Chem 9

• Kinetic Molecular Theory

  1. Gases have zero volume and are very far apart
• Kenetic Molecular Theory

  2. Gases move in straight lines and do not interact at all
• Kenetic Molecular Theory

  3. Gases do not attract or repel each other
• Kenetic Molecular Theory

  4. Average KE of gases is the same in proportion (proportional) to Kelvin Temperature
• Boyles Law

  P1V1 = P2V2 (as Pressure goes up, Volume goes down)
• Charles Law

  V1/T1 = V2/T2 (As Volume goes up, temperature goes up)
• Gay-Lussac Law

  P1/T1 = P2/T2 (As temperature goes up, pressure goes up)
• Combined Gas Law

  P1V1/T1 = P2V2/T2
• Avagadro's Law

  n1/V1 = n2/V2 (as the moles of a gas in ballon increase, the volume increases)
• Gas Law Constant

  PV = nRT
• Dalton's Law of Partial P

  Pt (total pressure) = Pp + Pp + Pp
• Also Avagadros Law

  PV/n
• Ridgid means that-

  volume can't change
• Molecular Weight

  MV = g / mol (n)