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Chapter 11 Gases

Chapter 11 Gases. 2009, Prentice Hall. Properties of Gases. Expand to completely fill their container = Compressible Take the shape of their container. Low density. Much less than solid or liquid state. Mixtures of gases are always homogeneous. The Structure of a Gas.

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Chapter 11 Gases

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  1. Chapter 11Gases 2009, Prentice Hall

  2. Properties of Gases • Expand to completely fill their container = Compressible • Take the shape of their container. • Low density. • Much less than solid or liquid state. • Mixtures of gases are always homogeneous

  3. The Structure of a Gas • Gases are composed of particles that are flying around very fast in their container(s). • They move in straight lines until they encounter either the container wall or another particle, then they bounce off. • If you were able to take a snapshot of the particles in a gas, you would find that there is a lot of empty space in there. • It’s why balloons look round

  4. Kinetic Molecular Theory • The particles of the gas (either atoms or molecules) are constantly moving & The attraction between particles is negligible. • Therefore: When the moving particles hit another particle or the container, they do not stick, but they bounce off and continue moving in another direction. • Like billiard balls.

  5. Kinetic Molecular Theory of Gases • The average kinetic energy of the particles is directly proportional to the Kelvin temperature. • As you raise the temperature of the gas, the average speed of the particles increases. • But don’t be fooled into thinking all the particles are moving at the same speed!!

  6. Kinetic Molecular Theory

  7. What does all this Pushing do? • Gas molecules are constantly in motion. • As they move and strike a surface, they push on that surface. • Push = force. • If we could measure the total amount of force exerted by gas molecules hitting the entire surface at any one instant, we would know the pressure the gas is exerting. • Pressure = force per unit area= pounds per square inch

  8. The Effect of Gas Pressure • The pressure exerted by a gas can cause some amazing and startling effects.

  9. Which Way Would Air Flow? Two filled balloons are connected with a long pipe. One of the balloons is plunged down into the water. Which way will the air flow? Will air flow from the lower balloon toward the top balloon; or will it flow from the top balloon to the bottom one? 9

  10. Is This Possible at a Depth of 20 m = 65.6 ft? 10

  11. Soda Straws and Gas Pressure The pressure of the air inside the straw is the same as the pressure of the air outside the straw—so liquid levels are the same on both sides. The pressure of the air inside the straw is lower than the pressure of the air outside the straw—so liquid is pushed up the straw by the outside air.

  12. Air Pressure • The atmosphere exerts a pressure • At sea level it is 14.7 psi. • The atmosphere goes up about 370 miles, but 80% is in the first 10 miles from Earth’s surface. • This is the same pressure that a column of water would exert if it were about 10.3 m high. • Therefore water can not be pumped higher, in a straw for instance, than 10.3 m/33.8 ft

  13. Measuring Air Pressure • Use a barometer. • Column of mercury supported by air pressure. • Force of the air on the surface of the mercury balanced by the pull of gravity on the column of mercury. gravity

  14. Atmospheric Pressure and Altitude • The higher up in the atmosphere you go, the lower the atmospheric pressure is around you. • At the surface, the atmospheric pressure is 14.7 psi, but at 29,028 ft it is only 4.9 psi (1/3) • Rapid changes in atmospheric pressure may cause your ears to “pop” due to an imbalance in pressure on either side of your ear drum.

  15. Pressure Imbalance in Ear If there is a difference in pressure across the eardrum membrane, the membrane will be pushed out—what we commonly call a “popped eardrum.”

  16. Common Units of Pressure

  17. psi atm mmHg Example 11.1—A High-Performance Bicycle Tire Has a Pressure of 125 psi. What Is the Pressure in mmHg? Given: Find: 125 psi mmHg Solution Map: Relationships: 1 atm = 14.7 psi, 1 atm = 760 mmHg Solution: Check: Since mmHg are smaller than psi, the answer makes sense.

  18. Boyle’s Law • Pressure of a gas is inversely proportional to its volume. • Constant T and amount of gas. • Graph P vs. V is curved. • Graph P vs. 1/V is in a straight line. • As P increases, V decreases by the same factor. • P x V = constant. • P1 x V1 = P2 x V2.

  19. When you double the pressure on a gas, the volume is cut in half (as long as the temperature and amount of gas do not change).

  20. Gas Laws Explained— Boyle’s Law • Boyle’s law says that the volume of a gas is inversely proportional to the pressure. • Decreasing the volume forces the molecules into a smaller space. • More molecules will collide with the container at any one instant, increasing the pressure.

  21. Boyle’s Law and Diving Scuba tanks have a regulator so that the air from the tank is delivered at the same pressure as the water surrounding you. This allows you to take in air even when the outside pressure is large. • Since water is more dense than air, for each 10 m you dive below the surface, the pressure on your lungs increases 1 atm. • At 20 m the total pressure is 3 atm. • If your tank contained air at 1 atm of pressure, you would not be able to inhale it into your lungs. • You can only generate enough force to overcome about 1.06 atm.

