Download study guide spring 2012

STUDY GUIDE SPRING 2012
Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
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1. The number of atoms in a mole of any pure substance is called
a. its atomic number.
c. its mass number.
b. Avogadro’s number.
d. its gram-atomic number.
2. What can be said about 1 mol Ag and 1 mol Au?
a. They are equal in mass.
b. They contain the same number of atoms.
c. Their molar masses are equal.
d. They have the same atomic mass.
3. An Avogadro’s number of any element is equivalent to
a. the atomic number of that element.
c. 6.022  1023 particles.
b. the mass number of that element.
d. 12 g of that element.
+
4. If 0.500 mol of Na combines with 0.500 mol of Cl– to form NaCl, how many formula units of NaCl are
present?
a. 3.01  1023
c. 6.02  1024
23
b. 6.02  10
d. 1.00
5. Using a periodic table, what is the average atomic mass of zinc?
a. 69.723 amu
c. 63.546 amu
b. 58.693 amu
d. 65.39 amu
6. The atomic mass of hydrogen is 1.008 amu. The reason that this value is not a whole number is that
a. hydrogen only exists as a diatomic molecule.
b. the mass of hydrogen is the sum of the masses of the protons and electrons in the atom.
c. the mass of a proton is not exactly equal to 1 amu.
d. hydrogen has more than one isotope.
7. A chemical formula includes the symbols of the elements in the compound and subscripts that indicate
a. the number of formula units present.
b. the number of atoms or ions of each type.
c. the formula mass.
d. the charges on the elements or ions.
8. How many atoms of fluorine are in a molecule of carbon tetrafluoride, CF4?
a. 1
c. 4
b. 2
d. 5
9. Changing a subscript in a correctly written chemical formula
a. changes the number of moles represented by the formula.
b. changes the charges on the other ions in the compound.
c. changes the formula so that it no longer represents that compound.
d. has no effect on the formula.
10. A formula that shows the simplest whole-number ratio of the atoms in a compound is the
a. molecular formula.
c. structural formula.
b. ideal formula.
d. empirical formula.
11. The molar mass of an element is the mass of one
a. atom of the element.
c. gram of the element.
b. liter of the element.
d. mole of the element.
12. To determine the molar mass of an element, one must know the element’s
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____ 15.
____ 16.
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____ 18.
____ 19.
____ 20.
____ 21.
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____ 23.
____ 24.
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____ 26.
____ 27.
a. Avogadro number.
c. number of isotopes.
b. atomic number.
d. average atomic mass.
What is the molar mass of magnesium?
a. 12.00 g
c. 24.305 g
b. 26.982 g
d. 22.990 g
What is the empirical formula for a compound that is 31.9% potassium, 28.9% chlorine, and 39.2% oxygen?
a. KClO2
c. K2Cl2O3
b. KClO3
d. K2Cl2O5
What is the empirical formula for a compound that is 43.6% phosphorus and 56.4% oxygen?
a. P3O7
c. P2O3
b. PO3
d. P2O5
What is the empirical formula for a compound that is 53.3% O and 46.7% Si?
a. SiO
c. Si2O
b. SiO2
d. Si2O3
A compound contains 259.2 g of F and 40.8 g of C. What is the empirical formula for this compound?
a. CF4
c. CF
b. C4F
d. CF2
A compound contains 64 g of O and 4 g of H. What is the empirical formula for this compound?
a. H2O
c. H4O4
b. H2O2
d. HO
What is the empirical formula for a compound that is 36.1% Ca and 63.9% Cl?
a. CaCl
c. CaCl2
b. Ca2Cl
d. Ca2Cl2
A compound contains 27.3 g of C and 72.7 g of O. What is the empirical formula for this compound?
a. CO
c. C2O
b. CO2
d. C2O4
To find the molecular formula from the empirical formula, one must determine the compound’s
a. density.
c. structural formula.
b. formula mass.
d. crystal lattice.
