1 / 15

The Gas Laws

The Gas Laws. A Tutorial on the Behavior of Gases. Kinetic Molecular Theory of Gases. Gases consist of small particles that are in constant random motion and are separated by great distances from one another . The individual particles occupy a negligible volume.

gerd
Download Presentation

The Gas Laws

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. The Gas Laws A Tutorial on the Behavior of Gases.

  2. Kinetic Molecular Theory of Gases • Gases consist of small particles that are in constant random motion and are separated by great distances from one another. • The individual particles occupy a negligible volume.

  3. Kinetic Molecular Theory of Gases • Collisions with walls of container are elastic and exert a measurable pressure. • Particles do not interact with one another. • Average kinetic energy is directly proportional to the Kelvin (absolute) temperature.

  4. Abbreviations P – Pressure V – Volume n – Moles R – Gas Constant T – Kelvin Temperature

  5. Units of Pressure atm - atmospheres mm Hg - millimeters of mercury torr – same as mm Hg Pa - Pascal kPa - kiloPascal

  6. Converting Pressures 1.00 atm = 760 mm Hg = 101.3 kPa = 101,300 Pa

  7. Units of Temperature K - Kelvin °C - degrees Celsius °F - degrees Fahrenheit

  8. Converting Temperatures (C x 1.8) + 32 = F (F - 32)/1.8 = C C + 273 = K

  9. Standard Conditions • STP: Standard Temperature and Pressure • Temperature: • 273 K = 0.0 °C • Pressure: • 1.00 atm = 760 mm Hg

  10. Boyles Law

  11. Robert Boyle (1627-1691) Boyle’s Law: the volume of a fixed mass of gas varies inversely with the pressure at constant temperature. Mathematically, it is expressed as PV = k Where k is a constant, V is volume and P is pressure.

  12. Sample Boyle’s Law ProblemP1V1 = P2V2#1 A gas occupies 12.3 liters at a pressure of 400 mm Hg. What is the volume when the pressure is increased to 600 mm Hg and the temperature remains constant?

  13. Answer #1

  14. Sample Boyle’s Law ProblemP1V1 = P2V2#2 • A container has volume of 13,240 L has a pressure of 4.78 atm. If the pressure inside the container becomes 260 atm, what would the new volume be?

  15. Sample Boyle’s Law ProblemP1V1 = P2V2#3 • A sample of neon occupies 105.0 L at a pressure of 190 kPa. At constant temperature, what is the volume of the neon when the pressure is increased to 631 kPa?

More Related