Water water interactions are weaker than water ethanol interactions
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In more generality, Raoult's law is stated as
Pi=xiPvapPi=xiPvap
and read "the partial vapor pressure of species ii is its (pure) vapor pressure multiplied by its mole fraction in the liquid phase." It assumes an ideal-gas gas phase and an ideal-solution liquid phase; an ideal solution is one in which all intermolecular attractions are of equal strength. More explicitly, the a−ba−binteractions are of equal strength to the a−aa−a and b−bb−b interactions, where aa and bbrepresent different chemical species in solution.
A positive deviation from Raoult's law occurs when the partial vapor pressure is greater than would be expected from Raoult's law. From a microscopic perspective, this implies that the a−b a−b interactions are weaker than the a−a a−a and b−b b−b interactions.
Pi=xiPvapPi=xiPvap
and read "the partial vapor pressure of species ii is its (pure) vapor pressure multiplied by its mole fraction in the liquid phase." It assumes an ideal-gas gas phase and an ideal-solution liquid phase; an ideal solution is one in which all intermolecular attractions are of equal strength. More explicitly, the a−ba−binteractions are of equal strength to the a−aa−a and b−bb−b interactions, where aa and bbrepresent different chemical species in solution.
A positive deviation from Raoult's law occurs when the partial vapor pressure is greater than would be expected from Raoult's law. From a microscopic perspective, this implies that the a−b a−b interactions are weaker than the a−a a−a and b−b b−b interactions.
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Water has strong intermolecular forces (hydrogen bonds). Ethanol (CH3CH2OH) and methylated spirits (mainly ethanol (CH3CH2OH) with some methanol (CH3OH)) both have hydrogen bonds but these are slightly weaker than the hydrogen bonds in water.
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