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Understanding the Physical Properties of Gases and the Kinetic Molecular Theory

This guide provides a comprehensive overview of the physical properties of gases based on the Kinetic Molecular Theory. It covers the characteristics of ideal gases, including their lack of volume, elastic collisions, and constant motion. Key concepts such as temperature in Kelvin, gas laws (Boyle's, Charles', and Gay-Lussac's), and their applications in real-world problems are explained. Significantly, the importance of standard temperature and pressure (STP) is discussed, which is crucial for understanding gas behavior and calculations in various scientific fields.

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Understanding the Physical Properties of Gases and the Kinetic Molecular Theory

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  1. I. Physical Properties

  2. A. Kinetic Molecular Theory • Particles in an ideal gas… • have no volume. • have elastic collisions. • are in constant, random, straight-line motion. • don’t attract or repel each other. • have an avg. KE directly related to Kelvin temperature.

  3. C. Characteristics of Gases • Gases expand to fill any container. • random motion, no attraction • Gases are fluids (like liquids). • no attraction • Gases have very low densities. • no volume = lots of empty space

  4. C. Characteristics of Gases • Gases can be compressed. • no volume = lots of empty space • Gases undergo diffusion & effusion. • random motion

  5. D. Temperature K = ºC + 273 ºF -459 32 212 ºC -273 0 100 K 0 273 373 • Always use absolute temperature (Kelvin) when working with gases.

  6. E. Pressure Which shoes create the most pressure?

  7. E. Pressure Aneroid Barometer Mercury Barometer • Barometer • measures atmospheric pressure

  8. E. Pressure U-tube Manometer Bourdon-tube gauge • Manometer • measures contained gas pressure

  9. E. Pressure • KEY UNITS AT SEA LEVEL 101.325 kPa (kilopascal) 1 atm 760 mm Hg 760 torr 14.7 psi

  10. F. STP Standard Temperature & Pressure 0°C273 K 1 atm101.325 kPa -OR- STP

  11. V T P II. The Gas LawsBOYLESCHARLESGAY-LUSSAC

  12. A. Boyle’s Law P V PV = k

  13. A. Boyle’s Law P V • The pressure and volume of a gas are inversely related • at constant mass & temp PV = k

  14. B. Charles’ Law V T

  15. B. Charles’ Law V T • The volume and absolute temperature (K) of a gas are directly related • at constant mass & pressure

  16. C. Gay-Lussac’s Law P T

  17. C. Gay-Lussac’s Law P T • The pressure and absolute temperature (K) of a gas are directly related • at constant mass & volume

  18. D. Combined Gas Law P1V1 T1 P2V2 T2 = P T V T PV T PV = k P1V1T2 =P2V2T1

  19. E. Gas Law Problems • A gas occupies 473 cm3 at 36°C. Find its volume at 94°C. CHARLES’ LAW GIVEN: V1 = 473 cm3 T1 = 36°C = 309K V2 = ? T2 = 94°C = 367K T V WORK: P1V1T2 = P2V2T1 (473 cm3)(367 K)=V2(309 K) V2 = 562 cm3

  20. E. Gas Law Problems • A gas occupies 100. mL at 150. kPa. Find its volume at 200. kPa. BOYLE’S LAW GIVEN: V1 = 100. mL P1 = 150. kPa V2 = ? P2 = 200. kPa P V WORK: P1V1T2 = P2V2T1 (150.kPa)(100.mL)=(200.kPa)V2 V2 = 75.0 mL

  21. E. Gas Law Problems • A gas occupies 7.84 cm3 at 71.8 kPa & 25°C. Find its volume at STP. COMBINED GAS LAW P T V GIVEN: V1=7.84 cm3 P1=71.8 kPa T1=25°C = 298 K V2=? P2=101.325 kPa T2=273 K WORK: P1V1T2 = P2V2T1 (71.8 kPa)(7.84 cm3)(273 K) =(101.325 kPa)V2 (298 K) V2 = 5.09 cm3

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