Gas Laws and Pressure Units

Explanation and application of gas laws, pressure units, and temperature-volume relationships through examples and images. Topics covered include Boyle's law, volume-temperature relationships, and identifying pressure units. Learn how to calculate and interpret pressure and volume changes in gas systems.

• Gas Laws
• Pressure Units
• Temperature
• Volume Relationship
• Boyles Law

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2. 1 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 2 3 4 5 6 7 8

4. Answer: B 80 mm Hg RETURN The mixture is 10% oxygen; 800 mm Hg x 0.10 = 80 mm Hg

6. Volume and Temperature are proportional. As one goes up, so does the other. RETURN

7. Which of the following is not a unit of pressure? A Newton B mm Hg C atmosphere D Pascal

8. Which of the following is not a unit of pressure? A Newton RETURN

9. The volume of a balloon is 20 L when the temperature is 20 degree celsius. If the temperature is raised to 50 degrees celsius, what is the new volume? A) 18.1 L B) 20 L C) 22.0 L D) 50 L

10. The volume of a balloon is 20 L when the temperature is 20 degree celsius. If the temperature is raised to 50 degrees celsius, what is the new volume? Answer: C) 22.0 L Remember, the temperature must be converted to Kelvin first (20 + 273) = 293 K, (50 + 273) = 323 K (20 L/293 K) = ( ?? L/323 K) ?? = 22.0 L RETURN

11. Free Point

12. Free Point RETURN

13. According to Boyles law, the relationship between the pressure and volume of a gas at constant temperature is a. numerically equivalent b. inversely proportional c. positively correlated d. totally unrelated

14. According to Boyles law, the relationship between the pressure and volume of a gas at constant temperature is Answer: b. inversely proportional RETURN

15. A balloon is filled with 3.8 L of helium gas at 22.4 atm pressure. If the pressure is lowered to 1.0 atm, what is the new volume? a. 0.17 L b. 0.26 L c. 72 L d. 85 L

16. A balloon is filled with 3.8 L of helium gas at 22.4 atm pressure. If the pressure is lowered to 1.0 atm, what is the new volume? Answer: d. 85 L When we eliminate temperature from the combined gas law, we get P1V1 = P2V2 (22.4 atm)(3.8 L) = (1.0 atm)P2 P2 = 85 L RETURN

17. What is standard temperature and pressure? A o K and 1 KPa B 0 C and 1 kPa C o K and 1 atm D 0 C and 1 atm

18. What is standard temperature and pressure? Answer: D 0 C and 1 atm RETURN

19. Whose law states that temperature and volume are proportional to one another? A Avogadro B Charles C Boyle D Dalton

20. Whose law states that temperature and volume are proportional to one another? Answer: B Charles RETURN

22. Answer: G 0.40 atm If 80% of the mixture is nitrogen, then 20% is oxygen. 0.20 x 2.0 atm = 0.40 atm RETURN

24. Answer: H 75.00 mL When temperature is excluded from the Combined Gas Law, you end up with P1V1 = P2V2. (100 mL)(600 mm Hg) = (800 mm Hg)(V2) V2 = 75.00 mL RETURN

25. A gas cylinder is filled with 2.00 moles of oxygen gas at 300.0 K. The piston is compressed to yield a pressure of 400.0 kPa. What is the volume inside the cylinder? a. 6.25 dm3 b. 12.47 dm3 c. 24.9 dm3 d. 31.5 dm3

26. A gas cylinder is filled with 2.00 moles of oxygen gas at 300.0 K. The piston is compressed to yield a pressure of 400.0 kPa. What is the volume inside the cylinder? Answer: b. 12.47 dm3 Use the ideal gas law, PV = nRT (400 kPa)V = (2.0 moles)(8.31)(300 K) V = 12.47 dm3 RETURN

27. The SI unit of pressure is: a. liters b. atmospheres c. newtons d. pascals

28. The SI unit of pressure is: Answer: d. pascals RETURN

29. Which of the properties below is not characteristic of gases? a. the ability to flow easily b. very high density c. compressibility d. takes the shape of its container

