AP Chemistry 2017 Summer
Assignment
Minor Grade
Due: 08/21/2017
Name ______________
Note: For all questions, assume that the temperature is 298 K, the pressure is 1.00 atmospheres and
solutions are aqueous unless otherwise specified.
Throughout the test the following symbols have the definitions specified unless otherwise noted.
T = temperature
P = pressure
V = volume
S = entropy
H = enthalpy
G = free energy
R = molar gas constant
n = number of moles
M
m
L, mL
g
nm
atm
J, kJ
V
mol
= molar
= molal
= liter(s), milliliter(s)
= gram(s)
= nanometers
= atmosphere(s)
= joule(s), kilojoule(s)
= volt(s)
= mole(s)
Part A
Directions: Each set of lettered choices below refers to the numbered statements immediately following
it. Select the one lettered choice that best fits each statement and then fill in the corresponding blank on
the answer sheet. A choice may be used once, more than once, or not at all in each set.
Questions 1-4 refer to the following elements
(A)
(B)
(C)
(D)
(E)
Lithium
Mercury
Iodine
Strontium
Fluorine
1.
Is a gas in its standard state at 298 K
2.
Reacts with water to form a strong base
3.
Is a liquid in its standard state at 298 K
4.
Is an alkali metal
Questions 5 - 7 refer to the following elements
(A)
(B)
(C)
(D)
(E)
F
S
Mg
Ar
Mn
5.
Has oxidation number always equal to -1
6.
Forms a compound having the formula KXO4
7.
Is a diatomic element in its standard state at 298 K
Part B
Directions: Each of the questions or incomplete statements below is followed by five suggested answers
or completions. Select the one that is best in each case and then fill in the corresponding blank on the
answer sheet.
8.
The addition of an acid to which of the following compounds will produce a gas?
(A) CaCO3
(B) ZnS
(C) NH4Br
(D) CH4
(E) NaOH
9.
The net ionic equation for the reaction between silver carbonate and hydrochloric acid is
(A) Ag2CO3(s) + 2 H+ + 2 Cl- à 2 AgCl(s) + H2O + CO2(g)
(B) 2 Ag+ + CO32- + 2 H+ + 2 Cl- à 2 AgCl(s) + H2O + CO2(g)
(C) CO32- + 2 H+ à H2O + CO2(g)
(D) Ag+ + Cl- à AgCl(s)
(E) Ag2CO3(s) + 2 H+ à 2 Ag+ + H2CO3
. . . H2S(aq) + . . . IO3-1(aq) à . . . I2(aq) + . . . SO32-(aq) + . . . H2O + . . . H+(aq)
10.
When the equation above is balanced with lowest whole-number coefficients, the coefficient for
H+ is
(A) 4
(B) 6
(C) 8
(D) 12
(E) 36
11.
A compound contains 1.10 mol of K, 0.55 mol of Te, and 1.65 mol of O. What is the simplest
formula of this compound?
(A) KTeO
(B) KTe2O
(C) K2TeO3
(D) K2TeO6
(E) K4TeO6
8 CN-(aq) + 4 Ag(s) + O2(g) + 2 H2O(l) à 4 Ag(CN)2-1(aq) + 4 OH-(aq)
12.
In the equation above, which of the following statements describes Ag(s)?
I.
II.
III.
It undergoes oxidation.
It is the oxidizing agent.
It has an oxidation number of +1.
(A)
I only
(B)
II only
(C)
III only
(D)
I and III
(E)
II and III
13.
A halogen, X, and an alkaline earth metal, M, will form a compound with the formula
(A) MX
(B) MX2
(C) MX3
(D) M2X3
(E) M3X2
14.
The atomic mass of chlorine is 35.45 amu. Given that there are only two naturally occurring
isotopes of chlorine, 35Cl and 37Cl, the natural abundance of the 37Cl isotope must be
approximately
(A) 90 %
(B) 75%
(C) 50%
(D) 25%
(E) 10%
15.
Place the following in order of increasing mass:
15.0 g of NaCl, 1.00 mol of H2O, 0.50 mol of CH4, and 0.25 mol of NaOH.
(A) CH4 < NaOH < NaCl < H2O
(B) NaOH < NaCl < H2O < CH4
(C) NaCl < H2O < CH4 < NaOH
(D) H2O < NaOH < NaCl < CH4
(E) NaOH < NaCl < CH4 < H2O
16.
