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.

____ 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 b. 6.02  1023 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 c. changes the formula so that it no longer represents that compound.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 a. Avogadro number. c. number of isotopes. b. atomic number. d. average atomic mass. ____ 13. What is the molar mass of magnesium? a. 12.00 g c. 24.305 g b. 26.982 g d. 22.990 g ____ 14. 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 ____ 15. 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 ____ 16. 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 ____ 17. 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 ____ 18. 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 ____ 19. 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 ____ 20. 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 ____ 21. 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.

____ 22. 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

____ 23. The molecular formula for vitamin C is C6H8O6. What is the empirical formula? a. CHO c. C3H4O3 b. CH2O d. C2H4O2

____ 24. 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

____ 25. 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

____ 26. 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

____ 27. 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. c. same formula must appear as the product. d. symbols in the formula must not appear on the product side of the equation. ____ 41. 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. ____ 42. 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. ____ 43. 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. ____ 44. 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

____ 45. 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 ____ 46. Which equation is NOT balanced?

a. 2H2 + O2  2H2O c. H2 + H2 + O2  H2O + H2O

b. 4H2 + 2O2  4H2O d. 2H2 + O2  H2O

____ 47. 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

____ 48. 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 ____ 49. 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 ____ 50. 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. ____ 51. 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 ____ 52. 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. ____ 53. 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

____ 54. The reaction 2KClO3(s)  2KCl(s) + 3O2(g) is a(n) a. synthesis reaction. c. combustion reaction. b. decomposition reaction. d. ionic reaction. ____ 55. 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 ____ 56. 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.

____ 57. 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. ____ 58. 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 ____ 59. 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. ____ 60. 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 ____ 61. 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. ____ 62. 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. ____ 63. 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. ____ 64. 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.

____ 65. How many mole ratios can be correctly obtained from the chemical equation 2NO  N2 + O2? a. 1 c. 4 b. 3 d. 6

____ 66. In the reaction Ca + Cl2  CaCl2, what is the mole ratio of chlorine to calcium chloride? a. 2:3 c. 1:2 b. 2:1 d. 1:1

____ 67. 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

____ 68. 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

____ 69. 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 ____ 70. 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. ____ 71. 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. ____ 72. 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 ____ 73. 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. ____ 74. 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. ____ 75. 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. ____ 76. 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. ____ 77. 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 ____ 78. What is the measured amount of a product obtained from a chemical reaction? a. mole ratio c. theoretical yield b. percentage yield d. actual yield ____ 79. Actual yield must be determined by a. experiments. c. theoretical yield. b. calculations. d. estimation. ____ 80. 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.

____ 81. 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%

____ 82. 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%

____ 83. 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%

____ 84. 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% ____ 85. 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 ____ 86. 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.

