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NEET AIPMT SOLVED PAPER 2003

  • question_answer
                    What is the entropy change (in \[J{{K}^{-1}}\,mo{{l}^{-1}}\]) when one mole of ice is converted into water at \[{{0}^{\text{o}}}C\]? (The enthalpy change for the conversion of ice to liquid water is \[6.0\,kJ\,mo{{l}^{-1}}\] at \[{{0}^{\text{o}}}C\].)                                          

    A)                            2.198     

    B)                 21.98     

    C)                 20.13     

    D)                 2.013

    Correct Answer: B

    Solution :

                    \[\Delta S=\frac{\Delta {{H}_{f}}\,}{T}=\frac{6.0}{273}=0.2198\,\,k\,J\,{{K}^{-1}}\,mo{{l}^{-1}}\]                 \[(T={{0}^{o}}C+273=273\,K)\]                 \[=0.02198\times 1000\,J{{K}^{-1}}\,mo{{l}^{-1}}\]                 \[=21.98\,J{{K}^{-1}}\,\,mo{{l}^{-1}}\]


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