) 1/s
D) 1/M
E) s/M2
96)
97) The overall order of a reaction is 2. The units of the rate constant for the reaction are ________.
A) M/s
B) M-1 s-1
C) 1/s
D) 1/M
E) s/M2
97)
98) The kinetics of the reaction below were studied and it was determined that the reaction rate
increased by a factor of 9 when the concentration of B was tripled. The reaction is ________ order
in B.
98)
A + B
A) zero
P
B) first
C) second
19
D) third
E) one-half
99) The kinetics of the reaction below were studied and it was determined that the reaction rate did not
change when the concentration of B was tripled. The reaction is ________ order in B.
A + B
A) zero
99)
P
B) first
C) second
D) third
E) one-half
100) A reaction was found to be third order in A. Increasing the concentration of A by a factor of 3 will
cause the reaction rate to ________.
A) remain constant
B) increase by a factor of 27
C) increase by a factor of 9
D) triple
E) decrease by a factor of the cube root of 3
100)
101) A reaction was found to be zero order in A. Increasing the concentration of A by a factor of 3 will
cause the reaction rate to ________.
A) remain constant
B) increase by a factor of 27
C) increase by a factor of 9
D) triple
E) decrease by a factor of the cube root of 3
101)
The data in the table below were obtained for the reaction:
A + B
P
Experiment
Initial Rate
Number
[A] (M) [B] (M)
(M/s)
1
0.273
0.763
2.83
2
0.273
1.526
2.83
3
0.819
0.763
25.47
102) The order of the reaction in A is ________.
A) 1
B) 2
C) 3
D) 4
E) 0
103) The order of the reaction in B is ________.
A) 1
B) 2
D) 4
E) 0
C) 3
104) The overall order of the reaction is ________.
A) 1
B) 2
C) 3
D) 4
20
E) 0
102)
103)
104)
105) The following reaction occurs in aqueous solution:
NH4+ (aq) + NO2 -
105)
N2 (g) + 2H2 O (l)
The data below is obtained at 25 °C.
[NH4 +] (M)
[NO2 - ] (M)
Initial rate (M/s)
0.0100
0.0200
0.200
0.200
3.2 × 10-3
6.4 × 10-3
The order of the reaction in NH4 + is ________.
A) -2
B) -1
C) +2
D) +1
106) For a first-order reaction, a plot of ________ versus ________ is linear.
1
1
,t
A) ln [A]t,
B) ln [A]t, t
C)
D) [A]t, t
[A]t
t
E) 0
1
E) t,
[A]t
106)
107) The half-life of a first-order reaction is 13 min. If the initial concentration of reactant is 0.085 M, it
takes ________ min for it to decrease to 0.055 M.
A) 8.2
B) 11
C) 3.6
D) 0.048
E) 8.4
107)
108) The half-life of a first-order reaction is 13 min. If the initial concentration of reactant is 0.13 M, it
takes ________ min for it to decrease to 0.085 M.
A) 12
B) 10.
C) 8.0
D) 11
E) 7.0
108)
109) The graph shown below depicts the relationship between concentration and time for the following
chemical reaction.
109)
The slope of this line is equal to ________.
A) k
B) -1/k
C) ln [A]o
D) -k
E) 1/k
110) The reaction below is first order in [H2O2 ]:
2H2 O2 (l)
110)
2H2 O (l) + O2 (g)
A solution originally at 0.600 M H2 O2 is found to be 0.075 M after 54 min. The half-life for this
reaction is ________ min.
A) 6.8
B) 18
C) 14
D) 28
21
E) 54
111) A second-order reaction has a half-life of 18 s when the initial concentration of reactant is 0.71 M.
The rate constant for this reaction is ________ M-1 s-1 .
A) 7.8 × 10-2
B) 3.8 × 10-2
C) 2.0 × 10-2
D) 1.3
E) 18
112) A second-order reaction has a half-life of 12 s when the initial concentration of reactant is 0.98 M.
The rate constant for this reaction is ________ M-1 s-1 .
A) 12
B) 2.0 × 10-2
C) 8.5 × 10-2
D) 4.3 × 10-2
111)
112)
E) 4.3
113) At equilibrium, ________.
A) all chemical reactions have ceased
B) the rates of the forward and reverse reactions are equal
C) the rate constants of the forward and reverse reactions are equal
D) the value of the equilibrium constant is 1
E) the limiting reagent has been consumed
113)
114) What role did Karl Bosch play in development of the Haber-Bosch process?
A) He discovered the reaction conditions necessary for formation of ammonia.
B) He originally isolated ammonia from camel dung and found a method for purifying it.
C) Haber was working in his lab with his instructor at the time he worked out the process.
D) He developed the equipment necessary for industrial production of ammonia.
E) He was the German industrialist who financed the research done by Haber.
114)
115) In what year was Fritz Haber awarded the Nobel Prize in chemistry for his development of a
process for synthesizing ammonia directly from nitrogen and hydrogen?
A) 1954
B) 1933
C) 1918
D) 1900
E) 1912
115)
116) Which one of the following is true concerning the Haber process?
A) It is a process used for shifting equilibrium positions to the right for more economical
chemical synthesis of a variety of substances.
B) It is a process used for the synthesis of ammonia.
C) It is another way of stating Le Châtelier's principle.
D) It is an industrial synthesis of sodium chloride that was discovered by Karl Haber.
E) It is a process for the synthesis of elemental chlorine.
116)
117) Which one of the following will change the value of an equilibrium constant?
A) changing temperature
B) adding other substances that do not react with any of the species involved in the equilibrium
C) varying the initial concentrations of reactants
D) varying the initial concentrations of products
E) changing the volume of the reaction vessel
117)
22
118) Which of the following expressions is the correct equilibrium-constant expression for the
equilibrium between dinitrogen tetroxide and nitrogen dioxide?
N2 O4 (g)
A)
[NO2 ]
[N2 O4 ]
B)
[NO2 ]2
[N2 O4 ]
C)
[NO2 ]
[N2 O4 ]2
118)
2NO2 (g)
D) [NO2 ][N2 O4]
E) [NO2 ]2 [N2 O4 ]
119) Which of the following expressions is the correct equilibrium-constant expression for the following
reaction?
