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When the volume of a gas is held constant, Gay-law Lussac’s (also known as Amonton’s law) asserts that the pressure of a given amount of gas varies directly with the absolute temperature of the gas. It may be stated mathematically as P/T=K. It’s a variation on the ideal gas law. Gay-Lussac is most known for his formulation of the Pressure Law, which states that the pressure of a confined gas is precisely proportional to its temperature (c. 1809). He is also recognised for being the first to provide solid data demonstrating the link between pressure and temperature of a given amount of gas maintained at a constant volume.
These laws are also known as Amontons’ law and Dalton’s law, respectively.
Pressure-Temperature Concept
The link between the pressure and temperature of a fixed amount of gas held at a constant volume was found by Gay-Lussac between 1800 and 1802, and is known as Gay-law Lussac’s of pressure–temperature. While constructing a “air thermometer,” Gay Lussac observed this.
The absolute temperature of a gas of given mass and volume is exactly proportional to its pressure.
If a gas’s temperature rises, its pressure rises as well, assuming the gas’s mass and volume remain unchanged. If the temperature is measured on an absolute scale, such as in kelvins, the rule has a particularly simple mathematical version. After that, the law may be stated numerically as:
P ∝ T ; P/T = k
where:
- P is the pressure of the gas,
- T is the temperature of the gas (measured in kelvins),
- k is a constant.
This equation holds because temperature is a measure of a substance’s average kinetic energy; when a gas’s kinetic energy rises, its particles hit the container walls more quickly, increasing pressure.
The law can be expressed as follows for comparing the same material under two distinct sets of conditions:
Because Amontons found the law first, Gay-name Lussac’s has become synonymous with the law of combining volumes explained earlier in this section. Gay-law Lussac’s is still used in some beginning physics textbooks to describe the pressure-temperature relationship. Gay-research Lussac’s focused on the link between volume and temperature, and he published his findings in 1802, but he also compared pressure and temperature. Given their respective technological capabilities, Amontons was limited to working with air as a gas, but Gay-Lussac was able to experiment with a variety of common gases, including oxygen, nitrogen, and hydrogen. Because he utilised most of Jacques Charles’s unpublished data from 1787, Gay-Lussac credited his results to him, and the rule became known as Charles’s law or the Law of Charles and Gay-Lussac.
The combined gas law is made up of Gay-(Amontons’) Lussac’s law, Charles’s law, and Boyle’s law. The ideal gas law may be used to generalise these three gas laws, as well as Avogadro’s law.
Varies Directly
When the volume is held constant, Gay-Law Lussac’s asserts that the pressure of a given amount of gas varies directly with the absolute temperature of the gas. The sole difference between Gay-Law Lussac’s and Charles’s Law is the type of container used.
Isochore
On the Kelvin scale, the temperature is measured here. Because the volume here is constant, the graph for Gay- Lussac’s Law is termed an isochore.
Conclusion
The pressure of the gas increases as the temperature rises. Gay-Lussac Law is the name given to this type of connection. Conclusion: The goal of this experiment is to learn more about the relationship between pressure, temperature, and volume in a gas.
