This Document Contains Chapters 11 to 12 Chapter 11 Gases True/False Questions 1. Straws work because sucking creates a pressure difference. Answer: True 2. Gases are a collection of particles in constant, unpredictable motion. Answer: False 3. Gas particles act independently of each other. Answer: True 4. Gas particles lose energy every time they collide with each other or the container wall. Answer: False 5. There is a large distance between gas particles as compared to their relative size. Answer: True 6. As you increase temperature, you increase the average energy of the gas particles. Answer: True 7. Gases and liquids are compressible, but solids are not. Answer: False 8. Gases fill the entire volume of their container. Answer: True 9. The expected order of density for matter is gases < liquids < solids. Answer: True 10. Pressure is calculated by: P = Area/Force. Answer: False 11. The unit of pressure known as the atmosphere (atm) is defined as the average pressure found at the top of Mount Everest. Answer: False 12. Pressure depends on how many gas particles are in a container. Answer: True 13. As we climb a mountain to a higher altitude, we experience a pressure decrease. Answer: True 14. If the column of mercury in a barometer drops to a lower reading, this means the measured pressure has decreased. Answer: True 15. A pedometer is a device created by Torricelli to measure pressure. Answer: False 16. The conversion factor for pressure is 1 mm Hg = 1 atm. Answer: False 17. Boyle's law states that as the volume of a gas increases so does the pressure. Answer: False 18. A sealed bag of potato chips will expand when taken to a higher altitude. This is an example of Boyle's law. Answer: True 19. The volume of a gas is independent of the temperature. Answer: False 20. For all gas law calculations, the temperature must be in kelvins. Answer: True 21. Charles's Law provides an explanation of why hot air balloons float. Answer: True 22. Absolute zero refers to 0°C. Answer: False 23. If the temperature of a gas is doubled, the volume is doubled provided that the pressure and the number of particles remains constant. Answer: True 24. The volume of a gas and the number of particles is inversely proportional. Answer: False 25. One mole of F2 gas at STP would take up twice the volume of one mole of Ar gas at STP. Answer: False 26. If the number of gas particles is halved, the volume of the gas will be halved given that the temperature and pressure do not change. Answer: True 27. If the number of gas particles is tripled, the volume will be 1/3 of the original given that temperature and pressure do not change. Answer: False 28. If a slow leak in an inner tube has reduced the volume of the tube to one-third its original inflated volume, this means that one-third of the moles of gas have escaped the tube. (Assume constant temperature and pressure.) Answer: False 29. If you had a five liter balloon of argon gas and a five liter balloon of xenon gas, and you removed 10 grams of gas from each balloon, the balloons would both shrink down to the same size. Answer: False 30. The main component of the air we breathe is oxygen gas. Answer: False 31. A gas may not behave ideally under conditions of low pressure or high temperature. Answer: False 32. Dalton's law of partial pressure is: P = nRT/V. Answer: False 33. "Molar Mass" can be calculated using the formula: Molar mass = moles/mass. Answer: False 34. Using pure oxygen in scuba diving tanks is a good method of preventing the nitrogen bends. Answer: False 35. Vapor pressure of water increases with increasing temperature because the higher temperature causes more water molecules to evaporate. Answer: True 36. The vapor pressure of water is independent of temperature. Answer: False 37. The molar volume of any gas at conditions of standard temperature and pressure is 22.4 liters. Answer: True 38. STP conditions are 273 K and 760 mm Hg. Answer: True 39. The volume of 9.00 grams of water vapor at STP is 11.2 L. Answer: True Multiple Choice Questions 40. Which of the following statements about pressure is FALSE? A) Pressure is caused by gas molecules colliding with surfaces. B) The atmosphere has a pressure as the components of air collide with surfaces. C) After creating a pressure difference, the atmospheric pressure can push liquid up a straw. D) A deep well dug in the ground must have the pump located at the bottom of well in order to have the water come to the surface. E) All of the above statements are true. Answer: E 41. Which of the following is NOT part of the Kinetic Molecular Theory? A) Gas particles do not repel each other. B) There is a large distance between gas particles as compared to their relative size. C) The size of the actual gas particles is small compared to the volume of the whole gas. D) The average energy of the particles is dependent on the molecular mass of the particle. E) All of the above statements are part of the Kinetic Molecular Theory. Answer: D 42. Which of following statements are consistent with the Kinetic Molecular Theory? A) Gases are compressible because the volume of atoms is almost entirely open space. B) Gases assume the shape