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NEET Sample Paper NEET Sample Test Paper-49

  • question_answer
    The molar entropies of HI(g), H(g) and I(g) at 298 K are 206.5, 114.6 and 180.7 J \[mo{{l}^{-1}}{{K}^{-1}}\] respectively. Using the AG given below, calculate the bond energy of HI \[HI\left( g \right)\,\,\to \,\,H\left( g \right)+I\left( g \right)\text{ }\Delta G=271.8\text{ }kJ\]

    A) 282.4 kJ                       

    B) 298.3 kJ

    C) 290.1 kJ                       

    D) 315.4 kJ

    Correct Answer: B

    Solution :

    \[\underset{g}{\mathop{HI}}\,\to \underset{g}{\mathop{H}}\,~\,\,\,\,\,\,\,\,+~\,\,\,\,\,\,\underset{g}{\mathop{I}}\,~~~~~\,\,\,\Delta G=\text{ }271.8\text{ }kJ\] \[\Delta S=\text{ }206.5\text{ }114.6~~\,\,180.7~~~J\,\,mo{{l}^{-}}^{1}\] \[\Delta S\text{ }=\left( 114.6+180.7 \right)-\left( 206.5 \right)\] \[=\text{ }295.3\,\,-\,\,206.5\] \[\Delta S\,\,=\,\,88.8\text{ }J\text{ }mo{{l}^{-1}}\,{{K}^{-}}^{1}\] \[\Delta G=\Delta H-T\Delta S\] \[=\text{ }271.8\,\,+\,\,298\,\,\times \,\,\frac{88.8}{1000}\,\,=\,\,298.3\text{ }kJ\]


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