General Chemistry 11th Edition by Darrell Ebbing - Test Bank Instant Download - Complete Test Bank With Answers Sample Questions Are Posted Below 1. Which of the following concerning a barometer or manometer is/are true? 1. Pressure is directly proportional to the height of the liquid used in the device. …
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General Chemistry 11th Edition by Darrell Ebbing – Test Bank
Instant Download – Complete Test Bank With Answers
Sample Questions Are Posted Below
1. Which of the following concerning a barometer or manometer is/are true?
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2. It is possible to make a barometer using a liquid other than mercury. What would be the height (in meters) of a column of dichloromethane at a pressure of 0.830 atm, given that 0.830 atm is equal to a 0.63522 m column of mercury and the densities of mercury and dichloromethane are 13.5 g/cm3 and 1.33 g/cm3, respectively.
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3. A particular gas exerts a pressure of 689 mmHg. What is this pressure in units of bar?
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4. A particular gas exerts a pressure of 731 mmHg. What is this pressure in units of atmospheres?
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5. A particular gas exerts a pressure of 2.52 bar. What is this pressure in units of pascals?
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6. A particular gas exerts a pressure of 4.33 bar. What is this pressure in units of atmospheres?
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7. A particular gas exerts a pressure of 2.42 atm. What is this pressure in units of mmHg?
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8. A particular gas exerts a pressure of 4.02 atm. What is this pressure in units of bar?
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9. A particular gas exerts a pressure of 5.56 × 104 Pa. What is this pressure in units of bar?
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10. A particular gas exerts a pressure of 4.09 × 104 Pa. What is this pressure in units of atmospheres?
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11. The pressure of a certain gas is measured to be 264.6 mmHg. What is this pressure expressed in units of pascals?
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12. The pressure of a certain gas is measured to be 4.304 × 103 Pa. What is this pressure expressed in units of mmHg?
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13. A flexible vessel contains 43 L of gas where the pressure is 1.3 atm. What will the volume be when the pressure is 0.61 atm, the temperature remaining constant?
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14. A flexible vessel contains 78.00 L of gas at a pressure of 1.50 atm. Under conditions of constant temperature and moles of gas, what is the pressure of the gas when the volume of the vessel is tripled?
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15. A flexible vessel is filled to a certain pressure with 28.00 L of gas. Under conditions of constant temperature and moles of gas, how does the pressure of the gas change when the volume of the gas is tripled?
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16. A flexible vessel contains 37 L of gas where the pressure is 1.0 atm. What will the volume be when the pressure is 0.70 atm, the temperature remaining constant?
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17. A 2.00-L glass soda bottle filled only with air is tightly capped at 25°C and 728.0 mmHg. If the bottle is placed in water at 65°C, what is the pressure in the bottle?
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18. A sample of methane, CH4, occupies a volume of 318.0 mL at 25°C and exerts a pressure of 1010.0 mmHg. If the volume of the gas is allowed to expand to 770.0 mL at 298 K, what will be the pressure of the gas?
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19. When the valve between the 2.00-L bulb, in which the gas pressure is 2.50 atm, and the 3.00-L bulb, in which the gas pressure is 1.50 atm, is opened, what will be the final pressure in the two bulbs? Assume the temperature remains constant.
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20. Absolute zero is the point at which
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21. The following volume-temperature plots were made at different values of constant pressure while the number of moles of gas in each experiment remained the same. Which plot represents measurements at the highest pressure?
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22. Which of the following is a correct statement of Charles’s law, ?
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23. The volume of a sample of gas measured at 35.0°C and 1.00 atm pressure is 2.00 L. What must the final temperature be in order for the gas to have a final volume of 3.00 L at 1.00 atm pressure?
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24. A flexible container is charged with 79.00 L of gas at 352 Κ. Under conditions of constant pressure and moles of gas, what is the volume of the gas when the temperature is decreased by a factor of three?
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25. A flexible container is charged with a certain volume of gas at 315.0 Κ. Under conditions of constant pressure and moles of gas, how does the temperature of the gas change when the volume is tripled?
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26. A gas occupies a volume of 2.75 L at 350 mmHg and 200°C. Which mathematical expression gives the correct volume at 600 mmHg and 250°C?
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27. A gas occupying a volume of 1.50 L exerts a pressure of 700 mmHg at 200°C. Which mathematical expression gives the correct pressure at 3.50 L and 350°C?
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28. A rigid container is charged with a gas to a pressure of 740 mmHg at 40.0°C and tightly sealed. If the temperature of the gas increases by 80.0°C what is the new pressure?
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29. The pressure of 6.2 L of nitrogen gas in a flexible container is decreased to one-half its original pressure, and its absolute temperature is increased to double the original temperature. The volume is now
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30. Which of the following concerning the ideal gas law is/are true?