A molecular compound has the empirical formula XY3. Which of the following is a possible molecular
formula?
a. X2Y3
c. X2Y5
b. XY4
d. X2Y6
The molecular formula for vitamin C is C6H8O6. What is the empirical formula?
a. CHO
c. C3H4O3
b. CH2O
d. C2H4O2
A compound’s empirical formula is NO2. If the formula mass is 92 amu, what is the molecular formula?
a. NO
c. NO2
b. N2O2
d. N2O4
What is the percentage composition of CF4?
a. 20% C, 80% F
c. 16.8% C, 83.2% F
b. 13.6% C, 86.4% F
d. 81% C, 19% F
What is the percentage composition of CuCl2?
a. 33% Cu, 66% Cl
c. 65.50% Cu, 34.50% Cl
b. 50% Cu, 50% Cl
d. 47.267% Cu, 52.733% Cl
The percentage of sulfur in SO2 is about 50%. What is the percentage of oxygen in this compound?
a. 25%
c. 75%
b. 50%
d. 90%
____ 28. What is the percentage of OH– in Ca(OH)2?
a. 45.9%
c. 75%
b. 66.6%
d. 90.1%
____ 29. Knowledge about what products are produced in a chemical reaction is obtained by
a. inspecting the chemical equation.
c. laboratory analysis.
b. balancing the chemical equation.
d. writing a word equation.
____ 30. A chemical reaction has NOT occurred if the products have
a. the same mass as the reactants.
b. more energy than the reactants.
c. less energy than the reactants.
d. the same chemical properties as the reactants.
____ 31. Which observation does NOT indicate that a chemical reaction has occurred?
a. formation of a precipitate
c. evolution of energy
b. production of a gas
d. change in total mass of substances
____ 32. The word equation solid carbon + oxygen gas  carbon dioxide gas + energy, represents a chemical reaction
because
a. the reaction releases energy.
b. CO2 has chemical properties that differ from those of C and O.
c. the reaction absorbs energy.
d. CO2 is a gas and carbon is a crystal.
____ 33. In the unbalanced formula equation CO + O2  CO2 + energy, energy
a. is absorbed.
c. is released.
b. can be considered a reactant.
d. Both (a) and (b)
____ 34. The word equation for the formula equation shown is
C2H5OH + O2  CO2 + H2O + energy
a. carbon dioxide + water  ethanol + oxygen + energy.
b. ethanol + oxygen  carbon dioxide + water + energy.
c. ethanol + oxygen + energy  carbon dioxide + water.
d. ethanol + oxygen + energy  carbon dioxide + water + energy.
____ 35. The state of matter for a reactant or a product in a chemical equation is indicated by a
a. coefficient before the formula.
c. symbol after the formula.
b. subscript after the formula.
d. superscript after the formula.
____ 36. The reaction, C2H5OH + 3O2
2CO2 + 3H2O, will occur most rapidly if
a. C2H5OH is a liquid and O2 is a liquid.
c. CO2 is a gas and H2O is a liquid.
b. C2H5OH and O2 are in close contact.
d. CO2 is a gas and H2O is a gas.
____ 37. An insoluble solid produced by a chemical reaction in solution is called
a. a precipitate.
c. a molecule.
b. a reactant.
d. the mass of the product.
____ 38. How would oxygen be represented in the formula equation for the reaction of methane and oxygen to yield
carbon dioxide and water?
a. oxygen
c. O2
b. O
d. O3
____ 39. The products of the reaction, C2H5OH + 3O2  2CO2 + 3H2O have the same _____ as the reactants.
a. atoms.
c. molecules.
b. coefficients.
d. subscripts.
____ 40. After the correct formula for a reactant in an equation has been written, the
a. subscripts are adjusted to balance the equation.
b. formula should not be changed.
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____ 54.
c. same formula must appear as the product.
d. symbols in the formula must not appear on the product side of the equation.
To balance a chemical equation, it may be necessary to adjust the
a. coefficients.
c. formulas of the products.
b. subscripts.
d. number of products.
A chemical equation is balanced when the
a. coefficients of the reactants equal the coefficients of the products.
b. same number of each kind of atom appears in the reactants and in the products.
c. products and reactants are the same chemicals.
d. subscripts of the reactants equal the subscripts of the products.
After the first steps in writing an equation, the equation is balanced by
a. adjusting subscripts to the formula(s).
b. adjusting coefficients to the smallest whole-number ratio.
c. changing the products formed.
d. making the number of reactants equal to the number of products.