____ 87. 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

122. The expression below converts the quantity, volume C5H12, to the quantity, ______.

16 123. The expression below can be used to find the ______of 10 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. ANS: B DIF: 1 REF: 1 OBJ: 1 2. ANS: B DIF: 1 REF: 1 OBJ: 1 3. ANS: C DIF: 1 REF: 1 OBJ: 2 4. ANS: A DIF: 3 REF: 1 OBJ: 2 5. ANS: D DIF: 1 REF: 2 OBJ: 1 6. ANS: D DIF: 1 REF: 2 OBJ: 1 7. ANS: B DIF: 1 REF: 2 OBJ: 2 8. ANS: C DIF: 2 REF: 2 OBJ: 2 9. ANS: C DIF: 1 REF: 2 OBJ: 2 10. ANS: D DIF: 1 REF: 3 OBJ: 1 11. ANS: D DIF: 1 REF: 2 OBJ: 3 12. ANS: D DIF: 2 REF: 2 OBJ: 3 13. ANS: C DIF: 3 REF: 2 OBJ: 3 14. ANS: B DIF: 3 REF: 3 OBJ: 1 15. ANS: D DIF: 3 REF: 3 OBJ: 1 16. ANS: B DIF: 3 REF: 3 OBJ: 1 17. ANS: A DIF: 3 REF: 3 OBJ: 1 18. ANS: D DIF: 2 REF: 3 OBJ: 1 19. ANS: C DIF: 3 REF: 3 OBJ: 1 20. ANS: B DIF: 3 REF: 3 OBJ: 1 21. ANS: B DIF: 3 REF: 3 OBJ: 2 22. ANS: D DIF: 2 REF: 3 OBJ: 2 23. ANS: C DIF: 3 REF: 3 OBJ: 2 24. ANS: D DIF: 3 REF: 3 OBJ: 2 25. ANS: B DIF: 3 REF: 3 OBJ: 3 26. ANS: D DIF: 3 REF: 3 OBJ: 3 27. ANS: B DIF: 2 REF: 3 OBJ: 3 28. ANS: A DIF: 3 REF: 3 OBJ: 3 29. ANS: C DIF: 1 REF: 1 OBJ: 1 30. ANS: D DIF: 1 REF: 1 OBJ: 1 31. ANS: D DIF: 1 REF: 1 OBJ: 1 32. ANS: B DIF: 1 REF: 1 OBJ: 2 33. ANS: C DIF: 1 REF: 1 OBJ: 2 34. ANS: B DIF: 1 REF: 1 OBJ: 2 35. ANS: C DIF: 1 REF: 1 OBJ: 3 36. ANS: B DIF: 1 REF: 1 OBJ: 3 37. ANS: A DIF: 1 REF: 1 OBJ: 3 38. ANS: C DIF: 1 REF: 2 OBJ: 1 39. ANS: A DIF: 1 REF: 2 OBJ: 1 40. ANS: B DIF: 1 REF: 2 OBJ: 2 41. ANS: A DIF: 1 REF: 2 OBJ: 2 42. ANS: B DIF: 1 REF: 2 OBJ: 2 43. ANS: B DIF: 2 REF: 2 OBJ: 2 44. ANS: B DIF: 2 REF: 2 OBJ: 2 45. ANS: A DIF: 1 REF: 2 OBJ: 2 46. ANS: D DIF: 2 REF: 2 OBJ: 2 47. ANS: B DIF: 2 REF: 2 OBJ: 2 48. ANS: D DIF: 2 REF: 2 OBJ: 2 49. ANS: C DIF: 3 REF: 2 OBJ: 2 50. ANS: B DIF: 1 REF: 3 OBJ: 1 51. ANS: D DIF: 1 REF: 3 OBJ: 2 52. ANS: C DIF: 2 REF: 3 OBJ: 2 53. ANS: A DIF: 1 REF: 3 OBJ: 3 54. ANS: B DIF: 1 REF: 3 OBJ: 3 55. ANS: A DIF: 1 REF: 3 OBJ: 4 56. ANS: C DIF: 2 REF: 3 OBJ: 4 57. ANS: C DIF: 2 REF: 3 OBJ: 4 58. ANS: C DIF: 1 REF: 3 OBJ: 4 59. ANS: B DIF: 1 REF: 3 OBJ: 4 60. ANS: A DIF: 2 REF: 3 OBJ: 4 61. ANS: C DIF: 2 REF: 3 OBJ: 4 62. ANS: B DIF: 1 REF: 3 OBJ: 5 63. ANS: A DIF: 1 REF: 1 OBJ: 1 64. ANS: B DIF: 1 REF: 1 OBJ: 1 65. ANS: D DIF: 2 REF: 1 OBJ: 1 66. ANS: D DIF: 1 REF: 1 OBJ: 1 67. ANS: B DIF: 1 REF: 1 OBJ: 1 68. ANS: A DIF: 1 REF: 1 OBJ: 1 69. ANS: C DIF: 1 REF: 1 OBJ: 1 70. ANS: A DIF: 1 REF: 1 OBJ: 3 71. ANS: A DIF: 1 REF: 1 OBJ: 3 72. ANS: C DIF: 2 REF: 1 OBJ: 4 73. ANS: B DIF: 2 REF: 2 OBJ: 1 74. ANS: A DIF: 1 REF: 2 OBJ: 1 75. ANS: C DIF: 1 REF: 2 OBJ: 1 76. ANS: C DIF: 2 REF: 2 OBJ: 1 77. ANS: B DIF: 1 REF: 2 OBJ: 2 78. ANS: D DIF: 1 REF: 2 OBJ: 2 79. ANS: A DIF: 1 REF: 2 OBJ: 2 80. ANS: A DIF: 1 REF: 2 OBJ: 2 81. ANS: D DIF: 2 REF: 2 OBJ: 2 82. ANS: C DIF: 2 REF: 2 OBJ: 2 83. ANS: C DIF: 2 REF: 2 OBJ: 2 84. ANS: B DIF: 2 REF: 2 OBJ: 2 85. ANS: B DIF: 2 REF: 1 OBJ: 1 86. ANS: B DIF: 1 REF: 1 OBJ: 1 87. ANS: D DIF: 2 REF: 1 OBJ: 3 88. ANS: D DIF: 1 REF: 2 OBJ: 1 89. ANS: A DIF: 2 REF: 2 OBJ: 2