30. Which of the properties below is not characteristic of gases? Answer: b. very high density Gases have a low density RETURN

31. A can contains a gas with a volume of 100 L at 0 C. What is the volume of the can if it is heated to 50 C? a. 200 L b. 150 L c. 118 L d. 93 L

32. A can contains a gas with a volume of 100 L at 0 C. What is the volume of the can if it is heated to 50 C? Answer: c. 118 L When pressure is left out of the combined gas law, V1/T1 = V2/T2 The temperatures must beconverted to Kelvin first, so T1=273 K and T2 = 323 K (100 L/273 K) = (V2/323 K) V2 = 118 L RETURN

33. A sample of nitrogen occupies 10.0 liters at 25 C and 98.7 kPa. What would be the volume at 20 C and 102.7 kPa? A 7.87 L B 9.45 L C 10.2 L D 10.6 L

34. A sample of nitrogen occupies 10.0 liters at 25 C and 98.7 kPa. What would be the volume at 20 C and 102.7 kPa? Answer: B 9.45 L Use thecombinedgas law, plugintothe formula, and makesure thetemperaturesare in Kelvin! RETURN

35. A gas cylinder with a volume of 3.00 dm3 contains 8.00 moles of oxygen gas at a temperature of 50.0 K. What is the pressure inside the cylinder? A 504 kPa B 1110 kPa C 2220 kP D 3320 kPa

36. A gas cylinder with a volume of 3.00 dm3 contains 8.00 moles of oxygen gas at a temperature of 50.0 K. What is the pressure inside the cylinder? Answer: B 1110 kPa Use theideal gas law, PV = nRT (3.00)P = (8.00)(8.31)(50.0) P = 1110 kPa RETURN

37. A balloon contains 8.0 liters of gas at 100 K. What is the balloon s volume at 200K? A 4.0 L B 8.0 L C 16.0 L D 24.0 L

38. A balloon contains 8.0 liters of gas at 100 K. What is the balloon s volume at 200K? Answer: C 16.0 L Using the combined gas law without temperature, V1/T1 = V2/T2 8.0/100 = V2/200 V2 = 16.0 L RETURN

39. When pressure, volume, and temperature are known, the ideal gas law can be used to calculate: a. the chemical formula b. the ideal gas constant c. compressibility d. the number of moles

40. When pressure, volume, and temperature are known, the ideal gas law can be used to calculate: Answer: d. the number of moles Ideal gas law includes temperature, pressure, volume and moles, PV = nRT RETURN

41. How many moles of Hydrogen gas are in a 20 L tank pressurized to 1000 kPa at 300K? A 4.0 moles B 8.0 moles C 16.0 moles D 32.0 moles

42. How many moles of Hydrogen gas are in a 20 L tank pressurized to 1000 kPa at 300K? Answer: B 8.0 moles P=1000., V=20. L, n=? T=300K (1000)(20) = n(8.31)(300) so n = 8.0 moles Hydrogen RETURN

43. What is the volume of 1 mole of gas at STP? A 1.0 L B 22.4 L C 100 L D 6.022 x 1023 L

44. What is the volume of 1 mole of gas at STP? Answer: B 22.4 L RETURN

45. A 15 liter tank contains 2.0 moles of nitrogen gas at 27 C. What is the pressure of nitrogen inside the tank? (R = 8.314) A 29.9 kPa B 101.3 kPa C 332.4 kPa D 664.8 kPa

46. A 15 liter tank contains 2.0 moles of nitrogen gas at 27 C. What is the pressure of nitrogen inside the tank? Answer: C 332.4 kPa P=?, V=15 L, n=2.0, T=300K (remember to convert) P(15)=2.0(8.31)(300) so P = 332.4 kPa RETURN

48. Answer: G a gas-filled balloon expands when it is heated None of the other choices mention a change in temperature ( heated ) or volume ( expands ) RETURN

49. According to the kinetic-molecular theory, gas particles: a. are in constant motion b. have different shapes c. have different colors d. are in contact with each other

50. According to the kinetic-molecular theory, gas particles: Answer: a. are in constant motion RETURN

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