Chemistry I - Spring Semester Exam

Transcription

1 Name: Class: Date: Chemistry I - Spring Semester Exam Multiple Choice Identify the choice that best completes the statement or answers the question. 1. What is the formula mass of (NH 4 ) 2 SO 4? a amu c amu b amu d amu 2. The molar mass of LiBr is g/mol. How many moles of LiBr are present in g? a mol c mol b mol d mol 3. How many valence electrons are in an atom of magnesium? a. 2 c. 4 b. 3 d How many valence electrons does a helium atom have? a. 2 c. 4 b. 3 d Which of the following is true about an ionic compound? a. It is a salt. c. It is composed of anions and cations. b. It is held together by ionic bonds. d. all of the above 6. What is the formula for potassium sulfide? a. KS c. KS 2 b. K 2 S d. K 2 S 2 7. Which of the following compounds has the formula KNO 3? a. potassium nitrate c. potassium nitrite b. potassium nitride d. potassium nitrogen oxide 8. 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. 9. For the reaction represented by the equation 2KlO 3 2KCl + 3O 2, how many moles of potassium chlorate are required to produce 250. g of oxygen? a mol c mol b mol d mol 10. For the reaction represented by the equation Cl 2 + 2KBr 2KCl + Br 2, how many grams of potassium chloride can be produced from 300. g each of chlorine and potassium bromide? a g c. 188 g b. 111 g d. 451 g 11. When the limiting reactant in a chemical reaction is completely used, the a. excess reactants begin combining. c. reaction speeds up. b. reaction slows down. d. reaction stops. 12. For the reaction represented by the equation SO 3 + H 2 O H 2 SO 4, 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% 1

2 Name: 13. How many hydrogen atoms are in 3 molecules of isopropyl alcohol, C 3 H 7 O? a. 3 ( ) c. 21 b. 3 d. 21 ( ) 14. Which of the following elements exists as a diatomic molecule? a. helium c. bromine b. potassium d. sulfur 15. How many moles of silver atoms are in atoms of silver? a c b d How many molecules are in 3.90 mol CO 2? a molecules c molecules b molecules d molecules 17. What is true about the molar mass of chlorine gas? a. The molar mass is 35.5 g. b. The molar mass is 71.0 g. c. The molar mass is equal to the mass of one mole of chlorine atoms. d. none of the above 18. The mass of a mole of NaBr is the. a. molar mass c. molecular mass b. atomic mass d. gram atomic mass 19. What is the mass in grams of 3.10 mol C 8 H 18? a g c g b g d. 354 g 20. The molar mass of a certain gas is 48 g. What is the density of the gas in g/l at STP? a g/l c. 2.1 g/l b g/l d. 71 g/l 21. If the density of a noble gas is g/l at STP, that gas is. a. Kr c. Ar b. Xe d. He 22. The lowest whole-number ratio of the elements in a compound is called the. a. empirical formula c. binary formula b. molecular formula d. representative formula 23. Which of the following has components in a nonuniform arrangement? a. homogeneous mixture c. salt water b. solution d. heterogeneous mixture 24. Sugar dissolved in water is an example of which solute-solvent combination? a. gas-liquid c. solid-liquid b. liquid-liquid d. liquid-solid 25. Oxygen in nitrogen is an example of which solute-solvent combination? a. gas-liquid c. gas-solid b. liquid-gas d. gas-gas 2

3 Name: 26. A metal solution is a(n) a. colloid. c. suspension. b. alloy. d. emulsion. 27. Which of the following is an electrolyte? a. sodium chloride c. pure water b. sugar d. glass 28. "Like dissolves like" is a very general rule used for predicting whether a. one substance will form a solution with another. b. one substance will react with another. c. a reaction will reach equilibrium. d. a mixture will contain two or three phases. 29. Effervescence is the a. dissolution of gas in liquid. b. escape of gas from a gas-liquid solution. c. escape of liquid from a liquid-liquid solution. d. escape of solid from a solid-liquid solution. 30. What is the molarity of a solution that contains mol KCl in 7.98 L solution? a M c M b M d M 31. What is the molarity of a solution that contains 125 g NaCl in 4.00 L solution? (molar mass of NaCl = g/mol) a M c M b M d M 32. The calculation of quantities in chemical equations is called. a. stoichiometry c. percent composition b. dimensional analysis d. percent yield 33. Which of the following is true about the total number of reactants and the total number of products in the reaction shown below? C 5 H 12 (l) + 8O 2 (g) 5CO 2 (g) + 6H 2 O(g) a. 9 moles of reactants chemically change into 11 moles of product. b. 9 grams of reactants chemically change into 11 grams of product. c. 9 liters of reactants chemically change into 11 liters of product. d. 9 atoms of reactants chemically change into 11 atoms of product. 34. At STP, how many liters of oxygen are required to react completely with 3.6 liters of hydrogen to form water? 2H 2 (g) + O 2 (g) 2H 2 O(g) a. 1.8 L c. 2.0 L b. 3.6 L d. 2.4 L 35. Mercury can be obtained by reacting mercury(ii) sulfide with calcium oxide. How many grams of calcium oxide are needed to produce 36.0 g of Hg? 4HgS(s) + 4CaO(s) 4Hg(l) + 3CaS(s) + CaSO 4 a g c g b g d g 3

