Boyle’s LawFor a gas, pressure and volume are inversely proportional.If you keep everything else constant, then asthe pressure on a gas goes up, its volume goes down.As the volume a gas occupies goes up, its pressuregoes down.Robert Boyle stated the inverse relationship between pressure and volume as a Gas Law.Boyle’s Lawsays that for a given amount of gas, at fixed temperature, pressure and volume are inverselyproportional.P1/V∝.You can write this mathematically asP = k/V. As per Boyle’s law, any change inthe volume occupied by a gas (at constant quantity and temperature) will result in a change in thepressure exerted by it. This law can be expressed mathematically asP1V1 = P2V2This expression can be obtained from the pressure-volume relationship suggested by Boyle’s law. For afixed amount of gas kept at a constant temperature, PV = k. Therefore,P1V1 = k(initial pressure * initial volume)P2V2 = k(final pressure * final volume)P1V1 = P2V2∴Example: A gas exerts a pressure of 3 kPa on the walls of container 1. When container 1 is emptied into a 10-liter container, the pressure exerted by the gas increases to 6 kPa. Find the volume of container 1. Assumethat the temperature and quantity of the gas remain constant.1 Charles’s law is a gas law relates volume to temperature. The law is named after (1) _____________________, who was a French inventor and scientist. He found through his experiment the volume of a gas increases linearly with an increase in the (2) _____________________. Shrinking of an inflated balloon and a bicycle tire in a very low temperature show the decrease of (3) ______________ which explains that the relationship of volume and temperature is directly related at constant (4) ______________. For a given sample of gas under two different conditions at a constant pressure, the equation can be written as (5) ________________________. 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:
This relationship of direct proportion can be written as: V ∝ T {\displaystyle V\propto T} So this means: V T = k , or V = k T {\displaystyle {\frac {V}{T}}=k,\quad {\text{or}}\quad V=kT} where:
This law describes how a gas expands as the temperature increases; conversely, a decrease in temperature will lead to a decrease in volume. For comparing the same substance under two different sets of conditions, the law can be written as: V 1 T 1 = V 2 T 2 {\displaystyle {\frac {V_{1}}{T_{1}}}={\frac {V_{2}}{T_{2}}}} The equation shows that, as absolute temperature increases, the volume of the gas also increases in proportion. The law was named after scientist Jacques Charles, who formulated the original law in his unpublished work from the 1780s. In two of a series of four essays presented between 2 and 30 October 1801,[2] John Dalton demonstrated by experiment that all the gases and vapours that he studied expanded by the same amount between two fixed points of temperature. The French natural philosopher Joseph Louis Gay-Lussac confirmed the discovery in a presentation to the French National Institute on 31 Jan 1802,[3] although he credited the discovery to unpublished work from the 1780s by Jacques Charles. The basic principles had already been described by Guillaume Amontons[4] and Francis Hauksbee[5] a century earlier. Dalton was the first to demonstrate that the law applied generally to all gases, and to the vapours of volatile liquids if the temperature was well above the boiling point. Gay-Lussac concurred.[6] With measurements only at the two thermometric fixed points of water, Gay-Lussac was unable to show that the equation relating volume to temperature was a linear function. On mathematical grounds alone, Gay-Lussac's paper does not permit the assignment of any law stating the linear relation. Both Dalton's and Gay-Lussac's main conclusions can be expressed mathematically as: V 100 − V 0 = k V 0 {\displaystyle V_{100}-V_{0}=kV_{0}\,}where V100 is the volume occupied by a given sample of gas at 100 °C; V0 is the volume occupied by the same sample of gas at 0 °C; and k is a constant which is the same for all gases at constant pressure. This equation does not contain the temperature and so is not what became known as Charles's Law. Gay-Lussac's value for k (1⁄2.6666), was identical to Dalton's earlier value for vapours and remarkably close to the present-day value of 1⁄2.7315. Gay-Lussac gave credit for this equation to unpublished statements by his fellow Republican citizen J. Charles in 1787. In the absence of a firm record, the gas law relating volume to temperature cannot be attributed to Charles. Dalton's measurements had much more scope regarding temperature than Gay-Lussac, not only measuring the volume at the fixed points of water but also at two intermediate points. Unaware of the inaccuracies of mercury thermometers at the time, which were divided into equal portions between the fixed points, Dalton, after concluding in Essay II that in the case of vapours, “any elastic fluid expands nearly in a uniform manner into 1370 or 1380 parts by 180 degrees (Fahrenheit) of heat”, was unable to confirm it for gases. Charles's law appears to imply that the volume of a gas will descend to zero at a certain temperature (−266.66 °C according to Gay-Lussac's figures) or −273.15 °C. Gay-Lussac was clear in his description that the law was not applicable at low temperatures:
At absolute zero temperature, the gas possesses zero energy and hence the molecules restrict motion. Gay-Lussac had no experience of liquid air (first prepared in 1877), although he appears to have believed (as did Dalton) that the "permanent gases" such as air and hydrogen could be liquified. Gay-Lussac had also worked with the vapours of volatile liquids in demonstrating Charles's law, and was aware that the law does not apply just above the boiling point of the liquid:
The first mention of a temperature at which the volume of a gas might descend to zero was by William Thomson (later known as Lord Kelvin) in 1848:[7]
However, the "absolute zero" on the Kelvin temperature scale was originally defined in terms of the second law of thermodynamics, which Thomson himself described in 1852.[8] Thomson did not assume that this was equal to the "zero-volume point" of Charles's law, merely that Charles's law provided the minimum temperature which could be attained. The two can be shown to be equivalent by Ludwig Boltzmann's statistical view of entropy (1870). However, Charles also stated: The volume of a fixed mass of dry gas increases or decreases by 1⁄273 times the volume at 0 °C for every 1 °C rise or fall in temperature. Thus: V T = V 0 + ( 1 273 × V 0 ) × T {\displaystyle V_{T}=V_{0}+({\tfrac {1}{273}}\times V_{0})\times T} V T = V 0 ( 1 + T 273 ) {\displaystyle V_{T}=V_{0}(1+{\tfrac {T}{273}})} where VT is the volume of gas at temperature T, V0 is the volume at 0 °C.The kinetic theory of gases relates the macroscopic properties of gases, such as pressure and volume, to the microscopic properties of the molecules which make up the gas, particularly the mass and speed of the molecules. To derive Charles's law from kinetic theory, it is necessary to have a microscopic definition of temperature: this can be conveniently taken as the temperature being proportional to the average kinetic energy of the gas molecules, Ek: T ∝ E k ¯ . {\displaystyle T\propto {\bar {E_{\rm {k}}}}.\,}Under this definition, the demonstration of Charles's law is almost trivial. The kinetic theory equivalent of the ideal gas law relates PV to the average kinetic energy:
The Wikibook School Science has a page on the topic of: Making Charles' law tubes
|