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| '''Raoult's law''' states that the [[vapour pressure]] of an [[ideal solution]] of <math>N</math> components is: | | '''Raoult's law''' states that the [[vapour pressure]] of an [[ideal solution]] of two components |
| :<math>P_v = \sum_{i=1}^{N} X_i P^*_{v,i} </math> | | :<math>P_v = X_A P^*_{v,A} + X_B P^*_{v,B}</math> |
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| where <math>X_i</math> is the [[molar fraction]] of component <math>i</math>, and <math>P^*_{v,i}</math> is the vapour pressure of pure <math>i</math>.
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| More generally, Raoult's law describes the [[partial pressure]] of component <math>A</math> in the vapour coexisting with a liquid mixture as:
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| :<math> P_A = X_A P^*_{v,A} </math>.
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| This law is obeyed for all components of an ideal solution, and is also obeyed for the solvent of an [[ideal dilute solution]]. The solute's partial pressure of such solutions then obey [[ Henry's law]]. Ideal dilute solutions describe the limiting behaviour of a mixture of infinite dilution. Therefore, all solutions in the limit of infinite dilution obey Raoult's law, i.e.:
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| :<math> \lim_{X_A \rightarrow 1} P_A = X_A P^*_{v,A} </math>.
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| ==References==
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| [[category: classical thermodynamics]] | | [[category: classical thermodynamics]] |