and volume of their container because they are in constant, straight-line motion. C) Gases have a low density because there is so much empty space between the particles. D) Gas particles collide with each other and surfaces without losing any energy. E) All of the above statements are consistent with the Kinetic Molecular Theory. Answer: E 43. All of the following statements are consistent with the kinetic molecular theory of gases EXCEPT A) The size of the gas molecules is negligible compared to the total volume of the gas. B) The average kinetic energy of the molecules of a gas is proportional to the temperature of the gas in kelvins. C) The gas molecules collide with each other and with the surfaces around them. D) Strong attractive forces hold the gas molecules together. E) none of the above Answer: D 44. 1 atm is equal to: A) 760 mm Hg. B) 760 torr. C) 101,325 Pa. D) 14.7 psi. E) all of the above Answer: E 45. 1 torr is equal to: A) 760 mm Hg. B) 1 mm Hg. C) 1 Pa. D) 14.7 psi. E) all of the above Answer: B 46. A barometer uses mercury because: A) it is a convenient, safe, lightweight material. B) the density of mercury is very large which allows the barometer to be short. C) it is the traditional substance used, water could be as easily used. D) it is the only liquid metal at room temperature. E) All of the above are true. Answer: B 47. What is the equivalent pressure of 0.905 atm in units of mm Hg? A) 688 B) 840 C) 0.905 D) 13.3 E) none of the above Answer: A 48. What is the equivalent pressure of 1520 torr in units of atm? A) 203,000 B) 380. C) 2.00 D) 1520 E) none of the above Answer: C 49. What is the equivalent pressure of 760 torr in units of mm Hg? A) 760 B) 1 C) 14.7 D) 29.92 E) none of the above Answer: A 50. What is the equivalent pressure of 968 mm Hg in units of atm? A) 1.27 atm B) 0.785 atm C) 968 atm D) 1.30 atm E) none of the above Answer: A 51. Which of the following statements is TRUE for gases? 1. The temperature of a gas is inversely proportional to its pressure. 2. The volume of a gas is directly proportional to the pressure in torr. 3. The pressure of a gas is due to collisions of the gas molecules. A) 1 only B) 2 only C) 3 only D) 1 and 2 only E) 1 and 3 only Answer: C 52. Boyle's Law is expressed as: A) V is proportional to 1/P B) P is proportional to V C) V is proportional to 1/T D) V is proportional to T E) none of the above Answer: A 53. To solve problems using Boyle's Law, which mathematical equation should be used? A) P1/V1 = P2/V2 B) P1V1 = P2V2 C) V1/P1 = V2/P2 D) P2V1 = P1V2 E) none of the above Answer: B 54. One liter of a gas is in a sealed chamber containing a moveable piston. If the piston is moved so that the volume of the gas is compressed to a volume of one-half liter, what will happen to the pressure on the gas? (Assume the temperature is constant and no gas particles are lost.) A) The pressure will remain the same. B) The pressure will be half of the original value. C) The pressure will be twice the original value. D) It would be impossible to move the piston since gases are not compressible. E) none of the above Answer: C 55. A balloon filled with 0.500 L of air at sea level is submerged in the water to a depth that produces a pressure of 3.25 atm. What is the volume of the balloon at this depth? A) 1.63 L B) 0.154 L C) 6.50 L D) 0.615 L E) none of the above Answer: B 56. Divers often inflate heavy duty balloons attached to salvage items on the sea floor. If a balloon is filled to a volume of 3.00 L at a pressure of 2.50 atm, what is the volume of the balloon when it reaches the surface? A) 7.50 L B) 1.20 L C) 0.833 L D) 5.50 L E) none of the above Answer: A 57. The initial volume of a gas cylinder is 750.0 mL. If the pressure of a gas inside the cylinder changes from 840.0 mm Hg to 360.0 mm Hg, what is the final volume the gas occupies? A) 3.151 L B) 630.0 mL C) 1.750 L D) 321.4 mL E) none of the above Answer: C 58. Charles's Law is expressed as: A) V is proportional to 1/P B) P is proportional to V C) V is proportional to 1/T D) V is proportional to T E) none of the above Answer: D 59. To solve problems using Charles's Law, which mathematical equation should be used? A) V1/T1 = V2/T2 B) T1V1 = T2V2 C) P1/V2 = P2/V1 D) P2V1 = P1V2 E) none of the above Answer: A 60. Which one of the following is impossible for an ideal gas? A) 1/V2 = T1/T2(1/V1) B) V1/T1 = V2/T2 C) V2 = (T2/T1) V1 D) V1T1 = V2T2 E) none of the above Answer: D 61. A gas sample occupies 3.50 liters of volume at 20.°C. What volume will this gas occupy at 100.