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Sieverts' law can be readily rationalized by considering the reaction of dissolution of the gas in the metal, which involves
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is the partial pressure of the gas at the interface with the metal (in the case above, the molecular nitrogen N
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is the concentration of the dissolved atoms into the metal (in the case above, atomic nitrogen N),
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C. K. Gupta, "Chemical metallurgy: principles and practice", Wiley-VCH, 2003, p.273.
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are examples of dissolved diatomic gases of frequent interest in metallurgy.
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172:{\displaystyle K={\frac {c_{\text{at}}^{2}}{p_{\text{mol}}}},}
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Sieverts, Adolf (1929). "The
Absorption of Gases by Metals".
255:{\displaystyle c_{\text{at}}={\sqrt {Kp_{\text{mol}}}}.}
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of the molecule of the gas. For example, for nitrogen:
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gas in metal is proportional to the square root of the
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113:(molecular gas) ⇌ 2 N (dissolved atoms)
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65:. It is named after German chemist
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117:For the above reaction, the
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53:, is a rule to predict the
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79:thermodynamic equilibrium
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119:equilibrium constant
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47:physical metallurgy
18:Sieverts's law
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16:(Redirected from
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75:partial pressure
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97:Justification
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277:Graham's law
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103:dissociation
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37:Sievers' law
272:Henry's law
209:Therefore,
33:linguistics
331:Metallurgy
325:Categories
283:References
55:solubility
51:chemistry
304:: 37–46.
266:See also
91:nitrogen
83:Hydrogen
71:diatomic
27:For the
182:where:
49:and in
31:law in
87:oxygen
63:metals
35:, see
59:gases
45:, in
89:and
243:mol
199:mol
160:mol
121:is
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61:in
57:of
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225:at
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190:at
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239:p
235:K
230:=
221:c
203:2
196:p
187:c
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156:p
150:2
141:c
135:=
132:K
111:2
109:N
39:.
20:)
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