InformaTION:
3. GAY LUSSAC’s LAW
Did you know?
- When the temperature of a sample of gas in a rigid container is increased, the pressure of the gas increases as well. The increase in kinetic energy results in the molecules of gas striking the walls of the container with more force, resulting in a greater pressure. The French chemist Joseph Gay-Lussac (1778- 1850) discovered the relationship between the pressure of gas and its absolute temperature.
- The relationship between the pressure and absolute temperature of a given mass of gas (at constant volume) can be illustrated graphically as follows.
- From the graph, it can be understood that the pressure of a gas (Kept at constant volume) reduces constantly as it is cooled until the gas eventually undergoes condensation and becomes a liquid.
Gay-Lussac's law implies that the ratio of the initial pressure and temperature is equal to the ratio of the final pressure and temperature for a gas of a fixed mass kept at a constant volume. This formula can be expressed as follows: P1/T1=K=P2/T2
WHEREIN:
P1-is the initial pressure
P2-is the final pressure
T1-is the initial temperature
T2-is the final temperature