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31. A given mass of gas occupies a volume of 4.00 L at 60°C and 550 mmHg. Which of the following mathematical expressions will yield its temperature at 2.50 L and 900 mmHg?
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32. A fixed amount of gas in a rigid container is heated from 300 to 600 K. Which of the following responses best describes what will happen to the pressure of the gas?
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33. A 23.6 -L sample of nitrogen at 4.45 atm and 23°C is simultaneously expanded to 50.8 L and heated to 37°C. What is the new pressure of the gas?
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34. A fixed amount of gas in a rigid container is heated from 100°C to 600°C. Which of the following responses best describes what will happen to the pressure of the gas?
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35. Equal volumes of propane, C3H8, and carbon monoxide, CO, at the same temperature and pressure have the same
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36. A 1.00-L bulb contains a sample of O2 at 25°C and 1.00 atm pressure. A second 1.00-L bulb contains a sample of CH4 at 25°C and 1.00 atm pressure. What is the ratio of the number of molecules of methane to the number of molecules of oxygen in each of the containers?
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37. Which of the following statements, concerning equal volumes of the gases dinitrogen monoxide, N2O, and propane, C3H8, at the same temperature and pressure, is not correct?
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38. What volume of sulfur trioxide gas, SO3, has the same number of atoms as 4 L of helium gas at the same temperature and pressure?
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39. What volume of gaseous oxygen, O2, has the same moles of gas as 3 L of argon gas at the same temperature and pressure?
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40. A gas occupies a volume of 2.00 L at 780 mmHg and 70.0°C. Which of the following mathematical expressions will yield its volume at STP?
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41. Which conditions of P, T, and n, respectively, are most ideal?
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42. The behavior of PH3(g) is most likely to approach ideal behavior at
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43. For an ideal gas, which of the following statements is true?
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44. The volume of 1 mol of nitrogen
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45. Which of the following graphs does not correctly describe the ideal gas law?
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46. What is the pressure of a 34.8-L gas sample containing 7.45 mol of gas at 19.9°C? (R = 0.0821 L • atm/(K • mol), 1 atm = 760 torr)
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47. How many moles of gas are in a gas sample occupying 0.816 L at 127 mmHg and 22°C?
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48. How many moles of gas are in a gas sample occupying 1.40 L at 553 mmHg and 294 K?
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49. Which of the following statements is incorrect regarding a 128-g sample of gaseous sulfur dioxide at 0°C and 760 mmHg pressure?
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50. The following gases are stored in identical flexible containers at 25°C and 1.00 atm pressure. Order the gases from highest to lowest density.
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51. Which of the following samples has the fewest moles of gas?
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52. A 3.74-L cylinder contains 4.17 g of methane, CH4, at a pressure of 3020 mmHg. What is the temperature of the gas?
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53. The number of molecules in 1.0 L of air at 0°C and 1.0 atm pressure is
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54. A mixture consisting of 0.140 mol N2, 0.037 mol O2, 0.104 mol CH4, and an unknown amount of CO2 occupies a volume of 8.48 L at 27°C and 1.06 atm pressure. How many moles of CO2 are there in this sample?
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55. Which of the following gases has the greatest density at 2.5 atm and 25°C?
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56. The density of ethane, C2H6 (30.1 g/mol), at 25°C and 1.13 atm pressure is
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57. The density of O2 gas at 16°C and 1.27 atm is
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58. A 1.00-L sample of a gas at STP has a mass of 0.759 g. The molar mass of the gas is
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59. The density of a gas is 0.803 g/L at STP. What is its molar mass?
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60. A 1.50-L sample of a gas at STP has a mass of 4.75 g. What is one possible formula of the gas?
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61. At 530.4 mmHg and 55.3oC, a 3.14-L sample of a hydrocarbon gas has a mass of 2.28 g. What is the formula of the gas?
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62. It is found that at 26°C and 1.00 atm pressure, 2.50 L of gas has a mass of 2.85 g. Its molar mass is
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63. At 25°C and 449 mmHg, an unknown pure gas has a density of 0.676 g/L. Which of the following gases could be the unknown gas?
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64. An unknown gaseous hydrocarbon consists of 85.63% carbon by mass. A 0.959-g sample of the gas occupies a volume of 0.51 L at STP. What is the identity of the gas?
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65. An excess of sodium hydroxide is treated with 2.9 L of dry hydrogen chloride gas measured at STP. What is the mass of sodium chloride is formed?
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| 66. The balanced chemical equation for the conversion of nitrogen to ammonia is:
2N2(g) + 3H2(g) → 2NH3(g) Which of the following statements concerning this chemical equation is/are correct?
