1. Which graph shows the pressure-temperature relationship expected for an ideal gas? 1) 3)

Size: px
Start display at page:

Download "1. Which graph shows the pressure-temperature relationship expected for an ideal gas? 1) 3)"

Transcription

1 1. Which graph shows the pressure-temperature relationship expected for an ideal gas? 2. Under which conditions does a real gas behave most like an ideal gas? 1) at low temperatures and high pressures 2) at low temperatures and low pressures 3) at high temperatures and high pressures 4) at high temperatures and low pressures 3. According to the kinetic theory of gases, which assumption is correct? 1) Gas particles strongly attract each other. 2) Gas particles travel in curved paths. 3) The volume of gas particles prevents random motion. 4) Energy may be transferred between colliding particles. 4. When a sample of a gas is heated at constant pressure, the average kinetic energy of its molecules 1) decreases, and the volume of the gas increases 2) decreases, and the volume of the gas decreases 3) increases, and the volume of the gas increases 4) increases, and the volume of the gas decreases 5. The concept of an ideal gas is used to explain 1) the mass of a gas sample 2) the behavior of a gas sample 3) why some gases are monatomic 4) why some gases are diatomic 6. Which gas would deviate least from ideal gas behavior at low temperatures? 1) CO 2 2) Cl 2 3) HCl 4) He 7. The behavior of real gases most closely resembles that of ideal gases under conditions of 1) high temperature and low pressure 2) high temperature and high pressure 3) low temperature and low pressure 4) low temperature and high pressure 8. The behavior of a real gas would be most similar to the behavior of an ideal gas under conditions of 1) high pressure and high temperature 2) high pressure and low temperature 3) low pressure and high temperature 4) low pressure and low temperature 9. Real gas behavior deviates from ideal gas behavior because real gas particles have 1) no volume and no attraction for each other 2) no volume but some attraction for each other 3) volume but no attraction for each other 4) volume and some attraction for each other 10. A real gas differs from an ideal gas because the molecules of real gas have 1) some volume and no attraction for each other 2) some volume and some attraction for each other 3) no volume and no attraction for each other 4) no volume and some attraction for each other 11. As the space between molecules in a gas sample decreases, the tendency for the behavior of this gas to deviate from the ideal gas laws 1) decreases 3) remains the same 2) increases 12. Under which conditions of temperature and pressure would gaseous molecules most likely be closest together? 1) high pressure and low temperature 2) high pressure and high temperature 3) low pressure and high temperature 4) low pressure and low temperature 13. A real gas would behave most like an ideal gas under conditions of 1) low pressure and low temperature 2) low pressure and high temperature 3) high pressure and low temperature 4) high pressure and high temperature 14. Helium is most likely to behave as an ideal gas when it is under 1) high pressure and high temperature 2) high pressure and low temperature 3) low pressure and high temperature 4) low pressure and low temperature 15. Which gas would behave most nearly like an ideal gas at STP? 1) CO 2 2) H 2 3) Cl 2 4) NH Which gas is least likely to obey the ideal gas laws at very high pressures and very low temperatures? 1) He 3) Kr 2) Ne 4) Xe

2 17. Which of the following gases behaves most like an ideal gas? 1) H 2 (g) 2) O 2 (g) 3) NH 3 (g) 4) CO 2 (g) 18. Under the same conditions of temperature and pressure, which of the following gases would behave most like an ideal gas? 1) He(g) 2) NH 3 (g) 3) Cl 2 (g) 4) CO 2 (g) 19. The diagrams below represent 1-mole samples of ammonia and hydrogen bromide gases at STP. Compared to the ammonia sample, the hydrogen bromide sample has a 1) larger mass and fewer molecules 2) smaller mass and fewer molecules 3) larger mass and an equal number of molecules 4) smaller mass and an equal number of molecules 20. A sample of H 2 (g) and a sample of N 2 (g) at STP contain the same number of molecules. Each sample must have 1) the same volume, but a different mass 2) the same mass, but a different volume 3) both the same volume and the same mass 4) neither the same volume nor the same mass 21. A closed container holds 3.0 moles of CO 2 gas at STP. What is the total number of moles of Ne(g) that can be placed in a container of the same size at STP? 1) 1.0 mole 3) 3.0 moles 2) 1.5 moles 4) 0.0 moles 22. The diagrams below represent four 500-milliliter flasks. Each flask contains the gas represented by its symbol. All gas samples are at STP. 23. The graph below illustrates the change in the volume of a gas sample as its temperature rises at constant pressure. What temperature is represented by point B? 1) 546 K 3) 273 K 2) 298 K 4) 0 K 24. A sample of gas has a volume of 12 liters at 0ºC and 380 torr. What will be its volume when the pressure is changed to 760 torr at constant temperature? 1) 24 L 3) 12 L 2) 18 L 4) 6.0 L 25. Which temperature change would cause the volume of a sample of an ideal gas to double when the pressure of the sample remains the same? 1) from 200ºC to 400ºC 3) from 200 K to 400 K 2) from 400ºC to 200ºC 4) from 400 K to 200 K 26. The volume of a gas is 250 liters at STP. If the pressure of the gas is held constant and the temperature is changed to 25ºC, the final volume of the gas, in liters, will be equal to 27. What is the difference in pressure between a gas at 50.0 kpa and a gas at standard pressure? 1) 0.0 kpa 3) kpa 2) 51.3 kpa 4) 223 kpa 28. A given sample of a gas has a volume of 3 liters at a pressure of 4 atmospheres. If temperature remains constant and the pressure is changed to 6 atmospheres, the P V product will equal 1) 9 3) 18 2) 12 4) If 10.0 liters of H 2 (g) at STP is heated to a temperature of 546 K, pressure remaining constant, the new volume of the gas will be 1) 5.00 L 3) 15.0 L 2) 20.0 L 4) 40.0 L Each flask contains the same number of 1) atoms, only 3) atoms and molecules 2) molecules, only

3 30. At constant temperature, the relationship between the volume (V) of a given mass of gas and its pressure (P) is 37. Base your answer to the following question on the information below: 31. If 60. liters of hydrogen gas at 546 K is cooled to 273 K at constant pressure, the new volume of the gas will be 1) 120 L 3) 30. L 2) 20. L 4) 40. L 32. A gas sample occupies 10. milliliters at one atmosphere of pressure. If the volume changes to 20. milliliters and the temperature remains the same, the pressure will be 1) 1.0 atm 3) 0.25 atm 2) 2.0 atm 4) 0.50 atm 33. If the pressure on a 3.0-liter sample of a gas is doubled at constant temperature, the new volume will be 1) 0.75 L 3) 6.0 L 2) 1.5 L 4) 9.0 L 34. The pressure on 20 milliliters of a gas at constant temperature is changed from 4 atmospheres to 2 atmospheres. The new volume of the gas is 1) 5 ml 3) 40 ml 2) 10 ml 4) 80 ml 35. At constant pressure, 200. milliliters of a gas at 10. C is heated to 27 C. The new volume of the gas, in milliliters, is equal to Which gas occupies the smallest volume? 1) A 3) C 2) B 4) D 38. Which graph best shows the change in the volume of 1 mole of nitrogen gas as pressure increases and temperature remains constant? 36. As the temperature of a gas is increased from 0 C to 10 C at constant pressure, the volume of the gas will 1) increase by ) increase by ) decrease by ) decrease by The temperature of a 2.0-liter sample of helium gas at STP is increased to 27 C and the pressure is decreased to 80. kpa What is the new volume of the helium sample? 1) 1.4 L 3) 2.8 L 2) 2.0 L 4) 4.0 L 40. If the Kelvin temperature of a gas sample is doubled while the pressure is halved, the volume of the gas will 1) remain the same 3) decrease by half 2) increase 2 times 4) increase 4 times 41. The volume of a sample of a gas at 273ºC is 200. liters. If the volume is decreased to 100. liters at constant pressure, what will be the new temperature of the gas? 1) 0 K 3) 273 K 2) 100. K 4) 546 K 42. A sample of a gas is at STP. As the pressure decreases and the temperature increases, the volume of the gas 1) decreases 3) remains the same 2) increases 43. A sample of a gas occupies 6.00 liters at a temperature of 200. K. If the pressure remains constant and the temperature is raised to 600. K, the volume of the gas sample would be 1) 18.0 L 3) 3.00 L 2) 2.00 L 4) 12.0 L