4 Name: 36. Which of the following statements is true about the following reaction? 3NaHCO 3 (aq) + C 6 H 8 O 7 (aq) 3CO 2 (g) + 3H 2 O(s) +Na 3 C 6 H 5 O 7 (aq) a L of CO 2 (g) are produced for every liter of C 6 H 8 O 7 (aq) reacted. b. 1 mole of water is produced for every mole of carbon dioxide produced. c molecules of Na 3 C 6 H 5 O 7 (aq) are produced for every mole of NaHCO 3 (aq) used. d. 54 g of water are produced for every mole of NaHCO 3 (aq) produced. 37. Calcium oxide, or lime, is produced by the thermal decomposition of limestone in the reaction CaCO 3 (s) CaO(s) + CO 2 (g). What mass of lime can be produced from kg of limestone? a kg c. 8.4 kg b kg d. none of the above 38. When two substances react to form products, the reactant which is used up is called the. a. determining reagent c. excess reagent b. limiting reagent d. catalytic reagent 39. Metallic copper is formed when aluminum reacts with copper(ii) sulfate. How many grams of metallic copper can be obtained when 54.0 g of Al react with 319 g of CuSO 4? Al + 3CuSO 4 Al 2 (SO 4 ) 3 + 3Cu a g c. 162 g b. 127 g d. 381 g 40. Bases feel a. rough. c. slippery. b. moist. d. dry. 41. An acid ending with the suffix -ic produces an anion with the a. suffix -ate. c. prefix hydro-. b. suffix -ite. d. suffix -ous. 42. Which acid is produced in the stomach? a. hydrochloric acid c. nitric acid b. phosphoric acid d. sulfuric acid 43. Which acid is found in vinegar? a. acetic acid c. phosphoric acid b. nitric acid d. hydrochloric acid 44. Arrhenius theorized that a base is a chemical compound that a. increases the concentration of hydrogen ions when dissolved in water. b. increases the concentration of hydroxide ions when dissolved in water. c. decreases the concentration of hydrogen ions when dissolved in water. d. decreases the concentration of hydroxide ions when dissolved in water. 45. Which of the following is a weak base? a. NH 3 c. NaOH b. KOH d. Ba(OH) Which of the following is a strong base? a. KOH c. NH 3 b. H 2 d. HCl 4

5 Name: 47. Which of the following is a diprotic acid? a. H 2 SO 4 c. HCl b. CH 3 COOH d. H 3 PO A Brønsted-Lowry acid is a(n) a. electron-pair acceptor. c. proton acceptor. b. electron-pair donor. d. proton donor. 49. A species that is formed when a base gains a proton is a a. conjugate base. c. strong base. b. conjugate acid. d. strong acid. 50. In the reaction represented by the equation HClO 3 +NH 3 NH 4 +ClO 3 the conjugate acid of NH 3 is a. HClO 3. c. NH 4. b. ClO 3. d. not shown. 51. The conjugate of a strong acid is a a. strong acid. c. strong base. b. weak acid. d. weak base. 52. The conjugate of a weak base is a a. strong acid. c. strong base. b. weak acid. d. weak base. 53. The volume of a gas is doubled while the temperature is held constant. How does the gas pressure change? a. It is reduced to one half. b. It does not change. c. It is doubled. d. It varies depending on the type of gas. 54. The volume of a gas is reduced from 2 L to 0.5 L while the temperature is held constant. How does the gas pressure change? a. It increases by a factor of two. c. It increases by a factor of four. b. It decreases by a factor of four. d. It increases by a factor of one. 55. If a balloon is heated, what happens to the volume of the air in the balloon if the pressure is constant? a. It increases. c. It decreases. b. It stays the same. d. The change cannot be predicted. 56. As the temperature of a fixed volume of a gas increases, the pressure will. a. vary inversely c. not change b. decrease d. increase 57. A gas occupies a volume of 2.4 L at 14.1 kpa. What volume will the gas occupy at 84.6 kpa? a. 497 L c. 14 L b. 2.5 L d L 58. A sample of gas occupies 17 ml at 112 C. What volume does the sample occupy at 70 C? a ml c. 36mL b. 27 ml d. 8.0mL 59. If a balloon containing 3000 L of gas at 39 C and 99 kpa rises to an altitude where the pressure is 45.5 kpa and the temperature is 16 C, the volume of the balloon under these new conditions would be calculated using the following conversion factor ratios:. a L b L c L d L