Aluminum reacts with oxygen to give aluminum oxide. If you have 6.0 moles of Al,
(A) you need 3.0 moles of O2 for complete reaction and produce 2.0 moles of Al2O3
(B) you need 18.0 moles of O2 for complete reaction and produce 2.0 moles of Al2O3
(C) you need 3.0 moles of O2 for complete reaction and produce 6.0 moles of Al2O3
(D) you need 4.5 moles of O2 for complete reaction and produce 3.0 moles of Al2O3
(E) you need 6.0 moles of O2 for complete reaction and produce 6.0 moles of Al2O3
2 N2H4(g) + N2O4(g) à 3 N2(g) + 4 H2O(g)
17.
When 8.0 g of N2H4 (32 g mol─1) and 48 grams of N2O4 (96 g mol─1) are mixed together and
react according to the equation above, what is the maximum mass of H2O that can be produced?
(A) 9.0 g
(B) 18 g
(C) 36 g
(D) 72 g
(E) 144 g
18.
All of the halogens in their elemental form at 25oC and 1 atm are
(A) conductors of electricity
(B) diatomic molecules
(C) odorless
(D) colorless
(E) gases
2H2O(l) + 4MnO4─(aq) + 3 ClO2─(aq) à 4MnO2(s) + 3 ClO4─(aq) + 4OH─(aq)
19.
According to the balanced equation above, how many moles of ClO2─(aq) are needed to react
completely with 20. mL of 0.20 M KMnO4 solution?
(A) 0.0030 mol
(B) 0.0053 mol
(C) 0.0075 mol
(D) 0.013 mol
(E) 0.030 mol
MnO2(s) + 2 I-1(aq) + 4 H+(aq) à I2(aq) + Mn2+(aq) + 2 H2O(l)
20.
Which answer correctly describes the reaction above?
(A) Mn in MnO2 is reduced to Mn2+ and I- is oxidized to I2
(B) I- is reduced to I2 and H+ is oxidized to H2O
(C) I- is the oxidizing agent and MnO2 is the reducing agent
(D) H+ is the oxidizing agent, and I- is the reducing agent
(E) MnO2 is the reducing agent and I- is reduced
21.
Commercial vinegar was titrated with NaOH solution to determine the content of acetic acid,
HCH3COO. For 20.0 milliliters of the vinegar, 32.0 milliliters of 0.500 M NaOH solution was
required. What was the concentration of acetic acid in the vinegar if no other acid was present?
(A) 1.60 M
(B) 0.800 M
(C) 0.640 M
(D) 0.600 M
(E) 0.400 M
22.
In which of the following compounds is the mass ratio of chromium to oxygen closest to
1.6 to 1.0?
(A) CrO3
(B) CrO2
(C) CrO
(D) Cr2O
(E) Cr2O3
23.
When a 1.25-gram sample of limestone was dissolved in acid, 0.33 grams of CO2 was
generated. If the rock contained no carbonate other than CaCO3, what was the percent of
CaCO3 by mass in the limestone?
(A) 35%
(B) 44%
(C) 60%
(D) 80%
(E) 100%
24.
Which of the following represents a pair of isotopes of element X?
(A) 2111X & 2412X
(B) 199X & 3919X
(C) 126X & 126X
(D) 146X & 147X
(E) 7935X & 8135X
25.
When a hydrate of Na2CO3 is heated until all the water of hydration is removed, it loses just
over 50% of its mass. The formula of the hydrate is
(A) Na2CO3 · 10 H2O
(B) Na2CO3 · 7 H2O
(C) Na2CO3 · 5 H2O
(D) Na2CO3 · 3 H2O
(E) Na2CO3 · H2O
. . . CN-1 + . . . CrO4-2 à . . .CNO-1 + . . . Cr(OH)4-1 (basic conditions)
26.
When the equation above is balanced with lowest whole number coefficients, the coefficient in
front of the OH-1 is
(A) 1
(B) 2
(C) 4
(D) 6
(E) 10
27.
Which half-reaction correctly represents reduction?
(A) Cr3+ + 3e- à Cr(s)
(B) Cr3+ à Cr(s) + 3e(C) Cr(s)à Cr3+ + 3e(D) Cr(s)+ 3e- à Cr3+
(E) Cr(s) + 3p+ à Cr3+
28.
Nitric acid in the chemical stockroom is 15.0 M, what volume of this solution must be taken in
order to make 5.00 liters of a 6.00 M solution?
(A) 2.00 L
(B) 450. L
(C) 18.0 L
(D) 12.5 L
(E) 0.500 L
29.
If 100. mL of 0.750 M MgCl2(aq) is added to 500. mL of distilled water, what is the
concentration of Cl1-(aq) in the resulting solution? (Assume volumes are additive.)
(A) 0.125 M
(B) 0.150 M
(C) 0.250 M
(D) 0.600 M
(E) 1.20 M
30.
