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Chm 2.2 Energy: Conservation and Transfer - Chemical Reactions and Energy of Reactions - Chapter 7, 8, 9 and 17

Multiple ChoiceIdentify the letter of the choice that best completes the statement or answers the question.

____ 1. In a chemical reactiona. the mass of the reactants equals the mass of the products.b. the mass of the products is greater than the mass of reactants.c. the number of atoms in the reactants and products must change.d. energy as heat must be added to the reactants.

____ 2. Which observation does not indicate that a chemical reaction has occurred?a. formation of a precipitate c. evolution of heat and lightb. production of a gas d. change in total mass of substances

____ 3. When a solid produced by a chemical reaction separates from the solution it is calleda. a precipitate. c. a molecule.b. a reactant. d. the mass of the product.

____ 4. In writing a chemical equation that produces hydrogen gas, the correct representation of hydrogen gas isa. H. c. H2.b. 2H. d. OH.

____ 5. What is the small whole number that appears in front of a formula in a chemical equation?a. a subscript c. a ratiob. a superscript d. a coefficient

____ 6. To balance a chemical equation, it may be necessary to adjust thea. coefficients. c. formulas of the products.b. subscripts. d. number of products.

____ 7. According to the law of conservation of mass, the total mass of the reacting substances isa. always more than the total mass of the products.b. always less than the total mass of the products.c. sometimes more and sometimes less than the total mass of the products.d. always equal to the total mass of the products.

____ 8. A chemical equation is balanced when thea. 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.

____ 9. In the word equation, sodium oxide + water sodium hydroxide, the formula forsodium hydroxide is represented bya. Na2OH. c. NaO2.b. NaOH. d. Na2O.

____ 10. Which word equation represents the reaction that produces water from hydrogen and oxygen?a. Water is produced from hydrogen and oxygen.b. Hydrogen plus oxygen yields water.c. H2 + O2 water.d. Water can be separated into hydrogen and oxygen.

____ 11. 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

____ 12. Which of the following is a formula equation for the formation of carbon dioxide from carbon and oxygen?a. Carbon plus oxygen yields carbon dioxide. c. CO2 C + O2

b. C + O2 CO2 d. 2C + O CO2

____ 13. In an equation, the symbol for a substance in water solution is followed bya. (1). c. (aq).b. (g). d. (s).

____ 14. When the equation Fe3O4 + Al Al2O3 + Fe is correctly balanced, what is the coefficient of Fe?a. 3 c. 6b. 4 d. 9

____ 15. Which coefficients correctly balance the formula equation NH4NO2(s) N2(g) + H2O(l)?a. 1, 2, 2 c. 2, 1, 1b. 1, 1, 2 d. 2, 2, 2

____ 16. Which coefficients correctly balance the formula equation CaO + H2O Ca(OH)2?a. 2, 1, 2 c. 1, 2, 1b. 1, 2, 3 d. 1, 1, 1

____ 17. After the first steps in writing an equation, the equation is balanced bya. 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.

____ 18. The complete balanced equation for the reaction between zinc hydroxide and acetic acid isa. ZnOH + CH3COOH ZnCH3COO + H2O.b. Zn(OH)2 + CH3COOH Zn + 2CO2 +3H2O.c. Zn(OH)2 + 2CH3COOH Zn(CH3COO)2 + 2H2O.d. Zn(OH)2 + 2CH3COOH Zn(CH3COO)2 + H2 + O2.

____ 19. Which equation is not balanced?a. 2H2 + O2 2H2Ob. 4H2 + 2O2 4H2Oc. H2 + H2 + O2 H2O + H2Od. 2H2 + O2 H2O

____ 20. In what kind of reaction do two or more substances combine to form a new compound?a. decomposition reaction c. double-displacement reactionb. ionic reaction d. synthesis reaction

____ 21. The equation AX A + X is the general equation for aa. synthesis reaction. c. combustion reaction.b. decomposition reaction. d. single-displacement reaction.

____ 22. In what kind of reaction does one element replace a similar element in a compound?a. displacement reaction c. decomposition reactionb. combustion d. ionic reaction

____ 23. The equation AX + BY AY + BX is the general equation for aa. synthesis reaction. c. single-displacement reaction.b. decomposition reaction. d. double-displacement reaction.