What is the balanced equation when aluminum reacts with copper(II) sulfate?
a. Al + Cu2S  Al2S + Cu
c. Al + CuSO4  AlSO4 + Cu
b. 2Al + 3CuSO4  Al2(SO4)3 + 3Cu
d. 2Al + Cu2SO4  Al2SO4 + 2Cu
Which coefficients correctly balance the formula equation CaCO3(s)  CaO(s) + CO2(g)?
a. 1, 1, 1
c. 2, 6, 3
b. 1, 3, 1
d. 3, 1, 2
Which equation is NOT balanced?
a. 2H2 + O2  2H2O
c. H2 + H2 + O2  H2O + H2O
b. 4H2 + 2O2  4H2O
d. 2H2 + O2  H2O
Which coefficients correctly balance the formula equation NH4NO2  N2 + H2O?
a. 1, 2, 2
c. 2, 1, 1
b. 1, 1, 2
d. 2, 2, 2
Which coefficients correctly balance the formula equation CaO + H2O  Ca(OH)2?
a. 2, 1, 2
c. 1, 2, 1
b. 1, 2, 3
d. 1, 1, 1
Which coefficients correctly balance the formula equation
Zn(OH)2 + CH3COOH  Zn(CH3COO)2 + H2O?
a. 1, 2, 1, 1
c. 1, 2, 1, 2
b. 2, 1, 2, 1
d. 2, 1, 1, 2
A reaction of a hydrocarbon, in which carbon dioxide and water are produced, is classified as a
a. decomposition reaction.
c. double-displacement reaction.
b. combustion reaction.
d. synthesis reaction.
In what kind of reaction do two or more substances combine to form a new compound?
a. decomposition reaction
c. double-displacement reaction
b. ionic reaction
d. synthesis reaction
The equation A + X  AX is the general equation for a(n)
a. combustion reaction.
c. synthesis reaction.
b. ionic reaction.
d. double-displacement reaction.
In what kind of reaction does a single compound produce two or more simpler substances?
a. decomposition reaction
c. displacement reaction
b. synthesis reaction
d. ionic reaction
The reaction 2KClO3(s)  2KCl(s) + 3O2(g) is a(n)
____ 55.
____ 56.
____ 57.
____ 58.
____ 59.
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____ 62.
____ 63.
____ 64.
____ 65.
____ 66.
a. synthesis reaction.
c. combustion reaction.
b. decomposition reaction.
d. ionic reaction.
In what kind of reaction does one element replace a similar element in a compound?
a. displacement reaction
c. decomposition reaction
b. combustion
d. ionic reaction
The equation A + BX  AX + B is the general equation for a
a. double-displacement reaction.
c. displacement reaction.
b. decomposition reaction.
d. combustion reaction.
The reaction Cl2(g) + 2KBr(aq)  2KCl(aq) + Br2(l) is a(n)
a. synthesis reaction.
c. displacement reaction.
b. ionic reaction.
d. combustion reaction.
What is the name of a list of elements arranged according to the ease with which they undergo certain
chemical reactions?
a. reactivity list
c. activity series
b. reaction sequence
d. periodic list
An element in the activity series can replace any element
a. in the periodic table.
c. above it on the list.
b. below it on the list.
d. in its group.
What can be predicted by using an activity series?
a. whether a certain chemical reaction will occur
b. the amount of energy released by a chemical reaction
c. the electronegativity values of elements
d. the melting points of elements
If metal X is lower than metal Y in the activity series, then metal X
a. replaces ions of metal Y in a solution.
b. is more active than metal Y.
c. is less active than metal Y.
d. forms positive ions more readily than does metal Y.
A precipitate forms in a double-displacement reaction when
a. hydrogen gas reacts with a metal.
b. positive ions combine with negative ions.
c. water boils out of the solution.
d. a gas escapes.
A balanced chemical equation allows one to determine the
a. mole ratio of any two substances in the reaction.
b. energy released in the reaction.
c. electron configuration of all elements in the reaction.
d. mechanism involved in the reaction.
The coefficients in a chemical equation represent the
a. masses, in grams, of all reactants and products.
b. relative numbers of moles of reactants and products.
c. number of atoms in each compound in a reaction.
d. number of valence electrons involved in the reaction.
How many mole ratios can be correctly obtained from the chemical equation 2NO  N2 + O2?
a. 1
c. 4
b. 3
d. 6
In the reaction Ca + Cl2  CaCl2, what is the mole ratio of chlorine to calcium chloride?
a. 2:3
c. 1:2
____ 67.
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____ 72.
