72.
Predict the products for this reaction:
potassium phosphate +
barium chloride -->
73.
Chlorine reacts with sodium oxide to produce oxygen and sodium
chloride. Give the correct, balanced equation for this reaction.
74. What is the
mass of one mole of neon?
75. What is the
volume of 3.00 moles of carbon dioxide at STP?
76. What is the
percentage composition of each element in ammonia (NH3)?
77. A compound
was analyzed and found to contain 13.5 g Ca, 10.8 g O, and 0.675 g H. What is
the empirical formula for the compound?
78. The molar
mass of a compound is 56 g/mol, and its empirical formula is CH2.
What is its molecular formula?
79. Determine the
number of atoms in 10.0 grams of sulfur.
80. What happens
to the bonds between atoms in a substance that undergoes a chemical reaction?
81. When the
following equation is balanced, what is the coefficient of H2SO4?
____ Al +
____ H2SO4 -->
____ Al2(SO4)3 + _____ H2
82. When the
following equation is balanced, what is the coefficient of C6H6?
_____ C6H6
+ _____ O2 -->
______ H2O + _____ CO2
83. According to
the chemical equation shown below, how many moles of O2 are produced
when 4.0 moles of H2O2 (l) decompose?
2 H2O2 (l) --> 2 H2O (l) + O2
(g)
84. How many
liters of hydrogen react with 2.00 mol nitrogen at STP in the following
reaction?
N2 + 3 H2 --> 2 NH3
85. A piece of
copper with a mass of 5.00 g is placed in a solution of silver nitrate
containing excess AgNO3. The
silver metal produced has a mass of 15.2 g. What is the percent yield for
this reaction?
Cu + 2 AgNO3 --> Cu
(NO3)2 + 2 Ag
86. If you add
0.10 moles of HCl to 0.10 moles of Mg in the following reaction,
which reactant will be limiting?
2 HCl + Mg -->
MgCl2 + H2
Questions 87 and 88 refer to the
following chemical reaction, in which a 2.00 g sample of ammonia is mixed
with 4.00 g of oxygen.
4 NH3 (g) + 5 O2 (g) -->
4 NO (g) + 6 H2O (g)
87.
Which is the limiting reactant?
88.
How much NO would be produced?
89. Figure 14-2
below represents the kinetic energies of the molecules in two systems, one at
temperature T1 and the other at temperature T2.
How do the two temperatures represented by curves T1 and T2
in Figure 14-2 compare?
Use Figure
14-4 to answer questions 90 and 91.
90.
In Figure 14-4, where do the three phases exist in equilibrium?
91.
In Figure 14-4, what phase would be present at 15 oC and 20
mmHg?
92. What kinds of
forces are responsible for the attraction between molecules in nonpolar
liquids?
93. A glass of
ice water at 0°C absorbs heat until all the ice melts. Even though heat is
being absorbed, the temperature does not change. Why is this true?
94. 
What phase(s) is/are present at point B
in the heating curve to the right?
95. At what
temperature does the motion of particles cease?
96. When a rigid
container of gas is heated, what happens to the pressure inside the container?
97. When the
amount and volume of a gas are kept constant and the pressure increases, what
happens to the temperature of the gas?
98. A gas at a
pressure of 608 mmHg is held in a container with a volume of 545 cm3.
The volume of the container is then increased to 1065 cm3
without change in temperature. What is the new pressure of the gas?
99. The
temperature inside of a car on a summer’s day is 42°C. What is that
temperature expressed in Kelvin?
100. How
many moles of a gas at 100°C does it take to fill a 1.00 l flask to a pressure of 1.50 atm?
{R = 0.0821 (L × atm) / (mol × K) }
101. How
does the rate of effusion of CO2 relate to that of CO at the same
temperature and pressure?
102. 
If the pressure of the gas in the open mercury manometer
at the right is 815 torr, what is the atmospheric pressure?
103. You
are given a mixture of gases consisting of only nitrogen, hydrogen and helium.
The pressure of the nitrogen is 33.4 kPa and the pressure of hydrogen is
58.1 kPa. If the total pressure of the mixture is 125.4 kPa, what is
the partial pressure of the helium?
104. According
to Kinetic-Molecular Theory, why does the pressure of a gas increase with a
decrease in volume?
105. A
fixed sample of gas occupies 40.0 ml
at –123°C. What volume does the sample occupy at 27°C, assuming constant
pressure?
106. How
does the mass of an inflated basketball compare with the mass of the same
basketball when it is deflated?