CO2 (g) + 2H2 (g)
A)
B)
CH3 OH (g)
[CH3 OH]
[CO2 ]
[CH3 OH]
[CO2 ][H2 ]
C)
[CO2 ][H2 ]2
[CH3 OH
D)
[CO2 ][H2 ]
[CH3 OH
E)
119)
[CH3 OH]
[CO2 ][H2 ]2
120) The equilibrium-constant expression depends on the ________ of the reaction.
A) stoichiometry
B) mechanism
C) stoichiometry and mechanism
D) the quantities of reactants and products initially present
E) temperature
120)
121) The equilibrium constant for reaction 1 is K. The equilibrium constant for reaction 2 is ________.
121)
(1) SO2 (g) + (1/2) O2 (g)
(2) 2SO3 (g)
A) K2
SO3 (g)
2SO2 (g) + O2 (g)
B) 2K
C) 1/2K
23
D) 1/K2
E) -K2
122) The equilibrium expression for Kp for the reaction below is ________.
2O3 (g)
A)
3O2 (g)
3PO
2
B)
2PO
3
2PO
3
C)
3PO
2
3PO
3
2PO
2
D)
PO 2
3
PO
123) The equilibrium expression for Kp for the reaction below is ________.
N2 (g) + O2 (g)
A)
B)
C)
D)
122)
2
2
E)
PO 3
2
PO 2
3
123)
2NO (g)
(2PO2) (2PN2)
2PNO
(PO2) (PN2)
2PNO
(PO2) (PN2)
PNO
(2PNO)
(2PN2)(2PO2)
E) none of the above
124) The Keq for the equilibrium below is 7.52 × 10-2 at 480.0 °C.
2Cl2 (g) + 2H2 O (g)
4HCl (g) + O2 (g)
What is the value of Keq at this temperature for the following reaction?
2HCl (g) +
1
O (g)
2 2
Cl2 (g) + H2 O (g)
A) 13.3
B) 3.65
C) -0.0376
D) 5.66 × 10-3
E) 0.274
24
124)
125) The Keq for the equilibrium below is 5.4 × 1013 at 480.0 °C.
2NO (g) + O2 (g)
125)
2NO2 (g)
What is the value of Keq at this temperature for the following reaction?
NO2 (g)
NO (g) + 1/2 O2 (g)
A) 5.4 × 10-13
B) 5.4 × 1013
C) 1.4 × 10-7
D) 5.66 × 10-3
E) none of the above
126) The Keq for the equilibrium below is 0.112 at 700.0 °C.
1
SO2 (g) + O2 (g)
2
126)
SO3 (g)
What is the value of Keq at this temperature for the following reaction?
SO3 (g)
SO2 (g) +
A) 0.224
1
O (g)
2 2
B) 0.0125
C) 0.112
D) 8.93
E) -0.112
127) The Keq for the equilibrium below is 0.112 at 700.0 °C.
1
SO2 (g) + O2 (g)
2
127)
SO3 (g)
What is the value of Keq at this temperature for the following reaction?
2SO3 (g)
A) 79.7
2SO2 (g) + O2 (g)
B) 2.99
C) 17.86
D) 4.46
E) 8.93
128) Given the following reaction at equilibrium, if Kc = 1.90 × 1019 at 25.0 °C, Kp = ________.
H2 (g) + Br2 (g)
2 HBr (g)
A) 5.26 × 10-20
B) 1.56 × 104
C) 6.44 × 105
D) 1.90 × 1019
E) none of the above
25
128)
129) Which of the following expressions is the correct equilibrium-constant expression for the reaction
below?
2SO2 (g) + O2 (g)
129)
2SO3 (g)
A) [SO3 ] / [SO2 ][O2 ]
B) [SO2 ] / [SO3 ]
C) [SO3 ]2 / [SO2 ]2 [O2]
D) [SO3 ]2 / [SO2 ]2 [O2]2
E) [SO3 ] / [SO2 ][O2 ]2
130) Which of the following expressions is the correct equilibrium-constant expression for the reaction
below?
(NH4 )2 Se (s)
130)
2NH3 (g) + H2 Se (g)
A) [NH3 ][H2 Se] / [(NH4 )2 Se]
B) [(NH4 )2 Se] / [NH3 ]2 [H2 Se]
C) 1 / [(NH4 )2 Se]
D) [NH3 ]2 [H2 Se]
E) [NH3 ]2 [H2 Se] / [(NH4 )2 Se]
131) Which of the following expressions is the correct equilibrium-constant expression for the reaction
below?
131)
H+ (aq) + HCO3 - (aq)
CO2 (s) + H2 O (l)
A) [H+ ][HCO3 -] / [CO2 ]
B) [CO2 ] / [H+ ][HCO3 - ]
C) [H+ ][HCO3 -] / [CO2 ][H2 O]
D) [CO2 ][H2 O] / [H+ ][HCO3 - ]
E) [H+ ][HCO3 -]
132) Which of the following expressions is the correct equilibrium-constant expression for the reaction
below?
HF (aq) + H2 O (l)
H3 O+ (aq) + F- (aq)
A) [HF][H2 O] / [H3 O+ ][F- ]
B) 1 / [HF]
C) [H3 O+ ][F- ] / [HF][H2 O]
D) [H3 O+ ][F- ] / [HF]
E) [F-] / [HF]
26
132)
133) The expression for Kp for the reaction below is ________.