4 44. A gas has a volume of 1,400 milliliters at a temperature of 20. K and a pressure of 1.0 atm. What will be the new volume when the temperature is changed to 40. K and the pressure is changed to 0.50 atm? 1) 350 ml 3) 1,400 ml 2) 750 ml 4) 5,600 ml 45. In the graph below, the product of the pressure (P) and the volume (V) is plotted against the pressure (P) for gases A, B, C, and D. 47. Which graph best shows the relationship between the pressure of a gas and its average kinetic energy at constant volume? 1) 2) 3) Which gas behaves like an ideal gas? 1) A 3) C 2) B 4) D 46. A sample of gas has a volume of 2.0 liters at a pressure of 1.0 atmosphere. When the volume increases to 4.0 liters, at constant temperature, the pressure will be 1) 1.0 atm 3) 0.50 atm 2) 2.0 atm 4) 0.25 atm 4) 48. Under which conditions will the volume of a given sample of a gas decrease? 1) decreased pressure and decreased temperature 2) decreased pressure and increased temperature 3) increased pressure and decreased temperature 4) increased pressure and increased temperature

5 49. Which graph represents the relationship between volume and Kelvin temperature for an ideal gas at constant pressure? 53. The volume of a 1.00-mole sample of an ideal gas will decrease when the 1) pressure decreases and the temperature decreases 2) pressure decreases and the temperature increases 3) pressure increases and the temperature decreases 4) pressure increases and the temperature increases 54. The volume of a sample of a gas is 1.0 liter at STP. If the pressure remains constant and the temperature is raised to 546 K, the new volume of the gas will be 1) 0.25 L 3) 0.50 L 2) 2.0 L 4) 4.0 L 55. The diagram below represents a gas sample confined in a cylinder fitted with a movable piston. 50. A gas occupies a volume of 500. milliliters at a pressure of 38.0 kpa and a temperature of 298 K. At what temperature will the gas occupy a volume of 250. milliliters and have a pressure of 76.0 kpa? 1) 149 K 3) 447 K 2) 298 K 4) 596 K 51. Which changes in pressure and temperature occur as a given mass of gas at 50.6 kpa and 546 K is changed to STP? 1) The pressure is doubled and the temperature is halved. 2) The pressure is halved and the temperature is doubled. 3) Both the pressure and the temperature are doubled. 4) Both the pressure and the temperature are halved. 52. At constant pressure, which graph shows the correct relationship between the volume of a gas (V) and its absolute temperature (T)? As the piston moves toward point A at constant temperature, which mathematical relationship between pressure (P) and volume (V) remains constant? 1) P + V 3) P V 2) P V 4) P ^ V 56. At constant pressure, the volume of a gas will increase when its temperature is changed from 10ºC to 1) 263 K 3) 273 K 2) 283 K 4) 293 K 57. If the pressure and Kelvin temperature of 2.00 moles of an ideal gas at STP are doubled, the resulting volume will be 1) 5.60 L 3) 11.2 L 2) 22.4 L 4) 44.8 L 58. A gas has a pressure of 120 kpa, a temperature of 400. K, and a volume of 50.0 milliliters. What volume will the gas have at a pressure of 60 kpa and a temperature of 200. K? 1) 12.5 ml 3) 100. ml 2) 50.0 ml 4) 200. ml 59. A gas at STP has a volume of 1.0 liter. If the pressure is doubled and the temperature remains constant, the new volume of the gas will be 1) 0.25 L 3) 0.50 L 2) 2.0 L 4) 4.0 L

6 60. Which graph best represents the pressure-volume relationship for an ideal gas at constant temperature? 64. A sample of gas occupies 15.0 liters at a pressure of 2.00 atmospheres and a temperature of 300. K. If the pressure is lowered to 1.00 atmosphere and the temperature is raised to 400. K, the volume of the gas sample would be 1) 5.63 L 3) 22.5 L 2) 10.0 L 4) 40.0 L Base your answers to questions 65 and 66 on the graphs shown below. 61. At constant pressure, what temperature must be reached to increase a 100.-milliliter sample of a gas initially at 300. K to a volume of 200. milliliters? 1) 150. K 3) 300. K 2) 200. K 4) 600. K 62. A 3.00-liter sample of gas is at 288 K and 1.00 atm. If the pressure of the gas is increased to 2.00 atm and its volume is decreased to 1.50 liters, the Kelvin temperature of the sample will be 1) 144 K 3) 432 K 2) 288 K 4) 576 K 63. At constant pressure, which curve best shows the relationship between the volume of an ideal gas and its absolute temperature? 1) A 3) C 2) B 4) D 65. Which graph best represents how the volume of a given mass of a gas varies with the pressure exerted on it at constant temperature? 1) 1 3) 3 2) Which graph best represents how the volume of a given mass of a gas varies with the Kelvin (absolute) temperature at constant pressure? 1) 1 3) 3 2) The volume of a sample of a gas at 0 C is 100 liters. If the volume of the gas is increased to 200 liters at constant pressure, what is the new temperature of the gas in degrees Kelvin? 1) 0 K 3) 100 K 2) 273 K 4) 546 K 68. At constant pressure, 50. milliliters (ml) of a gas at 20.ºC is heated to 30.ºC. The new volume of the gas in milliliters (ml) is equal to

7 69. The graph below represents the relationship between pressure and volume of a given mass of a gas at constant temperature. 75. If the pressure on 36.0 milliliters of a gas at STP is changed to a pressure of 25.3 kpa at constant temperature, the new volume of the gas is 1) 9.00 ml 3) 144 ml 2) 126 ml 4) 226 ml 76. The table above shows the changes in the volume of a gas as the pressure changes at constant temperature. The product of pressure and volume is constant. According to the graph, what is the product in atm ml? 1) 20. 3) 60. 2) 40. 4) A sample of oxygen gas in a closed system has a volume of 200 milliliters at 600 K. If the pressure is held constant and the temperature is lowered to 300 K, the new volume of the gas will be 1) 100 ml 3) 300 ml 2) 200 ml 4) 400 ml 71. A gas occupies a volume of 444 ml at 273 K and 79.0 kpa. What is the final kelvin temperature when the volume of the gas is changed to 1880 ml and the pressure is changed to 38.7 kpa? 1) 31.5 K 3) 566 K 2) 292 K 4) 2360 K 72. At a temperature of 273 K, a 400.-milliliter gas sample has a pressure of 760. millimeters of mercury. If the pressure is changed to 380. millimeters of mercury, at which temperature will this gas sample have a volume of 551 milliliters? 1) 100 K 3) 273 K 2) 188 K 4) 546 K 73. A gas sample has a volume of 25.0 milliliters at a pressure of 1.00 atmosphere. If the volume increases to 50.0 milliliters and the temperature remains constant, the new pressure will be 1) 1.00 atm 3) atm 2) 2.00 atm 4) atm 74. The volume of a gas is 4.00 liters at 293 K and constant pressure. For the volume of the gas to become 3.00 liters, the Kelvin temperature must be equal to 1) ) ) ) Which equation best expresses the relationship between pressure and volume for the gas? 1) 2) 3) 4) 77. A 2.5 liter sample of gas is at STP. When the temperature is raised to 273ºC and the pressure remains constant, the new volume of the gas will be 1) 1.25 L 3) 5.0 L 2) 2.5 L 4) 10. L 78. A sample of oxygen gas has a volume of 150. milliliters at 300 K. If the pressure of the sample is held constant and the temperature is raised to 600 K, the new volume of the sample will be 1) 75.0 ml 3) 300. ml 2) 150. ml 4) 600. ml 79. At a constant pressure, how does the volume of 1 mole of an ideal gas vary? 1) directly with the Kelvin temperature 2) indirectly with the Kelvin temperature 3) directly with the mass of the gas 4) indirectly with the mass of the gas 80. Compared to a 1 mole sample of hydrogen at 273 K and 1 atmosphere, a 1 mole sample of hydrogen at 298 K and 1 atmosphere contains 1) more molecules 2) fewer molecules 3) molecules having higher average kinetic energy 4) molecules having lower average kinetic energy