COMPLETION

90. ANS: two moles

DIF: 2 REF: 1 OBJ: 2 91. ANS: 6.022  1023 particles/1 mol

DIF: 2 REF: 1 OBJ: 3 92. ANS: 58.93 amu

DIF: 1 REF: 2 OBJ: 1 93. ANS: copper

DIF: 2 REF: 2 OBJ: 1 94. ANS: smallest whole-number ratio of the atoms

DIF: 1 REF: 2 OBJ: 2 95. ANS: four

DIF: 2 REF: 2 OBJ: 2 96. ANS: 0.33 mol one-third mole

DIF: 2 REF: 2 OBJ: 2 97. ANS: 261.35 g/mol

DIF: 3 REF: 2 OBJ: 3 98. ANS: 100.00

DIF: 1 REF: 3 OBJ: 1 99. ANS: molar mass

DIF: 2 REF: 3 OBJ: 1

100. ANS: N2O5

101. ANS: C2H6

102. ANS: the molar masses of Ni, Cl, and NiCl2

DIF: 2 REF: 3 OBJ: 3 103. ANS: precipitate DIF: 1 REF: 1 OBJ: 1

104. ANS: H2(g)

DIF: 1 REF: 1 OBJ: 1 105. ANS: atoms

DIF: 1 REF: 2 OBJ: 1 106. ANS: (aq)

DIF: 1 REF: 1 OBJ: 3 107. ANS: 9

DIF: 2 REF: 2 OBJ: 2 108. ANS: 2

DIF: 2 REF: 2 OBJ: 2 109. ANS: 3

DIF: 2 REF: 2 OBJ: 2 110. ANS: decomposition

DIF: 2 REF: 3 OBJ: 3 111. ANS: decomposition

DIF: 2 REF: 3 OBJ: 3 112. ANS: displacement

DIF: 2 REF: 3 OBJ: 4 113. ANS: hydrogen

DIF: 1 REF: 3 OBJ: 4 114. ANS: double-displacement

DIF: 1 REF: 3 OBJ: 5 115. ANS: spectator ions

DIF: 1 REF: 4 OBJ: 2 116. ANS: Al3+,

DIF: 2 REF: 4 OBJ: 2 117. ANS: mole ratios

118. ANS: mol H2O

119. ANS: mol H2O DIF: 2 REF: 1 OBJ: 3

120. ANS: mass Cl2

DIF: 1 REF: 1 OBJ: 3 121. ANS: volume

122. ANS: mass H2

DIF: 2 REF: 1 OBJ: 4 123. ANS: mass

DIF: 2 REF: 1 OBJ: 5 124. ANS: limiting reactant

DIF: 1 REF: 2 OBJ: 1 125. ANS: excess reactant

DIF: 1 REF: 2 OBJ: 1 126. ANS: nitrogen

DIF: 1 REF: 3 OBJ: 1 127. ANS: fuel

DIF: 1 REF: 3 OBJ: 2 128. ANS: catalytic converter

DIF: 1 REF: 3 OBJ: 3 129. ANS: coefficients

130. ANS: N2

DIF: 1 REF: 1 OBJ: 1 131. ANS: 1:3

DIF: 1 REF: 1 OBJ: 1 132. ANS: 2:1

133. ANS: g H2O

134. ANS: mol Cl2

DIF: 2 REF: 1 OBJ: 3 135. ANS: side

DIF: 1 REF: 2 OBJ: 1 136. ANS: carbon (C)

DIF: 1 REF: 2 OBJ: 1 137. ANS: percentage

DIF: 1 REF: 2 OBJ: 2 138. ANS: idling

DIF: 1 REF: 3 OBJ: 2 139. ANS: photochemical

PROBLEM

140. ANS:

DIF: 3 REF: 1 OBJ: 2 141. ANS:

2 mol Ag: 1 mol S; Ag2S

DIF: 3 REF: 3 OBJ: 3 145. ANS: DIF: 3 REF: 3 OBJ: 3 146. ANS:

Fe + 2CuNO3  Fe(NO3)2 + 2Cu

2HgO 2Hg + O2

CH4 + 2O2  CO2 + 2H2O

P4(s) + 6Cl2(g)  4PCl3(l)

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

Balanced AgNO3(aq) + KCl(aq)  AgCl(s) + KNO3(aq) Total ionic Ag+(aq) + (aq) + K+(aq) + Cl–(aq)  AgCl(s) + K+(aq) + (aq) Net ionic Ag+(aq) + Cl–(aq)  AgCl(s)