4CuO (s) + CH4 (g)
A)
B)
C)
D)
E)
133)
CO2 (g) + 4Cu (s) + 2H2 O (g)
PCH4
PCO2 PH22
[Cu] PCO2 PH2O 2
[CuO]4 PCH4
PCO2 PH2O 2
PCH4
PCO2 PH2O 2
PCuO
PCH4
PH2O 2 PCO2
134) The equilibrium-constant expression for the reaction
Ti (s) + 2Cl2 (g)
134)
TiCl4 (l)
is given by
[TiCl4 (l)]
A)
[Ti (s)] [Cl2 (g)]
B)
C)
[Ti (s)] [Cl2 (g)]2
[TiCl4 (l)]
[TiCl4 (l)]
[Cl2 (g)]2
D) [Cl2 (g)]-2
[TiCl4 (l)]
E)
[Ti (s)] [Cl2 ( g)]2
135) The equilibrium constant for the gas phase reaction
N2 (g) + 3H2 (g)
2NH3 (g)
is Keq = 4.34 × 10-3 at 300 °C. At equilibrium, ________.
A) products predominate
B) reactants predominate
C) roughly equal amounts of products and reactants are present
D) only products are present
E) only reactants are present
27
135)
136) The equilibrium constant for the gas phase reaction
2SO2 (g) + O2 (g)
136)
2SO3 (g)
is Keq = 2.80 × 102 at 999 K. At equilibrium, ________.
A) products predominate
B) reactants predominate
C) roughly equal amounts of products and reactants are present
D) only products are present
E) only reactants are present
137) The equilibrium constant for the gas phase reaction
2NH3 (g)
137)
N2 (g) + 3H2 (g)
is Keq = 230 at 300 °C. At equilibrium, ________.
A) products predominate
B) reactants predominate
C) roughly equal amounts of products and reactants are present
D) only products are present
E) only reactants are present
138) The equilibrium constant for the gas phase reaction
N2 (g) + O2 (g)
138)
2NO (g)
is Keq = 4.20 × 10-31 at 30 °C. At equilibrium, ________.
A) products predominate
B) reactants predominate
C) roughly equal amounts of products and reactants are present
D) only products are present
E) only reactants are present
139) Consider the following equilibrium.
2 SO2 (g) + O2 (g)
139)
2 SO3 (g)
The equilibrium cannot be established when ________ is/are placed in a 1.0-L container.
A) 0.25 mol SO2 (g) and 0.25 mol O2 (g)
B) 0.75 mol SO2 (g)
C) 0.25 mol of SO2 (g) and 0.25 mol of SO3 (g)
D) 0.50 mol O2 (g) and 0.50 mol SO3 (g)
E) 1.0 mol SO3 (g)
28
140) At 400 K, the equilibrium constant for the reaction
Br2 (g) + Cl2 (g)
140)
2BrCl (g)
is Kp = 7.0. A closed vessel at 400 K is charged with 1.00 atm of Br2 (g), 1.00 atm of Cl2 (g), and 2.00
atm of BrCl (g). Use Q to determine which of the statements below is true.
A) The equilibrium partial pressures of Br2 , Cl2 , and BrCl will be the same as the initial values.
B) The equilibrium partial pressure of Br2 will be greater than 1.00 atm.
C) At equilibrium, the total pressure in the vessel will be less than the initial total pressure.
D) The equilibrium partial pressure of BrCl (g) will be greater than 2.00 atm.
E) The reaction will go to completion since there are equal amounts of Br2 and Cl2 .
141) Which of the following statements is true?
A) Q does not change with temperature.
B) Keq does not change with temperature, whereas Q is temperature dependent.
141)
142) How is the reaction quotient used to determine whether a system is at equilibrium?
A) The reaction quotient must be satisfied for equilibrium to be achieved.
B) At equilibrium, the reaction quotient is undefined.
C) The reaction is at equilibrium when Q < Keq.
142)
C) K does not depend on the concentrations or partial pressures of reaction components.
D) Q does not depend on the concentrations or partial pressures of reaction components.
E) Q is the same as Keq when a reaction is at equilibrium.
D) The reaction is at equilibrium when Q > Keq.
E) The reaction is at equilibrium when Q = Keq.
143) Of the following equilibria, only ________ will shift to the left in response to a decrease in volume.
2 HCl (g)
A) H2 (g) + Cl2 (g)
143)
B) 2 SO3 (g)
2 SO2 (g) + O2 (g)
2 NH3 (g)
C) N2 (g) + 3H2 (g)
2 Fe2 O3 (s)
D) 4 Fe (s) + 3 O2 (g)
E) 2HI (g)
H2 (g) + I2 (g)
144) Of the following equilibria, only ________ will shift to the right in response to a decrease in
volume.
2 HCl (g)
A) H2 (g) + Cl2 (g)
B) 2 SO3 (g)
2 SO2 (g) + O2 (g)
2NH3 (g)
C) N2 (g) + 3H2 (g)
4 Fe (s) + 3O2 (g)
D) 2 Fe2 O3 (s)
E) 2HI (g)
H2 (g) + I2 (g)
29
144)
145) In which of the following reactions would increasing pressure at constant temperature not change
the concentrations of reactants and products, based on Le Châtelier's principle?
2NH3 (g)
A) N2 (g) + 3H2 (g)
B) N2 O4 (g)
2NO2 (g)
C) N2 (g) + 2O2 (g)
D) 2N2 (g) + O2 (g)
E) N2 (g) + O2 (g)
2NO2 (g)
2N2O (g)
2NO (g)
146) In which of the following reactions would increasing pressure at constant temperature change the
concentrations of reactants and products, based on Le Châteliers principle?
2NH3 (g)
A) N2 (g) + 3H2 (g)
B) N2 O4 (g)
2NO2 (g)
2N2O (g)
147) Consider the following reaction at equilibrium:
2NH3 (g)
146)
2NO2 (g)
C) N2 (g) + 2O2 (g)
D) 2N2 (g) + O2 (g)
E) all of the above
145)
147)
N2 (g) + 3H2 (g)
Le Châtelier's principle predicts that the moles of H2 in the reaction container will increase with
________.
A) some removal of NH3 from the reaction vessel (V and T constant)
B) a decrease in the total pressure (T constant)
C) addition of some N2 to the reaction vessel (V and T constant)
D) a decrease in the total volume of the reaction vessel (T constant)
E) an increase in total pressure by the addition of helium gas (V and T constant)
148) Consider the following reaction at equilibrium:
2CO2 (g)
2CO (g) + O2 (g)
148)
H° = -514 kJ
Le Châtelier's principle predicts that an increase in temperature will ________.
