Temperature & Pressure (Cambridge O Level Physics)

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Temperature & Energy of Particles

  • Molecules in a gas move around in constant random motion at high speeds
  • Random motion means that molecules
    • Travel in no specific direction
    • Undergo sudden changes in direction if they collide with either the walls of the container, or with other molecules

Random Motion of Gas Molecules

random-motion-of-gas-particles-igcse-and-gcse-chemistry-revision-notes

Gas molecules in a container move around randomly at high speeds

  • The motion of molecules in a gas depends on the temperature of the gas
  • More specifically, the temperature of a gas is related to the average kinetic energy of the molecules
    • The hotter the gas, the higher the average kinetic energy
    • The cooler the gas, the lower the average kinetic energy
  • Since the kinetic energy is related to speed, the speed of the molecules also changes with temperature (as long as the volume of the container is constant)
    • The hotter the gas, the faster the gas molecules move
    • The cooler the gas, the slower the gas molecules move

Absolute Zero

  • In 1848, the physicist Lord Kelvin recognised that there must be a temperature at which the particles in a gas must no longer be moving, or exerting pressure on their surroundings
  • This temperature is called absolute zero and is equal to −273 °C
  • Absolute zero is defined as:

The temperature at which the molecules in a substance have zero kinetic energy 

  • This means for a system at absolute zero, it is not possible to remove any more energy from it
  • Even in space, the temperature is roughly 2.7°C above absolute zero

Where does absolute zero come from?

Pressure Law, downloadable AS & A Level Physics revision notes

At absolute zero (−273°C) particles will have no net movement. It is therefore not possible to have a lower temperature than this

Motion of Particles in a Gas

  • A feature of gases is that they fill the space of any container that they occupy
  • As the gas particles move about randomly they collide with the walls of the container and exert a pressure
  • These collisions produce a net force at right angles to the wall of the container (or any surface)
  • This pressure is defined as the force per unit area

P space equals space F over A

  • Where:
    • P = pressure exerted by the gas (Pa)
    • F = force exerted by the gas (N)
    • A = area the force acts over (m2)
  • This equation means that
    • The higher the gas pressure, the more frequently the particles collide with the container walls and the greater the force exerted per unit area
    • The lower the gas pressure, the less frequently the particles collide with the container walls and the smaller the force exerted per unit area

Pressure & Force in a Gas

molecules-&-force, IGCSE & GCSE Physics revision notes

Gas molecules bouncing off the walls of a container

  • The pressure of a gas also depends on the temperature of the gas
    • This is because particles move with more energy as their temperature increases
    • As the temperature of the gas decreases, the pressure on the container also decreases

Gas Molecules in a Container

Gas molecules in a box_2, downloadable AS & A Level Physics revision notes

Gas molecules hit the sides of the container and exert a force, which creates pressure

Examiner Tip

You can experience the force exerted by a gas yourself by closing your mouth and forcing air into your cheeks

The strain you feel on your cheeks is due to the increased pressure of the gas particles pushing at right angles to your cheeks

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Katie M

Author: Katie M

Expertise: Physics

Katie has always been passionate about the sciences, and completed a degree in Astrophysics at Sheffield University. She decided that she wanted to inspire other young people, so moved to Bristol to complete a PGCE in Secondary Science. She particularly loves creating fun and absorbing materials to help students achieve their exam potential.