6 Name: 60. A breathing mixture used by deep-sea divers contains helium, oxygen, and carbon dioxide. What is the partial pressure of oxygen at kpa if P He = 82.5 kpa and P CO 2 = 0.4 kpa? a kpa c kpa b kpa d kpa 61. When a container is filled with 3.00 moles of H 2, 2.00 moles of O 2, and 1.00 mole of N 2, the pressure in the container is 768 kpa. What is the partial pressure of O 2? a. 256 kpa c. 128 kpa b. 128 kpa d. 192 kpa 62. How does the surface tension of water compare with the surface tensions of most other liquids? a. It is lower. b. It is about the same. c. It is higher. d. It is higher when a surfactant is added. 63. What causes water's low vapor pressure? a. dispersion forces c. hydrogen bonding b. covalent bonding d. ionic attractions 64. What is the shape of the water molecule? a. linear c. trigonal planar b. tetrahedral d. bent 65. Which atom in a water molecule has the greatest electronegativity? a. one of the hydrogen atoms b. both hydrogen atoms c. the oxygen atom d. There is no difference in the electronegativities of the atoms in a water molecule. 66. The bonds between adjacent water molecules are called. a. hydrogen bonds c. nonpolar covalent bonds b. ionic bonds d. polar covalent bonds 67. The bonds between the hydrogen and oxygen atoms in a water molecule are. a. hydrogen bonds c. nonpolar covalent bonds b. ionic bonds d. polar covalent bonds 68. An electric current can be conducted by. a. methane gas c. a salt solution b. a sugar solution d. rubbing alcohol 69. Which of the following mixtures is NOT a colloid? a. fog c. paint b. milk d. sugar water 70. The formula of the hydrogen ion is often written as. a. H 2 O c. H b. OH d. H 4 N 71. A Lewis acid is a substance that can. a. donate a pair of electrons c. donate a hydrogen ion b. accept a pair of electrons d. accept a hydrogen ion 72. Which of the following reactions illustrates amphoterism? a. H 2 O + H 2 O H 3 O + OH c. HCl + H 2 O H 3 O + Cl b. NaCl Na + OH d. NaOH Na + OH 6

7 Name: 73. What are the acids in the following equilibrium reaction? CN + H 2 O HCN + OH a. CN, H 2 O c. CN, OH b. H 2 O, HCN d. H 2 O, OH 74. The products of self-ionization of water are. a. H 3 O and H 2 O c. OH and H b. OH and OH d. OH and H 75. Which type of solution is one with a ph of 8? a. acidic b. basic c. neutral d. The type varies, depending on the solution. 76. An indicator is what type of compound? a. oxidizing agent c. strong base or acid b. weak base or acid d. salt 77. With solutions of strong acids and strong bases, the word strong refers to. a. normality c. solubility b. molarity d. degree of ionization 78. Which acid has the greatest acid dissociation constant? a. nitric acid c. carbonic acid b. acetic acid d. boric acid 79. The charge on a gamma ray is. a. +2 c. 0 b. 1 d What particle is emitted in alpha radiation? a. electron c. helium nucleus b. photon d. hydrogen nucleus 81. Ionizing radiation that consists of helium nuclei is. a. X radiation c. beta radiation b. gamma radiation d. alpha radiation 82. Which symbol is used for an alpha particle? a. 2 He c. He 1 1 b. 2 He d. 4 He Which of the following materials is necessary to stop an alpha particle? a. three feet of concrete c. single sheet of aluminum foil b. three inches of lead d. single sheet of paper 84. What symbol is used for beta radiation? a. 0 e c. e 0 0 b. 0 e d A neutron breaks down to form. a. an alpha particle c. a proton and an electron b. two protons d. a helium nucleus 1 e 7