A) increase the partial pressure of O2 (g)
B) decrease the partial pressure of CO2 (g)
C) decrease the value of the equilibrium constant
D) increase the value of the equilibrium constant
E) increase the partial pressure of CO
30
149) Consider the following reaction at equilibrium.
2CO2 (g)
2CO (g) + O2 (g)
149)
H° = -514 kJ
Le Châtelier's principle predicts that the equilibrium partial pressure of CO (g) can be maximized
by carrying out the reaction ________.
A) at high temperature and high pressure
B) at high temperature and low pressure
C) at low temperature and low pressure
D) at low temperature and high pressure
E) in the presence of solid carbon
150) The effect of a catalyst on an equilibrium is to ________.
A) increase the rate of the forward reaction only
B) increase the equilibrium constant so that products are favored
C) slow the reverse reaction only
D) increase the rate at which equilibrium is achieved without changing the composition of the
equilibrium mixture
E) shift the equilibrium to the right
150)
151) The value of Keq for the equilibrium
151)
H2 (g) + I2 (g)
2HI (g)
is 794 at 25 °C. What is the value of Keq for the equilibrium below?
1/2 H2 (g) + 1/2 I2 (g)
A) 397
HI (g)
B) 0.035
C) 28
D) 1588
E) 0.0013
152) The value of Keq for the equilibrium
H2 (g) + I2 (g)
152)
2HI (g)
is 794 at 25 °C. At this temperature, what is the value of Keq for the equilibrium below?
HI (g)
A) 1588
1/2 H2 (g) + 1/2 I2 (g)
B) 28
C) 397
D) 0.035
31
E) 0.0013
153) The value of Keq for the equilibrium
H2 (g) + I2 (g)
153)
2HI (g)
is 54.0 at 427 °C. What is the value of Keq for the equilibrium below?
HI (g)
1/2 H2 (g) + 1/2 I2 (g)
A) 27
B) 7.35
C) 0.136
D) 2.92 × 103
E) 3.43 × 10-4
154) The value of Keq for the equilibrium
CO2 (g) + 2H2 (g)
154)
CH3 OH (g)
is 14.5 at 483 °C. What is the value of Keq for the equilibrium below?
1/2 CO2 + H2 (g)
1/2 CH3 OH (g)
A) 7.30
B) 7.35
C) 0.136
D) 3.81
E) 6.90 × 10-2
155) The value of Keq for the equilibrium
N2 (g) + O2 (g)
155)
2 NO (g)
is 4.2 × 10-31 at 27 °C. What is the value of Keq for the equilibrium below?
4 NO (g)
2 N2 (g) + 2 O2 (g)
A) 5.7 × 1060
B) 8.4 × 10-31
C) 4.2 × 1031
D) 8.4 × 1031
E) none of the above
32
156) Consider the following chemical reaction:
CO (g) + 2H2 (g)
156)
CH3 OH(g)
At equilibrium in a particular experiment, the concentrations of CO and H2 were 0.15 M and
0.36 M,respectively. What is the equilibrium concentration of CH3 OH? The value of Keq for this
reaction is 14.5 at the temperature of the experiment.
A) 14.5
B) 7.61 × 10-3
C) 2.82 × 10-1
D) 3.72 × 10-3
E) 1.34 × 10-3
157) A reaction vessel is charged with hydrogen iodide, which partially decomposes to molecular
hydrogen and iodine:
2HI (g)
157)
H2 (g) + I2 (g)
When the system comes to equilibrium at 425 °C, PHI = 0.708 atm, and PH = PI = 0.0960 atm. The
2
value of Kp at this temperature is ________.
2
A) 6.80 × 10-2
B) 1.30 × 10-2
C) 54.3
D) 1.84 × 10-2
E) Kp cannot be calculated for this gas reaction when the volume of the reaction vessel is not
given.
158) Acetic acid is a weak acid that dissociates into the acetate ion and a proton in aqueous solution:
158)
C2 H3O2 - (aq) + H+ (aq)
HC2 H3 O2 (aq)
At equilibrium at 25 °C a 0.100 M solution of acetic acid has the following concentrations:
[HC2 H3 O2 ] = 0.0990 M, [C2H3 O2 - ] = 1.33 × 10-3 M, and [H+ ] = 1.33 × 10-3 M. The equilibrium
constant, Keq, for the ionization of acetic acid at 25°C is ________.
A) 5.71 × 104
B) 0.100
C) 1.75 × 10-7
D) 1.79 × 10-5
E) 5.71 × 106
159) Dinitrogentetraoxide partially decomposes according to the following equilibrium:
N2 O4 (g)
159)
2 NO2 (g)
A 1.00-L flask is charged with 0.0400 mol ofN2 O4. At equilibrium at 373 K, 0.0055 mol of N2 O4
remains. Keq for this reaction is ________.
A) 2.2 × 10-4
B) 13
C) 0.22
D) 0.022
33
E) 0.87
160) Given the following reaction:
160)
CO (g) + 2 H2 (g)
CH3 OH (g)
In an experiment, 0.42 mol of CO and 0.42 mol of H2 were placed in a 1.00-L reaction vessel. At
equilibrium, there were 0.29 mol of CO remaining. Keq at the temperature of the experiment is
________.
A) 2.80
B) 0.357
C) 14.5
D) 17.5
E) none of the above
161) A sealed 1.0 L flask is charged with 0.500 mol of I2 and 0.500 mol of Br2 . An equilibrium reaction
161)
ensues:
I2 (g) + Br2 (g)
2IBr (g)
When the container contents achieve equilibrium, the flask contains 0.84 mol of IBr. The value of
Keq is ________.
A) 11
B) 4.0
C) 110
D) 6.1
E) 2.8
162) The equilibrium constant (Kp) for the interconversion of PCl5 and PCl3 is 0.0121:
PCl5 (g)
162)
PCl3 (g) + Cl2 (g)
A vessel is charged with PCl5 giving an initial pressure of 0.123 atm. At equilibrium, the partial
pressure of PCl3 is ________ atm.
