1. Chapter 9 Gases: Their Properties and Behavior

2. Three States of Matter SolidsLiquidsGases

3. Properties of Gases Gases mix completely with one another to form homogenous mixtures Gases can be compressed (keyboard cleaner) Gases exert pressure on what ever is around them (balloon, canister) Gases expand into whatever volume is available (coke bottle and balloon) Gases are described in terms of their temperature and pressure, the volume occupied and the amount of gas present (gas properties)

4. Compressibility of Gases Airbags fill with N 2 gas in an accident.Airbags fill with N 2 gas in an accident. Gas is generated by the decomposition of sodium azide, NaN 3.Gas is generated by the decomposition of sodium azide, NaN 3. 2 NaN 3 2 Na + 3 N 22 NaN 3 2 Na + 3 N 2 Composition of Air Nitrogen Oxygen Argon Carbob dioxide

5. Gases and Gas Pressure Gas% by VolGas% by Vol Nitrogen78.084Krypton0.0001 Oxygen20.948Carbon monoxide0.00001 Argon0.934Xenon0.000008 Carbon dioxide0.033Ozone0.000002 Neon0.00182Ammonia0.000001 Hydrogen0.0010Nitrogen dioxide0.0000001 Helium0.00052Sulfur dioxide0.00000002 Methane0.0002

6. Factors Affecting Gas Pressure Temperature –Raising the temperature of a gas increases the pressure –The faster moving particles collide with the walls of the container more frequently –Temperature and pressure is also a linear relationship –In contrast, decreasing the temperature of a gas decreases the pressure

7. Properties of Gases Pressure (P) Pressure = force / area Force = mass x acceleration Units of Pressure –Atmosphere (atm) –Torr –Pascals (Pa) –mmHg Pressure conversions –1 atm = 1.01325 x 10 5 Pa –1 atm = 760 torr –1 atm = 760 mmHg

8. Atmospheric Pressure - pressure created from the mass of the atmosphere pressing down on the earth’s surface –Standard atmospheric pressure at sea level – 760 mmHg

9. Problem Convert these pressure values. –120 mmHg to atm –100 kPa to mmHg –270 torr to atm

10. Properties of Gases Volume (V) –mL –L –cm 3 Amount of gas (n) – moles Temperature (T) - Kelvins

11. The Gas Laws Gas properties –Gases are described in terms of their temperature and pressure, the volume occupied and the amount of gas present (gas properties) Gas Laws can be derived using –Kinetic Molecular Theory

12. The Gas Laws Ideal Gas: A gas whose behavior follows the gas laws exactly. The physical properties of a gas can be defined by four variables: Ppressure Ttemperature Vvolume nnumber of moles

13. The Gas Laws The Pressure-Volume Relationship: Boyle’s Law –The volume (V) of an ideal gas varies inversely with the applied pressure (P) when temperature (T) and the amount (n, moles) are constant P i V i = P f V f PV = k  V P 1

14. The Gas Laws Boyle’s Law  V P 1 (constant n and T)PV = k

15. Sample Problem Using Boyle’s Law A balloon contains 30.0 L of helium gas at 103kPa. What is the volume of the helium when the balloon rises to an altitude where the pressure is only 25.0 kPa? (assume the temperature remains constant) What do you think will happen to the volume at a higher temperature knowing what you know already about gases?

16. Sample Problem Using Boyle’s Law P1 = 103 kPa P2 = 25.0 kPa V1 = 30.0 LV2 = ? L P 1 V 1 = P 2 V 2 or P 1 V 1 / P 2 = V 2 V 2 = (30.0 L) (103 kPa) 25.0 KPa V 2 = 1.24 x 10 2 L (3 sig figs)

