The Gas Laws

properties Thornburg 2014

The gas laws are a set of empirical laws that describe the relationship between temperature (T), pressure (P) and volume (V) of gasses. They are a loose collection of rules developed between the late Rennaissance and early 19th century. The three gas laws: Boyle's law (1662, relatingBoyle's law pressure and volume): P1 V1 = P2 V2 Charles's law (1787, relating volume and temperature):Charles's law V1 / T1 = V2 / T2 Gay-Lussac's law (1809, relating temperature and pressure)Gay-Lussac's law P1 / T1 = P2 / T2 Thornburg 2014

Boyle’s Law Boyle's Law is named after the Irish natural philosopher Robert Boyle ( ) who was the first to publish it in 1662.Robert Boyle Boyle’s law states that at constant temperature, the pressure and the volume of a gas are inversely proportional. P1 V1 = P2 V2 Thornburg 2014

Charles’ Law Around 1787 Charles did an experiment where he filled 5 balloons to the same volume with different gases. He then raised the temperature of the balloons to 80 ˚ C and noticed that they all increased in volume by the same amount. This unpublished experiment demonstrated the direct relationship between the volume and temperature of a gas, which was named "Charles' Law" in honor of Jacques Charles' original experiment. The formula he created was V 1 = V 2 T 1 T 2

Thornburg 2014

Gay – Lussac’s Law Gay-Lussac's law describes the relationship between temperature and pressure of a gas, when volume is held constant. Gay – Lussac determined that there is a direct relationship between pressure and temperature named after the French chemist Joseph Louis Gay – Lussac P1 = P2 T1 T2 Thornburg 2014