°C (reported to three significant figures)? A) 0.224 L B) 2.75 L C) 4.46 L D) 17.5 L E) none of the above Answer: C 62. What is the final volume of a balloon that was initially 500.0 mL at 25°C and was then heated to 50°C? A) 461 mL B) 193 mL C) 1.00 L D) 542 mL E) none of the above Answer: D 63. If the volume of a gas container at 32.0°C changes from 1.55 L to 755 mL, what will the final temperature be? A) 149°C B) 353°C C) 273°C D) -124°C E) none of the above Answer: D 64. What is the initial temperature of a gas if the volume changed from 1.00 L to 1.10 L and the final temperature was determined to be 255.0°C? A) 480°C B) -41°C C) 232°C D) 207°C E) none of the above Answer: D 65. A balloon originally had a volume of 0.439 L at 44°C and a pressure of 729 torr. To what temperature must the balloon be cooled to reduce its volume to 378 mL if the pressure remained constant? A) 0°C B) 38°C C) 95°C D) 273°C E) none of the above Answer: A 66. Gas density can be calculated by dividing the mass of gas by its volume. If you took a balloon of gas and then warmed the balloon in a sunny window, what can now be said about the density of the gas in the balloon? A) The gas density will remain the same. B) The gas density will increase. C) The gas density will decrease. D) The density of gases is independent of temperature. E) none of the above Answer: C 67. What is the proper form of the combined gas law? A) P1T1/V1 = P2T2/V2 B) V1T1/P1 = V2T2/P2 C) P1V1/T1 = P2V2/T2 D) P1V1T1 = P2V2T2 E) none of the above Answer: C 68. A certain volume of gas was confined in a rigid container. If the pressure of the gas sample in the container was doubled, what happened to the temperature? A) The temperature became one half. B) The temperature doubled. C) The temperature increased four times. D) The temperature decreased one-third. E) not enough information Answer: B 69. Suppose a balloon was released from the ground and rose to such a height that both the atmospheric pressure and atmospheric temperature decreased. Which statement is TRUE? A) Both the temperature and pressure changes act to increase the balloon's volume. B) Both the temperature and pressure changes act to decrease the balloon's volume. C) The temperature change acts to increase the balloon's volume. D) The pressure change acts to decrease the balloon's volume. E) none of the above Answer: E 70. If the initial pressure of a system was 1.00 atm and the volume was halved and the temperature was tripled, what is the final pressure? A) 2.00 atm B) 0.667 atm C) 1.50 atm D) 6.00 atm E) not enough information Answer: D 71. A 325 mL sample of gas is initially at a pressure of 721 torr and a temperature of 32°C. If this gas is compressed to a volume of 286 mL and the pressure increases to 901 torr, what will be the new temperature of the gas (reported to three significant figures in °C)? A) 35.2°C B) 335°C C) 62.4°C D) 215°C E) none of the above Answer: C 72. A sample of helium gas initially at 37.0°C, 785 torr and 2.00 L was heated to 58.0°C while the volume expanded to 3.24 L. What is the final pressure in atm? A) 517 B) 0.681 C) 1.79 D) 3.21 E) none of the above Answer: B 73. What is the final volume of a 500.0 mL gas container that increased in temperature from 299 K to 333 K while the pressure increased from 1.00 atm to 1.54 atm? A) 0.691 L B) 2.77 L C) 0.362 L D) 1.45 L E) none of the above Answer: C 74. What is the initial temperature (°C) of a system that has the pressure decreased by 10 times while the volume increased by 5 times with a final temperature of 150 K? A) 27 B) 75 C) -198 D) 300 E) none of the above Answer: A 75. Avogadro's Law is expressed as: A) V is proportional to 1/n B) P is proportional to n C) n is proportional to 1/T D) V is proportional to n E) none of the above Answer: D 76. To solve problems using Avogadro's Law, which mathematical equation should be used? A) n1/P1 = n2/p2 B) n1V1 = n2V2 C) V1/n1 = V2/n2 D) P1V1 = P2V2 E) none of the above Answer: C 77. What happens to the volume of a gas when you double the number of moles of gas while keeping the temperature and pressure constant? A) The volume is halved. B) The volume doubles. C) The volume decreases, but more information is needed. D) The volume increases, but more information is needed. E) none of the above Answer: B 78. How many moles of gas were added to a balloon that started with 2.3 moles of gas and a volume of 1.4 L given that the final volume was 7.2 L? A) 9.5 B) 4.4 C) 12 D) 0.085 E) none of the above Answer: A 79. If each of the following gas samples have the same temperature and pressure, which sample has the greatest volume? A) 1 gram of O2 B) 1 gram of Ar C) 1 gram of H2 D) all have the same volume E) not enough information Answer: C 80. For an ideal gas, which of the following pairs of variables are inversely proportional to each other (if all other factors remain constant)? A) P, V B) P, T C) V, T D) n, P E) none of the above Answer: A 81. The ideal gas law is: A) PV = nRT B) P = nRT/V C) T = PV/nR D) V = nRT/P E) All of the above are forms of the ideal gas law. Answer: E 82. A sample of 0.255 mole of gas has a volume of 748 mL at 28°C. Calculate the pressure of this gas. (R = 0.0821 L⋅atm/mol⋅K) A) 8.42 atm B) 0.784 atm C) 0.00842 atm D) 7.84 × 10-4 atm E) none of the above Answer: A 83. What is the pressure of a 3.00 L gas vessel that has 18.0 grams of helium at 25°C? (R = 0.0821 L atm/ mol K) A) 147 atm B) 36.7 atm C) 32.6 atm D) 1.81 atm E) none of the above Answer: B 84. What is the temperature (°C) of 2.48 moles of gas stored in a 30.0 L container at 1559 mm Hg? (R = 0.0821 L atm/ mol K) A) 302 B) 189 C) 29 D) -84 E) none of the above Answer: C 85. Which conditions can cause nonideal gas behavior by 1) decreasing the space between gas particles or 2) by slowing gas particles so that interactions are