____ 73.
____ 74.
____ 75.
____ 76.
____ 77.
____ 78.
b. 2:1
d. 1:1
In the reaction N2 + 3H2  2NH3, what is the mole ratio of nitrogen to ammonia?
a. 1:1
c. 1:3
b. 1:2
d. 2:3
In the reaction 2H2 + O2  2H2O, what is the mole ratio of oxygen to water?
a. 1:2
c. 8:1
b. 2:1
d. 1:4
What is the mole ratio of oxygen to phosphorus(V) oxide in the reaction P4(s) + 5O2(g)  P4O10(s)?
a. 1:1
c. 5:1
b. 1:5
d. 4:10
In the chemical equation wA + xB  yC + zD, if one knows the mass of A and the molar masses of A, B, C,
and D, one can determine
a. the mass of any of the reactants or products.
b. the mass of B only.
c. the total mass of C and D only.
d. the total mass of A and B only.
If one knows the mass and molar mass of reactant A and the molar mass of product D in a chemical reaction,
one can determine the mass of product D produced by using the
a. mole ratio of D to A from the chemical equation.
b. group numbers of the elements of A and D in the periodic table.
c. estimating bond energies involved in the reaction.
d. electron configurations of the atoms in A and D.
What is needed to calculate the mass of ammonia gas produced from 2.0 L of nitrogen gas in excess hydrogen
gas in the reaction below?
N2(g) + 3H2(g)  2NH3(g)
a. one molar mass and one mole ratio
b. one molar masses and two mole ratios
c. two molar masses, one density, and one mole ratio
d. two densities, two molar masses, and two mole ratios
A chemical reaction involving substances A and B stops when B is completely used. B is the
a. excess reactant.
c. primary reactant.
b. limiting reactant.
d. primary product.
The substance that restricts the participation of other reactants in a chemical reaction is known as the
a. limiting reactant.
c. excess reactant.
b. limiting product.
d. excess product.
The substance not completely used up in a chemical reaction is known as the
a. limiting reactant.
c. excess reactant.
b. limiting product.
d. excess product.
To determine the limiting reactant in a chemical reaction, one must know the
a. available amount of one of the reactants.
b. amount of product formed.
c. available amount of each reactant.
d. speed of the reaction.
What is the ratio of the actual yield to the theoretical yield, multiplied by 100%?
a. mole ratio
c. molar yield
b. percentage yield
d. excess yield
What is the measured amount of a product obtained from a chemical reaction?
a. mole ratio
c. theoretical yield
____ 79.
____ 80.
____ 81.
____ 82.
____ 83.
____ 84.
____ 85.
____ 86.
____ 87.
b. percentage yield
d. actual yield
Actual yield must be determined by
a. experiments.
c. theoretical yield.
b. calculations.
d. estimation.
The actual yield of a chemical reaction is
a. less than the theoretical yield.
c. equal to the percentage yield.
b. greater than the theoretical yield.
d. greater than the percentage yield.
For the reaction SO3 + H2O  H2SO4, calculate the percentage yield if 500. g of sulfur trioxide react with
excess water to produce 575 g of sulfuric acid.
a. 82.7%
c. 91.2%
b. 88.3%
d. 93.9%
For the reaction Cl2 + 2KBr  2KCl + Br2, calculate the percentage yield if 200. g of chlorine react with
excess potassium bromide to produce 410. g of bromine.
a. 73.4%
c. 90.9%
b. 82.1%
d. 98.9%
For the reaction 2Na + 2H2O  2NaOH + H2, calculate the percentage yield if 80. g of water react with
excess sodium to produce 4.14 g of hydrogen.
a. 87%
c. 92%
b. 89%
d. 98%
For the reaction 2Na + Cl2  2NaCl, calculate the percentage yield if 200. g of chlorine react with excess
sodium to produce 240. g of sodium chloride.
a. 61.2%
c. 83.4%
b. 72.8%
d. 88.4%
In the chemical equation wA + xB  yC + zD, how many correct mole ratios can be obtained that relate only
the products?
a. 1
c. 4
b. 2
d. 6
In the chemical equation wA + xB  yC + zD, a comparison of the number of moles of A to the number of
moles of C would be a
a. mass ratio.
c. electron ratio.
b. mole ratio.
d. energy proportion.
In the reaction, CH4(g) + 2O2(g)  CO2(g) + 2H2O(g), a mass of 25 g CO2 is produced by reacting methane
with excess oxygen. The following expression calculates the
a. mass of water produced.
c. minimum mass of oxygen needed.
b. moles of carbon dioxide produced.
d. moles of methane consumed.
