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{{For|the [[Morphology (linguistics)|morphological]] law in [[linguistics]]|Sievers' law}} | |||
'''Sieverts's law''', in [[physical metallurgy]], is a rule to predict the [[solubility]] of [[gas]]es in [[metal]]s. It is named after German chemist [[Adolf Sieverts]] (1874–1947).<ref>{{cite journal | last = Sieverts | first = Adolf | title = The Absorption of Gases by Metals | journal = Zeitschrift für Metallkunde | volume = 21 | pages =37–46 | year = 1929}}</ref> The law states that the solubility of a [[Diatomic molecule|diatomic]] gas in metal is proportional to the square root of the [[partial pressure]] of the gas in thermodynamic equilibrium.<ref>C. K. Gupta, "Chemical metallurgy: principles and practice", Wiley-VCH, 2003, p.273.</ref> [[Hydrogen]], [[oxygen]] and [[nitrogen]] are examples of dissolved diatomic gases of frequent interest in metallurgy. | |||
== Justification == | |||
Sieverts's law can be readily rationalized by considering the reaction of dissolution of the gas in the metal, which involves [[Dissociation (chemistry)|dissociation]] of the molecule of the gas. For example, for nitrogen: | |||
:N<sub>2</sub>(gas) {{eqm}} 2 N(dissolved) | |||
For the above reaction, the [[equilibrium constant]], K, is: | |||
:<math>K^2 = {C_N^2 \over {p_{N_2}}}</math> | |||
Where: | |||
* C is the solubility | |||
* p is the partial pressure | |||
Therefore, | |||
:<math>C_N = {K \sqrt{p_{N_2}}}</math> | |||
== See also == | |||
* [[Henry's law]] | |||
== References == | |||
{{reflist}} | |||
[[Category:Metallurgy]] | |||
Revision as of 22:02, 25 January 2014
28 year-old Painting Investments Worker Truman from Regina, usually spends time with pastimes for instance interior design, property developers in new launch ec Singapore and writing. Last month just traveled to City of the Renaissance. Sieverts's law, in physical metallurgy, is a rule to predict the solubility of gases in metals. It is named after German chemist Adolf Sieverts (1874–1947).[1] The law states that the solubility of a diatomic gas in metal is proportional to the square root of the partial pressure of the gas in thermodynamic equilibrium.[2] Hydrogen, oxygen and nitrogen are examples of dissolved diatomic gases of frequent interest in metallurgy.
Justification
Sieverts's law can be readily rationalized by considering the reaction of dissolution of the gas in the metal, which involves dissociation of the molecule of the gas. For example, for nitrogen:
- N2(gas) Template:Eqm 2 N(dissolved)
For the above reaction, the equilibrium constant, K, is:
Where:
- C is the solubility
- p is the partial pressure
Therefore,
See also
References
43 year old Petroleum Engineer Harry from Deep River, usually spends time with hobbies and interests like renting movies, property developers in singapore new condominium and vehicle racing. Constantly enjoys going to destinations like Camino Real de Tierra Adentro.
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