Mass of an empty container = 3.0 grams
Mass of the container plus the solid sample = 25.0 grams
Volume of the solid sample = 11.0 cubic centimeters
The data above were gathered in order to determine the density of an unknown solid. The density
of the sample should be reported as
(A) 0.5 g/cm3
(B) 0.50 g/cm3
(C) 2.0 g/cm3
(D) 2.00 g/cm3
(E) 2.27 g/cm3
31.
How many grams of calcium nitrate, Ca(NO3)2, contains 24 grams of oxygen atoms?
(A) 41 grams
(B) 50. grams
(C) 62 grams
(D) 96 grams
(E) 164grams
32.
The mass of element Q found in 1.00 mole of each of four different compounds is 38.0 grams,
57.0 grams, 76.0 grams, and 114 grams, respectively. A possible atomic weight of Q is
(A) 12.7
(B) 19.0
(C) 27.5
(D) 38.0
(E) 57.0
33.
When 70. milliliter of 3.0-molar Na2CO3 is added to 30. milliliters of 1.0-molar NaHCO3 the
resulting concentration of Na+ is
(A) 2.0 M
(B) 2.4 M
(C) 4.0 M
(D) 4.5 M
(E) 7.0 M
34.
Propene gas, C3H8, burns in excess oxygen. When the equation for the reaction is balanced
correctly and all coefficients are reduced to lowest whole-number coefficients, the coefficient for
O2 is
(A) 3
(B) 5
(C) 9
(D) 10
(E) 18
35.
A mixture is prepared by adding 100. mL of 0.10 M Na2CrO4 to 100. mL of 0.10 M AgNO3. A
precipitate forms in this mixture. Which describes the changes in concentration of the spectator
ions, Na+ and NO31- in the mixture as the reaction occurs in the beaker containing AgNO3?
Concentration of Na+
A
B
C
D
E
36.
Increase
Decrease
Remains the same
Increase
Remains the same
Concentration of NO31Increase
Remains the same
Decrease
Decrease
Remains the same
Epsom salt, MgSO4 · 7 H2O (molar mass = 246 g mol-1) can be dehydrated by heating in an
open crucible. Which value is closest to the fraction of the mass of salt in the crucible lost when
the crucible is heated to a constant mass?
1
8
1
(B)
7
1
(C)
4
1
(D)
3
1
(E)
2
(A)
Name _____________________________ Period ____________
Answer Sheet Multiple Choice
1.
(a)
(b)
(c)
(d)
(e)
21.
(a)
(b)
(c)
(d)
(e)
2.
(a)
(b)
(c)
(d)
(e)
22.
(a)
(b)
(c)
(d)
(e)
3.
(a)
(b)
(c)
(d)
(e)
23.
(a)
(b)
(c)
(d)
(e)
4.
(a)
(b)
(c)
(d)
(e)
24.
(a)
(b)
(c)
(d)
(e)
5.
(a)
(b)
(c)
(d)
(e)
25.
(a)
(b)
(c)
(d)
(e)
6.
(a)
(b)
(c)
(d)
(e)
26.
(a)
(b)
(c)
(d)
(e)
7.
(a)
(b)
(c)
(d)
(e)
27.
(a)
(b)
(c)
(d)
(e)
8.
(a)
(b)
(c)
(d)
(e)
28.
(a)
(b)
(c)
(d)
(e)
9.
(a)
(b)
(c)
(d)
(e)
29.
(a)
(b)
(c)
(d)
(e)
10.
(a)
(b)
(c)
(d)
(e)
30.
(a)
(b)
(c)
(d)
(e)
11.
(a)
(b)
(c)
(d)
(e)
31.
(a)
(b)
(c)
(d)
(e)
12.
(a)
(b)
(c)
(d)
(e)
32.
(a)
(b)
(c)
(d)
(e)
13.
(a)
(b)
(c)
(d)
(e)
33.
(a)
(b)
(c)
(d)
(e)
14.
(a)
(b)
(c)
(d)
(e)
34.
(a)
(b)
(c)
(d)
(e)
15.
(a)
(b)
(c)
(d)
(e)
35.
(a)
(b)
(c)
(d)
(e)
16.
(a)
(b)
(c)
(d)
(e)
36.
(a)
(b)
(c)
(d)
(e)
17.
(a)
(b)
(c)
(d)
(e)
37.
(a)
(b)
(c)
(d)
(e)
18.
(a)
(b)
(c)
(d)
(e)
38.
(a)
(b)
(c)
(d)
(e)
19.
(a)
(b)
(c)
(d)
(e)
39.
(a)
(b)
(c)
(d)
(e)
20.
(a)
(b)
(c)
(d)
(e)
40.
(a)
(b)
(c)
(d)
(e)