____ 24. 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.

____ 25. In what kind of reaction does a single compound produce two or more simpler substances?

a. decomposition reaction c. single-displacement reactionb. synthesis reaction d. ionic reaction

____ 26. The equation A + BX AX + B is the general equation for aa. double-displacement reaction. c. single-displacement reaction.b. decomposition reaction. d. combustion reaction.

____ 27. In what kind of reaction do the ions of two compounds exchange places in aqueous solution to form two new compounds?a. synthesis reaction c. decomposition reactionb. double-displacement reaction d. combustion reaction

____ 28. The reaction represented by the equation 2Mg(s) + O2(g) 2MgO(s) is aa. synthesis reaction. c. single-displacement reaction.b. decomposition reaction. d. double-displacement reaction.

____ 29. The reaction represented by the equation Mg(s) + 2HCl(aq) H2(g) + MgCl2(aq) is aa. composition reaction. c. single-displacement reaction.b. decomposition reaction. d. double-displacement reaction.

____ 30. The reaction represented by the equation 2HgO(s) 2Hg(l) + O2(g) is a(n)a. single-displacement reaction. c. combustion reaction.b. synthesis reaction. d. decomposition reaction.

____ 31. The reaction represented by the equation Pb(NO3)2(aq) + 2KI(aq) PbI2(s) + 2KNO3(aq) is aa. double-displacement reaction. c. decomposition reaction.b. synthesis reaction. d. combustion reaction.

____ 32. The reaction represented by the equation 2KClO3(s) 2KCl(s) + 3O2(g) is a(n)a. synthesis reaction. c. combustion reaction.b. decomposition reaction. d. ionic reaction.

____ 33. The reaction represented by the equation Cl2(g) + 2KBr(aq) 2KCl(aq) + Br2(l) is a(n)a. synthesis reaction. c. single-displacement reaction.b. decomposition reaction. d. combustion reaction.

____ 34. In one type of synthesis reaction, an element combines with oxygen to yield a(n)a. acid. c. oxide.b. hydroxide. d. metal.

____ 35. When heated, a metal carbonate decomposes into a metal oxide anda. carbon. c. oxygen.b. carbon dioxide. d. hydrogen.

____ 36. Oxides of active metals, such as CaO, react with water to producea. metal carbonates. c. acids.b. metal hydrides. d. metal hydroxides.

____ 37. An active metal and a halogen react to form a(n)a. salt. c. acid.b. hydroxide. d. oxide.

____ 38. When a binary compound decomposes, what is produced?a. an oxide c. a tertiary compoundb. an acid d. two elements

____ 39. Many metal hydroxides decompose when heated to yield metal oxides anda. metal hydrides. c. carbon dioxide.b. water. d. an acid.

____ 40. When a metal chlorate is heated, it decomposes to yield a metal chloride anda. a metal oxide. c. hydrogen.b. a metal hydroxide. d. oxygen.

____ 41. Some acids, such as carbonic acid, decompose to nonmetal oxides anda. water. c. oxygen.b. a salt. d. peroxide.

____ 42. When heated, metallic chlorates decompose intoa. metallic oxides and chlorine.b. metallic chlorides and oxygen.c. a metal and a compound of chlorine and oxygen.d. a metal, chlorine, and oxygen.

____ 43. In the equation 2Al(s) + 3Fe(NO3)2(aq) 3Fe(s) + 2Al(NO3)3(aq), iron has been replaced bya. nitrate. c. aluminum.b. water. d. nitrogen.

____ 44. Group 1 metals react with water to produce metal hydroxides anda. metal hydroxides. c. oxygen.b. hydrochloric acid. d. hydrogen.

____ 45. The replacement of bromine by chlorine in a salt is an example of a single-displacement reaction bya. halogens. c. water.b. sodium. d. electrolysis.

____ 46. When a slightly soluble solid compound is produced in a double-displacement reaction, aa. gas bubbles off. c. combustion reaction takes place.b. precipitate is formed. d. halogen is produced.

____ 47. In a double-displacement reaction, hydrogen chloride and sodium hydroxide react to produce sodium chloride. Another product isa. sodium hydride. c. water.b. potassium chloride. d. hydrogen gas.