8 81. The diagram below represents a gas confined in a cylinder fitted with a movable piston. 86. The diagram below shows the collection of H 2 gas over water at 25 C. The total pressure in the tube is torr. As the piston moves toward point A at constant temperature, which relationship involving pressure (P) and volume (V) is correct? 1) P + V = k 3) P ^ V = k 2) P V = k 4) P V = k 82. A 16.0 liter sample of CH 4 (g) is at 0ºC and 1 atmosphere. The volume of the gas sample in liters at 27ºC and 1 atmosphere is equal to 83. A sample of a gas has a volume of 40. milliliters at 76.0 kpa. What will be the new volume of the gas if the pressure is increased to 80.0 kpa, temperature remaining constant? 1) 80 ml 3) 38 ml 2) 42 ml 4) 20 ml 84. The pressure on a 200-milliliter sample of CO 2 (g) at constant temperature is increased from 60 kpa to 120 kpa. What is the new volume of the gas? 1) 100 ml 3) 400 ml 2) 300 ml 4) 600 ml 85. When 500. milliliters of hydrogen gas is heated from 30ºC to 60ºC at constant pressure, the volume of the gas at 60ºC is equal to What is the pressure exerted by the hydrogen gas alone? 1) 23.8 torr 3) torr 2) torr 4) torr 87. The partial pressures of gases A, B, and C in a mixture are atmosphere, atmosphere, and 1.25 atmospheres, respectively. What is the total pressure of the gas mixture in kpa? 1) 2.25 kpa 3) 228 kpa 2) 202 kpa 4) 301 kpa 88. A cylinder is filled with 2.00 moles of nitrogen, 3.00 moles of argon, and 5.00 moles of helium. If the gas mixture is at STP, what is the partial pressure of the argon? 1) 20.3 kpa 3) 50.7 kpa 2) 30.4 kpa 4) 101 kpa 89. When 7.00 moles of gas A and 3.00 moles of gas B are combined, the total pressure exerted by the gas mixture is 76.0 kpa. What is the partial pressure exerted by gas A in this mixture? 1) 7.60 kpa 3) 53.2 kpa 2) 22.8 kpa 4) 76.0 kpa 90. Gases X, Y, and Z, in a closed system at constant temperature, have a total pressure of 80 kpa. The partial pressure of each gas is shown below. The partial pressure of gas X, in Pascals, is equal to 1) 80 (B + C) 2) (B + C) 80 3) (B + C) 80 4) 80 (B + C)

9 91. If 4.00 moles of oxygen gas, 3.00 moles of hydrogen gas, and 1.00 mole of nitrogen gas are combined in a closed container at standard pressure, what is the partial pressure exerted by the hydrogen gas? 1) 1.00 atm 3) 3.00 atm 2) atm 4) atm 92. A 300.-milliliter container that is filled with 100. milliliters of oxygen and 200. milliliters of hydrogen has a total pressure of 75 kpa. What is the partial pressure of the oxygen? 1) 10 kpa 3) 25 kpa 2) 20 kpa 4) 50 kpa 93. A gas volume that contains an equal number of hydrogen and oxygen molecules has a pressure of 0.6 atmosphere. The partial pressure due to the oxygen molecules is 1) 0.1 atm 3) 0.3 atm 2) 0.2 atm 4) 0.6 atm 94. A gas sample consisting of 2.0 moles of hydrogen and 1.0 mole of oxygen is collected over water at 29ºC and 75 kpa. What is the partial pressure of the hydrogen in the sample? 1) 24 kpa 3) 72 kpa 2) 48 kpa 4) 75 kpa 95. What is the pressure of a mixture of CO 2, SO 2, and H 2 O gases, if each gas has a partial pressure of 25 kpa? 1) 25 kpa 3) 75 kpa 2) 50 kpa 4) 101 kpa 96. A sealed container has 1 mole of helium and 2 moles of nitrogen at 30ºC. When the total pressure of the mixture is 60 kpa, what is the partial pressure of the nitrogen? 1) 10 kpa 3) 40 kpa 2) 20 kpa 4) 60 kpa 97. A sealed flask contains a mixture of 1.0 mole of N 2 (g) and 2.0 moles of O 2 (g) at 25ºC. If the total pressure of this gas mixture is 6.0 atmospheres, what is the partial pressure of the N 2 (g)? 1) 6.0 atm 3) 3.0 atm 2) 2.0 atm 4) 9.0 atm 98. A mixture of oxygen, nitrogen, and hydrogen gases exerts a total pressure of 74 kpa at 0ºC. The partial pressure of the oxygen is 20 kpa and the partial pressure of the nitrogen is 40 kpa. What is the partial pressure of the hydrogen gas in this mixture? 1) 14 kpa 3) 40 kpa 2) 20 kpa 4) 74 kpa 99. The diagram below shows two flasks connected by a stopcock. Flask A contains helium gas. Flask B contains a vacuum. What final volume will the gas occupy after the stopcock is opened? 1) 100 ml 3) 400 ml 2) 300 ml 4) 500 ml 100. Gases in the amounts shown in the table below were added to an empty 22.4 liter container at 0 C. How much argon gas should be added to the container at 0 C to produce a total pressure of 1.00 atmosphere? 1) 1.12 moles 3) mole 2) 2.24 moles 4) mole 101. What is the total pressure exerted by a mixture containing two gases if the partial pressure of one gas is 70 kpa and the partial pressure of the other gas is 30 kpa? 1) 30 kpa 3) 70 kpa 2) 40 kpa 4) 100 kpa 102. A flask contains a mixture of N 2 (g) and O 2 (g) at STP. If the partial pressure exerted by the N 2 (g) is 40.0 kpa, the partial pressure of the O 2 (g) is 1) 21.3 kpa 3) 61.3 kpa 2) 37.3 kpa 4) 720 kpa 103. A mixture of gases has a total pressure of 200 kpa. The mixture contains 8 moles of nitrogen gas and 2 moles of oxygen gas. What pressure is exerted by the oxygen gas molecules? 1) 20 kpa 3) 200 kpa 2) 40 kpa 4) 400 kpa 104. Gas samples A, B, and C are contained in a system at STP. The partial pressure of sample A is 38.0 kpa and the partial pressure of sample B is 19.0 kpa. What is the partial pressure of sample C? 1) 19.0 kpa 3) 44.3 kpa 2) 38.0 kpa 4) 63.3 kpa

10 105. At STP, which gas diffuses at the faster rate? 1) H 2 2) N 2 3) CO 2 4) NH Under the same conditions of temperature and pressure, which gas will diffuse at the slowest rate? 1) He 3) Ar 2) Ne 4) Rn 107. At STP, which of the following gases diffuses most rapidly? 1) H 2 2) F 2 3) Ne 4) Xe 108. Which gas would diffuse most rapidly under the same conditions of temperature and pressure? 1) gas A, molecular mass = 4 2) gas B, molecular mass = 16 3) gas C, molecular mass = 36 4) gas D, molecular mass = At STP, which gas will diffuse more rapidly than Ne? 1) He 3) Kr 2) Ar 4) Xe 110. At STP, which of the following gases will diffuse most rapidly? 1) hydrogen 3) fluorine 2) nitrogen 4) oxygen 111. Under the same conditions of temperature and pressure, which of the following gases has the greatest rate of diffusion? 1) H 2 (g) 2) He(g) 3) CH 4 (g) 4) NH 3 (g) 112. Which gas will diffuse at the fastest rate under the same conditions of temperature and pressure? 1) O 2 2) N 2 3) F 2 4) H At STP, which of the following gases will diffuse at the slowest rate? 1) CO 2 (g) 2) F 2 (g) 3) CO(g) 4) Ar(g) 114. The stoppered tubes below, labeled A through D, each contain a different gas. When the tubes are unstoppered at the same time and under the same conditions of temperature and pressure, from which tube will gas diffuse at the fastest rate? 1) A 3) C 2) B 4) D 115. Which of the following gases will diffuse most rapidly at STP? 1) He 2) Ne 3) O 2 4) N At STP, which of the following gases has the highest rate of diffusion? 1) He 3) Ar 2) Ne 4) Kr 117. Which of the following gases would have the slowest rate of diffusion when all of the gases are held at the same temperature and pressure? 1) N 2 2) NO 3) O 2 4) CO Which gas diffuses most rapidly at STP? 1) Ne 2) Ar 3) Cl 2 4) F Under the same conditions of temperature and pressure, which of the following noble gases diffuses most rapidly? 1) Ne 3) Kr 2) Ar 4) Xe 120. At the same temperature and pressure, which gas will diffuse through air at the fastest rate? 1) H 2 2) O 2 3) CO 4) CO At STP, which of the following gases will diffuse most rapidly? 1) Cl 2 2) NH 3 3) CO 2 4) N 2

11 122. The table below lists four gases and their molecular mass Given the same conditions of temperature and pressure, which noble gas will diffuse most rapidly? 1) He 3) Ar 2) Ne 4) Kr Which gas diffuses at the slowest rate at STP? 1) A 3) C 2) B 4) D

12 Reference Tables

13 Reference Tables

14 Reference Tables

15 Answer Key

16 Answer Key

17 Answer Key

5. Which temperature is equal to +20 K? 1) 253ºC 2) 293ºC 3) 253 C 4) 293 C

5. Which temperature is equal to +20 K? 1) 253ºC 2) 293ºC 3) 253 C 4) 293 C 1. The average kinetic energy of water molecules increases when 1) H 2 O(s) changes to H 2 O( ) at 0ºC 3) H 2 O( ) at 10ºC changes to H 2 O( ) at 20ºC 2) H 2 O( ) changes to H 2 O(s) at 0ºC 4) H 2 O( )

More information

Gas Laws. The kinetic theory of matter states that particles which make up all types of matter are in constant motion.

Gas Laws. The kinetic theory of matter states that particles which make up all types of matter are in constant motion. Name Period Gas Laws Kinetic energy is the energy of motion of molecules. Gas state of matter made up of tiny particles (atoms or molecules). Each atom or molecule is very far from other atoms or molecules.

More information

CHEMISTRY GAS LAW S WORKSHEET

CHEMISTRY GAS LAW S WORKSHEET Boyle s Law Charles Law Guy-Lassac's Law Combined Gas Law For a given mass of gas at constant temperature, the volume of a gas varies inversely with pressure PV = k The volume of a fixed mass of gas is

More information

Review - After School Matter Name: Review - After School Matter Tuesday, April 29, 2008

Review - After School Matter Name: Review - After School Matter Tuesday, April 29, 2008 Name: Review - After School Matter Tuesday, April 29, 2008 1. Figure 1 The graph represents the relationship between temperature and time as heat was added uniformly to a substance starting at a solid

More information

Exam 4 Practice Problems false false

Exam 4 Practice Problems false false Exam 4 Practice Problems 1 1. Which of the following statements is false? a. Condensed states have much higher densities than gases. b. Molecules are very far apart in gases and closer together in liquids

More information

Stoichiometry. 1. The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 0.1; (4) 0.2.

Stoichiometry. 1. The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 0.1; (4) 0.2. Stoichiometry 1 The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 01; (4) 02 2 A 44 gram sample of a hydrate was heated until the water of hydration was driven

More information

7. 1.00 atm = 760 torr = 760 mm Hg = 101.325 kpa = 14.70 psi. = 0.446 atm. = 0.993 atm. = 107 kpa 760 torr 1 atm 760 mm Hg = 790.

7. 1.00 atm = 760 torr = 760 mm Hg = 101.325 kpa = 14.70 psi. = 0.446 atm. = 0.993 atm. = 107 kpa 760 torr 1 atm 760 mm Hg = 790. CHATER 3. The atmosphere is a homogeneous mixture (a solution) of gases.. Solids and liquids have essentially fixed volumes and are not able to be compressed easily. have volumes that depend on their conditions,

More information

Boyles Law. At constant temperature the volume occupied by a fixed amount of gas is inversely proportional to the pressure on the gas 1 P = P

Boyles Law. At constant temperature the volume occupied by a fixed amount of gas is inversely proportional to the pressure on the gas 1 P = P Boyles Law At constant temperature the volume occupied by a fixed amount of gas is inversely proportional to the pressure on the gas 1 or k 1 Boyles Law Example ressure olume Initial 2.00 atm 100 cm 3

More information

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. Chapter 10 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) A gas at a pressure of 10.0 Pa exerts a force of N on an area of 5.5 m2. A) 1.8 B) 0.55

More information

The Gas Laws. Our Atmosphere. Pressure = Units of Pressure. Barometer. Chapter 10

The Gas Laws. Our Atmosphere. Pressure = Units of Pressure. Barometer. Chapter 10 Our Atmosphere The Gas Laws 99% N 2 and O 2 78% N 2 80 70 Nitrogen Chapter 10 21% O 2 1% CO 2 and the Noble Gases 60 50 40 Oxygen 30 20 10 0 Gas Carbon dioxide and Noble Gases Pressure Pressure = Force

More information

= 1.038 atm. 760 mm Hg. = 0.989 atm. d. 767 torr = 767 mm Hg. = 1.01 atm

= 1.038 atm. 760 mm Hg. = 0.989 atm. d. 767 torr = 767 mm Hg. = 1.01 atm Chapter 13 Gases 1. Solids and liquids have essentially fixed volumes and are not able to be compressed easily. Gases have volumes that depend on their conditions, and can be compressed or expanded by

More information

Gases and Kinetic-Molecular Theory: Chapter 12. Chapter Outline. Chapter Outline

Gases and Kinetic-Molecular Theory: Chapter 12. Chapter Outline. Chapter Outline Gases and Kinetic-Molecular heory: Chapter Chapter Outline Comparison of Solids, Liquids, and Gases Composition of the Atmosphere and Some Common Properties of Gases Pressure Boyle s Law: he Volume-Pressure

More information

CHAPTER 12. Gases and the Kinetic-Molecular Theory

CHAPTER 12. Gases and the Kinetic-Molecular Theory CHAPTER 12 Gases and the Kinetic-Molecular Theory 1 Gases vs. Liquids & Solids Gases Weak interactions between molecules Molecules move rapidly Fast diffusion rates Low densities Easy to compress Liquids

More information

CHEMISTRY. Matter and Change. Section 13.1 Section 13.2 Section 13.3. The Gas Laws The Ideal Gas Law Gas Stoichiometry

CHEMISTRY. Matter and Change. Section 13.1 Section 13.2 Section 13.3. The Gas Laws The Ideal Gas Law Gas Stoichiometry CHEMISTRY Matter and Change 13 Table Of Contents Chapter 13: Gases Section 13.1 Section 13.2 Section 13.3 The Gas Laws The Ideal Gas Law Gas Stoichiometry State the relationships among pressure, temperature,

More information

Page 2. Base your answers to questions 7 through 9 on this phase diagram

Page 2. Base your answers to questions 7 through 9 on this phase diagram 1. The normal boiling point of water is often depressed at high altitudes. Which of the following explains this phenomenon? t high altitudes, the lower atmospheric pressure equals the equilibrium water

More information

EXPERIMENT 15: Ideal Gas Law: Molecular Weight of a Vapor

EXPERIMENT 15: Ideal Gas Law: Molecular Weight of a Vapor EXPERIMENT 15: Ideal Gas Law: Molecular Weight of a Vapor Purpose: In this experiment you will use the ideal gas law to calculate the molecular weight of a volatile liquid compound by measuring the mass,

More information

Temperature. Number of moles. Constant Terms. Pressure. Answers Additional Questions 12.1

Temperature. Number of moles. Constant Terms. Pressure. Answers Additional Questions 12.1 Answers Additional Questions 12.1 1. A gas collected over water has a total pressure equal to the pressure of the dry gas plus the pressure of the water vapor. If the partial pressure of water at 25.0

More information

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. General Chemistry PHS 1015 Practice Exam 4 Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which of the following statements about pressure

More information

AS1 MOLES. oxygen molecules have the formula O 2 the relative mass will be 2 x 16 = 32 so the molar mass will be 32g mol -1

AS1 MOLES. oxygen molecules have the formula O 2 the relative mass will be 2 x 16 = 32 so the molar mass will be 32g mol -1 Moles 1 MOLES The mole the standard unit of amount of a substance the number of particles in a mole is known as Avogadro s constant (L) Avogadro s constant has a value of 6.023 x 10 23 mol -1. Example

More information

1.4.6-1.4.8 Gas Laws. Heat and Temperature

1.4.6-1.4.8 Gas Laws. Heat and Temperature 1.4.6-1.4.8 Gas Laws Heat and Temperature Often the concepts of heat and temperature are thought to be the same, but they are not. Perhaps the reason the two are incorrectly thought to be the same is because

More information

THE IDEAL GAS LAW AND KINETIC THEORY

THE IDEAL GAS LAW AND KINETIC THEORY Chapter 14 he Ideal Gas Law and Kinetic heory Chapter 14 HE IDEAL GAS LAW AND KINEIC HEORY REIEW Kinetic molecular theory involves the study of matter, particularly gases, as very small particles in constant

More information

A. Kinetic Molecular Theory (KMT) = the idea that particles of matter are always in motion and that this motion has consequences.

A. Kinetic Molecular Theory (KMT) = the idea that particles of matter are always in motion and that this motion has consequences. I. MOLECULES IN MOTION: A. Kinetic Molecular Theory (KMT) = the idea that particles of matter are always in motion and that this motion has consequences. 1) theory developed in the late 19 th century to

More information

Chemistry 13: States of Matter

Chemistry 13: States of Matter Chemistry 13: States of Matter Name: Period: Date: Chemistry Content Standard: Gases and Their Properties The kinetic molecular theory describes the motion of atoms and molecules and explains the properties

More information

CHEMICAL EQUILIBRIUM (ICE METHOD)

CHEMICAL EQUILIBRIUM (ICE METHOD) CHEMICAL EQUILIBRIUM (ICE METHOD) Introduction Chemical equilibrium occurs when opposing reactions are proceeding at equal rates. The rate at which the products are formed from the reactants equals the

More information

Kinetic Theory of Gases. 6.1 Properties of Gases 6.2 Gas Pressure. Properties That Describe a Gas. Gas Pressure. Learning Check.

Kinetic Theory of Gases. 6.1 Properties of Gases 6.2 Gas Pressure. Properties That Describe a Gas. Gas Pressure. Learning Check. Chapter 6 Gases Kinetic Theory of Gases 6.1 Properties of Gases 6.2 Gas Pressure A gas consists of small particles that move rapidly in straight lines. have essentially no attractive (or repulsive) forces.

More information

Study the following diagrams of the States of Matter. Label the names of the Changes of State between the different states.

Study the following diagrams of the States of Matter. Label the names of the Changes of State between the different states. Describe the strength of attractive forces between particles. Describe the amount of space between particles. Can the particles in this state be compressed? Do the particles in this state have a definite

More information

Lecture Notes: Gas Laws and Kinetic Molecular Theory (KMT).

Lecture Notes: Gas Laws and Kinetic Molecular Theory (KMT). CHEM110 Week 9 Notes (Gas Laws) Page 1 of 7 Lecture Notes: Gas Laws and Kinetic Molecular Theory (KMT). Gases Are mostly empty space Occupy containers uniformly and completely Expand infinitely Diffuse

More information

States of Matter CHAPTER 10 REVIEW SECTION 1. Name Date Class. Answer the following questions in the space provided.

States of Matter CHAPTER 10 REVIEW SECTION 1. Name Date Class. Answer the following questions in the space provided. CHAPTER 10 REVIEW States of Matter SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. Identify whether the descriptions below describe an ideal gas or a real gas. ideal gas

More information

F321 MOLES. Example If 1 atom has a mass of 1.241 x 10-23 g 1 mole of atoms will have a mass of 1.241 x 10-23 g x 6.02 x 10 23 = 7.

F321 MOLES. Example If 1 atom has a mass of 1.241 x 10-23 g 1 mole of atoms will have a mass of 1.241 x 10-23 g x 6.02 x 10 23 = 7. Moles 1 MOLES The mole the standard unit of amount of a substance (mol) the number of particles in a mole is known as Avogadro s constant (N A ) Avogadro s constant has a value of 6.02 x 10 23 mol -1.

More information

THE KINETIC THEORY OF GASES

THE KINETIC THEORY OF GASES Chapter 19: THE KINETIC THEORY OF GASES 1. Evidence that a gas consists mostly of empty space is the fact that: A. the density of a gas becomes much greater when it is liquefied B. gases exert pressure

More information

Stoichiometry. 1. The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 0.1; (4) 0.2.

Stoichiometry. 1. The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 0.1; (4) 0.2. Stoichiometry 1 The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 01; (4) 02 2 A 44 gram sample of a hydrate was heated until the water of hydration was driven

More information

IB Chemistry. DP Chemistry Review

IB Chemistry. DP Chemistry Review DP Chemistry Review Topic 1: Quantitative chemistry 1.1 The mole concept and Avogadro s constant Assessment statement Apply the mole concept to substances. Determine the number of particles and the amount

More information

Gases. Solids' particles vibrate. This is the only motion experienced by this state of matter.

Gases. Solids' particles vibrate. This is the only motion experienced by this state of matter. 1. Kinetic Molecular Theory A. Main Points 1. All matter consists of particles: either atoms or molecules. For a gas, if it is monoatomic (like He or Ar), it will consist of atoms. If it consists of I2,

More information

Chemistry 110 Lecture Unit 5 Chapter 11-GASES

Chemistry 110 Lecture Unit 5 Chapter 11-GASES Chemistry 110 Lecture Unit 5 Chapter 11-GASES I. PROPERITIES OF GASES A. Gases have an indefinite shape. B. Gases have a low density C. Gases are very compressible D. Gases exert pressure equally in all

More information

7. Gases, Liquids, and Solids 7.1 Kinetic Molecular Theory of Matter

7. Gases, Liquids, and Solids 7.1 Kinetic Molecular Theory of Matter 7. Gases, Liquids, and Solids 7.1 Kinetic Molecular Theory of Matter Kinetic Molecular Theory of Matter The Kinetic Molecular Theory of Matter is a concept that basically states that matter is composed

More information

Temperature Measure of KE At the same temperature, heavier molecules have less speed Absolute Zero -273 o C 0 K

Temperature Measure of KE At the same temperature, heavier molecules have less speed Absolute Zero -273 o C 0 K Temperature Measure of KE At the same temperature, heavier molecules have less speed Absolute Zero -273 o C 0 K Kinetic Molecular Theory of Gases 1. Large number of atoms/molecules in random motion 2.

More information

CHEMISTRY 113 EXAM 4(A)

CHEMISTRY 113 EXAM 4(A) Summer 2003 1. The molecular geometry of PF 4 + ion is: A. bent B. trigonal planar C. tetrahedral D. octahedral CHEMISTRY 113 EXAM 4(A) 2. The Cl-C-Cl bond angle in CCl 2 O molecule (C is the central atom)

More information

Test 5 Review questions. 1. As ice cools from 273 K to 263 K, the average kinetic energy of its molecules will

Test 5 Review questions. 1. As ice cools from 273 K to 263 K, the average kinetic energy of its molecules will Name: Thursday, December 13, 2007 Test 5 Review questions 1. As ice cools from 273 K to 263 K, the average kinetic energy of its molecules will 1. decrease 2. increase 3. remain the same 2. The graph below

More information

B) atomic number C) both the solid and the liquid phase D) Au C) Sn, Si, C A) metal C) O, S, Se C) In D) tin D) methane D) bismuth B) Group 2 metal

B) atomic number C) both the solid and the liquid phase D) Au C) Sn, Si, C A) metal C) O, S, Se C) In D) tin D) methane D) bismuth B) Group 2 metal 1. The elements on the Periodic Table are arranged in order of increasing A) atomic mass B) atomic number C) molar mass D) oxidation number 2. Which list of elements consists of a metal, a metalloid, and

More information

ESSAY. Write your answer in the space provided or on a separate sheet of paper.

ESSAY. Write your answer in the space provided or on a separate sheet of paper. Test 1 General Chemistry CH116 Summer, 2012 University of Massachusetts, Boston Name ESSAY. Write your answer in the space provided or on a separate sheet of paper. 1) Sodium hydride reacts with excess

More information

87 16 70 20 58 24 44 32 35 40 29 48 (a) graph Y versus X (b) graph Y versus 1/X

87 16 70 20 58 24 44 32 35 40 29 48 (a) graph Y versus X (b) graph Y versus 1/X HOMEWORK 5A Barometer; Boyle s Law 1. The pressure of the first two gases below is determined with a manometer that is filled with mercury (density = 13.6 g/ml). The pressure of the last two gases below

More information

Gases. States of Matter. Molecular Arrangement Solid Small Small Ordered Liquid Unity Unity Local Order Gas High Large Chaotic (random)

Gases. States of Matter. Molecular Arrangement Solid Small Small Ordered Liquid Unity Unity Local Order Gas High Large Chaotic (random) Gases States of Matter States of Matter Kinetic E (motion) Potential E(interaction) Distance Between (size) Molecular Arrangement Solid Small Small Ordered Liquid Unity Unity Local Order Gas High Large

More information

13.1 The Nature of Gases. What is Kinetic Theory? Kinetic Theory and a Model for Gases. Chapter 13: States of Matter. Principles of Kinetic Theory

13.1 The Nature of Gases. What is Kinetic Theory? Kinetic Theory and a Model for Gases. Chapter 13: States of Matter. Principles of Kinetic Theory Chapter 13: States of Matter The Nature of Gases The Nature of Gases kinetic molecular theory (KMT), gas pressure (pascal, atmosphere, mm Hg), kinetic energy The Nature of Liquids vaporization, evaporation,

More information

Chapter 4 Practice Quiz

Chapter 4 Practice Quiz Chapter 4 Practice Quiz 1. Label each box with the appropriate state of matter. A) I: Gas II: Liquid III: Solid B) I: Liquid II: Solid III: Gas C) I: Solid II: Liquid III: Gas D) I: Gas II: Solid III:

More information

CHEM 120 Online Chapter 7

CHEM 120 Online Chapter 7 CHEM 120 Online Chapter 7 Date: 1. Which of the following statements is not a part of kinetic molecular theory? A) Matter is composed of particles that are in constant motion. B) Particle velocity increases

More information

Chapter 10. Can You... 1. draw the Lewis structure for a given covalently bonded molecule?

Chapter 10. Can You... 1. draw the Lewis structure for a given covalently bonded molecule? Chapter 10 Can You... 1. draw the Lewis structure for a given covalently bonded molecule? e.g. SF 6 and CH 3 Cl 2. identify and count the number of non-bonding and bonding domains within a given covalently

More information

Chapter 13 Gases. Review Skills

Chapter 13 Gases. Review Skills Chapter 13 Gases t s Monday morning, and Lilia is walking out of the chemistry building, thinking about the introductory lecture on gases that her instructor just presented. Dr. Scanlon challenged the

More information

Name Class Date. In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question.

Name Class Date. In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. Assessment Chapter Test A Chapter: States of Matter In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1. The kinetic-molecular

More information

The Mole. Chapter 10. Dimensional Analysis. The Mole. How much mass is in one atom of carbon-12? Molar Mass of Atoms 3/1/2015

The Mole. Chapter 10. Dimensional Analysis. The Mole. How much mass is in one atom of carbon-12? Molar Mass of Atoms 3/1/2015 The Mole Chapter 10 1 Objectives Use the mole and molar mass to make conversions among moles, mass, and number of particles Determine the percent composition of the components of a compound Calculate empirical

More information

Unit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test

Unit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test Unit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test NAME Section 7.1 The Mole: A Measurement of Matter A. What is a mole? 1. Chemistry is a quantitative science. What does this term mean?

More information

Bonding Practice Problems

Bonding Practice Problems NAME 1. When compared to H 2 S, H 2 O has a higher 8. Given the Lewis electron-dot diagram: boiling point because H 2 O contains stronger metallic bonds covalent bonds ionic bonds hydrogen bonds 2. Which

More information

KINETIC MOLECULAR THEORY OF MATTER

KINETIC MOLECULAR THEORY OF MATTER KINETIC MOLECULAR THEORY OF MATTER The kinetic-molecular theory is based on the idea that particles of matter are always in motion. The theory can be used to explain the properties of solids, liquids,

More information

1. What is the molecular formula of a compound with the empirical formula PO and a gram-molecular mass of 284 grams?

1. What is the molecular formula of a compound with the empirical formula PO and a gram-molecular mass of 284 grams? Name: Tuesday, May 20, 2008 1. What is the molecular formula of a compound with the empirical formula PO and a gram-molecular mass of 284 grams? 2 5 1. P2O 5 3. P10O4 2. P5O 2 4. P4O10 2. Which substance

More information

Test Review # 9. Chemistry R: Form TR9.13A

Test Review # 9. Chemistry R: Form TR9.13A Chemistry R: Form TR9.13A TEST 9 REVIEW Name Date Period Test Review # 9 Collision theory. In order for a reaction to occur, particles of the reactant must collide. Not all collisions cause reactions.

More information

Multiple Choice questions (one answer correct)

Multiple Choice questions (one answer correct) Mole Concept Multiple Choice questions (one answer correct) (1) Avogadro s number represents the number of atoms in (a) 12g of C 12 (b) 320g of sulphur (c) 32g of oxygen (d) 12.7g of iodine (2) The number

More information

Chapter 8: Gases and Gas Laws.

Chapter 8: Gases and Gas Laws. 133 Chapter 8: Gases and Gas Laws. The first substances to be produced and studied in high purity were gases. Gases are more difficult to handle and manipulate than solids and liquids, since any minor

More information

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Given: 4 NO2(g) + O2(g) 2 N2O5(g) ΔH = -110.2 kj find ΔH for N2O5(g) 2 NO2(g) + 1/2 O2(g).

