AMU Medical AMU Solved Paper-2000

  • question_answer
    If the enthalpy of vaporisation of water is 186.5 J/mol, the entropy of its vaporization will be

    A)  \[0.5\,J{{K}^{-1}}\,mo{{l}^{-1}}\]             

    B)  \[1.0\,J{{K}^{-1}}\,mo{{l}^{-1}}\]

    C)  \[1.5\,J{{K}^{-1}}\,mo{{l}^{-1}}\]             

    D)  \[2.0\,J{{K}^{-1}}\,mo{{l}^{-1}}\]

    Correct Answer: A

    Solution :

                     Key Idea             \[\Delta S=\frac{\Delta {{H}_{vap}}}{{{T}_{b}}}\] Here,     \[\Delta {{H}_{vap}}=186.5\,\,J\,\,mo{{l}^{-1}}\]                 \[{{T}_{b}}=373\,K\] \[\therefore \]  \[\Delta S=\frac{186.5}{373}\]                 \[=0.5\,J{{K}^{-1}}mo{{l}^{-1}}\]


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