8 Name: 86. What particle is needed to complete this nuclear reaction? 251 Cf Cm + a. 4 He c. 1 H 2 1 b. 0 e d. n When radium-226 (atomic number 88) decays by emitting an alpha particle, it becomes. a. polonium-222 c. radium-222 b. polonium-224 d. radon What particle does nickel-57 emit when it decays to cobalt-57? (Remember to evaluate atomic numbers) a. neutron c. proton b. positron d. alpha particle 89. What particle is needed to complete the following equation? 14 N C H 7 a. 1 n c. 4 He 0 2 b. 0 e d Which of the following naturally occurring radioisotopes would be most useful in dating objects thought to be millions of years old? a. carbon-14; t 1 2 = years b. potassium-40; t 1 2 = years c. thorium-234; t 1 2 = 25 days d. radon-222; t 1 2 = 3.8 days 91. A reaction that results in the combining of smaller atomic nuclei is. a. chemical c. fusion b. fission d. ionization 92. For the reaction represented by the equation 2H 2 + O 2 2H 2 O, how many grams of water are produced from 6.00 mol of hydrogen? a g c g b g d. 144 g 0 e Short Answer 93. Determine the number of moles of N 2 that are required to produce 12 mol of NH 3 using the equation N 2 + 3H 2 2NH 3. Describe in words the method used. Then show the calculation. 94. Find the mass in grams of molecules of F Find the number of moles of argon in 607 g of argon. 96. What is the percent composition of NiO, if a sample of NiO with a mass of 41.9 g contains 33.1 g Ni and 8.8 g O? 97. If a total of 13.5 mol of NaHCO 3 and 4.5 mol of C 6 H 8 O 7 react, how many moles of CO 2 and Na 3 C 6 H 5 O 7 will be produced? 3NaHCO 3 (aq) + C 6 H 8 O 7 (aq) 3CO 2 (g) + 3H 2 O(s) +Na 3 C 6 H 5 O 7 (aq) 8

9 Name: 98. If 8.6 L of H 2 reacted with 4.3 L of O 2 at STP, what is the volume of the gaseous water collected (assuming that none of it condenses)? 2H 2 (g) + O 2 (g) 2H 2 O(g) 99. How many grams of CO are needed to react with an excess of Fe 2 O 3 to produce g Fe? Fe 2 O 3 (s) + 3CO(g) 3CO 2 (g) + 2Fe(s) 100. Solid sodium reacts violently with water, producing heat, hydrogen gas, and sodium hydroxide. How many molecules of hydrogen gas are formed when 48.7 g of sodium are added to water? 2Na + 2H 2 O 2NaOH + H The volume of a gas is 245 ml at kpa pressure. What will the volume be when the pressure is reduced to 48.5 kpa, assuming the temperature remains constant? 102. A balloon filled with helium has a volume of 36.5 L at a pressure of 160 kpa and a temperature of 11.5 C. What will the volume of the balloon be if the temperature is increased to 87.0 C and the pressure remains constant? 103. A gas has a volume of 615 ml at a temperature of 54.5 C. What volume will the gas occupy at 37.0 C? 104. A rigid container of O 2 has a pressure of 410 kpa at a temperature of 737 K. What is the pressure at 270 K? 105. The gaseous product of a reaction is collected in a 23.0-L container at 23 C. The pressure in the container is kpa and the gas has a mass of 97.0 g. How many moles of the gas are in the container? 106. A mixture of gases at a total pressure of 92 kpa contains N 2, CO 2, and O 2. The partial pressure of the CO 2 is 24 kpa and the partial pressure of the N 2 is 48 kpa. What is the partial pressure of the O 2? 107. How many grams of copper sulfate pentahydrate (CuSO 4 5H 2 O) would you heat to produce 29.8 g of water? 108. If the [H ] in a solution is mol/l, what is the [OH ]? 109. Calculate the hydrogen-ion concentration [H ] for an aqueous solution in which [OH ] is mol/l. Is this solution acidic, basic, or neutral? 110. If the ph is 2, what is the concentration of hydroxide ion? 111. A liter of impure water has 10 8 mol of hydroxide ions. What is the concentration of hydronium ions in this sample of water? 112. If the hydroxide-ion concentration is M, what is the ph of the solution? 113. If the hydrogen-ion concentration is M, what is the poh of the solution? 114. What is the ph if the hydrogen-ion concentration is M? 115. If the half-life of a radioactive material is 6 years, how many years will it take for one half of the original amount of material to decay? 116. After 56 days, 4 g of phosphorus-32 has decayed to 0.25 g. What is the half-life of phosphorus-32? 117. What is the half-life of phosphorus-32 if, after 42 days, g remains from a 3.00-g starting sample? 9

