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Gay-Lussac's law usually refers to Joseph-Louis Gay-Lussac's law of combining volumes of gases, discovered in 1808 and published in 1809.[1] However, it sometimes refers to the proportionality of the volume of a gas to its absolute temperature at constant pressure. The latter law was published by Gay-Lussac in 1802,[2] but in the article in which he described his work, he cited earlier unpublished work from the 1780s by Jacques Charles. Consequently, the volume-temperature proportionality is usually known as Charles's Law.
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Transcription
For a gas, temperature and pressure are directly proportional. When you keep everything else constant, as the temperature of a gas goes up, its pressure goes up. As the temperature of a gas goes down, its pressure goes down. If you heat up a gas, the gas particles move faster. If the gas is in a solid container, with fixed volume, this means that the faster the gas particles move, the more times per second they collide with the sides of the container. That registers as increased pressure. The converse is also true - if you cool down this container of gas, that means the gas particles are moving more slowly. So there will be fewer collisions with the sides of the container per second, which means lower pressure. Joseph Louis Gay-Lussac shares credit with Guillaume Amontons for establishing a Gas Law describing the relationship between temperature and pressure. Gay-Lussac’s Law says that when the volume and amount of gas is constant, pressure and temperature are directly proportional. P ∝ T You can write this mathematically as P = kT where P = pressure, T = temperature in Kelvin, and k = is a proportionality constant. We can rearrange this equation so it reads P/T = k, or the ratio of pressure to temperature is a constant, k. Very often, Gay-Lussac’s law is used to compare two situations, a “before” and an “after.” In that case, you can say P1 / T1= k, and P2 / T2 = k, so you can write Gay-Lussac’s law as P1 / T1= P2 / T2. Let’s see an example. Example 1: A canister of nitrogen gas has a pressure of 2000 psi (pounds per square inch) at 20 C°. What will the pressure be if you increase the temperature to 25 C° ? Let’s write down Gay-Lussac’s Law: P1/ T1= P2 / T2, because we have a “before” and “after.” Convert temperatures to Kelvin: Kelvin = C°+ 273.15. T1 = 293.15 K, T2 = 298.15 K Substitute in what we know: 2000 psi / 293.15K = P2/ 298.15 K Solve for P2 (multiply both sides by 298.15 K) P2 = (2000 psi )(298.15 K)/293.15 K P2 = 2034 psi Example 2. Here’s another example: At 10 C°, a gas exerts 0.95 atm of pressure. At what temperature (in Celsius) will it exert a pressure of 0.75 atm? P1 /T1= P2/T2. Convert temperatures to Kelvin: Kelvin = C°+ 273.15. T1 = 283.15 K 0.95 atm/ 283.15 K = 0.75 atm/T2 Solve for T2 T2 = (283.15 K)(0.75 atm)/0.95 atm T2 = 223.54 K Convert to Celsius: 223.54K - 273.15 = - 49.6 C° Gay-Lussac’s Law relates temperature and pressure for a gas, but there are other gas laws which relate the other essential variables associated with a gas. Charles’s Law is the relationship between temperature and volume. Boyle’s Law is the relationship between pressure and volume. And the combined gas law puts all 3 together: Temperature, Pressure, and Volume. Notice that to use any of these laws, the amount of gas must be constant. Avogadro’s Law describes the relationship between volume and the amount of a gas (usually in terms of n, the number of moles). When we combine all 4 laws, we get the Ideal Gas Law. To decide which of these gas laws to use when solving a problem, make a list of what information you have, and what information you need. If a variable doesn’t come up, or is held constant in the problem, you don’t need it in your equation.
Law of combining volumes
The law of combining volumes states that when gases chemically react together, they do so in amounts by volume which bear small whole-number ratios (the volumes calculated at the same temperature and pressure).
The ratio between the volumes of the reactant gases and the gaseous products can be expressed in simple whole numbers.
For example, Gay-Lussac found that two volumes of hydrogen react with one volume of oxygen to form two volumes of gaseous water. Expressed concretely, 100 mL of hydrogen combine with 50 mL of oxygen to give 100 mL of water vapor: Hydrogen(100 mL) + Oxygen(50 mL) = Water(100 mL). Thus, the volumes of hydrogen and oxygen which combine (i.e., 100mL and 50mL) bear a simple ratio of 2:1, as also is the case for the ratio of product water vapor to reactant oxygen.
Based on Gay-Lussac's results, Amedeo Avogadro hypothesized in 1811 that, at the same temperature and pressure, equal volumes of gases (of whatever kind) contain equal numbers of molecules (Avogadro's law). He pointed out that if this hypothesis is true, then the previously stated result
- 2 volumes of hydrogen + 1 volume of oxygen = 2 volume of gaseous water
could also be expressed as
- 2 molecules of hydrogen + 1 molecule of oxygen = 2 molecule of water.
