Kinetic theory

• Molecules in Random Motion


  A fundamental concept in kinetic theory: molecules are in constant, random motion due to their thermal energy.
• Temperature


  A measure of the average kinetic energy of particles in a system, directly proportional to the particles' motion.
• Gas Molecule Motion


  In a gas, molecules experience elastic collisions, maintaining their total kinetic energy and direction of motion.
• Root Mean Squared Speed (rms)

  A way to calculate the average speed of particles, with the symbol "c" often used for this value.
• Molecular Speed Distribution


  The distribution of speeds of gas molecules in a system, described by the Maxwell-Boltzmann distribution.
• Kinetic Energy Per Molecule (1/2mv^2)

  The energy of a molecule due to its motion, half the product of the mass and the square of the velocity.
• Viscosity


  The resistance to flow or motion between particles, resulting from their interactions and Brownian motion.
• Brownian Motion


  The random movement of particles due to collisions with surrounding particles, influencing viscosity.
• Perfect Gas


  A hypothetical ideal gas with no molecular interactions, obeying the ideal gas equation (pV = nRT).