____ 48. Active metals react with certain acids, such as hydrochloric acid, to yield a metal compound anda. oxygen. c. chlorine.b. hydrogen. d. sodium.

____ 49. Some metals, such as iron, react with steam to produce hydrogen gas and aa. metal hydroxide. c. metallic acid.b. metal hydride. d. metal oxide.

____ 50. When potassium reacts with water, one product formed isa. hydrogen gas. c. potassium oxide.b. oxygen gas. d. salt.

____ 51. The reaction of calcium oxide, CaO, with water yieldsa. calcium and oxygen gas. c. calcium and a salt.b. calcium hydroxide. d. carbon dioxide and water.

____ 52. Predict the product of the reaction represented by the following equation: MgO + CO2 a. MgCO3 c. MgC + O3

b. Mg + CO3 d. MgCO2 + O____ 53. Magnesium hydroxide decomposes to yield magnesium oxide and

a. hydrogen. c. water.b. oxygen. d. salt.

____ 54. When sodium chlorate, NaClO3, decomposes, the products area. sodium hydroxide and water. c. sodium and chlorine oxide.b. sodium oxide and chlorine. d. sodium chloride and oxygen.

____ 55. If chlorine gas is produced by halogen replacement, the other halogen in the reaction must bea. bromine. c. astatine.

b. iodine. d. fluorine.____ 56. The formulas for the products of the reaction between sodium hydroxide and sulfuric acid are

a. Na2SO4 and H2O. c. SI4 and Na2O.b. NaSO4 and H2O. d. S + O2 and Na.

____ 57. What is the balanced equation when aluminum reacts with copper(II) sulfate?a. Al + Cu2S Al2S + Cub. 2Al + 3CuSO4 Al2(SO4)3 + 3Cuc. Al + CuSO4 AlSO4 + Cud. 2Al + Cu2SO4 Al2SO4 + 2Cu

____ 58. The ability of an element to react is the element'sa. valence. c. stability.b. activity. d. electronegativity.

____ 59. 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 seriesb. reaction sequence d. periodic list

____ 60. An element in the activity series can replace any elementa. in the periodic table. c. above it on the list.b. below it on the list. d. in its group.

____ 61. What can be predicted by using an activity series?a. whether a certain chemical reaction will occurb. the amount of energy released by a chemical reactionc. the electronegativity values of elementsd. the melting points of elements

____ 62. Predict what happens when calcium metal is added to a solution of magnesium chloride.a. No reaction occurs. c. Magnesium calcite forms.b. Calcium chloride forms. d. Gaseous calcium is produced.

____ 63. Predict what happens when zinc is added to water.a. No reaction occurs. c. Zinc oxide forms.b. Steam is produced. d. Hydrogen is released.

____ 64. Predict what happens when lead is added to nitric acid.a. No reaction occurs. c. Lead oxide forms.b. Oxygen is released. d. Hydrogen is released.

____ 65. Predict what happens when nickel is added to a solution of potassium chloride.a. No reaction occurs. c. Potassium nickel chloride forms.b. Nickel chloride forms. d. Hydrochloric acid forms.

____ 66. Magnesium bromide (aq) + chlorine (g) yieldsa. Mg(s) and BrCl(aq). c. MgBrCl(aq).b. MgCl(aq) and Br2(l). d. MgCl2(aq) and Br2(l).

____ 67. Which reaction does not occur?a. 2HF(aq) + Cl2(g) F2(g) + 2HCl(aq)b. 2Na(s) + ZnF2(aq) 2NaF(aq) + Zn(s)c. Fe(s) + CuCl2(aq) FeCl2(aq) + Cu(s)d. 2HCl(aq) + Mg(s) MgCl2(aq) + H2(g)

____ 68. Which reaction can be predicted from the activity series?a. 2Cl(g) Cl2(g)b. HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l)c. 2H2O(aq) + 2Na(s) 2NaOH(aq) + H2(g)

d. Cl2(g) 2Cl(g)____ 69. 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.