A) 0.0782
B) 0.0455
C) 0.0908
D) 0.0330
E) 0.123
163) At 200 °C, the equilibrium constant (Kp) for the reaction below is 2.40 × 103 .
2NO (g)
N2 (g) + O2 (g)
A closed vessel is charged with 36.1 atm of NO. At equilibrium, the partial pressure of O2 is
________ atm.
A) 294
B) 35.7
C) 17.9
D) 6.00
E) 1.50 × 10-2
34
163)
164) Which of the following expressions is the correct equilibrium-constant expression for the
equilibrium between dinitrogen tetroxide and nitrogen dioxide?
5N2 O4(g)
164)
10NO2 (g)
A) [NO2 ]10/[N2O4 ]5
B) [N2 O4 ]10/[NO2 ]5
C) [NO2 ]5 /[N2 O4 ]10
D) [NO2 ]5 /[N2 O4 ]5
E) [N2 O4 ]5 /[NO2 ]5
165) Given the following reaction at equilibrium, if Kc = 5.84 x 105 at 230.0 °C, Kp = ________.
2NO (g) + O2 (g)
165)
2NO2 (g)
A) 3.67 × 10-2
B) 1.41 × 104
C) 6.44 × 105
D) 2.40 × 106
E) 2.41 × 107
166) Given the following reaction at equilibrium at 450.0 °C:
CaCO3 (s)
166)
CaO (s) + CO2 (g)
If pCO2 = 0.0155 atm, Kc = ________.
A) 155
B) 0.0821
C) 0.920
D) 2.61 × 10-4
E) 9.20
167) Given the following reaction at equilibrium, if Kp = 1.10 at 250.0 °C, Kc = ________.
PCl5 (g)
PCl3 (g) + Cl2 (g)
A) 3.90 × 10-6
B) 2.56 × 10-2
C) 1.10
D) 42.9
E) 47.2
35
167)
168) Given the following reaction at equilibrium at 300.0 K:
NH4 HS (s)
168)
NH3 (g) + H2 S (g)
If pNH3 = pH2 S = 0.105 atm, Kp = ________.
A) .0110
B) 4.99 × 10-4
C) .105
D) .0821
E) 5.66 × 10-3
169) The value of Keq for the following reaction is 0.25:
SO2 (g) + NO2 (g)
169)
SO3 (g) + NO (g)
The value of Keq at the same temperature for the reaction below is ________.
3SO2 (g) + 3NO2 (g)
A) 1.6 × 10-2
3SO3 (g) + 3NO (g)
B) 7.5 × 10-1
C) 8.3 × 10-2
D) 6.4 × 101
170) The Keq for the equilibrium below is 7.52 × 10-2 at 480.0 °C.
2Cl2 (g) + 2H2 O (g)
4HCl (g) + O2 (g)
What is the value of Keq at this temperature for the following reaction?
8HCl (g) + 2O2 (g)
4Cl2 (g) + 4H2 O (g)
A) 1.77 × 102
B) 5.66 × 10-3
C) 1.50 × 10-1
D) -7.52 × 10-2
E) 7.52 × 10-2
36
E) 0.25
170)
171) The Keq for the equilibrium below is 5.4 × 1013 at 480.0 °C.
2NO (g) + O2 (g)
171)
2NO2 (g)
What is the value of Keq at this temperature for the following reaction?
4NO (g) + 2O2 (g)
4NO2 (g)
A) 2.9 × 1027
B) 8.5 × 1054
C) 3.4 × 10-28
D) -1.1 × 1014
E) 5.4 × 1013
172) The Keq for the equilibrium below is 0.112 at 700.0 °C.
1
SO2 (g) + O2 (g)
2
172)
SO3 (g)
What is the value of Keq at this temperature for the following reaction?
2SO2 (g) + O2 (g)
2SO3 (g)
A) 1.25 × 10-2
B) 2.24 × 10-1
C) 7.97 × 101
D) 4.46
E) 0.112
173) The value of Keq for the following reaction is 0.26:
A (g) + B (g)
173)
C (g) + D (g)
The value of Keq at the same temperature for the reaction below is ________.
2A (g) + 2B (g)
A) 0.068
2C (g) + 2D (g)
B) 0.52
C) 1.2
D) 0.065
E) 0.26
174) The value of Keq for the following reaction is 0.16:
A (g) + B (g)
174)
C (g) + D (g)
The value of Keq at the same temperature for the reaction below is ________.
3C (g) + 3D (g)
A) 2.4 × 102
B) 2.1
3A (g) + 3B (g)
C) 4.1 × 10-3
37
D) 5.3 × 10-2
E) 6.3
175) The value of Keq for the following reaction is 0.50:
A (g) + 2B (g)
175)
C (g) + 4D (g)
The value of Keq at the same temperature for the reaction below is ________.
1/2A (g) + B (g)
A) 7.1 × 10-1
1/2C (g) + 2D (g)
B) 2.5 × 10-1
C) 0.25
D) 1.0
E) 0.50
176) The Keq for the equilibrium below is 7.16 × 10-2 at 440.0 °C.
2Cl2 (g) + 2H2 O (g)
176)
4HCl (g) + O2 (g)
What is the value of Keq at this temperature for the following reaction?
Cl2 (g) + H2 O (g)
2HCl (g) +
1
O (g)
2 2
A) 0.0716
B) 5.13 × 10-3
C) 0.268
D) 0.0376
E) 0.150
177) At 1000.0 K, the equilibrium constant for the reaction
2NO (g) + Br2 (g)
177)
2NOBr (g)
is Kp = 0.016. Calculate Kp for the reverse reaction,
2NOBr (g)
A) 0.016
2NO (g) + Br2 (g).
B) 1.6 × 10-4
C) 63
D) 0.99
178) The expression of Keq for the following reaction will not include ________.
