1 / 12

Kinetic Theory

Kinetic Theory. Kinetic Theory of Gases. Liquids. S olids. Gases. Temperature. Pressure. Kinetic Energy. The Kelvin Scale. Kinetic Theory.

aldona
Download Presentation

Kinetic Theory

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Kinetic Theory Kinetic Theory of Gases Liquids Solids Gases Temperature Pressure Kinetic Energy The Kelvin Scale

  2. Kinetic Theory

  3. To understand the kinetic theory, we must first understand that temperature is really a measure of how fast the particlesin a substance are moving Standard Temperature = 0o C

  4. Describe the spacing and movement of the particles in each picture that follows: States of Matter

  5. Kinetic Energy Kinetic energy = the energy of motion Objects with greater kinetic energy have a higher temperature Based on what you just watched, which state of matter has the highest relative kinetic energy? Gasses

  6. Kelvin Scale • The Kelvin scale reflects the relationship between temperature and kinetic energy • For example, a container of hydrogen gas at 25 Kelvin would have half as much kinetic energy as a sample of hydrogen gas at 50 Kelvin • Absolute zero (0 Kelvin) is the temperature at which particles in a sample of matter are completely motionless

  7. Liquids Particles are fairly close together and moving fast T T melting T T T freezing evaporation condensation Solids Particles are very close together and moving very slowly Gasses Particles are far apartand moving very fast T sublimation

  8. Kinetic Theory of Gasses A gas is composed of extremely small particles(atoms or molecules) The particles are constantly moving. The particles move in straight paths The particles move independently of each other The collisions are perfectly elastic (all of the energy of one particle is transferred to another particle during a collision)

  9. Atmospheric Pressure A barometer is a tool used to measure the earth’s atmospheric pressure Think of the earth’s atmosphere like a blanket of air pushing down upon us.

  10. Gas Pressure • The pressure exerted on an object by a gas • the gas particles are constantly colliding with the sides of a container, each collision exerts a force (pushes out) on the side of the container • Added together, these many small forces create a very large collective force

  11. Units of Pressure • The standard unit of pressure is based on the pressure of the earth’s atmosphere 1 atmosphere (atm) • We can use 3 different units to measure pressure: atmospheres (atm) kilopascals (kPa) mm of Mercury (mm Hg) 1 atm = 101.3 kPa = 760 mm Hg

  12. Temperature and pressure conversions Conversion factors you will use: K = oC + 273 oC = K – 273 1 atm = 101.3 kPa = 760 mmHg • Convert the following temperature into Kelvin a. -61oC b. 927oC c. 127oC d. -255oC • Convert the following temperature into Celsius a. 500K b. 893K c. 373K d. 293K • Convert the following measurements into atm a. 1520 mmHg b. 202.6 kPa • Convert the following measurements into kPa a. 1520 mmHg b. 1.5 atm • Convert the following measurements into mmHg a. 112 kPa b. 4 atm

More Related