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A swimmer coming out from a pool is covered with a film of water weighing about 18 g. how much heat must be supplied to evaporate this water at 298 K ? Calculate the internal energy of vaperization at `100^(@)C`. `Delta_(vap)H^(Theta)` for water at 373 K = 40.66 kJ `mol^(-1)`

Text Solution

Verified by Experts

We can represent the process of evaporation as
`H_(2)O_((l))overset("vaporisation")rarrH_(2)O_((g)),Deltan=1-0=1`
`Delta_(vap)E=Delta_(vap)H-pDeltaV=DeltavapH-DeltanRT`
(assuming steam behaving as an ideal gas).
`Delta_(vap)E=40.66kJmol^(-1)-(1)`
`(8.314xx10^(-3)KJk^(-1)mol^(-1))(373K)=37.56kJmol^(-1)`
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