1. Gases Dr. Ron Rusay Spring 2008 © Copyright 2008 R.J. Rusay

2. Gases  Uniformly fill any container.  Exert pressure on its surroundings.  Mix completely with other gases

3. Gases: Pressure, Mass, Volume, Temperature

4. Pressure  is equal to force/unit area  SI units = Newton/meter 2 = 1 Pascal (Pa)  1 standard atmosphere = 101,325 Pa  1 standard atmosphere = 1 atm = 760 mm Hg = 760 torr

5. QUESTION Four bicycle tires are inflated to the following pressures. Which one has the highest pressure? Tire A 3.42 atm; Tire B 48 lbs/sq in; Tire C 305 kPa; Tire D 1520 mmHg. (Recall; 1.00 atm = 760 mmHg = 14.7 lb/sq in = 101.3 kPa) 1.Tire A 2.Tire B 3.Tire C 4.Tire D

6. ANSWER Choice 1 Even though it has the smallest number, it represents the highest pressure of the four. When all four are changed to a common label (use conversion factors found on page 181 and dimensional analysis) 3.42 atm is a higher pressure than the others. Section 5.1: Pressure

8. Toricellian Barometer

10. Pressure & Volume Boyle’s Law *

11. Boyle’s Law *  Pressure  Volume = Constant (T = constant)  P 1 V 1 = P 2 V 2 (T = constant)  V  1/ P (T = constant)  ( * Holds precisely only at very low pressures.)

12. Changing Volume A) 4.0 L B) 0.57 L C) 5.7 L D) 0.4 L

13. Changing Volume A) 4.0 L B) 0.57 L C) 5.7 L D) 0.4 L

14. Pressure vs. Volume 

15. Definition: A gas that strictly obeys Boyle’s Law is called an ideal gas. Ideal Gases Real vs. “Ideal”

16. Temperature & Volume

18. Charles’s Law  The volume of a gas is directly proportional to temperature, and extrapolates to zero at zero Kelvin.  V =  T (P = constant)  = a proportionality constant

19. Temperature and Volume (@ constant P)

20. Charles’s Law

21. Pressure vs. Temperature (@ constant V) Changing Volume

22. The Meaning of Temperature  Kelvin temperature is an index of the random motions of gas particles (higher T means greater motion.)

23. QUESTION Kinetic molecular theory helps explain the definition of temperature based on molecular motion. Which statement describes an important aspect of this connection? 1.Temperature is inversely related to the kinetic energy of the gas particles. 2.At the same temperature, more massive gas particles will be moving faster than less massive gas particles. 3.As the temperature of a gas sample increases, the average velocity of the gas particles increases. 4.Kinetic energy is directly related to temperature. This is valid for any units of temperature.

24. ANSWER Choice 3 states a correct connection between temperature and velocity. The important relationship is summarized in the following equation: ½  mass  velocity 2 = 3/2 RT (T must be in K). Section 5.6: The Kinetic Molecular Theory of Gases

25. Kinetic Molecular Theory  1.Volume of individual particles is  zero.  2.Collisions of particles with container walls cause pressure exerted by gas.  3.Particles exert no forces on each other.  4.Average kinetic energy  Kelvin temperature of a gas.

26. Molecular Motion / Theory The Meaning of Temperature Temperature (Kelvin) is an index of the random motions of gas particles (higher T means greater motion.)

27. Velocity & Temperature

28. QUESTION Why is it critical that the temperature be held constant when applying Boyle’s law to changing the pressure of a trapped gas? 1.Gas molecules may expand at higher temperatures; this would change the volume. 2.Changing the temperature causes the gas to behave in non-ideal fashion. 3.Changing the temperature affects the average particle speed, which could affect the pressure. 4.Allowing the temperature to drop below 0°C would cause the trapped gas to no longer follow Boyle’s Law.

29. ANSWER Choice 3 provides the connection between temperature and pressure that would introduce another variable when studying the pressure- volume relationship. Boyle’s law shows that if the molecules of a trapped gas maintain the same average velocity when their volume is changed, the pressure will be inversely related to the volume change. Section 5.2: The Gas Laws of Boyle, Charles, and Avogadro

31. QUESTION As the temperature of a gas increases, which statement best correlates to information about molecular velocity? 1.The average molecular velocity will increase, but the distribution of molecular velocities will stay the same. 2.The average molecular velocity will stay the same, but the molecular velocity distribution will spread. 3.The average molecular velocity will increase, and the distribution of the molecular velocities will spread. 4.The average molecular velocity will stay the same, and the distribution of the molecular velocities will stay the same.