A(g) + B(g)
C(l) + D(g)
A) [C]
B) [A]
C) [B]
D) [D]
E) none of the above
38
E) 1.1
178)
179) Phosphorous trichloride and phosphorous pentachloride equilibrate in the presence of molecular
chlorine according to the reaction:
PCl3 (g) + Cl2 (g)
179)
PCl5 (g)
An equilibrium mixture at 450 K contains
PPCl3 = 0.224 atm,
PCl2 = 0.284 atm, and
PPCl5 = 4.24 atm. What is the value of Kp at this temperature?
A) 66.7
B) 1.50 × 10-2
C) 2.70 × 10-1
D) 3.74
E) 8.36
180) Consider the following chemical reaction:
H2 (g) + I2 (g)
180)
2HI (g)
At equilibrium in a particular experiment, the concentrations of H2 , I2 , and HI were 0.20 M,
0.034 M, and 0.55 M, respectively. The value of Keq for this reaction is ________.
A) 23
B) 81
C) 0.0090
D) 5.1
E) 44
181) Dinitrogen tetroxide partially decomposes according to the following equilibrium:
N2 O4 (g)
181)
2NO2 (g)
A 1.000-L flask is charged with 9.20 × 10-3 mol of N2 O4 . At equilibrium, 5.98 × 10-3 mol of N2 O4
remains. Keq for this reaction is ________.
A) 0.183
B) 0.197
C) 0.212
D) 6.94 × 10-3
E) 2.96 × 10-5
182) The Kp for the reaction below is 1.49 × 108 at 100.0 °C:
CO (g) + Cl2 (g)
COCl2 (g)
In an equilibrium mixture of the three gases, PCO = PCl2 = 1.00 × 10-4 atm. The partial pressure
of the product, phosgene (COCl2 ), is ________ atm.
A) 1.49
B) 1.49 × 1016
C) 6.71 × 10-17
D) 1.49 × 104
E) 1.49 × 1012
39
182)
183) At 900.0 K, the equilibrium constant (Kp) for the following reaction is 0.345.
2SO2 + O2 (g)
183)
2SO3 (g)
At equilibrium, the partial pressure of SO2 is 36.9 atm and that of O2 is 16.8 atm. The partial
pressure of SO3 is ________ atm.
A) 88.8
B) 3.89 × 10-3
C) 214
D) 5.57 × 10-4
E) 42.4
184) At elevated temperatures, molecular hydrogen and molecular bromine react to partially form
hydrogen bromide:
H2 (g) + Br2 (g)
184)
2HBr (g)
A mixture of 0.682 mol of H2 and 0.440 mol of Br2 is combined in a reaction vessel with a volume
of 2.00 L. At equilibrium at 700 K, there are 0.546 mol of H2 present. At equilibrium, there are
________ mol of Br2 present in the reaction vessel.
A) 0.000
B) 0.440
C) 0.546
D) 0.136
E) 0.304
185) At 24°C, Kp = 0.080 for the equilibrium:
NH4 HS (s)
185)
NH3 (g) + H2 S (g)
A sample of solid NH4 HS is placed in a closed vessel and allowed to equilibrate. Calculate the
equilibrium partial pressure (atm) of ammonia, assuming that some solid NH4 HS remains.
A) 0.28
B) 0.080
C) 0.052
D) 0.0049
E) 3.8
186) In the coal-gasification process, carbon monoxide is converted to carbon dioxide via the following
reaction:
CO (g) + H2 O (g)
186)
CO2 (g) + H2 (g)
In an experiment, 0.35 mol of CO and 0.40 mol of H2 O were placed in a 1.00-L reaction vessel. At
equilibrium, there were 0.22 mol of CO remaining. Keq at the temperature of the experiment is
________.
A) 5.5
B) 0.75
C) 3.5
D) 0.28
E) 1.0
187) Kp = 0.0198 at 721 K for the reaction
2HI (g)
187)
H2 (g) + I2 (g)
In a particular experiment, the partial pressures of H2 and I2 at equilibrium are 0.678 and 0.788
atm, respectively. The partial pressure of HI is ________ atm.
A) 7.87
B) 27.0
C) 5.19
40
D) 0.103
E) 0.0106
188) Nitrosyl bromide decomposes according to the following equation.
2NOBr (g)
188)
2NO (g) + Br2 (g)
A sample of NOBr (0.64 mol) was placed in a 1.00-L flask containing no NO or Br2 . At equilibrium
the flask contained 0.16 mol of NOBr. How many moles of NO and Br2 , respectively, are in the
flask at equilibrium?
A) 0.48, 0.24
B) 0.48, 0.48
C) 0.16, 0.08
D) 0.16, 0.16
E) 0.24, 0.42
189) The reaction below is exothermic:
2SO2 (g) + O2 (g)
189)
2SO3 (g)
Le Châtelier's Principle predicts that ________ will result in an increase in the number of moles of
SO3 (g) in the reaction container.
A) increasing the amount of SO2
B) decreasing the pressure
C) increasing the temperature
D) removing some oxygen
E) increasing the volume of the container
190) For the endothermic reaction
CaCO3 (s)
190)
CaO (s) + CO2 (g)
Le Châtelier's principle predicts that ________ will result in an increase in the number of moles of
CO2 .
A) increasing the temperature
B) decreasing the temperature
C) increasing the pressure
D) removing some of the CaCO3 (s)
E) none of the above
191) Consider the following reaction at equilibrium:
2NH3 (g)
N2 (g) + 3H2 (g)
191)
H° = +92.4 kJ
Le Châtelier's principle predicts that removing N2 (g) to the system at equilibrium will result in
________.
A) an increase in the concentration of H2
B) a decrease in the concentration of H2
C) removal of all of the H2
D) a lower partial pressure of H2
E) an increase in the value of the equilibrium constant
41
192) Consider the following reaction at equilibrium:
2CO2 (g)
2CO (g) + O2 (g)
192)
H° = -514 kJ
Le Châtelier's principle predicts that removing O2 (g) to the reaction container will ________.
A) increase the partial pressure of CO
B) decrease the partial pressure of CO
C) increase the partial pressure of CO2
D) increase the value of the equilibrium constant
E) decrease the value of the equilibrium constant
193) Consider the following reaction at equilibrium:
C (s) + H2O (g)
193)
CO (g) + H2 (g)
Which of the following conditions will decrease the partial pressure of CO?