17. Sample Problem Using Boyle’s Law Nitrous oxide (N 2 O) is used as an anesthetic. The pressure on 2.50 L of N 2 O changes from 105 KPa to 40.5 KPa. If the temperature does not change, what will the new volume be? P1 = 105 kPa P2 = 40.5 kPa V1 = 2.50 LV2 = ? L P 1 V 1 = P 2 V 2 or P 1 V 1 / P 2 = V 2 V 2 = (2.50 L) (105 kPa) 40.5 KPa V 2 = 6.48 L (3 sig figs)

18. Sample Problem Using Boyle’s Law A gas with a volume of 4.00 L at a pressure of 205 KPa is allowed to expand to a volume of 12.0 L. What is the pressure in the container if the temperature remains constant? P1 = 205 kPa P2 = ? kPa V1 = 4.00 LV2 = 12.0 L P 1 V 1 = P 2 V 2 or P 1 V 1 / V 2 = P 2 P 2 = (4.00 L) (205 kPa) 12.0 L P 2 = 68.3 KPa (3 sig figs)

19. Sample Problem Using Boyle’s Law The volume of a gas at 99.6 KPa and 24ºC is 4.23L. What volume will it occupy at 93.3 KPa and 24ºC? P1 = 99.6 kPa P2 = 93.3 kPaT1 = 24ºC V1 = 4.23 LV2 = ? L T2 = 24ºC P 1 V 1 = P 2 V 2 or P 1 V 1 / P 2 = V 2 V 2 = (4.23 L) (99.6 kPa) 93.3 kPa V 2 = 4.52 L (3 sig figs)

20. Problems A sample of nitrogen gas at 298 K and 745 torr has a volume of 37.42 L. What volume will it occupy if the pressure is increased to 894 torr at constant temperature? –A)22.3 L –B)31.2 L –C)44.9 L –D)112 L –E)380 L

21. Problems A sample of carbon dioxide gas at 125°C and 248 torr occupies a volume of 275 L. What will the gas pressure be if the volume is increased to 321 L at 125°C? –A)212 torr –B)289 torr –C)356 torr –D)441 torr –E)359 torr

22. The Gas Laws The Temperature-Volume Relationship – Charles Law –The volume (V) of an ideal gas varies directly with absolute temperature (T) when pressure (P) and amount (n) are constant. V i / T i = V f / T f = T final V final T initial V initial = k T V V  T

23. The Gas Laws Charles’ Law (constant n and P) = k T V

24. Sample Problem Using Charles’s Law A balloon inflated in a room at 24ºC has a volume of 4.00 L. The balloon is then heated to a temperature of 58ºC. What is the new volume if the pressure remains constant? T1 = 24ºC or 297 K V1 = 4.00 L T2 = 58ºC or 331 KV2 = ? L When using gas laws always express the temperatures in kelvins! T1 = 24ºC + 273 = 297 K T2 = 58ºC + 273 = 331 K

25. Sample Problem Using Charles’s Law A balloon inflated in a room at 24ºC has a volume of 4.00 L. The balloon is then heated to a temperature of 58ºC. What is the new volume if the pressure remains constant? T1 = 24ºC or 297 KV1 = 4.00 L T2 = 58ºC or 331 KV2 = ? L V 1 = V 2 or V 1 T 2 = V 2 T 1 T 2 T 1 V 2 = (4.00 L) (331 K) = 4.46 L 297 K

26. Sample Problem Using Charles’s Law If a sample of gas occupies 6.80 L at 325ºC, what will its volume be at 25ºC if the pressure does not change? T1 = 325ºC or 598 KV1 = 6.80 L T2 = 25ºC or 298 KV2 = ? L V 1 = V 2 or V 1 T 2 = V 2 T 1 T 2 T 1 V 2 = (6.80 L) (298 K) = 3.39 L 598 K

27. Problems A sample container of carbon monoxide occupies a volume of 435 mL at a pressure of 785 torr and a temperature of 298 K. What would its temperature be if the volume were changed to 265 mL at a pressure of 785 torr? –A)182 K –B)298 K –C)387 K –D)489 K –E)538 K