____ 88. To determine the limiting reactant in a chemical reaction involving known masses of the two reactants, A and
B, which of the following calculations would be the most useful?
a. determining the masses of 100 mol A and 100 mol B
b. finding the masses of the products
c. calculating bond energies
d. calculating the mass of a single product formed from each reactant
____ 89. For the reaction CH4(g) + 2O2(g)  CO2(g) + 2H2O(g), calculate the percentage yield of carbon dioxide if
1000. g of methane react with excess oxygen to produce 2300. g of carbon dioxide.
a. 83.88%
c. 92.76%
b. 89.14%
d. 96.78%
Completion
Complete each sentence or statement.
90. If you have 1.204  1024 atoms of nickel, you have ____________________ as the amount of nickel.
91. The conversion factor used to change moles to number of particles is _________________________.
92. The average atomic mass of cobalt is ____________________.
93. Comparing the average atomic masses of copper and zinc, the average atomic mass of
____________________ is larger.
94. The empirical formula for a compound shows the symbols of the elements with subscripts indicating the
________________________________________.
95. In one mole of acetic acid, CH3COOH, there are ____________________ moles of hydrogen atoms.
96. Two moles of carbon atoms are present in ______________________________ of C6H6.
97. The molar mass of barium nitrate, Ba(NO3)2, is ____________________.
98. The first step in finding an empirical formula from percentage composition is to assume that you have
____________________ grams of sample.
99. To find an empirical formula from percentage composition, you must divide the number of grams of each
element by that element’s ____________________.
100. A compound’s empirical formula is N2O5. If the formula mass is 108 amu, its molecular formula is
____________________.
101. A compound’s empirical formula is CH3. If the formula mass is 30 amu, its molecular formula is
____________________.
102. To calculate the percentage composition of NiCl2, you need to know
___________________________________.
103. A solid produced by a chemical reaction that then separates from the solution is called a(n)
____________________.
104. In writing a formula equation for a reaction that produces hydrogen gas, the correct representation of
hydrogen gas is ____________________.
105. The mass of the products of the reaction C2H5OH + 3O2  2CO2 + 3H2O equals the mass of the reactants
because the products are made up of the same ____________________ as the reactants.
106. In an equation, the symbol for a substance in water solution is ____________________.
107. When the formula equation Fe3O4 + Al  Al2O3 + Fe is correctly balanced, the coefficient of Fe is
____________________.
108. When the formula equation H2(g) + Cl2(g)  HCl(g) is correctly balanced, the coefficient of HCl is
____________________.
109. When the formula equation CuSO4(aq) + Fe(s)  Fe2(SO4)3(aq) + Cu(s) is correctly balanced, the coefficient
of CuSO4(aq) is ____________________.
110. The reaction 2HgO(s)  2Hg(l) + O2(g) is classified as a(n) ____________________ reaction.
111. The equation AX  A + X is the general equation for a(n) ____________________ reaction.
112. The reaction Mg(s) + 2HCl(aq)  H2(g) + MgCl2(aq) is classified as a(n) ____________________ reaction.
113. When placed in water, a metal more active than hydrogen will form two substances, a metal hydroxide and
____________________ gas.
114. In a(n) ____________________ reaction, ions of two compounds exchange places in aqueous solution to
form new compounds.
115. Ions that are present in solution in which a reaction is taking place but that do not participate in the reaction
are called ____________________.
116. In the chemical equation 2AlCl3(aq) + 3Pb(NO3)2(aq)  3PbCl2(s) + 2Al(NO3)2(aq), the spectator ions are
____________________ and ____________________.
117. The ratios obtained from the coefficients of substances in a balanced chemical equations are called
____________________ because they can be used to convert moles of one substance to moles of another
substance.
118. The unit of the following expression is ____________________.
119. The unit of the following expression is ____________________.
120. The expression below converts the quantity, mass HCl, to the quantity, ____________________.
121. The conversion factor
can be used to find the ____________________ of water if you know its
mass.
122. The expression below converts the quantity, volume C5H12, to the quantity, ____________________.
123. The expression below can be used to find the ____________________ of 1016 molecules of CCl4.
124. The substance that controls the quantity of product than can be formed in a chemical reaction is the
____________________.
125. The substance that is not used up completely in a chemical reaction is the ____________________.
126. Almost all of the gas inside an inflated automobile safety air bag is molecular ____________________.
127. The function of the carburetor in a small internal combustion engine is to control the ratio of
____________________ to oxygen.
128. One of the functions of a(n) _________________________ is to increase the rate of the decomposition of
NO(g) and NO2(g) found in the exhaust gases of a car into N2(g) and O2(g).
