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NEET AIPMT SOLVED PAPER SCREENING 2006

  • question_answer
                    The enthalpy and entropy change for the reaction:                                                                                          \[B{{r}_{2}}(l)+C{{l}_{2}}(g)\to 2BrCl(g)\]                 are \[30\,kJ\,mo{{l}^{-1}}\] and \[105\,\,J{{K}^{-1}}\,mo{{l}^{-1}}\] respectively. The temperature at which the reaction will be in equilibrium is:                                                                                                              

    A)                  285.7 K   

    B)                  273 K   

    C)                  450 K      

    D)                  300 K

    Correct Answer: A

    Solution :

                            At equilibrium Gibbs free energy change \[(\Delta {{G}^{o}})\] is equal to zero. The following thermodynamic relation is used to show the relation of \[\Delta {{G}^{o}}\] with enthalpy change \[(\Delta {{H}^{o}})\]and entropy change \[(\Delta {{S}^{o}})\]                 \[\Delta {{G}^{o}}=\Delta {{H}^{o}}-T\Delta S\]                 \[=30\times {{10}^{3}}\,(J\,mo{{l}^{-1}})-T\times 105\,(J{{K}^{-1}}\,mo{{l}^{-1}})\]                         \[\therefore \]            \[T=\frac{30\times {{10}^{3}}}{105}K=285.71\,K\]


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