Explain all gas laws ..................
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The gas laws were developed at the end of the 18th century, when scientists began to realize that relationships between pressure, volume and temperature of a sample of gas could be obtained which would hold to approximation for all gases. Gases behave in a similar way over a wide variety of conditions because they all have molecules which are widely spaced, and the equation of state for an ideal gas is derived from kinetic theory. The earlier gas laws are now considered as special cases of the ideal gas equation, with one or more variables held constant.
Boyle's law Edit
Main article: Boyle's law
In 1662 Robert Boyle studied the relationship between volume and pressure of a gas of fixed amount at constant temperature. He observed that volume of a given mass of a gas is inversely proportional to its pressure at a constant temperature. Boyle's law, published in 1662, states that, at constant temperature, the product of the pressure and volume of a given mass of an ideal gas in a closed system is always constant. It can be verified experimentally using a pressure gauge and a variable volume container. It can also be derived from the kinetic theory of gases: if a container, with a fixed number of molecules inside, is reduced in volume, more molecules will strike a given area of the sides of the container per unit time, causing a greater pressure.
A statement of Boyle's law is as follows:
The volume of a given mass of a gas is inversely related to pressure when the temperature is constant.
The concept can be represented with these formulae:
{\displaystyle V\propto {\frac {1}{P}}}{\displaystyle V\propto {\frac {1}{P}}}, meaning "Volume is inversely proportional to Pressure", or
{\displaystyle P\propto {\frac {1}{V}}}P\propto {\frac {1}{V}}, meaning "Pressure is inversely proportional to Volume", or
{\displaystyle PV=k_{1}}PV=k_{1}, or
{\displaystyle P_{1}V_{1}=P_{2}V_{2}\,}P_{1}V_{1}=P_{2}V_{2}\,
where P is the pressure, and V is the volume of a gas, and k1 is the constant in this equation
Charles's law, or the law of volumes, was found in 1787 by Jacques Charles. It states that, for a given mass of an ideal gas at constant pressure, the volume is directly proportional to its absolute temperature, assuming in a closed system.
The statement of Charles's law is as follows: the volume (V) of a given mass of a gas, at constant pressure (P), is directly proportional to its temperature (T). As a mathematical equation, Charles's law is written as either:
{\displaystyle V\propto T\,}V\propto T\,, or
{\displaystyle V/T=k_{2}}V/T=k_{2}, or
{\displaystyle V_{1}/T_{1}=V_{2}/T_{2}}V_{1}/T_{1}=V_{2}/T_{2},
where "V" is the volume of a gas, "T" is the absolute temperature and k2 is a proportionality constant.
Gay-Lussac's law, Amontons' law or the pressure law was found by Joseph Louis Gay-Lussac in 1808. It states that, for a given mass and constant volume of an ideal gas, the pressure exerted on the sides of its container is directly proportional to its absolute temperature.
As a mathematical equation, Gay-Lussac's law is written as either:
{\displaystyle P\propto T\,}P\propto T\,, or
{\displaystyle P/T=k}{\displaystyle P/T=k}, or
{\displaystyle P_{1}/T_{1}=P_{2}/T_{2}}P_{1}/T_{1}=P_{2}/T_{2},
where P is the pressure, T is the absolute temperature, and k is another proportionality constant.
Avogadro's law (hypothesized in 1811) states that the volume occupied by an ideal gas is directly proportional to the number of molecules of the gas present in the container. This gives rise to the molar volume of a gas, which at STP (273.15 K, 1 atm) is about 22.4 L. The relation is given by
{\displaystyle {\frac {V_{1}}{n_{1}}}={\frac {V_{2}}{n_{2}}}\,}{\frac {V_{1}}{n_{1}}}={\frac {V_{2}}{n_{2}}}\,
where n is equal to the number of molecules of gas (or the number of moles of gas).
The Combined gas law or General Gas Equation is obtained by combining Boyle's Law, Charles's law, and Gay-Lussac's Law. It shows the relationship between the pressure, volume, and temperature for a fixed mass (quantity) of gas:
{\displaystyle PV=k_{5}T\,}{\displaystyle PV=k_{5}T\,}
This can also be written as:
{\displaystyle \qquad {\frac {P_{1}V_{1}}{T_{1}}}={\frac {P_{2}V_{2}}{T_{2}}}}\qquad {\frac {P_{1}V_{1}}{T_{1}}}={\frac {P_{2}V_{2}}{T_{2}}}
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