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• Kinetic Molecular Theory (KMT)

  • no intermolecular forces, tiny volume, elastic collisions = no forces exerted by particles , and follow random motion.
  • Average Kinetic Energy (KE): Proportional to temperature in Kelvin; as temperature increases, KE increases. Temp = ke
• Ideal gasses =

  No IMF → no attraction

  High temperature → high kinetic energy, move faster

  Low pressure → gas particles are spaced far apart. This means there are fewer chances for them to bump into each other- less gas molecules

  Small molecules of gas / Lower molar mass → promotes faster particle movement and reduces interaction likelihood.
• • Diffusion: Gasses mixing together in a larger space.
• • Effusion: Gasses escaping through a small hole
• • P and moles proportional
• • M and velocity/speed inversely proportional
• • P and volume inversely proportional
• • Volume and t portional
• • P and t promotional
• • Mole fraction = X = n gas/ n total 
• • N gas/ n total = p gas / p total
• • Density Equation: d=PMm/RT​​
• • Dalton’s Law of Partial Pressures: Ptotal=P1+P2+P3+…
  • Partial Pressure: Ppartial=Mole Fraction×Ptotal
• Combined Gas Law :(P1V1)/T1=(P2V2)/T2
• Avogadro’s Law: n1/V1=n2/V2