A) decreasing the volume of the reaction vessel
B) increasing the volume of the reaction vessel
C) decreasing the amount of carbon in the system
D) decreasing the pressure of the reaction vessel
E) adding a catalyst to the reaction system
194) Consider the following reaction at equilibrium:
2SO2 (g) + O2 (g)
2SO3 (g)
194)
H° = -99 kJ
Le Châtelier's principle predicts that a(n) increase in temperature will result in ________.
A) an increase in the partial pressure of O2
B) a decrease in the partial pressure of O2
C) a decrease in the partial pressure of SO2
D) a(n) increase in Keq
E) no changes in equilibrium partial pressures
195) The beta decay of cesium-137 has a half-life of 30.0 years. How many years must pass to reduce a
25 mg sample of cesium 137 to 8.7 mg?
A) 46
B) 32
C) 3.2
D) 50
E) 52
195)
196) The half-life of 218Po is 3.1 minutes. How much of a 155 gram sample remains after 0.40 hours?
A) 0.00067 g
B) 0.0072 g
C) 0.72 g
D) 0.0047 g
E) none of the above
196)
42
197) Cesium-131 has a half-life of 9.7 days. What percent of a cesium-131 sample remains after 60
days?
A) 100
B) 0
C) 1.4
D) 98.6
E) more information is needed to solve the problem
197)
198) The half-life for beta decay of strontium-90 is 28.8 years. A milk sample is found to contain 10.3
ppm strontium-90. How many years would pass before the strontium-90 concentration would
drop to 1.0 ppm?
A) 92.3
B) 0.112
C) 186
D) 96.9
E) 131
198)
199) The half-life of carbon-11 is 20.3 minutes. How much of a 100.0 mg sample remains after 1.50
hours?
A) 8.48 mg
B) 4.63 mg
C) 12.9 mg
D) 22.6 mg
E) 7.70 mg
199)
200) The half-life of 131I is 0.220 years. How much of a 500.0 mg sample remains after 24 hours?
A) 496 mg
B) 560 mg
C) 219 mg
D) 405 mg
E) 337 mg
200)
201) The half-life of 223Ra is 11.4 days. How much of a 200.0 mg sample remains after 600 hours?
A) 0.219 mg
B) 21.9 mg
C) .0302 mg
D) 43.8 mg
E) 6.04 mg
201)
202) The half-life of 222Rn is 3.80 days. If a sample contains 36.0 g of Rn-222, how many years will it
take for the sample to be reduced to 1.00 mg of Rn-222?
A) 19.7
B) 0.1597
C) 8.53
D) 0.0234
E) none of the above
202)
203) The carbon-14 dating method can be used to determine the age of a ________.
A) flint arrowhead
B) papyrus scroll
C) stone axe head
D) clay pot
E) rock
203)
204) The basis for the carbon-14 dating method is that ________.
A) the amount of carbon-14 in all objects is the same
B) carbon-14 is very unstable and is readily lost from the atmosphere
C) the ratio of carbon-14 to carbon-12 in the atmosphere is a constant
D) living tissue will not absorb carbon-14 but will absorb carbon-12
E) All of the above are correct.
204)
205) 210Pb has a half-life of 22.3 years and decays to produce 206Hg. If you start with 7.50 g of 210Pb,
how many grams of 206Hg will you have after 17.5 years?
205)
A) 4.35
B) 3.15
C) 3.09
D) 0.0600
43
E) 1.71
206) The half-life of a radionuclide ________.
A) is constant
B) gets shorter with passing time
C) gets longer with passing time
D) gets shorter with increased temperature
E) gets longer with increased temperature
206)
207) The curie is a measure of the ________.
A) number of disintegrations per second of a radioactive substance
B) total energy absorbed by an object exposed to a radioactive source
C) lethal threshold for radiation exposure
D) number of alpha particles emitted by exactly one gram of a radioactive substance
E) None of the above is correct.
207)
Consider the following data for a particular radionuclide:
Time (min)
0
3
6
9
12
Nt (g)
1.23
1.15
1.08
1.01
0.940
208) What is the rate constant (in min-1 ) for the decay of this radionuclide?
A) 45
B) 32
C) 0.024
D) 0.032
209) What is the half-life (in min) of this radionuclide?
A) 0.024
B) 0.022
C) 32
D) 0.032
E) 0.022
E) 45
208)
209)
210) Cesium-137 undergoes beta decay and has a half-life of 30.0 years. How many beta particles are
emitted by a 14.0-g sample of cesium-137 in three minutes?
A) 6.1 × 1013
B) 6.2 × 1022
C) 8.4 × 1015
D) 1.3 × 10-8
E) 8.1 × 1015
210)
211) What order process is radioactive decay?
A) zeroth
B) first
211)
C) second
D) third
E) fourth
212) The half-life of cobalt-60 is 5.20 yr. How many milligrams of a 2.000-mg sample remain after 9.50
years?
A) 0.565
B) 7.03 × 10-22
212)
213) Strontium-90 is a byproduct in nuclear reactors fueled by the radioisotope uranium-235. The
half-life of strontium-90 is 28.8 yr. What percentage of a strontium-90 sample remains after 175.0
yr?
A) 84.8
B) 1.48
C) 0.230
D) 16.5
E) 6.08
213)
C) 7.076
D) 1.095
E) 1.435
44
214) Carbon-11 is used in medical imaging. The half-life of this radioisotope is 20.4 min. What
percentage of a sample remains after 50.0 min?
A) 66.5
B) 8.62
C) 18.3
D) 40.8
E) 2.45
214)
215) A rock contains 0.153 mg of lead-206 for each milligram of uranium-238. The half-life for the
decay of uranium-238 to lead-206 is 4.5 × 109 yr. The rock was formed ________ years ago.
215)
216) 131I has a half-life of 8.04 days. Assuming you start with a 1.03 mg sample of 131I, how many mg
will remain after 13.0 days?
