Gas Laws by VIVIAN PALOMAREZ https://padlet.com/188621/iu1mmyw9vbb2mr en-us 2019-02-06 15:54:07 UTC 2025-12-25 10:04:08 UTC hello@padlet.com https://padlet-assets.s3.amazonaws.com/icons/Lightdecrease.png Boyles Law 188621 https://padlet.com/188621/iu1mmyw9vbb2mr/wish/329244654 Boyle’s law, also called Mariotte’s law,  a relation concerning the compression and expansion of a gas at constant temperature. ]]> 2019-02-08 15:31:22 UTC https://padlet.com/188621/iu1mmyw9vbb2mr/wish/329244654 Boyles Law 188621 https://padlet.com/188621/iu1mmyw9vbb2mr/wish/329247964  pressure (p) of a given quantity of gas varies inversely with its volume (v) at constant temperature; i.e., in equation form, pv = k, a constant. The relationship was also discovered by the French physicist Edme Mariotte (1676).]]> 2019-02-08 15:37:04 UTC https://padlet.com/188621/iu1mmyw9vbb2mr/wish/329247964 Boyles life 188621 https://padlet.com/188621/iu1mmyw9vbb2mr/wish/329250017 Robert Boyle, (born January 25, 1627, Lismore Castle, County Waterford, Ireland—died December 31, 1691, London, England),. 17th-century intellectual culture. He was best known as a natural philosopher, particularly in the field of chemistry, but his scientific work covered many areas including hydrostatics, physics, medicine, earth sciences, natural history, and alchemy.]]> 2019-02-08 15:40:22 UTC https://padlet.com/188621/iu1mmyw9vbb2mr/wish/329250017 Jacques Charles 188621 https://padlet.com/188621/iu1mmyw9vbb2mr/wish/329911337 Jacques Charles, in full Jacques-Alexandre-César Charles, (born November 12, 1746, Beaugency, France—died April 7, 1823, Paris), French mathematician, physicist, and inventor who, with Nicolas Robert, was the first to ascend in a hydrogen balloon (1783). About 1787 he developed Charles’s law concerning the thermal expansion of gases.]]> 2019-02-11 15:32:09 UTC https://padlet.com/188621/iu1mmyw9vbb2mr/wish/329911337 Charles Law 188621 https://padlet.com/188621/iu1mmyw9vbb2mr/wish/329918727 Charles’s law, a statement that the volume occupied by a fixed amount of gas is directly proportional to its absolute temperature, if the pressure remains constant.]]> 2019-02-11 15:42:21 UTC https://padlet.com/188621/iu1mmyw9vbb2mr/wish/329918727 Avogadro's Law 188621 https://padlet.com/188621/iu1mmyw9vbb2mr/wish/330375048 Avogadro’s law, a statement that under the same conditions of temperature and pressure, equal volumes of different gases contain an equal number of molecules. This empirical relation can be derived from the kinetic theory of gases under the assumption of a perfect (ideal) gas. The law is approximately valid for real gases at sufficiently low pressures and high temperatures.]]> 2019-02-12 15:20:13 UTC https://padlet.com/188621/iu1mmyw9vbb2mr/wish/330375048 Dalton's Law 188621 https://padlet.com/188621/iu1mmyw9vbb2mr/wish/330386693 Dalton’s law, the statement that the total pressure of a mixture of gases is equal to the sum of the partial pressures of the individual component gases. The partial pressure is the pressure that each gas would exert if it alone occupied the volume of the mixture at the same temperature.]]> 2019-02-12 15:39:44 UTC https://padlet.com/188621/iu1mmyw9vbb2mr/wish/330386693 Ideal Gas https://padlet.com/188621/iu1mmyw9vbb2mr/wish/330854125 Perfect gas, also called ideal gas, a gas that conforms, in physical behaviour, to a particular, idealized relation between pressure, volume, and temperature called the general gas law. This law is a generalization containing both Boyle’s law and Charles’s law as special cases and states that for a specified quantity of gas, the product of the volume v and pressure p is proportional to the absolute temperature t; i.e., in equation form, pv = kt, in which k is a constant. Such a relation for a substance is called its equation of state and is sufficient to describe its gross behaviour.


]]> 2019-02-13 15:33:06 UTC https://padlet.com/188621/iu1mmyw9vbb2mr/wish/330854125 Ideal Gas https://padlet.com/188621/iu1mmyw9vbb2mr/wish/330855183 The general gas law can be derived from the kinetic theory of gases and relies on the assumptions that (1) the gas consists of a large number of molecules, which are in random motion and obey Newton’s laws of motion; (2) the volume of the molecules is negligibly small compared to the volume occupied by the gas; and (3) no forces act on the molecules except during elastic collisions of negligible duration.

Although no gas has these properties, the behaviour of real gases is described quite closely by the general gas law at sufficiently high temperatures and low pressures, when relatively large distances between molecules and their high speeds overcome any interaction. A gas does not obey the equation when conditions are such that the gas, or any of the component gases in a mixture, is near its condensation point, the temperature at which it liquefies.

]]> 2019-02-13 15:34:46 UTC https://padlet.com/188621/iu1mmyw9vbb2mr/wish/330855183 Ideal Gas https://padlet.com/188621/iu1mmyw9vbb2mr/wish/330856557 PV=nRT]]> 2019-02-13 15:36:48 UTC https://padlet.com/188621/iu1mmyw9vbb2mr/wish/330856557