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| 67. A 22.4 L high pressure reaction vessel is charged with 0.5020 mol of iron powder and 1.39 atm of oxygen gas at standard temperature. On heating, the iron and oxygen react according to the balanced reaction below.
4Fe(s) + 3O2(g) → 2Fe2O3(s) After the reaction vessel is cooled, and assuming the reaction goes to completion, what pressure of oxygen remains?
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| 68. A high temperature reaction vessel is charged with 0.5080 mol of iron powder and 42.1 L of oxygen gas at standard temperature at pressure. On heating, the iron and oxygen react according to the balanced reaction below.
4Fe(s) + 3O2(g) → 2Fe2O3(s) After the reaction vessel is cooled, and assuming the reaction goes to completion, what volume of oxygen remains?
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| 69. What is the total volume of gases produced at 1092 K and 1.00 atm pressure when 320 g of ammonium nitrite undergoes the following decomposition reaction?
NH4NO2(s) → N2(g) + 2H2O(g)
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70. In which of the following reactions will the pressure increase upon completion of the reaction at constant temperature?
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| 71. What volume of ammonia gas, measured at 547.9 mmHg and 27.6oC, is required to produce 8.98 g of ammonium sulfate according to the following balanced chemical equation?
2NH3(g) + H2SO4(aq) → (NH4)2SO4(s)
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| 72. If 636.0 mL of nitrogen gas, measured at 488.9 mmHg and 22.3oC, reacts with excess iodine according to the following reaction, what mass of nitrogen triiodide is produced?
N2(g) + 3I2(s) → 2NI3(s)
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| 73. The following equation represents the partial combustion of methane, CH4.
2CH4(g) + 3O2(g) → 2CO(g) + 4H2O(g) At constant temperature and pressure, what is the maximum volume of carbon monoxide that can be obtained from 6.62 × 102 L of methane and 3.31 × 102 L of oxygen?
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| 74. Calcium nitrate will react with ammonium chloride at slightly elevated temperatures, as represented in the equation below.
Ca(NO3)2(s) + 2NH4Cl(s) → 2N2O(g) + CaCl2(s) + 4H2O(g) What is the maximum volume of N2O at STP that could be produced using a 5.20-mol sample of each reactant?
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| 75. The following equation represents the oxidation of ammonia, NH3.
4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g) At the same temperature and pressure, what is the maximum volume of nitrogen monoxide that can be obtained from 7.55 × 102 L of ammonia and 7.55 × 102 L of oxygen?
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76. A vessel with a volume of 12.4 L contains 2.80 g of nitrogen gas, 0.403 g of hydrogen gas, and 79.9 g of argon gas. At 25°C, what is the pressure in the vessel?
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77. What is the volume occupied by a mixture of 0.774 mol of N2 and 0.774 mol of O2 gases at 1.04 atm and 25.6°C?
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78. In a mixture of argon and hydrogen, occupying a volume of 1.86 L at 626.0 mmHg and 46.8oC, it is found that the total mass of the sample is 1.8 g. What is the partial pressure of argon?
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79. The partial pressures of CH4, N2, and O2 in a sample of gas were found to be 183 mmHg, 443 mmHg, and 693 mmHg, respectively. What is the mole fraction of nitrogen?
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80. A 15.6-g mixture of nitrogen and carbon dioxide is found to occupy a volume of 9.9 L when measured at 940.2 mmHg and 54.9°C. What is the mole fraction of carbon dioxide in this mixture?
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81. A 28.3-g mixture of oxygen and argon is found to occupy a volume of 17.2 L when measured at 882.7 mmHg and 39.3oC. What is the partial pressure of oxygen in this mixture?
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82. In a mixture of helium and chlorine, occupying a volume of 12.8 L at 605.6 mmHg and 21.6oC, it is found that the partial pressure of chlorine is 143 mmHg. What is the total mass of the sample?
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83. What is the partial pressure of carbon dioxide in a container that contains 3.63 mol of oxygen, 1.49 mol of nitrogen, and 4.49 mol of carbon dioxide when the total pressure is 871 mmHg?
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84. A sample of oxygen is collected over water at a total pressure of 678.4 mmHg at 25°C. The vapor pressure of water at 25°C is 23.8 mmHg. The partial pressure of the O2 is
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85. A sample of hydrogen was collected by water displacement at 23.0°C and an atmospheric pressure of 735 mmHg. Its volume is 568 mL. After water vapor is removed, what volume would the hydrogen occupy at the same conditions of pressure and temperature? (The vapor pressure of water at 23.0°C is 21 mmHg.)