____ 70. In the reaction represented by the equation N2 + 3H2 2NH3, what is the mole ratio of nitrogen to ammonia?a. 1:1 c. 1:3b. 1:2 d. 2:3

____ 71. In the reaction represented by the equation 2Al2O3 4Al + 3O2, what is the mole ratio of aluminum to oxygen?a. 10:6 c. 2:3b. 3:4 d. 4:3

____ 72. In the reaction represented by the equation C + 2H2 CH4, what is the mole ratio of hydrogen to methane?a. 1:1 c. 1:2b. 2:1 d. 2:4

____ 73. In the reaction represented by the equation N2 + 3H2 2NH3, what is the mole ratio of hydrogen to ammonia?a. 1:1 c. 3:2b. 2:1 d. 6:8

____ 74. The Haber process for producing ammonia commercially is represented by the equation N2(g) + 3H2(g) 2NH3(g). To completely convert 9.0 mol hydrogen gas to ammonia gas, how many moles of nitrogen gas are required?a. 1.0 mol c. 3.0 molb. 2.0 mol d. 6.0 mol

____ 75. In the equation 2KClO3 2KCl + 3O2, how many moles of oxygen are produced when 3.0 mol of KClO3 decompose completely?a. 1.0 mol c. 3.0 molb. 2.5 mol d. 4.5 mol

____ 76. For the reaction represented by the equation C + 2H2 CH4, how many moles of hydrogen are required to produce 10 mol of methane, CH4?a. 2 mol c. 10 molb. 4 mol d. 20 mol

____ 77. For the reaction represented by the equation 2H2 + O2 2H2O, how many moles of water can be produced from 6.0 mol of oxygen?a. 2.0 mol c. 12 molb. 6.0 mol d. 18 mol

____ 78. For the reaction represented by the equation N2 + 3H2 2NH3, how many moles of nitrogen are required to produce 18 mol of ammonia?a. 9.0 mol c. 27 molb. 18 mol d. 36 mol

____ 79. For the reaction represented by the equation AgNO3 + NaCl NaNO3 + AgCl, how many moles of silver chloride, AgCl, are produced from 7.0 mol of silver nitrate AgNO3?a. 1.0 mol c. 7.0 molb. 2.3 mol d. 21 mol

Use the table below to answer the following questions.

Element Symbol Atomic Mass

Bromine Br 79.90Calcium Ca 40.08Carbon C 12.01Chlorine Cl 35.45Cobalt Co 58.93Copper Cu 63.55Fluorine F 19.00Hydrogen H 1.01Iodine I 126.90Iron Fe 55.85Lead Pb 207.2Magnesium Mg 24.30Mercury Hg 200.59Nitrogen N 14.01Oxygen O 15.00Potassium K 39.10Sodium Na 22.99Sulfur S 32.01

____ 80. For the reaction represented by the equation 2Na + 2H2O 2NaOH + H2, how many grams of sodium hydroxide are produced from 3.0 mol of sodium with an excess of water?a. 40. g c. 120 gb. 80. g d. 240 g

____ 81. For the reaction represented by the equation SO3 + H2O H2SO4, how many grams of sulfur trioxide are required to produce 4.00 mol of sulfuric acid in an excess of water?a. 80.0 g c. 240. gb. 160. g d. 320. g

____ 82. For the reaction represented by the equation 2Fe + O2 2FeO, how many grams of iron(II) oxide are produced from 8.00 mol of iron in an excess of oxygen?a. 71.8 g c. 712 gb. 575 g d. 1310 g

____ 83. For the reaction represented by the equation 2Na + Cl2 2NaCl, how many grams of chlorine gas are required to react completely with 2.00 mol of sodium?a. 35.5 g c. 141.8 gb. 70.9 g d. 212.7 g

____ 84. For the reaction represented by the equation 2HNO3 + Mg(OH)2 Mg(NO3)2 + 2H2O, how many grams of magnesium nitrate are produced from 8.00 mol of nitric acid, HNO3, and an excess of Mg(OH)2?a. 148 g c. 593 gb. 445 g d. 818 g

____ 85. For the reaction represented by the equation CH4 + 2O2 CO2 + 2H2O, how many moles of carbon dioxide are produced from the combustion of 100. g of methane?a. 6.23 mol c. 12.5 molb. 10.8 mol d. 25 mol