10 Name: Problem 118. Sulfur in gasoline can produce sulfuric acid, H 2 SO 4, according to the two-step process shown below. For each 125 g of sulfur in gasoline, how many moles of H 2 SO 4 will be produced? S(s) O 2 (g) SO 2 (g) 2SO 2 (g) 2H 2 O(l) O2(g) 2H 2 SO 4 (aq) 119. A solution contains 85.0 g of NaNO 3, and has a volume of 750. ml. Find the molarity of the solution. (molar mass of NaCl = g/mol) Essay 120. Why is it possible to calculate the density of a gas at STP, knowing only its molar mass, but it is not possible to make the same calculation for a solid or a liquid? 121. When a mixture of sulfur and metallic silver is heated, silver sulfide is produced. What mass of silver sulfide is produced from a mixture of 3.0 g Ag and 3.0 g S 8? 16Ag(s) + S 8 (s) 8Ag 2 S(s) Numeric Response 122. How many water molecules are in 39 formula units of calcium chloride dihydrate (CaCl 2 2H 2 O)? 123. If the hydrogen ion concentration is 10 3 M, what is the ph of the solution? 124. If the hydroxide ion concentration is M, what is the ph of the solution? 125. What is the ph when the hydrogen ion concentration is M? 10

11 Chemistry I - Spring Semester Exam Answer Section MULTIPLE CHOICE 1. ANS: D PTS: 1 DIF: III REF: 3 OBJ: 1 2. ANS: A Solution: g LiF 1molLiBr mol LiBr g LiBr PTS: 1 DIF: III REF: 3 OBJ: 2 3. ANS: A PTS: 1 DIF: L1 REF: p. 188 OBJ: ANS: A PTS: 1 DIF: L1 REF: p. 188 OBJ: ANS: D PTS: 1 DIF: L1 REF: p. 194 OBJ: ANS: B PTS: 1 DIF: L2 REF: p. 192 p. 195 OBJ: ANS: A PTS: 1 DIF: L2 REF: p. 192 p. 194 OBJ: ANS: B PTS: 1 DIF: I REF: 1 OBJ: 1 9. ANS: D Solution: 250. g O 2 1molO g O 2 2molKClO 3 3molO or5.21molKClO 3 PTS: 1 DIF: III REF: 2 OBJ: ANS: C Solution: 300. g Cl 2 1molCl 2 2molKCl 74.55gKCl g KCl 70.90gCl 2 1molCl 2 1molKCl 300. g KBr 1molKBr g KBr 2molKCl g KCl g KCl 2molKBr 1molKCl Since Cl 2 would produce the most KCl, KBr is the limiting reactant, thus 188 G KCl is produced. PTS: 1 DIF: III REF: 2 OBJ: ANS: D PTS: 1 DIF: I REF: 3 OBJ: 1 1