significant? A) 1) high pressure; 2) high temperature B) 1) high pressure; 2) low temperature C) 1) low pressure; 2) high temperature D) 1) low pressure ; 2) low temperature E) none of the above Answer: B 86. A 3.76 g sample of a noble gas is stored in a 2.00 L vessel at 874 torr and 25°C. What is the noble gas? (R = 0.0821 L atm/ mol K) A) He B) Ne C) Ar D) Kr E) not enough information Answer: C 87. Which of the following diatomic elements would have a mass of 19.08 grams stored in a 3.82 L container at 3,632 mm Hg and 100°C? A) H2 B) Br2 C) F2 D) O2 E) not enough information. Answer: D 88. What is the major component of the air we breathe? A) nitrogen B) oxygen C) argon D) carbon dioxide E) smog Answer: A 89. What is the third most abundant component of dry air? A) carbon dioxide B) oxygen C) nitrogen D) argon E) smog Answer: D 90. If a mixture of gases contained 78% nitrogen at a pressure of 984 torr and 22% carbon dioxide at 345 torr, what is the total pressure of the system? A) 1,329 atm B) 17.5 cm Hg C) 639 torr D) 1.75 atm E) none of the above Answer: D 91. A gas cylinder contains only the gases radon, nitrogen, and helium. The radon has a pressure of 222 torr while the nitrogen has a pressure of 446 torr. If the total pressure inside the cylinder is 771 torr, what is the pressure that is due to the helium? A) 771 torr B) 668 torr C) 549 torr D) 103 torr E) none of the above Answer: D 92. A "shielding gas" mixture of argon and carbon dioxide is sometimes used in welding to improve the strength of the weld. If a gas cylinder of this two-part mixture was at 4.0 atm pressure and this mixture was 90.% argon, what would be the pressure due to the carbon dioxide gas component? A) 3.6 atm B) 0.40 atm C) 10. atm D) 4.0 atm E) none of the above Answer: B 93. What problem could happen if deep sea divers used pure oxygen in their tanks? A) hypoxia B) oxygen toxicity C) nitrogen narcosis D) rapture of oxygen E) none of the above Answer: B 94. Human lungs have evolved to breathe oxygen at a pressure as that in the atmosphere, 0.21 atm. If a particular heliox mixture to be carried by a scuba diver is at a pressure of 7.00 atm, what should be the partial pressure due to helium in order to maintain the pressure due to oxygen at 0.21 atm? A) 0.21 atm B) 7.00 atm C) 6.79 atm D) 7.21 atm E) none of the above Answer: C 95. The vapor pressure of water at 20.0°C is 17.5 mm Hg. If the pressure of a gas collected over water was measured to be 453.0 mm Hg. What is the pressure of the pure gas? A) 0.0230 atm B) 0.619 atm C) 0.573 atm D) 0.596 atm E) none of the above Answer: C 96. Hydrogen gas produced in the laboratory by the reaction of zinc and hydrochloric acid was collected over water at 25°C. The barometric pressure at the time was 742.5 mm Hg. What is the pressure of dry hydrogen gas if the vapor pressure of water at 25°C is 23.8 mm Hg? A) 742.5 mm Hg B) 718.7 mm Hg C) 766.3 mm Hg D) 760.0 mm Hg E) none of the above Answer: B 97. Which set of conditions reflect STP? A) 298 K, 1 atm B) 25°C, 14.7 psi C) 373 K, 760 torr D) 273 K, 1 Pa E) 273 K, 760 mm Hg Answer: E 98. At STP, 12.69 g of a noble gas occupies 14.09 L. What is the identity of the noble gas? (R = 0.0821 L atm/ mol K) A) He B) Ne C) Ar D) Kr E) not enough information Answer: B 99. Suppose you had a balloon containing 1 mole of helium at STP and a balloon containing 1 mole of oxygen at STP. Which statement is TRUE? A) The balloons will have the same volume. B) The balloons will have the same mass. C) Both A) and B) are true. D) Neither A) nor B) are true. E) not enough information Answer: A 100. Ammonia gas decomposes according to the equation: 2NH3(g) → N2(g) + 3H2(g) If 15.0 L of nitrogen is formed at STP, how many liters of hydrogen will be produced (also measured at STP)? A) 15.0 L B) 30.0 L C) 45.0 L D) 90.0 L E) not enough information Answer: C 101. Water can be formed according to the equation: 2H2 (g) + O2 (g) → 2H2O (g) If 8.0 L of hydrogen is reacted at STP, exactly how many liters of oxygen at STP would be needed to allow complete reaction? A) 4.0 L B) 2.0 L C) 1.0 L D) 8.0 L E) none of the above Answer: A 102. How many liters of O2 (g) are needed to react completely with 56.0 L of CH4 (g) at STP to produce CO2 (g) and H2O (g)? Given: CH4 (g) + 2O2 (g) → CO2 (g) + H2O (g) A) 28.0 L B) 56.0 L C) 84.0 L D) 112. L E) none of the above Answer: D Algorithmic Questions 103. What is the pressure of 760 mm Hg when expressed in units of in Hg? A) 29.92 in Hg B) 101,325 in Hg C) 760 in Hg D) 1 in Hg E) none of the above Answer: A 104. What is the final pressure of a system (atm) that has the volume increased from 0.75 L to 1.1 L with an initial pressure of 1.25 atm? A) 1.1 B) 0.85 C) 1.8 D) 1.2 E) none of the above Answer: B 105. What is the final volume (L) of 10.0 L system that has the pressure quartered? A) 0.250 B) 17.1 C) 2.50 D) 40.0 E) none of the above Answer: D 106. What is the final volume of a gas that initially occupies 2.50 L at 298 K and is subsequently heated to 321 K? A) 2.69 L B) 2.96 L C) 2.23 L D) 2.32 L E) none of the above Answer: A 107. What is the change in temperature of a 2.50 L system when it is compressed to 1.75 L if the initial