Chemical Principles 8th Edition Zumdahl - Test Bank Instant Download - Complete Test Bank With Answers Sample Questions Are Posted Below 1. A glass column is filled with mercury and inverted in a pool of mercury. The mercury column stabilizes at a height of 735 mm above the pool of mercury. What …
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Chemical Principles 8th Edition Zumdahl – Test Bank
Instant Download – Complete Test Bank With Answers
Sample Questions Are Posted Below
1. A glass column is filled with mercury and inverted in a pool of mercury. The mercury column stabilizes at a height of 735 mm above the pool of mercury. What is the pressure of the atmosphere?
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2. The volume of a balloon is 3.02 L at 22.7°C. The balloon is heated to 43.6°C. Calculate the new volume of the balloon.
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| 3. Consider three 1-L flasks at the same temperature and pressure. Flask A contains CO gas, flask B contains N2 gas, and flask C contains O2 gas.
Which contains the lowest density?
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4. A cylinder of oxygen gas contains 26.4 g of O2. Another cylinder, twice the volume of the cylinder containing oxygen (and at the same conditions of pressure and temperature), contains CO2 gas. Assuming ideal behavior, what is the mass of the carbon dioxide?
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| 5. Samples of the gases H2(g) and SO2(g) have equal masses and are at the same temperature and pressure. Calculate the following:
The ratio of volumes .
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6. A balloon contains 10.0 g of neon gas. With the temperature kept constant, 10.0 g of argon gas is added. What happens?
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7. The volume of a helium balloon is 1.85 L at 24.0°C and 1.00 atm at sea level. The balloon is released and floats upward. At a certain altitude, the balloon has a volume of 2.14 L and the temperature is 15.2°C. What is the atmospheric pressure at this altitude?
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| 8. Three 1.00-L flasks at 25°C and 725 torr contain the gases CH4 (flask A), CO2 (flask B), and C2H6 (flask C).
In which flask is there 0.039 mol of gas?
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9. Body temperature is about 308 K. On a cold day, what volume of air at 273 K must a person with a lung capacity of 2.00 L breathe in to fill the lungs?
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| 10. Consider two samples of helium in separate containers of the same volume. Sample 1 has an absolute temperature four times that of Sample 2. Both samples are at the same pressure.
Calculate the ratio n1/n2.
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11. A cylinder is fitted with a movable piston. The pressure inside the cylinder is Pi and the volume is Vi. What is the new pressure in the system when the piston decreases the volume of the cylinder by half?
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12. A 8.80-g piece of solid CO2 (dry ice) is allowed to sublime in a balloon. The final volume of the balloon is 1.30 L at 290. K. What is the pressure of the gas?
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13. Given a cylinder of fixed volume filled with 1 mol of argon gas, which of the following is correct? (Assume all gases obey the ideal gas law.)
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14. Which of the following relationships is not true?
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15. A sample of oxygen gas has a volume of 4.50 L at 27°C and 800.0 torr. How many oxygen molecules does it contain?
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16. Mercury vapor contains Hg atoms. What is the volume of 200. g of mercury vapor at a temperature of 822 K and 0.500 atm?
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17. A sample of nitrogen gas has a volume of 180.0 mL at STP. What volume does the gas occupy if the absolute temperature and pressure are each doubled?
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18. Consider a sample of neon gas in a container fitted with a movable piston (assume the piston is massless and frictionless). The temperature of the gas is increased from 20.0°C to 40.0°C. The density of neon
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19. The valve between a 3.00-L tank containing O2(g) at 7.36 atm and a 2.10-L tank containing Ne(g) at 5.08 atm is opened. Calculate the ratio of partial pressures (O2:Ne) in the container.
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20. Air is 79% N2 and 21% O2 by volume. Calculate the density of air at 1.0 atm, 25°C.
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21. Air is 79% N2 and 21% O2 by volume. Calculate the mass of oxygen in a 2.0-L bottle of air at 1.0 atm, 25°C.
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22. At STP the mass of 680.0 mL of a certain gas is 0.850 g. What is a possible identity of this gas?
