Gas laws
This presentation is the property of its rightful owner.
Sponsored Links
1 / 31

Gas Laws PowerPoint PPT Presentation


  • 95 Views
  • Uploaded on
  • Presentation posted in: General

Gas Laws. Solid - Molecules are held close to each other by their attractions of charge. They will bend and/or vibrate, but will stay in close proximity.

Download Presentation

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.While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server.


- - - - - - - - - - - - - - - - - - - - - - - - - - E N D - - - - - - - - - - - - - - - - - - - - - - - - - -

Presentation Transcript


Gas laws

Gas Laws


Gas laws

  • Solid - Molecules are held close to each other by their attractions of charge. They will bend and/or vibrate, but will stay in close proximity.

  • Liquid - Molecules will flow or glide over one another, but stay toward the bottom of the container. Motion is a bit more random than that of a solid.

  • Gas - Molecules are in continual straightline motion. The kinetic energy of the molecule is greater than the attractive force between them, thus they are much farther apart and move freely of each other.


Nature of gases

Nature of Gases

  • No definite shape nor volume

  • Low density

  • Compressibility

  • Diffusion


Gas laws

  • How car engines work


Diffusion

Diffusion

  • Which molecules diffuse quicker?

    • Heavy, large

    • Light, small


Kinetic molecular theory

Kinetic Molecular Theory

  • Gases consist of large numbers of tiny particles that are far apart relative to their size

  • Collisions between gas particles and between particles and container walls are elastic (no loss of energy)

  • Gas particles are in continuous, rapid, random motion


Gas laws

  • There are no forces of attraction between gas particles

  • The temperature of gas depends on the average kinetic energy of the gas particles


Pressure

Pressure

  • Force per unit area on a surface

  • Pressure =force/ area


Gas laws

  • Increase in pressure

  • Increase in number of collisions of gas particles


Atmospheric pressure

Atmospheric Pressure

  • Weight of gases that compose the atmosphere

    • 78% nitrogen

    • 21% oxygen

    • 1% other gases


Ears pop in airplane

Ears “pop” in airplane

  • Density and pressure of air is lower

  • Air pressure inside ears changes to reach same pressure as air in cabin (6,000-8,000 ft above sea level)

  • Pressurized

    cabin


Measuring pressure

Measuring Pressure

  • Barometer- device to measure atmospheric pressure


Manometer measure pressure of an enclosed gas sample

Manometer- measure pressure of an enclosed gas sample


Standard pressure

Standard pressure

  • 760 mm of mercury (760 torr)

  • 1 atmosphere (atm)

  • 101.3 kilopascals (kPa)


Units of pressure

Units of Pressure


Practice question

Practice Question

  • The average atmospheric pressure in Denver, Colorado is 0.830 atm. Convert this to mm of Hg and kPa.

    0.830 atm x 760 mm Hg = 631 mm Hg

    1 atm

    0.830 atm x 101.3 kPa = 84.1 kPa

    1 atm


Gases collected by water displacement

Gases collected by water displacement

  • Gas produced by reaction displaces water which is more dense


Dalton s law of partial pressure

Dalton’s Law of Partial Pressure

  • Pressure of each gas in a mixture is called partial pressure

  • Dalton’s law states that the total pressure of a gas mixture is the sum of the partial pressures of the component gases

    PT= P1 + P2 + …


Gas laws1

Gas Laws

  • Boyle’s Law

  • Charles’ Law

  • Gay-Lussac’s Law


Boyle s law

Boyle’s Law

  • Pressure-volume relationship

  • Inverse relationship


Gas laws

  • PV= k

  • P1V1= P2V2

  • A sample of oxygen has a volume of 150.0 mL when its pressure is 0.947 atm. What will the volume of the gas be at a pressure of 0.987 atm if the temperature remains constant?

  • (0.947 atm)(150.0 mL)=(0.987 atm) V2

  • V2= 144 mL


Charles law

Charles’ Law

  • Volume- temperature relationship

  • Direct relationship

  • V = k

    T

  • V1 = V2

    T1 T2

Always use Kelvin temperature


Gas laws

  • A sample of neon gas occupies a volume of 752 mL at 25 degrees Celsius. What volume will the gas occupy at 50 degrees Celsius if the pressure remains constant?

  • 752 mL = V2

    298 K 323 K

  • V2= 815 mL


Gay lussac s law

Gay-Lussac’s Law

  • Pressure-temperature relationship

  • Direct relationship

  • P = k

    T

  • P1 = P2

    T1 T2

Always use Kelvin temperature


Gas laws

  • The gas in a container is at a pressure of 3.00 atm at 25 degrees Celsius. What would the gas pressure in the container be at 52 degrees Celsius?

  • 3.00 atm = P2

    298 K 325 K

  • P2= 3.27 atm


Combined gas law

Combined Gas Law

  • If something is constant in the problem, it can be canceled out


Gas laws

  • A helium balloon has a volume of 50.0 L at 25 degrees Celsius and 1.08 atm. What volume will it have at 0.855 atm and 10 degrees Celsius.

  • (1.08 atm) (50.L) = (0.855 atm)V2

    298 K 283 K

    V2= 60.0 L


Gas laws

  • A sample of helium gas has a volume of 200.0 mL at 0.960 atm. What pressure is needed to reduce the volume at constant temperature to 50.0 mL?

  • (0.960 atm)(200.0 mL) = P2 (50.0 mL)

  • P2= 3.84 atm


Scuba

SCUBA

  • Gas Laws WebQuest


  • Login