A) \[9.77J/mol-K\]
B) \[10.77\text{ }J/mol-K\]
C) \[9.07\text{ }J/mol-K\]
D) \[0.977\text{ }J/mol-K\]
Correct Answer: A
Solution :
\[\Delta {{S}_{fus}}=\frac{\Delta {{H}_{fus}}}{{{T}_{m}}}\] where, \[\Delta {{S}_{fus}}\] = entropy change of fusion \[\Delta {{H}_{fus}}\]= enthalpy change of fusion Since, the heat absorbed is equal to the latent heat of fusion. \[{{T}_{m}}\]= melting temperature in degree kelvin \[=\frac{2930J/mol}{300K}\] \[\therefore \]\[\Delta {{S}_{fus}}=9.766\,J\,mo{{l}^{-1}}\,{{K}^{-1}}\]
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