129. The proportions of the reactants and products involved in a chemical reaction are shown by the
____________________ in the balanced chemical equation describing the reaction.
130. In the equation N2 + 3H2  2NH3, the ratio 2:1 relates mol NH3 to mol ____________________.
131. In the equation N2 + 3H2  2NH3, the mole ratio of N2 to H2 is ____________________.
132. In the equation N2 + 3H2  2NH3, the mole ratio of NH3 to N2 is ____________________.
133. The unit of the expression mol H2O  molar mass H2O is ____________________.
134. The expression below converts the quantity, mass HCl, to the quantity, ____________________.
135. Unwanted reactions that can use up reactants without making the desired products are called
____________________ reactions
136. If 2 moles of each reactant are available for the reaction described by the following equation,
SiO2(s) + 3C(s)  SiC(s) + 2CO(g),
____________________ is the substance that is the limiting reactant.
137. The efficiency of a reaction is described by the ____________________ yield.
138. In an operating car engine, the least fuel-oxygen ratio should occur when the car’s engine is
____________________.
139. Reactions that are started by the sun’s ultraviolet light and involve nitrogen oxides emitted from car engines
form ____________________ smog.
Problem
140. The mass of 1 mol of gold atoms is 196.97 g. Find the mass of 1 atom of gold.
141. How many moles of copper are present in 180.0 g Cu?
142. How many moles of oxygen atoms are present in 2.0 grams of oxygen gas, O2?
143. Argentite is a silver ore that contains 87% silver and 13% sulfur. What is the empirical formula for argentite?
144. Calculate the percentage of sulfur in CuSO4.
145. Calculate the percentage of oxygen in Fe2SiO4.
146. Calculate the percentage of aluminum in Al2O3.
147. Write a balanced chemical equation for the following reaction. iron plus copper(I) nitrate yields iron(II)
nitrate plus copper.
148. Write a balanced chemical equation for the following reaction. mercury(II) oxide (heated) yields mercury +
oxygen
149. Write a balanced chemical equation for the following chemical reaction.
methane + oxygen  carbon dioxide + water
150. Write a balanced equation for the synthesis of liquid phosphorus trichloride, PCl3, from white phosphorus, P4,
and chlorine gas.
151. Tell what type of chemical reaction is represented by the following chemical equation. Then balance the
equation.
C3H8(g) + O2(g)
CO2(g) + H2O(l)
152. Write the total ionic equation and net ionic equation for the reaction of sodium hydroxide and potassium
bromide. Refer to Table 1.
153. Write the total ionic equation and net ionic equation for the reaction of silver nitrate and potassium chloride.
Refer to Table 1.
154. How many grams of ammonium sulfate can be produced if 30.0 mol of H2SO4 react with excess NH3
according to the equation 2NH3(aq) + H2SO4(aq)  (NH4)2SO4(aq)?
155. What mass in grams of sodium hydroxide is produced if 20.0 g of sodium metal react with excess water
according to the chemical equation
2Na(s) + 2H2O(l)  2NaOH(aq) + H2(g)?
156. How many silver atoms can be produced if 0.00350 g of Cu are reacted with excess AgNO3 according to the
equation Cu(s) + 2AgNO3(aq)  2Ag(s) + Cu(NO3)2(aq)?
157. In the decomposition of hydrogen peroxide, the percentage yield of oxygen is 93.0%. What is the actual yield
in grams of oxygen if you start with 100. g of H2O2? The reaction proceeds according to the equation
2H2O2(l)  2H2O(l) + O2(g).
158. The chemical reaction for the generation of gas in an automobile safety air bag is
2NaN3(s)  2Na(s) + 3N2(g).
What volume of gas is produced if there are 130.0 grams of NaN3 used in the reaction? (The density of
nitrogen gas is 0.916 g/L.)
159. Sulfur in gasoline can produce sulfuric acid, H2SO4, according to the two-step process shown below. For each
125 g of sulfur in gasoline, how many moles of H2SO4 will be produced? S(s) + O2(g)  SO2(g)
2SO2(g) + 2H2O(l) + O2(g)  2H2SO4(aq)
STUDY GUIDE SPRING 2012
Answer Section
MULTIPLE CHOICE
1.