____ 86. For the reaction represented by the equation Pb(NO3)2 + 2KI PbI2 + 2KNO3, how many moles of lead(II) iodide are produced from 300. g of potassium iodide and an excess of Pb(NO3)2?a. 0.904 mol c. 3.61 molb. 1.81 mol d. 11.0 mol

____ 87. For the reaction represented by the equation Cl2 + 2KBr 2KCl + Br2, how many moles of potassium chloride are produced from 119 g of potassium bromide?a. 0.119 mol c. 0.581 molb. 0.236 mol d. 1.00 mol

____ 88. For the reaction represented by the equation 3Fe + 4H2O Fe3O4 + 4H2, how many moles of iron(III) oxide are produced from 500. g of iron in an excess of H2O?a. 1.04 mol c. 8.95 molb. 2.98 mol d. 12.98 mol

____ 89. For the reaction represented by the equation 2KlO3 2KCl + 3O2, how many moles of potassium chlorate are required to produce 250. g of oxygen?a. 2.00 mol c. 4.97 molb. 4.32 mol d. 5.21 mol

____ 90. Ozone, O3, is produced by the reaction represented by the following equation:

What mass of ozone will form from the reaction of 2.0 g of NO2 in a car's exhaust and excess oxygen?a. 1.1 g O3 c. 2.1 g O3

b. 1.8 g O3 d. 4.2 g O3

____ 91. For the reaction represented by the equation Cl2 + 2KBr 2KCl + Br2, how many grams of potassium chloride can be produced from 300. g each of chlorine and potassium bromide?a. 98.7 g c. 188 gb. 111 g d. 451 g

____ 92. For the reaction represented by the equation 2Na + 2H2O 2NaOH + H2, how many grams of hydrogen are produced if 120. g of sodium and 80. g of water are available?a. 4.5 g c. 80. gb. 45 g d. 200 g

____ 93. For the reaction represented by the equation 2Na + Cl2 2NaCl, how many grams of sodium chloride can be produced from 500. g each of sodium and chlorine?a. 112 g c. 409 gb. 319 g d. 824 g

____ 94. For the reaction represented by the equation SO3 + H2O H2SO4, how many grams of sulfuric acid can be produced from 200. g of sulfur trioxide and 100. g of water?a. 100. g c. 245 gb. 200. g d. 285 g

____ 95. Which reactant controls the amount of product formed in a chemical reaction?a. excess reactant c. composition reactantb. mole ratio d. limiting reactant

____ 96. For the reaction represented by the equation 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%

____ 97. For the reaction represented by the equation 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. 91.0%b. 82.1% d. 98.9%

____ 98. For the reaction represented by the equation CH4 + 2O2 2H2O + CO2, 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%

____ 99. For the reaction represented by the equation Mg + 2HCl H2 + MgCl2, calculate the percentage yield of magnesium chloride if 100. g of magnesium react with excess hydrochloric acid to yield 330. g of magnesium chloride.a. 71.8% c. 81.6%b. 74.3% d. 84.2%

____ 100.What is E for the reaction in the diagram above?a. + 200 kJ c. +50 kJb. -200 kJ d. - 50 kJ

____ 101. The reaction illustrated in the diagram above is a. endothermic c. both endothermic and exothermicb. exothermic d. neither endothermic or exothermic

____ 102. Calcualte Ea for the reaction given by the diagram in question #100. a. +200 kJ c. +250b. -200 kJ d. - 250 kJ

____ 103. What is the percentage composition of CF4?a. 20% C, 80% F c. 16.8% C, 83.2% Fb. 13.6% C, 86.4% F d. 81% C, 19% F

____ 104. What is the percentage composition of CO?a. 50% C, 50% O c. 25% C, 75% Ob. 12% C, 88% O d. 43% C, 57% O

____ 105. What is the percentage composition of CuCl2?a. 33% Cu, 66% Cl c. 65.50% Cu, 34.50% Clb. 50% Cu, 50% Cl d. 47.27% Cu, 52.73% Cl

____ 106. The percentage composition of sulfur in SO2 is about 50%. What is the percentage of oxygen in this compound?a. 25% c. 75%b. 50% d. 90%

