1. Chapter 11, Part 1 Physical Characteristics of Gases

2. Kinetic –Molecular Theory  Particles of matter (solid, liquid, or gas) are always in motion. This motion has consequences. Solid (defined shape and definite volume) Liquid (undefined shape and definite volume) Gases (undefined shape and volu)me

3. Kinetic-Molecular Theory of Gases  Gases are large numbers of tiny particles  Particles always moving in straight lines in all directions. Therefore, they have “kinetic energy”  These particles have elastic collisions between other particles and the container Elastic – no loss of KE after collision  There is no attraction or repulsion between the particles  Kinetic energy of the particles is proportional to the temperature of the matter

4. Ideal Gas vs. Real gas  Ideal Gas: Completely follows kinetic molecular theory (K-M theory) of gases  Hydrogen, maybe  Helium, sometimes  Real Gas: Does not behave by K-M theory

5. K-M theory and nature of gases  Expansion  Fluidity (liquids and gases)  Low Density  Compressibility  Diffusion

6. Characteristics 1. Expansion 2. Fluidity

7. Characteristics 3. Low density

8. Characteristics 4. Compressibility 5. Diffusion

9. 4 quantities that can be measured  Volume – How much space it takes up  Pressure – Amount of collisions particles have with container  Temperature – Average kinetic energy of the gas particles  Quantity or number of molecules – moles  We use these quantities to “work” with gases

10. Pressure  Pressure = Force / Area  Units of Pressure 1 atm = 760 mm Hg = 760 torr = 1.01 x 10 5 pascals

11. Convert a pressure of 0.830 atm to mmHg

12. Temperature Scales  Absolute zero = -273.15 o C = 0 K (not 0 o K)  Therefore K = 273 + o C  0 o C = 273 K  As temperature increases, the number of gas collisions increases.

13. Temp. conversions K = o C + 273 25.0 o C = ? K

14. STP  “Slap The Pupils” -- No  “Such Total Pigs” -- No  Standard Temperature and Pressure  The volume of a gas depends on temperature and pressure. In order to compare volumes of gases, need a standard.  0 degrees Celsius, 273 K  1 atm of pressure

15. Boyle’s Law  Volume off a fixed mass of gas varies inversely with pressure at a constant temperature

16. Robert Boyle (1627-1691)  Born at Lismore Castle, Munster, Ireland, the 14th child of the Earl of Cork.  1662, delineated the quantitative relationship that the volume of a gas varies inversely with pressure.

17. Boyle’s Law  P 1 V 1 = k and P 2 V 2 = k  Therefore P 1 V 1 = P 2 V 2

18. A sample of oxygen gas occupies a vol. of 150 mL at a pressure of 720 mmHg. What would the volume be at 750 mmHg press.?

19. France, early 1800’s  Hot air balloons were extremely popular  Scientists were eager to improve the performance of their balloons. Two of the prominent French scientists were Jacques Charles and Joseph-Louis Gay- Lussac,

21. Charles’ Law  The volume of a fixed mass of gas varies directly with the Kelvin temperature at constant pressure

23. Charles’ Law  V 1 / T 1 = V 2 / T 2

24. A sample of Ne gas has a vol. of 752 mL at 25.0 deg. C. What is the vol. at 50.0 deg. C? T 1 = 25.0 deg. C = 298 K T 2 = 50.0 deg C = 323 K V 1 = 752 mL

25. Gay-Lussac’s Law  The pressure of a fixed mass of gas varies directly with the Kelvin temp. at constant volume  P 1 / T 1 = P 2 / T 2

26. P 1 / T 1 = P 2 / T 2

27. A sample of N gas is at 3.00 atm of pressure at 25 deg C what would the pressure be at 52 deg C? P 1 = 3.00 atm T 1 = 25 deg C = 298 K T 2 = 52 deg C = 325 K P 2 = ? P 1 / T 1 = P 2 / T 2 or P 2 = P 1 T 2 / T 1

28. Combined Gas Law  Relates Pressure, Volume, and Temperature  Notice it is a combination of Boyles, Charles, and Gay-Lussac’s Laws  P 1 V 1 / T 1 = P 2 V 2 / T 2

29. A helium filled balloon has a vol. of 50.0 L at 25 deg C and 820. mmHg of pressure. What would the vol. be at 650 mmHg pressure and 10. deg C?  P 1 V 1 / T 1 = P 2 V 2 / T 2 V 1 = 50.0 L T 1 = 25 deg C = 298 K P 1 = 820. mmHg T 2 = 10. deg C = 283 K P 2 = 650 mmHg V 2 = ?

30. Molar Volume of a Gas  One mole of gas (6.02 x 10 23 molecules) has the same volume at STP (0 deg C, 1 atm) as any other gas

31. Standard Molar Volume of a Gas = 22.4 L / mol therefore 1 mol gas = 22.4 L (at STP)