Dalton's law of partial pressures
Dalton's Law of Partial Pressures states that in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of the individual gases. This law is named after the English chemist John Dalton, who proposed it in the early 19th century. Dalton's Law is applicable under the assumption that the gases do not interact with each other.
Overview[edit | edit source]
The concept of partial pressure is crucial in understanding Dalton's Law. The partial pressure of a gas in a mixture is the pressure that the gas would exert if it alone occupied the entire volume of the mixture at the same temperature. Dalton's Law can be mathematically represented as: \[ P_{total} = P_1 + P_2 + P_3 + \ldots + P_n \] where \(P_{total}\) is the total pressure of the gas mixture, and \(P_1, P_2, P_3, \ldots, P_n\) are the partial pressures of the individual gases in the mixture.
Applications[edit | edit source]
Dalton's Law of Partial Pressures has several applications in various fields such as chemistry, physics, and engineering. It is particularly important in the calculation of gas mixtures in stoichiometry, the design of chemical reactors, and the analysis of atmospheric gases. Additionally, it plays a crucial role in the fields of respiratory physiology and anesthesiology, where it helps in understanding how gases are exchanged in the lungs and how they are administered during surgery.
Limitations[edit | edit source]
While Dalton's Law provides a good approximation in many cases, it has its limitations. It assumes that the gases in the mixture do not interact with each other, which is not always the case. Real gases can exhibit attractions or repulsions that can affect the total pressure of the mixture. Furthermore, the law is most accurate under conditions of low pressure and high temperature. At high pressures and low temperatures, deviations from the law can occur due to gas molecules being closer together, leading to interactions that are not accounted for in the law.
See Also[edit | edit source]
Search WikiMD
Ad.Tired of being Overweight? Try W8MD's physician weight loss program.
Semaglutide (Ozempic / Wegovy and Tirzepatide (Mounjaro / Zepbound) available.
Advertise on WikiMD
|
WikiMD's Wellness Encyclopedia |
| Let Food Be Thy Medicine Medicine Thy Food - Hippocrates |
Translate this page: - East Asian
中文,
日本,
한국어,
South Asian
हिन्दी,
தமிழ்,
తెలుగు,
Urdu,
ಕನ್ನಡ,
Southeast Asian
Indonesian,
Vietnamese,
Thai,
မြန်မာဘာသာ,
বাংলা
European
español,
Deutsch,
français,
Greek,
português do Brasil,
polski,
română,
русский,
Nederlands,
norsk,
svenska,
suomi,
Italian
Middle Eastern & African
عربى,
Turkish,
Persian,
Hebrew,
Afrikaans,
isiZulu,
Kiswahili,
Other
Bulgarian,
Hungarian,
Czech,
Swedish,
മലയാളം,
मराठी,
ਪੰਜਾਬੀ,
ગુજરાતી,
Portuguese,
Ukrainian
Medical Disclaimer: WikiMD is not a substitute for professional medical advice. The information on WikiMD is provided as an information resource only, may be incorrect, outdated or misleading, and is not to be used or relied on for any diagnostic or treatment purposes. Please consult your health care provider before making any healthcare decisions or for guidance about a specific medical condition. WikiMD expressly disclaims responsibility, and shall have no liability, for any damages, loss, injury, or liability whatsoever suffered as a result of your reliance on the information contained in this site. By visiting this site you agree to the foregoing terms and conditions, which may from time to time be changed or supplemented by WikiMD. If you do not agree to the foregoing terms and conditions, you should not enter or use this site. See full disclaimer.
Credits:Most images are courtesy of Wikimedia commons, and templates Wikipedia, licensed under CC BY SA or similar.
Contributors: Prab R. Tumpati, MD
