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All of the following are postulates of the kinetic molecular theory of gases EXCEPT:

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.

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All of the following are postulates of the kinetic molecular theory of gases EXCEPT:

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  1. 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. The attraction/repulsion between gas molecules is very weak or negligible. Gas molecules or atoms move in a straight line between collisions. All of the above are correct postulates.

  2. 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. The attraction/repulsion between gas molecules is very weak or negligible. Gas molecules or atoms move in a straight line between collisions. All of the above are correct postulates.

  3. Convert 580 mm Hg to atm: 11.2 0.763 atm 1.00 atm 5.80 atm 580 atm 4.41 x 105atm

  4. Convert 580 mm Hg to atm: 11.2 0.763 atm 1.00 atm 5.80 atm 580 atm 4.41 x 105atm

  5. Convert 35.5 psi to kPa. (Note: 1 atm = 14.7 psi and 1 atm = 101325 Pa.) 11.3 2.41 kPa 2.45 x 102kPa 5.29 x 102kPa 2.45 x 105kPa 5.29 x 105kPa

  6. Convert 35.5 psi to kPa. (Note: 1 atm = 14.7 psi and 1 atm = 101325 Pa.) 11.3 2.41 kPa 2.45 x 102kPa 5.29 x 102kPa 2.45 x 105kPa 5.29 x 105kPa

  7. 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.) 11.4 x 1 x 2 x 4 x 1/2 x 1/4

  8. 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.) 11.4 x 1 x 2 x 4 x 1/2 x 1/4

  9. 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.) 11.5 651 mL 1.65 x 103mL 0.151 mL 151 mL 500. mL

  10. 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.) 11.5 651 mL 1.65 x 103mL 0.151 mL 151 mL 500 mL

  11. What is absolute zero? 11.6 -273°F The freezing point of hydrogen The x-intercept of a straight-line graph of V versus 1/P The x-intercept of a straight-line graph of V versus T The temperature of deep outer space

  12. What is absolute zero? 11.6 -273°F The freezing point of hydrogen The x-intercept of a straight-line graph of V versus 1/P The x-intercept of a straight-line graph of V versus T The temperature of deep outer space

  13. 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.) 11.7 0.375 L 0.959 L 1.20 L 0.833 L 1.88 L

  14. 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.) 11.7 0.375 L 0.959 L 1.20 L 0.833 L 1.88 L

  15. 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? 11.8 100 mL 126 mL 180 mL 500 mL 680 mL

  16. 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? 11.8 100 mL 126 mL 180 mL 500 mL 680 mL

  17. What law is derived from the combined gas law under constant temperature and moles? 11.9 Avogadro’s Charles’s Dalton’s Gay-Lussac’s Boyle’s

  18. What law is derived from the combined gas law under constant temperature and moles? 11.9 Avogadro’s Charles’s Dalton’s Gay-Lussac’s Boyle’s

  19. 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? 11.10 1.00 mol 2.00 mol 3.00 mol 5.00 mol 10.0 mol

  20. 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? 11.10 1.00 mol 2.00 mol 3.00 mol 5.00 mol 10.0 mol

  21. 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? 11.11 37.8 psi 35.0 psi 0 psi 40.1 psi 29.9 psi

  22. 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? 11.11 37.8 psi 35.0 psi 0 psi 40.1 psi 29.9 psi

  23. 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). 11.12 1.32 mol 0.229 mol 0.174 mol 2.58 mol 5.73 mol

  24. 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). 11.12 1.32 mol 0.229 mol 0.174 mol 2.58 mol 5.73 mol

  25. 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). 11.13 0.0295 L 1.00 L 22.4 L 48.8 L 0.0446 L

  26. 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). 11.13 0.0295 L 1.00 L 22.4 L 48.8 L 0.0446 L

  27. 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). 11.14 H2 N2 F2 O2 Cl2

  28. 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). 11.14 H2 N2 F2 O2 Cl2

  29. A real gas can approach ideal behavior: 11.15 When both the pressure and temperature are high When the pressure is high and the temperature is low When both the pressure and temperature are low When the pressure is low and the temperature is high Real gases have ideal behavior no matter what the conditions are.

  30. A real gas can approach ideal behavior: 11.15 When both the pressure and temperature are high When the pressure is high and the temperature is low When both the pressure and temperature are low When the pressure is low and the temperature is high Real gases have ideal behavior no matter what the conditions are.

  31. Calculate the molar mass of a gas that has a density of 1.70 g/L at STP. 11.16 2.02 g/mol 4.00 g/mol 28.0 g/mol 32.0 g/mol 38.1 g/mol

  32. Calculate the molar mass of a gas that has a density of 1.70 g/L at STP. 11.16 2.02 g/mol 4.00 g/mol 28.0 g/mol 32.0 g/mol 38.1 g/mol

  33. 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. 11.17 5.00%, 70.3%, 24.7% 6.67%, 66.0%, 27.3% 0.500%, 49.5%, 50.0% 10.0%, 50.0%, 40.0% 1.50%, 75.5%, 23.0%

  34. 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. 11.17 5.00%, 70.3%, 24.7% 6.67%, 66.0%, 27.3% 0.500%, 49.5%, 50.0% 10.0%, 50.0%, 40.0% 1.50%, 75.5%, 23.0%

  35. 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. 11.18 9 mm Hg 69 mm Hg 626 mm Hg 635 mm Hg 644 mm Hg

  36. 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. 11.18 9 mm Hg 69 mm Hg 626 mm Hg 635 mm Hg 644 mm Hg

  37. 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). 11.19 0.225 L 36.3 L 201 L 403 L 0.0239 L

  38. 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). 11.19 0.225 L 36.3 L 201 L 403 L 0.0239 L

  39. How many grams of water are produced from the complete combustion of 15.8 L of propane (C3H8) gas at STP? 11.20 0.705 g 2.82 g 12.7 g 38.1 g 50.8 g

  40. How many grams of water are produced from the complete combustion of 15.8 L of propane (C3H8) gas at STP? 11.20 0.705 g 2.82 g 12.7 g 38.1 g 50.8 g

  41. Which of the following samples occupy the largest volume at STP? Note: R = 0.0821 L·atm/(mol·K). 11.21 1.00 mol O2 48.0 g O2 0.500 mol He 4.008 g H2 6.02 x 1023molecules of N2

  42. Which of the following samples occupy the largest volume at STP? Note: R = 0.0821 L·atm/(mol·K). 11.21 1.00 mol O2 48.0 g O2 0.500 mol He 4.008 g H2 6.02 x 1023molecules of N2

  43. For an ideal gas, which two variables are INVERSELY proportional to each other, assuming all the other conditions remain constant? 11.22 V and P T and P V and T V and n None of the above

  44. For an ideal gas, which two variables are INVERSELY proportional to each other, assuming all the other conditions remain constant? 11.22 V and P T and P V and T V and n None of the above

  45. 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.) 11.23 Increases by a factor of 75 Halves Doubles Remains the same None of the above

  46. 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.) 11.23 Increases by a factor of 75 Halves Doubles Remains the same None of the above

  47. Which of the following gas laws relate volume and temperature? 11.24 Avogadro’s law Boyle’s law Charles’s law Gay-Lussac’s law Dalton’s Law

  48. Which of the following gas laws relate volume and temperature? 11.24 Avogadro’s law Boyle’s law Charles’s law Gay-Lussac’s law Dalton’s Law

  49. What is the SI unit for pressure? 11.25 Pa atm mm Hg torr psi

  50. What is the SI unit for pressure? 11.25 Pa atm mm Hg torr psi

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