The law of combining volumes of gases was announced publicly by Joseph Louis Gay-Lussac on the last day of 1808, and published in 1809.[3][4] Since there was no direct evidence for Avogadro's molecular theory, very few chemists adopted Avogadro's hypothesis as generally valid until the Italian chemist Stanislao Cannizzaro argued convincingly for it during the First International Chemical Congress in 1860.[5]
Pressure-temperature law
In the 17th century Guillaume Amontons discovered a regular relationship between the pressure and temperature of a gas at constant volume. Some introductory physics textbooks still define the pressure-temperature relationship as Gay-Lussac's law.[6][7][8] Gay-Lussac primarily investigated the relationship between volume and temperature and published it in 1802, but his work did cover some comparison between pressure and temperature.[9] Given the relative technology available to both men, Amontons could only work with air as a gas, whereas Gay-Lussac was able to experiment with multiple types of common gases, such as oxygen, nitrogen, and hydrogen.[10]
Volume-temperature law
Regarding the volume-temperature relationship, Gay-Lussac attributed his findings to Jacques Charles because he used much of Charles's unpublished data from 1787 – hence, the law became known as Charles's law or the Law of Charles and Gay-Lussac.[11]
Amontons's, Charles', and Boyle's law form the combined gas law. These three gas laws in combination with Avogadro's law can be generalized by the ideal gas law.
Gay-Lussac used the formula acquired from ΔV/V = αΔT to define the rate of expansion α for gases. For air, he found a relative expansion ΔV/V = 37.50% and obtained a value of α = 37.50%/100 °C = 1/266.66 °C which indicated that the value of absolute zero was approximately 266.66 °C below 0 °C.[12] The value of the rate of expansion α is approximately the same for all gases and this is also sometimes referred to as Gay-Lussac's Law. See the introduction to this article, and Charles's Law.
See also
- Avogadro's law – Relationship between volume and amount of a gas at constant temperature and pressure
- Boyle's law – Relation between gas pressure and volume
- Charles's law – Relationship between volume and temperature of a gas at constant pressure
- Combined gas law – Combination of Charles', Boyle's and Gay-Lussac's gas laws
References
- ^ "Sur la combinaison des substances gazeuses, les unes avec les autres," Mémoires de physique et de chimie de la Société d’Arcueil, vol. 2 (1809), 207-34.
- ^ "Sur la dilatation des gaz," Annales de chimie, 43 (1802), 137-75.
- ^ Gay-Lussac (1809) "Mémoire sur la combinaison des substances gazeuses, les unes avec les autres" (Memoir on the combination of gaseous substances with each other), Mémoires de la Société d'Arcueil 2: 207–234. Available in English at: Le Moyne College.
- ^ "Joseph-Louis Gay-Lussac". chemistryexplained.com.
- ^ Hartley Harold (1966). "Stanislao Cannizzaro, F.R.S. (1826–1910) and the First International Chemical Conference at Karlsruhe". Notes and Records of the Royal Society of London. 21 (1): 56–63. doi:10.1098/rsnr.1966.0006. S2CID 58453894.
- ^ Tippens, Paul E. (2007). Physics, 7th ed. McGraw-Hill. 386–387.
- ^ Cooper, Crystal (Feb. 11, 2010). "Gay-Lussac's Law". Bright Hub Engineering. Retrieved from http://www.brighthubengineering.com/hvac/26213-gay-lussacs-law/ on July 8, 2013.
- ^ Verma, K.S. - Cengage Physical Chemistry Part 1 - Section 5.6.3
- ^ Crosland, Maurice P. (2004). Gay-Lussac: Scientist and Bourgeois. Cambridge University Press. 119–120.
- ^ Asimov, Isaac (1966). Understanding Physics – Motion, Sound, and Heat. Walker and Co. 191–192.
- ^ Gay-Lussac (1802), "Recherches sur la dilatation des gaz et des vapeurs" (Researches on the expansion of gases and vapors), Annales de Chimie 43: 137–175. On page 157, Gay-Lussac mentions the unpublished findings of Charles: "Avant d'aller plus loin, je dois prévenir que quoique j'eusse reconnu un grand nombre de fois que les gaz oxigène, azote, hydrogène et acide carbonique, et l'air atmosphérique se dilatent également depuis 0° jusqu'a 80°, le cit. Charles avait remarqué depuis 15 ans la même propriété dans ces gaz; mais n'avant jamais publié ses résultats, c'est par le plus grand hasard que je les ai connus." (Before going further, I should inform [you] that although I had recognized many times that the gases oxygen, nitrogen, hydrogen, and carbonic acid [i.e., carbon dioxide], and atmospheric air also expand from 0° to 80°, citizen Charles had noticed 15 years ago the same property in these gases; but having never published his results, it is by the merest chance that I knew of them.) Available in English at: Le Moyne College.
- ^ Gay-Lussac (1802). "Recherches sur la dilatation des gaz et des vapeurs". Annales de chimie, ou, Recueil de mémoires concernant la chimie (in French).
Further reading
- Castka, Joseph F.; Metcalfe, H. Clark; Davis, Raymond E.; Williams, John E. (2002). Modern Chemistry. Holt, Rinehart and Winston. ISBN 978-0-03-056537-3.
- Guch, Ian (2003). The Complete Idiot's Guide to Chemistry. Alpha, Penguin Group Inc. ISBN 978-1-59257-101-7.
- Mascetta, Joseph A. (1998). How to Prepare for the SAT II Chemistry. Barron's. ISBN 978-0-7641-0331-5.
This page was last edited on 21 March 2024, at 18:42