32. ANSWER Choice 3 accurately reflects the connection between molecular velocity and an increase in temperature. Figure 5.21 on page 206 visually shows the relationship. Kelvin temperature is directly related to molecular velocity - with greater temperature the distribution of available velocities also increases. Section 5.6: The Kinetic Molecular Theory of Gases

33. View Gas Molecules Applet View Gas Molecules Applet http://chemconnections.llnl.govJava/molecules/index.html View Molecular Vibrations: IRGasTutor http://chemistry.beloit.edu/Warming/pages/infrared.html

34. Changes in Temperature (  PV&T)

35. Pressure, Volume & Temperature

36. An empty one gallon can is hooked to a vacuum pump. What do you expect to happen?

37. Explain why the can collapsed.

38. Provide 3 different sets of conditions (Pressure and Temperature) which can account for the volume of the gas decreasing by 1/2. Cases 1-3 in the handout. Applying a Gas Law

39. Avogadro’s Law  For a gas at constant temperature and pressure, the volume is directly proportional to the number of moles of gas (at low pressures).  V =  n   = proportionality constant  V = volume of the gas  n = number of moles of gas

40. Volume vs. n (moles of a gas)

42. QUESTION Each of the balloons hold 1.0 L of different gases. All four are at 25°C and each contains the same number of molecules. Of the following which would also have to be the same for each balloon? (obviously not their color) 1.Their density 2.Their mass 3.Their atomic numbers 4.Their pressure

43. ANSWER Choice 4 is consistent with Avogadro’s Law. The temperature, pressure, number of moles, and volume are related for a sample of trapped gas. If two samples have three variables out of the four the same, the fourth variable must be the same as well. Section 5.2: The Gas Laws of Boyle, Charles, and Avogadro

44. Ideal Gas Law  An equation of state for a gas.  “state” is the condition of the gas at a given time.  PV = nRT  [Consider] If the moles remain constant and conditions change then:  P 1 V 1 / T 1 = P 2 V 2 / T 2

45. QUESTION If a person exhaled 125 mL of CO 2 gas at 37.0°C and 0.950 atm of pressure, what would this volume be at a colder temperature of 10.0°C and 0.900 atm of pressure? 1.3.12 mL 2.0.130 L 3.0.120 L 4.22.4 L

46. ANSWER Choice 3 correctly accounts for the changing conditions. The combination of Charles and Boyle’s laws provides the mathematical basis for the calculation. After converting the temperature to K units, the equation P 1 V 1 /T 1 = P 2 V 2 /T 2 may be used by solving for V 2. Section 5.3: The Ideal Gas Law

47. Ideal Gas Law  PV = nRT  R = proportionality constant = 0.08206 L atm   mol   P = pressure in atm  V = volume in liters  n = moles  T = temperature in Kelvins  Holds closely at P < 1 atm

48. Standard Temperature and Pressure  “STP”  For 1 mole of a gas at STP:  P = 1 atmosphere  T =  C  The molar volume of an ideal gas is 22.42 liters at STP

49. QUESTION If a 10.0 L sample of a gas at 25°C suddenly had its volume doubled, without changing its temperature what would happen to its pressure? What could be done to keep the pressure constant without changing the temperature? 1.The pressure would double; nothing else could be done to prevent this. 2.The pressure would double; the moles of gas could be doubled. 3.The pressure would decrease by a factor of two; the moles of gas could be halved. 4.The pressure would decrease by a factor of two; the moles could be doubled.

50. ANSWER Choice 4 describes two opposing changes. When the volume increases, the pressure of a trapped gas will decrease (at constant temperature and constant moles of gas). However, if the pressure drops, more collisions could be restored by adding more particles of gas in the same ratio as the pressure decline. Section 5.2: The Gas Laws of Boyle, Charles, and Avogadro

52. QUESTION A typical total capacity for human lungs is approximately 5,800 mL. At a temperature of 37°C (average body temperature) and pressure of 0.98 atm, how many moles of air do we carry inside our lungs when inflated? (R = 0.08206 L atm/ K mol) 1.1.9 mol 2.0.22 mol 3. 3.230 mol 4. 4.2.20 mol 5.0 mol: Moles can harm a person’s lungs.

