1.5.3 Kinetic Theory of Gases

• The Kinetic Theory of Gases explains gas behavior in terms of the motion and interactions of individual gas particles
• In the Kinetic Theory of Gases, collisions between gas particles and the container walls are assumed to be elastic
• The Kinetic Theory of Gases explains macroscopic gas properties based on the microscopic behavior of gas particles.

  True
• Greater mass and higher speed result in greater kinetic energy.

  True
• As temperature increases, the average kinetic energy of gas particles increases.


  True
• Gas particles in the Kinetic Theory are assumed to move in constant random motion.


  True
• Match the assumption of the Kinetic Theory with its description:

  Constant Random Motion ↔️ Gas particles move in all directions at varying speeds

  Negligible Volume ↔️ The volume of particles is negligible compared to the container

  Elastic Collisions ↔️ Collisions have no loss of kinetic energy
• Kinetic energy is directly proportional to the mass and the square
• Doubling the speed of an object increases its kinetic energy by a factor of four
• Lower temperatures correspond to lower average kinetic energies
• The Kinetic Theory of Gases explains the relationship between temperature and the kinetic energy of gas particles
• Lower temperatures correspond to lower average kinetic energies of gas particles.


  True
• In elastic collisions, the total kinetic energy of the system is conserved
• Increasing the velocity of an object significantly increases its kinetic energy
• What is pressure defined as in the Kinetic Theory of Gases?

  Force exerted by particles
• What increases the force and pressure exerted by gas particles in a container?

  Higher kinetic energy
• Increasing pressure reduces the volume of a gas, forcing particles to move faster.
• What is the Kinetic Theory of Gases used to explain?

  Behavior of gases
• What is the volume of individual gas particles assumed to be in the Kinetic Theory of Gases?

  Negligible
• How many main assumptions does the Kinetic Theory of Gases rely on?

  Three
• What is the formula for kinetic energy?

  $KE =$$\frac{1}{2}mv^{2}$
• What does temperature measure in terms of the Kinetic Theory of Gases?

  Average kinetic energy
• What happens to the average kinetic energy of gas particles as temperature increases?

  Increases
• Match the concept with its description:

  Temperature ↔️ Average kinetic energy

  Kinetic Energy ↔️ Square of particle velocity
• Main assumptions of the Kinetic Theory of Gases:

  1️⃣ Constant Random Motion

  2️⃣ Negligible Volume

  3️⃣ Elastic Collisions
• The volume of gas particles is negligible compared to the total gas volume.

  True
• If a car with a mass of 1000 kg travels at 20 m/s, what is its kinetic energy?

  $200,000 J$
• In the formula for pressure, $\overline{v^{2}}$ represents the average of the square of the particle speeds
• Pressure is solely due to the collisions of gas particles with the container walls.

  True
• Lower temperatures result in lower average kinetic energies of gas particles.

  True
• Why does increasing the temperature of a gas increase its average kinetic energy?

  Particles move faster
• What type of motion do gas particles exhibit according to the Kinetic Theory of Gases?

  Constant Random Motion
• What is the formula for kinetic energy?

  $KE =$$\frac{1}{2}mv^{2}$
• Temperature is directly related to the average kinetic energy of gas particles.


  True
• What happens to the motion of gas particles when temperature increases?

  Moves faster