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| Four identical 1.0-L flasks contain the gases He, Cl2, CH4, and NH3, each at 0°C and 1 atm pressure. |
23. Which gas sample has the greatest number of molecules?
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24. Which gas has the highest density?
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| A plastic bag is weighed and then filled successively with two gases, X and Y. The following data are gathered:
Temperature: 0.0°C |
25. The mass of 1.12 L of gas Y is found to be 6.23 g. The density of gas Y is
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26. The molar mass of gas Y is
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27. It is found that 250. mL of gas at STP has a mass of 1.00 g. What is the molar mass?
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28. Air has an average molar mass of 29.0 g/mol. The density of air at 1.00 atm and 30°C is
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29. Equimolar amounts of the gases N2 and H2 are mixed in a closed container fitted with a piston (allowing the volume of the container to change, thus keeping the pressure constant). Calculate the ratio of the final volume of the container to the initial volume of the container when the reaction N2 + 3H2 → 2NH3 goes to completion.
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30. The density of a certain diatomic gas is 1.696 g/L at STP. Identify the gas.
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| 31. Potassium chlorate decomposes upon heating as follows:
2KClO3(s) → 2KCl(s) + 3O2(g) A 2.72-g sample of KClO3 decomposes, and the oxygen at 23.4°C and 0.935 atm is collected. What volume of oxygen gas will be collected, assuming 100% yield?
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32. Calculate the density of nitrogen at STP.
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33. A volatile liquid produced 0.379 g of vapor in a 262.0-mL flask at 100.0°C and 0.960 atm. What is the molar mass of the liquid?
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34. What volume of carbon dioxide measured at STP will be formed by the reaction of 1.30 mol of oxygen with 9.00 × 10–1 mol of ethyl alcohol (CH3CH2OH)?
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35. If a 2.15-g sample of a gas occupies 750. mL at STP, what is the molar mass of the gas at 125°C?
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36. Into a 3.50-liter container at 25°C are placed 1.10 mol of O2 gas and 4.68 mol of solid C (graphite). If the carbon and oxygen react completely to form CO(g), what will be the final pressure in the container at 25°C?
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| 37. When a mixture is prepared from 15.0 L of ammonia and 15.0 L of chlorine measured at the same conditions, these compounds react according to the following equation:
2NH3(g) + 3Cl2(g) → N2(g) + 6HCl(g) When the reaction is completed, what are the volumes of the gases (NH3, Cl2, N2, and HCl, respectively)? Assume the final volumes are measured under identical conditions.
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| 38. A mixture of KCl and KClO3 weighing 1.80 g was heated; the dry O2 generated occupied 1.40 × 102 mL at STP. What percent of the original mixture was KClO3? KClO3 decomposes as follows:
2KClO3(s) → 2KCl(s) + 3O2(g)
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39. An excess of potassium hydroxide is treated with 1.6 L of dry hydrogen bromide gas measured at STP. What is the mass of potassium bromide formed?
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40. Magnesium metal reacts with hydrochloric acid to form aqueous magnesium chloride and hydrogen gas. An excess of magnesium is reacted with 20.0 mL of 3.00 M hydrochloric acid, and all of the hydrogen is collected in a balloon at 25°C and 1.00 atm. What is the expected volume of the balloon?
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41. When 0.72 g of a liquid is vaporized at 110°C and 0.967 atm, the gas occupies a volume of 0.559 L. The empirical formula of the gas is CH2. What is the molecular formula of the gas?
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| 42. A 3.82-g sample of lead(II) nitrate, Pb(NO3)2, molar mass = 331 g/mol, is heated in an evacuated cylinder with a volume of 1.70 L. The salt decomposes when heated, according to the equation
2Pb(NO3)2(s) → 2PbO(s) + 4NO2(g) + O2(g) Assuming complete decomposition, what is the pressure in the cylinder after decomposition and cooling to a temperature of 290. K? Assume the PbO(s) takes up negligible volume.
