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The entropy change in the conversion of ...

The entropy change in the conversion of water to ice at 272 k for the system is `-22.88 JK^(-1) mol^(-1)` and that of surrounding is `+24.85 jk^(-1) mol^(-1)` State whether the process is spontaneous or not ?

Text Solution

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`DeltaS_("univ")=DeltaS_("sys")+DeltaS_("surr")`
`=-22.88+(+24.85)`
`=1.97JK^(-1)mol^(-1)`
`:.DeltaS_("univ")gt0 "at "272K`
`:.` The process freezing of water is spontaneous.
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Knowledge Check

  • Entropy change involved in the conversion of 1 mole of liquid water at 373K to vapour at the same temperature will be ( Delta H_(vap) = 2.257 kJ g^(-1) ):

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