107. Under
what conditions does real gas deviate the most from ideal behavior?
108. List
at least three factors that affect the rate of a chemical reaction.
109. Which
will react faster with water, a lump of calcium, or finely powdered calcium?
Use Figure 15-1 to answer
questions 110 and 111.
110.
According to Figure 15-1, if 75 grams of KCl dissolve in 100 grams
of water at 90°C, describe the resulting solution.
111.
Use Figure 15-1 to determine how many grams of KNO3 you would
dissolve in 100 grams of water at 40°C to make a saturated solution.
112. What
is the term for solution concentration expressed as moles of solute/kilogram of
solvent?
113. A
solution which, upon mixing for a long period of time, still contains
undissolved particles is most likely what kind of solution.
114. How
many moles of sugar are present in 4.0 liters of a 0.25 M
solution?
115. A
substance dissolves in a polar solvent. What, if anything, can be inferred
about the chemical nature of the substance?
116. When a
solute is dissolved in a solvent, what is the effect on the boiling point of
the resulting solution?
117. How
does temperature affect the solubility of a gas?
118. A data
table and two prepared beakers are shown below.
Solid KNO3 was added to
each beaker. Each beaker was stirred at the same rate until all of the solid
dissolved. The table shows the solubilities of KNO3 at different
temperatures. How will the rates of dissolving compare?
119. How
many ml of 3.25 M
NaCl would be needed to make 15.5 ml
of a 0.500 M NaCl solution?
120. What
is the boiling point of a 0.222 m solution of K3PO4
in water? (Kb for water is 0.512°C/m)
121. At
equilibrium, how does the forward reaction rate compare with the reverse
reaction rate?
122. In an
equilibrium reaction with a Keq of 1 × 10−8,
which are favored, reactants or products?
123. What
is the equilibrium expression for the following hypothetical reaction:
A + 2 B 
C
124. Why
are the concentrations of solids and pure liquids not included in equilibrium
expressions?
Questions 125–127
refer to a hypothetical reversible reaction in which reactant Y is a bright
yellow color, reactant C is colorless, and the product B is a bright blue color
C (g) + Y (g) 3 B (g) + heat
The reaction is slightly exothermic, with Keq = 1.50.
The system is initially at equilibrium, with a green color. (Note that a green
color would indicate a roughly equal mixture of blue and yellow.)
125.
What color would result from adding a large quantity of C?
126. What
color would result from heating the system?
127.
What color would result from increasing the pressure on the system?
128. Ammonia
is made according to the following equation:
N2 (g) + H2 (g) 2 NH3 (g) + heat
In the Haber Process, NH3
is continuously removed as the above reaction occurs. What effect does this
have on the equilibrium?
129. Consider
the following equilibrium equation:
H2 (g) + I2 (g) 2HI (g)
At 448°C in a 2.0 l closed system, 2.0 × 10−2 mol
HI, 1.0 × 10−2 mol of H2, and
3.0 × 10−2 mol of I2 are present.
The equilibrium constant for the reaction is 51. Which direction would the
reaction need to proceed to reach equilibrium?
130. 25.0 ml of a HNO3 solution of
unknown concentration is titrated with 0.50 M NaOH. 75.0 ml of the sodium hydroxide solution are
required to reach the equivalence point. What was the original concentration
of the HNO3 solution?
131. What
is the pH of a solution that has an H+
concentration of 0.0001 M?
132. What
is the pOH of a solution that has a pH of 6?
133. What
is the name for substances that change color when added to acids or bases?
134. What
are typically the products of the reaction between an acid and a base?
135. What
is the [OH−] in a solution with a pH of 3.21?
136. Give
the formula for a compound that is both polyprotic and amphoteric.
137. What
is the conjugate base of HSO4−?
138.
What is the correct half reaction for aluminum in the following
unbalanced reaction: Al + FeSO4 -->
Al2(SO4)3 + Fe
139. In
question 138 above, which compound is the reducing agent?
140. In the
reaction 4 FeO + O2 -->
2 Fe2O3, which compound is oxidized and which
compound is reduced?
141.
What is the oxidation number of chlorine in the perchlorate ion, ClO4−?
A solid cube was put into a cylinder containing four
liquids with different densities, as shown in the figure at the right. The
cube fell quickly through layer A, fell slowly through layer B, and stopped
upon reaching layer C. Give upper and lower bounds on the density of the cube. 
Which is the proper reading of the thermometer shown in
the illustration at the right?
