WHAT GOVERNS THE WAY THAT GASES, IN OUR ATMOSPHERE, BEHAVE?

1. WHAT GOVERNS THE WAY THAT GASES, IN OUR ATMOSPHERE, BEHAVE?

2. CHARLES’ LAW Molecules of gas at a fixed pressure and temperature, vibrate sufficiently to occupy a fixed volume

3. CHARLES’ LAW Warm

4. CHARLES’ LAW Increased molecular vibration, spacing increases Warm

5. CHARLES’ LAW Increased molecular vibration, spacing increases Warm Volume Increases

6. CHARLES’ LAW Increased molecular vibration, spacing increases Warm Cool Volume Increases

7. CHARLES’ LAW Decreased molecular vibration, spacing decreases Increased molecular vibration, spacing increases Warm Cool Volume Increases

8. CHARLES’ LAW Decreased molecular vibration, spacing decreases Increased molecular vibration, spacing increases Warm Cool Volume Decreases Volume Increases

9. CHARLES’ LAW “If the atmospheric pressure is held constant, hot gases expand to occupy a bigger volume and cold gases contract to occupy a smaller volume.” Decreased molecular vibration, spacing decreases Increased molecular vibration, spacing increases Warm Cool Volume Decreases Volume Increases

10. CHARLES’ LAW V=k2.T At constant Pressure Decreased molecular vibration, spacing decreases Increased molecular vibration, spacing increases Warm Cool Volume Decreases Volume Increases

11. CHARLES’ LAW V=k2.T At constant Pressure Decreased molecular vibration, spacing decreases Increased molecular vibration, spacing increases Warm Cool Volume Decreases Volume Increases V↓=k2.T↓ V↑=k2.T↑

12. BOYLE’S LAW Molecules of gas at a fixed pressure and temperature, vibrate sufficiently to occupy a fixed volume M =1.0

13. BOYLE’S LAW Atmospheric Pressure M =1.0 Vibrating molecules of gas

14. BOYLE’S LAW Compress, squeeze, add “weight” M =1.0 M = 0.5 M = 1.0

15. BOYLE’S LAW Decompress, relax, reduce “weight” Compress, squeeze, add “weight” M = 0.5 M =1.0 M = 0.5 M = 1.0 Increased Pressure Volume contracts Decreased Pressure Volume expands

16. BOYLE’S LAW “At constant temperature, the pressure exerted on a gas is inversely related to the volume the gas occupies – gases are compressible.” M = 0.5 M =1.0 M = 0.5 M = 1.0

17. BOYLE’S LAW P = k1/V At constant Temperature M = 0.5 M =1.0 M = 0.5 M = 1.0 P↓…. V↑ P↑ ….. V↓

18. HOW ARE THESE LAWS GOING TO HELP TO MOVE MASS AND ENERGY IN THE ATMOSPERIC SYSTEM?

19. EQUAL PRESSURE (ATMOSPHERIC) Air Filled Balloon

20. Lower Pressure Higher Pressure Brick Air Flow Differences in pressures cause motion of the air

21. Air temperature ≈ Sensible heat flux from insolation = f(latitude,season)

22. Changes in temperature cause changes in volume occupied by air. Air temperature ≈ Sensible heat flux from insolation = ∫ (latitude,season) V=k2.T At constant Pressure

23. Changes in temperature cause changes in volume occupied by air. Air temperature ≈ Sensible heat flux from insolation = ∫ (latitude,season) V=k2.T At constant Pressure P = k1/V At constant Temperature Changes in volume occupied cause changes in pressure on air

24. Changes in temperature cause changes in volume occupied by air. Air temperature ≈ Sensible heat flux from insolation = ∫ (latitude,season) V=k2.T At constant Pressure P = k1/V At constant Temperature Changes in volume occupied cause changes in pressure on air Differences in pressure cause movements within the atmosphere

25. Changes in temperature cause changes in volume occupied by air. Air temperature ≈ Sensible heat flux from insolation = ∫ (latitude,season) V=k2.T At constant Pressure Temporal and spatial differences in insolation related to pressure that moves atmosphere P = k1/V At constant Temperature Changes in volume occupied cause changes in pressure on air Differences in pressure cause movements within the atmosphere

26. THE EQUATION OF STATE FOR AN IDEAL GAS.PUTTING IT ALL TOGETHER!

27. P = R. ρ. T P = Pressure on a gas R = Gas Constant ρ = Density of gas T = Temperature of gas

28. P = R. ρ. T P = Pressure on a gas R = Gas Constant ρ = Density of gas T = Temperature of gas ?

29. P = R. ρ. T P = Pressure on a gas R = Gas Constant ρ = Density of gas: ρ = Mass/Volume T = Temperature of gas

30. P = R. M/V. T P = Pressure on a gas R = Gas Constant ρ = Density of gas: ρ = Mass/Volume T = Temperature of gas

31. P = R. M. T V Charles’ Law: Fixed P, T and V directly related 9 = 1. 1 . 2.25 0.25 If T rises to 3.0, then V must rise to 0.33 to Keep P constant at 9! 9 = 1. 1 . 3.0 0.33

32. P = R. M. T V Boyle’s Law: Fixed T, P and V inversely related Multiply both sides by V V . P = R. M. T Pressure declines so volume occupied increases to keep T constant 3. 3 = 1. 1. 9 4. 2.25 = 1. 1. 9

33. PRACTICAL APPLICATION We know that Atmospheric Pressure declines with altitude, so what can we expect to happen to Temperatures and the Density of the air as you climb a mountain or go up in an airplane? P = R. ρ. T

34. PRACTICAL APPLICATION We know that Atmospheric Pressure declines with altitude, so what can we expect to happen to Temperatures and the Density of the air as you climb a mountain or go up in an airplane? P = R. ρ. T Should become colder and the atmosphere “thinner”!

35. PRACTICAL APPLICATION We know that Atmospheric Pressure declines with altitude, so what can we expect to happen to Temperatures and the Density of the air as you climb a mountain or go up in an airplane? P = R. ρ. T Normal Lapse Rate: Rate at which temperatures decline (increase) with increase (decrease) in altitude

36. PRACTICAL APPLICATION We know that Atmospheric Pressure declines with altitude, so what can we expect to happen to Temperatures and the Density of the air as you climb a mountain or go up in an airplane? P = R. ρ. T Normal Lapse Rate: Rate at which temperatures decline (increase) with increase (decrease) in altitude 6.5°C per Kilometer 3.6°F per 1000 ft.

37. 4.392 km -13°C 15°C 0 km