Gas law
Gas laws are a set of physical principles that describe the behavior of gases. These laws are fundamental to the understanding of physical science and chemistry. They describe how gases behave under varying conditions of pressure, volume, and temperature.
History[edit | edit source]
The development of gas laws began in the 17th century with the work of scientists such as Robert Boyle and Jacques Charles. Boyle's Law, established in 1662, states that the pressure and volume of a gas have an inverse relationship when temperature is held constant. Charles' Law, formulated in 1787, states that volume and temperature of a gas have a direct relationship when pressure is held constant.
Boyle's Law[edit | edit source]
Boyle's Law states that the pressure (P) and volume (V) of a gas are inversely proportional at a constant temperature. This means that as the volume of a gas increases, its pressure decreases and vice versa. The mathematical representation of Boyle's Law is P1V1 = P2V2, where P1 and V1 are the initial pressure and volume, and P2 and V2 are the final pressure and volume.
Charles' Law[edit | edit source]
Charles' Law states that the volume (V) of a gas is directly proportional to its absolute temperature (T) at a constant pressure. This means that as the temperature of a gas increases, so does its volume, and vice versa. The mathematical representation of Charles' Law is V1/T1 = V2/T2, where V1 and T1 are the initial volume and temperature, and V2 and T2 are the final volume and temperature.
Avogadro's Law[edit | edit source]
Avogadro's Law, named after scientist Amedeo Avogadro, states that equal volumes of gases, at the same temperature and pressure, contain an equal number of molecules. This law is fundamental to the theory of molecular gases.
Ideal Gas Law[edit | edit source]
The Ideal Gas Law is a combination of Boyle's Law, Charles' Law, and Avogadro's Law. It states that the pressure of a gas times its volume is directly proportional to the number of moles of gas and the temperature. The Ideal Gas Law is represented as PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is temperature.
Real Gas Law[edit | edit source]
The Real Gas Law, also known as the van der Waals equation, accounts for the behavior of real gases which deviate from the Ideal Gas Law due to intermolecular forces and molecular size.
See also[edit | edit source]
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