temperature was 298 K? A) 209 K B) 290 K C) -89 K D) -98 K E) none of the above Answer: C 108. What is the final volume (L) of a 1.00 L system at 315 K and 1.10 atm if STP conditions are established? A) 1.05 B) 0.935 C) 1.50 D) 0.953 E) none of the above Answer: D 109. What is the final pressure (atm) of a 3.05 L system initially at 724 mm Hg and 298 K that is compressed to a final volume of 2.51 L at 273 K? A) 1.06 B) 1.60 C) 806 D) 860 E) none of the above Answer: A 110. If the number of moles of a gas initially contained in a 2.10 L vessel is doubled, what is the final volume of the gas in liters? (Assume the pressure and temperature remain constant.) A) 6.30 B) 1.05 C) 4.20 D) 8.40 E) none of the above Answer: C 111. What is the molecular weight of a gas if a 15.0 g sample has a pressure of 836 mm Hg at 25°C in a 2.00 L flask? (R = 0.0821 L atm/ mol K) A) 176 amu B) 1.35 amu C) 167 amu D) 11.1 amu E) none of the above Answer: C 112. What is the pressure of a 1.0 L flask containing 0.60 g of He at 25°C? (R = 0.0821 L atm/ mol K) A) 98 atm B) 3.7 atm C) 7.3 atm D) 15 atm E) none of the above Answer: B 113. What is the volume of 28.0 g of nitrogen gas at STP? A) 33.6 L B) 11.2 L C) 22.4 L D) 44.8 L E) none of the above Answer: C Chapter 12 Liquids, Solids, and Intermolecular Forces True/False Questions 1. Intermolecular forces are the attractive forces between atoms within a compound. Answer: False 2. The shapes of protein molecules are determined by intermolecular forces. Answer: True 3. Intermolecular forces determine if a substance is a solid, liquid or gas at room temperature. Answer: True 4. Gases typically have high densities in comparison to solids. Answer: False 5. Liquids can be easily compressed. Answer: False 6. Atoms in a solid are always arranged in a well-ordered pattern. Answer: False 7. Solids usually have much greater densities than gases because molecules of a solid are much farther apart. Answer: False 8. Without intermolecular forces, solids and liquids would not exist and all matter would be gaseous. Answer: True 9. The strength of the surface tension is inversely related to the strength of the intermolecular forces. Answer: False 10. Liquids that are viscous flow more slowly than liquids that are not viscous. Answer: True 11. Viscosity increases with increased intermolecular force because the molecules attract each other strongly which hinders the flow. Answer: True 12. Evaporation is decreased by increasing the intermolecular forces. Answer: True 13. Compounds with very high vapor pressures must have very minimal intermolecular forces. Answer: True 14. The rate of evaporation will increase if you pour a liquid out onto a large surface. Answer: True 15. Increasing the temperature increases the vaporization rate of a liquid because the excess energy is used to break covalent bonds. Answer: False 16. Oil would be considered a nonvolatile liquid while gasoline would be considered volatile. Answer: True 17. The boiling point is the temperature at which the vapor pressure of a solution is equal to the intermolecular forces. Answer: False 18. Evaporation is an endothermic process. Answer: True 19. Evaporation and condensation are opposite processes. Answer: True 20. The process of heating a pot of water from room temperature to boiling temperature is an exothermic process. Answer: False 21. Water has a heat of vaporization of 44.0 kJ/mol while the chemical diethyl ether has a heat of vaporization of 27.1 kJ/mol. This shows that one mole of water would vaporize more easily than would one mole of diethyl ether. Answer: False 22. When one mole of water vapor at 100°C condenses, it will release an amount of energy equivalent to its heat of vaporization (40.7 kJ). Answer: True 23. Intermolecular forces hold atoms and molecules in place in a solid. Answer: True 24. The melting point is reached when sufficient energy has been added to the molecules in a substance to overcome the intermolecular forces holding them stationary. Answer: True 25. Heat is released when a liquid freezes into a solid. Answer: True 26. A glass of ice water containing nine ice cubes will be colder than a similar-size glass of ice water containing only three ice cubes. Answer: False 27. Sublimation is the process of a liquid being converted directly to a gas. Answer: False 28. The heat of fusion for water is significantly more than the heat of vaporization for water because fusion requires complete separation of one molecule from another. Answer: False 29. Dispersion forces result from the temporary distortion of the electron cloud in an atom or molecule which increases in magnitude with increasing size. Answer: True 30. Dipole-dipole forces are weaker than dispersion forces. Answer: False 31. H2 boils at a higher temperature than He because H2 undergoes hydrogen bonding. Answer: False 32. Hydrogen bonding occurs whenever hydrogen is present. Answer: False 33. For hydrogen bonding to occur, a molecule must have a hydrogen atom bonded directly to a fluorine, oxygen, or nitrogen atom. Answer: True 34. Ice is an example of a molecular solid. Answer: True 35. Atomic solids, such as graphite, have a weak dispersion force