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86. A small amount wet of hydrogen gas (H2) can be prepared by the reaction of zinc with excess hydrochloric acid and trapping the gas produced in an inverted tube initially filled with water. If the total pressure of the gas in the collection tube is 757.9 mmHg at 25°C, what is the partial pressure of the hydrogen? The vapor pressure of water is 23.8 mmHg.
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87. Which statement is inconsistent with the kinetic theory of an ideal gas?
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88. Which of the following is included as a postulate in the kinetic molecular theory of an ideal gas?
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89. Which of the following is not a postulates of the kinetic molecular theory of gases?
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90. Which of the following statements is least likely to be true of a sample of nitrogen gas at STP?
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91. If a sample of nitrogen gas in a sealed container of fixed volume is heated from 25°C to 125°C, the value of which of the following quantities will remain constant?
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92. A sealed 22.4 L flask contains pure O2 at STP. A second sealed 22.4 L flask contains CH4 at STP. Which of the following statements concerning the molecules in the flasks is/are true?
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93. Which of the following statements concerning a sample of oxygen gas at 1.00 atm pressure is incorrect?
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94. According to the postulates of the kinetic theory of gases, the root-mean-square (rms) speed of the molecules of a given gas is proportional to the
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95. At STP, as the molar mass of the molecules that make up a pure gas increases, the
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96. What is the ratio of the average speed of SO2 molecules to that of oxygen molecules at 298 K?
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97. Molecular speed distributions for a gas at two different temperatures are shown below. Which of the following graphs correctly describes the distributions at the two temperatures, where T2 > T1? NOTE: The small vertical lines indicate average speed.
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98. Calculate the root-mean-square velocity for the O2 molecules in a sample of O2 gas at 28.3°C. (R = 8.3145 J/K⋅mol)
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99. What is the ratio of the average speed of He molecules to that of CH4 molecules at 298 K?
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100. Which of the following relates the rate of effusion of a gas to the square root of its molar mass?
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101. What is the ratio of the average rate of effusion of CH4(g) to that of NOF(g) at 400 K?
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102. Which of the following gases will have the slowest rate of effusion at constant temperature?
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103. The molar mass of an unknown gas was measured by an effusion experiment. It was found that it took 60 s for the gas to effuse, whereas nitrogen gas required 48 s. The molar mass of the gas is
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104. If 250 mL of methane, CH4, effuses through a small hole in 20 s, the time required for the same volume of helium to pass through the hole under the same conditions will be
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105. Under what set of conditions does HCl(g) deviate the most from ideal behavior?
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106. Real gases deviate from ideal behavior for two reasons: (1) real gas molecules have intermolecular forces, and (2) real gas molecules have
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107. At 320 K and 16 atm pressure, the molar volume of ammonia, NH3, is about 10% less than the molar volume of an ideal gas. The best explanation for actual volume being this much smaller than ideal volume is that
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108. Which of the following statements concerning gas molecules is incorrect?
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109. Using the van der Waals equation, determine the pressure of 500.0 g of SO2(g) in a 6.30-L vessel at 633 K. For SO2(g), a = 6.865 L2 • atm/mol2 and b = 0.05679 L/mol. (R = 0.0821 L • atm/(K • mol))
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| 110. In the van der Waals equation,
the effect of intermolecular forces is accounted for by
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111. From a consideration of the van der Waals constants for water and sulfur dioxide,
we can conclude that
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112. How is kinetic energy (Ek) related to the mass of a body (m) and its speed (v)?
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| 113. Which of the following is/are true of Avogadro’s law?
1. Avogadro’s law relates the volume of a gas to the moles of the gas at constant temperature and pressure. 2. Avogadro’s law states that the pressure of a gas decreases if the volume is increased at constant temperature and molar concentration. 3. Avogadro’s law states that the pressure of a gas increases with the increase in its temperature at constant volume and molar concentration.
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114. What does R denote in the ideal gas equation, PV = nRT?
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| 115. Identify the true statement(s) about the van der Waals equation.
1. The volume, V, in the ideal gas equation is replaced by (V – nb) in the van der Waals equation. 2. The volume, V, in the ideal gas equation is replaced by (V + nb) in the van der Waals equation. 3. The pressure, P, in the ideal gas equation is replaced by (P + a2nV) in the van der Waals equation.
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116. The _____ is an equation similar to the ideal gas law, but includes two constants, a and b, to account for deviations from ideal behavior.
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Original price was: $30.00.$20.00Current price is: $20.00.
Original price was: $30.00.$20.00Current price is: $20.00.
Original price was: $30.00.$20.00Current price is: $20.00.
Original price was: $30.00.$20.00Current price is: $20.00.
Original price was: $30.00.$20.00Current price is: $20.00.
Original price was: $30.00.$20.00Current price is: $20.00.