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43. The purity of a sample containing zinc and weighing 0.198 g is determined by measuring the amount of hydrogen formed when the sample reacts with an excess of hydrochloric acid. The determination shows the sample to be 84.0% zinc. What amount of hydrogen (measured at STP) was obtained?
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44. At 1000°C and 10. torr, the density of a certain element in the gaseous state is 2.9 × 10–3 g/L. The element is
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45. A 1.00-g sample of a gaseous compound of boron and hydrogen occupies 0.820 L at 1.00 atm and 3°C. What is the molecular formula for the compound?
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| 46. How many of the following gases at STP are less dense than air at STP?
NH3, He, Kr, and F2
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| 47. The oxidation of nitric oxide to nitrogen dioxide is
2NO(g) + O2(g) → 2NO2(g) If 100.0 mL of NO (at STP) reacts with 400.0 mL of O2 at STP, calculate the partial pressure of NO2 in the final reaction mixture.
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| 48. A balloon contains an anesthetic mixture of cyclopropane (C3H6) and oxygen (O2) at 160 torr and 550 torr, respectively. What is the ratio of the number of moles of cyclopropane to the number of moles of oxygen?
ncp/no2 = ?
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49. A 250.0-L cylinder contains 65.0% He(g) and 35.0% Kr(g) by mass at 25.0°C and 1.35 atm total pressure. What is the partial pressure of He in this container?
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50. A 0.234-g sample of a gas in a 275-mL container at 23.5°C exerts a pressure of 0.292 atm What is the molar mass of the gas?
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51. A 130.-mL sample of gas is collected over water at 22°C and 753 torr. What is the volume of the dry gas at STP? (The vapor pressure of water at 22°C is 20. torr.)
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52. A vessel with a volume of 10.1 L contains 3.28 g of nitrogen gas, 0.400 g of hydrogen gas, and 85.0 g of argon gas. At 26.0°C, what is the pressure in the vessel?
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53. A 275.0-mL sample of O2 is collected over water at 60.0°C. The total pressure is 755 torr. What is the volume of the O2 at the STP? (The vapor pressure of water at 60°C is 149 torr).
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54. Oxygen gas, generated by the reaction 2KClO3(s) → 2KCl(s) + 3O2(g), is collected over water at 27°C in a 3.72-L vessel at a total pressure of 730. torr. (The vapor pressure of H2O at 27°C is 26.0 torr.) How many moles of KClO3 were consumed in the reaction?
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55. A gaseous mixture containing 1.5 mol Ar and 3.5 mol CO2 has a total pressure of 7.0 atm. What is the partial pressure of CO2?
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56. A 226.4-L cylinder contains 65.5% He(g) and 34.5% Kr(g) by mass at 27.0°C and 1.40 atm total pressure. What is the mass of He in this container?
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| 57. Three 1.00-L flasks at 25°C and 725 torr contain the gases CH4 (flask A), CO2 (flask B), and C2H6 (flask C).
In which single flask do the molecules have the greatest mass, the greatest average velocity, and the highest kinetic energy?
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| 58. Consider three 1.0-L flasks at STP. Flask A contains N2 gas, flask B contains Kr gas, and flask C contains H2 gas.
In which flask do the gas particles have the lowest average kinetic energy?
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| Four identical 1.0-L flasks contain the gases He, Cl2, CH4, and NH3, each at 0°C and 1 atm pressure. |
59. For which gas do the molecules have the highest average velocity?
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60. For which gas are the collisions elastic?
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61. For which gas do the molecules have the smallest average kinetic energy?
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| 62. Consider three 1-L flasks at the same temperature and pressure. Flask A contains CO gas, flask B contains N2 gas, and flask C contains O2 gas.
In which flask do the molecules have the greatest momentum per impact?
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63. Under which of the following conditions does a gas behave most ideally?
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| 64. Calculate the following ratios for a gas at Kelvin temperatures T1 and T2 where T2 = 2T1.
Average kinetic energy at T1 : Average kinetic energy at T2
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65. The kinetic-molecular theory of gases does not assume that
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66. Which statement about kinetic energy (K.E.) is true?