12 12. ANS: D Solution: 500. g SO 3 1molSO g SO 3 1molH 2 SO 4 1molSO g H 2 SO 4 1molH 2 SO g H 2 SO 4 percentage yield experimental yield actual yield 100 percentage yield 575 g 100 = or 93.9% g PTS: 1 DIF: III REF: 3 OBJ: ANS: C PTS: 1 DIF: L1 REF: p. 291 p. 292 OBJ: ANS: C PTS: 1 DIF: L1 REF: p. 290 OBJ: ANS: A PTS: 1 DIF: L2 REF: p. 290 p. 291 OBJ: ANS: D PTS: 1 DIF: L2 REF: p. 291 p. 292 OBJ: ANS: B PTS: 1 DIF: L2 REF: p. 294 OBJ: ANS: A PTS: 1 DIF: L1 REF: p. 295 OBJ: ANS: D PTS: 1 DIF: L2 REF: p. 297 p. 298 OBJ: ANS: C PTS: 1 DIF: L2 REF: p. 302 OBJ: ANS: C PTS: 1 DIF: L3 REF: p. 302 OBJ: ANS: A PTS: 1 DIF: L1 REF: p. 309 OBJ: ANS: D PTS: 1 DIF: I REF: 1 OBJ: ANS: C PTS: 1 DIF: II REF: 1 OBJ: ANS: D PTS: 1 DIF: II REF: 1 OBJ: ANS: B PTS: 1 DIF: I REF: 1 OBJ: ANS: A PTS: 1 DIF: II REF: 1 OBJ: ANS: A PTS: 1 DIF: I REF: 2 OBJ: ANS: B PTS: 1 DIF: I REF: 2 OBJ: 5 2

13 30. ANS: B Solution: M mol L mol 7.98 L M PTS: 1 DIF: III REF: 3 OBJ: ANS: A Solution: 125 g NaCl 1molNaCl mol NaCl 58.44gNaCl M mol L mol or M 4.00 L PTS: 1 DIF: III REF: 3 OBJ: ANS: A PTS: 1 DIF: L1 REF: p. 354 OBJ: ANS: A PTS: 1 DIF: L2 REF: p. 356 OBJ: ANS: A PTS: 1 DIF: L1 REF: p. 363 p. 364 p. 365 p. 366 OBJ: ANS: C PTS: 1 DIF: L2 REF: p. 360 p. 361 p. 362 OBJ: ANS: B PTS: 1 DIF: L2 REF: p. 363 p. 364 p. 365 p. 366 OBJ: ANS: B PTS: 1 DIF: L2 REF: p. 363 p. 364 p. 365 p. 366 OBJ: ANS: B PTS: 1 DIF: L1 REF: p. 369 OBJ: ANS: B PTS: 1 DIF: L2 REF: p. 371 OBJ: ANS: C PTS: 1 DIF: I REF: 1 OBJ: ANS: A PTS: 1 DIF: II REF: 1 OBJ: ANS: A PTS: 1 DIF: I REF: 1 OBJ: ANS: A PTS: 1 DIF: I REF: 1 OBJ: ANS: B PTS: 1 DIF: I REF: 1 OBJ: ANS: A PTS: 1 DIF: I REF: 1 OBJ: ANS: A PTS: 1 DIF: II REF: 1 OBJ: ANS: A PTS: 1 DIF: II REF: 1 OBJ: 5 3

14 48. ANS: D PTS: 1 DIF: I REF: 2 OBJ: ANS: B PTS: 1 DIF: I REF: 3 OBJ: ANS: C PTS: 1 DIF: II REF: 3 OBJ: ANS: D PTS: 1 DIF: I REF: 3 OBJ: ANS: A PTS: 1 DIF: I REF: 3 OBJ: ANS: A PTS: 1 DIF: L1 REF: p. 418 OBJ: ANS: C PTS: 1 DIF: L1 REF: p. 418 OBJ: ANS: A PTS: 1 DIF: L1 REF: p. 420 OBJ: ANS: D PTS: 1 DIF: L1 REF: p. 422 OBJ: ANS: D PTS: 1 DIF: L2 REF: p. 419 OBJ: ANS: C PTS: 1 DIF: L2 REF: p. 421 OBJ: ANS: C PTS: 1 DIF: L2 REF: p. 419 OBJ: ANS: C PTS: 1 DIF: L2 REF: p. 434 OBJ: ANS: A PTS: 1 DIF: L2 REF: p. 434 OBJ: ANS: C PTS: 1 DIF: L1 REF: p. 447 OBJ: ANS: C PTS: 1 DIF: L1 REF: p. 447 OBJ: ANS: D PTS: 1 DIF: L2 REF: p. 446 OBJ: ANS: C PTS: 1 DIF: L2 REF: p. 446 OBJ: ANS: A PTS: 1 DIF: L2 REF: p. 446 OBJ: ANS: D PTS: 1 DIF: L3 REF: p. 446 OBJ: ANS: C PTS: 1 DIF: L1 REF: p. 452 p. 453 OBJ: ANS: D PTS: 1 DIF: L1 REF: p. 460 OBJ: ANS: C PTS: 1 DIF: L1 REF: p. 588 OBJ: ANS: B PTS: 1 DIF: L1 REF: p. 592 OBJ:

15 72. ANS: A PTS: 1 DIF: L2 REF: p. 592 OBJ: ANS: B PTS: 1 DIF: L2 REF: p. 591 OBJ: ANS: D PTS: 1 DIF: L1 REF: p. 594 OBJ: ANS: B PTS: 1 DIF: L1 REF: p. 597 OBJ: ANS: B PTS: 1 DIF: L2 REF: p. 601 OBJ: ANS: D PTS: 1 DIF: L1 REF: p. 605 OBJ: ANS: A PTS: 1 DIF: L3 REF: p. 607 OBJ: ANS: C PTS: 1 DIF: L1 REF: p. 800 OBJ: ANS: C PTS: 1 DIF: L1 REF: p. 800 OBJ: ANS: D PTS: 1 DIF: L1 REF: p. 800 OBJ: ANS: D PTS: 1 DIF: L2 REF: p. 800 OBJ: ANS: D PTS: 1 DIF: L2 REF: p. 800 OBJ: ANS: B PTS: 1 DIF: L2 REF: p. 801 OBJ: ANS: C PTS: 1 DIF: L2 REF: p. 801 OBJ: ANS: A PTS: 1 DIF: L2 REF: p. 801 OBJ: ANS: D PTS: 1 DIF: L2 REF: p. 800 p. 804 OBJ: ANS: B PTS: 1 DIF: L2 REF: p. 801 OBJ: ANS: A PTS: 1 DIF: L3 REF: p. 803 p. 804 OBJ: ANS: B PTS: 1 DIF: L2 REF: p. 804 p. 805 OBJ: ANS: C PTS: 1 DIF: L1 REF: p. 810 OBJ: ANS: D Solution: 8.00 mol H 2 2molH 2 O 2molH g H 2 O 1molH 2 O 144 g H 2 O PTS: 1 DIF: III REF: 2 OBJ: 2 5

16 SHORT ANSWER 93. ANS: Mole ratios are necessary here. The balanced equation gives us a 1:2 ratio between nitrogen and ammonia. Since the product of the means equals the product of the extremes, 1 2 x 12 x 6molN 2 PTS: 1 DIF: II REF: 1 OBJ: ANS: molecules 1 mol F 2 / molecules 38.0 g F 2 /1 mol F 2 = 19.6 g F 2 PTS: 1 DIF: L2 REF: p. 297 OBJ: ANS: 607 g Ar 1 mol Ar/39.9 g Ar = 15.2 mol Ar PTS: 1 DIF: L2 REF: p. 299 OBJ: ANS: 33.1 g Ni/41.9 g NiO 100% = 79% Ni 8.8 g O/41.9 g NiO 100% = 21% O PTS: 1 DIF: L2 REF: p. 307 OBJ: ANS: 13.5 mol of CO 2 ; 4.5 mol of Na 3 C 6 H 5 O 7 PTS: 1 DIF: L1 REF: p. 359 OBJ: ANS: 8.6 L H 2 / (22.4 L/1 mol) 2 mol H 2 O/2 mol H L/ 1 mol = 8.6 L H 2 O PTS: 1 DIF: L2 REF: p. 363 OBJ: ANS: g Fe 1 mol Fe/55.85 g Fe 3 mol CO/2 mol Fe g CO/1 mol CO = g CO PTS: 1 DIF: L2 REF: p. 371 OBJ: ANS: Assume the sodium is limiting: 48.7 g Na 1 mol Na/23.0 g Na 1 mol H 2 /2 mol Na ( molecules H 2 )/1 mol H 2 = molecules H 2 PTS: 1 DIF: L3 REF: p. 371 OBJ:

17 101. ANS: V 2 = V 1 P 1 P 2 = 245 ml kpa 48.5 kpa = 1596 ml PTS: 1 DIF: L2 REF: p. 419 OBJ: ANS: V 2 = V 1 T 2 T 1 = 36.5 L.0K K = 46.2 L PTS: 1 DIF: L2 REF: p. 421 OBJ: ANS: T 1 = 54.5 C = 219 K T 2 = 37.0 C = 310 K V 2 = V 1 T 2 T 1 = 615 ml 310 K = 873 ml 219 K PTS: 1 DIF: L2 REF: p. 421 OBJ: ANS: P 2 = P 1 T 2 T ANS: n = PV RT = = 410 kpa 270 K = 150 kpa 737 K PTS: 1 DIF: L2 REF: p. 421 OBJ: kpa 23.0 L 8.31 (L kpa)/(k mol) 296 K = 3.0 mol PTS: 1 DIF: L2 REF: p. 427 OBJ: ANS: P O 2 = P total (P CO 2 + P N 2 ) = 92 kpa (48 kpa + 24 kp) = 20 kpa PTS: 1 DIF: L2 REF: p. 434 OBJ: ANS: 29.8 g H 2 O = 1.66 mol H 2 O molar mass CuSO 4 5H 2 O = g mol CuSO 4 5H 2 O 5 mol H 2 O g CuSO 4 5H 2 O 1mol CuSO 4 5H 2 O 1mol CuSO 5H O mol H 5molH 2 O 2 O = 82.6 g CuSO 4 5H 2 O PTS: 1 DIF: L3 REF: p. 454 p. 456 OBJ:

18 108. ANS: mol/l PTS: 1 DIF: L2 REF: p. 595 p. 596 OBJ: ANS: K w = [H ] [OH ] K [H w ] = [OH ] = mol 2 /L mol/l = mol/l The solution is acidic. PTS: 1 DIF: L3 REF: p. 595 OBJ: ANS: M PTS: 1 DIF: L1 REF: p. 598 OBJ: ANS: 10 6 M PTS: 1 DIF: L1 REF: p. 598 OBJ: ANS: K w = [H ] [OH ] K [H w ] = [OH ] = mol 2 /L mol/l = mol/l ph = - log [H ] = - log [ mol/l] = 2.0 PTS: 1 DIF: L2 REF: p. 598 OBJ:

19 113. ANS: K w = [H ] [OH ] [OH ] = K w [H ] = mol 2 /L mol/l = mol/l poh = log [OH ] = log [ mol/l] = 1.0 PTS: 1 DIF: L2 REF: p. 601 OBJ: ANS: ph = log [H ] = log ( ) = ( 6.2) = 6.2 or ph = (log log 10 7 ) = (0.833) ( 7) = 6.2 PTS: 1 DIF: L2 REF: p. 599 OBJ: ANS: 6 years PTS: 1 DIF: L1 REF: p. 804 OBJ: ANS: 14 days PTS: 1 DIF: L2 REF: p. 804 p. 806 OBJ: ANS: 0.375g 3.00g = number of half-lives (exponent of 1/2) 42 days / 3 half-lives = 14 days (the half-life time) PTS: 1 DIF: L3 REF: p. 804 OBJ: PROBLEM 118. ANS: 3.90 mol H 2 SO g S 1molSO g S 1molSO 2 1molS 1molH 2 SO 4 2molSO mol H 2 SO 4 PTS: 1 DIF: III REF: 2 OBJ: 2 9

20 119. ANS: 1.33 M NaNO 3 Solution: 85.0 g NaNO ml 1 molnano ml 1.33 M NaNO 85.0 g NaNO 3 1L 3 PTS: 1 DIF: III REF: 3 OBJ: 1 ESSAY 120. ANS: The molar volume of any gas is 22.4 L at STP. The density can be calculated in the following way: molar mass of ANY gas (g)/1 mol 1 mol/22.4 L = density of gas (g/l). The molar volumes of different solids and liquids are not uniformly the same at any prescribed condition. PTS: 1 DIF: L3 REF: p. 302 OBJ: ANS: The limiting reagent is silver. 3.0 g Ag 1 mol Ag/108 g Ag = 0.03 mol Ag 3.0 g S 8 1 mol S 8 /256 g S 8 = 0.01 mol S mol Ag 8 mol Ag 2 S/16 mol Ag 248 g Ag 2 S/1 mol Ag 2 S = 3.72 g Ag 2 S 3.72 g of silver sulfide is produced. PTS: 1 DIF: L3 REF: p. 363 p. 364 p. 365 p. 366 OBJ: NUMERIC RESPONSE 122. ANS: 78 PTS: 1 DIF: L3 REF: p. 454 OBJ: ANS: 3 PTS: 1 DIF: L1 REF: p. 596 p. 597 OBJ: ANS: 3 PTS: 1 DIF: L1 REF: p. 601 OBJ: ANS: 1.3 PTS: 1 DIF: L2 REF: p. 597 p. 598 OBJ: