all of the following are postulates of the kinetic molecular theory of gases except:
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All of the following are postulates of the kinetic molecular theory of gases EXCEPT:. 11.1. The volume occupied by a gas is mostly empty space. The average kinetic energy of the gas particles is proportional to the temperature in Celsius. - PowerPoint PPT PresentationTRANSCRIPT
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1. The volume occupied by a gas is mostly empty space.2. The average kinetic energy of the gas particles is
proportional to the temperature in Celsius.3. The attraction/repulsion between gas molecules is very
weak or negligible.4. Gas molecules or atoms move in a straight line between
collisions.5. All of the above are correct postulates.
11.1 All of the following are postulates of the kinetic molecular theory of gases EXCEPT:
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1. The volume occupied by a gas is mostly empty space.2. The average kinetic energy of the gas particles is
proportional to the temperature in Celsius.3. The attraction/repulsion between gas molecules is very
weak or negligible.4. Gas molecules or atoms move in a straight line between
collisions.5. All of the above are correct postulates.
11.1 All of the following are postulates of the kinetic molecular theory of gases EXCEPT:
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1. 0.763 atm2. 1.00 atm3. 5.80 atm4. 580 atm5. 4.41 x 105 atm
11.2 Convert 580 mm Hg to atm:
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1. 0.763 atm2. 1.00 atm3. 5.80 atm4. 580 atm5. 4.41 x 105 atm
11.2 Convert 580 mm Hg to atm:
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1. 2.41 kPa2. 2.45 x 102 kPa3. 5.29 x 102 kPa4. 2.45 x 105 kPa5. 5.29 x 105 kPa
11.3 Convert 35.5 psi to kPa. (Note: 1 atm = 14.7 psi and 1 atm = 101325 Pa.)
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1. 2.41 kPa2. 2.45 x 102 kPa3. 5.29 x 102 kPa4. 2.45 x 105 kPa5. 5.29 x 105 kPa
11.3 Convert 35.5 psi to kPa. (Note: 1 atm = 14.7 psi and 1 atm = 101325 Pa.)
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1. x 12. x 23. x 44. x 1/25. x 1/4
11.4 A gas has a volume of 1.0 L at 1 atm. By what factor must the pressure change in order to halve the volume of the gas? (Assume the temperature is constant.)
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1. x 12. x 23. x 44. x 1/25. x 1/4
11.4 A gas has a volume of 1.0 L at 1 atm. By what factor must the pressure change in order to halve the volume of the gas? (Assume the temperature is constant.)
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1. 651 mL2. 1.65 x 103 mL3. 0.151 mL4. 151 mL5. 500. mL
11.5 A bottle with 500 mL of a liquid is sealed on top of Mt. Everest (P = 230 torr). What is the volume of the liquid when the bottle is moved to sea level? (Assume the temperature is kept constant.)
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1. 651 mL2. 1.65 x 103 mL3. 0.151 mL4. 151 mL5. 500 mL
11.5 A bottle with 500 mL of a liquid is sealed on top of Mt. Everest (P = 230 torr). What is the volume of the liquid when the bottle is moved to sea level? (Assume the temperature is kept constant.)
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1. -273°F2. The freezing point of hydrogen3. The x-intercept of a straight-line graph of V versus 1/P4. The x-intercept of a straight-line graph of V versus T5. The temperature of deep outer space
11.6 What is absolute zero?
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1. -273°F2. The freezing point of hydrogen3. The x-intercept of a straight-line graph of V versus 1/P4. The x-intercept of a straight-line graph of V versus T5. The temperature of deep outer space
11.6 What is absolute zero?
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1. 0.375 L2. 0.959 L3. 1.20 L4. 0.833 L5. 1.88 L
11.7 A flexible container contains 1.50 L of gas at 25 °C. What is the new volume when the container is heated to 100 °C? (Assume the pressure is constant.)
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1. 0.375 L2. 0.959 L3. 1.20 L4. 0.833 L5. 1.88 L
11.7 A flexible container contains 1.50 L of gas at 25 °C. What is the new volume when the container is heated to 100 °C? (Assume the pressure is constant.)
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1. 100 mL2. 126 mL3. 180 mL4. 500 mL5. 680 mL
11.8 A bottle with 500 mL of a liquid is sealed on top of Mt. Everest (230 torr) at a temperature of -20 °C. What is the approximate volume of the liquid when the bottle is moved to sea level at a temperature of 30.0 °C?
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1. 100 mL2. 126 mL3. 180 mL4. 500 mL5. 680 mL
11.8 A bottle with 500 mL of a liquid is sealed on top of Mt. Everest (230 torr) at a temperature of -20 °C. What is the approximate volume of the liquid when the bottle is moved to sea level at a temperature of 30.0 °C?
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1. Avogadro’s 2. Charles’s3. Dalton’s 4. Gay-Lussac’s5. Boyle’s
11.9 What law is derived from the combined gas law under constant temperature and moles?
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1. Avogadro’s 2. Charles’s3. Dalton’s 4. Gay-Lussac’s5. Boyle’s
11.9 What law is derived from the combined gas law under constant temperature and moles?
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1. 1.00 mol2. 2.00 mol3. 3.00 mol4. 5.00 mol5. 10.0 mol
11.10 A container with 1.00 mol of gas is expanded from 5.00 L to 10.0 L by adding more gas. The temperature and pressure are kept constant. How many moles of gas are present after the expansion?
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1. 1.00 mol2. 2.00 mol3. 3.00 mol4. 5.00 mol5. 10.0 mol
11.10 A container with 1.00 mol of gas is expanded from 5.00 L to 10.0 L by adding more gas. The temperature and pressure are kept constant. How many moles of gas are present after the expansion?
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1. 37.8 psi2. 35.0 psi3. 0 psi4. 40.1 psi5. 29.9 psi
11.11 A set of car tires contain a volume of 45.5 L of air at 35.0 psi and 0 °C. When the car is driven, the temperature of the tires increases to 40 °C. What is the pressure (in psi) of each tire assuming constant volume?
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1. 37.8 psi2. 35.0 psi3. 0 psi4. 40.1 psi5. 29.9 psi
11.11 A set of car tires contain a volume of 45.5 L of air at 35.0 psi and 0 °C. When the car is driven, the temperature of the tires increases to 40 °C. What is the pressure (in psi) of each tire assuming constant volume?
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1. 1.32 mol2. 0.229 mol3. 0.174 mol4. 2.58 mol5. 5.73 mol
11.12 How many moles of an ideal gas are in a container with a volume of 5.50 L at 580 mm Hg and 20 °C?Note: R = 0.0821 L·atm/(mol·K).
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1. 1.32 mol2. 0.229 mol3. 0.174 mol4. 2.58 mol5. 5.73 mol
11.12 How many moles of an ideal gas are in a container with a volume of 5.50 L at 580 mm Hg and 20 °C?Note: R = 0.0821 L·atm/(mol·K).
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1. 0.0295 L2. 1.00 L3. 22.4 L4. 48.8 L5. 0.0446 L
11.13 What is the volume occupied by 28.0 g of nitrogen gas at 1.00 atm and 0 °C? Note: R = 0.0821 L·atm/(mol·K).
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1. 0.0295 L2. 1.00 L3. 22.4 L4. 48.8 L5. 0.0446 L
11.13 What is the volume occupied by 28.0 g of nitrogen gas at 1.00 atm and 0 °C? Note: R = 0.0821 L·atm/(mol·K).
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1. H2
2. N2
3. F2
4. O2
5. Cl2
11.14 A 4.17-g sample of particular ideal diatomic gas at 38 °C has a volume of 1.50 L at 1.00 atm. Identify the gas? Note: R = 0.0821 L·atm/(mol·K).
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1. H2
2. N2
3. F2
4. O2
5. Cl2
11.14 A 4.17-g sample of particular ideal diatomic gas at 38 °C has a volume of 1.50 L at 1.00 atm. Identify the gas? Note: R = 0.0821 L·atm/(mol·K).
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1. When both the pressure and temperature are high2. When the pressure is high and the temperature is low3. When both the pressure and temperature are low4. When the pressure is low and the temperature is high5. Real gases have ideal behavior no matter what the
conditions are.
11.15 A real gas can approach ideal behavior:
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1. When both the pressure and temperature are high2. When the pressure is high and the temperature is low3. When both the pressure and temperature are low4. When the pressure is low and the temperature is high5. Real gases have ideal behavior no matter what the
conditions are.
11.15 A real gas can approach ideal behavior:
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1. 2.02 g/mol2. 4.00 g/mol3. 28.0 g/mol4. 32.0 g/mol5. 38.1 g/mol
11.16 Calculate the molar mass of a gas that has a density of 1.70 g/L at STP.
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1. 2.02 g/mol2. 4.00 g/mol3. 28.0 g/mol4. 32.0 g/mol5. 38.1 g/mol
11.16 Calculate the molar mass of a gas that has a density of 1.70 g/L at STP.
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1. 5.00%, 70.3%, 24.7%2. 6.67%, 66.0%, 27.3% 3. 0.500%, 49.5%, 50.0%4. 10.0%, 50.0%, 40.0%5. 1.50%, 75.5%, 23.0%
11.17 The partial pressures in a mixture of CO2, N2, and O2 in a sample of gas are 50.0 atm, 495 atm, and 205 atm, respectively. Calculate the mole percentage of each gas.
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1. 5.00%, 70.3%, 24.7%2. 6.67%, 66.0%, 27.3% 3. 0.500%, 49.5%, 50.0%4. 10.0%, 50.0%, 40.0%5. 1.50%, 75.5%, 23.0%
11.17 The partial pressures in a mixture of CO2, N2, and O2 in a sample of gas are 50.0 atm, 495 atm, and 205 atm, respectively. Calculate the mole percentage of each gas.
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1. 9 mm Hg2. 69 mm Hg3. 626 mm Hg4. 635 mm Hg5. 644 mm Hg
11.18 A sample of hydrogen gas is collected over water at a pressure of 635 mm Hg at 10.0 °C. Calculate partial pressure of the hydrogen. The vapor pressure over water at 10.0 °C is 9.2 mm Hg.
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1. 9 mm Hg2. 69 mm Hg3. 626 mm Hg4. 635 mm Hg5. 644 mm Hg
11.18 A sample of hydrogen gas is collected over water at a pressure of 635 mm Hg at 10.0 °C. Calculate partial pressure of the hydrogen. The vapor pressure over water at 10.0 °C is 9.2 mm Hg.
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1. 0.225 L2. 36.3 L3. 201 L4. 403 L5. 0.0239 L
11.19 How many liters of dry oxygen gas are produced by the complete electrolysis of 225 mL of water? The oxygen gas is collected at 580 torr and 27 °C. The density of water at 27 °C is 1.00 g/mL. Note: R = 0.0821 L·atm/(mol·K).
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1. 0.225 L2. 36.3 L3. 201 L4. 403 L5. 0.0239 L
11.19 How many liters of dry oxygen gas are produced by the complete electrolysis of 225 mL of water? The oxygen gas is collected at 580 torr and 27 °C. The density of water at 27 °C is 1.00 g/mL. Note: R = 0.0821 L·atm/(mol·K).
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1. 0.705 g2. 2.82 g3. 12.7 g4. 38.1 g5. 50.8 g
11.20 How many grams of water are produced from the complete combustion of 15.8 L of propane (C3H8) gas at STP?
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1. 0.705 g2. 2.82 g3. 12.7 g4. 38.1 g5. 50.8 g
11.20 How many grams of water are produced from the complete combustion of 15.8 L of propane (C3H8) gas at STP?
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1. 1.00 mol O2
2. 48.0 g O2
3. 0.500 mol He4. 4.008 g H2
5. 6.02 x 1023 molecules of N2
11.21 Which of the following samples occupy the largest volume at STP? Note: R = 0.0821 L·atm/(mol·K).
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1. 1.00 mol O2
2. 48.0 g O2
3. 0.500 mol He4. 4.008 g H2
5. 6.02 x 1023 molecules of N2
11.21 Which of the following samples occupy the largest volume at STP? Note: R = 0.0821 L·atm/(mol·K).
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1. V and P2. T and P3. V and T4. V and n5. None of the above
11.22 For an ideal gas, which two variables are INVERSELY proportional to each other, assuming all the other conditions remain constant?
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1. V and P2. T and P3. V and T4. V and n5. None of the above
11.22 For an ideal gas, which two variables are INVERSELY proportional to each other, assuming all the other conditions remain constant?
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1. Increases by a factor of 752. Halves3. Doubles4. Remains the same5. None of the above
11.23 When the Celsius temperature of a gas sample is doubled from 75 °C to 150 °C, the volume of the gas: (Assume the pressure is constant.)
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1. Increases by a factor of 752. Halves3. Doubles4. Remains the same5. None of the above
11.23 When the Celsius temperature of a gas sample is doubled from 75 °C to 150 °C, the volume of the gas: (Assume the pressure is constant.)
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1. Avogadro’s law2. Boyle’s law3. Charles’s law4. Gay-Lussac’s law5. Dalton’s Law
11.24 Which of the following gas laws relate volume and temperature?
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1. Avogadro’s law2. Boyle’s law3. Charles’s law4. Gay-Lussac’s law5. Dalton’s Law
11.24 Which of the following gas laws relate volume and temperature?
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1. Pa2. atm3. mm Hg4. torr5. psi
11.25 What is the SI unit for pressure?
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1. Pa2. atm3. mm Hg4. torr5. psi
11.25 What is the SI unit for pressure?