2.
3.
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5.
6.
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9.
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11.
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40.
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B
B
C
A
D
D
B
C
C
D
D
D
C
B
D
B
A
D
C
B
B
D
C
D
B
D
B
A
C
D
D
B
C
B
C
B
A
C
A
B
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1
1
1
3
1
1
1
2
1
1
1
2
3
3
3
3
3
2
3
3
3
2
3
3
3
3
2
3
1
1
1
1
1
1
1
1
1
1
1
1
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1
1
1
1
2
2
2
2
2
3
2
2
2
3
3
3
3
3
3
3
3
3
3
3
3
3
3
3
1
1
1
1
1
1
1
1
1
2
2
2
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1
1
2
2
1
1
2
2
2
1
3
3
3
1
1
1
1
1
1
1
2
2
2
2
3
3
3
3
1
1
1
2
2
2
3
3
3
1
1
2
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86.
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A
B
B
B
A
D
B
D
C
B
D
C
A
B
A
C
C
C
B
A
C
B
A
B
D
D
B
A
C
A
A
C
B
A
C
C
B
D
A
A
D
C
C
B
B
B
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1
1
2
2
1
2
2
2
3
1
1
2
1
1
1
2
2
1
1
2
2
1
1
1
2
1
1
1
1
1
1
2
2
1
1
2
1
1
1
1
2
2
2
2
2
1
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2
2
2
2
2
2
2
2
2
3
3
3
3
3
3
3
3
3
3
3
3
3
1
1
1
1
1
1
1
1
1
1
2
2
2
2
2
2
2
2
2
2
2
2
1
1
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2
2
2
2
2
2
2
2
2
1
2
2
3
3
4
4
4
4
4
4
4
5
1
1
1
1
1
1
1
3
3
4
1
1
1
1
2
2
2
2
2
2
2
2
1
1
87. ANS: D
88. ANS: D
89. ANS: A
DIF: 2
DIF: 1
DIF: 2
REF: 1
REF: 2
REF: 2
COMPLETION
90. ANS: two moles
DIF: 2
REF: 1
23
91. ANS: 6.022  10 particles/1 mol
OBJ: 2
DIF: 2
92. ANS: 58.93 amu
REF: 1
OBJ: 3
DIF: 1
93. ANS: copper
REF: 2
OBJ: 1
DIF: 2
REF: 2
OBJ: 1
94. ANS: smallest whole-number ratio of the atoms
DIF: 1
95. ANS: four
REF: 2
OBJ: 2
DIF: 2
96. ANS:
0.33 mol
one-third mole
REF: 2
OBJ: 2
DIF: 2
REF: 2
97. ANS: 261.35 g/mol
OBJ: 2
DIF: 3
98. ANS: 100.00
REF: 2
OBJ: 3
DIF: 1
99. ANS: molar mass
REF: 3
OBJ: 1
DIF: 2
100. ANS: N2O5
REF: 3
OBJ: 1
DIF: 3
101. ANS: C2H6
REF: 3
OBJ: 2
DIF: 3
REF: 3
OBJ: 2
102. ANS: the molar masses of Ni, Cl, and NiCl2
DIF: 2
103. ANS: precipitate
REF: 3
OBJ: 3
OBJ: 3
OBJ: 1
OBJ: 2
DIF: 1
104. ANS: H2(g)
REF: 1
OBJ: 1
DIF: 1
105. ANS: atoms
REF: 1
OBJ: 1
DIF: 1
106. ANS: (aq)
REF: 2
OBJ: 1
DIF: 1
107. ANS: 9
REF: 1
OBJ: 3
DIF: 2
108. ANS: 2
REF: 2
OBJ: 2
DIF: 2
109. ANS: 3
REF: 2
OBJ: 2
DIF: 2
