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The entropy change associated with the c...

The entropy change associated with the conversion of 1 kg of ice at 273 K to water vapours at 383 K is :
(Specific heat of water liquid and water vapour are `4.2kJK^(-1)kg^(-1)` and `2.0kJK^(-1)kg^(-1)` , heat of liquid fusion and vapourisation of water are `334kJ kg^(-1)` and `2491kJ kg^(-1)`, respectively ). (`log 273=2.436,log373=2.572, log 383=2.583`)

A

`9.26 kJ kg^(-1)K^(-1)`

B

`2.64 kJ kg^(-1)K^(-1)`

C

`7.90 kJ kg^(-1)K^(-1)`

D

`8.49 kJ kg^(-1)K^(-1)`

Text Solution

Verified by Experts

The correct Answer is:
A
Overall process
`underset(273K)(H_(2)O" (ice)")overset(a)rarr underset(273K)(H_(2)O(l))overset(b)rarr underset(373K)(H_(2)O(l))overset(c ) rarr underset(373K)(H_(2)O(g))overset(d)rarr underset(383K)(H_(2)O(g))`
`DeltaS_(a)=(DeltaH_("fusion"))/(273)=(334)/(273)=1.22`
`DeltaS_(b)=4.2ln((373)/(273))=1.31`
`DeltaS_(c)=(DeltaH_("vapourisation"))/(373)=(2491)/(373)=6.67`
`DeltaS_(a)=2ln((383)/(373))=0.05`
`DeltaS_("Total")=DeltaS_(a)+DeltaS_(b)+DeltaS_(c)+DeltaS_(d)=1.22+1.31+6.67+0.05~="9.26 K J kg"^(-1)K^(-1)`
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