53. ANSWER Choice 2 is correct. The units for temperature must be in K, pressure in atm, and volume in L. Then using the universal constant 0.08206 L atm/ K mol in the PV = nRT equation moles may be solved. Section 5.3: The Ideal Gas Law n O 2 (g) = PV / RT

54. Do you have enough oxygen to climb Mt. Everest? http://www.chemcollective.org/applets/everest.php

55. An average pair of human lungs actually contains only about 3.5 L of air after inhalation and about 3.0 L after exhalation. Assuming that air in your lungs is at 37°C and 1.0 atm a) How many moles of O 2 are actually in a typical breath?. b) What is the mass of O 2 in a typical breath?. c) How much of the O 2 is essential biochemically?

56. QUESTION The primary source of exhaled CO 2 is from the combustion of glucose, C 6 H 12 O 6 (molar mass = 180. g/mol.). The balanced equation is shown here: C 6 H 12 O 6 (aq) + 6 O 2 (g)  6 CO 2 (g) + 6 H 2 O (l) If you oxidized 5.42 grams of C 6 H 12 O 6 while tying your boots to climb Mt. Everest, how many liters of O 2 @ STP conditions did you use? 1.0.737 L 2.0.672 L 3.4.05 L 4.22.4 L

57. ANSWER Choice 3, assuming you were not holding your breath, is correct. The number of moles of glucose must first be determined (5.42/180. = 0.0301 moles), then this is multiplied by 6 to account for the stoichiometric ratio between glucose and oxygen. From this, PV = nRT may be used with the appropriate substitutions. Section 5.4: Gas Stoichiometry

58. Dalton’s Law of Partial Pressures  For a mixture of gases, the total pressure is the sum of the pressures of each gas in the mixture. P Total = P 1 + P 2 + P 3 +... P Total  n Total n Total = n 1 + n 2 + n 3 +. n Total = n 1 + n 2 + n 3 +.

59. QUESTION If the mole fraction of O 2 in our atmosphere at standard conditions is approximately 0.209, what is the partial pressure of the oxygen in every breath you take? 1.1.00 atm 2.4.78 atm 3.159 torr 4.3640 mmHg

60. ANSWER Choice 3 shows the correct pressure. This calculation is based on the application of Dalton’s law of partial pressures. For one atmosphere of pressure 0.209 is caused by oxygen so 760 .209 = 159 torr. Section 5.5: Dalton’s Law of Partial Pressures

61. Dalton’s Law of Partial Pressures  For a mixture of gases, the partial gas pressure and total pressure equal the mole fraction of each gas in the mixture. For a mixture of gases, the partial gas pressure and total pressure equal the mole fraction of each gas in the mixture. For a mixture of gases, the partial gas pressure and total pressure equal the mole fraction of each gas in the mixture. P 1 / P Total = n 1 / n Total P 1 / P Total = n 1 / n Total

62. QUESTION Freon-12 had been widely used as a refrigerant in air conditioning systems. However, it has been shown to be related to destroying Earth’s important ozone layer. What is the molar mass of Freon-12 if 9.27 grams was collected by water displacement, in a 2.00 liter volume at 30.0°C and 764 mmHg. Water’s vapor pressure at this temperature is approximately 31.8 mmHg. 1.120. g/mol 2.12.0 g/mol 3.115 g/mol 4.92.7 g/mol

63. ANSWER Choice 1 is the molar mass of Freon-12. The pressure must be corrected for the presence of water by subtracting 31.8 mmHg from the total pressure. This should also be converted to atm. The temperature must be converted to K. Then PV = nRT can be used if n is written as g/mm and solved for mm. Section 5.5: Dalton’s Law of Partial Pressures

64. Applying the Ideal Gas Law  PV = n RT  n = g of gas/ MM gas [MM gas =g/mol]  PV = (g of gas/ MM gas )RT  MM gas = g of gas(RT)/PV  MM gas = g of gas/V (RT/P)  MM gas = density of gas (RT/P)

65. Applying the Ideal Gas Law The density of an unknown atmospheric gas pollutant was experimentally determined to be 1.964 g/ L @ 0 o C and 760 torr. What is the molar mass of the gas?What is the molar mass of the gas? What might the gas be?What might the gas be?