REF: 2
110. ANS: decomposition
OBJ: 2
DIF: 2
REF: 3
111. ANS: decomposition
OBJ: 3
DIF: 2
REF: 3
112. ANS: displacement
OBJ: 3
DIF: 2
113. ANS: hydrogen
REF: 3
OBJ: 4
DIF: 1
REF: 3
114. ANS: double-displacement
OBJ: 4
DIF: 1
REF: 3
115. ANS: spectator ions
OBJ: 5
DIF: 1
116. ANS: Al3+,
REF: 4
OBJ: 2
DIF: 2
117. ANS: mole ratios
REF: 4
OBJ: 2
DIF: 1
118. ANS: mol H2O
REF: 1
OBJ: 2
DIF: 1
119. ANS: mol H2O
REF: 1
OBJ: 3
DIF: 2
REF: 1
OBJ: 3
120. ANS: mass Cl2
DIF: 1
121. ANS: volume
REF: 1
OBJ: 3
DIF: 1
122. ANS: mass H2
REF: 1
OBJ: 4
DIF: 2
123. ANS: mass
REF: 1
OBJ: 4
DIF: 2
REF: 1
124. ANS: limiting reactant
OBJ: 5
DIF: 1
REF: 2
125. ANS: excess reactant
OBJ: 1
DIF: 1
126. ANS: nitrogen
REF: 2
OBJ: 1
DIF: 1
127. ANS: fuel
REF: 3
OBJ: 1
DIF: 1
REF: 3
128. ANS: catalytic converter
OBJ: 2
DIF: 1
129. ANS: coefficients
REF: 3
OBJ: 3
DIF: 1
130. ANS: N2
REF: 1
OBJ: 1
DIF: 1
131. ANS: 1:3
REF: 1
OBJ: 1
DIF: 1
132. ANS: 2:1
REF: 1
OBJ: 1
DIF: 1
133. ANS: g H2O
REF: 1
OBJ: 1
DIF: 1
134. ANS: mol Cl2
REF: 1
OBJ: 3
DIF: 2
135. ANS: side
REF: 1
OBJ: 3
DIF: 1
136. ANS: carbon (C)
REF: 2
OBJ: 1
DIF: 1
137. ANS: percentage
REF: 2
OBJ: 1
DIF: 1
138. ANS: idling
REF: 2
OBJ: 2
DIF: 1
REF: 3
139. ANS: photochemical
OBJ: 2
DIF: 1
REF: 3
OBJ: 3
DIF: 3
141. ANS:
REF: 1
OBJ: 2
DIF: 2
142. ANS:
REF: 1
OBJ: 3
DIF: 2
143. ANS:
REF: 1
OBJ: 3
PROBLEM
140. ANS:
2 mol Ag: 1 mol S; Ag2S
DIF: 3
144. ANS:
REF: 3
OBJ: 1
DIF: 3
145. ANS:
REF: 3
OBJ: 3
DIF: 3
146. ANS:
REF: 3
OBJ: 3
DIF: 3
REF: 3
147. ANS:
Fe + 2CuNO3  Fe(NO3)2 + 2Cu
OBJ: 3
DIF: 2
148. ANS:
OBJ: 2
2HgO
REF: 2
2Hg + O2
DIF: 2
REF: 2
149. ANS:
CH4 + 2O2  CO2 + 2H2O
OBJ: 2
DIF: 2
REF: 2
150. ANS:
P4(s) + 6Cl2(g)  4PCl3(l)
OBJ: 2
DIF: 2
151. ANS:
OBJ: 2
REF: 2
combustion, C3H8(g) + 5O2(g)
3CO2(g) + 4H2O(l)
DIF: 3
REF: 3
OBJ: 1
152. ANS:
Balanced KBr(aq) + NaOH(aq)  KOH(aq) + NaBr(aq)
Total ionic K+(aq) + Br–(aq) + Na+(aq) + OH–(aq)  K+(aq) + OH–(aq) + Na+(aq) + Br–(aq)
Net ionic none
DIF: 3
REF: 4
OBJ: 4
153. ANS:
Balanced AgNO3(aq) + KCl(aq)  AgCl(s) + KNO3(aq)
Total ionic Ag+(aq) +
(aq) + K+(aq) + Cl–(aq)  AgCl(s) + K+(aq) +
Net ionic Ag+(aq) + Cl–(aq)  AgCl(s)
DIF: 3
154. ANS:
REF: 4
OBJ: 4
DIF: 3
REF: 1
OBJ: 3
(aq)
155. ANS:
DIF: 2
156. ANS:
REF: 1
OBJ: 3
DIF: 2
157. ANS:
REF: 1
OBJ: 5
DIF: 2
158. ANS:
REF: 2
OBJ: 2
DIF: 2
159. ANS:
REF: 3
OBJ: 1
DIF: 2
REF: 3
OBJ: 3