holding them together. Answer: False 36. Attraction between the Na+ cation and Cl- anion holds the solid lattice of sodium chloride together. Answer: True 37. Water has unusual physical properties which enable life to exist on earth. Answer: True 38. Ice can float in a glass of liquid water because the solid form of water is more dense than the liquid form. Answer: False 39. Compounds that are similar to water in molecular mass all exist as solids. Answer: False Multiple Choice Questions 40. Intermolecular forces are responsible for: A) the taste sensations. B) the shape of protein molecules. C) the function of DNA. D) the existence of liquids and solids. E) all of the above Answer: E 41. Which state of matter has a high density and an indefinite shape? A) solids B) liquids C) gases D) both solids and liquids E) none of the above Answer: B 42. Which state of matter has a high density and a definite volume? A) solids B) liquids C) gases D) both solids and liquids E) none of the above Answer: D 43. Which state of matter has a low density and an indefinite volume? A) solids B) liquids C) gases D) both solids and liquids E) none of the above Answer: C 44. Which state of matter has a low density and is easily compressed? A) solids B) liquids C) gases D) both solids and liquids E) none of the above Answer: C 45. Which statement about surface tension is FALSE? A) Liquids tend to minimize their surface area. B) Molecules on the surface of the liquid have fewer molecules to interact with. C) Increased intermolecular forces increase surface tension. D) Items with densities lower than water will sink due to surface tension. E) All of the above statements are true. Answer: D 46. The tendency of a liquid to minimize its surface area is called: A) capillary action. B) viscosity. C) surface tension. D) vaporization. E) none of the above Answer: C 47. The measure of the resistance to the flow of a liquid is called: A) vapor pressure. B) sublimation. C) viscosity. D) condensation. E) none of the above Answer: C 48. The change of a substance from a liquid to a gaseous form is called: A) dynamic equilibrium. B) heat of fusion. C) condensation. D) vaporization. E) volatile. Answer: D 49. A situation where two opposite processes are occurring at equal rates, and no net change is taking place, is called: A) vaporization. B) condensation. C) evaporation. D) dynamic equilibrium. E) none of the above Answer: D 50. Increasing the intermolecular forces of a liquid will do which of the following? A) increase the viscosity B) decrease the evaporation rate C) increase the surface tension D) decrease the vapor pressure E) all of the above Answer: E 51. You can increase the vapor pressure of a liquid by: A) increasing temperature. B) increasing the viscosity. C) establishing dynamic equilibrium. D) using a nonvolatile compound. E) all of the above Answer: A 52. Which statement about boiling point is FALSE? A) The boiling point is higher for compounds with strong intermolecular forces. B) The boiling point is higher for compounds with a high viscosity. C) The boiling point of a compound is an absolute constant. D) The boiling point of a compound is higher for nonvolatile compounds. E) All of the above statements are true. Answer: C 53. Evaporation is: A) increased by increasing temperature. B) an endothermic process. C) the opposite process as condensation. D) a cooling process for humans when they sweat. E) all of the above Answer: E 54. Which of the following statements is FALSE? A) Evaporation is an endothermic process. B) A puddle of water cools down as it evaporates. C) As a liquid is converted into a gas, the liquid absorbs heat. D) All of the above are true. E) None of the above are true. Answer: D 55. The opposite process of freezing is: A) evaporation. B) sublimation. C) boiling. D) condensation. E) none of the above Answer: E 56. The rate of vaporization of a liquid can be increased by 1. increasing the surface area 2. increasing the temperature 3. increasing the strength of the intermolecular forces A) 1 only B) 2 only C) 3 only D) 1 and 2 only E) 2 and 3 only Answer: D 57. Liquids that have high vapor pressure and low boiling points are called A) abnormal liquids. B) volatile liquids. C) non-volatile liquids. D) viscous liquids. E) none of the above Answer: B 58. The amount of heat required to melt one mole of a solid is called the: A) heat of vaporization. B) heat of fusion. C) heating curve. D) cooling curve. E) none of the above Answer: B 59. What is the heat of vaporization(kJ/mol) if it takes 3,452 J of heat to completely vaporize 2.68 moles of the liquid at its boiling point? A) 1288 B) 1.29 C) 0.776 D) 12.2 E) none of the above Answer: B 60. How many joules of heat are needed to completely vaporize 24.40 grams of water at its boiling point? Given ΔHvap = 40.6 kJ/mol A) 54.97 B) 5.50 × 104 C) 29.98 D) 3.00 × 104 E) none of the above Answer: B 61. How many kilojoules of heat are needed to completely vaporize 42.8 g of C4H10O at its boiling point? Given ΔHvap = 26.5kJ/mol A) 74.12 B) 9.49 C) 15.3 D) 16.3 E) none of the above Answer: C 62. Compare a small pot of water that is boiling vigorously to a large pot of water