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According to Gay-law, Lussac’s the pressure exerted by a gas of a given mass and kept at a constant volume varies directly with its absolute temperature when the gas is kept at a constant volume (or when it is kept at a constant mass and kept at a constant volume when it is kept at a constant volume). In other words, when the mass of a gas is fixed and the volume of the gas is constant, the pressure exerted by the gas is proportional to the temperature of the gas.
In the year 1808, the French chemist Joseph Gay-Lussac came up with this law, which he published in his journal. According to Gay-law, Lussac’s the following mathematical expression can be written as follows:
P ∝ T ; P/T = k
Where:
The pressure exerted by the gas is denoted by the letter P.
The absolute temperature of the gas is denoted by the letter T.
k is a constant.
A graphic representation of the relationship between the pressure and absolute temperature of a given mass of gas (at constant volume).
Based on the graph, it can be deduced that the pressure of a gas (which is maintained at a constant volume) decreases continuously as it cools, until the gas eventually condenses and becomes a liquid.
Formula and Derivation
Because of the relationship between initial pressure and temperature and final pressure and temperature, Gay-law Lussac’s implies that the ratio of initial pressure and temperature is equal to the ratio of final pressure and temperature for a gas of fixed mass kept at a constant volume. The following is an expression for this formula:
(P1/T1) = (P2/T2)
Where:
The initial pressure is denoted by P1.
T1 is the temperature at which the experiment began.
The final pressure is denoted by P2.
The final temperature is denoted by T2.
When it comes to gas, this expression can be derived from the pressure-temperature proportionality. Since P ∝ T for gases with fixed mass but constant volume, the following is true:
When P1/T1 = k, it means the initial pressure/initial temperature are both constant.
Final pressure/final temperature equals k (final pressure/final temperature equals constant).
As a result, P1/T1 equals P2=/T2 equals k.
Alternatively, P1T2 = P2T1.
Gay-Law Lussac’s is illustrated by the following examples:
It is possible for an explosion to occur when a pressurised aerosol container (e.g., a deodorant can or a spray-paint can) is heated as a result of an increase in the pressure exerted by the gases on the container (due to Gay-law). For this reason, many pressurised containers are equipped with warning labels that state that the container must be kept away from flames and stored in a cool environment.
This section contains an illustration describing the increase in pressure that occurs when the absolute temperature of a gas is raised while the volume of the gas is maintained at its constant value. When using pressure cookers, another application of Gay-law Lussac’s can be observed. When the pressure exerted by the steam inside the container increases as the cooker heats up, the pressure inside the container increases. Because of the high temperature and pressure inside the container, the food cooks more quickly than usual.
Conclusion
When the volume of a gas is kept constant, Gay-law Lussac’s states that the pressure of a given mass of gas varies directly with the absolute temperature of the gas, and vice versa. It is a particular application of the ideal gas law. Known for the Pressure Law, which established that the pressure of an enclosed gas is directly proportional to its temperature and which he was the first to formulate, Gay-Lussac is credited with discovering the pressure law. Also, he is sometimes credited with being the first to publish convincing evidence demonstrating the relationship between the pressure and temperature of a fixed mass of gas maintained at a constant volume.
