A) 8.74
B) 18.76
C) 24.06
D) 26.06
Correct Answer: D
Solution :
The entropy change \[=\frac{\text{heat of vaporisation}}{\text{temperature}}\] Here, heat of vaporisation \[=540\,cal/gm\] \[=540\times 18\,cal\,mo{{l}^{-1}}\] Temperature of water \[=100+273=373K\] \[\therefore \] entropy change \[=\frac{540\times 18}{373}=26.06\,cal\,mo{{l}^{-1}}{{K}^{-1}}\]You need to login to perform this action.
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