Overview
This lecture explains the relationship between gas temperature and particle energy, and describes how temperature changes affect the pressure of a gas.
Particle Behavior in Gases
- Gas particles are far apart and move in constant, random motion.
- Gas pressure is caused by particles colliding with the walls of their container.
Temperature, Kinetic Energy, and Pressure
- Gas temperature is directly related to the average kinetic energy of its particles.
- Lower temperature means particles have less kinetic energy, resulting in fewer and less energetic collisions.
- At low temperatures, gas pressure is relatively low due to less frequent and weaker collisions.
- Higher temperature means particles have more kinetic energy, resulting in more frequent and more energetic collisions.
- At high temperatures, gas pressure is relatively high due to more frequent and stronger collisions.
- Increasing the temperature of a gas increases both the number and energy of collisions, thereby increasing pressure.
Key Terms & Definitions
- Pressure — The force exerted by gas particles colliding with the walls of their container.
- Kinetic Energy — The energy of motion; in gases, average kinetic energy is directly related to temperature.
- Temperature (of a gas) — A measure of the average kinetic energy of the particles in a gas.
Action Items / Next Steps
- Practice questions on gas pressure in the revision workbook as recommended.