____ 107. What is the mass percentage of chlorine in NaCl?a. 35.45% c. 60.7%b. 50% d. 64.5%

____ 108. 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

____ 109. 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

____ 110. What is the empirical formula for a compound that is 53.3% O and 46.7% Si?

a. SiO c. Si2Ob. SiO2 d. Si2O3

____ 111. 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. CFb. C4F d. CF2

____ 112. A compound contains 64 g of O and 8 g of H. What is the empirical formula for this compound?a. H2O c. HO2

b. H2O2 d. HO____ 113. 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

____ 114. 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. C2Ob. CO2 d. C2O4

____ 115. The molecular formula for vitamin C is C6H8O6. What is the empirical formula?a. CHO c. C3H4O3

b. CH2O d. C2H4O2

____ 116. Of the following molecular formulas for hydrocarbons, which is an empirical formula?a. CH4 c. C3H6

b. C2H2 d. C4H10

____ 117. A compound's empirical formula is C2H5. If the formula mass is 58 amu, what is the molecular formula?a. C3H6 c. C5H8

b. C4H10 d. C5H15

____ 118. A compound's empirical formula is N2O5. If the formula mass is 108 amu, what is the molecular formula?a. N2O5 c. NO3

b. N4O10 d. N2O4

____ 119. A compound's empirical formula is CH. If the formula mass is 26 amu, what is the molecular formula?a. C2H2 c. CH4

b. CH3 d. C4H____ 120. A compound's empirical formula is NO2. If the formula mass is 92 amu, what is the molecular formula?

a. NO c. NO4

b. N2O2 d. N2O4

____ 121. A compound's empirical formula is CH3. If the formula mass is 30 amu, what is the molecular formula?a. CH3 c. C2H6

b. CH4 d. C3H9

____ 122. A compound's empirical formula is HO. If the formula mass is 34 amu, what is the molecular formula?a. H2O c. HO3

b. H2O2 d. H2O3

Short Answer

123. When balancing a chemical equation, why must the formula subscripts remain unchanged?

124. Consider the reaction represented by the equation 2Al(s) + 3ZnCl2(aq) ?. Briefly explain how the activity series is used to predict the outcome and products of the reaction.

Essay

125. The two chemical equations below appear to describe the same chemical reaction. Explain how the two reactions are different from each other. Hypothesize any differences you might be able to observe in these two reactions represented by the following equations.Mg(s) + 2H2O(l) Mg(OH)2(aq) + H2(g)Mg(l) + 2H2O(g) Mg(OH)2(aq) + H2(g)

126. Consider the equation O2(g) + CS2(l) CO2(g) + SO2(g). How does the equation violate the law of conservation of mass? How can the equation be rewritten to conform to the law of conservation of mass?

Problem

127. Write a balanced chemical equation for the following reaction: iron plus copper(I) nitrate yields iron(II) nitrate plus copper.

128. Write a balanced chemical equation for the synthesis of liquid phosphorus trichloride, PCl3, from white phosphorus, P4, and chlorine gas.

129. Tell what type of chemical reaction is represented by the following formula equation. Then balance the equation.C3H8(g) + O2(g) CO2(g) + H2O(l)

130. Tell what type of chemical reaction is represented by the following formula equation. Then balance the equation.Ga(s) + S(s) Ga2S3(s)

131. Tell what type of chemical reaction is represented by the following formula equation. Then balance the equation.KBr(aq) + Mg(OH)2(aq) KOH(aq) + MgBr2(aq)

132. Use the activity series to determine if the following reaction is possible. If it is possible, write the products and balance the equation. If not, explain.4Cr(s) + 3O2(g)

133. Use the activity series to determine if the following reaction is possible. If it is possible, write the products and balance the equation. If not, explain.2Sb + 6HCl

134. Use the activity series to determine if the following reaction is possible. If it is possible, write the products and balance the equation. If not, explain.2K(s) + ZnCl2(aq)

Chm 2.2 Energy: Conservation and Transfer - Chemical Reactions and Energy of Reactions - Chapter 7, 8, 9 and 17Answer Section

