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Applied Physics and Chemistry

Explore the properties of gases, including no definite shape, volume, easy compressibility, and complete mixing capabilities. Learn about pressure, kinetic molecular theory, measuring techniques with barometers, and pressure units conversions in this lecture.

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Applied Physics and Chemistry

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  1. Applied Physics and Chemistry Gases Lecture 1

  2. Gases • Properties: • No definite shape • No definite volume • Easily compressed • Mixes completely with any other gas

  3. Pressure • Kinetic molecular theory: • All particles of matter are in constant motion • Particles of a gas move fast and hit the container • Pressure: • Force of collisions of gas particles over an area of the container

  4. Pressure! http://www.atmos.washington.edu/2005Q3/101/LINKS-html/MercuryBarometer.html • Atmosphere: • Due to the pull of gravity on gases • Measured by barometer • Evangelista Torricelli (1608-1647) • Measuring: • Mercury barometer • Anaeroid barometer http://www.free-online-private-pilot-ground-school.com/Aviation-Weather-Principles.html

  5. Measuring Pressure • Units commonly used: • Torricelli (torr) • Millimeters of mercury (mmHg) • Atmosphere (standard atmosphere) (atmo) • SI: Pascal (Pa)

  6. Pressure conversions • 1 atmosphere = • 760 mm Hg • 760 torr • 101 325 Pa • 101.325 kPa • 14.69 psi (ACK!) • Use conversion factors (carefully showing ALL WORK) to convert from one unit to another!

  7. Example of conversion! • The pressure of air in a tire is recorded as 192 000 Pa. What is this pressure in atmospheres? • What we know: • P = 192 000 Pa • Conversion factors: • 1 atmo = 101 325 Pa • 192 000 Pa x 1 atmo = 1.895 atmo • 101 325 Pa

  8. Another Example: • On a summer day in Breckenridge CO, the atmospheric pressure is 525 mm Hg. What is this pressure in atmospheres? • What we know: • P = 525 mm Hg • Conversion factor: • 1 atmo = 760 mm Hg • Do the math! • 525 mm Hg x 1 atmo = 0.69 atmo • 760 mm Hg

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