More information

Thermodynamics AP Physics B. Multiple Choice Questions

Thermodynamics AP Physics B. Multiple Choice Questions Thermodynamics AP Physics B Name Multiple Choice Questions 1. What is the name of the following statement: When two systems are in thermal equilibrium with a third system, then they are in thermal equilibrium

More information

Chem 112 Intermolecular Forces Chang From the book (10, 12, 14, 16, 18, 20,84,92,94,102,104, 108, 112, 114, 118 and 134)

Chem 112 Intermolecular Forces Chang From the book (10, 12, 14, 16, 18, 20,84,92,94,102,104, 108, 112, 114, 118 and 134) Chem 112 Intermolecular Forces Chang From the book (10, 12, 14, 16, 18, 20,84,92,94,102,104, 108, 112, 114, 118 and 134) 1. Helium atoms do not combine to form He 2 molecules, What is the strongest attractive

More information

CLASSICAL CONCEPT REVIEW 8

CLASSICAL CONCEPT REVIEW 8 CLASSICAL CONCEPT REVIEW 8 Kinetic Theory Information concerning the initial motions of each of the atoms of macroscopic systems is not accessible, nor do we have the computational capability even with

More information

Composition of the Atmosphere. Outline Atmospheric Composition Nitrogen and Oxygen Lightning Homework

Composition of the Atmosphere. Outline Atmospheric Composition Nitrogen and Oxygen Lightning Homework Molecules of the Atmosphere The present atmosphere consists mainly of molecular nitrogen (N2) and molecular oxygen (O2) but it has dramatically changed in composition from the beginning of the solar system.

More information

Materials 10-mL graduated cylinder l or 2-L beaker, preferably tall-form Thermometer

Materials 10-mL graduated cylinder l or 2-L beaker, preferably tall-form Thermometer VAPOR PRESSURE OF WATER Introduction At very low temperatures (temperatures near the freezing point), the rate of evaporation of water (or any liquid) is negligible. But as its temperature increases, more

More information

Chem 1A Exam 2 Review Problems

Chem 1A Exam 2 Review Problems Chem 1A Exam 2 Review Problems 1. At 0.967 atm, the height of mercury in a barometer is 0.735 m. If the mercury were replaced with water, what height of water (in meters) would be supported at this pressure?

More information

HEAT UNIT 1.1 KINETIC THEORY OF GASES. 1.1.1 Introduction. 1.1.2 Postulates of Kinetic Theory of Gases

HEAT UNIT 1.1 KINETIC THEORY OF GASES. 1.1.1 Introduction. 1.1.2 Postulates of Kinetic Theory of Gases UNIT HEAT. KINETIC THEORY OF GASES.. Introduction Molecules have a diameter of the order of Å and the distance between them in a gas is 0 Å while the interaction distance in solids is very small. R. Clausius

More information

CHEM 105 HOUR EXAM III 28-OCT-99. = -163 kj/mole determine H f 0 for Ni(CO) 4 (g) = -260 kj/mole determine H f 0 for Cr(CO) 6 (g)

CHEM 105 HOUR EXAM III 28-OCT-99. = -163 kj/mole determine H f 0 for Ni(CO) 4 (g) = -260 kj/mole determine H f 0 for Cr(CO) 6 (g) CHEM 15 HOUR EXAM III 28-OCT-99 NAME (please print) 1. a. given: Ni (s) + 4 CO (g) = Ni(CO) 4 (g) H Rxn = -163 k/mole determine H f for Ni(CO) 4 (g) b. given: Cr (s) + 6 CO (g) = Cr(CO) 6 (g) H Rxn = -26

More information

2. The percent yield is the maximum amount of product that can be produced from the given amount of limiting reactant.

2. The percent yield is the maximum amount of product that can be produced from the given amount of limiting reactant. UNIT 6 stoichiometry practice test True/False Indicate whether the statement is true or false. moles F 1. The mole ratio is a comparison of how many grams of one substance are required to participate in

More information

Mole Calculations Multiple Choice Review PSI Chemistry

Mole Calculations Multiple Choice Review PSI Chemistry Mole Calculations Multiple Choice Review PSI Chemistry Name The Mole and Avogadro's Number 1)What is the SI unit for measurement of number of particles in a substance? A) kilogram B) ampere C) candela

More information

Gas Laws. vacuum. 760 mm. air pressure. mercury

Gas Laws. vacuum. 760 mm. air pressure. mercury Gas Laws Some chemical reactions take place in the gas phase and others produce products that are gases. We need a way to measure the quantity of compounds in a given volume of gas and relate that to moles.

More information

EXPERIMENT 13: THE IDEAL GAS LAW AND THE MOLECULAR WEIGHT OF GASES

EXPERIMENT 13: THE IDEAL GAS LAW AND THE MOLECULAR WEIGHT OF GASES Name Section EXPERIMENT 13: THE IDEAL GAS LAW AND THE MOLECULAR WEIGHT OF GASES PRE-LABORATORY QUESTIONS The following preparatory questions should be answered before coming to lab. They are intended to

More information

Pressure -Temperature Relationship in Gases. Evaluation copy. Figure 1. 125 ml Erlenmeyer flask. Vernier computer interface

Pressure -Temperature Relationship in Gases. Evaluation copy. Figure 1. 125 ml Erlenmeyer flask. Vernier computer interface Pressure -Temperature Relationship in Gases Computer 7 Gases are made up of molecules that are in constant motion and exert pressure when they collide with the walls of their container. The velocity and

More information

Name Date Class STATES OF MATTER. SECTION 13.1 THE NATURE OF GASES (pages 385 389)

Name Date Class STATES OF MATTER. SECTION 13.1 THE NATURE OF GASES (pages 385 389) 13 STATES OF MATTER SECTION 13.1 THE NATURE OF GASES (pages 385 389) This section introduces the kinetic theory and describes how it applies to gases. It defines gas pressure and explains how temperature

More information

Standard Free Energies of Formation at 298 K. Average Bond Dissociation Energies at 298 K

Standard Free Energies of Formation at 298 K. Average Bond Dissociation Energies at 298 K 1 Thermodynamics There always seems to be at least one free response question that involves thermodynamics. These types of question also show up in the multiple choice questions. G, S, and H. Know what

More information

DETERMINING THE MOLAR MASS OF CARBON DIOXIDE

DETERMINING THE MOLAR MASS OF CARBON DIOXIDE DETERMINING THE MOLAR MASS OF CARBON DIOXIDE PURPOSE: The goal of the experiment is to determine the molar mass of carbon dioxide and compare the experimentally determined value to the theoretical value.

More information

Chapter Outline. 3 Elements and Compounds. Elements and Atoms. Elements. Elements. Elements 9/4/2013

Chapter Outline. 3 Elements and Compounds. Elements and Atoms. Elements. Elements. Elements 9/4/2013 3 Elements and Compounds Chapter Outline 3.1 Elements A. Distribution of Elements Foundations of College Chemistry, 14 th Ed. Morris Hein and Susan Arena Copyright This reclining Buddha in Thailand is

More information

UNIVERSITY OF VICTORIA CHEMISTRY 102 Midterm Test 1 January 31, 2014 5-6 pm (60 minutes) DISPLAY YOUR STUDENT ID CARD ON THE TOP OF YOUR DESK NOW

UNIVERSITY OF VICTORIA CHEMISTRY 102 Midterm Test 1 January 31, 2014 5-6 pm (60 minutes) DISPLAY YOUR STUDENT ID CARD ON THE TOP OF YOUR DESK NOW Version B UNIVERSITY OF VICTORIA CHEMISTRY 102 Midterm Test 1 January 31, 2014 5-6 pm (60 minutes) Version B DISPLAY YOUR STUDENT ID CARD ON THE TOP OF YOUR DESK NOW Answer all multiple choice questions

More information

Unit 3: States of Matter Practice Exam

Unit 3: States of Matter Practice Exam Page 1 Unit 3: States of Matter Practice Exam Multiple Choice. Identify the choice that best completes the statement or answers the question. 1. Two gases with unequal masses are injected into opposite

More information

Mole Notes.notebook. October 29, 2014

Mole Notes.notebook. October 29, 2014 1 2 How do chemists count atoms/formula units/molecules? How do we go from the atomic scale to the scale of everyday measurements (macroscopic scale)? The gateway is the mole! But before we get to the

More information

Introduction to the Ideal Gas Law

Introduction to the Ideal Gas Law Course PHYSICS260 Assignment 5 Consider ten grams of nitrogen gas at an initial pressure of 6.0 atm and at room temperature. It undergoes an isobaric expansion resulting in a quadrupling of its volume.