that is boiling gently. Which statement is TRUE? A) The small pot is boiling at higher temperature than the large pot. B) The large pot is boiling at a higher temperature than the small pot. C) Both pots are boiling at the same temperature. D) The vapor pressure of the liquid is greater than the pressure above the pot in each case. E) none of the above Answer: C 63. When sufficient quantity of heat has been added to reach the boiling point of a solution, what happens to any additional heat added? A) Additional heat is used to evaporate the liquid as the process is endothermic and requires continued input of energy. B) Additional heat raises the temperature of the liquid which in turn increases the rate at which boiling occurs. C) Additional heat lowers the intermolecular forces of the liquid which in turn increases the volatility of the liquid. D) Additional heat alters the viscosity and the surface tension of the liquid which raises the vapor pressure and increases the boiling point which is why you must continually heat the solution. E) None of the above are correct statements. Answer: A 64. What happens as you start to add heat to a solid substance? A) Thermal energy causes the components of the solid to vibrate faster. B) When the melting point is reached, the thermal energy is sufficient to overcome intermolecular forces holding the components at their stationary points. C) Increasing the rate of heating of a substance at its melting point only causes more rapid melting. D) Heating of the now formed liquid results in increasing the liquid temperature. E) all of the above Answer: E 65. If we supply additional heat to a solid in equilibrium with its liquid at the melting point, the thermal energy added is used to: A) overcome the intermolecular forces that hold the solid together. B) expand the solid. C) change the liquid back to solid. D) change solid to liquid. E) raise the temperature of the solid above its melting point. Answer: D 66. When you make ice cubes: A) it is an endothermic process. B) it is an exothermic process. C) the heat of vaporization must be removed. D) the process is referred to scientifically as sublimation. E) none of the above Answer: B 67. Which statement is TRUE in describing what occurs when a solid melts to a liquid? A) The process is endothermic and the heat of fusion is positive. B) The process is endothermic and the heat of fusion is negative. C) The process is exothermic and the heat of fusion is positive. D) The process is exothermic and the heat of fusion is negative. E) not enough information Answer: A 68. How much energy does it take to melt a 16.87 g ice cube? ΔHfus = 6.02 kJ/mol A) 102 kJ B) 108 kJ C) 936 J D) 5.64 kJ E) none of the above Answer: D 69. How many grams of C4H10O can be melted by 1.00 × 103 J? Given ΔHfus = 7.27 kJ/mol A) 14.5 B) 3.64 C) 20.4 D) 74.1 E) none of the above Answer: C 70. In northern climates, it is common to have a layer of frost form on cars that have been out overnight in the winter. During the day the frost layer disappears despite its temperature remaining below freezing. How? A) The frost melts due to the sun heating the surface of the car above the melting point. B) The frost evaporates due to the sun heating the solid. C) The frost cycles as does the saturation level of moisture in the winter air does from night to day. D) The frost sublimes directly from solid ice to water vapor. E) none of the above Answer: D 71. A mothball can change directly from its solid phase to its gaseous phase. This process is known as: A) deposition. B) melting. C) condensation. D) sublimation. E) none of the above Answer: D 72. Which intermolecular force is present in all molecules and atoms? A) dispersion forces B) dipole-dipole forces C) hydrogen bonding D) X-forces E) none of the above Answer: A 73. Which intermolecular force is due to the formation of an instantaneous dipole? A) dispersion forces B) dipole-dipole forces C) hydrogen bonding D) X-forces E) none of the above Answer: A 74. Which intermolecular force increases with increasing molar mass? A) dispersion forces B) dipole-dipole forces C) hydrogen bonding D) X-forces E) none of the above Answer: A 75. Which noble gas has the highest boiling point? A) He B) Ne C) Ar D) Kr E) Xe Answer: E 76. Assuming that the molecules carbon monoxide (CO) and nitrogen (N2) have similar electron clouds, which statement below is TRUE? A) CO has the higher boiling point because it experiences dipole-dipole forces. B) N2 has the higher boiling point because it experiences dipole-dipole forces. C) The N2 has the higher boiling point because it has greater dispersion forces. D) Both CO and N2 must have the same boiling point. E) none of the above Answer: A 77. Which intermolecular force is common to all polar molecules but NOT nonpolar molecules? A) dispersion forces B) dipole-dipole forces C) hydrogen bonding D) X-forces E) none of the above Answer: B 78. Substance A is a molecular compound that dissolves in gasoline but not in water. The molecules of A are very likely: A) metallic. B) nonmetallic. C) polar. D) nonpolar. E) none of the above Answer: D 79. Which substance is most likely to be miscible with