Answer:

Boyle's law, also referred to as the Boyle–Mariotte law, or Mariotte's law (especially in France), is an experimental gas law that describes how the pressure of a gas tends to decrease as the volume of the container increases. A modern statement of Boyle's law is:

The absolute pressure exerted by a given mass of an ideal gas is inversely proportional to the volume it occupies if the temperature and amount of gas remain unchanged within a closed system.[1][2]

Mathematically, Boyle's law can be stated as:

{\displaystyle P\propto {\frac {1}{V}}}P\propto {\frac {1}{V}} Pressure is inversely proportional to the volume

or

PV = k Pressure multiplied by volume equals some constant k

where P is the pressure of the gas, V is the volume of the gas, and k is a constant.

The equation states that the product of pressure and volume is a constant for a given mass of confined gas and this holds as long as the temperature is constant. For comparing the same substance under two different sets of conditions, the law can be usefully expressed as:

{\displaystyle P_{1}V_{1}=P_{2}V_{2}.}P_{1}V_{1}=P_{2}V_{2}.

This equation shows that, as volume increases, the pressure of the gas decreases in proportion. Similarly, as volume decreases, the pressure of the gas increases. The law was named after chemist and physicist Robert Boyle, who published the original law in 1662.

Charles's law (also known as the law of volumes) is an experimental gas law that describes how gases tend to expand when heated. A modern statement of Charles's law is:

When the pressure on a sample of a dry gas is held constant, the Kelvin temperature and the volume will be in direct proportion.[1]

This relationship of direct proportion can be written as:

{\displaystyle V\propto T}{\displaystyle V\propto T}

So this means:

{\displaystyle {\frac {V}{T}}=k,\quad {\text{or}}\quad V=kT}{\displaystyle {\frac {V}{T}}=k,\quad {\text{or}}\quad V=kT}

where:

V is the volume of the gas,

T is the temperature of the gas (measured in kelvins),

and k is a non-zero constant.

This law describes how a gas expands as the temperature increases; conversely, a decrease in temperature will lead to a decrease in volume.

Gay-Lussac's law (more correctly referred to as Amonton's law[citation needed]) states that the pressure of a given mass of gas varies directly with the absolute temperature of the gas when the volume is kept constant.[1]

Mathematically, it can be written as: {\displaystyle {\frac {P}{T}}=k}{\displaystyle {\frac {P}{T}}=k}. It is a special case of the ideal gas law.

Gay-Lussac is incorrectly[citation needed] recognized 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 (c. 1809).[2] He is also sometimes credited[3][4][5] with being the first to publish convincing evidence that shows the relationship between the pressure and temperature of a fixed mass of gas kept at a constant volume.[4]

These laws are also known variously as the Pressure Law or Amontons's law and Dalton's law respectively.[

The combined gas law combines the three gas laws: Boyle's Law, Charles' Law, and Gay-Lussac's Law. It states that the ratio of the product of pressure and volume and the absolute temperature of a gas is equal to a constant. ... The constant k is a true constant if the number of moles of the gas doesn't change.

Avogadro's law (sometimes referred to as Avogadro's hypothesis or Avogadro's principle) or Avogadro-Ampère's hypothesis is an experimental gas law relating the volume of a gas to the amount of substance of gas present.[1] The law is a specific case of the ideal gas law. A modern statement is:

Avogadro's law states that "equal volumes of all gases, at the same temperature and pressure, have the same number of molecules."[1]

For a given mass of an ideal gas, the volume and amount (moles) of the gas are directly proportional if the temperature and pressure are constant.

The law is named after Amedeo Avogadro who, in 1812,[2][3] hypothesized that two given samples of an ideal gas, of the same volume and at the same temperature and pressure, contain the same number of molecules. As an example, equal volumes of gaseous hydrogen and nitrogen contain the same number of atoms when they are at the same temperature and pressure, and observe ideal gas behavior. In practice, real gases show small deviations from the ideal behavior and the law holds only approximately, but is still a useful approximation for scientists.

The ideal gas law, also called the general gas equation, is the equation of state of a hypothetical ideal gas. It is a good approximation of the behavior of many gases under many conditions, although it has several limitations.