MULTIPLE CHOICE

1. ANS: A DIF: I REF: 1 OBJ: 12. ANS: D DIF: I REF: 1 OBJ: 13. ANS: A DIF: I REF: 1 OBJ: 14. ANS: C DIF: I REF: 1 OBJ: 25. ANS: D DIF: I REF: 1 OBJ: 26. ANS: A DIF: I REF: 1 OBJ: 27. ANS: D DIF: I REF: 1 OBJ: 28. ANS: B DIF: I REF: 1 OBJ: 29. ANS: B DIF: I REF: 1 OBJ: 3

10. ANS: B DIF: II REF: 1 OBJ: 311. ANS: C DIF: II REF: 1 OBJ: 312. ANS: B DIF: II REF: 1 OBJ: 313. ANS: C DIF: I REF: 1 OBJ: 314. ANS: D DIF: III REF: 1 OBJ: 415. ANS: B DIF: III REF: 1 OBJ: 416. ANS: D DIF: III REF: 1 OBJ: 417. ANS: B DIF: II REF: 1 OBJ: 418. ANS: C DIF: III REF: 1 OBJ: 419. ANS: D DIF: III REF: 1 OBJ: 420. ANS: D DIF: I REF: 2 OBJ: 121. ANS: B DIF: II REF: 2 OBJ: 122. ANS: A DIF: I REF: 2 OBJ: 123. ANS: D DIF: II REF: 2 OBJ: 124. ANS: C DIF: II REF: 2 OBJ: 125. ANS: A DIF: I REF: 2 OBJ: 126. ANS: C DIF: II REF: 2 OBJ: 127. ANS: B DIF: I REF: 2 OBJ: 128. ANS: A DIF: II REF: 2 OBJ: 229. ANS: C DIF: II REF: 2 OBJ: 230. ANS: D DIF: II REF: 2 OBJ: 231. ANS: A DIF: II REF: 2 OBJ: 232. ANS: B DIF: II REF: 2 OBJ: 233. ANS: C DIF: II REF: 2 OBJ: 234. ANS: C DIF: II REF: 2 OBJ: 335. ANS: B DIF: II REF: 2 OBJ: 336. ANS: D DIF: II REF: 2 OBJ: 337. ANS: A DIF: II REF: 2 OBJ: 338. ANS: D DIF: II REF: 2 OBJ: 339. ANS: B DIF: II REF: 2 OBJ: 340. ANS: D DIF: II REF: 2 OBJ: 3

41. ANS: A DIF: II REF: 2 OBJ: 342. ANS: B DIF: II REF: 2 OBJ: 343. ANS: C DIF: II REF: 2 OBJ: 444. ANS: D DIF: I REF: 2 OBJ: 445. ANS: A DIF: II REF: 2 OBJ: 446. ANS: B DIF: I REF: 2 OBJ: 447. ANS: C DIF: II REF: 2 OBJ: 448. ANS: B DIF: I REF: 2 OBJ: 449. ANS: D DIF: I REF: 2 OBJ: 450. ANS: A DIF: I REF: 2 OBJ: 451. ANS: B DIF: III REF: 2 OBJ: 552. ANS: A DIF: III REF: 2 OBJ: 553. ANS: C DIF: III REF: 2 OBJ: 554. ANS: D DIF: III REF: 2 OBJ: 555. ANS: D DIF: III REF: 2 OBJ: 556. ANS: A DIF: III REF: 2 OBJ: 557. ANS: B DIF: III REF: 2 OBJ: 558. ANS: B DIF: I REF: 3 OBJ: 159. ANS: C DIF: I REF: 3 OBJ: 160. ANS: B DIF: I REF: 3 OBJ: 161. ANS: A DIF: II REF: 3 OBJ: 162. ANS: B DIF: III REF: 3 OBJ: 263. ANS: A DIF: III REF: 3 OBJ: 264. ANS: D DIF: III REF: 3 OBJ: 265. ANS: A DIF: III REF: 3 OBJ: 266. ANS: D DIF: III REF: 3 OBJ: 267. ANS: A DIF: III REF: 3 OBJ: 268. ANS: C DIF: III REF: 3 OBJ: 269. ANS: B DIF: I REF: 1 OBJ: 170. ANS: B DIF: III REF: 1 OBJ: 371. ANS: D DIF: III REF: 1 OBJ: 372. ANS: B DIF: III REF: 1 OBJ: 373. ANS: C DIF: III REF: 1 OBJ: 374. ANS: C DIF: III REF: 1 OBJ: 375. ANS: D DIF: III REF: 1 OBJ: 376. ANS: D DIF: III REF: 1 OBJ: 377. ANS: C DIF: III REF: 1 OBJ: 378. ANS: A DIF: III REF: 1 OBJ: 379. ANS: C DIF: III REF: 2 OBJ: 180. ANS: C