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67. Consider separate samples of Ar(g) and Ne(g). For what ratio of absolute temperatures (Ne:Ar) are the average kinetic energies equal?
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68. Which of the following statements is true concerning ideal gases?
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| Samples of the gases H2(g) and SO2(g) have equal masses and are at the same temperature and pressure. Calculate the following: |
69. The ratio of the root-mean-square velocities .
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70. The ratio of the forces per wall impact .
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71. The ratio of average kinetic energies per molecule (H2:SO2)
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| Consider two 1.0-L containers, one containing He(g) at 2.50 atm and 24°C and the other containing Ar(g) at 5.00 atm and 48°C. |
72. Calculate the ratio of average velocities (He:Ar).
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73. Calculate the ratio of impacts with the wall per second (He:Ar).
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74. The root-mean-square velocity of N2 gas at 35°C is
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75. Calculate the temperature at which the average velocity of Ar(g) equals the average velocity of Ne(g) at 25°C.
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76. Calculate the ratio of the change in momentum per wall impact for Ar(g) to that for He(g) if the gases are at the same temperature and pressure.
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77. The root-mean-square velocity of a gas in a closed container of fixed volume is increased from 345 m/s to 690 m/s. Which one of the following statements might explain correctly how this change was accomplished?
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78. Calculate the temperature at which the average kinetic energy of O2 gas is twice that of He gas at 10.0°C.
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79. At 200 K, the molecules or atoms of an unknown gas, X, have an average velocity equal to that of Ar atoms at 400 K. What is X? (Assume ideal behavior.)
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| 80. Consider the following gas samples:
Which one of the following statements is false?
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| 81. Order the following according to increasing rate of effusion:
F2, Cl2, NO, NO2, CH4
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| 82. Calculate the following ratios for a gas at Kelvin temperatures T1 and T2 where T2 = 2T1.
Effusion rate at T1 : Effusion rate at T2
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83. The diffusion rate of H2 gas is 6.45 times as great as that of a certain noble gas (both gases are at the same temperature). What is the noble gas?
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84. A sample of N2 gas is contaminated with a gas (gas A) of unknown molar mass. The partial pressure of each gas is known to be 200. torr at 25°C. The gases are allowed to effuse through a pinhole, and it is found that gas A escapes at 2.65 times the rate of N2. The molar mass of gas A is
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| 85. Consider two samples of helium in separate containers of the same volume. Sample 1 has an absolute temperature four times that of Sample 2. Both samples are at the same pressure.
Calculate the ratio Z1/Z2.
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| 86. Consider two gas samples:
Calculate the temperature of the SF4(g) sample in which the number of wall impacts per second is the same as in the sample of SF6(g).
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| 87. Samples of the gases H2(g) and SO2(g) have equal masses and are at the same temperature and pressure. Calculate the following:
The ratio of rates of impact with the walls (H2:SO2)
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88. Consider two samples of gas at the same volume and temperature that each contains 1.0 mol of gas. Sample A contains H2 and sample B contains an unknown gas. The ratio of the impacts per second of gas A with the walls of the container to the impacts per second of gas B with the walls of the container is 4. Identify gas B.
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| Calculate the following ratios for a gas at Kelvin temperatures T1 and T2 where T2 = 2T1. |
89. Mean free path at T1 : Mean free path at T2
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90. Collision frequency between O2 molecules at T1 : Collision frequency between O2 molecules at T2
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| 91. Consider three 1-L flasks at the same temperature and pressure. Flask A contains CO gas, flask B contains N2 gas, and flask C contains O2 gas.
In which flask do the molecules have the greatest kinetic energy?
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| 92. Consider three 1.0-L flasks at STP. Flask A contains Ar gas, flask B contains O2 gas, and flask C contains He gas.
In which flask do the gas particles have the highest average velocity?
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93. How is the observed pressure of a gas related to the ideal pressure?
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94. How is the volume of the container related to the volume of an ideal gas?
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95. Which gas, He or H2O vapor, has the lower value of a in the van der Waals equation?
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96. Which gas, Kr or CO2 , has the lower value of b in the van der Waals equation?
