Gas Laws
Chemistry: IB Diploma Higher Level, topic 1.5.2
Molecular Kinetic Thoery
Molecular Kinetic theory is used to explain the way gases behave.
Molecular kinetic theory
- Kinetic molecular theory states the following assumptions:
- Gas molecules are always moving and move in randomly.
- Temperature and kinetic temperature are directly proportional. Gases of different masses at a particular temperature have the same kinetic energy.
- Collisions between gas molecules are elastic (no energy is lost when gas molecules collide).
- The majority of the volume of a gas is empty space. The distance between gas molecules is much bigger than the actual gas molecules.
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Boyle’s law
- Boyle’s Law states the pressure (P) of a fixed mass of gas is inversely proportional to its volume (V) at a constant temperature.
- For the same gas under different conditions:
- P1V1 = P2V2
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Charles’ law
- Charles’ Law states the volume (V) of a fixed mass of gas is directly proportional to its volume (T) at constant pressure.
- For the same gas under different conditions:
- V1/T1 = V2/T2
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Gay-Lussac's
- Gay-Lussac's sates the pressure (P) of a fixed mass of gas is directly proportional to its absolute temperature (T) at a constant volume.
- For the same gas under different conditions:
- P1/T1 = P2/T2