Solution:

DIF: III REF: 2 OBJ: 281. ANS: D

Solution:

DIF: III REF: 2 OBJ: 282. ANS: B

Solution:


Solution:

DIF: III REF: 2 OBJ: 284. ANS: C

Solution:

DIF: III REF: 2 OBJ: 285. ANS: A

Solution:


Solution:


Solution:


Solution:


Solution:


Solution:


Solution:

Since Cl2 would produce the most KCl, KBr is the limiting reactant, thus 188 G KCl is produced.


Solution:

Since Na would produce the most H2, H2O is the limiting reactant, thus 4.5 g H2 is produced.


Solution:

Since Na would produce the most NaCl, Cl2 is the limiting reactant, thus 824 g NaCl is produced.


Solution:

Since H2O would produce the most H2SO4, SO3 is the limiting reactant, thus 245 g H2SO4 is produced.

DIF: III REF: 2 OBJ: 495. ANS: D DIF: I REF: 3 OBJ: 196. ANS: D

Solution:


Solution:


Solution:


Solution:

DIF: III REF: 3 OBJ: 4100. ANS: C101. ANS: A102. ANS: A103. ANS: B

Solution:


Solution:


Solution:

DIF: III REF: 3 OBJ: 4106. ANS: B DIF: II REF: 3 OBJ: 4107. ANS: C

Solution:


Solution:


Solution:


Solution:


Solution:


Solution:


Solution:


Solution:

DIF: III REF: 4 OBJ: 2

115. ANS: C DIF: III REF: 4 OBJ: 3116. ANS: A DIF: III REF: 4 OBJ: 3117. ANS: B

Solution:


Solution:


Solution:


Solution:


Solution:


Solution:


SHORT ANSWER

123. ANS:Changing the subscript in a formula changes the chemical composition of the compound.

DIF: I REF: 2 OBJ: 2124. ANS:

In the activity series, aluminum is more active than zinc. Aluminum will replace zinc forming aluminum chloride and leaving zinc metal.

DIF: II REF: 3 OBJ: 2

ESSAY

125. ANS:The conditions under which the two reactions take place are different. In one case, solid magnesium is added to liquid water, while in the other case, liquid magnesium reacts with gaseous water (perhaps steam). Although the products are the same in each case, one might expect the second reaction to proceed more rapidly than the first because of the higher temperature of the water (steam) and the breaking of the crystal lattice in magnesium.

DIF: II REF: 1 OBJ: 3126. ANS:

In the equation shown, there are more oxygen atoms in the products than in the reactants and more sulfur atoms in the reactants than in the products. Both conditions violate the law of conservation of mass. The equation is balanced as follows: 3O2 + CS2 CO2 +2SO2.

DIF: II REF: 2 OBJ: 2

PROBLEM

127. ANS:Fe(s) + 2CuNO3(aq) Fe(NO3)2(aq) + 2Cu(s)


P4(s) + 6Cl2(g) 4PCl3(l)


combustion, C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(l)

DIF: III REF: 3 OBJ: 1130. ANS:

synthesis, 2Ga(s) + 3S(s) Ga2S3(s)


double-displacement, 2KBr(aq) + Mg(OH)2(aq) 2KOH(aq) + MgBr2(aq)


reaction will occur, 4Cr(s) + 3O2(g) 2Cr2O3(s)


no reaction; Antimony is not highly active and will not replace hydrogen in an acid.


reaction will occur, 2K(s) + ZnCl2(aq) 2KCl(aq) + Zn(s)


chm 2 - iredell-statesville€¦ · web viewin the word equation, sodium ... for the reaction...

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