1 / 17

Kinetic Molecular Theory

Kinetic Molecular Theory. The 3 states of matter are affected by 3 factors. The space between particles. The motion of the particles The energy of the matter. Solids can be described as. Particles very close together Particles move very slowly and vibrate in place Lowest amount of energy.

samson-conrad
Download Presentation

Kinetic Molecular 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 Molecular Theory

  2. The 3 states of matter are affected by 3 factors • The space between particles. • The motion of the particles • The energy of the matter.

  3. Solids can be described as • Particles very close together • Particles move very slowly and vibrate in place • Lowest amount of energy

  4. Liquids can be described as • More space between particles than solids • Able to move around each other • More energy than solids but less than gases.

  5. Gases can be described as • Particles very far apart. • Move very rapidly. • Highest amount of energy.

  6. Kinetic Molecular Theory (KMT) • Matter is made of tiny particles in constant motion • As energy is added particles move faster • In the gas phase there is no attraction between particles. • Pressure of a gas is caused by the collisions of particles with the wall of the container.

  7. Properties of Gases • Compressibility: a measure of how much the volume of matter decreases under pressure. • Gases are easily compressed because of the space between the particles. (remember KMT)

  8. Factors Affect Gas Pressure 1. Amount of Gas:by adding gas you increase the particles and number of collisions so the pressure increases, and vise versa.

  9. 2. Volume of Gas: by increasing the volume you increase the space that the particles can move in. Thus the pressure decreases as the number of collisions decreases, and vice versa.

  10. 3. Temperature: as the temperature increases the kinetic energy of the particles increases and they hit the walls of the container and each other with more energy, increasing the pressure, and vice versa. Warm temp.Hot temp.Cold temp.

  11. The Gas Laws • Boyle’s Law: If the temperature is constant, as the pressure of a gas increases, the volume decreases. P1V1 = P2V2

  12. Pressure units: kpa, atm, mmHg, psi, torr 101.3 kPa = 1 atm = 760 mmHg STP Standard Temperature and Pressure the values are 0°C and 101.3 kPa or 0°C and 1.0 atm or 0°C and 760 mmHg Volume units : mL or L Temperature units : C° or K However all calculations must have temperature in Kelvin when working gas law problems To change C° to Kelvin : C° + 273 = K

  13. Charles Law: As the temperature of an enclosed gas increases, the volume increases, if the pressure is constant.

  14. Gay-Lussac’s Law: As the temperature of an enclosed gas increases, the pressure increases, if the volume is constant.

  15. The Combined Gas Law: all three gas laws combined.

  16. Ideal Gas Law: includes the number of particles (n= moles) and the ideal gas constant (related to pressure).

More Related