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Gas Laws

Gas Laws. What is pressure?. Pressure is the force created by the collision of particles with the walls of their containers. As you decrease the volume of the container, the particles collide more often. Units: atm, kPa, mmHg, and torr. What is Pressure?.

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Gas Laws

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  1. Gas Laws

  2. What is pressure? • Pressure is the force created by the collision of particles with the walls of their containers. • As you decrease the volume of the container, the particles collide more often. • Units: atm, kPa, mmHg, and torr

  3. What is Pressure? • As you increase the temperature, the particles speed up, colliding more often, and with more force.

  4. What is temperature? Temperature: a measurement of the average kinetic energy of molecules Kelvin (ºC + 273) • 0 K = absolute zero; 298 K = room temperature

  5. Combined Gas Law • P1V1=P2V2 T1 T2 • Temperature in Kelvin!

  6. Kinetic Molecular Theory of Gases • 5 assumptions • Gases are made of tiny particles in constant random motion • The volume of the particles is small compared to the distance between them • Collisions between particles are completely elastic • There are no forces of attraction or repulsion between particles • The kinetic energy of the particles depends only on temperature

  7. What are Ideal Gases? • A hypothetical gas whose molecules occupy negligible space and have no interactions

  8. Ideal Gas Law • PV = nRT • n = number of moles • R = Ideal Gas Constant • depends on pressure unit • 8.314 L-kPa/mol-K • .0821 L-atm/mol-K • 62.4 L-mmHg/mol-K • Temperature in Kelvins!

  9. Example What is the volume of 0.29 mol of Fluorine if the pressure is 723 mmHg and the temperature is 28˚C?

  10. Dalton’s Law of Partial Pressures • PT = P1 + P2 + P3 + …

  11. Example A flask with a pressure of 3.56 atm contains 2 gases. If the partial pressure of gas A is 1.7 atm, what is the partial pressure of gas B?

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