66. Applying the Ideal Gas Law MM gas = density of gas (RT/P) MM gas = 1.964 g/ L x 0.08206 L atm   mol  x 273K/ 760 torr x 760 torr/ 1atm x 273K/ 760 torr x 760 torr/ 1atm 1.964 g/ L @ 0 o C and 760 torr. R = 0.08206 L atm   mol  o C  K torr  atm MM gas = MM gas = 44.0 g/mol

67. QUESTION Under STP conditions what is the density of O 2 gas? 1.Not enough information is given to solve this. 2.1.31 g/L 3.1.43 g/L 4.0.999 g/L

68. ANSWER Choice 3 is the correct density for O 2 at STP. At STP conditions the volume of one mole of a gas is approximately 22.4 L. One mole of oxygen = 32.0 grams. The density is calculated by dividing mass by volume. Or  density of gas (g/L) = MM gas P/ RT Section 5.4: Gas Stoichiometry

69. QUESTION The aroma of fresh raspberries can be attributed, at least in part, to 3-(para-hydroxyphenyl)-2-butanone. What is the molar mass of this pleasant smelling compound if at 1.00 atmosphere of pressure and 25.0°C, 0.0820 grams has a volume of 12.2 mL? 1.13.8 g/mol 2.164 g/mol 3.40.9 g/mol 4.224 g/mol

70. ANSWER Choice 2 is correct. Using PV = nRT and properly substituting 0.0122 L for V, 298 K for T, using 0.08206 for R and solving for n the number of moles represented by 0.0820 grams can be obtained. Then the grams in one mole can be found. Section 5.3: The Ideal Gas Law

71. Effusion: describes the passage of gas into an evacuated chamber. Diffusion: describes the mixing of gases. The rate of diffusion is the rate of gas mixing. Diffusion and Effusion

72. Effusion

73. Effusion: Diffusion: Effusion and Diffusion

74. Applying Gas Behavior Preparation of 235 U  235 UO 3 (s) + 238 UO 3 (s)  235 UF 6 (g) + 238 UF 6 (g)  235 U is the unstable isotope that is used in nuclear fission. Which isoptope is the most abundant?  Design a method to separate the isomers.  Be very careful

75. Applying Gas Behavior Centrification of 235 U/ 238 U  235 UF 6 (g) + 238 UF 6 (g) U-238, moves toward the outside of the cylinder and U- 235, collects closer to the center. The stream that is slightly enriched in U-235 is withdrawn and fed into the next higher stage, while the slightly depleted stream is recycled back into the next lower stage.

76. Applying Gas Behavior Centrification of 235 U/ 238 U  235 UF 6 (g) + 238 UF 6 (g)

77. Applying Gas Behavior Centrification of 235 U/ 238 U  235 UF 6 (g) + 238 UF 6 (g) February 25, 2008 AP) — Iran said Sunday that it started using new centrifuges that can enrich 235 U @ 2x the previous speed. The United Nations nuclear watchdog agency confirmed that Iran was using 10 of the new IR-2 centrifuges

78. Real Gases Must correct ideal gas behavior when at high pressure (smaller volume) and low temperature (attractive forces become important).

79. Real Gases  corrected pressure corrected volume P ideal V ideal

81. Real Gases Volume vs. Temperature @ constant P

82. QUESTION After examining the figure, which statement is accurate, and consistent about the real gases shown at constant pressure? 1.At –273°C all gases occupy nearly the same volume; the different slopes are because of differences in molar masses. 2.At zero Celsius the gases have different volumes because the larger the molecule, the larger the volume. 3.Since the pressure is constant, the only difference in volume that could cause the different slopes is in the attractive forces (Van der Waal’s forces). 4.Although it does appear to do so, the volumes do not reach zero but if the graph used K instead of °C the volume would reach zero for all the gases.

83. ANSWER Choice 3 is the correct conclusion. If all the gases had the same attractive forces (with constant pressure) the volumes would be proportional to their speeds and inversely proprtional to their molecular weights. Section Section 5.8: Real Gases

85. QUESTION Real gases exhibit their most “ideal” behavior at which relative conditions? 1.Low temperatures and low pressures 2.High temperatures and high pressures 3.High temperatures and low pressures 4.Low temperatures and high pressures

86. ANSWER Choice 3 provides the correct choice. At those conditions gas molecules are farthest apart and exert their least influence on each other thereby permitting their behavior to follow mathematical predictions. Section 5.8: Real Gases

87. Atmospheric Pollutants

90. Gases & Airbags Use of Chemical Reactions and Physical Properties Workshop: Gases II