Unit 6.2: Thermal physics

• Absolute Zero: The lowest possible temperature of a system, where no heat remains and the particles in the system have no kinetic energy.
• Boyle’s Law: The pressure of an ideal gas is inversely proportional to its volume when held at constant temperature.
• Avogadro Constant: The number of particles that make up one mole of any gas.
• Charles’ Law: The volume of an ideal gas is directly proportional to its absolute temperature when held at constant pressure.
• Boltzmann Constant: A constant relating the average kinetic energy of the particles in a gas, to the gas’ temperature.
• Brownian Motion: The random motion of particles.
• Ideal Gas: A gas that meets the ideal gas assumptions. All the gas laws are based on ideal gases.
• Molar Gas Constant: A fundamental constant, used in the ideal gas law.
• Internal Energy: The sum of the randomly distributed kinetic and potential energies of the particles in a given system.
• Pressure Law: The pressure of an ideal gas is directly proportional to its absolute temperature, when the volume is fixed.
• Specific Heat Capacity: The amount of energy required to increase the temperature of 1kg of a substance by 1 Kelvin.
• State Changes: During a state change, the potential energy of the system is changing but the kinetic energy is not.
• Specific Latent Heat: The amount of energy required to change the state of 1kg of a substance without a change of temperature.
• Molar Mass: The mass of one mole of the substance in question.