  22. Boyle’s Law and Diving, Continued • If a diver holds her breath and rises to the surface quickly, the outside pressure drops to 1 atm. • According to Boyle’s law, what should happen to the volume of air in the lungs? • Since the pressure is decreasing by a factor of 3, the volume will expand by a factor of 3, causing damage to internal organs. Always Exhale When Rising!!

  23. V1, P1, P2 V2 Example 11.2—A Cylinder with a Movable Piston Has a Volume of 6.0 L at 4.0 atm. What Is the Volume at 1.0 atm? Given: Find: V1 =6.0 L, P1 = 4.0 atm, P2 = 1.0 atm V2, L Solution Map: Relationships: P1∙ V1= P2∙ V2 Solution: Check: Since P and V are inversely proportional, when the pressure decreases ~4x, the volume should increase ~4x, and it does.

  24. Practice—A Balloon Is Put in a Bell Jar and the Pressure Is Reduced from 782 torr to 0.500 atm. If the Volume of the Balloon Is Now 2780 mL, What Was It Originally?(1 atm = 760 torr)

  25. V2, P1, P2 V1 Practice—A Balloon Is Put in a Bell Jar and the Pressure Is Reduced from 782 torr to 0.500 atm. If the Volume of the Balloon Is Now 2780 mL, What Was It Originally?, Continued Given: Find: V2 =2780 mL, P1 = 762 torr, P2 = 0.500 atm V1, mL Solution Map: Relationships: P1∙ V1= P2∙ V2 , 1 atm = 760 torr (exactly) Solution: Check: Since P and V are inversely proportional, when the pressure decreases ~2x, the volume should increase ~2x, and it does.

  26. Gas Laws and Temperature • Gases expand when heated and contract when cooled, so there is a relationship between volume and temperature. • Gas molecules move faster when heated, causing them to strike surfaces with more force, so there is a relationship between pressure and temperature. • In order for the relationships to be proportional, the temperature must be measured on an absolute scale. • When doing gas problems, always convert your temperatures to kelvins. K = °C + 273 & °C = K - 273 °F = 1.8 °C + 32 & °C = 0.556(°F-32)

  27. Standard Conditions • Common reference points for comparing. • Standard pressure = 1.00 atm. • Standard temperature = 0 °C. • 273 K. • STP.

  28. Volume and Temperature • In a rigid container, raising the temperature increases the pressure. • For a cylinder with a piston, the pressure outside and inside stay the same. • To keep the pressure from rising, the piston moves out increasing the volume of the cylinder. • As volume increases, pressure decreases.

  29. Volume and Temperature, Continued As a gas is heated, it expands. This causes the density of the gas to decrease. Because the hot air in the balloon is less dense than the surrounding air, it rises.

  30. Charles’s Law • Volume is directly proportional to temperature. • Constant P and amount of gas. • Graph of V vs. T is a straight line. • As T increases, V also increases. • Kelvin T = Celsius T + 273. • V = constant x T. • If T is measured in kelvin.

  31. We’re losing altitude. Quick, Professor, give your lecture on Charles’s law!

  32. Absolute Zero • Theoretical temperature at which a gas would have zero volume and no pressure. • Kelvin calculated by extrapolation. • 0 K = -273.15 °C = -459 °F • Never attainable. • Though we’ve gotten real close! • All gas law problems use the Kelvin temperature scale.

  33. Determining Absolute Zero William Thomson, the Lord of Kelvin, extrapolated the line graphs of volume vs. temp- erature to determine the theoretical temperature that a gas would have given a volume of 0.

  34. T(K) = t(°C) + 273, V1, V2, T2 T1 Example 11.3—A Gas Has a Volume of 2.57 L at 0 °C. What Was the Temperature at 2.80 L? Given: Find: V1 =2.80 L, V2 = 2.57 L, t2 = 0°C t1, K and °C Solution Map: Relationships: Solution: Check: Since T and V are directly proportional, when the volume decreases, the temperature should decrease, and it does.

  35. The Combined Gas Law • Boyle’s law shows the relationship between pressure and volume. • At constant temperature. • Charles’s law shows the relationship between volume and absolute temperature. • At constant pressure. • The two laws can be combined together to give a law that predicts what happens to the volume of a sample of gas when both the pressure and temperature change. • As long as the amount of gas stays constant.

  36. T(K) = t(°C) + 273, P1,V1, V2, T1, T2 P2 Example 11.4—A Sample of Gas Has an Initial Volume of 158 mL at a Pressure of 735 mmHg and a Temperature of 34 °C. If the Gas Is Compressed to 108 mL and Heated to 85 °C, What Is the Final Pressure? Given: Find: V1 = 158 mL, t1 = 34 °C L, P1 = 735 mmHg V2 = 108 mL, t2 = 85 °C P2, mmHg Solution Map: Relationships: Solution: Check: Since T increases and V decreases we expect the pressure should increase, and it does.

