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The entropy change for vaporisation of a...

The entropy change for vaporisation of a liquid is `109.3 JK^(-1)mol^(-1)`. The molar heat of vaporisation of that liquid is `40.77kJ mol^(-1)`. Calculate the boiling point of that liquid. 

Text Solution

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Entropy change for vapourisation,
`Delta S = 109.3 JK ^(-1) mol ^(-1).` Molal heat of vapourisation of water is `40.77 kJ mol^(-1).` From the entropy change,
`Delta S = q _(rev)//T. ` Boiling point, `T= (q _(rsv))/(Delta S) (or)`
`T= (40.77 xx 1000)/(109.3) = 373K.`
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