Gas Law's Unit Assessment

KMT
Conceptual questions about relationships between pressure, volume, temperature, and number of moles
Particle Diagrams
Gas Law Calculations
Unit Conversions

Kinetic-Molecular Theory

  • A theory that explains the states of matter and is based on the idea that matter is composed of tiny particles that are always in motion

  • Helps explain observable properties and behaviors of solids, liquids, and gases

  • Applies to Ideal Gas

  • Gas atoms/molecules move rapidly and randomly

    • The fast motion of gas particles gives them relatively large amount of kinetic energy

    • Even at room temperature, a molecule of oxygen travels at a speed of about 500 meters per second

    • At higher temperatures, the gas particles have even more energy and move even faster

    • This movement is random since the particles are moving/colliding too fast for us to predict


  • Gas particles are really spaced out

    • The size of the particles doesn’t matter. We treat all gases (ex. CO2 molecules as tiny spheres)

      • This means that we can compress gases – but this takes energy

      • The particles of gas may either be atoms or molecules

    • Ex: Squeezing a balloon


  • Gas particles bounce off each other without losing energy

    • In the real world, some energy is lost to friction

    • Elastic Collision: When there is no overall loss of kinetic energy; kinetic energy may be transferred from one particle to another during elastic collision, but there is no change in the total energy


  • Kinetic Energy: The energy an object possesses because of its motion

  • Ideal Gas: An imaginary gas whose behaviour fits perfectly fits all five assumptions of the Kinetic Molecular Theory

  • Real Gases: Gases that don’t follow KMT assumptions


Basic Gas Laws

  • Gay-Lussac Law: At constant volume (v) and moles (n); Pressure (P) & Temperature (T) are directly related

    • Equation: P1 / T1 = P2 / T2

    • Acronym: GPT

  • Charles Law: At constant pressure and moles, Volume (V) and Temperature (T) are directly related

    • Equation: V1 / T1 = V2 / T2

    • Acronym: CVT


  • Boyles Law: At constant temperature and moles; Pressure (P) and Volume (V) are inversely related

  • Equation: P1 ⋅ V1 = P1 ⋅ V2

  • Acronym: BPV


Ideal Gas Law

  • Equation PV = nRT

    OR


  • R = Universal gas constant

  • Have to use L


Combined Gas Law

  • PV/T = K

    OR



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