A) 0.326
B) 0.268
C) 0.422
D) 0.0781
E) 0.336
216)
217) The decay of a radionuclide with a half-life of 3.3 × 105 years has a rate constant (in yr-1 ) equal to
________.
A) 4.8 × 105
B) 2.1 × 10-6
C) 4.2 × 10-6
D) 2.8 × 103
E) 5.9 × 10-8
217)
218) Potassium-40 decays to argon-40 with a half-life of 1.27 × 109 yr. The age of a mineral sample that
has a mass ratio of 40Ar to 40K of 0.330 is ________ yr.
218)
219) If we start with 1.000 g of strontium-90, 0.805 g will remain after 9.00 yr. This means that the
half-life of strontium-90 is ________ yr.
A) 7.74
B) 11.2
C) 28.8
D) 7.25
E) 41.6
219)
220) If we start with 1.000 g of cobalt-60, 0.400 g will remain after 7.00 yr. This means that the half-life
of cobalt-60 is ________ yr.
A) 12.1
B) 17.5
C) 2.80
D) 5.30
E) 7.65
220)
221) A freshly prepared sample of curium-243 undergoes 3312 disintegrations per second. After 8.00 yr,
the activity of the sample declines to 2591 disintegrations per second. The half-life of curium-243 is
________ years.
A) 6.26
B) 32.6
C) 10.2
D) 1.36
E) 22.6
221)
222) The beta decay of cesium-137 has a half-life of 30.0 years. How many years must pass to reduce a
30 mg sample of cesium 137 to 5.2 mg?
A) 76 years
B) -76 years
C) 38 years
D) 0.040 years
E) 25 years
222)
223) The half-life of 218Po is 3.1 minutes. How much of a 170 gram sample remains after 0.64 hours?
A) 0.032 g
B) 150 g
C) 31 g
D) 4.7 × 10-10 g
223)
A) 6.89 × 108
A) 3.85 × 109
B) 5.60 × 108
B) 1.77 × 109
C) 7.33 × 108
C) 2.55 × 109
E) None of the original sample will remain.
45
D) 1.06 × 109
D) 3.62 × 108
E) 8.08 × 108
E) 5.23 × 108
224) Cesium-131 has a half-life of 9.7 days. What percent of a cesium-131 sample remains after 62
days?
A) 1.2 %
B) 100 %
C) 0 %
D) 99 %
E) 62%
224)
225) The half-life of carbon-11 is 20.3 minutes. How much of a 100.0 mg sample remains after 1.6
hours?
A) 3.77 mg
B) 0.0377 mg
C) 94.7 mg
D) 1.75 × 10-89 mg
225)
226) 210Pb has a half-life of 22.3 years and decays to produce 206Hg. If you start with 7.52 g of 210Pb,
how many grams of 206Hg will you have after 15.8 years?
226)
E) 99.9 mg
A) 4.60 g
B) 2.83 g
C) 9.20 g
46
D) 2.30 g
E) 12.5 g
Answer Key
Testname: COLLEGE CHEMISTRY II PHS 1035 PRACTICE EXAM 2
1) A
2) A
3) E
4) B
5) E
6) A
7) C
8) B
9) E
10) C
11) E
12) E
13) A
14) C
15) D
16) A
17) A
18) E
19) D
20) A
21) D
22) C
23) B
24) D
25) A
26) B
27) B
28) C
29) D
30) A
31) D
32) A
33) C
34) A
35) C
36) B
37) D
38) E
39) A
40) C
41) E
42) C
43) A
44) A
45) A
46) A
47) A
48) A
49) B
50) B
47
Answer Key
Testname: COLLEGE CHEMISTRY II PHS 1035 PRACTICE EXAM 2
51) A
52) B
53) A
54) E
55) A
56) A
57) A
58) A
59) A
60) A
61) A
62) A
63) D
64) E
65) C
66) C
67) C
68) A
69) C
70) E
71) C
72) D
73) E
74) A
75) B
76) B
77) B
78) A
79) A
80) B
81) A
82) C
83) D
84) E
85) A
86) B
87) C
88) D
89) E
90) A
91) D
92) A
93) D
94) C
95) D
96) C
97) B
98) C
99) A
100) B
48
Answer Key
Testname: COLLEGE CHEMISTRY II PHS 1035 PRACTICE EXAM 2
101)
102)
103)
104)
105)
106)
107)
108)
109)
110)
111)
112)
113)
114)
115)
116)
117)
118)
119)
120)
121)
122)
123)
124)
125)
126)
127)
128)
129)
130)
131)
132)
133)
134)
135)
136)
137)
138)
139)
140)
141)
142)
143)
144)
145)
146)
147)
148)
149)
150)
A
B
E
B
D
B
A
C
D
B
A
C
B
D
C
B
A
B
E
A
D
E
E
B
C
D
A
D
C
D
E
D
C
D
B
A
A
B
B
D
E
E
B
C
E
E
B
C
C
D
49
Answer Key
Testname: COLLEGE CHEMISTRY II PHS 1035 PRACTICE EXAM 2
151)
152)
153)
154)
155)
156)
157)
158)
159)
160)
161)
162)
163)
164)
165)
166)
167)
168)
169)
170)
171)
172)
173)
174)
175)
176)
177)
178)
179)
180)
181)
182)
183)
184)
185)
186)
187)
188)
189)
190)
191)
192)
193)
194)
195)
196)
197)
198)
199)
200)
C
D
C
D
A
C
D
D
E
D
C
D
C
A
B
D
B
A
A
A
A
A
A
A
A
C
C
A
A
E
D
A
A
E
A
D
C
A
A
A
A
A
A
A
A
C
C
D
B
A
50
Answer Key
Testname: COLLEGE CHEMISTRY II PHS 1035 PRACTICE EXAM 2
201)
202)
203)
204)
205)
206)
207)
208)
209)
210)
211)
212)
213)
214)
215)
216)
217)
218)
219)
220)
221)
222)
223)
224)
225)
226)
D
B
B
C
A
A
A
E
C
E
B
A
B
C
D
E
B
E
C
D
E
A
A
A
A
A
51