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