More information

THE HUMIDITY/MOISTURE HANDBOOK

THE HUMIDITY/MOISTURE HANDBOOK THE HUMIDITY/MOISTURE HANDBOOK Table of Contents Introduction... 3 Relative Humidity... 3 Partial Pressure... 4 Saturation Pressure (Ps)... 5 Other Absolute Moisture Scales... 8 % Moisture by Volume (%M

More information

Molar Mass of Butane

Molar Mass of Butane Cautions Butane is toxic and flammable. No OPEN Flames should be used in this experiment. Purpose The purpose of this experiment is to determine the molar mass of butane using Dalton s Law of Partial Pressures

More information

CHAPTER 8: CHEMICAL COMPOSITION

CHAPTER 8: CHEMICAL COMPOSITION CHAPTER 8: CHEMICAL COMPOSITION Active Learning: 1-4, 6-8, 12, 18-25; End-of-Chapter Problems: 3-4, 9-82, 84-85, 87-92, 94-104, 107-109, 111, 113, 119, 125-126 8.2 ATOMIC MASSES: COUNTING ATOMS BY WEIGHING

More information

Periodic Table Questions

Periodic Table Questions Periodic Table Questions 1. The elements characterized as nonmetals are located in the periodic table at the (1) far left; (2) bottom; (3) center; (4) top right. 2. An element that is a liquid at STP is

More information

(1) The size of a gas particle is negligible as compared to the volume of the container in which the gas is placed.

(1) The size of a gas particle is negligible as compared to the volume of the container in which the gas is placed. Gas Laws and Kinetic Molecular Theory The Gas Laws are based on experiments, and they describe how a gas behaves under certain conditions. However, Gas Laws do not attempt to explain the behavior of gases.

More information

Kinetic Theory of Gases

Kinetic Theory of Gases Kinetic Theory of Gases Physics 1425 Lecture 31 Michael Fowler, UVa Bernoulli s Picture Daniel Bernoulli, in 1738, was the first to understand air pressure in terms of molecules he visualized them shooting

More information

IONISATION ENERGY CONTENTS

IONISATION ENERGY CONTENTS IONISATION ENERGY IONISATION ENERGY CONTENTS What is Ionisation Energy? Definition of t Ionisation Energy What affects Ionisation Energy? General variation across periods Variation down groups Variation

More information

Chemistry 151 Final Exam

Chemistry 151 Final Exam Chemistry 151 Final Exam Name: SSN: Exam Rules & Guidelines Show your work. No credit will be given for an answer unless your work is shown. Indicate your answer with a box or a circle. All paperwork must

More information

Chemistry B11 Chapter 4 Chemical reactions

Chemistry B11 Chapter 4 Chemical reactions Chemistry B11 Chapter 4 Chemical reactions Chemical reactions are classified into five groups: A + B AB Synthesis reactions (Combination) H + O H O AB A + B Decomposition reactions (Analysis) NaCl Na +Cl

More information

EXPERIMENT 9 Evaluation of the Universal Gas Constant, R

EXPERIMENT 9 Evaluation of the Universal Gas Constant, R Outcomes EXPERIMENT 9 Evaluation of the Universal Gas Constant, R After completing this experiment, the student should be able to: 1. Determine universal gas constant using reaction of an acid with a metal.

More information

Sample Exercise 8.1 Magnitudes of Lattice Energies

Sample Exercise 8.1 Magnitudes of Lattice Energies Sample Exercise 8.1 Magnitudes of Lattice Energies Without consulting Table 8.2, arrange the following ionic compounds in order of increasing lattice energy: NaF, CsI, and CaO. Analyze: From the formulas

More information

10.7 Kinetic Molecular Theory. 10.7 Kinetic Molecular Theory. Kinetic Molecular Theory. Kinetic Molecular Theory. Kinetic Molecular Theory

10.7 Kinetic Molecular Theory. 10.7 Kinetic Molecular Theory. Kinetic Molecular Theory. Kinetic Molecular Theory. Kinetic Molecular Theory The first scheduled quiz will be given next Tuesday during Lecture. It will last 5 minutes. Bring pencil, calculator, and your book. The coverage will be pp 364-44, i.e. Sections 0.0 through.4. 0.7 Theory

More information

Kinetic Theory & Ideal Gas

Kinetic Theory & Ideal Gas 1 of 6 Thermodynamics Summer 2006 Kinetic Theory & Ideal Gas The study of thermodynamics usually starts with the concepts of temperature and heat, and most people feel that the temperature of an object

More information

Name Date Class STOICHIOMETRY. SECTION 12.1 THE ARITHMETIC OF EQUATIONS (pages 353 358)

Name Date Class STOICHIOMETRY. SECTION 12.1 THE ARITHMETIC OF EQUATIONS (pages 353 358) Name Date Class 1 STOICHIOMETRY SECTION 1.1 THE ARITHMETIC OF EQUATIONS (pages 353 358) This section explains how to calculate the amount of reactants required or product formed in a nonchemical process.

More information

Other Stoich Calculations A. mole mass (mass mole) calculations. GIVEN mol A x CE mol B. PT g A CE mol A MOLE MASS :

Other Stoich Calculations A. mole mass (mass mole) calculations. GIVEN mol A x CE mol B. PT g A CE mol A MOLE MASS : Chem. I Notes Ch. 12, part 2 Using Moles NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. 1 MOLE = 6.02 x 10 23 representative particles (representative particles

More information

What s in a Mole? Molar Mass

What s in a Mole? Molar Mass LESSON 10 What s in a Mole? Molar Mass OVERVIEW Key Ideas Lesson Type Lab: Groups of 4 Chemists compare moles of substances rather than masses because moles are a way of counting atoms. When considering

More information

neutrons are present?

neutrons are present? AP Chem Summer Assignment Worksheet #1 Atomic Structure 1. a) For the ion 39 K +, state how many electrons, how many protons, and how many 19 neutrons are present? b) Which of these particles has the smallest

More information

1. The Kinetic Theory of Matter states that all matter is composed of atoms and molecules that are in a constant state of constant random motion

1. The Kinetic Theory of Matter states that all matter is composed of atoms and molecules that are in a constant state of constant random motion Physical Science Period: Name: ANSWER KEY Date: Practice Test for Unit 3: Ch. 3, and some of 15 and 16: Kinetic Theory of Matter, States of matter, and and thermodynamics, and gas laws. 1. The Kinetic

More information

Summer Holidays Questions

Summer Holidays Questions Summer Holidays Questions Chapter 1 1) Barium hydroxide reacts with hydrochloric acid. The initial concentration of the 1 st solution its 0.1M and the volume is 100ml. The initial concentration of the

More information

ATOMS. Multiple Choice Questions

ATOMS. Multiple Choice Questions Chapter 3 ATOMS AND MOLECULES Multiple Choice Questions 1. Which of the following correctly represents 360 g of water? (i) 2 moles of H 2 0 (ii) 20 moles of water (iii) 6.022 10 23 molecules of water (iv)

More information

Untitled Document. 1. Which of the following best describes an atom? 4. Which statement best describes the density of an atom s nucleus?

Untitled Document. 1. Which of the following best describes an atom? 4. Which statement best describes the density of an atom s nucleus? Name: Date: 1. Which of the following best describes an atom? A. protons and electrons grouped together in a random pattern B. protons and electrons grouped together in an alternating pattern C. a core

More information

CHEMISTRY II FINAL EXAM REVIEW

CHEMISTRY II FINAL EXAM REVIEW Name Period CHEMISTRY II FINAL EXAM REVIEW Final Exam: approximately 75 multiple choice questions Ch 12: Stoichiometry Ch 5 & 6: Electron Configurations & Periodic Properties Ch 7 & 8: Bonding Ch 14: Gas

More information