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WorksheetsEpic AP Chem Review
Total questions: 31
Worksheet time: 1hrs 11mins
Name
Class
Date
1.
This electrode in a voltaic cell gains mass
a)
anode
b)
cathode
2.
This electrode loses mass
a)
anode
b)
cathode
3.
Reactions in voltaic cells are
a)
spontaneous, redox reactions
b)
non-spontaneous, redox reactions
c)
spontaneous, non-redox reactions
d)
non-spontaneous, non-redox reactions
4.
In a voltaic cell, the half cell that receives anions from the salt bridge is
a)
cathode
b)
anode
5.
In a voltaic cell, the half cell that receives cations from the salt bridge is
a)
cathode
b)
anode
6.
The following reaction has a ΔGₒ value of 48.47 kJ/mol at 25ₒC.
HB(aq) + H2O(l) <-> H3O+(aq) + B-(aq)
Calculate Ka for the acid HB.
HB(aq) + H2O(l) <-> H3O+(aq) + B-(aq)
Calculate Ka for the acid HB.
a)
0.981
b)
-19.6
c)
4.85 x 10-5
d)
3.19 x 10-9
7.
Which energy conversion shown below takes place in a galvanic cell?
a)
electrical to chemical
b)
mechanical to chemical
c)
mechanical to electrical
d)
chemical to electrical
8.
Consider the following numbered processes:
1. A -> 2B
2. B -> C + D
3. E -> 2D
ΔH for the process A -> 2C + E is
1. A -> 2B
2. B -> C + D
3. E -> 2D
ΔH for the process A -> 2C + E is
a)
ΔH1 + ΔH2 + ΔH3
b)
ΔH1 + ΔH2
c)
ΔH1 + ΔH2 - ΔH3
d)
ΔH1 + 2ΔH2 - ΔH3
9.
Consider the following processes:
I. condensation of a liquid
II. increasing volume of an ideal gas at constant temp
III. dissolving sugar in water
IV. heating 1.0 mol of an ideal gas at constant volume
For how many of these is ΔS positive?
I. condensation of a liquid
II. increasing volume of an ideal gas at constant temp
III. dissolving sugar in water
IV. heating 1.0 mol of an ideal gas at constant volume
For how many of these is ΔS positive?
a)
0
b)
1
c)
2
d)
3
10.
For the reaction A + B -> C + D, ΔHₒ = +40 kJ and ΔSₒ = +50 J/K. Therefore, the reaction under standard conditions is
a)
spontaneous at temps > 10K
b)
spontaneous at temps > 800K
c)
spontaneous at temps between 10K and 800K
d)
spontaneous at all temperatures
11.
Consider the reaction:
C2H5OH(l) + 3O2(g) -> 2CO2(g) + 3H2O(l), ΔH = -1.37 x 103kJ
When a 21.1g sample of ethyl alcohol (molar mass = 46.07 g/mol) is burned, how much energy is released as heat?
C2H5OH(l) + 3O2(g) -> 2CO2(g) + 3H2O(l), ΔH = -1.37 x 103kJ
When a 21.1g sample of ethyl alcohol (molar mass = 46.07 g/mol) is burned, how much energy is released as heat?
a)
0.627 kJ
b)
6.27 x 102 kJ
c)
2.89 x 104 kJ
d)
2.18 kJ
12.
Which is most acidic?
a)
pH = 8.5
b)
[H3O+] = 1 x 10-13
c)
[H3O+] = 1 x 10-2
d)
pH = 3
13.
Consider the following rate law: Rate = k[A]n[B]m
How are the exponents n and m determined?
How are the exponents n and m determined?
a)
by using balanced chemical equation
b)
By using the subscripts for the formulas
c)
By educated guess
d)
By experiment
14.
For 2A + B → 2C, the rate of production of C has been found to be 12 M/s. During that reaction, the rate of reaction was?
a)
12 M/s
b)
24 M/s
c)
6 M/s
d)
Cannot tell without more data
15.
step 1: O3 → O2 + O
step 2: O3 + O → 2 O2
The oxygen atom (O) is considered to be a(n)...
step 2: O3 + O → 2 O2
The oxygen atom (O) is considered to be a(n)...
a)
reactant
b)
catalyst
c)
reaction intermediate
d)
activated complex
16.
