2. THIS IS
Chapter 13 Jeopardy

3. With
Your
Host...
Ms. Siam

4. Jeopardy
Gas Stoichiometry
Matching/
Vocab
Boyles Law
Charles Law
Ideal Gas Law
Other Gas Laws
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5. A gas occupies a volume of 202 mL at a pressure of 505 torr
A gas occupies a volume of 202 mL at a pressure of 505 torr. To what pressure must the gas be subjected in order to change the volume to 65.0 mL? Assume constant temperature.
A 100

6. 1570 torr; 2.07 atm
A 100

7. A sample of helium gas occupies 2. 65 L at 1. 20 atm
A sample of helium gas occupies 2.65 L at 1.20 atm. What pressure would this sample of gas exert in a 1.50-L container at the same temperature?
A 200

8. 2.12 atm
A 200

9. Define Boyle’s Law
A 300

10. At constant temperature, the volume of a given amount of gas is inversely proportinal to its pressure
A 300

11. A gas has a volume of 5. 0 L at a certain pressure
A gas has a volume of 5.0 L at a certain pressure. How must the pressure be changed to double the volume of the gas at constant temperature?
A 400

12. The pressure must be halved

13. The pressure of a sample of gas is 500. mm Hg and the volume is 30.0 L. If the volume is changed to 50.0 L, what is the new pressure?
A 500

14. 833 mm Hg
A 500

15. A balloon has a volume of 1. 20 L at 24. 0°C
A balloon has a volume of 1.20 L at 24.0°C. The balloon is heated to 48.0°C. Calculate the new volume of the balloon.
B 100

16. 1.30 L
B 100

17. A gas sample is held at constant pressure. The gas occupies 3
A gas sample is held at constant pressure. The gas occupies 3.62 L of volume when the temperature is 21.6°C. Determine the temperature at which the volume of the gas is 3.45 L.
B 200

18. 281 K
B 200

19. Define Charles’s Law
B 300

20. At constant pressure, the volume of a given amount of gas is directly proportional to its kelvin temperature
B 300

21. A balloon has a volume of 1. 20 L at 24. 0°C
A balloon has a volume of 1.20 L at 24.0°C. The balloon is heated to 48.0°C. Calculate the new volume of the balloon.
B 400

22. 1.30 L
B 400

23. A sample of gas has a volume of 50. 0 L at a temperature of 300. K
A sample of gas has a volume of 50.0 L at a temperature of 300. K. What temperature would be needed for this sample to have a volume of 60.0 L if its pressure remains constant?
B 500

24. 87 °C
B 500

25. A sample of an ideal gas containing 0
A sample of an ideal gas containing mol is collected at 742 torr pressure and 31°C. Calculate the volume.
C 100

26. 24.4 L
C 100

27. A 36.0-g sample of acetylene, C2H2(g), at STP is subject to a new temperature and pressure of 35°C and 805 mm Hg. Calculate the volume of the acetylene under these new conditions.
C 200

28. 33.0 L
C 200

29. What volume will 28.0 g of N2 occupy at STP?

30. 22.4 L
C 300

31. DAILY DOUBLE
DAILY DOUBLE
Place A Wager
C 400

32. What volume is occupied by 19. 6 g of methane, CH4, at 27°C and 1
What volume is occupied by 19.6 g of methane, CH4, at 27°C and 1.59 atm?
C 400

33. 18.9 L
C 400

34. A 4.40-g piece of solid CO2 (dry ice) is allowed to vaporize (change to CO2(g)) in a balloon. The final volume of the balloon is 1.00 L at 300. K. What is the pressure of the gas?
C 500

35. 2.46 atm
C 500

36. C2H4 reacts with O2 according to the following equation:
C2H4(g) + 3O2(g) → 2CO2(g) + 2H2O(g)
What volume of oxygen at STP is needed to react with 1.50 mol of C2H4?
D 100

37. 101 L
D 100

38. How many liters of HCl(g) measured at STP can be produced from 4
How many liters of HCl(g) measured at STP can be produced from 4.00 g of Cl2 and excess H2 according to the following equation:
H2(g) + Cl2(g) → 2HCl(g)
D 200

39. 2.53 L
D 200

40. How many moles of O2(g) are needed to react completely with 52
How many moles of O2(g) are needed to react completely with 52.0 L of CH4(g) at STP to produce CO2(g) and H2O(g) according to the following reaction:
CH4(g) + 2O2 → CO2(g) + 2H2O(g)
D 300

41. 4.64 moles
D 300

42. What volume of carbon dioxide will be produced from the combustion of 4.50 moles of propane (C3H8) at STP?
D 400

43. 302 L
D 400

44. Calcium carbonate decomposes when heated to form calcium oxide and carbon dioxide. What volume of carbon dioxide can be produced from 37.0 g of calcium carbonate at a temperature of 25 °C and a pressure of 1.15 atm?
D 500

45. 7.87 L CO2
D 500

46. A helium balloon has a volume of 2.30 L at 23.5°C and a pressure of 1.00 atm at sea level. The balloon is released and floats upward. At a certain height the atmospheric pressure is atm and the temperature is 12.0°C. Calculate the volume of the balloon.
E 100

47. 2.73 L
E 100

48. independent of each other b. directly proportional
If temperature and pressure are held constant, the volume and number of moles of a gas are
independent of each other
b. directly proportional
c. inversely proportional
d. equal
E 200

49. b. directly proportional

50. A gas originally occupying 10. 1 L at 0
A gas originally occupying 10.1 L at atm and 25°C is changed to 12.2 L at 625 torr. What is the new temperature in °C?
E 300

51. 47 °C
E 300

52. A mole of a gas at STP has a volume of 22. 4 L
A mole of a gas at STP has a volume of 22.4 L. If the volume increases to 29.1 L and the pressure is changed to 813 torr, calculate the new temperature.
E 400

53. 379 K
E 400

54. 3. 50 g of CO2 and 11. 6 g of O2 are placed in a 3
3.50 g of CO2 and 11.6 g of O2 are placed in a 3.00 L container at 273 K. What will the total pressure in the container be?
E 500

55. 3.30 atm
E 500

56. absolute zero
F 100

57. Temperature at which a gas theoretically occupies zero volume
F 100

58. Universal gas constant
F 200

59. L·atm/(mol·K)
F 200

60. Define Avogadro’s Law
F 300

61. At constant temperature and pressure, the volume of a gas is directly proportional to the number of moles of gas
F 300

62. Define Dalton’s law of partial pressure

63. The total pressure of a mixture of gases is the sum of the pressures that each gas would exert if alone in the container
F 400

64. What is the molar volume of ideal gas at STP

65. 22.4 liters
F 500

66. The Final Jeopardy Category is:
Dalton’s Law of Partial Pressures
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67. Click on screen to continue
Consider the following: you have 2 liters of neon gas at a pressure of 2 atmospheres, 2 liters of carbon dioxide gas at a pressure of 3 atmospheres, and 2 liters of nitrogen gas at a pressure of 4 atmospheres. All three samples are at room temperature.
If you transfer all 3 gases to the same rigid 2 liter container, what is the pressure exerted by the nitrogen in the final mixture? What is the total pressure exerted by the gas mixture?
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68. Click on screen to continue
4 atm
9 atm
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