28. Problems A 0.850-mole sample of nitrous oxide, a gas used as an anesthetic by dentists, has a volume of 20.46 L at 123°C and 1.35 atm. What would be its volume at 468°C and 1.35 atm? –A)5.38 L –B)10.9 L –C)19.0 L –D)38.3 L –E)77.9 L

29. The Gas Laws The Amount-Volume Relationship: Avogadro’s Law –The volume (V) of an ideal gas varies directly with amount (n) when temperature (T) and pressure (P) are constant –V 1 / n 1 = V 2 / n 2 = n final V final n initial V initial = k n V V  n

30. The Gas Laws Avogadro’s Law V  n (constant T and P) = k n V twice as many molecules

31. Only at STP –0ºC –1 atm This way we compare gases at the same temperature and pressure. This is where we get the fact that 22.4 L =1 mole

32. Summary Boyle’s LawCharles’ LawAvogadro’s Law constant T & n constant P & n constant P & T V = 1/P V = T V = n P initial V initial = P final V final = T final V final T initial V initial = n final V final n initial V initial

34. The Ideal Gas Law Boyle’s, Charles’s and Avogadro’s Laws can be combined to form the Ideal Gas Law –PV = nRT R – ideal gas constant –R = 0.0821 atm L / mol K –R = 62.36 torr L / mol K –R = 8.314 J / mol K

35. Sample Problem Using Ideal Gas Law When the temperature of a rigid hollow sphere containing 685 L of helium gas is held at 621 K, the pressure of the gas is 1.89 x 10 3 kPa. How many moles of helium does the sphere contain? P = 1.89 x 10 3 kPa V = 685 LT = 621 K PV = nRT or PV / RT = n n = (1.89 x 10 3 kPa) (685 L) mol · K (8.31L · kPa) (621K) n = 251 mol He

36. Sample Problem Using Ideal Gas Law A child’s lungs can hold 2.20 L. How many grams of air do her lungs hold at a pressure of 102 kPa and a body temperature of 37ºC? Use a molar mass of 29 g for air. P = 102 kPaV = 2.20 LT = 310 K PV = nRT or PV / RT = n n = (102 kPa) (2.20 L) mol · K (8.31L · kPa) (310K) n = 0.087 mol air 0.087 mol air x 29g air / mol air = 2.5 g air

37. Problems A sample of nitrogen gas is confined to a 14.0 L container at 375 torr and 37.0°C. How many moles of nitrogen are in the container? –A)0.271 mol –B)2.27 mol –C)3.69 mo1 –D)206 mol –E)227 mol

38. Stoichiometric Relationships with Gases Various questions can be asked that relate gas laws to stoichiometry.

39. Problems A 250.0-mL sample of ammonia, NH 3 (g), exerts a pressure of 833 torr at 42.4°C. What mass of ammonia is in the container? –A)0.0787 g –B)0.180 g –C)8.04 g –D)17.0 g –E)59.8 g

40. Stoichiometric Relationships with Gases The ideal gas law can be used to determine density if the molar mass of the gas is known or the molar mass if the mass of gas is known d = m / V = PM / RT Density increases with molar mass

41. Problems What is the density of carbon dioxide gas at -25.2°C and 98.0 kPa? –A)0.232 g/L –B)0.279 g/L –C)0.994 g/L –D)1.74 g/L –E)2.09 g/L

42. Problems A flask with a volume of 3.16 L contains 9.33 grams of an unknown gas at 32.0°C and 1.00 atm. What is the molar mass of the gas? –A)7.76 g/mol –B)66.1 g/mol –C)74.0 g/mol –D)81.4 g/mol –E)144 g/mol

43. Problems Dr. I. M. A. Brightguy adds 0.1727 g of an unknown gas to a 125-mL flask. If Dr. B finds the pressure to be 736 torr at 20.0°C, is the gas likely to be methane, CH 4, nitrogen, N 2, oxygen, O 2, neon, Ne, or argon, Ar? –A)CH 4 –B)N 2 –C)Ne –D)Ar –E)O 2