A compound has a half-life of 14 min. How much time will it take a 12 mol sample to decay to 1.5 mol?
a)
14 min
b)
28 min
c)
42 min
d)
56 min
17.
a)
rate = k[CO]2[O2]2
b)
rate = k[CO]2[O2]
c)
rate = k[CO][O2]2
d)
rate = k[CO][O2]1/2
18.
Which one of the following elements has the greatest ionization energy?
a)
Al
b)
Cl
c)
Br
d)
S
19.
Which of the following is true of an element in an excited state?
a)
It has emitted a photon and its energy has decreased
b)
It has emitted a photon and its energy has increased
c)
It has absorbed a photon and its energy has increased
d)
It has absorbed a neutron and its energy has increased
20.
63Cu is 69% of the naturally occurring isotope of Cu. If only one other isotope is present for natural copper, what is it?
a)
59Cu
b)
65Cu
c)
61Cu
d)
62Cu
21.
Which molecular geometry tends to be nonpolar?
a)
Bent
b)
Trigonal Pyramidal
c)
Trigonal Bipyramidal
d)
Square Pyramidal
22.
Silver chromate, Ag2CrO4, has a Ksp of 8.96 x 10-12. Calculate the solubility in mol/L of silver chromate.
a)
1.31 x 10-4M
b)
1.65 x 10-4M
c)
2.25 x 10-12M
d)
2.08 x 10-4M
23.
The pH of a solution at 25ₒC in which [OH-] = 3.9 x 10-5M is:
a)
4.41
b)
3.90
c)
9.59
d)
4.80
24.
Calculate the pH of a 0.47M NH3 (Kb = 1.8 x 10-5) solution.
a)
2.54
b)
8.93
c)
5.07
d)
11.46
25.
The solubility of Cd(OH)2 in water is 1.67 x 10-5 mol/L. The Ksp value for Cd(OH)2 is
a)
1.86 x 10-14
b)
4.66 x 10-15
c)
5.58 x 10-10
d)
1.67 x 10-5
26.
A weak acid, HF, is in solution with dissolved sodium fluoride, NaF. If HCl is added, which ion will react with the extra hydrogen ions from the HCl to keep the pH from changing?
a)
OH-
b)
Na+
c)
F-
d)
Na-
27.
An unknown salt, M2Z, has a Ksp of 3.3 x 10-9. Calculate the solubility in mol/L of M2Z.
a)
1.2 x 10-3 M
b)
5.7 x 10-5 M
c)
9.4 x 10-4 M
d)
2.9 x 10-5 M
28.
Which one of the following will change the value of an equilibrium constant?
a)
Adding other substances that do not react with any of the species involved in the equilibrium.
b)
Varying the initial concentrations of reactants.
c)
Varying the initial concentrations of products.
d)
Changing temperature
29.
The equilibrium constant for reaction 1 is K. What is the equilibrium constant for equation 2?
(1) SO2(g) + 1/2O2(g) ↔ SO3(g)
(2) 2SO3(g) ↔ 2SO2(g) + O2(g)
(1) SO2(g) + 1/2O2(g) ↔ SO3(g)
(2) 2SO3(g) ↔ 2SO2(g) + O2(g)
a)
K squared (K2)
b)
2K
c)
1/2K
d)
1/K squared (1/K2)
30.
Initially, 0.84 moles of PCl5(g) is placed in a 1.0L flask. At equilibrium, 0.72 moles of PCl5(g) is present. What is the value of Kc for this reaction?
PCl5(g) ↔ PCl3(g) + Cl2(g)
PCl5(g) ↔ PCl3(g) + Cl2(g)
a)
0.62
b)
0.020
c)
0.72
d)
0.12
31.
A mixture of 0.500 mol H2 and 0.500 mol I2 was placed in a 1.00L flask. The equilibrium constant Kc for the reaction H2(g) + I2(g) ↔ 2HI(g) is 54.3. What is the concentration of HI at equilibrium?
a)
0.5M
b)
1.0M
c)
0.786M
d)
0.393M
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