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: 0.763 atm 1.00 atm 5.80 atm 580 atm
11.2
atm
atm
atm
atm
4.41 x 105 atm

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

5. Convert 35. 5 psi to kPa. (Note: 1 atm = 14
Convert 35.5 psi to kPa. (Note: 1 atm = 14.7 psi and 1 atm = Pa.)
11.3
kPa
2.45 x 102 kPa
5.29 x 102 kPa
2.45 x 105 kPa
5.29 x 105 kPa

6. Convert 35. 5 psi to kPa. (Note: 1 atm = 14
Convert 35.5 psi to kPa. (Note: 1 atm = 14.7 psi and 1 atm = Pa.)
11.3
kPa
2.45 x 102 kPa
5.29 x 102 kPa
2.45 x 105 kPa
5.29 x 105 kPa

7. A gas has a volume of 1. 0 L at 1 atm
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
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
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 mL
1.65 x 103 mL mL mL mL

10. A bottle with 500 mL of a liquid is sealed on top of Mt
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 mL
1.65 x 103 mL mL mL mL

11. What is absolute zero? -273°F The freezing point of hydrogen
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? -273°F The freezing point of hydrogen
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
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 L
0.833 L L

14. A flexible container contains 1. 50 L of gas at 25 °C
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 L
0.833 L L

15. A bottle with 500 mL of a liquid is sealed on top of Mt
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
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
A container with 1.00 mol of gas is expanded from 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
A container with 1.00 mol of gas is expanded from 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
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
psi
40.1 psi
29.9 psi

22. A set of car tires contain a volume of 45. 5 L of air at 35
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
psi
40.1 psi
29.9 psi

23. 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 = L·atm/(mol·K).
mol
0.229 mol
0.174 mol
mol
mol

24. 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 = L·atm/(mol·K).
mol
0.229 mol
0.174 mol
mol
mol

25. What is the volume occupied by 28. 0 g of nitrogen gas at 1
What is the volume occupied by 28.0 g of nitrogen gas at 1.00 atm and 0 °C? Note: R = L·atm/(mol·K).
11.13 L L L L L

26. What is the volume occupied by 28. 0 g of nitrogen gas at 1
What is the volume occupied by 28.0 g of nitrogen gas at 1.00 atm and 0 °C? Note: R = L·atm/(mol·K).
11.13 L L L L 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 = 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 = 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
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
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 = L·atm/(mol·K).
11.19 L L L L 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 = L·atm/(mol·K).
11.19 L L L L 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 g g g 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 g g g g

41. Which of the following samples occupy the largest volume at STP
Which of the following samples occupy the largest volume at STP? Note: R = 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 1023 molecules of N2

42. Which of the following samples occupy the largest volume at STP
Which of the following samples occupy the largest volume at STP? Note: R = 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 1023 molecules 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