water? A) CF4 B) Br2 C) CS2 D) CHCl3 E) none of the above Answer: D 80. Which statement below is FALSE? A) A hydrogen bond is the strongest of the intermolecular forces. B) A hydrogen atom must be bonded directly to fluorine, oxygen, or nitrogen to exhibit hydrogen bonding. C) The large electronegativity difference between hydrogen and an F, O, or N atom is essential for the formation of a hydrogen bond. D) A hydrogen bond is only 2-5% the strength of a typical covalent bond. E) none of the above Answer: E 81. Which molecule below has hydrogen bonding? A) CH4 B) HCl C) H2 D) CH3CH2OH E) all of the above Answer: D 82. Which molecule below has hydrogen bonding? A) NH3 B) CH3OH C) H2O D) HF E) all of the above Answer: E 83. Which compound will have the highest boiling point? A) CH4 B) CH3 CH3 C) CH3C(O)CH3 D) CH3CH2OH E) not enough information Answer: D 84. Which substance would be expected to have the highest boiling point? A) N2 B) O2 C) CO2 D) CO E) not enough information Answer: D 85. Which compound in liquid form will have the highest vapor pressure? A) CH4 B) CH3CH3 C) CH3C(O)CH3 D) CH3CH2OH E) not enough information Answer: A 86. Which intermolecular force is the strongest? A) dispersion forces B) dipole-dipole forces C) hydrogen bonding D) X-forces E) none of the above Answer: C 87. Which intermolecular forces are found in CCl4? A) dispersion forces B) dipole-dipole forces C) hydrogen bonding D) X-forces E) none of the above Answer: A 88. Which intermolecular forces are found in CO2? A) dispersion forces B) dipole-dipole forces C) hydrogen bonding D) dispersion forces and dipole-dipole forces E) none of the above Answer: A 89. Rank the compounds NH3, CH4, and PH3 in order of increasing boiling point. A) NH3 < CH4 < PH3 B) CH4 < NH3 < PH3 C) NH3 < PH3 < CH4 D) CH4 < PH3 < NH3 E) PH3 < NH3 < CH4 Answer: D 90. Which intermolecular force found in CCl2H2 is the strongest? A) dispersion forces B) dipole-dipole forces C) hydrogen bonding D) X-forces E) none of the above Answer: B 91. What types of forces exist between I2 molecules? A) dispersion forces B) dipole-dipole forces C) hydrogen bonding D) ion-dipole forces E) none of the above Answer: A 92. Dry ice (solid CO2) is which type of solid? A) molecular solid B) ionic solid C) covalent atomic solid D) nonbonding atomic solid E) metallic atomic solid Answer: A 93. NaCl is which type of solid? A) molecular solid B) ionic solid C) covalent atomic solid D) nonbonding atomic solid E) metallic atomic solid Answer: B 94. Silicon is which type of solid? A) molecular solid B) ionic solid C) covalent atomic solid D) nonbonding atomic solid E) metallic atomic solid Answer: C 95. Copper is which type of solid? A) molecular solid B) ionic solid C) covalent atomic solid D) nonbonding atomic solid E) metallic atomic solid Answer: E 96. Which atomic solid has the highest melting point? A) Cu B) Si C) Xe D) Fe E) not enough information Answer: B 97. What are the principal forces holding ice together? A) dispersion forces only B) electrostatic attraction C) intermolecular forces D) sea of electrons E) none of the above Answer: C 98. Why is water considered an unusual molecule? A) No molecule of similar size is a liquid at room temperature. B) No molecule of similar size has as high a boiling point. C) Water can dissolve many polar and ionic compounds. D) Water expands upon freezing. E) all of the above Answer: E 99. The reason for many of the unique properties of water is: A) dispersion forces. B) the ability to form hydrogen bonds. C) high surface tension and low volatility. D) moderate viscosity and expanding upon freezing. E) all of the above Answer: B 100. Which sequence correctly shows the increasing density of the three phases of water? A) solid < liquid < gas B) gas < liquid < solid C) gas < solid < liquid D) liquid < gas < solid E) none of the above Answer: C Algorithmic Questions 101. How many kJ of heat are needed to completely vaporize 3.30 moles of H2O? The heat of vaporization for water at the boiling point is 40.6 kJ/mole. A) 12.3 B) 134 C) 67.0 D) 2.26 E) none of the above Answer: B 102. How many kJ of heat are needed to completely vaporize 23.4 g of H2O? The heat of vaporization for water at the boiling point is 40.6 kJ/mole. A) 31.2 B) 52.8 C) 23.4 D) 2.26 E) none of the above Answer: B 103. A 250 gram sample of water at the boiling point had 45.0 kJ of heat added. How many grams of water were vaporized? Heat of vaporization for water is 40.6 kJ/mole. A) 1.11 B) 20.0 C) 0.902 D) 16.2 E) none of the above Answer: B 104. How many kJ of heat are needed to completely melt 1.70 moles of H2O, given that the water is at its melting point? The heat of fusion for water is 6.02 kJ/mole. A) 30.6 B) 10.2 C) 3.54 D) 63.7 E) none of the above Answer: B 105. How many kJ of heat are needed to completely melt 17.3 g of H2O, given that the water is at its melting point? The heat of fusion for water is 6.02 kJ/mole. A) 0.961 B) 5.79 C) 1.04 D) 6.26 E) none of the above Answer: B Test Bank for Introductory Chemistry Nivaldo J. Tro 9780321741028, 9780321687937, 9781256112938, 9781256161066, 9780134302386, 9780321910073
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