  37. Practice—A Gas Occupies 10.0 L When Its Pressure Is 3.00 atm and Temperature Is 27 °C. What Volume Will the Gas Occupy Under Standard Conditions?

  38. Avogadro’s Law • Volume is directly proportional to the number of gas molecules. • V = constant xn. • Constant P and T. • More gas molecules = larger volume. • Count number of gas molecules by moles, n. • Equal volumes of gases contain equal numbers of molecules. • The gas doesn’t matter.

  39. Avogadro’s Law, Continued

  40. mol added = n2– n1, V1, V2, n1 n2 Example 11.5—A 0.22 Mol Sample of He Has a Volume of 4.8 L. How Many Moles Must Be Added to Give 6.4 L? Given: Find: V1 =4.8 L, V2 = 6.4 L, n1 = 0.22 mol n2, and added moles Solution Map: Relationships: Solution: Check: Since n and V are directly proportional, when the volume increases, the moles should increase, and it does.

  41. Practice—If 1.00 Mole of a Gas Occupies 22.4 L at STP, What Volume Would 0.750 Moles Occupy?

  42. V1, n1, n2 V2 Practice—If 1.00 Mole of a Gas Occupies 22.4 L at STP, What Volume Would 0.750 Moles Occupy?, Continued Given: Find: V1 =22.4 L, n1 = 1.00 mol, n2 = 0.750 mol V2 Solution Map: Relationships: Solution: Check: Since n and V are directly proportional, when the moles decreases, the volume should decrease, and it does.

  43. Ideal Gas Law • By combining the gas laws, we can write a general equation. • R is called the Gas Constant. • The value of R depends on the units of P and V. • We will use 0.0821 and convert P to atm and V to L. • Use the ideal gas law when you have a gas at one condition, use the combined gas law when you have a gas whose condition is changing.

  44. P, V, T, R n Example 11.7—How Many Moles of Gas Are in a Basketball with Total Pressure 24.2 Psi, Volume of 3.2 L at 25 °C? Given: Find: V = 3.2 L, P = 24.2 psi, t = 25 °C, n, mol Solution Map: Relationships: 1 atm = 14.7 psi T(K) = t(°C) + 273 Solution: Check: 1 mole at STP occupies 22.4 L at STP; since there is a much smaller volume than 22.4 L, we expect less than 1 mole of gas.

  45. Molar Mass of a Gas • One of the methods chemists use to determine the molar mass of an unknown substance is to heat a weighed sample until it becomes a gas, measure the temperature, pressure, and volume, and use the ideal gas law.

  46. n, m P, V, T, R MM n 1 atm = 760 mmHg, T(K) = t(°C) + 273 Example 11.8—Calculate the Molar Mass of a Gas with Mass 0.311 g that Has a Volume of 0.225 L at 55 °C and 886 mmHg. Given: Find: m = 0.311g, V = 0.225 L, P = 1.1658 atm, T = 328 K Molar Mass,g/mol m=0.311g, V=0.225 L, P=886 mmHg, t=55°C, Molar Mass,g/mol Solution Map: Relationships: Solution: Check: The value 31.9 g/mol is reasonable.

  47. Practice—What Is the Molar Mass of a Gas if 12.0 g Occupies 197 L at 380 torr and 127 °C? 121

  48. Mixtures of Gases • According to the kinetic molecular theory, the particles in a gas behave independently. • Air is a mixture, yet we can treat it as a single gas. • Also, we can think of each gas in the mixture as independent of the other gases. • All gases in the mixture have the same volume and temperature. • All gases completely occupy the container, so all gases in the mixture have the volume of the container.

  49. Partial Pressure • Each gas in the mixture exerts a pressure independent of the other gases in the mixture. • The pressure of a component gas in a mixture is called a partial pressure. • The sum of the partial pressures of all the gases in a mixture equals the total pressure. • Dalton’s law of partial pressures. • Ptotal = Pgas A + Pgas B + Pgas C +...

  50. Example 11.9—A Mixture of He, Ne, and Ar Has a Total Pressure of 558 MmHg. If the Partial Pressure of He Is 341 MmHg and Ne Is 112 MmHg, Determine the Partial Pressure of Ar in the Mixture. Ptot, PHe, PNe PAr Given: Find: PHe= 341 mmHg, PNe= 112 mmHg, Ptot = 558 mmHg PAr, mmHg Solution Map: Relationships: PAr = Ptot – (PHe + PNe) Ptot= Pa + Pb + etc. Solution: Check: The units are correct, the value is reasonable.

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