CHEM gases

• Diffusion: mixing of gas
• Effusion: The process of a liquid flowing through a narrow opening.... how long it takes to reach ur nose
• Kinetic Energy theory

  1. volume of individual particles is zero
  2. collision of particles with walls case pressure exerted by gas
  3. particles exert no forces on each other
  4. average kinetic energy directly related to kelvin temp of gas
• gases are the ONLY states of matter that exerts pressure
• pressure = collision
• Gases

  • exert pressure
  • uniform - fills container's shape and volume
  • moves fast and changes direction when they hit something
  • mixes completely with ANY other gas
• Pressure measurement - Barometer

  1. pressure of atmo at sea level
  2. holds 760 mmhg
• pressure measurement - Manometer

  1. open end
  2. less pressure = gas more = minus h
  3. more pressure = gas less = plus h
• Boyle

  1. t constant
  2. p1v1=p2v2
  3. V and P are inverse
• Charles

  1. p constant
  2. v1/t1 = v2/t2
  3. high temp = high kinetic energy
  4. V and T are direct
• Gay - L

  1. v constant
  2. p1/t1=p2/t2
  3. P and T are direct
• Avogradros Law

  • n1/v1 = n2/v2
  • n1/p1=n2/p2
  • MOLES
• Ideal Gas Law only used when 1 condition
• Density and Mm

  1. n=m/Mm
  2. Mm=mRT/PV
  3. m/v=d=PMm/RT
• Ideal Gas

  • gas molecules don't interact with one another
  • small sized container
  • low IMF
• Ideal gas conditions are low pressure and high temperature
• STP (Standard temp and pressure)

  • P = 1atm
  • V = 22.4L
  • T = 273K or O C
  • 1 mol = 22.4L - at STP 1 mol of ANY gas occupies 22.4L
• Dalton

  • P total = p1 + p2 + p3
  • P1 = x times P total
  • x = mole fraction = moles of gas / total gas moles