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| 97. The ratio V/n versus the Kelvin temperature of an ideal gas (constant pressure)
Which graph represents the plot?
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| 98. The pressure of an ideal gas versus the volume at constant temperature and number of moles
Which graph represents the plot?
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| 99. Volume versus temperature in degrees Celsius for an ideal gas at constant volume and number of moles
Which graph represents the plot?
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| 100. The pressure of an ideal gas versus the number of moles at constant temperature and volume
Which graph represents the plot?
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| 101. Force per impact versus the molar mass of the ideal gas
Which graph represents the plot?
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| 102. The number of wall impacts per second versus the square root of Kelvin temperature for 1 mol of an ideal gas at constant volume
Which graph represents the plot?
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| 103. Consider the decomposition of C5H6O3 as follows:
When a 5.63-g sample of pure C5H6O3 was sealed into an otherwise empty 2.50-L flask and heated to 200°C, the pressure gradually rose to 1.63 atm and remained at that value. Calculate the fraction of C5H6O3 (by moles) that decomposed.
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104. A sample of helium gas has been contaminated with argon gas. At 1 atm and 25°C, the density of the mixture is 0.200 g/L. What is the volume percent argon in the sample?
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| 105. A certain element (Z) reacts to form three gaseous compounds. Consider the following data (pressure = 1.0 atm).
Determine the identity of element Z.
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106. A gaseous binary compound (which is known to contain nitrogen) has a density 1.94 times that of oxygen gas (at the same temperature and pressure). When 1.31 g of the compound is completely burned in excess oxygen, 1.21 g of water is formed. Determine the formula of the compound.
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107. Gas A (MM = 36.0 g/mol) and gas B (MM = 62 g/mol) are present in a mixture that contains 50 molecules A : 326 molecules B. If these gases effuse through a pinhole into a neighboring evacuated chamber, what will be the ratio of A:B in the chamber?
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108. A gaseous mixture is 50% helium gas and 50% nitrogen gas by mass. Determine the percent of the force on the container walls arising from the helium and the ratio of the number of helium impacts to the number of nitrogen impacts on the walls of the vessel.
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109. Suppose a sealed flask contains 1.0 L of oxygen gas that is completely converted to ozone (O3) at the same temperature. Calculate the ratio of the new pressure to the original pressure and the ratio of the number of impacts of ozone molecules with the walls of the container to the number of impacts of oxygen molecules with the walls of the container.
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| 110. Based on the van der Waals equation of state
Which of the following molecules – hydrogen chloride, nitrogen dioxide, or sulfur dioxide – should behave most like an ideal gas.
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111. With respect to the Maxwell-Boltzmann probability distribution function of molecular speeds, which of the following is true?
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112. Which impurity in mined coal, when burned, contributes to the production of acid rain?
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113. Near sea level, the atmosphere is composed of 78% nitrogen and 20% oxygen. Other trace gases make up the remaining 2%. At room temperature,
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| 114. Consider the ideal pressure equation for gases, where a is the proportionality constant, n is the moles of molecules, and V is the gas volume. Identify the correct statement(s) about the proportionality constant.
1. A low value for a reflects weak intermolecular forces among the gas molecules. 2. A high value for a reflects weak intermolecular forces among the gas molecules. 3. Among the gases H2, N2, CH4, and CO2, H2 has the lowest value for a.
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115. A scrubber removes the sulfur dioxide from the exhaust gas before it is emitted from a power plant stack. Which of the following compounds is used in the scrubbing process?
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116. Determine the collision frequency for an oxygen molecule (M = 3.20 × 10-2 kg/mol) in a sample of pure oxygen gas at 35°C and 1.7 atm. Assume that the diameter of an O2 molecule is 300 pm.
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117. Calculate the mean free path in a sample of oxygen gas (M = 3.20 × 10-2 kg/mol) at 35°C and 1.7 atm. Assume that the diameter of an O2 molecule is 300 pm.
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| 118. Complete the following conversion:
1 atm = 760 mm Hg = _____ torr = _____ pascals
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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.
